Hydrogen bonds form between water molecules due to the polarity of the water molecule. The oxygen atom in water is highly electronegative, pulling shared electrons toward itself and creating a partial negative charge (δ-) on the oxygen and a partial positive charge (δ+) on the hydrogen atoms. This polarity means that the slightly positive hydrogen atom of one water molecule is attracted to the slightly negative oxygen atom of a neighboring water molecule, resulting in a hydrogen bond. This intermolecular force is an electrostatic attraction that is weaker than covalent bonds but strong enough to form a dynamic network of hydrogen bonds between water molecules. This network gives water many unique properties such as a high boiling point, surface tension, and solvent capabilities. Each water molecule can form up to four hydrogen bonds due to the two hydrogen atoms and two lone pairs on the oxygen atom, creating an extensive hydrogen bonding network.
