Chemistry:Standard electrode potential (data page)

Short description: Data values of standard electrode potential

The data below tabulates standard electrode potentials (E°), in volts relative to the standard hydrogen electrode, at:

Temperature 298.15 K (25.00 °C; 77.00 °F);
Effective concentration 1 mol/L for each aqueous or amalgamated (mercury-alloyed) species;
Unit activity for each solvent and pure solid or liquid species; and
Absolute partial pressure 101.325 kPa (1.00000 atm; 1.01325 bar) for each gaseous reagent — the convention in most literature data but not the current standard state (100 kPa).

The Nernst equation adjusts for general concentrations, pressures, or temperatures.

Simultaneous half-reactions do not in general add voltages, but instead add Gibbs free energy change: the product of the voltage and the number of electrons transferred, typically the Faraday constant. For example, from FeTemplate:2+ + 2 e⁻ ⇌ Fe(s) (–0.44 V), the energy to create one neutral atom of Fe(s) from one FeTemplate:2+ ion and two electrons is 2 × 0.44 eV = 0.88 eV, or 84 895 J/(mol e⁻). That value is also the standard formation energy for an FeTemplate:2+ ion, since e⁻ and Fe(s) both have zero formation energy.

Data from different sources may cause table inconsistencies. For example: $\begin{aligned} C u^{+} + e^{-} & ⇌ & C u (s) & E_{1} = + 0.520 V \\ C u^{2 +} + 2 e^{-} & ⇌ & C u & E_{2} = + 0.337 V \\ C u^{2 +} + e^{-} & ⇌ & C u^{+} & E_{3} = + 0.159 V \end{aligned}$ Additivity of Gibbs energy implies $E_{3} = \frac{2 \cdot E_{2} - 1 \cdot E_{1}}{1} = 0.154 V,$ not the experimental 0.159 V.

