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 the type of chemical reaction represented by the equation:

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

we can analyze the reaction step by step.

### Step 1: Identify the components of the reaction
The reaction involves zinc ions (\( \text{Zn}^{2+} \)) and electrons (\( 2e^- \)), which combine to form elemental zinc (\( \text{Zn} \)).

### Step 2: Understand oxidation and reduction
In electrochemistry, oxidation refers to the loss of electrons and an increase in oxidation state, while reduction refers to the gain of electrons and a decrease in oxidation state.

### Step 3: Determine the oxidation states
- In the reactant \( \text{Zn}^{2+} \), the oxidation state of zinc is +2.
- In the product \( \text{Zn} \), the oxidation state of zinc is 0.

### Step 4: Analyze the change in oxidation state
The change in oxidation state from +2 (in \( \text{Zn}^{2+} \)) to 0 (in \( \text{Zn} \)) indicates a decrease in oxidation state. This decrease signifies that zinc is gaining electrons.

### Step 5: Conclude the type of reaction
Since the reaction involves the gain of electrons by zinc, it is classified as a reduction reaction.

Thus, the chemical reaction \( \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn} \) is an example of **reduction**.

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