Lewis vs Bronsted

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Armani Dodson 1A
Posts: 24
Joined: Fri Jul 22, 2016 3:00 am

Lewis vs Bronsted

Postby Armani Dodson 1A » Fri Nov 18, 2016 10:06 pm

I am confused on the concept of lewis acids and bases vs bronsted acids and bases.....can someone help me define how to figure out which is which?

Susanne_Taavitsa_2J
Posts: 20
Joined: Sat Jul 09, 2016 3:00 am

Re: Lewis vs Bronsted

Postby Susanne_Taavitsa_2J » Fri Nov 18, 2016 11:27 pm

I don't know if this helps or not:
-The Bronsted definition: an acid is a proton (H+ ion) donor, and a base is a proton acceptor.
-The Lewis definition: an acid is an electron acceptor, and a base is an electron donor.
Basically both are about acids and bases either accepting or donating electrons or protons.

Anna Makridis_L1
Posts: 13
Joined: Fri Jul 01, 2016 3:00 am

Re: Lewis vs Bronsted

Postby Anna Makridis_L1 » Sun Nov 20, 2016 2:26 pm

So according to this could both the Lewis and Bronsted explanations be describing the same acid? They just differ in what is accepted where?

Tyler_Ash_3C
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Joined: Wed Sep 21, 2016 2:57 pm
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Re: Lewis vs Bronsted

Postby Tyler_Ash_3C » Sun Nov 20, 2016 3:15 pm

That is correct. Both Lewis and Bronsted explanations can describe the same acid or base. Notice that for acids, the net change in charge is -1, while for bases, the net change in charge is +1. When an acid donates a proton its charge becomes more negative, and when it accepts an electron its charge becomes more negative. When a base accepts a proton, its charge becomes more positive, and when it donates an electron its charge becomes more positive.


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