Relevant bibliographies by topics / Lithium alkyls

Academic literature on the topic 'Lithium alkyls'

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Published: 9 March 2023

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Journal articles on the topic "Lithium alkyls"

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Charrier, Claude, Nicole Maigrot, Francois Mathey, Francis Robert, and Yves Jeannin. "Reactions of 1,2-diphosphetenes with lithium and lithium alkyls." Organometallics 5, no. 4 (April 1986): 623–30. http://dx.doi.org/10.1021/om00135a002.

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Jutzi, Peter, and Bernd Hielscher. "Reaction of decamethylstannocene with lithium alkyls." Organometallics 5, no. 12 (December 1986): 2511–14. http://dx.doi.org/10.1021/om00143a018.

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Martínez-Martínez, Antonio J., Alan R. Kennedy, Valerie Paprocki, Felipe Fantuzzi, Rian D. Dewhurst, Charles T. O’Hara, Holger Braunschweig, and Robert E. Mulvey. "Selective mono- and dimetallation of a group 3 sandwich complex." Chemical Communications 55, no. 65 (2019): 9677–80. http://dx.doi.org/10.1039/c9cc03825f.

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While lithium alkyls and lithium amides do not metallate the scandium compound [(η5-C5H5)Sc(η8-C8H8)], a synergistic lithium–aluminium base-trap partnership cannot resist taking a bite with one C–H bond selectively cleaved from both Cp and COT rings.
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Ballard, D. G. H., R. J. Bowles, D. M. Haddleton, S. N. Richards, R. Sellens, and D. L. Twose. "Controlled polymerization of methyl methacrylate using lithium aluminum alkyls." Macromolecules 25, no. 22 (October 1992): 5907–13. http://dx.doi.org/10.1021/ma00048a008.

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Sirsch, P., W. Scherer, M. Gardiner, S. A. Mason, and G. S. McGrady. "Electron delocalization in lithium alkyls: negative hyperconjugation and agostic bonding." Acta Crystallographica Section A Foundations of Crystallography 58, s1 (August 6, 2002): c352. http://dx.doi.org/10.1107/s0108767302099063.

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Schumann, Herbert, and Gerald Jeske. "Metallorganische Verbindungen der Lanthanoide, XXXIII [1] Dicyclopentadienyllanthanoid-alkyle und -hydride von Neodym, Samarium und Lutetium [2] / Organometallic Compounds of the Lanthanides, XXXIII [1] Dicyclopentadienyllanthanide Alkyls and Hydrides of Neodymium, Samarium and Lutetium [2]." Zeitschrift für Naturforschung B 40, no. 11 (November 1, 1985): 1490–94. http://dx.doi.org/10.1515/znb-1985-1112.

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Tricyclopentadienylneodymium and -lutetium react with sec-butyl lithium and terf-butyl lithium to form sec-butyl- and tert-butyl(dicyclopentadienyl)neodymium and -lutetium, which decompose to the corresponding dicyclopentadienyllanthanide hydride complexes. Dicyclopentadienyl-bis-(trimethylsilyl)methylsamarium and -lutetium are made from dicyclopentadienylsamarium or -lutetium chloride and bis(trimethylsilyl)methyl lithium. They react with hydrogen to form the corresponding dicyclopentadienyllanthanide hydride complexes.
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Seyam, Afif M. "Observations on the reaction of uranium tetrachloride and dichlorodioxouranium(VI) with lithium alkyls." Inorganica Chimica Acta 110, no. 2 (September 1985): 123–26. http://dx.doi.org/10.1016/s0020-1693(00)84567-3.

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Galliani, Guido, Bruno Rindone, Ricardo Suarez-Bertoa, Francesco Saliu, and Alberto Terraneo. "Stereoselective Addition of Grignard Reagents and Lithium Alkyls onto 3,5-Disubstituted-1,3-oxazolidine-2,4-diones." Synthetic Communications 43, no. 5 (November 13, 2012): 749–57. http://dx.doi.org/10.1080/00397911.2011.609301.

