What is the result when comparing the boiling points of H₂O and H₂S?

Water (H₂O) has a higher boiling point compared to hydrogen sulfide (H₂S) due to differences in molecular structure and intermolecular forces. While both molecules exhibit dipole-dipole interactions, water has strong hydrogen bonding capabilities due to the presence of highly electronegative oxygen atoms. Each water molecule can form hydrogen bonds with multiple neighboring water molecules, leading to a significant increase in the boiling point.

In contrast, H₂S molecules do not form hydrogen bonds as effectively, as sulfur is less electronegative than oxygen and does not create the same level of attraction between molecules. As a result, the intermolecular forces in H₂S are weaker, resulting in a lower boiling point compared to water.

This phenomenon illustrates the importance of intermolecular forces in determining the physical properties of substances, particularly in the case of polar molecules. Thus, H₂O's higher boiling point is attributed to the stronger hydrogen bonding that occurs in water compared to the weaker dipole-dipole interactions present in hydrogen sulfide.