Standard electrode potential (data page)

The data values of standard electrode potentials are given in the table below, in volts relative to the standard hydrogen electrode, and are for the following conditions:

  • A temperature of 298.15 K (25.00 °C; 77.00 °F).
  • An effective concentration of 1 mol/L for each aqueous species or a species in a mercury amalgam (an alloy of mercury with another metal).
  • A partial pressure of 101.325 kPa (absolute) (1 atm, 1.01325 bar) for each gaseous reagent. This pressure is used because most literature data are still given for this value (1 atm) rather than for the current standard of 100 kPa.
  • An activity of unity for each pure solid, pure liquid, or for water (solvent). The relation in electrode potential of metals in saltwater (as electrolyte) is given in the galvanic series.
  • Although many of the half cells are written for multiple-electron transfers, the tabulated potentials are for a single-electron transfer. All of the reactions should be divided by the stoichiometric coefficient for the electron to get the corresponding corrected reaction equation.
  • Divide the potentials by 0.059 V to get pe° values, which are necessary for the Nernst equation and other thermodynamic calculations.

Legend: (s) – solid; (l) – liquid; (g) – gas; (aq) – aqueous (default for all charged species); (Hg) – amalgam; bold – water electrolysis equations.

Half-reaction E° (V)
Oxidant ⇌ Reductant
Sr+ +  e− ⇌ Sr −4.101
Ca+ +  e− ⇌ Ca −3.8
Pr3+ +  e− ⇌ Pr2+ −3.1
3 N2(g) + 2 H+ + 2 e− ⇌ 2HN3(aq) −3.09
Li+ +  e− ⇌ Li(s) −3.0401
N2(g) + 4 H2O + 2 e− ⇌ 2 NH2OH(aq) + 2 OH− −3.04
Cs+ +  e− ⇌ Cs(s) −3.026
Ca(OH)2 + 2 e− ⇌ Ca + 2 OH− −3.02
Er3+ +  e− ⇌ Er2+ −3.0
Ba(OH)2 + 2 e− ⇌ Ba + 2 OH− −2.99
Rb+ +  e− ⇌ Rb(s) −2.98
K+ +  e− ⇌ K(s) −2.931
Ba2+ + 2 e− ⇌ Ba(s) −2.912
La(OH)3(s) + 3 e− ⇌ La(s) + 3 OH− −2.90
Fr+ +  e− ⇌ Fr −2.9
Sr2+ + 2 e− ⇌ Sr(s) −2.899
Sr(OH)2 + 2 e− ⇌ Sr + 2 OH− −2.88
Ca2+ + 2 e− ⇌ Ca(s) −2.868
Li+ + C6(s) +  e− ⇌ LiC6(s) −2.84
Eu2+ + 2 e− ⇌ Eu(s) −2.812
