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Article

Temperature-Induced Phase Transition in a Feldspar-Related Compound BaZn2As2O8∙H2O

by
Liudmila A. Gorelova
1,*,
Oleg S. Vereshchagin
1,
Vladimir N. Bocharov
2,
Dmitrii V. Pankin
3 and
Tamara Đorđević
4
1
Institute of Earth Sciences, Saint Petersburg State University, 199034 St. Petersburg, Russia
2
Center for Geo-Environmental Research and Modeling (Geomodel), Saint Petersburg State University, 198504 St. Petersburg, Russia
3
Center for Optical and Laser Materials Research, Saint Petersburg State University, 198504 St. Petersburg, Russia
4
Institut für Mineralogie und Kristallographie, Universität Wien, 1090 Vienna, Austria
*
Author to whom correspondence should be addressed.
Minerals 2022, 12(10), 1262; https://doi.org/10.3390/min12101262
Submission received: 22 September 2022 / Revised: 2 October 2022 / Accepted: 3 October 2022 / Published: 6 October 2022
(This article belongs to the Special Issue Mineral-Related Oxo-Salts: Synthesis and Structural Crystallography)
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Abstract

:
The high-temperature (HT) behavior of BaAs2Zn2O8∙H2O was studied by in situ single-crystal X-ray diffraction (SCXRD) and hot stage Raman spectroscopy (HTRS) up to dehydration and the associated phase transition. During heating, the studied compound undergoes the dehydration process with the formation of BaAs2Zn2O8, which is stable up to at least 525 °C. The evolution of the fourteen main Raman bands was traced during heating. The abrupt shift of all Raman bands in the 70–1100 cm−1 spectral region was detected at 150 °C, whereas in the spectral region 3000–3600 cm−1 all the bands disappeared, which confirms the dehydration process of BaAs2Zn2O8∙H2O. The transition from BaAs2Zn2O8∙H2O to BaAs2Zn2O8 is accompanied by symmetry increasing from P21 to P21/c with the preservation of the framework topology. Depending on the research method, the temperature of the phase transition is 150 °C (HTRS) or 300 °C (HT SCXRD). According to the HT SCXRD data, in the temperature range 25–300 °C the studied compound demonstrates anisotropic thermal expansion (αmax/αmin = 9.4), which is explained by flexible crankshaft chains of TO4 (T = As, Zn) tetrahedra. Additionally, we discussed some crystal-chemical aspects of minerals with both (ZnOn) and (AsOm) polyhedra (n = 4, 5, 6; m = 3, 4) as main structural units.

1. Introduction

Feldspars are one of the most widespread minerals in the Earth’s crust. Comprising up to 90 vol. % of magmatic rocks (e.g., anorthosites) their P–T behavior became one of the main focuses of mineralogists and petrologists. Therefore, the major rock-forming minerals related to this group were studied in detail under both ambient and extreme (high pressure (HP) and high-temperature (HT)) conditions (e.g., [1,2,3,4,5]). Other than general information on P–T stability, a number of rare structural units (e.g., SiO5, BeO5, PO5, BeO6, PO6, B2O6) were discovered in feldspar polymorphs [5,6,7,8,9,10,11], which emphasizes the importance of these studies for both Earth sciences and inorganic chemistry.
According to the recent review by Krivovichev [12], there are 29 feldspar-related minerals with the general formula M[T4O8] (M = Na, K, Rb, (NH4), Ca, Sr, Ba; T = Si, Al, B, Be, Zn, As, P, Fe), which could be divided into five groups based on their topology (feldspar, paracelsian, svyatoslavite, dmisteinbergite and hollandite). The crystal structures with feldspar, paracelsian, svyatoslavite and dmisteinbergite topologies are based on the corner-sharing of tetrahedrally coordinated T atoms and hollandite topology based on octahedrally coordinated T atoms. The most widespread minerals of this group relate to the feldspar topology, whereas all other minerals are quite rare.
One of the outstanding examples of feldspar-topology minerals is filatovite (K(Al,Zn)2(As,Si)2O8 [13]), which is the first example of a natural continuous solid solution series between silicate and arsenate minerals in nature [14]. This mineral was discovered in the fumaroles of the Tolbachik volcano, Kamchatka, Russia [13,15]. Although Vergasova et al. [13] and Filatov et al. [15] reported the chemical formula of filatovite as K[(Al,Zn)2(As,Si)2O8], later research by Shchipalkina et al. [14] showed that the amount of Zn (together with Cu) cannot exceed 1, i.e., the filatovite with K[(AlZn)As2O8] composition (most close to the studied here BaAs2Zn2O8∙H2O) is only a hypothetical species. Moreover, filatovite has variable As-content [14], which complicates the study of (AsO4) behavior in feldspars.
Among natural feldspars, only two contain H2O groups, namely cymrite BaAl2Si2O8∙H2O [16] and ‘K-cymrite’ KAlSi3O8∙H2O, the latter of which is described in detail but not approved by the Commission on New Minerals, Nomenclature and Classification [17,18,19,20]. Both relate to the dmisteinbergite topology, i.e., they are layered. To date, framework feldspars containing (OH) or H2O groups are not known in nature. There are only some synthetic compounds with paracelsian topology, containing well-defined H2O groups ([21], and references therein). Therefore, the high temperature behavior of BaAs2Zn2O8∙H2O is studied here.
Generally, the study of arsenates minerals is very important due to the high toxicity of arsenic (As), which is an element of concern, owing to its epidemic-like health problems over nearly three decades in southeastern Asia. Although the anthropogenic activities, such as the mining and smelting of sulfide ores, can increase As concentration in the soils, one of its key sources often remains geogenic, because it is one of the main constituents of the parental rocks [22]. The most important problems concerning As bioavailability and its toxicity are closely connected to the stability of As-containing compounds [23], which are very sensitive to the changes in the geochemical environment to more reductive conditions [24]. The decomposition and dissolution of As-containing compounds can lead to the transportation of As into groundwater. Therefore, the study of their temperature behavior and stability is very important.
The aim of the present study was to investigate the structural behavior of BaAs2Zn2O8∙H2O upon heating and analyze its thermal expansion when compared with other isotypical (or chemically related) minerals and compounds.

