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Review

The Thermodynamics of Selenium Minerals in Near-Surface Environments

by
Vladimir Krivovichev
1,*,
Marina Charykova
2 and
Andrey Vishnevsky
2
1
Department of Mineralogy, Institute of Earth Sciences, St. Petersburg State University, 7/9 University Embankment, Saint Petersburg 199034, Russia
2
Department of Geochemistry, Institute of Earth Sciences, St. Petersburg State University, 7/9 University Embankment, Saint Petersburg 199034, Russia
*
Author to whom correspondence should be addressed.
Minerals 2017, 7(10), 188; https://doi.org/10.3390/min7100188
Submission received: 18 August 2017 / Revised: 3 October 2017 / Accepted: 4 October 2017 / Published: 6 October 2017
(This article belongs to the Special Issue Se-Bearing Minerals: Structure, Composition, and Origin)
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Abstract

:
Selenium compounds are relatively rare as minerals; there are presently only 118 known mineral species. This work is intended to codify and systematize the data of mineral systems and the thermodynamics of selenium minerals, which are unstable (selenides) or formed in near-surface environments (selenites), where the behavior of selenium is controlled by variations of the redox potential and the acidity of solutions at low temperatures and pressures. These parameters determine the migration of selenium and its precipitation as various solid phases. All selenium minerals are divided into four groups—native selenium, oxide, selenides, and oxysalts—anhydrous selenites (I) and hydrous selenites and selenates (II). Within each of the groups, minerals are codified according to the minimum number of independent elements necessary to define the composition of the mineral system. Eh–pH diagrams were calculated and plotted using the Geochemist’s Workbench (GMB 9.0) software package. The Eh–pH diagrams of the Me–Se–H2O systems (where Me = Co, Ni, Fe, Cu, Pb, Zn, Cd, Hg, Ag, Bi, As, Sb, Al and Ca) were plotted for the average contents of these elements in acidic waters in the oxidation zones of sulfide deposits. The possibility of the formation of Zn, Cd, Ag and Hg selenites under natural oxidation conditions in near surface environments is discussed.

1. Introduction

Selenium release and pollution is a worldwide phenomenon that results from a wide variety of anthropogenic activities, such as agriculture, mining, and other process industries [1]. Selenium is a potentially toxic element, and mining-related selenium release was a major concern during the last decade as high concentrations were reported at some mine sites [2,3]. Selenium contamination is vast, affecting both aquatic and terrestrial ecosystems, and has therefore attracted the attention of natural resource and water quality regulators around the world [4,5]. Due to the high mobility of selenium in oxidizing geochemical environments, the behavior of selenium is also important in safety analyses of radioactive waste repositories [6,7]. Khamkhash et al. [1] reported a brief introduction to selenium chemistry and toxicity, presented a detailed review of currently available techniques for removing selenium from industrial/mining wastewater, and discussed mining-related selenium contamination from Alaskan mines. Se mobility, bioavailability and toxicity are controlled by the various possible oxidation states (the most common being −2, 0, +4 and +6) that prevail under various conditions. These characteristics of selenium are affected by the redox conditions and the pH, which also plays a crucial role in selenium behavior in near-surface environments.
The oxidation zone of selenide or selenium-bearing sulfide deposits is one of the prime contributors of selenium release into the environment. The mining of coal, precious metals (gold and silver), and metallic sulfides are key contributors of selenium from mining operations [2] exposing selenium-bearing compounds to air and water. This mobilizes selenium into aquatic systems where it bioaccumulates in the food chain, thereby escalating its hazardous effects [1].
Previously, we have characterized the selenium oxysalts (selenites and selenates) and evaluated the accuracy of the thermodynamic constants of the selenites [8]. The objective of this paper is to characterize all selenium minerals as natural mineral systems and to review the thermodynamic constants of the selenium minerals, which are unstable or formed during the oxidation of selenides and selenium-bearing sulfide ores, and to propose data at the standard state (25 °C, 1 bar pressure).

2. Materials and Methods

2.1. Mineral Systems of Selenium Minerals

The selenium minerals are relatively rare in nature; only 118 mineral species are presently known (Supplementary Table S1). As shown [9,10], any mineral can be assigned to a specific system, each component of which is a species-defining chemical element (cf. [11,12,13]) determined by the rules of the new mineral species definition [14,15,16]. For mineral coding, we used the sequence of species-defining chemical element symbols according to the so-called “thermochemical” sequence of chemical elements (Figure 1) [9,10]. For example, giraudite, Cu6Cu4Zn2(AsSe3)4S, responds to the system SSeAsZnCu, while prewittite, K2Pb3Zn2Cu12(SeO3)4O4Cl20, responds to the system OClSePbZnCuK.
As in all contemporary mineral classifications, selenium minerals is clearly divided into four groups—native selenium, oxide, selenides, and oxysalts—anhydrous selenites (I) and hydrous selenites and selenates (II). Within each of these groups, minerals can be classified according to the minimum number of components required for their formation [9,10]. The proposed classification of selenium mineral systems is given in Table 1. An important advantage of this classification of selenium mineral systems is the ability to use computer technology to organize, store and retrieve thermodynamic data.

