标准电极电势表
标准电极电位是以标准氢原子作为参比电极，即氢的标准电极电位值定为0，与氢标准电极比较，电位较高的为正，电位较低者为负。
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以下條件測得：
- 溫度在298.15K下，即攝氏25度。
- 在水溶液或汞齊中離子的有效濃度為1mol/L。
- 氣體反應物的分壓為大氣壓（1013.25百帕）
- 以标准氢电极为参比电极，所有离子的数据都在水溶液中测得。[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。
单击每栏上方的符号可将数据按元素符号、反應物、產物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] | |||
|---|---|---|---|---|
| 氧化劑 | ⇌ | 還原劑 | ||
| 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] |
| Er3+ + e− | ⇌ | Er2+ | −3.0 | [11] |
| Ba(OH)2(s) + 2 e− | ⇌ | Ba(s) + 2 OH− | −2.99 | [11] |
| Rb+ + e− | ⇌ | Rb(s) | −2.98 | [4] |
| K+ + e− | ⇌ | K(s) | −2.92 | [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] |
| NH4+ + e− | ⇌ | NH4• | −2.85 | |
| 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] |
| Ca2+ + e− | ⇌ | Ca+ | −1.936 | [5][11] |
| Am2+ + 2 e− | ⇌ | Am(s) | −1.9 | [11] |
| Fm3+ + 3 e− | ⇌ | Fm(s) | −1.89 | [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 | |
| C4+ + 4 e− | ⇌ | C | −1.3 | [14] |
| Ti2O3(s) + 2 H+ + 2 e− | ⇌ | 2 TiO(s) + H2O | −1.23 | |
| Zn(OH)42− + 2 e− | ⇌ | Zn(s) + 4 OH− | −1.199 | [15] |
| Mn2+ + 2 e− | ⇌ | Mn(s) | −1.185 | [15] |
| Fe(CN)64− + 6 H+ + 2 e− | ⇌ | Fe(s) + 4HCN(aq) | −1.16 | [16] |
| 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 | [16] |
| Fe2O3(s) + 3 H2O + 2 e− | ⇌ | 2Fe(OH)2(s) + 2 OH− | −0.86 | [16] |
| 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 | [15] |
| 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[17]) + 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)[17] + 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 | [18] |
| 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] |
| NAD(P)+ + H+ + 2e− | ⇌ | NAD(P)H | −0.32 | [19] |
| B3+ + 3e− | ⇌ | B(s) | −0.31 | |
| 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 | [15] |
| 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] |
| 2D+ + 2 e− | ⇌ | D2(g) | −0.044 | |
| Fe3+ + 3 e− | ⇌ | Fe(s) | −0.04 | [16] |
| 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 | [15] |
| 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 | |
| CO2(g) + 4 H+ + 4 e− | ⇌ | C(s) + 2 H2O | +0.205 | |
| AgCl(s) + e− | ⇌ | Ag(s) + Cl− | +0.22233 | [15] |
| 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 | [20] |
| + e− | ⇌ | Ag + | +0.643 | [11] |
| H2MoO4(aq) + 2 H+ + 2 e− | ⇌ | MoO2(s) + 2 H2O | +0.65 | |
 + 2 H+ + 2 e− |
⇌ |  |
+0.6992 | [15] |
| 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 | [16] |
| [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 | [21] |
| HNO2 + H+ + e- | ⇌ | NO(g) + H2O | +0.996 | |
| H6TeO6(aq) + 2 H+ + 2 e− | ⇌ | TeO2(s) + 4 H2O | +1.02 | [22] |
| 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 | [21] |
| 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 | [21] |
| 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 | [21] |
| F2O + 2 H+ + 4 e− | ⇌ | 2F− + H2O | +2.153 | [11] |
| H4XeO6(aq) + 8 H+ + 8 e− | ⇌ | Xe(g) + 6 H2O | +2.18 | [21] |
| FeO42− + 3 e− + 8 H+ | ⇌ | Fe3+ + 4 H2O | +2.20 | [23] |
| XeF2(aq) + 2 H+ + 2 e− | ⇌ | Xe(g) + 2HF(aq) | +2.32 | [21] |
| H4XeO6(aq) + 2 H+ + 2 e− | ⇌ | XeO3(aq) + H2O | +2.42 | [21] |
| 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] |
- 在Safari的v.4.0.3或更早版本（v4.0.5可正常工作）上单击这一列可能不会工作。在这种情况下仅仅需要刷新页面恢复原始顺序。
参考资料
- Milazzo, G., Caroli, S., and Sharma, V. K. (1978). Tables of Standard Electrode Potentials (Wiley, Chichester).
- Bard, A. J., Parsons, R., and Jordan, J. (1985). Standard Potentials in Aqueous Solutions (Marcel Dekker, New York).
- Bratsch, S. G. (1989). Journal of Physical Chemistry Reference Data Vol. 18, pp. 1–21.
- Vanýsek, Petr (2006). "Electrochemical Series," in Handbook of Chemistry and Physics: 87th Edition (Chemical Rubber Company).
- Vanýsek, Petr (2007). “Electrochemical Series”, in Handbook of Chemistry and Physics: 88th Edition (Chemical Rubber Company).
- Greenwood, N. N.; Earnshaw, A. 2nd. Oxford:Butterworth-Heinemann. 1997. ISBN 0-7506-3365-4.
- Bard, A.J., Faulkner, L.R.(2001). Electrochemical Methods. Fundamentals and Applications, 2nd edition (John Wiley and Sons Inc).
- Marcel Pourbaix (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions (NACE International, Houston, Texas; Cebelcor, Brussels).
- Peter Atkins (1997). Physical Chemistry, 6th edition (W.H. Freeman and Company, New York).
- 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
- 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.
- (PDF). web.anl.gov. [2013-06-06]. 可知碳之活性，九年義務教育課本《化學》九年級第一學期，上海教育出版社，2007年8月第2版，ISBN 978-7-5320-8481-4 第109、112頁、. [2013-06-06]. （原始内容存档于2016-03-05）.根據碳的相關安全資料，可之其活性範圍，推之
- Vanýsek, Petr (2007). “Electrochemical Series”, in Handbook of Chemistry and Physics: 88th Edition (Chemical Rubber Company).
- WebElements Periodic Table of the Elements | Iron | compounds information
- 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).
- Huang, Haiyan; Shuning Wang; Johanna Moll; Rudolf K. Thauer. . Journal of Bacteriology. 2012-07-15, 194 (14): 3689–3699 [2013-09-10]. ISSN 0021-9193. doi:10.1128/JB.00385-12.
- Connelly, Neil G.; Geiger, William E. . Chemical Reviews. 1 January 1996, 96 (2): 877–910. PMID 11848774. doi:10.1021/cr940053x.
- WebElements Periodic Table of the Elements | Xenon | compounds information
- Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred, 6th, New York: Wiley-Interscience, 1999, ISBN 0-471-19957-5
- Redox Reactions, Western Oregon University website
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