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Chlorides of Phosphorus

Question

Which one of $P C l_{4}^{+}$ and $P C l_{4}^{-}$ is not likely to exist and why?

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Solution

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When phosphorous accepts 3 electrons from 3 chlorine atoms it completes its octet, so it is unable to take one more electron from one more $C l^{-}$ so the fomation of $P C l_{4}^{-}$ is difficult.

As we move down the group, the stability of +5 oxidation state decreases and the stability of +3 oxidation state increases. Chlorine belongs to third period. Hence, $P C l_{4}^{+}$ compound is more likely to exist.

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Similar Questions

Q1

Which one of

P C l_{4}^{+}

and

P C l_{4}^{-}

is not likely to exist and why?

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Q2

The shapes of

P C l_{4}^{+}, P C l_{4}^{-}

and

A s C l_{5}

are respectively:

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Q3

The shapes

P C l_{4}^{+}, P C l_{4}^{-}

and

A s C l_{5}

are respectively:

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Q4

In solid state $P C l_{5}$ exists as

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Q5

P C l_{5}

exists as solid in the form of

[P C l_{4}]^{+} [P C l_{6}]^{-}

, and it is a non conductor of electricity.

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