Question

The d-electronic configuration of $\left[ CoCl _4\right]^{2-}$ in tetrahedral crystal field is $e ^{ m } t _2 ^n$ Sum of "$m$" and "number of unpaired electrons" is

Answer 1

Correct Answer: 7

To determine the d-electronic configuration of $[\text{CoCl}_4]^{2-}$ and the sum of $m$ and the number of unpaired electrons, follow these steps:

1. Identify the oxidation state: In $[\text{CoCl}_4]^{2-}$, chlorine (Cl) is -1, thus 4 Cl atoms contribute -4. Because the complex has a -2 charge, cobalt (Co) must be in the +2 oxidation state.
2. Determine the d-electron count: Cobalt has an atomic number of 27, corresponding to an electron configuration of [Ar] 3d⁷ 4s². In the +2 oxidation state, it loses two electrons (from 4s), resulting in 3d⁷.
3. Tetrahedral crystal field splitting: In tetrahedral fields, the energy level of $t_2$ orbitals is lower than $e$ orbitals. However, due to the weak field strength of Cl^- (a weak field ligand), the electrons remain in Hund's rule configuration.
4. Configuration identification: The $e$ and $t_2$ orbitals split into: $t_2^{3}$ and $e^{4}$ using 3 electrons in lower-energy $t_2$ and 4 electrons in higher-energy $e$ orbitals.
5. Unpaired electrons: The configuration $e^{4}$$t_2^{3}$ results in 3 unpaired electrons due to Hund’s rule.
6. Calculation of $m + \text{unpaired electrons}$: Here, $m=4$ (from $e^{m}$), and the number of unpaired electrons is 3. Thus, $m + \text{unpaired electrons} = 4 + 3 = 7$.

Conclusion: The sum is 7, which matches the expected range of (7,7).