Table of standard electrode potentials

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	Electrons	Ref.
Element	Oxidant	⇌	Reductant	E° / V	Electrons	Ref.
Sr	Sr⁺ + e⁻	⇌	Sr(s)	-4.101	1	^[1]
Ca	Ca⁺ + e⁻	⇌	Ca(s)	-3.8	1	^[1]
Th	Th⁴⁺ + e⁻	⇌	Th³⁺	-3.6	1	^[2]
Pr	Pr³⁺ + e⁻	⇌	Pr²⁺	-3.1	1	Estimated^[3]
N	3N₂(g) + 2 H⁺ + 2 e⁻	⇌	2HN₃(aq)	-3.09	2	^[4]^[5]
Li	Li⁺ + e⁻	⇌	Li(s)	-3.0401	1	^[5]^[6]^: 153
N	N₂(g) + 4H 2O + 2 e⁻	⇌	2NH₂OH(aq) + 2 OH⁻	-3.04	2	^[4]
Cs	Cs⁺ + e⁻	⇌	Cs(s)	-3.026	1	^[5]
Ca	Ca(OH)₂ + 2 e⁻	⇌	Ca(s) + 2 OH⁻	-3.02	2	^[1]
Er	Er³⁺ + e⁻	⇌	Er²⁺	-3	1	^[1]
Ba	Ba(OH)₂ + 2 e⁻	⇌	Ba(s) + 2 OH⁻	-2.99	2	^[1]
Rb	Rb⁺ + e⁻	⇌	Rb(s)	-2.98	1	^[5]
K	K⁺ + e⁻	⇌	K(s)	-2.931	1	^[5]
Ba	Ba²⁺ + 2 e⁻	⇌	Ba(s)	-2.912	2	^[5]
La	La(OH)₃(s) + 3 e⁻	⇌	La(s) + 3 OH⁻	-2.9	3	^[5]
Fr	Fr⁺ + e⁻	⇌	Fr(s)	-2.9	1	^[1]
Sr	Sr²⁺ + 2 e⁻	⇌	Sr(s)	-2.899	2	^[5]
Sr	Sr(OH)₂ + 2 e⁻	⇌	Sr(s) + 2 OH⁻	-2.88	2	^[1]
Ca	Ca²⁺ + 2 e⁻	⇌	Ca(s)	-2.868	2	^[5]^[6]^: 153
Li	Li⁺ + C₆(s) + e⁻	⇌	LiC₆(s)	-2.84	1	^[5]
Eu	Eu²⁺ + 2 e⁻	⇌	Eu(s)	-2.812	2	^[5]
Ra	Ra²⁺ + 2 e⁻	⇌	Ra(s)	-2.8	2	^[5]
Ho	Ho³⁺ + e⁻	⇌	-2.8	1	^[1]
Bk	Bk³⁺ + e⁻	⇌	Bk²⁺	-2.8	1	^[1]
Yb	Yb²⁺ + 2 e⁻	⇌	Yb(s)	-2.76	2	^[1]
Na	Na⁺ + e⁻	⇌	Na(s)	-2.71	1	^[5]^[7]
Mg	Mg⁺ + e⁻	⇌	Mg(s)	-2.7	1	^[1]
Nd	Nd³⁺ + e⁻	⇌	Nd²⁺	-2.7	1	^[1]
Mg	Mg(OH)₂ + 2 e⁻	⇌	Mg(s) + 2 OH⁻	-2.69	2	^[1]
Sm	Sm²⁺ + 2 e⁻	⇌	Sm(s)	-2.68	2	^[1]
Be	Be₂O2−3 + 3H 2O + 4 e⁻	⇌	2Be(s) + 6 OH⁻	-2.63	4	^[1]
Pm	Pm³⁺ + e⁻	⇌	Pm²⁺	-2.6	1	^[1]
Dy	Dy³⁺ + e⁻	⇌	Dy²⁺	-2.6	1	^[1]
No	No²⁺ + 2 e⁻	⇌	No	-2.5	2	^[1]
Hf	HfO(OH)₂ + H 2O + 4 e⁻	⇌	Hf(s) + 4 OH⁻	-2.5	4	^[1]
Th	Th(OH)₄ + 4 e⁻	⇌	Th(s) + 4 OH⁻	-2.48	4	^[1]
Md	Md²⁺ + 2 e⁻	⇌	Md	-2.4	2	^[1]
Tm	Tm²⁺ + 2 e⁻	⇌	Tm(s)	-2.4	2	^[1]
La	La³⁺ + 3 e⁻	⇌	La(s)	-2.379	3	^[5]
Y	Y³⁺ + 3 e⁻	⇌	Y(s)	-2.372	3	^[5]
Mg	Mg²⁺ + 2 e⁻	⇌	Mg(s)	-2.372	2	^[5]
Sc	ScF 3(aq) + 3 H⁺ + 3 e⁻	⇌	Sc(s) + 3HF(aq)	-2.37	3	^[6]^: 792
Zr	ZrO(OH)₂(s) + H 2O + 4 e⁻	⇌	Zr(s) + 4 OH⁻	-2.36	4	^[5]
Pr	Pr³⁺ + 3 e⁻	⇌	Pr(s)	-2.353	3	^[1]
Ce	Ce³⁺ + 3 e⁻	⇌	Ce(s)	-2.336	3	^[1]
Er	Er³⁺ + 3 e⁻	⇌	Er(s)	-2.331	3	^[1]
Ho	Ho³⁺ + 3 e⁻	⇌	Ho(s)	-2.33	3	^[1]
Al	H₂AlO−3 + H 2O + 3 e⁻	⇌	Al(s) + 4 OH⁻	-2.33	3	^[1]
Nd	Nd³⁺ + 3 e⁻	⇌	Nd(s)	-2.323	3	^[1]
Tm	Tm³⁺ + 3 e⁻	⇌	Tm(s)	-2.319	3	^[1]
Al	Al(OH)₃(s) + 3 e⁻	⇌	Al(s) + 3 OH⁻	-2.31	3	^[8]
Sm	Sm³⁺ + 3 e⁻	⇌	Sm(s)	-2.304	3	^[1]
Fm	Fm Template:2+ + 2 e⁻	⇌	Fm	-2.3	2	^[1]
Am	Am³⁺ + e⁻	⇌	Am²⁺	-2.3	1	^[1]
Dy	Dy³⁺ + 3 e⁻	⇌	Dy(s)	-2.295	3	^[1]
Lu	Lu³⁺ + 3 e⁻	⇌	Lu(s)	-2.28	3	^[1]
Sc	ScF+2 + 2 H⁺ + 3 e⁻	⇌	Sc(s) + 2HF(l)	-2.28	3	^[6]^: 792
Tb	Tb³⁺ + 3 e⁻	⇌	Tb(s)	-2.28	3	^[1]
Gd	Gd³⁺ + 3 e⁻	⇌	Gd(s)	-2.279	3	^[1]
H	H₂(g) + 2 e⁻	⇌	2H⁻	-2.23	2	^[1]
Es	Es²⁺ + 2 e⁻	⇌	Es(s)	-2.23	2	^[1]
Pm	Pm²⁺ + 2 e⁻	⇌	Pm(s)	-2.2	2	^[1]
Tm	Tm³⁺ + e⁻	⇌	-2.2	1	^[1]
Dy	Dy²⁺ + 2 e⁻	⇌	Dy(s)	-2.2	2	^[1]
Ac	Ac³⁺ + 3 e⁻	⇌	Ac(s)	-2.2	3	^[1]
Yb	Yb³⁺ + 3 e⁻	⇌	Yb(s)	-2.19	3	^[1]
Cf	Cf²⁺ + 2 e⁻	⇌	Cf(s)	-2.12	2	^[1]
Nd	Nd²⁺ + 2 e⁻	⇌	Nd(s)	-2.1	2	^[1]
Ho	Ho²⁺ + 2 e⁻	⇌	Ho(s)	-2.1	2	^[1]
Sc	Sc³⁺ + 3 e⁻	⇌	Sc(s)	-2.077	3	^[9]
Al	AlF3−6 + 3 e⁻	⇌	Al(s) + 6F⁻	-2.069	3	^[1]
Cm	Cm³⁺ + 3 e⁻	⇌	Cm(s)	-2.04	3	^[1]
Pu	Pu³⁺ + 3 e⁻	⇌	Pu(s)	-2.031	3	^[1]
Pr	Pr²⁺ + 2 e⁻	⇌	Pr(s)	-2	2	^[1]
Er	Er²⁺ + 2 e⁻	⇌	Er(s)	-2	2	^[1]
Eu	Eu³⁺ + 3 e⁻	⇌	Eu(s)	-1.991	3	^[1]
Lr	Lr³⁺ + 3 e⁻	⇌	Lr	-1.96	3	^[1]
Cf	Cf³⁺ + 3 e⁻	⇌	Cf(s)	-1.94	3	^[1]
Es	Es³⁺ + 3 e⁻	⇌	Es(s)	-1.91	3	^[1]
Pa	Pa⁴⁺ + e⁻	⇌	Pa³⁺	-1.9	1	^[1]
Am	Am²⁺ + 2 e⁻	⇌	Am(s)	-1.9	2	^[1]
Th	Th⁴⁺ + 4 e⁻	⇌	Th(s)	-1.899	4	^[1]
Fm	Fm³⁺ + 3 e⁻	⇌	Fm	-1.89	3	^[1]
N	N 2(g) + 2H 2O(l) + 4 H⁺ + 2 e⁻	⇌	2NH 3OH+	-1.87	2	^[6]^: 789
Np	Np³⁺ + 3 e⁻	⇌	Np(s)	-1.856	3	^[1]
