Question

The normal boiling point for HBr is higher than the normal boiling point for HCl. This can be explained by Select one: A. larger dispersion forces for HBr. B. larger hydrogen-bond forces for HBr. C. larger dipole-dipole forces for HBr. D. larger dipole-dipole forces, larger dispersion forces, and larger hydrogen-bond forces for HBr.

          The normal boiling point for HBr is higher than the normal boiling point for HCl. This can be explained by
Select one:
A. larger dispersion forces for HBr.
B. larger hydrogen-bond forces for HBr.
C. larger dipole-dipole forces for HBr.
D. larger dipole-dipole forces, larger dispersion forces, and larger hydrogen-bond forces for HBr.

The normal boiling point for HBr is higher than the normal boiling point for HCl. This can be explained by
Select one:
A. larger dispersion forces for HBr.
B. larger hydrogen-bond forces for HBr.
C. larger dipole-dipole forces for HBr.
D. larger dipole-dipole forces, larger dispersion forces, and larger hydrogen-bond forces for HBr.

Added by Javier P.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sahir S

02/20/2022

Step 1

Both HBr and HCl are polar molecules, so they exhibit dipole-dipole interactions. Additionally, both have dispersion forces (London dispersion forces) due to the presence of electrons. Show more…

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The normal boiling point for HBr is higher than the normal boiling point for HCl. This can be explained by Select one: A. larger dispersion forces for HBr. B. larger hydrogen-bond forces for HBr. C. larger dipole-dipole forces for HBr. D. larger dipole-dipole forces, larger dispersion forces, and larger hydrogen-bond forces for HBr.