Curriculum Standards:

Determine the conditions under which real gases are most likely to differ from ideal gases. - CHEM12_C14.3.2
Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. - CHEM12_C14.3.1
Explain how ions form. - CHEM12_C06.3.2
Describe trends among elements for atomic size. - CHEM12_C06.3.1
Describe periodic trends for first ionization energy, ionic size, and electronegativity. - CHEM12_C06.3.3
Identify two types of stereoisomers. - CHEM12_C22.3.2
Explain how the properties of constitutional isomers differ. - CHEM12_C22.3.1
Explain how anions form. - CHEM12_C07.1.4
Describe how cations form. - CHEM12_C07.1.3
Identify the atoms of elements that tend to lose and tend to gain electrons. - CHEM12_C07.1.2
Understand scientific notation. - CHEM12_MD2.3
Understand significant figures. - CHEM12_MD2.2
Understand ratios, rates, and proportions. - CHEM12_MD2.1
Describe some practical uses of radioisotopes. - CHEM12_C25.4.2
Compare three devices that are used to detect radiation. - CHEM12_C25.4.1
Write numbers in scientific notation. - CHEM12_C03.1.1
Explain why measurements must be reported to the correct number of significant figures. - CHEM12_C03.1.3
Evaluate accuracy and precision. - CHEM12_C03.1.2
Identify two ways that you can determine the heat of reaction when it cannot be directly measured. - CHEM12_C17.4.1
List the general guidelines that can help you write the name and formula of a chemical compound. - CHEM12_C09.5.2
Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. - CHEM12_C09.5.1
Describe the function of ATP in the cell. - CHEM12_C24.6.1
Describe the five general types of reactions. - CHEM12_C11.2.1
Predict the products of the five general types of reactions. - CHEM12_C11.2.2
Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. - CHEM12_C15.1.1
Distinguish between a substance and a mixture. - CHEM12_C02.3.2
Describe the structure of ice. - CHEM12_C15.1.2
Explain the difference between an element and a compound. - CHEM12_C02.3.1
Explain how a periodic table is useful. - CHEM12_C02.3.4
Describe what chemists use to represent elements and compounds. - CHEM12_C02.3.3
Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. - CHEM12_C18.2.1
Describe how most reactions progress from start to finish. - CHEM12_C18.2.2
List the types of information that can be displayed in a periodic table. - CHEM12_C06.2.1
Relate the total pressure of a mixture of gases to the partial pressures of the component gases. - CHEM12_C14.4.1
Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. - CHEM12_C14.4.2
Describe how to express the rate of a chemical reaction. - CHEM12_C18.1.1
Describe bonding in a benzene ring. - CHEM12_C22.4.2
Identify the general structure of a cyclic hydrocarbon. - CHEM12_C22.4.1
Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. - CHEM12_C24.6.3
Describe three properties of ionic compounds. - CHEM12_C07.2.2
Describe what happens to biological molecules and energy during catabolism and anabolism. - CHEM12_C24.6.2
Explain the electrical charge of an ionic compound. - CHEM12_C07.2.1
Understand measurements and conversions. - CHEM12_MD1.3
Understand integers and absolute values. - CHEM12_MD1.2
Multiply and divide fractions. - CHEM12_MD1.1
Describe what happens in a nuclear chain reaction. - CHEM12_C25.3.1
Distinguish fission reactions from fusion reactions. - CHEM12_C25.3.3
Describe what happens to spent fuel rods. - CHEM12_C25.3.2
Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. - CHEM12_C17.3.1
Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. - CHEM12_C17.3.2
Describe thermochemical changes that occur when a solution forms. - CHEM12_C17.3.3
Identify the number of bases of DNA required to specify one amino acid in a peptide chain. - CHEM12_C24.5.2
Describe how to write a skeleton equation. - CHEM12_C11.1.1
Determine the number of valence electrons in an atom of a representative element. - CHEM12_C07.1.1
Identify the functions of DNA and RNA. - CHEM12_C24.5.1
Describe the steps for writing and balancing a chemical equation. - CHEM12_C11.1.2
Identify the types of substances that dissolve most readily in water. - CHEM12_C15.2.1
Explain how mixtures can be separated. - CHEM12_C02.2.2
Explain why all ionic compounds are electrolytes. - CHEM12_C15.2.2
Explain why hydrates easily lose and regain water. - CHEM12_C15.2.3
Explain how mixtures are classified. - CHEM12_C02.2.1
Identify four factors that influence the rate of a chemical reaction. - CHEM12_C18.1.2
Calculate the percent by mass of an element in a compound. - CHEM12_C10.3.1
Distinguish between empirical and molecular formulas. - CHEM12_C10.3.3
Calculate the empirical formula of a compound. - CHEM12_C10.3.2
Describe the steps for solving nonnumeric problems. - CHEM12_C01.4.3
Describe the steps for solving numeric problems. - CHEM12_C01.4.2
Describe the three factors that affect gas pressure. - CHEM12_C14.1.2
Identify the general approach to solving a problem. - CHEM12_C01.4.1
Explain why gases are easier to compress than solids or liquids. - CHEM12_C14.1.1
Describe how [H+] and [OH+] are related in an aqueous solution. - CHEM12_C19.2.1
Classify a solution as neutral, acidic, or basic using pH. - CHEM12_C19.2.2
Identify two methods that are used to measure pH. - CHEM12_C19.2.3
Classify coal. - CHEM12_C22.5.3
Describe the first step in the refining of petroleum. - CHEM12_C22.5.2
Graph linear and nonlinear functions. - CHEM12_MD4.2
Identify the hydrocarbons found in natural gas. - CHEM12_C22.5.1
Describe how the structure and properties of solids are related. - CHEM12_C13.3.1
Identify the factors that determine the shape of a crystal. - CHEM12_C13.3.2
Explain the importance of alloys. - CHEM12_C07.3.3
Describe the arrangement of atoms in a metal. - CHEM12_C07.3.2
What are two examples of DNA technologies used today? - CHEM12_C24.5.4
Model the valence electrons of metal atoms. - CHEM12_C07.3.1
Define gene mutations. - CHEM12_C24.5.3
Understand slope and rate of change. - CHEM12_MD4.1
Identify instruments used to observe individual atoms. - CHEM12_C04.1.2
Explain how Democritus and John Dalton described atoms. - CHEM12_C04.1.1
Solve problems that involve half-life. - CHEM12_C25.2.2
Identify factors that determine the type of decay a radioisotope undergoes. - CHEM12_C25.2.1
Identify two ways transmutations can occur. - CHEM12_C25.2.3
Describe the representative units that define molecular compounds and ionic compounds. - CHEM12_C08.1.2
Identify the information a molecular formula provides. - CHEM12_C08.1.1
Describe the kinds of problems that can be easily solved using dimensional analysis. - CHEM12_C03.3.2
Explain what happens when a measurement is multiplied by a conversion factor. - CHEM12_C03.3.1
Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. - CHEM12_C20.1.1
Explain how the presence of salts and acids accelerates the corrosion of metals. - CHEM12_C20.1.2
Identify the physical property that distinguishes lipids from other biological molecules. - CHEM12_C24.4.1
Describe the relationship between the solubility product constant and the solubility of a compound. - CHEM12_C18.4.1
Predict whether a precipitation will occur when two solutions are mixed. - CHEM12_C18.4.2
Convert the volume of a gas at STP to the number of moles of the gas. - CHEM12_C10.2.2
Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. - CHEM12_C10.2.1
Describe the relationships among pressure, volume, and temperature of a gas. - CHEM12_C14.2.1
Define an acid and a base according to Arrhenius. - CHEM12_C19.1.1
Distinguish an acid from a base in the BrÌünsted-Lowry theory. - CHEM12_C19.1.2
Define an acid and a base according to Lewis. - CHEM12_C19.1.3
Identify the conditions necessary for sublimation. - CHEM12_C13.4.1
Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. - CHEM12_C13.4.2
Solve multi-step equations. - CHEM12_MD3.1
Explain the relationship between unstable isotopes and radioactivity. - CHEM12_C25.1.1
Describe three main types of nuclear radiation. - CHEM12_C25.1.2
Explain the result of electron sharing in covalent bonds. - CHEM12_C08.2.1
Identify some exceptions to the octet rule. - CHEM12_C08.2.3
Define oxidation and reduction in terms of a change in oxidation number. - CHEM12_C20.2.2
Describe how coordinate covalent bonds are different from other covalent bonds. - CHEM12_C08.2.2
Describe how resonance structures are used. - CHEM12_C08.2.5
Explain how the strength of a covalent bond is related to its bond dissociation energy. - CHEM12_C08.2.4
Calculate the density of a substance. - CHEM12_C03.2.3
Identify the temperature units scientists commonly use. - CHEM12_C03.2.2
Explain why metric units are easy to use. - CHEM12_C03.2.1
Describe how enzymes affect the rates of reactions in living things. - CHEM12_C24.3.3
State the general rule for assigning oxidation numbers. - CHEM12_C20.2.1
Identify what determines the differences in the chemical and physiological properties of peptides and proteins. - CHEM12_C24.3.2
Diagram the general structure of an amino acid. - CHEM12_C24.3.1
Describe what happens during a chemical change. - CHEM12_C02.4.1
Convert among the count, mass, and volume of something. - CHEM12_C10.1.1
Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. - CHEM12_C02.4.3
Identify four possible clues that a chemical change has taken place. - CHEM12_C02.4.2
Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. - CHEM12_C18.3.2
Describe what the size of an equilibrium constant indicates about a system at equilibrium. - CHEM12_C18.3.3
Describe what happens at the molecular level in a chemical system at equilibrium. - CHEM12_C18.3.1
Determine the molar mass of an element and of a compound. - CHEM12_C10.1.3
Explain how chemists count the number of atoms, molecules, or formula units in a substance. - CHEM12_C10.1.2
Identify the point in a titration when neutralization will occur. - CHEM12_C19.4.2
Identify some outcomes of modern research in chemistry. - CHEM12_C01.2.2
Identify three general reasons to study chemistry. - CHEM12_C01.2.1
Identify the products that form when an acid and a base react. - CHEM12_C19.4.1
Explain how sublevels of principal energy levels differ. - CHEM12_C05.1.3
Describe what the quantum mechanical model determines about the electrons in an atom. - CHEM12_C05.1.2
Describe what Bohr proposed in his model of the atom. - CHEM12_C05.1.1
Describe the three assumptions of the kinetic theory as it applies to gases. - CHEM12_C13.1.1
Interpret gas pressure in terms of kinetic theory. - CHEM12_C13.1.2
Define the relationship between the temperature in kelvins and the average kinetic energy of particles. - CHEM12_C13.1.3
Describe how a voltaic cell produces electrical energy. - CHEM12_C21.1.2
Identify the current applications that use electrochemical processes to produce electrical energy. - CHEM12_C21.1.3
Explain how isotopes of an element differ. - CHEM12_C04.3.2
Explain what makes one element different from another. - CHEM12_C04.3.1
Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. - CHEM12_C12.3.1
Explain what the percent yield of a reaction measures. - CHEM12_C12.3.2
Identify the type of chemical reaction that is involved in all electrochemical processes. - CHEM12_C21.1.1
Describe how VSEPR theory helps predict the shapes of molecules. - CHEM12_C08.3.2
Identify the two classes of chemical reactions. - CHEM12_C20.3.1
Describe the relationship between atomic and molecular orbitals. - CHEM12_C08.3.1
Describe two different methods for balancing a redox equation. - CHEM12_C20.3.2
Identify the ways in which orbital hybridization is useful in describing molecules. - CHEM12_C08.3.3
Explain how colligative properties can be explained on a particle basis. - CHEM12_C16.3.1
Construct the general formula for carbohydrates. - CHEM12_C24.2.1
Explain how polyatomic ions differ from and are similar to monatomic ions. - CHEM12_C09.1.2
Explain how to determine the charges of monatomic ions. - CHEM12_C09.1.1
Describe how condensation polymers are formed. - CHEM12_C23.4.2
Describe how addition polymers are formed. - CHEM12_C23.4.1
Explain the role collaboration and communication play in science. - CHEM12_C01.3.3
Identify three steps in the scientific method. - CHEM12_C01.3.2
Describe how Lavoisier transformed chemistry. - CHEM12_C01.3.1
Describe how acids and bases are classified as either strong or weak. - CHEM12_C19.3.1
Identify the factors that determine physical properties of a liquid. - CHEM12_C13.2.1
Define evaporation in terms of kinetic energy. - CHEM12_C13.2.2
Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. - CHEM12_C13.2.3
Identify the conditions under which boiling occurs. - CHEM12_C13.2.4
Identify what causes the electrical potential of an electrochemical cell. - CHEM12_C21.2.1
Determine the standard reduction potential of a half-cell. - CHEM12_C21.2.2
Determine if a redox reaction is spontaneous or nonspontaneous. - CHEM12_C21.2.3
Identify three types of subatomic particles. - CHEM12_C04.2.1
Describe the structure of atoms according to the Rutherford model. - CHEM12_C04.2.2
Identify the two ways of expressing the ratio of solute to solvent in a solution. - CHEM12_C16.4.1
Describe how the freezing-point depression and boiling-point elevation are related to molality. - CHEM12_C16.4.2
Describe how electronegativity values determine the charge distribution in a polar molecule. - CHEM12_C08.4.1
Explain why the properties of covalent compounds are so diverse. - CHEM12_C08.4.3
Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. - CHEM12_C08.4.2
Identify the compound that is reduced during photosynthesis and the compounds formed. - CHEM12_C24.1.2
Calculate the atomic mass of an element. - CHEM12_C04.3.3
Identify the two major cell types that occur in nature. - CHEM12_C24.1.1
Apply the rules for naming and writing formulas for compounds with polyatomic ions. - CHEM12_C09.2.2
Apply the rules for naming and writing formulas for binary ionic compounds. - CHEM12_C09.2.1
Describe how the value of ‰ö G is related to the spontaneity of a reaction. - CHEM12_C18.5.4
Identify the part entropy plays in a chemical reaction. - CHEM12_C18.5.2
Identify the two factors that determine whether a reaction is spontaneous. - CHEM12_C18.5.3
Identify the two characteristics of spontaneous reactions. - CHEM12_C18.5.1
Explain why dehydrogenation is classified as an oxidation reaction. - CHEM12_C23.3.3
Identify the general formula of a carboxylic acid. - CHEM12_C23.3.2
Identify the general formula of an ester. - CHEM12_C23.3.4
Identify the structural characteristic that an aldehyde and a ketone share. - CHEM12_C23.3.1
Identify three broad classes of elements. - CHEM12_C06.1.4
Describe how the modern periodic table is organized. - CHEM12_C06.1.3
Explain what causes atomic emission spectra. - CHEM12_C05.3.1
Explain why a carbon atom forms four covalent bonds. - CHEM12_C22.1.1
Identify two possible arrangements of carbon atoms in an alkane. - CHEM12_C22.1.2
Distinguish between electrolytic and voltaic cells. - CHEM12_C21.3.1
Describe some applications that use electrolytic cells. - CHEM12_C21.3.2
Describe how you measure the change in enthalpy of a reaction. - CHEM12_C17.2.1
Describe the quantities you can use to interpret a balanced chemical equation. - CHEM12_C12.1.2
Identify the questions that are always conserved in chemical reactions. - CHEM12_C12.1.3
Describe how chemists use balanced chemical equations. - CHEM12_C12.1.1
Describe the equilibrium in a saturated solution. - CHEM12_C16.1.2
Describe the factors that affect the solubility of a substance. - CHEM12_C16.1.3
Identify the factors that affect how fast a substance dissolves. - CHEM12_C16.1.1
Describe how you express the enthalpy change for a reaction in a chemical equation. - CHEM12_C17.2.2
Apply the rules for naming and writing formulas for binary molecular compounds. - CHEM12_C09.3.1
Classify physical changes. - CHEM12_C02.1.3
Distinguish between a suspension and a solution. - CHEM12_C15.3.1
Identify how to distinguish a colloid from a suspension and a solution. - CHEM12_C15.3.2
Identify the three states of matter. - CHEM12_C02.1.2
Explain why all samples of a substance have the same intensive properties. - CHEM12_C02.1.1
Identify the general formula of an amine. - CHEM12_C23.2.4
Identify the general formula of an ether. - CHEM12_C23.2.3
Explain how addition reactions are used in organic chemistry. - CHEM12_C23.2.2
Identify the general formula of an alcohol. - CHEM12_C23.2.1
Describe when a solution of a salt is acidic or basic. - CHEM12_C19.5.1
Identify the components of a buffer. - CHEM12_C19.5.2
Identify the central themes of chemistry. - CHEM12_C01.1.3
Identify five traditional areas of study in chemistry. - CHEM12_C01.1.2
Classify elements based on electron configuration. - CHEM12_C06.2.2
Explain why the scope of chemistry is so vast. - CHEM12_C01.1.1
List the three rules for writing the electron configurations of elements. - CHEM12_C05.2.1
Identify the structural characteristics of alkynes. - CHEM12_C22.2.2
Describe the structural characteristics of alkenes. - CHEM12_C22.2.1
Explain the ways in which energy changes can occur. - CHEM12_C17.1.1
Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. - CHEM12_C17.1.2
Explain how mole ratios are used in chemical calculations. - CHEM12_C12.2.1
Explain the general procedure for solving a stoichiometric problem. - CHEM12_C12.2.2
Express solution concentration as a percent by volume or percent by mass. - CHEM12_C16.2.3
Calculate the molarity of a solution. - CHEM12_C16.2.1
Describe the effect of dilution on the total moles of solute in solution. - CHEM12_C16.2.2
Identify two factors on which the heat capacity of an object depends. - CHEM12_C17.1.3
Determine the name and formula of a base. - CHEM12_C09.4.2
Determine the name and formula of an acid. - CHEM12_C09.4.1
Describe the information found in a net ionic equation. - CHEM12_C11.3.1
Predict the formation of a precipitate in a double-replacement reaction. - CHEM12_C11.3.2
Distinguish between quantum mechanics and classical mechanics. - CHEM12_C05.3.4
Explain how the frequencies of light are related to changes in electron energies. - CHEM12_C05.3.3
Describe how Einstein explained the photoelectric effect. - CHEM12_C05.3.2
Describe how Mendeleev organized his periodic table. - CHEM12_C06.1.2
Explain how chemists began to organize the known elements. - CHEM12_C06.1.1
Classify organic compounds. - CHEM12_C23.1.1
Describe how substitution reactions are used in organic chemistry. - CHEM12_C23.1.3
Identify the general formula of a halocarbon. - CHEM12_C23.1.2


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Title: Pearson Chemistry 2012 Realize


         Math Diagnostic and Remediation
         
            Using the Math Diagnostic Tests and Remediation

            Multiplying Fractions
              Curriculum Standards: Multiply and divide fractions. Understand integers and absolute values. Understand measurements and conversions. 

            Absolute Values
              Curriculum Standards: Multiply and divide fractions. Understand integers and absolute values. Understand measurements and conversions. 

            Converting Measurements
              Curriculum Standards: Multiply and divide fractions. Understand integers and absolute values. Understand measurements and conversions. 

            Dividing Fractions
              Curriculum Standards: Multiply and divide fractions. Understand integers and absolute values. Understand measurements and conversions. 

            Adding Integers
              Curriculum Standards: Multiply and divide fractions. Understand integers and absolute values. Understand measurements and conversions. 

            Using Conversion Factors
              Curriculum Standards: Multiply and divide fractions. Understand integers and absolute values. Understand measurements and conversions. 

            Multiplying Rational Expressions
              Curriculum Standards: Multiply and divide fractions. Understand integers and absolute values. Understand measurements and conversions. 

