Reactivity series

A ranking of elements, especially metals, by how readily they react. It predicts displacement reactions and reactions with water, acids, and oxygen.

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Displacement reaction: A reaction in which a more reactive element replaces a less reactive element in a compound. A metal higher in the series can displace one lower down from its compound.
Oxidation: The loss of electrons by an atom, ion, or molecule, often accompanied by an increase in oxidation state. Metals near the reactive end readily lose electrons as they form positive ions.
Metal: An element or material that typically conducts heat and electricity and can form positive ions. The familiar series ranks metals according to their chemical tendencies.
Galvanic series: An empirical ranking of materials by corrosion potential in a particular environment, such as seawater. Unlike a general reactivity series, it ranks practical corrosion behavior in a specified medium.
Metal–acid reaction: A reaction between a metal and an acid that often produces a salt and hydrogen gas. A metal’s position helps predict whether it reacts with dilute acids to release hydrogen.
Redox reaction: A chemical reaction involving electron transfer, with oxidation and reduction occurring together. Metal reactions behind the series are paired oxidation and reduction processes.
Reactivity: The tendency of a substance to undergo chemical reactions under specified conditions. The series orders elements by this underlying chemical tendency.
Corrosion: The deterioration of a material through chemical or electrochemical reactions with its environment. Observed corrosion can depart from simple rankings because surfaces and environments alter reactions.
Metal–water reaction: A reaction in which a metal reacts with water or steam to form hydrogen and a metal compound. The series helps compare how vigorously metals react with cold water or steam.
Standard electrode potential: The voltage of a half-cell measured relative to the standard hydrogen electrode under specified conditions. Electrode potentials provide a quantitative basis for comparing metal-ion reduction tendencies.