Nitrogen forms N_2,but phosphorus prefers to | vedclass

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(C) Nitrogen has a small atomic size and high electronegativity,which allows it to form stable $p\pi-p\pi$ multiple bonds,resulting in the diatomic $N

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

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(C) Nitrogen has a small atomic size and high electronegativity,which allows it to form stable $p\pi-p\pi$ multiple bonds,resulting in the diatomic $N_2$ molecule.In contrast,phosphorus has a larger atomic size,which makes the effective overlap of $p$-orbitals for $p\pi-p\pi$ bonding difficult.Therefore,phosphorus prefers to form three $P-P$ single bonds rather than one $P \equiv P$ triple bond.Since the $P-P$ single bond is much stronger than the $\pi$-component of the $P \equiv P$ bond,phosphorus exists as a tetrahedral $P_4$ molecule.

Nitrogen forms $N_2$,but phosphorus prefers to exist as $P_4$ rather than $P_2$. Which of the following is the reason for this?

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