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In $\mathrm{Pb}_3 \mathrm{O}_4$, the different oxidation states of $\mathrm{Pb}$ is/are
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2 and 4
$\mathrm{Pb}_3 \mathrm{O}_4$ exists as a mixture of $\mathrm{PbO}$ and $\mathrm{PbO}_2$ in the ratio of $2: 1$.
The oxidation state of $\mathrm{Pb}$ in each species is +2 and +4 respectively.
In $\mathrm{PbO} \rightarrow x+(-2)=0$
$\begin{aligned}
x & =+2 \\
\mathrm{PbO}_2 \rightarrow x+2 \times(-2) & =0 \\
x-4 & =0 \\
\Rightarrow \quad x & =+4
\end{aligned}$
The oxidation state of $\mathrm{Pb}$ in each species is +2 and +4 respectively.
In $\mathrm{PbO} \rightarrow x+(-2)=0$
$\begin{aligned}
x & =+2 \\
\mathrm{PbO}_2 \rightarrow x+2 \times(-2) & =0 \\
x-4 & =0 \\
\Rightarrow \quad x & =+4
\end{aligned}$
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