Which of the following complex ions has elect | vedclass

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(A) complex ion is considered to have symmetrically filled orbitals if the electrons are distributed equally among the degenerate orbitals of the $t_{

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$[FeF_6]^{3-}$

Vedclass · Answer

(A) complex ion is considered to have symmetrically filled orbitals if the electrons are distributed equally among the degenerate orbitals of the $t_{2g}$ and $e_g$ sets.$1$. For $[FeF_6]^{3-}$: $Fe^{3+}$ is $d^5$. $F^-$ is a weak field ligand,so the configuration is $t_{2g}^3 e_g^2$. Here,$t_{2g}$ has $3$ electrons (one in each orbital) and $e_g$ has $2$ electrons (one in each orbital). Both sets are symmetrically filled.$2$. For $[Mn(CN)_6]^{4-}$: $Mn^{2+}$ is $d^5$. $CN^-$ is a strong field ligand,so the configuration is $t_{2g}^5 e_g^0$. This is unsymmetrical.$3$. For $[CoF_6]^{3-}$: $Co^{3+}$ is $d^6$. $F^-$ is a weak field ligand,so the configuration is $t_{2g}^4 e_g^2$. This is unsymmetrical.$4$. For $[Co(NH_3)_6]^{2+}$: $Co^{2+}$ is $d^7$. $NH_3$ is a strong field ligand,so the configuration is $t_{2g}^6 e_g^1$. This is unsymmetrical.Therefore,$[FeF_6]^{3-}$ has symmetrically filled orbitals.

List-$I$ (Complex)	List-$II$ ($CFSE$ in $\Delta_0$)
$A$. $[Cu(NH_3)_6]^{2+}$	$I$. $-0.6$
$B$. $[Ti(H_2O)_6]^{3+}$	$II$. $-2.0$
$C$. $[Fe(CN)_6]^{3-}$	$III$. $-1.2$
$D$. $[NiF_6]^{4-}$	$IV$. $-0.4$

Which of the following complex ions has electrons that are symmetrically filled in both $t_{2g}$ and $e_g$ orbitals?

Similar Questions

Which of the following statements is not applicable to Valence Bond Theory?

The correct order of ligands arranged in increasing field strength.

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State the limitations of crystal field theory $(CFT)$.

Match List-$I$ with List-$II$:

List-$I$ (Complex) List-$II$ ($CFSE$ in $\Delta_0$)

$A$. $[Cu(NH_3)_6]^{2+}$ $I$. $-0.6$

$B$. $[Ti(H_2O)_6]^{3+}$ $II$. $-2.0$

$C$. $[Fe(CN)_6]^{3-}$ $III$. $-1.2$

$D$. $[NiF_6]^{4-}$ $IV$. $-0.4$

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