9 The Gaseous State
9.1 The Chemistry of Gases
9.2 Pressure and Temperature of Gases
9.3 The Ideal Gas Law
9.4 Mixtures of Gases
9.5 The Kinetic Theory of Gases
9.6 Real Gases: Intermolecular Forces
10 Solids, Liquids, and Phase Transitions
10.1 Bulk Properties of Gases, Liquids, and Solids: Molecular Interpretation
10.2 Intermolecular Forces: Origins in Molecular Structure
10.3 Intermolecular Forces in Liquids
10.4 Phase Equilibrium
10.5 Phase Transitions
10.6 Phase Diagrams
11 Solutions
11.1 Composition of Solutions
11.2 Nature of Dissolved Species
11.3 Reaction Stoichiometry in Solutions: Acid–Base Titrations
11.4 Reaction Stoichiometry in Solutions: Oxidation– Reduction Titrations
11.5 Phase Equilibrium in Solutions: Nonvolatile Solutes
11.6 Phase Equilibrium in Solutions: Volatile Solutes
11.7 Colloidal Suspensions
12 Thermodynamic Processes and Thermochemistry
12.1 Systems, States, and Processes
12.2 The First Law of Thermodynamics: Internal Energy, Work, and Heat
12.3 Heat Capacity, Calorimetry, and Enthalpy
12.4 The First Law and Ideal Gas Processes
12.5 Molecular Contributions to Internal Energy and Heat Capacity
12.6 Thermochemistry
12.7 Reversible Processes in Ideal Gases
13 Spontaneous Processes and Thermodynamic Equilibrium
13.1 The Nature of Spontaneous Processes
13.2 Entropy and Spontaneity: A Molecular Statistical Interpretation
13.3 Entropy and Heat: Macroscopic Basis of the Second Law of
Thermodynamics
13.4 Entropy Changes in Reversible Processes
13.5 Entropy Changes and Spontaneity
13.6 The Third Law of Thermodynamics
13.7 The Gibbs Free Energy
14 Chemical Equilibrium
14.1 The Nature of Chemical Equilibrium
14.2 The Empirical Law of Mass Action
14.3 Thermodynamic Description of the Equilibrium State
14.4 The Law of Mass Action for Related and Simultaneous Equilibria
14.5 Equilibrium Calculations for Gas-Phase and Heterogeneous Reactions
14.6 The Direction of Change in Chemical Reactions: Empirical Description
14.7 The Direction of Change in Chemical Reactions: Thermodynamic
Explanation
14.8 Distribution of a Single Species between Immiscible Phases: Extraction and
Separation Processes
15 Acid–Base Equilibria
15.1 Classifications of Acids and Bases
15.2 Properties of Acids and Bases in Aqueous Solutions: The Brønsted–Lowry
Scheme
15.3 Acid and Base Strength
15.4 Equilibria Involving Weak Acids and Bases
15.5 Buffer Solutions
15.6 Acid–Base Titration Curves
15.7 Polyprotic Acids
15.8 Organic Acids and Bases: Structure and Reactivity
16 Solubility and Precipitation Equilibria
16.1 The Nature of Solubility Equilibria
16.2 Ionic Equilibria between Solids and Solutions
16.3 Precipitation and the Solubility Product
16.4 The Effects of pH on Solubility
16.5 Complex Ions and Solubility
17 Electrochemistry
17.1 Electrochemical Cells
17.2 Cell Potentials and the Gibbs Free Energy
17.3 Concentration Effects and the Nernst Equation
17.4 Molecular Electrochemistry
17.5 Batteries and Fuel Cell
17.6 Corrosion and Corrosion Prevention
17.7 Electrometallurgy
18 Chemical Kinetics
18.1 Rates of Chemical Reactions
18.2 Rate Laws
18.3 Reaction Mechanisms
18.4 Reaction Mechanisms and Rate
18.5 Effect of Temperature on Reaction Rates
18.6 Molecular Theories of Elementary Reactions
18.7 Reactions in Solution
18.8 Catalysis
19 Nuclear Chemistry
19.1 Mass–Energy Relationships in Nuclei
19.2 Nuclear Decay Processes
19.3 Kinetics of Radioactive Decay
19.4 Radiation in Biology and Medicine
19.5 Nuclear Fission
19.6 Nuclear Fusion and Nucleosynthesis
20 Molecular Spectroscopy and Photochemistry
20.1 Introduction to Molecular Spectroscopy
20.2 Experimental Methods in Molecular Spectroscopy
20.3 Rotational and Vibrational Spectroscopy
20.4 Nuclear Magnetic Resonance Spectroscopy
20.5 Electronic Spectroscopy and Excited State Relaxation Processes
20.6 Introduction to Atmospheric Chemistry
20.7 Photosynthesis

評分方式
Midterm exam + Final exam + Quiz