Lewis vs. Bronsted Acids and Bases
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Lewis vs. Bronsted Acids and Bases
Can someone explain the difference between Lewis and Bronsted acids and bases? Thank you!
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- Posts: 40
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Re: Lewis vs. Bronsted Acids and Bases
A Lewis acid is an electron pair acceptor, and a Lewis base is an electron pair donor.
A Bronsted acid gives up an H+ (proton donor), and a Bronsted base receives an H+ (proton acceptor).
A Bronsted acid gives up an H+ (proton donor), and a Bronsted base receives an H+ (proton acceptor).
Re: Lewis vs. Bronsted Acids and Bases
The Bronsted-Lowry theory talks about removal or transfer of hydrogen ions (H+) ie. protons where as the Lewis theory talks about donation or acceptance of electron pairs. A Brønsted–Lowry acid is a chemical species being able to donate a hydrogen cation, H+. Obviously, it needs another chemical species ( a bronsted-lowry base) to accept the transferred hydrogen cation. A Lewis acid is a chemical species being able to accept an electron-pair, reacting thereby with a Lewis base to form a Lewis bond, ie. a shared electron pair between Lewis acid and base.
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