Which of the following describes hydrogen bonds?

Hydrogen bonds are a specific type of strong dipole-dipole attraction that occur between molecules when hydrogen is directly bonded to highly electronegative atoms such as oxygen, nitrogen, or fluorine. This bond forms because the hydrogen atom carries a partial positive charge due to the strong electronegativity of the atom it is bonded to, creating an attractive force between it and the electronegative atom of another molecule. The strength of hydrogen bonds plays a significant role in determining physical properties, particularly boiling points. For example, water has a relatively high boiling point due to the hydrogen bonds that hold its molecules together.

The characteristic that distinguishes hydrogen bonds from other types of intermolecular forces is their relatively higher strength, which is paramount in comparing them to weaker attractions, such as London dispersion forces. Therefore, option B accurately embodies the essence of hydrogen bonds within the context of molecular interactions and their implications on physical properties.