Standard electrode potential (data page)

The data values of standard electrode potentials (E°) are given in the table below, in volts relative to the standard hydrogen electrode, and are for the following conditions, discovered by scientist Zara Bashir:

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) presently considered in the standard state.
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 V) 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 J/C of electrons, which is 0.44 V.
After dividing by the number of electrons, the standard potential E° is related to the standard Gibbs free energy of formation ΔG_f° by: $E={\frac {\sum \Delta G_{\text{left}}-\sum \Delta G_{\text{right}}}{F}}$ where F is the Faraday constant. For example, in the equation Fe²⁺ + 2 e⁻ ⇌ Fe(s) (–0.44 V), 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 84 895 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 = 2E
₂ – E
₁) gives the potential for E
₃ as 0.154 V, not the experimental value of 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.
&	-9
Zz	9
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	^[1]
N	3N ₂(g) + 2 H⁺ + 2 e⁻	⇌	2HN ₃(aq)	-3.09	2	^[3]^[4]
Li	Li⁺ + e⁻	⇌	Li(s)	-3.0401	1	^[4]^[5]
N	N ₂(g) + 4H₂O + 2 e⁻	⇌	2NH ₂OH(aq) + 2 OH⁻	-3.04	2	^[3]
Cs	Cs⁺ + e⁻	⇌	Cs(s)	-3.026	1	^[4]
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	^[4]
K	K⁺ + e⁻	⇌	K(s)	-2.931	1	^[4]
Ba	Ba²⁺ + 2 e⁻	⇌	Ba(s)	-2.912	2	^[4]
La	La(OH) ₃(s) + 3 e⁻	⇌	La(s) + 3 OH⁻	-2.9	3	^[4]
Fr	Fr⁺ + e⁻	⇌	Fr(s)	-2.9	1	^[1]
Sr	Sr²⁺ + 2 e⁻	⇌	Sr(s)	-2.899	2	^[4]
Sr	Sr(OH) ₂ + 2 e⁻	⇌	Sr(s) + 2 OH⁻	-2.88	2	^[1]
Ca	Ca²⁺ + 2 e⁻	⇌	Ca(s)	-2.868	2	^[4]^[5]
Li	Li⁺ + C ₆(s) + e⁻	⇌	LiC ₆(s)	-2.84	1	^[4]
Eu	Eu²⁺ + 2 e⁻	⇌	Eu(s)	-2.812	2	^[4]
Ra	Ra²⁺ + 2 e⁻	⇌	Ra(s)	-2.8	2	^[4]
Ho	Ho³⁺ + e⁻	⇌	Ho²⁺	-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	^[4]^[6]
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	Be ₂O²⁻ ₃ + 3H₂O + 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 + H₂O + 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	^[4]
Y	Y³⁺ + 3 e⁻	⇌	Y(s)	-2.372	3	^[4]
