Pulse radiolysis study of monovalent cadmium, cobalt, nickel and zinc in aqueous solution. Part 2.—Reactions of the monovalent ions

Buxton, George V.; Sellers, Robin M.; McCracken, David R.

doi:10.1039/f19767201464

Cited by 54 publications

(38 citation statements)

References 2 publications

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“…The inability of t-BuOH to stimulate 2-OH-E + production by the Fenton's reagent can be attributed to the "non-reducing" nature of the radical formed from the reaction between · OH and t-BuOH [27]. With formate anion, the resulting carbon dioxide radical anion reacts very rapidly with oxygen by an electron transfer mechanism (reaction 12, k 12 = 2.0·10 9 M -1 s -1 [28]): (12) As ethanol was used in both pulse radiolysis and steady state measurements, we investigated the plausible mechanisms of O 2 ·-formation by modifying several factors (e.g., oxygen, the Fenton's reagent components, SOD and catalase) on 2-OH-E + formation (Fig. 7A).…”

Section: Reaction Of He With the Fenton's Reagentmentioning

confidence: 99%

Pulse radiolysis and steady-state analyses of the reaction between hydroethidine and superoxide and other oxidants

Zielonka¹,

Sarna²,

Roberts³

et al. 2006

Archives of Biochemistry and Biophysics

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Hydroethidine (HE) is a cell-permeable probe used for the intracellular detection of superoxide. Here we report the direct measurement of the rate constant between hydroethidine and superoxide radical anion using the pulse radiolysis technique. This reaction rate constant was calculated to be ca. 2·10 6 M -1 s -1 in water:ethanol (1:1) mixture. The spectral characteristics of the intermediates indicated that the one-electron oxidation product of HE was different from the one-electron reduction product of ethidium (E + ). The HPLC-electrochemical measurements of incubation mixtures containing HE and the oxygenated Fenton's reagent (Fe 2+ /DTPA/H 2 O 2 ) in the presence of aliphatic alcohols or formate as a superoxide generating system revealed 2-OH-E + as a major product. Formation of 2-OH-E + by the Fenton's reagent without additives was shown to be superoxide dismutase-sensitive and we attribute the formation of superoxide radical anion to the one-electron reduction of oxygen by the DTPA-derived radical. Addition of tert-butanol, DMSO, and potassium bromide to the Fenton's system caused inhibition of 2-OH-E + formation. Results indicate that reducing and oxidizing radicals have differential effects on the formation of 2-OH-E + .

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Section: Reaction Of He With the Fenton's Reagentmentioning

confidence: 99%

Pulse radiolysis and steady-state analyses of the reaction between hydroethidine and superoxide and other oxidants

Zielonka¹,

Sarna²,

Roberts³

et al. 2006

Archives of Biochemistry and Biophysics

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“…In one of those experiments to study the exchange of the ionic core, CO 2 was leaked into the UHV at a relatively high partial pressure of 1. − to O 2 was also observed in the condensed phase, with rate constants of 2.0-2.4 × 10 −9 dm 3 mol −1 s −1 at 298 K [58,59]. Although no activation energies are reported, comparison with charge-transfer reactions with similar rate constants [59], suggests that the activation energy for the CO 2 − /O 2 reaction lies around 10 kJ/mol.…”

Section: Core Exchange (C)mentioning

confidence: 89%

“…− to O 2 was also observed in the condensed phase, with rate constants of 2.0-2.4 × 10 −9 dm 3 mol −1 s −1 at 298 K [58,59]. Although no activation energies are reported, comparison with charge-transfer reactions with similar rate constants [59], suggests that the activation energy for the CO 2 − /O 2 reaction lies around 10 kJ/mol. This amount of energy is readily available in the large water clusters, which are continuously heated by collisions and black-body radiation.…”

Section: Core Exchange (C)mentioning

confidence: 89%

Free electrons, the simplest radicals of them all: chemistry of aqueous electrons as studied by mass spectrometry

Balaj

Siu

Balteanu

et al. 2004

International Journal of Mass Spectrometry

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“…Since C02-is known to be a very strong reductant (34), it can rapidly reduce another Mn(II1). But C O , may also initiate other reactions, e.g., [14]- [16] under aerobic conditions (14,(35)(36)(37).…”

Section: Resultsmentioning

confidence: 99%

Kinetics and mechanism of the oxidation of oxalate ion by tris(acetylacetonato)-manganese(III) and its hydrolytic derivatives in aqueous perchlorate media

Mukhopadhyay¹,

Chaudhuri²,

Das³

et al. 1993

Can. J. Chem.

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In the pH range 6.6–8.6, [MnL2(H2O)2]+ and [MnL2(H2O)(OH)] (HL = acetylacetone) oxidize oxalate ion (ox2−) to CO2 through the inner-sphere intermediates [MnL2(ox)]− and [MnL2(OH)(ox′)]2−, where ox′ is a half-bonded (unidentate) oxalate ion. Their rate constants of decomposition are 1.0 × 10−4 s−1 and 11.2 × 10−2 M−1 s−1 at 30 °C and at I = 1.0 M (NaClO4). Decomposition of these mixed complexes produces free radicals, presumably CO2−, which is further oxidized to CO2 by another Mn(III) in a fast step. At pH 4.2, [Mn(ox)3]3− is produced quantitatively when [ox]0 ≥ 0.12 M, which has been characterized spectrally, and its unimolecular decomposition rate constant k (= 2.7 × 10−4s−1 at 30 °C and I = 1.0 M) compares well with that reported earlier (2.44 × 10−4 s−1 at 25 °C and I = 1.0 M).

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Pulse radiolysis study of monovalent cadmium, cobalt, nickel and zinc in aqueous solution. Part 2.—Reactions of the monovalent ions

Cited by 54 publications

References 2 publications

Pulse radiolysis and steady-state analyses of the reaction between hydroethidine and superoxide and other oxidants

Pulse radiolysis and steady-state analyses of the reaction between hydroethidine and superoxide and other oxidants

Free electrons, the simplest radicals of them all: chemistry of aqueous electrons as studied by mass spectrometry

Kinetics and mechanism of the oxidation of oxalate ion by tris(acetylacetonato)-manganese(III) and its hydrolytic derivatives in aqueous perchlorate media

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