Be	Be²⁺ + 2 e⁻	⇌	Be(s)	-1.847	2	^[1]
P	H₂PO−2 + e⁻	⇌	P(s) + 2 OH⁻	-1.82	1	^[1]
U	U³⁺ + 3 e⁻	⇌	U(s)	-1.798	3	^[1]
Sr	Sr²⁺ + 2 e⁻	⇌	Sr(Hg)	-1.793	2	^[1]
B	H₂BO−3 + H 2O + 3 e⁻	⇌	B(s) + 4 OH⁻	-1.79	3	^[1]
Th	ThO₂ + 4 H⁺ + 4 e⁻	⇌	Th(s) + 2H 2O	-1.789	4	^[1]
Hf	HfO²⁺ + 2 H⁺ + 4 e⁻	⇌	Hf(s) + H 2O	-1.724	4	^[1]
P	HPO2−3 + 2H 2O + 3 e⁻	⇌	P(s) + 5 OH⁻	-1.71	3	^[1]
Si	SiO2−3 + 3H 2O + 4 e⁻	⇌	Si(s) + 6 OH⁻	-1.697	4	^[1]
Al	Al³⁺ + 3 e⁻	⇌	Al(s)	-1.662	3	^[1]
Ti	Ti²⁺ + 2 e⁻	⇌	Ti(s)	-1.63	2	^[7]
Zr	ZrO₂(s) + 4 H⁺ + 4 e⁻	⇌	Zr(s) + 2H 2O	-1.553	4	^[10]
Zr	Zr⁴⁺ + 4 e⁻	⇌	Zr(s)	-1.45	4	^[10]
Ti	Ti³⁺ + 3 e⁻	⇌	Ti(s)	-1.37	3	^[11]
Ti	TiO(s) + 2 H⁺ + 2 e⁻	⇌	Ti(s) + H 2O	-1.31	2	^[6]^: 792
B	B(OH)−4 + 4H 2O(l) + 8 e⁻	⇌	BH−4 + 8 OH⁻	-1.24	8	^[6]^: 788
Ga	GaO(OH)−2 + H 2O(l) + 3 e⁻	⇌	Ga(s) + 3 OH⁻	-1.22	3	^[6]^: 788
Ti	Ti₂O₃(s) + 2 H⁺ + 2 e⁻	⇌	2TiO(s) + H 2O	-1.23	2	^[6]^: 792
Zn	Zn(OH)2−4 + 2 e⁻	⇌	Zn(s) + 4 OH⁻	-1.199	2	^[10]
Mn	Mn²⁺ + 2 e⁻	⇌	Mn(s)	-1.185	2	^[10]
Fe	Fe(CN)4−6 + 6 H⁺ + 2 e⁻	⇌	Fe(s) + 6HCN(aq)	-1.16	2	^[12]
C	C(s) + 3H 2O(l) + 2 e⁻	⇌	CH 3OH(l) + 2 OH⁻	-1.148	2	^[6]^: 788
Cr	Cr(CN)3−6 + e⁻	⇌	Cr(CN)4−6	-1.143	1	^[6]^: 793
Te	Te(s) + 2 e⁻	⇌	Te²⁻	-1.143	2	^[13]
V	V²⁺ + 2 e⁻	⇌	V(s)	-1.13	2	^[13]
Nb	Nb³⁺ + 3 e⁻	⇌	Nb(s)	-1.099	3	^[8]
Sn	Sn(s) + 4 H⁺ + 4 e⁻	⇌	SnH₄(g)	-1.07	4
Po	Po(s) + 2 e⁻	⇌	Po²⁻	-1.021	2	^[14]
Cr	[Cr(edta)(H₂O)]⁻ + e⁻	⇌	[Cr(edta)(H₂O)]²⁻	-0.99	1	^[6]^: 793
P	2H 3PO 4(aq) + 2 H⁺ + 2 e⁻	⇌	(H 2PO 3) 2(aq) + H 2O(l)	-0.933	2	^[6]^: 789
C	CO2−3 + 3 H⁺ + 2 e⁻	⇌	HCO−2 + H 2O(l)	-0.93	2	^[6]^: 788
Ti	TiO²⁺ + 2 H⁺ + 4 e⁻	⇌	Ti(s) + H 2O	-0.93	4
Si	SiO₂(quartz) + 4 H⁺ + 4 e⁻	⇌	Si(s) + 2H 2O	-0.909	4	^[6]^: 788
Cr	Cr²⁺ + 2 e⁻	⇌	Cr(s)	-0.9	2	^[6]^: 793
B	B(OH)₃(aq) + 3 H⁺ + 3 e⁻	⇌	B(s) + 3H 2O	-0.89	3	^[6]^: 788
Fe	Fe(OH)₂(s) + 2 e⁻	⇌	Fe(s) + 2 OH⁻	-0.89	2	^[12]
Fe	Fe₂O₃(s) + 3H 2O + 2 e⁻	⇌	2Fe(OH)₂(s) + 2 OH⁻	-0.86	2	^[12]
H	2H 2O + 2 e⁻	⇌	H₂(g) + 2 OH⁻	-0.8277	2	^[10]
Bi	Bi(s) + 3 H⁺ + 3 e⁻	⇌	BiH₃	-0.8	3	^[10]
Zn	Zn²⁺ + 2 e⁻	⇌	Zn(Hg)	-0.7628	2	^[10]
Zn	Zn²⁺ + 2 e⁻	⇌	Zn(s)	-0.7618	2	^[10]
Ta	Ta₂O₅(s) + 10 H⁺ + 10 e⁻	⇌	2Ta(s) + 5H 2O	-0.75	10
Te	2Te(s) + 2 e⁻	⇌	Te2−2	-0.74	2	^[6]^: 790
Ni	Ni(OH)₂(s) + 2 e⁻	⇌	Ni(s) + 2 OH⁻	-0.72	2	^[1]
Nb	Nb 2O 5(s) + 10 H⁺ + 10 e⁻	⇌	2Nb(s) + 5H 2O(l)	-0.7	10	^[6]^: 793
Ag	Ag₂S(s) + 2 e⁻	⇌	2Ag(s) + S²⁻(aq)	-0.69	2
Te	Te2−2 + 4 H⁺ + 2 e⁻	⇌	2H 2Te(g)	-0.64	2	^[6]^: 790
Sb	Sb(OH)−4 + 3 e⁻	⇌	Sb(s) + 4 OH⁻	-0.639	3	^[6]^: 789
Au	[Au(CN)₂]⁻ + e⁻	⇌	Au(s) + 2CN⁻	-0.6	1
Ta	Ta³⁺ + 3 e⁻	⇌	Ta(s)	-0.6	3	^[8]
Pb	PbO(s) + H 2O + 2 e⁻	⇌	Pb(s) + 2 OH⁻	-0.580	2	^[8]
Ti	2TiO₂(s) + 2 H⁺ + 2 e⁻	⇌	Ti₂O₃(s) + H 2O	-0.56	2	^[6]^: 792
Ga	Ga³⁺ + 3 e⁻	⇌	Ga(s)	-0.549	3	^[8]
U	U⁴⁺ + e⁻	⇌	U³⁺	-0.52	1	^[15]
Sb	Sb + 3 e⁻	⇌	SbH₃	-0.51	3	^[6]^: 789
P	H₃PO₂(aq) + H⁺ + e⁻	⇌	P(white)^{[note 1]} + 2H 2O	-0.508	1	^[10]
P	H₃PO₃(aq) + 2 H⁺ + 2 e⁻	⇌	H₃PO₂(aq) + H 2O	-0.499	2	^[10]
Ni	NiO₂(s) + 2H 2O + 2 e⁻	⇌	Ni(OH)₂(s) + 2 OH⁻	-0.49	2	^[1]
Sb	Sb(OH)−6 + 2 e⁻	⇌	Sb(OH)−4 + 2 OH⁻	-0.465	2	^[6]^: 789
P	H₃PO₃(aq) + 3 H⁺ + 3 e⁻	⇌	P(red)^{[note 1]} + 3H 2O	-0.454	3	^[10]
Bi	Bi 2O 3(s) + 3H 2O(l) + 6 e⁻	⇌	Bi(s) + 6 OH⁻	-0.452	6	^[6]^: 789
Ta	TaF2−7 + 7 H⁺ + 5 e⁻	⇌	Ta(s) + 7HF(l)	-0.45	5	^[6]^: 793
In	In³⁺ + 2 e⁻	⇌	In+	-0.444	2	^[6]^: 788
Cu	Cu(CN)−2 + e⁻	⇌	Cu(s) + 2CN⁻	-0.44	1	^[13]
Fe	Fe²⁺ + 2 e⁻	⇌	Fe(s)	-0.44	2	^[7]
C	2CO₂(g) + 2 H⁺ + 2 e⁻	⇌	HOOCCOOH(aq)	-0.43	2
Cr	Cr³⁺ + e⁻	⇌	Cr²⁺	-0.407	1	^[8]
Cd	Cd²⁺ + 2 e⁻	⇌	Cd(s)	-0.4	2	^[7]
Ti	Ti³⁺ + e⁻	⇌	Ti²⁺	-0.37	1	^[6]^: 792
Cu	Cu₂O(s) + H 2O + 2 e⁻	⇌	2Cu(s) + 2 OH⁻	-0.36	2	^[10]
