What elements must hydrogen be bonded to for hydrogen bonding to occur?

Hydrogen bonding is a specific type of intermolecular attraction that occurs when hydrogen is covalently bonded to highly electronegative elements. The primary elements that hydrogen needs to be bonded to for hydrogen bonding to occur are nitrogen, oxygen, and fluorine.

These elements are highly electronegative, which means they attract electrons strongly and create a significant polarity in the covalent bond with hydrogen. As a result, the hydrogen atom becomes partially positive, allowing it to interact attractively with lone pairs of electrons on nearby atoms of these electronegative elements. This interaction is what defines hydrogen bonding, providing enhanced stability and properties to compounds, such as higher boiling points and unique solubility characteristics.

While carbon, chlorine, and sulfur may form bonds with hydrogen, they do not facilitate hydrogen bonding due to their lower electronegativity compared to nitrogen, oxygen, and fluorine. Therefore, the only correct set of elements that must be bonded to hydrogen for hydrogen bonding to occur is specifically nitrogen, oxygen, and fluorine.