Consider the metal complexes $[Ni(en)_3]^{2+}$ $(A)$, $[NiCl_4]^{2-}$ $(B)$ and $[Ni(NH_3)_6]^{2+}$ $(C)$. Choose the $\text{CORRECT}$ option by considering the number of unpaired electrons present in $(A)$, $(B)$ and $(C)$ respectively and the order of frequency of absorption.

If $\Delta_{0} < P$,then what is the electronic arrangement of the metal atom/ion in a complex with $d^4$ configuration?

Given below are two statements: Statement $I$: Each electron in $e_g$ orbitals destabilizes the orbitals by $+0.6\Delta_o$ and each electron in the $t_{2g}$ orbitals stabilizes the orbitals by $-0.4\Delta_o$ in an octahedral field on the basis of crystal field theory. Statement $II$: All the $d$-orbitals of the transition metals have the same energy in their free atomic state but when a complex is formed the ligands destroy the degeneracy of these orbitals on the basis of crystal field theory. In the light of the above statements, choose the correct answer from the options given below:

The electronic spectrum of $[Ti(H_2O)_6]^{3+}$ gives a single broad peak with a maxima at $20300 \, cm^{-1}$. The crystal field stabilization energy is equal to .......... $kJ \, mol^{-1}$

Why do transition elements form coloured compounds?

Which of the following is a high spin complex? (Where $\Delta_0$ = splitting energy of octahedral complex,$P.E.$ = Pairing energy)