Charge distribution in iodine monochloride is best represented as

Options

A. `I^+ Cl^+`
B. `I^(delta)Cl^(delta-)`
C. `I^(-) Cl^(+)`
D. `I^(delta-) Cl^(delta+)`

Answer

To determine the charge distribution in iodine monochloride (ICl), we need to analyze the electronegativity of the atoms involved and the nature of the bond formed between them.

### Step-by-Step Solution:

1. **Identify the Elements**:
- Iodine monochloride consists of two elements: iodine (I) and chlorine (Cl).

2. **Understand Electronegativity**:
- Electronegativity is the tendency of an atom to attract electrons towards itself in a bond.
- In the periodic table, electronegativity generally increases across a period and decreases down a group.

3. **Compare Electronegativity of Iodine and Chlorine**:
- Chlorine (Cl) is more electronegative than iodine (I).
- Typical electronegativity values: Cl ≈ 3.16 and I ≈ 2.66.

4. **Determine the Nature of the Bond**:
- Since chlorine is more electronegative than iodine, the bond between I and Cl will be polar covalent.
- In a polar covalent bond, electrons are not shared equally; they are pulled closer to the more electronegative atom.

5. **Assign Partial Charges**:
- Due to the difference in electronegativity, chlorine will have a partial negative charge (δ-) because it attracts the shared electrons more strongly.
- Iodine will have a partial positive charge (δ+) as it has a weaker attraction for the shared electrons.

6. **Represent the Charge Distribution**:
- The charge distribution in iodine monochloride can be represented as:
- I (δ+) — Cl (δ-)

7. **Conclusion**:
- Therefore, the charge distribution in iodine monochloride is best represented with iodine having a partial positive charge and chlorine having a partial negative charge.

### Final Answer:
The charge distribution in iodine monochloride (ICl) is best represented as I (δ+) — Cl (δ-).