`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 will analyze the process step by step.

### Step-by-Step Solution:

1. **Understanding the Cu\(^+\) Ion**:
- The Cu\(^+\) ion, also known as the cuprous ion, is known to be unstable in aqueous solutions. This instability is key to understanding its behavior in water.

**Hint**: Remember that certain ions can be unstable in solution, leading to further reactions.

2. **Identifying the Reaction**:
- In an aqueous medium, the Cu\(^+\) ion undergoes a process known as disproportionation. Disproportionation is a specific type of redox reaction where a single substance is both oxidized and reduced.

**Hint**: Look for reactions where one species is transformed into two different products, indicating both oxidation and reduction.

3. **Oxidation and Reduction**:
- In the case of Cu\(^+\), it can be oxidized to Cu\(^{2+}\) (cupric ion) and reduced to elemental copper (Cu). Therefore, the reaction can be represented as:
\[ 2 \text{Cu}^+ \rightarrow \text{Cu}^{2+} + \text{Cu} \]
- Here, one Cu\(^+\) ion is oxidized to Cu\(^{2+}\) and another Cu\(^+\) ion is reduced to Cu (metal).

**Hint**: Identify the changes in oxidation states to determine which species is oxidized and which is reduced.

4. **Conclusion**:
- Since both oxidation and reduction occur simultaneously in this reaction, we conclude that the Cu\(^+\) ion undergoes disproportionation in aqueous medium.

**Hint**: When faced with multiple-choice questions, eliminate options that do not fit the observed reaction behavior.

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