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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
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availability of vacant $d$ orbitals in P but not in $\mathrm{N}$
${ }_{7} \mathrm{~N}=1 s^{2} 2 s^{2} 2 p^{3} ; \quad{ }_{15} \mathrm{P}=1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3}$
In phosphorous the $3 d$-orbitals are available. Hence phosphorus can form pentahalides also but nitrogen cannot form pentahalide due to absence of $d$-orbitals.
In phosphorous the $3 d$-orbitals are available. Hence phosphorus can form pentahalides also but nitrogen cannot form pentahalide due to absence of $d$-orbitals.
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