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AUCHE 230 - Structure and Bonding (Elizabeth McGinitie)

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AUCHE 230 - Structure and Bonding (Elizabeth McGinitie)

Chemistry
Author
Elizabeth McGinitie
Publisher
University of Alberta - Augustana Faculty
Source
LibreTexts
License
CC BY-SA
Language
EN
Category
Basic Sciences
Read online Download PDF (open licence)
Contents· 63 sections
  1. 01: Atomic Structure
  2. 1.01: The History of the Periodic Table
  3. 1.02: Electromagnetic Radiation
  4. 1.03: Quantum Theory
  5. 1.04: Atomic Spectra
  6. 1.05: The Bohr Atom
  7. 1.06: Two Ideas Leading to a New Quantum Mechanics
  8. 1.07: Wave Mechanics and Quantum Numbers
  9. 1.08: Electron Spin- A Fourth Quantum Number
  10. 1.09: Orbital Shapes and Energies
  11. 1.10: Electron Configurations
  12. 1.11: Electron Configurations for Transition Metal Elements
  13. 1.12: Magnetic Properties
  14. 1.13: Shielding and Effective Nuclear Charge
  15. 1.14: Slater's Rules
  16. 02: Simple Bonding Theory
  17. 2.01: Prelude to Chemical Bonding and Molecular Geometry
  18. 2.02: Ionic Bonding
  19. 2.03: Covalent Bonding
  20. 2.04: Electronegativity
  21. 2.05: Lewis Theory- An Overview
  22. 2.06: Writing Lewis Structures
  23. 2.07: Resonance
  24. 2.08: Exceptions to the Octet Rule
  25. 2.09: Shapes of Molecules
  26. 2.10: Multiple Bonds
  27. 2.11: Electronegativity and Atomic Size Effects
  28. 03: Molecular Symmetry
  29. 3.01: Symmetry Elements and Operations
  30. 3.02: Symmetry Elements
  31. 3.03: Molecular Point Groups
  32. 04: Molecular Orbital (MO) Theory
  33. 4.01: Formation of Molecular Orbitals from Atomic Orbitals
  34. 4.02: Molecular Orbitals from s Orbitals
  35. 4.03: Molecular Orbitals from p Orbitals
  36. 4.04: Molecular orbitals from d orbitals
  37. 4.05: Nonbonding Orbitals and Other Factors
  38. 4.06: Homonuclear Diatomic Molecules
  39. 4.07: Molecular Orbitals
  40. 4.08: Orbital Mixing
  41. 4.09: Diatomic Molecules of the First and Second Periods
  42. 4.10: Heteronuclear Diatomic Molecules
  43. 4.11: Orbital ionization energies
  44. 4.12: Polar bonds
  45. 4.13: Ionic Compounds and Molecular Orbitals
  46. 05: Acid-Base and Donor-Acceptor Chemistry
  47. 5.01: Acid-Base Models as Organizing Concepts
  48. 5.02: Arrhenius Concept
  49. 5.03: Brnsted-Lowry Concept
  50. 5.04: Rules of Thumb for thinking about the relationship between Molecular Structure and Brnsted Acidity and Basicity
  51. 5.05: The acid-base behavior of binary element hydrides is determined primarily by the element's electronegativity and secondarily by the element-hydrogen bond strength.
  52. 5.06: The Acidity of an Oxoacid is Determined by the Electronegativity and Oxidation State of the Oxoacid's Central Atom
  53. 5.07: Lewis Concept and Frontier Orbitals
  54. 5.08: 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.
  55. 5.09: 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
  56. 5.10: Bulky groups weaken the strength of Lewis acids and bases because they introduce steric strain into the resulting acid-base adduct.
  57. 5.11: Hard and Soft Acids and Bases
  58. 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
  59. 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
  60. 06: Crystalline Solids
  61. 6.01: Crystalline and Amorphous Solids
  62. 6.02: The Solid State of Matter
  63. 6.03: Lattice Structures in Crystalline Solids