Ra2+ + 2 e− ⇌ Ra(s) −2.8
Ho3+ +  e− ⇌ Ho2+ −2.8
Bk3+ +  e− ⇌ Bk2+ −2.8
Yb2+ + 2 e− ⇌ Yb −2.76
Na+ +  e− ⇌ Na(s) −2.71
Mg+ +  e− ⇌ Mg −2.70
Nd3+ +  e− ⇌ Nd2+ −2.7
Mg(OH)2 + 2 e− ⇌ Mg + 2 OH− −2.690
Sm2+ + 2 e− ⇌ Sm −2.68
Be2O32− + 3 H2O + 4 e− ⇌ 2 Be + 6 OH− −2.63
Pm3+ +  e− ⇌ Pm2+ −2.6
Dy3+ +  e− ⇌ Dy2+ −2.6
No2+ + 2 e− ⇌ No −2.50
HfO(OH)2 + H2O + 4 e− ⇌ Hf + 4 OH− −2.50
Th(OH)4 + 4 e− ⇌ Th + 4 OH− −2.48
Md2+ + 2 e− ⇌ Md −2.40
Tm2+ + 2 e− ⇌ Tm −2.4
La3+ + 3 e− ⇌ La(s) −2.379
Y3+ + 3 e− ⇌ Y(s) −2.372
Mg2+ + 2 e− ⇌ Mg(s) −2.372
ZrO(OH)2(s) +  H2O + 4 e− ⇌ Zr(s) + 4 OH− −2.36
Pr3+ + 3 e− ⇌ Pr −2.353
Ce3+ + 3 e− ⇌ Ce −2.336
Er3+ + 3 e− ⇌ Er −2.331
Ho3+ + 3 e− ⇌ Ho −2.33
H2AlO3− + H2O + 3 e− ⇌ Al + 4 OH− −2.33
Nd3+ + 3 e− ⇌ Nd −2.323
Tm3+ + 3 e− ⇌ Tm −2.319
Al(OH)3(s) + 3 e− ⇌ Al(s) + 3 OH− −2.31
Sm3+ + 3 e− ⇌ Sm −2.304
Fm2+ + 2 e− ⇌ Fm −2.30
Am3+ +  e− ⇌ Am2+ −2.3
Dy3+ + 3 e− ⇌ Dy −2.295
Lu3+ + 3 e− ⇌ Lu −2.28
Tb3+ + 3 e− ⇌ Tb −2.28
Gd3+ + 3 e− ⇌ Gd −2.279
H2 + 2 e− ⇌ 2 H− −2.23
Es2+ + 2 e− ⇌ Es −2.23
Pm2+ + 2 e− ⇌ Pm −2.2
Tm3+ +  e− ⇌ Tm2+ −2.2
Dy2+ + 2 e− ⇌ Dy −2.2
Ac3+ + 3 e− ⇌ Ac −2.20
Yb3+ + 3 e− ⇌ Yb −2.19
Cf2+ + 2 e− ⇌ Cf −2.12
Nd2+ + 2 e− ⇌ Nd −2.1
Ho2+ + 2 e− ⇌ Ho −2.1
Sc3+ + 3 e− ⇌ Sc(s) −2.077
AlF63− + 3 e− ⇌ Al + 6 F− −2.069
Am3+ + 3 e− ⇌ Am −2.048
Cm3+ + 3 e− ⇌ Cm −2.04
Pu3+ + 3 e− ⇌ Pu −2.031
Pr2+ + 2 e− ⇌ Pr −2.0
Er2+ + 2 e− ⇌ Er −2.0
Eu3+ + 3 e− ⇌ Eu −1.991
Lr3+ + 3 e− ⇌ Lr −1.96
Cf3+ + 3 e− ⇌ Cf −1.94
Es3+ + 3 e− ⇌ Es −1.91
Pa4+ +  e− ⇌ Pa3+ −1.9
Am2+ + 2 e− ⇌ Am −1.9
Th4+ + 4 e− ⇌ Th −1.899
Fm3+ + 3 e− ⇌ Fm −1.89
Np3+ + 3 e− ⇌ Np −1.856
Be2+ + 2 e− ⇌ Be −1.847
H2PO2− +  e− ⇌ P + 2 OH− −1.82
U3+ + 3 e− ⇌ U −1.798
Sr2+ + 2 e− ⇌ Sr(Hg) −1.793
H2BO3− + H2O + 3 e− ⇌ B + 4 OH− −1.79
ThO2 + 4H+ + 4 e− ⇌ Th + 2 H2O −1.789
HfO2+ + 2 H+ + 4 e− ⇌ Hf + H2O −1.724
HPO32− + 2 H2O + 3 e− ⇌ P + 5 OH− −1.71
SiO32− + H2O + 4 e− ⇌ Si + 6 OH− −1.697
Al3+ + 3 e− ⇌ Al(s) −1.662
Ti2+ + 2 e− ⇌ Ti(s) −1.63
ZrO2(s) + 4 H+ + 4 e− ⇌ Zr(s) + 2 H2O −1.553
Zr4+ + 4 e− ⇌ Zr(s) −1.45
