Pentacyanoferrate

A = +14 cm3 mol-1 for both the forward and the reverse reaction. That this AV value is markedly less than the partial molar volumes of water and of ammonia (25 and 18 cm3 mol-1, respectively) indicates limiting dissociative (D) activation (133), as do the A values of close to +70JK-1mol-1 in both directions. Overall, the current situation with regard to thermal substitution at pentacyanoferrates(II) appears to be that an I,i mechanism can also operate for reactions of [Fe(CN)5(H20)]3-, whereas the D mechanism operates for all other [Fe(CN)5L]" complexes (134). 

Solvatochromism and piezochromism of a range of pentacyanoferrates(II) have been examined in binary aq ueous solvent mixtures, " and their solvatochromism in micelles and reversed micelles. The solvatochromism of [Fe(CN)5(nicotinamide)] has been established in several ranges of water-rich binary solvent mixtures, " of [Fe (CN)5(2,6-dimethylpyrazine)] in acetonitrile-water mixtures.The solvatochromism of [Fe(CN)5(4Phpy)] and [Fe(CN)5(4Bu py)] has been proposed as an indicator of selective solvation in binary aqueous solvent mixtures. ... 

Reviews " of pentacyanoferrate substitution kinetics have included a detailed consideration of high-pressure studies of thermal and photochemical substitution and electron transfer reactions of pentacyanoferrates-(II) and -(III). Photochemical activation can result in the loss of L or of CN . The best way to study the latter is through photochemical chelate ring closure in a pentacyanoferrate complex of a potentially bidentate ligand LL [Fe(CN)5(TL)]" rFe(CI 4(LL)] " +... 

Kinetic parameters k, often also and AS, occasionally AV ) for formation and dissociation of several pentacyanoferrate(II) complexes [Fe(CN)5L]" have been established. Ligands L include several S- and A-donor heterocycles,4-methyl- and 4-amino-pyridines, a series of alkylamines, 3- and 4-hydroxy- and 3- and 4-methoxy-pyridines, several amino acids, nicotinamide, " 4-pyridine aldoxime, 3-Me and 3-Ph sydnones, several bis-pyridine ligands,neutral, protonated, and methylated 4,4 -bipyridyl, 1,2-bis(4-pyridyl)ethane and traTO-l,2-bis0-pyridyl)ethene, pyrazine- 4,4 -bipyridyl- and bis(4-pyridyl)ethyne-pentaammine-cobalt(III), edta-ruthenium(III), and pentaammineruthenium-(II)and-(III) complexes of... 

Equilibrium constants for formation of complexes [Fe(CN)5L] can be derived from kinetics and independently from spectroscopic determinations. Values are given in many of the papers cited above stability constants for several pentacyanoferrate(II) complexes have been compared with those for their pentacyanoruthenate(II) analogues. " ... 

Table 6 Kinetic parameters for dissociation of pentacyanoferrates(II), [Fe(CN)5L] , in aqueous solution...

Reactivities of pentacyanoferrates(II) in micelles and reversed micelles have been studied. The hexadecyltrimethylammonium cation causes a modest increase in rate constant for the anion-anion reaction [Fe(CN)5(4-CNpy)] + CN. This can equally well be interpreted according to the pseudophase model developed from the Olson-Simonson treatment of kinetics in micellar systems or by the classical Bronsted equation. 

Redox potentials of pentacyanoferrates are often determined in association with kinetic and stability constant determinations. They are also available for 4-methyl- and 4-amino-pyri-dine pentacyanoferrates, and for [Fe(CS )5(2,6-dimethylpyrazine)] in acetonitrile-water mixtures.Oxidation potentials of [Fe(CN)5L] complexes correlate with the electron-withdrawing or -releasing properties of the ligands... 

The kinetics of formation of nitroprusside from [Fe VCN)5(H20)] indicate a mechanism of complex formation in which outer-sphere reduction to [Fe (CN)5(Fl20)] precedes substitution."" Reduction of the dimeric pentacyanoferrate(III) anion [Fe2(CI io]" by thiourea is a multi-stage process the first step is one-electron transfer to give [Fe2(CN)io], which dissociates to give [Fe(CN)5(tu)]2- and [Fe(CN)5(H20)] -.""... 

Fe(bpe)2(NCS)2 MeOH, bpe = tra x-l,2-bis(4-pyridyl)ethene, is a supramolecular coordinationpoly-catenane, consisting of two interlocked 2D networks. Bis-pyridylethane and bis-pyiidylethene also appear elsewhere as bridging ligands in binuclear complexes (e.g., pentacyanoferrates (Seetion 5.4.2.2)). 

