Final answer:
Water molecules can form hydrogen bonds both with themselves and with other polar molecules in solution due to their polarized covalent bonds. These hydrogen bonds contribute to water's high boiling point and its effectiveness as a solvent.
Step-by-step explanation:
Hydrogen Bonding in Water Molecules
Hydrogen bonds would form between molecules that possess significantly polarized covalent bonds. In the case of water (H2O), each molecule can form hydrogen bonds with itself because the oxygen atom has a partial negative charge, and the hydrogen atoms have a partial positive charge. These partial charges occur because oxygen is more electronegative than hydrogen, leading to a polar molecule. The hydrogen bond occurs when the partial positive hydrogen of one molecule is attracted to the partial negative oxygen of a nearby molecule. Furthermore, due to water's molecular structure, each water molecule is capable of forming up to four hydrogen bonds with surrounding water molecules, leading to a vast network of interacting molecules. This arrangement is responsible for many of water's unique properties, such as its high boiling point compared to other molecules of similar molar mass, like methane (CH4).
When water is in solution, it can also form hydrogen bonds with other polar molecules. For instance, if another molecule also has a hydrogen attached to a highly electronegative atom like oxygen, nitrogen, or fluorine, it will likely engage in hydrogen bonding with water. This characteristic enables water to be a powerful solvent for both ionic and polar molecular compounds.