标准电极电势表
维基百科，自由的百科全书
标准电极电势可以用来计算化学电池或原电池的电化学势或电极电势。本表中所给出的电极电势以标准氢电极为参比电极，溶液中离子有效浓度为1mol/L，气体分压为100kPa，温度为298K，所有离子的数据都在水溶液中测得。[1][2][3][4][5][6][7][8][9]单击每栏上方的符号可将数据按元素符号或标准电极电势值排序。
注：(s) – 固体；(l) – 液体；(g) – 气体；(aq) – 水溶液；(Hg) – 汞齐。
| 半反應 | E° (V)[註 1] | 来源 |
|---|---|---|
Ba+ + e−  Ba(s) |
−4.38 | [10][1][3] |
| Sr+ + e− Sr(s) |
−4.10 | [11][1][3] |
| Ca+ + e− Ca(s) |
−3.8 | [11][1][3] |
| Pr3+ + e− Pr2+ |
−3.1 | [11] |
 N2(g) + H+ + e− HN3(aq) |
−3.09 | [6] |
| Li+ + e− Li(s) |
−3.0401 | [5] |
| N2(g) + 4 H2O + 2 e− 2 NH2OH(aq) + 2 OH− |
−3.04 | [6] |
| Cs+ + e− Cs(s) |
−3.026 | [5] |
| Ca(OH)2(s) + 2 e− Ca(s) + 2 OH− |
−3.02 | [11] |
| Rb+ + e− Rb(s) |
−2.98 | [4] |
| K+ + e− K(s) |
−2.931 | [5] |
| Mg+ + e− Mg(s) |
−2.93 | [10] |
| Ba2+ + 2 e− Ba(s) |
−2.912 | [5] |
| La(OH)3(s) + 3 e− La(s) + 3OH− |
−2.90 | [5] |
| Fr+ + e− Fr(s) |
−2.9 | [11] |
| Sr2+ + 2 e− Sr(s) |
−2.899 | [5] |
| Sr(OH)2(s) + 2 e− Sr(s) + 2 OH− |
−2.88 | [11] |
| Ca2+ + 2 e− Ca(s) |
−2.868 | [5] |
| Eu2+ + 2 e− Eu(s) |
−2.812 | [5] |
| Ra2+ + 2 e− Ra(s) |
−2.8 | [5] |
| Yb2+ + 2 e− Yb(s) |
−2.76 | [11][1] |
| Na+ + e− Na(s) |
−2.71 | [5][9] |
| Sm2+ + 2 e− Sm(s) |
−2.68 | [11][1] |
| No2+ + 2 e− No(s) |
−2.50 | [11] |
| HfO(OH)2(s) + H2O + 4 e− Hf(s) + 4 OH− |
−2.50 | [11] |
| Th(OH)4(s) + 4 e− Th(s) + 4 OH− |
−2.48 | [11] |
| Md2+ + 2 e− Md(s) |
−2.40 | [11] |
| La3+ + 3 e− La(s) |
−2.379 | [5] |
| Y3+ + 3 e− Y(s) |
−2.372 | [5] |
| Mg2+ + 2 e− Mg(s) |
−2.372 | [5] |
| ZrO(OH)2(s) + H2O + 4 e− Zr(s) + 4OH− |
−2.36 | [5] |
| Pr3+ + 3 e− Pr(s) |
−2.353 | [11] |
| Ce3+ + 3 e− Ce(s) |
−2.336 | [11] |
| Er3+ + 3 e− Er(s) |
−2.331 | [11] |
| Ho3+ + 3 e− Ho(s) |
−2.33 | [11] |
| Al(OH)4− + 3 e− Al(s) + 4 OH− |
−2.33 | |
| Al(OH)3(s) + 3 e− Al(s) + 3OH− |
−2.31 | |
| Tb3+ + 3 e− Tb(s) |
−2.28 | |
| H2(g) + 2 e− 2 H− |
−2.25 | |
| Ac3+ + 3 e− Ac(s) |
−2.20 | |
| Be+ + e− Be(s) |
