Dissoution of iodine crystals in carbon tetrachlorides solvent can be attributed to

Options

A. Hydeogen bonding between them
B. dipole-induced dipole interactin between them
C. London dispersion force between them
D. Large molecular mass of iodine and hence large van-der waals forces

Answer

To solve the question regarding the dissolution of iodine crystals in carbon tetrachloride (CCl4), we will follow these steps:

### Step 1: Identify the solute and solvent
- **Solute**: Iodine crystals (I2)
- **Solvent**: Carbon tetrachloride (CCl4)

### Step 2: Determine the nature of the solute and solvent
- Both iodine (I2) and carbon tetrachloride (CCl4) are **non-polar** substances. Non-polar substances do not have a significant dipole moment.

### Step 3: Understand the interactions involved in the dissolution process
- The dissolution of iodine in carbon tetrachloride can be attributed to **London dispersion forces** (also known as van der Waals forces). These forces arise due to temporary dipoles that occur when the electron distribution around the molecules fluctuates.

### Step 4: Evaluate the options provided
- **Option A**: Hydrogen bonding - Incorrect, as hydrogen bonding requires specific atoms (like H bonded to F, O, or N).
- **Option B**: Dipole-induced dipole - Incorrect, since both iodine and CCl4 are non-polar and do not have permanent dipoles.
- **Option C**: Dipole-dipole interactions - Incorrect, for the same reason as option B.
- **Option D**: London dispersion forces - Correct, as these forces are present between non-polar molecules and can facilitate the dissolution of iodine in CCl4.

### Step 5: Conclusion
- The dissolution of iodine crystals in carbon tetrachloride can be attributed to **London dispersion forces** due to the non-polar nature of both substances and the presence of temporary dipoles.

### Final Answer
The dissolution of iodine crystals in carbon tetrachloride solvent can be attributed to **London dispersion forces**.

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