BrF5
SF6
[Co(NH3)6]3+
[PtCl4]2-
List-I ( Types of hybridisation ) | List-II ( Distribution of hybrid orbitals in space ) | ||
A | sp$^3$ | (I) | Trigonal bipyramidal |
B | dsp$^2$ | (II) | Octahedral |
C | sp$^3$d | (III) | Tetrahedral |
D | sp$^3$d$^2$ | (IV) | Square Planar |
Hybridization refers to the concept of combining atomic orbitals in order to form new hybrid orbitals that are appropriate to represent their bonding properties. Hybridization influences the bond length and bond strength in organic compounds.
sp hybridization is observed while one s and one p orbital inside the identical principal shell of an atom mix to shape two new equal orbitals. The new orbitals formed are referred to as sp hybridized orbitals.
sp2 hybridization is observed whilst ones and p orbitals of the same shell of an atom blend to shape three equivalent orbitals. The new orbitals formed are referred to as sp2 hybrid orbitals.
When one ‘s’ orbital and 3 ‘p’ orbitals belonging to the identical shell of an atom blend together to shape 4 new equal orbitals, the sort of hybridization is referred to as a tetrahedral hybridization or sp3.
sp3d hybridization involves the joining of 3p orbitals and 1d orbital to form 5 sp3d hybridized orbitals of identical energy. They possess trigonal bipyramidal geometry.
With 1 s three p’s and two d’s, there is a formation of 6 new and identical sp3d2 orbitals.