Reactivity series

Not to be confused with Electrochemical series.

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.[1][2][3] It is used to summarize information about the reactions of metals with acids and water, double displacement reactions and the extraction of metals from their ores.

Table

Metal Ion Reactivity Extraction
Caesium Cs Cs+ react with cold water electrolysis
Francium Fr Fr+
Rubidium Rb Rb+
Potassium K K+
Sodium Na Na+
Lithium Li Li+
Barium Ba Ba2+
Radium Ra Ra2+
Strontium Sr Sr2+
Calcium Ca Ca2+
Magnesium Mg Mg2+ reacts very slowly with cold water, but rapidly
in boiling water, and very vigorously with acids
Beryllium Be Be2+ react with acids and steam
Aluminium Al Al3+
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+ react with acids; very poor reaction with steam. smelting with coke
Zinc Zn Zn2+
Chromium Cr Cr3+ aluminothermic reaction
Iron Fe Fe2+ smelting with coke
Cadmium Cd Cd2+
Cobalt Co Co2+
Nickel Ni Ni2+
Tin Sn Sn2+
Lead Pb Pb2+
Antimony Sb Sb3+ may react with some strong oxidizing acids heat or physical extraction
Bismuth Bi Bi3+
Copper Cu Cu2+
Tungsten W W3+
Mercury Hg Hg2+
Silver Ag Ag+
Gold Au Au3+[4][5]
Platinum Pt Pt4+

Going from the bottom to the top of the table the metals:

Defining reactions

There is no unique and fully consistent way to define the reactivity series, but it is common to use the three types of reaction listed below, many of which can be performed in a high-school laboratory (at least as demonstrations).[4]

Reaction with water and acids

The most reactive metals, such as sodium, will react with cold water to produce hydrogen and the metal hydroxide:

2 Na (s) + 2 H2O (l) →2 NaOH (aq) + H2 (g)

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:

Fe (s) + H2SO4 (l) → FeSO4 (aq) + H2 (g)

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.

Single displacement reactions

An iron nail placed in a solution of copper sulfate will quickly change colour as metallic copper is deposited and the iron is converted into iron(II) sulfate:

Fe (s) + CuSO4 (aq) → Cu (s) + FeSO4 (aq)

In general, a metal can displace any of the metals which are lower in the reactivity series: the higher metal reduces the ions of the lower metal. This is used in the thermite reaction for preparing small quantities of metallic iron, and in the Kroll process for preparing titanium (Ti comes at about the same level as Al in the reactivity series). For example, aluminium will reduce iron(III) oxide to iron, becoming aluminium oxide in the process:

Al (s) + Fe2O3 (s) → Fe (s) + Al2O3 (s)

Similarly, magnesium can be used to extract titanium from titanium tetrachloride, forming magnesium chloride in the process:

2 Mg (s) + TiCl4 (l) → Ti (s) + 2 MgCl2 (s)

However, other factors can come into play, such as in the preparation of metallic potassium by the reduction of potassium chloride with sodium at 850 °C. Although sodium is lower than potassium in the reactivity series, the reaction can proceed because potassium is more volatile, and is distilled off from the mixture.

Na (g) + KCl (l) → K (g) + NaCl (l)

Comparison with standard electrode potentials

The reactivity series is sometimes quoted in the strict reverse order of standard electrode potentials, when it is also known as the "electrochemical series":

Li > K > Sr > Ca > Na > Mg > Al > Mn > Zn > Cr(+3) > Fe > Cd > Co > Ni > Sn > Pb > H > Cu > Hg > Ag > Pd > Ir > Pt > Au

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

potassium > sodium > lithium > alkaline earth metals,

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.[6]

See also

References

  1. ↑ France, Colin (2008), The Reactivity Series of Metals
  2. ↑ Briggs, J. G. R. (2005), Science in Focus, Chemistry for GCE 'O' Level, Pearson Education, p. 172
  3. ↑ Lim Eng Wah (2005), Longman Pocket Study Guide 'O' Level Science-Chemistry, Pearson Education, p. 190
  4. 1 2 http://www.cod.edu/people/faculty/jarman/richenda/1551_hons_materials/Activity%20series.htm
  5. ↑ Wulsberg, Gary (200). Inorganic Chemistry. p. 294.
  6. ↑ Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. pp. 82–87. ISBN 0-08-022057-6.
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