Talk:Organic chemistry/Acid–base chemistry

This page is weak and should be revised. TX. (The preceding unsigned comment was added by 193.190.187.220 (talk • contribs) 16:32, 31 October 2006)

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.

The above text should replace part of the current article. (The preceding unsigned comment was added by 67.161.126.88 (talk • contribs) 17:24, 8 December 2007)

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)