What's the difference between Lewis acid-base reactions and Bronsted acid-base reactions?

Answer 1

In a Lewis reaction, the base donates an electron pair and the acid accepts the electron pair.

In a Bronstead reaction, the acid donates a proton and the base accepts the proton.

Answer 2

Arrhenius variety states that an acid/base reaction will continually contain an H+ species and an OH-. Bronsted-Lowry states that a reaction is acid/base if it incorporates a proton donor and a proton acceptor. it truly is a extra extensive definition, as you do not choose an OH-. Lewis acids states that acid/base reactions have electron pair acceptors and donators. that's a good broader definition because it does no longer require both H+ or OH-, so it ought to contain so a lot extra reactions (gasoline-section acid/base reactions, to illustrate). For the get at the same time: HCl + H2O --> H3O+ + Cl- you are able to locate that H2O accepts the donated proton from HCl. at the same time, H2O is the Lewis base because it truly is accepting protons from HCl, that's the Lewis acid. It does no longer, even with the undeniable fact that, contain OH- species. So the reaction ought to nicely be seen a Bronsted-Lowry or a Lewis acid/base reaction.

Answer 3

Lewis acid-base reactions involve electron transfer, while Bronsted acid-base reactions involve transfer of H+.

Answer 4

Bronsted acid-base reactions:
ACID: Substance that can donate proton (H+1).

BASE: Substance that can accept proton (must contain lone pair of electrons).



Lewis acid-base reactions:
ACID: Substance that can accept a pair of electrons from another atom to form a new bond.

BASE: Substance that can donate a pair of electrons to another atom to form a new bond.