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Kershenbaum, I. L., I. A. Oreshkin, and B. A. Dolgoplosk. "Formation of carbene species in the reaction of lithium alkyls with molybdenum, tungsten, and cobalt chlorides." Bulletin of the Russian Academy of Sciences Division of Chemical Science 41, no. 1 (January 1992): 172–74. http://dx.doi.org/10.1007/bf00863939.

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Galliani, Guido, Bruno Rindone, Ricardo Suarez-Bertoa, Francesco Saliu, and Alberto Terraneo. "ChemInform Abstract: Stereoselective Addition of Grignard Reagents and Lithium Alkyls onto 3,5-Disubstituted-1,3-oxazolidine-2,4-diones." ChemInform 44, no. 24 (May 23, 2013): no. http://dx.doi.org/10.1002/chin.201324114.

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Dissertations / Theses on the topic "Lithium alkyls"

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Park, Bongjin. "Single electron transfer in reactions involving alkyl halides with lithium alkylamide, lithium alkyl and lithium metal." Diss., Georgia Institute of Technology, 1988. http://hdl.handle.net/1853/27052.

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Antolini, Floria. "Complexes of novel chiral alkyl and C←1-symmetric amido ligands." Thesis, University of Sussex, 2001. http://ethos.bl.uk/OrderDetails.do?uin=uk.bl.ethos.367353.

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Welder, Catherine Owens. "A mechanistic evaluation of the reactions of lithium aluminum hydride with alkyl halides." Diss., Georgia Institute of Technology, 1996. http://hdl.handle.net/1853/25958.

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Thornton, Terry L. (Terry Lee) 1962. "Mixed Alkyllithim/Lithium Alkoxide Aggregates with Less Sterically Crowded Alkyl Groups." Thesis, University of North Texas, 1997. https://digital.library.unt.edu/ark:/67531/metadc278441/.

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Mixed alkyllithium / lithium alkoxide aggregates in the form (RLi)n(ROLi)m were formed by addition of corresponding alcohol compounds at different Li/O ratios. Variable temperature 13C and 6Li NMR spectroscopy were used to verify the formation of the mixed aggregates and to study their behavior in hydrocarbon solution. Spectra for the lithium n-propoxide / n-propyllithium and iso-butyllithium / lithium iso-butoxide systems each indicated at least one mixed aggregate.
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Ullrich, Steven A. "Synthesis and Characterization of some Flourine-containing Lithium Alkyl Sulfonates: Flourinated Sulfonates and SF5-containing Sulfonates." PDXScholar, 1994. https://pdxscholar.library.pdx.edu/open_access_etds/4880.

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Lithium salts of pentafluorothio alkyl sulfonic acids and perfluoroalkyl disulfonic acids were prepared for testing for possible use as polymer electrolytes. Most of these lithium salts were made from the corresponding sodium, potassium or calcium salts. Aqueous solutions of these salts were passed through polystyrene sulfonate ion exchange resin in the acid form to obtain aqueous solutions of the corresponding acids. The acids were then neutralized with lithium hydroxide using a pH meter. One salt was made by reacting the barium salt of the corresponding acid with lithium sulfate. A sulfonyl fluoride polymer (-0-CH2-C (CH20CF2CF2S02F) H-) n was reacted with lithium hydroxide to give a lithium salt as well. Owing to the great length of time required to dry these hydroscopic salts so that they might be suitable for polymer electrolyte work, alternative, water-free methods of preparation were explored. These include the reaction of lithium trimethylsilanolate with a sulfonyl fluoride, and the reaction of trimethylsilyl triflate with lithium chloride. Conductivity studies were performed on samples of these salts, and the results so far obtained from these studies are presented. Mass spectrometry, 1H, 19F and 13C nuclear magnetic resonance spectroscopy, infrared spectroscopy, and elemental analysis were used to help characterize the new lithium salts.
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SUAREZ, BERTOA RICARDO. "Sustainable procedures in organic synthesis." Doctoral thesis, Università degli Studi di Milano-Bicocca, 2009. http://hdl.handle.net/10281/7474.

