Inorganic ChemistryAfter reviewing background information in the first two chapters, Bowser discusses the bonding models of greatest importance to inorganic chemistry, the primary types of chemical reactions (with examples from both aqueous and non-aqueous solutions), the main group elements (organized to demonstrate interrelationships throughout the periodic table), the transition metals (focusing on the structures, bonding, and reactions of both classical and organometallic complexes), and finally a variety of special topics. Reflecting the current state of the discipline, the text includes many examples from and references to the recent literature. |
Contents
Brief Table of Contents | 2 |
An Introduction to Symmetry and Group Theory | 45 |
Models of Structure and Bonding | 71 |
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Common terms and phrases
18-electron rule acid anion antibonding aqueous atomic orbitals axis bipyramidal bond angle bond energy bond length bond order boron C₂ calculated carbon cations central atom Chapter Chem chloride complexes compounds configuration contains coordination number covalent bonding CsCl cubic diatomic dissociation energies effect electron density electron pairs electronegativity elements equation example experimental Explain Figure fluorine geometry given in Table H₂ H₂O halides homonuclear hybridization increases Inorg Inorganic Chemistry interactions ionic ionization energy kJ/mol lattice energy Lewis structure ligand linear lone pair MO diagram MO's molecular orbital molecule N₂ NaCl nitrogen nonbonding nucleus O₂ octahedral orbital energies overlap oxidation oxygen point group predicted protons quantum number radius reaction reduced resonance result SALC's salts solution solvent species stability sulfur symmetry temperature tetrahedral theory transition metals trigonal valence electrons valence orbitals values Wiley York