Pb	PbSO₄(s) + 2 e⁻	⇌	Pb(s) + SO2−4	-0.3588	2	^[10]
Pb	PbSO₄(s) + 2 e⁻	⇌	Pb(Hg) + SO2−4	-0.3505	2	^[10]
Eu	Eu³⁺ + e⁻	⇌	Eu²⁺	-0.35	1	^[15]
In	In³⁺ + 3 e⁻	⇌	In(s)	-0.34	3	^[13]
Tl	Tl⁺ + e⁻	⇌	Tl(s)	-0.34	1	^[13]
Ge	Ge(s) + 4 H⁺ + 4 e⁻	⇌	GeH₄(g)	-0.29	4
Co	Co²⁺ + 2 e⁻	⇌	Co(s)	-0.28	2	^[10]
P	H₃PO₄(aq) + 2 H⁺ + 2 e⁻	⇌	H₃PO₃(aq) + H 2O	-0.276	2	^[10]
N	N₂(g) + 8 H⁺ + 6 e⁻	⇌	2NH+4	-0.27	6	^[16]
V	V³⁺ + e⁻	⇌	V²⁺	-0.26	1	^[7]
Ni	Ni²⁺ + 2 e⁻	⇌	Ni(s)	-0.257	2	^[8]
S	2HSO−4 + 2 H⁺ + 2 e⁻	⇌	S₂O2−6 + 2H 2O(l)	-0.253	2	^[6]^: 790
As	As(s) + 3 H⁺ + 3 e⁻	⇌	AsH₃(g)	-0.23	3	^[13]
N	N₂(g) + 5 H⁺ + 4 e⁻	⇌	N₂H+5	-0.23	4	^[6]^: 789
Ga	Ga⁺ + e⁻	⇌	Ga(s)	-0.2	1	^[8]
Ag	AgI(s) + e⁻	⇌	Ag(s) + I⁻	-0.15224	1	^[10]
Ge	GeO₂(s) + 4 H⁺ + 4 e⁻	⇌	Ge(s) + H₂O(l)	-0.15	4	^[16]
Mo	MoO₂(s) + 4 H⁺ + 4 e⁻	⇌	Mo(s) + 2H 2O	-0.15	4
Si	Si(s) + 4 H⁺ + 4 e⁻	⇌	SiH₄(g)	-0.14	4
Sn	Sn²⁺ + 2 e⁻	⇌	Sn(s)	-0.13	2
O	O₂(g) + H⁺ + e⁻	⇌	HO•2(aq)	-0.13	1
In	In+ + e⁻	⇌	In(s)	-0.126	1	^[6]^: 788
Pb	Pb²⁺ + 2 e⁻	⇌	Pb(s)	-0.126	2	^[7]
W	WO₂(s) + 4 H⁺ + 4 e⁻	⇌	W(s) + 2H 2O	-0.12	4
Ge	GeO₂(s) + 2 H⁺ + 2 e⁻	⇌	GeO(s) + H 2O	-0.118	2	^[8]
P	P(red) + 3 H⁺ + 3 e⁻	⇌	PH₃(g)	-0.111	3	^[10]
C	CO₂(g) + 2 H⁺ + 2 e⁻	⇌	HCOOH(aq)	-0.11	2
Se	Se(s) + 2 H⁺ + 2 e⁻	⇌	H₂Se(g)	-0.11	2	^[6]^: 790
C	CO₂(g) + 2 H⁺ + 2 e⁻	⇌	CO(g) + H 2O	-0.11	2
Sn	α-SnO(s) + 2 H⁺ + 2 e⁻	⇌	Sn(s) + H 2O	-0.104	2	^[6]^: 788
Cu	Cu(NH₃)+2 + e⁻	⇌	Cu(s) + 2NH₃(aq)	-0.1	1	^[13]
Nb	Nb 2O 5(s) + 10 H⁺ + 4 e⁻	⇌	2Nb³⁺ + 5H 2O(l)	-0.1	4	^[6]^: 793
W	WO₃(aq) + 6 H⁺ + 6 e⁻	⇌	W(s) + 3H 2O	-0.09	6	^[13]
Sn	SnO₂(s) + 2 H⁺ + 2 e⁻	⇌	α-SnO(s) + H 2O	-0.088	2	^[6]^: 788
Fe	Fe₃O₄(s) + 8 H⁺ + 8 e⁻	⇌	3Fe(s) + 4H 2O	-0.085	8	^[17]
V	VOH²⁺ + H⁺ + e⁻	⇌	V²⁺ + H 2O(l)	-0.082	1	^[6]^: 793
P	P(white) + 3 H⁺ + 3 e⁻	⇌	PH₃(g)	-0.063	3	^[10]
N	N 2O(g) + H 2O(l) + 6 H⁺ + 4 e⁻	⇌	2NH 3OH+	-0.05	4	^[6]^: 789
Fe	Fe³⁺ + 3 e⁻	⇌	Fe(s)	-0.04	3	^[12]
C	HCOOH(aq) + 2 H⁺ + 2 e⁻	⇌	HCHO(aq) + H 2O	-0.034	2	^[6]^: 788
H	2 H⁺ + 2 e⁻	⇌	H₂(g)	0	2
Ag	AgBr(s) + e⁻	⇌	Ag(s) + Br⁻	0.07133	1	^[10]
S	S₄O2−6 + 2 e⁻	⇌	2S₂O2−3	0.08	2
N	N₂(g) + 2H 2O + 6 H⁺ + 6 e⁻	⇌	2NH₄OH(aq)	0.092	6
Hg	HgO(s) + H 2O + 2 e⁻	⇌	Hg(l) + 2 OH⁻	0.0977	2
Cu	Cu(NH₃)2+4 + e⁻	⇌	Cu(NH₃)+2 + 2NH₃(aq)	0.1	1	^[13]
Ru	Ru(NH₃)3+6 + e⁻	⇌	Ru(NH₃)2+6	0.1	1	^[15]
N	N₂H₄(aq) + 4H 2O + 2 e⁻	⇌	2NH+4 + 4 OH⁻	0.11	2	^[4]
Mo	H₂MoO₄(aq) + 6 H⁺ + 6 e⁻	⇌	Mo(s) + 4H 2O	0.11	6
Ge	Ge⁴⁺ + 4 e⁻	⇌	Ge(s)	0.12	4
C	C(s) + 4 H⁺ + 4 e⁻	⇌	CH₄(g)	0.13	4	^[13]
C	HCHO(aq) + 2 H⁺ + 2 e⁻	⇌	CH₃OH(aq)	0.13	2
S	S(s) + 2 H⁺ + 2 e⁻	⇌	H₂S(g)	0.144	2	^[6]^: 790
Sb	Sb₂O₃(s) + 6 H⁺ + 6 e⁻	⇌	2Sb(s) + 3H₂O	0.15	6	^[6]^: 789
Sn	Sn⁴⁺ + 2 e⁻	⇌	Sn²⁺	0.151	2	^[8]
S	HSO−4 + 3 H⁺ + 2 e⁻	⇌	SO₂(aq) + 2H 2O	0.158	2	^[6]^: 790
Cu	Cu²⁺ + e⁻	⇌	Cu⁺	0.159	1	^[13]
U	UO2+2 + e⁻	⇌	UO+2	0.163	1	^[15]
S	SO2−4 + 4 H⁺ + 2 e⁻	⇌	SO₂(aq) + 2H 2O	0.17	2
Ti	TiO²⁺ + 2 H⁺ + e⁻	⇌	Ti³⁺ + H 2O	0.19	1
Sb	SbO⁺ + 2 H⁺ + 3 e⁻	⇌	Sb(s) + H 2O	0.2	3
Fe	3Fe₂O₃(s) + 2 H⁺ + 2 e⁻	⇌	2Fe₃O₄(s) + H 2O	0.22	2	^[18]^: p.100
Ag	AgCl(s) + e⁻	⇌	Ag(s) + Cl⁻	0.22233	1	^[10]
As	H₃AsO₃(aq) + 3 H⁺ + 3 e⁻	⇌	As(s) + 3H 2O	0.24	3	^[6]^: 789
Ru	Ru³⁺(aq) + e⁻	⇌	Ru²⁺(aq)	0.249	1	^[19]
Pb	PbO 2(s) + H 2O + 2 e⁻	⇌	α-PbO(s) + 2 OH⁻	0.254	2	^[6]^: 788
Ge	GeO(s) + 2 H⁺ + 2 e⁻	⇌	Ge(s) + H 2O	0.26	2
Hg	Hg 2Cl 2(s) + 2 e⁻	⇌	2Hg(l) + 2Cl−	0.27	2	^[16]
U	UO+2 + 4 H⁺ + e⁻	⇌	U⁴⁺ + 2H 2O	0.273	1	^[15]
Re	Re³⁺ + 3 e⁻	⇌	Re(s)	0.300	3	^[8]
At	At + e⁻	⇌	At⁻	0.3	1	^[20]
Bi	Bi³⁺ + 3 e⁻	⇌	Bi(s)	0.308	3	^[10]
C	2HCNO + 2 H⁺ + 2 e⁻	⇌	(CN)₂ + 2H 2O	0.330	2	^[8]
Cu	Cu²⁺ + 2 e⁻	⇌	Cu(s)	0.337	2	^[13]
V	VO²⁺ + 2 H⁺ + e⁻	⇌	V³⁺ + H 2O	0.337	1	^[6]^: 793
