$Ge(II)$ compounds are powerful reducing agents whereas $Pb(IV)$ compounds are strong oxidants. This can be attributed to:
- A$Pb$ is more electropositive than $Ge$
- BIonization potential of lead is less than that of $Ge$
- CIonic radii of $Pb^{2+}$ and $Pb^{4+}$ are larger than those of $Ge^{2+}$ and $Ge^{4+}$
- DMore pronounced inert pair effect in lead than in $Ge$
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Similar Questions
Given below are the two statements: one is labeled as Assertion $(A)$ and the other is labeled as Reason $(R)$.
Assertion $(A)$: There is a considerable increase in covalent radius from $N$ to $P$. However,from $As$ to $Bi$,only a small increase in covalent radius is observed.
Reason $(R)$: Covalent and ionic radii in a particular oxidation state increase down the group.
In the light of the above statements,choose the most appropriate answer from the options given below:
Assertion $(A)$: There is a considerable increase in covalent radius from $N$ to $P$. However,from $As$ to $Bi$,only a small increase in covalent radius is observed.
Reason $(R)$: Covalent and ionic radii in a particular oxidation state increase down the group.
In the light of the above statements,choose the most appropriate answer from the options given below:
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