Cupferron metal complexes

Hydroxylamine, IV-benzoyl-lV-phenyl-in gravimetry, 1, 532 liquid-liquid extraction, 1, 544 Hydroxylamine, A -cinnamoyl-A -phenyl-liquid-liquid extraction, 1,544 Hydroxylamine, Ar,A -di-(-butyl-metal complexes, 2, 798 Hydroxylamine, Ay/V-diethyl-metal complexes, 2,798 Hydroxylamine, AAmethyl-metal complexes, 2,798 Hydroxylamine, A -2-naphthol-A -nitroso-ammonium salt — see Ncocupferron Hydroxylamine, A -nilrosophenyl-ammonium salt — see Cupferron Hydroxylamine ligands, 2, 101 Hydroxylamine oxido reductase, 6, 727 Hydroxylases molybdenum, 6,658,662 Hydroxylation arenes... 

Dyrssen, D., Studies on the extraction of metal complexes. IV. The dissociation constants and partition coefficients of 8-quinolinol (oxine) and N-nitroso-N-phenylhydroxylamine (cupferron), Sv. Kern. Tidsks. 64, 213-224 (1952). 

Acoustic emission diazine metal complexes, 80 Acrylonitrile metal complexes, 263 Actinide complexes cupferron, 510 dimethyl sulfoxide IR spectra, 490 phosphines SHAB theory, 1040 phthalocyanines, 864 thiocyanates, 236 Actins, 973 Acylates H3-ligands... 

Iron(III) complexes, tetraphenylporphyrinatobenzene-thiolatobenzenethiol-, 517 Iron(IV) complexes phosphines SHAB theory, 1040 Iron cupferronate structure, 510 Iron methoxide physical properties, 346 Iron pivalate basic, 303 Iron proteins iron-sulfur group, 773 Isobacteriochlorins, 851 Isobutyric acid, hydroxy-metal complexes IR spectra, 470 Isobutyric acid, 2-hydroxy-metal complexes NMR, 467 Isocitric acid... 

Propionohydroxamic acid metal complexes, 506 Propylenediamine metal complexes, 34 Protactinium complexes cupferron, 510 Proteins... 

Naphthoic acid, 3-hydroxy-7-sulfonato-metal complexes structure, 482 1,8-Naphthyridine metal complexes, 92,93 Neoeupferron metd complexes, 509-512 Neptunium complexes cupferron, 510 Neutron diffraction hydrates... 

Propionohydroxamic acid metal complexes, 506 Propylenediamine metal complexes, 34 Protactinium complexes cupferron, 510 Proteins electron transfer active sites, 525 metal complexes, 759-774 binding sites, 769,771 naturally occurring, 974 occurrence, 962 Proton exchange amine ligands, 24 Protonolysis metal alkoxides, 352 Prussian blue, 7, 8 Pseudocubanes structure... 

Standards and Blank Samples. When extraction systems are used, it must be taken into account that the analyte is not always transferred completely into the organic phase. The extraction efficiency depends on the conditions such as pH of the aqueous phase and metal-ligand ratio. In addition to the organic solvent used, the ligand may also have an influence on the sensitivity of the analyte in FAAS. Thus, the sensitivity of the analyte may differ in the same solvent when different ligands are used, since the metal—ligand bonds in metal complexes formed possess different thermal properties. For example, the Mn sensitivity in MIBK is better with the cupferron complex than with the diethyldithiocarbamato or 8-hydroxyquinolato complexes. 

Analytical techniques such as adsorptive stripping voltammetry rely on complex formation to improve detection limits of metals such as V(IV) and V(V) [51]. An example is in the use of cupferron and KBr03 as additives to acidic aqueous solutions, which result in the adsorption of the V(V)-cupferron complex to the electrode surface that catalyzes the reduction of the Br03 ion in solution. This technique has good selectivity over Cu, Pb, Cd, Fe, and Ti, but the response is dependent on pH. 

Lobacz et al. [52] have described partial adsorption ofTl+-cryptand (2,2,2) complex on mercury electrode. From voltocoulom-etry, cyclic voltammetry, and chrono-coulometry, it has been deduced that electroreduction of this complex proceeds via two parallel pathways from the solution and from the adsorbed states, which are energetically close. Also, Damaskin and coworkers [53] have studied adsorption of the complexes of alkali metal cations with cryptand (2,2,2) using differential capacity measurements and a stationary drop electrode. It has been found that these complexes exhibit strong adsorption properties. Novotny etal. [54] have studied interfacial activity and adsorptive accumulation of U02 " "-cupferron and UO2 - chloranilic acid complexes on mercury electrodes at various potentials in 0.1 M acetate buffer of pH 4.6 and 0.1 M NaCl04, respectively. 

Partition behaviour of americium(III) chelates with cupferron and other bidentate reagents was studied spectrophotometrically between a number of inert solvents and dilute HC104 solutions.98 Of special interest may be the data on their extractability and colours of chloroform extracts, collected in a tabular form for cupferronate derivatives of 58 metals. The pH ranges for the formation of cupferronates of 39 metal ions have been shown graphically in this publication.99 Solvent extraction and polarographic techniques were employed to study the possible adducts between technetium and cupferron.100 Evidence indicates a Tcm cupferronate and possibly a pertechnitate adduct, but no indication of a technetium(IV) complex was obtained. 

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