Which of the following has maximum ionic character ?

Options

A. LiCl
B. NaCl
C. KCl
D. CsCl

Answer

To determine which of the given compounds has the maximum ionic character, we can use Fajans' rules, which state that the ionic character of a bond is influenced by the size and charge of the cation and anion involved in the bond.

### Step-by-Step Solution:

1. **Identify the Compounds**: The compounds given are:
- LiCl (Lithium Chloride)
- NaCl (Sodium Chloride)
- KCl (Potassium Chloride)
- CsCl (Cesium Chloride)

2. **Understand Fajans' Rules**: According to Fajans' rules:
- The ionic character increases with the size of the cation.
- The ionic character decreases with an increase in the charge of the cation.
- The ionic character decreases with the increase in the size of the anion.

3. **Analyze the Anion**: All the compounds listed have the same anion, Cl⁻ (chloride ion). Therefore, we only need to focus on the cations (Li⁺, Na⁺, K⁺, Cs⁺).

4. **Compare Cations**: The cations are:
- Li⁺ (Lithium)
- Na⁺ (Sodium)
- K⁺ (Potassium)
- Cs⁺ (Cesium)

As we move down the group in the periodic table (from Li to Cs), the size of the cation increases:
- Li⁺ < Na⁺ < K⁺ < Cs⁺

5. **Determine Ionic Character**: Since the ionic character is directly proportional to the size of the cation, Cs⁺, being the largest cation, will have the highest ionic character among the options given.

6. **Conclusion**: Therefore, CsCl (Cesium Chloride) has the maximum ionic character.

### Final Answer:
The compound with the maximum ionic character is **CsCl**.

---