Final answer:
Hydrogen bromide (HBr) is a polar molecule with a dipole moment directed from the hydrogen (Hδ+) to the bromine (Brδ-) indicating a partial positive charge on the H atom and a partial negative charge on the Br atom.
Step-by-step explanation:
A polar molecule such as hydrogen bromide (HBr) has a certain distribution of charges due to the difference in electronegativity between the hydrogen (H) and bromine (Br) atoms. In such molecules, the more electronegative atom acquires a partial negative charge (denoted as δ-) and the less electronegative atom acquires a partial positive charge (denoted as δ+). In the case of HBr, bromine is more electronegative than hydrogen, so the dipole moment of HBr has its negative pole at the Br end and its positive pole at the H end.
Therefore, for hydrogen bromide (HBr), the correct depiction of its dipole moment would show the delta negative (δ-) on the Br atom and the delta positive (δ+) on the H atom, indicating that Br has a partial negative charge and H has a partial positive charge. This can be visually represented as follows: Hδ+-Brδ-.