Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Lithium hydride is an inorganic compound with the formula LiH. This alkali metal hydride is a colorless solid, although commercial samples are grey. Characteristic of a salt-like (ionic) hydride, it has a high melting point, and it is not soluble but reactive with all organic and protic solvents. It is soluble and nonreactive with certain molten salts such as lithium fluoride, lithium borohydride, and sodium hydride. With a molecular mass of slightly less than 8.0, it is the lightest ionic compound.
Contents
1Physical properties
2Synthesis and processing
3Reactions
4Applications
4.1Hydrogen storage and fuel
4.2Precursor to complex metal hydrides
4.3In nuclear chemistry and physics
4.3.1Lithium deuteride
5Safety
6References
7External links
Physical properties
LiH is a diamagnetic and an ionic conductor with a conductivity gradually increasing from 6995200000000000000♠2×10−5 Ω−1cm−1 at 443 °C to 0.18 Ω−1cm−1 at 754 °C; there is no discontinuity in this increase through the melting point.[3]:36 The dielectric constant of LiH decreases from 13.0 (static, low frequencies) to 3.6 (visible-light frequencies).[3]:35 LiH is a soft material with a Mohs hardness of 3.5.[3]:42 Its compressive creep (per 100 hours) rapidly increases from < 1% at 350 °C to > 100% at 475 °C, meaning that LiH can't provide mechanical support when heated.[3]:39
The thermal conductivity of LiH decreases with temperature and depends on morphology: the corresponding values are 0.125 W/(cm·K) for crystals and 0.0695 W/(cm·K) for compacts at 50 °C, and 0.036 W/(cm·K) for crystals and 0.0432 W/(cm·K) for compacts at 500 °C.[3]:60 The linear thermal expansion coefficient is 4.2×10−5/°C at room temperature.[3]:49
Synthesis and processing
LiH is produced by treating lithium metal with hydrogen gas:
2 Li + H2 → 2 LiH
This reaction is especially rapid at temperatures above 600 °C. Addition of 0.001–0.003% carbon, or/and increasing temperature or/and pressure, increases the yield up to 98% at 2-hour residence time.[3]:147 However, the reaction proceeds at temperatures as low as 29 °C. The yield is 60% at 99 °C and 85% at 125 °C, and the rate depends significantly on the surface condition of LiH.[3]:5
Less common ways of LiH synthesis include thermal decomposition of lithium aluminium hydride (200 °C), lithium borohydride (300 °C), n-butyllithium (150 °C), or ethyllithium (120 °C), as well as several reactions involving lithium compounds of low stability and available hydrogen content.[3]:144–145
Chemical reactions yield LiH in the form of lumped powder, which can be compressed into pellets without a binder. More complex shapes can be produced by casting from the melt.[3]:160 ff. Large single crystals (about 80 mm long and 16 mm in diameter) can be then grown from molten LiH powder in hydrogen atmosphere by the Bridgman–Stockbarger technique. They often have bluish color owing to the presence of colloidal Li. This color can be removed by post-growth annealing at lower temperatures (~550 °C) and lower thermal gradients.[3]:154 Major impurities in these crystals are Na (20–200 parts per million, ppm), O (10–100 ppm), Mg (0.5–6 ppm), Fe (0.5-2 ppm) and Cu (0.5-2 ppm).[3]:155
Cracking in cast LiH after machining with a fly cutter. Scale is in inches.
Bulk cold-pressed LiH parts can be easily machined using standard techniques and tools to micrometer precision. However, cast LiH is brittle and easily cracks during processing.[3]:171
Reactions
LiH powder reacts rapidly with air of low humidity, forming LiOH, Li 2O and Li 2CO 3. In moist air the powder ignites spontaneously, forming a mixture of products including some nitrogenous compounds. The lump material reacts with humid air, forming a superficial coating, which is a viscous fluid. This inhibits further reaction, although the appearance of a film of "tarnish" is quite evident. Little or no nitride is formed on exposure to humid air. The lump material, contained in a metal dish, may be heated in air to slightly below 200 °C without igniting, although it ignites readily when touched by an open flame. The surface condition of LiH, presence of oxides on the metal dish, etc., have a considerable effect on the ignition temperature. Dry oxygen does not react with crystalline LiH unless heated strongly, when an almost explosive combustion occurs.[3]:6
LiH is highly reactive toward water and other protic reagents:[3]:7
LiH + H2O → Li+ + H2 + OH−
LiH is less reactive with water than Li and thus is a much less powerful reducing agent for water, alcohols, and other media containing reducible solutes. This is true for all the binary saline hydrides.[3]:22
LiH pellets slowly expand in moist air, forming LiOH; however, the expansion rate is below 10% within 24 hours in a pressure of 2 Torr of water vapor.[3]:7 If moist air contains carbon dioxide, then the product is lithium carbonate.[3]:8 LiH reacts with ammonia, slowly at room temperature, but the reaction accelerates significantly above 300 °C.[3]:10 LiH reacts slowly with higher alcohols and phenols, but vigorously with lower alcohols.[3]:14
LiH reacts with sulfur dioxide:
2 LiH + 2 SO2 → Li2S2O4 + H2
though above 50 °C the product is lithium dithionite.[3]:9
LiH reacts with acetylene to form lithium carbide and hydrogen. With anhydrous organic acids, phenols and acid anhydrides LiH reacts slowly, producing hydrogen gas and the lithium salt of the acid. With water-containing acids, LiH reacts faster than with water.[3]:8 Many reactions of LiH with oxygen-containing species yield LiOH, which in turn irreversibly reacts with LiH at temperatures above 300 °C:[3]:10
