Phu Xuan University Library
|
PXU E-LIB
Sign in
UM Rochester: CHEM 2333 General Chemistry II

External

UM Rochester: CHEM 2333 General Chemistry II

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.

Chemistry
Publisher
LibreTexts
Source
LibreTexts
License
CC BY-NC-SA
Language
EN
Category
Basic Sciences
Read online Download PDF (open licence)
Contents· 83 sections
  1. 1: Tools for quantitative chemistry
  2. 1.1: Chemistry in Context
  3. 1.2: Measurements
  4. 1.3: Mathematical Treatment of Measurement Results
  5. 1.4: Chemical Formulas
  6. 1.5: Chemical Nomenclature
  7. 1.6: Formula Mass and the Mole Concept
  8. 1.7: Molarity
  9. 1.8.0: Solutions and Colloids
  10. 1.8.1 Prelude to Solutions and Colloids
  11. 1.8.2 The Dissolution Process
  12. 1.8.3 Electrolytes
  13. 1.8.4 Solubility
  14. 1.9.0 : Fundamental Equilibrium Concepts
  15. 1.9.1 Prelude to Equilibrium
  16. 1.9.2 Chemical Equilibria
  17. 1.9.3 Equilibrium Constants
  18. 1.9.4 Shifting Equilibria - Le Châtelier’s Principle
  19. 1.9.5. Equilibrium Calculations
  20. 1.9.6 Fundamental Equilibrium Concepts (Exercises)
  21. 2: Acid-Base Equilibria
  22. 2.1: Brnsted-Lowry Acids and Bases
  23. 2.2: pH and pOH
  24. 2.3: Relative Strengths of Acids and Bases
  25. 2.4: Hydrolysis of Salt Solutions
  26. 2.5: Polyprotic Acids
  27. 2.6: Buffers
  28. 2.7: Acid-Base Titrations
  29. 2.8: Acid-Base Equilibria (Exercises)
  30. 2.9.0: Equilibria of Other Reaction Classes
  31. 2.9.1 Precipitation and Dissolution
  32. 2.9.2 Lewis Acids and Bases
  33. 2.9.3 Coupled Equilibria
  34. 2.9.4 Equilibria of Other Reaction Classes (Exercises)
  35. 3: Kinetics
  36. 3.01: Prelude to Kinetics
  37. 3.02: Chemical Reaction Rates
  38. 3.03: Factors Affecting Reaction Rates
  39. 3.04: Rate Laws
  40. 3.05: Integrated Rate Laws
  41. 3.06: Collision Theory
  42. 3.07: Reaction Mechanisms
  43. 3.08: Catalysis
  44. 3.09: Kinetics (Exercises)
  45. 3.9.0: Nuclear Chemistry
  46. 3.9.1 Nuclear Structure and Stability
  47. 3.9.2 Nuclear Equations
  48. 3.9.3 Radioactive Decay
  49. 3.9.4 Transmutation and Nuclear Energy
  50. 3.9.5 Uses of Radioisotopes
  51. 3.9.6 Biological Effects of Radiation
  52. 3.9.7 Nuclear Chemistry (Exercises)
  53. 4: Thermodynamics
  54. 4.1: Energy Basics
  55. 4.2: Calorimetry
  56. 4.3: Enthalpy
  57. 4.4: Thermochemistry (Exercises)
  58. 4.5: Spontaneity
  59. 4.6: Entropy
  60. 4.7: The Second and Third Laws of Thermodynamics
  61. 4.8: Gibbs Energy
  62. 4.9: Thermodynamics (Exercises)
  63. 5: Electrochemistry
  64. 5.1: Balancing Oxidation-Reduction Reactions
  65. 5.2: Galvanic Cells
  66. 5.3: Standard Reduction Potentials
  67. 5.4: The Nernst Equation
  68. 5.5: Batteries and Fuel Cells
  69. 5.6: Corrosion
  70. 5.7: Electrolysis
  71. 5.8: Electrochemistry (Exercises)
  72. 6: Advanced Theories of Covalent Bonding
  73. 6.1: Prelude to Covalent Bonding
  74. 6.2: Valence Bond Theory
  75. 6.3: Hybrid Atomic Orbitals
  76. 6.4: Multiple Bonds
  77. 6.5: Molecular Orbital Theory
  78. 6.6: Advanced Theories of Covalent Bonding (Exercises)
  79. 7: Transition Metals and Coordination Chemistry
  80. 7.1: Properties of Transition Metals and Their Compounds
  81. 7.2: Coordination Chemistry of Transition Metals
  82. 7.3: Optical and Magnetic Properties of Coordination Compounds
  83. 7.4: Transition Metals and Coordination Chemistry (Exercises)