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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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