Talk:Organic chemistry/Acid–base chemistry

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A Brønsted-Lowry acid is a species capable of "donating" a proton; a base is capable of "accepting" a proton (via a lone pair of electrons.) Hydroxyl groups actually tend to make a molecule acidic, while heteroatoms such as Oxygen or Nitrogen make a species basic. The Brønsted-Lowry acid/base theory is one of two major theories of acid/base reactions in Organic chemistry. Lewis acids and bases are the other major kinds of acids and bases considered in an Organic chemistry class. A lewis acid is any electron-deficient species capable of accepting a bond with a lone pair of electrons. A Lewis base is any species capable of donating an electron pair. A Lewis base is capable of acting as a Brønsted-Lowry base by "donating" it's lone pair of electrons to a proton (hydrogen ion). The molecule that results as from a Lewis acid-base reaction is called a Lewis adduct. If the Lewis acid in the reaction was a hydrogen ion, the Lewis adduct can also be a Brønsted-Lowry acid.

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 * Acid/Base chemistry began with the Lewis model of acids and bases. This model states molecules accapting electron pair are acids, while molecules donating electon pair are bases.--Abbatai 19:12, 13 October 2010 (UTC)