Bronsted Acid definition

[Shania Garrison Discussion 3E]

The Bronsted definition states that an acid is a proton donor. Is this proton always going to be H+? And if not, what are other examples of proton (if possible can you include a simpler and more complex example please)?

[Neelaj Das 3I]

Based on the problems we will have, yes the proton will essentially always be H+. We probably won't come across other examples of singular protons like H+ because they're hard to come by as a proton is simply an atom with only one proton and no electrons. This can only occur with H+.

[Baffour Adusei 1L]

Hey! I think we will only work with hydrogen for this class If you think about it, since a hydrogen atom is one proton and one electron, a H+ ion is just one proton. So this works simply for hydrogen in a way that wouldn't work for the other elements.

[Celine Khuu 2F]

For the scope of this class, I would generally always assume that the proton is H+.

[Jacob Bright 1C]

We visualize the H+ ion as a proton because this is an ion of hydrogen which has lost its one electron. Ground-state hydrogen also lacks a neutron, meaning all that H+ consists of is a single proton. The presence of a neutron may not actually matter (I'm not entirely sure), but I included it anyway for this explanation. It would be difficult and/or unnecessary to create another ion that represents a single proton when H+ is so simple and works for almost any example that requires it in this course. I also think it would be near impossible since every element after hydrogen features more than one proton and therefore even if electrons were removed the atom would no longer represent just a single proton. Therefore, I think all you should worry about for now is knowing H+ is a proton and try not considering other alternatives. Hope this helps!

[Isabelle Rieke-Wey 2G]

Hi!
As far as I know, yes, the proton will always be H+. This is because hydrogen has one proton and one electron, making the H+ ion have one proton.