標準電極電勢表

主條目：標準電極電勢

標準電極電勢可以用來計算化學電池或原電池的電化學勢或電極電勢。

標準電極電位是以標準氫原子作為參比電極，即氫的標準電極電位值定為0，與氫標準電極比較，電位較高者為正，電位較低者為負。

表中電極電勢以以下條件測得（(s)：固體；(l)：液體；(g)：氣體；(aq)：水溶液；(Hg)：汞齊）：

• 參比電極：標準氫電極，所有離子的數據都在水溶液測得^{[1][2][3][4][5][6][7][8][9]}
• 活性度：統一為純固體、純液體或水溶液
• 溫度：298.15K／25攝氏度
• 水溶液或汞齊之有效離子濃度：每公升1摩
• 氣體反應物分壓：1大氣壓／101325帕

單擊頂欄箭咀可將數據按元素符號、反應物、產物或標準電極電勢值排序。

元素	氧化劑	半反應	還原劑	E°（V）[註 1]	來源
	-9
	9
鋇	Ba+ ＋e⁻	⇌	Ba(s)	−4.38	[10][11][12]
鍶	Sr+ ＋e⁻	⇌	Sr(s)	−4.10	[13][10][11][14]
鈣	Ca+ ＋e⁻	⇌	Ca(s)	−3.8	[13][10][11][14]
釷	Th⁴⁺＋e⁻	⇌	Th³⁺	−3.6	[15]
鐠	Pr³⁺＋e⁻	⇌	Pr²⁺	−3.1	[13]
氮	3N 2(g)＋2H⁺＋2e⁻	⇌	2HN 3(aq)	−3.09	[16]
鋰	Li+ ＋e⁻	⇌	Li(s)	−3.0401	[17]
氮	N 2(g)＋4H₂O＋2e⁻	⇌	2NH 2OH(aq)＋2OH⁻	−3.04	[16]
銫	Cs+ ＋e⁻	⇌	Cs(s)	−3.026	[17]
鈣	Ca(OH) 2(s)＋2e⁻	⇌	Ca(s)＋2OH⁻	−3.02	[13]
鉺	Er3+ ＋e⁻	⇌	Er2+	−3.0	[13]
鋇	Ba(OH) 2(s)＋2e⁻	⇌	Ba(s)＋2OH⁻	−2.99	[13]
銣	Rb+ ＋e⁻	⇌	Rb(s)	−2.98	[18]
鉀	K+ ＋e⁻	⇌	K(s)	−2.92	[17]
鎂	Mg+ ＋e⁻	⇌	Mg(s)	−2.93	[12]
鋇	Ba2+ ＋2e⁻	⇌	Ba(s)	−2.912	[17]
鑭	La(OH) 3(s)＋3e⁻	⇌	La(s)＋3OH⁻	−2.90	[17]
鈁	Fr+ ＋e⁻	⇌	Fr(s)	−2.9	[13]
鍶	Sr2+ ＋2e⁻	⇌	Sr(s)	−2.899	[17]
鍶	Sr(OH) 2(s)＋2e⁻	⇌	Sr(s)＋2OH⁻	−2.88	[13]
鈣	Ca2+ ＋2e⁻	⇌	Ca(s)	−2.868	[17]
銨	NH+ 4＋e⁻	⇌	NH 4•	−2.85
銪	Eu2+ ＋2e⁻	⇌	Eu(s)	−2.812	[17]
鐳	Ra2+ ＋2e⁻	⇌	Ra(s)	−2.8	[17]
鐿	Yb2+ ＋2e⁻	⇌	Yb(s)	−2.76	[13][10]
鈉	Na+ ＋e⁻	⇌	Na(s)	−2.71	[17][19]
釤	Sm2+ ＋2e⁻	⇌	Sm(s)	−2.68	[13][10]
鍩	No2+ ＋2e⁻	⇌	No(s)	−2.50	[13]
鉿	HfO(OH) 2(s)＋H₂O＋4e⁻	⇌	Hf(s)＋4OH⁻	−2.50	[13]
釷	Th(OH) 4(s)＋4e⁻	⇌	Th(s)＋4OH⁻	−2.48	[13]
鍆	Md2+ ＋2e⁻	⇌	Md(s)	−2.40	[13]
