Final answer:
Water has strong intermolecular forces primarily in the form of hydrogen bonds, as well as dipole-dipole attractions and London dispersion forces.
Step-by-step explanation:
The type of intermolecular forces that water exhibits is primarily hydrogen bonding. In water molecules, the oxygen atom is highly electronegative and attracts the shared electrons within the molecule more strongly than the hydrogen atoms. This creates a polarity within the molecule due to an uneven distribution of charge.
Because of this polarity, the partially positive hydrogen atom of one water molecule can form a hydrogen bond with the partially negative oxygen atom of a neighboring water molecule. Additionally, water also exhibits dipole-dipole attraction and London dispersion forces, but to a lesser extent compared to hydrogen bonding. These intermolecular forces contribute to water's unique properties such as high boiling point and surface tension.