Lewis vs Bronsted [ENDORSED]
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Re: Lewis vs Bronsted
A lewis acid is a species that accepts an electron pair (examples: BF3 and H+). A bronsted acid is a proton donor (examples: HCl and HBr). I believe that bronsted acids are lewis acids but the reverse is not true.
Re: Lewis vs Bronsted
The main difference between a Lewis acid and a Bronsted acid is that Lewis acids are only able to accept an electron pair while Bronsted acids have the ability to donate a hydrogen cation (H+).
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Re: Lewis vs Bronsted
Lewis acids are compounds that accepts electron pairs. Bronsted acids are compounds that donate protons. Hope this helps!
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Re: Lewis vs Bronsted
In Lewis Acids and Bases, the structure is classified depending on its ability to accept or donate electrons.
Lewis Acid: Accepts a pair of electrons
Lewis Base: Donates a pair of electrons
On the other hand, Bronsted acids and bases are classified on their ability to donate or accept protons.
Bronsted Acid: Donates protons
Bronsted Base: Accepts protons
Lewis Acid: Accepts a pair of electrons
Lewis Base: Donates a pair of electrons
On the other hand, Bronsted acids and bases are classified on their ability to donate or accept protons.
Bronsted Acid: Donates protons
Bronsted Base: Accepts protons
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Re: Lewis vs Bronsted
Hi! To keep it simple, Lewis acids accept electron pairs while Bronstead acids donate protons. That is the easiest way to put it!
Re: Lewis vs Bronsted
Lewis acids accept electron pairs while Bronsted acids donate hydrogen ions. Lewis acids/bases deal with accepting/donating electron pairs while Bronsted acids/bases deal with accepting/donating hydrogen ions. Hope that helps!
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Re: Lewis vs Bronsted
A Bronsted acid is defined as a proton donator, while a Lewis acid has a more broad definition: referring to any species that is an electron pair acceptor.
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Re: Lewis vs Bronsted
A Bronsted acid is a proton donator, obtaining a negative charge, while a Lewis acid is an electron pair acceptor, obtaining a negative charge as well.
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