The Electromotive Series (Redox Potentials).  Reduction Reaction* --> Standard
Oxidation Reaction <-- i.e. the reverse of the reaction listed*. 

Reduction half reaction	Potential ,   Eo /V
Li+ + e- --> Li(s)	-3.045
K+ + e- --> K(s)	-2.924
Ca2+ + 2e- --> Ca(s)	-2.76
Na+ + e- --> Na(s)	-2.7109
Al3+ + 3e- --> Al(s)	-1.706
Mn2+ + 2e- --> Mn(s)	-1.029
Cd(OH)2(s) + 2e- --> Cd(s) + 2OH-	-0.812
Zn2+ + 2e- --> Zn(s)	-0.7628
Cr3+ + 3e- --> Cr(s)	-0.74
Fe2+ + 2e- --> Fe(s)	-0.409
PbSO4(s) + 2e- --> Pb(s) + SO42-	-0.356
Ni2+ + 2e- --> Ni(s)	-0.23
Sn2+ + 2e- --> Sn(s)	-0.1364
Pb2+ + 2e- --> Pb(s)	-0.1263
2H+ + 2e- --> H2(g)	0.0000000
Sn4+ + 2e- --> Sn2+	+0.15
IO3- + 2H2O +4e- --> IO- + 4OH-	+0.15
SO42- + 4H+ + 2e- --> H2SO3 + H2O	+0.20
Cu2+ + 2e- --> Cu(s)	+0.3419
O2(g) + 2H2O(l) + 4e- --> 4OH-	+0.401
IO- + H2O + 2e- --> I- + 2OH-	+0.485
NiO2(s) + 2H2O + 2e- --> Ni(OH)2(s) + 2OH-	+0.49
I2(s) + 2e- --> 2I-	+0.535
Fe3+ + e- --> Fe2+	+0.770
Ag+ + e- --> Ag(s)	+0.7996
ClO- + H2O(l) + 2e- --> Cl- + 2OH-	+0.90
NO3- + 4H+ + 3e- --> NO(g) + 2H2O(l)	+0.96
Br2(l) + 2e- --> 2Br-	+1.065
O2(g) + 4H+ + 4e- --> 2H2O(l)	+1.229
Cl2 + 2e- --> 2Cl-	+1.3583
MnO4- + 8H+ + 5e- --> Mn2+ + 4H2O	+1.507
Au+ + e- --> Au(s)	+1.68
PbO2(s) + 4H+ + SO42- + 2e- --> PbSO4(s) + 2H2O(l)	+1.685
F2(g) + 2e- --> 2F-	+2.87

Notes:
All ions are 1.0 M aqueous. (g) = gas at 1 atmosphere. (s) = solid and (l) = liquid.
*Reversing the reaction and changing the sign of the potential gives the oxidation reaction and the oxidation potential.
IThe international convention of the reduction potential as the standard is followed.
Source: CRC Handbook of Chemistry and Physics, 54th Edition, CRC Press, Inc. Boca Raton, FL, p D120.