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Chapter 12: Problem 9

The binary hydrogen compounds of the Group \(4 \mathrm{~A}\) elements are \(\mathrm{CH}_{4}\left(-162^{\circ} \mathrm{C}\right), \mathrm{SiH}_{4}\left(-112^{\circ} \mathrm{C}\right), \mathrm{GeH}_{4}\) \(\left(-88^{\circ} \mathrm{C}\right),\) and \(\mathrm{SnH}_{4}\left(-52^{\circ} \mathrm{C}\right) .\) The temperatures in parentheses are the corresponding boiling points. Explain the increase in boiling points from \(\mathrm{CH}_{4}\) to \(\mathrm{SnH}_{4}\)

Short Answer

Expert verified
The increase in boiling points from CH4 to SnH4 can be explained by the increase in the strength of the London dispersion forces. As the size and mass of the atoms (and thus, number of electrons) increase from carbon (C) to tin (Sn), the strength of these forces also increases, leading to higher boiling points.

Step by step solution

01

Explain London Dispersion Forces

London dispersion forces are the temporary attractive forces that occur when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. These forces are the weakest intermolecular force, but they become stronger as the number of electrons in a molecule increase.
02

Analyze the Binary Hydrogen Compounds of Group 4A Elements

The binary hydrogen compounds of Group 4A elements are CH4, SiH4, GeH4, and SnH4. The size and mass of the atoms increase from carbon (C), silicon (Si), germanium (Ge), to tin (Sn). Therefore, the number of electrons in each atom also increases from C to Sn, which leads to an increase in the strength of the London dispersion forces.
03

Connect the Increase of London Dispersion Forces to Boiling Points

Because the strength of London dispersion forces increases with the number of electrons, the intermolecular forces between molecules of SiH4, GeH4, and SnH4 are stronger than those of CH4. Therefore, more energy (heat) is needed to break these forces and convert the substance from a liquid to a gas, leading to a higher boiling point.

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