How does the hybridization of the sulfur atom change in the series SF2, SF4, SF6?
a. sp, sp³, sp³d²
b. sp³, sp³d, sp³d²
c.sp³, sp³d², sp³d²
d. sp³, sp³, sp³d²
e. sp, sp³d, sp³d²
The Correct Answer and Explanation is :
The correct answer is b. sp³, sp³d, sp³d².
Explanation:
The hybridization of a central atom depends on its bonding and the number of electron pairs (both bonding and lone pairs) around it. Let’s break it down for SF₂, SF₄, and SF₆.
- SF₂ (Sulfur Difluoride):
- Sulfur in SF₂ has 2 bonding pairs (from the two fluorine atoms) and 2 lone pairs.
- The total number of regions of electron density around sulfur is 4 (2 bonding pairs + 2 lone pairs).
- To minimize repulsion, these four regions arrange in a tetrahedral geometry, which requires sp³ hybridization.
- Therefore, the sulfur atom in SF₂ is sp³ hybridized.
- SF₄ (Sulfur Tetrafluoride):
- Sulfur in SF₄ has 4 bonding pairs (from the four fluorine atoms) and 1 lone pair.
- The total number of electron regions around sulfur is 5 (4 bonding pairs + 1 lone pair).
- A five-region electron configuration results in a trigonal bipyramidal geometry, which requires sp³d hybridization.
- Therefore, the sulfur atom in SF₄ is sp³d hybridized.
- SF₆ (Sulfur Hexafluoride):
- Sulfur in SF₆ has 6 bonding pairs (from the six fluorine atoms) and no lone pairs.
- The total number of regions of electron density around sulfur is 6 (all bonding pairs).
- A six-region electron configuration leads to an octahedral geometry, which requires sp³d² hybridization.
- Therefore, the sulfur atom in SF₆ is sp³d² hybridized.
Thus, the hybridization sequence follows: sp³ for SF₂, sp³d for SF₄, and sp³d² for SF₆.
This pattern corresponds to option b.