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Bronsted Acids and Bases

Posted: Mon Dec 03, 2018 8:21 pm
by Isabel Nakoud 4D
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)

Re: Bronsted Acids and Bases

Posted: Mon Dec 03, 2018 8:29 pm
by deepto_mizan1H
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.

Re: Bronsted Acids and Bases

Posted: Mon Dec 03, 2018 8:30 pm
by Brian Hom 2F
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.