UC Davis: Chem 2B General Chemistry II

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  1. AGENDA
  2. Text
  3. Front Matter
  4. TitlePage
  5. InfoPage
  6. Table of Contents
  7. Licensing
  8. Unit I: Fundamentals of Thermochemistry
  9. 7.1: The Nature of Energy
  10. 7.2: Heat
  11. 7.3: Heats of Reaction and Calorimetry
  12. 7.4: Work
  13. 7.5: The First Law of Thermodynamics
  14. 7.6: Heats of Reactions: ΔU and ΔH
  15. 7.7: Indirect Determination of ΔH: Hess's Law
  16. 7.8: Standard Enthalpies of Formation
  17. 7.9: Fuels as Sources of Energy
  18. 7.S: Temperature Conversions
  19. Unit II: States of Matter
  20. 12: Intermolecular Forces (Liquids and Solids)
  21. 12.1: Intermolecular Forces
  22. 12.2: Some Properties of Liquids
  23. 12.3: Some Properties of Solids
  24. 12.4: Phase Diagrams
  25. 12.5: Changes of State
  26. 12.5: Network Colvalent Solids and Ionic Solids
  27. 12.6: Crystal Structures
  28. 13: Solutions and their Physical Properties
  29. 13.1: Types of Solutions: Some Terminology
  30. 13.2: Solution Concentration
  31. 13.3: Intermolecular Forces and the Solution Process
  32. 13.4: Solution Formation and Equilibrium
  33. 13.5: Solubilities of Gases
  34. 13.6: Vapor Pressures of Solutions
  35. 13.7: Osmotic Pressure
  36. 13.8: Freezing-Point Depression and Boiling-Point Elevation of Nonelectrolyte Solutions
  37. 13.9: Solutions of Electrolytes
  38. 13.10: Colloidal Mixtures
  39. Unit III: Chemical Equilibria
  40. 14: Principles of Chemical Equilibria
  41. 15.1: Dynamic Equilibrium
  42. 15.2: The Equilibrium Constant Expression
  43. 15.3: Relationships Involving Equilibrium Constants
  44. 15.4: The Magnitude of an Equilibrium Constant
  45. 15.5: Factors That Affect Equilibrium
  46. 15.6: Altering Equilibrium Conditions: Le Châtelier’s Principle
  47. 15.7: Equilibrium Calculations: Some Illustrative Examples
  48. 15.S: The Quadratic Formula
  49. 17: Solubility and Complex-Ion Equilibria
  50. 17.1: Solubility Product Constant, Ksp
  51. 17.2: Relationship Between Solubility and Ksp
  52. 17.3: Common-Ion Effect in Solubility Equilibria
  53. 17.4: Limitations of the Ksp Concept
  54. 17.5: Criteria for Precipitation and its Completeness
  55. 17.6: Fractional Precipitation
  56. 17.7: Solubility and pH
  57. 17.8: Equilibria Involving Complex Ions
  58. 17.9: Qualitative Cation Analysis
  59. Unit IV: Acids and Bases
  60. 15: Acids and Bases
  61. 15.1: Arrhenius Theory: A Brief Review
  62. 15.2: Brønsted-Lowry Theory of Acids and Bases
  63. 15.3: Self-Ionization of Water and the pH Scale
  64. 15.4: Strong Acids and Strong Bases
  65. 15.5: Weak Acids and Weak Bases
  66. 15.6: Polyprotic Acids
  67. 15.7: Ions as Acids and Bases
  68. 15.8: Molecular Structure and Acid-Base Behavior
  69. 15.9: Lewis Acids and Bases
  70. 16: Additional Aspects of Acid-Base Equilibria
  71. 16.1: Common-Ion Effect in Acid–Base Equilibria
  72. 16.2: Buffer Solutions
  73. 16.3: Acid–Base Indicators
  74. 16.4: Neutralization Reactions and Titration Curves
  75. 16.5: Solutions of Salts of Polyprotic Acids
  76. 16.6: Acid–Base Equilibrium Calculations: ASummary
  77. Unit V: Principles of Thermodynamics
  78. 18.1: Spontaneity: The Meaning of Spontaneous Change
  79. 18.2: The Concept of Entropy
  80. 18.3: Evaluating Entropy and Entropy Changes
  81. 18.4: Criteria for Spontaneous Change: The Second Law of Thermodynamics
  82. 18.5: Standard Gibbs Energy Change, ΔG°
  83. 18.6: Gibbs Energy Change and Equilibrium
  84. 18.7: ΔG° and K as Functions of Temperature
  85. 18.8: Coupled Reactions
  86. Back Matter
  87. Index
  88. Glossary
  89. Detailed Licensing
  90. Exam Reviews
  91. Videos
  92. 00: Front Matter
  93. Table of Contents