MADE in the USA Powering America’S Clean Energy Transition
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Direct Preparation of Some Organolithium Compounds from Lithium and RX Compounds Katashi Oita Iowa State College
Iowa State University Capstones, Theses and Retrospective Theses and Dissertations Dissertations 1955 Direct preparation of some organolithium compounds from lithium and RX compounds Katashi Oita Iowa State College Follow this and additional works at: https://lib.dr.iastate.edu/rtd Part of the Organic Chemistry Commons Recommended Citation Oita, Katashi, "Direct preparation of some organolithium compounds from lithium and RX compounds " (1955). Retrospective Theses and Dissertations. 14262. https://lib.dr.iastate.edu/rtd/14262 This Dissertation is brought to you for free and open access by the Iowa State University Capstones, Theses and Dissertations at Iowa State University Digital Repository. It has been accepted for inclusion in Retrospective Theses and Dissertations by an authorized administrator of Iowa State University Digital Repository. For more information, please contact [email protected]. INFORMATION TO USERS This manuscript has been reproduced from the microfilm master. UMI films the text directly from the original or copy submitted. Thus, some thesis and dissertation copies are in typewriter face, while others may be from any type of computer printer. The quality of this reproduction is dependent upon the quality of the copy submitted. Broken or indistinct print, colored or poor quality illustrations and photographs, print bleedthrough, substandard margins, and improper alignment can adversely affect reproduction. In the unlikely event that the author did not send UMI a complete manuscript and there are missing pages, these will be noted. Also, if unauthorized copyright material had to be removed, a note will indicate the deletion. Oversize materials (e.g., maps, drawings, charts) are reproduced by sectioning the original, beginning at the upper left-hand comer and continuing from left to right in equal sections with small overiaps. -
Manufacturing Scalability Implications of Materials Choice in Inorganic Solid-State Batteries Abstract Context & Scale Intro
1 Manufacturing Scalability Implications of Materials Choice in Inorganic 2 Solid-State Batteries 3 Kevin J. Huang1, Gerbrand Ceder2, Elsa A. Olivetti1* 4 5 1Department of Materials Science & Engineering, MIT, Cambridge, MA 02139; 2Department of Materials 6 Science & Engineering, University of California Berkeley, Berkeley, CA 94720, USA 7 Abstract 8 The pursuit of scalable and manufacturable all-solid-state batteries continues to intensify, motivated by the 9 rapidly increasing demand for safe, dense electrical energy storage. In this Perspective, we describe the 10 numerous, often conflicting, implications of materials choices that have been made in the search for 11 effective mitigations to the interfacial instabilities plaguing solid-state batteries. Specifically, we show that 12 the manufacturing scalability of solid-state batteries can be governed by at least three principal 13 consequences of materials selection: (1) the availability, scaling capacity, and price volatility of the chosen 14 materials’ constituents, (2) the manufacturing processes needed to integrate the chosen materials into full 15 cells, and (3) the cell performance that may be practically achieved with the chosen materials and processes. 16 While each of these factors is, in isolation, a pivotal determinant of manufacturing scalability, we show that 17 consideration and optimization of their collective effects and tradeoffs is necessary to more completely 18 chart a scalable pathway to manufacturing. 19 Context & Scale 20 With examples pulled from recent developments in solid-state batteries, we illustrate the consequences of 21 materials choice on materials availability, processing requirements and challenges, and resultant device 22 performance. We demonstrate that while each of these factors is, by itself, essential to understanding 23 manufacturing scalability, joint consideration of all three provides for a more comprehensive understanding 24 of the specific factors that could impede the scale up to production. -
Alteration of Spodumene, Montebrasite and Lithiophilite In