2. Materials and Methods

The synthetic sample of BaAs2Zn2O8∙H2O, obtained using synthetic protocol given by Đorđević [21], was used for the high-temperature experiments. It could be considered as zincoarsenate, i.e., a compound isostructural framework of aluminosilicates containing Zn and As exclusively in tetrahedral coordination. Five crystals were chosen for the experiment. Each crystal was checked by single-crystal X-ray diffraction (SCXRD): one was used for the in situ high-temperature (HT) SCXRD experiment and another for the in situ hot-stage Raman spectroscopy (HTRS).
The crystal of BaAs2Zn2O8∙H2O with approximately the same size 30 × 10 × 10 μm was used for the hot-stage Raman spectroscopy. These experiments were conducted up to 425 °C with the temperature step of 25 °C and at 525 °C. The heating rate was about 25 °C/min. The unpolarized Raman spectra of the sample were recorded from a single crystal using a LabRam HR 800 spectrometer (Horiba Jobin-Yvon, Kyoto, Japan) equipped with a BX-41 (Olympus, Tokyo Japan) microscope and high-temperature attachment THMS600 System (Linkam, UK) in backscattering geometry system using a 532 nm laser. The sample, mounted on a 0.17-mm thick coverslip, was placed on a high-purity polished silver heating element, which guarantees efficient heat transfer as well as very high temperature sensitivity. The resistive platinum sensor ensures the accuracy of the setting and the temperature stability of 0.1 °C. The body of the system is water-cooled for operation at high temperatures. The Raman spectra were recorded in the range of 70–4000 cm−1 at a resolution of 1 cm−1 and 20 s acquisition time, and the power at the sample was 10 mW. To improve the signal-to-noise ratio, the number of acquisitions was set to 50.
The thermal behavior of BaAs2Zn2O8∙H2O under heating in the air was studied in situ by HT SCXRD using an XtaLAB Synergy-S diffractometer (Rigaku Oxford Diffraction, Japan) operated with monochromated MoKα radiation (λ[MoKα] = 0.71073 Å) at 50 kV and 40 mA. It was equipped with an HyPix-6000HE detector with a unique high-temperature FMB Oxford system (Oxford, UK). The sample heating was carried out using a gas blower up to 400 (±10) °C. For this experiment, the needle-like single crystal with the approximate size of 30 × 10 × 10 μm was mounted on the glass fiber, which was placed into the quartz capillary. Diffraction data were collected at different temperatures without changing the orientation of the crystal in the range of 27 to 300 °C with a temperature step of 50 °C. The crystal was also heated up to 400 °C, but due to the experimental features, the SCXRD data were not collected at this temperature—instead, they were collected at 27 °C after cooling. The data were integrated and corrected for background, Lorentz, and polarization effects. An empirical absorption correction based on the spherical harmonics implemented in the SCALE3 ABSPACK algorithm was applied in the CrysAlisPro program 171.37.35 [25]. The unit-cell parameters were refined using the least-square techniques. The SHELXL program package [26] was used for all structural calculations. The structure model of BaAs2Zn2O8∙H2O by Đorđević [21] was used as a starting model for structure refinements. The crystallographic information files (CIFs) for the crystal structures at all temperatures can be found as Supplementary Materials.
The temperature dependencies of the unit-cell parameters were described by quadratic and linear (for comparison with other minerals) polynomial functions in the whole temperature range (see below for more details). Based on these data, the thermal expansion coefficients were determined using the TTT program package [27]. This program package has also been used for the thermal-expansion parameter tensor visualization.

3. Results

3.1. Raman Spectra Evolution of BaAs2Zn2O8∙H2O upon Heating

The Raman spectrum of BaAs2Zn2O8∙H2O under ambient conditions (Figure 1a) is in a good agreement with the published data [21]. The bands in the regions from 800 to 1000 cm−1 correspond to the stretching vibrations of AsO4 only, whereas the bands from 350 to 550 cm−1 correspond to stretching vibrations of ZnO4 groups and the bending modes of the AsO4 groups, respectively. In the low-frequency region (below 350 cm−1), various lattice modes of the compound appear. In the high frequency region (3000–3600 cm−1) there are two bands at 3465 and 3271 cm−1, which correspond to the O–H stretching vibrations of the H2O molecule, but in contrast to the spectrum by Đorđević [21], the band at 3271 cm−1 has a very weak intensity.
A detailed study of the evolution of the Raman spectra of BaAs2Zn2O8∙H2O on heating from 27 to 525 °C showed a phase transition at 150 °C (Figure 1b,c and Figure 2). The most important changes are in the high-frequency region (3000–3600 cm−1), where all peaks disappear at the temperature above 150 °C (Figure 1c), which relates to the dehydration process. Moreover, the Raman spectrum in the low-frequency region (from 70 to 1000 cm−1) is changed significantly as well: the evolution of 14 Raman bands in this region was traced during heating (Figure 1b and Figure 2). In general, all of the Raman bands, except ν11 of the studied compound, move to lower wavenumbers, i.e., undergo a red shift. However, abrupt changes of almost all bands occur between 125 and 150 °C: some of them shift significantly; some of them appear or disappear. These changes indicate the phase transition from BaAs2Zn2O8∙H2O to BaAs2Zn2O8, which is most probably accompanied by symmetry increasing. It should be noted that the band at about 509–520 cm−1 (depending on temperature) undergoes a blue shift between 125 and 150 °C. As this band is associated with the ZnO4 group, the unusual moving of this band can be explained by the distortion of the ZnO4 tetrahedra in the crystal structure of BaAs2Zn2O8 (see below), which is typical for a ZnO4 tetrahedra comparison with AsO4 [21,28].

