What is the result of hydrogen bonding among water molecules?

The result of hydrogen bonding among water molecules significantly contributes to a higher boiling point. Water, being a polar molecule, has a partial positive charge on the hydrogen atoms and a partial negative charge on the oxygen atom. This polarity leads to the formation of hydrogen bonds between adjacent water molecules, where the positive hydrogen end of one molecule is attracted to the negative oxygen end of another.

These hydrogen bonds are relatively strong compared to other types of intermolecular forces, which means that a considerable amount of energy is required to break these bonds and convert water from its liquid phase to its gaseous phase (steam). Consequently, the boiling point of water is higher than that of many other similar molecular compounds that lack such hydrogen bonding.

In terms of the other options, the viscosity of water is actually relatively high due to these hydrogen bonds rather than lower. Electrical conductivity in pure water is not increased by hydrogen bonding; pure water is a poor conductor of electricity. Additionally, water’s density is not reduced due to hydrogen bonding; in fact, in its liquid state, water is denser than in its solid state (ice) due to the arrangement of hydrogen bonds.