LiH + LiOH → Li2O + H2
Applications
Hydrogen storage and fuel
With a hydrogen content in proportion to its mass three times that of NaH, LiH has the highest hydrogen content of any hydride. LiH is periodically of interest for hydrogen storage, but applications have been thwarted by its stability to decomposition. Thus removal of H2 requires temperatures above the 700 °C used for its synthesis, such temperatures are expensive to create and maintain. The compound was once tested as a fuel component in a model rocket.[7][8]
Precursor to complex metal hydrides
LiH is not usually a hydride-reducing agent, except in the synthesis of hydrides of certain metalloids. For example, silane is produced in the reaction of lithium hydride and silicon tetrachloride by the Sundermeyer process:
4 LiH + SiCl4 → 4 LiCl + SiH4
Lithium hydride is used in the production of a variety of reagents for organic synthesis, such as lithium aluminium hydride (LiAlH4) and lithium borohydride (LiBH4). Triethylborane reacts to give superhydride (LiBHEt3).[9]
In nuclear chemistry and physics
Lithium hydride (LiH) is sometimes a desirable material for the shielding of nuclear reactors, with the isotope lithium-7 (Li-7), and it can be fabricated by casting.[10][11]
Lithium deuteride
Lithium deuteride, in the form of lithium-7 deuteride, is a good moderator for nuclear reactors, because deuterium (H-2) has a lower neutron absorption cross-section than ordinary hydrogen (H-1) does, and the cross-section for Li-7 is also low, decreasing the absorption of neutrons in a reactor. Lithium-7 is preferred for a moderator because it has a lower neutron capture cross-section, and it also forms less tritium (H-3) under bombardment with neutrons.[12]
The corresponding lithium-6 deuteride, 6LiH, or 6LiD, is the primary fusion fuel in thermonuclear weapons. In hydrogen warheads of the Teller–Ulam design, a nuclear fission trigger explodes to heat and compress the lithium-6 deuteride, and to bombard the 6LiD with neutrons to produce tritium in an exothermic reaction: Li-6 + n --> He-4 + H-3. The deuterium and tritium (both isotopes of hydrogen) then fuse to produce helium-4, one neutron, and 17.59 MeV of free energy in the form of gamma rays, kinetic energy, etc. The helium is an inert byproduct.
Before the Castle Bravo nuclear weapons test in 1954, it was thought that only the less common isotope lithium-6 would breed tritium when struck with fast neutrons. The Castle Bravo test showed (accidentally) that the more plentiful lithium-7 also does so under extreme conditions, albeit by an endothermic reaction.
Safety
LiH reacts violently with water to give hydrogen gas and LiOH, which is caustic. Consequently, LiH dust can explode in humid air, or even in dry air due to static electricity. At concentrations of 5–55 mg/m3 in air the dust is extremely irritating to the mucous membranes and skin and may cause an allergic reaction. Because of the irritation, LiH is normally rejected rather than accumulated by the body.[3]:157,182
Some lithium salts, which can be produced in LiH reactions, are toxic. LiH fire should not be extinguished using carbon dioxide, carbon tetrachloride, or aqueous fire extinguishers; they should be smothered by covering with a metal object or graphite or dolomite powder. Sand is less suitable, as it can explode when mixed with burning LiH, especially if not dry. LiH is normally transported in oil, using containers made of ceramic, certain plastics or steel, and is handled in an atmosphere of dry argon or helium.[3]:156 Nitrogen can be used, but not at elevated temperatures, as it reacts with lithium.[3]:157 LiH normally contains some metallic lithium, which corrodes steel or silica containers at elevated temperatures.[3]:173–174, 179
References
^ abcLide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. p. 4.70. ISBN 0-8493-0486-5..mw-parser-output cite.citationfont-style:inherit.mw-parser-output qquotes:"""""""'""'".mw-parser-output code.cs1-codecolor:inherit;background:inherit;border:inherit;padding:inherit.mw-parser-output .cs1-lock-free abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/6/65/Lock-green.svg/9px-Lock-green.svg.png")no-repeat;background-position:right .1em center.mw-parser-output .cs1-lock-limited a,.mw-parser-output .cs1-lock-registration abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/d/d6/Lock-gray-alt-2.svg/9px-Lock-gray-alt-2.svg.png")no-repeat;background-position:right .1em center.mw-parser-output .cs1-lock-subscription abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/a/aa/Lock-red-alt-2.svg/9px-Lock-red-alt-2.svg.png")no-repeat;background-position:right .1em center.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registrationcolor:#555.mw-parser-output .cs1-subscription span,.mw-parser-output .cs1-registration spanborder-bottom:1px dotted;cursor:help.mw-parser-output .cs1-hidden-errordisplay:none;font-size:100%.mw-parser-output .cs1-visible-errorfont-size:100%.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registration,.mw-parser-output .cs1-formatfont-size:95%.mw-parser-output .cs1-kern-left,.mw-parser-output .cs1-kern-wl-leftpadding-left:0.2em.mw-parser-output .cs1-kern-right,.mw-parser-output .cs1-kern-wl-rightpadding-right:0.2em
^David Arthur Johnson; Open University (12 August 2002). Metals and chemical change. Royal Society of Chemistry. pp. 167–. ISBN 978-0-85404-665-2. Retrieved 1 November 2011.
