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CHEM 130: General Chemistry I

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CHEM 130: General Chemistry I

This course seeks to develop a working knowledge of the conceptual foundation and the quantitative chemical relationships on which subsequent chemistry courses are built. Atomic structure, chemical bonding, reaction stoichiometry, thermochemistry, and periodic trends are emphasized in this integrated lecture and laboratory course.

Chemistry
Author
Dr. Lisa Sharpe Elles
Publisher
University of Kansas
Source
LibreTexts
License
CC BY
Language
EN
Category
Basic Sciences
Read online Download PDF (open licence)
Contents· 200 sections
  1. 01: Essential Ideas of Chemistry
  2. 1.00: Introduction
  3. 1.01: Chemistry in Context
  4. 1.02: Phases and Classification of Matter
  5. 1.03: Physical and Chemical Properties
  6. 1.04: Measurements
  7. 1.05: Measurement Uncertainty Accuracy and Precision
  8. 1.06: Mathematical Treatment of Measurement Results
  9. 1.07: Summary
  10. 1.08: Exercises
  11. 02: Atoms Molecules and Ions
  12. 2.00: Introduction
  13. 2.01: Early Ideas in Atomic Theory
  14. 2.02: Evolution of Atomic Theory
  15. 2.03: Atomic Structure and Symbolism
  16. 2.04: The Periodic Table
  17. 2.05: Chemical Formulas
  18. 2.06: Formula Mass and the Mole Concept
  19. 2.07: Summary
  20. 2.08: Exercises
  21. 03: Electronic Structure and Periodic Properties
  22. 3.00: Introduction
  23. 3.01: Light and Electromagnetic Energy
  24. 3.02: The Bohr Model
  25. 3.03: Development of Quantum Theory
  26. 3.04: Electronic Structure of Atoms (Electron Configurations)
  27. 3.05: Periodic Variations in Element Properties
  28. 3.06: Ionic and Molecular Compounds
  29. 3.07: Summary
  30. 3.08: Exercises
  31. 04: Chemical Bonding and Molecular Geometry
  32. 4.00: Introduction
  33. 4.01: Ionic Bonding
  34. 4.02: Covalent Bonding
  35. 4.03: Chemical Nomenclature
  36. 4.04: Lewis Symbols and Structures
  37. 4.05: Formal Charges and Resonance
  38. 4.06: Molecular Structure and Polarity
  39. 4.07: Summary
  40. 4.08: Exercises
  41. 05: Advanced Theories of Covalent Bonding
  42. 5.00: Introduction
  43. 5.01: Valence Bond Theory
  44. 5.02: Hybrid Atomic Orbitals
  45. 5.03: Multiple Bonds
  46. 5.04: Molecular Orbital Theory
  47. 5.05: Summary
  48. 5.06: Exercises
  49. 06: Stoichiometry of Chemical Reactions
  50. 6.00: Introduction
  51. 6.01: Writing and Balancing Chemical Equations
  52. 6.02: Classifying Chemical Reactions
  53. 6.03: Reaction Stoichiometry
  54. 6.04: Reaction Yields
  55. 6.05: Summary
  56. 6.06: Exercises
  57. 07: Reactions in Aqueous Solution
  58. 7.00: Introduction
  59. 7.01: General Properties of Aqueous Solutions
  60. 7.02: Precipitation Reactions
  61. 7.03: Oxidation-Reduction Reactions
  62. 7.04: Concentration of Solutions
  63. 7.05: Stoichiometry of Reactions in Solution
  64. 7.06: Summary
  65. 7.07: Exercises
  66. 08: Thermochemistry
  67. 8.00: Introduction
  68. 8.01: Energy Basics
  69. 8.02: Calorimetry
  70. 8.03: Enthalpy
  71. 8.04: Strengths of Ionic and Covalent Bonds
  72. 8.05: Summary
  73. 8.06: Exercises
  74. 09: Gases
  75. 9.00: Introduction
  76. 9.01: Gas Pressure
  77. 9.02: Relating Pressure Volume Amount and Temperature- The Ideal Gas Law
  78. 9.03: Stoichiometry of Gaseous Substances Mixtures and Reactions
  79. 9.04: Effusion and Diffusion of Gases
  80. 9.05: The Kinetic-Molecular Theory
  81. 9.06: Non-Ideal Gas Behavior
  82. 9.07: Key Terms
  83. 9.08: Key Equations
  84. 9.09: Summary
  85. 9.10: Exercises
  86. 10: Liquids and Solids
  87. 10.00: Introduction
  88. 10.01: Intermolecular Forces
  89. 10.02: Properties of Liquids
  90. 10.03: Phase Transitions
  91. 10.04: Phase Diagrams
  92. 10.05: The Solid State of Matter
