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.
Show Solution
The Correct Option isD
Solution and Explanation
Examining each assertion to identify the inaccurate one:
PH3 exhibits a lower proton affinity than NH3.
This is accurate. Phosphorus (P) is larger than nitrogen (N), leading to a reduced propensity for PH3 to accept a proton relative to NH3, hence a lower proton affinity.
PF3 is stable, whereas NF5 is not.
This statement is valid. PF3 forms a stable compound. NF5, however, is nonexistent because nitrogen, with only five valence electrons, cannot exceed its octet and accommodate five fluorine atoms.
NO2 readily undergoes dimerization.
This statement is true. The presence of unpaired electrons facilitates the facile dimerization of NO2 into N2O4.
SO2 functions as an oxidizing agent but not as a reducing agent.
This statement is false. SO2 can function as both an oxidizing and a reducing agent. It can be reduced to sulfur or oxidize other species to form SO42- ions.
The correct identification of the incorrect statement is: "SO2 can act as an oxidizing agent, but not as a reducing agent."
