Question

predict what type of van der waals interactions occur between molecules of $o_{2}$, $scl_{2}$, and $ch_{4}$ in liquids of these substances?

Explanation:

• For \(O_2\):
• \(O_2\) is a non - polar molecule. Non - polar molecules have only London dispersion forces (also known as induced dipole - induced dipole forces). These forces are caused by the temporary fluctuations in electron distribution within the molecule, which induce dipoles in neighboring molecules.
• For \(SCl_2\):
• \(SCl_2\) has a bent molecular geometry. The \(S - Cl\) bonds are polar (due to the difference in electronegativity between \(S\) and \(Cl\)), and the molecule has a net dipole moment. So, \(SCl_2\) molecules experience dipole - dipole interactions (in addition to London dispersion forces, which are present in all molecules).
• For \(CH_4\):
• \(CH_4\) has a tetrahedral geometry and is non - polar (the symmetric distribution of \(C - H\) bonds cancels out any bond dipoles). Non - polar \(CH_4\) molecules have only London dispersion forces.

Answer:

• \(O_2\): London dispersion forces.
• \(SCl_2\): Dipole - dipole interactions and London dispersion forces.
• \(CH_4\): London dispersion forces.