In the reaction `NO_(2)^(-)+OCl^(-) to NO_(3)^(-)+Cl^(-)` the oxidation state of chlorine

Options

A. Does not change
B. Changes from +1 to -1
C. Changes from -2 to -1
D. Changes from 0 to -1

Answer

To determine the change in the oxidation state of chlorine in the reaction \( NO_2^- + OCl^- \rightarrow NO_3^- + Cl^- \), we will analyze the oxidation states of chlorine in both the reactants and products.

### Step-by-Step Solution:

1. **Identify the Reactants and Products**:
- Reactants: \( OCl^- \) (hypochlorite ion)
- Products: \( Cl^- \) (chloride ion)

2. **Determine the Oxidation State of Chlorine in the Reactant \( OCl^- \)**:
- The oxidation state of oxygen (O) is typically -2.
- Let the oxidation state of chlorine (Cl) be \( x \).
- The overall charge of the ion \( OCl^- \) is -1.
- Set up the equation based on the sum of oxidation states:
\[ x + (-2) = -1 \]
- Solve for \( x \):
\[ x - 2 = -1 \\ x = -1 + 2 \\ x = +1 \]
- Therefore, the oxidation state of chlorine in \( OCl^- \) is +1.

3. **Determine the Oxidation State of Chlorine in the Product \( Cl^- \)**:
- In the chloride ion \( Cl^- \), the oxidation state of chlorine is -1.

4. **Compare the Oxidation States**:
- In the reactant \( OCl^- \), chlorine has an oxidation state of +1.
- In the product \( Cl^- \), chlorine has an oxidation state of -1.
- The change in oxidation state is from +1 to -1.

5. **Conclusion**:
- The oxidation state of chlorine changes from +1 in \( OCl^- \) to -1 in \( Cl^- \).

### Final Answer:
The oxidation state of chlorine changes from +1 to -1 in the reaction.

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