Question

Ge (II) compounds are powerful reducing agents, whereas Pb (IV) compounds are strong oxidants. It can be due to ______.

Options

• Lead is more electropositive than germanium

• The ionization potential of lead is less than that of germanium 

• The ionic radii of Pb²⁺ and Pb⁴⁺ are larger than those of Ge²⁺ and Ge⁴⁺ 

• More pronounced inert pair effect in lead than in germanium

Answer 1

Ge (II) compounds are powerful reducing agents, whereas Pb (IV) compounds are strong oxidants. It can be due to more pronounced inert pair effect in lead than in germanium.

Explanation:

Due to inert pair effect Pb²⁺ oxidation state is more stable over Pb⁴⁺ oxidation state.

\[\ce{Ge^{2+} ->[2e^-] Ge^{4+}}\] (possible) reducing agent

\[\ce{Pb^{4+} ->[+2e^-] Pb^{2+}}\] (possible) oxidation

P\[\ce{Pb^{2+} > Pb^{+4}}\] due to inert pair effect

More-Pronounced inert pair effect in lead than Ge.