−2.12 | [10] |
| Cf2+ + 2 e− Cf(s) |
−2.12 | [11] |
| Am3+ + 3 e− Am(s) |
−2.048 | [11] |
| Cf3+ + 3 e− Cf(s) |
−1.94 | [11] |
| Am2+ + 2 e− Am(s) |
−1.9 | [11] |
| Be2+ + 2 e− Be(s) |
−1.85 | |
| Rf4+ + 4 e− Rf(s) |
−1.67 | [12] |
| U3+ + 3 e− U(s) |
−1.66 | [7] |
| Al3+ + 3 e− Al(s) |
−1.66 | [9] |
| Ti2+ + 2 e− Ti(s) |
−1.63 | [9] |
| Bk2+ + 2 e− Bk(s) |
−1.6 | [11] |
| ZrO2(s) + 4 H+ + 4 e− Zr(s) + 2 H2O |
−1.553 | [5] |
| Hf4+ + 4 e− Hf(s) |
−1.55 | [11] |
| Zr4+ + 4 e− Zr(s) |
−1.45 | [5] |
| Ti3+ + 3 e− Ti(s) |
−1.37 | [13] |
| TiO(s) + 2 H+ + 2 e− Ti(s) + H2O |
−1.31 | |
| Ti2O3(s) + 2 H+ + 2 e− 2 TiO(s) + H2O |
−1.23 | |
| Zn(OH)42− + 2 e− Zn(s) + 4 OH− |
−1.199 | [14] |
| Mn2+ + 2 e− Mn(s) |
−1.185 | [14] |
| Fe(CN)64− + 6 H+ + 2 e− Fe(s) + 4HCN(aq) |
−1.16 | [15] |
| V2+ + 2 e− V(s) |
−1.175 | [2] |
| Te(s) + 2 e− Te2− |
−1.143 | [2] |
| Nb3+ + 3 e− Nb(s) |
−1.099 | |
| Sn(s) + 4 H+ + 4 e− SnH4(g) |
−1.07 | |
| In(OH)3(s) + 3 e− In(s) + 3 OH− |
−0.99 | [11] |
| SiO2(s) + 4 H+ + 4 e− Si(s) + 2 H2O |
−0.91 | |
| B(OH)3(aq) + 3 H+ + 3 e− B(s) + 3 H2O |
−0.89 | |
| Fe(OH)2(s) + 2 e− Fe(s) + 2 OH− |
−0.89 | [15] |
| Fe2O3(s) + 3 H2O + 2 e− 2Fe(OH)2(s) + 2 OH− |
−0.86 | [15] |
| TiO2+ + 2 H+ + 4 e− Ti(s) + H2O |
−0.86 | |
| 2 H2O + 2 e− H2(g) + 2 OH− |
−0.8277 | [5] |
| Bi(s) + 3 H+ + 3 e− BiH3 |
−0.8 | [14] |
| Zn2+ + 2 e− Zn(Hg) |
−0.7628 | [5] |
| Zn2+ + 2 e− Zn(s) |
−0.7618 | [5] |
| Ta2O5(s) + 10 H+ + 10 e− 2 Ta(s) + 5 H2O |
−0.75 | |
| Cr3+ + 3 e− Cr(s) |
−0.74 | |
| [Au(CN)2]− + e− Au(s) + 2 CN− |
−0.60 | |
| Ta3+ + 3 e− Ta(s) |
−0.6 | |
| PbO(s) + H2O + 2 e− Pb(s) + 2 OH− |
−0.58 | |
| 2 TiO2(s) + 2 H+ + 2 e− Ti2O3(s) + H2O |
−0.56 | |
| Ga3+ + 3 e− Ga(s) |
−0.53 | |
| U4+ + e− U3+ |
−0.52 | [7] |
| H3PO2(aq) + H+ + e− P(白磷[16]) + 2 H2O |
−0.508 | [5] |
| H3PO3(aq) + 2 H+ + 2 e− H3PO2(aq) + H2O |
−0.499 | [5] |
| H3PO3(aq) + 3 H+ + 3 e− P(红磷)[16] + 3H2O |
