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Intermediate Physical Organic (Morsch)

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Intermediate Physical Organic (Morsch)

Physical organic chemistry refers to a discipline of organic chemistry that focuses on the relationship between chemical structures and reactivity, in particular, applying experimental tools of physical chemistry to the study of organic molecules. Specific focal points of study include the rates of organic reactions, the relative chemical stabilities of the starting materials, reactive intermediates, transition states, and products of chemical reactions, and non-covalent aspects of solvation.

Organic ChemistryChemistry
Author
Layne Morsch
Publisher
University of Illinois Springfield
Source
LibreTexts
Language
EN
Category
Basic Sciences
Read online Download PDF (open licence)
Contents· 105 sections
  1. 01: Models of Chemical Bonding
  2. 1.01: Atomic and Molecular Properties
  3. 1.1.01: Atomic and Ionic Radius
  4. 1.1.02: Bond Lengths and Double-Bond Character
  5. 1.1.03: Dipole Moments
  6. 1.1.04: Electronegativity
  7. 1.1.05: Molecular Polarity
  8. 1.02: Intermolecular Forces - Introduction and London Dispersion
  9. 1.2.01: Specific Interactions
  10. 1.2.02: Hydrogen Bonding
  11. 1.2.03: Dipole-Dipole Interactions
  12. 1.2.04: Polarizability
  13. 1.03: Overview of Valence Bond Theory
  14. 1.3.01: The Born-Oppenheimer Approximation Simplifies the Schrodinger Equation for Molecules
  15. 1.3.02: Covalent Bonding and Orbital Overlap
  16. 1.3.03: Hybrid Orbitals
  17. 1.3.04: Delocalization of Electrons
  18. 1.3.05: Lennard-Jones Potential
  19. 1.04: Molecular orbital theory- conjugation and aromaticity
  20. 1.4.01: The H Prototypical Species
  21. 1.4.02: Bonding and Antibonding Orbitals
  22. 1.4.03: A Simple Molecular-Orbital Treatment of H Places Both Electrons in a Bonding Orbital
  23. 1.4.04: Molecular Orbitals Can Be Ordered According to Their Energies
  24. 1.4.05: Molecular-Orbital Theory Also Applies to Heteronuclear Diatomic Molecules
  25. 1.4.06: Butadiene is Stabilized by a Delocalization Energy
  26. 1.4.6.01: Application of the MO Method to 13-Butadiene
  27. 1.4.07: Molecular Orbitals of Conjugated Pi Systems
  28. 1.4.08: Benzene and Aromaticity
  29. 1.4.8.01: Huckel's 4n 2 Rule
  30. 1.05: Comparison of the Resonance and Molecular-Orbital Methods
  31. 1.5.01: Which Is Better- MO or VB
  32. 02: Reaction Kinetics
  33. 2.01: Introduction to Reaction Kinetics
  34. 2.1.01: First-Order Reactions
  35. 2.1.02: Half-lives
  36. 2.1.03: Reaction Rate
  37. 2.1.3.01: The Speed of a Chemical Reaction
  38. 2.1.3.02: The Rate of a Chemical Reaction
  39. 2.1.04: Reaction Rates- A Microscopic View
  40. 2.1.05: Second-Order Reactions
  41. 2.1.5.01: Pseudo-1st-order reactions
  42. 2.1.06: Zero-Order Reactions
  43. 2.02: Introduction to reaction kinetics- Basic rate laws
  44. 2.2.01: Collision theory transition state theory and the prediction of rate laws and rate constants
  45. 2.2.02: Complex reaction mechanisms
  46. 2.2.03: Kinetics of catalysis
  47. 2.03: Chemical Kinetics II- Reaction Mechanisms
  48. 2.3.01: A Mechanism is a Sequence of Elementary Reactions
  49. 2.3.02: The Principle of Detailed Balance
  50. 2.3.03: Multiple Mechanisms are often Indistinguishable
  51. 2.3.04: The Steady-State Approximation
  52. 2.3.05: Rate Laws Do Not Imply Unique Mechanism
  53. 2.3.06: The Lindemann Mechanism
  54. 2.3.07: Some Reaction Mechanisms Involve Chain Reactions
  55. 2.3.08: A Catalyst Affects the Mechanism and Activation Energy
  56. 2.3.09: The Michaelis-Menten Mechanism for Enzyme Catalysis
  57. 2.3.10: Predicting Rate Laws from Proposed Mechanisms
  58. 2.3.E: Chemical Kinetics II- Reaction Mechanisms (Exercises)
  59. 03: Chemical Thermodynamics
  60. 3.01: Introduction to Thermodynamics
  61. 3.02: Bond Energies
  62. 3.2.01: Enthalpy Changes in Reactions
  63. 3.2.02: Enthalpy Changes in Reactions II
  64. 3.2.03: Entropy Changes in Reactions
  65. 3.2.04: Free Energy and Equilibrium
  66. 3.2.05: Free Energy Changes in Reactions
  67. 3.2.06: Reversibility and Le Chatelier
  68. 3.03: Describing a Reaction - Energy Diagrams and Transition States
  69. 3.3.01: Potential Energy Surfaces
  70. 3.3.02: The Potential-Energy Surface Can Be Calculated Using Quantum Mechanics
  71. 3.3.03: The Hammond Postulate
  72. 3.04: Reactivity and Selectivity
  73. 3.05: The Principle of Microscopic Reversibility
  74. 3.5.01: Microscopic Reversibility and the Second Law
  75. 3.06: Sterics and Conformation
  76. 04: Reagents and Reaction Mechanisms
  77. 4.01: Polar Reactions
  78. 4.1.01: Substitution Mechanisms
  79. 4.1.02: Elimination Mechanisms
  80. 4.02: Radical Reactions
  81. 4.03: Reactive Species
  82. 4.3.01: Carbocation Structure and Stability
  83. 4.3.02: Carbanions II
  84. 4.3.03: Carbenes
  85. 4.3.04: Free Radicals
  86. 4.3.05: Nucleophiles
  87. 4.3.06: Electrophiles
  88. 4.04: Bond Breaking and Bond Formation
  89. 4.4.01: Transition States
  90. 4.4.02: Reactive Intermediates
  91. 05: Structure Reactivity Relationships
  92. 5.01: Correlations of Structure with Reactivity of Aromatic Compounds
  93. 5.02: Linear Free Energy Relationships
  94. 06: Acidity and Basicity
  95. 6.01: New Page
  96. 07: Kinetic Isotope Effects
  97. 7.01: Kinetic Isotope Effects
  98. 08: Catalysis
  99. 8.01: A. Methods of Catalysis
  100. 8.1.01: A1. General Acid and Base Catalysis
  101. 8.1.02: A2. Metal Ion or Electrostatic Catalysis
  102. 8.1.03: A3. Covalent or Nucleophilic Catalysis
  103. 8.1.04: A4. Intramolecular Catalysis
  104. 8.1.05: A5. Transition State Stabilization
  105. 8.1.06: A6. Links and References