For which of the following types of ions is t | vedclass

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(A) In an octahedral complex,the $d$-orbitals split into $t_{2g}$ and $e_g$ sets.For a $d^3$ configuration,the three electrons occupy the three $t_{2g

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$d^3$

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(A) In an octahedral complex,the $d$-orbitals split into $t_{2g}$ and $e_g$ sets.For a $d^3$ configuration,the three electrons occupy the three $t_{2g}$ orbitals singly according to Hund's rule.Since the $e_g$ orbitals are higher in energy,these three electrons remain unpaired regardless of whether the ligand is a weak field or a strong field ligand.For $d^4, d^5,$ and $d^6$ configurations,the number of unpaired electrons changes depending on the crystal field splitting energy (pairing vs. excitation to $e_g$ orbitals).

$I$	$II$
$(a). [Cr(H_2O)_6]^{2+}$	$[Cr(H_2O)_6]^{3+}$
$(b). [Fe(H_2O)_6]^{3+}$	$[Fe(CN)_6]^{3-}$
$(c). [Fe(CN)_6]^{3-}$	$[Ru(CN)_6]^{3-}$
$(d). [NiF_6]^{4-}$	$[NiF_6]^{2-}$

For which of the following types of ions is the number of unpaired electrons in octahedral complexes fixed at the same number as in the free ion,no matter how weak or strong the crystal field is?

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