Reaction Of Solvated Electrons Research Articles

An Advanced Tool for the Selection of Electrolyte Components for Rechargeable Lithium Batteries

The solid electrolyte interphase (SEI) plays a key role in lithium‐metal, lithium‐alloy, and lithium‐ion batteries. The SEI on both lithium and carbonaceous electrodes consists of many different materials including LiF, , lithium alkoxides, nonconductive polymers, and more. Close to the lithium or the SEI consists of the thermodynamically stable anions, such as , and halides. Close to the solution the SEI also contains partially reduced materials such as polyolefins, semicarbonates, etc. These materials form simultaneously and precipitate on the electrode as a mosaic of microphases. These phases may, under certain conditions, form separate layers, but in general it is more appropriate to treat them as heteropolymicrophases. The SEI composition and properties depend strongly on electrolyte composition and on other factors. Rapid formation of the SEI is important in all lithium batteries, especially in the case of lithium‐ion cells with graphite anodes. Hence SEI precursors must be selected from a group of materials that have high exchange current density (i0) for reduction. As it is difficult to measure i0 on solid electrodes and only limited data, if any, are available, it is suggested to use the data bank for the rate constant for the reduction of electrolyte components by hydrated electrons . We have demonstrated that the rate constants of the reactions of solvated electrons and electrolyte components and impurities correlate well with the formation voltage of SEI and with SEI composition. Thus, the rate constants (ke) for these reactions are proposed as a tool for the first screening of electrolyte components when a new electrolyte is designed.

Effect of Halide Ion Adsorption upon Plasmon-Mediated Photoelectron Emission at the Silver/Solution Interface

The effect of the roughening of the silver surface upon photoemission observed in the presence of two different scavengers dissolved in an aqueous solution, CO2 and NO3- ions, was re-examined. The quantum yield of the photocurrent exhibits a sharp maximum at 370−380 nm in the frequency range of surface plasmons on silver. These photoyields were strongly affected by the extent of the roughening of the Ag surface and reached an unusually large value of 0.05 electron per incident photon. Electrochemical oxidation/reduction roughening performed in the presence of Cl-, Br-, and ClO4- ions, similar to that employed in enhanced Raman scattering (SERS) experiments, affected the maximum of the photocurrent and in some cases also its onset potential. Photocurrents arising at potentials more negative than the potential of zero charge (pzc) of silver were principally influenced by changing morphology of the surface resulting from more or less deep roughening performed in different solutions. On the other hand, the photoelectrochemical behavior of silver at potentials positive with respect to the pzc was clearly affected by the specific adsorption of anions of the supporting electrolyte. It was, in particular, the Br- anion that caused in this potential region the strongest enhancement of the photocurrent, associated with the reduction of scavengers and led to an apparent positive shift of the onset potential. The role played by the specifically adsorbed anions is interpreted in terms of slowing down the reverse reactions of solvated electrons and of reaction intermediates (such as, for example, the NO32- anion) returning to the electrode.

Computer simulation of ion migration in ionic micellar systems

A computer simulation method is applied to study the migration of an ionic species in 0.05 M micellar solution of hexadecyltrimethylammonium bromide (HTAB). The calculations model the pulse radiolysis experiments in which reactions of solvated electrons with scavengers bound to the micelles are observed. In the case when all the micelles contain scavenger molecules a pseudo first-order decay of the solvated electron is found, with the rate coefficient 5.3 × 10 11 M −1 s −1. When only a part of the micelles is occupied by scavengers, a two-exponential decay kinetics of the solvated electron is obtained.

