Which element is expected to have the highest electronegativity based on periodic trends, and how does this affect its bonding behavior?

Fluorine, the most electronegative element, sits at the top right of the periodic table where electronegativity increases from left to right and decreases from top to bottom; its small size and high nuclear charge pull shared electrons strongly toward itself. Because of this, fluorine readily attracts electrons from other atoms, forming polar covalent bonds or ionic bonds when paired with less electronegative partners. In a simple example, when fluorine bonds with hydrogen, the shared electron pair is pulled far toward fluorine, giving the hydrogen a slight positive charge and the fluorine a slight negative charge. This strong electron‑pulling ability makes fluorine an excellent oxidizing agent and causes it to form highly polar bonds with most other elements.