Hybridisation determines the shape of molecule. The types of hybridisation depends upon the number and types of orbitals mixed together. Here, we will discuss the shape of molecules having bond pairs and lone pairs.

What is Hybridisation

Covalent bond is formed by the overlap of half filled orbitals. (hybridised or unhybridised)

Shape of NH3 molecule on the basis of hybridisation

1. Atomic number of central atom N = 7
2. The ground state electronic configuration of N = 1s2, 2s2, 2p3
3. Excited state electronic configuration of N = 1s2, 2s2, 2px1, 2py1, 2pz1
4. The ground state electronic configuration of H = 1s1
5. One 2s and three 2p orbitals undergo the process forming 4 Sp3 hybridised orbitals.
6. The resulting hybridis^n is Sp3 for NH3 having 1 lone pair & 3 bond pairs
7. The shape of NH3 is triangular pyramidal.

Shape of H2O molecule on the basis of hybridised orbitals

1. Atomic number of central atom O = 8
2. The ground state electronic configuration of O = 1s2, 2s2, 2px2, 2Py1, 2Pz1
3. The ground state electronic configuration of H = 1s1
4. One 2s and three 2p orbitals undergo the process forming 4 Sp3 hybridised orbitals.
5. The resulting hybridis^n is Sp3 for H2O having 2 lone pairs & 2 bond pairs
6. The shape of H2O is bent or V shape.

Shape of SF4 molecule on the basis of hybridised orbitals

1. Atomic number of central atom S = 16
2. Excited state electronic configuration of S = 3s2, 3px1, 3py1, 3pz1, 3d1
3. The ground state electronic configuration of F = 1s2, 2s2, 2px2, 2py2, 2pz1
4. The resulting hybridis^n is Sp3d for SF4 having 1 lone pair and 4 bond pairs
5. The shape of SF4 molecule is see-saw.

Shape of ClF3 molecule on the basis of hybridised orbitals

1. Atomic number of central atom Cl = 17
2. Excited state electronic configuration of Cl = 3s2, 3px2, 3py1, 3pz1, 3d1
3. The ground state electronic configuration of F = 1s2, 2s2, 2px2, 2py2, 2pz1
4. The resulting hybridis^n is Sp3d for ClF3 having 2 lone pairs and 3 bond pairs.
5. The shape of ClF3 molecule is T-shaped

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