Hybridisation determines the shape of molecule. The types of hybridisation depends upon the number and types of orbitals mixed together.
What is Hybridisation
Covalent bond is formed by the overlap of half filled orbitals. (hybridised or unhybridised)
Shape of BeF2 molecule on the basis of hybridisation
- Atomic number of central atom Be = 4
- The ground state electronic configuration of Be = 1s2, 2s2
- Excited state electronic configuration of Be = 1s2, 2s1, 2px1
- The ground state electronic configuration of F = 1s2, 2s2, 2px2, 2py2, 2pz1
- 2 half-filled orbitals of Be will hybridise with the half filled orbitals of 2 F atoms.
- The resulting hybridisation is Sp for BeF2
- The shape of molecule is linear.
Shape of BF3 molecule on the basis of hybridised orbitals
- Atomic number of central atom B = 5
- The ground state E.C. of B = 1s2, 2s2, 2px1,
- Excited state E.C. of B = 1s2, 2s1, 2px1, 2py1
- The ground state electronic configuration of F atom = 1s2, 2s2, 2px2, 2py2, 2pz1
- 3 half-filled orbitals of B will hybridise with the half filled orbitals of 3 F atoms.
- The resulting hybridisation is Sp2 for BF3 molecule.
- The shape of molecule is trigonal planar.
Shape of CH4 molecule on the basis of hybridised orbitals
- Atomic number of central atom C = 6
- The ground state electronic configuration of C = 1s2, 2s2, 2p2
- Excited state electronic configuration of C = 1s2, 2s1, 2px1, 2py1, 2pz1
- The ground state electronic configuration of H = 1s1
- 4 half-filled orbitals of C will hybridise with the half filled orbitals of 4 H atoms.
- The resulting hybridisation is Sp3 for CH4
- The shape of molecule is tetrahedral.
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