`CI_(2)+2OH^(-) rarr CIO^(-)+CI^(-)` is a __________ type of reaction.

Answer

To determine the type of reaction represented by the equation \( \text{Cl}_2 + 2\text{OH}^- \rightarrow \text{ClO}^- + \text{Cl}^- \), we can analyze the oxidation states of the chlorine atoms involved in the reaction.

### Step 1: Identify the Reactants and Products
The reactants are chlorine gas (\( \text{Cl}_2 \)) and hydroxide ions (\( \text{OH}^- \)). The products are hypochlorite ions (\( \text{ClO}^- \)) and chloride ions (\( \text{Cl}^- \)).

### Step 2: Determine the Oxidation States
- In \( \text{Cl}_2 \), the oxidation state of chlorine is 0 (since it is in its elemental form).
- In \( \text{ClO}^- \), the oxidation state of chlorine can be calculated as follows:
- Let the oxidation state of Cl be \( x \).
- The equation for the hypochlorite ion is \( x + (-2) = -1 \) (since oxygen has an oxidation state of -2).
- Solving this gives \( x = +1 \).
- In \( \text{Cl}^- \), the oxidation state of chlorine is -1.

### Step 3: Analyze the Changes in Oxidation States
- The oxidation state of chlorine changes from 0 in \( \text{Cl}_2 \) to +1 in \( \text{ClO}^- \) (oxidation).
- The oxidation state of chlorine changes from 0 in \( \text{Cl}_2 \) to -1 in \( \text{Cl}^- \) (reduction).

### Step 4: Identify the Type of Reaction
Since the same element (chlorine) is undergoing both oxidation (increase in oxidation state) and reduction (decrease in oxidation state) in the same reaction, this is classified as a **disproportionation reaction**.

### Conclusion
The reaction \( \text{Cl}_2 + 2\text{OH}^- \rightarrow \text{ClO}^- + \text{Cl}^- \) is a **disproportionation reaction**.

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