Among the following pairs of complexes,in whi | vedclass

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(D) The crystal field splitting energy $\Delta_0$ depends on the nature of the ligand,the oxidation state of the metal,and the principal quantum numbe

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$[Rh(H_2O)_6]^{3+}$ and $[Co(H_2O)_6]^{3+}$

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(D) The crystal field splitting energy $\Delta_0$ depends on the nature of the ligand,the oxidation state of the metal,and the principal quantum number of the metal ion.For the pair $[Rh(H_2O)_6]^{3+}$ and $[Co(H_2O)_6]^{3+}$,both have the same ligand $(H_2O)$ and the same oxidation state $(+3)$.However,$Rh$ belongs to the $4d$ series while $Co$ belongs to the $3d$ series.As we move down a group,the size of the $d$-orbitals increases,leading to greater overlap with ligand orbitals and thus a larger $\Delta_0$ value.Therefore,$\Delta_0$ for $[Rh(H_2O)_6]^{3+} > \Delta_0$ for $[Co(H_2O)_6]^{3+}$.

Among the following pairs of complexes,in which case is the $\Delta_0$ value higher for the first one?

Similar Questions

What is the electronic arrangement of a metal atom/ion in an octahedral complex with $d^4$ configuration,if $\Delta_0 < P$ (pairing energy)?

Arrange the following ligands in the order of increasing field strength:
$H_2O$ $(I)$,$CO$ $(II)$,$NH_3$ $(III)$,$I^{-}$ $(IV)$,$F^{-}$ $(V)$

The increasing order of field strength of ligands is:

Which of the following is the strongest field ligand?

Identify the complex ion with electronic configuration $t_{2g}^3 e_g^2$.

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