`Cu^(+)ion` in aquous medium undergoes

Options

A. Oxidation only
B. Reduction only
C. Neither oxidation nor reduction
D. Disproportionation

Answer

To solve the question regarding the behavior of the Cu\(^+\) ion in an aqueous medium, we need to analyze the possible reactions that can occur.

### Step-by-Step Solution:

1. **Understanding the Cu\(^+\) Ion**:
- The copper ion in question is Cu\(^+\), which is a cuprous ion. It can either undergo oxidation or reduction depending on the conditions in the aqueous medium.

2. **Identifying Possible Reactions**:
- In an aqueous medium, Cu\(^+\) can either be oxidized to Cu\(^{2+}\) or can undergo a disproportionation reaction. Disproportionation is a specific type of redox reaction where a single substance is both oxidized and reduced.

3. **Considering Oxidation**:
- If Cu\(^+\) is oxidized, it would lose an electron to form Cu\(^{2+}\):
\[ \text{Cu}^+ \rightarrow \text{Cu}^{2+} + e^- \]

4. **Considering Disproportionation**:
- In a disproportionation reaction, Cu\(^+\) can convert into both Cu and Cu\(^{2+}\):
\[ 2 \text{Cu}^+ \rightarrow \text{Cu} + \text{Cu}^{2+} \]
- Here, one Cu\(^+\) ion is reduced to Cu (0 oxidation state), while another Cu\(^+\) ion is oxidized to Cu\(^{2+}\).

5. **Conclusion**:
- The Cu\(^+\) ion in aqueous medium can undergo disproportionation. Therefore, the correct answer is that Cu\(^+\) undergoes a disproportionation reaction.

### Final Answer:
The Cu\(^+\) ion in aqueous medium undergoes a disproportionation reaction.

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