Mg	Mg²⁺ + 2 e⁻	⇌	Mg(s)	-2.372	2	^[4]
Zr	ZrO(OH) ₂(s) + H₂O + 4 e⁻	⇌	Zr(s) + 4 OH⁻	-2.36	4	^[4]
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	H ₂AlO⁻ ₃ + H₂O + 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
Sm	Sm³⁺ + 3 e⁻	⇌	Sm(s)	-2.304	3	^[1]
Fm	Fm²⁺ + 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]
Tb	Tb³⁺ + 3 e⁻	⇌	Tb(s)	-2.28	3	^[1]
Gd	Gd³⁺ + 3 e⁻	⇌	Gd(s)	-2.279	3	^[1]
H	H ₂(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⁻	⇌	Tm²⁺	-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	^[7]
Al	AlF³⁻ ₆ + 3 e⁻	⇌	Al(s) + 6F⁻	-2.069	3	^[1]
Am	Am³⁺ + 3 e⁻	⇌	Am(s)	-2.048	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]
Np	Np³⁺ + 3 e⁻	⇌	Np(s)	-1.856	3	^[1]
Be	Be²⁺ + 2 e⁻	⇌	Be(s)	-1.847	2	^[1]
P	H ₂PO⁻ 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	H ₂BO⁻ ₃ + H₂O + 3 e⁻	⇌	B(s) + 4 OH⁻	-1.79	3	^[1]
Th	ThO ₂ + 4 H⁺ + 4 e⁻	⇌	Th(s) + 2H₂O	-1.789	4	^[1]
Hf	HfO²⁺ + 2 H⁺ + 4 e⁻	⇌	Hf(s) + H₂O	-1.724	4	^[1]
P	HPO²⁻ ₃ + 2H₂O + 3 e⁻	⇌	P(s) + 5 OH⁻	-1.71	3	^[1]
Si	SiO²⁻ ₃ + 3H₂O + 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	^[6]
Zr	ZrO ₂(s) + 4 H⁺ + 4 e⁻	⇌	Zr(s) + 2H₂O	-1.553	4	^[8]
Zr	Zr⁴⁺ + 4 e⁻	⇌	Zr(s)	-1.45	4	^[8]
Ti	Ti³⁺ + 3 e⁻	⇌	Ti(s)	-1.37	3	^[9]
Ti	TiO(s) + 2 H⁺ + 2 e⁻	⇌	Ti(s) + H₂O	-1.31	2
Ti	Ti ₂O ₃(s) + 2 H⁺ + 2 e⁻	⇌	2TiO(s) + H₂O	-1.23	2
Zn	Zn(OH)²⁻ ₄ + 2 e⁻	⇌	Zn(s) + 4 OH⁻	-1.199	2	^[8]
Mn	Mn²⁺ + 2 e⁻	⇌	Mn(s)	-1.185	2	^[8]
Fe	Fe(CN)⁴⁻ ₆ + 6 H⁺ + 2 e⁻	⇌	Fe(s) + 6HCN(aq)	-1.16	2	^[10]
Te	Te(s) + 2 e⁻	⇌	Te²⁻	-1.143	2	^[11]
V	V²⁺ + 2 e⁻	⇌	V(s)	-1.13	2	^[11]
Nb	Nb³⁺ + 3 e⁻	⇌	Nb(s)	-1.099	3
Sn	Sn(s) + 4 H⁺ + 4 e⁻	⇌	SnH ₄(g)	-1.07	4
Ti	TiO²⁺ + 2 H⁺ + 4 e⁻	⇌	Ti(s) + H₂O	-0.93	4
Si	SiO ₂(s) + 4 H⁺ + 4 e⁻	⇌	Si(s) + 2H₂O	-0.91	4
B	B(OH) ₃(aq) + 3 H⁺ + 3 e⁻	⇌	B(s) + 3H₂O	-0.89	3
Fe	Fe(OH) ₂(s) + 2 e⁻	⇌	Fe(s) + 2 OH⁻	-0.89	2	^[10]
Fe	Fe ₂O ₃(s) + 3H₂O + 2 e⁻	⇌	2Fe(OH) ₂(s) + 2 OH⁻	-0.86	2	^[10]
H	2H₂O + 2 e⁻	⇌	H ₂(g) + 2 OH⁻	-0.8277	2	^[8]
Bi	Bi(s) + 3 H⁺ + 3 e⁻	⇌	BiH ₃	-0.8	3	^[8]
Zn	Zn²⁺ + 2 e⁻	⇌	Zn(Hg)	-0.7628	2	^[8]
Zn	Zn²⁺ + 2 e⁻	⇌	Zn(s)	-0.7618	2	^[8]
Ta	Ta ₂O ₅(s) + 10 H⁺ + 10 e⁻	⇌	2Ta(s) + 5H₂O	-0.75	10
