3.5.3 Redox Equilibria - Electrochemical series
Students should:
|
Standard electrode potentials
These are often shown as a list of reductions with the most negative at the top:
Cathode (Reduction) Half-Reaction |
Standard Potential
E° (volts) |
---|---|
Li+(aq) + e- ![]() |
-3.04 |
K+(aq) + e- ![]() |
-2.92 |
Ca2+(aq) + 2e- ![]() |
-2.76 |
Na+(aq) + e- ![]() |
-2.71 |
Mg2+(aq) + 2e- ![]() |
-2.38 |
Al3+(aq) + 3e- ![]() |
-1.66 |
2H2O(l) + 2e- ![]() |
-0.83 |
Zn2+(aq) + 2e- ![]() |
-0.76 |
Cr3+(aq) + 3e- ![]() |
-0.74 |
Fe2+(aq) + 2e- ![]() |
-0.41 |
Cd2+(aq) + 2e- ![]() |
-0.40 |
Ni2+(aq) + 2e- ![]() |
-0.23 |
Sn2+(aq) + 2e- ![]() |
-0.14 |
Pb2+(aq) + 2e- ![]() |
-0.13 |
Fe3+(aq) + 3e- ![]() |
-0.04 |
2H+(aq) + 2e- ![]() |
0.00 |
S4O62-(aq) + 2e- ![]() |
+0.08 |
Sn4+(aq) + 2e- ![]() |
+0.15 |
Cu2+(aq) + e- ![]() |
+0.16 |
ClO4-(aq) + H2O(l)
+ 2e- ![]() |
+0.17 |
SO42-(aq) + 4H+ + 2e ![]() |
+0.17 |
AgCl(s) + e- ![]() |
+0.22 |
Cu2+(aq) + 2e- ![]() |
+0.34 |
ClO3-(aq) + H2O(l)
+ 2e- ![]() |
+0.35 |
IO-(aq) + H2O(l) + 2e- ![]() |
+0.49 |
Cu+(aq) + e- ![]() |
+0.52 |
I2(s) + 2e- ![]() |
+0.54 |
ClO2-(aq) + H2O(l)
+ 2e- ![]() |
+0.59 |
Fe3+(aq) + e- ![]() |
+0.77 |
Hg22+(aq) + 2e- ![]() |
+0.80 |
Ag+(aq) + e- ![]() |
+0.80 |
Hg2+(aq) + 2e- ![]() |
+0.85 |
ClO-(aq) + H2O(l) + 2e- ![]() |
+0.90 |
2Hg2+(aq) + 2e- ![]() |
+0.90 |
NO3-(aq) + 4H+(aq) + 3e- ![]() |
+0.96 |
Br2(l) + 2e- ![]() |
+1.07 |
O2(g) + 4H+(aq) + 4e- ![]() |
+1.23 |
Cr2O72-(aq) + 14H+(aq)
+ 6e- ![]() |
+1.33 |
Cl2(g) + 2e- ![]() |
+1.36 |
Ce4+(aq) + e- ![]() |
+1.44 |
MnO4-(aq) + 8H+(aq) + 5e-
![]() |
+1.49 |
H2O2(aq) + 2H+(aq)
+ 2e- ![]() |
+1.78 |
Co3+(aq) + e- ![]() |
+1.82 |
S2O82-(aq) + 2e-
![]() |
+2.01 |
O3(g) + 2H+(aq) + 2e- ![]() |
+2.07 |
F2(g) + 2e- ![]() |
+2.87 |