What is the difference between Arrhenius, Bronsted-Lowry, and Lewis acids and bases?

1 Answer
Dr. K.
Jul 11, 2018

Arrhenius => release of #H^+#/#OH^-# in aqueous solution

Bronsted-Lowry => donation/acceptance of proton

Lewis => acceptance/donation of electron pair

Explanation:

The definition of acid and base according to the three acid-base theories are:

Arrhenius acid-base theory

  • acid - a substance produces hydrogen ions (#H^+#) in aqueous solution.
  • base - a substance that produces hydroxide ions (#OH^-#) in aqueous solution.

Here's the general equation defining Arrhenius acid and base:
http://acidsandbasesfordummieschem.weebly.com/definition-and-theories.html

Bronsted-Lowry acid-base theory

  • acid - proton (hydrogen ion) donor

  • base - proton (hydrogen ion) acceptor

Here are examples showing general equation defining (a) acid and (b) base:
http://biology.reachingfordreams.com/chemistry-cheat-sheet/chemical-equilibrium/42-the-nature-of-acids-and-bases
In (a), HA is an acid since it donates proton(#H^+#) to water. In (b), B is a base because it accepts proton (#H^+#)from water.

Lewis acid-base theory

  • acid - electron pair acceptor

  • base - electron pair donor

An example illustrating Lewis acid-base:
http://acidsandbasesfordummieschem.weebly.com/definition-and-theories.html

#BH_3# in the given example is a Lewis acid since it accepts the electron pair from #NH_3#
#NH_3#, in this case, is a Lewis base since it donates the electron pair.

Related questions
See all questions in Acids and Bases
Impact of this question
15104 views around the world
You can reuse this answer
Creative Commons License