The strongest intermolecular interactions between hydrogen sulfide (H2S) molecules arise from dipole-dipole forces.
Hydrogen sulfide is a polar molecule due to the difference in electronegativity between hydrogen and sulfur. This dipole moment leads to dipole-dipole interactions, which are significant in polar molecules. While hydrogen bonding is a strong type of dipole-dipole interaction, H2S does not form hydrogen bonds because it lacks the highly electronegative elements (like nitrogen, oxygen, or fluorine) that would be necessary to create such bonds with hydrogen.
London dispersion forces exist in all molecules, but they are typically weaker than dipole-dipole interactions in polar substances like H2S. Ion-dipole interactions and disulfide linkages are not relevant in this context for the pure H2S molecules, as they either involve ions or require specific chemical structures that are not present in simple H2S.