DOCSLIB.ORG

Appendix a Further Reading

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text

Load more

Appendix A Further Reading D.M. Adams, Inorganic Solids, Wiley, New York, 1974. Very good older book with excellent figures. It emphasizes close packing. L.V. Azaroff, Introduction to Solids, McGraw-Hill, New York, 1960. L. Bragg, The Crystalline State, G. Bell and Sons, London, 1965. L. Bragg and G.F. Claringbull, Crystal Structures of Minerals, G. Bell, London, 1965. P.J. Brown and J.B. Forsyth. The Crystal Structure of Solids, E. Arnold, London, 1973. M.J. Buerger, Elementary Crystallography, Wiley, New York, 1956. J.K. Burdett, Chemical Bonding in Solids, Oxford University Press, Oxford, 1992. Cambridge Structural Data Base (CSD). Cambridge Crystallographic Data Centre, University Chemical Laboratory, Cambridge, England. C.R.A. Catlow, Ed., Computer Modelling in Inorganic Crystallography, Academic Press, San Diego, 1997. A.K. Cheetham and P. Day, Solid-State Chemistry, Techniques, Clarendon, Ox- ford, 1987. P.A. Cox, Transition Metal Oxides, Oxford University Press, Oxford, 1992. CrystalMaker, A powerful computer program for the Macintosh and Windows by David Palmer, CrystalMaker Software Ltd., Yarnton, Oxfordshire, UK. This program was used for many figures and it aided greatly in interpreting many structures for this book and accompanying CD. B.D. Cullity, Elements of X-ray Diffraction, Addison-Wesley, Reading, MA, 1956. J. Donohue, The Structure of The Elements, Wiley, New York, 1974. The most comprehensive coverage of the structures of elements. B.E. Douglas, D.H. McDaniel, and J.J. Alexander, Concepts and Models of Inor- ganic Chemistry, 3rd ed., Wiley, New York, 1994. The PTOT system is discussed and applied briefly. F.S. Galasso, Structure, Properties and Preparation of Perovskite-Type Compounds, Pergamon, Oxford, 1969. F.S. Galasso, Structure and Properties of Inorganic Solids, Pergamon, Oxford, 1970. Excellent figures to help to visualize structures. C. Hammond, Introduction to Crystallography, Oxford University Press, Oxford, 1990. N.B. Hannay, Solid-State Chemistry, Prentice-Hall, Englewood Cliffs, NJ, 1967. R.M. Hazen and L.W. Finger, Comparative Crystal Chemistry, Wiley, New York, 1984. Further Reading 307 W. Hume-Rothery, R.E. Smallman and C.W. Haworth, The Structure of Metals and Alloys, Institute of Metals and the Institution of Metallurgists, London, 1969. B.G. Hyde, and S. Anderson, Inorganic Crystal Structures, Wiley, New York, 1989. Inorganic Crystal Structural Data Base (ICSD). Fachinformationszentrum Karls- ruhe, Germany. International Tables for X-Ray Crystallography, Vol. 1, Symmetry Groups, N.F.M. Henry and K. Lonsdale, Eds, International Union of Crystallography, Kynoch Press, Birmingham, 1952. The complete source for space groups and crys- tallographic information. W.D. Kingery, Introduction to Ceramics, Wiley, New York, 1967. H. Krebs, Fundametals of Inorganic Crystal Chemistry, McGraw-Hill, London, 1968. M.F.C. Ladd, Structure and Banding in Solid State Chemistry, Wiley, New York, 1979. F. Liebau, Structural Chemistry of Silicates, Springer-Verlag, Berlin, 1985. Y. Matsushita, Chalcogenide Crystal Structure Data library, Version 5.5B, 2004, Institute for Solid State Physics, University of Tokyo. A library of about 10,000 structures including many other than chalcogenides. H.D. Megaw, Crystal Structures, A Working Approach, Saunders, Philadelphia, 1973. Metals Crystallographic Data File (CRYSTMET). National Research Council of Canada, Ottawa. U. Mu¨ ller, Inorganic Structural Chemistry, Wiley, New York, 1993. I. Naray-Szabo, Inorganic Crystal Chemistry, Akademiai Kiado, Budapest, 1969. R.E. Newnham, Structure–Property Relations, Springer-Verlag, New York, 1975. W.B. Pearson, The Crystal Chemistry and Physics of Metals and Alloys, Wiley, New York, 1972. An excellent book for intermetallic compounds, excellent figures, gives occupancies and spacings for close-packed layers for many structures. D. Pettifor, Bonding and Structure of Molecules and Solids, Oxford University Press, Oxford, 1995. F.C. Phillips, An Introduction to Crystallography, 4th ed., Wiley, New York, 1971. A. Putnis, A., Introduction to Mineral Sciences, Cambridge University Press, Cambridge, 1992. Good background on experimental methods and excellent coverage of metal silicates. G.V. Raynor, The Structure of Metals and Alloys, Institute of Metals, London, 1954. R. Roy, Ed., The Major Ternary Structural Families, Springer-Verlag, New York, 1974. D.F. Shriver and P.W. Atkins, Inorganic Chemistry, 3rd. ed., Freeman, New York, 1999. L. Smart and E. Moore, Solid State Chemistry, Chapman and Hall, London, 1992. A.R. Verma and P. Krishna, Polymorphism and Polytypism in Crystals, Wiley, New York, 1966. M.T. Weller, Inorganic Materials Chemistry, Oxford University Press, Oxford, 1994. A.F. Wells, Structural Inorganic Chemistry, 5th ed., Oxford University Press, Oxford, 1984. The most complete one-volume coverage of inorganic struc- tures. A.R. West, Basic Solid State Chemistry, 2nd ed., Wiley, New York, 1999. A. Wold and R. Dwight, Solid State Chemistry, Chapman and Hall, London 1993. 