Which of the following halogens has metallic character ?

Options

A. `F_2`
B. `CI_2`
C. `Br_2`
D. `I_2`

Answer

To determine which of the following halogens has metallic character, we need to analyze the properties of the halogens provided: fluorine (F2), chlorine (Cl2), bromine (Br2), and iodine (I2).

### Step-by-Step Solution:

1. **Understanding Metallic Character**:
- Metallic character refers to the ability of an element to lose electrons and form positive ions (cations). Elements with metallic character typically have lower electronegativities and larger atomic radii.

2. **Position of Halogens in the Periodic Table**:
- Halogens are located in Group 17 (VIIA) of the periodic table. As we move down the group from fluorine to iodine, the atomic size increases.

3. **Comparing Atomic Sizes**:
- Fluorine is the smallest halogen, followed by chlorine, bromine, and then iodine, which is the largest. Larger atoms generally have weaker nuclear forces acting on their valence electrons.

4. **Evaluating Each Halogen**:
- **Fluorine (F2)**: Small size, high electronegativity, and strong attraction between nucleus and valence electrons. No metallic character.
- **Chlorine (Cl2)**: Larger than fluorine but still has a strong attraction to its valence electrons. No metallic character.
- **Bromine (Br2)**: Larger than chlorine, but still retains non-metallic properties. No metallic character.
- **Iodine (I2)**: The largest among the given halogens, with weaker nuclear forces acting on its valence electrons. This allows for the possibility of losing electrons more easily compared to the others.

5. **Conclusion**:
- Among the halogens listed, iodine (I2) exhibits the most metallic character due to its larger atomic size and weaker attraction between the nucleus and the valence electrons. Therefore, the answer is iodine.

### Final Answer:
**Iodine (I2)** has metallic character.