2.2. Thermodynamics

The physico-chemical modeling of mineral equilibria is based on the thermodynamic constants of minerals and aqueous species (values of the Gibbs energy of formation, ΔfG0298). These data are mostly calculated from calorimetric measurements (e.g., [19,20,21,22,23,24,25,26,27,28,29,30,31,32,33,34]) or experimental determinations of solubility (e.g., [35,36,37,38,39,40,41,42,43,44]). Such works are very numerous; their results are not always consistent with each other. A detailed analysis of all thermodynamic data for selenium minerals is beyond the scope of this article; this can be found, for example, in the review [45], and primarily in the reference book [46], which presents a scrupulous critical review of all the published experimental measurements. We used this reference book [46] in the preparation of Table 1, which contains the values of the Gibbs energy of formation (ΔfG0298) for selenium minerals and their synthetic analogues. Additional thermodynamic data (ΔfG0298 for solid phases not containing selenium and aqueous species) for the calculation of diagrams have been taken from [47]. In addition, some of our recent articles were used as sources of ΔfG0298 for certain selenites [17,18,48,49]. It should be emphasized that the values of the Gibbs energy of formation are known only for 25 (Table 1) of the 118 selenium minerals.

3. Results and Discussion

Thermodynamic modeling of the mineral-forming processes in the oxidation zone of ore deposits is based on the analysis of Eh–pH diagrams. In this study, the calculation and construction of Eh–pH diagrams were carried out by means of the Geochemist’s Workbench software (GMB 9.0) [50]. The calculation of the diagrams was predated by the introduction of new thermodynamic data and some elements (Cd, Sb, Bi) into the database and the specification of some constants. The activity coefficients were calculated with the Debye–Hückel equation. Eh–pH diagrams of Me–Se–H2O systems (where Me = Co, Ni, Fe, Cu, Pb, Zn, Cd, Hg, Ag, Bi, As, Sb, Al and Ca) have been constructed for the average contents of these elements in acidic waters of the oxidation zones of sulfide deposits [51]. It should be noted that Eh–pH diagrams of Me–Se–H2O systems (where Me = Co, Ni, Fe, Cu, Pb, Zn, Al and Ca) have been discussed in detail previously [8] and therefore we present here only their brief description.

3.1. Thermodynamic System Co–Se–H2O

In this system, three selenides (bornhardtite, CoCo2Se4; freboldite, CoSe; and trogtalite, CoSe2) and one selenite (cobaltomenite, CoSeO3∙2H2O) were reported. For cobalt selenides the thermodynamic data are known only for trogtalite and freboldite (Table 1). These data were used for plotting the Eh–pH diagram of the Co–Se–H2O system (Figure 2). The thermal stability, solubility and thermochemical calorimetric investigations were carried out on a synthetic analogue of cobaltomenite [49,52,53]. The Eh–pH diagram of the Co–Se–H2O system (Figure 2) contains, in addition to the stability field of native selenium, a stability field of Co3O4, which is unknown in nature, and the stability field of trogdalite. Cobaltomenite appears in the environment covering the pH range of 4.5 to 7.5, while Eh is not too high.

3.2. Thermodynamic System Ni–Se–H2O

In this system six selenides (sederholmite, and mäkinenite, NiSe; penroseite, and kullerudite, NiSe2; trüstedtite, and wilkmanite, NiNi2Se4) were reported, but the thermodynamic data are known only for penroseite and sederholmite (Table 1). These data were used for plotting the Eh–pH diagram of the Ni–Se–H2O system (Figure 3). The thermal stability, the solubility and the thermochemical calorimetric investigations were carried out on a synthetic analogue of ahlfeldite [49,52,53]. The Eh–pH diagram of the Ni–Se–H2O system (Figure 3) contains the stability fields of native selenium, penroseite and sederholmite, and a wide field of bunsenite. Ahlfeldite appears in the environment covering the pH range of 4.3 to 8.2, while the Eh is not too high at the temperature fluctuations corresponding to the environmental conditions.