            Subtracting Integers
              Curriculum Standards: Multiply and divide fractions. Understand integers and absolute values. Understand measurements and conversions. 

            Comparing Unit Rates
              Curriculum Standards: Multiply and divide fractions. Understand integers and absolute values. Understand measurements and conversions. 

            Equivalent Fractions
              Curriculum Standards: Multiply and divide fractions. Understand integers and absolute values. Understand measurements and conversions. 

            Diagnostic Test 1: Fractions, Integers, and Measurements
              Curriculum Standards: Multiply and divide fractions. Understand integers and absolute values. Understand measurements and conversions. 

            Diagnostic 1 Posttest: Fractions, Integers, and Measurements
              Curriculum Standards: Multiply and divide fractions. Understand integers and absolute values. Understand measurements and conversions. 

            Solving Proportions
              Curriculum Standards: Understand ratios, rates, and proportions. Understand significant figures. Understand scientific notation. 

            Significant Figures Intervention
              Curriculum Standards: Understand ratios, rates, and proportions. Understand significant figures. Understand scientific notation. 

            Writing a Number in Scientific Notation
              Curriculum Standards: Understand ratios, rates, and proportions. Understand significant figures. Understand scientific notation. 

            Comparing Unit Rates
              Curriculum Standards: Understand ratios, rates, and proportions. Understand significant figures. Understand scientific notation. 

            Writing a Number in Standard Notation
              Curriculum Standards: Understand ratios, rates, and proportions. Understand significant figures. Understand scientific notation. 

            Writing Ratios
              Curriculum Standards: Understand ratios, rates, and proportions. Understand significant figures. Understand scientific notation. 

            Ordering Numbers in Scientific Notation
              Curriculum Standards: Understand ratios, rates, and proportions. Understand significant figures. Understand scientific notation. 

            Diagnostic Test 2: Ratios, Significant Figures, and Scientific Notation
              Curriculum Standards: Understand ratios, rates, and proportions. Understand significant figures. Understand scientific notation. 

            Diagnostic 2 Posttest: Ratios, Significant Figures, and Scientific Notation
              Curriculum Standards: Understand ratios, rates, and proportions. Understand significant figures. Understand scientific notation. 

            Solving Two-Step Equations
              Curriculum Standards: Solve multi-step equations. 

            Transforming Formulas
              Curriculum Standards: Solve multi-step equations. 

            Equations with Variables on Both Sides
              Curriculum Standards: Solve multi-step equations. 

            Diagnostic Test 3: Multi-Step Equations
              Curriculum Standards: Solve multi-step equations. 

            Diagnostic 3 Posttest: Multi-Step Equations
              Curriculum Standards: Solve multi-step equations. 

            Finding Slope Using Rise and Run
              Curriculum Standards: Understand slope and rate of change. Graph linear and nonlinear functions. 

            Graphing
              Curriculum Standards: Understand slope and rate of change. Graph linear and nonlinear functions. 

            Finding Slope Using Coordinates
              Curriculum Standards: Understand slope and rate of change. Graph linear and nonlinear functions. 

            Graphing nonlinear functions
              Curriculum Standards: Understand slope and rate of change. Graph linear and nonlinear functions. 

            Finding Rate of Change Using a Table
              Curriculum Standards: Understand slope and rate of change. Graph linear and nonlinear functions. 

            Graphing Linear Functions
              Curriculum Standards: Understand slope and rate of change. Graph linear and nonlinear functions. 

            Finding Rate of Change Using a Graph
              Curriculum Standards: Understand slope and rate of change. Graph linear and nonlinear functions. 

            Diagnostic Test 4 Pretest: Graphing
              Curriculum Standards: Understand slope and rate of change. Graph linear and nonlinear functions. 

            Diagnostic 4 Posttest: Graphing
              Curriculum Standards: Understand slope and rate of change. Graph linear and nonlinear functions. 

         Chapter 1: Introduction to Chemistry
         
            Chapter-Level Activities
            
               Ch. 1 Math Tutorial: Equations

               Ch. 1 Concepts in Action: What Would Happen in a World Without Chemistry?
                 Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

               Ch. 1 Directed Virtual Lab: Lab Safety
                 Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

               Ch. 1 Problem Set
                 Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

               Ch. 1 What Good Can Chemistry Do?

               Chapter 1 Flash Cards

            1.1 The Scope of Chemistry
            
               1.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. 

            1.2 Chemistry and You
            
               1.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. 

            1.3 Thinking Like a Scientist
            
               1.3 Kinetic Art: Three-Dimensional Molecular Models
                 Curriculum Standards: Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. 

               1.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. 

            1.4 Problem Solving in Chemistry
            
               1.4 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

               1.4 Chemistry Tutorial: Estimating Walking Time
                 Curriculum Standards: Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

               1.4 Foundations Chemistry Tutorial: Estimating Walking Time
                 Curriculum Standards: Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

            Chapter 1 Online Student Edition
              Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

            Chapter 1.2 Online Student Edition: Why Study Chemistry?
              Curriculum Standards: Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. 

            Chapter 1.4 Online Student Edition: Solving Nonnumeric Problems
              Curriculum Standards: Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

            Chapter 1.1 Online Student Edition: Big Ideas In Chemistry
              Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. 

            1.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. 

            Ch. 1 Concepts in Action: What Would Happen in a World Without Chemistry?
              Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

            Ch. 1 Directed Virtual Lab: Lab Safety
              Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

            1.4 Chemistry Tutorial: Estimating Walking Time
              Curriculum Standards: Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

            Chapter 1.3 Online Student Edition: Collaboration and Communication
              Curriculum Standards: Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. 

            Study WB Chapter 1 Lesson 4
              Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

            1.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. 

            1.4 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

            Chapter 1.4 Online Student Edition: Solving Numeric Problems
              Curriculum Standards: Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

            Chapter 1.2 Online Student Edition: Chemistry, Technology, and Society
              Curriculum Standards: Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. 

            Chapter 1.1 Online Student Edition: What Is Chemistry?
              Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. 

            Chapter 1.3 Online Student Edition: An Experimental Approach to Science
              Curriculum Standards: Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. 

            Chapter 1.3 Online Student Edition: The Scientific Method
              Curriculum Standards: Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. 

            Chapter 1.4 Online Student Edition: Skills Used in Solving Problems
              Curriculum Standards: Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

            Chapter 1 Pre-Test: Introduction to Chemistry
              Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

            Chapter 1 Post-Test: Introduction to Chemistry
              Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

            Chapter 1 Editable Study Workbook
            
               Study WB Chapter 1 Lesson 1
                 Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

               Study WB Chapter 1 Lesson 2
                 Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

               Study WB Chapter 1 Lesson 3
                 Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

               Study WB Chapter 1 Lesson 4
                 Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

               Foundations Study WB Chapter 1
                 Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

            Chapter 1 Editable Labs
            
               Ch. 1 Lab 1: Observing and Inferring
                 Curriculum Standards: Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. 

               Optional Lab Practicals: Laboratory Techniques
                 Curriculum Standards: Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. 

               Ch. 1 Quick Lab Record Sheet
                 Curriculum Standards: Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. 

            Chapter 1 Editable Assessments
            
               Diagnostic Test Part A
                 Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

               Ch. 1 Core TR: Chapter Quiz

               Ch. 1 Core TR: Chapter Test A

               Ch. 1 Core TR: Chapter Test B

               Diagnostic Test Part B
                 Curriculum Standards: Explain why the scope of chemistry is so vast. Identify five traditional areas of study in chemistry. Identify the central themes of chemistry. Identify three general reasons to study chemistry. Identify some outcomes of modern research in chemistry. Describe how Lavoisier transformed chemistry. Identify three steps in the scientific method. Explain the role collaboration and communication play in science. Identify the general approach to solving a problem. Describe the steps for solving numeric problems. Describe the steps for solving nonnumeric problems. 

            Chapter 1 Additional Editable Resources
            
               Ch. 1 Core TR: Section 1 Review

               Ch. 1 Core TR: Section 2 Review

               Ch. 1 Core TR: Section 3 Review

               Ch. 1 Core TR: Section 4 Review

               Ch. 1 Core TR: Practice Problems

               Ch. 1 Core TR: Interpreting Graphics

               Ch. 1 Core TR: Vocabulary Review

            Chapter 1 Image Library
            
               Figure 1.1

               Figure 1.2

               Figure 1.3

               Figure 1.4_part1

               Figure 1.4_part2

               Figure 1.6

               Figure 1.7

               Figure 1.8_part1

               Figure 1.8_part2

               Figure 1.9

               Image 1, p. 14

               Figure 1.10

               Figure 1.11

               Figure 1.12

               Figure 1.14

               Figure 1.16

               Figure 1.17

               Figure 1.19

               Figure 1.20

               Figure 1.21

               Image 1, p. 29

               Image 1, p. 30

               Image 1, p. 31

         Chapter 2: Matter and Change
         
            Chapter-Level Activities
            
               Ch. 2 Concepts in Action: Cooking up Physical and Chemical Changes
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Ch. 2 Directed Virtual Lab: Chemical Reactions
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Ch. 2 Problem Set
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Ch. 2 A New 'Roll' for Old Tires
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Chapter 2 Flash Cards

            2.1 Properties of Matter
            
               2.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. 

               2.1 Kinetic Art: States Of Matter
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. 

            2.2 Mixtures
            
               2.2 Kinetic Art: Distillation
                 Curriculum Standards: Explain how mixtures are classified. Explain how mixtures can be separated. 

               2.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain how mixtures are classified. Explain how mixtures can be separated. 

            2.3 Elements and Compounds
            
               2.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. 

            2.4 Chemical Reactions
            
               2.4 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

            Chapter 2 Online Student Edition
              Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

            Chapter 2.3 Online Student Edition: Distinguishing Elements and Compounds
              Curriculum Standards: Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. 

            Chapter 2.3 Online Student Edition: Distinguishing Substances and Mixtures
              Curriculum Standards: Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. 

            Chapter 2.3 Online Student Edition: Symbols and Formulas
              Curriculum Standards: Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. 

            Chapter 2.3 Online Student Edition: The Periodic Table-A Preview
              Curriculum Standards: Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. 

            Chapter 2.4 Online Student Edition: Conservation of Mass
              Curriculum Standards: Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

            Ch. 2 Concepts in Action: Cooking up Physical and Chemical Changes
              Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

            2.1 Kinetic Art: States Of Matter
              Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. 

            2.2 Kinetic Art: Distillation
              Curriculum Standards: Explain how mixtures are classified. Explain how mixtures can be separated. 

            Ch. 2 Directed Virtual Lab: Chemical Reactions
              Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

            Study WB Chapter 2 Lesson 3
              Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

            2.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. 

            2.2 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain how mixtures are classified. Explain how mixtures can be separated. 

            2.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. 

            2.4 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

            Chapter 2.1 Online Student Edition: States of Matter
              Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. 

            Chapter 2.1 Online Student Edition: Physical Changes
              Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. 

            Chapter 2.4 Online Student Edition: Recognizing Chemical Changes
              Curriculum Standards: Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

            Chapter 2.1 Online Student Edition: Describing Matter
              Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. 

            Chapter 2.2 Online Student Edition: Classifying Mixtures
              Curriculum Standards: Explain how mixtures are classified. Explain how mixtures can be separated. 

            Chapter 2.2 Online Student Edition:  Separating Mixtures
            Chapter 2.2 Online Student Edition: Separating MixturesThe Student eText presents the content necessary for a deep understanding of different types of mixtures.
              Curriculum Standards: Explain how mixtures are classified. Explain how mixtures can be separated. 

            Chapter 2 Pre-Test: Matter and Change
              Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

            Chapter 2 Post-Test: Matter and Change
              Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

            Chapter 2 Editable Study Workbook
            
               Study WB Chapter 2 Lesson 1
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Study WB Chapter 2 Lesson 2
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Study WB Chapter 2 Lesson 3
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Study WB Chapter 2 Lesson 4
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Foundations Study WB Chapter 2
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

            Chapter 2 Editable Labs
            
               Ch. 2 Lab 2: Physical and Chemical Change
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Ch. 2 Lab 3: Observing a Chemical Reaction
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Ch. 2 Lab 26: Distillation
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Ch. 2 Lab 32: Introduction to Chromatography
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Ch. 2 Quick Lab Record Sheet
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Ch. 2 Lab Practicals: Matter and Change
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Ch. 2 Lab Practical: Solutions
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Ch. 2 Quick Lab Record Sheet_1
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

            Chapter 2 Editable Assessments
            
               Ch. 2 Core TR: Chapter Quiz

               Ch. 2 Core TR: Chapter Test A

               Ch. 2 Core TR: Chapter Test B

            Chapter 2 Additional Editable Resources
            
               Ch. 2 Core TR: Section 1 Review

               Ch. 2 Core TR: Section 2 Review

               Ch. 2 Core TR: Section 3 Review

               Ch. 2 Core TR: Section 4 Review

               Ch. 2 Core TR: Practice Problems

               Ch. 2 Core TR: Interpreting Graphics

               Ch. 2 Core TR: Vocabulary Review

            Chapter 2 Image Library
            
               Figure 2.2_part1

               Figure 2.2_part2

               Table 2.1

               Figure 2.3_part1

               Figure 2.3_part2

               Figure 2.3_part3

               Figure 2.3_part4

               Figure 2.4

               Figure 2.5

               Figure 2.6_part1

               Figure 2.6_part2

               Figure 2.6_part3

               Figure 2.7

               Figure 2.8

               Figure 2.9_part1

               Figure 2.9_part2

               Figure 2.9_part3

               Figure 2.10_part1

               Figure 2.10_part2

               Figure 2.10_part3

               Figure 2.10_part4

               Figure 2.10_part5

               Figure 2.10_part6

               Figure 2.11_part1

               Figure 2.11_part2

               Figure 2.11_part3

               Figure 2.11_part4

               Figure 2.11_part5

               Figure 2.12

               Table 2.2

               Figure 2.13

               Figure 2.14_part1

               Figure 2.14_part2

               Figure 2.15_part1

               Figure 2.15_part2

               Figure 2.15_part3

               Figure 2.16_part1

               Figure 2.16_part2

               Image 1, p. 56

               Image 1_part1, p. 57

               Image 1_part2, p. 57

               Image 2, p. 57

               Image 1, p. 58

               Image 1, p. 59

               Image 2, p. 59

         Chapter 3: Scientific Measurement
         
            Chapter-Level Activities
            
               Ch. 3 Math Tutorial A: Converting Units

               Ch. 3 Math Tutorial B: Scientific Notation

               Ch. 3 Concepts in Action: SI Units! Exactly!
                 Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. Describe the relationship between the solubility product constant and the solubility of a compound. 

               Ch. 3 Directed Virtual Lab: The Density of Solids and Liquids
                 Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

               Ch. 3 Problem Set
                 Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

               Ch. 3 Being Precisely Accurate
                 Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

               Chapter 3 Flash Cards

            3.1 Using and Expressing Measurements
            
               3.1 Chemistry Tutorial: Significant Figures in Multiplication and Division
                 Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. 

               3.1 Kinetic Art: Precision in Measurement
                 Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. 

               3.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. 

               3.1 Foundations Chem Tutorial: Sign. Figures in Multip. and Division
                 Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. 

            3.2 Units of Measurement
            
               3.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. 

               3.2 Chemistry Tutorial: Converting Between Temperature Scales
                 Curriculum Standards: Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. 

               3.2 Foundations Chemistry Tutorial: Converting Between Temperature Scales
                 Curriculum Standards: Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. 

            3.3 Solving Conversion Problems
            
               3.3 Chemistry Tutorial: Using Dimensional Analysis
                 Curriculum Standards: Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

               3.3 Chemistry Tutorial: Using Density as a Conversion Factor
                 Curriculum Standards: Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

               3.3 Chemistry Tutorial: Converting Ratios of Units
                 Curriculum Standards: Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

               3.3 Kinetic Art: Conversion Factors
                 Curriculum Standards: Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

               3.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

               3.3 Foundations Chemistry Tutorial: Using Dimensional Analysis
                 Curriculum Standards: Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

               3.3 Foundations Chemistry Tutorial: Using Density as a Conversion Factor
                 Curriculum Standards: Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

               3.3 Foundations Chemistry Tutorial: Converting Ratios of Units
                 Curriculum Standards: Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

            Chapter 3 Online Student Edition
              Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

            Chapter 3.2 Online Student Edition: Using SI Units
              Curriculum Standards: Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. 

            3.3 Chemistry Tutorial: Using Dimensional Analysis
              Curriculum Standards: Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

            3.2 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. 

            3.1 Kinetic Art: Precision in Measurement
              Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. 

            3.3 Kinetic Art: Conversion Factors
              Curriculum Standards: Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

            Ch. 3 Concepts in Action: SI Units! Exactly!
              Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. Describe the relationship between the solubility product constant and the solubility of a compound. 

            Ch. 3 Directed Virtual Lab: The Density of Solids and Liquids
              Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

            3.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

            3.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. 

            Chapter 3.1 Online Student Edition, Scientific Notation
              Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. 

            Chapter 3.2 Online Student Edition: Density
              Curriculum Standards: Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. 

            Chapter 3.3 Online Student Edition: Conversion Factors
              Curriculum Standards: Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

            Chapter 3.1 Online Student Edition, Scientific Notation_1
              Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. 

            Chapter 3 Pre-Test: Scientific Measurement
              Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

            Chapter 3 Post-Test: Scientific Measurement
              Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

            Chapter 3 Editable Study Workbook
            
               Study WB Chapter 3 Lesson 1
                 Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

               Study WB Chapter 3 Lesson 2
                 Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

               Study WB Chapter 3 Lesson 3
                 Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

               Foundations Study WB Chapter 3
                 Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

            Chapter 3 Editable Labs
            
               Ch. 3 Lab 4: Mass, Volume and Density
                 Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

               Ch. 3 Lab Practicals: Scientific Measurement: Basic Measurement and Density
                 Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

               Ch. 3 Quick Lab Record Sheet
                 Curriculum Standards: Write numbers in scientific notation. Evaluate accuracy and precision. Explain why measurements must be reported to the correct number of significant figures. Explain why metric units are easy to use. Identify the temperature units scientists commonly use. Calculate the density of a substance. Explain what happens when a measurement is multiplied by a conversion factor. Describe the kinds of problems that can be easily solved using dimensional analysis. 

            Chapter 3 Editable Assessments
            
               Ch. 3 Core TR: Chapter Quiz

               Ch. 3 Core TR: Chapter Test A

               Ch. 3 Core TR: Chapter Test B

            Chapter 3 Additional Editable Resources
            
               Ch. 3 Core TR: Section 1 Review

               Ch. 3 Core TR: Section 2 Review

               Ch. 3 Core TR: Section 3 Review

               Ch. 3 Core TR: Section 4 Review

               Ch. 3 Core TR: Practice Problems

               Ch. 3 Core TR: Interpreting Graphics

               Ch. 3 Core TR: Vocabulary Review

            Chapter 3 Image Library
            
               Image 1, p. 60

               Figure 3.2

               Figure 3.3

               Figure 3.4

               Image 1, p. 74

               Table 3.1

               Table 3.2

               Table 3.3

               Figure 3.5_part1

               Figure 3.5_part2

               Table 3.4

               Table 3.5

               Figure 3.6

               Figure 3.7

               Image 1, p. 78

               Figure 3.8

               Figure 3.9

               Figure 3.10

               Table 3.6

               Figure 3.11

               Figure 3.12

               Figure 3.13

               Image 1, p. 95

               Image 1, p. 96

               Image 2, p. 96

               Image 1, p. 97

               Image 2, p. 97

               Image 1, p. 98

               Image 1, p. 99

         Chapter 4: Atomic Structure
         
            Chapter-Level Activities
            
               Ch. 4 Math Tutorial: Weighted Averages

               Ch. 4 Concepts in Action: If Atoms Were Pennies, Then Banks Would Be Huge
                 Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

               Ch. 4 Directed Virtual Lab: Rutherford's Experiment
                 Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

               Ch. 4 Problem Set
                 Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

               Ch. 4 What Can Bones Tell Us?
                 Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

               Chapter 4 Flash Cards

            4.1 Defining the Atom
            
               4.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. 