308 Appendix A R.W.G. Wyckoff,. Crystal Structures, Vols. 1–6, 2nd ed., Wiley, New York, 1963– 1968. The most comprehensive coverage of crystal structures with fine figures, space groups, unit cell constants and atom coordinates. Vols. 1–4, inorganic compounds and Vols. 5 and 6, organic compounds. Appendix B Polyhedra in Close-Packed Structures Lattice Types The Seven Systems of Crystals are shown in Figure 2.2. The relationship between the trigonal and rhombohedral systems is shown in Figure B.1a. The possibilities of body-centered and base-centered cells give the 14 Bravais Lattices, also shown in Figure 2.2. A face-centered cubic (fcc) cell can be represented as a 608 rhombohedron, as shown in Figure B.1b. The fcc cell is used because it shows the high symmetry of the cube. Polyhedra Figure B.2 shows polyhedra commonly encountered. The five Platonic (or regular) solids are shown at the top. Beside the octahedron and cube, the octahedron is shown inside a cube, oriented so the symmetry elements in common coincide. These solids are conjugates: one formed by connecting the face centers of the other. The tetrahedron is its own conjugate, because con- necting the face centers gives another tetrahedron. The icosahedron and pen- tagonal dodecahedron are conjugates. The square antiprism and trigonal Figure B.1 (a) The relationship of a hexagonal cell to trigonal (rhombohedral) cells. (b) the 608 rhombohedral cell related to a face-centered cubic cell. (CrystalMaker) 310 Appendix B Figure B.2. Platonic and other solids. The numbers of vertices (v) and faces (f) are shown. Models from Stacking Polyhedra 311 dodecahedron are common for coordination compounds with CN 8. The cuboctahedron is encountered in cubic close-packed structures. A cuboctahe- dron is formed by eight ReO6 octahedra in ReO3 (Figure 5.23b). The truncated tetrahedron is encountered in Laves phases (MgM2, Figure 9.43). The bucky ball (not shown in Figure B.2) is the structure of C60 (Figure 4.11). Figures B.3 and B.4 provide cutouts for some polyhedra. Enlarged copies work well. Figure B.3. Cutouts for an octahedron, tetrahedron, cube, and buckyball. 312 Appendix B Figure B.4. Cutouts for an icosahedron, trigonal dodecahedron, and pentagonal dodecahedron. Models from Stacking Polyhedra 313 Polyhedra in Cubic Close-Packed (ccp) and Hexagonal Close-Packed (hcp) Structures For a cubic close-packed (ccp) structure, each atom is surrounded by 12 atoms forming a cuboctahedron (Figure B.5). The six octahedral sites (O) form an octahedron around the central atom and the eight tetrahedral sites (T) form a cube (Figure 4.6). For a hexagonal close-packed (hcp) structure, the polyhedron is shown in Figure B.5. The square and trigonal faces above and below the central plane of the hexagonal plane are aligned. Models from Stacking Polyhedra Good models of many crystal structures can be built by stacking tetrahedra or octahedra. Such models can be helpful in visualizing the structure. Figure B.6 shows the wurtzite (ZnS, 22PT) structure with tetrahedra stacked along the c axis of the hexagonal cell. One of the two sets of T layers between two P layers is filled (Tþ or tetrahedra pointing upward as shown here). The S atoms (dark balls) are in an AB sequence. The zinc blende (or sphalerite, ZnS, 32PT, structure) is shown with tetrahedra stacked along the body diagonal of the cubic cell. The S atoms are in an ABC sequence, a ccp arrangement. The A, B,or C positions of Zn are the same as those of the S atom at the upward apex of each tetrahedron. Another view of the cell shows the positions of the tetrahe- dra in each cubic cell. The Zn atoms form a tetrahedron within the cubic cell. Fluorite (CaF2, 3 3PTT) has Ca in P layers with both sets of T layers filled by F. In Figure B.6 the fluorite cell is shown with Ca as spheres forming the fcc cell and F in tetrahedra pointed upward and downward. Figure B.5. The polyhedra of close neighbors of an atom in ccp and hcp structures. (Source: CrystalMaker, by David Palmer, CrystalMaker Software Ltd., Begbroke Science Park, Bldg. 5, Sandy Lane, Yarnton, Oxfordshire, OX51PF, UK.) Figure B.6. Structures built from stacking tetrahedra: ZnS, wurtzite, 22PT; ZnS, zinc blends, 3 2PT; and CaF2, fluorite 3 dPTT. (Source: CrystalMaker, by David Palmer, CrystalMaker Software Ltd., Begbroke Science Park, Bldg. 5, Sandy Lane, Yarnton, Oxfordshire, OX51PF, UK.) 314 Appendix B The structure of NaCl (3 2PO) is shown in Figure B.7 as NaCl6 octahedra À stacked along the body diagonal of the cubic cell. The Cl ions are in an ABC þ sequence and the Na ions in O sites are in an ABC sequence. The NiAs (22PO) structure is shown also. The As atoms are in an AB sequence and Ni atoms in O sites are all at C positions, aligned along the c axis of the cell. The CdCl2 structure [3 3POP(h)] shows layers of octahedra with gaps between them. The P layers are filled by Cl atoms in an ABC sequence, with alternate O layers vacant.
Recommended publications
  • Standardal /Z<-Z

