What is the difference between a lewis acid and bases and Bronsted acids and bases?

[vuongnaomi1L]

To my understanding, Bronsted acids and bases use the accepting or donating of H+ ions in their definition, while lewis acids and bases go by accepting or donating electrons in their definition. Is this correct?

[Valerie Tran 2B]

Yes, you are correct. Lewis acids and bases are defined in terms of being able to accept/donate electron pairs but Bronsted Lowry acids and bases are defined in terms of being able to accept/donate hydrogen ions ( H+ )

[claire ikemiya_2I]

Yes, and all Bronsted-Lowry acid/bases are lewis acids and bases, but not all lewis acids/bases are bronsted lowry.

[LeanneBagood_2F]

like others already said, yup! one is in term of electrons while the other is in terms of hydrogen ions

[Raashi Chaudhari 3B]

Lewis acids/bases pertain to the accepting (lewis acid) or donating (lewis base) of electrons. While Bronsted acids/bases have to do with donating H+ protons (Bronsted acid) and accepting H+ protons (bronsted base).

[Bella Bursulaya 3G]

Lewis acids and bases have to do with electrons, while the Bronsted definition includes H+ and OH- ions. Lewis acids accept electrons, Lewis bases donate electrons, Bronsted acids donate H+ and form H3O+ in solution and Bronsted bases accept H+ ions and form OH- ions solution.

[Giselle_zamora_1L]

Yes so like other people mentioned its all in how you define it, they are both happening at the same time so while a Lewis base is donating an electron it is also receiving a proton. They are just trying to get more neutral. Lewis is in terms of electrons and Bronsted's definition the roles kind of reverse but in terms of protons.

[Kelly Tran 1J]

Yes, you are correct. Bronsted acids are proton donors while bronsted bases are proton acceptors, and lewis acids are lone pair acceptors while lewis bases are lone pair donors.