Protic solvent
From Wikipedia, the free encyclopedia
In chemistry a protic solvent is a solvent that has a hydrogen atom bound to an oxygen as in a hydroxyl group or a nitrogen as in an amine group. More generally, any molecular solvent which contains dissociable H+, such as hydrogen fluoride, is called a protic solvent. The molecules of such solvents can donate an H+ (proton). Conversely, aprotic solvents cannot donate hydrogen.
Common characteristics of protic solvents:
- solvents display hydrogen bonding
- solvents have an acidic hydrogen (although they may be very weak acids)
- solvents are able to stabilize ions
- cations by unshared free electron pairs
- anions by hydrogen bonding
Examples are water, methanol, ethanol, formic acid, hydrogen fluoride and ammonia.
Polar aprotic solvents are solvents that share ion dissolving power with protic solvents but lack an acidic hydrogen. These solvents generally have high dielectric constants and high polarity.
Examples are dimethyl sulfoxide, dimethylformamide, dioxane and hexamethylphosphorotriamide, tetrahydrofuran.
Polar protic solvents are favorable for SN1 reactions, while polar aprotic solvents are favorable for SN2 reactions. Apart from solvent effects, polar aprotic solvents may also be essential for reactions which use strong bases, such as reactions involving Grignard reagents or n-butyllithium. If a protic solvent were to be used, the reagent would be consumed by a side reaction with the solvent.
An example of a dipolar aprotic solvent is methylpyrrolidone.
[edit] References
- Loudon, G. Mark. Organic Chemistry 4th ed. New York: Oxford University Press. 2002. pg 317.