Ti3+ + 3 e− ⇌ Ti(s) −1.37
TiO(s) + 2 H+ + 2 e− ⇌ Ti(s) +  H2O −1.31
Ti2O3(s) + 2 H+ + 2 e− ⇌ 2 TiO(s) +  H2O −1.23
Zn(OH)42− + 2 e− ⇌ Zn(s) + 4 OH− −1.199
Mn2+ + 2 e− ⇌ Mn(s) −1.185
Fe(CN)64− + 6 H+ + 2  e− ⇌ Fe(s) + 6HCN(aq) −1.16
Te(s) + 2 e− ⇌ Te2− −1.143
V2+ + 2 e− ⇌ V(s) −1.13
Nb3+ + 3 e− ⇌ Nb(s) −1.099
Sn(s) + 4 H+ + 4 e− ⇌ SnH4(g) −1.07
SiO2(s) + 4 H+ + 4 e− ⇌ Si(s) + 2 H2O −0.91
B(OH)3(aq) + 3 H+ + 3 e− ⇌ B(s) + 3 H2O −0.89
Fe(OH)2(s) + 2 e− ⇌ Fe(s) + 2 OH− −0.89
Fe2O3(s) + 3 H2O + 2 e− ⇌ 2Fe(OH)2(s) + 2 OH− −0.86
TiO2+ + 2 H+ + 4 e− ⇌ Ti(s) +  H2O −0.86
2H2O + 2 e− ⇌ H2(g) + 2 OH− −0.8277
Bi(s) + 3 H+ + 3 e− ⇌ BiH3 −0.8
Zn2+ + 2 e− ⇌ Zn(Hg) −0.7628
Zn2+ + 2 e− ⇌ Zn(s) −0.7618
Ta2O5(s) + 10 H+ + 10 e− ⇌ 2 Ta(s) + 5 H2O −0.75
Cr3+ + 3 e− ⇌ Cr(s) −0.74
Ag2S(s) + 2 e− ⇌ 2Ag(s) + S2−(aq) −0.69
[Au(CN)2]− +  e− ⇌ Au(s) + 2 CN− −0.60
Ta3+ + 3 e− ⇌ Ta(s) −0.6
PbO(s) +  H2O + 2 e− ⇌ Pb(s) + 2 OH− −0.58
2 TiO2(s) + 2 H+ + 2 e− ⇌ Ti2O3(s) +  H2O −0.56
Ga3+ + 3 e− ⇌ Ga(s) −0.53
U4+ +  e− ⇌ U3+ −0.52
H3PO2(aq) +  H+ +  e− ⇌ P(white)[note 1] + 2 H2O −0.508
H3PO3(aq) + 2 H+ + 2 e− ⇌ H3PO2(aq) +  H2O −0.499
H3PO3(aq) + 3 H+ + 3 e− ⇌ P(red)[note 1] + 3 H2O −0.454
Fe2+ + 2 e− ⇌ Fe(s) −0.44
2 CO2(g) + 2 H+ + 2 e− ⇌ HOOCCOOH(aq) −0.43
Cr3+ +  e− ⇌ Cr2+ −0.42
Cd2+ + 2 e− ⇌ Cd(s) −0.40
GeO2(s) + 2 H+ + 2 e− ⇌ GeO(s) +  H2O −0.37
Cu2O(s) +  H2O + 2 e− ⇌ 2 Cu(s) + 2 OH− −0.360
PbSO4(s) + 2 e− ⇌ Pb(s) + SO42− −0.3588
PbSO4(s) + 2 e− ⇌ Pb(Hg) + SO42− −0.3505
Eu3+ +  e− ⇌ Eu2+ −0.35
In3+ + 3 e− ⇌ In(s) −0.34
Tl+ +  e− ⇌ Tl(s) −0.34
Ge(s) + 4 H+ + 4 e− ⇌ GeH4(g) −0.29
Co2+ + 2 e− ⇌ Co(s) −0.28
H3PO4(aq) + 2 H+ + 2 e− ⇌ H3PO3(aq) +  H2O −0.276
V3+ +  e− ⇌ V2+ −0.26
Ni2+ + 2 e− ⇌ Ni(s) −0.25
As(s) + 3 H+ + 3 e− ⇌ AsH3(g) −0.23
AgI(s) +  e− ⇌ Ag(s) + I− −0.15224
MoO2(s) + 4 H+ + 4 e− ⇌ Mo(s) + 2 H2O −0.15
Si(s) + 4 H+ + 4 e− ⇌ SiH4(g) −0.14
Sn2+ + 2 e− ⇌ Sn(s) −0.13
O2(g) +  H+ +  e− ⇌ HO2•(aq) −0.13
Pb2+ + 2 e− ⇌ Pb(s) −0.126
WO2(s) + 4 H+ + 4 e− ⇌ W(s) + 2 H2O −0.12
P(red) + 3 H+ + 3 e− ⇌ PH3(g) −0.111