            4.2 Structure of the Nuclear Atom
            
               4.2 Kinetic Art: Cathode Ray
                 Curriculum Standards: Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. 

               4.2 Kinetic Art: Rutherford's Experiment
                 Curriculum Standards: Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. 

               4.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. 

            4.3 Distinguishing Among Atoms
            
               4.3 Chemistry Tutorial: Determining the Composition of an Atom
                 Curriculum Standards: Identify three types of subatomic particles. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

               4.3 Chemistry Tutorial: Calculating Atomic Mass
                 Curriculum Standards: Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

               4.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

               4.3 Foundations Chemistry Tutorial: Determining the Composition of an Atom
                 Curriculum Standards: Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

               4.3 Foundations Chemistry Tutorial: Calculating Atomic Mass
                 Curriculum Standards: Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

            Chapter 4 Online Student Edition
              Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

            Chapter 4.1 Online Student Edition: Early Models of the Atom
              Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. 

            Chapter 4.1 Online Student Edition: Sizing up the Atom
              Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. 

            Chapter 4.3 Online Student Edition: Isotopes
              Curriculum Standards: Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

            4.2 Kinetic Art: Rutherford's Experiment
              Curriculum Standards: Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. 

            Ch. 4 Directed Virtual Lab: Rutherford's Experiment
              Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

            4.3 Chemistry Tutorial: Calculating Atomic Mass
              Curriculum Standards: Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

            Chapter 4.3 Online Student Edition: Atomic Mass
              Curriculum Standards: Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

            4.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. 

            4.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

            Chapter 4 Pre-Test: Atomic Structure
              Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

            Chapter 4 Post-Test: Atomic Structure
              Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

            Chapter 4 Editable Study Workbook
            
               Study WB Chapter 4 Lesson 1
                 Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

               Study WB Chapter 4 Lesson 2
                 Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

               Study WB Chapter 4 Lesson 3
                 Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

               Foundations Study WB Chapter 4
                 Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

            Chapter 4 Editable Labs
            
               Ch. 4 Lab 5: Atomic Structure: Rutherford’s Experiment
                 Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

               Ch. 4 Lab Practicals: Modeling Atomic Structure
                 Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

               Ch. 4 Quick Lab Record Sheet
                 Curriculum Standards: Explain how Democritus and John Dalton described atoms. Identify instruments used to observe individual atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford model. Explain what makes one element different from another. Explain how isotopes of an element differ. Calculate the atomic mass of an element. 

            Chapter 4 Editable Assessments
            
               Ch. 4 Core TR: Chapter Quiz

               Ch. 4 Core TR: Chapter Test A

               Ch. 4 Core TR: Chapter Test B

            Chapter 4 Additional Editable Resources
            
               Ch. 4 Core TR: Section 1 Review

               Ch. 4 Core TR: Section 2 Review

               Ch. 4 Core TR: Section 3 Review

               Ch. 4 Core TR: Practice Problems

               Ch. 4 Core TR: Vocabulary Review

            Chapter 4 Image Library
            
               Image 1, p. 100

               Figure 4.1

               Figure 4.2

               Figure 4.3

               Figure 4.4

               Figure 4.5_part1

               Figure 4.5_part2

               Table 4.1

               Figure 4.6

               Figure 4.7

               Table 4.2

               Figure 4.8

               Figure 4.9

               Table 4.3

               Figure 4.10_part1

               Figure 4.10_part2

               Image 1, p. 122

               Image 1, p. 123

               Image 2, p. 123

               Image 3, p. 123

               Image 1, p. 125

         Chapter 5: Electrons in Atoms
         
            Chapter-Level Activities
            
               Ch. 5 Math Tutorial: Probability

               Ch. 5 Concepts in Action:  A Probably Swim in Lake S Orbital
               Ch. 5 Concepts in Action: A Probably Swim in Lake S OrbitalExplore examples of quantum theory in the real world in this activity.
                 Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

               Ch. 5 Directed Virtual Lab: Flame Tests
                 Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

               Ch. 5 The Chemistry of Fireworks
                 Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

               Ch. 5 Problem Set
                 Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

               Chapter 5 Flash Cards

            5.1 Revising the Atomic Model
            
               5.1 Kinetic Art: Electron Orbitals
                 Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. 

               5.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. 

            5.2 Electron Arrangement in Atoms
            
               5.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: List the three rules for writing the electron configurations of elements. 

               5.2 Chemistry Tutorial: Writing Electron Configurations
                 Curriculum Standards: Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. 

               5.2 Foundations Chemistry Tutorial: Writing Electron Configurations
                 Curriculum Standards: List the three rules for writing the electron configurations of elements. 

            5.3 Atomic Emission Spectra and QM Model
            
               5.3 Chemistry Tutorial: Calculating the Wavelength of Light
                 Curriculum Standards: Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

               5.3 Kinetic Art: The Hydrogen Emission Spectrum
                 Curriculum Standards: Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

               5.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

               5.3 Foundations Chemistry Tutorial: Calculating the Wavelength of Light
                 Curriculum Standards: Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

            Chapter 5 Online Student Edition
              Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

            Chapter 5.3 Online Student Edition: The Quantum Concept and Photons
              Curriculum Standards: Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

            Chapter 5.3 Online Student Edition: Quantum Mechanics
              Curriculum Standards: Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

            Chapter 5.2 Online Student Edition: Electron Configurations
              Curriculum Standards: List the three rules for writing the electron configurations of elements. 

            5.1 Kinetic Art: Electron Orbitals
              Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. 

            5.2 Chemistry Tutorial: Writing Electron Configurations
              Curriculum Standards: Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. 

            Ch. 5 Concepts in Action:  A Probably Swim in Lake S Orbital
            Ch. 5 Concepts in Action: A Probably Swim in Lake S OrbitalExplore examples of quantum theory in the real world in this activity.
              Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

            5.3 Kinetic Art: The Hydrogen Emission Spectrum
              Curriculum Standards: Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

            Study WB Chapter 5 Lesson 3
              Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

            5.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. 

            5.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

            Chapter 5.2 Online Student Edition: Atomic Orbitals
              Curriculum Standards: Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. 

            Chapter 5.2 Online Student Edition: Light and Atomic Emission Spectra
              Curriculum Standards: List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. 

            Chapter 5.1 The Bohr Model
              Curriculum Standards: Describe what Bohr proposed in his model of the atom. 

            Chapter 5 Pre-Test: Electrons in Atoms
              Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

            Chapter 5 Post-Test: Electrons in Atoms
              Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

            Chapter 5 Editable Study Workbook
            
               Study WB Chapter 5 Lesson 1
                 Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

               Study WB Chapter 5 Lesson 2
                 Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

               Study WB Chapter 5 Lesson 3
                 Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

               Foundations Study WB Chapter 5
                 Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

            Chapter 5 Editable Labs
            
               Ch. 5 Lab 6: Flame Tests for Metals
                 Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

               Ch. 5 Lab 7: Energies of Electrons
                 Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

               Ch. 5 Lab 8: Introduction to the Spectrophotometer
                 Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

               Ch. 5 Lab Practicals: Electrons in Atoms: Flame Tests and Spectroscopy
                 Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

               Ch. 5 Quick Lab Record Sheet
                 Curriculum Standards: Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ. List the three rules for writing the electron configurations of elements. Explain what causes atomic emission spectra. Describe how Einstein explained the photoelectric effect. Explain how the frequencies of light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 

            Chapter 5 Editable Assessments
            
               Ch. 5 Core TR: Chapter Quiz

               Ch. 5 Core TR: Chapter Test A

               Ch. 5 Core TR: Chapter Test B

               Benchmark Test 1 Part A (follows Chapters 1-5)

               Benchmark Test 1 Part B (follows Chapters 1-5)

            Chapter 5 Additional Editable Resources
            
               Ch. 5 Core TR: Section 1 Review

               Ch. 5 Core TR: Section 2 Review

               Ch. 5 Core TR: Section 3 Review

               Ch. 5 Core TR: Practice Problems

               Ch. 5 Core TR: Interpreting Graphics

               Ch. 5 Core TR: Vocabulary Review

            Chapter 5 Image Library
            
               Image 1, p. 126

               Figure 5.1

               Figure 5.2_part1

               Figure 5.2_part2

               Figure 5.3_part1

               Figure 5.3_part2

               Figure 5.4

               Table 5.1

               Figure 5.5

               Table 5.2

               Figure 5.6

               Figure 5.7

               Figure 5.8

               Figure 5.9_part1

               Figure 5.9_part2

               Figure 5.10_part1

               Figure 5.10_part2

               Figure 5.11

               Figure 5.12

               Figure 5.13

               Figure 5.14

               Image 1, p. 154

               Image 2_part1, p. 154

               Image 2_part2, p. 154

               Image 1, p. 155

               Image 1, p. 156

               Image 1, p. 157

         Chapter 6: Periodic Table
         
            Chapter-Level Activities
            
               Ch. 6 Math Tutorial: Trend Lines

               Ch. 6 Concepts in Action: The Periodic Table of Musical Instruments
                 Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

               Ch. 6 Directed Virtual Lab: Heat Energy and Metals
                 Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

               Ch. 6 The Name-the-Element Game
                 Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

               Ch. 6 Problem Set
                 Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

               Chapter 6 Flash Cards

            6.1 Organizing the Elements
            
               6.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. 

            6.2 Classifying the Elements
            
               6.2 Chem Tutorial: Using Energy Sublevels to Write Electron Config.
                 Curriculum Standards: List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. 

               6.2 Kinetic Art: Periodic Table Tour
                 Curriculum Standards: Describe how the modern periodic table is organized. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. 

               6.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. 

               6.2 Foundations Chem Tutorial: Energy Sublevels and Elect. Config.
                 Curriculum Standards: List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. 

            6.3 Periodic Trends
            
               6.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

               6.3 Kinetic Art: Trends in the Periodic Table
                 Curriculum Standards: Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

            Chapter 6 Online Student Edition
              Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

            Chapter 6.1 Online Student Edition: Metals, Nonmetals, and Metalloids
              Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. 

            Chapter 6.3 Online Student Edition: Ions
              Curriculum Standards: Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

            Ch. 6 Concepts in Action: The Periodic Table of Musical Instruments
              Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

            6.3 Kinetic Art: Trends in the Periodic Table
              Curriculum Standards: Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

            6.2 Kinetic Art: Periodic Table Tour
              Curriculum Standards: Describe how the modern periodic table is organized. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. 

            Study WB Chapter 6 Lesson 1
              Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

            6.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. 

            Chapter 6.1 Online Student Edition: Mendeleev's Periodic Table
              Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. 

            Chapter 6.2 Online Student Edition: Electron Configurations in Groups
              Curriculum Standards: List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. 

            6.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain how ions form. 

            Chapter 6.2: Reading the Periodic Table
              Curriculum Standards: List the types of information that can be displayed in a periodic table. 

            Chapter 6.3 Trends in Atomic Size
              Curriculum Standards: Describe trends among elements for atomic size. 

            Chapter 6 Pre-Test: Periodic Table
              Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

            Chapter 6 Post-Test: Periodic Table
              Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

            Chapter 6 Editable Study Workbook
            
               Study WB Chapter 6 Lesson 1
                 Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

               Study WB Chapter 6 Lesson 2
                 Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

               Study WB Chapter 6 Lesson 3
                 Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

               Foundations Study WB Chapter 6
                 Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

            Chapter 6 Editable Labs
            
               Ch. 6 Lab 9: Periodic Properties
                 Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

               Ch. 6 Lab Practicals: The Periodic Table: Density and Solubility
                 Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

               Ch. 6 Quick Lab Record Sheet
                 Curriculum Standards: Explain how chemists began to organize the known elements. Describe how Mendeleev organized his periodic table. Describe how the modern periodic table is organized. Identify three broad classes of elements. List the types of information that can be displayed in a periodic table. Classify elements based on electron configuration. Describe trends among elements for atomic size. Explain how ions form. Describe periodic trends for first ionization energy, ionic size, and electronegativity. 

            Chapter 6 Editable Assessments
            
               Ch. 6 Core TR: Chapter Quiz

               Ch. 6 Core TR: Chapter Test A

               Ch. 6 Core TR: Chapter Test B

            Chapter 6 Additional Editable Resources
            
               Ch. 6 Core TR: Section 1 Review

               Ch. 6 Core TR: Section 2 Review

               Ch. 6 Core TR: Section 3 Review

               Ch. 6 Core TR: Practice Problems

               Ch. 6 Core TR: Interpreting Graphics

               Ch. 6 Core TR: Vocabulary Review

            Chapter 6 Image Library
            
               Figure 6.1

               Figure 6.2_part1

               Figure 6.2_part2

               Figure 6.3

               Figure 6.4

               Figure 6.5_part1

               Figure 6.5_part2

               Figure 6.5_part3

               Figure 6.6_part1

               Figure 6.6_part2

               Figure 6.7

               Image 1, p. 166

               Figure 6.8

               Figure 6.9

               Figure 6.11

               Image 1, p. 171

               Image 2, p. 171

               Image 3, p. 171

               Figure 6.12

               Figure 6.13

               Figure 6.14

               Figure 6.15

               Figure 6.16

               Figure 6.17

               Figure 6.18

               Table 6.1

               Figure 6.19

               Figure 6.20

               Figure 6.21

               Figure 6.22

               Figure 6.23

               Table 6.2

               Figure 6.24

               Image 1, p. 187

               Image 2, p. 187

               Image 1, p. 188

               Image 2, p. 188

               Image 3, p. 188

               Image 1, p. 190

               Image 2, p. 190

               Image 1, p. 191

               Image 2, p. 191

         Chapter 7: Ionic and Metallic Bonding
         
            Chapter-Level Activities
            
               Ch. 7 Concepts in Action: Ionic Doubles Partners
                 Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

               Ch. 7 Directed Virtual Lab: The Formation of Ionic Compounds
                 Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

               Ch. 7 Problem Set
                 Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

               Ch. 7 Cave Crystals
                 Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

               Chapter 7 Flash Cards

            7.1 Ions
            
               7.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. 

            7.2 Ionic Bonds and Ionic Compounds
            
               7.2 Chemistry Tutorial: Predicting Formulas of Ionic Compounds
                 Curriculum Standards: Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. 

               7.2 Kinetic Art: Crystal Structures
                 Curriculum Standards: Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. 

               7.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. 

               7.2 Foundations Chemistry Tutorial: Predicting Formulas of Ionic Compounds
                 Curriculum Standards: Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. 

            7.3 Bonding in Metals
            
               7.3 Kinetic Art: Properties of Metals
                 Curriculum Standards: Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

               7.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

            Chapter 7 Online Student Edition
              Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

            Chapter 7.1 Online Student Edition: Valence Electrons
              Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. 

            Chapter 7.1 Online Student Edition: Formation of Cations
              Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. 

            Chapter 7.1 Online Student Edition: Formation of Anions
              Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. 

            Chapter 7.1 Online Student Edition: Alloys
              Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the importance of alloys. 

            7.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. 

            7.2 Chemistry Tutorial: Predicting Formulas of Ionic Compounds
              Curriculum Standards: Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. 

            7.3 Kinetic Art: Properties of Metals
              Curriculum Standards: Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

            Ch. 7 Concepts in Action: Ionic Doubles Partners
              Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

            Ch. 7 Directed Virtual Lab: The Formation of Ionic Compounds
              Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

            Study WB Chapter 7 Lesson 3
              Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

            7.2 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. 

            7.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

            Chapter 7.1 Online Student Edition: Valence Electrons_1
              Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. 

            Chapter 7.2 Online Student Edition: Properties of Ionic Compounds
              Curriculum Standards: Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. 

            Chapter 7 Pre-Test: Ionic and Metallic Bonding
              Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

            Chapter 7 Post-Test: Ionic and Metallic Bonding
              Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

            Chapter 7 Editable Study Workbook
            
               Study WB Chapter 7 Lesson 1
                 Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

               Study WB Chapter 7 Lesson 2
                 Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

               Study WB Chapter 7 Lesson 3
                 Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

               Foundations Study WB Chapter 7
                 Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

            Chapter 7 Editable Labs
            
               Ch. 7 Lab 10: Crystal Structures
                 Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

               Ch. 7 Lab Practicals: Crystal Structure: Ionic and Metallic Bonding
                 Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

               Ch. 7 Quick Lab Record Sheet
                 Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds. Model the valence electrons of metal atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 

            Chapter 7 Editable Assessments
            
               Ch. 7 Core TR: Chapter Quiz

               Ch. 7 Core TR: Chapter Test A

               Ch. 7 Core TR: Chapter Test B

            Chapter 7 Additional Editable Resources
            
               Ch. 7 Core TR: Section 1 Review

               Ch. 7 Core TR: Section 2 Review

               Ch. 7 Core TR: Section 3 Review

               Ch. 7 Core TR: Practice Problems

               Ch. 7 Core TR: Interpreting Graphics

               Ch. 7 Core TR: Vocabulary Review

            Chapter 7 Image Library
            
               Image 1, p. 192

               Image 1, p. 193

               Image 1, p. 194

               Figure 7.1_part1

               Figure 7.1_part2

               Table 7.1

               Figure 7.2

               Figure 7.3

               Figure 7.4

               Table 7.2

               Figure 7.6

               Figure 7.7

               Figure 7.8_part1

               Figure 7.8_part2

               Figure 7.8_part3

               Figure 7.8_part4

               Figure 7.8_part5

               Figure 7.8_part6

               Figure 7.8_part7

               Figure 7.8_part8

               Figure 7.9_part1

               Figure 7.9_part2

               Figure 7.10_part1

               Figure 7.10_part2

               Figure 7.11_part1

               Figure 7.11_part2

               Figure 7.12

               Figure 7.13

               Figure 7.14_part1

               Figure 7.14_part2

               Figure 7.14_part3

               Figure 7.14_part4

               Figure 7.14_part5

               Figure 7.14_part6

               Figure 7.15_part1

               Figure 7.15_part2

               Figure 7.15_part3

               Image 1, p. 215

               Image 1, p. 216

               Image 2, p. 216

               Image 1, p. 217

               Image 1, p. 219

         Chapter 8: Covalent Bonding
         
            Chapter-Level Activities
            
               Ch. 8 Math Tutorial: Tetrahedral Angles

               Ch. 8 Concepts in Action: The Air Up There
                 Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

               Ch. 8 Directed Virtual Lab: Covalent Bonding
                 Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

               Ch. 8 Problem Set
                 Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

               Ch. 8 Painting With Powder?
                 Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

               Chapter 8 Flash Cards

            8.1 Molecular Compounds
            
               8.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. 

            8.2 Nature of Covalent Bonding
            
               8.2 Chemistry Tutorial: Drawing Electron Dot Structures
                 Curriculum Standards: Determine the number of valence electrons in an atom of a representative element. Identify the atoms of elements that tend to lose and tend to gain electrons. Describe how cations form. Explain how anions form. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. 

               8.2 Kinetic Art: Covalent Bonds
                 Curriculum Standards: Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. 

               8.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. 

               8.2 Foundations Chemistry Tutorial: Drawing Electron Dot Structures
                 Curriculum Standards: Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. 

            8.3 Bonding Theories
            
               8.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. 

            8.4 Polar Bonds and Molecules
            
               8.4 Chemistry Tutorial: Identifying Bond Type
                 Curriculum Standards: Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

               8.4 Kinetic Art: Polar Molecules
                 Curriculum Standards: Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

               8.4 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

            Chapter 8 Online Student Edition
              Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

            Chapter 8.2 Online Student Edition: Resonance
              Curriculum Standards: Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. 

            Chapter 8.3 Online Student Edition: Molecular Orbits
              Curriculum Standards: Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. 

