Pick the compound with the highest boiling point in each...

Pick the compound with the highest boiling point in each pair. Explair your reasoning. a. $\mathrm{CH}_{3} \mathrm{OH}$ or $\mathrm{CH}_{3} \mathrm{SH}$ b. $\mathrm{CH}_{3} \mathrm{OCH}_{3}$ or $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}$ c. $\mathrm{CH}_{4}$ or $\mathrm{CH}_{3} \mathrm{CH}_{3}$

Pick the compound with the highest boiling point in each pair. Explair your reasoning.
a. $\mathrm{CH}_{3} \mathrm{OH}$ or $\mathrm{CH}_{3} \mathrm{SH}$
b. $\mathrm{CH}_{3} \mathrm{OCH}_{3}$ or $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}$
c. $\mathrm{CH}_{4}$ or $\mathrm{CH}_{3} \mathrm{CH}_{3}$

Key Concepts

London Dispersion Forces

London dispersion forces are weak intermolecular forces present in all molecules, stemming from temporary dipoles that occur due to the movement of electrons. Although individually weak, these forces become significant in larger or more massive molecules, where increased electron clouds lead to higher polarizability and thus higher boiling points.

Dipole–Dipole Interactions and Molecular Polarity

Dipole–dipole interactions arise from the attraction between the positive end of one polar molecule and the negative end of another. Molecular polarity, often dictated by the presence of electronegative atoms or particular functional groups, leads to these interactions, enhancing the intermolecular attractions and raising the boiling point compared to nonpolar counterparts.

Hydrogen Bonding

Hydrogen bonding is a specific and strong type of dipole–dipole interaction that occurs when a hydrogen atom is covalently bonded to a highly electronegative atom like oxygen, nitrogen, or fluorine. This bonding greatly increases the boiling point because it creates strong attractions between molecules, requiring more energy to overcome.

Intermolecular Forces

Intermolecular forces are the attractive forces between molecules that determine many physical properties such as boiling points. These forces include hydrogen bonds, dipole–dipole interactions, and London dispersion forces, and their relative strengths control how much energy is required to separate the molecules in the liquid phase.

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