The present volume is a non-thematic issue and includes seven contributions. The first chapter byAndreja Bakac presents a detailed account of the activation of dioxygen by transition metal complexes and the important role of atom transfer and free radical chemistry in aqueous solution. The second contribution comes from Jose Olabe, an expert in the field of pentacyanoferrate complexes, in which he describes the redox reactivity of coordinated ligands in such complexes. The third chapter deals with the activation of carbon dioxide and carbonato complexes as models for carbonic anhydrase, and comes from Anadi Dash and collaborators. This is followed by a contribution from Sasha Ryabov on the transition metal chemistry of glucose oxidase, horseradish peroxidase and related enzymes. In chapter five Alexandra Masarwa and Dan Meyerstein present a detailed report on the properties of transition metal complexes containing metal-carbon bonds in aqueous solution. Ivana Ivanovic and Katarina Andjelkovic describe the importance of hepta-coordination in complexes of 3d transition metals in the subsequent contribution. The final chapter by Sally Brooker and co-workers is devoted to the application of lanthanide complexes as luminescent biolabels, an exciting new area of development. 

Enantiomerically pure pipecolic acid (6) is accessible essentially by two well-established synthetic routes (i) cyclization of l- or D-lysine by reaction with disodium nitrosyl-pentacyanoferrate(II) with preservation of configuration at C2 215 216 (ii) ring closure of A ,Ae-bis(A-nitroso-A-tosyl) derivatives of l- or D-lysine, again with retention of chirality at C2. 217 Stereoselective synthesis of pipecolic acid derivatives, substituted in position 4, is achieved using the aza-Diels-Alder reaction of imines with dienes 218-220 or via an ene-iminium cyclization. 221 222 ... 

Further variations on the theme have been achieved54 by anchoring species such as [RuivO-(terpy)(py)]2+ or complexes of osmium.55 Iron complexes have also been studied for example, evaporation of a solution containing [Fe(CN)5(H20)]3 and PVP on to an electrode will immobilize the pentacyanoferrate as a pyridyl complex, one in three available pyridyl groups being used to avoid precipitation prior to evaporation of solvent. 

When oxidised, di-potassium perferricyanide, K2Fe(CN)6, is stated to be produced,2 but the salt is probably a pentacyanoferrate, K2Fe (CN)5.3 With solutions of ferrous salts potassium ferricyanide yields a deep blue precipitate, originally called TurribulVs blue, but now believed to be identical with Prussian blue.4... 

The markedly negative redox potentials of tris-catecholate and tris-hydroxamate iron complexes (Figure 4) may be ascribed to the high stabilities of the iron(III) complexes and the rather low stabilities of their iron(II) analogues. Table 9 details the relevant data (interconnected by a thermochemical cycle earlier applied to amino acid pentacyanoferrate complexes ), and documents the remarkably higher stabilities of tris-catecholate than of tris-hydroxamate complexes of iron(III). 

Espenson JH, Wolenuk SGJ. (1972) Kinetics and mechanisms of some substitution reactions of pentacyanoferrate(III) complexes. Inorpr Chem 11 2034-2041. 

Sodium nitroprusside (sodium nitrosyl pentacyanoferrate dihydrate) is administered in hypertensive crisis by IV infusion, using a controlled infusion device. The drug is commercially available as reddish-brown lyophilized powder. Prior to infusion, it is reconstituted and diluted with 5% dextrose injection. 

The pentacyanoferrate(II) group is known to have a strong affinity for aromatic A -heterocycles and rapidly binds to both ends of the self-assembled a-cyclodextrin/ligand complex to yield the rotaxane 56. Alternatively, the product... 

The transport of charge by electron hopping is an attractive model for these systems. In the case mentioned above, the electrode response is better from the precomplexed polymer film than from one prepared by first coating with PVP, then dipping into a solution containing a source of [Fe(CN)5(H20)] thus the spatial distribution of redox centres is important as well as their number in determining electrode response. Data for the pentacyanoferrate system support charge transport via adjacent redox sites and the rate of this transport falls off rapidly below a critical concentration of centres. ... 

The preparation of substituted pentacyanoferrate(II) ion complexes involves a series of ligand exchange reactions at the iron(II) metal center. Equations (4.1)-(4.3) outline the synthesis of amino acid (AA) metal complexes in aqueous solution. Starting from sodium nitroprusside ion, [Fe(CN)5(NO)]2, equation (4.1), the nitrosyl ligand, NO+, is replaced by an ammine moiety, NH3. The aquapentacyanoferrate(II) ion, [Fe(CN)5(H20)]3, is then generated in situ, equation (4.2), followed by reaction with an AA to yield the desired [Fe(CN)5(AA)](3+n) complex, equation (4.3). 

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