Among the following complexes ( K − P ): K₃[Fe(CN)₆] (K), [Co(NH₃)₆]Cl₃ (L), Na₃[Co(oxalate)₃] (M), [Ni(H₂O)₆]Cl₂ (N), K₂[Pt(CN)₄] (O), and [Zn(H₂O)₆](NO₃)₂ (P) The diamagnetic complexes are:

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To identify diamagnetic complexes, we determine the number of unpaired electrons. Diamagnetic complexes have all electrons paired.

K: K₃[Fe(CN)₆]. Fe³⁺ is $d^{5}$ . CN⁻ is a strong field ligand, causing pairing. $t_{2 g}^{6} e_{g}^{0}$ . One unpaired electron. Paramagnetic.

L: [Co(NH₃)₆]Cl₃. Co³⁺ is $d^{6}$ . NH₃ is a strong field ligand, causing pairing. $t_{2 g}^{6} e_{g}^{0}$ . Zero unpaired electrons. Diamagnetic.

M: Na₃[Co(oxalate)₃]. Co³⁺ is $d^{6}$ . Oxalate is a strong field ligand, causing pairing. $t_{2 g}^{6} e_{g}^{0}$ . Zero unpaired electrons. Diamagnetic.

N: [Ni(H₂O)₆]Cl₂. Ni²⁺ is $d^{8}$ . H₂O is a weak field ligand. $t_{2 g}^{6} e_{g}^{2}$ . Two unpaired electrons. Paramagnetic.

O: K₂[Pt(CN)₄]. Pt²⁺ is $d^{8}$ . CN⁻ is a strong field ligand, causing pairing. Square planar complexes are typically diamagnetic. Zero unpaired electrons. Diamagnetic.

P: [Zn(H₂O)₆](NO₃)₂. Zn²⁺ is $d^{10}$ . All electrons are paired. Zero unpaired electrons. Diamagnetic.

Therefore, L, M, O, and P are diamagnetic.

Chemistry - Coordination Chemistry Question with Solution | TestHub

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