Bronsted vs Lewis Acid/Base
Moderators: Chem_Mod, Chem_Admin
Bronsted vs Lewis Acid/Base
Hi, I'm a little confused about the difference between bronsted and lewis acid/bases. I know the definitions but I'm wondering practically is there a difference? Is one a more correct depiction of acids and bases than the other? Thanks in advance.
-
- Posts: 105
- Joined: Thu Jul 25, 2019 12:17 am
Re: Bronsted vs Lewis Acid/Base
I believe that they are just different ways to identify acids/bases. The two definitions just represent different properties of acids/bases.
-
- Posts: 120
- Joined: Sat Aug 17, 2019 12:17 am
Re: Bronsted vs Lewis Acid/Base
Bronsted and Lewis acids/bases are just two different ways to define acids/bases. Neither is more correct, and there is no difference in the actual compounds.
The Bronsted definition is based on the donation/reception of protons. The Lewis definition is based on the donation/reception of lone pairs of electrons.
The Bronsted definition is based on the donation/reception of protons. The Lewis definition is based on the donation/reception of lone pairs of electrons.
Re: Bronsted vs Lewis Acid/Base
Thanks everyone. The other thing that's confusing to me is how does an atom donate a proton? I thought interactions between atoms were all through electrons.
-
- Posts: 109
- Joined: Sat Aug 17, 2019 12:18 am
Re: Bronsted vs Lewis Acid/Base
S 1C wrote:Thanks everyone. The other thing that's confusing to me is how does an atom donate a proton? I thought interactions between atoms were all through electrons.
Maybe an example will help. Let's say that we have a reaction that is between hydrochloric acid and water.
HCl(aq) + H2O (l) --> H3O+ (aq) + Cl- (aq).
In this case, HCl is the acid because it is donating the proton (H+) to water. In other words, the proton (H+) is being transfered from HCl to H2O. I hope this helps.
Return to “Bronsted Acids & Bases”
Who is online
Users browsing this forum: No registered users and 4 guests