When a Bronsted Lowery acid loses a proton ( +H ion ), an electron ( e- ) pair and NET negative charge remain on the proton donor. For example, hydrochloric acid ( HCl ) readily forms +H and -Cl ions when placed within an aqueous solution. Lewis acids, however, expand upon this concept to include ANY atom or molecule capable of accepting an electron ( e- ) pair as being an acid.
Since the +H ion from the previous example has the ability to accept and SHARE an electron pair with a donor, EVERY BRONSTED LOWERY ACID IS ALSO A LEWIS ACID BY DEFINITION, but PLENTY OF LEWIS ACIDS ARE NOT BRONSTED LOWERY ACIDS, BECAUSE THEY DON’T RELEASE HYDROGEN IONS INTO SOLUTIONS.
ANY NOTABLE CHEMIST WILL INCLUDE TRICK QUESTIONS REGARDING BRONSTED LOWERY AND LEWIS ACIDS ON EXAMINATIONS!!! Just relate ” Lewis ” to ” eLectron “, and you’ll be good to go.
RENAISSANCE PHYSICS 