鑭	La3+ ＋3e⁻	⇌	La(s)	−2.379	[17]
釔	Y3+ ＋3e⁻	⇌	Y(s)	−2.372	[17]
鎂	Mg2+ ＋2e⁻	⇌	Mg(s)	−2.372	[17]
鋯	ZrO(OH) 2(s)＋H₂O＋4e⁻	⇌	Zr(s)＋4OH⁻	−2.36	[17]
鐠	Pr3+ ＋3e⁻	⇌	Pr(s)	−2.353	[13]
鈰	Ce3+ ＋3e⁻	⇌	Ce(s)	−2.336	[13]
鉺	Er3+ ＋3e⁻	⇌	Er(s)	−2.331	[13]
鈥	Ho3+ ＋3e⁻	⇌	Ho(s)	−2.33	[13]
鋁	Al(OH)− 4＋3e⁻	⇌	Al(s)＋4OH⁻	−2.33
鋁	Al(OH) 3(s)＋3e⁻	⇌	Al(s)＋3OH⁻	−2.31
鋱	Tb3+ ＋3e⁻	⇌	Tb(s)	−2.28
氫	H 2(g)＋2e⁻	⇌	2H−	−2.25
錒	Ac3+ ＋3e⁻	⇌	Ac(s)	−2.20
鈹	Be+ ＋e⁻	⇌	Be(s)	−2.12	[12]
鉲	Cf2+ ＋2e⁻	⇌	Cf(s)	−2.12	[13]
鋂	Am3+ ＋3e⁻	⇌	Am(s)	−2.048	[13]
鉲	Cf3+ ＋3e⁻	⇌	Cf(s)	−1.94	[13]
鈣	Ca2+ ＋e⁻	⇌	Ca+	−1.936	[17][13]
鋂	Am2+ ＋2e⁻	⇌	Am(s)	−1.9	[13]
鐨	Fm3+ ＋3e⁻	⇌	Fm(s)	−1.89	[13]
鈹	Be2+ ＋2e⁻	⇌	Be(s)	−1.85
鑪	Rf4+ ＋4e⁻	⇌	Rf(s)	−1.67	[20]
鈾	U3+ ＋3e⁻	⇌	U(s)	−1.66	[21]
鋁	Al3+ ＋3e⁻	⇌	Al(s)	−1.66	[19]
鈦	Ti2+ ＋2e⁻	⇌	Ti(s)	−1.63	[19]
鉳	Bk2+ ＋2e⁻	⇌	Bk(s)	−1.6	[13]
鋯	ZrO 2(s)＋4H⁺＋4e⁻	⇌	Zr(s)＋2H₂O	−1.553	[17]
鉿	Hf4+ ＋4e⁻	⇌	Hf(s)	−1.55	[13]
鋯	Zr4+ ＋4e⁻	⇌	Zr(s)	−1.45	[17]
鈦	Ti3+ ＋3e⁻	⇌	Ti(s)	−1.37	[22]
鈦	TiO(s)＋2H⁺＋2e⁻	⇌	Ti(s)＋H₂O	−1.31
鈦	Ti 2O 3(s)＋2H⁺＋2e⁻	⇌	2TiO(s)＋H₂O	−1.23
鋅	Zn(OH)2− 4＋2e⁻	⇌	Zn(s)＋4OH⁻	−1.199	[23]
錳	Mn2+ ＋2e⁻	⇌	Mn(s)	−1.185	[23]
鐵	Fe(CN)4− 6＋6H⁺＋2e⁻	⇌	Fe(s)＋6HCN(aq)	−1.16	[24]
釩	V2+ ＋2e⁻	⇌	V(s)	−1.175	[25]
碲	Te(s)＋2e⁻	⇌	Te²⁻	−1.143	[25]
鈮	Nb3+ ＋3e⁻	⇌	Nb(s)	−1.099
錫	Sn(s)＋4H⁺＋4e⁻	⇌	SnH 4(g)	−1.07
銦	In(OH) 3(s)＋3e⁻	⇌	In(s)＋3OH⁻	−0.99	[13]
矽	SiO 2(s)＋4H⁺＋4e⁻	⇌	Si(s)＋2H₂O	−0.91
硼	B(OH) 3(aq)＋3H⁺＋3e⁻	⇌	B(s)＋3H₂O	−0.89
鐵	Fe(OH) 2(s)＋2e⁻	⇌	Fe(s)＋2OH⁻	−0.89	[24]
鐵	Fe₂O₃(s)＋3H₂O＋2e⁻	⇌	2Fe(OH) 2(s)＋2OH⁻	−0.86	[24]
