Question

It is because of inability of ns² electrons of the valence shell to participate in bonding that

(a) Sn²⁺ is oxidising while Pb⁴⁺ is reducing

(b) Sn²⁺ and Pb²⁺ are both oxidising and reducing

(c) Sn⁴⁺ is reducing while Pb⁴⁺ is oxidising

(d) Sn²⁺ is reducing while Pb⁴⁺ is oxidising.

Answer 1

Ans : (d) Sn²⁺ is reducing while Pb⁴⁺ is oxidising.

Explanation :

Inability of ns2 electrons of the valence shell to participate in bonding on moving down the group in heavier p-block elements is called inert pair effect.

As a result, Pb(II) is more stable than Pb(IV)

Sn(IV) is more stable than Sn(II) 

Pb(IV) is easily reduced to Pb(II)

→ Pb(IV) is oxidising agent

Sn(II) is easily oxidised to Sn(IV)

→ Sn(II) is reducing agent