AUCHE 230 - Structure and Bonding (Elizabeth McGinitie)

by Elizabeth McGinitie

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Publisher
University of Alberta - Augustana Faculty
Subjects
Chemistry
Licence
CC BY-SA 4.0, as LibreTexts states it
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: Atomic Structure
  7. 1.1: The History of the Periodic Table
  8. 1.2: Electromagnetic Radiation
  9. 1.3: Quantum Theory
  10. 1.4: Atomic Spectra
  11. 1.5: The Bohr Atom
  12. 1.6: Two Ideas Leading to a New Quantum Mechanics
  13. 1.7: Wave Mechanics and Quantum Numbers
  14. 1.8: Electron Spin- A Fourth Quantum Number
  15. 1.9: Orbital Shapes and Energies
  16. 1.10: Electron Configurations
  17. 1.11: Electron Configurations for Transition Metal Elements
  18. 1.12: Magnetic Properties
  19. 1.13: Shielding and Effective Nuclear Charge
  20. 1.14: Slater's Rules
  21. 2: Simple Bonding Theory
  22. 2.1: Prelude to Chemical Bonding and Molecular Geometry
  23. 2.2: Ionic Bonding
  24. 2.3: Covalent Bonding
  25. 2.4: Electronegativity
  26. 2.5: Lewis Theory- An Overview
  27. 2.6: Writing Lewis Structures
  28. 2.7: Resonance
  29. 2.8: Exceptions to the Octet Rule
  30. 2.9: Shapes of Molecules
  31. 2.10: Multiple Bonds
  32. 2.11: Electronegativity and Atomic Size Effects
  33. 3: Molecular Symmetry
  34. 3.1: Symmetry Elements and Operations
  35. 3.2: Symmetry Elements
  36. 3.3: Molecular Point Groups
  37. 4: Molecular Orbital (MO) Theory
  38. 4.1: Formation of Molecular Orbitals from Atomic Orbitals
  39. 4.2: Molecular Orbitals from s Orbitals
  40. 4.3: Molecular Orbitals from p Orbitals
  41. 4.4: Molecular orbitals from d orbitals
  42. 4.5: Nonbonding Orbitals and Other Factors
  43. 4.6: Homonuclear Diatomic Molecules
  44. 4.7: Molecular Orbitals
  45. 4.8: Orbital Mixing
  46. 4.9: Diatomic Molecules of the First and Second Periods
  47. 4.10: Heteronuclear Diatomic Molecules
  48. 4.11: Orbital ionization energies
  49. 4.12: Polar bonds
  50. 4.13: Ionic Compounds and Molecular Orbitals
  51. 5: Acid-Base and Donor-Acceptor Chemistry
  52. 5.1: Acid-Base Models as Organizing Concepts
  53. 5.2: Arrhenius Concept
  54. 5.3: Brønsted-Lowry Concept
  55. 5.4: Rules of Thumb for thinking about the relationship between Molecular Structure and Brønsted Acidity and Basicity*
  56. 5.5: The acid-base behavior of binary element hydrides is determined primarily by the element's electronegativity and secondarily by the element-hydrogen bond strength.*
  57. 5.6: The Acidity of an Oxoacid is Determined by the Electronegativity and Oxidation State of the Oxoacid's Central Atom*
  58. 5.7: Lewis Concept and Frontier Orbitals
  59. 5.8: 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.
  60. 5.9: 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
  61. 5.10: Bulky groups weaken the strength of Lewis acids and bases because they introduce steric strain into the resulting acid-base adduct.
  62. 5.11: Hard and Soft Acids and Bases
  63. 5.12: 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
  64. 5.13: 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
  65. 6: Crystalline Solids
  66. 6.1: Crystalline and Amorphous Solids
  67. 6.2: The Solid State of Matter
  68. 6.3: Lattice Structures in Crystalline Solids
  69. Back Matter
  70. Index
  71. Glossary
  72. Detailed Licensing
  73. Detailed Licensing