Solvent effects on the reactivity of solvated electrons with organic solutes in 1-butylamine–water mixtures

The values of the rate constants of the reactions of es− with the efficient scavengers nitrobenzene and acetone are ≥ 2 × 106 m3 mol−1 s−1 in the whole range of 1-butylamine–water mixtures at 298 K; the reaction rates in the mixed solvents vary approximately as the solvent fluidity. In pure butylamine at 298 K, k2(es− + nitrobenzene) = 84 × 106 m3 mol−1 s−1 and k2(es− + acetone) = 7.3 × 106 m3 mol−1 s−1. The values of the rate constants of the reactions of es− with the inefficient scavengers phenol and toluene are < 2 × 105 m3 mol−1 s−1 in the whole range of 1-butylamine–water mixtures at 298 K and have a maximum at 50 mol% water and a minimum at 99 mol% water. In pure 1-butylamine at 298 K, k2(es− + phenol) = 1.0 × 104 m3 mol−1 s−1 and k2(es− + toluene) = 0.28 × 104 m3 mol−1 s−1. The reaction rates with inefficient scavengers show strong dependence on the solvent composition and selective solvation of electron and scavenger. In the amine-rich region (0–30 mol% water), the rate constants increase with the increase of viscosity, indicating the chemical participation of solvent molecules in the reaction. In the water-rich region from 50 to 99 mol% water, the decrease of the rate constants indicates the nonhomogeneous solvation of the electrons by water and of the organic solutes by 1-butylamine. From 99 mol% to pure water the rate constant increases rapidly, which we attribute to insufficient 1-butylamine to coat the phenol or toluene molecules. The variation of the activation energies E2 for the efficient scavengers, 14–27 kJ mol−1, are similar to the variation of Eη in the mixed solvents. The values of E2 for the inefficient scavengers are from 15 to 38 kJ mol−1 for phenol and from 6 to 21 kJ mol−1 for toluene. Both k2 and E2 for the inefficient scavenger reactions show a correlation with the temperature coefficient −dEAmax/dT of the optical absorption of es− in the mixed solvents, but the reason is obscure. Key words: 1-butylamine–water solvent, solvated electron, organic solutes, reactivity, solvent effects.

Studies in mixed solvents: Comparison between solvated electron reactions and quenching of excited states

AbstractThe rate constants for the reaction of electron pulse produced solvated electrons and a number of solutes in water‐isopropanol mixtures have been measured. The quenching of the singlet excited state of naphthalene has also been studied in the same mixtures, using triethylamine and acrylamide as quenchers. The variation of the bimolecular solvated electron reaction rate constants with the composition of the solvent has been compared with the variation in the quenching constants with the composition of the solvent. Both these variations are surprisingly similar, with acrylamide behaving in a reverse manner (to the other solutes) in both the cases. It has been possible to quantitatively correlate both sets of data using dielectric constant (ϵ) as a measure of polarity and the viscosity (η) as an index of the microstructure. The curves obtained provide insights with respect to the nature of charge transfer processes involved. © 1995 John Wiley & Sons, Inc.

Solvent Effects on Reactivity of Solvated Electrons with Nitrate Ion and on Electrolyte Conductivity in C1 to C10 n-Alcohols

Solvent Effects on Reactivity of Solvated Electrons with Nitrate Ion and on Electrolyte Conductivity in C1 to C10 n-Alcohols

Scavenging Reaction of Solvated Electrons Produced by UV Laser from Iodide Anion in Liquid Beam

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTScavenging Reaction of Solvated Electrons Produced by UV Laser from Iodide Anion in Liquid BeamHisashi Matsumura, Fumitaka Mafune, and Tamotsu KondowCite this: J. Phys. Chem. 1995, 99, 16, 5861–5864Publication Date (Print):April 1, 1995Publication History Published online1 May 2002Published inissue 1 April 1995https://doi.org/10.1021/j100016a020RIGHTS & PERMISSIONSArticle Views225Altmetric-Citations24LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InReddit PDF (1 MB) Get e-Alerts

Solvent effects on the reactivity of solvated electrons with ions in tert-butanol/water mixtures

