Chemical bonding - Noncentral Atoms, Molecules

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

Images & Videos

Witness a combustion reaction between oxygen and cellulose to produce water, carbon dioxide, and carbon

See how John Dalton built his atomic theory on principles laid out by Henry Cavendish and Joseph-Louis Proust

Investigate the magnetlike ionic bond formed when electrons transfer from one atom to another

For Students

bonding summary

Read Next

Molecular Machines: Making for the Future

Discover

Adolf Hitler (Nazi, nazism, German leader).

9 Things You Might Not Know About Adolf Hitler

Vietnam War. U.S. President Lyndon B. Johnson awards the Distinguished Service Cross to First Lieutenant Marty A. Hammer, during a visit to military personnel, Cam Ranh Bay, South Vietnam, October 26, 1966. President Johnson

Vietnam War Timeline

Two chicks near an egg with a white background (poultry, chick, chickens, birds).

What Do Eggs Have to Do with Easter?

Mona Lisa, oil on wood panel by Leonardo da Vinci, c. 1503-06; in the Louvre, Paris, France. 77 x 53 cm.

Why Is the Mona Lisa So Famous?

Still from the film Deliverance, 1919. The story of Helen Keller and Anne Sullivan. View shows Keller in the cockpit/front seat of an airplane.

How Did Helen Keller Fly a Plane?

United States Electoral College votes by state

How Many Electoral College Votes Does Each U.S. State Have?

earthquake. Heavily damaged school in the town of Yingxiu after a major earthquake struck China's Sichuan Province on May 12, 2008.

The 6 Deadliest Earthquakes Since 1950

Examples of the manner in which VSEPR theory is applied to species in which there is no central atom are provided by ethane (C₂H₆), ethylene (C₂H₄), and acetylene (C₂H₂), the Lewis structures for which are, respectively, the following: In each case, consider the local environment of each carbon atom. In ethane there are four bonding pairs around each carbon atom, so every carbon atom is linked to its four neighbours (one carbon atom and three hydrogen atoms) by a tetrahedral array of bonds. The bond angles in ethane are indeed all close to 109°. In ethylene each carbon atom possesses ...(100 of 27318 words)

Access the full article

Help support true facts by becoming a member.