Solution and Flotation Chemistry of Sulfide Minerals

Pritzker, Mark; Yoon, R. U.; Basilio, C.I.; Vincent, Choi, Wing-sang,

doi:10.1179/cmq.1985.24.1.27

Cited by 15 publications

(8 citation statements)

References 12 publications

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“…The compound is also a mixed electronic and ionic (copper) conductor. The compound has become of interest for several unconnected reasons: as a source of copper metal (natural ore) [1][2][3][4][5], for its photovoltaic properties [6][7][8][9], and for fundamental studies [10][11][12][13][14][15]. For each of these aspects, Cu diffusion has to be taken into account.…”

Section: Introductionmentioning

confidence: 99%

Copper diffusion in copper sulfide: a systematic study

Cassaignon

Pauporté

Guillemoles

et al. 1998

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Abstract.Copper sulfide Cu2_xS is a model mineral for chalcogenides because of the existence of a non-stoichiometric compounds series in the range Cu2S -CuS in which properties change with x. For this reason, we have studied the influence of the mineral composition on the diffusion in this solid.Electrochemical Impedance Spectroscopy (EIS) applied to CU2_xS/cupric sulfate electrolyte was the main investigation technique. It enabled us to work at the equilibrium potential at which the composition is fixed and known. Changing the composition by electrochemically removing (or adding) a known amount of Cu, we were able to determine the chemical diffusion coefficient of copper in the composition range (from x = 0 to 0.066). In this work, we present the results obtained in the chalcocite and djurleite phases. These results were compared to other values reported in the literature. From this systematic study we discuss various diffusion mechanisms. Our observations support that in chalcocite and djurleite Cu diffuses via a vacancy mechanism.

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Section: Introductionmentioning

confidence: 99%

Copper diffusion in copper sulfide: a systematic study

Cassaignon

Pauporté

Guillemoles

et al. 1998

Ionics

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“…Numerous electrochemical and spectroscopic studies of its interactions with galena PbS, 1-12 silver, [13][14][15] silver sulfide, 15 copper, [16][17][18][19][20] and copper sulfide 3,11,18, have been published. The generally recognized adsorption mechanism of EtX Ϫ occurs by two steps a charge transfer induced chemisorption process EtX Ϫ r EtX ads ϩ e Ϫ [1] the formation of the M-EtX compound EtX Ϫ ϩ M r M-EtX ϩ e Ϫ for a metal or [2] EtX Ϫ ϩ MS r M-EtX ϩ S ϩ e Ϫ for a sulfide [3] The ethylxanthate anion is chemically bound to the metal atom that remains in the copper sulfide crystal structure after the first step. Underpotential deposition (UPD) is invoked and can be used to explain the formation of such an adsorbed ethylxanthate.…”

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confidence: 99%

“…Ethylxanthate (EtX Ϫ ) is a typical member of the o-alkyldithiocarbonates R-O-CS 2Ϫ collector family. Numerous electrochemical and spectroscopic studies of its interactions with galena PbS, [1][2][3][4][5][6][7][8][9][10][11][12] silver, [13][14][15] silver sulfide, 15 copper, [16][17][18][19][20] and copper sulfide 3,11,18, have been published. The generally recognized adsorption mechanism of EtX Ϫ occurs by two steps a charge transfer induced chemisorption process EtX Ϫ r EtX ads ϩ e Ϫ [1] the formation of the M-EtX compound…”

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Ethylxanthate Adsorption on Copper Sulfide Influence of the Copper Sulfide Composition