3.2. Crystal Structure Evolution of BaAs2Zn2O8∙H2O upon Heating

The crystal structure of the studied sample was refined at eight temperature points (Table 1 and Table 2), including room temperature (ambient conditions) after cooling. The positions of H atoms could not be determined due to their low scattering power and the features of the high-temperature experiments. Anisotropic displacement parameters were refined for all atoms, except O1 and O5 atoms at 50 and 100 °C, respectively.
The crystal structure of BaAs2Zn2O8∙H2O is monoclinic with the P21 space group [21] under ambient conditions (before cooling). It relates to the feldspar-type structures with the paracelsian topology, i.e., the crystal structure is based on a three-dimensional tetrahedral framework and consists of four- and eight-membered rings of alternate corner-sharing ZnO4 and AsO4 tetrahedra. The cavities of the eight-membered rings are occupied by Ba atoms coordinated by eight oxygen atoms and H2O groups, which are bonded only to Ba atoms (Table 2, Figure 1a). Though the framework topology of BaAs2Zn2O8∙H2O relates to the paracelsian, due to the existence of H2O groups, its crystal structure has lower symmetry and is not identical with the danburite- and paracelsian-like compounds.
The diffraction pattern of studied crystal changed dramatically after heating above 300 °C: the quality of the SCXRD data deteriorated significantly, which is reflected in the intensity decrease and transformation of the single crystal into a polycrystalline sample. It was impossible to perform an SCXRD experiment for this sample at 400 °C due to the features of the high-temperature experiment (large distance from the crystal to the detector and the lower frame intensities as a consequence). Only a pre-experiment, allowing the unit-cell parameters to be determined, was performed at these temperatures. Thus, after heating up to 400 °C, the studied sample was cooled to 27 °C and the full SCXRD data were collected in “normal” geometry.
It was found that the crystal structure of BaAs2Zn2O8∙H2O undergoes the dehydration process at a temperature above 300 °C. This process is accompanied by symmetry increasing from P21 to P21/c (Figure 3, Table 1). The resulting phase transition is irreversible, which is confirmed by the similarity of the unit-cell parameters obtained at 400 and 27 °C (crystal data after cooling). The crystal structure of anhydrous phase BaAs2Zn2O8 preserves the initial paracelsian topology, but the framework becomes more symmetric. The cavities of the eight-membered rings in the anhydrous phase are occupied by Ba atoms only, whereas in the hydrated phase they are occupied by both Ba and H2O. Previously, this phase was synthesized by Lucas et al. [28,29], who refined its crystal structure using the Rietveld refinement method. Moreover, this phase crystallizes as the major phase in the synthesis of BaAs2Zn2O8∙H2O [21].
The comparison of the Raman spectra obtained during the in situ high-temperature experiment and the spectrum obtained from the cooled crystal, which was heated during the SCXRD experiment, demonstrates their similarity (Figure 4). In both cases there are no Raman bands in the high frequency region (3000–3600 cm−1), which confirms the dehydration state of the compound for the cooled sample. All existing bands between 70 and 1000 cm−1 are similar and corrected for the shift caused by different temperatures. Moreover, it is one more confirmation that BaAs2Zn2O8 is a quenchable phase.
The significant difference in the dehydration temperatures obtained by the SCXRD (300 °C) and Raman (150 °C) experiments cannot be explained with certainty. As mentioned above, the error for each of the methods does not exceed 10 °C. Therefore, the possible reasons for the obtained results could be: (1) the process kinetics, which are associated with the different crystal size and the speed of the heating; (2) a variable amount of H2O groups in different crystals.
The relation between H2O content, unit-cell parameters and phase stability has been previously discovered in calcium oxalates [30,31,32]. According to these studies, the amount of H2O in weddellite crystal structure can vary, and the end-membered formula should be written as CaC2O4∙(2.5–x)H2O, where 0 ≤ x ≤ 0.25. Izatulina et al. [30] noted that there is a positive correlation between H2O content and the a parameter. She suggested to use this for the precise determination of the H2O content. However, verification of the unit-cell parameters of five crystals of BaAs2Zn2O8∙H2O under ambient conditions does not reveal any significant and regular variations. From crystal to crystal, the changes of the unit-cell parameters vary by ~0.01–0.03 Å, which is more than the error of their nominal determination but is close to the real error for the single crystal data [33].
Consequently, the most probably difference between HTRS and HT SCXRD data is connected to the experimental features of each of the methods. The most important aspects influencing the kinetic process are preparative routine, environmental conditions, the heating rate and the presence and nature of the flowing gas [32,34,35,36,37,38,39,40]. The most reliable results derive from the experiments with the low mass and slow heating rate [41,42], but not always [38]. In our case, the size of the studied crystals was approximately the same, but the heating method and sample preparation were different. This is a potential explanation for such a great difference in the temperature of the dehydration process.
The dehydration of other Zn- and As-containing compounds with zeolitic water usually occurred at ~100–200 °C, depending on the initial crystal structure, chemical composition and speed of heating, e.g., Na3Zn4O(AsO4)3∙6H2O lose all H2O groups at 150 °C [43], whereas the dehydration of Cs2(ZnAsO3OH)(ZnAsO4)2∙H2O occurred at 200 °C [44]. Moreover, BaAs2Zn2O8 was the main phase in the synthesis of BaAs2Zn2O8∙H2O Đorđević [21], which was conducted at temperatures below 220 °C.