            Chapter 8.3 Online Student Edition: VSEPR Theory
              Curriculum Standards: Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. 

            Chapter 8.2 Online Student Edition: Exceptions to the Octet Rule
              Curriculum Standards: Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. 

            Chapter 8.2 Online Student Edition: Bond Dissociation Energies
              Curriculum Standards: Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. 

            8.4 Online Stu. Ed.: Intermolecular Attractions and Molecular Prop.
              Curriculum Standards: Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

            8.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. 

            8.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. 

            8.4 Chemistry Tutorial: Identifying Bond Type
              Curriculum Standards: Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

            8.2 Kinetic Art: Covalent Bonds
              Curriculum Standards: Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. 

            8.4 Kinetic Art: Polar Molecules
              Curriculum Standards: Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

            8.2 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. 

            8.4 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

            Ch. 8 Concepts in Action: The Air Up There
              Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

            Ch. 8 Directed Virtual Lab: Covalent Bonding
              Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

            Study WB Chapter 8 Lesson 1
              Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

            Study WB Chapter 8 Lesson 2
              Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

            Chapter 8 Pre-test: Covalent Bonding
              Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

            Chapter 8 Post-Test: Covalent Bonding
              Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

            Chapter 8 Editable Study Workbook
            
               Study WB Chapter 8 Lesson 1
                 Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

               Study WB Chapter 8 Lesson 2
                 Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

               Study WB Chapter 8 Lesson 3
                 Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

               Study WB Chapter 8 Lesson 4
                 Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

               Foundations Study WB Chapter 8
                 Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

            Chapter 8 Editable Labs
            
               Ch. 8 Lab 11: Molecular Models
                 Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

               Ch. 8 Lab Practicals: Empirical Formula of a Hydrated Compound
                 Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

               Ch. 8 Quick Lab Record Sheet
                 Curriculum Standards: Identify the information a molecular formula provides. Describe the representative units that define molecular compounds and ionic compounds. Explain the result of electron sharing in covalent bonds. Describe how coordinate covalent bonds are different from other covalent bonds. Identify some exceptions to the octet rule. Explain how the strength of a covalent bond is related to its bond dissociation energy. Describe how resonance structures are used. Describe the relationship between atomic and molecular orbitals. Describe how VSEPR theory helps predict the shapes of molecules. Identify the ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the charge distribution in a polar molecule. Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and covalent bonds. Explain why the properties of covalent compounds are so diverse. 

            Chapter 8 Editable Assessments
            
               Ch. 8 Core TR: Chapter Quiz

               Ch. 8 Core TR: Chapter Test A

               Ch. 8 Core TR: Chapter Test B

            Chapter 8 Additional Editable Resources
            
               Ch. 8 Core TR: Section 1 Review

               Ch. 8 Core TR: Section 2 Review

               Ch. 8 Core TR: Section 3 Review

               Ch. 8 Core TR: Section 4 Review

               Ch. 8 Core TR: Practice Problems

               Ch. 8 Core TR: Interpreting Graphics

               Ch. 8 Core TR: Vocabulary Review

            Chapter 8 Image Library
            
               Image 1, p. 220

               Image 1, p. 222

               Figure 8.1_part 1

               Figure 8.1_part2

               Figure 8.1_part3

               Figure 8.1_part4

               Figure 8.2

               Figure 8.3

               Figure 8.4

               Figure 8.5_part1

               Figure 8.5_part2

               Figure 8.5_part3

               Figure 8.5_part4

               Figure 8.7

               Table 8.1

               Figure 8.9

               Table 8.2

               Figure 8.10

               Figure 8.11

               Table 8.3

               Figure 8.12

               Figure 8.13

               Figure 8.14

               Figure 8.15

               Figure 8.16

               Figure 8.17

               Figure 8.18

               Figure 8.19

               Figure 8.20

               Figure 8.21

               Figure 8.22_part1

               Figure 8.22_part2

               Figure 8.23

               Table 8.4

               Figure 8.24

               Figure 8.25

               Figure 8.26

               Figure 8.27

               Figure 8.28

               Figure 8.29

               Table 8.5

               Image 1, p. 257

               Image 1, p. 258

               Image 2, p. 258

               Image 1, p. 261

               Image 2, p. 261

               Image 3, p. 261

         Chapter 9: Chemical Names and Formulas
         
            Chapter-Level Activities
            
               Ch. 9 Math Tutorial: Unit Ratios

               Ch. 9 Concepts in Action: Your Ionic Kitchen (and Bathroom)
                 Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

               Ch. 9 Directed Virtual Lab: Ionic Naming
                 Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

               Ch. 9 Problem Set
                 Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

               Ch. 9 Pass Me the Glauber’s Salt?
                 Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

               Chapter 9 Flash Cards

            9.1 Naming Ions
            
               9.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. 

            9.2 Naming and Writing Form. Ionic Compounds
            
               9.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. 

               9.2 Chemistry Tutorial: Writing Formulas for Binary Ionic Compounds
                 Curriculum Standards: Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. 

               9.2 Foundations Chem Tutorial: Writing Form. for Binary Ionic Compounds
                 Curriculum Standards: Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. 

            9.3 Naming and  Writing Form. Molec Compounds
            
               9.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Apply the rules for naming and writing formulas for binary molecular compounds. 

            9.4 Naming and Writing Form. Acids and Bases
            
               9.4 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Determine the name and formula of an acid. Determine the name and formula of a base. 

            9.5 Laws Governing How Compounds Form
            
               9.5 Chemistry Tutorial: Calculating Mass Ratios
                 Curriculum Standards: Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

               9.5 Kinetic Art: Naming Compounds
                 Curriculum Standards: Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

               9.5 Kinetic Art: The Law of Multiple Proportions
                 Curriculum Standards: Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

               9.5 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

               9.5 Foundations Chemistry Tutorial: Calculating Mass Ratios
                 Curriculum Standards: Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

            Chapter 9 Online Student Edition
              Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

            Chapter 9.3 Online Student Edition: Binary Molecular Compounds
              Curriculum Standards: Apply the rules for naming and writing formulas for binary molecular compounds. 

            Chapter 9.4 Online Student Edition: Names and Formulas of Bases
              Curriculum Standards: Determine the name and formula of an acid. Determine the name and formula of a base. 

            9.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. 

            9.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Apply the rules for naming and writing formulas for binary molecular compounds. 

            9.4 Lesson Overview (PowerPoint file)
              Curriculum Standards: Determine the name and formula of an acid. Determine the name and formula of a base. 

            9.2 Chemistry Tutorial: Writing Formulas for Binary Ionic Compounds
              Curriculum Standards: Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. 

            9.5 Kinetic Art: Naming Compounds
              Curriculum Standards: Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

            Ch. 9 Concepts in Action: Your Ionic Kitchen (and Bathroom)
              Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

            Chapter 9.2 Online Student Edition: Binary Ionic Compounds
              Curriculum Standards: Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. 

            9.5 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

            Chapter 9.4 Online Student Edition: Names and Formulas of Acids
              Curriculum Standards: Determine the name and formula of an acid. Determine the name and formula of a base. 

            9.4 Online Stu. Ed.: The Laws of Definite and Multiple Proportions
              Curriculum Standards: Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. 

            Chapter 9.1: Monatomic Ions
              Curriculum Standards: Explain how to determine the charges of monatomic ions. 

            Chapter 9.5: Practicing Skills: Chemical Names and Formulas
              Curriculum Standards: List the general guidelines that can help you write the name and formula of a chemical compound. 

            Chapter 9 Pre-Test: Chemical Names and Formulas
              Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

            Chapter 9 Post-Test: Chemical Names and Formulas
              Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

            Chapter 9 Editable Study Workbook
            
               Study WB Chapter 9 Lesson 1
                 Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

               Study WB Chapter 9 Lesson 2
                 Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

               Study WB Chapter 9 Lesson 3
                 Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

               Study WB Chapter 9 Lesson 4
                 Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

               Study WB Chapter 9 Lesson 5
                 Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

               Foundations Study WB Chapter 9
                 Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

            Chapter 9 Editable Labs
            
               Ch. 9 Lab Practicals: Nomenclature: Chemical Names and Formulas
                 Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

               Ch. 9 Quick Lab Record Sheet
                 Curriculum Standards: Explain how to determine the charges of monatomic ions. Explain how polyatomic ions differ from and are similar to monatomic ions. Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for  naming and writing formulas for compounds with polyatomic ions. Apply the rules for naming and writing formulas for binary molecular compounds. Determine the name and formula of an acid. Determine the name and formula of a base. Explain how the law of definite proportions is consistent with Dalton‰Ûªs atomic theory. List the general guidelines that can help you write the name and formula of a chemical compound. 

            Chapter 9 Editable Assessments
            
               Ch. 9 Core TR: Chapter Quiz

               Ch. 9 Core TR: Chapter Test A

               Ch. 9 Core TR: Chapter Test B

            Chapter 9 Additional Editable Resources
            
               Ch. 9 Core TR: Section 1 Review

               Ch. 9 Core TR: Section 2 Review

               Ch. 9 Core TR: Section 3 Review

               Ch. 9 Core TR: Section 4 Review

               Ch. 9 Core TR: Section 5 Review

               Ch. 9 Core TR: Practice Problems

               Ch. 9 Core TR: Interpreting Graphics

               Ch. 9 Core TR: Vocabulary Review

            Chapter 9 Image Library
            
               Figure 9.1

               Table 9.1

               Figure 9.2

               Figure 9.3

               Figure 9.4

               Table 9.2

               Figure 9.5

               Table 9.3

               Figure 9.6_part1

               Figure 9.6_part2

               Figure 9.7

               Figure 9.8

               Figure 9.10_part1

               Figure 9.10_part2

               Table 9.4

               Figure 9.12

               Figure 9.13

               Table 9.5

               Table 9.6

               Figure 9.14

               Figure 9.15

               Figure 9.16

               Figure 9.17

               Figure 9.18

               Figure 9.19

               Image 1, p. 298

               Image 1, p. 299

               Image 1, p. 300

               Image 2, p. 300

               Image 1, p. 301

               Image 1, p. 302

               Image 1, p. 303

               Image 2, p. 303

         Chapter 10: Chemical Quantities
         
            Chapter-Level Activities
            
               Ch. 10 Math Tutorial A: Unit Conversion

               Ch. 10 Math Tutorial B: Circle Graphs

               Ch. 10 Concepts in Action: Your Daily Percent Composition
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

               Ch. 10 Directed Virtual Lab: Counting Atoms by Measuring Mass
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

               Ch. 10 Problem Set
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

               Ch. 10 It’s the Mole…So What?
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

               Chapter 10 Flash Cards

            10.1 The Mole: A Measurement of Matter
            
               10.1 Chemistry Tutorial: Converting Number of Atoms to Moles and Vice Versa
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. 

               10.1 Chemistry Tutorial: Finding the Molar Mass of a Compound
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. 

               10.1 Kinetic Art: Molar Mass
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. 

               10.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. 

               10.1 Foundations Chem Tutorial: Converting # of Atoms to Moles
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. 

               10.1 Foundations Chemistry Tutorial: Finding the Molar Mass of a Compound
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. 

            10.2 Mole-Mass and Mole-Vol Relationships
            
               10.2 Chemistry Tutorial: Converting Moles to Mass and Mass to Moles
                 Curriculum Standards: Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. 

               10.2 Kinetic Art: The Mole Map
                 Curriculum Standards: Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. 

               10.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. 

               10.2 Foundations Chem Tutorial: Convert Moles to Mass,  Mass to Moles
               10.2 Foundations Chem Tutorial: Convert Moles to Mass, Mass to MolesExplore conversions between mass and moles in this tutorial.
                 Curriculum Standards: Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. 

            10.3 % Composition and Chemical Formulas
            
               10.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

               10.3 Chem Tutorial: Calculating % Comp. from Mass and from a Formula
                 Curriculum Standards: Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

               10.3 Chemistry Tutorial: Determining the Empirical Formula of a Compound
                 Curriculum Standards: Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

               10.3 Foundations Chem Tutorial: Calculating % Comp. from Mass/Formula
                 Curriculum Standards: Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

               10.3 Foundations Chem Tutorial: Determining the Emp. Form. of Compound
                 Curriculum Standards: Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

            Chapter 10 Online Student Edition
              Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

            Chapter 10.3 Online Student Edition: Percent Composition of a Compound
              Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

            10.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

            10.3 Chem Tutorial: Calculating % Comp. from Mass and from a Formula
              Curriculum Standards: Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

            10.2 Chemistry Tutorial: Converting Moles to Mass and Mass to Moles
              Curriculum Standards: Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. 

            10.3 Chemistry Tutorial: Determining the Empirical Formula of a Compound
              Curriculum Standards: Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

            10.2 Kinetic Art: The Mole Map
              Curriculum Standards: Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. 

            10.1 Chemistry Tutorial: Converting Number of Atoms to Moles and Vice Versa
              Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. 

            10.1 Chemistry Tutorial: Finding the Molar Mass of a Compound
              Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. 

            10.1 Kinetic Art: Molar Mass
              Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. 

            10.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. 

            Chapter 10.1 Binary Ionic Compounds
              Curriculum Standards: Convert among the count, mass, and volume of something. 

            Chapter 10.1 What is a Mole?
              Curriculum Standards: Explain how chemists count the number of atoms, molecules, or formula units in a substance. 

            Chapter 10.2: The Mole-Volume Relationship
              Curriculum Standards: Convert the volume of a gas at STP to the number of moles of the gas. 

            Chapter 10.3: Empirical Formulas
              Curriculum Standards: Distinguish between empirical and molecular formulas. 

            Chapter 10 Pre-Test: Chemical Quantities
              Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

            Chapter 10 Post-Test: Chemical Quantities
              Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

            Chapter 10 Editable Study Workbook
            
               Study WB Chapter 10 Lesson 1
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

               Study WB Chapter 10 Lesson 2
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

               Study WB Chapter 10 Lesson 3
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

               Foundations Study WB Chapter 10
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

            Chapter 10 Editable Labs
            
               Ch. 10 Lab 12: The Masses of Equal Volumes of Gases
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

               Ch. 10 Lab 13: Empirical Formula Determination
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

               Ch. 10 Lab Practicals: Chemical Quantities: Empirical Formulas
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

               Ch. 10 Quick Lab Record Sheet
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

            Chapter 10 Editable Assessments
            
               Ch. 10 Core TR: Chapter Quiz

               Ch. 10 Core TR: Chapter Test A

               Ch. 10 Core TR: Chapter Test B

               Benchmark Test 2 Part A (follows Chapters 6-10)
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

               Benchmark Test 2 Part B (follows Chapters 6-10)
                 Curriculum Standards: Convert among the count, mass, and volume of something. Explain how chemists count the number of atoms, molecules, or formula units in a substance. Determine the molar mass of an element and of a compound. Describe how to convert the mass of a substance to the number of moles of a substance, and moles to mass. Convert the volume of a gas at STP to the number of moles of the gas. Calculate the percent by mass of an element in a compound. Calculate the empirical formula of a compound. Distinguish between empirical and molecular formulas. 

            Chapter 10 Additional Editable Resources
            
               Ch. 10 Core TR: Section 1 Review

               Ch. 10 Core TR: Section 2 Review

               Ch. 10 Core TR: Section 3 Review

               Ch. 10 Core TR: Practice Problems

               Ch. 10 Core TR: Interpreting Graphics

               Ch. 10 Core TR: Vocabulary Review

            Chapter 10 Image Library
            
               Figure 10.1

               Table 10.1

               Figure 10.3

               Table 10.2

               Figure 10.5

               Figure 10.6

               Figure 10.7_part1

               Figure 10.7_part2

               Figure 10.8

               Figure 10.9_part1

               Figure 10.9_part2

               Figure 10.10

               Figure 10.11_part1

               Figure 10.11_part2

               Table 10.3

               Figure 10.12

               Image 1, p. 339

               Image 1, p. 340

               Image 2, p. 340

               Image 1, p. 341

         Chapter 11: Chemical Reactions
         
            Chapter-Level Activities
            
               Ch. 11 Math Tutorial: Balancing Equations

               Ch. 11 Concepts in Action: A Balanced Equation for Fire
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Predict the products of the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

               Ch. 11 Directed Virtual Lab: Identification of Cations in Solution
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Predict the products of the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

               Ch. 11 Problem Set
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Predict the products of the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

               Ch. 11 Nobel Efforts
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Predict the products of the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

               Chapter 11 Flash Cards

            11.1 Describing Chemical Reactions
            
               11.1 Kinetic Art: Balancing Equations
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. 

               11.1 Chemistry Tutorial: Balancing a Chemical Equation
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. 

               11.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. 

               11.1 Foundations Chemistry Tutorial: Balancing a Chemical Equation
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. 

            11.2 Types of Chemical Reactions
            
               11.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe the five general types of reactions. Predict the products of the five general types of reactions. 

               11.2 Chemistry Tutorial: Writing Equations for Double-Replacement Reactions
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Predict the products of the five general types of reactions. 

               11.2 Foundations Chem Tutorial: Writing Eq for Double-Replacement Rxns
                 Curriculum Standards: Describe the five general types of reactions. Predict the products of the five general types of reactions. 

            11.3 Reactions in Aqueous Solution
            
               11.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

               11.3 Chemistry Tutorial: Writing and Balancing Net Ionic Equations
                 Curriculum Standards: Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

               11.3 Foundations Chem Tutorial: Writing and Balancing Net Ionic Eq.
                 Curriculum Standards: Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

            Chapter 11 Online Student Edition
              Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Predict the products of the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

            Chapter 11.2 Online Student Edition: Classifying Reactions
              Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

            Ch. 11 Concepts in Action: A Balanced Equation for Fire
              Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Predict the products of the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

            Ch. 11 Directed Virtual Lab: Identification of Cations in Solution
              Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Predict the products of the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

            11.1 Kinetic Art: Balancing Equations
              Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. 

            11.3 Chemistry Tutorial: Writing and Balancing Net Ionic Equations
              Curriculum Standards: Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

            11.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. 

            Chapter 11.1 Introduction to Chemical Equations
              Curriculum Standards: Describe how to write a skeleton equation. 

            Chapter 11.1: Balancing Chemical Equations
              Curriculum Standards: Describe the five general types of reactions. 

            Chapter 11.3: Net Ionic Equations
              Curriculum Standards: Describe the information found in a net ionic equation. 

            Chapter 11.3: Predicting the Formation of a Precipitate
              Curriculum Standards: Predict the formation of a precipitate in a double-replacement reaction. 

            Chapter 11 Pre-Test: Chemical Reactions
              Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

            Chapter 11 Post-Test: Chemical Reactions
              Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

            Chapter 11 Editable Study Workbook
            
               Study WB Chapter 11 Lesson 1
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

               Study WB Chapter 11 Lesson 2
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

               Study WB Chapter 11 Lesson 3
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

               Foundations Study WB Chapter 11
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

            Chapter 11 Editable Labs
            
               Ch. 11 Lab 14: Types of Chemical Reactions
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

               Ch. 11 Lab 15: Reactivity of Metals
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

               Ch. 11 Lab 16: Identification of Anions and Cations in Solution
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

               Ch. 11 Lab 17: Precipitation Reactions
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

               Ch. 11 Lab 18: Qualitative Analysis
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

               Ch. 11 Lab Practicals: Chemical Reactions
                 Curriculum Standards: Describe how to write a skeleton equation. Describe the steps for writing and balancing a chemical equation. Describe the five general types of reactions. Describe the information found in a net ionic equation. Predict the formation of a precipitate in a double-replacement reaction. 

