Observe the following complex ions:Complex Io | vedclass

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(D) To determine the number of unpaired electrons,we analyze the electronic configuration of the central metal ion in each complex:$1$. $[Mn(CN)_6]^{3

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$D < B < A < C$

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(D) To determine the number of unpaired electrons,we analyze the electronic configuration of the central metal ion in each complex:$1$. $[Mn(CN)_6]^{3-}$ $(A)$: $Mn^{3+}$ is $3d^4$. $CN^-$ is a strong field ligand,causing pairing. Configuration: $t_{2g}^4 e_g^0$. Unpaired electrons = $2$.$2$. $[Fe(CN)_6]^{3-}$ $(B)$: $Fe^{3+}$ is $3d^5$. $CN^-$ is a strong field ligand. Configuration: $t_{2g}^5 e_g^0$. Unpaired electrons = $1$.$3$. $[CoF_6]^{3-}$ $(C)$: $Co^{3+}$ is $3d^6$. $F^-$ is a weak field ligand. Configuration: $t_{2g}^4 e_g^2$. Unpaired electrons = $4$.$4$. $[Co(C_2O_4)_3]^{3-}$ $(D)$: $Co^{3+}$ is $3d^6$. $C_2O_4^{2-}$ is a strong field ligand. Configuration: $t_{2g}^6 e_g^0$. Unpaired electrons = $0$.Comparing the number of unpaired electrons: $D (0) The correct increasing order is $D < B < A < C$.

Complex Ion	Label
$[Mn(CN)_6]^{3-}$	$A$
$[Fe(CN)_6]^{3-}$	$B$
$[CoF_6]^{3-}$	$C$
$[Co(C_2O_4)_3]^{3-}$	$D$

Observe the following complex ions:
Complex Ion Label
$[Mn(CN)_6]^{3-}$ $A$
$[Fe(CN)_6]^{3-}$ $B$
$[CoF_6]^{3-}$ $C$
$[Co(C_2O_4)_3]^{3-}$ $D$

Identify the option in which the unpaired electrons in the complex ions are in correct increasing order.

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Observe the following complex ions:Complex IonLabel$[Mn(CN)_6]^{3-}$$A$$[Fe(CN)_6]^{3-}$$B$$[CoF_6]^{3-}$$C$$[Co(C_2O_4)_3]^{3-}$$D$Identify the option in which the unpaired electrons in the complex ions are in correct increasing order.