American Mineralogist, Volume 67, pages 97-113, 1982 Alteration of spodumene,montebrasite and lithiophilite in pegmatites of the White PicachoDistrict, Arizona Davrp Lor.rooxrnNo DoNer-uM. Bunr Department of Geology Arizona State University Tempe, Arizona 85281 Abstract The crystallization sequence and metasomatic alteration of spodumene (LiAlSizOe), montebrasite(LiAIPO4(OH,F)), and lithiophilite (Li(Mn,Fe)PO+)are describedfor nine zoned lithium pegmatitesin the White Picacho district, Arizona. The observedcrystalliza- tion trends suggesta progressiveincrease in the activities of lithium species(spodumene follows microcline as the principal alkali aluminosilicate), as well as an increase in the activities of the acidic volatiles phosphorus and fluorine (montebrasite succeedsspodu- mene as the stableprimary lithium phase).Much of the lithiophilite occurs with columbite, apatite, beryl, zircon, and tourmaline in cleavelanditecomplexes that formed in part at the expenseof quartz-spodumenepegmatite. Fracture-controlledpseudomorphic alteration of the primary lithium minerals is widespread and apparently is the result of subsolidus reactionswith residualpegmatitic fluids. Spodumenehas been replacedby eucryptite, albite, and micas. Alteration products of montebrasite include low-fluorine secondary montebrasite,crandallite (tentative), hydroxylapatite, muscovite, brazilianite, augelite (tentative),scorzalite, kulanite, wyllieite, and carbonate-apatite.Secondary phases identi- fied in altered lithiophilite include hureaulite, triploidite, eosphorite, -
Lithium in Lithium-Ion Batteries for Electric Vehicles
Office of Industries Working Paper ID-069 July 2020 Global Value Chains: Lithium in Lithium-ion Batteries for Electric Vehicles Gregory M. LaRocca Abstract Lithium is an essential material in the production of lithium-ion batteries (LIBs), which power electric vehicles. This paper examines the global value chain (GVC) for lithium as part of a series of working papers that map out the global sources of mining, refining, and value-added for the key LIB materials. Results show that few countries have economically viable resources of the upstream raw materials that supply the lithium GVC. Most lithium-rich ores are exported from Australia to China for processing, while most lithium brine concentrates are exported from Chile to South Korea, Japan, and China for processing. The large inflows of lithium to China support its dominant position in the downstream refining process, which is where the largest share of value-added occurs. Consequently, China is capturing the largest shares of value-added along the lithium GVC, despite lacking in resource endowment. Disclaimer: Office of Industries working papers are the result of the ongoing professional research of USITC staff and solely represent the opinions and professional research of individual authors. These papers do not necessarily represent the views of the U.S. International Trade Commission or any of its individual Commissioners. U.S. International Trade Commission Global Value Chains: Lithium in Lithium-ion Batteries for Electric Vehicles Gregory M. LaRocca Office of Industries U.S. International Trade Commission (USITC) July 2020 The author is staff with the Office of Industries of the U.S. -
Dilithium Sequestrene As Ananticoagulant
J Clin Pathol: first published as 10.1136/jcp.12.3.254 on 1 May 1959. Downloaded from J. clin. Path. (1959), 12, 254. DILITHIUM SEQUESTRENE AS AN ANTICOAGULANT BY L. S. SACKER,* K. E. SAUNDERS,t BERYL PAGE, AND MARGARET GOODFELLOW From the Departments of Pathology, Dulwich and Lewisham Hospitals, London (RECEIVED FOR PUBLICATION SEPTEMBER 20, 1958) The variety of different anticoagulants used for Ethylene diamine tetra-acetic acid (E.D.T.A.), 29.2 blood samples has increased, but there is still need g., and 7.4 g. of lithium carbonate were intimately for a suitable anticoagulant for the routine mixed. Then 200 ml. of water was added and solution estimation of sodium and potassium by flame took place with vigorous evolution of carbon dioxide. photometry. So far the only satisfactory substance for this purpose has been the expensive calcium Method 2 heparin (King and Wootton, 1956). Disodium sequestrene (Proescher, 1951 ; Hadley E.D.T.A., 29.2 g., was dissolved in 200 ml. of normal and Larson, 1953) and dipotassium sequestrene lithium hydroxide solution (41.96 g. LiOH.H20 per are the most valuable of litre). (Hadley and Weiss, 1955) In both cases the resulting solution contained the the recently introduced anticoagulants for routine dilithium salt. haematological procedures because they preserve Dilithium sequestrene was obtained from these morphology of leucocytes for short periods the solutions after filtration to remove a small quantity copyright. better than the ammonium and potassium oxalate of amorphous debris, by precipitation on the addition mixture or heparin, and they prevent platelets of an equal volume of absolute methyl alcohol and clumping and preserve them. -
