Which of the following statement is correct ? .

Options

A. `FeCI_(2)` is more covalent than `FeCI_(2)`
B. `FeCI_(3)` is more covalent than `FeCI_(2)`
C. Both `FeCI_(2)` and `FeCI_(3)` are equally covalent
D. `FeCI_(2)` and `FeCI_(3)` do not have any covalent character

Explanation

To determine which statement is correct regarding the covalent character of FeCl2 and FeCl3, we can follow these steps:

### Step 1: Understand the Compounds
- **FeCl2** contains iron in the +2 oxidation state (Fe²⁺) and chloride ions (Cl⁻).
- **FeCl3** contains iron in the +3 oxidation state (Fe³⁺) and chloride ions (Cl⁻).

### Step 2: Apply Feynman's Rule
- Feynman's rule states that the covalent character of an ionic compound increases with the polarization of the anion by the cation.
- Polarization occurs when the electron cloud of the anion is distorted by the cation.

### Step 3: Analyze Cation Size and Charge
- The ability of a cation to polarize an anion depends on its size and charge.
- A smaller cation with a higher charge has a greater polarizing power.
- In this case, Fe³⁺ (from FeCl3) is smaller and has a higher charge compared to Fe²⁺ (from FeCl2).

### Step 4: Compare Covalent Character
- Since Fe³⁺ is smaller and has a higher charge, it will polarize the chloride ion (Cl⁻) more effectively than Fe²⁺.
- Therefore, FeCl3 will exhibit more covalent character than FeCl2.

### Step 5: Conclusion
- Based on the analysis, the correct statement is:
- **Option B: FeCl3 is more covalent than FeCl2.**