Adsorption of halide anions on bismuth single crystal plane electrodes

Lust, Karmen; Väärtnõu, Mart; Lust, Enn

doi:10.1016/s0013-4686(00)00432-1

Cited by 57 publications

(78 citation statements)

References 29 publications

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“…However, we can still use B eff for qualitative comparison of mutual interaction of adsorbed ions in different systems. On the other hand, as was shown in [11,19], at r = 0 isotherm (3) yields to the same value of ÀDG A as isotherm (2), so this parameter can be used for further quantitative treatment.…”

Section: Discussionmentioning

confidence: 64%

“…At first sight it seems to be a problem for the present system but since Li + ions are strongly solvated and TEA + cations are practically not solvated, the radii of these ions in the solution are probably comparable [16]. So, it seems that the Hurwitz-Parsons-Dutkiewicz method can be applied to the present system but the possibility exists that systematic errors may be larger than in the case of simple ions [6][7][8][9][10][11][12].…”

Section: Discussionmentioning

confidence: 99%

“…The following calculations of adsorption characteristics were performed similarly to the other ionic systems [8,11,12,18,19]. As was found in these studies, it is not possible to estimate which quantity (r or E) is the better choice as the independent electrical variable.…”

Section: Discussionmentioning

confidence: 99%

“…Thereafter the electrode was carefully rinsed with ultra purified (Millipore) water and ethanol and polarised at E = À1.2 V (against SCE) in the working solutions. All experimental details are more thoroughly described in our previous studies [6,[10][11][12].…”

Section: Methodsmentioning

confidence: 99%

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Adsorption of tetraethylammonium ions on Bi(111) single crystal plane from solutions in ethanol

Väärtnõu

Lust

2006

Journal of Electroanalytical Chemistry

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Section: Discussionmentioning

confidence: 64%

Section: Discussionmentioning

confidence: 99%

Section: Discussionmentioning

confidence: 99%

Section: Methodsmentioning

confidence: 99%

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Adsorption of tetraethylammonium ions on Bi(111) single crystal plane from solutions in ethanol

Väärtnõu

Lust

2006

Journal of Electroanalytical Chemistry

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“…However, while the areas of the peaks "E1" and "E4", and "E3" and "E5" are almost equal, the electrooxidation process of iodide ions in EMImBF 4 (in the reduced pressure conditions) has preserved nearly quasi-reversible charge transfer nature. 39 Two step halide adsorption (including so-called partial charge transfer step) at metal electrodes has been discussed in many papers 35,44,46,47 including strong specific adsorption of I − at Bi(111) and Bi(hkl) planes, 48,49 Au(111) 50 and Ag(111). 51 Very complicated CV curves have been measured for Pt | 1-buthyl-3-methylimidazolium tetrafluoroborate (BMImBF 4 ) + EMImI system (a three step process: i.e.…”

Section: Resultsmentioning

confidence: 99%

Influence of Iodide Ions Concentration on the Stability of 1-Ethyl-3-methylimidazolium Tetrafluoroborate | Molybdenum Carbide Derived Carbon Electrode Interface