Electrolyte Stability and Discharge Products of an Ionic-Liquid-Based Li-O2 Battery Revealed by Soft X-Ray Emission Spectroscopy
Lawrence Berkeley National Laboratory Recent Work Title Electrolyte Stability and Discharge Products of an Ionic-Liquid-Based Li-O2 Battery Revealed by Soft X-Ray Emission Spectroscopy Permalink https://escholarship.org/uc/item/6gd3f1x1 Journal Journal of Physical Chemistry C, 123(51) ISSN 1932-7447 Authors León, A Fiedler, A Blum, M et al. Publication Date 2019-12-26 DOI 10.1021/acs.jpcc.9b08777 Peer reviewed eScholarship.org Powered by the California Digital Library University of California Electrolyte Stability and Discharge Products of an Ionic- Liquid-based Li-O2 Battery Revealed by Soft X-Ray Emission Spectroscopy Aline Léon*1, Andy Fiedler2, Monika Blum3,4, Wanli Yang4, Marcus Bär5,6,7, Frieder Scheiba2, Helmut Ehrenberg2, Clemens Heske1,3,8, and Lothar Weinhardt1,3,8 1) Institute for Photon Science and Synchrotron Radiation (IPS), Karlsruhe Institute of Technology (KIT), Hermann-von-Helmholtz-Platz 1, 76344 Eggenstein-Leopoldshafen, Germany 2) Institute for Applied Materials (IAM), Karlsruhe Institute of Technology (KIT), Hermann-von-Helmholtz-Platz 1, 76344 Eggenstein-Leopoldshafen, Germany 3) Department of Chemistry and Biochemistry, University of Nevada, Las Vegas (UNLV), NV 89154-4003, USA 4) Advanced Light Source (ALS), Lawrence Berkeley National Laboratory, Berkeley, California 94720, United States 5) Department of Interface Design, Helmholtz-Zentrum Berlin für Materialien und Energie GmbH (HZB), Albert-Einstein-Str. 15, 12489 Berlin, Germany 6) Helmholtz-Institute Erlangen-Nürnberg for Renewable Energy (HI ERN), Albert-Einstein-Str. 15, 12489 Berlin, Germany 1 7) Department of Chemistry and Pharmacy, Friedrich-Alexander- Universität Erlangen-Nürnberg, Egerlandstr. 3, 91058 Erlangen, Erlangen, Germany 8) Institute for Chemical Technology and Polymer Chemistry (ITCP), Karlsruhe Institute of Technology (KIT), Engesserstr. -
Lithium 2017
2017 Minerals Yearbook LITHIUM [ADVANCE RELEASE] U.S. Department of the Interior September 2020 U.S. Geological Survey Lithium By Brian W. Jaskula Domestic survey data and tables were prepared by Annie Hwang, statistical assistant. In the United States, one lithium brine operation with an cobalt oxide and 2,160 kg of lithium-nickel-cobalt-aluminum associated lithium carbonate plant operated in Silver Peak, oxide (Defense Logistics Agency Strategic Materials, 2017). At NV. Domestic and imported lithium carbonate, lithium yearend 2017, the NDS held 540 kg of lithium-cobalt oxide and chloride, and lithium hydroxide were consumed directly 1,620 kg of lithium-nickel-cobalt-aluminum oxide. in industrial applications and used as raw materials for downstream lithium compounds. In 2017, lithium consumption Production in the United States was estimated to be equivalent to The U.S. Geological Survey (USGS) collected domestic 3,000 metric tons (t) of elemental lithium (table 1) [16,000 t production data for lithium from a voluntary canvass of the of lithium carbonate equivalent (LCE)], primarily owing to only U.S. lithium carbonate producer, Rockwood Lithium Inc. demand for lithium-based battery, ceramic and glass, grease, (a subsidiary of Albemarle Corp. of Charlotte, NC). Production pharmaceutical, and polymer products. In 2017, the gross weight and stock data collected from Rockwood Lithium were withheld of lithium compounds imported into the United States increased from publication to avoid disclosing company proprietary data. by 7% and the gross weight of exports increased by 29% from The company’s 6,000-metric-ton-per-year (t/yr) Silver Peak those in 2016. -
Common Name: LITHIUM ALUMINUM HYDRIDE HAZARD
