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Hybridization (or hybridization) may be a process of mathematically combining two or more atomic orbitals from an equivalent atom to make a completely new orbital different from its components and hence being called as a hybrid orbital.The original atomic orbitals are similar in energy, but not equivalent (for example, a 2s orbital might hybridize with a 2p orbital). The resulting hybrid orbitals are equivalent in energy to at least one another and are oriented in order that they will form bonds with other atoms. Hybridisation helps to predict the form of molecules, particularly in chemistry .Hybridization is defined because the concept of blending two atomic orbitals with an equivalent energy levels to offer a degenerated new sort of orbitals. This intermixing is predicated on quantum physics . The atomic orbitals of an equivalent energy state can only participate in hybridization and both full filled and half-filled orbitals also can participate during this process provided they need equal energy.During the method of hybridization, the atomic orbitals of comparable energy are mixed together like the blending of two ‘s’ orbitals or two ‘p’ orbital’s or mixing of an ‘s’ orbital with a ‘p’ orbital or ‘s’ orbital with a ‘d’ orbital. Hybrid orbitals are very useful within the explanation of molecular geometry and atomic bonding properties and are symmetrically disposed in space. Although sometimes taught alongside the valence shell electron-pair repulsion (VSEPR) theory, valence bond and hybridisation are actually not associated with the VSEPR model.    

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