To solve the question, we need to analyze the given orders for oxidizing power, acidic strength, bond dissociation enthalpy, and boiling points of the halogens (F2, Cl2, Br2, I2) and their corresponding acids (HF, HCl, HBr, HI).
### Step-by-Step Solution:
1. **Understanding Oxidizing Power:**
- The order given is: F2 > Cl2 > Br2 > I2.
- This order is correct because fluorine is the most electronegative element, making it a strong oxidizing agent. As we move down the group, the electronegativity decreases, thus reducing oxidizing power.
2. **Understanding Acidic Strength:**
- The order given is: HF < HCl < HBr < HI.
- This order is also correct. As we move down the group, the bond strength between H and the halogen decreases, making it easier for the acid to donate a proton (H+). Therefore, HI is the strongest acid, and HF is the weakest due to the strong H-F bond.
3. **Understanding Bond Dissociation Enthalpy:**
- The order given is: HF > HCl > HBr > HI.
- This order is incorrect. The bond dissociation enthalpy decreases as we move down the group because the bond length increases and the bond strength decreases. The correct order should be: HCl > HBr > HI > HF. HF has a high bond dissociation enthalpy due to the small size of fluorine leading to strong bond formation, but the order places HF incorrectly at the top.
4. **Understanding Boiling Points:**
- The order given is: HF > HCl > HBr > HI.
- This order is correct. HF has a higher boiling point than the other hydrogen halides due to hydrogen bonding. As we move down the group, the boiling points increase due to increased Van der Waals forces, but HF remains higher due to its hydrogen bonding.
### Conclusion:
The incorrectly given order is for bond dissociation enthalpy, where the correct order should be HCl > HBr > HI > HF instead of HF > HCl > HBr > HI.
### Final Answer:
**Option C (Bond Dissociation Enthalpy) is incorrectly given according to the order indicated.**
