Aluminium electrodeposition under ambient conditions

Abbott, Andrew P.; Harris, Robert C.; Hsieh, Yi‐Ting; Ryder, Karl S.; Sun, I‐Wen

doi:10.1039/c4cp01508h

Cited by 141 publications

(136 citation statements)

References 18 publications

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“…Abbott et al reported the NMR spectra of cationic complexes derived from AlCl 3 and urea mixtures. They also outlined the effect of diluent on the resolution of the NMR spectra of these species [35].…”

Section: Resultsmentioning

confidence: 99%

Electrodeposition of Al from a 1-butylpyrrolidine-AlCl3 ionic liquid

Pulletikurthi

Bödecker

Borodin

et al. 2015

Progress in Natural Science: Materials International

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The addition of 1-butylpyrrolidine to AlCl 3 results in the formation of an electrolyte that is suited to Al deposition. The feasibility of electrodepositing Al from the synthesized electrolyte was investigated. Several compositions of AlCl 3 and 1-butylpyrrolidine were prepared for this purpose. These mixtures show a different phase behavior at various compositions of AlCl 3 and 1-butylpyrrolidine. IR, Raman and NMR spectroscopy were employed to characterize the synthesized liquids. Among the prepared compositions, 1:1.2 mol ratio of 1-butylpyrrolidine: AlCl 3 and the upper phase of 1:1.3 mol ratio of 1-butylpyrrolidine:AlCl 3 were found to be suitable for Al electrodeposition at room temperature (RT). Uniform and thick ( $mm thick) layers of Al were obtained on copper at RT. Al deposition occured from the cationic species of AlCl 3 À x L þ y (where x r2, y ¼ 1-2, and L¼1-butylpyrrolidine) in this electrolyte. This behavior is contrary to the well investigated classic AlCl 3 based ionic liquids, where the deposition of Al occurs mainly from anionic Al 2 Cl À 7 ions.

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Section: Resultsmentioning

confidence: 99%

Electrodeposition of Al from a 1-butylpyrrolidine-AlCl3 ionic liquid

Pulletikurthi

Bödecker

Borodin

et al. 2015

Progress in Natural Science: Materials International

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“…2AlCl3 + urea → [AlCl2.urea] + + AlCl4 -These liquids have been studied for metal deposition applications. 6 Gambino et al 7 have…”

Section: Introductionmentioning

confidence: 99%

Do group 1 metal salts form deep eutectic solvents?

Abbott

D’Agostino

Davis

et al. 2016

Phys. Chem. Chem. Phys.

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Mixtures of metal salts such as ZnCl2, AlCl3 and CrCl3·6H2O form eutectic mixtures with complexing agents, such as urea, liquids. The aim of this research was to see if alkali metal salts also formed eutectics in the same way. It is shown that only a limited number of sodium salts form homogeneous liquids at ambient temperatures and then only with glycerol. None of these mixtures showed eutectic behaviour but the liquids showed the physical properties similar to the group of mixtures classified as deep eutectic solvents. This study focussed on four sodium salts: NaBr, NaOAc, NaOAc·3H2O and Na2B4O7·10H2O. The ionic conductivity and viscosity of these salts with glycerol were studied, and it was found that unlike previous studies of quaternary ammonium salts with glycerol, where the salt decreased the viscosity, most of the sodium salts increased the viscosity. This suggests that sodium salts have a structure making effect on glycerol. This phenomenon is probably due to the high charge density of Na + , which coordinates to the glycerol. 1 H and 23 Na NMR diffusion and relaxation methods have been used to understand the molecular dynamics in the glycerol-salt mixtures, and probe the effect of water on some of these systems. The results reveal a complex dynamic behaviour of the different species within these liquids. Generally, the translational dynamics of the 1 H species, probed by means of PFG NMR diffusion coefficients, is in line with the viscosity of these liquids. However, 1 H and 23 Na T1 relaxation measurements suggest that the Na-containing species also play a crucial role in the structure of the liquids.

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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.…”

mentioning

confidence: 99%

“…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. Thus, more investigations of this promising, but largely untested strategy are warranted.…”

mentioning

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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Aluminium electrodeposition under ambient conditions

Cited by 141 publications

References 18 publications

Electrodeposition of Al from a 1-butylpyrrolidine-AlCl3 ionic liquid

Electrodeposition of Al from a 1-butylpyrrolidine-AlCl3 ionic liquid

Do group 1 metal salts form deep eutectic solvents?

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

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