2. Understanding Corrosion

2.3 Electromotive Series [1/2]


In an electromotive force series (Table 2.1), the potentials of pure metals are listed in accordance with their tendencies to corrode, the metals with the most positive potentials on the top  (like Ag, Au, Pt, etc.) followed by metals with negative potentials in the decreasing order (Na, Mg, K, etc.). The potentials listed in the table given below are called "Standard Reduction Potentials" as the half cell reaction are written in the reduction form (Au3+ + 3e- Au). Chemists generally use the emf series in which potentials are written as oxidation reactions (Au Au3+ + 3e-), and they are termed as "Standard Oxidation Potentials". The standard potentials (Eo) are measured against a standard hydrogen electrode which is at 1 atm pressure and the H+ concentration is 1 molar. The standard hydrogen electrode has been assigned a potential of 0 V at 25oC. 

 

Table 2.1: Standard Oxidation-Reduction Potentials, Volts (25oC, against Normal Hydrogen Electrode)

 

Au Au3+ + 3e 

+ 1.498

O2 + 4H+ + 4e 2H2O

+ 1.229

Pt Pt2+ + 2e

+ 1.200

Pd Pd2+ + 2e

+ 0.987

Ag Ag+ + e

+ 0.799

2Hg Hg2+ + 2e

+ 0.788

Fe Fe3+ + 3e

+ 0.771

O2 + 2H2O + 4e 4OH-

+ 0.401

Cu Cu2+ + 2e

+ 0.337

Sn4+ + 2e Sn2+

+ 0.150

2H+ + 2e H2

   0.000

Pb Pb2+ + 2e

- 0.126

Sn Sn2+ + 2e

- 0.135

Ni Ni2+ + 2e

- 0.250

Co Co2+ + 2e

- 0.277

Cd Cd2+ + 2e

- 0.403

Fe Fe2+ + 2e

- 0.440

Cr Cr2+ + 2e

- 0.744

Zn Zn2+ + 2e

- 0.763

Al Al3+ + 3e

- 1.662

Mg Mg2+ + 2e

- 2.363

Na Na+ + e

- 2.714

K K+ + e

- 2.925

The method of measurement is shown below.