Lewis Acids and Bases Vs. Bronsted Acids and Bases

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Michelle Dong 1F
Posts: 110
Joined: Fri Sep 29, 2017 7:04 am

Lewis Acids and Bases Vs. Bronsted Acids and Bases

Postby Michelle Dong 1F » Sat Dec 02, 2017 6:00 pm

Can someone explain the relationship between Lewis acids and Bronsted acids, and Lewis bases and Bronsted bases? Eg: is a Lewis acid the same as a Bronsted acid (the electron acceptor is the same as the proton donor)?

Ashin_Jose_1H
Posts: 51
Joined: Fri Sep 29, 2017 7:04 am

Re: Lewis Acids and Bases Vs. Bronsted Acids and Bases

Postby Ashin_Jose_1H » Sat Dec 02, 2017 8:09 pm

So a Bronsted acid is a proton donor and a Bronsted base is a proton acceptor. A Lewis acid is an electron pair acceptor and a Lewis base is an electron pair donor.

On pg. 467 in TB, it says:
"In the Lewis theory, the proton is an acid; in the Bronsted theory, the species that supplies the proton is the acid. In both the Lewis and Bronsted theories, the species that accepts a proton is a base."

In the case of bases, a Bronsted base is a Lewis base but not every Lewis base is a Bronsted base.

For example, in the reaction (On page 468 in TB):

HNO2 (aq) + HPO42- (aq) = NO2- (aq) + H2PO4- (aq)

The Bronsted Acids are HNO2 and H2PO4-
The Bronsted Bases are: HPO42- and NO2-

The Lewis Acid is H+
The Lewis Bases are: HPO42- and NO2-

Matthew 1C
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Joined: Fri Sep 29, 2017 7:06 am

Re: Lewis Acids and Bases Vs. Bronsted Acids and Bases

Postby Matthew 1C » Sat Dec 02, 2017 11:54 pm

will we be asked to identify which molecule is a bronsted acid/base or Lewis acid/base like in your example above on the final?

Peter Dis1G
Posts: 97
Joined: Fri Sep 29, 2017 7:04 am

Re: Lewis Acids and Bases Vs. Bronsted Acids and Bases

Postby Peter Dis1G » Sun Dec 03, 2017 10:52 am

From the experience of Test 4,I feel like we definitely need to remember that.

Paula Dowdell 1F
Posts: 72
Joined: Tue Nov 15, 2016 3:00 am

Re: Lewis Acids and Bases Vs. Bronsted Acids and Bases

Postby Paula Dowdell 1F » Sun Dec 03, 2017 11:16 am

It is helpful to note that a pH balance of 7 is ideal for neutral water solutions! In this situation, acids and bases neutralize each other's effects and characteristics.


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