How many unpaired $e^{⊖}$ are present in $t_{2 g}$ orbital of $[C r (N H_{3})_{6}]^{3 +}$ ?

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Solution

In $[C o (N H_{3})_{6}]^{3 +}$ , the central cobalt atom has +3 oxidation state and has electronic configuration $3 d^{6}$ . Since, ammonia is a strong ligand, the electrons will prefer to pair up rather than go to $e_{g}$ level. Hence, the outer electronic configuration will be $t_{2 g}^{6} e_{g}^{0}$ .

$[C o (N H_{3})_{6}]^{3 +}$ has 0 unpaired electron(s) in $t_{2 g}$ orbitals.

Hence , correct answer is 0.

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