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Synthesis of Liebigite and Andersonite, and Study

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1.67 Canadian Mineralogist Vol. 31, pp. 167-171(t993) SYNTHESISOF LIEBIGITEAND ANDERSONITE, ANDSTUDY OFTHEIRTHERMAL BEHAVIOR AND LUMINESCENCE RENATID VOCHTEN I' Inboratorium voor chemischeenfusische mineralogie, Ilniversiteit Antwerpen(RUCA), Middelheimlann B - 2020AntwerPen, Belgium LAURENTVAN HAVERBEKE 1, Laboratoriumvoor anorganischechtmie, UniversiteitAnwerpen (RUCA),Groenenborgerlaan 17 B - 2020AnwerPen, Belgium KARELVAN SPRINGEL I' Iaboratorium voor chemischeenfusische m.ineralogie, Universiteit Annverpen (RUCA)' Middelheimlaan B - 2020AntwerPen, Belgium ABS'IRAC| TheirH2o content, Andersoniteand liebigite weresynthesized starting from tetrasodiumuranyl tricarbonate[NaaUO2(CO3)3]. a bandgapenergy studiedby thermatanal/sis, is estimatedto be 10.5and 6 moles,respectivet. From the fluorescencespectr4 of approximately2.5 eV wascalculated. It is not affectedby temperature' Keywords:liebigite, andersonite,syntheses' thermal behavior, fluorescence' SOMMAIRE Leur teneuren Nous avonssynth6tis6 I'andersonite et la liebigite i partir du tricarbonateuranyl6 de sodiumfNaaUO2(COr)rl' l'6nergie H2O,6tudi& pal. uoulyr" thermique,serait de ldj et 6moles, respectivement.n!nO| les spectresde fluorescence, caicul6ede lai6paration entrebandes serait d'environ 2.5 eV. Elle ne semblepas affect6e par la temp€rature'. (Traduit Parla R6daction) Mots-cl6s:andersonite, liebigite, synthbses,comportement thermique, fluorescence' INTRODUC"I]ON Germany(Walenta 1977) andin the orebody of theTono mine,Gifu, Japan@4atsubwa1976). Several syntheses ofliebigite andandersoniie have been described starting In theuranyl carbonate system, the liebigite groupcan from oure chemicals (Blinkoff 1906, Axekod et al' be representedby the generalformula: R[UO2(CO3)3]' 1951,Bachelet et al. 1952,Meyrowitz & Ross 1961, nH2O.In this formula, R representsNarCa in anderson- Meyrowitzet al. 1963,dejka 1969,Coda et al. -1981)- ile, Ca, in liebigite, CaMg in swartzite, and Mg2 in in the presentpaper, a new methodof s;'nthesisof bayleyite,and n has a correspondingvalue of 6' 10 or andersoniteand liebigite is described,starting from the 11,12 wtd18, respectively. On thebasis of thestability complex tetrasodium uranyl trigSrbonqe diagrams(Alwan & Williams 1980),it may be expected Naa[UOr(CO3)r].This methodof synthesisallows-the that liebigite and andersonitecan coexist.Associations preparationof sufficientquantities of both minerals. The of liebigite and andersonitehave been found at the iOentityof the specieswas verified by X-ray diffraction Hillside mine,Yavapai County, Arizona (Axelrod el a/. andby chemicaland thermogravimetricanalyses. 1951) and at Stripa, Vdstrnanland,Sweden (Wellin 1958). Andersoniteoccurs by itself in the gypsum depositsof Myrthengraben,Semmering' Austria (Tufar SYNTmSIS 1967) and Jachymov,Czechoslovakia (Cejka & Ur- banec 1988).Liebigite also occurs at Shinkolobwe' ShabaZaire (Deliens 1985), Miillenbach, BlackForest, In this section,we discussthe synthesisof tetraso- 168 T}IE CANADIAN MINERALOGIST dium uranyl tricarbonate (NauTC) and its further rA3Lr1. cHErdrcArrcoMposrrroNoFsyNxEETrcLrEBrcrrEAND conversion into liebigite and andersonite EBSoNITE Synthesisof tetrasodiumuranyl tricarbonate Lieblgtte A!demDlte rc. of atomlc m. of atodc NaUTCwas synthesized atroom temperatureaccord- atoml mtlo atom0 mdo ing to the method of Blake et al. (1956), slightly cao' r5,29 0,2128 X.93 Nr2O 9.80 0.1580 2.06 modified to obtain pure crystals.These were washed UO: 39.60 0.1384 0.98 CaO 8.S2 0.1590 1.03 coz 18.97 0.40U 3.05 UO3 M.29 0.1548 1.00 with 2M NaCl. In this way, crystalsfree of any Na2CO3 f,zo 28.53 ' caz 20.10 0.4568 2.58 were obtained. The residual NaCl was subsequentlv E2o 78,72 Tolal 100.39 removedby dissolutionin a 50/50ethanol-water mix- 9S.83 ture. The identity of the air-dried NaUTC crystalswas . verified by chemicalanalysis and by comparisonof the ca2lUO2(co3)31 X0-11820 N%caIUo2(co3)31.8s2o X-ray-diffraction data with those given by Douglas (1956). I t! spight S. I Ume tO4. Conversionof NaUTC into liebigite and andersonite X-Rav CRYSTAIOGRAPHY Accordingto the stability fields of the mineralsof the liebigitegroup (Alwan & Williams 1980),andersonite X-ray-diffraction datawere recorded at 40 kV and20 can only be formed at a high NayCa} concentration mA usingCuKcrl radiation (1, = 1.540564).The diffrac- ratio, whereasliebigite is formed at a low Na*/Ca2* tion patternswere recorded by meansof a Guinier-Hiigg concentrationratio. This was confirmed in our experi- c,rmer4with a diameterof 100 mm. Silicon powder men$. (NBS640)was used as an intemal standard.The relative Two gramsof NaUTCwere dissolved in 100mL of intensitiesof the diffraction lines were measuredwitl a 0.04M CaCl2and left to evaporateat25oC in an open Carl ZeissJena MDl00 microdensitometer.Usine the vessel.After oneweek, well-formed hemimomhic crvs- cell parametersof liebigite(space group Bba2), .virth a tals of liebigite startedto grow. After 3 weetcs,typical 16.699,b 17.557and c 13.697A(Mereiter 1982), and cubic crystalsof andersonitewere formed as a result of thoseof andersonite(space group R3m), wrth a 17.902 the changedNa+/Ca2+ concentration ratio. andc 23.7344 (Codaet al. 1981),rhe powderpatierns The formationof liebigite can be written as: were indexed with the computer program of Visser (1969). 