. Cu + + e – → Cu(s) . Cu + + 2e – → Cu(s) . AgCl(s) + e – → Ag(s) + Cl – .
AgBr(s) + e – → Ag(s) + Br – . 2H + + 2e – → H (g) . Pb + + 2e – → Pb(s) – . Sn + + 2e – → Sn(s) – .
Ni + + 2e – → Ni(s) – . Fe + + 2e – → Fe(s) – . Cr + + 3e – → Cr(s) – . Zn + + 2e – → Zn(s) – .
2H O + 2e – → H (g) + 2OH – – . Al + + 3e – → Al(s) – . Mg + + 2e – → Mg(s) – . Na + + e – → Na(s) – .
Ca + + 2e – → Ca(s) – . K + + e – → K(s) – . Li + + e – → Li(s) – . Increasing strength of oxidising agent Increasing strength of reducing agent .
A negative E means that the redox couple is a stronger reducing agent than the H + /H couple. . A positive E means that the redox couple is a weaker reducing agent than the H + /H couple. Table .
The Standard Electrode Potentials at K Ions are present as aqueous species and H O as liquid; gases and solids are shown by g and s respectively. reducing agent than the H + /H couple. A positive E means that the redox couple is a weaker reducing agent than the H + /H couple. The standard electrode potentials are very important and we can get a lot of other useful information from them.
The values of standard electrode potentials for some selected electrode processes (reduction reactions) are given in Table . . You will learn more about electrode reactions and cells in Class XII. SUMMARY Redox reactions form an important class of reactions in which oxidation and reduction occur simultaneously.
Three tier conceptualisation viz, classical, electronic and oxidation number, which is usually