Nitrogen forms N_2,but phosphorus is converte | vedclass

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(B) Nitrogen forms a stable $N \equiv N$ triple bond due to effective $p\pi - p\pi$ overlapping,which is possible because of its small size. In the ca

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$P-P$ single bond is weaker than $P \equiv P$ bond.

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(B) Nitrogen forms a stable $N \equiv N$ triple bond due to effective $p\pi - p\pi$ overlapping,which is possible because of its small size. In the case of phosphorus,the atomic size is larger,making $p\pi - p\pi$ overlapping ineffective. Therefore,phosphorus prefers to form three $P-P$ single bonds rather than one $P \equiv P$ triple bond. As a result,phosphorus exists as $P_4$ molecules where each phosphorus atom is linked by single bonds.

Nitrogen forms $N_2$,but phosphorus is converted from $P_2$ to $P_4$. Which of the following is the reason for this?

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