Solvation of inorganic complexes in octanol-water, hexanol-water, and related microemulsions

Ahmed, Suada; Burgess, John; Capper, Glen; Fellowes, Nicola C.; Patel, M. N.

doi:10.1016/s0277-5387(00)88204-2

Cited by 10 publications

(4 citation statements)

References 20 publications

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“…4). This situation closely parallels that of Fe(etmalt) 3 , where etmalt = ethylmaltolate (2-ethyl-3-hydroxy-4-pyranonate), in water-1-octanol and in water-1-hexanol mixtures, where strong preferential solvation by water leads to much increased solubility on adding small amounts of water to the respective alcohol [46]. The connection between indications of preferential solvation from solvatochromism and from transfer chemical potentials has been discussed elsewhere [49].…”

Section: Mo(co) 4 (Diimine)supporting

confidence: 64%

“…This is apparent from Fig. 10, where miscibility limits are shown as well as k max values [46] for Fe(CN) 2 (bipy) 2 in water-1-hexanol-CTAB mixtures. As the contour lines in Fig.…”

Section: Mo(co) 4 (Diimine)mentioning

confidence: 82%

“…Water-n-hexane-i-PrOH [45] Mo(CO) 4 (phen) Mo(CO) 4 (fz) 2-Water-n-hexane-i-PrOH b [38] Fe(CN) 5 (Xpy) mWater-1-hexanol-CTAB [9] Fe(CN) 2 (bipy) 2 Water-1-hexanol-CTABwater-1-octanol-DME or PEG [46] Fe(CN) 2 (Rsb) 2 Water-1-hexanol-AOT [30] Fe(CN) 2 (Fsb) 2 Water-1-hexanol-DEGDE [28] Fe(CN) 2 (acpyox) 2 Water-t-BuOH-PGE [47] a Ligand abbreviations : phen 1,10-phenanthroline; fz ferrozine; Xpy 4-(t-butyl)pyridine, 4-(1-butylpentyl)pyridine, or 2-methylpyrazinium; bipy 2,2 0 -bipyridyl; Rsb Schiff base from 2-acetyl pyridine and a long-chain amine, 1-Me(CH 2 ) n NH 2 with n = 11, 15, or 17; Fsb Schiff base from 2-acetylpyridine and 3-fluoro-4-methylaniline; acpyox 2-acetylpyridineketoximate b Also n-BuOH/toluene/water/SDS Fig. 1 Wavelengths of maximum absorption, k max /nm, for the charge-transfer band of Fe(CN) 2 (bipy) 2 in DEGDME-tBuOH-water solvent media Fig.…”

Section: Mo(co) 4 (Diimine)mentioning

confidence: 99%

“…References to scattered and isolated earlier articles of solvatochromism in threecomponent solvent systems are collected in Table 1 [9,28,30,38,[45][46][47], while a selection of more recent results is presented and discussed below. This selection has been chosen to provide representative illustrations of systems, results and insights-further information, including precise details of solvent compositions and wavelengths or wavenumbers of maximum absorption for the systems illustrated below, and results for a number of related systems, may be obtained from the author for correspondence.…”

Section: Introductionmentioning

confidence: 99%

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Solvatochromism and solvation of transition metal complexes in ternary aqueous solvent media

Burgess

Hubbard

2009

Struct Chem

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Section: Mo(co) 4 (Diimine)supporting

confidence: 64%

“…This is apparent from Fig. 10, where miscibility limits are shown as well as k max values [46] for Fe(CN) 2 (bipy) 2 in water-1-hexanol-CTAB mixtures. As the contour lines in Fig.…”

Section: Mo(co) 4 (Diimine)mentioning

confidence: 82%

Section: Mo(co) 4 (Diimine)mentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

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Solvatochromism and solvation of transition metal complexes in ternary aqueous solvent media

Burgess

Hubbard

2009

Struct Chem

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Iron: Inorganic & Coordination ChemistryBased in part on the article Iron: Inorganic & Coordination Chemistry by Pelham N. Hawker & Martyn V. Twigg which appeared in theEncyclopedia of Inorganic Chemistry, First Edition.

Burgess

Twigg

2005

Encyclopedia of Inorganic Chemistry

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Iron, the most abundant transition element in the biosphere, is essential in higher forms of life and its compounds have numerous industrial applications. The element has catalytic properties. Several simple iron compounds are industrially important, for example, large amounts of iron oxides are produced for pigment and magnetic recording media applications. Oxidation states ranging from −2 to +6 are known, the most familiar are +2 (ferrous iron) and +3 (ferric iron). Most common complexes are octahedral, although examples of higher (e.g. seven coordinate) and lower (e.g. tetrahedral and square planar) geometries are well known, as are a variety of mixed oxidation state compounds. Depending on ligands involved high‐ and low‐spin complexes can be formed, and temperature‐dependent spin‐state crossover complexes are well documented. The thermodynamics and kinetics of reactions of low‐spin iron(II) complexes with ligands such as 1,4‐diimines and CN − have been extensively studied. While low‐spin iron(II) is present in biological systems such as oxygenated heme centered oxygen carriers and thiolate clusters, iron(III) is more common. Thiolate‐containing iron clusters form readily, and here mixed oxidation states are a prominent feature that is exploited in some important electron transfer proteins. Microorganism iron uptake is facilitated by tris‐catecholate and tris‐hydroxamate ligands like enterobactin that have an extraordinarily high affinity for iron(III) that results in a dramatic enhancement of the 3+ relative to the 2+ state in terms of redox potential.

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Iron: Inorganic & Coordination ChemistryBased in part on the article Iron: Inorganic & Coordination Chemistry by Pelham N. Hawker & Martyn V. Twigg which appeared in theEncyclopedia of Inorganic Chemistry, First Edition.

Burgess¹,

Twigg²

2005

Encyclopedia of Inorganic and Bioinorganic Chemistry

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Solvation of inorganic complexes in octanol-water, hexanol-water, and related microemulsions

Cited by 10 publications

References 20 publications

Solvatochromism and solvation of transition metal complexes in ternary aqueous solvent media

Solvatochromism and solvation of transition metal complexes in ternary aqueous solvent media

Iron: Inorganic & Coordination ChemistryBased in part on the article Iron: Inorganic & Coordination Chemistry by Pelham N. Hawker & Martyn V. Twigg which appeared in theEncyclopedia of Inorganic Chemistry, First Edition.

Iron: Inorganic & Coordination ChemistryBased in part on the article Iron: Inorganic & Coordination Chemistry by Pelham N. Hawker & Martyn V. Twigg which appeared in theEncyclopedia of Inorganic Chemistry, First Edition.

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