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Chapter 2 Chapter 2 1.1 Werner’s Coordination Theory 1.2 Coordination Geometries Oxidation state Possible geometries with coordination number = 6 1 Coordination number M 2 3 5 4 1 4 6 2 M 3 5 M 6 3 2 M 2 4 5 6 Chapter 2 3 1 1 5 5 6 6 2 M M 3 4 Isomer 6 4 2 5 1 1 3 4 Chapter 2 1.3 Isomers for MA4B2 A A A A M A A B B A M A A B A A B B B B M A M B A A 1.4 Isomers for Co(NH3)4Cl2 A A A B A M A A A M A B A B B A B B B A M A A A M A A A A B 1 Chapter 2 Chapter 2 2.1 Writing Modern Formulas Examples 2.2 Ligands Ligands – molecules or ions (Lewis bases) that bind to the metal by sharing (donating) a pair of electrons Denticity – number of pairs of electrons donated by a particular ligand Chelate – ligand that binds to a metal through more th one pair than i off electrons l t Bridging ligands – ligands that donate electron pairs to more than one metal Chapter 2 Chapter 2 2.3 Common Ligands Common monodentate ligands 2.4 Common Ligands Common bridging ligands 2 Chapter 2 Chapter 2 2.5 Common Ligands Ambidentate ligands Chapter 2 2.6 Common Ligands Common multidentate (chelating) ligands Chapter 2 2.7 Writing Modern Formulas A Ni2+ is bound to two H2O and two oxalate ligands, with two NH4+ counterions A Co3+ is bound to one chloride, one NH3, and two ethylenediamine ligands, with a SO42- counterion A Cr3+ is bound to two phenanthroline and two nitrite ligands What’s the charge on the complex? 2.8 Writing Formulas A compound with composition CuCl2 4NH3 is comprised of a Cu2+ ion and has an overall metal complex charge of 2+ 2 What’s the coordination number of Cu? What’s the modern formula? A complex consists of a Mo ion bound by three CO and three thiocyanate ligands. If the overall charge on the metal complex is 1+, what’s the oxidation state of Mo? 3 Chapter 2 Chapter 2 3.1 Nomenclature 1. 3.2 Nomenclature If the compound is ionic, name the cation portion first 2. When naming the metal complex, first name the ligands, in alphabetical order, followed f by the name off the metal a. If ligand is an anion whose name ends in –ite or –ate, the final “e” is change to an “o” Sulfate sulfato; nitrite nitrito b. If ligand is an anion whose name ends in –ide, the ending is changed to “o” y cyano y Chloride chloro;; cyanide c. If ligand is neutral the common name is used Exceptions include water (aqua), ammonia (ammine), carbon monoxide (carbonyl) d. e. 3. 4. Chapter 2 If there is more than one of a particular monodentate ligand, the number of ligands is indicated by a prefix (di, tri, tetra, penta, hexa) If the ligand name is more complicated or already contains numerical prefixes (such as di, tri), the ligand prefix becomes bis, tris, tetrakis, with the ligand name in parentheses If the metal complex is an anion, the suffix –ate is added to the metal name a. If necessary, drop -ium, -en, -ese ending before adding –ate b. “cobaltate”, “nickelate”, “chromate” (not chromiumate), “manganate” (not manganeseate) c. What if the metal is iron, gold, or copper? Following the metal’s name, its oxidation state is given by a Roman numeral in parentheses Chapter 2 3.3 Nomenclature Examples [Cu(NH3)4]SO4 = tetraamminecopper(II) sulfate K2[CoCl4] = potassium tetrachlorocobaltate(II) Co(phen)2Cl2 = dichlorobis(phenanthroline)cobalt(II) [Co(en)2(H2O)Cl](NO3)2 = aquachlorobis(ethylenediamine)cobalt(III) nitrate Name the compounds: [[Ru(en) ( )2((H2O)SCN]Cl ) ] 3.4 Nomenclature Name the compounds: [Mo(ox)2(H2O)SCN]NO3 K4[Cr(CN)4Br2] (both isomers) Fe(CO)3(py)2 Pt(NH3)2Cl2 4 Chapter 2 3.5 Nomenclature Deduce the formula from the name: potassium tetracyanonickelate(II) amminebis(ethylenediamine)thiocyanatocobalt(III) nitrate tetraaquadihydroxomanganese(III) bromide tetrakis(pyridine)platinum(II) tetrachlorocuprate(II) 5