3.3. Thermal Expansion of BaAs2Zn2O8∙H2O

The temperature dependencies of the unit-cell parameters obtained during the SCXRD experiment are shown in Figure 5. The changes of the unit-cell parameters are relatively linear in the temperature range from 27 to 300 °C. Therefore, no phase transition was supposed. The crystal structure refinements confirm the absence of phase transition or dehydration process at the temperatures below 300 °C (Table 1 and Table 2). According to SCXRD data, the site of the O atom belonging to a H2O molecule (namely, the O9 atom) is clearly defined.
Thermal expansion coefficients (TECs) calculated with the linear approximation of the unit-cell parameters’ temperature dependencies are the following: α11 = 16.0(8), α33 = 3.5(9), μ(α33^c) = 22.6(6), αa = 13.2(9), αb = α22 = 1.7(5), αc = 5.3(9), αβ = –6(2), αV = 21(1) ×106 °C−1. The thermal expansion of BaAs2Zn2O8∙H2O has an extremely anisotropic character: αmax/αmin = 9.4. The maximum and minimum expansion was observed practically along the a and b axes, respectively (Figure 5 and Figure 6). Thus, the direction of the maximal thermal expansion is along the flexible crankshaft chains and can be explained by their straightening, which is typical for feldspar-related compounds with feldspar topology [45]. The expansion of the pseudo-layer (bc plane) is more isotropic (αc/αb = 3.1) but, compared with other feldspar-related compounds, is still anisotropic. Such expansion in this plane was previously observed for another feldspar-related compound with paracelsian topology, maleevite BaB2Si2O8 [46], wherein its Sr and Ca analogues did not demonstrate sharp anisotropy. This phenomenon was explained by hinge deformations [47] of the four-fold rings [46].
The volume thermal expansion of BaAs2Zn2O8∙H2O (αV = 21 × 10−6 °C−1) is very close to the mean value of the volume thermal expansion of the feldspar-related natural and synthetic compounds with feldspar topology (<αV> = 20 × 10−6 °C−1, calculated on the base of 27 different compounds from Henderson [48]). The thermal expansion of feldspar-related compounds with paracelsian topology is studied in less detail. As far as we know, only the danburite group of minerals [46] and slawsonite [49] have been studied under high-temperature conditions. Their <αV> = 22 × 10−6 °C−1, calculated on the base of four compounds, is very close to the thermal expansion of compounds with feldspar topology.
Little is known about the high-temperature behavior of compounds containing Zn, As and O as the main structural constituents. Among them, only adamite, Zn2(AsO4)(OH), has been studied under high-temperature conditions [50]. The volume thermal expansion of adamite equals 34 × 10−6 °C−1 and is more intense than of BaAs2Zn2O8∙H2O. The extension of ZnO6 octahedra dimers is the main cause of the expansion [50]. ZnO6 octahedra undergo a sharp distortion during heating, whereas other crystal structure components (ZnO5 trigonal bipyramids and AsO4 tetrahedra) behave as quite rigid units.
The character of the thermal deformations of any compounds depends on their symmetry and topology, whereas the deformations value depends on chemical composition and topology [51]. Nevertheless, each compound has some individual features of the thermal deformations that allow the groups with isostructural compounds to be divided into subgroups. The studied high-temperature behavior of BaAs2Zn2O8∙H2O is one more example confirming this thesis.

4. Discussion

According to the International Mineralogical Association (IMA) List of Minerals, only 66 minerals containing Zn, As and O are known to date (Table 3). The crystal structures of these minerals usually contain As, coordinated by four oxygen atoms (tetrahedral coordination), but there are some arsenide minerals, where As is present in trigonal coordination. Simultaneously, the Zn atom can be surrounded by four, five or six O atoms. Consequently, these minerals could be considered as zincoarsenites (ZnO4 + AsO3), zincoarsenates (ZnO4 + AsO4), zinc arsenates (ZnO5/ZnO6 ± ZnO4 + AsO4 ± AsO3), and more complex compounds, whose crystal structures include ZnOn (n = 4, 5, 6), AsOm (m = 3, 4) and other polyhedra, e.g., FeO6, PO4, CO3, SiO4, TeO3, etc. The majority of these 66 minerals adopt framework structures (36 minerals); layered structures comprise a quarter (19), whereas minerals with chains structures are rare (3). The crystal structure of eight of them is either not determined or yet to be published (Table 3). Interestingly, crystal structures containing only isolated ZnO4- and AsO4-groups are unknown.
There are only two natural zincoarsenites: reinerite, Zn3(AsO3)2 [52] and leiteite, ZnAs2O4 [53,54]. Both were found in the oxidation zone of the famous lead-zinc-copper Tsumeb mine (Namibia) and were probably formed at lower (<50 °C) temperature conditions [54]. Similarly, only two natural zincoarsenates are known: filatovite K(Al,Zn)2(As,Si)2O8 and pharmazincite KZnAsO4. As mentioned above, filatovite belongs to the feldspar group of minerals [15], whereas pharmazincite is isostructural with nepheline, i.e., it is part of the feldspathoid group minerals [64]. Both are found only in one place with very specific geological conditions, namely in the fumaroles of the Tolbachik volcano, Kamchatka, Russia [13,64]. It is supposed that pharmazincite is deposited from the gas phase at a temperature above 360 °C [64], whereas the temperature of the filatovite formation is most probably above 500 °C [119].
There are no natural anhydrous zinc arsenates (ZnO–As2O5 system). In the ZnO–As2O5–H2O system, there are two hydroxyl and eight hydrated zinc arsenate minerals (Table 3). However, none of them contain Zn in exclusively tetrahedral coordination. Legrandite, adamite, paradamite and warikahnite crystallize as the framework structures [55,62,63], while ianbruceite, koritnigite and köttigite adopt layered structures [59,60,61]. Arsenohopeite and davidlloydite are sheet structures with infinite sheets of tetrahedra linked by interlayer octahedral sites [56,58]. As in cardite, H2O is bonded to the structural unit in each of these structures [57], except for ianbruceite, which contains interstitial H2O groups [61]. All of the minerals mentioned above can be found as the supergene phases that are typical for the oxidation zones of polymetallic deposits, such as Tsumeb (Namibia) or Broken Hill (Australia).
Zinc arsenates (and zinc arsenate-arsenites) comprise a large group of 52 minerals, which contain ZnOn (n = 4, 5, 6) and AsOm (m = 3, 4) polyhedra. Almost half of them belongs to PbO–ZnO–As2O5–H2O (six minerals), CaO–ZnO–As2O5–H2O (six minerals), CuO–ZnO–As2O5–H2O (six minerals) and Fe2O3–ZnO–As2O5–H2O (four minerals) systems (Table 3). The remaining 30 minerals have a more complex chemical composition and cannot be easily divided into separate groups. It should be noted that the vast majority of the minerals containing Zn and As are hydrous, i.e., contain (OH) or H2O groups. According to the IMA list of minerals, there are only seven anhydrous zinc arsenate minerals: dugganite, filatovite, leiteite, pharmazincite, reinerite, stranskiite and zincobradaczekite, whereas duggianite can contain a small amount of (OH) groups [121]. Three of the six remaining anhydrous minerals (filatovite, pharmazincite and zincobradaczekite) are formed in specific geological conditions, such as fumaroles on the Tolbachik volcano, Kamchatka, Russia, i.e., they are formed under high-temperature conditions (above 350 °C) directly from gas [119]. Leiteite and reinerite, as mentioned above, are zinc arsenides and, as a consequence, there is only one anhydrous zinc arsenate mineral—stranskiite, which was first described by Strunz [122] from the oxidation zone in the Tsumeb mine, Africa, but is also known on the Tolbachik volcano [119].
It should be separately highlighted that among all 66 minerals there are only 12 containing Zn and As in exclusively tetrahedral coordination: cardite, dugganite, ekatite, filatovite, goldhillite, holdenite, joelbruggerite, kolicite, magnesiochlorophoenicite, pharmazincite, philipsburgite and stergiouite. Five-fold coordinated Zn is known for nine minerals only: adamite, claraite, ianbruceite, kolitschite, lengradite, paradamite, stranskiite, warikahnite and zincolivenite. Thus, most of the minerals contain Zn in octahedral coordination. Additionally, arakiite, mcgovemite and wiklundite can be mentioned as minerals containing As in both trigonal and tetrahedral coordination.
The crystals of BaAs2Zn2O8∙H2O were obtained at 120–220 °C and a moderate acidity (pH = 6), whereas BaAs2Zn2O8 was obtained during both the synthesis and heating of BaAs2Zn2O8∙H2O to 150–300 °C. Considering the above, both BaAs2Zn2O8∙H2O and BaAs2Zn2O8 can also be found in nature. Their formation can be realized in very specific geological conditions, such as volcanic fumaroles or the oxidation zones of polymetallic deposits.

