Solubility of iodine in `CS_2` is due to :

Options

A. Van der Waal's forces
B. Ionic bond formation
C. Covalent bond attraction
D. Coordinate bond interaction

Answer

To determine the solubility of iodine (I2) in carbon disulfide (CS2), we need to analyze the nature of both substances and the type of interactions that can occur between them.

### Step-by-Step Solution:

1. **Identify the Nature of Iodine (I2)**:
- Iodine (I2) is a diatomic molecule consisting of two iodine atoms.
- Since both atoms have the same electronegativity, the bond between them is non-polar.
- Therefore, I2 is a non-polar molecule.

2. **Identify the Nature of Carbon Disulfide (CS2)**:
- CS2 has a linear structure with carbon (C) bonded to two sulfur (S) atoms.
- The C-S bonds have a slight electronegativity difference, but because the molecule is symmetrical, the dipoles cancel each other out.
- Thus, CS2 is also a non-polar molecule.

3. **Determine the Type of Interaction**:
- Since both I2 and CS2 are non-polar molecules, the primary type of interaction between them will be Van der Waals forces (also known as London dispersion forces).
- These forces arise due to temporary dipoles that occur when the electron distribution around non-polar molecules becomes uneven.

4. **Eliminate Other Options**:
- **Ionic Bond Formation**: This cannot occur as there are no metals involved and both molecules are non-polar.
- **Covalent Bond Attraction**: There is no formation of covalent bonds between I2 and CS2 as they do not share electrons in a bond.
- **Coordinate Bond Interaction**: This also does not apply since there is no donor-acceptor pair interaction between the two non-polar molecules.

5. **Conclusion**:
- The solubility of iodine in CS2 is primarily due to Van der Waals forces, which facilitate the interaction between the two non-polar molecules.

### Final Answer:
The solubility of iodine in CS2 is due to Van der Waals forces.