−0.454 | [5] |
| Fe2+ + 2 e− Fe(s) |
−0.44 | [9] |
| 2 CO2(g) + 2 H+ + 2 e− HOOCCOOH(aq) |
−0.43 | |
| Cr3+ + e− Cr2+ |
−0.42 | |
| Cd2+ + 2 e− Cd(s) |
−0.40 | [9] |
| SeO32− + 4e− + 3H2O ⇌ Se + 6OH− | −0.37 | [17] |
| GeO2(s) + 2 H+ + 2 e− GeO(s) + H2O |
−0.37 | |
| Cu2O(s) + H2O + 2 e− 2 Cu(s) + 2 OH− |
−0.360 | [5] |
| PbSO4(s) + 2 e− Pb(s) + SO42− |
−0.3588 | [5] |
| PbSO4(s) + 2 e− Pb(Hg) + SO42− |
−0.3505 | [5] |
| Eu3+ + e− Eu2+ |
−0.35 | [7] |
| In3+ + 3 e− In(s) |
−0.34 | [2] |
| Tl+ + e− Tl(s) |
−0.34 | [2] |
| Ge(s) + 4 H+ + 4 e− GeH4(g) |
−0.29 | |
| Co2+ + 2 e− Co(s) |
−0.28 | [5] |
| H3PO4(aq) + 2 H+ + 2 e− H3PO3(aq) + H2O |
−0.276 | [5] |
| V3+ + e− V2+ |
−0.26 | [9] |
| Ni2+ + 2 e− Ni(s) |
−0.25 | |
| As(s) + 3 H+ + 3 e− AsH3(g) |
−0.23 | [2] |
| AgI(s) + e− Ag(s) + I− |
−0.15224 | [14] |
| MoO2(s) + 4 H+ + 4 e− Mo(s) + 2 H2O |
−0.15 | |
| Si(s) + 4 H+ + 4 e− SiH4(g) |
−0.14 | |
| Sn2+ + 2 e− Sn(s) |
−0.13 | |
| O2(g) + H+ + e− HO2•(aq) |
−0.13 | |
| Pb2+ + 2 e− Pb(s) |
−0.13 | [9] |
| WO2(s) + 4 H+ + 4 e− W(s) + 2 H2O |
−0.12 | |
| P(红磷) + 3 H+ + 3 e− PH3(g) |
−0.111 | [5] |
| CO2(g) + 2 H+ + 2 e− HCOOH(aq) |
−0.11 | |
| Se(s) + 2 H+ + 2 e− H2Se(g) |
−0.11 | |
| CO2(g) + 2 H+ + 2 e− CO(g) + H2O |
−0.11 | |
| SnO(s) + 2 H+ + 2 e− Sn(s) + H2O |
−0.10 | |
| SnO2(s) + 2 H+ + 2 e− SnO(s) + H2O |
−0.09 | |
| WO3(aq) + 6 H+ + 6 e− W(s) + 3 H2O |
−0.09 | [2] |
| P(白磷) + 3 H+ + 3 e− PH3(g) |
−0.063 | [5] |
| Fe3+ + 3 e− Fe(s) |
−0.04 | [15] |
| HCOOH(aq) + 2 H+ + 2 e− HCHO(aq) + H2O |
−0.03 | |
| 2 H+ + 2 e− H2(g) |
−0.00 | ≡ 0 |
| AgBr(s) + e− Ag(s) + Br− |
+0.07133 | [14] |
| S4O62− + 2 e− 2 S2O32− |
+0.08 | |
| Fe3O4(s) + 8 H+ + 8 e− 3 Fe(s) + 4 H2O |
+0.085 | [8] |
| N2(g) + 2 H2O + 6H+ + 6 e− 2 NH4OH(aq) |
+0.092 | |
| HgO(s) + H2O + 2 e− Hg(l) + 2 OH− |
+0.0977 | |
| Cu(NH3)42+ + e− Cu(NH3)2+ + 2 NH3 |
+0.10 | [2] |
