Give one chemical reaction to show that tin (II) is a reducing agent whereas `Pb` (II) is not .

Explanation

Both tin and lead exhilbit two oxidation states i.e, and `+4 +2` due to inert paire effect . As inert paire effect increase down the froup `(narr)` stabillity of `+2` oxidation state increases and that of `+4` oxidation states decerases . Hence `+2` oxidations tate is mores stable in tin than in lead. Therefore tin (II) is a reducing agent as tin (II) oxidatises to tine (IV) i.e., more stabel oxdiations tate and `Pb` (II) being more stable oxidations tate will not behave as reducing agent .
Example : `Sn^(2+) + 2 Fe^(3+) rarr Sn^(4+) + 2 Fe^(2+)`
`Sn` (II) behaves as reducing agnet it self gets oxidised to `Sn` (IV) and reduces `Fe` (III) to `fe` (II) .