Be sure to answer all parts. Arrange the following substances in order of increasing strength of intermolecular forces. Click in the answer box to open the symbol palette. a. H2
b. Ne
c. O2
d. NH3

Intermolecular forces are those forces that bind the molecules of the substance and the polarity of molecules. These forces range from the strongest to the weakest in ion-dipole, hydrogen bonding, and dipole to dipole.

Hence the form the strongest to the weakest is NH3, 02, Ne and H2.

Learn more about the substances in order of increasing the strength of intermolecular forces.

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H2<Ne<O2<NH3

Explanation:

Intermolecular forces refer to the force of attraction between molecules of a substance in any given state of matter whether solid, liquid or gas. Molecules in a substance must be held together by intermolecular forces of attraction. The magnitude of these intermolecular forces of attraction depends on many factors.

For H2, He and O2, the intermolecular force present in these gases are London forces. As the relative molecular mass of individual gas molecules becomes greater, London forces increases significantly with molecular mass. This explains the sequence shown in the answer.

NH3 has the strongest intermolecular interaction because it contains hydrogen bonds since nitrogen is an electronegative element. This a greater intermolecular interaction than dispersion forces.

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