鈦	TiO2+ ＋2H⁺＋4e⁻	⇌	Ti(s)＋H₂O	−0.86
氫	2H₂O＋2e⁻	⇌	H 2(g)＋2OH⁻	−0.8277	[17]
鉍	Bi(s)＋3H⁺＋3e⁻	⇌	BiH 3	−0.8	[23]
鋅	Zn2+ ＋2e⁻	⇌	Zn(Hg)	−0.7628	[17]
鋅	Zn2+ ＋2e⁻	⇌	Zn(s)	−0.7618	[17]
鉭	Ta 2O 5(s)＋10H⁺＋10e⁻	⇌	2Ta(s)＋5H₂O	−0.75
鉻	Cr3+ ＋3e⁻	⇌	Cr(s)	−0.74
金	[Au(CN)− 2]＋e⁻	⇌	Au(s)＋2CN−	−0.60
鉭	Ta3+ ＋3e⁻	⇌	Ta(s)	−0.6
鉛	PbO(s)＋H₂O＋2e⁻	⇌	Pb(s)＋2OH⁻	−0.58
鈦	2TiO 2(s)＋2H⁺＋2e⁻	⇌	Ti 2O 3(s)＋H₂O	−0.56
鎵	Ga3+ ＋3e⁻	⇌	Ga(s)	−0.53
鈾	U4+ ＋e⁻	⇌	U3+	−0.52	[21]
磷	H 3PO 2(aq)＋H⁺＋e⁻	⇌	P（白）[26]＋2H₂O	−0.508	[17]
磷	H 3PO 3(aq)＋2H⁺＋2e⁻	⇌	H 3PO 2(aq)＋H₂O	−0.499	[17]
磷	H 3PO 3(aq)＋3H⁺＋3e⁻	⇌	P（紅）[26]＋3H₂O	−0.454	[17]
鐵	Fe2+ ＋2e⁻	⇌	Fe(s)	−0.44	[19]
碳	2CO 2(g)＋2H⁺＋2e⁻	⇌	(HO₂C)₂(aq)	−0.43
鉻	Cr3+ ＋e⁻	⇌	Cr2+	−0.42
鎘	Cd2+ ＋2e⁻	⇌	Cd(s)	−0.40	[19]
硒	SeO2− 3＋4e⁻＋3H₂O	⇌	Se＋6OH⁻	−0.37	[27]
鍺	GeO 2(s)＋2H⁺＋2e⁻	⇌	GeO(s)＋H₂O	−0.37
銅	Cu 2O(s)＋H₂O＋2e⁻	⇌	2Cu(s)＋2OH⁻	−0.360	[17]
鉛	PbSO 4(s)＋2e⁻	⇌	Pb(s)＋SO2− 4	−0.3588	[17]
鉛	PbSO 4(s)＋2e⁻	⇌	Pb(Hg)＋SO2− 4	−0.3505	[17]
銪	Eu3+ ＋e⁻	⇌	Eu2+	−0.35	[21]
銦	In3+ ＋3e⁻	⇌	In(s)	−0.34	[25]
鉈	Tl+ ＋e⁻	⇌	Tl(s)	−0.34	[25]
硼	B3+ ＋3e⁻	⇌	B(s)	−0.31
鍺	Ge(s)＋4H⁺＋4e⁻	⇌	GeH 4(g)	−0.29
鈷	Co2+ ＋2e⁻	⇌	Co(s)	−0.28	[17]
磷	H 3PO 4(aq)＋2H⁺＋2e⁻	⇌	H 3PO 3(aq)＋H₂O	−0.276	[17]
釩	V3+ ＋e⁻	⇌	V2+	−0.26	[19]
鎳	Ni2+ ＋2e⁻	⇌	Ni(s)	−0.25
砷	As(s)＋3H⁺＋3e⁻	⇌	AsH 3(g)	−0.23	[25]
銀	AgI(s)＋e⁻	⇌	Ag(s)＋I−	−0.15224	[23]
鉬	MoO 2(s)＋4H⁺＋4e⁻	⇌	Mo(s)＋2H₂O	−0.15
矽	Si(s)＋4H⁺＋4e⁻	⇌	SiH 4(g)	−0.14
錫	Sn2+ ＋2e⁻	⇌	Sn(s)	−0.13
氧	O 2(g)＋H⁺＋e⁻	⇌	HO 2•(aq)	−0.13
鉛	Pb2+ ＋2e⁻	⇌	Pb(s)	−0.13	[19]
