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

Pick the compound with the highest boiling point in each pair. Explain your reasoning.
a. $\mathrm{NH}_{3}$ or $\mathrm{CH}_{4}$
b. $\mathrm{CS}_{2}$ or $\mathrm{CO}_{2}$
c. $\mathrm{CO}_{2}$ or $\mathrm{NO}_{2}$

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Key Concepts

London Dispersion Forces

London dispersion forces, present in all molecules, are weak intermolecular attractions that arise due to temporary fluctuations in electron density. While individually weak, their cumulative effect can influence boiling points, especially in larger or heavier nonpolar molecules.

Molecular Polarity

Molecular polarity refers to the uneven distribution of electric charge within a molecule, resulting in a dipole moment. Polar molecules can engage in dipole-dipole interactions, which are generally stronger than the London dispersion forces found in nonpolar molecules and lead to higher boiling points.

Hydrogen Bonding

Hydrogen bonding is a particularly strong type of dipole-dipole interaction that occurs when hydrogen is bonded to highly electronegative elements like nitrogen, oxygen, or fluorine. Compounds capable of hydrogen bonding typically exhibit higher boiling points due to the extra energy required to break these bonds.

Intermolecular Forces

Intermolecular forces are the attractions between molecules that must be overcome for a substance to change phase, such as boiling. These forces include hydrogen bonding, dipole-dipole interactions, and London dispersion forces, and they largely determine a compound's boiling point.

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