Common Name: LITHIUM ALUMINUM HYDRIDE CAS Number: 16853-85-3 RTK Substance number: 1121 DOT Number: UN 1410 Date: April 1986 Revision: November 1999 ----------------------------------------------------------------------- ----------------------------------------------------------------------- HAZARD SUMMARY * Lithium Aluminum Hydride can affect you when * Exposure to hazardous substances should be routinely breathed in. evaluated. This may include collecting personal and area * Contact can cause severe skin and eye irritation and burns. air samples. You can obtain copies of sampling results * Breathing Lithium Aluminum Hydride can irritate the from your employer. You have a legal right to this nose and throat. information under OSHA 1910.1020. * Breathing Lithium Aluminum Hydride can irritate the * If you think you are experiencing any work-related health lungs causing coughing and/or shortness of breath. Higher problems, see a doctor trained to recognize occupational exposures can cause a build-up of fluid in the lungs diseases. Take this Fact Sheet with you. (pulmonary edema), a medical emergency, with severe shortness of breath. WORKPLACE EXPOSURE LIMITS * Exposure can cause loss of appetite, nausea, vomiting, The following exposure limits are for Aluminum pyro powders diarrhea and abdominal pain. (measured as Aluminum): * Lithium Aluminum Hydride can cause headache, muscle weakness, loss of coordination, confusion, seizures and NIOSH: The recommended airborne exposure limit is coma. 5 mg/m3 averaged over a 10-hour workshift. * High exposure can affect the thyroid gland function resulting in an enlarged thyroid (goiter). ACGIH: The recommended airborne exposure limit is * Lithium Aluminum Hydride may damage the kidneys. 5 mg/m3 averaged over an 8-hour workshift. * Lithium Aluminum Hydride is a REACTIVE CHEMICAL and an EXPLOSION HAZARD. -
Lithium Aluminum Hydride
Lithium aluminum hydride sc-215254 Material Safety Data Sheet Hazard Alert Code EXTREME HIGH MODERATE LOW Key: Section 1 - CHEMICAL PRODUCT AND COMPANY IDENTIFICATION PRODUCT NAME Lithium aluminum hydride STATEMENT OF HAZARDOUS NATURE CONSIDERED A HAZARDOUS SUBSTANCE ACCORDING TO OSHA 29 CFR 1910.1200. NFPA FLAMMABILITY4 HEALTH3 HAZARD INSTABILITY2 W SUPPLIER Santa Cruz Biotechnology, Inc. 2145 Delaware Avenue Santa Cruz, California 95060 800.457.3801 or 831.457.3800 EMERGENCY ChemWatch Within the US & Canada: 877-715-9305 Outside the US & Canada: +800 2436 2255 (1-800-CHEMCALL) or call +613 9573 3112 SYNONYMS Li-Al-H4, Al-H4-Li, "lithium aluminum hydride", "lithium aluminum tetrahydride", "lithium aluminium tetrahydride", "lithium tetrahydroaluminate", "aluminate, tetrahydro-, lithium", "lithium aluminohydride", "aluminum lithium hydride", "lithium alanate", LAH Section 2 - HAZARDS IDENTIFICATION CHEMWATCH HAZARD RATINGS Min Max Flammability 4 Toxicity 2 Body Contact 4 Min/Nil=0 Low=1 Reactivity 2 Moderate=2 High=3 Chronic 2 Extreme=4 CANADIAN WHMIS SYMBOLS 1 of 10 CANADIAN WHMIS CLASSIFICATION CAS 16853-85-3Lithium tetrahydroaluminate E-Corrosive Material EMERGENCY OVERVIEW RISK Causes severe burns. Risk of serious damage to eyes. Reacts violently with water liberating extremely flammable gases. Extremely flammable. POTENTIAL HEALTH EFFECTS ACUTE HEALTH EFFECTS SWALLOWED ■ The material can produce severe chemical burns within the oral cavity and gastrointestinal tract following ingestion. ■ Ingestion of alkaline corrosives may produce burns around the mouth, ulcerations and swellings of the mucous membranes, profuse saliva production, with an inability to speak or swallow. Both the oesophagus and stomach may experience burning pain; vomiting and diarrhoea may follow. ■ Accidental ingestion of the material may be damaging to the health of the individual. -
Chemical List
1 EXHIBIT 1 2 CHEMICAL CLASSIFICATION LIST 3 4 1. Pyrophoric Chemicals 5 1.1. Aluminum alkyls: R3Al, R2AlCl, RAlCl2 6 Examples: Et3Al, Et2AlCl, EtAlCl2, Me3Al, Diethylethoxyaluminium 7 1.2. Grignard Reagents: RMgX (R=alkyl, aryl, vinyl X=halogen) 8 1.3. Lithium Reagents: RLi (R = alkyls, aryls, vinyls) 9 Examples: Butyllithium, Isobutyllithium, sec-Butyllithium, tert-Butyllithium, 10 Ethyllithium, Isopropyllithium, Methyllithium, (Trimethylsilyl)methyllithium, 11 Phenyllithium, 2-Thienyllithium, Vinyllithium, Lithium acetylide ethylenediamine 12 complex, Lithium (trimethylsilyl)acetylide, Lithium phenylacetylide 13 1.4. Zinc Alkyl Reagents: RZnX, R2Zn 14 Examples: Et2Zn 15 1.5. Metal carbonyls: Lithium carbonyl, Nickel tetracarbonyl, Dicobalt octacarbonyl 16 1.6. Metal powders (finely divided): Bismuth, Calcium, Cobalt, Hafnium, Iron, 17 Magnesium, Titanium, Uranium, Zinc, Zirconium 18 1.7. Low Valent Metals: Titanium dichloride 19 1.8. Metal hydrides: Potassium Hydride, Sodium hydride, Lithium Aluminum Hydride, 20 Diethylaluminium hydride, Diisobutylaluminum hydride 21 1.9. Nonmetal hydrides: Arsine, Boranes, Diethylarsine, diethylphosphine, Germane, 22 Phosphine, phenylphosphine, Silane, Methanetellurol (CH3TeH) 23 1.10. Non-metal alkyls: R3B, R3P, R3As; Tributylphosphine, Dichloro(methyl)silane 24 1.11. Used hydrogenation catalysts: Raney nickel, Palladium, Platinum 25 1.12. Activated Copper fuel cell catalysts, e.g. Cu/ZnO/Al2O3 26 1.13. Finely Divided Sulfides: Iron Sulfides (FeS, FeS2, Fe3S4), and Potassium Sulfide 27 (K2S) 28 REFERRAL -
