Which type of intermolecular attractions holds ammonia molecules together with other ammonia molecules?

Hydrogen bonds (strongest).Dipole-dipole interactions (weaker than hydrogen bonds).Explanation

There are three major types of intermolecular attractions:

Hydrogen bonds,Dipole-dipole interactions, andLondon dispersion forces.

London dispersion forces exist between all molecules. It is the weakest among the three types of forces.

Dipole-dipole interactions exist between polar molecules. It is stronger than London dispersion forces.

Hydrogen bonds are attractions between

H atoms directly bonded to atoms of N, O, or F; andLone pairs of electrons on other molecules.

Hydrogen bonds is the strongest among the three types of forces.

Consider the structure of an ammonia molecule.

All three H atoms are bonded to an N atom.There is one lone pair of electrons on the central N atom.N-H bonds are highly polar.The shape of the molecule is pyramidal. As a result, dipoles from the three N-H bond remain not balanced. The molecule is overall polar.

As a result, molecules will form both hydrogen bonds and dipole-dipole interactions between them. There's also going to be London dispersion forces. Nonetheless, hydrogen bonds and dipole-dipole interactions will contribute to the majority of attractions between the molecules.

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16- counting by fours