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)
P Prateek Shrivastava

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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