Which statement is wrong:

Options

A. Bond energy of `F_(2) gt CI_(2)`
B. Electronegatively of `F gt CI`
C. F is more oxidising than CI
D. Electron affinity of `CI gt F`

Answer

To determine which statement is wrong, we will analyze each option provided in the question.

### Step-by-Step Solution:

1. **Understanding Bond Energies**:
- Bond energy refers to the amount of energy required to break a bond between two atoms. Generally, smaller atoms with high electronegativity can have weaker bonds due to electron repulsion.

2. **Analyzing Option 1**:
- The statement is: "Bond energy of F2 is greater than Cl2."
- Fluorine (F) is a smaller atom compared to chlorine (Cl). Due to its small size, the electron-electron repulsion between the two fluorine atoms in F2 is significant, which leads to a weaker bond compared to Cl2.
- Therefore, this statement is incorrect because the bond energy of F2 is actually less than that of Cl2.

3. **Analyzing Option 2**:
- The statement is: "Fluorine is the most electronegative element."
- This statement is correct. Fluorine has the highest electronegativity value in the periodic table.

4. **Analyzing Option 3**:
- The statement is: "Chlorine is more oxidizing than fluorine."
- This statement is incorrect. Fluorine is a stronger oxidizing agent than chlorine due to its higher electronegativity.

5. **Analyzing Option 4**:
- The statement is: "Electron affinity of Cl is greater than F."
- This statement is also incorrect. Fluorine has a higher electron affinity than chlorine because it is more electronegative and has a greater tendency to attract electrons.

### Conclusion:
The wrong statement is **Option 1**: "Bond energy of F2 is greater than Cl2."