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  • Give reasons: (a)    Of the  species, <img alt="\textup{Cr}^{2+}" src="https://entrancecorner.codecogs.com/gif.latex?%

Give reasons:

(a)    Of the \textup{d}^4 species, \textup{Cr}^{2+} is strongly reducing while \textup{Mn}^{3+} is strongly oxidizing.

(b)    The \textup{d}^1configuration is very unstable in ions.

 

 

 

 
 
 
 
 

Answers (1)

(a)    Of the \textup{d}^4 species, \textup{Cr}^{2+} is strongly reducing while \textup{Mn}^{3+} is strongly oxidizing. For Manganese \textup{Mn}^{2+} is more stable  than \textup{Mn}^{3+} due to extra stable half-filled configuration in \textup{Mn}^{2+}. \therefore \textup{Mn}^{3+} gets reduced easily to \textup{Mn}^{2+} and hence is strongly oxidizing.

For Chromium, \textup{Cr}^{3+} is more stable than \textup{Cr}^{2+} due to extra stable half-filled  t_2g level (t_2g^3eg^0) in \textup{Cr}^{3+}. \therefore \textup{Cr}^{2+} gets oxidized easily to \textup{Cr}^{3+} and hence strongly reducing.

(b)    \textup{d}^1 is very unstable in ions. since these have a strong tendecy to lose the remaining d electron and acquire noble gas configuration.

Posted by

Sumit Saini

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