Coordination Compounds

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Primary valence = ionizable bonds (oxidation state). Secondary valence = non-ionizable bonds (coordination number). Example: [Co(NH₃)₆]Cl₃ - Co³⁺ has primary valence 3 (satisfied by 3Cl⁻) and secondar

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Step 1: Identify charges - NH₃ = 0, Cl⁻ = -1, overall charge = +1 Step 2: Let oxidation state of Cr = x Step 3: x + 4(0) + 2(-1) = +1 Step 4: x - 2 = +1 Step 5: x = +3 Answer: Chromium is in +3 oxidat

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Coordination number = number of ligand donor atoms directly bonded to metal. Oxidation number = charge on metal if all ligands removed. In [Fe(CN)₆]³⁻: Coordination number = 6 (six CN⁻ ligands), Oxida

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Cu²⁺(aq) + 4NH₃(aq) → [Cu(NH₃)₄]²⁺(aq) Lewis acid: Cu²⁺ (electron pair acceptor) Lewis base: NH₃ (electron pair donor) This is a coordination complex formation where NH₃ donates lone pairs to vacant o

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dichlorido-bis(ethane-1,2-diamine)cobalt(III) chloride Rules applied: 1) Ligands in alphabetical order (chlorido before ethane-1,2-diamine), 2) bis- for complex ligand names, 3) Roman numeral for oxid

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Chelating ligands = polydentate ligands that bind through 2 or more donor atoms to same metal ion. More stable due to chelate effect (entropy increase when multiple monodentate ligands replaced). Exam

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Step 1: Co³⁺ configuration = 3d⁶ Step 2: F⁻ is weak field ligand → high spin Step 3: Electron arrangement in octahedral field: t₂g: ↑↓ ↑ ↑ eg: ↑ ↑ Step 4: Unpaired electrons = 4 Step 5: Paramagnetic (

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Both contain Co³⁺ (3d⁶). NH₃ is strong field ligand causing large Δₒ > P (pairing energy), forcing electrons to pair: t₂g⁶eg⁰ → diamagnetic. F⁻ is weak field ligand with small Δₒ < P, electrons remain