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Chem 321: Physical Chemistry I

Nguồn ngoài

Chem 321: Physical Chemistry I

This text is a introduction to thermodynamics and quantum chemistry. The macroscopic behavior of matter as embodied in thermodynamics and kinetics is correlated with the microscopic model of matter based on atomic-molecular theory.

Chemistry
Tác giả
Mary Crawford
Nhà xuất bản
Knox College
Nguồn
LibreTexts
Ngôn ngữ
EN
Danh mục
Khoa học cơ bản
Đọc trực tuyến Tải PDF (nguồn mở)
Mục lục· 88 mục
  1. 01: Enery Levels and Spectroscopy
  2. 1.01: Electromagnetic Radiation
  3. 1.02: The Wave Theory of Light
  4. 1.03: Bohr's Theory of the Hydrogen Emission Spectrum
  5. 1.04: Hydrogen's Atomic Emission Spectrum
  6. 1.05: The Schrodinger Wave Equation
  7. 1.06: Particle in a One-Dimensional Box
  8. 1.07: Electronic Spectroscopy
  9. 1.08: The Harmonic Oscillator Approximates Vibrations
  10. 1.09: The Harmonic Oscillator and Infrared Spectra
  11. 1.10: Microwave Spectroscopy
  12. 02: Atomic Structure
  13. 2.01: The Schrodinger Wave Equation for the Hydrogen Atom
  14. 2.02: Many-Electron Atoms and the Periodic Table
  15. 2.03: Quantum-Mechanical Tunneling
  16. 03: Chemical Bond
  17. 3.01: Lewis Structures
  18. 3.02: Valence Bond Theory
  19. 3.03: Hybridization of Atomic Orbitals
  20. 3.04: Molecular Orbital Theory
  21. 3.05: Diatomic Molecules
  22. 04: Gases
  23. 4.01: The Perfect Gas
  24. 4.02: Real Gases (Deviations From Ideal Behavior)
  25. 4.03: The Repulsive Term in the Lennard-Jones Potential
  26. 05: Boltzmann
  27. 5.01: The Boltzmann Factor
  28. 5.02: The Thermal Boltzman Distribution
  29. 5.03: The Average Ensemble Energy
  30. 5.04: Heat Capacity at Constant Volume
  31. 5.05: Partition Functions can be Decomposed
  32. 5.06: Translational Partition Functions of Monotonic Gases
  33. 5.07: Most Atoms are in the Ground Electronic State
  34. 5.08: The Energy of a Diatomic Molecule Can Be Approximated as a Sum of Separate Terms
  35. 5.09: Most Molecules are in the Ground Vibrational State
  36. 5.10: Most Molecules are Rotationally Excited at Ordinary Temperatures
  37. 5.11: Rotational Partition Functions of Diatomic Gases
  38. 06: The First Law
  39. 6.01: Internal Energy
  40. 6.02: Enthalpy
  41. 6.03: Thermochemistry
  42. 07: Entropy and the Second Law
  43. 7.01: A System and Its Surroundings
  44. 7.02: The Second Law of Thermodynamics
  45. 7.03: We Must Always Devise a Reversible Process to Calculate Entropy Changes
  46. 7.04: The Statistical Interpretation of Entropy
  47. 7.05: Entropy Can Be Expressed in Terms of a Partition Function
  48. 08: The Third Law
  49. 8.01: Heat Capacity as A Function of Temperature
  50. 8.02: Evaluating Entropy Changes Using Thermochemical Cycles
  51. 8.03: The Third Law of Thermodynamics
  52. 09: Helmholtz and Gibbs Energies
  53. 9.01: Helmholtz Energy
  54. 9.02: Gibbs Energy
  55. 9.03: The Maxwell Relations
  56. 9.04: The Enthalpy of an Ideal Gas
  57. 9.05: Gibbs-Helmholtz Relation (Gibbs Energy-Chang)
  58. 9.06: The Gibbs-Helmholtz Equation
  59. 10: Phase Equilibria
  60. 10.01: A Phase Diagram Summarizes the Solid-Liquid-Gas Behavior of a Substance
  61. 10.02: Gibbs Energies and Phase Diagrams
  62. 10.03: The Chemical Potentials of a Pure Substance in Two Phases in Equilibrium
  63. 10.04: The Clausius-Clapeyron Equation
  64. 11: Solutions I- Liquid-Liquid Solutions
  65. 11.01: Partial Molar Quantities in Solutions
  66. 11.02: The Gibbs-Duhem Equation
  67. 11.03: Chemical Potential of Each Component Has the Same Value in Each Phase in Which the Component Appears
  68. 11.04: Ideal Solutions obey Raoult's Law
  69. 11.05: Most Solutions are Not Ideal
  70. 11.06: Vapor Pressures of Volatile Binary Solutions
  71. 11.07: Activities of Nonideal Solutions
  72. 12: Chemical Equilibriium
  73. 12.01: The Standard Gibbs Free Energy Change and Equilibrium in Ideal Gas Reactions
  74. 12.02: Equilibrium Results when Gibbs Energy is Minimized
  75. 12.03: The Equilibrium Constant
  76. 12.04: Calculating an Equilibrium Constant Kp with Partial Pressures
  77. 12.05: The Van't Hoff Equation
  78. 13: MathChapters
  79. 13.01: A- Complex Numbers
  80. 13.02: B- Probability and Statistics
  81. 13.03: C- Vectors
  82. 13.04: D- Spherical Coordinates
  83. 13.05: E- Determinants
  84. 13.06: F- Matrices
  85. 13.07: G- Numerical Methods
  86. 13.08: H- Partial Differentiation
  87. 13.09: I- Series and Limits
  88. 13.10: J- The Binomial Distribution and Stirling's Appromixation