Correlations

Chemistry: The Central Science, 10th Edition AP* Edition ©2006

Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten, Julia R. Burdge

Correlated to: Advanced Placement* (AP*) Chemistry Course Description (Grades 9–12)

SE = Student Edition
TECH = Technology

I. Structure of Matter

A. Atomic theory and atomic structure
1. Evidence for the atomic theory	SE: 38–40, 41–42
2. Atomic masses; determination by chemical and physical means	SE: 43–44, 45–47, 48
3. Atomic number and mass number; isotopes	SE: 45–46, 902, 908
4. Electron energy levels: atomic spectra, quantum numbers atomic orbitals	SE: 224–242, 373–75
5. Periodic relationships including, for example, atomic radii, ionization energies, electron affinities, oxidation states	SE: 137–43, 248–50, 266–70, 271–76, 322, 1011–12
B. Chemical bonding
1. Binding forces	SE: 918–20
2. Types: ionic, covalent, metallic hydrogen bonding, van der Waals (including London dispersion forces)	SE: 303–307, 309–12, 447–51, 429–430
3. Relationships to states, structure, and properties of matter	SE: 4–5, 7–9, 9–12
4. Polarity of bonds, electronegativities	SE: 312–16
5. Molecular models	SE: 345–395, 373–375, 360–367
6. Lewis structures	SE: 317–21
7. Valence bond: hybridization of orbitals, resonance, sigma and pi bonds	SE: 360–61, 302, 367–73, 322–25
8. VSEPR	SE: 348–57
9. Geometry of molecules and ions, structural isomerism of simple organic molecules and coordination complexes; dipole moments of molecules; relation of properties to structure	SE: 346–366, 446–48, 1038–43, 1069–70, 1075
C. Nuclear chemistry: nuclear equations, half-lives and radioactivity; chemical applications	SE: 902–06, 910–13, 915–16, 921–23, 916–20, 925–29

II. States of Matter

A. Gases
1. Laws of ideal gases
—a. Equation of state for an ideal gas	SE: 408–413, 413–15 TECH: Virtual ChemLab 10-6
—b. Partial pressures	SE: 417–419, 419–420 TECH: Virtual ChemLab 10-5
2. Kinetic-molecular theory
—a. Interpretation of ideal gas laws on the basis of this theory	SE: B420–23 TECH: Virtual ChemLab 10-4
—b. Avogadro's hypothesis and the mole concept	SE: 407–08, 90–96 TECH: Virtual ChemLab 10-3
—c. Dependence of kinetic energy of molecules on temperature	SE: 406–407
—d. Deviations from ideal gas laws	SE: 427–30
B. Liquids and solids
1. Liquids and solids from the kinetic-molecular viewpoint	SE: 444–46
2. Phase diagrams of one-component systems	SE: 455–457, 462–63
3. Changes of state, including critical points and triple points	SE: 461–464
4. Structure of solids; lattice energies	SE: 464–75
C. Solutions
1. Types of solutions and factors affecting solubility	SE: 529–541, 8–9, 122–124
2. Methods of expressing concentration (The use of normalities is not tested)	SE: 543–47 TECH: Virtual ChemLab 13-1, 13-2
3. Raoult's law and colligative properties (nonvolatile solutes); osmosis	SE: 548–550, 785–87, 553–55
4. Non–ideal behavior (qualitative aspects)	SE: 558–562 TECH: Virtual ChemLab 10-7

III. Reactions

A. Reaction types
1. Acid-base reactions; concepts of Arrhenius, Brønsted-Lowry, and Lewis; coordination complexes; amphoterism	SE: 131–36, 670–75, 706–709
2. Precipitation reactions	SE: 126–30 TECH: Virtual ChemLab 3-8
3. Oxidation-reduction reactions	SE: 137–44, 848–50 TECH: Virtual ChemLab 20-1
—a. Oxidation number	SE: 137–44, 317–22
—b. The role of the electron in oxidation-reduction	SE: 137–4, 848–50
—c. Electrochemistry: electrolytic and galvanic cells; Faraday's laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions	SE: 871–76
B. Stoichiometry
1. Ionic and molecular species present in chemical systems: net ionic equations	SE: 126–30
2. Balancing of equations, including those for redox reactions	SE: 80–84, 100–04, 850–54
3. Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants	SE: 52–54, 90–96, 96–100, 104–108, 408–13
C. Equilibrium
1. Concept of dynamic equilibrium, physical and chemical; Le Chatelier's principle; equilibrium constants	SE: 459–61, 632–37, 637–40, 684–87
2. Quantitative treatment
—a. Equilibrium constants for gaseous reactions: Kp, Kc	SE: 632–37
—b. Equilibrium constants for reactions in solution	SE: 676–682, 739–743B
——i. Constants for acids and bases; pK; pH	SE: 676–82
——ii. Solubility product constants and their application to precipitation and the dissolution of slightly soluble compounds	SE: 739–43
——iii. Common ion effect; buffers; hydrolysis	SE: 722–24, 725–31, 706–10
D. Kinetics
1. Concept of rate of reaction	SE: 577–82
2. Use of experimental data and graphical analysis to determine reactant order, rate constants, and reaction rate laws	SE: 582–86, 587–93
3. Effect of temperature change on rates	SE: 393–98
4. Energy of activation; the role of catalysts	SE: 393–98, 607–13
5. The relationship between the rate-determining step and a mechanism	SE: 599–606
E. Thermodynamics
1. State functions	SE: 172–76, 804–08
2. First law: change in enthalpy; heat of formation; heat of reaction; Hess's law; heats of vaporization and fusion; calorimetry	SE: 187–91, 192–95, 803–04
3. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes	SE: 530–35, 808–11
4. Relationship of change in free energy to equilibrium constants and electrode potentials	SE: 286–90, 312–16

IV. Descriptive Chemistry

1. Chemical reactivity and products of chemical reactions	SE: 85–88
2. 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	SE: 49–51, 260–62, 276–81, 281–85, 286–90
3. Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties).	SE: 67–69, 1064–1090

V. Laboratory

1. Making observations of chemical reactions and substances	TECH: Virtual ChemLab 3-8, 4-2, 17-4, 17-9 to 17-12
2. Recording data	TECH: Virtual ChemLab 1-20
3. Calculating and interpreting results based on the quantitative data obtained	TECH: Virtual ChemLab 2-1, 2-2, 3-1 to 3-7, 4-4 to 4-8, 10-1 to 10-7, 13-1 to 13-8
4. Communicating effectively the results of experimental work	TECH: Virtual ChemLab 1-20

Chemical Calculations

1. Percentage composition	SE: 88–89
2. Empirical and molecular formulas from experimental data	SE: 53–54, 92–95
3. Molar masses from gas density, freezing-point, and boiling-point measurements	SE: 92–96, 413–416
4. Gas laws, including the ideal gas law, Dalton's law, and Graham's law	SE: 404–07, 408–411
5. Stoichiometric relations using the concept of the mole; titration calculations	SE: 90–96, 151–53, 732–39
6. Mole fractions; molar and molal solutions	SE: 543–547, 739–41
7. Faraday's law of electrolysis	SE: 868–70
8. Equilibrium constants and their applications, including their use for simultaneous equilibria	SE: 632–36, 684–90
9. Standard electrode potentials and their use; Nernst equation	SE: 655–59, 871–74
10. Thermodynamic and thermochemical calculations	SE: 168–70, 172–75, 804–06, 808–11
11. Kinetics calculations	SE: 576, 577–80, 582–85, 587–91, 593–97, 599–605