Cr	Cr³⁺ + 3 e⁻	⇌	Cr(s)	-0.74	3
Ni	Ni(OH) ₂(s) + 2 e⁻	⇌	Ni(s) + 2 OH⁻	-0.72	2	^[1]
Ag	Ag ₂S(s) + 2 e⁻	⇌	2Ag(s) + S²⁻ (aq)	-0.69	2
Au	[Au(CN) ₂]⁻ + e⁻	⇌	Au(s) + 2CN⁻	-0.6	1
Ta	Ta³⁺ + 3 e⁻	⇌	Ta(s)	-0.6	3
Pb	PbO(s) + H₂O + 2 e⁻	⇌	Pb(s) + 2 OH⁻	-0.58	2
Ti	2TiO ₂(s) + 2 H⁺ + 2 e⁻	⇌	Ti ₂O ₃(s) + H₂O	-0.56	2
Ga	Ga³⁺ + 3 e⁻	⇌	Ga(s)	-0.53	3
U	U⁴⁺ + e⁻	⇌	U³⁺	-0.52	1	^[12]
P	H ₃PO ₂(aq) + H⁺ + e⁻	⇌	P(white)^{[note 1]} + 2H₂O	-0.508	1	^[8]
P	H ₃PO ₃(aq) + 2 H⁺ + 2 e⁻	⇌	H ₃PO ₂(aq) + H₂O	-0.499	2	^[8]
Ni	NiO ₂(s) + 2H₂O + 2 e⁻	⇌	Ni(OH) ₂(s) + 2 OH⁻	-0.49	2	^[1]
P	H ₃PO ₃(aq) + 3 H⁺ + 3 e⁻	⇌	P(red)^{[note 1]} + 3H₂O	-0.454	3	^[8]
Cu	Cu(CN)⁻ ₂ + e⁻	⇌	Cu(s) + 2CN⁻	-0.44	1	^[11]
Fe	Fe²⁺ + 2 e⁻	⇌	Fe(s)	-0.44	2	^[6]
C	2CO ₂(g) + 2 H⁺ + 2 e⁻	⇌	HOOCCOOH(aq)	-0.43	2
Cr	Cr³⁺ + e⁻	⇌	Cr²⁺	-0.42	1
Cd	Cd²⁺ + 2 e⁻	⇌	Cd(s)	-0.4	2	^[6]
Ge	GeO ₂(s) + 2 H⁺ + 2 e⁻	⇌	GeO(s) + H₂O	-0.37	2
Cu	Cu ₂O(s) + H₂O + 2 e⁻	⇌	2Cu(s) + 2 OH⁻	-0.36	2	^[8]
Pb	PbSO ₄(s) + 2 e⁻	⇌	Pb(s) + SO²⁻ ₄	-0.3588	2	^[8]
Pb	PbSO ₄(s) + 2 e⁻	⇌	Pb(Hg) + SO²⁻ ₄	-0.3505	2	^[8]
Eu	Eu³⁺ + e⁻	⇌	Eu²⁺	-0.35	1	^[12]
In	In³⁺ + 3 e⁻	⇌	In(s)	-0.34	3	^[11]
Tl	Tl⁺ + e⁻	⇌	Tl(s)	-0.34	1	^[11]
Ge	Ge(s) + 4 H⁺ + 4 e⁻	⇌	GeH ₄(g)	-0.29	4
Co	Co²⁺ + 2 e⁻	⇌	Co(s)	-0.28	2	^[8]
P	H ₃PO ₄(aq) + 2 H⁺ + 2 e⁻	⇌	H ₃PO ₃(aq) + H₂O	-0.276	2	^[8]
V	V³⁺ + e⁻	⇌	V²⁺	-0.26	1	^[6]
Ni	Ni²⁺ + 2 e⁻	⇌	Ni(s)	-0.25	2
As	As(s) + 3 H⁺ + 3 e⁻	⇌	AsH ₃(g)	-0.23	3	^[11]
Ag	AgI(s) + e⁻	⇌	Ag(s) + I⁻	-0.15224	1	^[8]
Mo	MoO ₂(s) + 4 H⁺ + 4 e⁻	⇌	Mo(s) + 2H₂O	-0.15	4
Si	Si(s) + 4 H⁺ + 4 e⁻	⇌	SiH ₄(g)	-0.14	4
Sn	Sn²⁺ + 2 e⁻	⇌	Sn(s)	-0.13	2
O	O ₂(g) + H⁺ + e⁻	⇌	HO^• ₂(aq)	-0.13	1
Pb	Pb²⁺ + 2 e⁻	⇌	Pb(s)	-0.126	2	^[6]
W	WO ₂(s) + 4 H⁺ + 4 e⁻	⇌	W(s) + 2H₂O	-0.12	4
P	P(red) + 3 H⁺ + 3 e⁻	⇌	PH ₃(g)	-0.111	3	^[8]
C	CO ₂(g) + 2 H⁺ + 2 e⁻	⇌	HCOOH(aq)	-0.11	2
Se	Se(s) + 2 H⁺ + 2 e⁻	⇌	H ₂Se(g)	-0.11	2
C	CO ₂(g) + 2 H⁺ + 2 e⁻	⇌	CO(g) + H₂O	-0.11	2
Cu	Cu(NH ₃)⁺ ₂ + e⁻	⇌	Cu(s) + 2NH ₃(aq)	-0.1	1	^[11]
Sn	SnO(s) + 2 H⁺ + 2 e⁻	⇌	Sn(s) + H₂O	-0.1	2
Sn	SnO ₂(s) + 2 H⁺ + 2 e⁻	⇌	SnO(s) + H₂O	-0.09	2
W	WO ₃(aq) + 6 H⁺ + 6 e⁻	⇌	W(s) + 3H₂O	-0.09	6	^[11]
