Here's why:
* Hydrogen Bonding Requirements: Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom like oxygen (O), fluorine (F), or nitrogen (N). This creates a strong dipole moment, where the hydrogen atom has a partial positive charge and the electronegative atom has a partial negative charge.
* Sulphur's Electronegativity: Sulphur is less electronegative than oxygen, fluorine, or nitrogen. This means the S-H bond is less polar, and the hydrogen atom doesn't carry a strong enough positive charge to participate in hydrogen bonding.
* Weak Interactions: While there might be some weak interactions between S-H groups due to Van der Waals forces, these are not considered true hydrogen bonds.
In summary, the lack of strong dipole moments in S-H bonds prevents the formation of hydrogen bonds in sulphides.