3.3. Thermodynamic System Fe–Se–H2O

The Table 1 shows that in this system, three selenides (achávalite, FeSe; dzharkenite, and ferroselite, FeSe2), native selenium, and one selenite, mandarinoite (Fe2(SeO3)3·6H2O), were reported. The composition, solubility, and the thermal behavior of iron selenite were discussed earlier [8]. Figure 4 presents Eh–pH diagrams of the Fe–Se–H2O system, which contains wide stability fields of native selenium, hematite and ferroselite, and small fields corresponding to the crystallization of oxides (magnetite, wüstite). The field of mandarinoite appears in acid areas at a high positive Eh.

3.4. Thermodynamic System Cu–Se–H2O

In this thermodynamic system, nine selenides (klockmannite, CuSe; krut’aite, petříčekite, and bambollaite, CuSe2; bellidoite, and berzelianite, Cu2Se; umangite, Cu3Se2; athabascaite, Cu5Se4; geffroyite, Cu9Se8) were reported, but the thermodynamic data are only available for CuSe (Table 1) and it was used for plotting the Eh–pH diagram of the Cu–Se–H2O system (Figure 5). Also in this system, two natural polymorphous modifications exist among water-containing selenites without additional anions. They have the CuSeO3·2H2O formula: chalcomenite (orthorhombic) and clinochalcomenite (monoclinic). Chalcomenite is the more abundant mineral; clinochalcomenite is poorly documented and remains a controversial mineral species. The thermal stability, the solubility and thermochemical calorimetric investigations were carried out on a synthetic analogue of chalcomenite [17,54,55].
The Eh–pH diagram of the Cu–Se–H2O system is shown in Figure 5. It is seen that klockmannite, copper oxides (cuprite, tenorite), native selenium, and native copper (in the alkaline region of negative Eh) are stable. Chalcomenite (CuSeO3·2H2O) occurs in a slightly acid environment and at a rather high positive Eh.

3.5. Thermodynamic System Pb–Se–H2O

In this thermodynamic system, one selenide (clausthalite, PbSe), and two anhydrous lead selenites (molybdomenite, PbSeO3, and plumboselite, Pb3(SeO3)O2) were reported (Table 1), but the thermodynamic data are only available for PbSe, and PbSeO3 (Table 1). These data were used for plotting the Eh–pH diagram of the Pb–Se–H2O system (Figure 6). The greatest part of the diagram contains stability fields of solid phases and is characterized by the fields of native selenium, claustalite (PbSe), plattnerite (PbO2), litharge (Pb3O4) and massicot (PbO). It is noteworthy that a wide stability field of molybdomenite (PbSeO3) appears covering the pH range of 4 to 9.5.

3.6. Thermodynamic System Zn–Se–H2O

In this system only one selenide, stilleite (ZnSe), was reported (Table 1). Natural hydrous Zn selenites have not yet been found, but their formation in nature is quite possible, for example, in the oxidation zones of Se-bearing sulfide ores, in which sphalerite or stilleite (ZnSe) is a source of Zn. The rarity and difficulty of their identification may explain why hydrous zinc selenites have not yet been detected in nature. However, Pekov et al. [56] have recently found a new anhydrous Zn selenite mineral (zincomenite, ZnSeO3) in fumarole products in the Tolbachik volcano.
The solubility and the thermal behavior of synthetic ZnSeO3·2H2O, and ZnSeO3·H2O were discussed in [55,57]. It was shown that ZnSeO3·2H2O is a more stable phase than ZnSeO3·H2O under environmental conditions. The monohydrate appears to be a metastable phase. The thermochemical calorimetric investigations were carried out on synthetic zinc selenites, ZnSeO3·2H2O and ZnSeO3·H2O [18].
Finally, the Eh–pH plot of the Zn–Se–H2O system is shown in Figure 7. This system attracts interest because it allows the estimation of the physico-chemical parameters of the formation of hydrous Zn selenite. As we see in Figure 7, the diagram contains the stability fields of native selenium, stilleite, zincite (ZnO), and zinc selenite (ZnSeO3·2H2O). As follows from this diagram, the physico-chemical parameters of zinc selenite stability—pH, Eh, and the activities of Zn and Se—are close to those of cobalt and nickel selenites (ahlfeldite and cobaltomenite) [49], and ZnSeO3·2H2O is the stable phase at the temperature fluctuations corresponding to environmental conditions.

3.7. Thermodynamic System Cd–Se–H2O

In this thermodynamic system, only one selenide (cadmoselite, CdSe) was reported (Table 1). Cadmoselite was found in Ust’ Uyok deposit (Turan District, Tuva Republic, Eastern-Siberian Region, Russia) as fine xenomorphic disseminations cementing sandstone associated with ferroselite, clausthalite, amorphous selenium, Cd-bearing sphalerite, and pyrite [58]. The thermodynamic constants of synthetic hydrous cadmium selenite were reported [18]. These data were used for plotting the Eh–pH diagram of the Cd–Se–H2O system (Figure 8). The greatest part of the diagram contains stability fields of solid phases and is characterized by the fields of native selenium, cadmoselite and hydrous Cd selenite. It is noteworthy that a wide stability field of hydrous Cd selenite (CdSeO3·H2O) appears covering the pH range of 2 to 12.5. Therefore, in terms of geochemistry, hydrous cadmium selenite is theoretically able to form in the oxidation zones of Se-bearing sulfide ores, in which Cd-bearing sphalerite (Zn, Cd)S or Cd-bearing is a source of Cd. The rarity and difficulty of their identification may explain why hydrous cadmium selenites have not yet been detected in nature.