5. Conclusions

The high-temperature behavior of BaAs2Zn2O8∙H2O was studied using single-crystal X-ray diffraction and hot-stage Raman spectroscopy. It undergoes a phase transition as the temperature increases with the formation of the anhydrous phase (BaAs2Zn2O8), which is clearly defined using both methods by abrupt changes of the Raman bands’ position and unit-cell parameters. This process is accompanied by an increase in symmetry. The difference between two phases is in the channel occupancy: it could be occupied by H2O groups and/or Ba atoms. However, both crystal structures have the similar topology of a three-dimensional framework of AsO4 and ZnO4 tetrahedra. Generally, the thermal expansion of the initial phase is similar to other feldspar-related compounds with paracelsian topology. However, it has an extremely anisotropic character that can be caused by the “preparation” of the crystal structure for the dehydration process and following phase transition. It is assumed that both hydrous and anhydrous phases can be found in nature, but for their formation, very specific geological conditions are needed.

Supplementary Materials

The CIF-files at all temperature points are available online at https://www.mdpi.com/article/10.3390/min12101262/s1.

Author Contributions

L.A.G. wrote the original manuscript; L.A.G. and O.S.V. obtained the high-temperature X-ray diffraction data; D.V.P. obtained the Raman spectra at room temperature; O.S.V. and V.N.B. obtained the Raman spectra under high-temperature conditions; L.A.G. performed crystal structure calculations and Raman spectra processing; T.Đ. provided the studied sample and made a significant contribution to writing the discussion section of the manuscript. The manuscript was written through contributions made by all authors. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by the Russian Science Foundation, grant number 22-77-10033 (to L.A.G. and O.S.V.).

Data Availability Statement

Not applicable.

Acknowledgments

The authors thank the X-ray Diffraction Centre of the Resource Centre of Saint Petersburg State University for providing instrumental and computational resources. The Raman measurements were performed at the Centre for Geo-Environmental Research and Modelling (GEOMODEL) and the center for optical and laser materials research of Research Park, Saint Petersburg State University.

Conflicts of Interest

The authors declare no conflict of interest.

