Statement-1 . `LiCl` is covalent whereas NaCl is ionic.
Statement-2. Greater the size of the cation, greater is its polarising power.

Options

A. Statement-1 is Ture , Statement-2 is Ture , Statement-2 is a correct explanation for Statement-1.
B. Statement-1 is Ture , Statement-2 is Ture , Statement-2 is not a correct explanation for Statement-1.
C. Statement-1 is True , Statement-2 is False .
D. Statement-1 is False, Statement-2 is True.

Explanation

To analyze the statements provided regarding the nature of `LiCl` and `NaCl`, we can break down the reasoning as follows:

### Step 1: Understanding Ionic and Covalent Bonds
- **Ionic Bonds**: Formed when there is a complete transfer of electrons from one atom to another, typically between metals and non-metals. The resulting ions are held together by electrostatic forces.
- **Covalent Bonds**: Formed when two atoms share electrons. This usually occurs between non-metals.

### Step 2: Analyzing LiCl
- Lithium (Li) is a small cation with a high charge density. Chlorine (Cl) is a larger anion.
- According to Fajans' rules, a small cation with a high charge can polarize the electron cloud of a larger anion, leading to covalent character in the bond.
- Therefore, `LiCl` exhibits more covalent character due to the small size and high polarizing power of the Li⁺ ion.

### Step 3: Analyzing NaCl
- Sodium (Na) is a larger cation compared to lithium. While Na⁺ can still polarize Cl⁻, it does so to a lesser extent than Li⁺ due to its larger size.
- As a result, `NaCl` is more ionic in nature because the bond is primarily formed through the electrostatic attraction between Na⁺ and Cl⁻ without significant polarization.

### Step 4: Evaluating the Statements
- **Statement-1**: `LiCl` is covalent whereas `NaCl` is ionic. This statement is true based on the analysis above.
- **Statement-2**: Greater the size of the cation, greater is its polarizing power. This statement is false. In fact, the opposite is true: smaller cations have greater polarizing power.

### Conclusion
- **Final Evaluation**: Statement-1 is true, and Statement-2 is false.