A. Water Exchange 2326 B. Proton Exchange 2327 C. Electronic Relaxation 2327 D. Relaxivity 2331 E. Outerand Second-Sphere Relaxivity 2334 F. Methods of Improving Relaxivity 2336 V. Macromolecular Conjugates 2336 A. Introduction 2336 B. General Conjugation Methods 2336 C. Synthetic Linear Polymers 2336 D. Synthetic Dendrimer-Based Agents 2338 E. Naturally Occurring Polymers (Proteins, Polysaccharides, and Nucleic Acids) 2339

https://mriquestions.com/uploads/3/4/5/7/34572113/lauffer_1999_review.pdf

Gadolinium(III) Chelates as MRI Contrast Agents: Structure, Dynamics, and Applications

Lithium-ion batteries raise safety, environmental, and cost concerns, which mostly arise from their nonaqueous electrolytes. The use of aqueous alternatives is limited by their narrow electrochemical stability window (1.23 volts), which sets an intrinsic limit on the practical voltage and energy output. We report a highly concentrated aqueous electrolyte whose window was expanded to ~3.0 volts with the formation of an electrode-electrolyte interphase. A full lithium-ion battery of 2.3 volts using such an aqueous electrolyte was demonstrated to cycle up to 1000 times, with nearly 100% coulombic efficiency at both low (0.15 C) and high (4.5 C) discharge and charge rates.

"Water-in-salt" electrolyte enables high-voltage aqueous lithium-ion chemistries.

Artificial Organic Host Molecules for Anions

Structure and nanostructure in ionic liquids.

4. Structure of Ionic Hydration Shells 1351 4.1. Results from Diffraction Experiments 1351 4.1.1. X-ray Diffraction 1351 4.1.2. Neutron Diffraction 1351 4.2. Results from Computer Simulations 1352 4.3. Results from Spectroscopic Measurements 1354 4.3.1. Vibrational Spectroscopic Measurements 1354 4.3.2. EXAFS Spectroscopy 1354 4.3.3. NMR Relaxation Studies 1355 4.3.4. Dielectric Relaxation Studies 1355 4.4. Summary of the Structure of Ionic Hydration Shells 1355

Effect of ions on the structure of water: structure making and breaking.

Formation equilibria of ternary zinc(II) complexes with chloride ions and 2,2′-bipyridyl (bpy) have been calorimetrically studied in N,N-dimethylformamide (DMF) containing 0.4 mol dm−3 (C2H5)4NClO4 as a constant ionic medium at 25 °C. Formation of binary (2,2′-bipyridyl)zinc(II) complexes has also been explored. The calorimetric data were satisfactorily explained in terms of formation of the ternary [ZnCl(bpy)]+ and [ZnCl2(bpy)] complexes together with the binary [Zn(bpy)n]2+ (n=1–3) ones, and their formation constants and enthalpies were determined. The formation of the ternary [ZnCl(bpy)]+ and [ZnCl2(bpy)] complexes is not so favorable in DMF. It is suggested that both [ZnCl(bpy)]+ and [ZnCl2(bpy)] complexes have the four-coordinate tetrahedral structure in DMF.

A calorimetric study of ternary zinc(II) complexes with chloride ions and 2,2'-bipyridyl in N,N-dimethylformamide

Complex formation of silver(I) ion with 1,3-propanediamine and 1,4-butanediamine has been studied poten-tiometrically at 25 °C in 3 mol dm−3 LiClO4 aqueous solution. Some additional experiments have been carried out in the system of silver-1,2-ethanediamine of large diamine/Ag ratios, the system having been examined in a previous work at small diamine/Ag ratios. Over the pH range of 6—10.4, the emf data obtained in the silver-diamine solutions could be explained in terms of the formation of the following complexes (L denotes the free diamine molecule): In a solution of low pH (pH=6—8), the AgHL2+ and AgH2L23+ complexes are formed. In an alkaline solution, the AgL+, Ag2L22+, and AgL2+ complexes are formed, and the relative amounts of the complexes depend on the concentrations of the metal and ligand (L) and also the ratio of these concentrations. The Ag(OH)L complex becomes a main species at the highest pH examined. In some cases the formation of the AgHL22+, Ag2HL23+, and Ag2L2+ complexes is suggested fro...

Complex Formation of Silver(I) Ion with Some Aliphatic Diamines

Abstract Molecular dynamics simulations of concentrated aqueous Csl solutions have been performed for Csl: H2O = 1:20 (2.78 molal) at 298 K and 341 K and 1:10 (5.56 molal) at 349 K. Effects of temperature and concentration on the structures of the hydrated ions, the ion pairs, and ionic aggregates are discussed by comparing the results with X-ray diffraction data obtained under similar conditions [1]

An MD Simulation of Concentrated Aqueous Solutions of Caesium Iodide

Structures of zinc(II) and copper(II) chloride N,N‐dimethylformamide solvates

X-ray diffraction measurements on 1M yttrium(III) and erbium(III) nitrate and chloride solutions in dimethyl sulfoxide (DMSO) have shown that Er(III) and Y(III) solutions of equal compositions are isostructural. The intensity difference functions can then be used to derive the detailed structure of the coordination sphere around the metal ions. The DMSO molecules are coordinated over oxygen with average M-O-S bond angles of about 130°. Two different conformations, corresponding to different relative orientations of the M-O and O-S bonds, seem to be prevalent. In the nitrate solutions an average of about 1.5 nitrate ions are coordinated as bidentate ligands to each metal ion. In the chloride solutions about 1.3 chloride ions belong to the inner-coordination sphere.

Hitoshi Ohtaki

Papers

A calorimetric study of ternary zinc(II) complexes with chloride ions and 2,2'-bipyridyl in N,N-dimethylformamide

Complex Formation of Silver(I) Ion with Some Aliphatic Diamines

An MD Simulation of Concentrated Aqueous Solutions of Caesium Iodide

Structures of zinc(II) and copper(II) chloride N,N‐dimethylformamide solvates

Structure of solvated metal ions in nitrate and chloride solutions of erbium(III) and yttrium(III) in dimethyl sulfoxide