Identify the predominant type of intermolecular force in each of the following compounds Drag each item to the appropriate bin.

All molecules will have London dispersion forces which get stronger as the molecule gets heavier (more electrons causes a shift in electron cloud distribution resulting in a temporary dipole).

CHF₃ is a polar molecule. So it will have dipole - dipole interaction along with the weaker dispersion forces.

OF₂ is a polar molecule with a bent shape just like H₂O. There are two pairs of bonded electrons and two pairs of non bonded lone pair electrons. These lone pairs repel the bonded electrons resulting in a bent shape with an angle less than 105 degree. The dominant inter molecular forces would be dipole-dipole.

HF is a polar molecule. Hence the primary inter molecular forces would be dipole - dipole and hydrogen bond which is a special type of dipole - dipole interaction between the hydrogen atom and electronegative F atom.

CF4 has a tetrahedral structure. It is non-polar molecule. The dominant inter molecular force would be London dispersion force.

Thus we can sum up here as ----

CHF₃ - dipole-dipole

OF₂ -dipole-dipole

HF- hydrogen bonding

CF₄ - London force