For the crystal field splitting in octahedral | vedclass

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(B) In an octahedral complex,the five degenerate $d$-orbitals split into two sets due to the approach of ligands along the axes.The two orbitals $d_{x

Vedclass · Accepted Answer

the energy of the $e_{g}$ orbitals will increase by $(3/5) \Delta_{o}$ and that of the $t_{2g}$ will decrease by $(2/5) \Delta_{o}$

Vedclass · Answer

(B) In an octahedral complex,the five degenerate $d$-orbitals split into two sets due to the approach of ligands along the axes.The two orbitals $d_{x^2-y^2}$ and $d_{z^2}$ (collectively called $e_{g}$ orbitals) point directly towards the ligands and experience greater repulsion,thus their energy increases by $+(3/5) \Delta_{o}$.The three orbitals $d_{xy}$,$d_{yz}$,and $d_{zx}$ (collectively called $t_{2g}$ orbitals) point between the axes and experience less repulsion,thus their energy decreases by $-(2/5) \Delta_{o}$ relative to the barycenter.

For the crystal field splitting in octahedral complexes,

Similar Questions

Consider the following complexes:
$[CoCl(NH_3)_5]^{2+},$ $[Co(CN)_6]^{3-}$
$(A)$ $(B)$
$[Co(NH_3)_5(H_2O)]^{3+},$ $[Cu(H_2O)_4]^{2+}$
$(C)$ $(D)$
The correct order of $A, B, C,$ and $D$ in terms of the wavenumber of light absorbed is:

Write down the number of $3d$ electrons in each of the following ions:
$Ti^{2+}, V^{2+}, Cr^{3+}, Mn^{2+}, Fe^{2+}, Fe^{3+}, Co^{2+}, Ni^{2+}$ and $Cu^{2+}$
Indicate how you would expect the five $3d$ orbitals to be occupied for these hydrated ions (octahedral).

Absorbed colour of the solutions of the following complexes $[M(NH_3)_6]^{2+}$,$[M(H_2O)_6]^{2+}$ and $[MCl_4]^{2-}$ are respectively (having the same metal ion):

The electronic spectrum of $[Ti(H_2O)_6]^{3+}$ shows a single broad peak with a maximum at $20,300 \, cm^{-1}$. The crystal field stabilization energy $(CFSE)$ of the complex ion,in $kJ \, mol^{-1}$,is :

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