    Standardal /Z<-Z

    Hamilton Ui StandardAl HANL1r0N STNTVI) Bi;.TVGircr1h VP0FT SVHCA, 5712 1 0 L 'K-KY-o LaIUI P~FrcX.-19F TEST2 ?i0&at CONrxyhCT NO. TIAS 9-8159 NASA Aid!,zj.. SACECAFT CF.CErR ,_eb-r 1970 Prepared Byi/kA / 70 L.A. Wilis, axrer.mwtal Enineer Pae Aproved ByA1"" /Z<-Z -;' W. A. Blezhcr0 Chiet Pa tc Advanced -nginee.rin­ ONUMBE) AHRU) U NASA CR OR ?MX OR AD NUMBER) (CATEGORY) Hamilton L Standard cnisni _ This report contairs test results defining the operating chsractcristics of lithin peroxide to the extcnt required to quantify system level ponalties. The effects of chemical caulysts, bed cooling, che.,ical Panufacturing tech­ uiques, opera ing conditions, and cheaica) handling jroc Curea are evaluated. ii! StandardHamilton i5U TAlBLE OF CO_&E!PS Section me No. 1.0 SUMM4ARY 1 2 .0 INTRODUCTION 3 3.0 PROGRAM DEFINITION 3.1 Program Objectives 4 3.2 Test Objectives 4 3.3 Program Description 5 3.4 Test Conitions T 3.5 Test Facility 7 3.6 - Test Hardware 12 3.7 Planned Test Sequence 18 3.8 Test.Results 21 ho TEST DATA PRESENTATION 22 4.1 Performance Data 22 4.2 Chemical Analysis Data 1o6 5.0 PERFOrd4ICE ANALYSIS 109 5.1 Catalyst Evaluation 109 5.2 Bed Cooling Evaluation 134 5.3 Procedural Test Evaluation 0h5 5.4 Off Design Test Evaluation 153 5.5 End Item Canister Evaluation 157 5.6 Li 2O2 System Penalty Evaluation 163 6.0 RECOM ENDED FUTURE EFFORT 165 7.0 APPENDIX 167 7.1 Specification for Lithium Peroxide 167 Manufacturing 7.2 Specification for Lithium Peroxide Storage a68 7.3 Specification for Lithium Peroxide 170 Cartridge Loading iv Standard 5712 LIST OP TABLFS Table No.
  • Transport of Dangerous Goods

