Electrochemical copper deposition from an ethaline-CuCl2·2H2O DES

Swatilekha Ghosh, Sudipta Roy

Research output: Contribution to journalArticle

27 Citations (Scopus)

Abstract

Cu electroplating was carried out using a pure ethaline melt, a 1:2 ratio of choline chloride and ethylene glycol, at room temperature by potentiostatic and galvanostatic methods. Hydrated cupric chloride was added to the pure ethaline melt. Polarisation data for cupric ion reduction to copper was collected using an RDE to determine where metal deposition was feasible. Smooth Cu deposits were obtained at -4.7×10-3A/cm2 using 0.2M CuCl2·2H2O at 25°C at a current efficiency of (95±5)% at a rotation speed of 700rpm. XRD analysis of the deposit showed a polycrystalline face centred cubic structure with (111) texture. The crystalline size was 66±10nm with some internal strain. EDX analysis showed the presence of carbon and chlorine with copper in the deposit, which was due to the break-down of the DES. Several deposition processes were carried out from a single bath to examine bath stability. The bath was found to be stable when a soluble anode was employed, and became unstable when an insoluble anode was used due to other reactions proceeding at the cathode.

LanguageEnglish
Pages165-173
Number of pages9
JournalSurface and Coatings Technology
Volume238
DOIs
Publication statusPublished - 15 Jan 2014

Fingerprint

Copper
baths
Deposits
deposits
copper
Anodes
anodes
chlorides
choline
Ethylene Glycol
Chlorine
electroplating
Electroplating
Choline
Ethylene glycol
chlorine
glycols
Energy dispersive spectroscopy
Cathodes
ethylene

Keywords

  • choline chloride
  • copper deposition
  • electrodeposition
  • electroplating
  • ethaline
  • ionic liquids

Cite this

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abstract = "Cu electroplating was carried out using a pure ethaline melt, a 1:2 ratio of choline chloride and ethylene glycol, at room temperature by potentiostatic and galvanostatic methods. Hydrated cupric chloride was added to the pure ethaline melt. Polarisation data for cupric ion reduction to copper was collected using an RDE to determine where metal deposition was feasible. Smooth Cu deposits were obtained at -4.7×10-3A/cm2 using 0.2M CuCl2·2H2O at 25°C at a current efficiency of (95±5){\%} at a rotation speed of 700rpm. XRD analysis of the deposit showed a polycrystalline face centred cubic structure with (111) texture. The crystalline size was 66±10nm with some internal strain. EDX analysis showed the presence of carbon and chlorine with copper in the deposit, which was due to the break-down of the DES. Several deposition processes were carried out from a single bath to examine bath stability. The bath was found to be stable when a soluble anode was employed, and became unstable when an insoluble anode was used due to other reactions proceeding at the cathode.",
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Electrochemical copper deposition from an ethaline-CuCl2·2H2O DES. / Ghosh, Swatilekha; Roy, Sudipta.

In: Surface and Coatings Technology, Vol. 238, 15.01.2014, p. 165-173.

Research output: Contribution to journalArticle

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AB - Cu electroplating was carried out using a pure ethaline melt, a 1:2 ratio of choline chloride and ethylene glycol, at room temperature by potentiostatic and galvanostatic methods. Hydrated cupric chloride was added to the pure ethaline melt. Polarisation data for cupric ion reduction to copper was collected using an RDE to determine where metal deposition was feasible. Smooth Cu deposits were obtained at -4.7×10-3A/cm2 using 0.2M CuCl2·2H2O at 25°C at a current efficiency of (95±5)% at a rotation speed of 700rpm. XRD analysis of the deposit showed a polycrystalline face centred cubic structure with (111) texture. The crystalline size was 66±10nm with some internal strain. EDX analysis showed the presence of carbon and chlorine with copper in the deposit, which was due to the break-down of the DES. Several deposition processes were carried out from a single bath to examine bath stability. The bath was found to be stable when a soluble anode was employed, and became unstable when an insoluble anode was used due to other reactions proceeding at the cathode.

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