Sb	Sb 2O 4(s) + 2 H⁺ + 2 e⁻	⇌	Sb 2O 3(s) + H 2O(l)	0.342	2	^[6]^: 789
At	At⁺ + 2 e⁻	⇌	At^-	0.36	2	^[21]
Fe	[Fe(CN)₆]³⁻ + e⁻	⇌	[Fe(CN)₆]⁴⁻	0.3704	1	^[22]
C	(CN)₂ + 2 H⁺ + 2 e⁻	⇌	2HCN	0.373	2	^[8]
P	(H 2PO 3) 2(aq) + 2 H⁺ + 2 e⁻	⇌	2H 3PO 3	0.38	2	^[6]^: 789
S	2SO₂(aq) + 2 H⁺ + 2 e⁻	⇌	S₂O2−3 + H₂O(l)	0.4	2	^[6]^: 790
O	O₂(g) + 2H 2O + 4 e⁻	⇌	4 OH⁻(aq)	0.401	4	^[7]
Mo	H₂MoO₄ + 6 H⁺ + 3 e⁻	⇌	Mo³⁺ + 4H 2O	0.43	3
Ru	Ru²⁺(aq) + 2 e⁻	⇌	Ru	0.455	2	^[19]
V	VO(OH)+ + 2 H⁺ + e⁻	⇌	VOH²⁺ + H 2O(l)	0.481	1	^[6]^: 793
C	CH₃OH(aq) + 2 H⁺ + 2 e⁻	⇌	CH₄(g) + H 2O	0.5	2
S	SO₂(aq) + 4 H⁺ + 4 e⁻	⇌	S(s) + 2H 2O	0.5	4	^[6]^: 790
S	4SO₂(aq) + 4 H⁺ + 8 e⁻	⇌	S₄O4−6 + 2H 2O(l)	0.51	8	^[16]
Cu	Cu⁺ + e⁻	⇌	Cu(s)	0.52	1	^[13]
C	CO(g) + 2 H⁺ + 2 e⁻	⇌	C(s) + H 2O	0.52	2	^[6]^: 788
I	I−3 + 2 e⁻	⇌	3I⁻	0.53	2	^[7]
Te	TeO 2(s) + 4 H⁺ + 4 e⁻	⇌	Te(s) + 2H 2O(l)	0.53	4	^[6]^: 790
Cu	Cu²⁺ + Cl− + e⁻	⇌	CuCl(s)	0.54	1	^[16]
I	I₂(s) + 2 e⁻	⇌	2I⁻	0.54	2	^[7]
Au	[AuI₄]⁻ + 3 e⁻	⇌	Au(s) + 4I⁻	0.56	3
As	H₃AsO₄(aq) + 2 H⁺ + 2 e⁻	⇌	H₃AsO₃(aq) + H 2O	0.56	2	^[6]^: 789
S	S₂O2−6 + 4 H⁺ + 2 e⁻	⇌	2H 2SO 3	0.569	2	^[6]^: 790
Au	[AuI₂]⁻ + e⁻	⇌	Au(s) + 2I⁻	0.58	1
Mn	MnO−4 + 2H 2O + 3 e⁻	⇌	MnO₂(s) + 4 OH⁻	0.595	3	^[1]
S	S₂O2−3 + 6 H⁺ + 4 e⁻	⇌	2S(s) + 3H 2O	0.6	4	^[6]^: 790
Fe	Fc⁺ + e⁻	⇌	Fc(s)	0.63	1	Substantial literature variation^[23]
Mo	H₂MoO₄(aq) + 2 H⁺ + 2 e⁻	⇌	MoO₂(s) + 2H 2O	0.65	2
N	HN₃(aq) + 11 H⁺ + 8 e⁻	⇌	3NH+4	0.69	8	^[16]
O	O₂(g) + 2 H⁺ + 2 e⁻	⇌	H₂O₂(aq)	0.695	2	^[8]
Sb	Sb 2O 5(s) + 4 H⁺ + 4 e⁻	⇌	Sb 2O 3(s) + 2H 2O	0.699	4	^[6]^: 789
C	+ 2 H⁺ + 2 e⁻	⇌		0.6992	2	^[10]
V	H₂V₁₀O4−28 + 24 H⁺ + 10 e⁻	⇌	10VO(OH)+ + 8H 2O(l)	0.723	10	^[6]^: 793
Pt	PtCl2−6 + 2 e⁻	⇌	PtCl2−4 + 2Cl⁻	0.726	2	^[15]
Fe	Fe₂O₃(s) + 6 H⁺ + 2 e⁻	⇌	2Fe²⁺ + 3H 2O	0.728	2	^[18]^: p.100
Se	H₂SeO₃(aq) + 4 H⁺ + 4 e⁻	⇌	Se(s) + 3H 2O	0.74	4	^[8]
At	AtO⁺ + 2 H⁺ + 2 e⁻	⇌	At⁺ + H 2O	0.74	2	^[21]
Tl	Tl³⁺ + 3 e⁻	⇌	Tl(s)	0.741	3	^[8]
No	No³⁺ + e⁻	⇌	No²⁺	0.75	1	^[24]
Pt	PtCl2−4 + 2 e⁻	⇌	Pt(s) + 4Cl⁻	0.758	2	^[15]
Br	BrO− + H 2O(l) + 2 e⁻	⇌	Br− + 2 OH⁻	0.76	2	^[6]^: 791
Po	Po⁴⁺ + 4 e⁻	⇌	Po	0.76	4	^[8]
S	(SCN)₂ + 2 e⁻	⇌	2SCN^-	0.77	2	^[8]
Fe	Fe³⁺ + e⁻	⇌	Fe²⁺	0.771	1	^[8]
Hg	Hg2+2 + 2 e⁻	⇌	2Hg(l)	0.7973	2	^[8]
Ag	Ag⁺ + e⁻	⇌	Ag(s)	0.7996	1	^[10]
N	2NO−3(aq) + 4 H⁺ + 2 e⁻	⇌	N₂O₄(g) + 2H 2O	0.803	2	^[6]^: 789
Fe	2FeO2−4 + 5H 2O + 6 e⁻	⇌	Fe₂O₃(s) + 10 OH⁻	0.81	6	^[12]
Au	[AuBr₄]⁻ + 3 e⁻	⇌	Au(s) + 4Br⁻	0.85	3
Hg	Hg²⁺ + 2 e⁻	⇌	Hg(l)	0.85	2
Ir	[IrCl₆]²⁻ + e⁻	⇌	[IrCl₆]³⁻	0.87	1	^[6]^: 153
Mn	MnO−4 + H⁺ + e⁻	⇌	HMnO−4	0.9	1
Po	Po⁴⁺ + 2 e⁻	⇌	Po²⁺	0.9	2	^[8]
Hg	2Hg²⁺ + 2 e⁻	⇌	Hg2+2	0.91	2	^[13]
Pd	Pd²⁺ + 2 e⁻	⇌	Pd(s)	0.915	2	^[15]
Au	[AuCl₄]⁻ + 3 e⁻	⇌	Au(s) + 4Cl⁻	0.93	3
N	NO−3 + 3 H⁺ + 2 e⁻	⇌	HNO 2(aq)	0.94	2	^[6]^: 789
Mn	MnO₂(s) + 4 H⁺ + e⁻	⇌	Mn³⁺ + 2H 2O	0.95	1
N	NO−3(aq) + 4 H⁺ + 3 e⁻	⇌	NO(g) + 2H 2O(l)	0.958	3	^[7]
Au	[AuBr₂]⁻ + e⁻	⇌	Au(s) + 2Br⁻	0.96	1
Fe	Fe₃O₄(s) + 8 H⁺ + 2 e⁻	⇌	3Fe²⁺ + 4H 2O	0.98	2	^[18]^: p.100
Xe	[HXeO₆]³⁻ + 2H 2O + 2 e⁻	⇌	[HXeO₄]⁻ + 4 OH⁻	0.99	2	^[6]^: 792^[25]
N	HNO 2(aq) + H⁺ + e⁻	⇌	NO(g) + H 2O(l)	0.996	1	^[6]^: 789
At	HAtO + H⁺ + e⁻	⇌	At + H 2O	1.0	1	^[20]
V	[VO₂]⁺(aq) + 2 H⁺ + e⁻	⇌	[VO]²⁺(aq) + H 2O	1	1	^[26]
Te	H₆TeO₆(aq) + 2 H⁺ + 2 e⁻	⇌	TeO₂(s) + 4H 2O	1.02	2	^[26]
N	NO₂(g) + 2 H⁺ + 2 e⁻	⇌	NO(g) + H₂O(l)	1.03	2	^[16]
Br	Br−3 + 2 e⁻	⇌	3Br⁻	1.05	2	^[16]
Sb	Sb 2O 5(s) + 2 H⁺ + 2 e⁻	⇌	Sb 2O 4(s) + H 2O(l)	1.055	2	^[6]^: 789
I	ICl−2 + e⁻	⇌	2Cl⁻ + I(s)	1.06	1	^[16]
Br	Br₂(l) + 2 e⁻	⇌	2Br⁻	1.066	2	^[10]
N	N 2O 4(g) + 2 H⁺ + 2 e⁻	⇌	2HNO 2	1.07	2	^[6]^: 789
Br	Br₂(aq) + 2 e⁻	⇌	2Br⁻	1.0873	2	^[10]
