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(C) To determine the number of unpaired electrons,we analyze the oxidation state of the metal and the nature of the ligand:$I.$ $[MnCl_6]^{3-}$: $Mn^{

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$IV < III < I < II$

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(C) To determine the number of unpaired electrons,we analyze the oxidation state of the metal and the nature of the ligand:$I.$ $[MnCl_6]^{3-}$: $Mn^{3+}$ $(3d^4)$,$Cl^-$ is a weak field ligand. Unpaired electrons = $4$.$II.$ $[FeF_6]^{3-}$: $Fe^{3+}$ $(3d^5)$,$F^-$ is a weak field ligand. Unpaired electrons = $5$.$III.$ $[Mn(CN)_6]^{3-}$: $Mn^{3+}$ $(3d^4)$,$CN^-$ is a strong field ligand. Unpaired electrons = $2$.$IV.$ $[Fe(CN)_6]^{3-}$: $Fe^{3+}$ $(3d^5)$,$CN^-$ is a strong field ligand. Unpaired electrons = $1$.Comparing the number of unpaired electrons: $IV (1) Thus,the increasing order is $IV < III < I < II$.

Column-$I$	Column-$II$
$(a) [Pt(NH_3)_3Cl]Br$	$(P) \text{Coordination isomerism}$
$(b) [Cr(NH_3)_5(NCS)]^{+2}$	$(Q) \text{Ionisation isomerism}$
$(c) [Co(H_2O)_6]Cl_3$	$(R) \text{Linkage isomerism}$
$(d) [PtCl_4][Pt(NH_3)_4]$	$(S) \text{Hydrate isomerism}$

Arrange the following in the increasing order of the number of unpaired electrons present in the central metal ion:
$I.$ $[MnCl_6]^{3-}$
$II.$ $[FeF_6]^{3-}$
$III.$ $[Mn(CN)_6]^{3-}$
$IV.$ $[Fe(CN)_6]^{3-}$

Similar Questions

Give an example of ionization isomerism.

Match the column:
Column-$I$ Column-$II$
$(a) [Pt(NH_3)_3Cl]Br$ $(P) \text{Coordination isomerism}$
$(b) [Cr(NH_3)_5(NCS)]^{+2}$ $(Q) \text{Ionisation isomerism}$
$(c) [Co(H_2O)_6]Cl_3$ $(R) \text{Linkage isomerism}$
$(d) [PtCl_4][Pt(NH_3)_4]$ $(S) \text{Hydrate isomerism}$

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Which of the following complexes has the possibility to exist as a meridional isomer?

The most paramagnetic complex is

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Arrange the following in the increasing order of the number of unpaired electrons present in the central metal ion:$I.$ $[MnCl_6]^{3-}$$II.$ $[FeF_6]^{3-}$$III.$ $[Mn(CN)_6]^{3-}$$IV.$ $[Fe(CN)_6]^{3-}$