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(C) To determine the number of paramagnetic complexes, we analyze the electronic configuration of the central metal ion in each complex:$1$. $[MnBr_4]

Vedclass · Accepted Answer

$6$

Vedclass · Answer

(C) To determine the number of paramagnetic complexes, we analyze the electronic configuration of the central metal ion in each complex:$1$. $[MnBr_4]^{2-}$: $Mn^{2+}$ $(d^5)$, weak field ligand, $5$ unpaired electrons. (Paramagnetic)$2$. $[NiCl_4]^{2-}$: $Ni^{2+}$ $(d^8)$, weak field ligand, $2$ unpaired electrons. (Paramagnetic)$3$. $[Ni(CN)_4]^{2-}$: $Ni^{2+}$ $(d^8)$, strong field ligand, $dsp^2$ hybridization, $0$ unpaired electrons. (Diamagnetic)$4$. $[Ni(CO)_4]$: $Ni^0$ $(d^{10})$, strong field ligand, $sp^3$ hybridization, $0$ unpaired electrons. (Diamagnetic)$5$. $[CoF_6]^{3-}$: $Co^{3+}$ $(d^6)$, weak field ligand, $4$ unpaired electrons. (Paramagnetic)$6$. $[Fe(CN)_6]^{4-}$: $Fe^{2+}$ $(d^6)$, strong field ligand, $t_{2g}^6 e_g^0$, $0$ unpaired electrons. (Diamagnetic)$7$. $[Mn(CN)_6]^{3-}$: $Mn^{3+}$ $(d^4)$, strong field ligand, $t_{2g}^3 e_g^1$, $2$ unpaired electrons. (Paramagnetic)$8$. $[Ti(CN)_6]^{3-}$: $Ti^{3+}$ $(d^1)$, $1$ unpaired electron. (Paramagnetic)$9$. $[Cu(H_2O)_6]^{2+}$: $Cu^{2+}$ $(d^9)$, $1$ unpaired electron. (Paramagnetic)$10$. $[Co(C_2O_4)_3]^{3-}$: $Co^{3+}$ $(d^6)$, strong field ligand, $t_{2g}^6 e_g^0$, $0$ unpaired electrons. (Diamagnetic)Total paramagnetic complexes = $6$.

Number of paramagnetic complexes among the following is . . . . . . . $[MnBr_4]^{2-}$, $[NiCl_4]^{2-}$, $[Ni(CN)_4]^{2-}$, $[Ni(CO)_4]$, $[CoF_6]^{3-}$, $[Fe(CN)_6]^{4-}$, $[Mn(CN)_6]^{3-}$, $[Ti(CN)_6]^{3-}$, $[Cu(H_2O)_6]^{2+}$, $[Co(C_2O_4)_3]^{3-}$

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