Identify the oxidant and the reductant respectively in the following reaction.
`Cl_(2)(g) + 2Br^(-)(aq) to 2Cl^(-)(aq) + Br_(2)(aq)`

Options

A. Chlorine and Bromide
B. Bromide and Chlorine
C. Bromide and Bromide
D. Chlorine and Chlorine

Explanation

To identify the oxidant and the reductant in the reaction:

\[ \text{Cl}_2(g) + 2\text{Br}^-(aq) \rightarrow 2\text{Cl}^-(aq) + \text{Br}_2(aq) \]

we can follow these steps:

### Step 1: Identify the oxidation states of the elements in the reaction.

- In the reactants:
- For \(\text{Cl}_2\), the oxidation state of chlorine (Cl) is 0 because it is in its elemental form.
- For \(\text{Br}^-\), the oxidation state of bromine (Br) is -1.

- In the products:
- For \(\text{Cl}^-\), the oxidation state of chlorine is -1.
- For \(\text{Br}_2\), the oxidation state of bromine is 0 because it is in its elemental form.

### Step 2: Determine the changes in oxidation states.

- Chlorine changes from 0 (in \(\text{Cl}_2\)) to -1 (in \(\text{Cl}^-\)). This indicates that chlorine is gaining electrons and is therefore being reduced.
- Bromine changes from -1 (in \(\text{Br}^-\)) to 0 (in \(\text{Br}_2\)). This indicates that bromine is losing electrons and is therefore being oxidized.

### Step 3: Identify the oxidant and reductant.

- The substance that gets reduced (gains electrons) is the oxidizing agent (oxidant). In this case, chlorine (\(\text{Cl}_2\)) is the oxidant.
- The substance that gets oxidized (loses electrons) is the reducing agent (reductant). In this case, bromide ion (\(\text{Br}^-\)) is the reductant.

### Conclusion:

Thus, the oxidant is \(\text{Cl}_2\) and the reductant is \(\text{Br}^-\).

### Final Answer:
- Oxidant: \(\text{Cl}_2\)
- Reductant: \(\text{Br}^-\)

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