Ru	RuO₂ + 4 H⁺ + 2 e⁻	⇌	Ru²⁺(aq) + 2H 2O	1.120	2	^[19]
Cu	Cu²⁺ + 2CN⁻ + e⁻	⇌	Cu(CN)−2	1.12	1	^[13]
I	IO−3 + 5 H⁺ + 4 e⁻	⇌	HIO(aq) + 2H 2O	1.13	4	^[6]^: 791
O	H 2O 2(aq) + H⁺ + e⁻	⇌	H 2O(l) + HO•	1.14	1	^[6]^: 790
Au	[AuCl₂]⁻ + e⁻	⇌	Au(s) + 2Cl⁻	1.15	1
Se	HSeO−4 + 3 H⁺ + 2 e⁻	⇌	H₂SeO₃(aq) + H 2O	1.15	2	^[6]^: 790
Ag	Ag₂O(s) + 2 H⁺ + 2 e⁻	⇌	2Ag(s) + H 2O	1.17	2
Cl	ClO−3 + 2 H⁺ + e⁻	⇌	ClO₂(g) + H 2O	1.175	1	^[6]^: 791
Xe	[HXeO₆]³⁻ + 5H 2O + 8 e⁻	⇌	Xe(g) + 11 OH⁻	1.18	8	^[25]
Pt	Pt²⁺ + 2 e⁻	⇌	Pt(s)	1.188	2	^[15]
Cl	ClO₂(g) + H⁺ + e⁻	⇌	HClO₂(aq)	1.19	1	^[27]
I	2IO−3 + 12 H⁺ + 10 e⁻	⇌	I₂(s) + 6H 2O	1.2	10	^[16]
Mn	MnO₂(s) + 4 H⁺ + 2 e⁻	⇌	Mn²⁺ + 2H 2O	1.224	2	^[10]
O	O₂(g) + 4 H⁺ + 4 e⁻	⇌	2H 2O	1.229	4	^[7]
N	N₂H+5 + 3 H⁺ + 2 e⁻	⇌	2NH+4	1.28	2	^[6]^: 789
Cl	ClO−4 + 2 H⁺ + 2 e⁻	⇌	ClO−3 + H 2O	1.23	2	^[28]
Ru	[Ru(bipy)₃]³⁺ + e⁻	⇌	[Ru(bipy)₃]²⁺	1.24	1	^[1]
Xe	[HXeO₄]⁻ + 3H 2O + 6 e⁻	⇌	Xe(g) + 7 OH⁻	1.24	6	^[6]^: 792^[25]
N	2NO−3 + 12 H⁺ + 10 e⁻	⇌	N 2(g) + 6H 2O(l)	1.25	10	^[6]^: 789
Tl	Tl³⁺ + 2 e⁻	⇌	Tl⁺	1.25	2	^[6]^: 788
N	2HNO 2(aq) + 4 H⁺ + 4 e⁻	⇌	N 2O(g) + 3H 2O(l)	1.297	4	^[6]^: 789
Cr	Cr₂O2−7 + 14 H⁺ + 6 e⁻	⇌	2Cr³⁺ + 7H 2O	1.38	6	^[6]^: 793
N	NH 3OH+ + 2 H⁺ + 2 e⁻	⇌	NH+4 + H 2O(l)	1.35	2	^[6]^: 789
Cl	Cl₂(g) + 2 e⁻	⇌	2Cl⁻	1.36	2	^[7]
Ru	RuO−4(aq) + 8 H⁺ + 5 e⁻	⇌	Ru²⁺(aq) + 4H 2O	1.368	5	^[19]
Ru	RuO₄ + 4 H⁺ + 4 e⁻	⇌	RuO₂ + 2H 2O	1.387	4	^[19]
Co	CoO₂(s) + 4 H⁺ + e⁻	⇌	Co³⁺ + 2H 2O	1.42	1
N	2NH₃OH⁺ + H⁺ + 2 e⁻	⇌	N₂H+5 + 2H 2O	1.42	2	^[4]
I	2HIO(aq) + 2 H⁺ + 2 e⁻	⇌	I₂(s) + 2H 2O	1.44	2	^[6]^: 791
Br	BrO−3 + 5 H⁺ + 4 e⁻	⇌	HBrO(aq) + 2H 2O	1.447	4	^[6]^: 791
Pb	β-PbO₂(s) + 4 H⁺ + 2 e⁻	⇌	Pb²⁺ + 2H 2O	1.46	2	^[13]
Pb	α-PbO₂(s) + 4 H⁺ + 2 e⁻	⇌	Pb²⁺ + 2H 2O	1.468	2	^[13]
Br	2BrO−3 + 12 H⁺ + 10 e⁻	⇌	Br₂(l) + 6H 2O	1.48	10
At	HAtO₃ + 4 H⁺ + 4 e⁻	⇌	HAtO + 2H 2O	1.5	4	^[20]
Mn	MnO−4 + 8 H⁺ + 5 e⁻	⇌	Mn²⁺ + 4H 2O	1.51	5	^[16]
O	HO•2 + H⁺ + e⁻	⇌	H₂O₂(aq)	1.51	1
Au	Au³⁺ + 3 e⁻	⇌	Au(s)	1.52	3
Ru	RuO2−4(aq) + 8 H⁺ + 4 e⁻	⇌	Ru²⁺(aq) + 4H 2O	1.563	4	^[19]
N	2NO(g) + 2 H⁺ + 2 e⁻	⇌	N 2O(g) + H 2O(l)	1.59	2	^[6]^: 789
Ni	NiO₂(s) + 2 H⁺ + 2 e⁻	⇌	Ni²⁺ + 2 OH⁻	1.59	2
Ce	Ce⁴⁺ + e⁻	⇌	Ce³⁺	1.61	1
Cl	2HClO(aq) + 2 H⁺ + 2 e⁻	⇌	Cl₂(g) + 2H 2O	1.63	2	^[27]
I	IO−4 + 2 H⁺ + 2 e⁻	⇌	IO−3 + H 2O	1.64	2	^[28]
Ag	Ag₂O₃(s) + 6 H⁺ + 4 e⁻	⇌	2Ag⁺ + 3H 2O	1.67	4
Cl	HClO₂(aq) + 2 H⁺ + 2 e⁻	⇌	HClO(aq) + H 2O	1.67	2	^[27]
Pb	Pb⁴⁺ + 2 e⁻	⇌	Pb²⁺	1.69	2	^[13]
Mn	MnO−4 + 4 H⁺ + 3 e⁻	⇌	MnO₂(s) + 2H 2O	1.7	3	^[16]
Br	BrO−4 + 2 H⁺ + 2 e⁻	⇌	BrO−3 + H 2O	1.74	2	^[28]
Ag	AgO(s) + 2 H⁺ + e⁻	⇌	Ag⁺ + H 2O	1.77	1
N	N 2O(g) + 2 H⁺ + 2 e⁻	⇌	N 2(g) + H 2O(l)	1.77	2	^[6]^: 789
O	H₂O₂(aq) + 2 H⁺ + 2 e⁻	⇌	2H 2O	1.78	2	^[27]
Au	Au⁺ + e⁻	⇌	Au(s)	1.83	1	^[13]
Co	Co³⁺ + e⁻	⇌	Co²⁺	1.92	1	^[8]
Ag	Ag²⁺ + e⁻	⇌	Ag⁺	1.98	1	^[13]
O	S₂O2−8 + 2 e⁻	⇌	2SO2−4	2.01	2	^[10]
O	O₃(g) + 2 H⁺ + 2 e⁻	⇌	O₂(g) + H 2O	2.075	2	^[15]
Mn	HMnO−4 + 3 H⁺ + 2 e⁻	⇌	MnO₂(s) + 2H 2O	2.09	2
Xe	XeO₃(aq) + 6 H⁺ + 6 e⁻	⇌	Xe(g) + 3H 2O	2.12	6	^[6]^: 792^[25]
Xe	H₄XeO₆(aq) + 8 H⁺ + 8 e⁻	⇌	Xe(g) + 6H 2O	2.18	8	^[6]^: 792^[25]
Fe	FeO2−4 + 8 H⁺ + 3 e⁻	⇌	Fe³⁺ + 4H 2O	2.2	3	^[29]
Xe	XeF₂(aq) + 2 H⁺ + 2 e⁻	⇌	Xe(g) + 2HF(aq)	2.32	2	^[25]^[27]
O	HO• + H⁺ + e⁻	⇌	H 2O(l)	2.38	1	^[6]^: 790
Xe	H₄XeO₆(aq) + 2 H⁺ + 2 e⁻	⇌	XeO₃(aq) + 3H 2O	2.42	2	^[25]^[6]^: 792
F	F₂(g) + 2 e⁻	⇌	2F⁻	2.87	2	^[6]^: 153^[7]^[13]
Cm	Cm⁴⁺ + e^–	⇌	Cm³⁺	3.0	1	Estimated^[3]
F	F₂(g) + 2 H⁺ + 2 e⁻	⇌	2HF(aq)	3.077	2	^[3]
Tb	Tb⁴⁺ + e^–	⇌	Tb³⁺	3.1	1	Estimated^[3]
Pr	Pr⁴⁺ + e^–	⇌	Pr³⁺	3.2	1	Estimated^[3]
Kr	KrF₂(aq) + 2 e⁻	⇌	Kr(g) + 2F⁻(aq)	3.27	2	Estimated^[30]