    Transport of Dangerous Goods

    ST/SG/AC.10/1/Rev.16 (Vol.I) Recommendations on the TRANSPORT OF DANGEROUS GOODS Model Regulations Volume I Sixteenth revised edition UNITED NATIONS New York and Geneva, 2009 NOTE The designations employed and the presentation of the material in this publication do not imply the expression of any opinion whatsoever on the part of the Secretariat of the United Nations concerning the legal status of any country, territory, city or area, or of its authorities, or concerning the delimitation of its frontiers or boundaries. ST/SG/AC.10/1/Rev.16 (Vol.I) Copyright © United Nations, 2009 All rights reserved. No part of this publication may, for sales purposes, be reproduced, stored in a retrieval system or transmitted in any form or by any means, electronic, electrostatic, magnetic tape, mechanical, photocopying or otherwise, without prior permission in writing from the United Nations. UNITED NATIONS Sales No. E.09.VIII.2 ISBN 978-92-1-139136-7 (complete set of two volumes) ISSN 1014-5753 Volumes I and II not to be sold separately FOREWORD The Recommendations on the Transport of Dangerous Goods are addressed to governments and to the international organizations concerned with safety in the transport of dangerous goods. The first version, prepared by the United Nations Economic and Social Council's Committee of Experts on the Transport of Dangerous Goods, was published in 1956 (ST/ECA/43-E/CN.2/170). In response to developments in technology and the changing needs of users, they have been regularly amended and updated at succeeding sessions of the Committee of Experts pursuant to Resolution 645 G (XXIII) of 26 April 1957 of the Economic and Social Council and subsequent resolutions.
  • LOW TEMPERATURE HYDROTHERMAL COPPER, NICKEL, and COBALT ARSENIDE and SULFIDE ORE FORMATION Nicholas Allin

    LOW TEMPERATURE HYDROTHERMAL COPPER, NICKEL, and COBALT ARSENIDE and SULFIDE ORE FORMATION Nicholas Allin

    Montana Tech Library Digital Commons @ Montana Tech Graduate Theses & Non-Theses Student Scholarship Spring 2019 EXPERIMENTAL INVESTIGATION OF THE THERMOCHEMICAL REDUCTION OF ARSENITE AND SULFATE: LOW TEMPERATURE HYDROTHERMAL COPPER, NICKEL, AND COBALT ARSENIDE AND SULFIDE ORE FORMATION Nicholas Allin Follow this and additional works at: https://digitalcommons.mtech.edu/grad_rsch Part of the Geotechnical Engineering Commons EXPERIMENTAL INVESTIGATION OF THE THERMOCHEMICAL REDUCTION OF ARSENITE AND SULFATE: LOW TEMPERATURE HYDROTHERMAL COPPER, NICKEL, AND COBALT ARSENIDE AND SULFIDE ORE FORMATION by Nicholas C. Allin A thesis submitted in partial fulfillment of the requirements for the degree of Masters in Geoscience: Geology Option Montana Technological University 2019 ii Abstract Experiments were conducted to determine the relative rates of reduction of aqueous sulfate and aqueous arsenite (As(OH)3,aq) using foils of copper, nickel, or cobalt as the reductant, at temperatures of 150ºC to 300ºC. At the highest temperature of 300°C, very limited sulfate reduction was observed with cobalt foil, but sulfate was reduced to sulfide by copper foil (precipitation of Cu2S (chalcocite)) and partly reduced by nickel foil (precipitation of NiS2 (vaesite) + NiSO4·xH2O). In the 300ºC arsenite reduction experiments, Cu3As (domeykite), Ni5As2, or CoAs (langisite) formed. In experiments where both sulfate and arsenite were present, some produced minerals were sulfarsenides, which contained both sulfide and arsenide, i.e. cobaltite (CoAsS). These experiments also produced large (~10 µm along longest axis) euhedral crystals of metal-sulfide that were either imbedded or grown upon a matrix of fine-grained metal-arsenides, or, in the case of cobalt, metal-sulfarsenide. Some experimental results did not show clear mineral formation, but instead demonstrated metal-arsenic alloying at the foil edges.
  • An Investigation of the Crystal Growth of Heavy Sulfides in Supercritical