Kruusma

Tõnisoo

Pärna

et al. 2017

J. Electrochem. Soc.

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Influence of the iodide ions adsorption on the in situ measured X-ray photoelectron spectra of C 1s, N 1s, B 1s, F 1s and I 3d photoelectrons, indicating the changes in the chemical composition taking place at the carbon (C) | 1-ethyl-3-methylimidazolium tetrafluoroborate (EMImBF 4 ) + 1-ethyl-3-methylimidazolium iodide mixed ionic liquids interface, has been studied. Simultaneously, the stability of the formed C electrode | ionic liquid interface has been analyzed electrochemically. Electroreduction of the BF 4 − anion seems to start at less negative potential than the 1-ethyl-3-methylimidazolium (EMIm + ) cation. Addition of the I − ions to the EMImBF 4 initiates the electrochemical processes at C electrode at lower negative or positive potentials. However, intensity of the electrochemical reduction of EMIm + cation was suppressed. The experiments, performed in the vacuum conditions, indicated that slow faradaic oxidation processes started already at E ≥ 1.0 V (vs. Ag/AgCl in EMImBF 4 ). Our investigations clearly show that the formed passivating layer at the carbon electrode is unstable and decomposes slowly producing gaseous products. Based on the analysis of results collected the electrode materials for electrochemical double layer capacitors should be tested in the vacuum conditions in order to detect the early start of very slow faradaic processes producing gaseous products. Electrochemical double layer capacitors (EDLCs) are one of the electric charge storage systems. Very high specific capacitance values (from 75 to 175 F g −1 for aqueous and from 40 to 100 F g −1 for nonaqueous electrolytes based commercial EDLC cells, 1-3 and 100 -150 F g −1 for micro-mesoporous carbon electrodes or nonaqueous electrolytes and ionic liquid based EDLC cells 4-10 ) have been measured. These devices are also called as "supercapacitors" 1-3,11-17 and used as short term high electric power density systems or as filtering or stabilizing elements in the electric circuits.12,14 It should be noted that the EDLCs are composed of various electrode materials and electrolyte solutions (ionic liquids and non-aqueous solutions are often used [14][15][16][17] ). The power density of an EDLC depends on the mobility of the electrolyte ions (on the electric conductivity of a system 13,14 ) and the specific capacitance depends on the total gravimetric area of the electrode. To expand the specific capacitance of an EDLC the electrochemically active area and/or the applicable cell potential should be increased, because the energy and power densities are root functions of the cell potential.1-17 However, the value of the maximum achievable electrochemically active specific area is limited by the optimal pore diameter determined by the size of the dissolved electrolyte ions (solvated or partially desolvated 8 ) and the solvent molecules dimensions. Thus, the expansion of the applicable cell potential seems to be the only solution for the significant expansion of the EDLCs specific energy (measured in Wh kg −1 ) and specific power (measured i...

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Iodine as a Temperature‐Responsive Redox Shuttle Additive for Swelling Suppression of Lithium‐Ion Batteries at Elevated Temperatures

et al. 2016

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The swelling issue by gas evolution at elevated temperatures (85–90 °C) is one of the major challenges related to current Li‐ion batteries (LIBs). We herein demonstrate that iodine (I2) as a redox shuttle additive, when its dose is properly determined, can suppress the swelling behavior of LiCoO2/graphite Al‐pouch cells during storage at 90 °C without sacrificing other cell performances. This approach is based on two findings: 1) swelling during 90 °C storage is severe only when the cells are fully charged, and 2) the shuttling reaction of I2 can be tuned to be activated only when the temperature is as high as 90 °C by employing an appropriate amount of I2. Therefore, when a fully charged cell is exposed to a temperature of 90 °C, the self‐discharge by I2 lowers the state of charge of the cell, suppressing the swelling. This temperature‐responsive shuttling behavior of I2 is ascribed to the preferential adsorption of I2 on the cathode surface. It is also confirmed that inclusion of the I2 additive does not lead to deterioration in other aspects of cell performance, such as the discharge capacity or long‐term cyclability. Along with the improved cell performance, the low‐cost and environmental compatibility of I2 makes it a promising electrolyte additive for thermally robust LIBs.

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Adsorption of halide anions on bismuth single crystal plane electrodes

Cited by 57 publications

References 29 publications

Adsorption of tetraethylammonium ions on Bi(111) single crystal plane from solutions in ethanol

Adsorption of tetraethylammonium ions on Bi(111) single crystal plane from solutions in ethanol

Influence of Iodide Ions Concentration on the Stability of 1-Ethyl-3-methylimidazolium Tetrafluoroborate | Molybdenum Carbide Derived Carbon Electrode Interface

Iodine as a Temperature‐Responsive Redox Shuttle Additive for Swelling Suppression of Lithium‐Ion Batteries at Elevated Temperatures

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