Nitrogen gas ( ) is sparingly soluble in two polar liquids at 25 °C

CHEMISTRY · Single correct · A Level · Chemistry · Bonding · Bonding

Problem

Nitrogen gas (

\mathrm{N_2}

) is sparingly soluble in two polar liquids at 25 °C. The dipole moments of the liquids are: methanol,

1.7\,\text{D}

; dichloromethane,

1.1\,\text{D}

. All other molecular properties are comparable. Which of the following best predicts the relative strength of the attractive interaction between

\mathrm{N_2}

and each solvent? (a)

\mathrm{N_2}

interacts more strongly with dichloromethane because its greater molar mass produces stronger London dispersion forces. (b)

\mathrm{N_2}

interacts more strongly with methanol because the larger dipole moment produces a greater induced dipole in

\mathrm{N_2}

. (c)

\mathrm{N_2}

interacts more strongly with dichloromethane because a non-polar gas dissolves better in a less polar solvent ("like dissolves like"). (d)

\mathrm{N_2}

interacts more strongly with methanol because hydrogen bonding can occur between

\mathrm{N_2}

and the O–H group.