            Chapter 11 Editable Assessments
            
               Ch. 11 Core TR: Chapter Quiz

               Ch. 11 Core TR: Chapter Test A

               Ch. 11 Core TR: Chapter Test B

            Chapter 11 Additional Editable Resources
            
               Ch. 11 Core TR: Section 1 Review

               Ch. 11 Core TR: Section 2 Review

               Ch. 11 Core TR: Section 3 Review

               Ch. 11 Core TR: Practice Problems

               Ch. 11 Core TR: Interpreting Graphics

               Ch. 11 Core TR: Vocabulary Review

            Chapter 11 Image Library
            
               Image 1, p. 344

               Figure 11.3_part1

               Figure 11.3_part2

               Table 11.1

               Image 1, p. 350

               Image 2, p. 350

               Figure 11.4

               Figure 11.5

               Figure 11.6

               Table 11.2

               Figure 11.7

               Figure 11.8

               Image 1, p. 366_part1

               Image 1, p. 366_part2

               Image 2, p. 366_part1

               Image 2, p. 366_part2

               Image 2, p. 366_part3

               Image 3, p. 366_part1

               Image 3, p. 366_part2

               Image 3, p. 366_part3

               Image 1, p. 367_part1

               Image 1, p. 367_part2

               Image 2, p. 367

               Image 1, p. 369

               Figure 11.9

               Figure 11.10

               Table 11.3

               Figure 11.11

               Image 1, p. 378_part1

               Image 1, p. 378_part2

               Image 1, p. 378_part3

               Image 1, p. 378_part4

               Image 1, p. 379

               Image 1, p. 380

               Image 2, p. 380

               Image 1, p. 381

               Image 2, p. 381

         Chapter 12: Stoichiometry
         
            Chapter-Level Activities
            
               Ch. 12  Math Tutorial A: Percents
               Ch. 12 Math Tutorial A: PercentsExplore percents in this tutorial.

               Ch. 12 Math Tutorial B: Limiting Factors

               Ch. 12 Concepts in Action: Skateboard Stoichiometry
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               Ch. 12 Directed Virtual Lab: Analysis of Baking Soda
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               Ch. 12 Problem Set
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               Ch. 12 Avogadro's Cookies
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               Chapter 12 Flash Cards

            12.1 The Arithmetic of Equations
            
               12.1 Chemistry Tutorial: Using a Balanced Equation as a Recipe
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. 

               12.1 Kinetic Art: Interpreting a Balanced Chemical Equation
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. 

               12.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. 

               12.1 Foundations Chemistry Tutorial: Using a Balanced Equation as a Recipe
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. 

            12.2 Chemical Calculations
            
               12.2 Chemistry Tutorial: Calculating the Mass of a Product
                 Curriculum Standards: Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. 

               12.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. 

               12.2 Foundations Chemistry Tutorial: Calculating the Mass of a Product
                 Curriculum Standards: Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. 

            12.3 Limiting Reagent and Percent Yield
            
               12.3 Chemistry Tutorial: Determining the Limiting Reagent in a Reaction
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               12.3 Chemistry Tutorial: Calculating Yield of a Reaction
                 Curriculum Standards: Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               12.3 Kinetic Art: Limiting Reagents
                 Curriculum Standards: Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               12.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               12.3 Foundations Chem Tutorial: Determine Limiting Reagent in a Rxn
                 Curriculum Standards: Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               12.3 Foundations Chem Tutorial: Calculating Yield of a Reaction
                 Curriculum Standards: Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

            Chapter 12 Online Student Edition
              Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

            Chapter 12.1 Online Student Edition: Chemical Equations
              Curriculum Standards: Describe the quantities you can use to interpret a balanced chemical equation. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. 

            12.2 Chemistry Tutorial: Calculating the Mass of a Product
              Curriculum Standards: Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. 

            Ch. 12 Directed Virtual Lab: Analysis of Baking Soda
              Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

            12.3 Chemistry Tutorial: Determining the Limiting Reagent in a Reaction
              Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

            12.1 Kinetic Art: Interpreting a Balanced Chemical Equation
              Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. 

            12.3 Chemistry Tutorial: Calculating Yield of a Reaction
              Curriculum Standards: Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

            12.3 Kinetic Art: Limiting Reagents
              Curriculum Standards: Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

            Chapter 12.1 Online Student Edition: Using Equations
              Curriculum Standards: Describe how chemists use balanced chemical equations. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. 

            12.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. 

            Chapter 12.3: Percent Yield
              Curriculum Standards: Explain what the percent yield of a reaction measures. 

            Chapter 12 Pre-Test: Stoichiometry
              Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

            Chapter 12 Post-Test: Stoichiometry
              Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

            Chapter 12 Editable Study Workbook
            
               Study WB Chapter 12 Lesson 1
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               Study WB Chapter 12 Lesson 2
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               Study WB Chapter 12 Lesson 3
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               Foundations Study WB Chapter 12
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

            Chapter 12 Editable Labs
            
               Ch. 12  Lab 19: Quantitative Analysis
               Ch. 12 Lab 19: Quantitative AnalysisStudent Lab Manual pages
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               Ch. 12 Lab 20: Balanced Chemical Equations
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               Ch. 12 Lab Practicals: Stoichiometry in a Reaction and Limiting Reagants
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               Optional Lab Practicals: Quantitative Analysis
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

               Ch. 12 Quick Lab Record Sheet
                 Curriculum Standards: Describe how chemists use balanced chemical equations. Describe the quantities you can use to interpret a balanced chemical equation. Identify the questions that are always conserved in chemical reactions. Explain how mole ratios are used in chemical calculations. Explain the general procedure for solving a stoichiometric problem. Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants. Explain what the percent yield of a reaction measures. 

            Chapter 12 Editable Assessments
            
               Ch. 12 Core TR: Chapter Quiz

               Ch. 12 Core TR: Chapter Test A

               Ch. 12 Core TR: Chapter Test B

            Chapter 12 Additional Editable Resources
            
               Ch. 12 Core TR: Section 1 Review

               Ch. 12 Core TR: Section 2 Review

               Ch. 12 Core TR: Section 3 Review

               Ch. 12 Core TR: Practice Problems

               Ch. 12 Core TR: Interpreting Graphics

               Ch. 12 Core TR: Vocabulary Review

            Chapter 12 Image Library
            
               Image 1, p. 384

               Figure 12.2

               Figure 12.3

               Figure 12.4

               Figure 12.5

               Figure 12.7

               Figure 12.9_part1

               Figure 12.9_part2

               Figure 12.9_part3

               Image 1, p. 409

               Image 1, p. 412

               Image 1, p. 413

               Image 2, p. 413

               Image 1, p. 414

               Image 1, p. 417

               Image 2, p. 417

         Chapter 13: States of Matter
         
            Chapter-Level Activities
            
               Ch. 13 Math Tutorial: Reading Graphs

               Ch. 13 Concepts in Action: Brick and Mortar Crystal Palaces
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

               Ch. 13 Directed Virtual Lab: Ionic Compounds and Water
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

               Ch. 13 Allotrope Applications
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

               Ch 13 Problem Set
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

               Chapter 13 Flash Cards

            13.1 Nature of Gases
            
               13.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. 

               13.1 Chemistry Tutorial: Converting Between Units of Pressure
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. 

               13.1 Foundations Chemistry Tutorial: Converting Between Units of Pressure
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. 

            13.2 Nature of Liquids
            
               13.2 Kinetic Art: Evaporation
                 Curriculum Standards: Interpret gas pressure in terms of kinetic theory. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. 

               13.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. 

            13.3 Nature of Solids
            
               13.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. 

            13.4 Changes of States
            
               13.4 Kinetic Art: Change In State
                 Curriculum Standards: Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

               13.4 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

            Chapter 13 Online Student Edition
              Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

            Chapter 13.2 Online Student Edition: Evaporation
              Curriculum Standards: Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. 

            Ch. 13 Concepts in Action: Brick and Mortar Crystal Palaces
              Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

            13.4 Kinetic Art: Change In State
              Curriculum Standards: Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

            Chapter 13.2 Online Student Edition: Boiling Point
              Curriculum Standards: Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. 

            Study WB Chapter 13 Lesson 1
              Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

            Study WB Chapter 13 Lesson 2
              Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

            13.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. 

            13.2 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. 

            13.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. 

            13.4 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

            Chapter 13.3 Online Student Edition: A Model for Solids
              Curriculum Standards: Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. 

            Chapter 13.4 Online Student Edition: Sublimation
              Curriculum Standards: Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

            Chapter 13.4 Online Student Edition: Phase Diagrams
              Curriculum Standards: Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

            Chapter 13.1 Online Student Edition: Kinetic Energy and Temperature
              Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. 

            Chapter 13.2 Online Student Edition: Vapor Pressure
              Curriculum Standards: Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. 

            Chapter 13.2 Online Student Edition: A Model for Liquids
              Curriculum Standards: Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. 

            Chapter 13.1 Online Student Edition: Kinetic Theory and a Model for Gases
              Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. 

            Chapter 13.1 Online Student Edition: Kinetic Theory and a Model for Gases_1
              Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. 

            Chapter 13 Pre-Test: States of Matter
              Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

            Chapter 13 Post-Test: States of Matter
              Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

            Chapter 13 Editable Study Workbook
            
               Study WB Chapter 13 Lesson 1
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

               Study WB Chapter 13 Lesson 2
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

               Study WB Chapter 13 Lesson 3
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

               Study WB Chapter 13 Lesson 4
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

               Foundations Study WB Chapter 13
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

            Chapter 13 Editable Labs
            
               Ch. 13 Lab 21: Allotropic Forms of Sulfur
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

               Ch. 13 Lab 22: Changes of Physical State
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

               Ch. 13 Lab Practicals: The States of Matter
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

               Ch. 13 Quick Lab Record Sheet
                 Curriculum Standards: Describe the three assumptions of the kinetic theory as it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between the temperature in kelvins and the average kinetic energy of particles. Identify the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor. Identify the conditions under which boiling occurs. Describe how the structure and properties of solids are related. Identify the factors that determine the shape of a crystal. Identify the conditions necessary for sublimation. Determine how the conditions at which phases are in equilibrium are represented on a phase diagram. 

            Chapter 13 Editable Assessments
            
               Ch. 13 Core TR: Chapter Quiz

               Ch. 13 Core TR: Chapter Test A

               Ch. 13 Core TR: Chapter Test B

            Chapter 13 Additional Editable Resources
            
               Ch. 13 Core TR: Section 1 Review

               Ch. 13 Core TR: Section 2 Review

               Ch. 13 Core TR: Section 3 Review

               Ch. 13 Core TR: Section 4 Review

               Ch. 13 Core TR: Practice Problems

               Ch. 13 Core TR: Interpreting Graphics

               Ch. 13 Core TR: Vocabulary Review

            Chapter 13 Image Library
            
               Image 1, p. 418

               Figure 13.1_part1

               Figure 13.1_part2

               Figure 13.2

               Figure 13.3

               Figure 13.4

               Figure 13.5_part1

               Figure 13.5_part2

               Figure 13.6_part1

               Figure 13.6_part2

               Figure 13.6_part3

               Table 13.1

               Figure 13.7_part1

               Figure 13.7_part2

               Figure 13.7_part3

               Figure 13.8_part1

               Figure 13.8_part2

               Figure 13.8_part3

               Figure 13.9

               Table 13.2

               Image 1, p. 431

               Figure 13.11

               Figure 13.12_part1

               Figure 13.12_part2

               Figure 13.12_part3

               Figure 13.12_part4

               Figure 13.12_part5

               Figure 13.12_part6

               Figure 13.12_part7

               Figure 13.12_part8

               Figure 13.13

               Figure 13.14_part1

               Figure 13.14_part2

               Figure 13.14_part3

               Figure 13.15_part1

               Figure 13.15_part2

               Figure 13.17

               Figure 13.18

               Image 1, p. 443

               Image 1, p. 444

               Image 2, p. 444

               Image 1, p. 445

               Image 1, p. 447

               Image 2, p. 447

         Chapter 14: The Behavior of Gases
         
            Chapter-Level Activities
            
               Ch. 14 Math Tutorial A: Multistep Equations

               Ch. 14 Math Tutorial A: Multistep Equations

               Ch. 14 Directed Virtual Lab: Comparing Real and Ideal Gases
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               Ch. 14 Concepts in Action: Triathlons are a Gas!
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               Ch. 14 Problem Set
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               Ch. 14 A Fresh Look at Fresh Fruit
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               Chapter 14 Flash Cards

            14.1 Properties of Gases
            
               14.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. 

            14.2 The Gas Laws
            
               14.2 Chemistry Tutorial: Using the Gas Laws
                 Curriculum Standards: Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. 

               14.2 Chemistry Tutorial: Using the Combined Gas Law
                 Curriculum Standards: Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. 

               14.2 Kinetic Art: Charles's Law
                 Curriculum Standards: Describe the relationships among pressure, volume, and temperature of a gas. 

               14.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe the relationships among pressure, volume, and temperature of a gas. 

               14.2 Foundations Chemistry Tutorial: Using the Gas Laws
                 Curriculum Standards: Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. 

               14.2 Foundations Chemistry Tutorial: Using the Combined Gas Law
                 Curriculum Standards: Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. 

            14.3 Ideal Gases
            
               14.3 Chemistry Tutorial: Using the Ideal Gas Law
                 Curriculum Standards: Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. 

               14.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. 

               14.3 Foundations Chemistry Tutorial: Using the Ideal Gas Law
                 Curriculum Standards: Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. 

            14.4 Gases: Mixtures and Movements
            
               14.4 Chemistry Tutorial: Using Dalton's Law of Partial Pressures
                 Curriculum Standards: Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               14.4 Kinetic Art: Partial Pressure of Gases
                 Curriculum Standards: Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               14.4 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               14.4 Foundations Chemistry Tutorial: Dalton's Law of Partial Pressures
                 Curriculum Standards: Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

            Chapter 14 Online Student Edition
              Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

            Chapter 14.4 Online Student Edition: Graham's Law
              Curriculum Standards: Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

            Chapter 14.1 Online Student Edition: Compressibility
              Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. 

            Chapter 14.1 Online Student Edition: Compressibility_1
              Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. 

            Ch. 14 Directed Virtual Lab: Comparing Real and Ideal Gases
              Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

            14.3 Chemistry Tutorial: Using the Ideal Gas Law
              Curriculum Standards: Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. 

            Ch. 14 Concepts in Action: Triathlons are a Gas!
              Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

            14.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. 

            14.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. 

            14.4 Chemistry Tutorial: Using Dalton's Law of Partial Pressures
              Curriculum Standards: Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

            14.4 Kinetic Art: Partial Pressure of Gases
              Curriculum Standards: Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

            14.2 Chemistry Tutorial: Using the Gas Laws
              Curriculum Standards: Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. 

            14.4 Lesson Overview (PowerPoint file)
              Curriculum Standards: Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

            14.2 Chemistry Tutorial: Using the Combined Gas Law
              Curriculum Standards: Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. 

            Chapter 14.3: Ideal Gases and Real Gases
              Curriculum Standards: Determine the conditions under which real gases are most likely to differ from ideal gases. 

            Chapter 14 Pre-Test: The Behavior of Gases
              Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

            Chapter 14 Post-Test: The Behavior of Gases
              Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

            Chapter 14 Editable Study Workbook
            
               Study WB Chapter 14 Lesson 1
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               Study WB Chapter 14 Lesson 2
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               Study WB Chapter 14 Lesson 3
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               Study WB Chapter 14 Lesson 4
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               Foundations Study WB Chapter 14
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

            Chapter 14 Editable Labs
            
               Ch. 14 Lab 23: Pressure-Volume Relationships of Gases
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               Ch. 14 Lab 24: Temperature-Volume Relationships of Gases
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               Ch. 14 Lab 25: Diffusion of Gases
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               Ch. 14 Lab Practicals: The Behavior of Gases: Boyle's Law and Charles's Law
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               Ch. 14 Quick Lab Record Sheet
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

            Chapter 14 Editable Assessments
            
               Ch. 14 Core TR: Chapter Quiz

               Ch. 14 Core TR: Ch. Test A

               Ch. 14 Core TR: Ch. Test B

            Chapter 14 Additional Editable Resources
            
               Ch. 14 Core TR: Section 1 Review

               Ch. 14 Core TR: Section 2 Review

               Ch. 14 Core TR: Section 3 Review

               Ch. 14 Core TR: Section 4 Review

               Ch. 14 Core TR: Practice Problems

               Ch. 14 Core TR: Interpreting Graphics

               Ch. 14 Core TR: Vocabulary Review

            Chapter 14 Image Library
            
               Image 1, p. 448

               Figure 14.1

               Figure 14.2

               Figure 14.4

               Figure 14.5

               Figure 14.6

               Figure 14.7

               Figure 14.8

               Figure 14.9_part1

               Figure 14.9_part2

               Figure 14.9_part3

               Figure 14.10

               Figure 14.11

               Figure 14.13

               Figure 14.14

               Figure 14.15

               Table 14.1

               Figure 14.16

               Figure 14.17_part1

               Figure 14.17_part2

               Figure 14.17_part3

               Figure 14.18

               Image 1, p. 480

               Image 1, p. 481

               Image 1, p. 482

               Image 2, p. 482

               Image 3, p. 482

               Image 1, p. 483

               Image 1, p. 484

               Image 2, p. 484

               Image 1, p. 485

               Image 2, p. 485

         Chapter 15: Water and Aqueous Systems
         
            Chapter-Level Activities
            
               Ch. 15 Concepts in Action: An Afternoon at Home, Emulsified
                 Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

               Ch. 15 Directed Virtual Lab: The Conductivity of Electrolyte Solutions
                 Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

               Ch. 15 S’mores the Merrier
                 Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

               Ch. 15 Problem Set
                 Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

               Chapter 15 Flash Cards

            15.1 Water and Its Properties
            
               15.1 Kinetic Art: Hydrogen Bonding
                 Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. 

               15.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. 

            15.2 Homogeneous Aqueous Solutions
            
               15.2 Chemistry Tutorial: Finding the Percent by Mass of Water in a Hydrate
                 Curriculum Standards: Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. 

               15.2 Kinetic Art: Solvation of Ionic Compounds
                 Curriculum Standards: Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. 

               15.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. 

               15.2 Foundations Chem Tutorial: Find  % by Mass of Water in a Hydrate
               15.2 Foundations Chem Tutorial: Find % by Mass of Water in a HydrateExplore the percent of water in a hydrate in this tutorial.
                 Curriculum Standards: Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. 

            15.3 Heterogeneous Aqueous Systems
            
               15.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

            Chapter 15 Online Student Edition
              Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

            Chapter 15.2 Online Student Edition: Hydrates
              Curriculum Standards: Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. 

            Chapter 15.3 Online Student Edition: Colloids
              Curriculum Standards: Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

            Ch. 15 Directed Virtual Lab: The Conductivity of Electrolyte Solutions
              Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

            15.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

            15.1 Kinetic Art: Hydrogen Bonding
              Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. 

            15.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. 

            15.2 Kinetic Art: Solvation of Ionic Compounds
              Curriculum Standards: Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. 

            15.2 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. 

            Study WB Chapter 15 Lesson 2
              Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

            Chapter 15.1: Water in the Liquid State
              Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. 

            Chapter 15.3: Solutions
              Curriculum Standards: Distinguish between a suspension and a solution. 

            Chapter 15 Pre-Test: Water and Aqueous Systems
              Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

            Chapter 15 Post-Test: Water and Aqueous Systems
              Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

            Chapter 15 Editable Study Workbook
            
               Study WB Chapter 15 Lesson 1
                 Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

               Study WB Chapter 15 Lesson 2
                 Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

               Study WB Chapter 15 Lesson 3
                 Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

               Foundations Study WB Chapter 15
                 Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

            Chapter 15 Editable Labs
            
               Ch. 15 Lab 27: The Solvent Properties of Water
                 Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

               Ch. 15 Lab 28: Water of Hydration
                 Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

               Ch. 15 Lab 29: Electrolytes and Nonelectrolytes
                 Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

               Ch. 15 Lab Practicals: Water and Aqueous Systems
                 Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

               Ch. 15 Quick Lab Record Sheet
                 Curriculum Standards: Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water. Describe the structure of ice. Identify the types of substances that dissolve most readily in water. Explain why all ionic compounds are electrolytes. Explain why hydrates easily lose and regain water. Distinguish between a suspension and a solution. Identify how to distinguish a colloid from a suspension and a solution. 

