A. Higher electronegativity difference leads to more polar covalent bonds.

Sun, 03 May 2026 09:59:35 +0000

# A. Higher Electronegativity Difference Leads to More Polar Covalent Bonds Understanding bond polarity is fundamental to grasping molecular behavior, intermolecular forces, and chemical reactivity. In covalent bonding, electrons are shared between atoms, but this sharing is rarely equal. A key factor influencing bond polarity is the electronegativity difference between bonding atoms. A fundamental principle in chemistry is that a greater electronegativity difference results in a more polar covalent bond. This article explores how electronegativity drives bond polarity, its quantitative basis, and practical implications in chemical systems. ## What Is Electronegativity? Electronegativity is a measure of an atom’s ability to attract shared electrons in a chemical bond. It increases across a period and decreases down a group in the periodic table. Commonly used electronegativity scales include the Pauling scale, where fluorine (F) has the highest value (4.0), and cesium (Cs) the lowest (0.7). The greater the electronegativity difference between two bonded atoms, the more unevenly electrons are distributed, shaping the bond’s character.