9.2 Applications of electrochemical series

2.1 Difference between metallic conduction and electrolytic conduction

3.1 Difference Between Electrolytic Cell and Galvanic Cell

5.1 Salt Bridge

9.1 Characteristics of electrochemical series
9.2 Applications of electrochemical series

10.1 Reducing power of Metals
10.2 Oxidising Nature of Non-metals

13.1 Faraday's first law
13.2 Farady's Second Law

15.1 Condition of Equilibrium
15.2 Spontaneity of the Reaction

17.1 Primary Battery or Voltaic Cells (Dry Cells):
17.2 Secondary Cells

Activity of metals depends on the tendency of losing electrons i.e., tendency of forming cation $(M^+)$, which further depends on the magnitude of standard reduction potential .

A metal is said to be chemically active if metal (having small positive value or large negative value of standard reduction potential) readily loses electrons and gets converted into cation.

Reactivity of metals decreases from top to bottom.

For example Alkali metals and alkaline earth metals have high standard reduction potential value and are chemically active. These react with cold water and evolve hydrogen. These can readily combine with acids and form corresponding salts. These combine with those which accept electron.

Metals like $Fe$, $Pb$, $Sn$, $Ni$ etc do not react with cold water but readily react with steam to evolve hydrogen.

Metals which lie below hydrogen like $Cu$, $Ag$, $Au$ etc are less reactive and do not evolve hydrogen from water.