Question

How is the Lewis definition for an acid and a base different from the Arrhenius and Bronsted-Lowry definitions?  If you haven’t done so, include the chemical formulas for each of your examples and tell us which of these 3 definitions is most useful when looking at these formulas.
I am not understanding and really need help.

Answer 1

Go to this link if you do not understand then again ask.
http://www.chemguide.co.uk/physical/acidbaseeqia/theories.html

Answer 2

thank you, I will

Answer 3

The Arrhenius model says that acids always contain H+ and that bases always contain OH-.
The Bronsted-Lowry model thinks of acids as being proton donors and proton acceptors, so bases no longer need to contain OH-, and acids donate a proton to water forming H3O+.

Answer 4

lewis acids are e^- donators while lewis bases are e^- acceptors
refer to Arrhenius theory
# acids produce H+ ions in aqueous solutions
# bases produce OH- ions in aqueous solutions
There are several methods of defining acids and bases. While these definitions don't contradict each other, they do vary in how inclusive they are. Antoine Lavoisier, Humphry Davy, and Justus Liebig also made observations regarding acids and bases, but didn't formalize definitions.
*
o water required, so only allows for aqueous solutions
o only protic acids are allowed; required to produce hydrogen ions
o only hydroxide bases are allowed

Johannes Nicolaus Brønsted - Thomas Martin Lowry

* acids are proton donors
* bases are proton acceptors

o aqueous solutions are permissible
o bases besides hydroxides are permissible
o only protic acids are allowed

Answer 5

I am still a bit confused with the Arrhenius model, but the others are very clear. Thank you for your help

Answer 6

Thank you so much for your help

Answer 7

Arrhenius model tells us that acids are those substances which produce H+ ions in a solution

Like

H2SO4= 2H+ + SO4-

this acid produced 2H+ thus its an acid.

Hope this helps :D