Bronsted Acid vs Lewis Acid  [ENDORSED]

Moderators: Chem_Mod, Chem_Admin

Hector Acosta Discussion 1H
Posts: 51
Joined: Fri Sep 29, 2017 7:04 am

Bronsted Acid vs Lewis Acid

Postby Hector Acosta Discussion 1H » Fri Dec 01, 2017 11:00 pm

Are there any other differences between the two acids except for the fact that by definition a lewis acid is an electron acceptor and a bronsted acid a proton donor?

Lily Sperling 1E
Posts: 49
Joined: Tue Oct 10, 2017 7:14 am

Re: Bronsted Acid vs Lewis Acid  [ENDORSED]

Postby Lily Sperling 1E » Sat Dec 02, 2017 9:12 am

I believe that is the only difference. The bronsted acid is a proton (or H+ ion) donor, and base is the acceptor. The lewis acid is an electron acceptor, and base is the donor. Different definitions arose because of the context of different reactions. As our knowledge of different fields of chemistry expanded, we had to find different ways to classify acids and bases depending on the context and reaction.

Alexia Joseph 2B
Posts: 56
Joined: Thu Jul 27, 2017 3:01 am

Re: Bronsted Acid vs Lewis Acid

Postby Alexia Joseph 2B » Sat Dec 02, 2017 5:11 pm

No, the only difference is the definition. The Bronsted acid is a proton donor, the Bronsted base is a proton acceptor. A Lewis acid is an electron pair acceptor, while a lewis base is an electron pair donor. The Lewis definitions are broader than Bronsted definitions. The Bronsted definitions are more useful for this specific topic of acids and bases, but when it comes to studying coordinate covalent bonds, Lewis acids and bases are more useful definitions.

Rachel Formaker 1E
Posts: 86
Joined: Fri Sep 29, 2017 7:04 am
Been upvoted: 2 times

Re: Bronsted Acid vs Lewis Acid

Postby Rachel Formaker 1E » Sat Dec 02, 2017 8:49 pm

Another difference is that all Bronsted acids are Lewis acids, but not all Lewis acids are Bronsted acids.

This is because when a molecule is a proton donor, that proton is an electron pair acceptor, making the molecule both a Bronsted acid(proton donor) and a Lewis acid (electron pair acceptor).

Some molecules, like BF3, are only electron pair acceptors, and are therefore Lewis acids but not Bronsted acids.


Return to “Bronsted Acids & Bases”

Who is online

Users browsing this forum: No registered users and 1 guest