Final answer:
The HBr molecule is polar, with the hydrogen (H) side having a partial positive charge (δ+) and the bromine (Br) side having a partial negative charge (δ-), because the electrons are closer to the more electronegative bromine atom.
Step-by-step explanation:
The charge associated with each side of the HBr molecule relates to the electronegativity difference between hydrogen (H) and bromine (Br). Hydrogen has a lower electronegativity compared to bromine, which means the electrons in the H-Br bond are more attracted to the bromine atom. Consequently, the bromine side of the molecule takes on a partial negative charge, represented by δ- (δ is the lowercase Greek letter delta), whereas the hydrogen side adopts a partial positive charge, represented by δ+. Since HBr is a diatomic molecule, it acts as a dipole with these two charged regions, resembling a magnet with a north pole and a south pole.