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 (1 bar).
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. For example, the equation Fe²⁺+2 e⁻ ⇌ Fe(s) (-0.44 Volt) means that it requires 2 × 0.44 ev=0.88 eV of energy to be absorbed (hence the minus sign) in order to create one neutral atom of Fe(s) from one Fe²⁺ ion and two electrons, or 0.44 eV per electron, which is 0.44 Joules per coulomb of electrons, which is 0.44 Volts.

After dividing by the number of electrons, the standard potential E is related to the standard Gibbs free energy of formation ΔG by:

E=(\sum \Delta G_{left}-\sum \Delta G_{right})/F

where F is the Faraday constant. For example, in the equation Fe²⁺+2 e⁻ ⇌ Fe(s) (-0.44 Volt) , the Gibbs energy required to create one neutral atom of Fe(s) from one Fe²⁺ ion and two electrons is 2 × 0.44 ev=0.88 ev, or 84895 J/mol of electrons, which is just the Gibbs energy of formation of an Fe²⁺ ion, since the energies of formation of e⁻ and Fe(s) are both zero.

The Nernst equation will then give potentials at concentrations, pressures, and temperatures other than standard.

Note that the table may lack consistency due to data from different sources. For example:

Cu⁺	+ e⁻	⇌	Cu(s)	(E ₁ = +0.520 V)
Cu²⁺	+ 2 e⁻	⇌	Cu(s)	(E ₂ = +0.337 V)
Cu²⁺	+ e⁻	⇌	Cu⁺	(E ₃ = +0.159 V)

Calculating the potential using Gibbs Free Energy (E
₃=2 E
₂-E
₁) gives the potential for E
₃ as 0.154 V, not the experimental value of 0.159 V.

