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,$E(d_{xy}) > E(d_{z^2})$.

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

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