Chemistry: The Central Science Twelfth Edition, AP* Edition 2012

Transcription

1 A Correlation of The Central Science Twelfth Edition, AP* Edition 2012 to the AP* Chemistry Topics

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

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

4 4. Non-ideal behavior (qualitative aspects) SECTIONS: 13.6 III. Reactions A. Reaction types 1. Acid-base reactions; concepts of Arrhenius, Brønsted- Lowry and Lewis; coordination complexes; amphoterism SECTIONS: 4.3, 16.2, Precipitation reactions SECTIONS: Oxidation-reduction reactions SECTIONS: 4.4, 20.1 a. Oxidation number SECTIONS: 4.4, 8.5 b. The role of the electron in oxidation-reduction SECTIONS: 4.4 c. Electrochemistry: electrolytic and galvanic cells; Faraday s laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions B. Stoichiometry 1. Ionic and molecular species present in chemical systems: net ionic equations SECTIONS: 20.6 SECTIONS: Balancing of equations, including those for redox reactions SECTIONS: 3.1, 3.6, Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants C. Equilibrium 1. Concept of dynamic equilibrium, physical and chemical; Le Chatelier s principle; equilibrium constants SECTIONS: 2.6, 3.4, 3.5, 3.7, 10.4 SECTIONS: 11.5, 15.2, 15.4, Quantitative treatment a. Equilibrium constants for gaseous reactions: Kp, Kc SECTIONS: 15.2 b. Equilibrium constants for reactions in solution (1) Constants for acids and bases; pk; ph SECTIONS:

5 (2) Solubility product constants and their application to precipitation and the dissolution of slightly soluble compounds SECTIONS: 17.4 (3) Common ion effect; buffers; hydrolysis SECTIONS: 17.1, 17.2, D. Kinetics 1. Concept of rate of reaction SECTIONS: Use of experimental data and graphical analysis to determine reactant order, rate constants and reaction rate laws SECTIONS: 14.3, Effect of temperature change on rates SECTIONS: Energy of activation; the role of catalysts SECTIONS: 14.5, The relationship between the rate-determining step and a mechanism SECTIONS: 14.6 E. Thermodynamics 1. State functions SECTIONS: 5.2, First law: change in enthalpy; heat of formation; heat of reaction; Hess s law; heats of vaporization and fusion; calorimetry 3. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes 4. Relationship of change in free energy to equilibrium constants and electrode potentials SECTIONS: 5.6, 5.7, 19.0 SECTIONS: 13.1, 19.2 SECTIONS: 7.8, 8.4 IV. Descriptive Chemistry 1. Chemical reactivity and products of chemical reactions SECTIONS: 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 SECTIONS: 2.5, 7.0, 7.1, 7.6, 7.7, 7.8 4

6 3. Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties) SECTIONS: 2.9, 25.1, 25.2, 25.3, 25.4, 25.5, 25.6, 25.7 V. Chemical Calculations A. Percentage composition SECTIONS: 3.3 B. Empirical and molecular formulas from experimental data SECTIONS: 2.6, 3.5 C. Molar masses from gas density, freezing-point, and boiling- point measurements SECTIONS: 3.4, 10.5 D. Gas laws, including the ideal-gas law, Dalton s law, and Graham s law SECTIONS: 10.4 E. Stoichiometric relations using the concept of the mole; titration calculations SECTIONS: 3.4, 4.6, 17.3 F. Mole fractions; molar and molal solutions SECTIONS: 13.4, 17.4 G. Faraday s law of electrolysis SECTIONS: 20.5 H. Equilibrium constants and their applications, including their use for simultaneous equilibria SECTIONS: 15.2, 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, 19.1, 19.2 K. Kinetics calculations SECTIONS: 14.0, 14.1, 14.2, 14.3, 14.4, 14.5, 14.6,