    An Investigation of the Crystal Growth of Heavy Sulfides in Supercritical

    AN ABSTRACT OF THE THESIS OF LEROY CRAWFORD LEWIS for the Ph. D. (Name) (Degree) in CHEMISTRY presented on (Major) (Date) Title: AN INVESTIGATION OF THE CRYSTAL GROWTH OF HEAVY SULFIDES IN SUPERCRITICAL HYDROGEN SULFIDE Abstract approved Redacted for privacy Dr. WilliarriIJ. Fredericks Solubility studies on the heavy metal sulfides in liquid hydrogen sulfide at room temperature were carried out using the isopiestic method. The results were compared with earlier work and with a theoretical result based on Raoult's Law. A relative order for the solubilities of sulfur and the sulfides of tin, lead, mercury, iron, zinc, antimony, arsenic, silver, and cadmium was determined and found to agree with the theoretical result. Hydrogen sulfide is a strong enough oxidizing agent to oxidize stannous sulfide to stannic sulfide in neutral or basic solution (with triethylamine added). In basic solution antimony trisulfide is oxi- dized to antimony pentasulfide. In basic solution cadmium sulfide apparently forms a bisulfide complex in which three moles of bisul- fide ion are bonded to one mole of cadmium sulfide. Measurements were made extending the range over which the volumetric properties of hydrogen sulfide have been investigated to 220 °C and 2000 atm. A virial expression in density was used to represent the data. Good agreement, over the entire range investi- gated, between the virial expressions, earlier work, and the theorem of corresponding states was found. Electrical measurements were made on supercritical hydro- gen sulfide over the density range of 10 -24 moles per liter and at temperatures from the critical temperature to 220 °C. Dielectric constant measurements were represented by a dielectric virial ex- pression.
  • Washington State Minerals Checklist

    Washington State Minerals Checklist

    Division of Geology and Earth Resources MS 47007; Olympia, WA 98504-7007 Washington State 360-902-1450; 360-902-1785 fax E-mail: [email protected] Website: http://www.dnr.wa.gov/geology Minerals Checklist Note: Mineral names in parentheses are the preferred species names. Compiled by Raymond Lasmanis o Acanthite o Arsenopalladinite o Bustamite o Clinohumite o Enstatite o Harmotome o Actinolite o Arsenopyrite o Bytownite o Clinoptilolite o Epidesmine (Stilbite) o Hastingsite o Adularia o Arsenosulvanite (Plagioclase) o Clinozoisite o Epidote o Hausmannite (Orthoclase) o Arsenpolybasite o Cairngorm (Quartz) o Cobaltite o Epistilbite o Hedenbergite o Aegirine o Astrophyllite o Calamine o Cochromite o Epsomite o Hedleyite o Aenigmatite o Atacamite (Hemimorphite) o Coffinite o Erionite o Hematite o Aeschynite o Atokite o Calaverite o Columbite o Erythrite o Hemimorphite o Agardite-Y o Augite o Calciohilairite (Ferrocolumbite) o Euchroite o Hercynite o Agate (Quartz) o Aurostibite o Calcite, see also o Conichalcite o Euxenite o Hessite o Aguilarite o Austinite Manganocalcite o Connellite o Euxenite-Y o Heulandite o Aktashite o Onyx o Copiapite o o Autunite o Fairchildite Hexahydrite o Alabandite o Caledonite o Copper o o Awaruite o Famatinite Hibschite o Albite o Cancrinite o Copper-zinc o o Axinite group o Fayalite Hillebrandite o Algodonite o Carnelian (Quartz) o Coquandite o o Azurite o Feldspar group Hisingerite o Allanite o Cassiterite o Cordierite o o Barite o Ferberite Hongshiite o Allanite-Ce o Catapleiite o Corrensite o o Bastnäsite
  • Theoretical Studies on As and Sb Sulfide Molecules

