In `Znaps(Zn^(2+))abs(Cu^(2+))Cu`, the following is correct:

Options

A. Zn undergoes reduction
B. Cu undergoes reduction
C. `Cu^(2+)` undergoes reduction
D. None of the above

Answer

To solve the question regarding the reaction between zinc and copper ions, we need to analyze the oxidation states of the elements involved and determine which statements about oxidation and reduction are correct.

### Step-by-Step Solution:

1. **Identify the Reactants and Products**:
- The reaction can be written as:
\[ \text{Zn} + \text{Cu}^{2+} \rightarrow \text{Zn}^{2+} + \text{Cu} \]
- Here, zinc (Zn) is in its elemental form, and copper is in the form of copper ions (Cu²⁺).

2. **Determine the Oxidation States**:
- In the reactants:
- Zinc (Zn) has an oxidation state of 0 (elemental state).
- Copper (Cu²⁺) has an oxidation state of +2.
- In the products:
- Zinc (Zn²⁺) has an oxidation state of +2.
- Copper (Cu) has an oxidation state of 0 (elemental state).

3. **Identify Oxidation and Reduction**:
- **Oxidation**: This is the process where an element increases its oxidation state. In this case, zinc goes from 0 to +2, indicating that it is oxidized.
- **Reduction**: This is the process where an element decreases its oxidation state. Here, copper goes from +2 to 0, indicating that it is reduced.

4. **Summarize the Changes**:
- Zinc is oxidized (0 to +2).
- Copper is reduced (+2 to 0).

5. **Evaluate the Statements**:
- **Statement 1**: "Zinc undergoes reduction." - This is incorrect because zinc is oxidized.
- **Statement 2**: "Copper undergoes reduction." - This is misleading because it states that copper itself undergoes reduction, but it is actually the Cu²⁺ ion that is reduced.
- **Statement 3**: "Cu²⁺ undergoes reduction." - This is correct because Cu²⁺ is reduced to Cu (0).

### Conclusion:
The correct statement is that Cu²⁺ undergoes reduction.