In water, the specific intermolecular forces present are hydrogen bonding, dipole-dipole interactions, and London dispersion forces.1. Hydrogen bonding: This is the strongest intermolecular force present in water. It occurs between the highly electronegative oxygen atom and the hydrogen atom of another water molecule. The partially negative oxygen atom attracts the partially positive hydrogen atom, forming a strong hydrogen bond.2. Dipole-dipole interactions: Water is a polar molecule, meaning it has a positive and a negative end or poles . The oxygen atom carries a partial negative charge, while the hydrogen atoms carry partial positive charges. This creates an electrostatic attraction between the positive and negative poles of adjacent water molecules, resulting in dipole-dipole interactions.3. London dispersion forces: These are the weakest intermolecular forces and are present in all molecules, including water. They result from temporary fluctuations in electron distribution around the molecules, which create instantaneous dipoles that induce dipoles in neighboring molecules.The boiling point of a substance is affected by the strength of its intermolecular forces. In the case of water, the strong hydrogen bonding significantly raises its boiling point compared to other molecules of similar size and mass. This is because more energy is required to break the hydrogen bonds and overcome the dipole-dipole interactions and London dispersion forces, allowing the water molecules to transition from the liquid phase to the gas phase. As a result, water has a relatively high boiling point of 100C 212F at standard atmospheric pressure.