Nitrogen exists as N_2,whereas phosphorus exi | vedclass

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(A) Nitrogen has a small atomic size and high electronegativity,which allows it to form stable $p\pi - p\pi$ multiple bonds,leading to the formation o

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$p\pi - p\pi$ bonding is weak.

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(A) Nitrogen has a small atomic size and high electronegativity,which allows it to form stable $p\pi - p\pi$ multiple bonds,leading to the formation of diatomic $N_2$ molecules.In contrast,phosphorus has a larger atomic size,which makes the $p\pi - p\pi$ overlap ineffective and weak.Therefore,phosphorus prefers to form single $P-P$ bonds,resulting in a tetrahedral $P_4$ structure where each phosphorus atom is bonded to three other phosphorus atoms.

Nitrogen exists as $N_2$,whereas phosphorus exists as $P_4$. This is because ..........

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