Hybridization in ethylene molecule (C2H4) occurs due to the overlapping of the two 2s atomic orbitals as well as one 2p atomic orbital of the two carbon atoms.
This overlapping produces four identical sp hybrid orbitals, each containing one electron from each carbon atom. Hybridization allows the bonding between the two carbon atoms, forming the carbon-carbon double bond. The sp2 hybridization of the carbon atoms results in the formation of a linear shape of the ethylene molecule.
The two unhybridized p atomic orbitals of the two carbon atoms lie perpendicular to each other. This results in the formation of a π bond between the two carbon atoms, as the electrons in the two unhybridized p orbitals can move freely between the two carbon atoms.
The linear shape of the ethylene molecule is due to the fact that the two sp2 hybrid orbitals of the two carbon atoms are oriented in opposite directions and are parallel to each other. The two hydrogen atoms are bonded to the carbon atoms through single covalent bonds, forming the carbon-hydrogen single bonds.
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