Cassaignon

Gomez‐Meier

Vedel

2000

J. Electrochem. Soc.

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In this work, the influence of a mineral composition (copper sulfide) on the adsorption of a surfactant molecule used for mineral flotation is studied. Flotation is the method used to separate minerals (e.g., copper minerals) from gangue. The process is based on the adsorption of air bubbles on the particles of the mineral making them lighter than water and giving the possibility of separation. The extent of adsorption of air bubbles depends on the mineral hydrophobicity and is improved by adding a surfactant molecule (the collector) which adsorbs on the mineral particles in the ore suspension.Ethylxanthate (EtX Ϫ ) is a typical member of the o-alkyldithiocarbonates R-O-CS 2Ϫ collector family. Numerous electrochemical and spectroscopic studies of its interactions with galena PbS, 1-12 silver, 13-15 silver sulfide, 15 copper, [16][17][18][19][20] and copper sulfide 3,11,18,21-48 have been published. The generally recognized adsorption mechanism of EtX Ϫ occurs by two steps a charge transfer induced chemisorption process EtX Ϫ r EtX ads ϩ e Ϫ [1] the formation of the M-EtX compound EtX Ϫ ϩ M r M-EtX ϩ e Ϫ for a metal or [2]The ethylxanthate anion is chemically bound to the metal atom that remains in the copper sulfide crystal structure after the first step. Underpotential deposition (UPD) is invoked and can be used to explain the formation of such an adsorbed ethylxanthate. 3,11,18, After the second step, the metal has left the crystalline framework and binds to the ethylxanthate ions to form the compound M-EtX. Both steps involve electron transfer and may be observed by electrochemical methods such as voltammetry. In the case of copper, 16,18,36 the chemisorption peak (sometimes split into two subpeaks) has been observed at about Ϫ0.46 V vs. standard hydrogen electrode (SHE), followed by the Cu-EtX formation at Ϫ0.250 V vs. SHE. On copper sulfide, 3,11,18,21,25,33,36,40,44 all the authors refer to two chemisorption peaks followed by the formation of Cu-EtX multilayers. However, from one study to another the characteristic potentials vary between Ϫ0.346 and Ϫ0.130 V vs. SHE for the first peak and between Ϫ0.256 and Ϫ0.360 V vs. SHE for the second one, whereas the second step of the mechanism takes place between 0.115 and 0.120 V vs. SHE. It is known that at room temperature, the copper-sulfur phase diagram shows four stable and distinct phases: chalcocite (Cu 2 S), djurleite (Cu 1.96 S), anilite (Cu 1.75 S), and covellite (CuS). 49-57 Each phase presents a small domain of deviation from ideal composition. For instance, the chalcocite domain extends from Cu/S ϭ 2 to Cu/S ϭ 1.993. Thus, the copper sulfide formula is generally represented by Cu 2Ϫx S; x being called the deviation from stoichiometry (0 < x < 1). The exact composition of the sulfide used for these studies is not always specified; it is often referenced as chalcocite (Cu 2 S) but without a precise indication of composition verification. This indicates that according to the copper sulfide composition, the ethylxanthate adsorption is not carried out in the...

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“…The proIt has become common during the last few years to use ther-posed mechanism is modynamics as a tool in explaining the behavior of flotation systems. Powerful computer programs allow the comprehensive calculations needed to determine the concentrations of possible species in different flotation systems [1][2][3][4][5]. Until now the calculations have been based on the tabulated thermodynamic data of existing bulk compounds such as metal-eollector complexes.…”

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Calculations of Thermodynamic Equilibria in Lead Sulfide Surface–Thiol Collector Systems, Part I: Ethyl Xanthate Ion as Collector

Rastas¹,

Stén²,

Leppinen³

1990

Canadian Metallurgical Quarterly

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The chemisorption of ethyl xanthate ion on lead sulfide surface is examined by means of thermodynamic calculations with special attention to the surface behavior. The calculations are based on balance equations written in terms of equilibrium constants and solved to determine the surface coverage and the concentrations of various species under different conditions. The calculations cover various ways of regulating the chemisorption such as the addition of oxygen, sodium sulfide, sulfuric acid, and sodium hydroxide, the evaporation of hydrogen sulfide, and change in the initial concentration of the collector.

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Solution and Flotation Chemistry of Sulfide Minerals

Cited by 15 publications

References 12 publications

Copper diffusion in copper sulfide: a systematic study

Copper diffusion in copper sulfide: a systematic study

Ethylxanthate Adsorption on Copper Sulfide Influence of the Copper Sulfide Composition

Calculations of Thermodynamic Equilibria in Lead Sulfide Surface–Thiol Collector Systems, Part I: Ethyl Xanthate Ion as Collector

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