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Maya Pakulski 3D wrote:Why are there there two definitions for acids and bases? Why not just one?
the two definitions focus on different things. Bronstead focuses on the transfer of protons or H+ ions and Lewis focuses on electrons
Darren Nguyen 1F wrote:What makes them different
The Bronsted-Lowry definition of acids and bases are focused on the proton (H+). Bronsted Acids are proton (H+) donors and Bronsted Bases are the proton (H+) acceptors. My high school chemistry teacher used the phrase "shake and take", where acids "shake" off an H+ and bases "take" an H+.
The Lewis Definition of acids and bases focuses on the lone pairs, where Lewis acids are the lone pair acceptor and Lewis bases are the lone pair donor.
The end result of which compound is an acid and which is the base is still the same, it's just whether you are using the transfer of lone pairs or protons to figure it out.
Bronsted has to do with protons(more protons means more acidic). A Bronsted acid is a proton donor(HCl donates H+) and the Bronsted base is a proton acceptor. Lewis has to do with electrons, a Lewis acid is an electron acceptor and a Lewis base is an electron donor. All Bronsted acids are Lewis acids but not all Lewis acids are Bronsted acids as HCl dissociates in water it will donate its proton, and the lone pairs on the chlorine will donate electrons(lewis and Bronsted acid), but some electron donors such as a chlorine on its own will not donate a proton as they do not have one thus it is just a Lewis acid and not a Bronsted acid.
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