鎢	WO 2(s)＋4H⁺＋4e⁻	⇌	W(s)＋2H₂O	−0.12
磷	P（紅）＋3H⁺＋3e⁻	⇌	PH 3(g)	−0.111	[17]
碳	CO 2(g)＋2H⁺＋2e⁻	⇌	HCOOH(aq)	−0.11
硒	Se(s)＋2H⁺＋2e⁻	⇌	H 2Se(g)	−0.11
碳	CO 2(g)＋2H⁺＋2e⁻	⇌	CO(g)＋H₂O	−0.11
錫	SnO(s)＋2H⁺＋2e⁻	⇌	Sn(s)＋H₂O	−0.10
錫	SnO 2(s)＋2H⁺＋2e⁻	⇌	SnO(s)＋H₂O	−0.09
鎢	WO 3(aq)＋6H⁺＋6e⁻	⇌	W(s)＋3H₂O	−0.09	[25]
磷	P（白）＋3H⁺＋3e⁻	⇌	PH 3(g)	−0.063	[17]
氘	2D+ ＋2e⁻	⇌	D 2(g)	−0.044
鐵	Fe3+ ＋3e⁻	⇌	Fe(s)	−0.04	[24]
碳（甲酸）	HCO₂H(aq)＋2H⁺＋2e⁻	⇌	HCHO(aq)＋H₂O	−0.03
氫	2H⁺＋2e⁻	⇌	H 2(g)	−0.00	≡0
銀	AgBr(s)＋e⁻	⇌	Ag(s)＋Br⁻	+0.07133	[23]
硫	S 4O2− 6＋2e⁻	⇌	2S 2O2− 3	+0.08
鐵	Fe 3O 4(s)＋8H⁺＋8e⁻	⇌	3Fe(s)＋4H₂O	+0.085	[28]
氮	N 2(g)＋2H₂O＋6H⁺＋6e⁻	⇌	2NH 4OH(aq)	+0.092
汞	HgO(s)＋H₂O＋2e⁻	⇌	Hg(l)＋2OH⁻	+0.0977
銅	Cu(NH 3)2+ 4＋e⁻	⇌	Cu(NH 3)+ 2＋2NH 3	+0.10	[25]
釕	Ru(NH₃)₆³⁺＋e⁻	⇌	Ru(NH₃)₆²⁺	+0.10	[21]
肼	N 2H 4(aq)＋4H₂O＋2e⁻	⇌	2NH+ 4＋4OH⁻	+0.11	[16]
鉬	H 2MoO 4(aq)＋6H⁺＋6e⁻	⇌	Mo(s)＋4H₂O	+0.11
鍺	Ge4+ ＋4e⁻	⇌	Ge(s)	+0.12
碳	C(s)＋4H⁺＋4e⁻	⇌	CH 4(g)	+0.13	[25]
碳	HCHO(aq)＋2H⁺＋2e⁻	⇌	CH 3OH(aq)	+0.13
硫	S(s)＋2H⁺＋2e⁻	⇌	H 2S(g)	+0.14
錫	Sn4+ ＋2e⁻	⇌	Sn2+	+0.15
銅	Cu2+ ＋e⁻	⇌	Cu+	+0.159	[25]
硫	HSO− 4＋3H⁺＋2e⁻	⇌	SO 2(aq)＋2H₂O	+0.16
鈾	UO2+ 2＋e⁻	⇌	UO+ 2	+0.163	[21]
硫	SO2− 4＋4H⁺＋2e⁻	⇌	SO 2(aq)＋2H₂O	+0.17
鈦	TiO2+ ＋2H⁺＋e⁻	⇌	Ti3+＋H₂O	+0.19
鉍	Bi3+ ＋2e⁻	⇌	Bi+	+0.2
銻	SbO+ ＋2H⁺＋3e⁻	⇌	Sb(s)＋H₂O	+0.20
碳	CO 2(g)＋4H⁺＋4e⁻	⇌	C(s)＋2H₂O	+0.205
銀	AgCl(s)＋e⁻	⇌	Ag(s)＋Cl−	+0.22233	[23]
砷	H 3AsO 3(aq)＋3H⁺＋3e⁻	⇌	As(s)＋3H₂O	+0.24
鍺	GeO(s)＋2H⁺＋2e⁻	⇌	Ge(s)＋H₂O	+0.26
鈾	UO+ 2＋4H⁺＋e⁻	⇌	U4+ ＋2H₂O	+0.273	[21]
砹	At 2＋e⁻	⇌	2At−	+0.3	[13]
錸	Re3+ ＋3e⁻	⇌	Re(s)	+0.300
