The correct answer is Option (2) → (A) (IV), (B)-(III), (C)-(II), (D)-(I)
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List-I Complex
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List-II Oxidation state and type of complex
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(A) $[Co(NH_3)_6]^{3+}$
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(IV) +3 and Inner orbital complex
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(B) $[COF_6]^{3-}$
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(III) +3 and Outer orbital complex
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(C) $[NiCl_4]^{2-}$
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(II) +2 and Outer orbital complex
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(D) $[Ni(CN)_4]^{2-}$
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(I) +2 and Inner orbital complex
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(A) [Co(NH₃)₆]³⁺
- Co has a +3 oxidation state (since 6 NH₃ ligands are neutral).
- NH₃ is a strong field ligand → causes low-spin (inner orbital) complex.
✅ So, Oxidation state +3, Inner orbital complex → IV
(B) [CoF₆]³⁻
- Co must be +3 (because 6 F⁻ ligands, each −1 → total −6 charge, complex charge is −3 → Co = +3).
- F⁻ is a weak field ligand → high-spin, outer orbital complex.
✅ So, Oxidation state +3, Outer orbital complex → III
(C) [NiCl₄]²⁻
- Ni must be +2 (Cl⁻ is −1, 4 Cl⁻ → −4, complex charge −2 → Ni = +2).
- Cl⁻ is a weak field ligand → outer orbital, high-spin complex.
✅ So, +2, Outer orbital complex → II
(D) [Ni(CN)₄]²⁻
- Ni is +2 (CN⁻ is −1, 4 CN⁻ → −4, complex charge −2 → Ni = +2).
- CN⁻ is a strong field ligand → low-spin, inner orbital complex.
✅ So, +2, Inner orbital complex → I
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