A new method for practical electrodeposition of aluminium from ionic liquids

Bakkar, Ashraf; Neubert, Volkmar

doi:10.1016/j.elecom.2014.12.012

Cited by 81 publications

(47 citation statements)

References 14 publications

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“…For all the organic AlCl 3 ‐based electrolytes described above, the moisture sensitivity limits their application. However, reversible aluminum deposition under ambient conditions has been achieved using a floating layer of alkane or decane, which is moisture‐insensitive and does not react with the electrolyte . A polymer‐gel electrolyte that enables reversible aluminum deposition has also been prepared to reduce moisture sensitivity in the chloroaluminate ionic‐liquid electrolyte …”

Section: Alcl3‐based Electrolytes For Aluminum Batteriesmentioning

confidence: 99%

Halide‐Based Materials and Chemistry for Rechargeable Batteries

et al. 2020

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Rechargeable batteries are considered one of the most effective energy storage technologies to bridge the production and consumption of renewable energy. The further development of rechargeable batteries with characteristics such as high energy density, low cost, safety, and a long cycle life is required to meet the ever‐increasing energy‐storage demands. This Review highlights the progress achieved with halide‐based materials in rechargeable batteries, including the use of halide electrodes, bulk and/or surface halogen‐doping of electrodes, electrolyte design, and additives that enable fast ion shuttling and stable electrode/electrolyte interfaces, as well as realization of new battery chemistry. Battery chemistry based on monovalent cation, multivalent cation, anion, and dual‐ion transfer is covered. This Review aims to promote the understanding of halide‐based materials to stimulate further research and development in the area of high‐performance rechargeable batteries. It also offers a perspective on the exploration of new materials and systems for electrochemical energy storage.

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Section: Alcl3‐based Electrolytes For Aluminum Batteriesmentioning

confidence: 99%

Halide‐Based Materials and Chemistry for Rechargeable Batteries

et al. 2020

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“…49 On the basis of this data, we can say that the chloroaluminate RTIL is stable below 363 K. However, decomposition of the [C 2 mim] + cation, especially through cleavage of the alkyl chain, is initiated at 368 K. 50 In order to simplify the conditions for practical plating, two different research groups have proposed a biphasic plating bath for the electrodeposition of Al from chloroaluminates in air by covering the bath with a layer of an immiscible, low vapor pressure hydrophobic organic solvent, such as decane. 51,52 Toluene has been considered also. 51 This practice may seem to facilitate the Al electroplating process, but it may also induce variations in the physicochemical properties and ionic/chemical speciation in the plating bath during long-term operations.…”

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confidence: 99%

Review—Electrochemical Surface Finishing and Energy Storage Technology with Room-Temperature Haloaluminate Ionic Liquids and Mixtures

Tsuda

Stafford

Hussey

2017

J. Electrochem. Soc.

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In this article, we review the progress in the area of electrochemical technology with Lewis acidic haloaluminate room-temperature ionic liquids (RTILs), such as AlCl 3 -1-ethyl-3-methylimidazolium chloride and AlBr 3 -1-ethyl-3-methylimidazolium bromide, and novel chloroaluminate mixtures consisting of AlCl 3 and polarizable molecules, e.g., dimethylsulfone and urea, during this decade. The number of researchers in the field seems to increase steadily, because now we can handle haloaluminate RTILs and their mixtures with other solvents and materials more easily than we could in the past. In this review, we have categorized the electrochemical technology based on these RTILs into two topics: electroplating and energy storage. In fact, much of the current research is based on work begun during the period from ∼1970 until the 1990's. Room-temperature ionic liquids (RTILs), which is a name synonymous with room-temperature molten salts, have received considerable attention as novel reaction media, liquid materials, and starting materials for functional carbon material. (The name "ionic liquid" was arbitrarily chosen to represent what are actually salts that liquefy at temperatures below 373 K.) The interest in these materials stems from their favorable physicochemical properties, such as low-flammability, negligible vapor pressure, relatively high ionic conductivity, and high electrochemical stability. [1][2][3][4][5][6][7] It is now common knowledge in the chemistry community that many RTILs are stable in air or even water. The "first generation ionic liquids" were difficult to handle because the typical anions known at that time, e.g., AlCl 4 − and Al 2 Cl 7 − , reacted strongly with moisture in the air. Only a very limited number of laboratories with special skills for handling them could effectively use these RTILs. No doubt, the flourishing interest in RTIL chemistry was heavily abetted by the discovery of air and water stable systems, i.e., the so-called "second generation ionic liquids".However, we should not devalue the first generation systems such as those based on quaternary organic halide salts and aluminum halides, e.g., AlBr 3 and AlCl 3 , known as haloaluminates. The reactivity of the haloaluminates as well as their adjustable Lewis acidity is precisely what makes them interesting and very versatile. By contrast, the second-generation "inert" ionic liquids, are just that: inert and nonreactive, both chemically and electrochemically. Furthermore, the ionic conductivity and viscosity of the haloaluminates, which are important factors for the electrochemical applications described herein, exceed those for the comparable second-generation RTILs. For example, the ionic conductivity and viscosity for 60.0-40.0 mole percent (or 60 mol%) AlCl 3 -1-ethyl-3-methylimidazolium chloride ([C 2 mim]Cl) are 17.1 mS cm −1 and 15.35 mPa s, respectively, at 298 K.8 (In the interest of brevity, we will refer to the composition of these ionic liquids by simply stating only the amount of the aluminum halide.) On the other ...