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

Element	Half-reaction			E° (V)
Element	Oxidant	⇌	Reductant	E° (V)
&
Zz
Sr	Sr⁺ + e⁻	⇌	Sr	−4.101
Ca	Ca⁺ + e⁻	⇌	Ca	−3.8
Pr	Pr³⁺ + e⁻	⇌	Pr²⁺	−3.1
N	3 N₂(g) + 2 H⁺ + 2 e⁻	⇌	2HN ₃(aq)	−3.09
Li	Li⁺ + e⁻	⇌	Li(s)	−3.0401
N	N ₂(g) + 4H 2O + 2 e⁻	⇌	2 NH ₂OH(aq) + 2 OH⁻	−3.04
Cs	Cs⁺ + e⁻	⇌	Cs(s)	−3.026
Ca	Ca(OH) ₂ + 2 e⁻	⇌	Ca + 2 OH⁻	−3.02
Er	Er³⁺ + e⁻	⇌	Er²⁺	−3.0
Ba	Ba(OH) ₂ + 2 e⁻	⇌	Ba + 2 OH⁻	−2.99
Rb	Rb⁺ + e⁻	⇌	Rb(s)	−2.98
K	K⁺ + e⁻	⇌	K(s)	−2.931
Ba	Ba²⁺ + 2 e⁻	⇌	Ba(s)	−2.912
La	La(OH) ₃(s) + 3 e⁻	⇌	La(s) + 3 OH⁻	−2.90
Fr	Fr⁺ + e⁻	⇌	Fr	−2.9
Sr	Sr²⁺ + 2 e⁻	⇌	Sr(s)	−2.899
Sr	Sr(OH) ₂ + 2 e⁻	⇌	Sr + 2 OH⁻	−2.88
Ca	Ca²⁺ + 2 e⁻	⇌	Ca(s)	−2.868
Li	Li⁺ + C6(s) + e⁻	⇌	LiC6(s)	−2.84
Eu	Eu²⁺ + 2 e⁻	⇌	Eu(s)	−2.812
Ra	Ra²⁺ + 2 e⁻	⇌	Ra(s)	−2.8
Ho	Ho³⁺ + e⁻	⇌	Ho²⁺	−2.8
Bk	Bk³⁺ + e⁻	⇌	Bk²⁺	−2.8
Yb	Yb²⁺ + 2 e⁻	⇌	Yb	−2.76
Na	Na⁺ + e⁻	⇌	Na(s)	−2.71
Mg	Mg⁺ + e⁻	⇌	Mg	−2.70
Nd	Nd³⁺ + e⁻	⇌	Nd²⁺	−2.7
Mg	Mg(OH) ₂ + 2 e⁻	⇌	Mg + 2 OH⁻	−2.690
Sm	Sm²⁺ + 2 e⁻	⇌	Sm	−2.68
Be	Be ₂O²⁻ ₃ + 3H 2O + 4 e⁻	⇌	2 Be + 6 OH⁻	−2.63
Pm	Pm³⁺ + e⁻	⇌	Pm²⁺	−2.6
Dy	Dy³⁺ + e⁻	⇌	Dy²⁺	−2.6
No	No²⁺ + 2 e⁻	⇌	No	−2.50
Hf	HfO(OH) ₂ + H 2O + 4 e⁻	⇌	Hf + 4 OH⁻	−2.50
Th	Th(OH) ₄ + 4 e⁻	⇌	Th + 4 OH⁻	−2.48
Md	Md²⁺ + 2 e⁻	⇌	Md	−2.40
Tm	Tm²⁺ + 2 e⁻	⇌	Tm	−2.4
La	La³⁺ + 3 e⁻	⇌	La(s)	−2.379
Y	Y³⁺ + 3 e⁻	⇌	Y(s)	−2.372
Mg	Mg²⁺ + 2 e⁻	⇌	Mg(s)	−2.372
Zr	ZrO(OH)₂(s) + H 2O + 4 e⁻	⇌	Zr(s) + 4 OH⁻	−2.36
Pr	Pr³⁺ + 3 e⁻	⇌	Pr	−2.353
Ce	Ce³⁺ + 3 e⁻	⇌	Ce	−2.336
Er	Er³⁺ + 3 e⁻	⇌	Er	−2.331
Ho	Ho³⁺ + 3 e⁻	⇌	Ho	−2.33
Al	H ₂AlO⁻ ₃ + H 2O + 3 e⁻	⇌	Al + 4 OH⁻
Nd	Nd³⁺ + 3 e⁻	⇌	Nd	−2.323
Tm	Tm³⁺ + 3 e⁻	⇌	Tm	−2.319
Al	Al(OH) ₃(s) + 3 e⁻	⇌	Al(s) + 3 OH⁻	−2.31
Sm	Sm³⁺ + 3 e⁻	⇌	Sm	−2.304
Fm	Fm²⁺ + 2 e⁻	⇌	Fm	−2.30
Am	Am³⁺ + e⁻	⇌	Am²⁺	−2.3
Dy	Dy³⁺ + 3 e⁻	⇌	Dy	−2.295
Lu	Lu³⁺ + 3 e⁻	⇌	Lu	−2.28
Tb	Tb³⁺ + 3 e⁻	⇌	Tb	−2.28
