Question

The hybridisation of carbon in carbon dioxide molecule is:
A.$s{p^2}$
B.$sp$
C.$s{p^3}$
D.None

Answer 1

The hybridization of an atom can be identified by the number of bonds and the type of bond it makes with other atomic orbitals. If we want to find the hybridization of carbon, in the carbon dioxide we need to draw the structure of the carbon dioxide molecule.

Complete step by step answer:
As we know that the formula for carbon dioxide is $C{O_2}$ . From the formula we can see that the atom of carbon contains one atom of carbon and two atoms of oxygen.
According to valence bond theory, we know that the atomic orbitals overlap with other atomic orbital and result in formation of a molecule. This is known as hybridization. Hybridization leads to affect the bonds and the type of bonds molecule makes with different atoms
Now carbon dioxide has a linear structure with carbon in the middle and oxygen on the sides doubly bonded with carbon atoms.
$O = C = O$
If the atom has no double bond the hybridization thus formed is $s{p^3}$ . if the atom has a single double bond the resulting hybridization is $s{p^2}$ . but in the above representation of carbon dioxide we can clearly see there are two double bonds hence the resulting hybridization is $sp$
Hence option (B) is the correct answer

Note:
The VSEPR theory or the valence bond theory can be used in the valence shell electron pair repulsion theory for the correlation of hybridization with the shape and geometry of the molecule. Molecules settle where there is minimum electronic repulsion and hence create a low energy shape.