Valence Bond Theory || VBT || Coordination Compounds || Complex Compounds || Coordination Chemistry

Many approaches have been put forth to explain the nature of bonding in coordination compounds. One of them is the Valence Bond (VB) Theory. The Valence Bond Theory was developed in order to explain chemical bonding using the method of quantum mechanics. This theory primarily focuses on the formation of individual bonds from the atomic orbitals of the participating atoms during the formation of a molecule.

According to the valence bond theory,
Electrons in a molecule occupy atomic orbitals rather than molecular orbitals. The atomic orbitals overlap on the bond formation and the larger the overlap the stronger the bond.

The important postulates of the valence bond theory are listed below.

1.) Covalent bonds are formed when two valence orbitals (half-filled) belonging to two different atoms overlap on each other. The electron density in the area between the two bonding atoms increases as a result of this overlapping, thereby increasing the stability of the resulting molecule.
2.) The presence of many unpaired electrons in the valence shell of an atom enables it to form multiple bonds with other atoms. The paired electrons present in the valence shell do not take participate in the formation of chemical bonds as per the valence bond theory.
3.) Covalent chemical bonds are directional and are also parallel to the region corresponding to the atomic orbitals that are overlapping.
4.) Sigma bonds and pi bonds differ in the pattern that the atomic orbitals overlap in, i.e. pi bonds are formed from sidewise overlapping whereas the overlapping along the axis containing the nuclei of the two atoms leads to the formation of sigma bonds.


In this video I have discussed about the Valence Bond Theory for complex compounds / Coordination Compounds. I have explained the different hybridizations and the geometries associated with them. The difference between VBT for normal Covalent compound and Complex compound is explained with an example.

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