Gd	Gd³⁺ + 3 e⁻	⇌	Gd	−2.279
H	H₂ + 2 e⁻	⇌	2 H⁻	−2.23
Es	Es²⁺ + 2 e⁻	⇌	Es	−2.23
Pm	Pm²⁺ + 2 e⁻	⇌	Pm	−2.2
Tm	Tm³⁺ + e⁻	⇌	Tm²⁺	−2.2
Dy	Dy²⁺ + 2 e⁻	⇌	Dy	−2.2
Ac	Ac³⁺ + 3 e⁻	⇌	Ac	−2.20
Yb	Yb³⁺ + 3 e⁻	⇌	Yb	−2.19
Cf	Cf²⁺ + 2 e⁻	⇌	Cf	−2.12
Nd	Nd²⁺ + 2 e⁻	⇌	Nd	−2.1
Ho	Ho²⁺ + 2 e⁻	⇌	Ho	−2.1
Sc	Sc³⁺ + 3 e⁻	⇌	Sc(s)	−2.077
Al	AlF³⁻ ₆ + 3 e⁻	⇌	Al + 6F⁻	−2.069
Am	Am³⁺ + 3 e⁻	⇌	Am	−2.048
Cm	Cm³⁺ + 3 e⁻	⇌	Cm	−2.04
Pu	Pu³⁺ + 3 e⁻	⇌	Pu	−2.031
Pr	Pr²⁺ + 2 e⁻	⇌	Pr	−2.0
Er	Er²⁺ + 2 e⁻	⇌	Er	−2.0
Eu	Eu³⁺ + 3 e⁻	⇌	Eu	−1.991
Lr	Lr³⁺ + 3 e⁻	⇌	Lr	−1.96
Cf	Cf³⁺ + 3 e⁻	⇌	Cf	−1.94
Es	Es³⁺ + 3 e⁻	⇌	Es	−1.91
Pa	Pa⁴⁺ + e⁻	⇌	Pa³⁺	−1.9
Am	Am²⁺ + 2 e⁻	⇌	Am	−1.9
Th	Th⁴⁺ + 4 e⁻	⇌	Th	−1.899
Fm	Fm³⁺ + 3 e⁻	⇌	Fm	−1.89
Np	Np³⁺ + 3 e⁻	⇌	Np	−1.856
Be	Be²⁺ + 2 e⁻	⇌	Be	−1.847
P	H ₂PO⁻ ₂ + e⁻	⇌	P + 2 OH⁻	−1.82
U	U³⁺ + 3 e⁻	⇌	U	−1.798
Sr	Sr²⁺ + 2 e⁻	⇌	Sr(Hg)	−1.793
B	H ₂BO⁻ ₃ + H 2O + 3 e⁻	⇌	B + 4 OH⁻	−1.79
Th	ThO ₂ + 4 H⁺ + 4 e⁻	⇌	Th + 2H 2O	−1.789
Hf	HfO²⁺ + 2 H⁺ + 4 e⁻	⇌	Hf + H 2O	−1.724
P	HPO²⁻ ₃ + 2H 2O + 3 e⁻	⇌	P + 5 OH⁻	−1.71
Si	SiO²⁻ ₃ + H 2O + 4 e⁻	⇌	Si + 6 OH⁻	−1.697
Al	Al³⁺ + 3 e⁻	⇌	Al(s)	−1.662
Ti	Ti²⁺ + 2 e⁻	⇌	Ti(s)	−1.63
Zr	ZrO₂(s) + 4 H⁺ + 4 e⁻	⇌	Zr(s) + 2H 2O	−1.553
Zr	Zr⁴⁺ + 4 e⁻	⇌	Zr(s)	−1.45
Ti	Ti³⁺ + 3 e⁻	⇌	Ti(s)	−1.37
Ti	TiO(s) + 2 H⁺ + 2 e⁻	⇌	Ti(s) + H 2O	−1.31
Ti	Ti ₂O ₃(s) + 2 H⁺ + 2 e⁻	⇌	2 TiO(s) + H 2O	−1.23
Zn	Zn(OH)²⁻ ₄ + 2 e⁻	⇌	Zn(s) + 4 OH⁻	−1.199
Mn	Mn²⁺ + 2 e⁻	⇌	Mn(s)	−1.185
Fe	Fe(CN)⁴⁻ ₆ + 6 H⁺ + 2 e⁻	⇌	Fe(s) + 6HCN(aq)	−1.16
Te	Te(s) + 2 e⁻	⇌	Te²⁻	−1.143
V	V²⁺ + 2 e⁻	⇌	V(s)	−1.13
Nb	Nb³⁺ + 3 e⁻	⇌	Nb(s)	−1.099
Sn	Sn(s) + 4 H⁺ + 4 e⁻	⇌	SnH ₄(g)	−1.07
Si	SiO₂(s) + 4 H⁺ + 4 e⁻	⇌	Si(s) + 2H 2O	−0.91
B	B(OH) ₃(aq) + 3 H⁺ + 3 e⁻	⇌	B(s) + 3H 2O	−0.89
Fe	Fe(OH)₂(s) + 2 e⁻	⇌	Fe(s) + 2 OH⁻	−0.89
Fe	Fe ₂O ₃(s) + 3H 2O + 2 e⁻	⇌	2Fe(OH)₂(s) + 2 OH⁻	−0.86
Ti	TiO²⁺ + 2 H⁺ + 4 e⁻	⇌	Ti(s) + H 2O	−0.93
