Bronsted vs Lewis Acids and Bases

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RichardValdez1L
Posts: 59
Joined: Fri Apr 06, 2018 11:05 am

Bronsted vs Lewis Acids and Bases

Postby RichardValdez1L » Sun Jun 10, 2018 8:33 pm

Does Bronsted just tell you whether the atom is a hydrogen donor or accepter while the lewis tells you whether the atom is an electron donor or accepter? Or is there more to it than that?

Kara Justeson 1B
Posts: 31
Joined: Fri Apr 06, 2018 11:03 am

Re: Bronsted vs Lewis Acids and Bases

Postby Kara Justeson 1B » Sun Jun 10, 2018 8:39 pm

Yes, Bronstead Acid is a H+ donor, while a Bronstead base is a H+ acceptor. Lewis Acid acid accepts the electron pair while the Lewis base donates the electron pair. I think the difference is just in the way they define the exchange.

Chris Fults 1C
Posts: 27
Joined: Wed Nov 15, 2017 3:01 am

Re: Bronsted vs Lewis Acids and Bases

Postby Chris Fults 1C » Sun Jun 10, 2018 8:39 pm

Bronsted defines an acid as a proton donor whereas Lewis defines an acid as an electron pair acceptor. Conversely to the Bronsted theory, a base is a proton acceptor and in Lewis theory, a base is an electron pair donor. Therefore, some molecules, which don’t possess protons, can be acids according to the Lewis theory.

204917020
Posts: 31
Joined: Fri Apr 06, 2018 11:05 am

Re: Bronsted vs Lewis Acids and Bases

Postby 204917020 » Sun Jun 10, 2018 8:43 pm

Brønsted acids are H+ donors while Brønsted bases are H+ acceptors.
Lewis acids accept an e- pair, Lewis bases donate an e- pair.

MinyoungHong_1L
Posts: 12
Joined: Fri Apr 06, 2018 11:03 am

Re: Bronsted vs Lewis Acids and Bases

Postby MinyoungHong_1L » Sun Jun 10, 2018 9:29 pm

I found this sentence from the textbook helpful in understanding the terminology behind Lewis acids being electron acceptors.

"A proton (H+) is an electron pair acceptor. It is therefore a Lewis acid because it can attach to ("accept") a lone pair of electrons on a Lewis base" (p.467)

Alejandro Salazar 1D
Posts: 31
Joined: Fri Sep 29, 2017 7:05 am

Re: Bronsted vs Lewis Acids and Bases

Postby Alejandro Salazar 1D » Sun Jun 10, 2018 9:34 pm

Arrhenius Acid is a compound that releases hydrogen ions in water
Arrhenius Base is a compound that releases hydroxide ions in water

Lewis Acid: is a species that ACCEPTS an electron pair
Lewis Base is a species that DONATES an electron pair

Bronsted acid is a proton donor and donates a hydrogen ion
Bronsted Base is a proton acceptor and accepts a hydrogen ion


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