The chemical reaction:
`Zn^(2+)+2e^(-)rarrZn`
Is an example of

Options

A. Redox process
B. Reversible process
C. Oxidation
D. Reduction

Explanation

To determine what type of chemical reaction is represented by the equation:

\[ \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn} \]

we can analyze the reaction step by step.

### Step 1: Identify the Species Involved
In the reaction, we have:
- **Zn²⁺**: This is the zinc ion with a +2 charge.
- **2e⁻**: These are two electrons.
- **Zn**: This is the elemental form of zinc, which has an oxidation state of 0.

### Step 2: Determine the Change in Oxidation State
- The oxidation state of Zn²⁺ is +2.
- The oxidation state of Zn (metal) is 0.

Since Zn²⁺ is gaining electrons (2 electrons in this case), it is undergoing a reduction process. Reduction is defined as the gain of electrons, which results in a decrease in oxidation state.

### Step 3: Classify the Reaction
Since the reaction involves the gain of electrons by Zn²⁺, it is classified as a **reduction reaction**.

### Step 4: Consider the Options Given
The options provided in the question are:
1. Redox process
2. Reversible process
3. Oxidation process
4. Reduction process

Since we have established that the reaction is a reduction process (Zn²⁺ is reduced to Zn), the correct answer is:

**Reduction process.**

### Final Answer
The chemical reaction \( \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn} \) is an example of a **reduction process**.

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