the redistribution of the energy of orbitals of individual atoms to give new orbitals of equivalent energy and named the process as hybridisation. In this process, the new orbitals come into existence and named as the hybrid orbitals

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Dr. Mohd Kamil Hussain
Department of Chemistry
Govt. Raza P.G. College Rampur, U.P. India
Hybridization and Molecular Geometry
Of Organic and Inorganic Molecules

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What is Hybridization?
Linus Pauling introduced the revolutionary concept of hybridization in the year
1931.
Dr. Mohd Kamil Hussain
Types of Hybridisation
He described it as
“the redistribution of the energy of orbitals of individual atoms to give new orbitals of
equivalent energy and named the process as hybridisation. In this process, the new
orbitals come into existence and named as the hybrid orbitals”.

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Hybridization of Organic Molecules
Dr. Mohd Kamil Hussain
In case of neutral molecules or carocations lps = 0
 hence Hybrid orbitals = no of sigma bond of perticular carbon

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Some examples

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Hybridization in inorganic molecules
No of Hybrid orbitals = Sigma bonds + Lone pairs
Sigma bonds = no of atoms attached to Central atom
ie: AXn n = no of sigma bonds
Molecule σ bonds LPs Hybrid orbitals Hybridization
BeCl2 2 0 2 sp
BF3 3 0 3 sp2
CH4 4 0 4 sp3
PCl5 5 0 5 sp3d
SF6 6 0 6 sp3d2
IF7 7 0 7 sp3d3
When no of lone pairs are zero

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LPs = (Ve - (σ+π)/2
Hybridization in inorganic molecules
No of Hybrid orbitals = Sigma bonds + Lone pairs
When lone pairs are present

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Molecular Geometry of Molecules

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Regular Geometries

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Hybridization Hybrid orbitals Bond angle Geometry Example
sp 2 1800 Linear BeCl2, CO2
sp2 3 1200 Planer BF3
sp3 4 1090 28’ Tetrahedral CCl4, XeO4
sp3d 5 900 and 1200 Trigonal bipyramidal PCl5
sp3d2 6 900 octahedral PCl5
sp3d3 7 720 and 900 Pentagonal
bipyramidal
IF7
Some examples of various molecules

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Central atom having lone pairs of electrons

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