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
Let's evaluate each statement to identify which one is incorrect:
PH3 shows lower proton affinity than NH3: This statement is correct. Ammonia (NH3) is more basic than phosphine (PH3) due to nitrogen's higher electronegativity, resulting in higher proton affinity.
PF3 exists but NF5 does not: This statement is accurate. Phosphorus readily forms PF3 with three available valence electrons. Fluorine forms a stable bond with phosphorus, whereas nitrogen has only three valence electrons and cannot form a stable NF5 compound.
NO2 can dimerise easily: This is true. Nitrogen dioxide (NO2) has an unpaired electron, which makes it highly reactive and likely to dimerize, forming dinitrogen tetroxide (N2O4).
SO2 can act as an oxidizing agent, but not as a reducing agent: This is incorrect. Sulfur dioxide (SO2) can indeed act as both an oxidizing and a reducing agent depending on the reacting chemical species, due to its ability to undergo both reduction and oxidation reactions.
Therefore, the incorrect statement is: SO2 can act as an oxidizing agent, but not as a reducing agent.