3.8. Thermodynamic System Hg–Se–H2O

In this thermodynamic system, one selenide, tiemannite (HgSe) was reported. Natural Hg selenites have not yet been found in nature. Tiemannite was described for the first time at the St Lorenz Mine, Burgstatt veins, Clausthal-Zellerfeld, Harz, Lower Saxony, Germany [59] in association with clausthalite, berzelianite, naumannite, pyrite, sphalerite, galena, quartz, bournonite. Tiemannite is a common mineral, it has been found in 75 localities (according www.mindat.org), associated with low-sulfur hydrothermal deposits with other selenides, and also in mercury deposits. The Eh–pH plots of the Hg–Se–H2O system are shown in Figure 9. This system is interesting because it allows the estimation of the physico-chemical parameters of the formation of anhydrous Hg selenites. The greatest part of the diagram contains the stability fields of tiemannite, mercury and anhydrous Hg selenites (HgSeO3, Hg2SeO3).

3.9. Thermodynamic System Ag–Se–H2O

In this thermodynamic system, only one mineral, naumannite (Ag2Se) was reported. Naumannite was found in Germany, in the Harz Mountains, at Tilkerode [60], in hydrothermal veins deficient in sulfur, associated with other selenides, quartz, and carbonates. Natural Ag selenites have not yet been found, but their formation in nature is quite possible in the oxidation zones of Se-bearing sulfide ores, because naumannite is a widespread mineral (according to mindat.org it was discovered in 156 localities). The thermodynamic data recommended in the directory [46] was used for plotting the Eh–pH diagram of the Ag–Se–H2O system (Figure 10). The greatest part of the diagram contains stability fields of naumannite, native selenium and silver, with small field of Ag2O in extremely alkaline areas at a high positive Eh. It is noteworthy that a small stability field of Ag selenite (Ag2SeO3) appears covering the pH range of 6 to 7.5.

3.10. Thermodynamic System Bi–Se–H2O

The Table 1 shows that in this system four mineral species—nevskite (BiSe), guanajuatite (Bi2Se3), paraguanajuatite (Bi2Se3), and laitakarite (Bi4Se3)—were reported, but only for two of them (nevskite and paraguanajuatite) are the thermodynamic data available (Table 1). Both minerals occur in hydrothermal deposits of low to medium temperatures. The greatest part of the Eh–pH diagram of Bi–Se–H2O system is characterized by the fields of paraguanajuatite, native selenium, and a small bismuth stability field. It is noteworthy that a wide stability field of paraguanajuatite appears covering the wide pH range (Figure 11).

3.11. Thermodynamic System As–Se–H2O

In this system only one selenide mineral (laphamite, As2Se3) was reported. Laphamite was found in one locality (Burnside, Northumberland County, PA, USA) as a secondary incrustation, probably by sublimation, on a burning pile of waste material from an anthracite coal mine in association with arsenolite, bararite, downeyite, galena, orpiment, selenium, and sulfur [61].
The Eh–pH diagram of the As–Se–H2O system (Figure 12) shows that the larger part of the diagram contains stability fields of native selenium and laphamite. A small stability field of arsenic corresponds to the alkaline region with a negative Eh.

3.12. Thermodynamic System Sb–Se–H2O

In this system only one selenide, antimonselite (Sb2Se3), was reported (Table 1). Antimonselite was found in uraniferous calcite veins in a hydrothermal U–Hg–Mo polymetallic deposit in association with pyrite, sphalerite, galena, ferroselite, clausthalite, uraninite, cinnabar, hematite, and calcite (near Kaiyan, Guizhou Province, China) [62].
The Eh–pH diagram of the Sb–Se–H2O system (Figure 13) shows that the larger part of the diagram contains stability fields of antimonselite and native selenium.