2Ca2++ [uo2(co3)3]4-+ l0H2o --> For both syntheticspecimens, all the observed Ca2[UO2(CO)3].10H2O reflectionscould be indexed,with AQo6,< AQd" (Ae The tranformationof liebigite into andersonitecan be 0.05'), in agreementwith PDF20-1092 and 1I-246. representedas: The densities of the two synthetic minerals were Ca2[UO2(CO)3].l0H2O+ 2Na+ --) measuredin tolueneat 25'C + 0. I by meansof a Cahn Electrobalance Na2Ca[UO2(CO)3].6H2O+ C*+ + 4H"O RG. The measureddensity of anderson- It should be mentioned that the formation of an ite is 2.834 t 0.005 g/cm3,which agreeswith the intermediatephase, consisting of lath-like crystals,was calculatedvalue of 2.860g/cm3, corresponding to Z = observed,as previously reportedby Meyrowia et al. 18.For liebigite,a densityof 2.416t 0.005g/cm3 was (1963).The study of theintermediate compound will be found,which corresponds to Z=8, the subjectof a separatepaper. The crystalsof liebigite The morphologyof andersoniteand liebigite crystals and andersonitewere handpicked. is shownin theelectron micrographs @igs. lA, B). The dimensionsof theliebigite crystals range from 0.1to 0.6 CnBnarcelCoMposmoN mm,whereas thoseof andersonite range from 0.051o 0.1 mm.The crystalsof andersoniteare clearly pseudocubic, and thoseof liebigite have a pronOuncedhemimorphic The air-dried syntheticspecimens were dissolvedin morphology(Mereiter 1986). 6 M HCl. The Na2Oand CaO contentwas determined by atomicabsorption spectroscopy (AAS), whereasUO3 was determinedspectrophotometrically with Arsenazo Thermslbehavior Itr as the reagent,the optical densitiesbeing measured at662.5 nm (Singer & Matucha1962).Tl-rcH2O and CO2 Concerningthe water content of the two minerals, contentswere measured on separatesamples by thermo- there is some confusion in the literature. Synthetic gravimetric analysis.Table I summarizesthe results. liebigite having-10 moles of H20 was describedby From the compositionin terms of oxides,the chemical Frondel(1958), Cejka & Urbanec(1979) nd Alwan & formulae were calculated by the classic method of Williams(1980). Appleman (1956) and Meyrowitzet al. residualoxygen. (1963)suggested a watercontent ranging berween 10 SYNTHESISOF LIEBIGITE AND ANDERSOMIE t69 100 Frc. 1. SEM micrographsof syntheticcrystals of liebigite (A) andandersonite (B). scale b4r: Fm. and l l moles of HrO. For synthetic andersonite,the Na2Ca[UO2(CO3)3]'6H2O 25-150"C watercontent was studied by a numbe.rof investigators -tilroo'" (dejka1969, Urbanec & dejka1979,Cejkaet a/. 1987). Na2ca[uo2(cot3]'H2o Theseauthors accept a water contentranging between ----------) 5.4 and5.8 molesof HrO. NarCa[UO2(CO)r] 300-1000'Coxides The thermalstability of both syntheticminerals was (TGA) investigated by thermogravimetric analyses Since liebigite does not **in *r.t'uf cavities (DSC). combinedwith differential scanningcalorimery (Mereiter l98t), and andersoniteis structurallycharac- was used, A DuPontDSC9IO and TGA95I apparatus ierized by the presenceof channelsalong the three-fold flow of N2 with an appliedheating rate of 5'C/min anda axis (Coda it al. l98l), the water molecules are atwhich of 30 mUmin. In orderto detectthe temperature structurallybonded in liebigite, whereasin andersonite, passed CO2is liberared,the outlet of the gas-streamwas zeolitic water may occur. througha solutionof Ba(OH)2.The results,summarized in Table 2, showthat syntheticliebigite andandersonite contain10.53 and 5.99 moles of H2O,respectively. Luminescencesqectra The decompositionof liebigite and andersoniteas be representedas: function of temperaturecan Both synthetic specimensfluoresce intensely blue- green bolh under short- and long-wave ultraviolet Caz[UOu(CO:)3]'llH2O 25-150'C iudiution. The fluorescencespectra were recordedby meansof a Perkin-Elmer MPS44B spectrofluorimeter Ca2[UO2(CO)3]'H2O 150-300"C at298 and77 K, with an excitationwavelength of 366 nm. CazlUOz(CO:)rl :OO-tOO0do*id", The slight differencesin the fluorescencespectra are -_---t characterizedby the modeof bonding of the U ator-nin the crystal structure.No phosphorescence.could.be detectedfor either specimensin a measuringinterval of 2 ms.The spectrafor syntheticliebigite andandersonite TABLX 2. BESULTS OF TSEAII@BAVIMSrBIC ANAI,YSES aI 298 and77 K are representedin Figures 2 aad
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  • Crystal Chemistry and Structural Complexity of Natural and Synthetic Uranyl Selenites