Reactions of [Formula: see text] with the ions [Formula: see text] showed different variations of rate with solvent composition in tert-butanol/water mixtures from 0 to 100 mol% water. In pure tert-butanol solvent at 298 K the respective values of k2 (106 m3 mol−1 s−1) are 3.2, 13, and 42. The estimated value of reaction radius Rr depends on the minimum number of solvent molecules needed between [Formula: see text] and the reactant ion to attain the static values of ε of the bulk solvent used in the calculation of the Debye factor f; Rr is assumed to be larger in the alcohol-rich region than in the water-rich region, because the solvent molecules are larger. The Smoluchowski–Debye–Nernst–Einstein model is used to evaluate the effective reaction radius κRr, where κ is the probability of reaction per encounter; κRr decreases from pure tert-butanol to pure water. In the water-rich region the activation energies E2 of the efficient reactions, 11–24 kJ mol−1, are similar to EΛ0 of the reactant electrolyes, 12–23 kJ mol−1. For the inefficient reactant [Formula: see text] E2 = 30 kJ mol−1. The high values of E2 = 43–53 kJ mol−1 in pure tert-butanol solvent are attributed to a high activation energy for diffusion of [Formula: see text] in this solvent. Keywords:tert-butanol/water solvents, solvated electron, ions, reactivity, solvent effects.

Solvent effects on the reactivity of solvated electrons with in C1 to C4 alcohols

The rate constants [Formula: see text] in pure C1 to C4 alcohol solvents at 298 K increase with increasing viscosity and decreasing permittivity. Thus the reactivity increases with decreasing diffusivity and increasing coulombic repulsion, so the Debye–Smoluchowski model does not apply. The effective reaction radius κRr increases with decrease of effective trap depth Er/τ of the electrons in the solvent: κRr = CτRr(Er/τ)pτ. Values of κRr and Er/τ change with temperature, and values of Pτ fall in four categories: ∼0.0 for water and methanol; ∼1.3 for primary alcohols; 0.6 for secondary alcohols; 1.8 for tert-butanol. The C—H groups participate in the [Formula: see text] reaction. Keywords: alcohol solvents, solvated electron, nitrate ion, reactivity, solvent effects.

Solvent effects on the reactivity of solvated electrons with ions in isobutanol/water mixed solvents

The effective reaction radii KRr, where Rr is the reactive encounter radius and K is the probability of reaction per encounter, for [Formula: see text] with [Formula: see text], are all 0.7 ± 0.1 nm in isobutanol containing 10–20 mol% water. The value remains at 0.7 ± 0.1 nm for [Formula: see text] in pure isobutanol, and for the two transition metal ions in pure water solvent. The value for [Formula: see text] reduces to 0.35 nm in pure isobutanol and pure water solvents, whereas for [Formula: see text] in pure water solvent it is only 0.14 nm and 2.6 × 10−5 nm, respectively. The low reactivity of [Formula: see text] with [Formula: see text] in water is attributed to the symmetry of the hydrogen-bonded solvation structure of [Formula: see text] in water, and the higher reactivity of [Formula: see text] is attributed to the lower symmetry of its hydrogen-bonded solvation structure. The [Formula: see text] ions have no low-lying orbital for an electron to occupy, so either reaction occurs by proton transfer to the electron site or the neutral species must decompose. We suggest that the proton transfer or the decomposition of the neutral species is facilitated by an unsymmetrical solvation structure.Reaction of [Formula: see text] in Al(ClO4)3 solutions in water is due mainly to [Formula: see text] from hydrolysis of [Formula: see text] and partly to partially hydroxylated aluminum(III) species. Reaction of [Formula: see text] with [Formula: see text] itself appears to be negligible in water. The reactivity of the solutions of Al(ClO4)3 in isobutanol-rich solvents is 3–5 times greater than that in water.In pure C1 to C4 1-alcanol solvents the value of [Formula: see text] increases linearly with the dielectric relaxation time τ1 of the solvent. In these solvents the probability of permanent capture per encounter increases approximately as the square of the encounter duration.

