Relative Acidity Concept Question

[Grace Lee 3G]

If an atom has a higher electronegativity, is it a stronger acid?

[skalvakota2H]

Atoms with higher electronegativity will be less inclined to share its electrons with a proton. Thus, increasing electronegativity of an atom will decrease basicity, and weaker bases have stronger conjugate acids.

Another way to think about this is that with increasing electronegativity, the H-A bond in the acid becomes more polar and demonstrate more ionic character; this implies that the proton in HA will be lost and the proton is more readily lost only when the acid is strong.

[Clara Hu 1G]

In the example given in class, hypochlorous acid was the most acidic out of HClO, HBrO, and HIO because CL has the highest electronegativity which stabilizes the negatively charged O by withdrawing electron density.

[Kyle Alves 3K]

electronegativity can also be seen as in making the conjugate base more stable and therefore showing it is a stronger acid. For example:
between HIO and HIO3, HIO3 is a stronger acid with a more stable conjugate base as the e- charge is more equally dispersed between 3 Os than one O. The more dispersed, the more stable the atom, the more stable the conjugate base= the stronger an acid.

[Kyle Alves 3K]

Probably a simpler example because the last one is confusing:
between HCl and HBr, Cl is more electronegative so pulls in e- greater, making the bond stronger
therefore, HBr would e a stronger acid as it is less stable with its longer bond length