Chem 102 1st Edition Lecture 18Outline of Last Lecture I. Transition Metal PropertiesII. Coordinate Covalent BondIII. Ligands and ClassificationOutline of Current LectureI. ChelatesA. Coordination SphereB. Coordination GeometryII. Naming ComplexesCurrent LectureI. Chelates- 1 molecule attaching to a metal multiple times. Bi- and Polydentate ligands arechelates. The chelating agent is what the ligand is referred to as. -Chelating complexes are more stable. They have a larger formation constant value than monodentates. -Entropy? More products compared to reactants when a chelate is involved. A. Coordination Sphere- Some molecules/ions are tightly bonded to TM, located inside brackets []. -Primary Valence- Oxidation state of metal ion.-Secondary Valence- Number of bonds to the metal ion. (coordination #)B. Coordination Geometry- Co#2-Linear. Co#4-Tetrahedral or square planar. Co#5-trigonal bipyramidal, square pyramidal. Co#6-octahedral. These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.-What affects coordination number? Larger the ligand, fewer can coordinate. More ligand charge, fewer can coordinate. II. Naming Complexes- Similar to chapter 2. Cation comes first followed by anion. FormulaOrder: Metal first, ligands second. Naming Order- Ligands first, metal second. -Ligands name altered. Negative ligand ends in –o. Neutral ligands= common name. -Greek prefixes used to indicate how many ligands are attached. (never use mono)-Transition metals in the complex always has the oxidation # roman numeral. Positive or neutral complex=normal name. Negative complex= ending in –ate.-We can split the compound to determine the charge of cation and
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