Given that the molecules HF and HCl have similar structures and valence electrons, why are their boiling points so different? (HCl is -85°C and HF is 20°C)

A. Both are polar. HCl has hydrogen bonding, and HF has dipole-dipole forces of attraction.
B. Both are polar. HF has hydrogen bonding, and HCl has dipole-dipole forces of attraction.
C. Both are polar. HCl has London dispersion forces, and HF has dipole-dipole forces of attraction.
D. Both are polar. Both have hydrogen bonding forces, but HF is higher on the periodic table.

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GinnyAnswer GinnyAnswer · Answer 1 · 2024-06-27T09:40:52-04:00

Intermolecular forces such as dipole-dipole attractions and hydrogen bonding influence the boiling points of hydrogen halides like HCl and HF.

The boiling points of hydrogen halides are influenced by the strength of intermolecular forces present in the molecules:

Dipole-dipole attractions between HCl molecules are stronger than London dispersion forces in nonpolar F₂, leading to a higher boiling point for HCl.
HF forms hydrogen bonding due to the hydrogen present at the positive end of the polar bond, resulting in a much higher boiling point compared to other hydrogen halides.
As the dipole moment increases, the boiling point generally increases because larger dipole moments indicate stronger intermolecular forces.

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