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O-acyl-N-benzyllactamides are obtained in good yield by reaction of 4-benzyl-5-methyl-1,3-oxazolidine-2,4-diones with Grignards reagents and with lithium alkyls. Three alkanes and two ethers were oxidised with ozone in dichloromethane solution or in aqueous pH 3 suspension. Cyclodecane and cyclododecane were converted into the corresponding cycloalkanones. n-decane was converted into a mixture of isomeric n-decanones and carboxylic acids. An ester was formed from the ethers. Hence, one of the methylene groups of these substrates is generally converted into a carbonyl group. Some of these reactions have preparative value. The oxidation of naphthalene in dichloromethane or acetonitrile with excess ozone gives phthalic aldehyde, 2-formyl benzoic acid and phthalic anhydride. Small amounts of the (E)- and (Z)-isomer of 3-phenyl-(2-formyl)-propenal and are also observed in some cases. The reaction is faster in acetonitrile than in dichloromethane owing to the higher solubility of ozone in the former solvent. The reaction is faster on lowering the temperature because of the increase of the concentration of ozone in solution at lower temperature. With a 1:1 or a 1:2 naphthalene:ozone ratio high conversion and low selectivity for the anhydride is observed. The ozonation of cyclohexane in dichloromethane or acetonitrile gives cycloxexanone, cyclohexanol and acidic material. The influence of solvent, reactant concentration, amount of ozone, temperature, reaction time is studied. A reaction mechanism is proposed based on the results of a simulation of the reaction energetics. The ozonation of N-phenylmorpholine in dichloromethane or acetonitrile produced a lactame and a diformylderivative. These products derive from the attack of ozone at the heterocyclic ring. The reaction mechanism has been investigated by DFT calculations which show that the reaction occurs through the insertion of ozone at the carbon-hydrogen bond of a methylenic group of the morpholine ring. The regioselectivity is due to the to the significantly lower energy barrier calculated for the attack of ozone in α to nitrogen than in α to oxygen. Also, the energy barrier decreases with increasing the polarity of the solvent, accounting for the higher reaction rate observed for the reaction carried out in acetonitrile than in dichloromethane. The ozonation of trans- and cis-decalin in dichloromethane or acetonitrile gives the corresponding 9-hydroxydecalinns, 2- and 3-decalones and acidic material. The influence of solvent, reactant concentration, amount of ozone, temperature, reaction time is studied. A reaction mechanism is proposed based on the results of a simulation of the reaction energetics. The N,N bis(salicylidene)ethylenediaminocobalt(II) catalysed oxidative carbonylation of para-substituted aromatic primary amines at 100 °C in methanol gives carbamates in high yields. In presence of excess dimethylamine also N-aryl-N’,N’-dimethylureas are formed. In methylene chloride moderate yields in isocyanate are obtained. 1-methylbenzylamine gives the carbamate and the urea in high yield. i-propylamine gives only the urea. An α-aminoalcohol gives a 1,3-oxazolidin-2-one. Aliphatic secondary amines react faster and give carbamates in methanol and ureas in methylene chloride. The turnover frequency is also measured in two cases.
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Millard, Marcus J. "Effects of Lithium Nitrate Admixture on Early Age Concrete Behavior." Thesis, Georgia Institute of Technology, 2006. http://hdl.handle.net/1853/11615.

