$Ge(II)$ compounds are powerful reducing agents whereas $Pb(IV)$ compounds are strong oxidants. This can be attributed to:

• A
  $Pb$ is more electropositive than $Ge$
• B
  Ionization potential of lead is less than that of $Ge$
• C
  Ionic radii of $Pb^{2+}$ and $Pb^{4+}$ are larger than those of $Ge^{2+}$ and $Ge^{4+}$
• D
  More pronounced inert pair effect in lead than in $Ge$