Hydrogen peroxide (H2 O2) and water (H2 O) are both liquids at room temperature, but their stand

step 1 Lewis structures of both hydrogen peroxide and water, we will see that they are both relatively

Hydrogen peroxide (H2 O2) and water (H2 O) are both liquids...

Hydrogen peroxide $\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)$ and water $\left(\mathrm{H}_{2} \mathrm{O}\right)$ are both liquids at room temperature, but their standard heats of vaporization $\Delta H_{\mathrm{vap}}^{o}$ are different: $52 \mathrm{kJ} / \mathrm{mol}$ and $41 \mathrm{kJ} / \mathrm{mol},$ respectively. Which substance has the stronger intermolecular forces? Can you suggest why?

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Key Concepts

Intermolecular Forces

Intermolecular forces encompass all the attractive forces acting between molecules, including hydrogen bonding, dipole?dipole interactions, and London dispersion forces. These forces are responsible for the physical properties of substances, such as boiling points and heats of vaporization, because they determine how strongly molecules are held together in the liquid state.

Hydrogen Bonding

Hydrogen bonding is a particularly strong type of dipole–dipole attraction that occurs when a hydrogen atom covalently bonded to a highly electronegative atom (such as oxygen) interacts with a lone pair on another electronegative atom. In compounds where hydrogen bonding is present, it substantially increases the strength of the intermolecular attractions and, consequently, the heat of vaporization.

Heat of Vaporization

The heat of vaporization is the amount of energy required to convert one mole of a liquid into its vapor phase. It is a direct measure of the strength of the intermolecular forces in the liquid; higher values indicate that more energy is needed to overcome the attractions between molecules, which means those intermolecular forces are stronger.

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