    Theoretical Studies on As and Sb Sulfide Molecules

    Mineral Spectroscopy: A Tribute to Roger G. Bums © The Geochemical Society, Special Publication No.5, 1996 Editors: M. D. Dyar, C. McCammon and M. W. Schaefer Theoretical studies on As and Sb sulfide molecules J. A. TOSSELL Department of Chemistry and Biochemistry University of Maryland, College Park, MD 20742, U.S.A. Abstract-Dimorphite (As4S3) and realgar and pararealgar (As4S4) occur as crystalline solids con- taining As4S3 and As4S4 molecules, respectively. Crystalline As2S3 (orpiment) has a layered structure composed of rings of AsS3 triangles, rather than one composed of discrete As4S6 molecules. When orpiment dissolves in concentrated sulfidic solutions the species produced, as characterized by IR and EXAFS, are mononuclear, e.g. ASS3H21, but solubility studies suggest trimeric species in some concentration regimes. Of the antimony sulfides only Sb2S3 (stibnite) has been characterized and its crystal structure does not contain Sb4S6 molecular units. We have used molecular quantum mechanical techniques to calculate the structures, stabilities, vibrational spectra and other properties of As S , 4 3 As4S4, As4S6, As4SIO, Sb4S3, Sb4S4, Sb4S6 and Sb4SlO (as well as S8 and P4S3, for comparison with previous calculations). The calculated structures and vibrational spectra are in good agreement with experiment (after scaling the vibrational frequencies by the standard correction factor of 0.893 for polarized split valence Hartree-Fock self-consistent-field calculations). The calculated geometry of the As4S. isomer recently characterized in pararealgar crystals also agrees well with experiment and is calculated to be about 2.9 kcal/mole less stable than the As4S4 isomer found in realgar. The calculated heats of formation of the arsenic sulfide gas-phase molecules, compared to the elemental cluster molecules As., Sb, and S8, are smaller than the experimental heats of formation for the solid arsenic sulfides, but shown the same trend with oxidation state.
  • Rediscovery of the Elements — a Historical Sketch of the Discoveries

    Rediscovery of the Elements — a Historical Sketch of the Discoveries

    REDISCOVERY OF THE ELEMENTS — A HISTORICAL SKETCH OF THE DISCOVERIES TABLE OF CONTENTS incantations. The ancient Greeks were the first to Introduction ........................1 address the question of what these principles 1. The Ancients .....................3 might be. Water was the obvious basic 2. The Alchemists ...................9 essence, and Aristotle expanded the Greek 3. The Miners ......................14 philosophy to encompass a obscure mixture of 4. Lavoisier and Phlogiston ...........23 four elements — fire, earth, water, and air — 5. Halogens from Salts ...............30 as being responsible for the makeup of all 6. Humphry Davy and the Voltaic Pile ..35 materials of the earth. As late as 1777, scien- 7. Using Davy's Metals ..............41 tific texts embraced these four elements, even 8. Platinum and the Noble Metals ......46 though a over-whelming body of evidence 9. The Periodic Table ................52 pointed out many contradictions. It was taking 10. The Bunsen Burner Shows its Colors 57 thousands of years for mankind to evolve his 11. The Rare Earths .................61 thinking from Principles — which were 12. The Inert Gases .................68 ethereal notions describing the perceptions of 13. The Radioactive Elements .........73 this material world — to Elements — real, 14. Moseley and Atomic Numbers .....81 concrete basic stuff of this universe. 15. The Artificial Elements ...........85 The alchemists, who devoted untold Epilogue ..........................94 grueling hours to transmute metals into gold, Figs. 1-3. Mendeleev's Periodic Tables 95-97 believed that in addition to the four Aristo- Fig. 4. Brauner's 1902 Periodic Table ...98 telian elements, two principles gave rise to all Fig. 5. Periodic Table, 1925 ...........99 natural substances: mercury and sulfur.
  • ARSENIC in DRINKING-WATER Pp33-40.Qxd 11/10/2004 10:08 Page 40 Pp41-96.Qxd 11/10/2004 10:19 Page 41

    ARSENIC in DRINKING-WATER Pp33-40.Qxd 11/10/2004 10:08 Page 40 Pp41-96.Qxd 11/10/2004 10:19 Page 41