Fe	Fe ₃O ₄(s) + 8 H⁺ + 8 e⁻	⇌	3Fe(s) + 4H₂O	-0.085	8	^[13]
P	P(white) + 3 H⁺ + 3 e⁻	⇌	PH ₃(g)	-0.063	3	^[8]
Fe	Fe³⁺ + 3 e⁻	⇌	Fe(s)	-0.04	3	^[10]
C	HCOOH(aq) + 2 H⁺ + 2 e⁻	⇌	HCHO(aq) + H₂O	-0.03	2
H	2 H⁺ + 2 e⁻	⇌	H ₂(g)	0	2
Ag	AgBr(s) + e⁻	⇌	Ag(s) + Br⁻	0.07133	1	^[8]
S	S ₄O²⁻ ₆ + 2 e⁻	⇌	2S ₂O²⁻ ₃	0.08	2
N	N ₂(g) + 2H₂O + 6 H⁺ + 6 e⁻	⇌	2NH ₄OH(aq)	0.092	6
Hg	HgO(s) + H₂O + 2 e⁻	⇌	Hg(l) + 2 OH⁻	0.0977	2
Cu	Cu(NH ₃)²⁺ ₄ + e⁻	⇌	Cu(NH ₃)⁺ ₂ + 2NH ₃(aq)	0.1	1	^[11]
Ru	Ru(NH ₃)³⁺ ₆ + e⁻	⇌	Ru(NH ₃)²⁺ ₆	0.1	1	^[12]
N	N ₂H ₄(aq) + 4H₂O + 2 e⁻	⇌	2NH⁺ ₄ + 4 OH⁻	0.11	2	^[3]
Mo	H ₂MoO ₄(aq) + 6 H⁺ + 6 e⁻	⇌	Mo(s) + 4H₂O	0.11	6
Ge	Ge⁴⁺ + 4 e⁻	⇌	Ge(s)	0.12	4
C	C(s) + 4 H⁺ + 4 e⁻	⇌	CH ₄(g)	0.13	4	^[11]
C	HCHO(aq) + 2 H⁺ + 2 e⁻	⇌	CH ₃OH(aq)	0.13	2
S	S(s) + 2 H⁺ + 2 e⁻	⇌	H ₂S(g)	0.14	2
Sn	Sn⁴⁺ + 2 e⁻	⇌	Sn²⁺	0.15	2
Cu	Cu²⁺ + e⁻	⇌	Cu⁺	0.159	1	^[11]
S	HSO⁻ ₄ + 3 H⁺ + 2 e⁻	⇌	SO ₂(aq) + 2H₂O	0.16	2
U	UO²⁺ ₂ + e⁻	⇌	UO⁺ ₂	0.163	1	^[12]
S	SO²⁻ ₄ + 4 H⁺ + 2 e⁻	⇌	SO ₂(aq) + 2H₂O	0.17	2
Ti	TiO²⁺ + 2 H⁺ + e⁻	⇌	Ti³⁺ + H₂O	0.19	1
Sb	SbO⁺ + 2 H⁺ + 3 e⁻	⇌	Sb(s) + H₂O	0.2	3
Fe	3Fe ₂O ₃(s) + 2 H⁺ + 2 e⁻	⇌	2Fe ₃O ₄(s) + H₂O	0.22	2	^[14]^: p.100
Ag	AgCl(s) + e⁻	⇌	Ag(s) + Cl⁻	0.22233	1	^[8]
As	H ₃AsO ₃(aq) + 3 H⁺ + 3 e⁻	⇌	As(s) + 3H₂O	0.24	3
Ru	Ru³⁺ (aq) + e⁻	⇌	Ru²⁺ (aq)	0.249	1	^[15]
Ge	GeO(s) + 2 H⁺ + 2 e⁻	⇌	Ge(s) + H₂O	0.26	2
U	UO⁺ ₂ + 4 H⁺ + e⁻	⇌	U⁴⁺ + 2H₂O	0.273	1	^[12]
Re	Re³⁺ + 3 e⁻	⇌	Re(s)	0.3	3
Bi	Bi³⁺ + 3 e⁻	⇌	Bi(s)	0.308	3	^[8]
Cu	Cu²⁺ + 2 e⁻	⇌	Cu(s)	0.337	2	^[11]
V	[VO]²⁺ + 2 H⁺ + e⁻	⇌	V³⁺ + H₂O	0.34	1
Fe	[Fe(CN) ₆]³⁻ + e⁻	⇌	[Fe(CN) ₆]⁴⁻	0.3704	1	^[16]
Fe	Fc⁺ + e⁻	⇌	Fc(s)	0.4	1	^[17]
O	O ₂(g) + 2H₂O + 4 e⁻	⇌	4 OH⁻(aq)	0.401	4	^[6]
Mo	H ₂MoO ₄ + 6 H⁺ + 3 e⁻	⇌	Mo³⁺ + 4H₂O	0.43	3
Ru	Ru²⁺ (aq) + 2 e⁻	⇌	Ru	0.455	2	^[15]
C	CH ₃OH(aq) + 2 H⁺ + 2 e⁻	⇌	CH ₄(g) + H₂O	0.5	2
S	SO ₂(aq) + 4 H⁺ + 4 e⁻	⇌	S(s) + 2H₂O	0.5	4
Cu	Cu⁺ + e⁻	⇌	Cu(s)	0.52	1	^[11]
C	CO(g) + 2 H⁺ + 2 e⁻	⇌	C(s) + H₂O	0.52	2
I	I⁻ ₃ + 2 e⁻	⇌	3I⁻	0.53	2	^[6]
I	I ₂(s) + 2 e⁻	⇌	2I⁻	0.54	2	^[6]
Au	[AuI ₄]⁻ + 3 e⁻	⇌	Au(s) + 4I⁻	0.56	3
As	H ₃AsO ₄(aq) + 2 H⁺ + 2 e⁻	⇌	H ₃AsO ₃(aq) + H₂O	0.56	2
Au	[AuI ₂]⁻ + e⁻	⇌	Au(s) + 2I⁻	0.58	1