CO2(g) + 2 H+ + 2 e− ⇌ HCOOH(aq) −0.11
Se(s) + 2 H+ + 2 e− ⇌ H2Se(g) −0.11
CO2(g) + 2 H+ + 2 e− ⇌ CO(g) +  H2O −0.11
SnO(s) + 2 H+ + 2 e− ⇌ Sn(s) +  H2O −0.10
SnO2(s) + 4 H+ + 4 e− ⇌ SnO(s) + 2 H2O −0.09
WO3(aq) + 6 H+ + 6 e− ⇌ W(s) + 3 H2O −0.09
P(white) + 3 H+ + 3 e− ⇌ PH3(g) −0.063
Fe3+ + 3 e− ⇌ Fe(s) −0.04
HCOOH(aq) + 2 H+ + 2 e− ⇌ HCHO(aq) +  H2O −0.03
2 H+ + 2 e− ⇌ H2(g) 0.0000
AgBr(s) +  e− ⇌ Ag(s) + Br− +0.07133
S4O62− + 2 e− ⇌ 2 S2O32− +0.08
Fe3O4(s) + 8 H+ + 8 e− ⇌ 3 Fe(s) + 4 H2O +0.085
N2(g) + 2 H2O + 6 H+ + 6 e− ⇌ 2 NH4OH(aq) +0.092
HgO(s) +  H2O + 2 e− ⇌ Hg(l) + 2 OH− +0.0977
Cu(NH3)42+ +  e− ⇌ Cu(NH3)2+ + 2 NH3 +0.10
Ru(NH3)63+ +  e− ⇌ Ru(NH3)62+ +0.10
N2H4(aq) + 4 H2O + 2 e− ⇌ 2 NH4+ + 4 OH− +0.11
H2MoO4(aq) + 6 H+ + 6 e− ⇌ Mo(s) + 4 H2O +0.11
Ge4+ + 4 e− ⇌ Ge(s) +0.12
C(s) + 4 H+ + 4 e− ⇌ CH4(g) +0.13
HCHO(aq) + 2 H+ + 2 e− ⇌ CH3OH(aq) +0.13
S(s) + 2 H+ + 2 e− ⇌ H2S(g) +0.14
Sn4+ + 2 e− ⇌ Sn2+ +0.15
Cu2+ +  e− ⇌ Cu+ +0.159
HSO4− + 3 H+ + 2 e− ⇌ SO2(aq) + 2 H2O +0.16
UO22+ +  e− ⇌ UO2+ +0.163
SO42− + 4 H+ + 2 e− ⇌ SO2(aq) + 2 H2O +0.17
TiO2+ + 2 H+ +  e− ⇌ Ti3+ +  H2O +0.19
SbO+ + 2 H+ + 3 e− ⇌ Sb(s) +  H2O +0.20
AgCl(s) +  e− ⇌ Ag(s) + Cl− +0.22233
H3AsO3(aq) + 3 H+ + 3 e− ⇌ As(s) + 3 H2O +0.24
GeO(s) + 2 H+ + 2 e− ⇌ Ge(s) +  H2O +0.26
UO2+ + 4 H+ +  e− ⇌ U4+ + 2 H2O +0.273
Re3+ + 3 e− ⇌ Re(s) +0.300
Bi3+ + 3 e− ⇌ Bi(s) +0.308
Cu2+ + 2 e− ⇌ Cu(s) +0.337
VO2+ + 2 H+ +  e− ⇌ V3+ +  H2O +0.34
[Fe(CN)6]3− +  e− ⇌ [Fe(CN)6]4− +0.36
Fc+ +  e− ⇌ Fc(s) +0.4
O2(g) + 2 H2O + 4 e− ⇌ 4 OH−(aq) +0.401
H2MoO4 + 6 H+ + 3 e− ⇌ Mo3+ + 4 H2O +0.43
CH3OH(aq) + 2 H+ + 2 e− ⇌ CH4(g) +  H2O +0.50
SO2(aq) + 4 H+ + 4 e− ⇌ S(s) + 2 H2O +0.50
Cu+ +  e− ⇌ Cu(s) +0.520
CO(g) + 2 H+ + 2 e− ⇌ C(s) +  H2O +0.52
I3− + 2 e− ⇌ 3 I− +0.53
I2(s) + 2 e− ⇌ 2 I− +0.54
[AuI4]− + 3 e− ⇌ Au(s) + 4 I− +0.56
H3AsO4(aq) + 2 H+ + 2 e− ⇌ H3AsO3(aq) +  H2O +0.56
[AuI2]− +  e− ⇌ Au(s) + 2 I− +0.58
S2O32 − + 6 H+ + 4 e− ⇌ 2 S(s) + 3 H2O +0.60
H2MoO4(aq) + 2 H+ + 2 e− ⇌ MoO2(s) + 2 H2O +0.65
3Fe2O3(s) + 2 H+ + 2 e− ⇌ 2 Fe3O4(s) +  H2O +0.66
