Arrange these compounds in order of increasing boiling...

Arrange these compounds in order of increasing boiling point. Values in $^{\circ} \mathrm{C}$ are $0,35,$ and 97 (a) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}$ (b) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OCH}_{2} \mathrm{CH}_{3}$ (c) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3}$

Arrange these compounds in order of increasing boiling point. Values in $^{\circ} \mathrm{C}$ are $0,35,$ and 97
(a) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}$
(b) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OCH}_{2} \mathrm{CH}_{3}$
(c) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3}$

Key Concepts

Hydrogen Bonding

Hydrogen bonding is a particularly strong type of dipole-dipole interaction that occurs when hydrogen is covalently bonded to highly electronegative atoms such as oxygen. Molecules capable of hydrogen bonding typically have significantly higher boiling points compared to similar molecules that do not hydrogen bond, due to the additional energy required to break these bonds.

Molecular Polarity

Molecular polarity refers to the distribution of electrical charge within a molecule. Polar molecules have uneven charge distributions, leading to dipole-dipole interactions between molecules, which increase the boiling point. Nonpolar molecules, with more even charge distributions, generally have only weak London dispersion forces leading to lower boiling points.

Intermolecular Forces

Intermolecular forces are the attractions between molecules that influence physical properties such as boiling points. The strengths of these forces, which include hydrogen bonding, dipole-dipole interactions, and London dispersion forces, determine how much energy is needed to separate the molecules during the phase transition from liquid to gas.

London Dispersion Forces

London dispersion forces are the weakest intermolecular force and arise due to temporary fluctuations in electron density within molecules. These forces are the only attractions in nonpolar molecules and typically result in lower boiling points when compared to molecules with stronger intermolecular forces, such as hydrogen bonds or dipole-dipole interactions.

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