    pp33-40.qxd 11/10/2004 10:08 Page 39 ARSENIC IN DRINKING-WATER pp33-40.qxd 11/10/2004 10:08 Page 40 pp41-96.qxd 11/10/2004 10:19 Page 41 ARSENIC IN DRINKING-WATER 1. Exposure Data 1.1 Chemical and physical data Arsenic is the 20th most common element in the earth’s crust, and is associated with igneous and sedimentary rocks, particularly sulfidic ores. Arsenic compounds are found in rock, soil, water and air as well as in plant and animal tissues. Although elemental arsenic is not soluble in water, arsenic salts exhibit a wide range of solubilities depending on pH and the ionic environment. Arsenic can exist in four valency states: –3, 0, +3 and +5. Under reducing conditions, the +3 valency state as arsenite (AsIII) is the dominant form; the +5 valency state as arsenate (AsV) is generally the more stable form in oxygenized environ- ments (Boyle & Jonasson, 1973; National Research Council, 1999; O’Neil, 2001; WHO, 2001). Arsenic species identified in water are listed in Table 1. Inorganic AsIII and AsV are the major arsenic species in natural water, whereas minor amounts of monomethylarsonic acid (MMA) and dimethylarsinic acid (DMA) can also be present. The trivalent mono- methylated (MMAIII) and dimethylated (DMAIII) arsenic species have been detected in lake water (Hasegawa et al., 1994, 1999). The presence of these trivalent methylated arsenical species is possibly underestimated since only few water analyses include a solvent sepa- ration step required to identify these trivalent species independently from their respective a Table 1. Some arsenic species identified in water Name Abbreviation Chemical formula CAS No.
  • Polymetallic Mineralization in Ediacaran Sediments in the Żarki-Kotowice Area, Poland

    Polymetallic Mineralization in Ediacaran Sediments in the Żarki-Kotowice Area, Poland

    MINERALOGIA, 43, No 3-4: 199-212 (2012) DOI: 10.2478/v10002-012-0008-0 www.Mineralogia.pl MINERALOGICAL SOCIETY OF POLAND POLSKIE TOWARZYSTWO MINERALOGICZNE __________________________________________________________________________________________________________________________ Original paper Polymetallic mineralization in Ediacaran sediments in the Żarki-Kotowice area, Poland Łukasz KARWOWSKI1*, Marek MARKOWIAK2 1University of Silesia, Faculty of Earth Sciences, ul. Będzińska 60, 41-200 Sosnowiec, Poland; e-mail: [email protected] 2Polish Geological Institute - Research and Development Unit, Upper Silesian Branch, ul. Królowej Jadwigi 1, 41-200 Sosnowiec, Poland; e-mail: [email protected] * Corresponding author Received: September 5, 2012 Received in revised form: February 20, 2013 Accepted: March 17, 2013 Available online: March 30, 2013 Abstract. In one small mineral vein in core from borehole 144-Ż in the Żarki-Kotowice area, almost all of the ore minerals known from related deposits in the vicinity occur. Some of the minerals in the vein described in this paper, namely, nickeline, hessite, native silver and minerals of the cobaltite-gersdorffite group, have not previously been reported from elsewhere in the Kraków-Lubliniec tectonic zone. The identified minerals are chalcopyrite, pyrite, marcasite, sphalerite, Co-rich pyrite, tennantite, tetrahedrite, bornite, galena, magnetite, hematite, cassiterite, pyrrhotite, wolframite (ferberite), scheelite, molybdenite, nickeline, minerals of the cobaltite- gersdorffite group, carrollite, hessite and native silver. Moreover, native bismuth, bismuthinite, a Cu- and Ag-rich sulfosalt of Bi (cuprobismutite) and Ni-rich pyrite also occur in the vein. We suggest that, the ore mineralization from the borehole probably reflects post-magmatic hydrothermal activity related to an unseen granitic intrusion located under the Mesozoic sediments in the Żarki-Pilica area.
  • United States Patent Office Patented May 26, 964 1

    United States Patent Office Patented May 26, 964 1

    3,134,646 United States Patent Office Patented May 26, 964 1. 2 3,134,646 anhydrous lithium peroxide. The rapid drying step PREPARATION 6Fiff UM PEROXIDE. serves not only to effect the removal of water added Ricardo O. Bach, Gastonia, N.C., assignor to Lithium through the water solutions of the reactants and, addi Corporation of America, inc., New York, N.Y., a cor tionally, formed in the course of the reaction, but serves, poration of Minnesota also, and quite surprisingly, to bring about the important No Drawing, Filed Jan. 5, 1962, Set. No. 166,395 function of effecting rapid transfer of the active oxygen 10 Claims. (CI. 23-184) of the hydrogen peroxide to the lithium hydroxide to consummate formation of the desired lithium peroxide. This invention relates to an improved method of pro The lithium hydroxide (which term also includes ducing substantially anhydrous lithium peroxide, and to O lithium hydroxide hydrates such as lithium hydroxide the product produced thereby. monohydrate) is most advantageously used in the form Methods for the production of substantially anhydrous of a strong to substantially saturated aqueous solution, lithium peroxide have long been known in the art. More for instance, from about 8 or 10 to 12% concentration. recently, improvements in such methods have been pro In those instances where the resulting lithium hydroxide posed as disclosed, for instance, in U.S. Patents Nos. 5 solutions contain insoluble impurities as, for instance, 2,448,485 and 2,962,358. However, each of the methods lithium carbonate, it is desirable to filter the solutions disclosed in these patents has certain significant disad to remove said impurities so as to bring about greater vantages, particularly from an economic standpoint, purity of the final substantially anhydrous lithium which make their utilization in commercial operations peroxide.
  • Removal of 2, 4-Dinitrophenol by Ferrate

