The Lowry and Brønsted Theory

The Lowry and Brønsted theory suggest that defining acids as chemicals that donate a proton (H +) in a chemical reaction and bases as chemicals that accept a proton. This definition is slightly more useful than Arrhenius's definition. Gilbert Lewis definition of acids and bases was different. Lewis suggested that an acid could be any compound that accepts a pair of electrons from another substance and bases could be compounds that donate a pair of electrons (Chang, 2007). Although almost all acids and bases correspond to all of these definitions, some only correspond by one or both of the definitions.

“Lewis’s theory is another way of explaining reactions between H+ and OH- ions. However, the most important aspect of this theory is that it extends the definition of an acid and base beyond the H+ and OH- ions that Brønsted describes. Thus, allowing one to predict and rationalize reactions between species lacking H+ and OH- ions” (Abudra, Badial, 2011). Chemist can use Lewis’s theory to predict a wider range of acid-base reactions. Lewis' theory used electrons instead of proton transfer and stated that an acid is a species that accepts an electron pair while a base donates an electron pair. The reaction of a Lewis acid and base will produce a coordinate covalent bond, where the lewis base donates its electrons to the lewis acid, resulting in an adduct.

Works Cited

Abudra, A., Badial, T. (2011). Lewis concept of acid and bases. Retrieved from http://chemwiki.ucdavis.edu/Physical_Chemistry/Acids_and_Bases/Acid/Lewis_Concept_of_Acids_and_Bases

Chang, R. (2007). Chemistry. (9th ed.). New York, NY: McGraw-Hill.