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Alkali silica reaction (ASR), a reaction which occurs between reactive siliceous mineral components in the aggregate and the alkaline pore solution in concrete, is responsible for substantial damage to concrete structures in the U. S. and across the world. Lithium admixtures, including lithium nitrate (LiNO3), have been demonstrated to mitigate ASR damage, and are of particular interest for use in concrete airfield pavement construction, where ASR damage has been recently linked to the use of certain de-icing chemicals. Although the effectiveness of lithium admixtures at ASR-mitigation is well-researched, relatively less is known regarding the potential effects, including negative effects, on overall concrete behavior. The goal of this research is to better understand the influence of LiNO3 admixture on early age concrete behavior, and to determine if a maximum dosage rate for its use exists. Isothermal calorimetry, rheology and bleed water testing, time of setting, chemical shrinkage, autogenous shrinkage, free and restrained concrete shrinkage, and compressive and flexural strength were measured for pastes and concretes prepared with a range of LiNO3 dosages (i.e., 0, 50, 100, 200, and 400% of the recommended dosage). In addition, the interaction of LiNO3 with cement was evaluated by comparing results obtained with six cements of varying alkali and tricalcium aluminate (C3A) contents. Additionally, one of these cements, was examined alone and with 20% by weight Class F fly ash replacement. Results indicate that the hydration of the tricalcium silicate and tricalcium aluminate components of cement are accelerated by the use of LiNO3, and that low alkali cements (typically specified to avoid damage by ASR) may be particularly susceptible to this acceleration. However, inclusion of Class F fly ash at 20% by weight replacement of cement (also common in applications where ASR is a concern) appears to diminish these possibly negative effects of LiNO3 on early age hydration acceleration and heat generation. Dosages higher than the current standard dosage of LiNO3 may have minor effects on fresh concrete workability, causing slight decreases in Bingham yield stress, corresponding to slightly higher slump. Fresh concrete viscosity may also be affected, though more research is necessary to confirm this effect. LiNO3 had no effect on quantity of bleed water in the mixes tested. Generally, LiNO3 had no effect on initial and final setting times, although increasing dosages caused faster set times in the lowest alkali (Na2Oeq = 0.295%) cement examined. In shrinkage testing, higher LiNO3 dosages appeared to cause initial expansion in some sealed paste specimens, but in all cases the highest dosage led to greater autogenous shrinkage after 40 days. In concrete specimens, however, the restraining effect of aggregates diminished shrinkage, and no effect of the LiNO3 was apparent. In no cases, with any dosage of lithium tested, with or without fly ash replacement, did restrained shrinkage specimens show any cracking. Strength testing produced mixed results, with laboratory specimens increasing in 28-day compressive strength, but companion specimens cast in the field and tested by an outside laboratory, exhibited lower 28-day compressive strength, with increasing lithium dosages. Flexural specimens, also cast in the field and tested by an outside laboratory, appeared to show an increase in 28-day flexural strength with increasing lithium dosages. However, because of the conflicting results when comparing the various strength data, further research is necessary for conclusive evidence of LiNO3 effects on concrete strength.
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Collins, Courtney Lloyd. "Examination of the mechanism by which lithium additives inhibit alkali-silica reaction gel expansion." Thesis, Georgia Institute of Technology, 2002. http://hdl.handle.net/1853/21295.

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Robertson, Alan. "Elaboration and expansion of the chemistry of alkali metal primary amide complexes." Thesis, University of Strathclyde, 2000. http://ethos.bl.uk/OrderDetails.do?uin=uk.bl.ethos.248701.

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Murphy, Denissa Tjiadarma. "Structural Investigation of Electrodes for Rechargeable Alkali Ion Batteries." Thesis, The University of Sydney, 2017. http://hdl.handle.net/2123/17699.

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This thesis describes the in-depth characterisation of the structure, including detailed cation distributions, of positive electrode materials for lithium and sodium ion batteries. As the crystal chemistry influences the mobility of lithium and sodium ions, the structure and electrochemical property relationships for select compounds have been established. The majority of this thesis is focused on the structural characterisation of LiMn2-xTixO4 (0.2 ≤ x ≤ 1.5). A combination of X-ray and neutron powder diffraction studies along with spectroscopic techniques and physical property measurements were employed to elucidate the complex metal ion ordering of the spinel electrodes. It was found that the synthesis conditions, particularly cooling regimes, play an important part in the final structures of LiMn1.8Ti0.2O4 and LiMnTiO4. The bulk substitution of 10% and 50% manganese with titanium heavily influenced the cation distribution and consequently, the electrochemistry of these compounds. In situ diffraction studies revealed the contrasting structural evolutions of LiMn1.8Ti0.2O4 and LiMnTiO4 during charge and discharge cycles. The potential of sodium silicate materials as positive electrodes for sodium ion batteries was explored. The fundamental crystal chemistry of Na2MnSiO4 and Na2CoSiO4 was established prior to electrochemical cycling. The as prepared Na2CoSiO4 exhibited better conductivity than the manganese analogue. Improvement of the conductivity of Na2MnSiO4 was achieved through carbon coating of the material. Finally, the addition of Li2RuO3 to form the lithium rich 0.5Li2RuO3∙0.5LiMO2 (M = Co and Ni) electrodes has resulted in the increased the stability of the layered structures of the compounds. The electrochemically active Li2RuO3 contributed to the excellent specific capacity and rate capability of the cobalt compound. Overall superior electrochemical performance was achieved by the nickel analogue.
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Books on the topic "Lithium alkyls"

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The alkali metals: Lithium, sodium, potassium, rubidium, cesium, francium. New York: Rosen Central, 2010.

