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Please give me a list of Bronsted- Lowry  and Lewis acids and bases with explanation of how to distinguish between them.

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Bronsted-Lowry Acid

A Bronsted-Lowry acid, like an Arrhenius acid, is a compound that breaks down to give an H+ in solution.

Bronsted-Lowry Base

The Bronsted-Lowry base refers to any atom or ion capable of accepting or bonding to a free proton in solution.

examples include:

  • Methanol – CH3OH
  • Formaldehyde – H2CO
  • And water – H2O

Lewis Acid

A Lewis acid refers to an atom or molecule that accepts an electron pair. 

Lewis Acid Examples in Organic Chemistry

  • Borane – BH3 (hydroboration reaction)
  • Aluminum Chloride – AlCl3 (electrophilic aromatic substitution reaction)
  • Iron (III) Bromide – FeCl3 (electrophilic aromatic substitution reaction)
  • and H+

Lewis Base

Since the Lewis definition has to do with the transfer of electrons, a Lewis Base is an electron pair donor. 

  • A Lewis acid is an electron pair acceptor.

  • A Lewis base is an electron pair donor.

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