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Minerals 12 01262 g001 550
Figure 1. Raman spectra of BaAs2Zn2O8∙H2O under ambient conditions from 70 to 4000 cm−1 (a); at different temperatures from 70 to 1070 cm−1 (b) and from 2650 to 3850 cm−1 (c).
Figure 1. Raman spectra of BaAs2Zn2O8∙H2O under ambient conditions from 70 to 4000 cm−1 (a); at different temperatures from 70 to 1070 cm−1 (b) and from 2650 to 3850 cm−1 (c).
Minerals 12 01262 g001
Minerals 12 01262 g002 550
Figure 2. Temperature evolution of some selected Raman bands from 85 to 265 cm−1 (a), from 300 to 550 cm−1 (b), and from 800 to 940 cm−1 (c). The broken vertical lines demonstrate the abrupt changes in the temperature evolution of the Raman bands. The errors are smaller than the size of the symbols.
Figure 2. Temperature evolution of some selected Raman bands from 85 to 265 cm−1 (a), from 300 to 550 cm−1 (b), and from 800 to 940 cm−1 (c). The broken vertical lines demonstrate the abrupt changes in the temperature evolution of the Raman bands. The errors are smaller than the size of the symbols.
Minerals 12 01262 g002
Minerals 12 01262 g003 550
Figure 3. Crystal structure of BaAs2Zn2O8∙H2O (a) and BaAs2Zn2O8 (b) under ambient condition. AsO4 and ZnO4 tetrahedra are given in purple and grey, respectively. Ba and O atoms are presented as blue and red spheres, respectively.
Figure 3. Crystal structure of BaAs2Zn2O8∙H2O (a) and BaAs2Zn2O8 (b) under ambient condition. AsO4 and ZnO4 tetrahedra are given in purple and grey, respectively. Ba and O atoms are presented as blue and red spheres, respectively.
Minerals 12 01262 g003
Minerals 12 01262 g004 550
Figure 4. Raman spectra of BaAs2Zn2O8 at 175 °C, obtained during in situ high-temperature Raman experiment (a) and at 27 °C from the crystal, which has been studied by high-temperature SCXRD (b).
Figure 4. Raman spectra of BaAs2Zn2O8 at 175 °C, obtained during in situ high-temperature Raman experiment (a) and at 27 °C from the crystal, which has been studied by high-temperature SCXRD (b).
Minerals 12 01262 g004
Minerals 12 01262 g005 550
Figure 5. The temperature-induced evolution of the unit-cell parameters (a, b, c, β and V) of BaAs2Zn2O8∙H2O. The errors are smaller than the size of the symbols.
Figure 5. The temperature-induced evolution of the unit-cell parameters (a, b, c, β and V) of BaAs2Zn2O8∙H2O. The errors are smaller than the size of the symbols.
Minerals 12 01262 g005
Minerals 12 01262 g006 550
Figure 6. Crystal structure of BaAs2Zn2O8∙H2O with the section of thermal deformations. AsO4 and ZnO4 tetrahedra are given in purple and grey, respectively. Ca and O atoms are presented as blue and red spheres, respectively. a, b and c denote the crystallographic axes, α11, α22 and α33 show the thermal expansion coefficients along crystal-physical axes.
Figure 6. Crystal structure of BaAs2Zn2O8∙H2O with the section of thermal deformations. AsO4 and ZnO4 tetrahedra are given in purple and grey, respectively. Ca and O atoms are presented as blue and red spheres, respectively. a, b and c denote the crystallographic axes, α11, α22 and α33 show the thermal expansion coefficients along crystal-physical axes.
Minerals 12 01262 g006
Table
Table 1. Crystallographic data and refinement parameters for BaZn2As2O8∙H2O at different temperatures and BaZn2As2O8 at room temperature (T07).
Table 1. Crystallographic data and refinement parameters for BaZn2As2O8∙H2O at different temperatures and BaZn2As2O8 at room temperature (T07).
Temperature, °C275010015020025030023
T00T01T02T03T04T05T06T07
Space groupP21P21/c
a, Å 5.2854 (4)5.2840 (3)5.2882 (3)5.2918 (3)5.2957 (3)5.2986 (3)5.3037 (4)8.8073 (11)
b, Å 10.3919 (8)10.3901 (5)10.3940 (5)10.3948 (6)10.3964 (6)10.3948 (6)10.3959 (7)9.9861 (11)
c, Å8.0394 (7)8.0347 (5)8.0395 (5)8.0425 (5)8.0451 (5)8.0462 (5)8.0483 (6)9.4060 (11)
β, ° 95.445 (8)95.359 (5)95.346 (5)95.309 (5)95.262 (6)95.263 (6)95.285 (7)91.471 (10)
Volume, Å3439.58 (6)439.19 (4)439.97 (4)440.49 (4)441.07 (5)441.30 (5)441.87 (5)826.99 (17)
Z22
Data collection
Wavelength, Å 0.710730.71073
Max. θ°31.67229.30029.28529.28029.35529.36029.48633.799
Index ranges−7 ≤ h ≤ 7
−14 ≤ k ≤ 15
−9 ≤ l ≤ 11		−7 ≤ h ≤ 4
−14 ≤ k ≤ 13
−10 ≤ l ≤ 10		−7 ≤ h ≤ 4
−14 ≤ k ≤ 13
−10 ≤ l ≤ 10		−7 ≤ h ≤ 4
−14 ≤ k ≤ 13
−10 ≤ l ≤ 10		−4 ≤ h ≤ 7