3.13. Thermodynamic System Al–Se–H2O

Recently, the compound Al2(SeO3)3·6H2O was found in nature as the mineral alfredopetrovite (Table 1). The mineral occurs in the El Dragón mine, Antonio Quijarro Province, Potosí Department, Bolivia. The El Dragón mine is situated in a telethermal deposit consisting of a single selenide vein hosted by sandstones and shales. Selenide oxidation has produced a wide range of secondary rare selenites (ahlfeldite, chalcomenite, mandarinoite, favreauite, molybdomenite, olsacherite, schmiederite and others), one of which is alfredopetrovite [63].
The Eh–pH diagram of the Al–Se–H2O system is shown in Figure 14. At the background concentration of Al and Se, the larger section of the diagram contains stability fields of gibbsite (Al(OH)3) and native selenium. A small stability field corresponds to alfredopetrovite in the diagram’s acidic section, with a high positive Eh.

3.14. Thermodynamic System Ca–Se–H2O

In this system, hydrous calcium selenite (CaSeO3·H2O) has recently been found in nature as the mineral nestolaite (Table 1). Specimens containing nestolaite were collected in the Little Eva mine, Yellow Cat District, Grand County, UT, USA. The mineral is very rare and occurs as light violet, round aggregations on sandstone associated with cobaltomenite, gypsum, orschallite, ferroselite, native selenium and others. Nestolaite was formed due to the supergene oxidation of primary Se minerals, such as native selenium and ferroselite [64].
The Eh–pH diagram of the Ca–Se–H2O system is shown in Figure 15. The larger part of the diagram contains stability fields of native selenium and portlandite, Ca(OH)2. A stability field of nestolaite corresponds to the alkaline region with a positive Eh.

3.15. Selenates

In conclusion, we dwell on the probable formation of natural Co, Ni, Fe, Cu, Zn and Pb selenates. We calculated the Eh–pH diagrams within a wide range of activities of the components and found values corresponding to the appearance of the stability fields of CoSeO4·6H2O, CuSeO4·5H2O, NiSeO4·6H2O, PbSeO4 and ZnSeO4·6H2O [65].
The calculations indicate that, among all the discussed systems, selenates are formed only in the Pb–Se–H2O and Cu–Se–H2O systems at 25 °C with more or less real (although high) activities of metals and Se in the solution: aΣSe = 10−3 and aΣPb = 10−3; aΣSe = 10−1 and aΣCu = 10−1.
The activities of Co, Ni and Zn necessary for the formation of their selenate hydrates are extremely high and cannot be encountered in nature. The Eh–pH diagrams of the Cu–Se–H2O and Pb–Se–H2O systems show crystallization fields of CuSeO4·5H2O and PbSeO4 [65]. The results are consistent with the list of the three known mineral species containing selenate ions: schmiederite (Pb2Cu2(SeO3)(SeO4)(OH)4); olsacherite (Pb2(SeO4)(SO4)), which is found at the Dragon and Pacajake deposits in Bolivia and the Baccu Locci deposit in Sardinia, Italy together with selenites; and carlosruizite (K6Na10Mg10(IO3)12(SeO4)12·12H2O), a very specific mineral differing in its formation conditions, which are found at a niter deposit in association with nitratine, fuenzalidaite, and halite [66]. Kerstenite, PbSeO4 [67], a single simple selenate, has turned out to be a molybdomenite after a detailed study [68].

3.16. Thermodynamic Data

Unfortunately, for most selenium minerals no data on the thermodynamic functions of the formation have been reported. Additional experimental investigations are needed in order to produce reliable and accurate standard thermodynamic data, which will enable researchers to adequately describe Se migration behavior in the oxidation zones of sulfide and selenide ores and contaminated areas. It should be noted that the experimental determination of the thermodynamic data of rare minerals in general, and of the title compounds in particular, on the basis of studying their solubility or by calorimetric measurements, can hardly rely on natural samples, because these usually do not occur in sufficient amounts, forming only tiny crystals which may incorporate inclusions, be covered by weathering crusts, and almost inevitably contain impurities. All these defects influence many properties of the samples studied and certainly their thermodynamic parameters. Therefore, the investigation of the thermodynamic properties of selenium minerals is carried out on their synthetic analogues.

4. Conclusions

The obtained data show that the behavior of selenium, the nearest geochemical counterpart of sulfur, in the surface environment can be quantitatively explained by variations of the redox potential and the acidity–basicity of the mineral-forming medium. Precisely these parameters determine the migration ability of selenium compounds and their precipitation in the form of various solid phases.

Supplementary Materials

The following are available online at www.mdpi.com/2075-163X/7/10/188/s1, Table S1: Selenim minerals: Chemical formula, type locality (TL) and number of localities (NL).

Acknowledgments

The three anonymous reviewers are thanked for their useful comments, which led to many important clarifications. This study was supported by St. Petersburg State University (Grants No. 3.38.286.2015; 3.42.732.2017) and the Russian Foundation for Basic Research (Grant No. 16-05-00293). The St. Petersburg State University Resource Centers “X-Ray Diffraction Methods” and “Geomodel” made their equipment available for this study.