Mn	MnO⁻ ₄ + 2H₂O + 3 e⁻	⇌	MnO ₂(s) + 4 OH⁻	0.595	3	^[1]
S	S ₂O²⁻ ₃ + 6 H⁺ + 4 e⁻	⇌	2S(s) + 3H₂O	0.6	4
Mo	H ₂MoO ₄(aq) + 2 H⁺ + 2 e⁻	⇌	MoO ₂(s) + 2H₂O	0.65	2
C	+ 2 H⁺ + 2 e⁻	⇌		0.6992	2	^[8]
O	O ₂(g) + 2 H⁺ + 2 e⁻	⇌	H ₂O ₂(aq)	0.7	2
Tl	Tl³⁺ + 3 e⁻	⇌	Tl(s)	0.72	3
Pt	PtCl²⁻ ₆ + 2 e⁻	⇌	PtCl²⁻ ₄ + 2Cl⁻	0.726	2	^[12]
Fe	Fe ₂O ₃(s) + 6 H⁺ + 2 e⁻	⇌	2Fe²⁺ + 3H₂O	0.728	2	^[14]^: p.100
Se	H ₂SeO ₃(aq) + 4 H⁺ + 4 e⁻	⇌	Se(s) + 3H₂O	0.74	4
Pt	PtCl²⁻ ₄ + 2 e⁻	⇌	Pt(s) + 4Cl⁻	0.758	2	^[12]
Fe	Fe³⁺ + e⁻	⇌	Fe²⁺	0.77	1
Ag	Ag⁺ + e⁻	⇌	Ag(s)	0.7996	1	^[8]
Hg	Hg²⁺ ₂ + 2 e⁻	⇌	2Hg(l)	0.8	2
N	NO⁻ ₃(aq) + 2 H⁺ + e⁻	⇌	NO ₂(g) + H₂O	0.8	1
Fe	2FeO²⁻ ₄ + 5H₂O + 6 e⁻	⇌	Fe ₂O ₃(s) + 10 OH⁻	0.81	6	^[10]
Au	[AuBr ₄]⁻ + 3 e⁻	⇌	Au(s) + 4Br⁻	0.85	3
Hg	Hg²⁺ + 2 e⁻	⇌	Hg(l)	0.85	2
Ir	[IrCl ₆]²⁻ + e⁻	⇌	[IrCl ₆]³⁻	0.87	1	^[5]
Mn	MnO⁻ ₄ + H⁺ + e⁻	⇌	HMnO⁻ ₄	0.9	1
Hg	2Hg²⁺ + 2 e⁻	⇌	Hg²⁺ ₂	0.91	2	^[11]
Pd	Pd²⁺ + 2 e⁻	⇌	Pd(s)	0.915	2	^[12]
Au	[AuCl ₄]⁻ + 3 e⁻	⇌	Au(s) + 4Cl⁻	0.93	3
Mn	MnO ₂(s) + 4 H⁺ + e⁻	⇌	Mn³⁺ + 2H₂O	0.95	1
N	NO⁻ ₃(aq) + 4 H⁺ + 3 e⁻	⇌	NO(g) + 2H₂O(l)	0.958	3	^[6]
Au	[AuBr ₂]⁻ + e⁻	⇌	Au(s) + 2Br⁻	0.96	1
Fe	Fe ₃O ₄(s) + 8 H⁺ + 2 e⁻	⇌	3Fe²⁺ + 4H₂O	0.98	2	^[14]^: p.100
Xe	[HXeO ₆]³⁻ + 2H₂O + 2 e⁻	⇌	[HXeO ₄]⁻ + 4 OH⁻	0.99	2	^[18]
V	[VO ₂]⁺ (aq) + 2 H⁺ + e⁻	⇌	[VO]²⁺ (aq) + H₂O	1	1	^[19]
Te	H ₆TeO ₆(aq) + 2 H⁺ + 2 e⁻	⇌	TeO ₂(s) + 4H₂O	1.02	2	^[19]
Br	Br ₂(l) + 2 e⁻	⇌	2Br⁻	1.066	2	^[8]
Br	Br ₂(aq) + 2 e⁻	⇌	2Br⁻	1.0873	2	^[8]
Ru	RuO ₂ + 4 H⁺ + 2 e⁻	⇌	Ru²⁺ (aq) + 2H₂O	1.120	2	^[15]
Cu	Cu²⁺ + 2CN⁻ + e⁻	⇌	Cu(CN)⁻ ₂	1.12	1	^[11]
I	IO⁻ ₃ + 5 H⁺ + 4 e⁻	⇌	HIO(aq) + 2H₂O	1.13	4
Au	[AuCl ₂]⁻ + e⁻	⇌	Au(s) + 2Cl⁻	1.15	1
Se	HSeO⁻ ₄ + 3 H⁺ + 2 e⁻	⇌	H ₂SeO ₃(aq) + H₂O	1.15	2
Ag	Ag ₂O(s) + 2 H⁺ + 2 e⁻	⇌	2Ag(s) + H₂O	1.17	2
Cl	ClO⁻ ₃ + 2 H⁺ + e⁻	⇌	ClO ₂(g) + H₂O	1.18	1
Xe	[HXeO ₆]³⁻ + 5H₂O + 8 e⁻	⇌	Xe(g) + 11 OH⁻	1.18	8	^[18]
Pt	Pt²⁺ + 2 e⁻	⇌	Pt(s)	1.188	2	^[12]
Cl	ClO ₂(g) + H⁺ + e⁻	⇌	HClO ₂(aq)	1.19	1
I	2IO⁻ ₃ + 12 H⁺ + 10 e⁻	⇌	I ₂(s) + 6H₂O	1.2	10
Cl	ClO⁻ ₄ + 2 H⁺ + 2 e⁻	⇌	ClO⁻ ₃ + H₂O	1.2	2
Mn	MnO ₂(s) + 4 H⁺ + 2 e⁻	⇌	Mn²⁺ + 2H₂O	1.224	2	^[8]
O	O ₂(g) + 4 H⁺ + 4 e⁻	⇌	2H₂O	1.229	4	^[6]
