The reaction
`3ClO^(ө)(aq)rarrClO_(3)^(-)(aq)+2Cl^(ө)(aq)`
is an example of

Options

A. Oxidation
B. Reduction
C. Disproprtionation
D. Decomposition

Explanation

To determine the type of reaction represented by the equation:

\[ 3 \text{ClO}^- (aq) \rightarrow \text{ClO}_3^- (aq) + 2 \text{Cl}^- (aq) \]

we will analyze the oxidation states of chlorine in the reactants and products.

### Step 1: Identify the oxidation states of chlorine in the reactants
In the reactant \( \text{ClO}^- \):
- Let the oxidation state of chlorine be \( x \).
- The oxidation state of oxygen is \(-2\).
- The overall charge of the ion is \(-1\).

Setting up the equation:
\[ x + (-2) = -1 \]
\[ x - 2 = -1 \]
\[ x = +1 \]

So, the oxidation state of chlorine in \( \text{ClO}^- \) is \( +1 \).

### Step 2: Identify the oxidation states of chlorine in the products
In the product \( \text{ClO}_3^- \):
- Let the oxidation state of chlorine be \( y \).
- The oxidation state of oxygen is \(-2\).
- There are three oxygen atoms, contributing \(-6\) to the overall charge.

Setting up the equation:
\[ y + 3(-2) = -1 \]
\[ y - 6 = -1 \]
\[ y = +5 \]

So, the oxidation state of chlorine in \( \text{ClO}_3^- \) is \( +5 \).

### Step 3: Identify the oxidation states of chlorine in the other product
In the product \( \text{Cl}^- \):
- The oxidation state of chlorine is \(-1\).

### Step 4: Determine the changes in oxidation states
- Chlorine in \( \text{ClO}^- \) changes from \( +1 \) to \( +5 \) (oxidation).
- Chlorine in \( \text{ClO}^- \) also changes from \( +1 \) to \( -1 \) (reduction).

### Step 5: Conclusion
Since chlorine undergoes both oxidation (increase in oxidation state) and reduction (decrease in oxidation state) in the same reaction, this reaction is classified as a **disproportionation reaction**.

### Final Answer
The reaction is an example of **disproportionation**.

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