Author Contributions

Vladimir Krivovichev and Marina Charykova wrote the article. Marina Charykova and Andrey Vishnevskiy collected the thermodynamic data and calculated the Eh–pH diagrams.

Conflicts of Interest

The authors declare no conflict of interest.

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Figure 1. Thermochemical sequence of chemical elements and corresponding single-component systems.
Figure 1. Thermochemical sequence of chemical elements and corresponding single-component systems.
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Figure 2. Eh–pH diagram of the system OHSeCo (Co–Se–H2O) at 25 °C and the activities of the components: aΣSe = 10−4, aΣCo = 10−3. Here and in Figure 3, Figure 4, Figure 5, Figure 6, Figure 7, Figure 8, Figure 9, Figure 10, Figure 11, Figure 12, Figure 13, Figure 14 and Figure 15, the solid lines are boundaries of the stability fields of the solid phases.
Figure 2. Eh–pH diagram of the system OHSeCo (Co–Se–H2O) at 25 °C and the activities of the components: aΣSe = 10−4, aΣCo = 10−3. Here and in Figure 3, Figure 4, Figure 5, Figure 6, Figure 7, Figure 8, Figure 9, Figure 10, Figure 11, Figure 12, Figure 13, Figure 14 and Figure 15, the solid lines are boundaries of the stability fields of the solid phases.
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Figure 3. Eh–pH diagram of the system OHSeNi (Ni–Se–H2O) at 25 °C and the activities of the components: aΣSe = 10−4, aΣNi = 10−2.
Figure 3. Eh–pH diagram of the system OHSeNi (Ni–Se–H2O) at 25 °C and the activities of the components: aΣSe = 10−4, aΣNi = 10−2.
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Figure 4. Eh–pH diagram of the OHSeFe (Fe–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣFe = 10−2. The dotted line is the boundary between fields of Fe2+ and Fe3+.
Figure 4. Eh–pH diagram of the OHSeFe (Fe–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣFe = 10−2. The dotted line is the boundary between fields of Fe2+ and Fe3+.
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Figure 5. Eh–pH diagram of the OHSeCu (Cu–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣCu = 10−2.
Figure 5. Eh–pH diagram of the OHSeCu (Cu–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣCu = 10−2.
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Figure 6. Eh–pH diagram of the OSePb (Pb–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣPb = 10−4.
Figure 6. Eh–pH diagram of the OSePb (Pb–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣPb = 10−4.
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Figure 7. Eh–pH diagram of the OHSeZn (Zn–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣZn = 10−2.
Figure 7. Eh–pH diagram of the OHSeZn (Zn–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣZn = 10−2.
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Figure 8. Eh–pH diagram of the OHSeCd (Cd–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣCd = 10−2. The dotted lines are the boundaries between fields of Cd2+, Cd(OH)+ and Cd(OH)20.
Figure 8. Eh–pH diagram of the OHSeCd (Cd–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣCd = 10−2. The dotted lines are the boundaries between fields of Cd2+, Cd(OH)+ and Cd(OH)20.
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Figure 9. Eh–pH diagram of the OHSeHg (Hg–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣHg = 10−5. The dotted lines are the boundaries between fields of Hg2+, Hg22+, and Hg(OH)20.