鉍	Bi3+ ＋3e⁻	⇌	Bi(s)	+0.32
釩	VO2+ ＋2H⁺＋e⁻	⇌	V3+ ＋H₂O	+0.34
銅	Cu2+ ＋2e⁻	⇌	Cu(s)	+0.340	[25]
鐵氰	[Fe(CN) 6]3− ＋e⁻	⇌	[Fe(CN)₆]₄⁻	+0.36
鎝	Tc2+ ＋2e⁻	⇌	Tc(s)	+0.40	[13]
氧	O 2(g)＋2H₂O＋4e⁻	⇌	4OH⁻(aq)	+0.40	[19]
鉬	H 2MoO 4＋6H⁺＋3e⁻	⇌	Mo3+ ＋2H₂O	+0.43
釕	Ru2+ ＋2e⁻	⇌	Ru(s)	+0.455	[13]
鉍	Bi+ ＋e⁻	⇌	Bi(s)	+0.50
碳	CH 3OH(aq)＋2H⁺＋2e⁻	⇌	CH 4(g)＋H₂O	+0.50
硫	SO 2(aq)＋4H⁺＋4e⁻	⇌	S(s)＋2H₂O	+0.50
銅	Cu+ ＋e⁻	⇌	Cu(s)	+0.520	[25]
碳	CO(g)＋2H⁺＋2e⁻	⇌	C(s)＋H₂O	+0.52
碘	I− 3＋2e⁻	⇌	3I−	+0.53	[19]
碘	I 2(s)＋2e⁻	⇌	2I−	+0.54	[19]
金	[AuI− 4]＋3e⁻	⇌	Au(s)＋4I−	+0.56
砷	H 3AsO 4(aq)＋2H⁺＋2e⁻	⇌	H 3AsO 3(aq)＋H₂O	+0.56
金	[AuI 2]− ＋e⁻	⇌	Au(s)＋2I−	+0.58
錳	MnO− 4＋2H₂O＋3e⁻	⇌	MnO 2(s)＋4OH⁻	+0.59
銠	Rh+ ＋e⁻	⇌	Rh(s)	+0.600	[13]
硫	S 2O2− 3＋6H⁺＋4e⁻	⇌	2S(s)＋3H₂O	+0.60
鐵（二茂鐵）	Fe(C 5H 5) 2＋e⁻	⇌	Fe(C 5H 5) 2(s)	+0.641	[29]
銀	CH₃CO₂Ag＋e⁻	⇌	Ag＋CH₃CO₂⁻	+0.643	[13]
鉬	H 2MoO 4(aq)＋2H⁺＋2e⁻	⇌	MoO 2(s)＋2H₂O	+0.65
苯醌	＋2H⁺＋2e⁻	⇌		+0.6992	[23]
氧	O 2(g)＋2H⁺＋2e⁻	⇌	H 2O 2(aq)	+0.70
鉈	Tl3+ ＋3e⁻	⇌	Tl(s)	+0.72
鉑氯	PtCl2− 6＋2e⁻	⇌	PtCl2− 4＋2Cl−	+0.726	[21]
硒	H 2SeO 3(aq)＋4H⁺＋4e⁻	⇌	Se(s)＋3H₂O	+0.74
銠	Rh3+ ＋3e⁻	⇌	Rh(s)	+0.758	[13]
鉑	PtCl2− 4＋2e⁻	⇌	Pt(s)＋4Cl−	+0.758	[21]
鐵	Fe3+ ＋e⁻	⇌	Fe2+	+0.77
銀	Ag+ ＋e⁻	⇌	Ag(s)	+0.7996	[17]
汞	Hg2+ 2＋2e⁻	⇌	2Hg(l)	+0.80
氮（硝）	NO− 3(aq)＋2H⁺＋e⁻	⇌	NO 2(g)＋H₂O	+0.80
鐵	FeO2− 4＋5H₂O＋6e⁻	⇌	Fe 2O 3(s)＋10OH⁻	+0.81	[24]
金	[AuBr 4]− ＋3e⁻	⇌	Au(s)＋4Br−	+0.85
汞	Hg2+ ＋2e⁻	⇌	Hg(l)	+0.85
錳	MnO− 4＋H⁺＋e⁻	⇌	HMnO− 4	+0.90
汞	2Hg2+ ＋2e⁻	⇌	Hg2+ 2	+0.91	[25]
鈀	Pd2+ ＋2e⁻	⇌	Pd(s)	+0.915	[21]
金	[AuCl 4]− ＋3e⁻	⇌	Au(s)＋4Cl−	+0.93
