| 词条 | Sodium aluminium hydride |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 443346228 | ImageFile1 = CaWO4.tif | ImageSize1 = | ImageFile2 = File:NaAlH4.png | ImageSize2 = | IUPACName = Sodium aluminium hydride | OtherNames =Sodium tetrahydroaluminate |Section1={{Chembox Identifiers | CASNo_Ref = {{cascite|correct|??}} | CASNo = 13770-96-2 | EINECS = 237-400-1 | PubChem = 26266 | InChI = 1S/Al.Na.4H/q-1;+1;;;; | SMILES = [Na+].[AlH4-] |Section2={{Chembox Properties | Na=1 | Al=1 | H=4 | Appearance = White crystalline solid | Density = 1.24 g/cm3 | MeltingPtC = 183 | MeltingPt_notes = (decomposes) | BoilingPt = | Solubility = | SolubleOther = soluble in THF (16 g/100 mL at room temperature) |Section3={{Chembox Hazards | ExternalSDS = External MSDS | FlashPtF = -7 | AutoignitionPtC = }}Sodium aluminium hydride or sodium alanate is an inorganic compound with the chemical formula NaAlH4. It is a white pyrophoric solid that dissolves in tetrahydrofuran (THF), but not in diethyl ether or hydrocarbons. It has been evaluated as an agent for the reversible storage of hydrogen and it is used as a reagent for the chemical synthesis of organic compounds. Similar to lithium aluminium hydride, it is a salt consisting of separated sodium cations and tetrahedral AlH{{su|b=4|p=−}} anions.[1] Structure, preparation, and reactionsSodium tetrahydroaluminate adopts the structure of (is isostructural with) calcium tungstate. As such, the tetrahedral AlH{{su|b=4|p=−}} centers are linked with eight-coordinat Na+ cations.[2] The compound is prepared from the elements under high pressures of H2 at 200 °C using triethylaluminium catalyst:[3] Na + Al + 2 H2 → NaAlH4 As a suspension in diethyl ether, it reacts with lithium chloride to give the popular reagent lithium aluminium hydride: LiCl + NaAlH4 → LiAlH4 + NaCl The compound reacts rapidly, even violently, with protic reagents, such as water, as described in this idealized equation: 4 H2O + NaAlH4 → "NaAl(OH)4" + 4 H2 ApplicationsHydrogen storageSodium alanate[4] has been explored for hydrogen storage in hydrogen tanks.[5] The relevant reactions are: 3 NaAlH4 → Na3AlH6+ Al + H2 Na3AlH6 → 3 NaH + Al + 3/2 H2 Sodium tetrahydroaluminate can release up to 7.4 wt % of hydrogen when heated at {{convert|200|°C|°F}}. Absorption can be slow, with several minutes being required to fill a tank. Both release and uptake are catalysed by titanium.[6] Reagent in organic chemistrySodium aluminium hydride is a strong reducing agent, very similar in reactivity to lithium aluminum hydride (LAH) and, to some extent, Diisobutylaluminium hydride (DIBAL) in organic reactions.[7] It is much more powerful reducing agent than sodium borohydride due to the weaker and more polar Al-H bond compared to the B-H bond. Like LAH, it reduces esters to alcohols. SafetySodium aluminium hydride is highly flammable. It does not react in dry air at room temperature but is very sensitive to moisture. It ignites or explodes on contact with water. See also
References1. ^J. W. Lauher, D. Dougherty P. J. Herley "Sodium tetrahydroaluminate" Acta Crystallogr. 1979, volume B35, pp.1454-1456. {{doi|10.1107/S0567740879006701}} {{sodium compounds}}{{aluminium compounds}}2. ^Dougherty, D.; Herley, P. J.; Lauher, J. W. "Sodium tetrahydridoaluminate"Acta Crystallographica B (24,1968-38,1982) (1979) 35, p1454-p1456. 3. ^Peter Rittmeyer, Ulrich Wietelmann "Hydrides" in Ullmann's Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinheim. {{DOI|10.1002/14356007.a13_199}} 4. ^[https://books.google.com/books?id=LgEXet3y4PQC&pg=PA45&dq=sodium+alanate&hl=en&sa=X&ved=0CCoQ6AEwAWoVChMIjfbll8ikxwIVCROQCh056wIG#v=onepage&q=sodium%20alanate&f=false Computational Study of Pristine and Titanium-doped Sodium Alanates for ...] 5. ^{{ cite journal |author1=Zaluska, A. |author2=Zaluski, L. |author3=Ström-Olsen, J. O. | title = Sodium Alanates for Reversible Hydrogen Storage | journal = Journal of Alloys and Compounds | year = 2000 | volume = 298 | issue = 1–2 | pages = 125–134 | doi = 10.1016/S0925-8388(99)00666-0 }} 6. ^{{ cite web | url = http://phys.org/news123307288.html | title = Researchers Solve Decade-Old Mystery of Hydrogen Storage Material | publisher = Phys.Org | date = 2008-02-27 }} 7. ^Melinda Gugelchuk "Sodium Aluminum Hydride" Encyclopedia of Reagents for Organic Synthesis, 2001, John Wiley. {{DOI|10.1002/047084289X.rs039}} 5 : Sodium compounds|Aluminium complexes|Hydrogen storage|Metal hydrides|Reducing agents |
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