Global Lithium Sources—Industrial Use and Future in the Electric Vehicle Industry: a Review
resources Review Global Lithium Sources—Industrial Use and Future in the Electric Vehicle Industry: A Review Laurence Kavanagh * , Jerome Keohane, Guiomar Garcia Cabellos, Andrew Lloyd and John Cleary EnviroCORE, Department of Science and Health, Institute of Technology Carlow, Kilkenny, Road, Co., R93-V960 Carlow, Ireland; [email protected] (J.K.); [email protected] (G.G.C.); [email protected] (A.L.); [email protected] (J.C.) * Correspondence: [email protected] Received: 28 July 2018; Accepted: 11 September 2018; Published: 17 September 2018 Abstract: Lithium is a key component in green energy storage technologies and is rapidly becoming a metal of crucial importance to the European Union. The different industrial uses of lithium are discussed in this review along with a compilation of the locations of the main geological sources of lithium. An emphasis is placed on lithium’s use in lithium ion batteries and their use in the electric vehicle industry. The electric vehicle market is driving new demand for lithium resources. The expected scale-up in this sector will put pressure on current lithium supplies. The European Union has a burgeoning demand for lithium and is the second largest consumer of lithium resources. Currently, only 1–2% of worldwide lithium is produced in the European Union (Portugal). There are several lithium mineralisations scattered across Europe, the majority of which are currently undergoing mining feasibility studies. The increasing cost of lithium is driving a new global mining boom and should see many of Europe’s mineralisation’s becoming economic. The information given in this paper is a source of contextual information that can be used to support the European Union’s drive towards a low carbon economy and to develop the field of research. -
Synthesis of Lithium Peroxide from Hydrogen Peroxide and Lithium Hydroxide in Aqueous-Organic Medium: Wasteless Technology
MATEC Web of Conferences 96, 00004 (2017) DOI: 10.1051/ matecconf/20179600004 REE-2016 Synthesis of Lithium Peroxide from Hydrogen Peroxide and Lithium Hydroxide in Aqueous-Organic Medium: Wasteless Technology Roman Nefedov* and Yury Ferapontov Tambov State Technical University, Tambov, Russia Abstract. Lithium is a rare element, and widely used in manufacturing, electronics, medicine, and etc. One of the important lithium compounds is lithium peroxide. It is a component of regenerating products to protect the human respiratory system from damaging factors of chemical and biological nature. This paper describes the methods of obtaining the lithium peroxide. All industrial techniques for the synthesis of lithium peroxide are presented. A critical assessment of these techniques is given. A new wasteless synthesis technology of lithium peroxide from Hydrogen Peroxide and Lithium Hydroxide in Aqueous-Organic Medium is presented. This technology allows obtaining the pure product containing Li2O2 up to 94 %. The possibility of the solvent regeneration by the anhydrous lithium hydroxide has been shown. The yield of the lithium – 98 % and a significant reduction in solvent consumption per unit of finished product has been obtained. 1 Introduction The use of ethanol is not a prerequisite for obtaining lithium peroxide, although it is beneficial in terms of that The inorganic peroxide compounds based on rare, lithium peroxide contained in it unlike other organic radioactive, and especially alkali metals have a wide substances practically insoluble (dissolved in methanol range of industrial applications (e.g., energy storage and about 3.5 g/L Li2O2. Ethanol can be replaced by other oxygen source, etc.) [1, 2]. organic solvents (methanol, pyridine, propanol, kenotic An identifying characteristic of inorganic peroxide and others [12, 14]).