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Folliard, Kevin J. Guidelines for the use of lithium to mitigate or prevent alkali-silica reaction (ASR). McLean, VA: U.S. Department of Transportation, Federal Highway Administration, Office of Infrastructure R&D, Turner-Fairbank Highway Research Center, 2003.

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A, Thomas Michael D., Kurtis Kimberly E, Transtec Group Inc, United States. Federal Highway Administration. Office of Infrastructure Research and Development., and Turner-Fairbank Highway Research Center, eds. Guidelines for the use of lithium to mitigate or prevent alkali-silica reaction (ASR). McLean, VA: U.S. Dept. of Transportation, Federal Highway Administration, Research, Development, and Technology, Turner-Fairbank Highway Research Center, 2003.

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Lew, Kristi. Alkali Metals Lithium, Sodium, Potassium, Rubidium, Cesium, Francium. Rosen Publishing Group, 2009.

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Book chapters on the topic "Lithium alkyls"

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Mota de Freitas, Duarte, Brian D. Leverson, and Jesse L. Goossens. "Lithium in Medicine: Mechanisms of Action." In The Alkali Metal Ions: Their Role for Life, 557–84. Cham: Springer International Publishing, 2016. http://dx.doi.org/10.1007/978-3-319-21756-7_15.

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Li, Wei-bang, Ngoc Thanh Thuy Tran, and Shih-Yang Lin. "Diverse Phenomena in Stage-n Graphite Alkali-Intercalation Compounds." In Lithium-Ion Batteries and Solar Cells, 19–43. First edition. | Boca Raton, FL : CRC Press/ Taylor & Francis Group, LLC, 2021.: CRC Press, 2020. http://dx.doi.org/10.1201/9781003138327-2.

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Rösch, L. "From Germyl-Alkali Metal Reagent with Lithium Aluminum Hydride." In Inorganic Reactions and Methods, 226. Hoboken, NJ, USA: John Wiley & Sons, Inc., 2007. http://dx.doi.org/10.1002/9780470145241.ch127.

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Bartoli, Giuseppe, Marcella Bosco, Renato Dalpozzo, and Loris Grossi. "Polar Versus Electron Transfer Pathway in the Reaction of Alkyl Lithium and Alkyl Grignard Reagents with Mononttroarenes: Factors Affecting Product Distribution." In Paramagnetic Organometallic Species in Activation/Selectivity, Catalysis, 489–502. Dordrecht: Springer Netherlands, 1989. http://dx.doi.org/10.1007/978-94-009-0877-2_34.

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Nojima, M., and S. Kusabayashi. "Reaction of Alkyl Halides with Lithium and Magnesium Reagents. Nucleophilic Substitution vs. Single Electron Transfer." In Paramagnetic Organometallic Species in Activation/Selectivity, Catalysis, 503–17. Dordrecht: Springer Netherlands, 1989. http://dx.doi.org/10.1007/978-94-009-0877-2_35.

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Eysseltová, J., and M. Salomon. "Lithium Phosphate." In Alkali Metal Orthophosphates, 1–10. Elsevier, 1988. http://dx.doi.org/10.1016/b978-0-08-035937-3.50007-x.

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Scerri, Eric. "More Chemistry." In The Periodic Table. Oxford University Press, 2019. http://dx.doi.org/10.1093/oso/9780190914363.003.0019.