Notes

↑ ^1.0 ^1.1 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

↑ ^1.00 ^1.01 ^1.02 ^1.03 ^1.04 ^1.05 ^1.06 ^1.07 ^1.08 ^1.09 ^1.10 ^1.11 ^1.12 ^1.13 ^1.14 ^1.15 ^1.16 ^1.17 ^1.18 ^1.19 ^1.20 ^1.21 ^1.22 ^1.23 ^1.24 ^1.25 ^1.26 ^1.27 ^1.28 ^1.29 ^1.30 ^1.31 ^1.32 ^1.33 ^1.34 ^1.35 ^1.36 ^1.37 ^1.38 ^1.39 ^1.40 ^1.41 ^1.42 ^1.43 ^1.44 ^1.45 ^1.46 ^1.47 ^1.48 ^1.49 ^1.50 ^1.51 ^1.52 ^1.53 ^1.54 ^1.55 ^1.56 ^1.57 ^1.58 ^1.59 ^1.60 ^1.61 ^1.62 ^1.63 ^1.64 ^1.65 ^1.66 ^1.67 ^1.68 ^1.69 ^1.70 ^1.71 ^1.72 ^1.73 Lide, David R., ed (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
↑ Greenwood and Earnshaw, p. 1263
↑ ^3.0 ^3.1 ^3.2 ^3.3 ^3.4 Bratsch, Stephen G. (July 29, 1988). "Standard electrode potentials and temperature coefficients in water at 298.15 K". Journal of Physical and Chemical Reference Data (American Institute of Physics) 18 (1): 1-21. 1989. doi:10.1063/1.555839. https://srd.nist.gov/jpcrdreprint/1.555839.pdf.
↑ ^4.0 ^4.1 ^4.2 ^4.3 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
↑ ^5.00 ^5.01 ^5.02 ^5.03 ^5.04 ^5.05 ^5.06 ^5.07 ^5.08 ^5.09 ^5.10 ^5.11 ^5.12 ^5.13 ^5.14 ^5.15 ^5.16 Vanýsek, Petr (2011). "Electrochemical Series". in Haynes, William M.. CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. pp. 5–80–9. ISBN 978-1-4398-5512-6. https://books.google.com/books?id=pYPRBQAAQBAJ&pg=SA5-PA80.
↑ ^6.00 ^6.01 ^6.02 ^6.03 ^6.04 ^6.05 ^6.06 ^6.07 ^6.08 ^6.09 ^6.10 ^6.11 ^6.12 ^6.13 ^6.14 ^6.15 ^6.16 ^6.17 ^6.18 ^6.19 ^6.20 ^6.21 ^6.22 ^6.23 ^6.24 ^6.25 ^6.26 ^6.27 ^6.28 ^6.29 ^6.30 ^6.31 ^6.32 ^6.33 ^6.34 ^6.35 ^6.36 ^6.37 ^6.38 ^6.39 ^6.40 ^6.41 ^6.42 ^6.43 ^6.44 ^6.45 ^6.46 ^6.47 ^6.48 ^6.49 ^6.50 ^6.51 ^6.52 ^6.53 ^6.54 ^6.55 ^6.56 ^6.57 ^6.58 ^6.59 ^6.60 ^6.61 ^6.62 ^6.63 ^6.64 ^6.65 ^6.66 ^6.67 ^6.68 ^6.69 ^6.70 ^6.71 ^6.72 ^6.73 ^6.74 ^6.75 ^6.76 ^6.77 ^6.78 ^6.79 ^6.80 ^6.81 ^6.82 ^6.83 Atkins, Peter; Overton, Tina; Rourke, Jonathan; Weller, Mark; Armstrong, Fraser; Hagerman, Michael (2010). Inorganic Chemistry (5th ed.). New York: W. H. Freeman. ISBN 978-1-42-921820-7.
↑ ^7.00 ^7.01 ^7.02 ^7.03 ^7.04 ^7.05 ^7.06 ^7.07 ^7.08 ^7.09 ^7.10 ^7.11 ^7.12 Atkins, Peter W. (1997). Physical Chemistry (6th ed.). W.H. Freeman. ISBN 9780716734659.
↑ ^8.00 ^8.01 ^8.02 ^8.03 ^8.04 ^8.05 ^8.06 ^8.07 ^8.08 ^8.09 ^8.10 ^8.11 ^8.12 ^8.13 ^8.14 ^8.15 ^8.16 ^8.17 ^8.18 ^8.19 ^8.20 ^8.21 Petr Vanysek. "Electrochemical series". http://depa.fquim.unam.mx/amyd/archivero/TablasdepotencialesREDOX_26700.pdf.
↑ David R. Lide, ed., CRC Handbook of Chemistry and Physics, Internet Version 2005, http://www.hbcpnetbase.com , CRC Press, Boca Raton, FL, 2005.
↑ ^10.00 ^10.01 ^10.02 ^10.03 ^10.04 ^10.05 ^10.06 ^10.07 ^10.08 ^10.09 ^10.10 ^10.11 ^10.12 ^10.13 ^10.14 ^10.15 ^10.16 ^10.17 ^10.18 ^10.19 ^10.20 ^10.21 ^10.22 ^10.23 ^10.24 ^10.25 ^10.26 ^10.27 Vanýsek, Petr (2012). "Electrochemical Series". in Haynes, William M.. Handbook of Chemistry and Physics (93rd ed.). CRC Press. pp. 5–80. ISBN 9781439880494. https://books.google.com/books?id=-BzP7Rkl7WkC&pg=SA5-PA80.
↑ Aylward, Gordon; Findlay, Tristan (2008). SI Chemical Data (6th ed.). Wiley. ISBN 978-0-470-81638-7.
↑ ^12.0 ^12.1 ^12.2 ^12.3 ^12.4 "compounds information". Iron. WebElements Periodic Table of the Elements. http://www.webelements.com/iron/compounds.html.
↑ ^13.00 ^13.01 ^13.02 ^13.03 ^13.04 ^13.05 ^13.06 ^13.07 ^13.08 ^13.09 ^13.10 ^13.11 ^13.12 ^13.13 ^13.14 ^13.15 ^13.16 ^13.17 ^13.18 ^13.19 ^13.20 Bard, Allen J.; Parsons, Roger; Jordan, Joseph (1985). Standard Potentials in Aqueous Solution. CRC Press. ISBN 978-0-8247-7291-8. https://books.google.com/books?id=fuJV1H18KtEC.
↑ Brown, Susan A.; Brown, Paul L. (2020). "The pH-potential diagram for polonium". The Aqueous Chemistry of Polonium and the Practical Application of its Thermochemistry. Elsevier. doi:10.1016/b978-0-12-819308-2.00004-8. ISBN 978-0-12-819308-2.
↑ ^15.00 ^15.01 ^15.02 ^15.03 ^15.04 ^15.05 ^15.06 ^15.07 ^15.08 ^15.09 Bard, A.J.; Faulkner, L.R. (2001). Electrochemical Methods. Fundamentals and Applications (2nd ed.). Wiley. ISBN 9781118312803.
↑ ^16.00 ^16.01 ^16.02 ^16.03 ^16.04 ^16.05 ^16.06 ^16.07 ^16.08 ^16.09 ^16.10 ^16.11 Lee, J. L. (1983). A New Concise Inorganic Chemistry (3rd ed.). London / Wokingham, Berkshire: English Language Book Society & Van Nostrand Reinhold (UK). ISBN 0-442-30179-0.
↑ Pourbaix, Marcel (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions. Houston, Texas; Cebelcor, Brussels: NACE International. OCLC 475102548.
↑ ^18.0 ^18.1 ^18.2 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. doi:10.1016/j.jcis.2007.02.058. PMID 17395194. Bibcode: 2007JCIS..311...94P. https://www.academia.edu/9254087. Retrieved 2017-03-26.
↑ ^19.0 ^19.1 ^19.2 ^19.3 ^19.4 ^19.5 Greenwood and Earnshaw, p. 1077
↑ ^20.0 ^20.1 ^20.2 Lavrukhina, Avgusta Konstantinovna; Pozdni︠a︡kov, Aleksandr Aleksandrovich (1970). Analytical chemistry of technetium, promethium, astatine and francium. Ann Arbor: Ann Arbor-Humphrey Science Publishers. p. 237. ISBN 0-250-39923-7. OCLC 186926.
↑ ^21.0 ^21.1 Champion, J.; Alliot, C.; Renault, E.; Mokili, B. M.; Chérel, M.; Galland, N.; Montavon, G. (2009-12-16). "Astatine Standard Redox Potentials and Speciation in Acidic Medium". The Journal of Physical Chemistry A (American Chemical Society (ACS)) 114 (1): 576–582. doi:10.1021/jp9077008. ISSN 1089-5639. PMID 20014840. http://hal.in2p3.fr/in2p3-00450771/file/JPCA_2010.pdf.
↑ 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.
↑ Pavlishchuk, Vitaly V.; Addison, Anthony W. (January 2000). "Conversion constants for redox potentials measured versus different reference electrodes in acetonitrile solutions at 25°C". Inorganica Chimica Acta 298 (1). doi:10.1016/S0020-1693(99)00407-7.
↑ Toyoshima, A.; Kasamatsu, Y.; Tsukada, K.; Asai, M.; Kitatsuji, Y.; Ishii, Y.; Toume, H.; Nishinaka, I. et al. (8 July 2009). "Oxidation of element 102, nobelium, with flow electrolytic column chromatography on an atom-at-a-time scale". Journal of the American Chemical Society 131 (26): 9180–1. doi:10.1021/ja9030038. PMID 19514720. https://figshare.com/articles/Oxidation_of_Element_102_Nobelium_with_Flow_Electrolytic_Column_Chromatography_on_an_Atom_at_a_Time_Scale/2844817.
↑ ^25.0 ^25.1 ^25.2 ^25.3 ^25.4 ^25.5 ^25.6 "compounds information". Xenon. WebElements Periodic Table of the Elements. http://www.webelements.com/xenon/compounds.html.
↑ ^26.0 ^26.1 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 .
↑ ^27.0 ^27.1 ^27.2 ^27.3 ^27.4 Ghosh, Abhik; Berg, Steffen (2014). Arrow Pushing in Inorganic Chemistry: A logical approach to the chemistry of the main-group elements. Hoboken: Wiley. ISBN 978-1-118-17398-5.
↑ ^28.0 ^28.1 ^28.2 Appelman, Evan H. (1973-04-01). "Nonexistent compounds. Two case histories". Accounts of Chemical Research (American Chemical Society (ACS)) 6 (4): 113–117. doi:10.1021/ar50064a001. ISSN 0001-4842.
↑ Courtney, Arlene. "Oxidation Reduction Chemistry of the Elements". Ch 412 Advanced Inorganic Chemistry: Reading Materials. Western Oregon University. https://people.wou.edu/~courtna/ch412/redox.htm.
↑ Leszczyński, P.J.; Grochala, W. (2013). "Strong Cationic Oxidizers: Thermal Decomposition, Electronic Structure and Magnetism of Their Compounds". Acta Chim. Slov. 60 (3): 455–470. PMID 24169699. http://acta-arhiv.chem-soc.si/60/60-3-455.pdf.

External links

Chemistry LibreTexts (2021-04-26). "P1: Standard Reduction Potentials by Element". Chemistry LibreTexts. https://chem.libretexts.org/Ancillary_Materials/Reference/Reference_Tables/Electrochemistry_Tables/P1%3A_Standard_Reduction_Potentials_by_Element.
California State University, Northridge (CSUN). "Standard Reduction Potentials" (in English). csun.edu. https://www.csun.edu/~hcchm003/321/Ered.pdf.
Wardman, Peter (1989). "Reduction potentials of one-electron couples involving free radicals in aqueous solution" (in English). srd.nist.gov. https://srd.nist.gov/JPCRD/jpcrd372.pdf.
http://www.jesuitnola.org/upload/clark/Refs/red_pot.htm
https://web.archive.org/web/20150924015049/http://www.fptl.ru/biblioteka/spravo4niki/handbook-of-Chemistry-and-Physics.pdf
http://hyperphysics.phy-astr.gsu.edu/Hbase/tables/electpot.html#c1

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Original source: https://en.wikipedia.org/wiki/Standard electrode potential (data page). Read more

[rwP-16] 1.0 ^1.1 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] 1.00 ^1.01 ^1.02 ^1.03 ^1.04 ^1.05 ^1.06 ^1.07 ^1.08 ^1.09 ^1.10 ^1.11 ^1.12 ^1.13 ^1.14 ^1.15 ^1.16 ^1.17 ^1.18 ^1.19 ^1.20 ^1.21 ^1.22 ^1.23 ^1.24 ^1.25 ^1.26 ^1.27 ^1.28 ^1.29 ^1.30 ^1.31 ^1.32 ^1.33 ^1.34 ^1.35 ^1.36 ^1.37 ^1.38 ^1.39 ^1.40 ^1.41 ^1.42 ^1.43 ^1.44 ^1.45 ^1.46 ^1.47 ^1.48 ^1.49 ^1.50 ^1.51 ^1.52 ^1.53 ^1.54 ^1.55 ^1.56 ^1.57 ^1.58 ^1.59 ^1.60 ^1.61 ^1.62 ^1.63 ^1.64 ^1.65 ^1.66 ^1.67 ^1.68 ^1.69 ^1.70 ^1.71 ^1.72 ^1.73 Lide, David R., ed (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.

[Greenwood1263-2] Greenwood and Earnshaw, p. 1263

[VanSrc-3] 3.0 ^3.1 ^3.2 ^3.3 ^3.4 Bratsch, Stephen G. (July 29, 1988). "Standard electrode potentials and temperature coefficients in water at 298.15 K". Journal of Physical and Chemical Reference Data (American Institute of Physics) 18 (1): 1-21. 1989. doi:10.1063/1.555839. https://srd.nist.gov/jpcrdreprint/1.555839.pdf.

[Gre-4] 4.0 ^4.1 ^4.2 ^4.3 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.

[van92-5] 5.00 ^5.01 ^5.02 ^5.03 ^5.04 ^5.05 ^5.06 ^5.07 ^5.08 ^5.09 ^5.10 ^5.11 ^5.12 ^5.13 ^5.14 ^5.15 ^5.16 Vanýsek, Petr (2011). "Electrochemical Series". in Haynes, William M.. CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. pp. 5–80–9. ISBN 978-1-4398-5512-6. https://books.google.com/books?id=pYPRBQAAQBAJ&pg=SA5-PA80.