Figure 9. Eh–pH diagram of the OHSeHg (Hg–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣHg = 10−5. The dotted lines are the boundaries between fields of Hg2+, Hg22+, and Hg(OH)20.
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Figure 10. Eh–pH diagram of the OHSeAg (Ag–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣAg = 10−5.
Figure 10. Eh–pH diagram of the OHSeAg (Ag–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣAg = 10−5.
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Figure 11. Eh–pH diagram of the OHSeBi (Bi–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣBi = 10−5. The dotted lines are the boundaries between fields of Bi3+, BiO+ and Bi6O6(OH)33+.
Figure 11. Eh–pH diagram of the OHSeBi (Bi–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣBi = 10−5. The dotted lines are the boundaries between fields of Bi3+, BiO+ and Bi6O6(OH)33+.
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Figure 12. Eh–pH diagram of the OHSeAs (As–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣAs = 10−3. The dotted lines are the boundaries between fields of H3AsO40, H2AsO4−, HAsO42− and AsO43−.
Figure 12. Eh–pH diagram of the OHSeAs (As–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣAs = 10−3. The dotted lines are the boundaries between fields of H3AsO40, H2AsO4−, HAsO42− and AsO43−.
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Figure 13. Eh–pH diagram of the OHSeSb (Sb–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣSb = 10−5. The dotted lines are the boundaries between fields of SbO+, HSbO20 and SbO2.
Figure 13. Eh–pH diagram of the OHSeSb (Sb–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣSb = 10−5. The dotted lines are the boundaries between fields of SbO+, HSbO20 and SbO2.
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Figure 14. Eh–pH diagram of the OHSeAl (Al–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣAl = 10−3.
Figure 14. Eh–pH diagram of the OHSeAl (Al–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣAl = 10−3.
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Figure 15. Eh–pH diagram of the OHSeCa (Ca–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣCa = 10−2.
Figure 15. Eh–pH diagram of the OHSeCa (Ca–Se–H2O) system at 25 °C and the activities of the components: aΣSe = 10−4, aΣCa = 10−2.
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Table
Table 1. Mineral systems and ΔfG0298 of selenium minerals.
Table 1. Mineral systems and ΔfG0298 of selenium minerals.
nSystemMineralChemical FormulaΔfG0298, kJ/mol
Native Elements
1SeSeleniumSe0
Oxides
2OSeDowneyiteSeO2−171.80 ± 0.62
Selenides
2SeAsLaphamite As2Se3 −83.9 ± 4.2
SeSbAntimonselite Sb2Se3−127.4 ± 3.7
SeBiNevskite BiSe−46.8 ± 5.7
Guanajuatite Bi2Se3−146.6 ± 10.1
Paraguanajuatite Bi2Se3 –
Laitakarite Bi4Se3–
SePbClausthalite PbSe−97.9 ± 7.7
SeMoDrysdallite MoSe2–
SeFeAchávaliteFeSe−70.1 ± 4.0
Dzharkenite (cub)FeSe2–
Ferroselite (orth)FeSe2−101.3 ± 15.0
SeCoBornhardtite CoCo2Se4–
Freboldite CoSe −56.3 ± 6.5
Trogtalite CoSe2 −100.4 ± 15.0
SeNiSederholmiteNiSe−69.8 ± 1.6
Mäkinenite NiSe–
Penroseite NiSe2−112.4 ± 7.0
KulleruditeNiSe2–
Trüstedtite NiNi2Se4–
Wilkmanite Ni3Se4–
SePdVerbeekite PdSe2–
Oosterboschite Pd7Se5–
Palladseite Pd17Se15–
SePtSudovikovite PtSe2–
Luberoite Pt5Se4–
SeCuKlockmanniteCuSe−36.8 ± 0.6
Krut’aite CuSe2–
PetříčekiteCuSe2–
Bambollaite CuSe2–
Bellidoite Cu2Se–
Berzelianite Cu2Se–
Umangite Cu3Se2–
AthabascaiteCu5Se4
Geffroyite Cu9Se8 –
SeAgNaumannite Ag2Se−46.9 ± 1.3
SeZnStilleite ZnSe−172.5 ± 4.0
SeCdCadmoselite CdSe −140.9 ± 1.9
SeHgTiemannite HgSe−51.2 ± 4.0
