Final answer:
Ethanol (CH₃CH₂OH) exhibits London dispersion forces, dipole-dipole forces, and hydrogen bonding. These forces arise due to temporary dipoles, a permanent dipole caused by an electronegative oxygen atom, and the special interaction of hydrogen bonded to oxygen respectively.
Step-by-step explanation:
The substance CH₃CH₂OH, also known as ethanol, exhibits all of the above intermolecular forces: London dispersion forces, dipole-dipole forces, and hydrogen bonding. London dispersion forces are the weakest type of van der Waals force and are present in all molecules, regardless of their polarity. They arise due to the momentary distribution of electrons that create temporary dipoles.
Dipole-dipole forces occur when there is an asymmetrical distribution of electrons within the molecular structure, leading to a permanent dipole. In ethanol, the presence of an electronegative oxygen atom causes a part of the molecule to be more negative and the other part more positive, resulting in a dipole. Hydrogen bonding is a special type of dipole-dipole interaction found in molecules where hydrogen is directly bonded to a highly electronegative atom like nitrogen, oxygen, or fluorine. In ethanol, a hydrogen atom is bonded to an oxygen atom, which allows for the formation of hydrogen bonds with other ethanol molecules or other electronegative atoms.