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UC Davis: Chem 4B General Chemistry for Majors II
This text is designed for the second-semester general chemistry course honors course and has been developed to meet the scope and sequence of most general chemistry courses. The text materials covers three primary units: Thermodynamics, Physical Equilibria and Chemical Equilibria with seven Chapters. The organization was careful formulated to introduce enthalpy, entropy, and Gibbs energy, and then use these skills to understand physical and chemical equilibria.
- Author
- Delmar Larsen
- Publisher
- University of California, Davis
- Source
- LibreTexts
- License
- CC BY-NC-SA
- Language
- EN
- Category
- Basic Sciences
Contents· 73 sections
- Unit I: Chemical Thermodynamics
- I: Fundamentals of Thermochemistry (Heat and Enthalpy)
- 1.01: Systems States and Processes
- 1.02: Heat
- 1.03: Work
- 1.04: The First Law of Thermodynamics
- 1.05: Heat Capacity and Calorimetry
- 1.06: Molecules as Energy Carriers and Converters
- 1.07: Heats of Reactions - U and H
- 1.08: Indirect Determination of H - Hess's Law
- 1.09: Standard Enthalpies of Formation
- 1.10: Fuels as Sources of Energy
- 1.E: Fundamentals of Thermochemistry (Exercises)
- II: Principles of Thermodynamics (Entropy and Gibbs Energy)
- 2.01: The Nature of Spontaneous Processes
- 2.02: Entropy and Spontaneity: A Molecular Statistical Interpretation
- 2.03: Entropy and Heat: Experimental Basis of the Second Law of Thermodynamics
- 2.04: Entropy Changes and Spontaneity
- 2.05: Entropy Changes in Reversible Processes
- 2.06: Quantum states Microstates and Energy spreading in Reactions
- 2.07: The Third Law of Thermodynamics
- 2.08: Gibbs Energy
- 2.E: Principles of Thermodynamics (Exercises)
- Unit II: Physical Equilibria
- III: Solids Liquids and Phase Transitions
- 3.1: Bulk Properties of Gases Liquids and Solids - Molecular Interpretation
- 3.2: Intermolecular Forces - Origins in Molecular Structure
- 3.3: Intermolecular Forces in Liquids
- 3.4: Phase Equilibrium
- 3.5: Phase Transitions
- 3.6: Phase Diagrams
- 3.7: Clausius-Clapeyron Equation
- 3.8: The Solid State
- 3.9: Bonding in Metals
- 3.E: Solids Liquids and Phase Transitions (Exercises)
- IV: Solutions
- 4.0: Types of Solutions - Some Terminology
- 4.1: Composition of Solutions
- 4.2: Nature of Dissolved Species
- 4.3: Phase Equilibrium in Solutions - Nonvolatile Solutes
- 4.4: Phase Equilibrium in Solutions - Volatile Solutes
- 4.5: Separating Volatile Solutions - Distillation
- 4.6: Colloidal Suspensions
- 4.E: Solutions (Exercises)
- Unit III: Chemical Equilibria
- V: Chemical Equilibrium
- 5.1: The Nature of Chemical Equilibrium
- 5.2: The Empirical Law of Mass Action
- 5.3: Thermodynamic Description of the Equilibrium State
- 5.4: The Law of Mass Action for Related and Simultaneous Equilibria
- 5.5: Gas-Phase and Heterogeneous Reaction Equilibria
- 5.6: The Direction of Change in Chemical Reactions: Empirical Description
- 5.7: The Direction of Change in Chemical Reactions - Thermodynamic Explanation
- 5.8: Distribution between Immiscible Phases - Extraction and Separation Processes
- 5.E: Chemical Equilibrium (Exercises)
- VI: AcidBase Equilibria
- 6.01: Classifications of Acids and Bases
- 6.02: The Brnsted-Lowry Scheme
- 6.03: Acid and Base Strength
- 6.04: Equilibria Involving Weak Acids and Bases
- 6.05: Buffer Solutions
- 6.06: Acid-Base Titration Curves
- 6.07: Polyprotic Acids
- 6.08: A Deeper Look: Exact Treatment of Acid-Base Equilibria
- 6.09: Organic Acids and Bases: Structure and Reactivity
- 6.10: Lewis Bases as Nucleophilic Reactants in Organic Reactions
- VII: Solubility and Precipitation Equilibria
- 7.1: The Nature of Solubility Equilibria
- 7.2: Ionic Equilibria between Solids and Solutions
- 7.3: Precipitation and the Solubility Product
- 7.4: The Effects of pH on Solubility
- 7.5: Complex Ions and Solubility
- 7.6: A Deeper Look - Selective Precipitation of Ions