Correlations

Chemistry: The Central Science, 11th Edition AP* Edition ©2009

Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten, Catherine J. Murphy with contributions from Patrick Woodward

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

I. Structure of Matter

A. Atomic theory and atomic structure
1. Evidence for the atomic theory	Sections 2.1, 2.2
2. Atomic masses; determination by chemical and physical means	Section 2.4
3. Atomic number and mass number; isotopes	Section 2.3
4. Electron energy levels: atomic spectra, quantum numbers atomic orbitals	Section 6.5, Section 9.7
5. Periodic relationships including, for example, atomic radii, ionization energies, electron affinities, oxidation states	Section 4.4, Sections 7.3, 7.4, Section 8.5
B. Chemical bonding
1. Binding forces
—a. Types: ionic, covalent, metallic hydrogen bonding, van der Waals (including London dispersion forces)	Sections 8.1, 8.2, 8.3, 8.8, Section 11.2, Section 11.8, Section 23.5
—b. Relationships to states, structure, and properties of matter	Sections 1.2, 1.3
—c. Polarity of bonds, electronegativities	Section 8.4., Section 22.1
2. Molecular models
—a. Lewis structures	Section 9.1
—b. Valence bond: hybridization of orbitals, resonance, sigma and pi bonds	Section 8.6, Section 9.4
—c. VSEPR	Section 9.2
3. Geometry of molecules and ions, structural isomerism of simple organic molecules and coordination complexes; dipole moments of molecules; relation of properties to structure	Sections 9.1–9.8, Section 24.4
C. Nuclear chemistry: nuclear equations, half-lives and radioactivity; chemical applications	Section 14.4, Sections 21.1, 21.4

II. States of Matter

A. Gases
1. Laws of ideal gases	Section 10.4
—a. Equation of state for an ideal gas	Section 10.4
—b. Partial pressures	Section 10.6
2. Kinetic-molecular theory
—a. Interpretation of ideal gas laws on the basis of this theory	Section 10.8
—b. Avogadro's hypothesis and the mole concept	Section 10.3
—c. Dependence of kinetic energy of molecules on temperature	Section 10.8
—d. Deviations from ideal gas laws	Section 10.8
B. Liquids and solids
1. Liquids and solids from the kinetic-molecular viewpoint	Section 11.1
2. Phase diagrams of one-component systems	Section 11.6
3. Changes of state, including critical points and triple points	Section 11.6
4. Structure of solids; lattice energies	Section 8.2, Section 11.7
C. Solutions
1. Types of solutions and factors affecting solubility	Section 13.3
2. Methods of expressing concentration (The use of normalities is not tested)	Section 13.4
3. Raoult's law and colligative properties (nonvolatile solutes); osmosis	Section 13.5, Section 18.5
4. Non–ideal behavior (qualitative aspects)	Section 13.6

III. Reactions

A. Reaction types
1. Acid-base reactions; concepts of Arrhenius, Brønsted-Lowry, and Lewis; coordination complexes; amphoterism	Section 4.3, Sections 16.2, 16.11
2. Precipitation reactions	Section 4.2
3. Oxidation-reduction reactions	Section 4.4, Section 20.1
—a. Oxidation number	Section 4.4, Section 8.5
—b. The role of the electron in oxidation-reduction	Section 4.4, Section 20.1
—c. Electrochemistry: electrolytic and galvanic cells; Faraday's laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions	Section 20.6
B. Stoichiometry
1. Ionic and molecular species present in chemical systems: net ionic equations	Section 4.2
2. Balancing of equations, including those for redox reactions	Sections 3.1, 3.6, Section 20.2
3. Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants	Section 2.6, Sections 3.4, 3.5, 3.7, Section 10.4
C. Equilibrium
1. Concept of dynamic equilibrium, physical and chemical; Le Châtelier's principle; equilibrium constants	Section 11.5, Sections 15.2, 15.4, Section 16.6
2. Quantitative treatment
—a. Equilibrium constants for gaseous reactions: Kp, Kc	Section 15.2
—b. Equilibrium constants for reactions in solution
——i. Constants for acids and bases; pK; pH	Section 16.3
——ii. Solubility-product constants and their application to precipitation and the dissolution of slightly soluble compounds	Section 17.4
——iii. Common ion effect; buffers; hydrolysis	Sections 17.1, 17.2, Section 16.11
D. Kinetics
1. Concept of rate of reaction	Section 14.2
2. Use of experimental data and graphical analysis to determine reactant order, rate constants, and reaction rate laws	Sections 14.3, 14.4
3. Effect of temperature change on rates	Section 14.5
4. Energy of activation; the role of catalysts	Sections 14.5, 14.7
5. The relationship between the rate-determining step and a mechanism	Section 14.6
E. Thermodynamics
1. State functions	Section 5.2, Section 19.1
2. First law: change in enthalpy; heat of formation; heat of reaction; Hess's law; heats of vaporization and fusion; calorimetry	Sections 5.6, 5.7, Section 19.0
3. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes	Section 13.1, Section 19.2
4. Relationship of change in free energy to equilibrium constants and electrode potentials	Section 7.8, Section 8.4

IV. Descriptive Chemistry

1. Chemical reactivity and products of chemical reactions	Section 3.2
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	Section 2.5, Sections 7.0, 7.1, 7.6, 7.7, 7.8
3. Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties).	Section 2.9,Section 25.1, 25.2, 25.3, 25.4, 25.5, 25.6, 25.7

V. Chemical Calculations

A. Percentage composition	Section 3.3
B. Empirical and molecular formulas from experimental data	Section 2.6, Section 3.5
C. Molar masses from gas density, freezing-point, and boiling-point measurements	Section 3.4, Section 10.5
D. Gas laws, including the ideal gas law, Dalton's law, and Graham's law	Section 10.4
E. Stoichiometric relations using the concept of the mole; titration calculations	Section 3.4, Section 4.6, Section 17.3
F. Mole fractions; molar and molal solutions	Section 13.4, Section 17.4
G. Faraday's law of electrolysis	Section 20.5
H. Equilibrium constants and their applications, including their use for simultaneous equilibria	Section 15.2, Section 16.6
I. Standard electrode potentials and their use; Nernst equation	Sections 20.3, 20.6
J. Thermodynamic and thermochemical calculations	Sections 5.1, 5.2, Sections 19.1, 19.2
K. Kinetics calculations	Sections 14.0, 14.1, 14.2, 14.3, 14.4, 14.5, 14.6, 14.7