Final answer:
The difference in boiling points between CH3CH2OH and CH3OCH3 can be attributed to a difference in hydrogen bonding.
Step-by-step explanation:
The difference in boiling points between CH3CH2OH and CH3OCH3 is attributed to a difference in hydrogen bonding.
Hydrogen bonding is a type of intermolecular force that occurs when hydrogen atoms are bonded to highly electronegative atoms such as oxygen or nitrogen. The presence of hydrogen bonding leads to stronger intermolecular interactions, resulting in higher boiling points.
In the case of CH3CH2OH (ethanol), the -OH group allows for hydrogen bonding, which increases the strength of intermolecular forces and raises the boiling point. CH3OCH3 (dimethylether), on the other hand, lacks hydrogen bonding and exhibits weaker intermolecular forces, leading to a lower boiling point.