The order of covalent character of KF, Kl, KCl is

Options

A. KCl lt KF lt KI
B. KI lt KCl lt KF
C. KF lt KI lt KCl
D. KF lt KCl lt KI

Answer

To determine the order of covalent character of KF, KCl, and KI, we need to analyze the electronegativity differences between potassium (K) and the halogens (F, Cl, I).

### Step-by-Step Solution:

1. **Identify the Electronegativity Values**:
- The electronegativity values of the halogens are approximately:
- Fluorine (F): 4.0
- Chlorine (Cl): 3.0
- Iodine (I): 2.5

2. **Calculate the Electronegativity Differences**:
- Since potassium (K) has a fixed electronegativity value (approximately 0.8), we can calculate the differences:
- For KF:
\[ \text{Difference} = |4.0 - 0.8| = 3.2 \]
- For KCl:
\[ \text{Difference} = |3.0 - 0.8| = 2.2 \]
- For KI:
\[ \text{Difference} = |2.5 - 0.8| = 1.7 \]

3. **Analyze the Electronegativity Differences**:
- The larger the difference in electronegativity, the more ionic the character of the bond. Conversely, a smaller difference indicates a greater covalent character.
- From the calculations:
- KF has the largest electronegativity difference (3.2) → more ionic character, less covalent character.
- KCl has a moderate electronegativity difference (2.2).
- KI has the smallest electronegativity difference (1.7) → more covalent character.

4. **Determine the Order of Covalent Character**:
- Since KI has the smallest electronegativity difference, it has the highest covalent character.
- KCl has a moderate covalent character.
- KF has the least covalent character.
- Therefore, the order of covalent character is:
\[ \text{KI} > \text{KCl} > \text{KF} \]

### Final Answer:
The order of covalent character of KF, KCl, KI is:
\[ \text{KI} > \text{KCl} > \text{KF} \]