            Chapter 15 Editable Assessments
            
               Ch. 15 Core TR: Chapter Quiz

               Ch. 15 Core TR: Chapter Test A

               Ch. 15 Core TR: Chapter Test B

            Chapter 15 Additional Editable Resources
            
               Ch. 15 Core TR: Section 1 Review

               Ch. 15 Core TR: Section 2 Review

               Ch. 15 Core TR: Section 3 Review

               Ch. 15 Core TR: Practice Problems

               Ch. 15 Core TR: Vocabulary Review

            Chapter 15 Image Library
            
               Figure 15.2

               Figure 15.3

               Figure 15.4_part1

               Figure 15.4_part2

               Table 15.1

               Figure 15.6_part1

               Figure 15.6_part2

               Figure 15.7

               Image 1, p. 494

               Figure 15.8

               Figure 15.10_part1

               Figure 15.10_part2

               Figure 15.10_part3

               Figure 15.12_part1

               Figure 15.12_part2

               Figure 15.13

               Table 15.2

               Figure 15.14

               Figure 15.15

               Figure 15.16_part1

               Figure 15.16_part2

               Table 15.3

               Figure 15.17_part1

               Figure 15.17_part2

               Table 15.4

               Image 1, p. 511

               Image 1, p. 512

               Image 1, p. 513

               Image 1, p. 514

               Image 1, p. 515

               Image 2, p. 515

         Chapter 16: Solutions
         
            Chapter-Level Activities
            
               Ch. 16 Math Tutorial A: Converting Units

               Ch. 16 Math Tutorial B: Solving Equations

               Ch. 16 Concepts in Action: Sorbet Solutions
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               Ch. 16 Directed Virtual Lab: Solutions
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               Ch. 16 Problem Set
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               Ch. 16 The Truth About Solutions
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               Chapter 16 Flash Cards

            16.1 Properties of Solutions
            
               16.1 Chemistry Tutorial: Using Henry's Law
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. 

               16.1 Kinetic Art: Dynamic Equilibrium of Saturated Solutions
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. 

               16.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. 

               16.1 Foundations Chemistry Tutorial: Using Henrys Law
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. 

            16.2 Concentrations of Solutions
            
               16.2 Chemistry Tutorial: Calculating Molarity
                 Curriculum Standards: Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. 

               16.2 Chemistry Tutorial: Preparing a Dilute Solution
                 Curriculum Standards: Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. 

               16.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. 

               16.2 Foundations Chemistry Tutorial: Calculating Molarity
                 Curriculum Standards: Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. 

               16.2 Foundations Chemistry Tutorial: Preparing a Dilute Solution
                 Curriculum Standards: Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. 

            16.3 Colligative Properties
            
               16.3 Kinetic Art: Vapor Pressure
                 Curriculum Standards: Explain how colligative properties can be explained on a particle basis. 

               16.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain how colligative properties can be explained on a particle basis. 

            16.4 Calculations Involving Colligative Properties
            
               16.4 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               16.4 Chemistry Tutorial: Calculating Freezing-Point Depression
                 Curriculum Standards: Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               16.4 Foundations Chem Tutorial: Calc. the Freezing-Point Depr. of Sol.
                 Curriculum Standards: Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

            Chapter 16 Online Student Edition
              Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

            Chapter 16.1 Online Student Edition: Properties of Solutions
              Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. 

            Chapter 16.1 Online Student Edition: Solubility
              Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. 

            Chapter 16.2 Online Student Edition: Molarity
              Curriculum Standards: Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. 

            Chapter 16.2 Online Student Edition:  Molarity
            Chapter 16.2 Online Student Edition: MolarityThe Student eText presents the content necessary for a deep understanding of solutions.
              Curriculum Standards: Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. 

            Chapter 16.4 Online Student Edition: Molality and Mole Fraction
              Curriculum Standards: Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

            16.4 Online Stu. Ed.: Freezing Point Depress. and Boiling-Point Elev.
              Curriculum Standards: Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

            Chapter 16.1 Online Student Edition: Solubility
              Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. 

            16.4 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

            16.2 Chemistry Tutorial: Calculating Molarity
              Curriculum Standards: Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. 

            16.4 Chemistry Tutorial: Calculating Freezing-Point Depression
              Curriculum Standards: Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

            Ch. 16 Directed Virtual Lab: Solutions
              Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

            16.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain how colligative properties can be explained on a particle basis. 

            16.1 Kinetic Art: Dynamic Equilibrium of Saturated Solutions
              Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. 

            16.2 Chemistry Tutorial: Preparing a Dilute Solution
              Curriculum Standards: Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. 

            16.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. 

            16.2 Lesson Overview (PowerPoint file)
              Curriculum Standards: Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. 

            Chapter 16 Pre-Test: Solutions
              Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

            Chapter 16 Post-Test: Solutions
              Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

            Chapter 16 Editable Study Workbook
            
               Study WB Chapter 16 Lesson 1
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               Study WB Chapter 16 Lesson 2
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               Study WB Chapter 16 Lesson 3
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               Study WB Chapter 16 Lesson 4
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               Foundations Study WB Chapter 16
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

            Chapter 16 Editable Labs
            
               Ch. 16 Lab 30: Factors Affecting Solution Formation
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               Ch. 16 Lab 31: Supersaturation
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               Ch. 16 Lab 33: Freezing Point
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               Ch. 16 Quick Lab Record Sheet
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               Chs. 2 and 16 Lab Practicals: Chromatography
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

            Chapter 16 Editable Assessments
            
               Ch. 16 Core TR: Chapter Quiz

               Ch. 16 Core TR: Chapter Test A

               Ch. 16 Core TR: Chapter Test B

               Benchmark Test 3 Part A (follows Chapters 11-16)
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               Benchmark Test 3 Part B (follows Chapters 11-16)
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

            Chapter 16 Image Library
            
               Figure 16.1_part1

               Figure 16.1_part2

               Figure 16.1_part3

               Figure 16.2

               Figure 16.3

               Figure 16.4

               Figure 16.5

               Table 16.1

               Figure 16.6_part1

               Figure 16.6_part2

               Figure 16.6_part3

               Figure 16.6_part4

               Figure 16.7

               Figure 16.8_part1

               Figure 16.8_part2

               Figure 16.8_part3

               Figure 16.9

               Figure 16.10_part1

               Figure 16.10_part2

               Figure 16.10_part3

               Figure 16.11

               Figure 16.12_part1

               Figure 16.12_part2

               Figure 16.12_part3

               Figure 16.12_part4

               Figure 16.13_part1

               Figure 16.13_part2

               Figure 16.15

               Figure 16.16

               Table 16.2

               Image 1, p. 549

               Image 2, p. 549

               Image 1, p. 550

               Image 2, p. 550

               Image 1, p. 551

               Image 1, p. 552

               Image 1, p. 553

               Image 2, p. 553

         Chapter 17: Thermochemistry
         
            Chapter-Level Activities
            
               Ch. 17 Math Tutorial:  Solving Multistep Literal Equations
               Ch. 17 Math Tutorial: Solving Multistep Literal EquationsExplore multistep literal equations in this tutorial.
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

               Ch. 17 Concepts in Action: A Tremendous Capacity for Heat
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

               Ch. 17 Directed Virtual Lab: Heat of Combustion

               Ch. 17 Problem Set
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

               Ch. 17 Turning Up the Heat
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

               Chapter 17 Flash Cards

            17.1 The Flow of Energy
            
               17.1 Chemistry Tutorial: Calculating the Specific Heat of a Substance
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. 

               17.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. 

               17.1 Foundations Chem Tutorial: Calc. the Specific Heat of a Substance
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. 

            17.2 Measuring and Expressing Enthalpy Changes
            
               17.2 Chemistry Tutorial: Enthalpy Change in a Calorimetry Experiment
                 Curriculum Standards: Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. 

               17.2 Kinetic Art: Bomb Calorimeter
                 Curriculum Standards: Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. 

               17.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. 

               17.2 Foundations Chemistry Tutorial: Enthalpy Change in a Calorimetry Experiment
                 Curriculum Standards: Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. 

            17.3 Heat in Changes of State
            
               17.3 Chemistry Tutorial: Using the Heat of Fusion and Vaporization in Phase-Change Calculations
                 Curriculum Standards: Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. 

               17.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. 

               17.3Foundations Chemistry Tutorial: Using the Heat of Fusion and Vaporization
                 Curriculum Standards: Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. 

            17.4 Calculating Heats of Reaction
            
               17.4 Chemistry Tutorial: Calculating the Standard Heat of Reaction
                 Curriculum Standards: Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

               17.4 Kinetic Art: Hess's Law
                 Curriculum Standards: Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

               17.4 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

               17.4 Foundations Chem Tutorial: Calc. the Standard Heat of Reaction
                 Curriculum Standards: Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

            Chapter 17 Online Student Edition
              Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

            Chapter 17.1 Online Student Edition: Heat Capacity and Specific Heat
              Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. 

            Chapter 17.3 Online Student Edition: Heats of Vaporization and Condensation
              Curriculum Standards: Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. 

            17.2 Chemistry Tutorial: Enthalpy Change in a Calorimetry Experiment
              Curriculum Standards: Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. 

            17.4 Chemistry Tutorial: Calculating the Standard Heat of Reaction
              Curriculum Standards: Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

            17.2 Kinetic Art: Bomb Calorimeter
              Curriculum Standards: Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. 

            17.4 Kinetic Art: Hess's Law
              Curriculum Standards: Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

            Ch. 17 Concepts in Action: A Tremendous Capacity for Heat
              Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

            17.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. 

            17.2 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. 

            17.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. 

            Chapter 17.1 Online Student Edition: The Flow of Energy
              Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. 

            Chapter 17.3 Online Student Edition: Thermochemical Equations
              Curriculum Standards: Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. 

            Chapter 17.4 Online Student Edition: Heats of Solution
              Curriculum Standards: Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

            Chapter 17.3 Online Student Edition: Heats of Fusion and Solidification
              Curriculum Standards: Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. 

            Chapter 17.1 Online Student Edition: The Flow of Energy_1
              Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. 

            Chapter 17 Pre-Test: Thermochemistry
              Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

            Chapter 17 Post-Test: Thermochemistry
              Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

            Chapter 17 Editable Study Workbook
            
               Study WB Chapter 17 Lesson 1
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

               Study WB Chapter 17 Lesson 2
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

               Study WB Chapter 17 Lesson 3
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

               Study WB Chapter 17 Lesson 4
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

               Foundations Study WB Chapter 17
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

            Chapter 17 Editable Labs
            
               Ch. 17 Lab 34: The Specific Heat of a Metal
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

               Ch. 17 Lab 35: Heats of Reaction
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

               Ch. 17 Lab Practicals: Thermochemistry: Specific Heat
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

               Ch. 17 Quick Lab Record Sheet
                 Curriculum Standards: Explain the ways in which energy changes can occur. Explain how the energy of the universe before a chemical or physical process is related to the energy of the universe after a chemical or physical process. Identify two factors on which the heat capacity of an object depends. Describe how you measure the change in enthalpy of a reaction. Describe how you express the enthalpy change for a reaction in a chemical equation. Compare the quantity of heat absorbed by a melting solid to the quantity of heat released when the liquid solidifies. Compare the quantity of heat absorbed by a vaporizing liquid to the quantity of heat released when the vapor condenses. Describe thermochemical changes that occur when a solution forms. Identify two ways that you can determine the heat of reaction when it cannot be directly measured. 

            Chapter 17 Editable Assessments
            
               Ch. 17 Core TR: Chapter Quiz

               Ch. 17 Core TR: Chapter Test A

               Ch. 17 Core TR: Chapter Test B

            Chapter 17 Additional Editable Resources
            
               Ch. 17 Core TR: Section 1 Review

               Ch. 17 Core TR: Section 2 Review

               Ch. 17 Core TR: Section 3 Review

               Ch. 17 Core TR: Section 4 Review

               Ch. 17 Core TR: Practice Problems

               Ch. 17 Core TR: Interpreting Graphics

               Ch. 17 Core TR: Vocabulary Review

            Chapter 17 Image Library
            
               Image 1, p. 556

               Figure 17.2_part1

               Figure 17.2_part2

               Table 17.1

               Figure 17.4

               Figure 17.6

               Figure 17.7

               Figure 17.8_part1

               Figure 17.8_part2

               Figure 17.9_part1

               Figure 17.9_part2

               Figure 17.10

               Table 17.2

               Table 17.3

               Figure 17.11

               Figure 17.12

               Figure 17.14

               Figure 17.15

               Table 17.4

               Figure 17.16

               Figure 17.17

               Image 1, p. 587

               Image 1, p. 589

               Image 591.1_part1

               Image 591.1_part2

         Chapter 18: Reaction Rates and Equilibrium
         
            Chapter-Level Activities
            
               Ch. 18 Math Tutorial: Slope of a Curve

               Ch. 18 Concepts in Action: Entropy - Gone to the Dogs
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

               Ch. 18 Directed Virtual Lab: Enthalpy and Entropy
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

               Ch. 18 Problem Set
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

               Ch. 18 The Chemistry of Diabetes
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

               Chapter 18 Flash Cards

            18.1 Rates of Reaction
            
               18.1 Kinetic Art: Collision Theory
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. 

               18.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. 

            18.2 The Progress of Chemical
            
               18.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. 

            18.3 Reversible Reactions and Equilibrium
            
               18.3 Chemistry Tutorial: Expressing and Calculating Keq
                 Curriculum Standards: Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. 

               18.3 Kinetic Art: Reversible Reactions
                 Curriculum Standards: Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. 

               18.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. 

               18.3 Foundations Chemistry Tutorial: Expressing and Calculating Keq
                 Curriculum Standards: Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. 

            18.4 Solubility Equilibrium
            
               18.4 Chem Tutorial: Finding Eq. Ion Conc. in Sat. Solution
                 Curriculum Standards: Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. 

               18.4 Chem Tutorial: Find Eq Ion Conc. in the Presence of a Common Ion
                 Curriculum Standards: Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. 

               18.4 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. 

               18.4 Foundations Chem Tutorial: Finding Eq. Ion Conc. in Sat. Solution
                 Curriculum Standards: Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. 

               18.4 Foundations Chemistry Tutorial: Finding Equilibrium Ion Concentrations
                 Curriculum Standards: Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. 

            18.5 Entropy and Free Energy
            
               18.5 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

            Chapter 18 Online Student Edition
              Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

            Chapter 18.1 Online Student Edition: Describing Reaction Rates
              Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. 

            Chapter 18.2 Online Student Edition: Rate Laws
              Curriculum Standards: Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. 

            Ch. 18 Concepts in Action: Entropy - Gone to the Dogs
              Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

            18.3 Chemistry Tutorial: Expressing and Calculating Keq
              Curriculum Standards: Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. 

            Ch. 18 Directed Virtual Lab: Enthalpy and Entropy
              Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

            18.3 Kinetic Art: Reversible Reactions
              Curriculum Standards: Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. 

            18.2 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. 

            18.4 Chem Tutorial: Finding Eq. Ion Conc. in Sat. Solution
              Curriculum Standards: Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. 

            18.4 Chem Tutorial: Find Eq Ion Conc. in the Presence of a Common Ion
              Curriculum Standards: Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. 

            Study WB Chapter 18 Lesson 1
              Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

            Study WB Chapter 18 Lesson 5
              Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

            18.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. 

            18.5 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

            Chapter 18.5 Online Student Edition: Entropy
              Curriculum Standards: Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

            Chapter 18.5 Online Student Edition: Enthalpy and Entropy
              Curriculum Standards: Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

            Chapter 18.3 Online Student Edition: Reversible Reactions
              Curriculum Standards: Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. 

            Chapter 18.4 Online Student Edition: Solubility Product Constant
              Curriculum Standards: Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. 

            Chapter 18.4 Online Student Edition: The Common Ion Effect
              Curriculum Standards: Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. 

            Chapter 18.5 Online Student Edition: Free Energy Change
              Curriculum Standards: Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

            18.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. 

            Chapter 18.2: The Progress of Chemical Reactions
              Curriculum Standards: Describe how most reactions progress from start to finish. 

            Chapter 18.3: Factors Affecting Equilibrium: Le Chatelier's Principle
              Curriculum Standards: Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. 

            Chapter 18 Pre-Test: Reaction Rates and Equilibrium
              Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

            Chapter 18 Post-Test: Reaction Rates and Equilibrium
              Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

            Chapter 18 Editable Study Workbook
            
               Study WB Chapter 18 Lesson 1
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

               Study WB Chapter 18 Lesson 2
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

               Study WB Chapter 18 Lesson 3
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

               Study WB Chapter 18 Lesson 4
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

               Study WB Chapter 18 Lesson 5
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

               Foundations Study WB Chapter 18
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

            Chapter 18 Editable Labs
            
               Ch. 18 Lab 36: Factors Affecting Reaction Rates
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

               Ch. 18 Lab 37: The Clock Reaction
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

               Ch. 18 Lab 38: Disturbing Equilibrium
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

               Ch. 18 Lab 39: A Solubility Product Constant
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

               Ch. 18 Lab Practicals: Reaction Rates and Equilibrium
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

               Ch. 18 Quick Lab Record Sheet
                 Curriculum Standards: Describe how to express the rate of a chemical reaction. Identify four factors that influence the rate of a chemical reaction. Describe the relationship between the value of the specific rate constant and the speed of a chemical reaction. Describe how most reactions progress from start to finish. Describe what happens at the molecular level in a chemical system at equilibrium. Identify the three stresses that can cause aåÊchange in the equilibrium position of a chemical system. Describe what the size of an equilibrium constant indicates about a system at equilibrium. Describe the relationship between the solubility product constant and the solubility of a compound. Predict whether a precipitation will occur when two solutions are mixed. Identify the two characteristics of spontaneous reactions. Identify the part entropy plays in a chemical reaction. Identify the two factors that determine whether a reaction is spontaneous. Describe how the value of ‰ö G is related to the spontaneity of a reaction. 

            Chapter 18 Editable Assessments
            
               Ch. 18 Core TR: Chapter Quiz

               Ch. 18 Core TR: Ch. Test A

               Ch. 18 Core TR: Ch. Test B

            Chapter 18 Additional Editable Resources
            
               Ch. 18 Core TR: Section 1 Review

               Ch. 18 Core TR: Section 2 Review

               Ch. 18 Core TR: Section 3 Review

               Ch. 18 Core TR: Section 4 Review

               Ch. 18 Core TR: Section 5 Review

               Ch. 18 Core TR: Practice Problems

               Ch. 18 Core TR: Interpreting Graphics

               Ch. 18 Core TR: Vocabulary Review

            Chapter 18 Image Library
            
               Figure 18.2

               Figure 18.3

               Figure 18.4

               Figure 18.5_part1

               Figure 18.5_part2

               Figure 18.6_part1

               Figure 18.6_part2

               Figure 18.7

               Figure 18.8

               Figure 18.9

               Figure 18.10

               Image 1, p. 606

               Figure 18.11

               Figure 18.12

               Figure 18.13

               Figure 18.14

               Figure 18.15_part1

               Figure 18.15_part2

               Figure 18.16

               Figure 18.17

               Table 18.1

               Figure 18.18_part1

               Figure 18.18_part2

               Table 18.2

               Figure 18.19_part1

               Figure 18.19_part2

               Figure 18.20

               Figure 18.22

               Figure 18.23_part1

               Figure 18.23_part2

               Figure 18.25

               Table 18.3

               Figure 18.26

               Image 1, p. 639

               Image 1, p. 640

               Image 1, p. 641

               Image 2, p. 641

               Image 1, p. 643

               Image 2, p. 643

         Chapter 19: Acids, Bases, and Salts
         
            Chapter-Level Activities
            
               Ch. 19 Math Tutorial: Logarithmic Scale

               Ch. 19 Concepts in Action: Acid Clues to a Marble Mystery
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               Ch. 19 Directed Virtual Lab: Acids and Bases
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               Ch. 19 Problem Set
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               Ch. 19 CO2 and Thinning Shells
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               Chapter 19 Flash Cards

            19.1 Acid-Base Theories
            
               19.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. 

