Lewis Acids/Bases vs Bronsted

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salvadorramos3k
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Lewis Acids/Bases vs Bronsted

Postby salvadorramos3k » Thu Dec 05, 2019 9:04 pm

I know the definitions of Lewis acids/bases and Bronsted acids/bases, but I'm having trouble being able to tell which on is which when looking at molecules. What should I look for in order to be able to differentiate the two?

Kassidy Ford 1I
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Joined: Sat Aug 17, 2019 12:16 am
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Re: Lewis Acids/Bases vs Bronsted

Postby Kassidy Ford 1I » Fri Dec 06, 2019 9:36 am

A bronsted acid is a proton donor, and a bronsted base is a proton acceptor. This is easy to see in chemical reactions, because you can usually see the transfer of H+ going on. For example, HCl + H2O --> H3O + Cl, HCl is the bronsted base because it donated an H+ to H20, in this case the bronsted acid.

A Lewis acid is any electron pair acceptor, while a Lewis base is any electron pair donor. You can think of H+ as an electron pair acceptor. So a bronsted acid is a supplier of one particular lewis acid, H+


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