The boiling point of a substance is greatly influenced by the type and strength of intermolecular forces present in the substance.
1. Hydrogen ([tex]$H_2$[/tex]): Hydrogen molecules exhibit weak London dispersion forces as they are non-polar and there are no permanent dipoles.
2. Fluorine ([tex]$F_2$[/tex]): Similar to hydrogen, fluorine molecules are also non-polar and experience London dispersion forces, which are relatively weak.
3. Hydrogen fluoride (HF): Hydrogen fluoride has very strong hydrogen bonding due to the high electronegativity of fluorine, which makes the H-F bond highly polar. Hydrogen bonds are much stronger compared to London dispersion forces.
Given these points, we can compare the boiling points:
- The boiling point of HF is much higher than the boiling point of [tex]$H_2$[/tex], because hydrogen bonding is significantly stronger than the weak dispersion forces in [tex]$H_2$[/tex].
- The boiling point of HF is also higher than the boiling point of [tex]$F_2$[/tex], for the same reason: hydrogen bonding in HF is stronger than the dispersion forces in [tex]$F_2$[/tex].
Therefore, the correct answers from each drop-down menu are:
- The boiling point of HF is higher than the boiling point of [tex]$H_2$[/tex], and it is higher than the boiling point of [tex]$F_2$[/tex].
