MCQ
The element exhibiting most stable $ + \,2$ oxidation state among the following is
- A$Ag$
- B$Fe$
- C$Sn$
- ✓$Pb$
✓
Answer
Correct option: D.
$Pb$
d
$Ag$ has the electronic configuration $[ Kr ] \,4 d ^{10} \,5 s ^1$ Hence $+1$ is a stable oxidation state for it.
$Ag$ has the electronic configuration $[ Kr ] \,4 d ^{10} \,5 s ^1$ Hence $+1$ is a stable oxidation state for it.
$Fe ^{3+}$ ion is more stable due to its half-filled $3 d ^5$ electron configuration. As half filled and completely filled shells are more stable $Fe ^{3+}$ ion is more stable than $Fe ^{2+}$
The $Sn ^{2+}$ ions convert to $Sn ^{4+}$ ions because the tin$(IV)$ oxidation state is more stable than tin$(II)$.
In non-transition elements of p-block, lower oxidation state is more stable due to inert pair effect e.g., $Pb ^{2+}$ is more stable than $Pb ^{4+}$
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