Character of Acids

[ELee_3F]

Hi! I understand that a strong acid loses H+ more easily than a weak acid, that H+ are more likely to be lost in weaker (longer) bonds, and that H+ are readily lost if the ion is stabilized by resonance. This being said, I'm confused on something we learned in class on 11/27. HF < HCl < HBr < HI and H2O < H2S < H2Se < H2Te due to bond length. However, When looking at hypochlorous acid, hypobromous acid, and hypoiodous acid, or ClOH, BrOH, andd IOH, ClOH is the most acidic. Professor Lavelle said this is due to Cl's property of electronegativity, but I'm confused as to why the bond lengths due not determine the acidity levels in these acids? Could someone clarify? Thanks!

[AnnabelleDeng2J]

The bonds lengths usually do not determine acidity because the length of the bonds only show the strength in attraction with the distance between atoms. The bond length would only determine acidity when relating to a hydrogen atom. For example, when there is a weaker bond between an atom and H, it would then be easier to remove the H+ and the molecule would be more acidic. Since chlorine is the most electronegative, it would then stabilize the negatively charged oxygen by withdrawing the electron density. A more electronegative central atom would result in a more polarized O-H bond and a more acidic compound.