錳	MnO 2(s)＋4H⁺＋e⁻	⇌	Mn3+ ＋2H₂O	+0.95
金	[AuBr 2]− ＋e⁻	⇌	Au(s)＋2Br−	+0.96
氙	[HXeO 6]3− ＋2H₂O＋2e⁻	⇌	[HXeO 4]− ＋4OH⁻	+0.99	[30]
氮（硝）	HNO 2＋H⁺＋e⁻	⇌	NO(g)＋H₂O	+0.996
碲	H 6TeO 6(aq)＋2H⁺＋2e⁻	⇌	TeO 2(s)＋4H₂O	+1.02	[31]
溴	Br 2(l)＋2e⁻	⇌	2Br−	+1.065
溴	Br 2(aq)＋2e⁻	⇌	2Br−	+1.087	[19]
氮（硝）	NO 2(g)＋H⁺＋e⁻	⇌	HNO 2	+1.093
碘	IO− 3＋5H⁺＋4e⁻	⇌	HIO(aq)＋2H₂O	+1.13
	[AuCl− 2]＋e⁻	⇌	Au(s)＋2Cl−	+1.15
硒	HSeO− 4＋3H⁺＋2e⁻	⇌	H 2SeO 3(aq)＋H₂O	+1.15
銥	Ir3+ ＋3e⁻	⇌	Ir(s)	+1.156	[13]
銀	Ag 2O(s)＋2H⁺＋2e⁻	⇌	2Ag(s)＋H₂O	+1.17
氯	ClO− 3＋2H⁺＋e⁻	⇌	ClO 2(g)＋H₂O	+1.18
氙	[HXeO 6]3− ＋5H₂O＋8e⁻	⇌	Xe(g)＋11OH⁻	+1.18	[30]
鉑	Pt2+ ＋2e⁻	⇌	Pt(s)	+1.188	[21]
氯	ClO 2(g)＋H⁺＋e⁻	⇌	HClO 2(aq)	+1.19
碘	2IO− 3＋12H⁺＋10e⁻	⇌	I 2(s)＋6H₂O	+1.20
氯	ClO− 4＋2H⁺＋2e⁻	⇌	ClO− 3＋H₂O	+1.20
氧	O 2(g)＋4H⁺＋4e⁻	⇌	2H₂O	+1.229	[19]
錳	MnO 2(s)＋4H⁺＋2e⁻	⇌	Mn2+ ＋2H₂O	+1.23
氙	[HXeO 4]− ＋3H₂O＋6e⁻	⇌	Xe(g)＋7OH⁻	+1.24	[30]
鉈	Tl3+ ＋2e⁻	⇌	Tl+	+1.25
鉻	Cr 2O2− 7＋14H⁺＋6e⁻	⇌	2Cr3+ ＋7H₂O	+1.33
氯	Cl 2(g)＋2e⁻	⇌	2Cl−	+1.36	[19]
鈷	CoO 2(s)＋4H⁺＋e⁻	⇌	Co3+ ＋2H₂O	+1.42
	2NH3OH+ ＋H⁺＋2e⁻	⇌	N 2H+ 5＋2H₂O	+1.42	[16]
碘	2HIO(aq)＋2H⁺＋2e⁻	⇌	I 2(s)＋2H₂O	+1.44
鈰	Ce4+ ＋e⁻	⇌	Ce3+	+1.44
溴	BrO− 3＋5H⁺＋4e⁻	⇌	HBrO(aq)＋2H₂O	+1.45
鉛	β-PbO 2(s)＋4H⁺＋2e⁻	⇌	Pb2+ ＋2H₂O	+1.460	[25]
鉛	α-PbO 2(s)＋4H⁺＋2e⁻	⇌	Pb2+ ＋2H₂O	+1.468	[25]
溴	2BrO− 3＋12H⁺＋10e⁻	⇌	Br 2(l)＋6H₂O	+1.48
氯	2ClO− 3＋12H⁺＋10e⁻	⇌	Cl 2(g)＋6H₂O	+1.49
氧（超氧）	HO 2＋H⁺＋e⁻	⇌	H 2O 2	+1.495	[13]
錳	MnO− 4＋8H⁺＋5e⁻	⇌	Mn2+ ＋4H₂O	+1.51
	HO 2•＋H⁺＋e⁻	⇌	H 2O 2(aq)	+1.51
金	Au3+ ＋3e⁻	⇌	Au(s)	+1.52
鎳	NiO 2(s)＋4H⁺＋2e⁻	⇌	Ni2+ ＋2OH⁻	+1.59
