Chemistry: Molecules, Matter, and Change, Fourth Edition Loretta Jones and Peter Atkins Correlated with AP Chemistry, May 2002, May 2003
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1 Chemistry: Molecules, Matter, and Change, Fourth Edition Loretta Jones and Peter Atkins Correlated with AP Chemistry, May 2002, May 2003 ST=Student textbook I. Structure of Matter A. Atomic theory and atomic structure 1. Evidence for the atomic theory ST: Atomic masses; determination by chemical and physical means ST: 10, 12, 75-77, 622, Atomic number and mass number; isotopes ST: 8-9, 9-10, 11-13, Electron energy levels: atomic spectra, quantum numbers atomic orbitals ST: , , Periodic relationships including, for example, atomic radii, ionization energies, electron affinities, oxidation states ST: 118, , , B. Chemical bonding 1. Binding forces a. Types: ionic, covalent, metallic hydrogen bonding, van der Waals (including London dispersion forces) ST: 209, , , , 422, , 431 b. Relationships to states, structure, and properties of matter ST: 19, 25-27, 92, 225, 472, , 494 c. Polarity of bonds, electronegativities ST: 332, , , 377, 381, Molecular models a. Lewis structures ST: , , , , 661 b. Valence bond: hybridization of orbitals, resonance, sigma and pi bonds ST: , , , , , c. VSEPR ST: , , Geometry of molecules and ions, structural isomerism of simple organic molecules and coordination complexes; dipole moments of molecules; relation of properties to structure ST: , 494, 496, 939, 941 C. Nuclear chemistry: nuclear equations, half-lives and radioactivity; chemical applications ST: , 586, 960, 962, , 973, ,
2 II. States of Matter A. Gases 1. Laws of ideal gases a. Equation of state for an ideal gas ST: 188, , 208 b. Partial pressures ST: 197, , Kinetic-molecular theory a. Interpretation of ideal gas laws on the basis of this theory ST: , 208 b. Avogadro s hypothesis and the mole concept ST: 64-65, 66, 68, 70, 72-75, 187, 188, 192, 195 c. Dependence of kinetic energy of molecules on temperature ST: , , , 782 d. Deviations from ideal gas laws ST: 188, , 208 B. Liquids and solids 1. Liquids and solids from the kinetic-molecular viewpoint ST: 26, 428, , 433, , , Phase diagrams of one-component systems ST: , , Changes of state, including critical points and triple points ST: 460, 462, Structure of solids; lattice energies ST: , 433, C. Solutions 1. Types of solutions and factors affecting solubility ST: 27-28, , , Methods of expressing concentration (The use of normalities is not tested) ST: 96, 154, , Raoult s law and colligative properties (nonvolatile solutes); osmosis ST: , 551, Non-ideal behavior (qualitative aspects) ST: 49, , 740, 742 III. Reactions A. Reaction types 1. Acid-base reactions; concepts of Arrhenius, Bronsted-Lowry, and Lewis; coordination complexes; amphoterism ST: 113, 161, 163, 322, 330, 400, 588, 590, 593, , 687, 699, 719, 720, 845,
3 2. Precipitation reactions ST: 96-98, 98-99, 99, , 126, Oxidation-reduction reactions a. Oxidation number ST: 34, , b. The role of the electron in oxidation-reduction ST: , 351, 576, 791, 823 c. Electrochemistry: electrolytic and galvanic cells; Faraday s laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions ST: 755, , , B. Stoichiometry 1. Ionic and molecular species present in chemical systems: net ionic equations ST: , , Balancing of equations, including those for redox reactions ST: 91, , 161, 792, Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants ST: 75, 77, 79-80, , C. Equilibrium 1. Concept of dynamic equilibrium, physical and chemical; Le Chatelier s principle; equilibrium constants ST: , 526, 642, 643, , 646, , Quantitative treatment a. Equilibrium constants for gaseous reactions: Kp, Kc ST: , , , 780 b. Equilibrium constants for reactions in solution (1) Constants for acids and bases; pk; ph ST: 668, , , , 752 (2) Solubility product constants and their application to precipitation and the dissolution of slightly soluble compounds ST: 99, , 126, , 750 (3) Common ion effect; buffers; hydrolysis ST: , , ,
4 D. Kinetics 1. Concept of rate of reaction ST: , , Use of differential rate laws to determine order of reaction and rate constant from experimental data ST: , , 583, Effect of temperature change on rates ST: , 579, Energy of activation; the role of catalysts ST: 478, 569, 595, 597, 598, 600, The relationship between the rate-determining step and a mechanism ST: 603, E. Thermodynamics 1. State functions ST: 221, 225, 755, First law: change in enthalpy; heat of formation; heat of reaction; Hess s law; heats of vaporization and fusion; calorimetry ST: , Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes ST: 542, 755, Relationship of change in free energy to equilibrium constants and electrode potentials ST: , , , 797,
5 IV. Descriptive Chemistry 1. Chemical reactivity and products of chemical reactions ST: 89-90, 96, 98, , Relationships in the periodic table: horizontal, vertical, and diagonal with examples from alkali metals, alkaline earth metals, halogens, and the first series of transition elements ST: 14-16, 21-22, , Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties). ST: ,
6 See the pages listed below for explanations in the text pertaining to the various problem types and for sample end-of-chapter exercises: 1. Percentage composition ST: 2. Empirical and molecular formulas from experimental data ST: 20, 66-67, 75, 77, 79-80, 3. Molar masses from gas density, freezing-point, and boiling-point measurements ST: , Gas laws, including the ideal gas law, Dalton s law, and Graham s law ST: 6, 90, , 201, 989, 5. Stoichiometric relations using the concept of the mole; titration calculations ST: 161, Mole fractions; molar and molal solutions ST: 197, Faraday s law of electrolysis ST: 811, Equilibrium constants and their applications, including their use for simultaneous equilibria ST: , , Standard electrode potentials and their use; Nernst equation ST: 815, Thermodynamic and thermochemical calculations ST: 241, Kinetics calculations ST: , , 569 ISBN:
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