    Removal of 2, 4-Dinitrophenol by Ferrate

    University of Central Florida STARS Electronic Theses and Dissertations, 2004-2019 2008 Removal Of 2, 4-dinitrophenol By Ferrate Gianna Cooley University of Central Florida Part of the Environmental Engineering Commons Find similar works at: https://stars.library.ucf.edu/etd University of Central Florida Libraries http://library.ucf.edu This Masters Thesis (Open Access) is brought to you for free and open access by STARS. It has been accepted for inclusion in Electronic Theses and Dissertations, 2004-2019 by an authorized administrator of STARS. For more information, please contact [email protected]. STARS Citation Cooley, Gianna, "Removal Of 2, 4-dinitrophenol By Ferrate" (2008). Electronic Theses and Dissertations, 2004-2019. 3619. https://stars.library.ucf.edu/etd/3619 REMOVAL OF 2, 4-DINITROPHENOL BY FERRATE by GIANNA GRIFFITH COOLEY B.S. Loyola Univeristy New Orleans, 2002 A thesis submitted in partial fulfillment of the requirements for the degree of Master of Environmental Engineering in the Department of Civil and Environmental Engineering in the College of Engineering and Computer Science at the University of Central Florida Orlando, Florida Fall Term 2008 Major Professor: Debra R. Reinhart © 2008 Gianna Griffith Cooley ii ABSTRACT VI 2- Ferrate (molecular formula, Fe O4 ) has been studied increasingly since the 1970s as a disinfectant and coagulant for domestic wastewater and also as an oxidant for industrial wastewaters (Murmann and Roginson, 1974, Gilbert et al., 1978, Kazama, 1994, Jiang et al., 2002, and Sharmaet al., 2005). This research was performed to explore whether ferrate could possibly be used as chemical treatment for industrial wastewaters from plastic, chemical, dye, soap, and wood stain producing plants that contain 2, 4-Dinitrophenol (DNP).
  • The Structure of Alkali Silicate Glasses and Melts: a Multi-Spectroscopic Approach

    The Structure of Alkali Silicate Glasses and Melts: a Multi-Spectroscopic Approach

    The structure of alkali silicate glasses and melts: A multi-spectroscopic approach by Cedrick A. O'Shaughnessy A thesis submitted in conformity with the requirements for the degree of Doctor of Philosophy in Geology Graduate Department of Earth Sciences University of Toronto c Copyright 2019 by Cedrick A. O'Shaughnessy Abstract The structure of alkali silicate glasses and melts: A multi-spectroscopic approach Cedrick A. O'Shaughnessy Doctor of Philosophy in Geology Graduate Department of Earth Sciences University of Toronto 2019 The structure of alkali silicate glasses and melts is investigated using a multi-spectroscopic approach. Raman spectroscopy is used to characterize the local to intermediate range order within the glasses. We show that the distribution of rings varies as a function of composition, with 3-membered rings gaining importance with increasing alkali content. We apply a newly developed model for the fitting of the high n frequency envelope related to SiO4 symmetric stretch vibrations of Q species. These fits are interpreted using the idea of modifier bound bridging oxygen. The proportions of the different Qn species vary with alkali concentration with Q4 species breaking down to form lower order Qn species with increasing alkali 2 content. The Q peak appears at increasingly higher concentrations of M2O with increasing cation size. This leads us to believe that cations with a higher charge density cluster more readily than cations with a lower charge density. At the ∼20 mol. % composition we see a change in the silicate network, as shown by the absence of a Q4 peak and the proportion of 3-membered rings.