H	2H 2O + 2 e⁻	⇌	H₂(g) + 2 OH⁻	−0.8277
Bi	Bi(s) + 3 H⁺ + 3 e⁻	⇌	BiH ₃	−0.8
Zn	Zn²⁺ + 2 e⁻	⇌	Zn(Hg)	−0.7628
Zn	Zn²⁺ + 2 e⁻	⇌	Zn(s)	−0.7618
Ta	[Ta ₂O ₅(s) + 10 H⁺ + 10 e⁻	⇌	2 Ta(s) + 5H 2O	−0.75
Cr	Cr³⁺ + 3 e⁻	⇌	Cr(s)	−0.74
Ag	Ag ₂S(s) + 2 e⁻	⇌	2Ag(s) + S²⁻ (aq)	−0.69
Au	[Au(CN) ₂]⁻ + e⁻	⇌	Au(s) + 2 CN⁻	−0.60
Ta	Ta³⁺ + 3 e⁻	⇌	Ta(s)	−0.6
Pb	PbO(s) + H 2O + 2 e⁻	⇌	Pb(s) + 2 OH⁻	−0.58
Ti	2 TiO₂(s) + 2 H⁺ + 2 e⁻	⇌	Ti ₂O ₃(s) + H 2O	−0.56
Ga	Ga³⁺ + 3 e⁻	⇌	Ga(s)	−0.53
U	U⁴⁺ + e⁻	⇌	U³⁺	−0.52
P	H ₃PO ₂(aq) + H⁺ + e⁻	⇌	P(white)[note 1] + 2H 2O	−0.508
P	H ₃PO ₃(aq) + 2 H⁺ + 2 e⁻	⇌	H ₃PO ₂(aq) + H 2O	−0.499
P	H ₃PO ₃(aq) + 3 H⁺ + 3 e⁻	⇌	P(red)[note 1] + 3H 2O	−0.454
Fe	Fe²⁺ + 2 e⁻	⇌	Fe(s)	−0.44
C	2 CO₂(g) + 2 H⁺ + 2 e⁻	⇌	HOOCCOOH(aq)	−0.43
Cr	Cr³⁺ + e⁻	⇌	Cr²⁺	−0.42
Cd	Cd²⁺ + 2 e⁻	⇌	Cd(s)	−0.40
Ge	GeO₂(s) + 2 H⁺ + 2 e⁻	⇌	GeO(s) + H 2O	−0.37
Cu	Cu₂O(s) + H 2O + 2 e⁻	⇌	2 Cu(s) + 2 OH⁻	−0.360
Pb	PbSO ₄(s) + 2 e⁻	⇌	Pb(s) + SO²⁻ ₄	−0.3588
Pb	PbSO ₄(s) + 2 e⁻	⇌	Pb(Hg) + SO²⁻ ₄	−0.3505
Eu	Eu³⁺ + e⁻	⇌	Eu²⁺	−0.35
In	In³⁺ + 3 e⁻	⇌	In(s)	−0.34
Tl	Tl⁺ + e⁻	⇌	Tl(s)	−0.34
Ge	Ge(s) + 4 H⁺ + 4 e⁻	⇌	GeH ₄(g)	−0.29
Co	Co²⁺ + 2 e⁻	⇌	Co(s)	−0.28
P	H ₃PO ₄(aq) + 2 H⁺ + 2 e⁻	⇌	H ₃PO ₃(aq) + H 2O	−0.276
V	V³⁺ + e⁻	⇌	V²⁺	−0.26
Ni	Ni²⁺ + 2 e⁻	⇌	Ni(s)	−0.25
As	As(s) + 3 H⁺ + 3 e⁻	⇌	AsH ₃(g)	−0.23
Ag	AgI(s) + e⁻	⇌	Ag(s) + I⁻	−0.15224
Mo	MoO₂(s) + 4 H⁺ + 4 e⁻	⇌	Mo(s) + 2H 2O	−0.15
Si	Si(s) + 4 H⁺ + 4 e⁻	⇌	SiH ₄(g)	−0.14
Sn	Sn²⁺ + 2 e⁻	⇌	Sn(s)	−0.13
O	O₂(g) + H⁺ + e⁻	⇌	HO₂•(aq)	−0.13
Pb	Pb²⁺ + 2 e⁻	⇌	Pb(s)	−0.126
W	WO₂(s) + 4 H⁺ + 4 e⁻	⇌	W(s) + 2H 2O	−0.12
P	P(red) + 3 H⁺ + 3 e⁻	⇌	PH ₃(g)	−0.111
C	CO₂(g) + 2 H⁺ + 2 e⁻	⇌	HCOOH(aq)	−0.11
Se	Se(s) + 2 H⁺ + 2 e⁻	⇌	H₂Se(g)	−0.11
C	CO₂(g) + 2 H⁺ + 2 e⁻	⇌	CO(g) + H 2O	−0.11
Sn	SnO(s) + 2 H⁺ + 2 e⁻	⇌	Sn(s) + H 2O	−0.10
Sn	SnO₂(s) + 2 H⁺ + 2 e⁻	⇌	SnO(s) + H 2O	−0.09