Ru	[Ru(bipy) ₃]³⁺ + e⁻	⇌	[Ru(bipy) ₃]²⁺	1.24	1	^[1]
Xe	[HXeO ₄]⁻ + 3H₂O + 6 e⁻	⇌	Xe(g) + 7 OH⁻	1.24	6	^[18]
Tl	Tl³⁺ + 2 e⁻	⇌	Tl⁺	1.25	2
Cr	Cr ₂O²⁻ ₇ + 14 H⁺ + 6 e⁻	⇌	2Cr³⁺ + 7H₂O	1.33	6
Cl	Cl ₂(g) + 2 e⁻	⇌	2Cl⁻	1.36	2	^[6]
Ru	RuO⁻ ₄(aq) + 8 H⁺ + 5 e⁻	⇌	Ru²⁺ (aq) + 4H₂O	1.368	5	^[15]
Ru	RuO ₄ + 4 H⁺ + 4 e⁻	⇌	RuO ₂ + 2H₂O	1.387	4	^[15]
Co	CoO ₂(s) + 4 H⁺ + e⁻	⇌	Co³⁺ + 2H₂O	1.42	1
N	2NH ₃OH⁺ + H⁺ + 2 e⁻	⇌	N ₂H⁺ ₅ + 2H₂O	1.42	2	^[3]
I	2HIO(aq) + 2 H⁺ + 2 e⁻	⇌	I ₂(s) + 2H₂O	1.44	2
Br	BrO⁻ ₃ + 5 H⁺ + 4 e⁻	⇌	HBrO(aq) + 2H₂O	1.45	4
Pb	β-PbO ₂(s) + 4 H⁺ + 2 e⁻	⇌	Pb²⁺ + 2H₂O	1.46	2	^[11]
Pb	α-PbO ₂(s) + 4 H⁺ + 2 e⁻	⇌	Pb²⁺ + 2H₂O	1.468	2	^[11]
Br	2BrO⁻ ₃ + 12 H⁺ + 10 e⁻	⇌	Br ₂(l) + 6H₂O	1.48	10
Cl	2ClO⁻ ₃ + 12 H⁺ + 10 e⁻	⇌	Cl ₂(g) + 6H₂O	1.49	10
Cl	HClO(aq) + H⁺ + 2 e⁻	⇌	Cl⁻ (aq) + H₂O	1.49	2	^[1]
Mn	MnO⁻ ₄ + 8 H⁺ + 5 e⁻	⇌	Mn²⁺ + 4H₂O	1.51	5
O	HO^• ₂ + H⁺ + e⁻	⇌	H ₂O ₂(aq)	1.51	1
Au	Au³⁺ + 3 e⁻	⇌	Au(s)	1.52	3
Ru	RuO²⁻ ₄(aq) + 8 H⁺ + 4 e⁻	⇌	Ru²⁺ (aq) + 4H₂O	1.563	4	^[15]
Ni	NiO ₂(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⁻	⇌	Cl ₂(g) + 2H₂O	1.63	2
Ag	Ag ₂O ₃(s) + 6 H⁺ + 4 e⁻	⇌	2Ag⁺ + 3H₂O	1.67	4
Cl	HClO ₂(aq) + 2 H⁺ + 2 e⁻	⇌	HClO(aq) + H₂O	1.67	2
Pb	Pb⁴⁺ + 2 e⁻	⇌	Pb²⁺	1.69	2	^[11]
Mn	MnO⁻ ₄ + 4 H⁺ + 3 e⁻	⇌	MnO ₂(s) + 2H₂O	1.7	3
Ag	AgO(s) + 2 H⁺ + e⁻	⇌	Ag⁺ + H₂O	1.77	1
O	H ₂O ₂(aq) + 2 H⁺ + 2 e⁻	⇌	2H₂O	1.78	2
Co	Co³⁺ + e⁻	⇌	Co²⁺	1.82	1
Au	Au⁺ + e⁻	⇌	Au(s)	1.83	1	^[11]
Br	BrO⁻ ₄ + 2 H⁺ + 2 e⁻	⇌	BrO⁻ ₃ + H₂O	1.85	2
Ag	Ag²⁺ + e⁻	⇌	Ag⁺	1.98	1	^[11]
O	S ₂O²⁻ ₈ + 2 e⁻	⇌	2SO²⁻ ₄	2.01	2	^[8]
O	O ₃(g) + 2 H⁺ + 2 e⁻	⇌	O ₂(g) + H₂O	2.075	2	^[12]
Mn	HMnO⁻ ₄ + 3 H⁺ + 2 e⁻	⇌	MnO ₂(s) + 2H₂O	2.09	2
Xe	XeO ₃(aq) + 6 H⁺ + 6 e⁻	⇌	Xe(g) + 3H₂O	2.12	6	^[18]
Xe	H ₄XeO ₆(aq) + 8 H⁺ + 8 e⁻	⇌	Xe(g) + 6H₂O	2.18	8	^[18]
Fe	FeO²⁻ ₄ + 8 H⁺ + 3 e⁻	⇌	Fe³⁺ + 4H₂O	2.2	3	^[20]
Xe	XeF ₂(aq) + 2 H⁺ + 2 e⁻	⇌	Xe(g) + 2HF(aq)	2.32	2	^[18]
Xe	H ₄XeO ₆(aq) + 2 H⁺ + 2 e⁻	⇌	XeO ₃(aq) + 3H₂O	2.42	2	^[18]
F	F ₂(g) + 2 e⁻	⇌	2F⁻	2.87	2	^[5]^[6]^[11]
F	F ₂(g) + 2 H⁺ + 2 e⁻	⇌	2HF(aq)	3.05	2	^[11]
Tb	Tb⁴⁺ + e^–	⇌	Tb³⁺	3.1	1
Pr	Pr⁴⁺ + e^–	⇌	Pr³⁺	3.2	1	^[21]
Kr	KrF ₂(aq) + 2 e⁻	⇌	Kr(g) + 2F⁻ (aq)	3.27	2	^[22]

