JEE MainChemistryp Block Elements (Group 13 & 14)
Which of the following statements is correct regarding the redox properties of the compounds of Group 14 elements?
Options
- APb ²⁺ is a strong reducing agent because the +4 oxidation state is more stable for lead.
- BSn ²⁺ acts as a reducing agent whereas Pb ⁴⁺ acts as an oxidizing agent.
- CSn ²⁺ acts as an oxidizing agent whereas Pb ⁴⁺ acts as a reducing agent.
- DBoth Sn ²⁺ and Pb ²⁺ act as strong reducing agents to achieve the +4 oxidation state.
Correct answer
B. Sn ²⁺ acts as a reducing agent whereas Pb ⁴⁺ acts as an oxidizing agent.
Step-by-step solution
In Group 14, the stability of the +2 oxidation state increases and that of the +4 oxidation state decreases down the group due to the inert pair effect. For tin (Sn), the +4 oxidation state is more stable than the +2 oxidation state. Therefore, Sn ²⁺ tends to lose two electrons to form Sn ⁴⁺ , acting as a reducing agent. For lead (Pb), the +2 oxidation state is more stable than the +4 oxidation state due to the strong inert pair effect. Therefore, Pb ⁴⁺ readily accepts two electrons to form the more stable Pb ²⁺ st