            19.2 Hydrogen Ions and Acidity
            
               19.2 Chemistry Tutorial: Calculating pH from [H+] and [OH-]
                 Curriculum Standards: Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. 

               19.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. 

               19.2 Foundations Chemistry Tutorial: Calculating pH from H ion and OH ion.
                 Curriculum Standards: Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. 

            19.3 Strengths of Acids and Bases
            
               19.3 Chemistry Tutorial: Calculating a Dissociation Constant
                 Curriculum Standards: Describe how acids and bases are classified as either strong or weak. 

               19.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe how acids and bases are classified as either strong or weak. 

               19.3 Foundations Chemistry Tutorial: Calculating a Dissociation Constant
                 Curriculum Standards: Describe how acids and bases are classified as either strong or weak. 

            19.4 Neutralization Reactions
            
               19.4 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. 

               19.4 Chemistry Tutorial: Determining Concentration by Titration
                 Curriculum Standards: Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. 

            19.5 Salts in Solution
            
               19.5 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               19.5 Chem Tutorial: Using Equations to Illustrate Buffers
                 Curriculum Standards: Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               19.5 Foundations Chem Tutorial: Using Eq. to Illustrate Buffers
                 Curriculum Standards: Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

            Chapter 19 Online Student Edition
              Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

            Chapter 19.2 Online Student Edition: The pH concept
              Curriculum Standards: Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. 

            Chapter 19.2 Online Student Edition: Measuring pH
              Curriculum Standards: Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. 

            Chapter 19.3 Online Student Edition: Strenghts of Acids and Bases
              Curriculum Standards: Describe how acids and bases are classified as either strong or weak. 

            19.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. 

            19.4 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. 

            19.4 Chemistry Tutorial: Determining Concentration by Titration
              Curriculum Standards: Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. 

            19.5 Chem Tutorial: Using Equations to Illustrate Buffers
              Curriculum Standards: Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

            Ch. 19 Directed Virtual Lab: Acids and Bases
              Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

            19.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe how acids and bases are classified as either strong or weak. 

            19.5 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

            19.2 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. 

            Chapter 19.1 Online Student Edition: Arrhenius Acids and Bases
              Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. 

            Chapter 19.2 Online Student Edition: Hydrogen Ions from Water
              Curriculum Standards: Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. 

            Chapter 19.5 Online Student Edition: Salt Hydrolysis
              Curriculum Standards: Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

            Chapter 19.5 Online Student Edition: Buffers
              Curriculum Standards: Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

            Chapter 19.1 Online Student Edition: Bronsted-Lowry Acids and Bases
              Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. 

            19.2 Chemistry Tutorial: Calculating pH from [H+] and [OH-]
              Curriculum Standards: Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. 

            Chapter 19.1: Lewis Acids and Bases
              Curriculum Standards: Define an acid and a base according to Lewis. 

            Chapter 19.4: Acid-Base Reactions
              Curriculum Standards: Identify the products that form when an acid and a base react. 

            Chapter 19 Pre-Test: Acids, Bases, and Salts
              Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

            Chapter 19 Post-Test: Acids, Bases, and Salts
              Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

            Chapter 19 Editable Study Workbook
            
               Study WB Chapter 19 Lesson 1
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               Study WB Chapter 19 Lesson 2
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               Study WB Chapter 19 Lesson 3
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               Study WB Chapter 19 Lesson 4
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               Study WB Chapter 19 Lesson 5
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               Foundations Study WB Chapter 19
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

            Chapter 19 Editable Labs
            
               Ch. 19 Lab 40: Estimation of pH
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               Ch. 19 Lab 42: Neutralization Reactions
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               Ch. 19 Lab 43: Acid-Base Titrations
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               Ch. 19 Lab 44: Salt Hydrolysis
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               Ch. 19 Lab 45: Buffers
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               Ch. 19 Lab Practicals: Acids, Bases, and Salts
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

               Ch. 19 Quick Lab Record Sheet
                 Curriculum Standards: Define an acid and a base according to Arrhenius. Distinguish an acid from a base in the BrÌünsted-Lowry theory. Define an acid and a base according to Lewis. Describe how [H+] and [OH+] are related in an aqueous solution. Classify a solution as neutral, acidic, or basic using pH. Identify two methods that are used to measure pH. Describe how acids and bases are classified as either strong or weak. Identify the products that form when an acid and a base react. Identify the point in a titration when neutralization will occur. Describe when a solution of a salt is acidic or basic. Identify the components of a buffer. 

            Chapter 19 Editable Assessments
            
               Ch. 19 Core TR: Chapter Quiz

               Ch. 19 Core TR: Chapter Test A

               Ch. 19 Core TR: Chapter Test B

            Chapter 19 Additional Editable Resources
            
               Ch. 19 Core TR: Section 1 Review

               Ch. 19 Core TR: Section 2 Review

               Ch. 19 Core TR: Section 3 Review

               Ch. 19 Core TR: Section 4 Review

               Ch. 19 Core TR: Section 5 Review

               Ch. 19 Core TR: Practice Problems

               Ch. 19 Core TR: Interpreting Graphics

               Ch. 19 Core TR: Vocabulary Review

            Chapter 19 Image Library
            
               Table 19.1

               Figure 19.2

               Table 19.2

               Figure 19.5

               Figure 19.6

               Table 19.3

               Table 19.4

               Table 19.5

               Figure 19.8

               Figure 19.9_part1

               Figure 19.9_part2

               Figure 19.10

               Table 19.6

               Figure 19.11

               Table 19.7

               Figure 19.12_part1

               Figure 19.12_part2

               Table 19.8

               Figure 19.14_part1

               Figure 19.14_part2

               Figure 19.14_part3

               Figure 19.15

               Figure 19.16_part1

               Figure 19.16_part2

               Figure 19.16_part3

               Figure 19.17

               Figure 19.18_part1

               Figure 19.18_part2

               Table 19.9

               Image 1, p. 685

               Image 2, p. 685

               Image 1, p. 686

               Image 2, p. 686

               Image 1, p. 687

               Image 1, p. 688

               Image 1, p. 689

         Chapter 20: Oxidation-Reduction Reactions
         
            Chapter-Level Activities
            
               Ch. 20 Math Tutorial: Balanced Equations

               Ch. 20 Concepts in Action: Used Cars 101: Where your Car Used to Live
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

               Ch. 20 Directed Virtual Lab: Redox Titrations: Determine Sample Purity
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

               Ch. 20 Problem Set
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

               Ch. 20 Building Better Bridges
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

               Chapter 20 Flash Cards

            20.1 Meaning of Oxidation and Reduction
            
               20.1 Chemistry Tutorial: Identifying Oxidized and Reduced Reactants
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. 

               20.1 Kinetic Art: Corrosion
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. 

               20.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. 

               20.1 Foundations Chemistry Tutorial: Identifying Oxidized and Reduced Reactants
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. 

            20.2 Oxidation Numbers
            
               20.2 Chemistry Tutorial: Assigning Oxidation Numbers to Atoms
                 Curriculum Standards: State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. 

               20.2  Lesson Overview (PowerPoint file)
               20.2 Lesson Overview (PowerPoint file)Lesson Overview is a PowerPoint presentation of each lesson for use as a presentation or study resource.
                 Curriculum Standards: State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. 

               20.2 Foundations Chemistry Tutorial: Assigning Oxidation Numbers to Atoms
                 Curriculum Standards: State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. 

            20.3 Describing Redox Equations
            
               20.3 Chem Tutorial: Balancing Redox Eq. by Oxidation-Number Change
                 Curriculum Standards: Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

               20.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

            Chapter 20 Online Student Edition
              Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

            20.2 Online Student Edition: Ox.-Number Changes in Chemical Rxns
              Curriculum Standards: State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. 

            Chapter 20.3 Online Student Edition: Balancing Redox Reactions
              Curriculum Standards: Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

            Ch. 20 Concepts in Action: Used Cars 101: Where your Car Used to Live
              Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

            20.1 Chemistry Tutorial: Identifying Oxidized and Reduced Reactants
              Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. 

            20.2 Chemistry Tutorial: Assigning Oxidation Numbers to Atoms
              Curriculum Standards: State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. 

            20.3 Chem Tutorial: Balancing Redox Eq. by Oxidation-Number Change
              Curriculum Standards: Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

            20.2  Lesson Overview (PowerPoint file)
            20.2 Lesson Overview (PowerPoint file)Lesson Overview is a PowerPoint presentation of each lesson for use as a presentation or study resource.
              Curriculum Standards: State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. 

            20.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

            20.1 Kinetic Art: Corrosion
              Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. 

            20.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. 

            Chapter 20 Pre-Test: Oxidation-Reduction Reactions
              Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

            Chapter 20 Post-Test: Oxidation-Reduction Reactions
              Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

            Chapter 20 Editable Study Workbook
            
               Study WB Chapter 20 Lesson 1
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

               Study WB Chapter 20 Lesson 2
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

               Study WB Chapter 20 Lesson 3
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

               Foundations Study WB Chapter 20
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

            Chapter 20 Editable Labs
            
               Ch. 20 Lab 41: Reactions of Acids
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

               Ch. 20 Lab 46: Oxidation-Reduction Reactions
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

               Ch. 20 Lab 47: Corrosion
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

               Ch. 20 Lab Practicals: Oxidation-Reduction Reactions
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

               Ch. 20 Quick Lab Record Sheet
                 Curriculum Standards: Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction. Explain how the presence of salts and acids accelerates the corrosion of metals. State the general rule for assigning oxidation numbers. Define oxidation and reduction in terms of a change in oxidation number. Identify the two classes of chemical reactions. Describe two different methods for balancing a redox equation. 

            Chapter 20 Editable Assessments
            
               Ch. 20 Core TR: Chapter Quiz

               Ch. 20 Core TR: Chapter Test A

               Ch. 20 Core TR: Chapter Test B

            Chapter 20 Additional Editable Resources
            
               Ch. 20 Core TR: Section 1 Review

               Ch. 20 Core TR: Section 2 Review

               Ch. 20 Core TR: Section 3 Review

               Ch. 20 Core TR: Practice Problems

               Ch. 20 Core TR: Interpreting Graphics

               Ch. 20 Core TR: Vocabulary Review

            Chapter 20 Image Library
            
               Figure 20.1_part1

               Figure 20.1_part2

               Figure 20.2_part1

               Figure 20.2_part2

               Figure 20.2_part3

               Figure 20.3

               Figure 20.4

               Table 20.1

               Figure 20.6

               Figure 20.8

               Figure 20.9_part1

               Figure 20.9_part2

               Figure 20.10_part1

               Figure 20.10_part2

               Figure 20.11_part1

               Figure 20.11_part2

               Figure 20.12

               Figure 20.13_part1

               Figure 20.13_part2

               Figure 20.13_part3

               Figure 20.14

               Table 20.2

               Image 1, p. 718

               Image 1, p. 721

               Image 1, p. 724

               Image 2, p. 724_part1

               Image 2, p. 724_part2

               Image 2, p. 724_part3

               Image 1, p. 725

               Image 2, p. 725

         Chapter 21: Electrochemistry
         
            Chapter-Level Activities
            
               Ch. 21 Concepts in Action: Chemistry Lessons from Lasagne and Lemons
                 Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

               Ch. 21 Directed Virtual Lab: Electrochemistry
                 Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. 

               Ch. 21 Math Tutorial: Systems of Equations

               Ch. 21 Problem Set
                 Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

               Ch. 21 Better Batteries Through Chemistry
                 Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

               Chapter 21 Flash Cards

            21.1 Electrochemical Cells
            
               21.3 Kinetic Art: Voltaic Cell
                 Curriculum Standards: Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

               21.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. 

            21.2 Half-Cells and Cell Potentials
            
               21.2 Chemistry Tutorial: Writing the Cell Reaction
                 Curriculum Standards: Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. 

               21.2 Chemistry Tutorial: Calculating the Standard Cell Potential
                 Curriculum Standards: Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. 

               21.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. 

            21.3 Electrolytic Cells
            
               21.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

            Chapter 21 Online Student Edition
              Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

            Chapter 21.2 Online Student Edition: Calculating Standard Cell Potentials
              Curriculum Standards: Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. 

            Chapter 21.3 Online Student Edition: Electrolytic vs. Voltaic Cells
              Curriculum Standards: Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

            Ch. 21 Concepts in Action: Chemistry Lessons from Lasagne and Lemons
              Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

            Ch. 21 Directed Virtual Lab: Electrochemistry
              Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. 

            21.3 Kinetic Art: Voltaic Cell
              Curriculum Standards: Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

            21.2 Chemistry Tutorial: Calculating the Standard Cell Potential
              Curriculum Standards: Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. 

            21.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. 

            21.2 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. 

            21.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

            Chapter 21.1 Online Student Edition: Using Voltaic Cells as Energy Sources
              Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. 

            Chapter 21.2 Online Student Edition: Standard Reduction Potentials
              Curriculum Standards: Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. 

            Chapter 21 Pre-Test: Electrochemistry
              Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

            Chapter 21 Post-Test: Electrochemistry
              Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

            Chapter 21 Editable Study Workbook
            
               Study WB Chapter 21 Lesson 1
                 Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

               Study WB Chapter 21 Lesson 2
                 Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

               Study WB Chapter 21 Lesson 3
                 Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

               Foundations Study WB Chapter 21
                 Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

            Chapter 21 Editable Labs
            
               Ch. 21 Lab 48: Electrochemistry
                 Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

               Ch. 21 Lab Practicals: Electrochemistry
                 Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

               Ch. 21 Quick Lab Record Sheet
                 Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

            Chapter 21 Editable Assessments
            
               Ch. 21 Core TR: Chapter Quiz

               Ch. 21 Core TR: Chapter Test A

               Ch. 21 Core TR: Chapter Test B

               Benchmark Test 4 Part A (follows Chapters 17-21)
                 Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

               Benchmark Test 4 Part B (follows Chapters 17-21)
                 Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

            Chapter 21 Additional Editable Resources
            
               Ch. 21 Core TR: Section 1 Review

               Ch. 21 Core TR: Section 2 Review

               Ch. 21 Core TR: Section 3 Review

               Ch. 21 Core TR: Practice Problems

               Ch. 21 Core TR: Interpreting Graphics

               Ch. 21 Core TR: Vocabulary Review

            Chapter 21 Image Library
            
               Figure 21.1_part1

               Figure 21.1_part2

               Table 21.1

               Figure 21.2

               Figure 21.3

               Figure 21.4_part1

               Figure 21.4_part2

               Figure 21.5_part1

               Figure 21.5_part2

               Figure 21.6

               Figure 21.7_part1

               Figure 21.7_part2

               Figure 21.8

               Figure 21.9

               Table 21.2

               Figure 21.11_part1

               Figure 21.11_part2

               Figure 21.12_part1

               Figure 21.12_part2

               Figure 21.13

               Figure 21.14

               Image 1, p. 754

               Image 1, p. 755

               Image 1, p. 756

               Image 2, p. 756

               Image 3, p. 756

               Image 1, p. 757

               Image 1, p. 759

               Image 2, p. 759

         Chapter 22: Hydrocarbon Compounds
         
            Chapter-Level Activities
            
               Ch. 22 Math Tutorial: Graphing Inequalities

               Ch. 22 Concepts in Action: Hydrocarbon Inferno
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

               Ch. 22 Problem Set
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

               Ch. 22 Directed Virtual Lab: Saturated and Unsaturated
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

               Ch. 22 Cracking the Crude
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

               Chapter 22 Flash Cards

            22.1 Hydrocarbons
            
               22.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. 

               22.1 Chemistry Tutorial: Naming Branched-Chain Alkanes
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. 

            22.2 Unsaturated Hydrocarbons
            
               22.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. 

            22.3 Isomers
            
               22.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. 

               22.3 Chemistry Tutorial: Identifying Asymmetric Carbon Atoms
                 Curriculum Standards: Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. 

               22.3 Kinetic Art: Asymmetric Carbons
                 Curriculum Standards: Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. 

            22.4 Hydrocarbon Rings
            
               22.4 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. 

            22.5 Hydrocarbon's From Earth's Crust
            
               22.5 Kinetic Art: Fractional Distillation of Hydrocarbons
                 Curriculum Standards: Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

               22.5 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

            Chapter 22 Online Student Edition
              Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

            Chapter 22.4 Online Student Edition: Cyclic Hydrocarbons
              Curriculum Standards: Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. 

            22.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. 

            22.2 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. 

            22.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. 

            Ch. 22 Concepts in Action: Hydrocarbon Inferno
              Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

            Ch. 22 Directed Virtual Lab: Saturated and Unsaturated
              Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

            22.3 Chemistry Tutorial: Identifying Asymmetric Carbon Atoms
              Curriculum Standards: Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. 

            22.5 Kinetic Art: Fractional Distillation of Hydrocarbons
              Curriculum Standards: Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

            Study WB Chapter 22 Lesson 1
              Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

            22.4 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. 

            Chapter 22.1 Online Student Edition: Alkane
              Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. 

            Chapter 22.2 Online Student Edition: Alkenes
              Curriculum Standards: Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. 

            Chapter 22.3 Online Student Edition: Constitutional Isomers
              Curriculum Standards: Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. 

            Chapter 22.5 Online Student Edition: Petroleum
              Curriculum Standards: Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

            Chapter 22 Pre-Test: Hydrocarbon Compounds
              Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

            Chapter 22  Post-Test: Hydrocarbon Compounds
            Chapter 22 Post-Test: Hydrocarbon Compounds
              Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

            Chapter 22 Editable Study Workbook
            
               Study WB Chapter 22 Lesson 1
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

               Study WB Chapter 22 Lesson 2
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

               Study WB Chapter 22 Lesson 3
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

               Study WB Chapter 22 Lesson 4
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

               Study WB Chapter 22 Lesson 5
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

               Foundations Study WB Chapter 22
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

            Chapter 22 Editable Labs
            
               Ch. 22 Lab 49: Hydrocarbons: A Structural Study
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

               Ch. 22 Lab Practicals: Hydrocarbon Compounds
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

               Ch. 22 Quick Lab Record Sheet
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Describe the structural characteristics of alkenes. Identify the structural characteristics of alkynes. Explain how the properties of constitutional isomers differ. Identify two types of stereoisomers. Identify the general structure of a cyclic hydrocarbon. Describe bonding in a benzene ring. Identify the hydrocarbons found in natural gas. Describe the first step in the refining of petroleum. Classify coal. 

