Write redox reactions between fluorine and water.

Explanation

To write the redox reactions between fluorine and water, we need to analyze the processes involved. Fluorine (F2) is a strong oxidizing agent and can react with water (H2O) to produce oxygen gas (O2), hydrogen ions (H+), and fluoride ions (F-).

### Step-by-Step Solution:

1. **Identify the Reactants**:
- The reactants in this reaction are fluorine gas (F2) and liquid water (H2O).

2. **Determine the Products**:
- The products of the reaction are oxygen gas (O2), hydrogen ions (H+), and fluoride ions (F-).

3. **Write the Balanced Redox Reaction**:
- The balanced redox reaction can be written as follows:
\[ 2 \, \text{F}_2(g) + 2 \, \text{H}_2\text{O}(l) \rightarrow 4 \, \text{HF}(aq) + \text{O}_2(g) \]
- This equation shows that fluorine oxidizes water, resulting in the formation of hydrogen fluoride (HF) and oxygen gas.

4. **Identify Oxidation and Reduction**:
- In this reaction, fluorine (F2) is reduced to fluoride ions (F-), and water (H2O) is oxidized to oxygen (O2).
- The oxidation half-reaction is:
\[ 2 \, \text{H}_2\text{O} \rightarrow \text{O}_2 + 4 \, \text{H}^+ + 4 \, e^- \]
- The reduction half-reaction is:
\[ 2 \, \text{F}_2 + 4 \, e^- \rightarrow 4 \, \text{F}^- \]

5. **Combine the Half-Reactions**:
- By combining the oxidation and reduction half-reactions, we confirm the overall balanced redox reaction.

### Final Balanced Redox Reaction:
\[ 2 \, \text{F}_2(g) + 2 \, \text{H}_2\text{O}(l) \rightarrow 4 \, \text{HF}(aq) + \text{O}_2(g) \]