The bond strengths of the compounds HF, HCl, HBr, and HI are as follows:

Question

compound bond strength, kJ/mol
HF 569.87
HCl 431.62
HBr 366.35
HI 298.407
Briefly explain why the bond strengths are ranked in this order.

My guess is: They are ranked in this order because of the electronegativity value. The trend for electronegativity as go up and to the right of the periodic table, the electronegativity increases. Therefore, F would have the strongest bond, then Cl, Br, and I.

I don't think this is right because electronegativity was not in this chapter.

Answer 1

I think EN does have an influence, the other one is the size of the anion. The greater the distance (HI for example) the weaker the bond.