When dealing with oxidation and reduction reactions, keep in mind that many compounds can function as both oxidizing and reducing agents depending on the conditions. SO\(_2\) is a classic example of such a compound.
PH\(_3\) shows lower proton affinity than NH\(_3\).
PF\(_3\) exists but NF\(_5\) does not.
NO\(_2\) can dimerise easily.
SO\(_2\) can act as an oxidizing agent, but not as a reducing agent.
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The Correct Option isD
Solution and Explanation
Statement (1): PH\(_3\) has lower proton affinity than NH\(_3\), which is true. The lone pair in NH\(_3\) is less hindered, and thus NH\(_3\) can donate the lone pair more easily than PH\(_3\), making PH\(_3\) less basic. Statement (2): PF\(_3\) exists, but NF\(_5\) does not, which is also correct. NF\(_5\) is not stable due to the larger atomic radius and the lack of sufficient electronegativity to stabilize the structure. Statement (3): NO\(_2\) can easily dimerize to form N\(_2\)O\(_4\), which is true under normal conditions. Statement (4): SO\(_2\) can act both as an oxidizing agent and a reducing agent. SO\(_2\) can reduce to SO\(_3\) and also oxidize to other compounds like sulfuric acid. Hence, the statement in option (4) is incorrect. Thus, the incorrect statement is Statement (4).
