Chemical bonding - Intermolecular, Forces, Attraction

chemical bonding

Table of Contents

Introduction
Historical review
- Emergence of quantitative chemistry
  - The law of conservation of mass
  - The law of definite proportions
  - The law of multiple proportions
  - Dalton’s atomic theory
- Features of bonding
  - Valence
  - Ionic and covalent compounds
- The periodic table
- Additional evidence of atoms
  - Avogadro’s law
  - Kinetic theory of gases
  - Visual images of atoms
- Molecular structure
- Internal structure of atoms
  - Discovery of the electron
  - Contributions of Lewis
Atomic structure and bonding
- Atomic structure
  - The Bohr model
  - The quantum mechanical model
    - The location of the electron
    - Quantum numbers
  - Shapes of atomic orbitals
  - The building-up principle
    - Hydrogen and helium
    - Lithium through neon
    - Sodium through argon
    - Potassium through krypton
- Periodic arrangement and trends
  - Arrangement of the elements
  - Periodic trends in properties
    - Atomic size
    - Ionization energy
    - Electron affinity
    - Electronegativity
Bonds between atoms
- The formation of ionic bonds
  - Lewis formulation of an ionic bond
  - The Born-Haber cycle
  - Factors favouring ionic bonding
- Covalent bonds
  - Lewis formulation of a covalent bond
  - Advanced aspects of Lewis structures
    - Multiple bonds
    - Resonance
    - Hypervalence
    - Incomplete-octet compounds
    - Electron-deficient compounds
- Molecular shapes and VSEPR theory
  - Applying VSEPR theory to simple molecules
  - Molecules with multiple bonds
  - Molecules with no central atom
  - Limitations of the VSEPR model
- The polarity of molecules
The quantum mechanics of bonding
- Valence bond theory
  - Formation of σ and π bonds
  - Promotion of electrons
  - Hybridization
  - Resonant structures
- Molecular orbital theory
  - Molecular orbitals of H₂ and He₂
  - Molecular orbitals of period-2 diatomic molecules
  - Molecular orbitals of polyatomic species
  - The role of delocalization
  - Comparison of the VB and MO theories
Intermolecular forces
- Repulsive force
- Dipole–dipole interaction
- Dipole–induced-dipole interaction
- Dispersion interaction
- The hydrogen bond
Varieties of solids
- Ionic solids
- Molecular solids
- Network solids
- Metals
Advanced aspects of chemical bonding
- Theories of bonding in complexes
  - Crystal field theory
  - Ligand field theory
- Compounds displaying unique bonding
  - Organometallic compounds
  - Boranes
  - Metal cluster compounds
- Computational approaches to molecular structure

References & Edit History Related Topics

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Molecules cohere even though their ability to form chemical bonds has been satisfied. The evidence for the existence of these weak intermolecular forces is the fact that gases can be liquefied, that ordinary liquids exist and need a considerable input of energy for vaporization to a gas of independent molecules, and that many molecular compounds occur as solids. The role of weak intermolecular forces in the properties of gases was first examined theoretically by the Dutch scientist Johannes van der Waals, and the term van der Waals forces is used synonymously with intermolecular forces. Under certain conditions, weakly bonded clusters ...(100 of 27318 words)

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