Identify the incorrect statement for $\mathrm{PCl}_{5}$ from the following.

(C) $\mathrm{PCl}_{5}$ has two axial bonds stronger than three equatorial bonds.

(A) In this molecule, orbitals of phosphorous are assumed to undergo $\mathrm{sp}^{3} \mathrm{~d}$ hybridization.

(B) The geometry of $\mathrm{PCl}_{5}$ is trigonal bipyramidal.

(D) The three equatorial bonds of $\mathrm{PCl}_{5}$ lie in a plane.

JEE Main · 2022 · 27 Jun 2022 · Shift 2 · Chemical Bonding and Molecular Structure

Identify the incorrect statement for

PCl_{5}

from the following.

(A)In this molecule, orbitals of phosphorous are assumed to undergo $sp^{3} d$ hybridization.
(B)The geometry of $PCl_{5}$ is trigonal bipyramidal.
(C) $PCl_{5}$ has two axial bonds stronger than three equatorial bonds.✓ Correct
(D)The three equatorial bonds of $PCl_{5}$ lie in a plane.

Answer: (C)

Solution

PCl_{5}

, phosphorus undergoes

sp^{3} d

hybridization forming a trigonal bipyramidal geometry. The three equatorial bonds lie in a plane and are stronger than the two axial bonds. The axial bonds are longer and weaker due to greater repulsion from the three equatorial bonds. Therefore, statement (C) is incorrect.

JEE Main · 2022 · 27 Jun 2022 · Shift 2 · Single correct option

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