W	WO ₃(aq) + 6 H⁺ + 6 e⁻	⇌	W(s) + 3H 2O	−0.09
Fe	Fe ₃O ₄(s) + 8 H⁺ + 8 e⁻	⇌	3 Fe(s) + 4H 2O	−0.085
P	P(white) + 3 H⁺ + 3 e⁻	⇌	PH ₃(g)	−0.063
Fe	Fe³⁺ + 3 e⁻	⇌	Fe(s)	−0.04
C	HCOOH(aq) + 2 H⁺ + 2 e⁻	⇌	HCHO(aq) + H 2O	−0.03
H	2 H⁺ + 2 e⁻	⇌	H₂(g)	0.0000
Ag	AgBr(s) + e⁻	⇌	Ag(s) + Br⁻	+0.07133
S	S ₄O²⁻ ₆ + 2 e⁻	⇌	2 S ₂O²⁻ ₃	+0.08
N	N₂(g) + 2H 2O + 6 H⁺ + 6 e⁻	⇌	2 NH ₄OH(aq)	+0.092
Hg	HgO(s) + H 2O + 2 e⁻	⇌	Hg(l) + 2 OH⁻	+0.0977
Cu	Cu(NH ₃)²⁺ ₄ + e⁻	⇌	Cu(NH²⁰⁻ ₃ + 2 NH ₃	+0.10
Ru	Ru(NH ₃)³⁺ ₆ + e⁻	⇌	Ru(NH ₃)²⁺ ₆	+0.10
N	N ₂H ₄(aq) + 4H 2O + 2 e⁻	⇌	2 NH⁺ ₄ + 4 OH⁻	+0.11
Mo	H ₂MoO ₄(aq) + 6 H⁺ + 6 e⁻	⇌	Mo(s) + 4H 2O	+0.11
Ge	Ge⁴⁺ + 4 e⁻	⇌	Ge(s)	+0.12
C	C(s) + 4 H⁺ + 4 e⁻	⇌	CH ₄(g)	+0.13
C	HCHO(aq) + 2 H⁺ + 2 e⁻	⇌	CH ₃OH(aq)	+0.13
S	S(s) + 2 H⁺ + 2 e⁻	⇌	H₂S(g)	+0.14
Sn	Sn⁴⁺ + 2 e⁻	⇌	Sn²⁺	+0.15
Cu	Cu²⁺ + e⁻	⇌	Cu⁺	+0.159
S	HSO⁻ ₄ + 3 H⁺ + 2 e⁻	⇌	SO₂(aq) + 2H 2O	+0.16
U	UO²⁺ ₂ + e⁻	⇌	UO₂⁺	+0.163
S	SO²⁻ ₄ + 4 H⁺ + 2 e⁻	⇌	SO₂(aq) + 2H 2O	+0.17
Ti	TiO²⁺ + 2 H⁺ + e⁻	⇌	Ti³⁺ + H 2O	+0.19
Sb	SbO⁺ + 2 H⁺ + 3 e⁻	⇌	Sb(s) + H 2O	+0.20
Fe	3Fe ₂O ₃(s) + 2 H⁺ + 2 e⁻	⇌	2 Fe ₃O ₄(s) + H 2O	+0.22
Ag	AgCl(s) + e⁻	⇌	Ag(s) + Cl⁻	+0.22233
As	H ₃AsO ₃(aq) + 3 H⁺ + 3 e⁻	⇌	As(s) + 3H 2O	+0.24
Ge	GeO(s) + 2 H⁺ + 2 e⁻	⇌	Ge(s) + H 2O	+0.26
U	UO⁺ ₂ + 4 H⁺ + e⁻	⇌	U⁴⁺ + 2H 2O	+0.273
Re	Re³⁺ + 3 e⁻	⇌	Re(s)	+0.300
Bi	Bi³⁺ + 3 e⁻	⇌	Bi(s)	+0.308
Cu	Cu²⁺ + 2 e⁻	⇌	Cu(s)	+0.337
V	VO²⁺ + 2 H⁺ + e⁻	⇌	V³⁺ + H 2O	+0.34
Fe	[Fe(CN) ₆]³⁻ + e⁻	⇌	[Fe(CN) ₆]⁴⁻	+0.3704
Fe	Fc⁺ + e⁻	⇌	Fc(s)	+0.4
O	O₂(g) + 2H 2O + 4 e⁻	⇌	4 OH⁻(aq)	+0.401
Mo	H ₂MoO ₄ + 6 H⁺ + 3 e⁻	⇌	Mo³⁺ + 4H 2O	+0.43
C	CH ₃OH(aq) + 2 H⁺ + 2 e⁻	⇌	CH ₄(g) + H 2O	+0.50
S	SO₂(aq) + 4 H⁺ + 4 e⁻	⇌	S(s) + 2H 2O	+0.50
Cu	Cu⁺ + e⁻	⇌	Cu(s)	+0.520
C	CO(g) + 2 H⁺ + 2 e⁻	⇌	C(s) + H 2O	+0.52
I	I⁻ ₃	⇌	3 I⁻	+0.53
I	I ₂(s) + 2 e⁻	⇌	2 I⁻	+0.54
Au	[AuI ₄]⁻ + 3 e⁻	⇌	Au(s) + 4 I⁻	+0.56
