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Chemistry 201: General Chemistry II

Nguồn ngoài

Chemistry 201: General Chemistry II

Emphasis is placed on the fundamental principles of physical and inorganic chemistry. Topics include techniques of data analysis, chemical kinetics, chemical equilibrium, acids, bases, and salts, thermochemistry, electrochemistry, coordination chemistry. Computer skills are introduced and applied to data analysis, laboratory simulations, and computer interfacing with laboratory equipment.

Chemistry
Tác giả
Fred Garces
Nhà xuất bản
San Diego Miramar College
Nguồn
LibreTexts
Ngôn ngữ
EN
Danh mục
Khoa học cơ bản
Đọc trực tuyến Tải PDF (nguồn mở)
Mục lục· 93 mục
  1. 01: Liquids Solids and Intermolecular Forces
  2. 1.01: Structure Determines Properties
  3. 1.02: Solids Liquids and Gases- A Molecular Comparison
  4. 1.03: Intermolecular Forces- The Forces that Hold Condensed Phases Together
  5. 1.04: Intermolecular Forces in Action- Surface Tension Viscosity and Capillary Action
  6. 1.05: Vaporization and Vapor Pressure
  7. 1.06: Sublimation and Fusion
  8. 1.07: Heating Curve for Water
  9. 1.08: Water - An Extraordinary Substance
  10. 02: Solutions
  11. 2.01: Types of Solutions and Solubility
  12. 2.02: Energetics of Solution Formation
  13. 2.03: Solution Equilibrium and Factors Affecting Solubility
  14. 2.04: Expressing Solution Concentration
  15. 2.05: Colligative Properties- Freezing Point Depression Boiling Point Elevation and Osmosis
  16. 2.06: The Colligative Properties of Strong Electrolyte Solutions
  17. 03: Chemical Kinetics
  18. 3.01: Catching Lizards
  19. 3.02: Rates of Reaction and the Particulate Nature of Matter
  20. 3.03: Defining and Measuring the Rate of a Chemical Reaction
  21. 3.04: The Rate Law- The Effect of Concentration on Reaction Rate
  22. 3.05: The Integrated Rate Law- The Dependence of Concentration on Time
  23. 3.06: The Effect of Temperature on Reaction Rate
  24. 3.07: Reaction Mechanisms
  25. 3.08: Catalysis
  26. 04: Chemical Equilibrium
  27. 4.01: Fetal Hemoglobin and Equilibrium
  28. 4.02: The Concept of Dynamic Equilibrium
  29. 4.03: The Equilibrium Constant (K)
  30. 4.04: Expressing the Equilibrium Constant in Terms of Pressure
  31. 4.05: Heterogenous Equilibria - Reactions Involving Solids and Liquids
  32. 4.06: The Reaction Quotient- Predicting the Direction of Change
  33. 4.07: Finding Equilibrium Concentrations
  34. 4.08: Le Chateliers Principle- How a System at Equilibrium Responds to Disturbances
  35. 4.09: Solubility Equilibria and the Solubility Product Constant
  36. 4.10: Precipitation
  37. 4.11: Complex Ion Equilibria
  38. 05: Acids and Bases
  39. 5.01: Batmans Basic Blunder
  40. 5.02: The Nature of Acids and Bases
  41. 5.03: Definitions of Acids and Bases
  42. 5.04: Acid Strength and Molecular Structure
  43. 5.05: Acid Strength and the Acid Ionization Constant (Ka)
  44. 5.06: Autoionization of Water and pH
  45. 5.07: Finding the H3O and pH of Strong and Weak Acid Solutions
  46. 5.08: Finding the OH- and pH of Strong and Weak Base Solutions
  47. 5.09: The Acid-Base Properties of Ions and Salts
  48. 5.10: Polyprotic Acids
  49. 5.11: Lewis Acids and Bases
  50. 5.12: The Danger of Antifreeze
  51. 5.13: Buffers- Solutions That Resist pH Change
  52. 5.14: Buffer Effectiveness- Buffer Capacity and Buffer Range
  53. 5.15: Titrations and pH Curves
  54. 06: Free Energy and Thermodynamics
  55. 6.01: Energy Spreads Out
  56. 6.02: Spontaneous and Nonspontaneous Processes
  57. 6.03: Entropy and the Second Law of Thermodynamics
  58. 6.04: Predicting Entropy and Entropy Changes for Chemical Reactions
  59. 6.05: Heat Transfer and Changes in the Entropy of the Surroundings
  60. 6.06: Gibbs Energy
  61. 6.07: Free Energy Changes in Chemical Reactions- Calculating
  62. 6.08: Free Energy Changes for Nonstandard States - The Relationship between and
  63. 6.09: Free Energy and Equilibrium- Relating to the Equilibrium Constant (K)
  64. 07: Electrochemistry
  65. 7.01: Lightning and Batteries
  66. 7.02: Balancing Oxidation-Reduction Equations
  67. 7.03: Voltaic (or Galvanic) Cells- Generating Electricity from Spontaneous Chemical Reactions
  68. 7.04: Standard Reduction Potentials
  69. 7.05: Cell Potential Gibbs Energy and the Equilibrium Constant
  70. 7.06: Cell Potential and Concentration
  71. 7.07: Batteries- Using Chemistry to Generate Electricity
  72. 7.08: Electrolysis- Driving Non-spontaneous Chemical Reactions with Electricity
  73. 7.09: Corrosion- Undesirable Redox Reactions
  74. 08: Transition Metals and Coordination Compounds
  75. 8.01: The Colors of Rubies and Emeralds
  76. 8.02: Properties of Transition Metals
  77. 8.03: Coordination Compounds
  78. 8.04: Structure and Isomerization
  79. 8.05: Bonding in Coordinate Compounds
  80. 8.06: Applications of Coordination Compounds
  81. 09: Radioactivity and Nuclear Chemistry
  82. 9.01: Diagnosing Appendicitis
  83. 9.02: The Discovery of Radioactivity
  84. 9.03: Types of Radioactivity
  85. 9.04: The Valley of Stability- Predicting the Type of Radioactivity
  86. 9.05: Detecting Radioactivity
  87. 9.06: The Kinetics of Radioactive Decay and Radiometric Dating
  88. 9.07: The Discovery of Fission- The Atomic Bomb and Nuclear Power
  89. 9.08: Converting Mass to Energy- Mass Defect and Nuclear Binding Energy
  90. 9.09: Nuclear Fusion - The Power of the Sun
  91. 9.10: Nuclear Transmutation and Transuranium Elements
  92. 9.11: The Effects of Radiation on Life
  93. 9.12: Radioactivity in Medicine and Other Applications