Which statement best describes the intermolecular forces between N2

molecules and NH3 molecules in the solid phase?

A. Dipole-dipole forces are the strongest force between N2

molecules, and Van der Waals forces are the strongest between

NH3 molecules

B. Van der Waals forces are the strongest force between N2

molecules and between NH3 molecules.

C. Dipole-dipole forces are the strongest force between N2

molecules and between NH3 molecules.

D. Van der Waals forces are the strongest force between N2

molecules, and hydrogen bonding is the strongest between NHS

molecules

D. Van der Waals forces are the strongest force between N2 molecules, and hydrogen bonding is the strongest between NHS molecules

Explanation:

Vander Waal's forces are the forces which arises due to disturbance in the electron density of the molecule.

These are usually found in non polar molecules. Hence N2 is said to exhibit this force.

The bond between H atom and highly electronegative atom like N, O and F is said to be Hydrogen Bonding.

Molecules like HF, H2O, NH3 all have Hydrogen bonding in it.

The order of strength of the various intermolecular forces are as follows:

Metallic bond covalent bond (Intra molecular) > hydrogen bonding > dipole-dipole forces > Vander Waals forces

Out of these Vander Waals is the weakest force we can see.