As	H ₃AsO ₄(aq) + 2 H⁺ + 2 e⁻	⇌	H ₃AsO ₃(aq) + H 2O	+0.56
Au	[AuI₂]⁻ + e⁻	⇌	Au(s) + 2 I⁻	+0.58
Mn	MnO⁻ ₄ + 2H 2O + 3 e⁻	⇌	MnO₂(s) + 4 OH⁻	+0.595
S	S ₂O²⁻ ₃ + 6 H⁺ + 4 e⁻	⇌	2 S(s) + 3H 2O	+0.60
Mo	H ₂MoO ₄(aq) + 2 H⁺ + 2 e⁻	⇌	MoO₂(s) + 2H 2O	+0.65
C	+ 2 H⁺ + 2 e⁻	⇌		+0.6992
O	O₂(g) + 2 H⁺ + 2 e⁻	⇌	H₂O₂(aq)	+0.70
Tl	Tl³⁺ + 3 e⁻	⇌	Tl(s)	+0.72
Pt	PtCl²⁻ ₆ + 2 e⁻	⇌	PtCl²⁻ ₄ + 2 Cl⁻	+0.726
Fe	Fe ₂O ₃(s) + 6 H⁺ + 2 e⁻	⇌	2Fe²⁺ + 3H 2O	+0.728
Se	H ₂SeO ₃(aq) + 4 H⁺ + 4 e⁻	⇌	Se(s) + 3H 2O	+0.74
Pt	PtCl²⁻ ₄ + 2 e⁻	⇌	Pt(s) + 4 Cl⁻	+0.758
Fe	Fe³⁺ + e⁻	⇌	Fe²⁺	+0.77
Ag	Ag⁺ + e⁻	⇌	Ag(s)	+0.7996
Hg	Hg₂²⁺ + 2 e⁻	⇌	2 Hg(l)	+0.80
N	NO⁻ ₃(aq) + 2 H⁺ + e⁻	⇌	NO₂(g) + H 2O	+0.80
Fe	2FeO²⁻ ₄ + 5H 2O + 6 e⁻	⇌	Fe ₂O ₃(s) + 10 OH⁻	+0.81
Au	[AuBr ₄]⁻ + 3 e⁻	⇌	Au(s) + 4 Br⁻	+0.85
Hg	Hg²⁺ + 2 e⁻	⇌	Hg(l)	+0.85
Ir	[IrCl ₆]²⁻ + e⁻	⇌	[IrCl ₆]³⁻	+0.87
Mn	MnO⁻ ₄ + H⁺ + e⁻	⇌	HMnO⁻ ₄	+0.90
Hg	2 Hg²⁺ + 2 e⁻	⇌	Hg₂²⁺	+0.91
Pd	Pd²⁺ + 2 e⁻	⇌	Pd(s)	+0.915
Au	[AuCl ₄]⁻ + 3 e⁻	⇌	Au(s) + 4 Cl⁻	+0.93
Mn	MnO₂(s) + 4 H⁺ + e⁻	⇌	Mn³⁺ + 2H 2O	+0.95
N	NO⁻ ₃(aq) + 4 H⁺ + 3 e⁻	⇌	NO(g) + 2H 2O(l)	+0.958
Au	[AuBr₂]⁻ + e⁻	⇌	Au(s) + 2 Br⁻	+0.96
Fe	Fe ₃O ₄(s) + 8 H⁺ + 2 e⁻	⇌	3Fe²⁺ + 4H 2O	+0.98
Xe	[HXeO ₆]³⁻ + 2H 2O + 2 e⁻	⇌	[HXeO ₄]⁻ + 4 OH⁻	+0.99
V	[VO ₂]⁺ (aq) + 2 H⁺ + e⁻	⇌	[[VO]²⁺ (aq) + H 2O	+1.0
Te	H ₆TeO ₆(aq) + 2 H⁺ + 2 e⁻	⇌	TeO₂(s) + 4H 2O	+1.02
Br	Br₂(l) + 2 e⁻	⇌	2 Br⁻	+1.066
Br	Br₂(aq) + 2 e⁻	⇌	2 Br⁻	+1.0873
I	IO⁻ ₃ + 5 H⁺ + 4 e⁻	⇌	HIO(aq) + 2H 2O	+1.13
Au	[AuCl₂]⁻ + e⁻	⇌	Au(s) + 2 Cl⁻	+1.15
Se	HSeO⁻ ₄ + 3 H⁺ + 2 e⁻	⇌	H ₂SeO ₃(aq) + H 2O	+1.15
Ag	Ag ₂O(s) + 2 H⁺ + 2 e⁻	⇌	2 Ag(s) + H 2O	+1.17
Cl	ClO⁻ ₃ + 2 H⁺ + e⁻	⇌	ClO ₂(g) + H 2O	+1.18
Xe	[HXeO ₆]³⁻ + 5H 2O + 8 e⁻	⇌	Xe(g) + 11 OH⁻	+1.18
Pt	Pt²⁺ + 2 e⁻	⇌	Pt(s)	+1.188
Cl	ClO₂(g) + H⁺ + e⁻	⇌	HClO₂(aq)	+1.19
I	2 IO⁻ ₃ + 12 H⁺ + 10 e⁻	⇌	I₂(s) + 6H 2O	+1.20
Cl	ClO⁻ ₄ + 2 H⁺ + 2 e⁻	⇌	ClO⁻ ₃ + H 2O	+1.20
