Question

In which of the following species S-atom assumes $s{{p}^{3}}$-hybrid state?
(I)- $S{{O}_{3}}$
(II)- ${{H}_{2}}S$
(III)- $S{{O}_{2}}$
(IV)- ${{S}_{8}}$

(a)- (I) and (II)
(b)- (II) and (III)
(c)- (II) and (IV)
(d)- (III) and (IV)

Answer 1

In the compound, if the central atom should have $s{{p}^{3}}$-hybrid state, then all the bonds in the compound must be a single bond. If the compound has a double or triple bond then the central atom cannot have $s{{p}^{3}}$-hybrid state. If a single bond is not present, then the lone pair also contributes to $s{{p}^{3}}$-hybrid state.

Complete step by step solution:
In the compound, if the central atom should have $s{{p}^{3}}$-hybrid state, then all the bonds in the compound must be a single bond. If the compound has a double or triple bond then the central atom cannot have $s{{p}^{3}}$-hybrid state. If a single bond is not present, then the lone pair also contributes to $s{{p}^{3}}$-hybrid state.
In $S{{O}_{3}}$, all the sulfur atoms are joined to oxygen atoms through a double bond as shown below. So the hybridization of sulfur in $S{{O}_{3}}$ is $s{{p}^{2}}$.

In ${{H}_{2}}S$, there are two single bonds and there are two lone pairs as shown below. So the hybridization of sulfur in ${{H}_{2}}S$ is $s{{p}^{3}}$.

In $S{{O}_{2}}$, there are double bonds and there is one lone pair as shown below. So, the hybridization of sulfur in $S{{O}_{2}}$ is $s{{p}^{2}}$.

In ${{S}_{8}}$, all the bonds in this molecule are single as shown below. So, the hybridization of sulfur in ${{S}_{8}}$ is $s{{p}^{3}}$.

So, in compound (II) and (IV) the hybrid state is $s{{p}^{3}}$.
So, the correct answer is “Option C”.

Note: If the compound is having a double bond then the hybrid state will be $s{{p}^{2}}$ and if the compound is having a triple bond then the hybrid state will be $sp$.