Grand Rapids Community College: CHM 120 Survey of General Chemistry

by Thomas Neils

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Publisher
Grand Rapids Community College
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: Matter and Energy
  7. 1.1 The Terms of Science
  8. 1.2: A First Look at the Periodic Table
  9. 1.3: The Classification of Matter
  10. 1.4: A First Look at Energy
  11. 1.5: Making Measurements
  12. 1.6: Limits on Measurements
  13. 1.7: Dimensional Analysis
  14. 1.8: Matter, Measurement, and Problem Solving (Exercises)
  15. 2: Atomic Structure
  16. 2.1: Modern Atomic Theory and the Laws That Led to It
  17. 2.2 The Structure of the Atom
  18. 2.3 Molar Mass - Counting Atoms by Weighing Them
  19. 2.4 Nuclear Reactions
  20. 2.5 The Belt of Stability - Predicting the Type of Radioactivity
  21. 2.6 Half-lives and the Rate of Radioactive Decay
  22. 2.7 Mass Defect - The Source of Nuclear Energy
  23. 2.8 Nuclear Energy - Fission and Fusion
  24. 2.9 The Nature of Light
  25. 2.10 Quantum Mechanics and The Atom
  26. 2.11 Trends of the Periodic Table
  27. 2.12 Example Problems
  28. 3: Chemical Formulas and Bonding
  29. 3.1 An Atomic-Level Perspective of Ionic and Covalent Compounds
  30. 3.2 Composition of Compounds
  31. 3.3 Chemical Bonds
  32. 3.4 Ionic Compounds: Formulas and Names
  33. 3.5 Covalently-Bonded Species: Formulas and Names
  34. 3.6 Electronegativity and Bond Polarity
  35. 3.7 Lewis Structures
  36. 3.8 Resonance and Formal Charge Revisited
  37. 3.9 Exceptions to the Octet Rule
  38. 3.10 Shapes of Molecules - VSEPR Theory and Valence Bond Theory
  39. 3.11 Practice Problems
  40. 4: Intermolecular Forces, Phases, and Solutions
  41. 4.1 Water in Zero Gravity - an Introduction to Intermolecular Forces
  42. 4.2 Intermolecular Forces
  43. 4.3 Application of IMFs: Evaporation, Vapor Pressure, and Boiling Points
  44. 4.4: Intermolecular Forces in Action: Surface Tension, Viscosity, and Capillary Action
  45. 4.5: Solids, Liquids, and Gases: A Molecular Comparison
  46. 4.6 Phase Changes
  47. 4.7: Pressure: The Result of Particle Collisions
  48. 4.8: Gases
  49. 4.9 Solutions - What Mixes Together and Why
  50. 4.10 Factors Affecting Solubility
  51. 4.11 Suspensions and Colloids
  52. 4.12 Practice Problems
  53. Intermolecular Forces
  54. 5: The Numbers Game - Solutions and Stoichiometry
  55. 5.1 Expressing Solution Concentration
  56. 5.2 Types of Aqueous Solutions and Solubility
  57. 5.3 Colligative Properties and Freezing Point Depression and Boiling Point Elevation and Osmosis
  58. 5.4 Writing and Balancing Chemical Equations
  59. 5.4a Example How Much Carbon Dioxide
  60. 5.5 Limiting Reactant and Theoretical Yield and Percent Yield
  61. 5.6 Representing Aqueous Reactions Molecular and Ionic and Complete Ionic Equations
  62. 5.7 Chemical Reactions and Aqueous Reactions (Exercises)
  63. 6: Reaction Kinetics
  64. 6.1: Chemical Kinetics
  65. 6.2 The Effect of Concentration on Reaction Rate
  66. 6.3: Reaction Mechanisms
  67. 6.4: The Effect of Temperature on Reaction Rate
  68. 6.5 Catalysts
  69. 7: Equilibrium and Thermodynamics
  70. 7.1: The Concept of Dynamic Equilibrium
  71. 7.2 The Equilibrium Constant
  72. 7.3: Calculating the Equilibrium Constant From Measured Equilibrium Concentrations
  73. 7.4 Predicting the Direction of a Reaction
  74. 7.5 Le Châtelier’s Principle: How a System at Equilibrium Responds to Disturbances
  75. 7.6: The First Law of Thermodynamics
  76. 7.7: Enthalpy: The Heat Evolved in a Chemical Reaction at Constant Pressure
  77. 7.8 Quantifying Heat
  78. 7.9: Entropy and the Second Law of Thermodynamics
  79. 7.10: Gibbs Free Energy
  80. 7.11 Gibbs Free Energy and Equilibrium
  81. What we are studying
  82. 8: Acids and Bases
  83. 8.1: An Introduction to Acids and Bases
  84. 8.2: Brønsted-Lowry Acids and Bases
  85. 8.3 Lewis Acids and Bases
  86. 8.4: Acid Strength and the Acid Dissociation Constant (Ka)
  87. 8.5: Autoionization of Water and pH
  88. 8.6 - Finding the Hydronium Ion Concentration and pH of Strong and Weak Acid Solutions
  89. 8.7: The Acid-Base Properties of Ions and Salts
  90. 8.8: Buffers: Solutions That Resist pH Change
  91. 8.9 Buffer Capacity and Buffer Range
  92. 8.10: Lewis Acids and Bases
  93. 8.11: Acid/Base (Exercises)
  94. 9: Electrochemistry
  95. 9.1: Oxidation-Reduction Reactions
  96. 9.2: Standard Reduction Potentials
  97. 9.3 Cell Potential, Gibbs Free Energy, and Equilibrium
  98. 9.4: Batteries: Using Chemistry to Generate Electricity
  99. 9.5 Driving Reactant-Favored Reactions Using Electricity
  100. 9.6 Undesirable Redox Reactions
  101. Back Matter
  102. Index
  103. Glossary
  104. Detailed Licensing