What property of water explains why it has a high boiling point compared to other similar-sized molecules?

Water's high boiling point compared to other similar-sized molecules is primarily attributed to hydrogen bonding. In a water molecule, each hydrogen atom is covalently bonded to an oxygen atom, and the oxygen atom is more electronegative than hydrogen. This difference in electronegativity results in a polar molecule, meaning that there is an uneven distribution of electron density, leading to partial positive charges on the hydrogen atoms and a partial negative charge on the oxygen atom.

The polar nature of water allows for the formation of hydrogen bonds between water molecules. Each water molecule can form up to four hydrogen bonds with neighboring water molecules, creating a strong intermolecular attraction. These hydrogen bonds require significant energy to break, which means that as heat is added, more energy is needed to overcome these attractive forces to transition from the liquid phase to the gas phase. This is what results in an elevated boiling point when compared to molecules of similar size that do not exhibit such extensive hydrogen bonding.

Other properties, while important in their own respects, do not directly relate to the boiling point in the context of causing a dramatic increase due to intermolecular forces. For instance, low density, surface tension, and high specific heat are characteristics that stem from the unique structure and behaviors of water, but