            Chapter 22 Editable Assessments
            
               Ch. 22 Core TR: Chapter Quiz

               Ch. 22 Core TR: Chapter Test A

               Ch. 22 Core TR: Chapter Test B

            Chapter 22 Additional Editable Resources
            
               Ch. 22 Core TR: Section 1 Review

               Ch. 22 Core TR: Section 2 Review

               Ch. 22 Core TR: Section 3 Review

               Ch. 22 Core TR: Section 4 Review

               Ch. 22 Core TR: Section 5 Review

               Ch. 22 Core TR: Practice Problems

               Ch. 22 Core TR: Interpreting Graphics

               Ch. 22 Core TR: Vocabulary Review

            Chapter 22 Image Library
            
               Table 22.1

               Figure 22.1

               Figure 22.2_part1

               Figure 22.2_part2

               Figure 22.2_part3

               Figure 22.3

               Table 22.2

               Table 22.3

               Figure 22.4_part1

               Figure 22.4_part2

               Figure 22.5

               Figure 22.6

               Figure 22.7

               Figure 22.8

               Figure 22.9

               Figure 22.10

               Figure 22.11

               Figure 22.12

               Figure 22.14

               Figure 22.15

               Figure 22.16_part1

               Figure 22.16_part2

               Figure 22.16_part3

               Figure 22.16_part4

               Figure 22.16_part5

               Figure 22.17

               Image 1, p. 791

               Image 2, p. 791

               Image 1, p. 792

               Image 1, p. 793

         Chapter 23: Functional Groups
         
            Chapter-Level Activities
            
               Ch. 23 Directed Virtual Lab: Properties of Organic Molecules
                 Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

               Ch. 23 Problem Set
                 Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

               Ch. 23 Concepts in Action: Organic Compounds
                 Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

               Ch. 23 Protection From the Flames
                 Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

               Chapter 23 Flash Cards

            23.1 Introduction to Functional Groups
            
               23.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. 

            23.2 Alcohols, Ethers, and Amines
            
               23.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. 

               23.2 Kinetic Art: Hydration And Hydrogenation
                 Curriculum Standards: Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. 

            23.3 Carbonyl Compounds
            
               23.3 Kinetic Art: Redox Reactions
                 Curriculum Standards: Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Explain why dehydrogenation is classified as an oxidation reaction. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Identify the general formula of an ester. 

               23.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. 

            23.4 Polymers
            
               23.4 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe how addition polymers are formed. Describe how condensation polymers are formed. 

            Chapter 23 Online Student Edition
              Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

            Chapter 23.1 Online Student Edition: Halocarbons
              Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. 

            Ch. 23 Directed Virtual Lab: Properties of Organic Molecules
              Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

            23.2 Kinetic Art: Hydration And Hydrogenation
              Curriculum Standards: Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. 

            23.3 Kinetic Art: Redox Reactions
              Curriculum Standards: Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Explain why dehydrogenation is classified as an oxidation reaction. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Identify the general formula of an ester. 

            Ch. 23 Concepts in Action: Organic Compounds
              Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

            Chapter 23.2 Online Student Edition: Ethers
              Curriculum Standards: Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. 

            23.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. 

            23.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. 

            23.2 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. 

            23.4 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe how addition polymers are formed. Describe how condensation polymers are formed. 

            Chapter 23.3 Online Student Edition: Aldehydes and Ketones
              Curriculum Standards: Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. 

            Chapter 23.2 Online Student Edition: Amines
              Curriculum Standards: Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. 

            Chapter 23.3 Online Student Edition: Oxidation-Reduction Reactions
              Curriculum Standards: Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. 

            Chapter 23.3 Online Student Edition: Carbonyl Compounds
              Curriculum Standards: Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. 

            Chapter 23.4 Online Student Edition: Polymers
              Curriculum Standards: Describe how addition polymers are formed. Describe how condensation polymers are formed. 

            Chapter 23.4 Online Student Edition: Condensation Polymers
              Curriculum Standards: Describe how addition polymers are formed. Describe how condensation polymers are formed. 

            Chapter 23 Pre-Test: Functional Groups
              Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

            Chapter 23 Post-Test: Functional Groups
              Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

            Chapter 23 Editable Study Workbook
            
               Study WB Chapter 23 Lesson 1
                 Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

               Study WB Chapter 23 Lesson 2
                 Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

               Study WB Chapter 23 Lesson 3
                 Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

               Study WB Chapter 23 Lesson 4
                 Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

               Foundations Study WB Chapter 23
                 Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

            Chapter 23 Editable Labs
            
               Ch. 23 Lab 50: Esters of Carboxylic Acids
                 Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

               Ch. 23 Lab Practicals: Functional Groups
                 Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

               Ch. 23 Quick Lab Record Sheet
                 Curriculum Standards: Classify organic compounds. Identify the general formula of a halocarbon. Describe how substitution reactions are used in organic chemistry. Identify the general formula of an alcohol. Explain how addition reactions are used in organic chemistry. Identify the general formula of an ether. Identify the general formula of an amine. Identify the structural characteristic that an aldehyde and a ketone share. Identify the general formula of a carboxylic acid. Explain why dehydrogenation is classified as an oxidation reaction. Identify the general formula of an ester. Describe how addition polymers are formed. Describe how condensation polymers are formed. 

            Chapter 23 Editable Assessments
            
               Ch. 23 Core TR: Chapter Quiz

               Ch. 23 Core TR: Chapter Test A

               Ch. 23 Core TR: Chapter Test B

            Chapter 23 Additional Editable Resources
            
               Ch. 23 Core TR: Section 1 Review

               Ch. 23 Core TR: Section 2 Review

               Ch. 23 Core TR: Section 3 Review

               Ch. 23 Core TR: Section 4 Review

               Ch. 23 Core TR: Practice Problems

               Ch. 23 Core TR: Interpreting Graphics

               Ch. 23 Core TR: Vocabulary Review

            Chapter 23 Image Library
            
               Table 23.1

               Figure 23.2

               Table 23.2

               Table 23.3

               Table 23.4

               Figure 23.4_part1

               Figure 23.4_part2

               Figure 23.4_part3

               Figure 23.5_part1

               Figure 23.5_part2

               Figure 23.6_part1

               Figure 23.6_part2

               Figure 23.6_part3

               Figure 23.6_part4

               Figure 23.7_part1

               Figure 23.7_part2

               Figure 23.8

               Table 23.5

               Table 23.6

               Figure 23.10

               Table 23.7

               Figure 23.11_part1

               Figure 23.11_part2

               Figure 23.13

               Figure 23.14_part1

               Figure 23.14_part2

               Figure 23.17_part1

               Figure 23.17_part2

               Figure 23.17_part3

               Image 1, p. 829

               Image 1, p. 831

               Image 1, p. 832

               Image 2, p. 832

               Image 1, p. 835

         Chapter 24: Chemistry of Life
         
            Chapter-Level Activities
            
               Ch. 24 Concepts in Action: A Fish's Life
                 Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

               Ch. 24 Directed Virtual Lab: Food Calorimetry
                 Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

               Ch. 24 The Secret’s in the Muscles
                 Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

               Ch. 24 Problem Set
                 Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

               Chapter 24 Flash Cards

            24.1 A Basis for Life
            
               24.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. 

            24.2 Carbohydrates
            
               24.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Construct the general formula for carbohydrates. 

            24.3 Amino Acids and Their Polymers
            
               24.3 Kinetic Art: Peptide Structures
                 Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Diagram the general structure of an amino acid. Describe how enzymes affect the rates of reactions in living things. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? 

               24.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. 

            24.4 Lipids
            
               24.4 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the physical property that distinguishes lipids from other biological molecules. 

            24.5 Nucleic Acids
            
               24.5 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? 

            24.6 Metabolism
            
               24.6 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

               24.6 Kinetic Art: The Nitrogen Cycle

            Chapter 24 Online Student Edition
              Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

            Chapter 24.5 Online Student Edition: DNA and RNA
              Curriculum Standards: Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? 

            Chapter 24.5 Online Student Edition: DNA Technologies
              Curriculum Standards: Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? 

            Chapter 24.6 Online Student Edition: Metabolism Reactions
              Curriculum Standards: Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

            Chapter 24.1 Online Student Edition: A Basis for Life
              Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. 

            Chapter 24.2 Online Student Edition: Classifying Carbohydrates
              Curriculum Standards: Construct the general formula for carbohydrates. 

            Chapter 24.3 Online Student Edition: Amino Acids
              Curriculum Standards: Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. 

            Chapter 24.3 Online Student Edition: Peptides and Proteins
              Curriculum Standards: Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. 

            Chapter 24.3 Online Student Edition: Enzymes
              Curriculum Standards: Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. 

            Chapter 24.4 Online Student Edition: Describing Lipids
              Curriculum Standards: Identify the physical property that distinguishes lipids from other biological molecules. 

            Chapter 24.5 Online Student Edition: DNA and RNA
              Curriculum Standards: Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? 

            Chapter 24.5 Online Student Edition: Gene Mutation
              Curriculum Standards: Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? 

            Chapter 24.6 Online Student Edition: ATP
              Curriculum Standards: Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

            24.3 Kinetic Art: Peptide Structures
              Curriculum Standards: Explain why a carbon atom forms four covalent bonds. Identify two possible arrangements of carbon atoms in an alkane. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Diagram the general structure of an amino acid. Describe how enzymes affect the rates of reactions in living things. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? 

            24.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. 

            24.2 Lesson Overview (PowerPoint file)
              Curriculum Standards: Construct the general formula for carbohydrates. 

            24.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. 

            24.4 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the physical property that distinguishes lipids from other biological molecules. 

            24.5 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? 

            24.6 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

            Ch. 24 Concepts in Action: A Fish's Life
              Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

            Study WB Chapter 24 Lesson 5
              Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

            Study WB Chapter 24 Lesson 6
              Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

            24.6 Kinetic Art: The Nitrogen Cycle
              Curriculum Standards: Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

            Chapter 24 Pre-Test: The Chemistry of Life
              Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

            Chapter 24 Post-Test: The Chemistry of Life
              Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

            Chapter 24 Editable Study Workbook
            
               Study WB Chapter 24 Lesson 1
                 Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

               Study WB Chapter 24 Lesson 2
                 Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

               Study WB Chapter 24 Lesson 3
                 Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

               Study WB Chapter 24 Lesson 4
                 Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

               Study WB Chapter 24 Lesson 5
                 Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

               Study WB Chapter 24 Lesson 6
                 Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

               Foundations Study WB Chapter 24
                 Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

            Chapter 24 Editable Labs
            
               Ch. 24 Lab 51: Preparation of Soap
                 Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

               Ch. 24 Quick Lab Record Sheet
                 Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

            Chapter 24 Editable Assessments
            
               Ch. 24 Core TR: Chapter Quiz

               Ch. 24 Core TR: Chapter Test A

               Ch. 24 Core TR: Chapter Test B

            Chapter 24 Additional Editable Resources
            
               Ch. 24 Core TR: Section 1 Review

               Ch. 24 Core TR: Section 2 Review

               Ch. 24 Core TR: Section 3 Review

               Ch. 24 Core TR: Section 4 Review

               Ch. 24 Core TR: Section 5 Review

               Ch. 24 Core TR: Section 6 Review

               Ch. 24 Core TR: Interpreting Graphics

               Ch. 24 Core TR: Vocabulary Review

            Chapter 24 Image Library
            
               Figure 24.1

               Figure 24.2_part1

               Figure 24.2_part2

               Figure 24.3

               Figure 24.6

               Table 24.1

               Figure 24.8

               Figure 24.9_part1

               Figure 24.9_part2

               Figure 24.10

               Figure 24.11_part1

               Figure 24.11_part2

               Figure 24.14_part1

               Figure 24.14_part2

               Figure 24.14_part3

               Figure 24.15

               Figure 24.16_part1

               Figure 24.16_part2

               Figure 24.17_part1

               Figure 24.17_part2

               Figure 24.18_part1

               Figure 24.18_part2

               Table 24.2

               Figure 24.19_part1

               Figure 24.19_part2

               Figure 24.21

               Figure 24.22

               Figure 24.24_part1

               Figure 24.24_part2

               Figure 24.25

               Figure 24.27

               Figure 24.28

         Chapter 25: Nuclear Chemistry
         
            Chapter-Level Activities
            
               Ch. 25 Math Tutorial: Exponential Decay

               Ch. 25 Concepts in Action: Happy Birthday Half-Life
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

               Ch. 25 Directed Virtual Lab: Radiation
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

               Ch. 25 Curie’s Cures
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

               Ch. 25 Problem Set
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

               Chapter 25 Flash Cards

            25.1 Nuclear Radiation
            
               25.1 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. 

               25.1 Kinetic Art: Alpha and Beta Decay
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. 

            25.2 Nuclear Transformations
            
               25.2 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. 

               25.2 Chemistry Tutorial: Using Half-lives in Calculations
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. 

               25.2 Foundations Chemistry Tutorial: Using Half-lives in Calculations
                 Curriculum Standards: Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. 

            25.3 Fission and Fusion
            
               25.3 Kinetic Art: How a Nuclear Reactor Works
                 Curriculum Standards: Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. 

               25.3 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. 

            25.4 Radiation in Your Life
            
               25.4 Lesson Overview (PowerPoint file)
                 Curriculum Standards: Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

            Chapter 25 Online Student Edition
              Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

            Chapter 25.2 Online Student Edition: Radioactivity
              Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. 

            25.2 Lesson Overview (PowerPoint file)
              Curriculum Standards: Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. 

            Ch. 25 Concepts in Action: Happy Birthday Half-Life
              Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

            Ch. 25 Directed Virtual Lab: Radiation
              Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

            25.3 Kinetic Art: How a Nuclear Reactor Works
              Curriculum Standards: Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. 

            25.1 Lesson Overview (PowerPoint file)
              Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. 

            25.3 Lesson Overview (PowerPoint file)
              Curriculum Standards: Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. 

            25.4 Lesson Overview (PowerPoint file)
              Curriculum Standards: Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

            Chapter 25.2 Online Student Edition: Transmutattion Reactions
              Curriculum Standards: Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. 

            Chapter 25.3 Online Student Edition: Nuclear Fission
              Curriculum Standards: Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. 

            Chapter 25.4 Online Student Edition: Detecting Radiation
              Curriculum Standards: Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. 

            Chapter 25.4 Online Student Edition: Using Radiation
              Curriculum Standards: Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

            Chapter 25.3 Online Student Edition: Nuclear Fusion
              Curriculum Standards: Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. 

            25.1 Kinetic Art: Alpha and Beta Decay
              Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. 

            25.2 Chemistry Tutorial: Using Half-lives in Calculations
              Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. 

            Chapter 25 Pre-Test: Nuclear Chemistry
              Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

            Chapter 25 Post-Test: Nuclear Chemistry
              Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

            Chapter 25 Editable Study Workbook
            
               Study WB Chapter 25 Lesson 1
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

               Study WB Chapter 25 Lesson 2
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

               Study WB Chapter 25 Lesson 3
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

               Study WB Chapter 25 Lesson 4
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

               Foundations Study WB Chapter 25
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

            Chapter 25 Editable Labs
            
               Ch. 25 Lab 52: Radioactivity and Radiation
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

               Ch. 25 Lab Practicals: Nuclear Chemistry
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

               Ch. 25 Quick Lab Record Sheet
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

            Chapter 25 Editable Assessments
            
               Ch. 25 Core TR: Chapter Quiz

               Ch. 25 Core TR: Chapter Test A

               Ch. 25 Core TR: Chapter Test B

               Benchmark Test 5 Part A (follows Chapters 22-25)
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

               Benchmark Test 5 Part B (follows Chapters 22-25)
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

               Outcome Test Part A (administered at the end of the course)
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

               Outcome Test Part B (administered at the end of the course)
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

            Chapter 25 Additional Editable Resources
            
               Ch. 25 Core TR: Section 1 Review

               Ch. 25 Core TR: Section 2 Review

               Ch. 25 Core TR: Section 3 Review

               Ch. 25 Core TR: Section 4 Review

               Ch. 25 Core TR: Interpreting Graphics

               Ch. 25 Core TR: Vocabulary Review

            Chapter 25 Image Library
            
               Image 1, p. 874

               Figure 25.1

               Table 25.1

               Figure 25.2

               Figure 25.3

               Figure 25.4

               Figure 25.5

               Figure 25.6

               Figure 25.7

               Table 25.2

               Figure 25.8

               Table 25.3

               Figure 25.9

               Figure 25.10

               Figure 25.11

               Figure 25.12

               Figure 25.13

               Figure 25.14

               Figure 25.15

               Figure 25.16

               Figure 25.17

               Figure 25.18

               Image 1, p. 901

               Image 1, p. 902

               Image 2, p. 902

               Image 1, p. 903

               Image 1, p. 904

               Image 1, p. 905

               Image 2, p. 905

            Editable SAT and ACT-type Tests
            
               SAT-like Practice Test 1
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

               SAT-like Practice Test 2
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

               ACT-like Practice Test
                 Curriculum Standards: Explain the relationship between unstable isotopes and radioactivity. Describe three main types of nuclear radiation. Identify factors that determine the type of decay a radioisotope undergoes. Solve problems that involve half-life. Identify two ways transmutations can occur. Describe what happens in a nuclear chain reaction. Describe what happens to spent fuel rods. Distinguish fission reactions from fusion reactions. Compare three devices that are used to detect radiation. Describe some practical uses of radioisotopes. 

         Probeware Lab Manual
         
            PASCO
            
               Starter Lab
               
                  Data Studio Version (student)

                  Xplorer GLX Version (student)

                  SPARK Learning System Version (student)

                  SPARKvue Version (student)

               Chapter Labs
               
                  Chapter 8 lab: Properties of Ionic and Covalent Compounds (student)

                  Chapter 14 lab: Ideal Gas Law (student)

                  Chapter 16 lab: Concentration of a Solution: Beer’s Law (student)

                  Chapter 21 lab: Electrochemical Battery: Energy from Electrons (student)

                  Chapter 23 lab: Intermolecular Forces (student)

            Vernier
            
               Chapter 2 lab: Fractional Distillation (student)
                 Curriculum Standards: Explain why all samples of a substance have the same intensive properties. Identify the three states of matter. Classify physical changes. Explain how mixtures are classified. Explain how mixtures can be separated. Explain the difference between an element and a compound. Distinguish between a substance and a mixture. Describe what chemists use to represent elements and compounds. Explain how a periodic table is useful. Describe what happens during a chemical change. Identify four possible clues that a chemical change has taken place. Describe how the mass of the reactants and the mass of the products of a chemical reaction are related. 

               Chapter 14 lab: Boyle's Law (student)
                 Curriculum Standards: Explain why gases are easier to compress than solids or liquids. Describe the three factors that affect gas pressure. Describe the relationships among pressure, volume, and temperature of a gas. Calculate the amount of a contained gas when the pressure, volume, and temperature are specified. Determine the conditions under which real gases are most likely to differ from ideal gases. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses. 

               Chapter 16 lab: Determining the Concentration of a Solution: Beer's Law (student)
                 Curriculum Standards: Identify the factors that affect how fast a substance dissolves. Describe the equilibrium in a saturated solution. Describe the factors that affect the solubility of a substance. Calculate the molarity of a solution. Describe the effect of dilution on the total moles of solute in solution. Express solution concentration as a percent by volume or percent by mass. Explain how colligative properties can be explained on a particle basis. Identify the two ways of expressing the ratio of solute to solvent in a solution. Describe how the freezing-point depression and boiling-point elevation are related to molality. 

               Chapter 21 lab: Microvoltaic Cells (student)
                 Curriculum Standards: Identify the type of chemical reaction that is involved in all electrochemical processes. Describe how a voltaic cell produces electrical energy. Identify the current applications that use electrochemical processes to produce electrical energy. Identify what causes the electrical potential of an electrochemical cell. Determine the standard reduction potential of a half-cell. Determine if a redox reaction is spontaneous or nonspontaneous. Distinguish between electrolytic and voltaic cells. Describe some applications that use electrolytic cells. 

               Chapter 24 lab: Energy Content of Foods (student)
                 Curriculum Standards: Identify the two major cell types that occur in nature. Identify the compound that is reduced during photosynthesis and the compounds formed. Construct the general formula for carbohydrates. Diagram the general structure of an amino acid. Identify what determines the differences in the chemical and physiological properties of peptides and proteins. Describe how enzymes affect the rates of reactions in living things. Identify the physical property that distinguishes lipids from other biological molecules. Identify the functions of DNA and RNA. Identify the number of bases of DNA required to specify one amino acid in a peptide chain. Define gene mutations. What are two examples of DNA technologies used today? Describe the function of ATP in the cell. Describe what happens to biological molecules and energy during catabolism and anabolism. Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. 

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