Lewis Acids and Bases Vs. Bronsted Acids and Bases

[Michelle Dong 1F]

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]

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) + HPO₄^2- (aq) = NO₂^- (aq) + H₂PO₄^- (aq)

The Bronsted Acids are HNO₂ and H₂PO₄^-
The Bronsted Bases are: HPO₄^2- and NO₂^-

The Lewis Acid is H⁺
The Lewis Bases are: HPO₄^2- and NO₂^-

[Matthew 1C]

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]

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

[Paula Dowdell 1F]

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.