Organization: Pearson
Product Name: Chemistry 2012 Foundations
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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
List the general guidelines that can help you write the name and formula of a chemical compound. - CHEM12_C09.5.2
Identify two ways that you can determine the heat of reaction when it cannot be directly measured. - CHEM12_C17.4.1
Explain how the law of definite proportions is consistent with Dalton??�s 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
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
Describe three properties of ionic compounds. - CHEM12_C07.2.2
Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen. - CHEM12_C24.6.3
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
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 number of bases of DNA required to specify one amino acid in a peptide chain. - CHEM12_C24.5.2
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
Identify four factors that influence the rate of a chemical reaction. - CHEM12_C18.1.2
Explain how mixtures are classified. - CHEM12_C02.2.1
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
Describe how [H+] and [OH+] are related in an aqueous solution. - CHEM12_C19.2.1
Explain why gases are easier to compress than solids or liquids. - CHEM12_C14.1.1
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
Model the valence electrons of metal atoms. - CHEM12_C07.3.1
What are two examples of DNA technologies used today? - CHEM12_C24.5.4
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 Br?�nsted-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
Define oxidation and reduction in terms of a change in oxidation number. - CHEM12_C20.2.2
Identify some exceptions to the octet rule. - CHEM12_C08.2.3
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
State the general rule for assigning oxidation numbers. - CHEM12_C20.2.1
Describe how enzymes affect the rates of reactions in living things. - CHEM12_C24.3.3
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 a�?change 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 the three assumptions of the kinetic theory as it applies to gases. - CHEM12_C13.1.1
Describe what Bohr proposed in his model of the atom. - CHEM12_C05.1.1
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
Identify the two classes of chemical reactions. - CHEM12_C20.3.1
Describe how VSEPR theory helps predict the shapes of molecules. - CHEM12_C08.3.2
Describe two different methods for balancing a redox equation. - CHEM12_C20.3.2
Describe the relationship between atomic and molecular orbitals. - CHEM12_C08.3.1
Explain how colligative properties can be explained on a particle basis. - CHEM12_C16.3.1
Identify the ways in which orbital hybridization is useful in describing molecules. - CHEM12_C08.3.3
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 ?��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
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
Classify elements based on electron configuration. - CHEM12_C06.2.2
Identify five traditional areas of study in chemistry. - CHEM12_C01.1.2
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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