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(D) In an octahedral complex,the $d$-orbitals split into $t_{2g}$ (lower energy) and $e_g$ (higher energy) sets.For a high spin $d^4$ configuration,th

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$- 0.6 \Delta_o$

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(D) In an octahedral complex,the $d$-orbitals split into $t_{2g}$ (lower energy) and $e_g$ (higher energy) sets.For a high spin $d^4$ configuration,the electrons occupy the orbitals according to Hund's rule because the crystal field splitting energy $\Delta_o$ is less than the pairing energy $P$.The electronic configuration is $t_{2g}^3 e_g^1$.The Crystal Field Stabilization Energy $(CFSE)$ is calculated as:$CFSE = (n_{t_{2g}} 	imes -0.4 \Delta_o) + (n_{e_g} 	imes 0.6 \Delta_o)$$CFSE = (3 	imes -0.4 \Delta_o) + (1 	imes 0.6 \Delta_o)$$CFSE = -1.2 \Delta_o + 0.6 \Delta_o = -0.6 \Delta_o$.

Crystal field stabilization energy for high spin $d^4$ octahedral complex is

Similar Questions

The octahedral complex of a metal ion $M^{3+}$ with four monodentate ligands $L_1, L_2, L_3$ and $L_4$ absorb wavelengths in the region of red,green,yellow and blue,respectively. The increasing order of ligand strength of the four ligands is:

Which ligand among the following has the highest splitting power of $d$-orbitals of the central metal ion?

Identify the weak field ligand from the following.

If $\Delta_{0} < P$,then what is the electronic arrangement of the metal atom/ion in a complex with $d^4$ configuration?

Which one of the following is a strong field ligand?

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