A solvent is a substance that dissolves a solute resulting in a solution. Solvents can be classified into two categories: polar and non-polar.
Polar solvents contain bonds between atoms with very different electronegativities, such as oxygen and hydrogen, and have large dipole moments. Non-polar solvents contain bonds between atoms with similar electronegativities, such as carbon and hydrogen. These polar solvents are capable of forming hydrogen bonds with water to dissolve in water whereas non-polar solvents are not capable of strong hydrogen bonds.
Polar solvents can be further divided into protic and aprotic.
Polar protic solvents are capable of hydrogen bonding because they contain at least one hydrogen atom connected directly to an electronegative atom (such as O-H or N-H bonds). They solvate cations and anions effectively. Polar protic solvents are water, ethanol, methanol, ammonia, acetic acid, and others.
Polar aprotic solvents contain no hydrogen atoms connected directly to an electronegative atom and they are not capable of hydrogen bonding. These are acetone, dimethyl sulfoxide, DMF (N,N-dimethylformamide), acetonitrile, HMF (hydroxymethylfurfural), crown ethers and others.
These two different kinds of solvents have different effects on the rates of SN1 and SN2 processes. In those reactions, the use of polar protic solvents favors the SN1 reaction mechanism, while polar aprotic solvents favor the SN2 reaction mechanism.
The SN1 reaction works well for tertiary alkyl halide because the loss of the leaving group forms a tertiary carbocation which is the most stable form of carbocations. A polar protic solvent will stabilize this carbocation.