氯	HClO(aq)＋2H⁺＋2e⁻	⇌	Cl 2(g)＋2H₂O	+1.63
銀	Ag 2O 3(s)＋6H⁺＋4e⁻	⇌	2Ag+ ＋3H₂O	+1.67
氯	HClO 2(aq)＋2H⁺＋2e⁻	⇌	HClO(aq)＋H₂O	+1.67
鉛	Pb4+ ＋2e⁻	⇌	Pb2+	+1.69	[25]
錳	MnO− 4＋4H⁺＋3e⁻	⇌	MnO 2(s)＋2H₂O	+1.70
銀	AgO(s)＋2H⁺＋e⁻	⇌	Ag+ ＋H₂O	+1.77
氧（過氧）	H 2O 2(aq)＋2H⁺＋2e⁻	⇌	2H₂O	+1.776
鈷	Co3+ ＋e⁻	⇌	Co2+	+1.82
金	Au+ ＋e⁻	⇌	Au(s)	+1.83	[25]
溴	BrO− 4＋2H⁺＋2e⁻	⇌	BrO− 3＋H₂O	+1.85
銀	Ag2+ ＋e⁻	⇌	Ag+	+1.98	[25]
氧（過氧）	S 2O2− 8＋2e⁻	⇌	2SO2− 4	+2.07
氧	O 3(g)＋2H⁺＋2e⁻	⇌	O 2(g)＋H₂O	+2.075	[21]
錳	HMnO− 4＋3H⁺＋2e⁻	⇌	MnO 2(s)＋2H₂O	+2.09
氙	XeO 3(aq)＋6H⁺＋6e⁻	⇌	Xe(g)＋3H₂O	+2.12	[30]
氧（氟氧）	OF₂＋2H⁺＋4e⁻	⇌	2F− ＋H₂O	+2.153	[13]
氙	H 4XeO 6(aq)＋8H⁺＋8e⁻	⇌	Xe(g)＋6H₂O	+2.18	[30]
鐵	FeO2− 4＋8H⁺＋3e⁻	⇌	Fe3+ ＋4H₂O	+2.20	[32]
氙	XeF 2(aq)＋2H⁺＋2e⁻	⇌	Xe(g)＋2HF(aq)	+2.32	[30]
氙	H 4XeO 6(aq)＋2H⁺＋2e⁻	⇌	XeO 3(aq)＋H₂O	+2.42	[30]
氟	F 2(g)＋2e⁻	⇌	2F−	+2.87	[25][19]
氟	F 2(g)＋2H⁺＋2e⁻	⇌	2HF(aq)	+3.05	[25]
鋱	Tb4+ ＋e⁻	⇌	Tb3+	+3.05	[13]

1. 在Safari的v.4.0.3或更早版本（v4.0.5可正常工作）上單擊這一列可能不會工作。在這種情況下僅僅需要刷新頁面恢復原始順序。

參見

• 標準電極電勢
• 金屬活動性
• 元素活性

參考資料

1. Milazzo, G., Caroli, S., and Sharma, V. K. (1978). Tables of Standard Electrode Potentials (Wiley, Chichester).
2. Bard, A. J., Parsons, R., and Jordan, J. (1985). Standard Potentials in Aqueous Solutions (Marcel Dekker, New York).
3. Bratsch, S. G. (1989). Journal of Physical Chemistry Reference Data Vol. 18, pp. 1–21.
4. Vanýsek, Petr (2006). "Electrochemical Series," in Handbook of Chemistry and Physics: 87^th Edition （頁面存檔備份，存於互聯網檔案館） (Chemical Rubber Company).
