In chemistry, a reactivity series (or activity series) is an empirical, calculated, and structurally analytical progression of a series of metals, arranged by their "reactivity" from highest to lowest. It is used to summarize information about the reactions of metals with acids and water, single displacement reactions and the extraction of metals from their ores.
|Caesium Cs||Cs+||reacts with cold water||electrolysis|
|Magnesium Mg||Mg2+||reacts very slowly with cold water, but rapidly|
in boiling water, and very vigorously with acids
|Beryllium Be||Be2+||reacts with acids and steam|
|Titanium Ti||Ti4+||reacts with concentrated mineral acids||pyrometallurgical extraction using magnesium,|
or less commonly other alkali metals, hydrogen or calcium in the Kroll process
|Manganese Mn||Mn2+||reacts with acids; very poor reaction with steam||smelting with coke|
|Chromium Cr||Cr3+||aluminothermic reaction|
|Iron Fe||Fe2+||smelting with coke|
|Antimony Sb||Sb3+||may react with some strong oxidizing acids||heat or physical extraction|
|Copper Cu||Cu2+||reacts slowly with air|
|Tungsten W||W3+||may react with some strong oxidizing acids|
Going from the bottom to the top of the table the metals:
There is no unique and fully consistent way to define the reactivity series, but it is common to use the three[failed verification] types of reaction listed below, many of which can be performed in a high-school laboratory (at least as demonstrations).
Metals in the middle of the reactivity series, such as iron, will react with acids such as sulfuric acid (but not water at normal temperatures) to give hydrogen and a metal salt, such as iron(II) sulfate:
There is some ambiguity at the borderlines between the groups. Magnesium, aluminium and zinc can react with water, but the reaction is usually very slow unless the metal samples are specially prepared to remove the surface layer of oxide which protects the rest of the metal. Copper and silver will react with nitric acid; but because nitric acid is an oxidizing acid, the oxidizing agent is not the H+ ion as in normal acids, but the NO3− ion.
The positions of lithium and sodium are changed on such a series; gold and platinum are in joint position and not gold leading, although this has little practical significance as both metals are highly unreactive.
Standard electrode potentials offer a quantitative measure of the power of a reducing agent, rather than the qualitative considerations of other reactive series. However, they are only valid for standard conditions: in particular, they only apply to reactions in aqueous solution. Even with this proviso, the electrode potentials of lithium and sodium – and hence their positions in the electrochemical series – appear anomalous. The order of reactivity, as shown by the vigour of the reaction with water or the speed at which the metal surface tarnishes in air, appears to be
the same as the reverse order of the (gas-phase) ionization energies. This is borne out by the extraction of metallic lithium by the electrolysis of a eutectic mixture of lithium chloride and potassium chloride: lithium metal is formed at the cathode, not potassium.