Due to ppi - ppi bonding interactions, nitrog | vedclass

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(C) Nitrogen and phosphorus belong to the same group but have different atomic sizes. Due to the larger atomic size of phosphorus, the $3p-3p$ overlap

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$P_4$

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(C) Nitrogen and phosphorus belong to the same group but have different atomic sizes. Due to the larger atomic size of phosphorus, the $3p-3p$ overlap is not effective for forming $p\pi - p\pi$ bonds. Therefore, phosphorus exists as a tetra-atomic molecule, $P_4$, where each phosphorus atom is linked to $3$ other phosphorus atoms by $3$ sigma bonds. In contrast, nitrogen has a smaller atomic size, allowing for effective $2p-2p$ overlap, which leads to the formation of a triple bond ($1$ sigma and $2$ $\pi$ bonds) between two nitrogen atoms, resulting in a diatomic $N_2$ molecule.

Due to $p\pi - p\pi$ bonding interactions, nitrogen forms $N_2$ but phosphorus forms $X$ and does not form a diatomic molecule. Identify $X$.

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