## "electron-withdrawing atoms" - stability & acidity

Acidity $K_{a}$
Basicity $K_{b}$
The Conjugate Seesaw $K_{a}\times K_{b}=K_{w}$

Ashley Wang 4G
Posts: 83
Joined: Wed Sep 11, 2019 12:16 am

### "electron-withdrawing atoms" - stability & acidity

Hi,

In lecture, Dr. Lavelle went over how atoms with higher electronegativity delocalize and stabilize the negative charge on the oxygen atom in oxoacids, accounting for higher acidity. It made sense when he was explaining it, but I don't really understand why a stable anion means that it's a stronger acid. Or is it just a trend that has been observed?

Thank you so much!

zoedfinch1K
Posts: 57
Joined: Thu Jul 25, 2019 12:16 am

### Re: "electron-withdrawing atoms" - stability & acidity

I think its because when the anion is stable by the process you mentioned below, oxoacids readily lose H+. If you remember, stronger acids dissociate completly in water so the more H+ given off would correlate to a stronger acid.

Amy Pham 1D
Posts: 88
Joined: Fri Aug 09, 2019 12:15 am

### Re: "electron-withdrawing atoms" - stability & acidity

If the anion in an acid is stable, then it is able to exist stably on its own without the presence of the H+ ion (proton). So it more readily loses its proton in solution and dissociates more completely, thus making it a stronger acid.