Question

The following table lists the boiling points for hydrogen halides. Hydrogen halide Boiling point HF 20° C HCI -85°C HBr -66°C HI -35°C Select the explanation for why the boiling point of HF does not follow the observed trend of the other three hydrogen halides. HF exhibits hydrogen bonds, whereas the other hydrogen halides exhibit London dispersion forces. HF is polymeric in its liquid form, whereas the other hydrogen halides are monomeric in liquid form. HCI, HBr, and HI have polar covalent bonds, whereas HF has a strong ionic bond. The larger hydrogen halides possess more electrons, so they more easily form ionic liquids than HF.

          The following table lists the boiling points for hydrogen halides.
Hydrogen halide Boiling point
HF
20° C
HCI
-85°C
HBr
-66°C
HI
-35°C
Select the explanation for why the boiling point of HF does not follow the observed trend of the other three
hydrogen halides.
HF exhibits hydrogen bonds, whereas the other
hydrogen halides exhibit London dispersion forces.
HF is polymeric in its liquid form, whereas the other
hydrogen halides are monomeric in liquid form.
HCI, HBr, and HI have polar covalent bonds, whereas
HF has a strong ionic bond.
The larger hydrogen halides possess more electrons,
so they more easily form ionic liquids than HF.

The following table lists the boiling points for hydrogen halides.
Hydrogen halide Boiling point
HF
20° C
HCI
-85°C
HBr
-66°C
HI
-35°C
Select the explanation for why the boiling point of HF does not follow the observed trend of the other three
hydrogen halides.
HF exhibits hydrogen bonds, whereas the other
hydrogen halides exhibit London dispersion forces.
HF is polymeric in its liquid form, whereas the other
hydrogen halides are monomeric in liquid form.
HCI, HBr, and HI have polar covalent bonds, whereas
HF has a strong ionic bond.
The larger hydrogen halides possess more electrons,
so they more easily form ionic liquids than HF.

Added by Shannon H.

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