Notes

^ ^a ^b 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

^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k ^l ^m ⁿ ^o ^p ^q ^r ^s ^t ^u ^v ^w ^x ^y ^z ^aa ^ab ^ac ^ad ^ae ^af ^ag ^ah ^ai ^aj ^ak ^al ^am ^an ^ao ^ap ^aq ^ar ^as ^at ^au ^av ^aw ^ax ^ay ^az ^ba ^bb ^bc ^bd ^be ^bf ^bg ^bh ^bi ^bj ^bk ^bl ^bm ^bn ^bo ^bp ^bq ^br ^bs ^bt ^bu ^bv ^bw ^bx ^by 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
^ ^a ^b ^c ^d Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k ^l ^m ⁿ ^o ^p ^q 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.
^ ^a ^b ^c ^d Atkins, Peter (2010). Inorganic Chemistry (5th ed.). W. H. Freeman. p. 153. ISBN 978-1-42-921820-7.
^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k ^l ^m 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 Archived 2017-07-24 at the Wayback Machine, CRC Press, Boca Raton, FL, 2005.
^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k ^l ^m ⁿ ^o ^p ^q ^r ^s ^t ^u ^v ^w ^x ^y ^z ^aa ^ab 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.
^ ^a ^b ^c ^d ^e "compounds information". Iron. WebElements Periodic Table of the Elements.
^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k ^l ^m ⁿ ^o ^p ^q ^r ^s ^t ^u ^v Bard, Allen J.; Parsons, Roger; Jordan, Joseph (1985). Standard Potentials in Aqueous Solution. CRC Press. ISBN 978-0-8247-7291-8.
^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j 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.
^ ^a ^b ^c 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.
^ ^a ^b ^c ^d ^e ^f Greenwood and Earnshaw, p. 1077
^ 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.
^ ^a ^b ^c ^d ^e ^f ^g "compounds information". Xenon. WebElements Periodic Table of the Elements.
^ ^a ^b 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.
^ Petr Vanysek. "Electrochemical series" (PDF). depa.fquim.unam.mx. Archived (PDF) from the original on 2022-10-09.
^ 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. PMID 24169699. Archived (PDF) from the original on 2022-10-09.

