Question

Hydrogen sulfide (H2S) is a gas at room temperature, whereas water (H2O) is a liquid. Which of the following intermolecular interactions is the main reason for this difference in boiling point?

A) London dispersion forces
B) dipole-diople interactions
C) ion-dipole interactions
D) hydrogen bonds
E) covalent bonds

Answer 1

Water (H₂O) has a higher boiling point than hydrogen sulfide (H₂S) due to the presence of hydrogen bonds, a strong form of dipole-dipole interaction, in water molecules (Option D).

Step-by-step explanation:

The main reason for the difference in boiling point between hydrogen sulfide (H₂S) and water (H₂O) is due to the presence of hydrogen bonds in water. Molecules like H₂O, which have an H atom bonded to highly electronegative atoms like O, exhibit these strong intermolecular forces.

Hydrogen sulfide lacks such bonds because sulfur is less electronegative and cannot form hydrogen bonds as oxygen does. Water's high boiling point compared to hydrogen sulfide's is a direct result of hydrogen bonding, necessitating more energy to separate its molecules during boiling.

Thus, the correct option is D.