Question

Which of the following molecules are polar and $s{p}^3{d}^2$ hybridized?

• A. $I{F}_5$
• B. $Xe{F}_4$
• C. $XeO{F}_4$
• D. $IC{l}_4^{-}$

Answer 1

Answer: (A), (C)

$I{F}_5$
$XeO{F}_4$

$\left(A\right)$ $I{F}_5$ has $5$ bond pairs and $1$ lone pair of electrons on the central iodine atom. It undergoes $s{p}^3{d}^2$ hybridization which results in square pyramidal geometry. The individual bond dipoles do not cancel each other and the molecule is polar.
$\left(B\right)$ $Xe{F}_4$ has $4$ bond pairs of electrons and $2$ lone pairs of electrons on the central xenon atom. It undergoes $s{p}^3{d}^2$ hybridisation which results in square planar geometry. The individual bond dipoles cancel each other and the molecule is non-polar.
$\left(C\right)$ $XeO{F}_4$ has $5$ bonding domains and $1$ lone pair of electrons on the central Xe atom. It undergoes $s{p}^3{d}^2$ hybridization and has square planar geometry. The molecule is polar.
$\left(D\right)$ $IC{l}_4^{-}$ has $4$ bond pairs of electrons on the central iodine atom and $2$ orbitals contain non bonding electrons. It undergoes $s{p}^3{d}^2$ hybridization with square planar geometry. The individual bond dipoles cancel each other and the molecule is non-polar.

Hence, both $I{F}_5$ and $XeO{F}_4$ are polar and $s{p}^3{d}^2$ hybridised.