I am wondering why H2S has only London Dispersion forces and not Hydrogen Bonding?
For Hydrogen Bonding to be present, the Hydrogen atom must be covalently bonded to N, O or F atoms. Since N, O, or F are not present in H2S, there is no Hydrogen Bonding.
Thank you!
H2S (hydrogen sulfide) is a chemical compound composed of two hydrogen atoms bonded to a sulfur atom. When analyzing its intermolecular forces, we consider the forces that exist between different molecules, not within the molecule itself.
H2S molecules are held together by London dispersion forces, also known as van der Waals forces. These forces arise from temporary variations in the electron distribution around the atoms, resulting in temporary dipoles. These temporary dipoles can induce dipoles in neighboring molecules, creating attractive forces.
Although hydrogen is involved in the molecule, H2S does not exhibit hydrogen bonding. Hydrogen bonding occurs when hydrogen is attached to an electronegative atom (such as oxygen, nitrogen, or fluorine), and this hydrogen atom interacts with another electronegative atom in a different molecule. In H2S, while the sulfur atom is slightly electronegative, it is not electronegative enough to form hydrogen bonds.
To determine the type of intermolecular force involved, it is important to consider the polarity, electronegativity, and molecular structure of the molecule. In the case of H2S, the relatively low electronegativity difference between sulfur and hydrogen results in London dispersion forces being the dominant intermolecular force.