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The trends within rows and columns of the periodic table are quite well known and are not repeated here. Instead, I concentrate on a number of other chemical trends, some of which challenge the form of reductionism that attempts to provide explanations based on electronic configurations alone. In the case of one particular trend described here, the knight’s move, the chemical behavior defies any theoretical understanding whatsoever, at least at the present time. As is well known to students of inorganic chemistry, a small number of elements display what is termed diagonal behavior where, in apparent violation of group trends, two elements from adjacent groups show greater similarity than is observed between these elements and the members of their own respective groups. Of these three classic examples of diagonal behavior, let us concentrate on the first one to the left in the periodic table, that between lithium and magnesium. The similarities between these two elements are as follows:1. Whereas the alkali metals form peroxides and superoxides, lithium behaves like a typical alkaline earth in forming only a normal oxide with formula Li2O. 2.Unlike the other alkali metals, lithium forms a nitride, Li3N, as do the alkaline earths. 3.Although the salts of most alkali metals are soluble, the carbonate, sulfate, and fluorides of lithium are insoluble, as in the case of the alkaline earth elements. 4.Lithium and magnesium both form organometallic compounds that act as useful reagents in organic chemistry. Lithium typically forms such compounds as Li(CH3)3, while magnesium forms such compounds as CH3MgBr, a typical Grignard reagent that is used in nucleophilic addition reactions. Organolithium and organomagnesium compounds are very strong bases that react with water to form alkanes. 5.Lithium salts display considerable covalent character, unlike their alkali metal homologues but in common with many alkaline earth salts. 6.Whereas the carbonates of the alkali metals do not decompose on heating, that of lithium behaves like the carbonates of the alkaline earths in forming the oxide and carbon dioxide gas. 7.Lithium is a considerably harder metal than other alkali metals and similar in hardness to the alkaline earths.
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Nagai, Hiroki, and Mitsunobu Sato. "Highly Functionalized Lithium-Ion Battery." In Alkali-ion Batteries. InTech, 2016. http://dx.doi.org/10.5772/63491.

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Miyamoto, H., and M. Salomon. "Lithium Chlorate." In Alkali Metal Halates, Ammonium Iodate & Iodic Acid, 1–23. Elsevier, 1987. http://dx.doi.org/10.1016/b978-0-08-029210-6.50009-1.

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Miyamoto, H., and M. Salomon. "Lithium Bromate." In Alkali Metal Halates, Ammonium Iodate & Iodic Acid, 184–94. Elsevier, 1987. http://dx.doi.org/10.1016/b978-0-08-029210-6.50014-5.

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Conference papers on the topic "Lithium alkyls"

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Loubriel, G. M., T. A. Green, N. H. Tolk, and R. F. Haglund. "The Role of F-Centers in Electron- and Photon-Stimulated Desorption from Alkali Halides." In Microphysics of Surfaces, Beams, and Adsorbates. Washington, D.C.: Optica Publishing Group, 1987. http://dx.doi.org/10.1364/msba.1987.wc9.

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Bienert, Walter B., Peter C. Cologer, Karen J. Fenzi, David A. Wolf, Mohamed S. El-Genk, and Mark D. Hoover. "Containment of Lithium Hydride in Alkali Metal Heat Pipes." In SPACE NUCLEAR POWER AND PROPULSION: Eleventh Symposium. AIP, 1994. http://dx.doi.org/10.1063/1.2950295.

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Saldin, Vitaly, and Vasily Sukhovey. "Study of alkali tetrahydroborate—lithium tetrafluoroborate mixtures at heating." In International Conference on Environment and Sustainability. Southampton, UK: WIT Press, 2014. http://dx.doi.org/10.2495/ices140091.

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Albers, Dylan, and Mileva Radonjic. "Prevention of Alkali-Silica Reaction (ASR) in Light-Weight Wellbore Cement Comprising Silicate-Based Microspheres." In ASME 2017 36th International Conference on Ocean, Offshore and Arctic Engineering. American Society of Mechanical Engineers, 2017. http://dx.doi.org/10.1115/omae2017-62015.

