Statement-1 : In LiCl more covalent character is present in LiF.
and
Statement-2 : Polarizability of `Br^(-)` is more than `Cl^(-)`

Options

A. (A) Statement-1 is True , Statement-2 is True , Statement-2 is a correct explanation for Statement-1
B. (B) Statement-1 is True , Statement-2 is True , Statement-2 is NOT a correct explanation for Statement-1
C. (C) Statement-1 is True , Statement-2 is False
D. (D) Statement-1 is False , Statement-2 is True

Answer

To analyze the statements given in the question, we will break down the reasoning step by step.

### Step 1: Understanding Statement 1
**Statement 1:** In LiCl, more covalent character is present than in LiF.

- To evaluate this statement, we need to consider the nature of the bonds formed in LiF and LiCl.
- LiF consists of Li^+ and F^− ions, while LiCl consists of Li^+ and Cl^− ions.
- According to Fajans' rules, the covalent character of an ionic bond increases with the size of the anion and the charge on the anion.
- The size of Cl^− is larger than that of F^−. Therefore, Cl^− can polarize the Li^+ ion more effectively than F^− can polarize it.

**Conclusion for Statement 1:** Since Cl^− is larger, LiCl has more covalent character than LiF. Thus, Statement 1 is **True**.

### Step 2: Understanding Statement 2
**Statement 2:** Polarizability of Br^− is more than Cl^−.

- Polarizability refers to the ability of an anion's electron cloud to be distorted by an external electric field or by nearby cations.
- Generally, larger anions have greater polarizability because their electron clouds are held less tightly by the nucleus and can be distorted more easily.
- Comparing Br^− and Cl^−, Br^− is larger in size than Cl^−. Thus, Br^− will have a higher polarizability.

**Conclusion for Statement 2:** Since Br^− is larger than Cl^−, it has more polarizability. Therefore, Statement 2 is **True**.

### Step 3: Relationship Between the Statements
- Statement 2 provides an explanation for why LiCl has more covalent character than LiF. The larger size and higher polarizability of Cl^− compared to F^− contribute to the increased covalent character in LiCl.
- Thus, Statement 2 correctly explains Statement 1.

### Final Conclusion
Both statements are true, and Statement 2 correctly explains Statement 1. Therefore, the correct answer is that both statements are true, and Statement 2 is a correct explanation for Statement 1.