Aquation

About: Aquation is a research topic. Over the lifetime, 1443 publications have been published within this topic receiving 17507 citations.

Synthesis and technique in inorganic chemistry : a laboratory manual

Abstract: Introduction Safety Laboratory Procedures Research Notebook Standard References Part I. Solid State Chemistry Experiment 1--High-Temperature Synthesis of the Superconductor YBa2Cu3O7 Tube Furnace Preparation Superconductivity Iodometric Titrations Experiment 2--The Layered Solids VOPO4(H2O)2 and VO(HPO4)(H2O)0.5 Powder X-Ray Diffraction Oxidation of Alcohols to Ketones Experiment 3--The Molecular Sieve Zeolite-X Sol-gel Synthesis High Pressure Synthesis Ion Exchange in Microporous Solids Part II. Main Group Chemistry Experiment 4--The Borane-Amine Adduct BH3NH2C(CH3)3 Lewis Acids and Bases Experiment 5--Buckminsterfullerene, C60, and Its Electrochemistry Soxhlet Extraction Cyclic Voltammetry Experiment 6--Vacuum-Line Synthesis of GeH4 Vacuum Line and Trap-to-Trap Purification Vapor Pressure and Molecular Weight Determination of a Volatile Compound Gas Phase IR Spectroscopy Experiment 7--Tin Chemistry: Coordination Complexes and Organometallic Derivatives NMR Spectroscopy Linkage Isomerism Experiment 8--Synthesis of (C6H5)2PCH2CH2P(C6H5)2 in Liquid Ammonia Synthesis in Liquid Ammonia Experiment 9--Electrolytic Synthesis of K2S2O8 Electrolytic Preparation Part III. Coordination Chemistry Experiment 10--Ion Exchange Separation of Chromium Complexes Ion Exchange Chromatography Experiment 11--Metal-Metal Quadruple Bonds Molecular Orbital Theory Experiment 12--The Magnetic Susceptibility of Mn(acac)3 Magnetism of Transition Metal Complexes The Gouy Method The Evans Methods Experiment 13--Cobalt Ammines and their Ligand Substitution Kinetics Conductivity of Ionic Complexes Kinetics of Aquation of [Co(NH3)5Cl]2+ Experiment 14--Optical Resolution of Co(en)33+ Separation of Diastereomers by Crystallization Optical Rotations Suction Filtration Experiment 15--Metal Dithiolenes and the Use of Quaternary Ammonium Salts Quaternary Ammonium Salts Part IV. Organometallic Chemistry Experiment 16--The Metal-Arene Complex [1,3,5-C6H3(CH3)3]Mo(CO)3 IR Spectra of Metal Carbonyls Experiment 17--Organo-iron Chemistry: (C5H5)2Fe2(CO)4 and (C5H5)Fe(CO)2(CH3) Schlenk Line Synthesis Infrared Spectra of Solutions Experiment 18--The Metal Carbonyl Cluster Fe3(CO)12 Mass Spectrometry Experiment 19--Microscale Synthesis of Vaska's Complex Microscale Synthesis Solid State IR Spectra Experiment 20--The Air-Sensitive Sandwich Complex Nickelocene Glove Bag Manipulations Sublimation Part V. Bioinorganic Chemistry Experiment 21--Cobaloximes: Models of Vitamin-B12 Coenzymes Enzyme Models Experiment 22--Amino Acid Complexes: Stability Constants of Ni(glycinate)n(2 - n)+ Amino Acid Chemistry pH Titrations pKa and Successive Stability Constant Determination Experiment 23--Bioinorganic Coordination Chemistry: Copper (II) Tetraphenylporphyrinate Porphyrin Chemistry Thin-Layer Chromatography Column Chromatography Notes to the Instructor Appendices NMR and Mass Spectra Index

Kinetic and mechanistic studies on the oxidation of hydroxylamine by a tri-bridged manganese(IV,IV) dimer in weakly acidic media

Abstract: The complex ion, [MnIV2(μ-O)2(μ-MeCO2)(bipy)2(H2O)2]3+ (13+) (bipy = 2,2′-bipyridine) and its aqua derivatives [Mn2IV(μ-O)2(bipy)2(H2O)4]4+ (24+) and [Mn2IV(μ-O)2(μ-MeCO2)(bipy)(H2O)4]3+ (33+) coexists in rapid equilibria in aqueous buffer in the presence of excess of bipy and MeCO2− in the range pH 4.00–5.30. The solutions are reasonably stable up to pH 5.50 and react quantitatively with hydroxylamine to produce manganese(II) and N2O. The reactions follow simple first-order kinetics in the presence of excess hydroxylamine. There is UV–vis spectral evidence for the intermediate MnIII,IV complex, [(bipy)2MnIII(μ-O)2MnIV(bipy)2]3+, in the presence of excess bipy and deficit hydroxylamine which supports that 13+ and its hydrolytic derivatives are reduced by one-electron steps. Increased extent of aquation at the manganese(IV) centre leads to increased kinetic activity in the order: 13+ < 24+ < 33+. The rate of reduction increased with an increase in the concentration of hydroxylamine but decreased with increase in cbipy and cOAc. The mild oxidising character of the complex ion along with major structural changes associated with one-electron oxidation of hydroxylamine disfavours an outer-sphere pathway. The overall first-order rate constants decrease linearly with increased mol% of D2O suggesting proton-coupled electron transfer pathways.

Activation volumes for aquation of chromium(III) pentaammine complexes with neutral leaving groups: comparison with and mechanistic differentiation from cobalt(III) analogues

Abstract: Influence de la temperature et de la pression sur l'Aquation d'une serie de complexes avec des coordinats: carboxamides, DMSO et trimethylphosphate. Comparaison de profil de volume avec une serie de complexes du cobalt(III), suggestion d'un mecanisme reactionnel

Catalysis and Inhibition in the Electrochemical Reduction of CO2 on Platinum in the Presence of Protonated Pyridine. New Insights into Mechanisms and Products.

Abstract: In the framework of modern energy challenges, the reduction of CO2 into fuels calls for electrogenerated low-valent transition metal complexes catalysts designed with considerable ingenuity and sophistication. For this reason, the report that a molecule as simple as protonated pyridine (PyH+) could catalyze the formation of methanol from the reduction of CO2 on a platinum electrode triggered great interest and excitement. Further investigations revealed that no methanol is produced. It appears that CO2 is not really reduced but rather participates, on the basis of its aquation into carbonic acid, in hydrogen evolution. Actually, the situation is not that straightforward, as revealed by scrutinizing what happens at the platinum electrode surface. The present study confirms the lack of methanol formation upon bulk electrolysis of PyH+ solutions at Pt and provides a detailed account of the Faradaic yield for H2 production as a function of the electrode potential, but the main finding is that CO2 reduction is...