Explain why the boiling point of ethylene glycol (198^∘ C) is so much higher than that of 1 -pro

step 1 Okay, so we're back to talking about boiling point. And this is more of a applied question. So w

Explain why the boiling point of ethylene glycol (198^∘ C)...

Explain why the boiling point of ethylene glycol $\left(198^{\circ} \mathrm{C}\right)$ is so much higher than that of 1 -propanol $\left(97^{\circ} \mathrm{C}\right)$, even though their molecular weights are about the same.

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Key Concepts

Intermolecular Forces

The boiling point of a substance is largely influenced by the strength of the intermolecular forces between its molecules. These forces include dispersion forces, dipole-dipole interactions, and hydrogen bonds. Stronger intermolecular attractions result in a higher boiling point because more energy is required to separate the molecules into the gas phase.

Hydrogen Bonding

Hydrogen bonding is a particularly strong type of intermolecular force occurring when hydrogen is bonded to a highly electronegative atom, such as oxygen. Molecules capable of hydrogen bonding form networks that require significantly higher energy to break apart. The more sites available for hydrogen bonding, the stronger the overall intermolecular interactions, leading to an increase in boiling point.

Molecular Structure and Functional Groups

The arrangement of atoms and the presence of specific functional groups in a molecule play a critical role in determining its physical properties. Functional groups like hydroxyl groups can donate or accept hydrogen bonds. When a molecule contains multiple such groups, it can form a more extensive network of hydrogen bonds compared to a molecule with only one hydroxyl group, thus elevating its boiling point even if the molecular weight remains similar.

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