The energies of d_{xy} and d_{z^2}-orbitals i | vedclass

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(C) In an octahedral complex,the ligands approach along the axes. The $d_{x^2-y^2}$ and $d_{z^2}$ orbitals (axial orbitals) point directly towards the

Vedclass · Accepted Answer

$E(d_{xy}) > E(d_{z^2})$ in tetrahedral but $E(d_{xy}) < E(d_{z^2})$ in octahedral complexes

Vedclass · Answer

(C) In an octahedral complex,the ligands approach along the axes. The $d_{x^2-y^2}$ and $d_{z^2}$ orbitals (axial orbitals) point directly towards the ligands and experience greater repulsion,thus having higher energy. The $d_{xy}$,$d_{yz}$,and $d_{zx}$ orbitals (non-axial) point between the axes and have lower energy. Thus,in octahedral complexes,$E(d_{xy}) In a tetrahedral complex,the ligands approach from the corners of a tetrahedron,which is between the axes. The $d_{xy}$,$d_{yz}$,and $d_{zx}$ orbitals point closer to the ligands and experience greater repulsion,thus having higher energy than the $d_{x^2-y^2}$ and $d_{z^2}$ orbitals. Thus,in tetrahedral complexes,$E(d_{xy}) > E(d_{z^2})$.

List-$I$	List-$II$
$P$. $t_{2g}^6 e_g^0$	$1$. $[Fe(H_2O)_6]^{2+}$
$Q$. $t_{2g}^3 e_g^2$	$2$. $[Mn(H_2O)_6]^{2+}$
$R$. $e^2 t_2^3$	$3$. $[Co(NH_3)_6]^{3+}$
$S$. $t_{2g}^4 e_g^2$	$4$. $[FeCl_4]^{-}$
	$5$. $[CoCl_4]^{2-}$

The energies of $d_{xy}$ and $d_{z^2}$-orbitals in octahedral and tetrahedral transition metal complexes are such that

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