| Ru(NH3)63+ + e− Ru(NH3)62+ |
+0.10 | [7] |
| N2H4(aq) + 4 H2O + 2 e− 2 NH4+ + 4 OH− |
+0.11 | [6] |
| H2MoO4(aq) + 6 H+ + 6 e− Mo(s) + 4 H2O |
+0.11 | |
| Ge4+ + 4 e− Ge(s) |
+0.12 | |
| C(s) + 4 H+ + 4 e− CH4(g) |
+0.13 | [2] |
| HCHO(aq) + 2 H+ + 2 e− CH3OH(aq) |
+0.13 | |
| S(s) + 2 H+ + 2 e− H2S(g) |
+0.14 | |
| Sn4+ + 2 e− Sn2+ |
+0.15 | |
| Cu2+ + e− Cu+ |
+0.159 | [2] |
| HSO4− + 3 H+ + 2 e− SO2(aq) + 2 H2O |
+0.16 | |
| UO22+ + e− UO2+ |
+0.163 | [7] |
| SO42− + 4 H+ + 2 e− SO2(aq) + 2 H2O |
+0.17 | |
| TiO2+ + 2 H+ + e− Ti3+ + H2O |
+0.19 | |
| Bi3+ + 2e− Bi+ |
+0.2 | |
| SbO+ + 2 H+ + 3 e− Sb(s) + H2O |
+0.20 | |
| AgCl(s) + e− Ag(s) + Cl− |
+0.22233 | [14] |
| H3AsO3(aq) + 3 H+ + 3 e− As(s) + 3 H2O |
+0.24 | |
| GeO(s) + 2 H+ + 2 e− Ge(s) + H2O |
+0.26 | |
| UO2+ + 4 H+ + e− U4+ + 2 H2O |
+0.273 | [7] |
| At2 + e− 2 At- |
+0.3 | [11] |
| Re3+ + 3 e− Re(s) |
+0.300 | |
| Bi3+ + 3 e− Bi(s) |
+0.32 | |
| VO2+ + 2 H+ + e− V3+ + H2O |
+0.34 | |
| Cu2+ + 2 e− Cu(s) |
+0.340 | [2] |
| [Fe(CN)6]3− + e− [Fe(CN)6]4− |
+0.36 | |
| Tc2+ + 2 e− Tc(s) |
+0.40 | [11] |
| O2(g) + 2 H2O + 4 e− 4 OH−(aq) |
+0.40 | [9] |
| H2MoO4 + 6 H+ + 3 e− Mo3+ + 2 H2O |
+0.43 | |
| Ru2+ + 2 e− Ru(s) |
+0.455 | [11] |
| Bi+ + e− Bi(s) |
+0.50 | |
| CH3OH(aq) + 2 H+ + 2 e− CH4(g) + H2O |
+0.50 | |
| SO2(aq) + 4 H+ + 4 e− S(s) + 2 H2O |
+0.50 | |
| Cu+ + e− Cu(s) |
+0.520 | [2] |
| CO(g) + 2 H+ + 2 e− C(s) + H2O |
+0.52 | |
| I3− + 2 e− 3 I− |
+0.53 | [9] |
| I2(s) + 2 e− 2 I− |
+0.54 | [9] |
| [AuI4]− + 3 e− Au(s) + 4 I− |
+0.56 | |
| H3AsO4(aq) + 2 H+ + 2 e− H3AsO3(aq) + H2O |
+0.56 | |
| [AuI2]− + e− Au(s) + 2 I− |
+0.58 | |
| MnO4− + 2 H2O + 3 e− MnO2(s) + 4 OH− |
+0.59 | |
| Rh+ + e− Rh(s) |
+0.600 | [11] |
| S2O32 − + 6 H+ + 4 e− 2 S(s) + 3 H2O |
+0.60 | |
| Fc+ + e− Fc(s) |
+0.641 | [18] |
   + e− Ag + − |
+0.643 | [11] |
| H2MoO4(aq) + 2 H+ + 2 e− MoO2(s) + 2 H2O |
