Ge(II) compounds are powerful reducing agents whereas Pb(IV…

Chemistry S and P - Block Elements (S - Block Elements Not In Syllabus ) Physical and Chemical Properties of Group 14th Elements Single Correct MCQ

Published by: CGP EDU Academic Team

Published on: August 13, 2026

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

Pb is more electropositive than Ge.

ionization potential of lead is less than that of Ge.

ionic radii of Pb 2+ and Pb 4+ are larger than those of Ge 2+ and Ge 4+ .

more pronounced inert pair effect in lead than in Ge.

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The correct answer is:

The common oxidation states exhibited by the elements of 14 th group are +4 and +2. In heavier members the tendency to show +2 oxidation state increases in the sequence Ge < Sn < Pb. It is due to the inability of ns 2 electrons of valence shell to participate in bonding (inert pair effect). As a consequence of inert pair effect, the stable oxidation state of Pb is +2 and thus the compounds of Pb(IV) have the tendency to oxidise the compounds and reduced ourselves to Pb(II).

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