* Weak intermolecular forces: SO₂ molecules are held together by relatively weak van der Waals forces, specifically dipole-dipole interactions. This is because the molecule has a bent shape, creating a permanent dipole moment. However, these forces are weaker than hydrogen bonding or strong dipole-dipole interactions found in some other molecules.
* Small molecular size: SO₂ has a relatively small molecular size, which reduces the surface area available for intermolecular interactions. This leads to weaker overall attractions between molecules.
* Low molecular weight: The low molecular weight of SO₂ (64 g/mol) also contributes to its low boiling point. Lighter molecules tend to have lower boiling points because they require less energy to overcome the intermolecular forces and enter the gaseous state.
In contrast to other molecules:
* Molecules with strong hydrogen bonding, like water, have significantly higher boiling points because these bonds are much stronger than van der Waals forces.
* Larger molecules with more surface area, such as hydrocarbons, also have higher boiling points due to increased van der Waals interactions.
In summary: The combination of weak intermolecular forces, small molecular size, and low molecular weight all contribute to the relatively low boiling point of sulfur dioxide.