    Crystal Chemistry and Structural Complexity of Natural and Synthetic Uranyl Selenites

    Review Crystal Chemistry and Structural Complexity of Natural and Synthetic Uranyl Selenites Vladislav V. Gurzhiy 1,*, Ivan V. Kuporev 1, Vadim M. Kovrugin 1, Mikhail N. Murashko 1, Anatoly V. Kasatkin 2 and Jakub Plášil 3 1 Institute of Earth Sciences, St. Petersburg State University, University Emb. 7/9, St. Petersburg, 199034, Russian Federation; [email protected] (I.V.K.); [email protected] (V.M.K.); [email protected] (M.N.M.) 2 Fersman Mineralogical Museum of the Russian Academy of Sciences, Leninskiy pr. 18, 2, Moscow, 119071, Russian Federation; [email protected] 3 Institute of Physics, The Academy of Sciences of the Czech Republic, v.v.i., Na Slovance 2, Praha 8, 18221, Czech Republic; [email protected] * Correspondence: [email protected], [email protected] Received: 10 November 2019; Accepted: 28 November 2019; Published: 30 November 2019 Abstract: Comparison of the natural and synthetic phases allows an overview to be made and even an understanding of the crystal growth processes and mechanisms of the particular crystal structure formation. Thus, in this work, we review the crystal chemistry of the family of uranyl selenite compounds, paying special attention to the pathways of synthesis and topological analysis of the known crystal structures. Comparison of the isotypic natural and synthetic uranyl-bearing compounds suggests that uranyl selenite mineral formation requires heating, which most likely can be attributed to the radioactive decay. Structural complexity studies revealed that the majority of synthetic compounds have the topological symmetry of uranyl selenite building blocks equal to the structural symmetry, which means that the highest symmetry of uranyl complexes is preserved regardless of the interstitial filling of the structures.
  • How Geochemical Modelling Helps Understanding Processes in Mine Water Treatment Plants – Examples from Former Uranium Mining Sites in Germany

