The carbon atom in phosgene (Cl2CO) exhibits sp2 hybridization. In this molecule, the carbon is bonded to two chlorine atoms and one oxygen atom through a double bond.
To explain this further, let’s look at the structure of phosgene. The carbon atom is at the center surrounded by two chlorine atoms and one oxygen atom. The carbon forms one double bond with oxygen and two single bonds with chlorine. In order to accommodate these bonding scenarios, the carbon atom undergoes hybridization.
During sp2 hybridization, one s orbital and two p orbitals from the carbon atom combine to form three equivalent sp2 hybrid orbitals. These three hybrid orbitals are used to form sigma bonds with the adjacent atoms (two Cl and one O). The remaining unhybridized p orbital participates in the formation of the double bond with the oxygen atom.
This arrangement results in a trigonal planar geometry around the carbon atom, which is consistent with the bond angles of approximately 120 degrees. The presence of the electronegative chlorine and oxygen atoms also influences the molecular properties, contributing to the overall toxicity and reactivity of phosgene.