Explain why Cr ^ 2+ is strongly reducing while Mn ^ 3+ is strongl…

Question

Explain why $Cr ^{2+}$ is strongly reducing while $Mn ^{3+}$ is strongly oxidizing.

✓

Answer

$Cr ^{2+}$ is strong reducing while $Mn ^{3+}$ is strongly oxidising.
$
\begin{aligned}
& E _{ Cr ^{3+} / Cr ^{2+}}^0 \text { is }-0.41 V \\
& Cr ^{2+}+2 e ^{-} \longrightarrow Cr \\
& E ^0=-0.91 V
\end{aligned}
$
If the standard electrode potential $E ^0$ of metal is large and negative, the metal is a powerful reducing agent because it loses electrons easily.
$
\begin{gathered}
Mn \longrightarrow Mn ^{3+}+3 e ^{-} \\
Mn ^{3+}+ e ^{-} \longrightarrow Mn ^{2+}
\end{gathered}
$
$
\begin{aligned}
& Mn ^{3+}[ Ar ] 3 d ^4 \\
& E ^0=+1.51 V
\end{aligned}
$
If the standard electrode potential $E ^0$ of metal is large and positive, the metal is a powerful oxidising agent because it gains electrons easily.

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