Which of the following has the highest value of `E_("red")^(@)` ?

Options

A. `P_(4)`
B. `Cl_(2)`
C. `I_(2)`
D. `F_(2)`

Answer

To determine which of the given species has the highest standard reduction potential (E°_red), we will analyze the provided options: P4, Chlorine (Cl2), Iodine (I2), and Fluorine (F2).

### Step-by-Step Solution:

1. **Understanding Standard Reduction Potential (E°_red)**:
- The standard reduction potential is a measure of the tendency of a chemical species to acquire electrons and thereby be reduced. A higher E°_red value indicates a stronger oxidizing agent.

2. **Reviewing the Options**:
- We have four species to consider: P4, Cl2, I2, and F2.

3. **Consulting the Electrochemical Series**:
- The electrochemical series lists the standard reduction potentials for various half-reactions. We will look for the E°_red values for the species in question.

4. **Finding E°_red Values**:
- From the electrochemical series:
- **Fluorine (F2)**: E°_red = +2.87 V
- **Chlorine (Cl2)**: E°_red = +1.36 V
- **Iodine (I2)**: E°_red = +0.54 V
- **Phosphorus (P4)**: Not listed in the electrochemical series as it does not have a standard reduction potential.

5. **Comparing the Values**:
- Now we compare the E°_red values:
- F2: +2.87 V
- Cl2: +1.36 V
- I2: +0.54 V
- P4: Not applicable

6. **Conclusion**:
- Among the given species, Fluorine (F2) has the highest standard reduction potential of +2.87 V. This indicates that F2 is the strongest oxidizing agent among the options provided.

### Final Answer:
The species with the highest value of E°_red is **Fluorine (F2)**.

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