−14 ≤ k ≤ 14
−10 ≤ l ≤ 10		−4 ≤ h ≤ 7
−14 ≤ k ≤ 14
−10 ≤ l ≤ 10		−7 ≤ h ≤ 4
−13 ≤ k ≤ 14
−10 ≤ l ≤ 11		−13 ≤ h ≤ 13
−15 ≤ k ≤ 14
−14 ≤ l ≤ 14
No.meas.refl.542248534848487943834883463510016
No.uniq.refl.23562033203420401997202620612957
No.obs.refl
(I > 2σ(I))		20831755172817091570165015771319
Refinement of the structure
No. of variables128123123128128128128118
Rint0.06570.04800.04950.04950.05850.05330.05250.1495
R1, all data0.05260.05070.05260.05400.06170.06060.07060.2347
R1, I > 2σ(I)0.04430.03880.03810.03990.04100.04230.04590.1052
wR2, all data0.09650.06920.06800.06910.06510.07790.08010.2999
wR2, I > 2σ(I)0.09380.06640.06370.06570.06080.07250.07390.2259
GooF0.9901.0151.0071.0040.9451.0091.0111.031
Table
Table 2. Bond distances and polyhedral parameters in BaZn2As2O8∙H2O at different temperatures.
Table 2. Bond distances and polyhedral parameters in BaZn2As2O8∙H2O at different temperatures.
Temperature, °C2350100150200250300
T00T01T02T03T04T05T06
AsO4 tetrahedra
As1–O2 (Å)1.680 (12)1.672 (11)1.682 (11)1.679 (12)1.662 (12)1.675 (12)1.676 (14)
As1–O4 (Å)1.691 (11)1.679 (10)1.675 (12)1.669 (11)1.686 (12)1.684 (13)1.677 (13)
As1–O5 (Å)1.674 (10)1.695 (10)1.701 (10)1.681 (10)1.700 (11)1.691 (11)1.679 (12)
As1–O6 (Å)1.678 (10)1.670 (9)1.670 (10)1.662 (10)1.672 (10)1.672 (11)1.651 (11)
<As1–O> (Å)1.6811.6791.6821.6731.6801.6811.670
Volume (Å3)2.4362.4282.4412.4012.4342.4352.390
As2–O1 (Å)1.678 (12)1.684 (12)1.685 (11)1.683 (12)1.685 (12)1.686 (12)1.680 (13)
As2–O3 (Å)1.681 (12)1.670 (11)1.667 (11)1.664 (11)1.680 (12)1.663 (13)1.671 (13)
As2–O7 (Å)1.688 (11)1.686 (10)1.674 (10)1.679 (10)1.691 (10)1.664 (11)1.684 (12)
As2–O8 (Å)1.667 (11)1.672 (11)1.660 (11)1.675 (12)1.660 (12)1.658 (13)1.661 (13)
<As2–O> (Å)1.6781.6781.6721.6751.6791.6681.674
Volume (Å3)2.4242.4232.3952.4112.4282.3802.408
ZnO4 tetrahedra
Zn1–O1 (Å)1.975 (12)1.980 (12)1.979 (11)1.979 (12)1.972 (12)1.977 (12)1.982 (13)
Zn1–O3 (Å)1.953 (11)1.964 (11)1.965 (11)1.965 (11)1.959 (12)1.960 (13)1.964 (13)
Zn1–O5 (Å)1.935 (10)1.929 (9)1.922 (9)1.931 (9)1.935 (10)1.926 (10)1.931 (11)
Zn1–O6 (Å)1.903 (12)1.909 (11)1.910 (12)1.913 (13)1.882 (13)1.895 (14)1.909 (14)
<Zn1–O> (Å)1.9421.9461.9441.9471.9371.9391.946
Volume (Å3)3.6453.6673.6553.6763.6143.6273.661
Zn2–O2 (Å)1.968 (11)1.969 (11)1.961 (11)1.971 (12)1.974 (12)1.967 (13)1.969 (13)
Zn2–O4 (Å)1.955 (11)1.968 (10)1.955 (12)1.959 (11)1.945 (13)1.948 (13)1.959 (13)
Zn2–O7 (Å)1.941 (12)1.934 (11)1.935 (12)1.938 (12)1.947 (12)1.949 (13)1.947 (14)
Zn2–O8 (Å)1.934 (10)1.940 (10)1.941 (10)1.934 (10)1.935 (11)1.939 (11)1.936 (11)
<Zn2–O> (Å)1.9491.9531.9481.9511.9501.9511.953
Volume (Å3)3.6993.7233.7023.7113.7013.7093.711
BaO8 polyhedra
Ba–O1 (Å)2.726 (11)2.715 (10)2.723 (10)2.728 (11)2.728 (11)2.725 (11)2.734 (12)
Ba–O2 (Å)2.770 (13)2.774 (11)2.783 (11)2.778 (12)2.794 (12)2.789 (12)2.785 (14)
Ba–O3 (Å)2.697 (11)2.702 (9)2.708 (9)2.711 (10)2.701 (11)2.726 (11)2.711 (11)
Ba–O4 (Å)2.761 (10)2.763 (10)2.781 (11)2.782 (11)2.781 (12)2.783 (12)2.787 (12)
Ba–O5 (Å)2.902 (10)2.879 (10)2.880 (11)2.897 (11)2.874 (12)2.888 (12)2.896 (13)
Ba–O7 (Å)2.744 (11)2.752 (11)2.756 (11)2.761 (12)2.736 (11)2.766 (12)2.746 (14)
Ba–O9 (Å)2.897 (11)2.905 (9)2.912 (10)2.916 (10)2.904 (11)2.924 (11)2.908 (12)
Ba–O9 (Å)2.985 (11)2.971 (10)2.988 (11)2.980 (11)2.999 (11)3.000 (12)3.010 (13)
<Ba–O> (Å)2.8102.8082.8162.8192.8152.8252.822
Volume (Å3)36.10636.11936.32236.46136.24536.60636.465
Table
Table 3. List of minerals containing ZnOn (n = 4, 5, 6) and AsOn (n = 3, 4) polyhedra.
Table 3. List of minerals containing ZnOn (n = 4, 5, 6) and AsOn (n = 3, 4) polyhedra.
Mineral NameChemical FormulaStructural MotifReference
ZnO–As2O3 System
Reinerite[4]Zn3([3]AsO3)2Framework[52]
Leiteite[4]Zn[3]As2O4Layers[53,54]
ZnO–As2O5–H2O System
Adamite[5]Zn6]Zn([4]AsO4)(OH)Framework[55]
Arsenohopeite[6]Zn[4]Zn2([4]AsO4)2·4H2OFramework[56]
Cardite[4]Zn5.5([4]AsO4)2([4]AsO3OH)(OH)3·3H2OFramework[57]
Davidlloydite[6]Zn[4]Zn2([4]AsO4)2·4H2OFramework[58]
Koritnigite[6]Zn([4]AsO3OH)·H2OLayers[59]
Köttigite[6]Zn3([4]AsO4)2·8H2OLayers[60]
Ianbruceite[5]Zn[6]ZnO[[4]AsO3(OH)](H2O)3.53Layers[61]
Legrandite[5]Zn[6]Zn([4]AsO4)(OH)·H2OFramework[55,62]
Paradamite[5]Zn2([4]AsO4)(OH)Framework[55]
Warikahnite[4]Zn[5]Zn2[6]Zn3([4]AsO4)4·4H2OFramework[63]
K2O–ZnO–As2O3 System
