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In this type of bonding the 2s orbital and the three 2p orbitals of the carbon atom are mixed to produce four identical orbitals, a process known as sp3 hybridization. The CS2 molecule is linear and the carbon atom is bonded to each sulphur by a double bond.
The oxygen is also sp2 hybridized, with the 2 lone pairs occupying sp2 orbitals. This leaves one electron in a p. orbital. These p orbitals form the carbon oxygen ï° bond. The C=O double bond is like a C=C double bond except the carbonyl double bond is shorter and stronger. The carbonyl group has a large dipole moment due to the polarity of the double bond. Oxygen is more electronegative than carbon, and so the bond is polarized toward the oxygen. The attraction of the weakly held ï° electrons toward oxygen can be represented by the two following resonance. structures.