The hydrogen sulfide molecule (H2S) and the water molecule (H2O) are very similar. However, the boiling point of hydrogen sulfide is -60*C whereas the boiling point of water is 100*C. How can the intermolecular forces explain this difference?

Both molecules, the hydrogen sulfide molecule and the water molecule, are polar. Therefore, 2H2S bonded together and 2H2O bonded together creating a dipole-dipole force between them. But in 2H2O the dipole-dipole force is hydrogen bonding with Oxygen since Oxygen is more elegronegative therefore the intermolecular force between 2H2O is hydrogen bond. Moreover, to form a hydrogen bond, hydrogen must bond with Oxygen , Fluorine, or Nitrogen. Sulfur is not from these elements, therefore the dipole-dipole force between 2H2S is not a hydrogen bond. Knowing that hydrogen bonds are stronger than dipole-dipole forces, this leads to : water has a higher boiling point than hydrogen sulfide because hydrogen bonds are much stronger than dipole-dipole bonds.