Lewis v Bronsted v Arrhenius

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Rohan Kubba Dis 4B
Posts: 50
Joined: Sat Aug 17, 2019 12:18 am

Lewis v Bronsted v Arrhenius

Postby Rohan Kubba Dis 4B » Fri Nov 22, 2019 9:09 pm

Can someone differentiate between the Lewis base/acid, the Bronsted/Lowry base/acid, and Arrhenius base/acid definitions?

TYun_1C
Posts: 52
Joined: Wed Sep 11, 2019 12:16 am

Re: Lewis v Bronsted v Arrhenius

Postby TYun_1C » Fri Nov 22, 2019 9:14 pm

Bronsted acids and bases deal with the donation and acceptance of a hydrogen ion. Lewis acids and bases deal with the donation and acceptance of an electron. I'm not completely sure about Arrhenius acids and bases but I think it has something to do with hydroxide ions.

Vincent Leong 2B
Posts: 207
Joined: Fri Aug 09, 2019 12:15 am

Re: Lewis v Bronsted v Arrhenius

Postby Vincent Leong 2B » Fri Nov 22, 2019 10:30 pm

They are all the same in the way, it's just the way you look at them. For example, Lewis acids are electron acceptors and that can be see with a molecule containing Boron (Lavelle showed this example in class). When putting HCl in water, H+ or a Hydrogen proton is being donated to the H2O molecule, hence the proton donor definition. Arrhenius deals with OH-. In a sense, each of these 3 definitions are just looking at diff components that a molecule, acid or base, will contribute, making them a acid or base in terms of classification.

Kayli Choy 2F
Posts: 100
Joined: Sat Aug 24, 2019 12:17 am

Re: Lewis v Bronsted v Arrhenius

Postby Kayli Choy 2F » Sat Nov 30, 2019 10:48 am

Arrhenius acid: reacts with water to produce H+
Arrhenius base: reacts with water to produce OH-
Bronsted acid: donates protons
Bronsted base: accepts protons
Lewis acid: electron pair acceptor
Lewis base: electron pair donator

Melvin Reputana 1L
Posts: 55
Joined: Sat Aug 17, 2019 12:16 am

Re: Lewis v Bronsted v Arrhenius

Postby Melvin Reputana 1L » Sat Nov 30, 2019 11:05 pm

I would also like to add on that the Arrhenius definition involves acids/bases being dissolved in water, while the Bronsted-Lowry definition considers how acids/bases can be dissolved in other solvents besides water.


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