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In case of nitrogen, \mathrm{NCl_{3}}  is possible but not \mathrm{NCl_{5}} while in case of phosphorus, \mathrm{PCl_{3}} as well as \mathrm{PCl_{5}} are possible. It is due to

Option: 1

availability of vacant \mathrm{d} orbitals in \mathrm{P} but not in \mathrm{N}


Option: 2

lower electronegativity of  \mathrm{P} than  \mathrm{N}


Option: 3

lower tendency of H-­bond formation in \mathrm{P} than  \mathrm{N}


Option: 4

occurrence of \mathrm{P} in solid while \mathrm{N} in gaseous state at room temperature.


Answers (1)

best_answer

As we have learnt ,

Nitrogen does not have vacant d orbitals to expand its octet whereas Phosphorus does.

Hence, Phosphorus can form compounds with an over expanded octet as it can accomodate those electrons in the vacant d orbital.

Therefore, option (1)  is correct.

Posted by

avinash.dongre

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