Bronsted Acids and Bases

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Isabel Nakoud 4D
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Joined: Fri Sep 28, 2018 12:27 am

Bronsted Acids and Bases

Postby Isabel Nakoud 4D » Mon Dec 03, 2018 8:21 pm

Does the classification of Bronsted Acids and Bases go beyond the idea that acids are proton donors and bases are proton acceptors?

Are the Lewis and Bronsted definitions of Acids and Bases direct opposites of each other? (i.e. Lewis acids accept protons but Bronsted acids donate protons)

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Joined: Fri Sep 28, 2018 12:16 am

Re: Bronsted Acids and Bases

Postby deepto_mizan1H » Mon Dec 03, 2018 8:29 pm

Bronsted Acids and Bases don't really go beyond that definition as it's a proton-centric model of how we can understand acid and base compounds. Proton donation and accepting are characteristics of acids and bases in this definition and that is how we can analyze in a reaction what our acid and base would be.

Lewis bases and acids are essentially electron-centric, where a base donates electrons and acids receive electrons. One way to think of the difference is to think of the charges, how if in the Bronsted definition we are losing a +1 charge (from acids) then it is the electrical equivalent of gaining a -1 charge which could mirror the gain of an electron. They are different models, but by definition of the particle exchanges. They seem like opposites but looking at what is happening chemically between ions can help to differentiate.

Brian Hom 2F
Posts: 60
Joined: Fri Sep 28, 2018 12:24 am

Re: Bronsted Acids and Bases

Postby Brian Hom 2F » Mon Dec 03, 2018 8:30 pm

Bronsted acid are molecules that give off a hydrogen ion. Lewis acids are molecules that accept an electron pair. In the reaction HCl+water= H3O+ + Cl-, HCl is the Bronsted acid, while H+ is the Lewis acid since it accepts electrons from the O on H2O.

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