Interaction of beryllium(II) in aqueous solution with bidentate ligands containing phosphonate groups

Alderighi, Lucia; Vacca, Alberto; Cecconi, Franco; Midollini, Stefano; Chinea, E.; Domı́nguez, Sixto; Valle, A.I.; Dakternieks, Dainis; Duthie, Andrew

doi:10.1016/s0020-1693(98)00302-8

Cited by 31 publications

(27 citation statements)

References 20 publications

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“…Note that the coordination sphere of beryllium will be completed by water molecules which are not shown in the structures. Although the agreement with published stability constants is poor, we believe that the present results are correct because of the consistency of the models for AMP, ADP and ATP, not only amongst themselves, but also with the models proposed for other ligands such as oxalate, malonate, succinate [13,24], phosphonoacetate and methylenediphosphonate [25]. The stability constants for formation of [BeL] (zÀ2)À and [Be(HL)] (zÀ3)À increase in the order AMP 5 ADP 5 ATP, that is, with the length of the polyphosphate chain and the overall charge.…”

Section: Beryllium(ii) Complexessupporting

confidence: 72%

Beryllium binding to adenosine 5′-phosphates in aqueous solution at 25°C

Alderighi

Domı́nguez

Gans

et al. 2008

Journal of Coordination Chemistry

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Equilibrium constants for the binding of beryllium(II) to the nucleotides: adenosine 5 0 -monophosphate, -diphosphate, and -triphosphate have been determined. The species formed are [BeL] (zÀ2)À , [Be(HL)] (zÀ3)À , [Be 2 (OH)L 2 ] (2zÀ3)À and [Be 3 (OH) 3 (HL) 3 ] (3zÀ6)À , where L zÀ represents the fully deprotonated nucleotide. When the complex contains a protonated ligand, the protonation site is an adenosine nitrogen. Formation of these complexes is unlikely to interfere, under physiological conditions, with the functioning of the nucleotides due to the precipitation of beryllium hydroxide in the pH range 6-7.

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Section: Beryllium(ii) Complexessupporting

confidence: 72%

Beryllium binding to adenosine 5′-phosphates in aqueous solution at 25°C

Alderighi

Domı́nguez

Gans

et al. 2008

Journal of Coordination Chemistry

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“…The complexation of beryllium by these two ligands is very similar. [20,26] Similarly, sulfonate was used as a representative for sulfate. We also selected cellulose (Sigma-Aldrich) and lignin (Tokyo Chemical Industry Co., Tokyo, Japan) because they are the most abundant biopolymers, are insoluble and contain numerous alcohol functional groups.…”

Section: Organic Compound Selection and Preparationmentioning

confidence: 99%

“…Conversely, work published in the field of inorganic and medicinal chemistry discusses the aqueous coordination chemistry of beryllium, particularly the strength of various beryllium-ligand complexes, for medicinal applications related to the toxicity of beryllium. [20][21][22][23][24][25] Many of these studies report the stability constants for various inorganic and organic beryllium complexes. Unfortunately, no single study examined the various ligands and biomolecules expected to exist in natural organic matter and soils with varying acidity and time.…”

Section: Introductionmentioning

confidence: 99%

The effect of pH, organic ligand chemistry and mineralogy on the sorption of beryllium over time

Boschi

Willenbring

2016

Environ. Chem.

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Environmental contextBeryllium is a toxic environmental contaminant but has many industrial and scientific applications. Our work explores the effects of soil composition on beryllium retention, focussing on organic matter, mineralogy and pH and concludes that phosphorus and sulfur oxides in addition to soil acidity are strong controls on beryllium mobility. These results aid in future predictions regarding the fate of beryllium in the environment. AbstractUnderstanding the chemical controls on beryllium sorption is fundamental when assessing its mobility as a pollutant and interpreting its concentration as a geochemical tracer of erosion, weathering and landscape surface stability. In order to evaluate the interactions of beryllium with soil- and aquatic-related materials, we selected model organic compounds and minerals to perform sorption experiments. The retention of beryllium by each of these compounds and minerals was evaluated over a pH range of 3–6 and at various equilibration times to determine which conditions allowed the greatest retention of beryllium. We conclude that most beryllium sorption occurred within 24h for both organic and mineral materials. However, equilibration required longer periods of time and was dependent on the solution pH and sorbent material. The pH exhibited a strong control on beryllium sorption with distribution coefficient (Kd) values increasing non-linearly with increasing pH. A system with a pH of 6 is likely to retain 79–2270% more beryllium than the same system at a pH of 4. Phosphonate retained the greatest amount of beryllium, with Kd values 2–30× greater than all other materials tested at a pH of 6. Therefore, soils containing larger amounts of phosphorus-bearing minerals could result in greater retention of beryllium relative to phosphorus-limited soils. Overall, soil composition, with an emphasis on phosphorus oxide content and pH, is an important property to consider when evaluating the capacity of a system to retain beryllium.

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“…There are only a few organic ligands that can compete with the formation of Be(OH)2 (solubility product (Ksp) = 1 x 10 -20 ) at a higher pH (Wong and Woolins 1994;Keizer et al 2015). Acetate Be although some five membered rings also exhibit stability (Wong and Woolins 1994, Alderighi et al 1998, Alderighi et al 1999. Be ligands with carboxylates such as acetate and dicarboxylic acids such as oxalic [C2H2O4] and malonic [C3H4O4] acids are thermodynamically favorable because these ligands preserve the tetrahedral geometry.…”

Section: Berylliummentioning

confidence: 99%