Which of the following complexes exhibits the | vedclass

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(B) To determine the paramagnetic behavior,we calculate the number of unpaired electrons $(n)$ in each complex:$1. [Co(ox)_3]^{3-}: Co^{3+}$ is $d^6$.

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$[Cr(NH_3)_6]^{3+}$

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(B) To determine the paramagnetic behavior,we calculate the number of unpaired electrons $(n)$ in each complex:$1. [Co(ox)_3]^{3-}: Co^{3+}$ is $d^6$. Oxalate $(ox^{2-})$ is a strong field ligand,causing pairing. $n = 0$.$2. [Cr(NH_3)_6]^{3+}: Cr^{3+}$ is $d^3$. $NH_3$ is a strong field ligand,but for $d^3$,the configuration is $t_{2g}^3 e_g^0$. $n = 3$.$3. [V(gly)_2(OH)_2(NH_3)_2]^+: V^{5+}$ is $d^0$. $n = 0$.$4. [Fe(en)(bipy)(NH_3)_2]^{2+}: Fe^{2+}$ is $d^6$. $en$,$bipy$,and $NH_3$ are strong field ligands,causing pairing. $n = 0$.Comparing the number of unpaired electrons,$[Cr(NH_3)_6]^{3+}$ has the highest value $(n = 3)$,hence it exhibits the highest paramagnetic behavior.

Which of the following complexes exhibits the highest paramagnetic behaviour? (Where $gly = \text{glycine}$,$en = \text{ethylenediamine}$ and $bipy = \text{bipyridyl}$) (At. nos. $Ti = 22, V = 23, Cr = 24, Fe = 26, Co = 27$)

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