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Chapter 7: Problem 27

Would you expect \(\mathrm{CCl}_{4}\) or \(\mathrm{CBr}_{4}\) to have the higher boiling point? Explain your answer.

Short Answer

Expert verified
We expect \(\mathrm{CBr}_{4}\) to have a higher boiling point than \(\mathrm{CCl}_{4}\) because it has a greater molecular weight, leading to stronger London dispersion forces, which are the dominant intermolecular forces in both compounds.

Step by step solution

01

Identify the types of intermolecular forces present in both compounds

In both \(\mathrm{CCl}_{4}\) and \(\mathrm{CBr}_{4}\), the central carbon atom is covalently bonded to four halogen atoms. Since both compounds are nonpolar due to their symmetrical shape, there are no dipole-dipole forces or hydrogen bonding present. The only type of intermolecular forces present in both compounds are London dispersion forces.
02

Compare the London dispersion forces of both compounds

London dispersion forces increase with molecular weight and larger surface area. In \(\mathrm{CCl}_{4}\), the molecular weight is about 154 g/mol, while in \(\mathrm{CBr}_{4}\), the molecular weight is about 332 g/mol. Therefore, \(\mathrm{CBr}_{4}\) has a greater molecular weight.
03

Relate London dispersion forces to boiling point

The stronger the intermolecular forces within a compound, the higher its boiling point will be. Since \(\mathrm{CBr}_{4}\) has a greater molecular weight, it will have stronger London dispersion forces than \(\mathrm{CCl}_{4}\).
04

Conclude which compound has a higher boiling point

As a result of the stronger London dispersion forces present in \(\mathrm{CBr}_{4}\) compared to \(\mathrm{CCl}_{4}\), we expect \(\mathrm{CBr}_{4}\) to have a higher boiling point.

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Most popular questions from this chapter

Why does a gas expand to fill the container it is in, but a liquid and a solid do not?

Eicosane, \(\mathrm{C}_{20} \mathrm{H}_{42}\), has a higher melting point and a higher boiling point than water, even though water has hydrogen bonds between molecules and eicosane does not. Explain how this can be.

Which of the following does not form hydrogen bonds? Justify your choice. (a) Methyl alcohol, \(\mathrm{CH}_{3} \mathrm{OH}\) (b) Hydrofluoric acid, HF (c) Ammonia, \(\mathrm{NH}_{3}\) (d) Methane, \(\mathrm{CH}_{4}\)

Which of the following best describes a liquid: (a) The phase of matter in which particles are typically separated by the least distance (b) The phase of matter in which particles are in a fixed, rigid arrangement (c) The phase of matter in which particles completely fill the volume of their container (d) The phase of matter in which particles are in a loose, changeable arrangement but do not completely fill the volume of their container

In which of the following are there no dipoledipole forces between molecules? Justify your answer. (a) \(\mathrm{AsH}_{3}\) (b) \(\mathrm{CO}_{2}\) (c) \(\mathrm{H}_{2} \mathrm{O}\) (d) \(\mathrm{SeCl}_{2}\)
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