Reduction potential

Reduction potential is the electric potential associated with a chemical species gaining electrons. Measured relative to a reference electrode, it indicates the species’ tendency to undergo reduction.

Standard electrode potential: An electrode potential measured under defined standard conditions and reported relative to the standard hydrogen electrode. It gives reduction potentials a common scale for comparing half-reactions.
Galvanic cell: An electrochemical cell that produces electrical energy from a spontaneous redox reaction. The difference in half-cell reduction potentials predicts its voltage.
Reduction: A chemical process in which a species gains electrons or its oxidation state decreases. Reduction potential describes the electrical tendency for this electron-gain process.
Oxidation potential: The electrode potential written for a species undergoing oxidation, with the sign opposite its reduction potential. Changing a half-reaction from reduction to oxidation reverses the potential’s sign.
Standard hydrogen electrode: A reference electrode assigned a potential of zero volts under standard conditions. Reduction potentials are conventionally measured against this reference.
Electrolysis: The use of electrical energy to drive a nonspontaneous chemical reaction. Reduction potentials help determine the voltage needed to drive electrode reactions.
Oxidation: A chemical process in which a species loses electrons or its oxidation state increases. Every reduction is paired with oxidation in a redox reaction.
Formal potential: An electrode potential defined for specified solution conditions, accounting for effects such as pH and complexation. It differs from a standard potential because its conditions are not the standard state.
Nernst equation: An equation relating an electrochemical cell potential to reactant activities, temperature, and electron transfer. It shows how a reduction potential shifts away from standard conditions.
Corrosion: The deterioration of a material through chemical or electrochemical reactions with its environment. Potential differences help predict which metals oxidize in a given environment.

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