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Chapter 9: Problem 122

Which of the following statements about intermolecular forces is(are) true? a. London dispersion forces are the only type of intermolecular force that nonpolar molecules exhibit. b. Molecules that have only London dispersion forces will always be gases at room temperature \(\left(25^{\circ} \mathrm{C}\right).\) c. The hydrogen-bonding forces in \(\mathrm{NH}_{3}\) are stronger than those in \(\mathrm{H}_{2} \mathrm{O}\). d. The molecules in \(\mathrm{SO}_{2}(g)\) exhibit dipole-dipole intermolecular interactions. e. \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{3}\) has stronger London dispersion forces than does \(\mathrm{CH}_{4}.\)

Short Answer

Expert verified
The true statements about intermolecular forces are a, d, and e. In nonpolar molecules, London dispersion forces are the only type of intermolecular force present (a). The polar molecule \(\mathrm{SO}_{2}(g)\) exhibits dipole-dipole intermolecular interactions (d). \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{3}\) (propane) has stronger London dispersion forces than \(\mathrm{CH}_{4}\) (methane) due to its larger size (e).

Step by step solution

01

Statement a: London dispersion forces in nonpolar molecules

London dispersion forces are the weakest of the intermolecular forces, and they occur in all molecules, both polar and nonpolar. In nonpolar molecules, London dispersion forces are the only type of intermolecular force present. Thus, statement a is true.
02

Statement b: Molecules with only London dispersion forces at room temperature

While it is true that London dispersion forces are weaker than other intermolecular forces, we cannot make the general claim that all molecules with only London dispersion forces will always be gases at room temperature. The boiling points of such molecules could vary depending on factors such as molecular size. Therefore, statement b is false.
03

Statement c: Hydrogen-bonding forces in NH3 and H2O

Hydrogen bonding forces occur when a strong dipole-dipole interaction exists between a hydrogen atom in one molecule and a highly electronegative atom (typically O, N, or F) in another molecule. In \(\mathrm{NH}_{3}\), nitrogen (with three hydrogen atoms) forms hydrogen bonds; similarly, in \(\mathrm{H}_{2} \mathrm{O}\), oxygen forms hydrogen bonds with two hydrogen atoms. However, comparing the strengths of the hydrogen bonds in these two molecules, we find that the hydrogen bonds in water are stronger due to the higher electronegativity of oxygen compared to nitrogen. Therefore, statement c is false.
04

Statement d: Intermolecular interactions in SO2(g)

\(\mathrm{SO}_{2}(g)\) is a polar molecule because it has a bent molecular geometry and sulfur is bonded to two more electronegative oxygen atoms. Thus, the molecule exhibits a difference in electron distribution, leading to the formation of a dipole. Dipole-dipole intermolecular interactions occur between polar molecules, so in the case of \(\mathrm{SO}_{2}(g)\), statement d is true.
05

Statement e: London dispersion forces in CH3CH2CH3 and CH4

The strength of London dispersion forces is influenced by the size and shape of the molecules. Larger molecules have more electrons and a greater surface area, which in turn leads to stronger London dispersion forces. \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{3}\) (propane) has a larger size compared to \(\mathrm{CH}_{4}\) (methane), so the London dispersion forces in propane are stronger than those in methane. Therefore, statement e is true. In conclusion, the true statements about intermolecular forces are a, d, and e.

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