+ 2 H+ + 2 e− ⇌ +0.6992
O2(g) + 2 H+ + 2 e− ⇌ H2O2(aq) +0.70
Tl3+ + 3 e− ⇌ Tl(s) +0.72
PtCl62− + 2 e− ⇌ PtCl42− + 2 Cl− +0.726
H2SeO3(aq) + 4 H+ + 4 e− ⇌ Se(s) + 3 H2O +0.74
PtCl42− + 2 e− ⇌ Pt(s) + 4 Cl− +0.758
Fe3+ +  e− ⇌ Fe2+ +0.77
Ag+ +  e− ⇌ Ag(s) +0.7996
Hg22+ + 2 e− ⇌ 2 Hg(l) +0.80
NO3−(aq) + 2 H+ +  e− ⇌ NO2(g) +  H2O +0.80
2FeO42− + 5 H2O + 6 e− ⇌ Fe2O3(s) + 10  OH− +0.81
[AuBr4]− + 3 e− ⇌ Au(s) + 4 Br− +0.85
Hg2+ + 2 e− ⇌ Hg(l) +0.85
[IrCl6]2− +  e− ⇌ [IrCl6]3− +0.87
MnO4− +  H+ +  e− ⇌ HMnO4− +0.90
2 Hg2+ + 2 e− ⇌ Hg22+ +0.91
Pd2+ + 2 e− ⇌ Pd(s) +0.915
[AuCl4]− + 3 e− ⇌ Au(s) + 4 Cl− +0.93
Fe2O3(s) + 6 H+ + 2 e− ⇌ 2Fe2+ + 3 H2O +0.94
MnO2(s) + 4 H+ +  e− ⇌ Mn3+ + 2 H2O +0.95
NO3−(aq) + 4 H+ + 3 e− ⇌ NO(g) + 2 H2O(l) +0.958
[AuBr2]− +  e− ⇌ Au(s) + 2 Br− +0.96
[HXeO6]3− + 2 H2O + 2 e− ⇌ [HXeO4]− + 4  OH− +0.99
[VO2]+(aq) + 2 H+ +  e− ⇌ [VO]2+(aq) +  H2O +1.0
H6TeO6(aq) + 2 H+ + 2 e− ⇌ TeO2(s) + 4 H2O +1.02
Br2(l) + 2 e− ⇌ 2 Br− +1.066
Br2(aq) + 2 e− ⇌ 2 Br− +1.0873
Fe3O4(s) + 8 H+ + 2 e− ⇌ 3Fe2+ + 4 H2O +1.09
IO3− + 5 H+ + 4 e− ⇌ HIO(aq) + 2 H2O +1.13
[AuCl2]− +  e− ⇌ Au(s) + 2 Cl− +1.15
HSeO4− + 3 H+ + 2 e− ⇌ H2SeO3(aq) +  H2O +1.15
Ag2O(s) + 2 H+ + 2 e− ⇌ 2 Ag(s) +  H2O +1.17
ClO3− + 2 H+ +  e− ⇌ ClO2(g) +  H2O +1.18
[HXeO6]3− + 5 H2O + 8  e− ⇌ Xe(g) + 11 OH− +1.18
Pt2+ + 2 e− ⇌ Pt(s) +1.188
ClO2(g) +  H+ +  e− ⇌ HClO2(aq) +1.19
2 IO3− + 12 H+ + 10 e− ⇌ I2(s) + 6 H2O +1.20
ClO4− + 2 H+ + 2 e− ⇌ ClO3− +  H2O +1.20
O2(g) + 4 H+ + 4 e− ⇌ 2 H2O +1.229
MnO2(s) + 4 H+ + 2 e− ⇌ Mn2+ + 2 H2O +1.23
[HXeO4]− + 3 H2O + 6  e− ⇌ Xe(g) + 7 OH− +1.24
Tl3+ + 2 e− ⇌ Tl+ +1.25
Cr2O72− + 14 H+ + 6 e− ⇌ 2 Cr3+ + 7 H2O +1.33
Cl2(g) + 2 e− ⇌ 2 Cl− +1.36
CoO2(s) + 4 H+ +  e− ⇌ Co3+ + 2 H2O +1.42
2 NH3OH+ +  H+ + 2 e− ⇌ N2H5+ + 2 H2O +1.42
2 HIO(aq) + 2 H+ + 2 e− ⇌ I2(s) + 2 H2O +1.44
BrO3− + 5 H+ + 4 e− ⇌ HBrO(aq) + 2 H2O +1.45
β-PbO2(s) + 4 H+ + 2 e− ⇌ Pb2+ + 2 H2O +1.460
α-PbO2(s) + 4 H+ + 2 e− ⇌ Pb2+ + 2 H2O +1.468
2 BrO3− + 12 H+ + 10 e− ⇌ Br2(l) + 6 H2O +1.48
