Coordination Compounds

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A coordination compound contains a central metal atom or ion surrounded by molecules or ions called ligands. These compounds retain their identity even in solution, though partial dissociation may occ

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Double salts completely dissociate into simple ions in water, while coordination compounds dissociate to give complex ions and counter ions. Example: Mohr's salt FeSO₄.(NH₄)₂SO₄.6H₂O dissociates compl

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1. Metals exhibit two types of valence: Primary valence (ionizable) corresponding to oxidation state, and Secondary valence (non-ionizable) equal to coordination number. 2. Secondary valence is direct

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Ligand: Molecules or ions attached to the metal in a complex ion. Coordination number: Number of ligand atoms directly bonded to the central metal. Examples: Monodentate - NH₃, H₂O, Cl⁻; Bidentate - e

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Coordination sphere: The central metal atom and directly attached ligands enclosed in square brackets, behaving as a single unit. For [PtCl₆]²⁻: Let oxidation state of Pt = x. Each Cl⁻ has charge = -1

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[Co(NH₃)₄Cl₂]Cl: tetraamminedichlorocobalt(III) chloride. K₄[Fe(CN)₆]: potassium hexacyanoferrate(II). Key rules: Ligands named alphabetically before metal, anionic ligands end in 'o', neutral ligands

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(a) [NiCl₄]²⁻ - Tetrachloronickelate(II) indicates Ni²⁺ with four Cl⁻ ligands, overall charge = 2+ + 4(-1) = -2. (b) [Co(NH₃)₅(NO₂)]²⁺ - Pentaammine = 5 NH₃, nitro = NO₂⁻, cobalt(III) = Co³⁺, overall

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Fe²⁺ configuration: 3d⁶. CN⁻ is a strong field ligand causing pairing. Electron arrangement: ↑↓ ↑↓ ↑↓ | | | (3d) ↑↓ ↑↓ ↑↓ | | (4s,4p,4d). Hybridization: d²sp³ (inner orbital complex). Shape: Octahedra