Which intermolecular force is predominantly responsible for...

Which intermolecular force is predominantly responsible for each observation below? (a) $\mathrm{CH}_{3}\left(\mathrm{CH}_{3}\right)_{29} \mathrm{CH}_{3}$, a component found in paraffin wax, is a solid at room temperature while octane is a liquid. (b) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}$ has a higher boiling point than $\mathrm{CH}_{4}$. (c) $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H},$ which is found in vinegar, will dissolve in water but not in oil - for simplicity you may assume oil is $\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{4} \mathrm{CH}_{3}$

Which intermolecular force is predominantly responsible for each observation below?
(a) $\mathrm{CH}_{3}\left(\mathrm{CH}_{3}\right)_{29} \mathrm{CH}_{3}$, a component found in paraffin wax, is a solid at room temperature while octane is a liquid.
(b) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}$ has a higher boiling point than $\mathrm{CH}_{4}$.
(c) $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H},$ which is found in vinegar, will dissolve in water but not in oil - for simplicity you may assume oil is $\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{4} \mathrm{CH}_{3}$

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Key Concepts

Solubility and the 'Like Dissolves Like' Principle

The solubility of substances is largely determined by the polarity of both the solute and the solvent. Polar molecules tend to dissolve in polar solvents, while nonpolar molecules dissolve in nonpolar environments. This concept explains why polar compounds can mix with water, a polar solvent, but not with nonpolar substances like most oils.

London Dispersion Forces

These are weak intermolecular forces present in all molecules, but they are the only type of intermolecular interaction in nonpolar compounds. Their strength increases with increasing molecular size and surface area, which explains why larger hydrocarbon chains have stronger attractions and can exhibit solid or higher boiling phases compared to smaller molecules.

Hydrogen Bonding

Hydrogen bonding is a strong type of dipole-dipole interaction that occurs when hydrogen is covalently bonded to highly electronegative atoms such as oxygen, nitrogen, or fluorine. This interaction significantly increases boiling points and solubility in polar solvents because it leads to stronger intermolecular attractions between molecules.

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