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In my book it is given that the crystal field stabilisation energy for $\ce{[Cr(en)3]Cl3}$ is more than that of the complex $\ce{[Cr(H2O)6]Cl3}.$ By what I have studied, the crystal field stabilisation energy depends on the number of electrons in $\mathrm{t_{2g}}$ and $\mathrm{e_g}$ orbitals and the pairing energy.

The number of electrons in both the compounds is the same and both undergo octahedral splitting, so that term is same for both.

Now coming to pairing energy is the energy of $\ce{en}$ more than $\ce{H2O}$ since it is a chelating group? Or it depends upon the position of the ligands in the spectrochemical series?

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    $\begingroup$ it depends upon the position of the ligands in the spectrochemical series $\endgroup$ – user600016 Oct 30 '19 at 2:02
  • $\begingroup$ ok thank you i got it $\endgroup$ – studious Oct 30 '19 at 3:21

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