Question:
Explain the following:
(i) NCl\(_3\) occurs but NCl\(_5\) does not. Why?
(ii) Why are halogens strong oxidising agents?
Explain the following:
(i) NCl\(_3\) occurs but NCl\(_5\) does not. Why?
(ii) Why are halogens strong oxidising agents?
Show Hint
NCl\(_5\) cannot form as nitrogen lacks d-orbitals; halogens are strong oxidisers due to high electron affinity.
Updated On: Oct 7, 2025
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Solution and Explanation
(i) Explanation.
Nitrogen has only \(2s\) and \(2p\) orbitals, no vacant d-orbitals. Therefore, nitrogen cannot expand its octet to form NCl\(_5\). But phosphorus (in PCl\(_5\)) can, due to vacant 3d orbitals. Hence only NCl\(_3\) exists.
(ii) Explanation.
Halogens have high electronegativity and very high electron affinity. They readily accept electrons to form halide ions, making them strong oxidising agents.
Nitrogen has only \(2s\) and \(2p\) orbitals, no vacant d-orbitals. Therefore, nitrogen cannot expand its octet to form NCl\(_5\). But phosphorus (in PCl\(_5\)) can, due to vacant 3d orbitals. Hence only NCl\(_3\) exists.
(ii) Explanation.
Halogens have high electronegativity and very high electron affinity. They readily accept electrons to form halide ions, making them strong oxidising agents.
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