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

Identify the correct decreasing order of wavelength of light absorbed for the following complex ions:
$I. [Co(H_2O)_6]^{3+}$
$II. [Co(CN)_6]^{3-}$
$III. [CoI_6]^{3-}$
$IV. [Co(en)_3]^{3+}$

In which case is a $d^7$ complex species more stable?

The $d-$electron configuration of $[Ru(en)_3]Cl_2$ and $[Fe(H_2O)_6]Cl_2,$ respectively are :

The order of energy absorbed, which is responsible for the color of the following complexes, is:
$A: [Ni(H_{2}O)_{2}(en)_{2}]^{2+}$
$B: [Ni(H_{2}O)_{4}(en)]^{2+}$
$C: [Ni(en)_{3}]^{2+}$

The transition metal complex with the highest value of crystal field splitting $(\Delta_{0})$ is ........ .

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