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Hydrogen bonding is when a compound that's highly electronegative is bonded to F, O or N, and has a hydrogen that can participate in bonding, as well as Lp electrons that can act as an H bond acceptor HF has this.
H-Br is best described as dipole dipole, covalent, because Br isn't electronegative enough to be considered H bonding.
Now we know that hydrogen bonding or molecules that experience it will have a higher than average boiling point because all that energy will be invested into breaking the bonds made between molecules. So because H-F has this effect and not HBr, H-F will have stronger intermolecular forces.
To think about this in another way, fluorine is the more electronegative element, much more than bromine, and as you go down the group with the halogens number of shells increases, as well as another factor called polarizibilty, the - negative charge is more spread out in bromine so HBr will exist as Br- b.c of weak intermolecular forces. But Florine not so much it wants that electron so badly that it won't be F- . This also explains why HF is a bad acid.
Molecular shape I believe that