CHEM 122 Lecture Notes - Lecture 4: Lewis Structure, Conjugate Acid, Lone Pair
Document Summary
Many reactions between seemingly unrelated compound have splendid similarities. It is useful to think about these as a reaction of one type of compound (base) and. Key features of acid-base reactions: another kind (acid) Where the equilibrium sits can be predicted by knowing properties of the base, keeping balance in a particular position and the acid. Arrhenius definition, by svante arrhenius in 1884: *now this definition is outdated (though still valid)* Bronsted-lowry definition: by johannes bronsted and thomas lowry in 1932: The reactions is, thus, a transfer of h+ (proton) from an acid to a base. *the most used definition currently, encapsulates arrhenius definition, and covers more* The acid loses h+ to form its conjugate base. The base accepts an h+ to form its conjugate acid. The reverse reaction is also an acid-base reaction. Acid must have at least one h. Oxygen (o) loses a bond, and gets an extra pair of electrons.
