Bronsted vs Lewis Acids and Bases

[Charlene D 3H]

When asked to simply identify the acid or base in a reaction, how do I distinguish between the type of acid/base? I know in some cases the terms can be used interchangeably, but are there examples when it would be incorrect to call a bronsted base/acid a lewis, or vice verse?
Thank you!

[Ryan_Page_1J]

Almost all of the textbook questions regarding this asked specifically for you to identify the Bronsted version or specifically for you to identify the Lewis version, so I think this is the typical format. You can do either by examining the reaction, but I would respond with what the question asks.

[Isaac Wen]

All Bronsted acids can be considered Lewis acids and all Bronsted bases can be considered Lewis bases. However, the opposite does not apply. Not all lewis acids and bases are Bronsted acids and bases. Basically, Lewis acids/bases are the more general terms.

[Xavier Herrera 3H]

All Bronsted acids/bases are Lewis acids/bases, but not the other way around. So, in the case of Cl- + SO2 --> SO2Cl, H+ isn't involved at all, so there can't be any Bronsted acids or bases. The Cl- does donate a lone pair to the SO2 to create SO2Cl, so the Cl- is a lewis base and the SO2 is a lewis acid.

[Can Yilgor 2D]

There are a lot of exceptions in chemistry, so I recommend thinking about the definitions depending on the reaction you are given.

Bronsted acid: proton donor
Bronsted base: proton acceptor
Lewis acid: electron pair acceptor
Lewis base electron pair donor

Hope this helps

[Taha 2D]

lewis acids are e- acceptors, bronsted are proton donators
lewis bases are e- donors, and bronsted bases are proton acceptors
all bronsted are lewis but not the other way around

[DavidTabib 3H]

All Bronsted acids are Lewis acids and all Bronsted bases are Lewis bases, but not the opposite way.

[Jose Miguel Conste 3H]

I believe the lewis theory was based off the bronsted

[Christine Ma 3L]

You can always call a Bronsted acid/base a Lewis acid/base too because every chemical reaction involves a transfer of electrons (so the Lewis definition can always be applied). However, not all Lewis acids/bases are Bronsted acids/bases because not every reaction involves the transfer of H+'s, so the Bronsted definition can't be applied when there are no protons involved. In those cases, the species involved would only be Lewis acids/bases and not Bronsted ones.