Which statement describes a polar covalent bond?

A polar covalent bond is characterized by the unequal sharing of electrons between two atoms. This occurs when the atoms involved have different electronegativities, which is the tendency of an atom to attract electrons. In a polar covalent bond, the atom with the higher electronegativity attracts the bonded electrons more strongly, resulting in a partial negative charge on that atom and a partial positive charge on the other atom. This unequal sharing creates a dipole moment, which is the hallmark of polarity in covalent bonds.

In contrast, atoms sharing electrons equally would indicate a nonpolar covalent bond, not a polar one. Complete loss or transfer of an electron signifies ionic bonding, where one atom donates an electron entirely to another, leading to the formation of charged ions. Therefore, the correct description of a polar covalent bond focuses on the unequal sharing of electrons between atoms, leading to a distribution of charge that reflects a partial polarity.