Electron Migration along 5-Bromouracil-Substituted DNA Irradiated in Solution and in Cells

Solvated electrons generated in aqueous solution after exposure to ionizing radiation can be scavenged by DNA and then transferred along the DNA molecule. This mechanism of charge transfer provides an opportunity for radiation damage to be targeted to certain regions in the DNA molecule and is a mechanism by which single-strand breaks contribute to locally multiply damaged sites to enhance cell lethality. Experiments were performed in which different amounts of 5-bromouracil (5-BrU) were substituted for thymine in Escherichia coli DNA. The amount of bromide released was assayed after quantitative reaction of radiation-induced solvated electrons with 5-BrU in DNA samples irradiated in solution and irradiated in the cellular environment. By varying the amount of 5-BrU incorporated in the DNA, the average distance between 5-BrU molecules was systematically changed and, because the number of 5-BrU/electron reactions was monitored by the amount of bromine released, the maximum average electron migration distance along the 5-BrU DNA could be estimated. Using this approach, the maximum average electron migration distance in aqueous solutions of 5-BrU DNA was about 6.5 to 10 base distances in nonhybrid 5-BrU DNA (assuming only intrastrand migration). Similar methods revealed charge migration in 5-BrU DNA incorporated into E. coli, and the maximum average migration distance was about 5 to 6 base distances (assuming only intrastrand migration). Only 11-16% of the electrons produced during radiolysis were scavenged by 5-BrU DNA in aqueous solution, and only 1% resulted in the release of bromide from 5-BrU-DNA inside E. coli.

Solvent effects on the reactivity of solvated electrons with ammonium and nitrate ions in 1-butanol–water solvents

Values of the rate constants, k2 (106 m3 mol−1 s−1), of solvated electrons,[Formula: see text] with several related salts, in pure water and pure 1-butanol solvents at 298 K are, respectively, as follows: LiNO3, 9.2, 0.19; NH4NO3, 10, 8.3; NH4ClO4, 1.5 × 10−3, 12 in 20 mol% water; LiClO4, 1.0 × 10−4, < 1.0 × 10−4. The value of [Formula: see text] in water solvent is 48 times larger than that in 1-butanol solvent, whereas [Formula: see text] in water is 10−4 times smaller than the value in 1-butanol. This enormous reversal of solvent effects on [Formula: see text] reaction rates is the first observed for ionic reactants. The solvent participates chemically in the [Formula: see text] reaction, and the overall rate constant increases with increasing viscosity and dielectric relaxation time. This unusual behavior is attributed to a greatly increased probability of reaction of an encounter pair with increasing duration of the encounter. Effective reaction radii κRr for [Formula: see text] and [Formula: see text] were estimated with the aid of measured electrical conductances of the salt solutions in all the solvents. Values of κRr are (2–7) × 10−10 m, except for NH4,s+ in 100 and 99 mol% water, which are 2.6 and 2.7 × 10−14 m, respectively. The effective radii of the ions for mutual diffusion increase with increasing butanol content of the solvent, from ~50 pm in water to ~150 pm in 1-butanol, due to the increasing average size of the molecules that solvate the ions.

Switchover of reactions of solvated electrons with nitrate ions and ammonium ions in propanol–water solvents

The reaction rate constants of [Formula: see text] with ammonium nitrate (~ 0.1 mol m−3) in 1-propanol-water and 2-propanol–water binary solvents correspond to [Formula: see text] reaction in the water-rich solvents, and to [Formula: see text] reaction in alcohol-rich solvents. The overall rate constant is smaller in solvents with 40–99 mol% water, with a minimum at 70 mol% water. The Arrhenius temperature coefficient is 26 kJ mol−1 in each pure propanol solvent, increases to 29 kJ mol−1 at 40 mol% water, then decreases to 17 kJ mol−1 in pure water solvent. The high reaction rates in the single component solvents, alcohol or water, are limited mainly by solvent processes related to shear viscosity (diffusion) and dielectric relaxation (dipole reorientation). Rate constants reported for concentrated solutions (50–1000 mol m−3) of ammonium and nitrate salts in methanol (Duplâtre and Jonah. J. Phys. Chem. 95, 897 (1991)) have been quantitatively reinterpreted in terms of the ion atmosphere model.

