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The solid $PCl_{5}$ exists as

Option 1)
$PCl_{3}$

Option 2)
$PCl_{4}^{+}$

Option 3)
$PCl_{6}^{-}$

Option 4)
$PCl_{4}^{+}\, \, and\, \, PCl_{6}^{-}$

Answers (1)

best_answer

As we learnt in

Structure of phosphorus pentachloride -

Trigonal bipyramidal structure (liquid and gas). In solid state as $\left [ PCl_{4} \right ]^{+} \left [ PCl_{6} \right ]^{-} , \left [ PCl_{4} \right ]^{+}$ is tetrahedral and $[ PCl_{6} \right ]]^{-}$ is octahedral.

- wherein

In solid state Phosphorus Pentochloride exists as $\left [ PCl_{4} \right ]^{+} \left [ PCl_{6} \right ]^{-}\ where\ \left [ PCl_{4} \right ]^{+}$ is thetrahedral and $[ PCl_{6} \right ]]^{-}$ is Octahedral.

Option 1)

$PCl_{3}$

This option is incorrect

Option 2)

$PCl_{4}^{+}$

This option is incorrect

Option 3)

$PCl_{6}^{-}$

This option is incorrect

Option 4)

$PCl_{4}^{+}\, \, and\, \, PCl_{6}^{-}$

This option is correct

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