Chapter 11: Problem 15

Which member of each of the following pairs of substances would you expect to have a higher boiling point? (a) \(\mathrm{O}_{2}\) and \(\mathrm{Cl}_{2},\) (b) \(\mathrm{SO}_{2}\) and \(\mathrm{CO}_{2}\), (c) \(\mathrm{HF}\) and \(\mathrm{HI}\)

Short Answer

Expert verified

The substances with higher boiling points are: (a) \(\mathrm{Cl}_{2}\), (b) \(\mathrm{SO}_{2}\), and (c) \(\mathrm{HF}\)

Step by step solution

Consider pair (a) \(\mathrm{O}_{2}\) and \(\mathrm{Cl}_{2}\)

Consider the molecule sizes and electron configurations of these two substances. Oxygen is a smaller molecule than Chlorine. Larger molecules and those with more electrons produce stronger London dispersion forces, which are the primary intermolecular forces for nonpolar molecules like these. Thus, \(\mathrm{Cl}_{2}\) has higher boiling point because it has stronger London dispersion forces.

Think over pair (b) \(\mathrm{SO}_{2}\) and \(\mathrm{CO}_{2}\)

Although \(\mathrm{SO}_{2}\) and \(\mathrm{CO}_{2}\) are both linear molecules consisting of two double bonds, \(\mathrm{SO}_{2}\) is a polar molecule and \(\mathrm{CO}_{2}\) is nonpolar. Polar molecules experience dipole-dipole interactions along with London dispersion forces, while nonpolar molecules only experience London dispersion forces. Therefore, \(\mathrm{SO}_{2}\) has a higher boiling point.

Evaluate pair (c) \(\mathrm{HF}\) and \(\mathrm{HI}\)

Both \(\mathrm{HF}\) and \(\mathrm{HI}\) are polar molecules that exhibit dipole-dipole intermolecular forces. However, \(\mathrm{HF}\) participates in hydrogen bonding, a special kind of dipole-dipole interaction. The presence of hydrogen bonding in \(\mathrm{HF}\) significantly increases its boiling point over \(\mathrm{HI}\). Thus, \(\mathrm{HF}\) has a higher boiling point.

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Which member of each of the following pairs of substances would you expect to have a higher boiling point? (a) \(\mathrm{O}_{2}\) and \(\mathrm{Cl}_{2},\) (b) \(\mathrm{SO}_{2}\) and \(\mathrm{CO}_{2}\), (c) \(\mathrm{HF}\) and \(\mathrm{HI}\)

Short Answer

Step by step solution

Consider pair (a) \(\mathrm{O}_{2}\) and \(\mathrm{Cl}_{2}\)

Think over pair (b) \(\mathrm{SO}_{2}\) and \(\mathrm{CO}_{2}\)

Evaluate pair (c) \(\mathrm{HF}\) and \(\mathrm{HI}\)

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