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Aluminium hydride
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<h2 id="structure">Structure</h2> <p>Alane can adopt 3-, 4-, or 6-coordination, depending on conditions. </p> <h3>Gaseous alane</h3> <p>Monomeric AlH3 has been isolated at low temperature in a solid <a href="/facts/Noble_gas/j0yHMEAE">noble gas</a> matrix. It was shown to be planar.<a class="footnote-ref" id="fnref:2" href="#fn:2"><sup>2</sup></a> The dimeric form, Al2H6, has been isolated in solid hydrogen. It is <a href="/facts/Isostructural/xWlgsQ95">isostructural</a> with <a href="/facts/Diborane/k7egwbPf">diborane</a> (B2H6) and <a href="/facts/Digallane/Mnn9azCN">digallane</a> (Ga2H6).<a class="footnote-ref" id="fnref:3" href="#fn:3"><sup>3</sup></a><a class="footnote-ref" id="fnref:4" href="#fn:4"><sup>4</sup></a><a class="footnote-ref" id="fnref:5" href="#fn:5"><sup>5</sup></a> </p> <h3>Solid alane</h3> <p>Solid alane, which is colorless and nonvolatile, precipitates from etherial solutions over the course of hours at room temperature. Numerous <a href="/facts/Polymorphism_(materials_science)/bu2tqsB9">polymorphs</a> can be obtained, which have been labeled α-, α’-, β-, γ-, ε-, and ζ-alanes.<a class="footnote-ref" id="fnref:6" href="#fn:6"><sup>6</sup></a> The best characterized solid alane is α-alane. According to <a href="/facts/X-ray_crystallography/WtI0F5DN">X-ray crystallography</a>, adopts a cubic or rhombohedral morphology. It features octahedral AlH6 centers interconnected by Al-H-Al bridges. The Al-H distances are all equivalent (172 pm) and the Al-H-Al angles are 141°.<a class="footnote-ref" id="fnref:7" href="#fn:7"><sup>7</sup></a> α’-Alane forms needle-like crystals, and γ-alane forms bundles of fused needles. </p> <table><tbody><tr><th colspan="6">Crystallographic Structure of α-AlH3<a class="footnote-ref" id="fnref:8" href="#fn:8"><sup>8</sup></a></th></tr><tr><th>The α-AlH3 <a href="/facts/Unit_cell/znygJqdx">unit cell</a></th><th>Aluminium coordination</th><th>Hydrogen coordination</th></tr><tr><td></td><td></td><td></td></tr></tbody></table> <h2 id="handling">Handling</h2> <p>Alane is not spontaneously flammable.<a class="footnote-ref" id="fnref:9" href="#fn:9"><sup>9</sup></a> Even so, "similar handling and precautions as... exercised for Li[AlH4]" (the chemical reagent, <a href="/facts/Lithium_aluminium_hydride/QMMhdqEy">lithium aluminium hydride</a>) are recommended, as its "reactivity [is] comparable" to this related reducing reagent.<a class="footnote-ref" id="fnref:10" href="#fn:10"><sup>10</sup></a> For these reagents, both preparations in solutions and isolated solids are "highly flammable and must be stored in the absence of moisture".<a class="footnote-ref" id="fnref:11" href="#fn:11"><sup>11</sup></a> Laboratory guides recommend alane use inside a <a href="/facts/Fume_hood/dIsosPMN">fume hood</a>.<a class="footnote-ref" id="fnref:12" href="#fn:12"><sup>12</sup></a>[<i>why?</i>] Solids of this reagent type carry recommendations of handling "in a glove bag or <a href="/facts/Glove_box/NnR37n6E">dry box</a>".<a class="footnote-ref" id="fnref:13" href="#fn:13"><sup>13</sup></a> After use, solution containers are typically sealed tightly with concomitant flushing with inert gas to exclude the oxygen and moisture of ambient air.<a class="footnote-ref" id="fnref:14" href="#fn:14"><sup>14</sup></a> </p><p><a href="/facts/Passivation_(chemistry)/tPADJj5G">Passivation</a> greatly diminishes the decomposition rate associated with alane preparations. Passivated alane nevertheless retains a hazard classification of 4.3 (chemicals which in contact with water, emit flammable gases).<a class="footnote-ref" id="fnref:15" href="#fn:15"><sup>15</sup></a> </p> <h3>Reported accidents</h3> <p>Alane reductions are believed to proceed via an intermediate <a href="/facts/Coordination_complex/1tCyeQUm">coordination complex</a>, with aluminum attached to the partially reduced functional group, and liberated when the reaction undergoes protic <a href="/facts/Quenching_(chemistry)/LURlLf4C">quenching</a>. If the substrate is also <a href="/facts/Fluoroalkane/EwWmHflJ">fluorinated</a>, the intermediate may instead explode if exposed to a hot spot above 60°C.