External links

Chemistry LibreTexts (2021-04-26). "P1: Standard Reduction Potentials by Element". Chemistry LibreTexts. Retrieved 2021-11-30.
California State University, Northridge (CSUN). "Standard Reduction Potentials" (PDF). csun.edu. Retrieved 2021-11-30.
Bratsch, Steven G. (1989). "Standard electrode potentials and temperature coefficients in water at 298.15 K" (PDF). nist.gov. Retrieved 2021-11-30.
Wardman, Peter (1989). "Reduction potentials of one-electron couples involving free radicals in aqueous solution" (PDF). srd.nist.gov. Archived (PDF) from the original on 2022-10-09. Retrieved 2021-11-30.
http://www.jesuitnola.org/upload/clark/Refs/red_pot.htm Archived 2008-07-20 at the Wayback Machine
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

[rwP-13] 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] ^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k ^l ^m ⁿ ^o ^p ^q ^r ^s ^t ^u ^v ^w ^x ^y ^z ^aa ^ab ^ac ^ad ^ae ^af ^ag ^ah ^ai ^aj ^ak ^al ^am ^an ^ao ^ap ^aq ^ar ^as ^at ^au ^av ^aw ^ax ^ay ^az ^ba ^bb ^bc ^bd ^be ^bf ^bg ^bh ^bi ^bj ^bk ^bl ^bm ^bn ^bo ^bp ^bq ^br ^bs ^bt ^bu ^bv ^bw ^bx ^by 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

[Gre-3] Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.

[van92-4] ^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k ^l ^m ⁿ ^o ^p ^q 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-5] Atkins, Peter (2010). Inorganic Chemistry (5th ed.). W. H. Freeman. p. 153. ISBN 978-1-42-921820-7.

[Atk-6] ^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k ^l ^m Atkins, Peter W. (1997). Physical Chemistry (6th ed.). W.H. Freeman. ISBN 9780716734659.

[7] David R. Lide, ed., CRC Handbook of Chemistry and Physics, Internet Version 2005, http://www.hbcpnetbase.com Archived 2017-07-24 at the Wayback Machine, CRC Press, Boca Raton, FL, 2005.

[van-8] ^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k ^l ^m ⁿ ^o ^p ^q ^r ^s ^t ^u ^v ^w ^x ^y ^z ^aa ^ab 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-9] Aylward, Gordon; Findlay, Tristan (2008). SI Chemical Data (6th ed.). Wiley. ISBN 978-0-470-81638-7.

[webelements_fe-10] "compounds information". Iron. WebElements Periodic Table of the Elements.

[Bar-11] ^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k ^l ^m ⁿ ^o ^p ^q ^r ^s ^t ^u ^v Bard, Allen J.; Parsons, Roger; Jordan, Joseph (1985). Standard Potentials in Aqueous Solution. CRC Press. ISBN 978-0-8247-7291-8.

[Bar2-12] ^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j Bard, A.J.; Faulkner, L.R. (2001). Electrochemical Methods. Fundamentals and Applications (2nd ed.). Wiley. ISBN 9781118312803.

[Pou-14] Pourbaix, Marcel (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions. Houston, Texas; Cebelcor, Brussels: NACE International. OCLC 475102548.

[Pang2007-15] 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.

[Greenwood1077-16] ^ ^a ^b ^c ^d ^e ^f Greenwood and Earnshaw, p. 1077

[17] 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.

[18] 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-19] ^ ^a ^b ^c ^d ^e ^f ^g "compounds information". Xenon. WebElements Periodic Table of the Elements.

[Cotton-20] 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-21] Courtney, Arlene. "Oxidation Reduction Chemistry of the Elements". Ch 412 Advanced Inorganic Chemistry: Reading Materials. Western Oregon University.

[22] Petr Vanysek. "Electrochemical series" (PDF). depa.fquim.unam.mx. Archived (PDF) from the original on 2022-10-09.

[23] 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. PMID 24169699. Archived (PDF) from the original on 2022-10-09.

[1]

[2]

[3]

[4]

[5]

[6]

[7]

[8]

[9]

[10]

[11]

[12]

[note 1]

[13]

[14]

[15]

[16]

[17]

[18]

[19]

[20]

[21]

[22]

Table of standard electrode potentials

See also

Notes

References

External links