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Table of electrochemical potentials of elements
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Table shows electrochemical potential of selected elements i.e. so-called galvanic series.

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Galvanic series#

Element nameElement symbolChemical reaction on electrodePotential relative to hydrogen electrode [V]
LithiumLiShow sourceLi++e−⇌LiLi^{+} +e ^{-} \rightleftharpoons Li-3
RubidiumRbShow sourceRb++e−⇌RbRb^{+} +e ^{-} \rightleftharpoons Rb-2.97
PotassiumKShow sourceK++e−⇌KK ^{+} +e ^{-} \rightleftharpoons K-2.92
RadiumRaShow sourceRa2++2e−⇌RaRa^{2+}+2e^{-} \rightleftharpoons Ra-2.92
BariumBaShow sourceBa2++2e−⇌BaBa^{2+}+2e^{-} \rightleftharpoons Ba-2.9
StrontiumSrShow sourceSr2++2e−⇌SrSr^{2+}+2e^{-} \rightleftharpoons Sr-2.89
CalciumCaShow sourceCa2++2e−⇌CaCa^{2+}+2e^{-} \rightleftharpoons Ca-2.84
SodiumNaShow sourceNa++e−⇌NaNa^{+} +e ^{-} \rightleftharpoons Na-2.71
LanthanumLaShow sourceLa3++3e−⇌LaLa^{3+}+3e^{-} \rightleftharpoons La-2.52
MagnesiumMgShow sourceMg2++2e−⇌MgMg^{2+}+2e^{-} \rightleftharpoons Mg-2.38
YttriumYShow sourceY2++2e−⇌YY ^{2+}+2e^{-} \rightleftharpoons Y-2.37
BerylliumBeShow sourceBe2++2e−⇌BeBe^{2+}+2e^{-} \rightleftharpoons Be-1.7
AluminiumAlShow sourceAl3++3e−⇌AlAl^{3+}+3e^{-} \rightleftharpoons Al-1.66
NiobiumNbShow sourceNb3++3e−⇌NbNb^{3+}+3e^{-} \rightleftharpoons Nb-1.1
ManganeseMnShow sourceMn2++2e−⇌MnMn^{2+}+2e^{-} \rightleftharpoons Mn-1.05
ZincZnShow sourceZn2++2e−⇌ZnZn^{2+}+2e^{-} \rightleftharpoons Zn-0.76
ChromiumCrShow sourceCr3++3e−⇌CrCr^{3+}+3e^{-} \rightleftharpoons Cr-0.71
GalliumGaShow sourceGa3++3e−⇌GaGa^{3+}+3e^{-} \rightleftharpoons Ga-0.56
IronFeShow sourceFe2++2e−⇌FeFe^{2+}+2e^{-} \rightleftharpoons Fe-0.44
CadmiumCdShow sourceCd2++2e−⇌CdCd^{2+}+2e^{-} \rightleftharpoons Cd-0.4
ThaliumTlShow sourceTl++e−⇌TlTl^{+} +e ^{-} \rightleftharpoons Tl-0.33
IndiumInShow sourceIn3++3e−⇌InIn^{3+}+3e^{-} \rightleftharpoons In-0.33
CobaltCoShow sourceCo2++2e−⇌CoCo^{2+}+2e^{-} \rightleftharpoons Co-0.28
NickelNiShow sourceNi2++2e−⇌NiNi^{2+}+2e^{-} \rightleftharpoons Ni-0.24
MolybdeniumMoShow sourceMo3++3e−⇌MoMo^{3+}+3e^{-} \rightleftharpoons Mo-0.2
TinSnShow sourceSn2++2e−⇌SnSn^{2+}+2e^{-} \rightleftharpoons Sn-0.14
LeadPbShow sourcePb2++2e−⇌PbPb^{2+}+2e^{-} \rightleftharpoons Pb-0.13
HydrogenHShow source2H++2e−⇌H22H^{+} +2e^{-} \rightleftharpoons H_20
AntimonySbShow sourceSb3++3e−⇌SbSb^{3+}+3e^{-} \rightleftharpoons Sb0.2
BismuthBiShow sourceBi3++3e−⇌BiBi^{3+}+3e^{-} \rightleftharpoons Bi0.23
CopperCuShow sourceCu2++2e−⇌CuCu^{2+}+2e^{-} \rightleftharpoons Cu0.34
RutheniumRuShow sourceRu2++2e−⇌RuRu^{2+}+2e^{-} \rightleftharpoons Ru0.45
SilverAgShow sourceAg++e−⇌AgAg^{+} +e ^{-} \rightleftharpoons Ag0.8
OsmiumOsShow sourceOs2++2e−⇌OsOs^{2+}+2e^{-} \rightleftharpoons Os0.85
MercuryHgShow sourceHg2++2e−⇌HgHg^{2+}+2e^{-} \rightleftharpoons Hg0.85
PalladiumPdShow sourcePd2++2e−⇌PdPd^{2+}+2e^{-} \rightleftharpoons Pd0.85
IridiumIrShow sourceIr3++3e−⇌IrIr^{3+}+3e^{-} \rightleftharpoons Ir1.15
PlatinumPtShow sourcePt2++2e−⇌PtPt^{2+}+2e^{-} \rightleftharpoons Pt1.2
GoldAuShow sourceAu3++3e−⇌AuAu^{3+}+3e^{-} \rightleftharpoons Au1.42

Some facts#

  • Galwanic series (voltage, electrochemical) sets up elements according to their standard potential.
  • The standard potential is measured relative to the hydrogen electrode. The potential of this electrode is assumed to be equal to zero.
  • The position of the element in the galvanic series corresponds to its chemical activity.
  • Metal located lower in the galvanic series (i.e. metal with a lower normal potential) can displace atoms of other metals from their salts.
  • Metals whose standard potential is less than the potential of a hydrogen electrode can displace hydrogen atoms from water. Such metals are usually called active metals or non-noble metals.
    ⓘ Example: Sodium displaces hydrogen atoms from water to form a sodium base:
    2Na+2H2O→2NaOH+H2↑2Na + 2H_2O \rightarrow 2NaOH + H_2\uparrow
  • The lower potential of the element, the stronger reducer it is.
  • The higher potential of the element, the stronger oxidiser it is.

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