TRU: Fundamentals and Principles of Chemistry (CHEM 1510 and CHEM 1520)

by Sharon Brewer and Lindsay Blackstock

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This is the remix textbook to accompany both CHEM 1510 (Fundamentals of Chemistry) and CHEM 1520 (Principles of Chemistry at Thompson Rivers University. These are the second single semester courses in general chemistry.

Description from LibreTexts.

Publisher
Thompson Rivers University
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

LibreTexts writes equations in TeX, and here they show as TeX; the PDF has them typeset.

  1. Front Matter
  2. TitlePage
  3. InfoPage
  4. Table of Contents
  5. Licensing
  6. 1: Background
  7. 1.1: Essential Ideas of Chemistry
  8. 1.1.1: Chemistry in Context
  9. 1.1.2: Phases and Classification of Matter
  10. 1.1.3: Physical and Chemical Properties
  11. 1.1.4: Measurements
  12. 1.1.5: Measurement Uncertainty, Accuracy, and Precision
  13. 1.1.6: Mathematical Treatment of Measurement Results
  14. 1.1.7: How to Solve Chemistry Problems
  15. 1.1.E: Essential Ideas of Chemistry (Exercises)
  16. 1.1.S: Essential ideas of Chemistry (Study Guide)
  17. 1.2: Atoms, Molecules, and Ions
  18. 1.2.1: Prelude to Atoms
  19. 1.2.2: Early Ideas in Atomic Theory
  20. 1.2.3: Evolution of Atomic Theory
  21. 1.2.4: Atomic Structure and Symbolism
  22. 1.2.5: Chemical Formulas
  23. 1.2.6: The Periodic Table
  24. 1.2.7: Molecular and Ionic Compounds
  25. 1.2.8: Chemical Nomenclature
  26. 1.2.E: Atoms, Molecules, and Ions (Exercises)
  27. 1.2.S: Atoms, Molecules, and Ions (Study Guide)
  28. 1.3: Composition of Substances and Solutions
  29. 1.3.1: Formula Mass and the Mole Concept
  30. 1.3.2: Determining Empirical and Molecular Formulas
  31. 1.3.3: Molarity
  32. 1.3.4: Other Units for Solution Concentrations
  33. 1.3.5: Composition of Substances and Solutions (Study Guide)
  34. 1.3.E: Composition of Substances and Solutions (Exercises)
  35. 1.4: Stoichiometry of Chemical Reactions
  36. 1.4.1: Prelude to Stoichiometry
  37. 1.4.2: Writing and Balancing Chemical Equations
  38. 1.4.3: Classifying Chemical Reactions
  39. 1.4.4: Reaction Stoichiometry
  40. 1.4.5: Reaction Yields
  41. 1.4.6: Quantitative Chemical Analysis
  42. 1.4.E: Stoichiometry of Chemical Reactions (Exercises)
  43. 1.4.S: Stoichiometry of Chemical Reactions (Summary)
  44. 2: Gases
  45. 2.1: Characteristics of Gases
  46. 2.2: Gas Pressure
  47. 2.3: Relating Pressure, Volume, Amount, and Temperature - The Ideal Gas Law
  48. 2.4: Stoichiometry of Gaseous Substances, Mixtures, and Reactions
  49. 2.5: The Kinetic-Molecular Theory
  50. 2.6: Effusion and Diffusion of Gases
  51. 2.7: Non-Ideal Gas Behavior
  52. 2.E: Gases (Exercises)
  53. 2.S: Gases (Study Guide)
  54. 3: Thermochemistry
  55. 3.1: The Nature of Energy
  56. 3.2: The First Law of Thermodynamics
  57. 3.3: Enthalpy
  58. 3.4: Enthalpy of Reaction
  59. 3.5: Calorimetry
  60. 3.6: Hess's Law
  61. 3.7: Enthalpies of Formation
  62. 3.8: Types of Solutions and Solubility
  63. 3.9: Foods and Fuels
  64. 3.E: Thermochemistry (Exercises)
  65. 3.S: Thermochemistry (Study Guide)
  66. 4: Kinetics
  67. 4.1: Prelude to Kinetics
  68. 4.2: Chemical Reaction Rates
  69. 4.3: Factors Affecting Reaction Rates
  70. 4.4: Rate Laws
  71. 4.5: Integrated Rate Laws
  72. 4.6: Collision Theory
  73. 4.7: Reaction Mechanisms
  74. 4.8: Catalysis
  75. 4.E: Kinetics (Exercises)
  76. 4.S: Kinetics (Study Guide)
  77. 5: Chemical Equilibrium
  78. 5.1: Prelude to Equilibrium
  79. 5.2: Chemical Equilibria
  80. 5.3: Equilibrium Constants
  81. 5.4: Equilibrium Calculations
  82. 5.5: Shifting Equilibria - Le Chatelier’s Principle
  83. 5.6: Applications of Equilibrium, Henry's Law
  84. 5.E: Fundamental Equilibrium Concepts (Exercises)
  85. 5.S: Fundamental Equilibrium Concepts (Study Guide)
  86. 6: Acid-Base Equilibrium
  87. 6.1: Brønsted-Lowry Acids and Bases
  88. 6.2: pH and pOH
  89. 6.3: Relative Strengths of Acids and Bases
  90. 6.4: Polyprotic Acids
  91. 6.5: Hydrolysis of Salt Solutions
  92. 6.6: Lewis Acids and Bases
  93. 6.E: Acid-Base Equilibrium (Exercises)
  94. 6.S: Acid–Base Equilibrium (Study Guide)
  95. 7: Buffers, Titrations and Solubility Equilibria
  96. 7.1: Acid-Base Buffers
  97. 7.2: Practical Aspects of Buffers
  98. 7.3: Acid-Base Titrations
  99. 7.4: Solving Titration Problems
  100. 7.5: Solubility Equilibria
  101. 7.E: Buffers, Titrations and Solubility Equilibria (Exercises)
  102. 7.S: Buffers, Titrations and Solubility Equilibria (Study Guide)
  103. 8: Entropy and Free Energy
  104. 8.1: Spontaneity
  105. 8.2: Entropy
  106. 8.3: The Second and Third Laws of Thermodynamics
  107. 8.4: Gibbs Free Energy
  108. 8.E: Entropy and Free Energy (Exercises)
  109. 8.S: Entropy and Free Energy (Study Guide)
  110. 9: Electrochemistry
  111. 9.1: Balancing Oxidation-Reduction Reactions
  112. 9.2: Galvanic Cells
  113. 9.3: Standard Reduction Potentials
  114. 9.4: The Nernst Equation
  115. 9.5: Batteries and Fuel Cells
  116. 9.6: Electrolysis
  117. 9.E: Exercises on Electrochemistry
  118. 9.S: Electrochemistry (Study Guide)
  119. Back Matter
  120. Index
  121. Glossary
  122. Detailed Licensing