An Introduction to the Electronic Structure of Atoms and Molecules

by McMaster University

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The beginning student of chemistry must have a knowledge of the theory which forms the basis for our understanding of chemistry and he must acquire this knowledge before he has the mathematical background required for a rigorous course of study in quantum mechanics. The present approach is designed to meet this need by stressing the physical or observable aspects of the theory through an extensive use of the electronic charge density.

Description from LibreTexts.

Publisher
Richard F. W. Bader
Subjects
Chemistry, Physical and Theoretical Chemistry Textbook Maps
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

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  1. Front Matter
  2. TitlePage
  3. InfoPage
  4. Table of Contents
  5. Licensing
  6. 1: The Nature of the Problem
  7. 1.1: Introduction
  8. 1.2: Some Important Experiments with Electrons and Light
  9. 1.3: Units of Measurement used in Atomic Physics
  10. 1.4: Further Reading
  11. 1.E: Exercises
  12. 2: The New Physics
  13. 2.1: A Contrast of the Old and New Physics
  14. 2.2: Probability Amplitudes
  15. 2.3: Further Reading
  16. 2.E: Exercises
  17. 3: The Hydrogen Atom
  18. 3.1: Introduction
  19. 3.2: The Quantization of Energy
  20. 3.3: The Probability Distribution of the Hydrogen Atom
  21. 3.4: Angular Momentum of an Electron in a Hydrogen Atom
  22. 3.5: Some Useful Expressions
  23. 3.E: Exercises
  24. 4: Many-Electron Atoms
  25. 4.1: Introduction
  26. 4.2: The Atomic Orbital Concept
  27. 4.3: The Magnetic Properties of the Electron
  28. 4.4: The Electronic Basis of the Periodic Table
  29. 4.5: Further Reading
  30. 4.E: Exercises
  31. 5: Electronic Basis for the Properties of the Elements
  32. 5.1: Introduction
  33. 5.2: Horizontal Variations
  34. 5.3: Vertical Relationships
  35. 5.4: Some Chemical Implications
  36. 5.E: Exercises
  37. 6: The Chemical Bond
  38. 6.1: Introduction
  39. 6.2: An Electrostatic Interpretation of the Chemical Bond
  40. 6.3: The Effect of the Pauli Principle on Chemical Binding
  41. 6.4: The Quantum Mechanical Explanation of Valency
  42. 6.5: Molecular Geometry
  43. 6.6: Literature References
  44. 6.E: Exercises
  45. 7: Ionic and Covalent Bonding
  46. 7.1: Introduction
  47. 7.2: Classification of Chemical Bonds
  48. 7.3: Molecular Charge Distribution of Homonuclear Diatomic Molecules
  49. 7.4: Dipole Moments and Polar Bonds
  50. 7.5: Electronegativity
  51. 7.6: Interaction Between Molecules
  52. 7.7: Literature References
  53. 7.8: Further Reading
  54. 7.A: Appendix
  55. 7.E: Exercises
  56. 8: Molecular Orbitals
  57. 8.1: Introduction
  58. 8.2: Angular Momentum in Diatomic Molecules
  59. 8.3: Symmetry Considerations
  60. 8.4: Molecular Orbitals for Homonuclear Diatomics
  61. 8.5: The Relative Binding Ability of Molecular Orbitals
  62. 8.6: Molecular Orbitals for Heteronuclear Molecules
  63. 8.7: Molecular Orbitals for Polyatomic Molecules
  64. 8.8: Further Reading
  65. 8.E: Exercises
  66. 9: Preface to Calculations
  67. Back Matter
  68. Index
  69. Index
  70. Detailed Licensing