The carbon in CO2 exhibits sp hybridization due to the formation of two double bonds with oxygen atoms, leading to a linear molecular geometry with bond angles of 180 degrees.
The hybridization of the carbon atom in carbon dioxide (CO2) is sp hybridization. This is because the carbon atom forms two double bonds with two oxygen atoms, resulting in a linear molecule with bond angles of 180 degrees.
When a carbon atom forms two double bonds, the s orbital and one p orbital hybridize to form two sp orbitals, which are used to form the σ bonds in CO2.
The remaining two p orbitals on the carbon atom form π bonds with the oxygen atoms.