Question

The hybrid state of sulphur in \[{\rm{S}}{{\rm{O}}_{\rm{3}}}\] molecules is,
A) \[s{p^3}d\]
B) \[s{p^3}\]
C) \[s{p^3}{d^2}\]
D) \[s{p^2}\]

Answer 1

Hint: Here, to calculate the hybrid state of the Sulphur atom in the sulphur trioxide molecule, we have to count the groups surrounding the sulphur atom in the molecule.

Complete step by step solution:Let’s understand how to count the groups surrounding the central atom. We have to count the atoms bonded to the atom. And we should also count the lone pairs on the atom. So, the total group is the summation of the count of bonded atoms and lone pairs. If the count of groups is 4, then the atom is \[s{p^3}\] hybridised. And if the count of groups is 3, then the atom is \[s{p^2}\] hybridised. And the count of groups of 2 means the atom is \[sp\] hybridised.
Let’s find out the hybridization of the atom of S in \[{\rm{S}}{{\rm{O}}_{\rm{3}}}\]. The structure of sulphur trioxide is,

Image: Sulphur trioxide
So, we see that three atoms of oxygen are bonded to the sulphur atom and there is no pair present. So, the sulphur atom is \[s{p^2}\] hybridised.

Hence, option D is right.

Additional Information:The formula to calculate hybridization of an atom is,
\[H = \dfrac{{V + X - C + A}}{2}\]
Here, V is for the valence electron, X is for the count of monovalent atoms, C is for the cationic charge and A is for anionic charge.

Note: It is to be noted that hybridization also tells the shape of a molecule. If no lone pair is present in an \[s{p^2}\]hybridised molecule , then the shape of the molecule is trigonal planar. So, sulphur dioxide has a trigonal planar shape.