Choose the complexes which are paramagnetic f | vedclass

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(C) To determine paramagnetism,we check for unpaired electrons in the central metal ion:$(i)$ $K_4[Fe(CN)_6]$: $Fe^{2+}$ is $d^6$. $CN^-$ is a strong

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$(ii)$ and $(iii)$

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(C) To determine paramagnetism,we check for unpaired electrons in the central metal ion:$(i)$ $K_4[Fe(CN)_6]$: $Fe^{2+}$ is $d^6$. $CN^-$ is a strong field ligand,causing pairing. Configuration: $t_{2g}^6 e_g^0$. No unpaired electrons (diamagnetic).(ii) $K_3[Cr(CN)_6]$: $Cr^{3+}$ is $d^3$. Configuration: $t_{2g}^3 e_g^0$. Three unpaired electrons (paramagnetic).(iii) $K_3[Fe(CN)_6]$: $Fe^{3+}$ is $d^5$. $CN^-$ is a strong field ligand,causing pairing. Configuration: $t_{2g}^5 e_g^0$. One unpaired electron (paramagnetic).(iv) $K_2[Ni(CN)_4]$: $Ni^{2+}$ is $d^8$. $CN^-$ is a strong field ligand,causing pairing in square planar geometry. Configuration: $d_{xy}^2 d_{yz}^2 d_{xz}^2 d_{z^2}^2 d_{x^2-y^2}^0$. No unpaired electrons (diamagnetic).Thus,$(ii)$ and $(iii)$ are paramagnetic.

Complex	Magnetic Moment $(BM)$
$K_4[Mn(CN)_6]$	$2.2$
$[Fe(H_2O)_6]^{2+}$	$5.3$
$K_2[MnCl_4]$	$5.9$

List-$I$ (Coordination compounds)	List-$II$ (Number of unpaired electrons)
$A$. $[Cr(CN)_6]^{3-}$	$I$. $0$
$B$. $[Fe(H_2O)_6]^{2+}$	$II$. $3$
$C$. $[Co(NH_3)_6]^{3+}$	$III$. $2$
$D$. $[Ni(NH_3)_6]^{2+}$	$IV$. $4$

Choose the complexes which are paramagnetic from the following:
$(i)$ $K_4[Fe(CN)_6]$
(ii) $K_3[Cr(CN)_6]$
(iii) $K_3[Fe(CN)_6]$
(iv) $K_2[Ni(CN)_4]$

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Choose the complexes which are paramagnetic from the following:$(i)$ $K_4[Fe(CN)_6]$(ii) $K_3[Cr(CN)_6]$(iii) $K_3[Fe(CN)_6]$(iv) $K_2[Ni(CN)_4]$