5. Vanýsek, Petr (2007). 「Electrochemical Series」 （頁面存檔備份，存於互聯網檔案館）, in Handbook of Chemistry and Physics: 88^th Edition （頁面存檔備份，存於互聯網檔案館） (Chemical Rubber Company).
6. Greenwood, N. N.; Earnshaw, A. Chemistry of the Elements 2nd. Oxford:Butterworth-Heinemann. 1997. ISBN 0-7506-3365-4.
7. Bard, A.J., Faulkner, L.R.(2001). Electrochemical Methods. Fundamentals and Applications, 2nd edition (John Wiley and Sons Inc).
8. Marcel Pourbaix (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions (NACE International, Houston, Texas; Cebelcor, Brussels).
9. Peter Atkins (1997). Physical Chemistry, 6th edition (W.H. Freeman and Company, New York).
10. Milazzo, G., Caroli, S., and Sharma, V. K. (1978). Tables of Standard Electrode Potentials (Wiley, Chichester).
11. Bratsch, S. G. (1989). Journal of Physical Chemistry Reference Data Vol. 18, pp. 1–21.
12. Ca Sr Ba一價^[11]與兩價間的標準電極電勢正好有規律關係，因此可以估計近似值
13. Standard Redox Potential Table. [2012-01-14]. （原始內容存檔於2021-02-06）.
14. Lide, David R. (編), CRC Handbook of Chemistry and Physics 87th, Boca Raton, FL: CRC Press, 2006, ISBN 0-8493-0487-3
15. Greenwood and Earnshaw, p. 1263
16. Greenwood, N. N.; Earnshaw, A. Chemistry of the Elements 2nd. Oxford:Butterworth-Heinemann. 1997. ISBN 0-7506-3365-4.
17. Vanýsek, Petr (2007). 「Electrochemical Series」 （頁面存檔備份，存於互聯網檔案館）, in Handbook of Chemistry and Physics: 88^th Edition （頁面存檔備份，存於互聯網檔案館） (Chemical Rubber Company).
18. Vanýsek, Petr (2006). "Electrochemical Series," in Handbook of Chemistry and Physics: 87^th Edition （頁面存檔備份，存於互聯網檔案館） (Chemical Rubber Company).
19. Peter Atkins (1997). Physical Chemistry, 6th edition (W.H. Freeman and Company, New York).
20. Ti Zr Hf 的標準電極電勢變化較規律，因此可估計 Rf的標準電極電勢
21. Bard, A.J., Faulkner, L.R.(2001). Electrochemical Methods. Fundamentals and Applications, 2nd edition (John Wiley and Sons Inc).
22. Gordon Aylward & Tristan Findlay (2008). "SI Chemical Data", 6th edition (John Wiley & Sons, Australia), ISBN 9780470816387.
23. Vanýsek, Petr (2007). 「Electrochemical Series」, in Handbook of Chemistry and Physics: 88th Edition (Chemical Rubber Company).
24. WebElements Periodic Table of the Elements | Iron | compounds information. [2012-01-14]. （原始內容存檔於2021-01-18）.
25. Bard, A. J., Parsons, R., and Jordan, J. (1985). Standard Potentials in Aqueous Solutions (Marcel Dekker, New York).
26. 由−0.454和(2×−0.499＋−0.508)÷3＝−0.502推算出。
27. 「Glyoxal Bisulfite」 （頁面存檔備份，存於互聯網檔案館）, Organic Syntheses, Collected Volume 3, p.438 (1955).
28. Marcel Pourbaix (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions (NACE International, Houston, Texas; Cebelcor, Brussels).
29. Connelly, Neil G.; Geiger, William E. Chemical Redox Agents for Organometallic Chemistry. Chemical Reviews. 1 January 1996, 96 (2): 877–910. PMID 11848774. doi:10.1021/cr940053x. 引文使用過時參數coauthors (幫助)
30. WebElements Periodic Table of the Elements | Xenon | compounds information. [2012-01-14]. （原始內容存檔於2021-03-22）.
31. Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred, Advanced Inorganic Chemistry 6th, New York: Wiley-Interscience, 1999, ISBN 0-471-19957-5
32. Redox Reactions, Western Oregon University website. [2012-01-15]. （原始內容存檔於2019-08-30）.

• Standard Reduction Potentials （頁面存檔備份，存於互聯網檔案館）
• Standard Electrode Potentials in Aqueous Solution at 25°C （頁面存檔備份，存於互聯網檔案館）