What does a greater difference in electronegativity mean for bonded atoms?

A greater difference in electronegativity between bonded atoms indicates that one atom is much better at attracting electrons than the other. This results in an unequal sharing of electron density in the bond, leading to the formation of a polar bond. The atom with higher electronegativity will attract the bonding electrons closer to itself, creating a dipole moment within the bond. This polarity affects the physical and chemical properties of substances, such as solubility and boiling points.

In contrast, a smaller difference in electronegativity tends to produce bonds that are more covalent in nature, where electrons are shared more equally between the two atoms. Stability and reactivity of the atoms involved do not directly correlate with the electronegativity difference in this context, as they depend on a variety of other factors, such as overall molecular structure and external conditions. Therefore, the concept of bond polarity is directly connected to the extent of electronegativity difference, affirming the correctness of identifying that a greater difference leads to a more polar bond.