Which type of bonds would be expected between two atoms with significant difference in electronegativity?

Ionic bonds form when there is a significant difference in electronegativity between two atoms. When one atom has a much higher electronegativity, it can attract electrons from a less electronegative atom, resulting in the transfer of electrons. This transfer leads to the formation of charged ions: the more electronegative atom becomes a negatively charged anion, and the less electronegative atom becomes a positively charged cation. The electrostatic attraction between these oppositely charged ions constitutes an ionic bond.

In contrast, covalent bonds typically occur between atoms with similar electronegativities, where electrons are shared rather than transferred. Hydrogen bonds are a type of weak interaction that occurs due to polar covalent bonds, particularly involving hydrogen, but they are not relevant when discussing significant electronegativity differences. Metallic bonds involve the delocalization of electrons among a lattice of metal atoms and are not influenced by electronegativity differences in the same way. Thus, when considering the interactions between atoms with significantly different electronegativities, ionic bonds are the expected outcome.