Strong/Weak acids

[Eden Breslauer-Friedman 2A]

When the hydrogen is directly bonded to the X atom (Cl, Br, I etc.), the strength of the acid is based on the length of the bond (the bigger the atom, the longer the bond, the stronger the acid)

Then, when there is an intermediary atom (like O or C) between the X atom and the hydrogen, since it is all a H-O or H-C etc bond being broken, we consider the electronegativity of the atom on the other side and the higher the electronegativity, the more it stabilizes the charge, so the stronger the atom?

Can someone just confirm that I understand this correctly! Thank you!!!

[Ethan Laureano 3H]

I believe you are correct.

[Steph Du 1H]

You consider the electronegativity because you are trying to determine the stability of the resulting anion. If the resulting anion is stable, it makes it so that the acid is more likely to lose its H+ atom, so that is what makes it a stronger acid.

[SavannahScriven_1F]

Another helpful note is that I learned in a UA worksop is that if you are trying to determine the stability of anions that are all within the same group, the stability increases down a group because the charge is "diluted" more in larger atoms. I believe this only holds true if you are looking at the anions in acids like HCl/HF/HBr, where hydrogen is directly bond to a single-element anion.

[AJForte-2C]

Another helpful note is that I learned in a UA worksop is that if you are trying to determine the stability of anions that are all within the same group, the stability increases down a group because the charge is "diluted" more in larger atoms. I believe this only holds true if you are looking at the anions in acids like HCl/HF/HBr, where hydrogen is directly bond to a single-element anion.

Hi! Can you explain about the charge being "diluted" a bit more?

[Vince Li 2A]

What Savannah means AJ is that because as you go down a group, the electrons densities are farther away from the positive attraction from the nucleus. As a result, the "dilution" is due to the spread of the electrons around the atom. As a result, it is difficult for the atom to hold onto the Hydrogen, due to the lack of concentration of the charge.