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Definition: The phenomenon of mixing up of atomic orbitals of similar energies and formation of equivalent number of entirely new orbitals of identical shape and energy is known as "hybridization" and the new orbitals so formed is called as "hybrid orbitals".
Important points for understanding the hybridization:
(i) The number of hybrid orbitals generated is equal to the number of pure atomic orbitals that participate in hybridization process. (ii) Hybridization concept is not applicable to isolated atoms. It is used to explain the bonding scheme in a molecule. (iii) Covalent bonds is polyatomic molecules are formed by the overlap of hybrid orbitals or of hybrid orbitals with unhybridized ones.
Types of Hybridization
(1) sp-hybridization: The combination of one s and one p- orbitals to form two hybrid orbitals of equal energy is known as sp-hybridization.
Example: In BeF 2 Molecule the sp-hybridized orbitals of Be overlap with the half-filled orbitals of two fluorine atoms to give a linear shape.
sp^2 -hybridization: The combination of one s and two p-orbitals to form three hybrid orbitals of equal energy is known as sp^2 - hybridization.
Example : BF 3 Molecule.
These sp2 hybridized orbitals are oriented at an angle of 120°. When three sp2 hybridized orbitals of B overlaps with three p- orbitals of fluorine, three σ - bonds are formed with bond angle 120 °. The shape of BF3 molecule is thus trigonal planar
These sp3-hybridized orbitals are oriented at an angle of 109°28'. When these four sp3 hybrid orbitals overlaps with four 1s orbitals of hydrogen, a symmetrical tetrahedral shaped CH4 molecule form.
