Final answer:
Hydrogen bonds are unique dipole-dipole interactions that occur specifically when hydrogen is bonded to nitrogen, oxygen, or fluorine, which are highly electronegative elements, leading to strong intermolecular forces and unusual material properties.
Step-by-step explanation:
Yes, hydrogen bonds are formed predominantly when hydrogen is covalently bonded to one of the three most electronegative elements: nitrogen (N), oxygen (O), or fluorine (F). These elements have high electronegativity, meaning they attract electrons strongly when forming a bond with hydrogen. As a result, the bond between hydrogen and any of these elements is highly polarized, with hydrogen carrying a significant positive charge, and either N, O, or F carrying a negative charge. This partial positive charge on the hydrogen allows it to act as a hydrogen bond donor, forming a special type of dipole-dipole interaction with a lone pair of electrons on a nearby electronegative atom—making it the hydrogen bond acceptor.
The large bond dipoles and short dipole-dipole distances between these atoms lead to strong intermolecular forces, which are responsible for higher boiling points, melting points, and unusual properties like high enthalpies of vaporization seen in substances with hydrogen bonding.