Which of the following statements best explains the trends in boiling points?

A.)The atomic size increases down the group, and this decreases the strength of the intermolecular forces.

B.)The total number of electrons decreases down the group, and this decreases the strength of the intermolecular forces.
C.)The total number of electrons increases down the group, and this increases the strength of the intermolecular forces.

D.)The chances of forming a permanent dipole increases down the group, and this increases the strength of the intermolecular forces.

Down the group there is increase in atomic size of the elements of a group due to the increase in atomic mass which increases the number of electrons in the atoms.

These electrons are held by Vander waal forces (or intermolecular forces) and strength of these forces increase down the group. As a result, more heat is required to move the electrons due to which there occurs increase in boiling point of atoms.

Thus, we can conclude that the statement total number of electrons increases down the group, and this increases the strength of the intermolecular forces, best explains the trends in boiling points.

Parrain Parrain · Answer 2 · 2021-10-28T16:25:48+02:00

Based on the trend in the table, we can infer that C.)The total number of electrons increases down the group, and this increases the strength of the intermolecular forces.

More electrons on the valence shell means that:

There will be more electrons to bond with for diatomic atoms
The bonding between the atoms will be stronger

As a result of the stronger bond, boiling points will have to be higher to break the forces of attraction between the molecules. This is why the boiling point is increasing as we go down the group.

In conclusion, more electrons means greater strength and higher boiling points.

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