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Can anyone explain why the melting and boiling points of the noble gases increase as you go down the periodic table?

Edit: What causes the melting and boiling points to rise when the atomic number increases? What role do the valence electrons play in this?

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2 Answers 2

The melting and boiling points of noble gases are very low in comparison to those of other substances of comparable atomic and molecular masses. This indicates that only weak van der Waal's forces or weak London dispersion forces are present between the atoms of the noble gases in the liquid or the solid state.

The van der Waal's force increases with the increase in the size of the atom, and therefore, in general, the boiling and melting points increase from $He$ to $Rn$.

Helium boils at $-269^0C$. Argon has larger mass than helium and have larger dispersion forces. Because of larger size the outer electrons are less tightly held in the larger atoms so that instantaneous dipoles are more easily induced resulting in greater interaction between argon atoms. Therefore, its boiling point ($-186^0C$) is more than that of $He$.

Similarly, because of increased dispersion forces, the boiling and melting points of monoatomic noble gases increase from helium to radon.

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$\large{\color{green}{\checkmark}}$For more data of melting and boiling points of noble gas compounds, read this page

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Valence electrons have not much to do with this, as their outer shell is closed. As the other answer mentioned, dispersion forces are the ones responsible for any interaction between these atoms.

The size dependence therefore is directly coming from the size dependence of dispersion forces:

In a very simplistic way, a random charge fluctuation can polarize the otherwise perfectly apolar atoms. This induced dipole moment is then responsible for the dispersion interactions. The polarizibility of an atom increases (easier to polarize) if the atomic number increases, therefore the interactions in nobel gases will reflect this behavior.

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