Question

Using VSEPR theory, choose the correct options regarding ${PCl}_5$ and ${BrF}_5$ molecules.

• A. ${PCl}_5$ has $s{p}^{3}d$ hybridization having a trigonal bipyramidal shape.
• B. ${BrF}_5$ has $s{p}^3{d}^2$ hybridization having an octahedral shape.
• C. There are five lone pairs of electrons around $P$.
• D. There are six lone pairs of electrons around $Br$.

Answer 1

Answer: (A), (B)

The correct options are
A ${PCl}_5$ has $s{p}^{3}d$ hybridization having a trigonal bipyramidal shape.
B ${BrF}_5$ has $s{p}^3{d}^2$ hybridization having an octahedral shape.

According to the VSEPR theory,

• $PC{l}_5$ is $s{p}^{3}d$ hybridized with $5$ sigma bond pairs and no lone pair on the central atom, $P$. Thus, it is trigonal bipyramidal in shape, with a bond angle of $\left({120}^{\circ }\right)$ .
  
• $Br{F}_5$is $s{p}^3{d}^2$ hybridized with $5$ sigma bond pairs and $1$ lone pair of electrons on the central atom, $Br$. Thus, its shape becomes square pyramidal due to the presence of a lone pair, but its basic shape isoctahedral $(bondangle={90}^{\circ })$.

Hence, options (A) and (B) are correct.