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Drilling through low pressure formations, either offshore or through depleted formations, requires the use of low density fluids to prevent lost circulation and as well as to properly place cement during cementing applications. Achieving these densities in cements can be done through foaming the cement, increasing water content, or through the addition of silica based microspheres. Each of these methods have individual limitations, and in the case of silica based microspheres, their specific fallback is a chemical instability with the microsphere itself reacting with the cement pore fluid. This chemical instability creates a hydrophilic gel that is expansive and creates fractures in the cement as it expands, which is more formally referred to as alkali-silica reactivity (ASR). Prevention of ASR involves the application of additives to the cement that acts as a sink for the alkalinity in which prevents the expansion of ASR. A specific application that this paper investigates for this prevention is the use of Lithium nitrate. This study looks at the effects of a high alkalinity environment onto the microspheres by visualizing the reactions that are occurring using Scanning Electron Microscopy (SEM), and confirming the presence of ASR when silica based microspheres encounter a high pH environment. Then cement samples were created to compare the effects lithium nitrate has on cements created with silica based microspheres. SEM and micro indentation was conducted on these samples, which showed that lithium nitrate prevents reactions, but after 28-day hydration a loss of mechanical properties is present.
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"Lithium alkali halides - New thermal neutron detectors with n-γ discrimination." In 2013 IEEE Nuclear Science Symposium and Medical Imaging Conference (2013 NSS/MIC). IEEE, 2013. http://dx.doi.org/10.1109/nssmic.2013.6829581.

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D’Hooghe, Matthias, and Norbert De Kimpe. "Reactivity of 1-arenesulfonyl- and 1-alkyl-2-(bromomethyl)aziridines towards Lithium Cuprate Reagents." In The 9th International Electronic Conference on Synthetic Organic Chemistry. Basel, Switzerland: MDPI, 2005. http://dx.doi.org/10.3390/ecsoc-9-01474.

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Mohd, Isneini, Sagawa Yasutaka, Hamada Hidenori, and Daisuke Yamamoto. "An experimental study on mitigating alkali silica reaction by using lithium hydroxide monohydrate." In PROCEEDINGS OF THE 3RD INTERNATIONAL CONFERENCE ON CONSTRUCTION AND BUILDING ENGINEERING (ICONBUILD) 2017: Smart Construction Towards Global Challenges. Author(s), 2017. http://dx.doi.org/10.1063/1.5011512.

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"Practical Implications of Lithium-Based Chemicals and Admixtures in Controlling Alkali-Aggregate Reactions." In SP-148: Fourth CANMET/ACI International Conference on Superplasticizers and chemical admixtures in Concrete. American Concrete Institute, 1994. http://dx.doi.org/10.14359/4111.

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Mo, Tiande, Chi Kin POON, Yu Li, Yang LUO, Kin Tak Lau, and Pui Yan Hung. "System Design and Control Strategy of Fuel Cell/Lithium-ion Battery Hybrid Electric Vehicles." In FISITA World Congress 2021. FISITA, 2021. http://dx.doi.org/10.46720/f2020-adm-019.

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Economic and/or practical points to be addressed As kind of critical materials handling vehicle, forklift has been widely used in various places, such as warehouses, logistics centers, airport, and distribution centers etc. However, the conventional forklifts are majorly powered by fossil fuel or lead-acid batteries that still causing serious environmental problems. Hydrogen fuel cell powered forklifts will provide notable advantages, because of hydrogen is a zero-emission fuel, it only produce electricity and water through chemical reaction that will improve the safety of the working environment. The lithium battery can provide auxiliary power supply for accelerating, climbing, lifting, and the forklift can still move to the hydrogen refueling equipment when the hydrogen fuel runs out. Besides the application in forklifts, the hydrogen fuel cell electric commercial vehicles will take very short time (i.e. 3 minutes) for refueling that will greatly reduce the downtime to help improve operation efficiency. Methodology There are different kinds of hydrogen fuel cells, including Alkali Fuel Cells (AFC), Molten Carbonate Fuel Cells (MCFC), Phosphoric Acid Fuel Cells (PAFC), Proton Exchange Membrane Fuel Cells (PEMFC) etc. Each type of fuel cells has different characteristic suits for different conditions or applications. The PEMFC can be constructed as fuel cell stack, designed for power output up to 250kw, operated at low enough temperature from 50 ℃ to 100 ℃ that most suitable for the application such as cars, buses, forklifts and trains etc. At current development stage, at a nominal driving speed (less than 30 mph), the power efficiency of a fuel cell electric drive using direct hydrogen is two times higher than that of a conventional internal combustion engine, so it is especially suitable for low driving speed application like forklifts. Main scientific and technical The hydrogen fuel cell/lithium battery hybrid system will comprise the hydrogen fuel cell stack and lithium battery pack. The hydrogen fuel cell stack has a high energy density and is suitable to be the primary energy source for forklift driving and static loading. The lithium battery pack has a high power density and is suitable as an auxiliary power source for power assisting of dynamic loading like forklift startup, accelerating, climbing and lifting. If the required power exceeds the output power of the fuel cell, the lithium battery will provide auxiliary power for the extra demand power of the forklift operation. If the required power is lower than the fuel cell output power, the fuel cell will provide power supply for the lithium battery. Achieved results We propose to develop the system design and control strategy for the hydrogen fuel cell/lithium battery hybrid electric commercial vehicles. The hybrid electric commercial vehicles will comprise two kinds of energy source, including hydrogen fuel cell stack and auxiliary lithium battery pack. Two DC/DC converters, a DC/AC converter and BMS for the battery pack will be designed to provide energy management strategy for the hybrid system. It would be a good reference for the future development for other applications.
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10

