Re: TOJC--Lewis acids
boldtbm@PLU.edu
Fri, 27 Sep 1996 08:36:00 -0800 (PST)
No. A lewis acid is not a Bronsted-Lowry base. The Bronsted-Lowry
theory states that an acid is a proton donor and a base is a proton
acceptor. In order to accept a proton a base must donate an electron,
and in order to donate a proton an acid must recieve an electron.
Thus, Bronsted-Lowry acids are also lewis acids because they must recieve
an electron ( as stated in the lewis theory) in order to donate a
proton. The lewis theory has a broader definition of acids (an
electron acceptor) and includes all Bronsted-Lowry acid/base reactions
and other reactions that are not included in Bronsted-Lowry theory
because they don't involve protons. Check out the example of aluminum
chloride on page 92.
Hoped that helped,
Hope I know what I am talking about,
Brian
On Thu, 26 Sep 1996 ulamce@PLU.edu wrote:
> I have a question I'd like for someone to clear up. CHem 115 is kind of
> a blank now.
>
> Is a Lewis acid a Bronsted-Lowry base, or is an acid an acid no matter
> what specific definition you use?
>
> Thanks,
> ulamce
>