2ClO3− + 12 H+ + 10 e− ⇌ Cl2(g) + 6 H2O +1.49
HClO(aq) +  H+ + 2 e− ⇌ Cl−(aq) +  H2O +1.49
MnO4− + 8 H+ + 5 e− ⇌ Mn2+ + 4 H2O +1.51
HO2• +  H+ +  e− ⇌ H2O2(aq) +1.51
Au3+ + 3 e− ⇌ Au(s) +1.52
NiO2(s) + 2 H+ + 2 e− ⇌ Ni2+ + 2 OH− +1.59
Ce4+ +  e− ⇌ Ce3+ +1.61
2 HClO(aq) + 2 H+ + 2 e− ⇌ Cl2(g) + 2 H2O +1.63
Ag2O3(s) + 6 H+ + 4 e− ⇌ 2 Ag+ + 3 H2O +1.67
HClO2(aq) + 2 H+ + 2 e− ⇌ HClO(aq) +  H2O +1.67
Pb4+ + 2 e− ⇌ Pb2+ +1.69
MnO4− + 2 H2O + 3 e− ⇌ MnO2(s) + 4 OH− +1.692
MnO4− + 4 H+ + 3 e− ⇌ MnO2(s) + 2 H2O +1.70
AgO(s) + 2 H+ +  e− ⇌ Ag+ +  H2O +1.77
H2O2(aq) + 2 H+ + 2 e− ⇌ 2 H2O +1.78
Co3+ +  e− ⇌ Co2+ +1.82
Au+ +  e− ⇌ Au(s) +1.83
BrO4− + 2 H+ + 2 e− ⇌ BrO3− +  H2O +1.85
Ag2+ +  e− ⇌ Ag+ +1.98
S2O82− + 2 e− ⇌ 2 SO42− +2.010
O3(g) + 2 H+ + 2 e− ⇌ O2(g) +  H2O +2.075
HMnO4− + 3 H+ + 2 e− ⇌ MnO2(s) + 2 H2O +2.09
XeO3(aq) + 6 H+ + 6  e− ⇌ Xe(g) + 3 H2O +2.12
H4XeO6(aq) + 8 H+ + 8  e− ⇌ Xe(g) + 6  H2O +2.18
FeO42− + 3 e− + 8 H+ ⇌ Fe3+ + 4 H2O +2.20
XeF2(aq) + 2 H+ + 2 e− ⇌ Xe(g) + 2HF(aq) +2.32
H4XeO6(aq) + 2 H+ + 2 e− ⇌ XeO3(aq) + 3 H2O +2.42
F2(g) + 2 e− ⇌ 2 F− +2.87
F2(g) + 2 H+ + 2 e− ⇌ 2 HF(aq) +3.05
KrF2(aq) + 2 e− ⇌  Kr(g) + 2 F−(aq) +3.27
  1. 1 2 Not specified in the indicated reference, but assumed due to the difference between the value −0.454 and that computed by (2×(−0.499) + (−0.508))/3 = −0.502, exactly matching the difference between the values for white (−0.063) and red (−0.111) phosphorus in equilibrium with PH3.

References

  1. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 72 73 Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
  2. 1 2 3 4 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
  3. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 Vanýsek, Petr (2011). “Electrochemical Series”, in Handbook of Chemistry and Physics: 92nd Edition (Chemical Rubber Company).
  4. 1 2 3 4 Atkins, Peter (2010). Inorganic Chemistry (5th Edition). New York: W. H. Freeman and Company. p. 153. ISBN 978-1-42-921820-7.
