Bronsted vs. Lewis

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Rebecca Doan 2L
Posts: 51
Joined: Thu Jul 27, 2017 3:01 am

Bronsted vs. Lewis

Postby Rebecca Doan 2L » Sun Dec 03, 2017 11:30 pm

What is the difference between Bronsted and Lewis acids?

Gurshaan Nagra 2F
Posts: 49
Joined: Thu Jul 27, 2017 3:01 am

Re: Bronsted vs. Lewis

Postby Gurshaan Nagra 2F » Sun Dec 03, 2017 11:36 pm

A bronsted acid is a proton donor, while a Lewis acid is an electron acceptor

Pooja Nair 1C
Posts: 55
Joined: Thu Jul 13, 2017 3:00 am

Re: Bronsted vs. Lewis

Postby Pooja Nair 1C » Tue Dec 05, 2017 3:02 am

A Lewis acid id more broadly defined, because while the compound may be able to give accept electrons, it may not have a proton to give. For example, when carbon dioxide reacts with water, the CO2 is the Lewis acid, as it accepts an electron pair from the oxygen of H20. However, CO2 is not a Bronsted acid, because it doesn't have any protons to give. The resultant H2CO3 is a Bronsted acid because in solution, it will donate H+ to form [H30+] with water molecules.

Leanne Wong 1H
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Joined: Tue Oct 10, 2017 7:13 am
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Re: Bronsted vs. Lewis

Postby Leanne Wong 1H » Tue Dec 05, 2017 4:21 pm

For a bronsted-lowry acid, the acid is a electron donor, whereas in a lewis acid, it is an electron acceptor.

Yizhou Liu 3L
Posts: 19
Joined: Fri Sep 29, 2017 7:07 am

Re: Bronsted vs. Lewis

Postby Yizhou Liu 3L » Tue Dec 05, 2017 7:41 pm

The bronsted acid donates the H+; while the lewis acid accepts a lone pair.


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