Mn	MnO ₂(s) + 4 H⁺ + 2 e⁻	⇌	Mn²⁺ + 2H 2O	+1.224
O	O₂(g) + 4 H⁺ + 4 e⁻	⇌	2H 2O	+1.229
Xe	[HXeO ₄]⁻ + 3H 2O + 6 e⁻	⇌	Xe(g) + 7 OH⁻	+1.24
Tl	Tl³⁺ + 2 e⁻	⇌	Tl⁺	+1.25
Cr	Cr ₂O²⁻ ₇ + 14 H⁺ + 6 e⁻	⇌	2 Cr³⁺ + 7H 2O	+1.33
Cl	Cl₂(g) + 2 e⁻	⇌	2 Cl⁻	+1.36
Co	CoO₂(s) + 4 H⁺ + e⁻	⇌	Co³⁺ + 2H 2O	+1.42
N	2 NH ₃OH⁺ + H⁺ + 2 e⁻	⇌	N ₂H⁺ ₅ + 2H 2O	+1.42
I	2 HIO(aq) + 2 H⁺ + 2 e⁻	⇌	I₂(s) + 2H 2O	+1.44
Br	BrO⁻ ₃ + 5 H⁺ + 4 e⁻	⇌	HBrO(aq) + 2H 2O	+1.45
Pb	β-PbO₂(s) + 4 H⁺ + 2 e⁻	⇌	Pb²⁺ + 2H 2O	+1.460
Pb	α-PbO₂(s) + 4 H⁺ + 2 e⁻	⇌	Pb²⁺ + 2H 2O	+1.468
Br	2 BrO⁻ ₃ + 12 H⁺ + 10 e⁻	⇌	Br₂(l) + 6H 2O	+1.48
Cl	2ClO⁻ ₃ + 12 H⁺ + 10 e⁻	⇌	Cl₂(g) + 6H 2O	+1.49
Cl	HClO(aq) + H⁺ + 2 e⁻	⇌	Cl⁻ (aq) + H 2O	+1.49
Mn	MnO⁻ ₄ + 8 H⁺ + 5 e⁻	⇌	Mn²⁺ + 4H 2O	+1.51
O	HO₂^• + H⁺ + e⁻	⇌	H₂O₂(aq)	+1.51
Au	Au³⁺ + 3 e⁻	⇌	Au(s)	+1.52
Ni	NiO₂(s) + 2 H⁺ + 2 e⁻	⇌	Ni²⁺ + 2 OH⁻	+1.59
Ce	Ce⁴⁺ + e⁻	⇌	Ce³⁺	+1.61
Cl	2 HClO(aq) + 2 H⁺ + 2 e⁻	⇌	Cl₂(g) + 2H 2O	+1.63
Ag	Ag ₂O ₃(s) + 6 H⁺ + 4 e⁻	⇌	2 Ag⁺ + 3H 2O	+1.67
Cl	HClO ₂(aq) + 2 H⁺ + 2 e⁻	⇌	HClO(aq) + H 2O	+1.67
Pb	Pb⁴⁺ + 2 e⁻	⇌	Pb²⁺	+1.69
Mn	MnO⁻ ₄ + 4 H⁺ + 3 e⁻	⇌	MnO₂(s) + 2H 2O	+1.70
Ag	AgO(s) + 2 H⁺ + e⁻	⇌	Ag⁺ + H 2O	+1.77
O	H ₂O ₂(aq) + 2 H⁺ + 2 e⁻	⇌	2H 2O	+1.78
Co	Co³⁺ + e⁻	⇌	Co²⁺	+1.82
Au	Au⁺ + e⁻	⇌	Au(s)	+1.83
Br	BrO⁻ ₄ + 2 H⁺ + 2 e⁻	⇌	BrO⁻ ₃ + H 2O	+1.85
Ag	Ag²⁺ + e⁻	⇌	Ag⁺	+1.98
O	S ₂O²⁻ ₈ + 2 e⁻	⇌	2 SO²⁻ ₄	+2.010
O	O ₃(g) + 2 H⁺ + 2 e⁻	⇌	O₂(g) + H 2O	+2.075
Mn	HMnO⁻ ₄ + 3 H⁺ + 2 e⁻	⇌	MnO₂(s) + 2H 2O	+2.09
Xe	XeO ₃(aq) + 6 H⁺ + 6 e⁻	⇌	Xe(g) + 3H 2O	+2.12
Xe	H ₄XeO ₆(aq) + 8 H⁺ + 8 e⁻	⇌	Xe(g) + 6 H 2O	+2.18
Fe	FeO²⁻ ₄ + 3 e⁻ + 8 H⁺	⇌	Fe³⁺ + 4H 2O	+2.20
Xe	XeF₂(aq) + 2 H⁺ + 2 e⁻	⇌	Xe(g) + 2HF(aq)	+2.32
Xe	H ₄XeO ₆(aq) + 2 H⁺ + 2 e⁻	⇌	XeO ₃(aq) + 3H 2O	+2.42
F	F₂(g) + 2 e⁻	⇌	2 F⁻	+2.87
F	F₂(g) + 2 H⁺ + 2 e⁻	⇌	2 HF(aq)	+3.05
Kr	KrF₂(aq) + 2 e⁻	⇌	Kr(g) + 2 F⁻(aq)	+3.27