Bradshaw, Robert W., Joseph G. Cordaro, and Nathan P. Siegel. "Molten Nitrate Salt Development for Thermal Energy Storage in Parabolic Trough Solar Power Systems." In ASME 2009 3rd International Conference on Energy Sustainability collocated with the Heat Transfer and InterPACK09 Conferences. ASMEDC, 2009. http://dx.doi.org/10.1115/es2009-90140.

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Multi-component molten salts have been formulated recently that may enhance thermal energy storage for parabolic trough solar power plants. This paper presents further developments regarding molten salt mixtures consisting of common alkali nitrates and either alkaline earth nitrates or alkali nitrite salts that have advantageous properties for applications as heat transfer fluids in parabolic trough systems. We report results for formulations of inorganic molten salt mixtures that display freeze-onset temperatures below 100°C. In addition to phasechange behavior, several properties of these molten salts that significantly affect their suitability as thermal energy storage fluids were evaluated, including chemical stability and viscosity. The nitrate-based molten salts have demonstrated chemical stability in the presence of air up to 500°C. The capability to operate at temperatures up to 500°C may allow an increase in maximum temperature operating capability vs. organic fluids in existing trough systems and will enable increased power cycle efficiency. Experimental measurements of viscosity were performed from near the freeze-onset temperature to about 200°C. Viscosities can exceed 100 cP near the freezing temperature but are 4 to 5 cP in the anticipated operating temperature range. Experimental measurements of density, thermal conductivity and heat capacity are in progress and will be reported at the meeting. Corrosion tests were conducted for several thousand hours at 500°C with stainless steels and at 350°C for carbon and chromium-molybdenum steels. Examination of the specimens demonstrated good compatibility of these materials with the molten nitrate salt mixtures. Laboratory studies were conducted to identify mixtures of nitrate and nitrite (NO2−) salts as additional candidates for a low-melting heat transfer fluid. Mixtures in which the cations were potassium, sodium and lithium, in various proportions, demonstrated freezing points as low as 70°C for a particular nitrate/nitrite anion composition. Development has emphasized mixtures that minimize lithium content in order to reduce the cost as the lithium salt is the most expensive constituent. Work is in progress to explore the phase diagram of the 1:1 mol ratio of nitrate/nitrite and to evaluate physical properties such as viscosity, density and thermal conductivity. Results to date indicate that the viscosity of these mixtures is considerably less than nitrate-only melts, which necessarily contain calcium cations to suppress freezing to similarly low temperatures.
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Reports on the topic "Lithium alkyls"

1

Ullrich, Steven. Synthesis and Characterization of some Flourine-containing Lithium Alkyl Sulfonates: Flourinated Sulfonates and SF5-containing Sulfonates. Portland State University Library, January 2000. http://dx.doi.org/10.15760/etd.6756.

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2

Hsu, H. S., J. H. DeVan, and M. Howell. Equilibrium solubilities of LiFeO/sub 2/ and (Li,K)/sub 2/CrO/sub 4/ in molten alkali carbonates at 650/sup 0/C. [Lithium and potassium chromates]. Office of Scientific and Technical Information (OSTI), August 1986. http://dx.doi.org/10.2172/5279867.

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