Bronsted v Lewis

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Layla Manoochehri
Posts: 29
Joined: Fri Sep 28, 2018 12:28 am

Bronsted v Lewis

Postby Layla Manoochehri » Mon Dec 03, 2018 1:38 am

Can someone explain why every Bronsted base is a Lewis base, but not every Lewis base is a Bronsted base?

Sydney To 1D
Posts: 60
Joined: Fri Sep 28, 2018 12:15 am

Re: Bronsted v Lewis

Postby Sydney To 1D » Mon Dec 03, 2018 9:12 am

All Bronsted-Lowry bases must have a lone pair to accept a hydrogen, and all Lewis bases have lone pairs. However, Lewis bases may act as nucleophiles (a chemical species that donates an electron pair to form a chemical bond in a reaction) for any number of atoms and not just for H.

Kirsty Star 2H
Posts: 48
Joined: Fri Sep 28, 2018 12:24 am

Re: Bronsted v Lewis

Postby Kirsty Star 2H » Mon Dec 03, 2018 1:28 pm

The difference between bronsted and lewis acids is basically if you're focusing on H+ ions or electrons. Bronsted acids donate hydrogen ions and bronsted bases accept hydrogen ions where as lewis acids accept a lone pair while lewis bases donate lone pair.

Posts: 35
Joined: Fri Sep 28, 2018 12:17 am

Re: Bronsted v Lewis

Postby danicatran4 » Tue Dec 04, 2018 2:20 pm

Will we ever have to determine if a compound is a Bronsted acid or Lewis acid on a test? If so, how would you determine if an electron or proton is being moved?

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