Final answer:
In a polar bond, the more electronegative atom carries a partial negative charge while the other atom has a partial positive charge.
Step-by-step explanation:
In a polar bond, the more electronegative atom has a partial negative charge (indicated by δ−), and the other atom has a partial positive charge (indicated by δ−).
The distribution of electron density in such a bond is uneven, with the electronegative atom attracting electrons more strongly, thus possessing more electron density and acquiring the partial negative charge. Conversely, the other atom, which has less attraction for the bonding electrons, ends up with a partial positive charge. This leads to a polar covalent bond exemplified by the H-Cl molecule, where the chlorine atom becomes slightly negative (δ−) due to a higher electronegativity than hydrogen, which becomes slightly positive (δ−).
It is important to understand that the polarity of a molecule can be affected by its shape. In cases where there are multiple polar bonds, the geometry of the molecule may result in the polarity vectors cancelling each other out, leading to a nonpolar molecule overall despite having polar bonds.