Intermolecular forces of attraction are more in

Options

A. Fluorine
B. Iodine
C. Bromine
D. Chlorine

Answer

### Step-by-Step Solution:

1. **Understanding Intermolecular Forces**: Intermolecular forces are the forces of attraction or repulsion between neighboring particles (molecules, atoms, or ions). In this case, we are focusing on halogens: fluorine, chlorine, bromine, and iodine.

2. **Identifying the Type of Intermolecular Forces**: For the halogens mentioned, the primary type of intermolecular force present is London dispersion forces (also known as van der Waals forces). These forces arise due to temporary dipoles that occur when electron distributions around atoms fluctuate.

3. **Analyzing the Halogens**: The halogens in question are:
- Fluorine (F)
- Chlorine (Cl)
- Bromine (Br)
- Iodine (I)

4. **Comparing Atomic Sizes**: The strength of London dispersion forces increases with the size of the atom. This is because larger atoms have more electrons, which can lead to greater polarizability (the ability to form temporary dipoles).

5. **Order of Atomic Size**: The atomic sizes of the halogens increase as follows:
- Fluorine (smallest)
- Chlorine
- Bromine
- Iodine (largest)

6. **Conclusion on Intermolecular Forces**: Since iodine is the largest atom among the given halogens, it will have the strongest London dispersion forces due to its greater polarizability. Therefore, the intermolecular forces of attraction are the strongest in iodine.

7. **Final Answer**: The intermolecular forces of attraction are more in **iodine (option B)**.