The structure of $\mathrm{PCl}_{5}$ in the solid state is:

(C) tetrahedral $\left[\mathrm{PCl}_{4}\right]^{+}$ and octahedral $\left[\mathrm{PCl}_{6}\right]^{-}$

(A) square planar $\left[\mathrm{PCl}_{4}\right]^{+}$ and octahedral $\left[\mathrm{PCl}_{6}\right]^{-}$

JEE Main · 2020 · 05 Sep 2020 · Shift 1 · p-Block Elements

The structure of

PCl_{5}

in the solid state is:

(A)square planar $[PCl_{4}]^{+}$ and octahedral $[PCl_{6}]^{-}$
(B)trigonal biphyramidal
(C)tetrahedral $[PCl_{4}]^{+}$ and octahedral $[PCl_{6}]^{-}$ ✓ Correct
(D)square pyramidal

Answer: (C)

Solution

Solid

P C l_{5}

is an ionic solid built from

[P C l_{4}]^{+}

and

[P C l_{6}]^{-}

ions. In the cation phosphorus forms four bond pairs with no lone pair, so it is

s p^{3}

hybridised and tetrahedral; in the anion phosphorus forms six bond pairs, so it is

s p^{3} d^{2}

hybridised and octahedral. Describing

[P C l_{4}]^{+}

as square planar is wrong, since a four-coordinate centre carrying no lone pair must be tetrahedral.

JEE Main · 2020 · 05 Sep 2020 · Shift 1 · Single correct option

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