UM Rochester: CHEM 2333 General Chemistry II

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This is the second semester of General Chemistry at the University of Minnesota Rochester. Given that students at UMR have already taken at least one semester in Organic Chemistry before enrolling in General Chemistry, this course already assumes knowledge of inorganic and organic chemical structures as well as chemical equilibrium concepts.

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Subjects
Chemistry
Licence
CC BY-NC-SA 4.0, as LibreTexts states it. Non-commercial use only.
Who can read
Tweens profiles and older, judged from its title and subjects

Contents

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  1. Front Matter
  2. TitlePage
  3. InfoPage
  4. Table of Contents
  5. Licensing
  6. 1: Tools for quantitative chemistry
  7. 1.1: Chemistry in Context
  8. 1.2: Measurements
  9. 1.3: Mathematical Treatment of Measurement Results
  10. 1.4: Chemical Formulas
  11. 1.5: Chemical Nomenclature
  12. 1.6: Formula Mass and the Mole Concept
  13. 1.7: Molarity
  14. 1.8.0: Solutions and Colloids
  15. 1.8.1 Prelude to Solutions and Colloids
  16. 1.8.2 The Dissolution Process
  17. 1.8.3 Electrolytes
  18. 1.8.4 Solubility
  19. 1.9.0 : Fundamental Equilibrium Concepts
  20. 1.9.1 Prelude to Equilibrium
  21. 1.9.2 Chemical Equilibria
  22. 1.9.3 Equilibrium Constants
  23. 1.9.4 Shifting Equilibria - Le Châtelier’s Principle
  24. 1.9.5. Equilibrium Calculations
  25. 1.9.6 Fundamental Equilibrium Concepts (Exercises)
  26. 2: Acid-Base Equilibria
  27. 2.1: Brønsted-Lowry Acids and Bases
  28. 2.2: pH and pOH
  29. 2.3: Relative Strengths of Acids and Bases
  30. 2.4: Hydrolysis of Salt Solutions
  31. 2.5: Polyprotic Acids
  32. 2.6: Buffers
  33. 2.7: Acid-Base Titrations
  34. 2.8: Acid-Base Equilibria (Exercises)
  35. 2.9.0: Equilibria of Other Reaction Classes
  36. 2.9.1 Precipitation and Dissolution
  37. 2.9.2 Lewis Acids and Bases
  38. 2.9.3 Coupled Equilibria
  39. 2.9.4 Equilibria of Other Reaction Classes (Exercises)
  40. 3: Kinetics
  41. 3.1: Prelude to Kinetics
  42. 3.2: Chemical Reaction Rates
  43. 3.3: Factors Affecting Reaction Rates
  44. 3.4: Rate Laws
  45. 3.5: Integrated Rate Laws
  46. 3.6: Collision Theory
  47. 3.7: Reaction Mechanisms
  48. 3.8: Catalysis
  49. 3.9.a: Kinetics (Exercises)
  50. 3.9.0: Nuclear Chemistry
  51. 3.9.1 Nuclear Structure and Stability
  52. 3.9.2 Nuclear Equations
  53. 3.9.3 Radioactive Decay
  54. 3.9.4 Transmutation and Nuclear Energy
  55. 3.9.5 Uses of Radioisotopes
  56. 3.9.6 Biological Effects of Radiation
  57. 3.9.7 Nuclear Chemistry (Exercises)
  58. 4: Thermodynamics
  59. 4.1: Energy Basics
  60. 4.2: Calorimetry
  61. 4.3: Enthalpy
  62. 4.4: Thermochemistry (Exercises)
  63. 4.5: Spontaneity
  64. 4.6: Entropy
  65. 4.7: The Second and Third Laws of Thermodynamics
  66. 4.8: Gibbs Energy
  67. 4.9: Thermodynamics (Exercises)
  68. 5: Electrochemistry
  69. 5.1: Balancing Oxidation-Reduction Reactions
  70. 5.2: Galvanic Cells
  71. 5.3: Standard Reduction Potentials
  72. 5.4: The Nernst Equation
  73. 5.5: Batteries and Fuel Cells
  74. 5.6: Corrosion
  75. 5.7: Electrolysis
  76. 5.8: Electrochemistry (Exercises)
  77. 6: Advanced Theories of Covalent Bonding
  78. 6.1: Prelude to Covalent Bonding
  79. 6.2: Valence Bond Theory
  80. 6.3: Hybrid Atomic Orbitals
  81. 6.4: Multiple Bonds
  82. 6.5: Molecular Orbital Theory
  83. 6.6: Advanced Theories of Covalent Bonding (Exercises)
  84. 7: Transition Metals and Coordination Chemistry
  85. 7.1: Properties of Transition Metals and Their Compounds
  86. 7.2: Coordination Chemistry of Transition Metals
  87. 7.3: Optical and Magnetic Properties of Coordination Compounds
  88. 7.4: Transition Metals and Coordination Chemistry (Exercises)
  89. Back Matter
  90. Index
  91. Glossary
  92. Detailed Licensing