^ abcdefghijklmnopqrstuvwxyzaaabacadSmith, R. L.; Miser, J. W. (1963). Compilation of the properties of lithium hydride. NASA.
^ abc"NIOSH Pocket Guide to Chemical Hazards #0371". National Institute for Occupational Safety and Health (NIOSH).
^Chambers, Michael. "ChemIDplus - 7580-67-8 - SIAPCJWMELPYOE-UHFFFAOYSA-N - Lithium hydride - Similar structures search, synonyms, formulas, resource links, and other chemical information". chem.sis.nlm.nih.gov. Retrieved 10 April 2018.
^"Lithium hydride". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
^Lex Archived 2008-07-23 at the Wayback Machine.. Astronautix.com (1964-04-25). Retrieved on 2011-11-01.
^Empirical laws for hybrid combustion of lithium hydride with fluorine in small rocket engines. Ntrs.nasa.gov. Retrieved on 2011-11-01.
^Peter Rittmeyer, Ulrich Wietelmann "Hydrides" in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a13_199
^Peter J. Turchi (1998). Propulsion techniques: action and reaction. AIAA. pp. 339–. ISBN 978-1-56347-115-5. Retrieved 2 November 2011.
^Welch, Frank H. (February 1974). "Lithium hydride: A space age shielding material". Nuclear Engineering and Design. 26 (3): 440–460. doi:10.1016/0029-5493(74)90082-X.
^Massie, Mark; Dewan, Leslie C. "US 20130083878 A1, April 4, 2013, NUCLEAR REACTORS AND RELATED METHODS AND APPARATUS". U.S. Patent Office. U.S. Government. Retrieved 2 June 2016.
External links
Look up lithium hydride in Wiktionary, the free dictionary.
University of Southampton, Mountbatten Centre for International Studies, Nuclear History Working Paper No5.
CDC - NIOSH Pocket Guide to Chemical Hazards
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Lithium compounds
Inorganic
LiAlCl4
LiAlH4
LiAlO2
LiBF4
LiBH4
LiBO2
LiB3O5
Li2B4O7
LiBr
Li2CO3
Li2C2
LiCl
LiClO
LiClO3
LiClO4
LiCoO2
LiF
LiH
LiI
LiIO3
Li2IrO3
Li2MoO4
LiNH2
Li2NH
LiN3
Li3N
LiNO2
LiNO3
LiNbO3
LiOH
LiO2
Li2O
Li2O2
LiPF6
Li2PtO3
Li2Po
Li2RuO3
Li2S
Li2SO3
Li2SO4
Li3H(CO3)2
Li2SiO3
LiTaO3
Li2TiO3
Organic
12-hydroxystearate
acetate
aspartate
citrate
diisopropylamide
orotate
succinate
stearate
organolithiums
Minerals
Amblygonite
Elbaite
Eucryptite
Jadarite
Lepidolite
Lithiophilite
Petalite
Pezzottaite
Saliotite
Spodumene
Sugilite
Tourmaline
Zabuyelite
Zinnwaldite
v
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e
Binary compounds of hydrogen
Alkali metal hydrides
LiH
NaH
KH
RbH
CsH
Lithium hydride, LiH ionic metal hydride
Beryllium hydride Left (gas phase): BeH2 covalent metal hydride Right: (BeH2)n (solid phase) polymeric metal hydride
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Art museum in Rovereto TN, Italy Museum of Modern and Contemporary Art of Trento and Rovereto Museo d'arte moderna e contemporanea di Trento e Rovereto MART, Entrance Location Corso Angelo Bettini, 43, 38068 Rovereto TN, Italy Coordinates 45°53′38″N 11°02′42″E / 45.8940°N 11.0450°E / 45.8940; 11.0450 Coordinates: 45°53′38″N 11°02′42″E / 45.8940°N 11.0450°E / 45.8940; 11.0450 Type Art museum Director Gianfranco Maraniello Public transit access Trento train station. Taxis outside station. Website mart.trento.it The Museum of Modern and Contemporary Art of Trento and Rovereto (MART) ( Museo d'Arte Moderna e Contemporanea di Trento e Rovereto , in Italian) is a museum centre in the Italian province of Trento. The main site is in Rovereto, and contains mostly modern and contemporary artworks, including works from renowned Giorgio Morandi, Giorgio de...