Phu Xuan University Library
|
PXU E-LIB
Sign in
Grand Rapids Community College: CHM 120 Survey of General Chemistry

External

Grand Rapids Community College: CHM 120 Survey of General Chemistry

Chemistry
Author
Thomas Neils
Publisher
Grand Rapids Community College
Source
LibreTexts
License
CC BY-NC-SA
Language
EN
Category
Basic Sciences
Read online Download PDF (open licence)
Contents· 95 sections
  1. 1: Matter and Energy
  2. 1.1 The Terms of Science
  3. 1.2: A First Look at the Periodic Table
  4. 1.3: The Classification of Matter
  5. 1.4: A First Look at Energy
  6. 1.5: Making Measurements
  7. 1.6: Limits on Measurements
  8. 1.7: Dimensional Analysis
  9. 1.8: Matter, Measurement, and Problem Solving (Exercises)
  10. 2: Atomic Structure
  11. 2.01: Modern Atomic Theory and the Laws That Led to It
  12. 2.02 The Structure of the Atom
  13. 2.03: Molar Mass - Counting Atoms by Weighing Them
  14. 2.04: Types of Radioactivity
  15. 2.05: The Belt of Stability: Predicting the Type of Radioactivity
  16. 2.06 Half-lives and the Rate of Radioactive Decay
  17. 2.07 Mass Defect - The Source of Nuclear Energy
  18. 2.08: The Discovery of Fission: The Atomic Bomb and Nuclear Power
  19. 2.09: The Nature of Light
  20. 2.10: Quantum Mechanics and The Atom
  21. 2.11: Electron Configurations, Valence Electrons, and the Periodic Table
  22. 2.12 Example Problems
  23. 3: Chemical Formulas and Bonding
  24. 3.01: An Atomic-Level Perspective of Elements and Compounds
  25. 3.02: Composition of Compounds
  26. 3.03: Chemical Bonds
  27. 3.04: Ionic Compounds: Formulas and Names
  28. 3.05: Covalently-Bonded Species: Formulas and Names
  29. 3.05: Electronegativity and Bond Polarity
  30. 3.06: Lewis Structures
  31. 3.07: Resonance and Formal Charge
  32. 3.08: Exceptions to the Octet Rule
  33. 3.10 Valence Bond Theory: Hybridization of Atomic Orbitals
  34. 3.12: Practice Problems
  35. 4: Intermolecular Forces Phases and Solutions
  36. 4.01: Water in Zero Gravity - an Introduction to Intermolecular Forces
  37. 4.02 Intermolecular Forces
  38. 4.03 An Application of IMFs: Evaporation Vapor Pressure and Boiling Points
  39. 4.04: Intermolecular Forces in Action: Surface Tension Viscosity and Capillary Action
  40. 4.05: Solids Liquids and Gases: A Molecular Comparison
  41. 4.06 Phase Changes
  42. 4.07: Pressure: The Result of Particle Collisions
  43. 4.08: Gases
  44. 4.09 Solutions - What Mixes Together and Why
  45. 4.10 Factors Affecting Solubility
  46. 4.11 Solutions Part 1
  47. 4.12 Practice Problems
  48. Intermolecular Forces
  49. 5: The Numbers Game - Solutions and Stoichiometry
  50. 5.1: Expressing Solution Concentration
  51. 5.2: Types of Aqueous Solutions and Solubility
  52. 5.3 Colligative Properties: Freezing Point Depression, Boiling Point Elevation, and Osmosis
  53. 5.4 Writing and Balancing Chemical Equations
  54. 5.4a Example How Much Carbon Dioxide?
  55. 5.5 Limiting Reactant, Theoretical Yield, and Percent Yield
  56. 5.6 Representing Aqueous Reactions: Molecular, Ionic, and Complete Ionic Equations
  57. 5.7 Chemical Reactions and Aqueous Reactions (Exercises)
  58. 6: Reaction Kinetics
  59. 6.01: Chemical Kinetics
  60. 6.02 The Effect of Concentration on Reaction Rate
  61. 6.03: Reaction Mechanisms
  62. 6.04: The Effect of Temperature on Reaction Rate
  63. 6.05 Catalysts
  64. 7: Equilibrium and Thermodynamics
  65. 7.01: The Concept of Dynamic Equilibrium
  66. 7.02 The Equilibrium Constant
  67. 7.03: Calculating the Equilibrium Constant From Measured Equilibrium Concentrations
  68. 7.04 Predicting the direction of a reaction
  69. 7.05\(:\) Le Châtelier’s Principle: How a System at Equilibrium Responds to Disturbances
  70. 7.06: The First Law of Thermodynamics
  71. 7.07: Enthalpy: The Heat Evolved in a Chemical Reaction at Constant Pressure
  72. 7.08 Quantifying Heat
  73. 7.09: Entropy and the Second Law of Thermodynamics
  74. 7.10: Gibbs Free Energy
  75. 7.11: Gibbs Free Energy and Equilibrium
  76. What we are studying
  77. 8: Acids and Bases
  78. 8.01: An Introduction to Acids and Bases
  79. 8.02: Brønsted-Lowry Acids and Bases
  80. 8.03 Lewis Acids and Bases
  81. 8.04: Acid Strength and the Acid Dissociation Constant (Ka)
  82. 8.05: Autoionization of Water and pH
  83. 8.06: Finding the Hydronium Ion Concentration and pH of Strong and Weak Acid Solutions
  84. 8.07: The Acid-Base Properties of Ions and Salts
  85. 8.08: Buffers: Solutions That Resist pH Change
  86. 8.09 Buffer Capacity and Buffer Range
  87. 8.10: Lewis Acids and Bases
  88. 8.11: Acid Base (Exercises)
  89. 9: Electrochemistry
  90. 9.1: Oxidation-Reduction Reactions
  91. 9.2: Standard Reduction Potentials
  92. 9.3 Cell Potential, Gibbs Free Energy, and Equilibrium
  93. 9.4: Batteries: Using Chemistry to Generate Electricity
  94. 9.5 Driving ReactantFavored Reactions Using Electricity
  95. 9.6 Undesirable Redox Reactions