  93. 10.06: Lattice Structures in Crystalline Solids
  94. 10.07: Key Terms
  95. 10.08: Key Equations
  96. 10.09: Summary
  97. 10.10: Exercises
  98. 11: Solutions and Colloids
  99. 11.00: Introduction
  100. 11.01: The Dissolution Process
  101. 11.02: Electrolytes
  102. 11.03: Solubility
  103. 11.04: Ways of Expressing Concentration
  104. 11.05: Colligative Properties
  105. 11.06: Colloids
  106. 11.07: Key Terms
  107. 11.08: Key Equations
  108. 11.09: Summary
  109. 11.10: Exercises
  110. 12: Chemical Kinetics
  111. 12.00: Introduction
  112. 12.01: Factors that Affect Reaction Rates
  113. 12.02: Reaction Rates
  114. 12.03: Concentration and Rates (Differential Rate Laws)
  115. 12.04: The Change of Concentration with Time (Integrated Rate Laws)
  116. 12.05: Temperature and Rate
  117. 12.06: Reaction Mechanisms
  118. 12.07: Catalysis
  119. 12.E: Exercises
  120. 12.S: Chemical Kinetics (Summary)
  121. 13: Chemical Equilibrium
  122. 13.00: Introduction
  123. 13.01: The Concept of Equilibrium
  124. 13.02: The Equilibrium Constant
  125. 13.03: Interpreting and Working with Equilibrium Constants
  126. 13.04: Heterogeneous Equilibria
  127. 13.05: Calculating Equilibrium Constants
  128. 13.06: Applications of Equilibrium Constants
  129. 13.07: Le Chatelier's Principle
  130. 13.E: Exercises
  131. 13.S: Chemical Equilibrium (Summary)
  132. 14: Acid-Base Equilibria
  133. 14.00: Introduction
  134. 14.01: Acids and Bases - A Brief Review
  135. 14.02: Brnsted-Lowry Acids and Bases
  136. 14.03: pH and pOH
  137. 14.04: Relative Strengths of Acids and Bases
  138. 14.05: Hydrolysis of Salt Solutions
  139. 14.06: Polyprotic Acids
  140. 14.07: Key Terms
  141. 14.08: Key Equations
  142. 14.09: Summary
  143. 14.10: Exercises
  144. 15: Equilibria of Other Reaction Classes
  145. 15.00: Introduction
  146. 15.01: The Common-Ion Effect
  147. 15.02: Buffers
  148. 15.03: Acid-Base Titrations
  149. 15.04: Precipitation and Dissolution
  150. 15.05: Lewis Acids and Bases
  151. 15.06: Coupled Equilibria
  152. 15.07: Key Terms
  153. 15.08: Key Equations
  154. 15.09: Summary
  155. 15.10: Exercises
  156. 16: Chemical Thermodynamics
  157. 16.00: Spontaneous Processes
  158. 16.01: Entropy and the Second Law of Thermodynamics
  159. 16.02: The Molecular Interpretation of Entropy
  160. 16.03: Entropy Changes in Chemical Reactions
  161. 16.04: Gibbs Free Energy
  162. 16.05: Free Energy and Temperature
  163. 16.06: Free Energy and the Equilibrium Constant
  164. 16.E: Chemical Thermodynamics (Exercises)
  165. 17: Appendices
  166. 17.00: The Periodic Table
  167. 17.01: Essential Mathematics
  168. 17.02: Units and Conversion Factors
  169. 17.03: Fundamental Physical Constants
  170. 17.04: Water Properties
  171. 17.05: Composition of Commercial Acids and Bases
  172. 17.06: Standard Thermodynamic Properties for Selected Substances
  173. 17.07: Ionization Constants of Weak Acids
  174. 17.08: Ionization Constants of Weak Bases
  175. 17.09: Solubility Products
  176. 17.10: Formation Constants for Complex Ions
  177. 17.11: Standard Electrode (Half-Cell) Potentials
  178. 17.12: Half-Lives for Several Radioactive Isotopes
  179. 17.13: Answer Key
  180. 17.13.00: Chapter 1
  181. 17.13.01: Chapter 2
  182. 17.13.02: Chapter 3
  183. 17.13.03: Chapter 4
  184. 17.13.04: Chapter 5
  185. 17.13.05: Chapter 6
  186. 17.13.06: Chapter 7
  187. 17.13.07: Chapter 8
  188. 17.13.08: Chapter 9
  189. 17.13.09: Chapter 10
  190. 17.13.10: Chapter 11
  191. 17.13.11: Chapter 12
  192. 17.13.12: Chapter 13
  193. 17.13.13: Chapter 14
  194. 17.13.14: Chapter 15
  195. 17.13.15: Chapter 16
  196. 17.13.16: Chapter 17
  197. 17.13.17: Chapter 18
  198. 17.13.18: Chapter 19
  199. 17.13.19: Chapter 20
  200. 17.13.20: Chapter 21