    How Geochemical Modelling Helps Understanding Processes in Mine Water Treatment Plants – Examples from Former Uranium Mining Sites in Germany

    Lappeenranta, Finland Mine Water and Circular Economy IMWA 2017 How geochemical modelling helps understanding processes in mine water treatment plants – examples from former uranium mining sites in Germany Anne Weber1, Andrea Kassahun2 1 GFI Grundwasser-Consulting-Institut GmbH Dresden, Meraner Straße 10, 01217 Dresden, Germany, [email protected] 2Wismut GmbH, Jagdschänkenstraße 29, 09117 Chemnitz, Germany Abstract Mine waters from former uranium mining sites in Germany contain high concentrations of metal(loids). They are treated by lime precipitation and adsorption technologies. In this work well- defined lab scale experiments were modelled to elucidate reaction networks and their susceptibility to varying water composition. Both treatment technologies involve mineral precipitation-dissolution, gas exchange, surface complexation at ferrihydrite. It was shown that the formation of alkaline earth uranyl carbonato complexes and the precipitation of liebigite-group minerals determine uranium retention in WISMUT’s mine water treatment operations. Sensitivity towards sludge composition and stability of arsenic sorption even at reducing conditions were derived from scenario simulations. Key words: mine water treatment, geochemical modelling, uranium, arsenic Introduction In the course of remediation of the former Eastern German uranium mining sites, WIS- MUT GmbH operates six water treatment plants (WTPs). More than 25 Mm³ of tailings management facility seepage and mine waters are treated annually to remove site specific contaminants (e.g. uranium, radium, arsenic, iron, manganese). Modified lime precipita- tion is the prevailing technology, immobilizing contaminants by lime addition and induced precipitation of ferrihydrite Fe(OH)3. Evolving changes in mine water composition will influence the efficiency of water treatment with respect to the specific contaminants and require adjustments in the treatment technol- ogies.
  • Minerals of Arizona Report

    Minerals of Arizona Report

    MINERALS OF ARIZONA by Frederic W. Galbraith and Daniel J. Brennan THE ARIZONA BUREAU OF MINES Price One Dollar Free to Residents of Arizona Bulletin 181 1970 THE UNIVERSITY OF ARIZONA TUCSON TABLE OF CONT'ENTS EIements .___ 1 FOREWORD Sulfides ._______________________ 9 As a service about mineral matters in Arizona, the Arizona Bureau Sulfosalts ._. .___ __ 22 of Mines, University of Arizona, is pleased to reprint the long-standing booklet on MINERALS OF ARIZONA. This basic journal was issued originally in 1941, under the authorship of Dr. Frederic W. Galbraith, as Simple Oxides .. 26 a bulletin of the Arizona Bureau of Mines. It has moved through several editions and, in some later printings, it was authored jointly by Dr. Gal­ Oxides Containing Uranium, Thorium, Zirconium .. .... 34 braith and Dr. Daniel J. Brennan. It now is being released in its Fourth Edition as Bulletin 181, Arizona Bureau of Mines. Hydroxides .. .. 35 The comprehensive coverage of mineral information contained in the bulletin should serve to give notable and continuing benefits to laymen as well as to professional scientists of Arizona. Multiple Oxides 37 J. D. Forrester, Director Arizona Bureau of Mines Multiple Oxides Containing Columbium, February 2, 1970 Tantaum, Titanium .. .. .. 40 Halides .. .. __ ____ _________ __ __ 41 Carbonates, Nitrates, Borates .. .... .. 45 Sulfates, Chromates, Tellurites .. .. .. __ .._.. __ 57 Phosphates, Arsenates, Vanadates, Antimonates .._ 68 First Edition (Bulletin 149) July 1, 1941 Vanadium Oxysalts ...... .......... 76 Second Edition, Revised (Bulletin 153) April, 1947 Third Edition, Revised 1959; Second Printing 1966 Fourth Edition (Bulletin 181) February, 1970 Tungstates, Molybdates.. _. .. .. .. 79 Silicates ...