Which type of bonding is primarily responsible for the properties of water?

The properties of water, such as its high boiling and melting points, surface tension, and solvent capabilities, are primarily due to hydrogen bonding between water molecules. Water has a polar covalent bond, where the oxygen atom is more electronegative than the hydrogen atoms, creating a dipole moment. This polarity allows individual water molecules to form hydrogen bonds with one another, where the positively charged hydrogen atoms of one water molecule are attracted to the negatively charged oxygen atoms of neighboring molecules.

These hydrogen bonds are much weaker than covalent bonds but are significant in number, contributing to the unique properties of water. For instance, the ability of water to remain liquid over a wide range of temperatures, its high specific heat, and its solvent properties for many polar substances are all manifestations of hydrogen bonding.

In contrast, covalent bonding between oxygen and hydrogen describes the bonds within individual water molecules but does not explain the intermolecular interactions that give water its distinct characteristics. Ionic bonding is not relevant to water, as water is a molecular compound rather than an ionic one. While Van der Waals forces occur between water molecules, they are significantly weaker than hydrogen bonds and do not play a primary role in determining the properties of water. Thus, hydrogen bonding is the key factor responsible