How do hydrogen bonds affect boiling points?
A. Molecules with hydrogen bonds will have very high boiling points.
B. Molecules with hydrogen bonds will have very low boiling points.
C. Molecules with hydrogen bonds will have higher boiling points than molecules with dipole forces, but lower boiling points than molecules with van der Waals forces.
D. Boiling points are not affected by hydrogen bonds.
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A hydrogen bond exists as an especially electrostatic force of attraction between a hydrogen atom which stands covalently bound to a more electromotive "donor" atom or group, and another electronegative atom carrying a lone pair of electrons—the hydrogen bond acceptor.

A hydrogen bond (or H-bond) exists as an especially electrostatic force of inducement between a hydrogen (H) atom which exists covalently bound to a more electronegative "donor" atom or group, and another electronegative atom maintaining a lone pair of electrons—the hydrogen bond acceptor (Ac).

Hydrogen bonding exists as a special kind of dipole-dipole attraction between molecules, not a covalent bond to a hydrogen atom. It results from the engaging force between a hydrogen atom covalently bonded to the same electronegative atom such as an N, O, or F atom and another very electronegative atom.

Molecules with hydrogen bonds will consistently have higher boiling points than also sized molecules that don't have an -O-H or an -N-H group. The hydrogen bonding creates the molecules "stickier," such that more heat (energy) exists needed to separate them.

Hence, Option A. Molecules with hydrogen bonds will have very high boiling points.

To learn more about hydrogen refer to:

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