make a prediction about the relative boiling point of the nobel gases. give a reason for you answer.

Isn't the general theme is that boiling points increase with increasing molar mass.

The boiling points of the noble gases generally increase as we move down the periodic table. The reason for this trend is the increase in atomic radius, which leads to an increase in London dispersion forces.

Noble gases are known for their low reactivity and stable electron configurations. Their boiling points, however, are affected by intermolecular forces. The only intermolecular force acting between noble gas atoms is the London dispersion force, which results from temporary fluctuations in electron density.

As we move down the group, the atomic radius increases due to the addition of electron shells. With larger atoms, the dispersion forces become stronger. As a result, the boiling points increase because more energy is required to overcome these stronger intermolecular forces.

To summarize, the relative boiling points of the noble gases increase as we move down the periodic table due to the increase in atomic radius and subsequent increase in London dispersion forces.

To make a prediction about the relative boiling point of the noble gases, we need to consider their atomic properties and the trends in boiling points within the noble gas group.

The noble gases belong to Group 18 of the periodic table, which includes helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn).

The boiling point of a substance is determined by intermolecular forces, specifically the strength of the forces of attraction between its particles. These intermolecular forces are influenced by factors such as molecular size, molecular shape, and the strength of London dispersion forces.

In general, the boiling points of noble gases increase as we move down the group. This is due to the increase in atomic size and the corresponding increase in the strength of the London dispersion forces.

Helium has the lowest boiling point among the noble gases because it has the smallest atomic size. With only two electrons, helium experiences very weak London dispersion forces compared to the other noble gases, which have larger atomic sizes. This results in a lower boiling point for helium.

As we move down the group, the atomic size increases, causing an increase in the strength of London dispersion forces. Therefore, the boiling points of the noble gases increase as we move from helium to neon, argon, krypton, xenon, and radon, in that order. Radon is expected to have the highest boiling point among the noble gases due to its larger atomic size and stronger intermolecular forces.

In summary, based on the trend in atomic size and the strength of intermolecular forces, we predict that the noble gases will have boiling points in the following order: helium < neon < argon < krypton < xenon < radon.