Please explain the difference between Lewis and Bronstead Lowry acids and bases. I understand that the defintion is that one is an electron pair acceptor/donor and the other is a proton acceptor/donor. However, I am not able to differentiate between the two when asked to identify if something is either a Bronstead acid/base or Lewis acid/base. Thanks! Solution In some cases like NH3, we can say that it is Bronsted base as well as Lewis base also. So, all the lewis bases are Bronsted bases too. But all the lewis acids need not be bronsted acids. NH 3 + H + ---> NH 4 + ( NH 3 is a Bronted base as well as lewis base) BF 3 + NH 3 ----> NH 3 -BF 3 Here BF 3 is only lewis acid but not be a Bronsted acid. .

1. Please explain the difference between Lewis and Bronstead Lowry acids and bases. I understand
that the defintion is that one is an electron pair acceptor/donor and the other is a proton
acceptor/donor. However, I am not able to differentiate between the two when asked to identify
if something is either a Bronstead acid/base or Lewis acid/base. Thanks!
Solution
In some cases like NH3, we can say that it is Bronsted base as well as Lewis base also.
So, all the lewis bases are Bronsted bases too. But all the lewis acids need not be bronsted
acids.
NH 3 + H + ---> NH 4
+ ( NH 3 is a Bronted base as well as lewis base)
BF 3 + NH 3 ----> NH 3 -BF 3
Here BF 3 is only lewis acid but not be a Bronsted acid.