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In PCl(5) phosphorus is in sp^(3) d hybr...

In `PCl_(5)` phosphorus is in `sp^(3)` d hybridised state but all its five bonds are not equivalent. Justify your answer with reason.

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`PCl_(5)` has trigonal bipyramid geometry. It has three equatorial and two axial bonds. Since each axial P-Cl bond is repelled by three bond pairs and each equatorial P-Ci bond is repelled by only two bond pairs, therefore, axial bonds are longer (240 pm) than equatorial bonds (202 pm) than equatorial bonds (202 pm). Thus, all the five P-Cl bonds in `PCl_(5)` are nt equivalent.
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Explore conceptually related problems

(a) Why does PCl_3 fume in moisture ? (b) Are all the five bonds in PCl_5 molecule equivalent ? Justify your answer. ( c) How do you account for the reducing behaviour of H_3 PO_2 on the basic of its structure ? (d) Give the disproportional reaction of H_3PO_3 .

All bonds in the molecule of PCl_(5) are not equivalent. Explain.

The hybrid states of phosphorous atoms in each PCl_(5) and PBr_(5) in gasesous phase are sp^(3)d . But, in solid PCl_(5) ,phosphorous shows sp^(3)d^(2) and sp^(3) hybrid states. While,P in PBr_(5) is in sp^(3) hybrid state. This is because:

All five bonds of PCl_(5) are not equilvalent and PCl_(5) is less stable. Explain.

Explain the structure of PCl_(5) according to hybridization. Why all P – Cl bonds lengths are not equivalent in PCl_(5) ?

PRADEEP-P-BLOCK ELEMENTS -SHORT ANSWER QUESTIONS
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  15. Nitric acid forms an oxide of nitrogen on reaction with P(4)O(10). Wri...

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  16. Phosphorus has three allotropic forms : (i) white phosphorus (ii) red ...

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