Chemical Principles

by Ta-Wei Li

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Study of the essential principles of chemistry including atomic and molecular science, states of matter, thermodynamics, chemical equilibrium, and reaction kinetics, which constitutes the foundation of modern chemistry.

Description from LibreTexts.

Publisher
National Yang Ming Chiao Tung University
Subjects
Chemistry
Licence
CC BY-SA 3.0, as LibreTexts states it
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: Electronic Structure of Atoms
  7. 1.1: The Wave Nature of Light
  8. 1.2: Quantized Energy and Photons
  9. 1.3: Line Spectra and the Bohr Model
  10. 1.4: The Wave Behavior of Matter
  11. 1.5: Quantum Mechanics and Wavefunctions
  12. 1.6: The Schrödinger Wave Equation for the Hydrogen Atom
  13. 1.7: Many-Electron Atoms - Penetration and Shielding
  14. 1.8: Electron Configurations
  15. 1.9: Electron Configurations and the Periodic Table
  16. 1.E: Electronic Structure of Atoms (Exercises)
  17. 1.S: Electronic Structure of Atoms (Summary)
  18. 2: Periodic Properties of the Elements
  19. 2.1: Development of the Periodic Table
  20. 2.2: Shielding and Effective Nuclear Charge
  21. 2.3: Sizes of Atoms and Ions
  22. 2.4: Ionization Energy
  23. 2.5: Electron Affinities
  24. 2.E: Periodic Properties of the Elements (Exercises)
  25. 2.S: Periodic Properties of the Elements (Summary)
  26. 3: Basic Concepts of Chemical Bonding
  27. 3.1: Chemical Bonds, Lewis Symbols, and the Octet Rule
  28. 3.2: Ionic Bonding
  29. 3.3: Covalent Bonding
  30. 3.4: Bond Polarity and Electronegativity
  31. 3.5: Drawing Lewis Structures
  32. 3.6: Resonance Structures
  33. 3.7: Exceptions to the Octet Rule
  34. 3.8: Strength of Covalent Bonds
  35. 3.E: Basic Concepts of Chemical Bonding (Exercises)
  36. 3.S: Basic Concepts of Chemical Bonding (Summary)
  37. 4: Molecular Geometry and Bonding Theories
  38. 4.1: Molecular Shapes
  39. 4.2: The VSEPR Model
  40. 4.3: Molecular Shape and Molecular Polarity
  41. 4.4: Covalent Bonding and Orbital Overlap
  42. 4.5: Hybrid Orbitals
  43. 4.6: Multiple Bonds
  44. 4.7: Molecular Orbitals (Supplementary)
  45. 4.8: Second-Row Diatomic Molecules (Supplementary)
  46. 4.E: Exercises
  47. 4.S: Molecular Geometry and Bonding Theories (Summary)
  48. 5: Chemical Kinetics
  49. 5.1: Factors that Affect Reaction Rates
  50. 5.2: Reaction Rates
  51. 5.3: Concentration and Rates (Differential Rate Laws)
  52. 5.4: The Change of Concentration with Time (Integrated Rate Laws)
  53. 5.5: Temperature and Rate
  54. 5.6: Reaction Mechanisms 1 - Rate-Determining Step
  55. 5.7: Reaction Mechanisms 2 - Steady-State Approximation
  56. 5.8: Catalysis
  57. 5.E: Exercises
  58. 5.S: Chemical Kinetics (Summary)
  59. 6: Gases
  60. 6.1: Characteristics of Gases
  61. 6.2: Pressure
  62. 6.3: The Gas Laws
  63. 6.4: The Ideal Gas Equation
  64. 6.5: Further Applications of the Ideal-Gas Equations
  65. 6.6: Gas Mixtures and Partial Pressures
  66. 6.7: Kinetic-Molecular Theory
  67. 6.8: Molecular Effusion and Diffusion
  68. 6.9: Real Gases - Deviations from Ideal Behavior
  69. 6.E: Exercises
  70. 6.S: Gases (Summary)
  71. 7: Fundamentals of Thermochemistry (Heat and Enthalpy)
  72. 7.1: Systems, States and Processes
  73. 7.2: Heat as a Mechanism to Transfer Energy
  74. 7.3: Work as a Mechanism to Transfer Energy
  75. 7.4: The First Law of Thermodynamics
  76. 7.5: Heat Capacity and Calorimetry
  77. 7.6: Molecules as Energy Carriers and Converters
  78. 7.7: Heats of Reactions - ΔU and ΔH
  79. 7.8: Indirect Determination of ΔH - Hess's Law
  80. 7.9: Standard Enthalpies of Formation
  81. 7.E: Fundamentals of Thermochemistry (Exercises)
  82. 8: Principles of Thermodynamics (Entropy and Gibbs Energy)
  83. 8.1: The Nature of Spontaneous Processes
  84. 8.2: Entropy and Spontaneity - A Molecular Statistical Interpretation
  85. 8.3: Entropy and Heat - Experimental Basis of the Second Law of Thermodynamics
  86. 8.4: Entropy Changes and Spontaneity
  87. 8.5: Entropy Changes in Reversible Processes
  88. 8.6: Quantum States, Microstates, and Energy Spreading
  89. 8.7: The Third Law of Thermodynamics
  90. 8.8: Gibbs Energy
  91. 8.E: Principles of Thermodynamics (Exercises)
  92. 9: Chemical Equilibrium
  93. 9.1: The Nature of Chemical Equilibrium
  94. 9.2: The Empirical Law of Mass Action
  95. 9.3: Thermodynamic Description of the Equilibrium State
  96. 9.4: The Law of Mass Action for Related and Simultaneous Equilibria
  97. 9.5: Gas-Phase and Heterogeneous Reaction Equilibria
  98. 9.6: The Direction of Change in Chemical Reactions- Empirical Description
  99. 9.7: The Direction of Change in Chemical Reactions - Thermodynamic Explanation
  100. 9.8: Distribution between Immiscible Phases - Extraction and Separation Processes
  101. 9.E: Chemical Equilibrium (Exercises)
  102. 10: Electrochemistry (Supplementary)
  103. 10.1: Electrochemical Cells
  104. 10.2: The Gibbs Free Energy and Cell Voltage
  105. 10.3: Concentration Effects and the Nernst Equation
  106. 10.4: Batteries and Fuel Cells
  107. 10.5: Corrosion and Its Prevention
  108. 10.6: Electrolysis - A Deeper Look
  109. 10.E: Electrochemistry (Exercises)
  110. Back Matter
  111. A1: Periodic Table of the Elements
  112. A2: Standard Thermodynamic Quantities
  113. A3: Standard Reduction Potentials by Value
  114. A4: Standard Reduction Potentials by Element
  115. Index
  116. Glossary
  117. Detailed Licensing
  118. Detailed Licensing