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 additio

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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