Of the substances xe, ch3cl, hf, which has: (a) the smallest dipole–dipole forces? (b) the largest hydrogen bond forces? (c) the largest dispersion forces?

(a) Xe

(b) HF

(c) Xe

Explanation:

Dipole-dipole interaction:-

This is the interaction between the two dipoles in the molecule which is formed by varying electronegativities.

Hydrogen bonding:-

Hydrogen bonding is a special type of the dipole-dipole interaction and it occurs between hydrogen atom that is bonded to highly electronegative atom which is either fluorine, oxygen or nitrogen atom.

Partially positive end of the hydrogen atom is attracted to partially negative end of these atoms which is present in another molecule. It is strong force of attraction between the molecules.

London dispersion forces:-

The intermolecular force acting in the molecule are induced dipole-dipole forces or London Dispersion forces / van der Waals forces which are the weakest intermolecular force.

Thus, Xe will have the smallest dipole–dipole forces because there is no chances of forming a dipole. Also, it has the largest dispersion forces as the other both has dipole and involved in other interactions.

Also, H-F bond is more polar than C-Cl bond and thus HF has the largest hydrogen bond forces.

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nacl or sodium chloride is an ionic compound. this is because an ionic compound pertains to a compound that consists of positively and negatively charged ions. in this case, na (sodium) has a tendency to lose one electron when it reacts with with other atoms, so the resulting sodium ion contains 11 protons and 10 electrons, thus making it positively charged (na+), when chlorine reacts, it usually gains one electron to form an ion called chloride, thus making it negatively charged ( since the ions are oppositely charged, they attract.