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“…[75][76][77][78][79][80][81][82][83][84][85] Aluminum, therefore, does not deposit from neutral or basic melts (excess of EMIMCl). The mixture becomes liquid at room temperature (an ionic liquid) due to the acid-base reaction between AlCl 3 (Lewis acid) and Cl − (Lewis base) forming AlCl 4 − anions charge-balanced with, for instance, EMIM + cation.…”

Section: Aluminum Gdibsmentioning

confidence: 99%

Rechargeable Dual‐Ion Batteries with Graphite as a Cathode: Key Challenges and Opportunities

Kravchyk

Kovalenko

2019

Advanced Energy Materials

116

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friendliness. Additionally, there are numerous additional electrochemical battery performance characteristics that play an equally important role such as longterm cycling performance (cycle life), calendar life, Coulombic efficiency (measure for charge loss due to irreversible side reactions), energy efficiency, and the performance at different charge/discharge rates or at different temperatures. From this perspective, researchers constantly explore new anode and cathode materials for existing battery technologies as well as conceive new electrochemical energy storage concepts. In this context, the last two decades have seen a surge of reports on various low-cost anodes and cathodes for Li-ion and post-Li-ion batteries (Na-, K-, Ca-, Mg-, and Al-ion batteries). Moreover, new electrochemical concepts called graphite dual-ion batteries (GDIBs) have recently attracted significant attention. GDIBs show high potential for the use in grid-scale energy storage applications due to their low cost, relatively high energy densities of up to ≈200 Wh kg −1 and cyclic stability (thousands of cycles and potentially more). In this review, we provide an introduction to the basics of GDIBs. In particular, we discuss their operating mechanisms and cover the topic of energy density calculations. In addition, we highlight the importance of correct reporting of the performance metrics with respect to the energy density of GDIBs. Next, we discuss in detail factors governing the electrochemical performance of graphite cathodes in dual-ion batteries, such as graphite structure, morphology, and particle size. The factors that impact the voltage of electrochemical anion intercalation/deintercalation into graphite will be described as well. With respect to the practical application of the GDIBs, the current collector issues and volume changes of GDIBs will be discussed in the final sections. Historical AspectsAlthough GDIBs may appear to be newcomers in battery research, they have a long and tangible history. The concept of GDIBs was introduced in the patents of McCullough et al. [1,2] in 1989. The experimental example consisted of two graphite electrodes acting as an anode and a cathode, and a 15 wt% solution of LiClO 4 in propylene carbonate acting as an electrolyte. The oxidation and reduction of cathodic and anodic graphite electrodes occur with concomitant intercalation of Li + cations and ClO 4 − anions, respectively. The latter process is known as the formation of donor-type (cationic) or acceptor-type (anionic) graphite intercalation compounds (GICs). Some years later, in the 1990s, the intercalation of various anions into graphite Rechargeable graphite dual-ion batteries (GDIBs) have attracted the attention of electrochemists and material scientists in recent years due to their low cost and high-performance metrics, such as high power density (≈3-175 kW kg −1 ), energy efficiency (≈80-90%), long cycling life, and high energy density (up to 200 Wh kg −1 ), suited for grid-level stationary storage of electricity.The key feature of GD...

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A new method for practical electrodeposition of aluminium from ionic liquids

Cited by 81 publications

References 14 publications

Halide‐Based Materials and Chemistry for Rechargeable Batteries

Halide‐Based Materials and Chemistry for Rechargeable Batteries

Review—Electrochemical Surface Finishing and Energy Storage Technology with Room-Temperature Haloaluminate Ionic Liquids and Mixtures

Rechargeable Dual‐Ion Batteries with Graphite as a Cathode: Key Challenges and Opportunities

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