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UC Davis: Chem 2B General Chemistry II

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UC Davis: Chem 2B General Chemistry II

Chemistry
Author
LibreTexts
Publisher
LibreTexts
Source
LibreTexts
License
CC BY-NC-SA
Language
EN
Category
Basic Sciences
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Contents· 82 sections
  1. AGENDA
  2. Exam Reviews
  3. Text
  4. Unit I: Fundamentals of Thermochemistry
  5. 7.1: The Nature of Energy
  6. 7.2: Heat
  7. 7.3: Heats of Reaction and Calorimetry
  8. 7.4: Work
  9. 7.5: The First Law of Thermodynamics
  10. 7.6: Heats of Reactions: U and H
  11. 7.7: Indirect Determination of H: Hess's Law
  12. 7.8: Standard Enthalpies of Formation
  13. 7.9: Fuels as Sources of Energy
  14. 7.S: Temperature Conversions
  15. Unit II: States of Matter
  16. 12: Intermolecular Forces (Liquids and Solids)
  17. 12.1: Intermolecular Forces
  18. 12.2: Some Properties of Liquids
  19. 12.3: Some Properties of Solids
  20. 12.4: Phase Diagrams
  21. 12.5: Changes of State
  22. 12.5: Network Colvalent Solids and Ionic Solids
  23. 12.6: Crystal Structures
  24. 13: Solutions and their Physical Properties
  25. 13.01: Types of Solutions: Some Terminology
  26. 13.02: Solution Concentration
  27. 13.03: Intermolecular Forces and the Solution Process
  28. 13.04: Solution Formation and Equilibrium
  29. 13.05: Solubilities of Gases
  30. 13.06: Vapor Pressures of Solutions
  31. 13.07: Osmotic Pressure
  32. 13.08: Freezing-Point Depression and Boiling-Point Elevation of Nonelectrolyte Solutions
  33. 13.09: Solutions of Electrolytes
  34. 13.10: Colloidal Mixtures
  35. Unit III: Chemical Equilibria
  36. 14: Principles of Chemical Equilibria
  37. 15.1: Dynamic Equilibrium
  38. 15.2: The Equilibrium Constant Expression
  39. 15.3: Relationships Involving Equilibrium Constants
  40. 15.4: The Magnitude of an Equilibrium Constant
  41. 15.5: Factors That Affect Equilibrium
  42. 15.6: Altering Equilibrium Conditions: Le Chateliers Principle
  43. 15.7: Equilibrium Calculations: Some Illustrative Examples
  44. 15.S: The Quadratic Formula
  45. 17: Solubility and Complex-Ion Equilibria
  46. 17.1: Solubility Product Constant Ksp
  47. 17.2: Relationship Between Solubility and Ksp
  48. 17.3: Common-Ion Effect in Solubility Equilibria
  49. 17.4: Limitations of the Ksp Concept
  50. 17.5: Criteria for Precipitation and its Completeness
  51. 17.6: Fractional Precipitation
  52. 17.7: Solubility and pH
  53. 17.8: Equilibria Involving Complex Ions
  54. 17.9: Qualitative Cation Analysis
  55. Unit IV: Acids and Bases
  56. 15: Acids and Bases
  57. 15.1: Arrhenius Theory: A Brief Review
  58. 15.2: Brnsted-Lowry Theory of Acids and Bases
  59. 15.3: Self-Ionization of Water and the pH Scale
  60. 15.4: Strong Acids and Strong Bases
  61. 15.5: Weak Acids and Weak Bases
  62. 15.6: Polyprotic Acids
  63. 15.7: Ions as Acids and Bases
  64. 15.8: Molecular Structure and Acid-Base Behavior
  65. 15.9: Lewis Acids and Bases
  66. 16: Additional Aspects of Acid-Base Equilibria
  67. 16.1: Common-Ion Effect in AcidBase Equilibria
  68. 16.2: Buffer Solutions
  69. 16.3: AcidBase Indicators
  70. 16.4: Neutralization Reactions and Titration Curves
  71. 16.5: Solutions of Salts of Polyprotic Acids
  72. 16.6: AcidBase Equilibrium Calculations: ASummary
  73. Unit V: Principles of Thermodynamics
  74. 18.1: Spontaneity: The Meaning of Spontaneous Change
  75. 18.2: The Concept of Entropy
  76. 18.3: Evaluating Entropy and Entropy Changes
  77. 18.4: Criteria for Spontaneous Change: The Second Law of Thermodynamics
  78. 18.5: Standard Gibbs Energy Change G
  79. 18.6: Gibbs Energy Change and Equilibrium
  80. 18.7: G and K as Functions of Temperature
  81. 18.8: Coupled Reactions
  82. Videos