Some aspects of radiation-induced free-radical chemistry of biologically important molecules

Biologically relevant material is usually associated with considerable amounts of water; e.g. the living cell contains about 70% water. When ionizing radiation interacts with such material one must consider two modes of energy deposition: the direct effect (ionizing radiation is absorbed by the biomolecules) and the indirect effect (ionizing radiation is absorbed by the surrounding water). In the direct effect, radical cations plus electrons, and excited states of the biomolecules are formed. In the indirect effect the water is decomposed resulting in the formation of the water radicals .OH, H . and e - aq. These reactive intermediates then interact with the biomolecules. When such systems are irradiated oxygen is often present. As a result of this, the radicals formed in the biomolecules by the various routes are converted into the corresponding peroxyl radicals. In certain cases, e.g. with the nucleobases of DNA, radical cations can be produced in dilute aqueous solutions by radiation-generated SO· − 4 radicals, and the fate of these nucleobase radical cations studied by pulse radiolysis and product analysis. Attention will be drawn to the fact that frequently some of the reaction products of the radical cations with water are identical to those formed by OH radical attack, but that there are also marked differences. Similarly, protonation of radical anions (formed by the reaction of solvated electrons with the biomolecules) and the reaction of H-atoms with these molecules can lead to radical intermediates with considerably differing characteristics. Our present knowledge of the variety of reactions of the peroxyl radicals occuring in aqueous solutions will be briefly discussed, emphasizing the large variety of HO . 2/O· - 2 elimination reactions and pointing to the reversibility of the oxygen addition (RO . 2→R . + O 2) in some systems recently studied.

Erratum: Solvent structure effects on solvated electron reactions in mixed solvents: Negative ions in 1-propanol–water and 2-propanol–water

In models of the kinetics of chemical reactions in solution the solvent is commonly assumed to be a uniform continuum. An example is the Smoluchowski–Debye–Stokes–Einstein equation for the rate constant k2 of a bimolecular reaction between charged or polar species: k2 = κRTfrr/1.5ηrd where κ = probability that a reactant encounter pair will react, R = gas constant, T = temperature, f = Coulombic interaction factor, rr = effective radius for reaction, η = solvent viscosity, and rd = effective radius for mutual diffusion. The equation is useful in evaluating effects of bulk-fluid properties on reaction rates. Residual effects are attributed to more specific solvent behaviour. Rate constants and activation energies E2 of reactions of solvated electrons with and ions vary with the composition of 1-propanol–water and 2-propanol–water mixed solvents. Plots of k2η/fT against solvent composition are nonlinear and change with solvent pair and with reactant pair. Measured molar conductivities Λ0(Li+, ) and Λ0(2Li+,...

Simulation of the Passage of Fast Electrons and the Early Stage of Water Radiolysis by the Monte Carlo Method

A numerical computer simulation of the processes of the interaction of electrons with liquid water and vapor was performed, beginning with the absorption of the energy of ionizing radiation and including the chemical changes in the medium. The specific features of the liquid phase compared with the gaseous phase were taken into account. Among them are the decrease of the ionization potential and collective excitations of the plasmon type. The mass stopping powers and ranges of electrons in liquid water and vapor were calculated. Within the frames of the stochastic model the kinetics of water radiolysis in the picosecond range of radiolysis was calculated by the Monte Carlo method. The mechanism of water radiolysis was found with the electron-ion recombination and the reactions of quasi-free and solvated electrons taken into account.

Solvent structure effects on solvated electron reactions with ions in 2-butanol/water mixed solvents

The Smoluchowski–Debye–Stokes–Einstein equation for the rate constant k2 of a bimolecular reaction between charged or polar species[Formula: see text]was used to evaluate effects of bulk solvent properties on reaction rates of solvated electrons with [Formula: see text] and [Formula: see text] in 2-butanol/water mixed solvents. To explain detailed effects it was necessary to consider more specific behavior of the solvent. Rate constants k2, activation energies E2, and pre-exponential factors A2 of these reactions vary with the composition of 2-butanol/water mixtures. The values of E2 were in general similar to activation energies of ionic conductance EΛ0 of the solutions, except for much higher values of E2 of [Formula: see text] in alcohol-rich solvents and of [Formula: see text] in pure water solvent. The solvent apparently participates chemically in the [Formula: see text] reaction, and the [Formula: see text] reaction is multistep. Rate constant and conductance measurements of thallium acetate solutions in 2-butanol containing zero and 10 mol% water were complicated by the formation of ion clusters larger than pairs. Key words: alcohol/water mixed solvents, ions, reaction kinetics, solvated kinetics, solvated electron, solvent effects.

