Arrange the following compounds in order of increasing boiling point. Explain why you placed the

step 1 Hello everyone. So in these questions we have to just identify the category of boiling point in

Arrange the following compounds in order of increasing...

Key Concepts

Intermolecular Forces

Boiling points are largely determined by the strength and type of intermolecular forces acting between molecules. These forces dictate how much energy is required to separate the molecules during the phase transition from liquid to gas. The stronger the intermolecular forces (whether they be dispersion forces, dipole-dipole interactions, or hydrogen bonds), the higher the boiling point.

London Dispersion Forces

London dispersion forces are the weakest intermolecular forces that arise due to the momentary fluctuations in electron density, which induce temporary dipoles. These are present in all molecules, but become more significant for larger, more polarizable molecules. Typically, compounds with increased molecular weight or a more extended surface area exhibit stronger dispersion forces, contributing to higher boiling points.

Dipole-Dipole Interactions

Dipole-dipole interactions occur between polar molecules that possess permanent dipoles. The alignment of these dipoles leads to relatively stronger attractions compared to London dispersion forces alone. As a result, compounds with significant permanent dipoles usually boil at higher temperatures than nonpolar compounds of similar size.

Hydrogen Bonding

Hydrogen bonding is a particularly strong type of dipole-dipole interaction that occurs when hydrogen is directly bonded to highly electronegative atoms like oxygen, nitrogen, or fluorine. This bonding significantly raises the boiling point of a compound, as the energy required to overcome these attractions is much higher compared to other types of intermolecular forces.

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