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(B) $1$. Analyze the electronic configuration and crystal field splitting for each complex:$2$. $[Cr(CN)_6]^{4-}$: $Cr^{2+}$ is $d^4$. $CN^-$ is a str

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$[Ni(en)_3]Cl_2$

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(B) $1$. Analyze the electronic configuration and crystal field splitting for each complex:$2$. $[Cr(CN)_6]^{4-}$: $Cr^{2+}$ is $d^4$. $CN^-$ is a strong field ligand,causing pairing. Configuration: $t_{2g}^4 e_g^0$. Unpaired electrons in $e_g = 0$.$3$. $[Ni(en)_3]Cl_2$: $Ni^{2+}$ is $d^8$. Configuration: $t_{2g}^6 e_g^2$. Unpaired electrons in $e_g = 2$.$4$. $[Sc(H_2O)_6]^{3+}$: $Sc^{3+}$ is $d^0$. Configuration: $t_{2g}^0 e_g^0$. Unpaired electrons in $e_g = 0$.$5$. $[V(H_2O)_6]^{2+}$: $V^{2+}$ is $d^3$. Configuration: $t_{2g}^3 e_g^0$. Unpaired electrons in $e_g = 0$.$6$. Re-evaluating the options: The question asks for the maximum number of unpaired electrons in the $e_g$ set. Based on the configurations,$[Ni(en)_3]^{2+}$ has $2$ unpaired electrons in the $e_g$ orbitals.

$I$. $NCS^{-}$	$II$. $S^{2-}$
$III$. $en$	$IV$. $SCN^{-}$

Which of the following complexes has the maximum number of unpaired electrons in the $e_g$ set of orbitals?

Similar Questions

Arrange the following ligands in the order of increasing field strength:
$H_2O$ $(I)$,$CO$ $(II)$,$NH_3$ $(III)$,$I^{-}$ $(IV)$,$F^{-}$ $(V)$

The crystal field stabilisation energy of $[Co(NH_3)_6]Cl_3$ is

In an octahedral crystal field,the $t_{2g}$ orbitals are:

The correct order of decreasing field strength of the below given ligands is
$I$. $NCS^{-}$ $II$. $S^{2-}$
$III$. $en$ $IV$. $SCN^{-}$

In which of the following,complex ions are not in correct order with respect to their magnitude of crystal field splitting?

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