Question

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

Answer 1

Hint: We can find out hybridisation of an atom by identifying the number and the types of bond it makes with other atomic orbitals. To find the hybridisation of carbon here, firstly draw the structure of the carbon dioxide molecule with its proper bonding with the oxygen atoms. If there are no double bonds, the hybridisation is $s{{p}^{3}}$, if there is one double bond hybridisation is $s{{p}^{2}}$ and if there are two or more than two double bonds, hybridisation is sp.

Complete step by step answer:
We know that the formula of carbon dioxide is $C{{O}_{2}}$ . As we can see, it contains one atom of carbon and a molecule of oxygen.
In the valence bond theory, as we know atomic orbitals overlap with other atomic orbitals to form a molecule and thus creating new hybrid orbitals. This is known as the phenomenon of hybridisation.
In carbon dioxide, carbon serves as the central atom and it is bonded to the two oxygen atoms through a covalent double bonding. We know that a double bonding involves a –sigma bond and a –pi bond.
Now that we know the type of bonds in carbon dioxide thus to find the hybridisation of a molecule of carbon dioxide, firstly we have to draw its structure which is-

We define hybridisation in terms of -‘s’ and ‘p’ orbitals. If there are no double bonds, the hybridisation is $s{{p}^{3}}$ but we can see that this is not the case here. An atom with a single double bond has a hybridisation of $s{{p}^{2}}$ and an atom with two or more double bonds has a hybridisation of sp. Now, here we can see that there are two double bonds thus hybridisation of carbon in carbon dioxide is sp. So, the correct answer is “Option B”.

Note: We can use the VSEPR theory which is the valence shell electron pair repulsion theory to correlate the hybridisation with the shape as well as the geometry of a molecule. Molecules settle in a shape where the electronic repulsion is the minimum and thus creates as lower energy shape as possible. Hybridization affects the bonds and the types of the bonds the molecule makes and thus is correlated to the shape of the molecule.