Solvent structure effects on solvated electron reactions in mixed solvents: positive ions in 1-propanol/water and 2-propanol/water

In models of the kinetics of chemical reactions in solution the solvent is commonly assumed to be a uniform continuum. An example is the Smoluchowski–Debye–Stokes–Einstein equation for the rate constant k2 of a bimolecular reaction between charged or polar species:[Formula: see text]where κ is the probability that a reactant encounter pair will react, R is the gas constant, T is the temperature, f is a factor that reflects the effect of electrostatic interaction between the reactants on their probability of attaining the closeness of approach rr at which reaction occurs, η is the solvent viscosity, and rd is the effective radius of the reactant entities for mutual diffusion. The equation is useful in evaluating effects of bulk fluid properties on reaction rates. Residual effects are attributed to more specific solvent behaviour.Rate constants k2, activation energies E2, and pre-exponential factors A2 of reactions of solvated electrons [Formula: see text] with [Formula: see text] [Formula: see text] and [Formula: see text] ions vary with the composition of 1-propanol/water and 2-propanol/water mixed solvents. Plots of k2η/fT against solvent composition are nonlinear and change with the solvent pair and with reactant pair. Measured molar conductivities [Formula: see text] [Formula: see text] [Formula: see text] and [Formula: see text] indicate that the values of rd for the mutual diffusion of the cations and anions have a minimum near 90 mol% water, and that the values in pure propanol-1 or −2 (150–190 pm) are larger than those in pure water solvent (26 pm for [Formula: see text] 70 pm for the metal ions). The liquid structure influences both the rate of diffusion and the probability of reaction of a reactant encounter pair. Key words: alcohol/water mixed solvents, positive ions, reaction kinetics, solvated electron, solvent effects.

Solvent structure effects on solvated electron reactions in mixed solvents: Negative ions in 1-propanol–water and 2-propanol–water

In models of the kinetics of chemical reactions in solution the solvent is commonly assumed to be a uniform continuum. An example is the Smoluchowski–Debye–Stokes–Einstein equation for the rate constant k2 of a bimolecular reaction between charged or polar species: k2 = κRTfrr/1.5ηrd where κ = probability that a reactant encounter pair will react, R = gas constant, T = temperature, f = Coulombic interaction factor, rr = effective radius for reaction, η = solvent viscosity, and rd = effective radius for mutual diffusion. The equation is useful in evaluating effects of bulk-fluid properties on reaction rates. Residual effects are attributed to more specific solvent behaviour. Rate constants and activation energies E2 of reactions of solvated electrons [Formula: see text] with [Formula: see text] and [Formula: see text] ions vary with the composition of 1-propanol–water and 2-propanol–water mixed solvents. Plots of k2η/fT against solvent composition are nonlinear and change with solvent pair and with reactant pair. Measured molar conductivities Λ0(Li+, [Formula: see text]) and Λ0(2Li+, [Formula: see text]) indicate the solvent dependence of rd for the mutual diffusion of Li+ and [Formula: see text] or [Formula: see text]. The liquid structure influences both the rate of diffusion of the reactants and the probability of reaction of a reactant encounter pair.

Solvent effects on the reactivity of solvated electrons with charged solutes in methanol/water and ethanol/water mixed solvents

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTSolvent effects on the reactivity of solvated electrons with charged solutes in methanol/water and ethanol/water mixed solventsCharles C. Lai and Gordon R. FreemanCite this: J. Phys. Chem. 1990, 94, 12, 4891–4896Publication Date (Print):June 1, 1990Publication History Published online1 May 2002Published inissue 1 June 1990https://doi.org/10.1021/j100375a026RIGHTS & PERMISSIONSArticle Views82Altmetric-Citations10LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InReddit PDF (558 KB) Supporting Info (1)»Supporting Information Supporting Information Get e-Alerts