Ethanol is a molecular polar compound. It is not ionic because it does not consist of ions. Instead, it is made up of molecules that have a polar nature due to the presence of a hydroxyl (-OH) group.
The polarity in ethanol arises because the oxygen atom in the -OH group is more electronegative than the hydrogen and carbon atoms. This creates a dipole moment, making ethanol a polar molecule.
The intermolecular forces present in ethanol include:
- Hydrogen Bonding: This is the strongest intermolecular force in ethanol. It occurs between the hydrogen atom of the -OH group of one ethanol molecule and the oxygen atom of the -OH group of another ethanol molecule.
- Dipole-Dipole Interactions: These occur between the positive end of one polar molecule and the negative end of another polar molecule. In ethanol, these interactions are present due to the polar nature of the molecule.
- London Dispersion Forces: These are weak forces that occur between all molecules, including nonpolar ones. In ethanol, these forces are present but are much weaker compared to hydrogen bonding and dipole-dipole interactions.
In summary, ethanol is a polar molecule with hydrogen bonding, dipole-dipole interactions, and London dispersion forces as the primary intermolecular forces.