Using these standard reduction potentials, which species is the strongest oxidizing agent? F₂ + 2 e⁻ → 2 F⁻ (E° = +2.87 V); O₂ + 4 H⁺ + 4 e⁻ → 2 H₂O (E° = +1.23 V); Cu²⁺ + 2 e⁻ → Cu (E° = +0.34 V); Zn²⁺ + 2 e⁻ → Zn (E° = −0.76 V)

Core Concept

An oxidizing agent accepts electrons, so strength tracks the couple with the highest reduction potential. Fluorine tops this list at +2.87 V, more than a volt ahead of oxygen, so F₂ takes electrons from every other species shown. Ranking reduction potentials from highest to lowest orders oxidizing power, and reversing that order ranks the metals as reducing agents.