Bronsted vs. Lewis

Moderators: Chem_Mod, Chem_Admin

Hannah Morales 1D
Posts: 31
Joined: Fri Sep 29, 2017 7:06 am

Bronsted vs. Lewis

Postby Hannah Morales 1D » Sun Dec 02, 2018 11:09 am

What is an example (problem) where we are using a Bronsted Acid/ Base or a Lewis Acid/Base?

Can Bronsted acid/base be in a same problem(chemical reaction equation) as lewis acids/ bases? When would I know to label something as a bronsted acid/base or lewis acid/base?

MaiaRodriguezChoi3E
Posts: 32
Joined: Fri Sep 28, 2018 12:25 am

Re: Bronsted vs. Lewis

Postby MaiaRodriguezChoi3E » Sun Dec 02, 2018 11:54 am

I'm also confused about this. What is the definition of a Lewis acid/base and Bronsted acid/base? What is the significance of the difference between these terms?

Sara Flynn 2C
Posts: 60
Joined: Fri Sep 28, 2018 12:23 am

Re: Bronsted vs. Lewis

Postby Sara Flynn 2C » Sun Dec 02, 2018 11:57 am

A Bronsted base is just a proton acceptor and a bronsted acid is a proton donor. A Lewis base is an electron pair acceptor and a Lewis base is an electron pair donor. In almost all cases the molecule that is the bronsted base will also contain the molecule that is a lewis base and same for acids.
Example: HF is a bronsted acid becasue it donates the proton, the H is an lewis acid because it accepts the electrons from the base

shouse1f
Posts: 63
Joined: Fri Sep 28, 2018 12:18 am

Re: Bronsted vs. Lewis

Postby shouse1f » Sun Dec 02, 2018 9:09 pm

A bronsted acid is a proton donor and a bronsted base is a proton acceptor. A lewis acid is an electron acceptor and a lewis base is a electron donor.


Return to “Lewis Acids & Bases”

Who is online

Users browsing this forum: No registered users and 1 guest