Standard Course of Study :: Advanced Placement Chemistry

Objective 4.01

Analyze the various types of common chemical reactions

Oxidation number.
The role of the electron in oxidation-reduction.
Electrochemistry: electrolytic and galvanic cells; Faraday's laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions.

Objective 4.02

Apply the principles of stoichiometry

Ionic and molecular species present in chemical systems: net ionic equations.
Balancing of equations including those for redox reactions.
Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants.

Objective 4.03

Analyze systems in dynamic equilibrium

Concept of dynamic equilibrium, both physical and chemical; Le Chatelier's principle; equilibrium constants.
Quantitative treatment for gaseous reactions using Kp and Kc.
Quantitative treatment for reactions in solution Kc.
Quantitative treatment of for acids and bases; using Ka and Kb, pKa and pKb and pH.
Quantitative treatment for precipitation reactions and the dissolution of slightly soluble compounds using the solubility product constant, Ksp.
Common ion effect; buffers; hydrolysis.

Objective 4.04

Analyze chemical kinetics

Concept of rate of reaction.
Use of differential rate laws to determine order of reaction and rate constant from experimental data.
Effect of temperature change on rates.
Energy of activation; the role of catalysts.
The relationship between the rate-determining step and a mechanism.

Objective 4.05

Analyze chemical thermodynamics

State functions.
First law: change in enthalpy; heat of formation; heat of reaction; Hess's law; heats of vaporization and fusion; calorimetry.
Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes.
Relationship of change in free energy to equilibrium constants and electrode potentials.

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