+0.65 | |
 + 2 H+ + 2 e−  |
+0.6992 | [14] |
| O2(g) + 2 H+ + 2 e− H2O2(aq) |
+0.70 | |
| Tl3+ + 3 e− Tl(s) |
+0.72 | |
| PtCl62− + 2 e− PtCl42− + 2 Cl− |
+0.726 | [7] |
| H2SeO3(aq) + 4 H+ + 4 e− Se(s) + 3 H2O |
+0.74 | |
| Rh3+ + 3 e− Rh(s) |
+0.758 | [11] |
| PtCl42− + 2 e− Pt(s) + 4 Cl− |
+0.758 | [7] |
| Fe3+ + e− Fe2+ |
+0.77 | |
| Ag+ + e− Ag(s) |
+0.7996 | [5] |
| Hg22+ + 2 e− 2 Hg(l) |
+0.80 | |
| NO3−(aq) + 2 H+ + e− NO2(g) + H2O |
+0.80 | |
| FeO42− + 5 H2O + 6 e− Fe2O3(s) + 10 OH− |
+0.81 | [15] |
| H2(g) + 2 OH− 2 H2O + 2 e− |
+0.828 | [19] |
| [AuBr4]− + 3 e− Au(s) + 4 Br− |
+0.85 | |
| Hg2+ + 2 e− Hg(l) |
+0.85 | |
| MnO4− + H+ + e− HMnO4− |
+0.90 | |
| 2 Hg2+ + 2 e− Hg22+ |
+0.91 | [2] |
| Pd2+ + 2 e− Pd(s) |
+0.915 | [7] |
| [AuCl4]− + 3 e− Au(s) + 4 Cl− |
+0.93 | |
| MnO2(s) + 4 H+ + e− Mn3+ + 2 H2O |
+0.95 | |
| [AuBr2]− + e− Au(s) + 2 Br− |
+0.96 | |
| [HXeO6]3− + 2 H2O + 2 e− + [HXeO4]− + 4 OH− |
+0.99 | [20] |
| HNO2 + H+ + e- = NO(g) + H2O | +0.996 | |
| H6TeO6(aq) + 2 H+ + 2 e− TeO2(s) + 4 H2O |
+1.02 | [21] |
| Br2(l) + 2 e− 2 Br− |
+1.07 | |
| Br2(aq) + 2 e− 2 Br− |
+1.09 | [9] |
| NO2(g) + H+ + e- = HNO2 | +1.093 | |
| IO3− + 5 H+ + 4 e− HIO(aq) + 2 H2O |
+1.13 | |
| [AuCl2]− + e− Au(s) + 2 Cl− |
+1.15 | |
| HSeO4− + 3 H+ + 2 e− H2SeO3(aq) + H2O |
+1.15 | |
| Ir3+ + 3 e− Ir(s) |
+1.156 | [11] |
| Ag2O(s) + 2 H+ + 2 e− 2 Ag(s) + H2O |
+1.17 | |
| ClO3− + 2 H+ + e− ClO2(g) + H2O |
+1.18 | |
| [HXeO6]3− + 5 H2O + 8 e− Xe(g) + 11 OH− |
+1.18 | [20] |
| Pt2+ + 2 e− Pt(s) |
+1.188 | [7] |
| ClO2(g) + H+ + e− HClO2(aq) |
+1.19 | |
| 2 IO3− + 12 H+ + 10 e− I2(s) + 6 H2O |
+1.20 | |
| ClO4− + 2 H+ + 2 e− ClO3− + H2O |
+1.20 | |
| O2(g) + 4 H+ + 4 e− 2 H2O |
+1.229 | [9] |
| MnO2(s) + 4 H+ + 2 e− Mn2+ + 2H2O |
+1.23 | |
| [HXeO4]− + 3 H2O + 6 e− Xe(g) + 7 OH− |
+1.24 | [20] |
| Tl3+ + 2 e− Tl+ |
+1.25 | |
| Cr2O72 − + 14 H+ + 6 e− 2 Cr3+ + 7 H2O |
