CHEM 3110: Descriptive Inorganic Chemistry

by Catherine McCusker

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Publisher
East Tennessee State 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

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  1. Front Matter
  2. TitlePage
  3. InfoPage
  4. Table of Contents
  5. Licensing
  6. 1: Introduction to Inorganic Chemistry
  7. 1.1: What is Inorganic Chemistry?
  8. 1.2: Inorganic vs Organic Chemistry
  9. 1.3: History of Inorganic Chemistry
  10. 2: Atomic Theory
  11. 2.1: Quantum Numbers and Atomic Wavefunctions
  12. 2.2: Shielding
  13. 2.3: Aufbau Principle
  14. 2.4: Periodic Properties of Atoms
  15. 3: Bonding Theories
  16. 3.1: Types of Bonding
  17. 3.2: Electronegativity Values
  18. 3.2A: Pauling Electronegativity Values
  19. 3.2B: Mulliken Electronegativity Values
  20. 3.2C: Allred-Rochow Electronegativity Values
  21. 3.3: Lewis Electron-Dot Diagrams
  22. 3.3A: Formal Charge
  23. 3.3B: Resonance
  24. 3.3C: Expanded Octets
  25. 3.3D: Limitation of Lewis Theory
  26. 3.4: Valence-Shell Electron-Repulsion Theory
  27. 3.5: Molecular Polarity
  28. 3.6: Valence Bond Theory
  29. 3.7: Molecular Orbital Theory
  30. 3.7A: Orbital Overlap
  31. 3.7B: Homonuclear Diatomic Molecules
  32. 3.7C: Heteronuclear Diatomic Molecules
  33. 4: Molecular Symmetry and Point Groups
  34. 4.1: Symmetry Operations and Elements
  35. 4.2: Point Groups
  36. 4.3: Introduction to Character Tables
  37. 4.4: Applications of Symmetry in Chemistry
  38. 5: Structure and Energetics of Solids
  39. 5.1: Crystal Structures and Unit Cells
  40. 5.2: Energetics of Ionic Solids- Lattice Energy
  41. 5.3: Lattice Enthalpies and Born Haber Cycles
  42. 5.4: Lattice Energy and Solubility
  43. 5.5: Bonding in Metals and Semicondoctors
  44. 5.6: Nanomaterials
  45. 6: Acid-Base and Donor-Acceptor Chemistry
  46. 6.1: Arrhenius Model
  47. 6.2: Brønsted-Lowry Model
  48. 6.3: Lewis Concept and Frontier Orbitals
  49. 6.4: Hard and Soft Acids and Bases
  50. 7: Reduction and Oxidation Chemistry
  51. 7.1: Balancing Redox Reactions
  52. 7.2: Electrochemical Potentials
  53. 7.3: Latimer Diagrams
  54. 7.4: Frost Diagrams
  55. 7.5: Pourbaix Diagrams
  56. 8: Coordination Chemistry- Structure and Isomers
  57. 8.1: History
  58. 8.2: Nomenclature and Ligands
  59. 8.3: Coordination Numbers and Structures
  60. 8.4: Isomerism
  61. 9: Coordination Chemistry- Bonding
  62. 9.1: Crystal Field Theory
  63. 9.2: Crystal Field Stabilization Energy
  64. 9.3: Jahn-Teller Distortions
  65. 9.4: Factors That Affect Crystal Field Splitting
  66. 9.5: Ligand Field Theory
  67. 10: Coordination Chemistry- Reactions and Mechanisms
  68. 10.1: Thermodynamic Stability of Metal Complexes
  69. 10.2: Trends in Kinetic Lability
  70. 10.3: Ligand Substitution Mechanisms
  71. 10.4: The Trans Effect
  72. 10.5: Electron Transfer Reactions
  73. 11: Organometallic Chemistry
  74. 11.1: Organometallic Ligands
  75. 11.2: The 18 Electron Rule
  76. 11.3: Oxidative Addition
  77. 11.4: Reductive Elimination
  78. 11.5: Migratory Insertion- 1,2-Insertions
  79. 11.6: β-Elimination Reactions
  80. 11.7: Organometallic Catalysts
  81. 12: Bioinorganic Chemistry
  82. 12.1: Biological Significance of Metals
  83. 12.2: Introduction to Amino Acids and Proteins
  84. 12.3: Biological Dioxygen Transport and Storage
  85. 12.4: Biological Metal Storage
  86. 12.5: Zinc as Lewis Acid and Template
  87. 12.6: Electron Transfer
  88. Back Matter
  89. Index
  90. Glossary
  91. Detailed Licensing