Lewis vs. Bronsted

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Alex Tchekanov Dis 2k
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Joined: Sat Aug 24, 2019 12:16 am

Lewis vs. Bronsted

Postby Alex Tchekanov Dis 2k » Mon Dec 02, 2019 4:43 pm

Is a molecule that is considered a lewis acid also considered a Bronsted acid and vice versa?

Brian_Ho_2B
Posts: 221
Joined: Fri Aug 09, 2019 12:16 am

Re: Lewis vs. Bronsted

Postby Brian_Ho_2B » Mon Dec 02, 2019 4:48 pm

Most of the time, the definitions will overlap and a lewis acid is also a bronsted acid b/c the acid satisfies both definitions. For instance, HCl is both a bronsted/lewis acid because it loses a proton to form Cl-, and when it forms Cl-, it "receives" a lone pair due to the fact that Cl- now has an extra lone pair than it did before. Some lewis bases may not explicitly look like a bronsted base, but both definitions still hold. For instance, NH3 is a lewis base because it can donate a lone pair in a coordination covalent compound, and it is also a bronsted base that can form NH4+.

Abby Soriano 1J
Posts: 103
Joined: Sat Aug 24, 2019 12:16 am

Re: Lewis vs. Bronsted

Postby Abby Soriano 1J » Mon Dec 02, 2019 4:56 pm

A molecule that is a Lewis acid can also be considered a Bronsted acid (and vice versa) since their definitions do line up. In order for a molecule to accept an electron pair (be a Bronsted acid), it donates a proton (is a Lewis acid). Typically you can use both definitions to define an acid unless otherwise specified.

005321227
Posts: 90
Joined: Sat Sep 07, 2019 12:15 am

Re: Lewis vs. Bronsted

Postby 005321227 » Tue Dec 03, 2019 11:42 am

Abby Soriano 1H wrote:A molecule that is a Lewis acid can also be considered a Bronsted acid (and vice versa) since their definitions do line up. In order for a molecule to accept an electron pair (be a Bronsted acid), it donates a proton (is a Lewis acid). Typically you can use both definitions to define an acid unless otherwise specified.

Is there a situation in which the definitions do not overlap? And is bronsted considered the more general definition?


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