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These lectures vary in length, and will open in a new window when you click on the provided link.
Arrhenius, Brönsted-Lowry, and Lewis Acids and Bases
There are three major ways in which we can categorize acids and bases. Arrhenius acids are defined as molecules that can readily dissociate in water and increase hydrogen ion concentration while Arrhenius bases are those molecules that dissociate in water and increase the hydroxide concentration. A Brönsted-Lowry acid is a compound that can donate a hydrogen ion while a Brönsted-Lowry base is a compound that can accept a hydrogen ion. A Lewis base is a compound that can donate a pair of electrons while a Lewis acid is a compound that can accept a pair of electrons.
Lewis Acids and Lewis Bases
Let us briefly extend the information we just learned in the following two chapters to Lewis Acid and Bases. The definition of the Lewis Acid-Base reaction is one of the most general definitions. It describes a reaction between a pair of electrons in a filled orbital and an empty orbital, as we will see in this lecture.