References

Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
Vanýsek, Petr (2011). "Electrochemical Series". In Haynes, William M. (ed.). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. pp. 5-80–9. ISBN 978-1-4398-5512-6.
Atkins, Peter (2010). Inorganic Chemistry (5th ed.). W. H. Freeman. p. 153. ISBN 978-1-42-921820-7.
Atkins, Peter W. (1997). Physical Chemistry (6th ed.). W.H. Freeman. ISBN 9780716734659.
David R. Lide, ed., CRC Handbook of Chemistry and Physics, Internet Version 2005, http://www.hbcpnetbase.com, CRC Press, Boca Raton, FL, 2005.
Vanýsek, Petr (2012). "Electrochemical Series". In Haynes, William M. (ed.). Handbook of Chemistry and Physics (93rd ed.). CRC Press. pp. 5–80. ISBN 9781439880494.
Aylward, Gordon; Findlay, Tristan (2008). SI Chemical Data (6th ed.). Wiley. ISBN 978-0-470-81638-7.
"compounds information". Iron. WebElements Periodic Table of the Elements.
Bard, Allen J.; Parsons, Roger; Jordan, Joseph (1985). Standard Potentials in Aqueous Solution. CRC Press. ISBN 978-0-8247-7291-8.
Bard, A.J.; Faulkner, L.R. (2001). Electrochemical Methods. Fundamentals and Applications (2nd ed.). Wiley. ISBN 9781118312803.
Pourbaix, Marcel (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions. Houston, Texas; Cebelcor, Brussels: NACE International. OCLC 475102548.
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.
Rock, Peter A. (February 1966). "The Standard Oxidation Potential of the Ferrocyanide-Ferricyanide Electrode at 25° and the Entropy of Ferrocyanide Ion". The Journal of Physical Chemistry. 70 (2): 576–580. doi:10.1021/j100874a042. ISSN 0022-3654.
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.
"compounds information". Xenon. WebElements Periodic Table of the Elements.
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.
Courtney, Arlene. "Oxidation Reduction Chemistry of the Elements". Ch 412 Advanced Inorganic Chemistry: Reading Materials. Western Oregon University.
Leszczyński, P.J.; Grochala, W. (2013). "Strong Cationic Oxidizers: Thermal Decomposition, Electronic Structure and Magnetism of Their Compounds" (PDF). Acta Chim. Slov. 60 (3): 455–470.

General

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[rwP-12] 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.

[CRC-1] Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.

[Gre-2] Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.

[van92-3] Vanýsek, Petr (2011). "Electrochemical Series". In Haynes, William M. (ed.). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. pp. 5-80–9. ISBN 978-1-4398-5512-6.

[atkinshriver-4] Atkins, Peter (2010). Inorganic Chemistry (5th ed.). W. H. Freeman. p. 153. ISBN 978-1-42-921820-7.

[Atk-5] Atkins, Peter W. (1997). Physical Chemistry (6th ed.). W.H. Freeman. ISBN 9780716734659.

[6] David R. Lide, ed., CRC Handbook of Chemistry and Physics, Internet Version 2005, http://www.hbcpnetbase.com, CRC Press, Boca Raton, FL, 2005.

[van-7] Vanýsek, Petr (2012). "Electrochemical Series". In Haynes, William M. (ed.). Handbook of Chemistry and Physics (93rd ed.). CRC Press. pp. 5–80. ISBN 9781439880494.

[si-8] Aylward, Gordon; Findlay, Tristan (2008). SI Chemical Data (6th ed.). Wiley. ISBN 978-0-470-81638-7.

[webelements_fe-9] "compounds information". Iron. WebElements Periodic Table of the Elements.

[Bar-10] Bard, Allen J.; Parsons, Roger; Jordan, Joseph (1985). Standard Potentials in Aqueous Solution. CRC Press. ISBN 978-0-8247-7291-8.

[Bar2-11] Bard, A.J.; Faulkner, L.R. (2001). Electrochemical Methods. Fundamentals and Applications (2nd ed.). Wiley. ISBN 9781118312803.

[Pou-13] Pourbaix, Marcel (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions. Houston, Texas; Cebelcor, Brussels: NACE International. OCLC 475102548.

[Pang2007-14] 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] Rock, Peter A. (February 1966). "The Standard Oxidation Potential of the Ferrocyanide-Ferricyanide Electrode at 25° and the Entropy of Ferrocyanide Ion". The Journal of Physical Chemistry. 70 (2): 576–580. doi:10.1021/j100874a042. ISSN 0022-3654.

[16] 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.

[webelements_xe-17] "compounds information". Xenon. WebElements Periodic Table of the Elements.

[Cotton-18] 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.

[wou-19] Courtney, Arlene. "Oxidation Reduction Chemistry of the Elements". Ch 412 Advanced Inorganic Chemistry: Reading Materials. Western Oregon University.

[20] Leszczyński, P.J.; Grochala, W. (2013). "Strong Cationic Oxidizers: Thermal Decomposition, Electronic Structure and Magnetism of Their Compounds" (PDF). Acta Chim. Slov. 60 (3): 455–470.

Standard electrode potential (data page)

See also

References