Consider the following Assertion (A): Phospho | vedclass

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(C) Phosphorus has vacant $d$-orbitals in its valence shell, which allows it to expand its octet and form $PCl_5$ (phosphorus$(V)$ chloride) in additi

Vedclass · Accepted Answer

Both $(A)$ and $(R)$ are correct, $(R)$ is not the correct explanation of $(A)$

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(C) Phosphorus has vacant $d$-orbitals in its valence shell, which allows it to expand its octet and form $PCl_5$ (phosphorus$(V)$ chloride) in addition to $PCl_3$ (phosphorus$(III)$ chloride). Nitrogen, being in the second period, lacks vacant $d$-orbitals and cannot expand its octet beyond a covalency of $4$. Therefore, it cannot form $NCl_5$. The assertion $(A)$ is correct. The reason $(R)$ states that the electronegativity of nitrogen is higher than that of phosphorus, which is a true statement. However, the inability of nitrogen to form $NCl_5$ is due to the absence of vacant $d$-orbitals, not due to its electronegativity. Thus, $(R)$ is a true statement but not the correct explanation for $(A)$.

Consider the following Assertion $(A)$: Phosphorus can form both phosphorus$(III)$ and phosphorus$(V)$ chlorides, but nitrogen cannot form nitrogen$(V)$ chloride. Reason $(R)$: The electronegativity of nitrogen is more than that of phosphorus. The correct answer is

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