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The oxidation state of $\mathrm{Cr}$ in $\mathrm{CrO}_5$ is
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The correct answer is:
+6
$\text {The structure of } \mathrm{CrO}_5 \text { is }$
Oxidation state of $\mathrm{Cr}$ is +6 due to the presence of two peroxide linkages, which can be calculated as. In $\mathrm{CrO}\left(\mathrm{O}_2\right)_2$, let the oxidation state of $\mathrm{Cr}$ be $\mathrm{x}$
$\begin{aligned}
\mathrm{x}+(-1) 4+(-2) & =0 \\
\mathrm{x}-6 & =0 \\
\mathrm{x} & =+6
\end{aligned}$
Oxidation state of $\mathrm{Cr}$ is +6 due to the presence of two peroxide linkages, which can be calculated as. In $\mathrm{CrO}\left(\mathrm{O}_2\right)_2$, let the oxidation state of $\mathrm{Cr}$ be $\mathrm{x}$
$\begin{aligned}
\mathrm{x}+(-1) 4+(-2) & =0 \\
\mathrm{x}-6 & =0 \\
\mathrm{x} & =+6
\end{aligned}$
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