+1.33 | |
| Cl2(g) + 2 e− 2 Cl− |
+1.36 | [9] |
| CoO2(s) + 4 H+ + e− Co3+ + 2 H2O |
+1.42 | |
| 2 NH3OH+ + H+ + 2 e− N2H5+ + 2 H2O |
+1.42 | [6] |
| 2 HIO(aq) + 2 H+ + 2 e− I2(s) + 2 H2O |
+1.44 | |
| Ce4+ + e− Ce3+ |
+1.44 | |
| BrO3− + 5 H+ + 4 e− HBrO(aq) + 2 H2O |
+1.45 | |
| β-PbO2(s) + 4 H+ + 2 e− Pb2+ + 2 H2O |
+1.460 | [2] |
| α-PbO2(s) + 4 H+ + 2 e− Pb2+ + 2 H2O |
+1.468 | [2] |
| 2 BrO3− + 12 H+ + 10 e− Br2(l) + 6 H2O |
+1.48 | |
| 2ClO3− + 12 H+ + 10 e− Cl2(g) + 6 H2O |
+1.49 | |
| HO2 + H+ + e− H2O2 |
+1.495 | [11] |
| MnO4− + 8 H+ + 5 e− Mn2+ + 4 H2O |
+1.51 | |
| HO2• + H+ + e− H2O2(aq) |
+1.51 | |
| Au3+ + 3 e− Au(s) |
+1.52 | |
| NiO2(s) + 4 H+ + 2 e− Ni2+ + 2 OH− |
+1.59 | |
| 2 HClO(aq) + 2 H+ + 2 e− Cl2(g) + 2 H2O |
+1.63 | |
| Ag2O3(s) + 6 H+ + 4 e− 2 Ag+ + 3 H2O |
+1.67 | |
| HClO2(aq) + 2 H+ + 2 e− HClO(aq) + H2O |
+1.67 | |
| Pb4+ + 2 e− Pb2+ |
+1.69 | [2] |
| MnO4− + 4 H+ + 3 e− MnO2(s) + 2 H2O |
+1.70 | |
| AgO(s) + 2 H+ + e− Ag+ + H2O |
+1.77 | |
| H2O2(aq) + 2 H+ + 2 e− 2 H2O |
+1.776 | |
| Co3+ + e− Co2+ |
+1.82 | |
| Au+ + e− Au(s) |
+1.83 | [2] |
| BrO4− + 2 H+ + 2 e− BrO3− + H2O |
+1.85 | |
| Ag2+ + e− Ag+ |
+1.98 | [2] |
| S2O82− + 2 e− 2 SO42− |
+2.07 | |
| O3(g) + 2 H+ + 2 e− O2(g) + H2O |
+2.075 | [7] |
| HMnO4− + 3 H+ + 2 e− MnO2(s) + 2 H2O |
+2.09 | |
| XeO3(aq) + 6 H+ + 6 e− Xe(g) + 3 H2O |
+2.12 | [20] |
| H4XeO6(aq) + 8 H+ + 8 e− Xe(g) + 6 H2O |
+2.18 | [20] |
| FeO42− + 3 e− + 8 H+ Fe3+ + 4 H2O |
+2.20 | [22] |
| XeF2(aq) + 2 H+ + 2 e− Xe(g) + 2HF(aq) |
+2.32 | [20] |
| H4XeO6(aq) + 2 H+ + 2 e− XeO3(aq) + H2O |
+2.42 | [20] |
| F2(g) + 2 e− 2 F− |
+2.87 | [2][9] |
| F2(g) + 2 H+ + 2 e− 2 HF(aq) |
+3.05 | [2] |
| Tb4+ + e− Tb3+ |
+3.05 | [11] |
参考资料 [编辑]
- ^ 1.0 1.1 1.2 1.3 1.4 1.5 Milazzo, G., Caroli, S., and Sharma, V. K. (1978). Tables of Standard Electrode Potentials (Wiley, Chichester).
