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CHEM 3110: Descriptive Inorganic Chemistry

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CHEM 3110: Descriptive Inorganic Chemistry

Chemistry
Author
Catherine McCusker
Publisher
East Tennessee State University
Source
LibreTexts
License
CC BY-NC-SA
Language
EN
Category
Basic Sciences
Read online Download PDF (open licence)
Contents· 82 sections
  1. 01: Introduction to Inorganic Chemistry
  2. 1.01: What is Inorganic Chemistry
  3. 1.02: Inorganic vs Organic Chemistry
  4. 1.03: History of Inorganic Chemistry
  5. 02: Atomic Theory
  6. 2.01: Quantum Numbers and Atomic Wavefunctions
  7. 2.02: Shielding
  8. 2.03: Aufbau Principle
  9. 2.04: Periodic Properties of Atoms
  10. 03: Bonding Theories
  11. 3.01: Types of Bonding
  12. 3.02: Electronegativity Values
  13. 3.2A: Pauling Electronegativity Values
  14. 3.2B: Mulliken Electronegativity Values
  15. 3.2C: Allred-Rochow Electronegativity Values
  16. 3.03: Lewis Electron-Dot Diagrams
  17. 3.3A: Formal Charge
  18. 3.3B: Resonance
  19. 3.3C: Expanded Octets
  20. 3.3D: Limitation of Lewis Theory
  21. 3.04: Valence-Shell Electron-Repulsion Theory
  22. 3.05: Molecular Polarity
  23. 3.06: Valence Bond Theory
  24. 3.07: Molecular Orbital Theory
  25. 3.7A: Orbital Overlap
  26. 3.7B: Homonuclear Diatomic Molecules
  27. 3.7C: Heteronuclear Diatomic Molecules
  28. 04: Molecular Symmetry and Point Groups
  29. 4.01: Symmetry Operations and Elements
  30. 4.02: Point Groups
  31. 4.03: Introduction to Character Tables
  32. 4.04: Applications of Symmetry in Chemistry
  33. 05: Structure and Energetics of Solids
  34. 5.01: Crystal Structures and Unit Cells
  35. 5.02: Energetics of Ionic Solids- Lattice Energy
  36. 5.03: Lattice Enthalpies and Born Haber Cycles
  37. 5.04: Lattice Energy and Solubility
  38. 5.05: Bonding in Metals and Semicondoctors
  39. 5.06: Nanomaterials
  40. 06: Acid-Base and Donor-Acceptor Chemistry
  41. 6.01: Arrhenius Model
  42. 6.02: Brnsted-Lowry Model
  43. 6.03: Lewis Concept and Frontier Orbitals
  44. 6.04: Hard and Soft Acids and Bases
  45. 07: Reduction and Oxidation Chemistry
  46. 7.01: Balancing Redox Reactions
  47. 7.02: Electrochemical Potentials
  48. 7.03: Latimer Diagrams
  49. 7.04: Frost Diagrams
  50. 7.05: Pourbaix Diagrams
  51. 08: Coordination Chemistry- Structure and Isomers
  52. 8.01: History
  53. 8.02: Nomenclature and Ligands
  54. 8.03: Coordination Numbers and Structures
  55. 8.04: Isomerism
  56. 09: Coordination Chemistry- Bonding
  57. 9.01: Crystal Field Theory
  58. 9.02: Crystal Field Stabilization Energy
  59. 9.03: Jahn-Teller Distortions
  60. 9.04: Factors That Affect Crystal Field Splitting
  61. 9.05: Ligand Field Theory
  62. 10: Coordination Chemistry- Reactions and Mechanisms
  63. 10.01: Thermodynamic Stability of Metal Complexes
  64. 10.02: Trends in Kinetic Lability
  65. 10.03: Ligand Substitution Mechanisms
  66. 10.04: The Trans Effect
  67. 10.05: Electron Transfer Reactions
  68. 11: Organometallic Chemistry
  69. 11.01: Organometallic Ligands
  70. 11.02: The 18 Electron Rule
  71. 11.03: Oxidative Addition
  72. 11.04: Reductive Elimination
  73. 11.05: Migratory Insertion- 12-Insertions
  74. 11.06: -Elimination Reactions
  75. 11.07: Organometallic Catalysts
  76. 12: Bioinorganic Chemistry
  77. 12.01: Biological Significance of Metals
  78. 12.02: Introduction to Amino Acids and Proteins
  79. 12.03: Biological Dioxygen Transport and Storage
  80. 12.04: Biological Metal Storage
  81. 12.05: Metal Lewis Acids
  82. 12.06: Biological Redox Components