# Electrode Potential

When a metal rod is placed in a solution of metal ions the metal rod become oppositely charged to solution ions. As a result a potential develops between them. It is called electrode potential.

E.g. Zn-rod becomes (-)vely charged in $ZnSO_4[Zn^{2+}]$ solution.

In fact electrode potential is the tendency of a metal to loose or to gain electrons, i.e. It is measurement if tendency to get oxidize or to get reduced. It is denoted by E.

The value of electrode potential depends upon:

(A)   Nature of electrode

(B)   Temperature

(C)   Concentration of ions in solution

Types: It is of two types:

Oxidation potential: It is due to oxidation, here metal becomes (-)vely charged w.r.t. solution and acts as anode

$M \to M^{n+} + ne^-$

It is denoted by $E_{O.P.}$

• $E_{O.P.} \propto$ tendency to get oxidised or reducing nature at reactivity of a metal

It means greater is the value of more will be the tendency of metal to get oxidised and a stronger reducing agent with high reactivity.

Reduction potential :It is due reduction. Here metal becomes positively charged with respect to solution ions and acts like a cathode.

$M^{n+} + ne^- \to M$

It is denoted by $E_{R.P.}$

$E_{R.P.} \propto$ tendency to get reduced $\propto$ oxidising nature

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