- ^ 2.00 2.01 2.02 2.03 2.04 2.05 2.06 2.07 2.08 2.09 2.10 2.11 2.12 2.13 2.14 2.15 2.16 2.17 2.18 2.19 Bard, A. J., Parsons, R., and Jordan, J. (1985). Standard Potentials in Aqueous Solutions (Marcel Dekker, New York).
- ^ 3.0 3.1 3.2 3.3 Bratsch, S. G. (1989). Journal of Physical Chemistry Reference Data Vol. 18, pp. 1–21.
- ^ 4.0 4.1 Vanýsek, Petr (2006). "Electrochemical Series," in Handbook of Chemistry and Physics: 87th Edition (Chemical Rubber Company).
- ^ 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 5.17 5.18 5.19 5.20 5.21 5.22 5.23 5.24 5.25 5.26 5.27 5.28 5.29 5.30 Vanýsek, Petr (2007). “Electrochemical Series”, in Handbook of Chemistry and Physics: 88th Edition (Chemical Rubber Company).
- ^ 6.0 6.1 6.2 6.3 6.4 Greenwood, N. N.; Earnshaw, A. Chemistry of the Elements 2nd Edition. Oxford:Butterworth-Heinemann. 1997. ISBN 0-7506-3365-4.
- ^ 7.00 7.01 7.02 7.03 7.04 7.05 7.06 7.07 7.08 7.09 7.10 7.11 Bard, A.J., Faulkner, L.R.(2001). Electrochemical Methods. Fundamentals and Applications, 2nd edition (John Wiley and Sons Inc).
- ^ 8.0 8.1 Marcel Pourbaix (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions (NACE International, Houston, Texas; Cebelcor, Brussels).
- ^ 9.00 9.01 9.02 9.03 9.04 9.05 9.06 9.07 9.08 9.09 9.10 9.11 9.12 9.13 9.14 Peter Atkins (1997). Physical Chemistry, 6th edition (W.H. Freeman and Company, New York).
- ^ 10.0 10.1 10.2 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
- ^ 11.00 11.01 11.02 11.03 11.04 11.05 11.06 11.07 11.08 11.09 11.10 11.11 11.12 11.13 11.14 11.15 11.16 11.17 11.18 11.19 11.20 11.21 11.22 11.23 11.24 11.25 11.26 11.27 11.28 11.29 11.30 11.31 Standard Redox Potential Table
- ^ 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
- ^ Gordon Aylward & Tristan Findlay (2008). "SI Chemical Data", 6th edition (John Wiley & Sons, Australia), ISBN 9780470816387.
- ^ 14.0 14.1 14.2 14.3 14.4 14.5 14.6 Vanýsek, Petr (2007). “Electrochemical Series”, in Handbook of Chemistry and Physics: 88th Edition (Chemical Rubber Company).
- ^ 15.0 15.1 15.2 15.3 15.4 WebElements Periodic Table of the Elements | Iron | compounds information
- ^ 16.0 16.1 由−0.454和(2×−0.499 + −0.508) ÷ 3 = −0.502推算出。
- ^ “Glyoxal Bisulfite”, Organic Syntheses, Collected Volume 3, p.438 (1955).
- ^ Connelly, Neil G.; Geiger, William E. Chemical Redox Agents for Organometallic Chemistry. Chemical Reviews. 1 January 1996, 96 (2): 877–910. doi:10.1021/cr940053x. PMID 11848774.
- ^ WebElements Periodic Table of the Elements | Hydrogen | compounds information
- ^ 20.0 20.1 20.2 20.3 20.4 20.5 20.6 WebElements Periodic Table of the Elements | Xenon | compounds information
- ^ Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred, Advanced Inorganic Chemistry. 6th, New York: Wiley-Interscience. 1999, ISBN 0-471-19957-5
- ^ Redox Reactions, Western Oregon University website
