CHE 332: Inorganic Chemistry

by Karin Young

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This textbook is for CHE 332: Inorganic Chemistry at Centre College.

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Publisher
Centre College
Subjects
Chemistry
Licence
CC BY-NC-SA, 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. Chapter 1: Introduction to Inorganic Chemistry
  7. Section 1.1: What is Inorganic Chemistry?
  8. Section 1.2: Inorganic vs Organic Chemistry
  9. Section 1.3: History of Inorganic Chemistry
  10. Chapter 2: Atomic Theory
  11. Section 2.1: Quantum Numbers and Atomic Wavefunctions
  12. Section 2.2: Aufbau Principle
  13. Section 2.3: Shielding
  14. Section 2.4: Periodic Properties of Atoms
  15. Chapter 3: Molecular Symmetry and Point Groups
  16. Section 3.1: Symmetry Operations and Elements
  17. Section 3.2: Point Groups
  18. Section 3.3: Properties and Representations of Groups
  19. Section 3.3.1: Representations of Symmetry Operations
  20. Section 3.3.2: Matrices
  21. Section 3.3.3: Mathematical Notation of Representations
  22. Section 3.3.4: Character Tables
  23. Section 3.4: Examples and Applications of Symmetry
  24. Section 3.4.1: Chirality
  25. Section 3.4.2: Molecular Vibrations
  26. Chapter 4: Molecular Orbitals
  27. Section 4.1: Formation of Molecular Orbitals from Atomic Orbitals
  28. Section 4.1.1: Molecular Orbitals from s Orbitals
  29. Section 4.1.2: Molecular Orbitals from p Orbitals
  30. Section 4.1.3: Molecular orbitals from d orbitals
  31. Section 4.1.4: Nonbonding Orbitals and Other Factors
  32. Section 4.2: Molecular Orbital Theory of Diatomic Molecules
  33. Section 4.2.1: Orbital Overlap
  34. Section 4.2.2: Homonuclear Diatomic Molecules
  35. Section 4.2.3: Heteronuclear Diatomic Molecules
  36. Section 4.2.4: Orbital Mixing
  37. Section 4.2.5: Diatomic Molecules of the First and Second Periods
  38. Section 4.2.6: Photoelectron Spectroscopy
  39. Section 4.3: Larger (Polyatomic) Molecules
  40. Section 4.3.1: Bifluoride anion
  41. Section 4.3.2: Carbon Dioxide
  42. Section 4.3.3: H₂O
  43. Section 4.3.4: NH₃
  44. Section 4.3.5: CO₂ (Revisted with Projection Operators)
  45. Section 4.3.6: BF₃
  46. Section 4.4: Problems
  47. Chapter 5: Coordination Chemistry- Structure and Isomers
  48. Section 5.1: History
  49. Section 5.2: Nomenclature and Ligands
  50. Section 5.3: Acid-Base and Donor-Acceptor Chemistry
  51. Section 5.3.1: Acid-Base Models as Organizing Concepts
  52. Section 5.3.2: Lewis Concept and Frontier Orbitals
  53. Section 5.3.2.1: The frontier orbital approach considers Lewis acid-base reactions in terms of the donation of electrons from the base's highest occupied orbital into the acid's lowest unoccupied orbital.
  54. Section 5.3.2.2: All other things being equal, electron withdrawing groups tend to make Lewis acids stronger and bases weaker while electron donating groups tend to make Lewis bases stronger and acids weaker
  55. Section 5.3.2.3: The electronic spectra of charge transfer complexes illustrate the impact of frontier orbital interactions on the electronic structure of Lewis acid-base adducts
  56. Section 5.3.2.4: Substances' solution phase Lewis basicity towards a given acid may be estimated using the enthalphy change for dissociation of its adduct with a reference acid of similar hardness.
  57. Section 5.3.2.5: In the boron trifluoride affinity scale, the enthalphy change on formation of an adduct between the base and boron trifluoride is taken as a measure of Lewis basicity.
  58. Section 5.3.2.6: Lewis base strength may also be estimated by measuring structural or energy changes upon formation of a Lewis acid-base complex, as illustrated by efforts to spectroscopically assess the strengths of halogen bonds
  59. Section 5.3.2.7: Bulky groups weaken the strength of Lewis acids and bases because they introduce steric strain into the resulting acid-base adduct.
  60. Section 5.3.2.8: Frustrated Lewis pair chemistry uses Lewis acid and base sites within a molecule that are sterically restricted from forming an adduct with each other.
  61. Section 5.3.3: Hard and Soft Acids and Bases
  62. Section 5.3.3.1: Hard-Hard and Soft-Soft preferences may be explained and quantified in terms of electrostatic and covalent and electronic stabilization on the stability of Lewis acid-base adducts
