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(A) The stability of the $+2$ oxidation state in transition metals is influenced by the electronic configuration and exchange energy.$1$. $Mn^{2+}$ ha

Vedclass · Accepted Answer

$Mn > Fe > Cr > Co$

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(A) The stability of the $+2$ oxidation state in transition metals is influenced by the electronic configuration and exchange energy.$1$. $Mn^{2+}$ has a $d^5$ configuration,which is half-filled and highly stable due to maximum exchange energy.$2$. $Fe^{2+}$ has a $d^6$ configuration. While it has one electron paired,it still possesses significant exchange energy,making it more stable than $Cr^{2+}$ $(d^4)$.$3$. $Cr^{2+}$ has a $d^4$ configuration,which is less stable than $d^5$ and $d^6$ due to lower exchange energy.$4$. $Co^{2+}$ has a $d^7$ configuration,which is the least stable among these due to increased inter-electronic repulsion.Thus,the order of stability is $Mn^{2+} > Fe^{2+} > Cr^{2+} > Co^{2+}$.

For the four successive transition elements $(Cr, Mn, Fe, \text{ and } Co)$,the stability of $+2$ oxidation state will be in which of the following order?
(Atomic numbers: $Cr = 24, Mn = 25, Fe = 26, Co = 27$)

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For the four successive transition elements $(Cr, Mn, Fe, \text{ and } Co)$,the stability of $+2$ oxidation state will be in which of the following order?(Atomic numbers: $Cr = 24, Mn = 25, Fe = 26, Co = 27$)