3SSeAgAguilariteAg4SeS–
SeTeBiKawazuliteBi2Te2Se–
SkippeniteBi2Se2Te–
TelluronevskiteBi3TeSe2–
VihorlatiteBi24Se17Te4–
SeTeNiKitkaiteNiTeSe–
SeTePdMiessiitePd11Te2Se2–
SeTeAgKuriliteAg8Te3Se–
SeAsNiJolliffeiteNiAsSe–
SeAsPdKalungaitePdAsSe–
SeAsCuMgriiteCu3AsSe3–
SeSbPdMilotaitePdSbSe–
SeSbCuBytíziteCu3SbSe3–
PermingeatiteCu3SbSe4–
PříbramiteCuSbSe2–
SeSbAgSelenostephaniteAg5(SbSe3)Se–
SeBiPbPoubaite PbBi2Se4–
SeBiPdPadmaitePdBiSe–
SeBiCuGrundmanniteCuBiSe2–
HansblockiteCuBiSe2–
EldragóniteCu6BiSe4(Se2) –
SeBiAgBohdanowicziteAgBiSe2–
SePbCuSchlemaiteCu6PbSe4–
SeTlCuBukoviteCu4Tl2Se4–
SabatieriteCu6TlSe4–
CrookesiteCu7TlSe4–
SeFeCuEskeborniteCuFeSe2–
SeCoCuTyrrelliteCuCo2Se4–
SePdCuJagüéiteCu2Pd3Se4–
SePdAgChrisstanleyiteAg2Pd3Se4–
SePdHgTischendorfiteHg3Pd8Se9–
SePtHgJacutingaitePt2HgSe3–
SeCuAgEucairiteCuAgSe–
SelenojalpaiteAg3CuSe2–
SeCuHgBrodtkorbiteCu2HgSe2–
SeAgAuFischesseriteAgAuSe2–
4SeAsFeCuChaméanite (Cu3Fe)Σ4AsSe4 –
SeSbCuHgHakite Cu6Cu4Hg2(SbSe3)4Se–
SeBiPbCuWatkinsonite Cu2PbBi4Se8–
SeBiPbAgLitochlebiteAg2PbBi4Se8–
5SSeAsZnCuGiraudite Cu6Cu4Zn2(AsSe3)4S–
SSeSbCuAgSelenopolybasite CuAg6Ag9Sb2S9Se2 –
SeBiPbCuHgPetrovicite Cu3HgPbBiSe5–
QuijarroiteCu6HgPb2Bi4Se12–
I. Selenites without H2O
3OSePbMolybdomenitePbSeO3−458.0 ± 6.0
PlumboselitePb3(SeO3)O2–
4OSeZnZincomeniteZnSeO3–
OSSePbOlsacheritePb2(SeO4)(SO4)–
OClSeCuGeorgbokiiteCu5(SeO3)2O2Cl2–
ParageorgbokiiteCu5(SeO3)2O2Cl2–
NicksoboleviteCu7(SeO3)2O2Cl6–
ChloromeniteCu9(SeO3)4O2Cl6–
OClSeZnSofiiteZn2(SeO3)Cl2–
5OClSeBiCuFrancisiteCu3Bi(SeO3)2O2Cl–
OClSePbCuSarrabusitePb5Cu(SeO3)4Cl4–
AllochalcoseliteCuCu5PbO2(SeO3)2Cl5–
OClSeCuNaIlinskiteNaCu5(SeO3)2O2Cl3–
6OClSeCdCuKBurnsiteKCdCu7(SeO3)2O2Cl9–
7OClSePbZnCuKPrewittiteK2Pb3Zn2Cu12(SeO3)4O4Cl20–
II. Selenites and Selenates Containing H2O
4OHSeAlAlfredopetroviteAl2(SeO3)3·6H2O−3657.4
OHSeCoCobaltomeniteCoSeO3·2H2O−937.4 ± 2.5 1
OHSeFeMandarinoiteFe2(SeО3)3·6H2O−2756.80 ± 7.3
OHSeNiAhlfelditeNiSeO3⋅2H2O−932.4 ± 2.5 1
OHSeCuChalcomeniteCuSeO3⋅2Н2О−835.3 ± 5.3 2
OHSeUHaynesite(UO2)3(SeO3)2(OH)2⋅5H2O–
OHSeCaNestolaiteCaSeO3·H2O−1188.9 ± 2.5
5OHClSePbOrlandiitePb3(SeO3)Cl4⋅H2O–
OHSSeCuPauladamsiteCu4(SeO3)(SO4)(OH)4·2H2O–
OHSePbCuSchmiederitePb2Cu2(SeO3)(SeO4)(OH)4–
OHSeCuUDerriksiteCu4(UO2)(SeO3)2(OH)6·H2O–
MarthoziteCu(UO2)3(SeO3)2O2·8H2O–
OHSeUCaPiretiteCa(UO2)3(SeO3)2(OH)4⋅4H2O–
OHSeUBaGuilleminiteBa(UO2)3(SeO3)2(OH)4·3H2O–
OHSeUNaLarisaiteNa(H3O)(UO2)3(SeO3)2O2⋅4H2O–
6OHSSePbCuMunakataitePb2Cu2(SeO3)(SO4)(OH)4–
OHSeBiPbCuFavreauitePbBiCu6O4(SeO3)4(OH)·H2O–
OHSePbCuUDemesmaekeritePb2Cu5(UO2)2(SeO3)6(OH)6⋅2H2O–
7OHISeMgNaKCarlosruiziteK6Na4Na6Mg10(SeO4)12(IO3)12·12H2O–
Notes: 1 [17]; 2 [18].

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Krivovichev, V.; Charykova, M.; Vishnevsky, A. The Thermodynamics of Selenium Minerals in Near-Surface Environments. Minerals 2017, 7, 188. https://doi.org/10.3390/min7100188

AMA Style

Krivovichev V, Charykova M, Vishnevsky A. The Thermodynamics of Selenium Minerals in Near-Surface Environments. Minerals. 2017; 7(10):188. https://doi.org/10.3390/min7100188

Chicago/Turabian Style

Krivovichev, Vladimir, Marina Charykova, and Andrey Vishnevsky. 2017. "The Thermodynamics of Selenium Minerals in Near-Surface Environments" Minerals 7, no. 10: 188. https://doi.org/10.3390/min7100188

APA Style

Krivovichev, V., Charykova, M., & Vishnevsky, A. (2017). The Thermodynamics of Selenium Minerals in Near-Surface Environments. Minerals, 7(10), 188. https://doi.org/10.3390/min7100188

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