Chemistry Bonding

A detailed Summary of Chemistry Bonding


The electron pair repulsion theory states that the electron pairs in the valence energy level of an atom repel each other, and therefore are arranged as far apart as possible. For example, H2O:

Due to this theory, different molecules with different amounts of pairs of electrons have different shapes.

Some common shapes of molecules include linear, trigonal planar, tetrahedral, trigonal pyramidal and v-shaped (bent) molecules. Examples are drawn below-

a) linear (CO2)

The electron dot diagrams must be drawn first in order to work out the shape of the molecule.

The polarity can be determined from the shape of the molecule. In essence, a molecule is polar if there is an overall electro


If a molecule is of the form AB2 and is linear, it is non-polar.

negativity difference in the molecule. This can be determined using some basic rules, which state that:

a) AB2 Ö b) AB4 Ö c) AB2 Ö d) AB3 Ö e) AB3 Ö

d) dispersion forces e) dipole-dipole forces (hydrogen bonding)

All other molecules are polar. Using these rules, we can determine the polarity of the earlier used examples.



Some common words found in the essay are:
Intermolecular Forces, Molecular Polarity, Shapes Molecules, Repulsion Theory, H2O Due, dispersion forces, hydrogen bonding, intermolecular forces, trigonal planar, molecule form, trigonal pyramidal, molecular polarity, forces dipole-dipole forces, bonding hydrogen bonding, dipole-dipole forces hydrogen, forces shown, bonding hydrogen, type intermolecular, forces hydrogen bonding, intermolecular forces shown,

Approximate Word count = 687
Approximate Pages = 3 (250 words per page double spaced)

Category: Miscellaneous

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