What is the Hybridization of the Carbon atoms in Ethylene

What is the Hybridization of the Carbon atoms in Ethylene

sp² Hybridisation

Consider ethene (ethylene, CH₂ = CH₂) molecule as the example.

In the formation of CH₂ = CH₂ each carbon atom in its excited state undergoes sp² hybridisation by intermixing one s-orbital (2s) and two p-orbitals (say 2p_x , 2p_y) and reshuffling to form three sp² orbitals. Now each carbon atom is left with one ‘p’ orbital (say p_z) unhybridised. The three sp² orbitals having one electron each get separated around the nucleus of carbon atoms at an angle of 120o. When carbon is ready to form bonds one sp² orbital of one carbon atom overlaps the sp² orbital of the other  carbon atom to form sp² – sp² sigma (σ) bond.

The remaining two sp² orbitals of each carbon atom get overlapped by‘s’ orbitals of two hydrogen
atoms containing unpaired electrons. The unhybridised p_z orbitals on the two carbon atoms overlap laterally as shown in figure to form a π bond.That means there exists a sigma (σ) bond and a pi (π) bond between two carbon atoms in ethene molecule. Hence, the molecule ethene (C₂H₄) is

The common name for Ethene is Ethylene.