FilatoviteK[4](Al,Zn)2[4](As,Si)2O8Framework[15]
PharmazinciteK[4]Zn[4]AsO4Framework[64]
PbO–ZnO–As2O5–H2O System
ArsenbrackebuschitePb2(Fe,[6]Zn)([4]AsO4)2(OH,H2O)Chains[65]
ArsendescloizitePb[6]Zn([4]AsO4)(OH)Framework[66]
FeinglositePb2Zn(AsO4)2·H2ONo structure[67]
HelmutwinkleritePb[6]Zn2([4]AsO4)2·2H2OLayers[68]
TsumcoritePb[6]Zn2([4]AsO4)2·2H2OLayers[69]
ZincgartrellitePb[6]Zn2([4]AsO4)2(H2O,OH)2Layers[70]
CaO–ZnO–As2O5–H2O System
Austinite Ca [6] Zn( [4] AsO4)(OH) Framework[71,72]
GaititeCa2[6]Zn([4]AsO4)2·2H2OChains[73]
Lotharmeyerite Ca [6] Zn2( [4] AsO4)2·2H2O Framework[74]
ProsperiteCa2[6]Zn4([4]AsO4)4·H2OFramework[75]
StergiouiteCa[4]Zn2([4]AsO4)2·4H2OFramework[76]
Zincroselite Ca2[6]Zn([4]AsO4)2·2H2O Chains[73]
CuO–ZnO–As2O5–H2O and CuO–ZnO–As2O5 Systems
ArsenoveszelyiteCu2[4]Zn([4]AsO4)(OH)3·2H2OLayers[77]
GoldhilliteCu5[4]Zn([4]AsO4)2(OH)6·H2OLayers[78]
Sabelliite Cu2[4],[6] Zn( [4] AsO4)(OH)3Framework[79,80]
StranskiiteCu[5]Zn2([4]AsO4)2Framework[81,82]
TheisiteCu5Zn5(AsO4)2(OH)14No structure[83]
Veselovskite[6]ZnCu4([4]AsO4)2([4]AsO3OH)2·9H2OFramework[84]
ZincoliveniteCu[5]Zn([4]AsO4)(OH)Framework[85]
Fe2O3–ZnO–As2O5–H2O System
Mapimite[6]Zn2Fe3([4]AsO4)3(OH)4·10H2OFramework[86]
Metaköttigite([6]Zn,Fe)3([4]AsO4)2·8(H2O,OH)Layers[87]
Ojuelaite[6]ZnFe2([4]AsO4)2(OH)2·4H2OFramework[88]
Wilhelmkleinite [6] ZnFe2([4]AsO4)2(OH)2Framework[89]
Other Minerals Containing ZnOn and AsOn Polyhedra
Arakiite[4]ZnMn12Fe2([3]AsO3)([4]AsO4)2(OH)23Layers[90,91]
Chlorophoenicite(Mn,Mg,[6]Zn)3[4]Zn2([4]AsO4)(OH,O)6Layers[92]
Claraite(Cu,[5],[6]Zn)15(CO3)4([4]AsO4)2(SO4)(OH)14·7H2OLayers[93]
CuprozheshengitePb4CuZn2(AsO4)2(PO4)2(OH)2No structure[94]
DugganitePb3[4]Zn3(TeO6)([4]AsO4)2Framework[95]
Ekatite(Fe,Fe,[4]Zn)12([4]AsO3)6([4]AsO3,SiO3OH)2(OH)6Framework[96]
Erikapohlite(□0.5Cu0.5)CuCa[6]Zn2([4]AsO4)3·H2OFramework[97]
Eurekadumpite(Cu,Zn)16(TeO3)2(AsO4)3Cl(OH)18·7H2OLayers(?)[98]
FahleiteCaZn5Fe2(AsO4)6·14H2ONo structure[99]
FerrilotharmeyeriteCaZn[6]Fe([4]AsO4)2(OH)·H2OLayers[68]
Gerdtremmelite ZnAl2(AsO4)(OH)5No structure[100]
HoldeniteMn6[4]Zn3([4]AsO4)2(SiO4)(OH)8Framework[101]
JamesitePb2[6]ZnFe2(Fe,[6]Zn)4([4]AsO4)4(OH)8(OH,O)2Framework[102]
JoelbruggeritePb3[4]Zn3Sb[4]As2O13(OH)Framework[103]
Keyite(□0.5Cu0.5)CuCd[6]Zn2([4]AsO4)3·H2OFramework[104]
Kolicite[4]Zn4Mn2+7([4]AsO4)2(SiO4)2(OH)8Framework[105]
KolitschitePb[[5]Zn0.5,□0.5]Fe3([4]AsO4)2(OH)6Framework[106]
Kraisslite[4]Zn3(Mn,Mg)25(Fe,Al)([3]AsO3)2[(Si,[4]As)O4]10(OH)16Framework[107]
MagnesiochlorophoeniciteMg3[4]Zn2([4]AsO4)(OH,O)6Layers[108]
Mcgovernite[4]Zn3(Mn,Mg,Fe,Al)42([3]AsO3)2([4]AsO4)4[(Si,[4]As)O4]8(OH)42Layers[109]
MetalodèviteZn(UO2)2(AsO4)2·10H2ONo structure[110]
NyholmiteCd3[6]Zn2([4]AsO3OH)2([4]AsO4)2·4H2OFramework[111]
OdanieliteNa□[6]Zn[6]Zn2([4]AsO4)[[4]AsO3(OH)]2Framework[112,113]
OgdensburgiteCa2Fe4Zn(AsO4)4(OH)6·6H2ONo structure (layers?)[114]
PhilipsburgiteCu5[4]Zn([4]AsO4)(PO4)(OH)6·H2OFramework[115]
PuttapaitePb2Mn2ZnCr4O2(AsO4)4(OH)6·12H2ONo structure[116]
WiklunditePb2(Mn,[6]Zn)3(Fe,Mn)2(Mn,Mg)19([3]AsO3)2[(Si,[4]As)O4]6(OH)18Cl6Layers[117]
ZheshengitePb4ZnZn2(AsO4)2(PO4)2(OH)2No structure[118]
ZincobradaczekiteNaCuCu[6]Zn2([4]AsO4)3Framework[113,119,120]
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Gorelova, L.A.; Vereshchagin, O.S.; Bocharov, V.N.; Pankin, D.V.; Đorđević, T. Temperature-Induced Phase Transition in a Feldspar-Related Compound BaZn2As2O8∙H2O. Minerals 2022, 12, 1262. https://doi.org/10.3390/min12101262

AMA Style

Gorelova LA, Vereshchagin OS, Bocharov VN, Pankin DV, Đorđević T. Temperature-Induced Phase Transition in a Feldspar-Related Compound BaZn2As2O8∙H2O. Minerals. 2022; 12(10):1262. https://doi.org/10.3390/min12101262

Chicago/Turabian Style

Gorelova, Liudmila A., Oleg S. Vereshchagin, Vladimir N. Bocharov, Dmitrii V. Pankin, and Tamara Đorđević. 2022. "Temperature-Induced Phase Transition in a Feldspar-Related Compound BaZn2As2O8∙H2O" Minerals 12, no. 10: 1262. https://doi.org/10.3390/min12101262

APA Style

Gorelova, L. A., Vereshchagin, O. S., Bocharov, V. N., Pankin, D. V., & Đorđević, T. (2022). Temperature-Induced Phase Transition in a Feldspar-Related Compound BaZn2As2O8∙H2O. Minerals, 12(10), 1262. https://doi.org/10.3390/min12101262

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