  5. 1 2 3 4 5 6 7 8 9 10 11 12 13 Peter Atkins (1997). Physical Chemistry, 6th edition (W.H. Freeman and Company, New York).
  6. ↑ David R. Lide, ed., CRC Handbook of Chemistry and Physics, Internet Version 2005, http://www.hbcpnetbase.com, CRC Press, Boca Raton, FL, 2005.
  7. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 Vanýsek, Petr (2012). "Electrochemical Series". In Haynes, William M. Handbook of Chemistry and Physics: 93rd Edition. Chemical Rubber Company. pp. 5–80. ISBN 9781439880494. .
  8. ↑ Gordon Aylward & Tristan Findlay (2008). "SI Chemical Data", 6th edition (John Wiley & Sons, Australia), ISBN 978-0-470-81638-7.
  9. 1 2 3 4 5 WebElements Periodic Table of the Elements | Iron | compounds information.
  10. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 Bard, A. J., Parsons, R., and Jordan, J. (1985). Standard Potentials in Aqueous Solutions (Marcel Dekker, New York).
  11. 1 2 3 4 5 6 7 8 9 10 Bard, A.J., Faulkner, L.R.(2001). Electrochemical Methods. Fundamentals and Applications, 2nd edition (John Wiley and Sons Inc).
  12. ↑ Marcel Pourbaix (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions (NACE International, Houston, Texas; Cebelcor, Brussels).
  13. ↑ Connelly, Neil G.; Geiger, William E. (1 January 1996). "Chemical Redox Agents for Organometallic Chemistry". Chemical Reviews. 96 (2): 877–910. doi:10.1021/cr940053x. PMID 11848774.
  14. 1 2 3 Pang, Suh Cem; Chin, Suk Fun; Anderson, Marc A. (July 2007). "Redox equilibria of iron oxides in aqueous-based magnetite dispersions: Effect of pH and redox potential". J. Colloid Interface Sci. 311 (1): 94–101. Bibcode:2007JCIS..311...94P. doi:10.1016/j.jcis.2007.02.058. PMID 17395194. Retrieved 2017-03-26.
  15. 1 2 3 4 5 6 7 WebElements Periodic Table of the Elements | Xenon | compounds information.
  16. 1 2 Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, ISBN 0-471-19957-5 .
  17. ↑ Redox Reactions, Western Oregon University website.
  18. ↑ http://acta.chem-soc.si/60/60-3-455.pdf.
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