Question

rank the following molecules by the strength of the intermolecular forces they would have in a pure solution. strongest hcl h2 hf weakest

Explanation:

Step1: Identify intermolecular forces

• HF: It has hydrogen bonding (a strong type of dipole - dipole interaction). Hydrogen bonding occurs when \(H\) is bonded to a highly electronegative atom (\(F\) in this case).
• HCl: It has dipole - dipole forces. The \(HCl\) molecule is polar (\(\mu

eq0\)), so there are dipole - dipole interactions between \(HCl\) molecules.

• H₂: It is a non - polar molecule. The only intermolecular forces in \(H₂\) are London dispersion forces (the weakest type of intermolecular forces for small molecules).

Step2: Compare the strength of intermolecular forces

• Hydrogen bonding (\(HF\)) is stronger than dipole - dipole forces (\(HCl\)).
• Dipole - dipole forces (\(HCl\)) are stronger than London dispersion forces (\(H₂\)).

Answer:

Strongest: \(HF\), Middle: \(HCl\), Weakest: \(H₂\)