  63. Section 5.3.3.2: Quantitative Measures of Hardness, Softness, and Acid-Base Interactions from a Hard Soft Acid-Base Principle Perspective Involve Orbital Energies and/or Apportioning Acid-Base Bonding in Terms of Electrostatic and Covalent Factors
  64. Section 5.3.4: Problems
  65. Section 5.4: Coordination Numbers and Structures
  66. Section 5.5: Isomerism
  67. Chapter 6: Coordination Chemistry- Bonding
  68. Section 6.1: Crystal Field Theory
  69. Section 6.2: Crystal Field Stabilization Energy
  70. Section 6.3: Factors That Affect Crystal Field Splitting
  71. Section 6.4: Ligand Field Theory
  72. Section 6.5: Metal-Metal Bonds
  73. Section 6.5.1: Metal-Metal Multiple Bonds
  74. Section 6.6: Jahn-Teller Distortions
  75. Chapter 7: Coordination Chemistry- Reactions and Mechanisms
  76. Section 7.1: Thermodynamic Stability of Metal Complexes
  77. Section 7.2: Trends in Kinetic Lability
  78. Section 7.3: Ligand Substitution Mechanisms
  79. Section 7.4: The Trans Effect Observation
  80. Section 7.5: The Trans Effect Explanation
  81. Section 7.6: Electron Transfer Reactions
  82. Chapter 8: Coordination Chemistry - Electronic Spectra
  83. Section 8.1: Absorption of Light
  84. Section 8.1.1: Beer-Lambert Absorption Law
  85. Section 8.2: Quantum Numbers of Multielectron Atoms
  86. Section 8.2.1: Finding Microstates and Term Symbols
  87. Section 8.2.2: Spin-Orbit Coupling
  88. Section 8.3: Electronic Spectra of Coordination Compounds
  89. Section 8.3.1: Tanabe-Sugano Diagrams
  90. Section 8.3.2: Symmetry labels for split terms
  91. Section 8.3.3: Selection Rules
  92. Section 8.3.4: Correlation Diagrams
  93. Section 8.3.5: Applications of Tanabe-Sugano Diagrams
  94. Section 8.3.6: Tetrahedral Complexes
  95. Section 8.3.7: Charge-Transfer Spectra
  96. Section 8.3.8: Applications of Charge-Transfer
  97. Chapter 9: Structure and Energetics of Solids
  98. Section 9.1: Crystal Structures and Unit Cells
  99. Section 9.2: Energetics of Ionic Solids- Lattice Energy
  100. Section 9.3: Lattice Enthalpies and Born Haber Cycles
  101. Section 9.4: Lattice Energy and Solubility
  102. Section 9.5: Bonding in Metals and Semicondoctors
  103. Section 9.6: Nanomaterials
  104. Section 9.1b: Ionic Radii and Radius Ratios
  105. Chapter 10: Organometallic Chemistry
  106. Section 10.1: The 18 Electron Rule
  107. Section 10.2: Organometallic Ligands
  108. Section 10.3: Characterization of Organometallic Complexes
  109. Chapter 11: Organometallic Reactions and Catalysis
  110. Section 11.1: Reactions Involving Gain or Loss of Ligands
  111. Section 11.1.1: Ligand Dissociation and Substitution
  112. Section 11.1.2: Oxidative Addition
  113. Section 11.1.3: Reductive Elimination
  114. Section 11.1.4: Sigma Bond Metathasis
  115. Section 11.1.5: Application of Pincer Ligands
  116. Section 11.2: Reactions Invloving Modification of Unsaturated Ligands
  117. Section 11.2.1: Introduction to Insertion
  118. Section 11.2.2: CO Insertions (Alkyl Migration)
  119. Section 11.2.3: Migratory Insertion-1,2-Insertions
  120. Section 11.2.4: β-Elimination Reactions
  121. Section 11.2.5: Abstraction and Addition
  122. Section 11.3: Organometallic Catalysts
  123. Section 11.3.1: Catalytic Deuteration
  124. Section 11.3.2: Hydroformylation
  125. Section 11.3.3: Monsanto Acetic Acid Process
  126. Section 11.3.4: Wacker (Smidt) Process
  127. Section 11.3.5: Hydrogenation by Wilkinson's Catalyst
  128. Section 11.3.6: Olefin Metathesis
  129. Section 11.4: Heterogeneous Catalysts
  130. Section 11.4.1: Ziegler-Natta Polymerizations
  131. Section 11.4.2: Water-Gas Shift Reaction
  132. Section 11.5: Problems
  133. Section 11.5.1: Concept Review Questions Chapter 12
  134. Section 11.5.2: Homework Problems Chapter 12
  135. Chapter 12: Bioinorganic Chemistry
  136. Section 12.1: Biological Significance of Metals
  137. Section 12.2: Introduction to Amino Acids and Proteins
  138. Section 12.3: Biological Dioxygen Transport and Storage
  139. Section 12.4: Biological Metal Storage
  140. Section 12.5: Zinc as Lewis Acid and Template
  141. Section 12.6: Electron Transfer
  142. Back Matter
  143. Index
  144. Glossary
  145. Detailed Licensing