[AS5-6] 6.00 ^6.01 ^6.02 ^6.03 ^6.04 ^6.05 ^6.06 ^6.07 ^6.08 ^6.09 ^6.10 ^6.11 ^6.12 ^6.13 ^6.14 ^6.15 ^6.16 ^6.17 ^6.18 ^6.19 ^6.20 ^6.21 ^6.22 ^6.23 ^6.24 ^6.25 ^6.26 ^6.27 ^6.28 ^6.29 ^6.30 ^6.31 ^6.32 ^6.33 ^6.34 ^6.35 ^6.36 ^6.37 ^6.38 ^6.39 ^6.40 ^6.41 ^6.42 ^6.43 ^6.44 ^6.45 ^6.46 ^6.47 ^6.48 ^6.49 ^6.50 ^6.51 ^6.52 ^6.53 ^6.54 ^6.55 ^6.56 ^6.57 ^6.58 ^6.59 ^6.60 ^6.61 ^6.62 ^6.63 ^6.64 ^6.65 ^6.66 ^6.67 ^6.68 ^6.69 ^6.70 ^6.71 ^6.72 ^6.73 ^6.74 ^6.75 ^6.76 ^6.77 ^6.78 ^6.79 ^6.80 ^6.81 ^6.82 ^6.83 Atkins, Peter; Overton, Tina; Rourke, Jonathan; Weller, Mark; Armstrong, Fraser; Hagerman, Michael (2010). Inorganic Chemistry (5th ed.). New York: W. H. Freeman. ISBN 978-1-42-921820-7.

[Atk-7] 7.00 ^7.01 ^7.02 ^7.03 ^7.04 ^7.05 ^7.06 ^7.07 ^7.08 ^7.09 ^7.10 ^7.11 ^7.12 Atkins, Peter W. (1997). Physical Chemistry (6th ed.). W.H. Freeman. ISBN 9780716734659.

[van??-8] 8.00 ^8.01 ^8.02 ^8.03 ^8.04 ^8.05 ^8.06 ^8.07 ^8.08 ^8.09 ^8.10 ^8.11 ^8.12 ^8.13 ^8.14 ^8.15 ^8.16 ^8.17 ^8.18 ^8.19 ^8.20 ^8.21 Petr Vanysek. "Electrochemical series". http://depa.fquim.unam.mx/amyd/archivero/TablasdepotencialesREDOX_26700.pdf.

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

[van-10] 10.00 ^10.01 ^10.02 ^10.03 ^10.04 ^10.05 ^10.06 ^10.07 ^10.08 ^10.09 ^10.10 ^10.11 ^10.12 ^10.13 ^10.14 ^10.15 ^10.16 ^10.17 ^10.18 ^10.19 ^10.20 ^10.21 ^10.22 ^10.23 ^10.24 ^10.25 ^10.26 ^10.27 Vanýsek, Petr (2012). "Electrochemical Series". in Haynes, William M.. Handbook of Chemistry and Physics (93rd ed.). CRC Press. pp. 5–80. ISBN 9781439880494. https://books.google.com/books?id=-BzP7Rkl7WkC&pg=SA5-PA80.

[si-11] Aylward, Gordon; Findlay, Tristan (2008). SI Chemical Data (6th ed.). Wiley. ISBN 978-0-470-81638-7.

[webelements_fe-12] 12.0 ^12.1 ^12.2 ^12.3 ^12.4 "compounds information". Iron. WebElements Periodic Table of the Elements. http://www.webelements.com/iron/compounds.html.

[Bar-13] 13.00 ^13.01 ^13.02 ^13.03 ^13.04 ^13.05 ^13.06 ^13.07 ^13.08 ^13.09 ^13.10 ^13.11 ^13.12 ^13.13 ^13.14 ^13.15 ^13.16 ^13.17 ^13.18 ^13.19 ^13.20 Bard, Allen J.; Parsons, Roger; Jordan, Joseph (1985). Standard Potentials in Aqueous Solution. CRC Press. ISBN 978-0-8247-7291-8. https://books.google.com/books?id=fuJV1H18KtEC.

[14] Brown, Susan A.; Brown, Paul L. (2020). "The pH-potential diagram for polonium". The Aqueous Chemistry of Polonium and the Practical Application of its Thermochemistry. Elsevier. doi:10.1016/b978-0-12-819308-2.00004-8. ISBN 978-0-12-819308-2.

[Bar2-15] 15.00 ^15.01 ^15.02 ^15.03 ^15.04 ^15.05 ^15.06 ^15.07 ^15.08 ^15.09 Bard, A.J.; Faulkner, L.R. (2001). Electrochemical Methods. Fundamentals and Applications (2nd ed.). Wiley. ISBN 9781118312803.

[Lee-17] 16.00 ^16.01 ^16.02 ^16.03 ^16.04 ^16.05 ^16.06 ^16.07 ^16.08 ^16.09 ^16.10 ^16.11 Lee, J. L. (1983). A New Concise Inorganic Chemistry (3rd ed.). London / Wokingham, Berkshire: English Language Book Society & Van Nostrand Reinhold (UK). ISBN 0-442-30179-0.

[Pou-18] Pourbaix, Marcel (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions. Houston, Texas; Cebelcor, Brussels: NACE International. OCLC 475102548.

[Pang2007-19] 18.0 ^18.1 ^18.2 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. doi:10.1016/j.jcis.2007.02.058. PMID 17395194. Bibcode: 2007JCIS..311...94P. https://www.academia.edu/9254087. Retrieved 2017-03-26.

[Greenwood1077-20] 19.0 ^19.1 ^19.2 ^19.3 ^19.4 ^19.5 Greenwood and Earnshaw, p. 1077

[:0-21] 20.0 ^20.1 ^20.2 Lavrukhina, Avgusta Konstantinovna; Pozdni︠a︡kov, Aleksandr Aleksandrovich (1970). Analytical chemistry of technetium, promethium, astatine and francium. Ann Arbor: Ann Arbor-Humphrey Science Publishers. p. 237. ISBN 0-250-39923-7. OCLC 186926.

[:2-22] 21.0 ^21.1 Champion, J.; Alliot, C.; Renault, E.; Mokili, B. M.; Chérel, M.; Galland, N.; Montavon, G. (2009-12-16). "Astatine Standard Redox Potentials and Speciation in Acidic Medium". The Journal of Physical Chemistry A (American Chemical Society (ACS)) 114 (1): 576–582. doi:10.1021/jp9077008. ISSN 1089-5639. PMID 20014840. http://hal.in2p3.fr/in2p3-00450771/file/JPCA_2010.pdf.

[23] 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.

[24] Pavlishchuk, Vitaly V.; Addison, Anthony W. (January 2000). "Conversion constants for redox potentials measured versus different reference electrodes in acetonitrile solutions at 25°C". Inorganica Chimica Acta 298 (1). doi:10.1016/S0020-1693(99)00407-7.

[25] Toyoshima, A.; Kasamatsu, Y.; Tsukada, K.; Asai, M.; Kitatsuji, Y.; Ishii, Y.; Toume, H.; Nishinaka, I. et al. (8 July 2009). "Oxidation of element 102, nobelium, with flow electrolytic column chromatography on an atom-at-a-time scale". Journal of the American Chemical Society 131 (26): 9180–1. doi:10.1021/ja9030038. PMID 19514720. https://figshare.com/articles/Oxidation_of_Element_102_Nobelium_with_Flow_Electrolytic_Column_Chromatography_on_an_Atom_at_a_Time_Scale/2844817.

[webelements_xe-26] 25.0 ^25.1 ^25.2 ^25.3 ^25.4 ^25.5 ^25.6 "compounds information". Xenon. WebElements Periodic Table of the Elements. http://www.webelements.com/xenon/compounds.html.

[Cotton-27] 26.0 ^26.1 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 .

[AP-28] 27.0 ^27.1 ^27.2 ^27.3 ^27.4 Ghosh, Abhik; Berg, Steffen (2014). Arrow Pushing in Inorganic Chemistry: A logical approach to the chemistry of the main-group elements. Hoboken: Wiley. ISBN 978-1-118-17398-5.

[:1-29] 28.0 ^28.1 ^28.2 Appelman, Evan H. (1973-04-01). "Nonexistent compounds. Two case histories". Accounts of Chemical Research (American Chemical Society (ACS)) 6 (4): 113–117. doi:10.1021/ar50064a001. ISSN 0001-4842.

[wou-30] Courtney, Arlene. "Oxidation Reduction Chemistry of the Elements". Ch 412 Advanced Inorganic Chemistry: Reading Materials. Western Oregon University. https://people.wou.edu/~courtna/ch412/redox.htm.

[31] Leszczyński, P.J.; Grochala, W. (2013). "Strong Cationic Oxidizers: Thermal Decomposition, Electronic Structure and Magnetism of Their Compounds". Acta Chim. Slov. 60 (3): 455–470. PMID 24169699. http://acta-arhiv.chem-soc.si/60/60-3-455.pdf.

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