<a class="footnote-ref" id="fnref:16" href="#fn:16"><sup>16</sup></a> </p> <h2 id="preparation">Preparation</h2> <p>Aluminium hydrides and various complexes thereof have long been known.<a class="footnote-ref" id="fnref:17" href="#fn:17"><sup>17</sup></a> Its first synthesis was published in 1947, and a patent for the synthesis was assigned in 1999.<a class="footnote-ref" id="fnref:18" href="#fn:18"><sup>18</sup></a><a class="footnote-ref" id="fnref:19" href="#fn:19"><sup>19</sup></a> Aluminium hydride is prepared by treating <a href="/facts/Lithium_aluminium_hydride/QMMhdqEy">lithium aluminium hydride</a> with <a href="/facts/Aluminium_trichloride/xrhvSxDr">aluminium trichloride</a>.<a class="footnote-ref" id="fnref:20" href="#fn:20"><sup>20</sup></a> The procedure is intricate: attention must be given to the removal of <a href="/facts/Lithium_chloride/mNbthJx2">lithium chloride</a>. </p> 3 Li[AlH4] + AlCl3 → 4 AlH3 + 3 LiCl <p>The ether solution of alane requires immediate use, because polymeric material rapidly precipitates as a solid. Aluminium hydride solutions are known to degrade after 3 days. Aluminium hydride is more reactive than Li[AlH4].<a class="footnote-ref" id="fnref:21" href="#fn:21"><sup>21</sup></a> </p><p>Several other methods exist for the preparation of aluminium hydride: </p> 2 Li[AlH4] + BeCl2 → 2 AlH3 + Li2[BeH2Cl2] 2 Li[AlH4] + H2SO4 → 2 AlH3 + Li2SO4 + 2 H2 2 Li[AlH4] + ZnCl2 → 2 AlH3 + 2 LiCl + ZnH2 2 Li[AlH4] + I2 → 2 AlH3 + 2 LiI + H2 <h3>Electrochemical synthesis</h3> <p>Several groups have shown that alane can be produced <a href="/facts/Electrochemistry/C0RUWpBH">electrochemically</a>.<a class="footnote-ref" id="fnref:22" href="#fn:22"><sup>22</sup></a><a class="footnote-ref" id="fnref:23" href="#fn:23"><sup>23</sup></a><a class="footnote-ref" id="fnref:24" href="#fn:24"><sup>24</sup></a><a class="footnote-ref" id="fnref:25" href="#fn:25"><sup>25</sup></a><a class="footnote-ref" id="fnref:26" href="#fn:26"><sup>26</sup></a> Different electrochemical alane production methods have been patented.<a class="footnote-ref" id="fnref:27" href="#fn:27"><sup>27</sup></a><a class="footnote-ref" id="fnref:28" href="#fn:28"><sup>28</sup></a> Electrochemically generating alane avoids chloride impurities. Two possible mechanisms are discussed for the formation of alane in Clasen's electrochemical cell containing <a href="/facts/Tetrahydrofuran/P5t6SkMK">THF</a> as the solvent, <a href="/facts/Sodium_aluminium_hydride/HIXNehLt">sodium aluminium hydride</a> as the electrolyte, an aluminium anode, and an iron (Fe) wire submerged in <a href="/facts/Mercury_(element)/WlxfoHva">mercury</a> (Hg) as the cathode. The sodium forms an <a href="/facts/Amalgam_(chemistry)/5dRXJyt3">amalgam</a> with the Hg cathode preventing side reactions and the hydrogen produced in the first reaction could be captured and reacted back with the sodium mercury amalgam to produce sodium hydride. Clasen's system results in no loss of starting material. For insoluble anodes, reaction 1 occurs, while for soluble anodes, anodic dissolution is expected according to reaction 2: </p> <ol><li>[AlH4]− − <a href="/facts/Electron/L0KBo5cW">e−</a> + <i>n</i> THF → AlH3·<i>n</i>THF + 1/2 H2</li> <li>3 [AlH4]− + Al − 3 e− + 4<i>n</i> THF → 4 AlH3·<i>n</i>THF</li></ol> <p>In reaction 2, the aluminium anode is consumed, limiting the production of aluminium hydride for a given electrochemical cell. </p><p>The crystallization and recovery of aluminium hydride from electrochemically generated alane has been demonstrated.<a class="footnote-ref" id="fnref:29" href="#fn:29"><sup>29</sup></a><a class="footnote-ref" id="fnref:30" href="#fn:30"><sup>30</sup></a> </p> <h3>High pressure hydrogenation of aluminium</h3> <p>α-AlH3 can be produced by hydrogenation of aluminium at 10 <a href="/facts/GPa/Am1To2Qm">GPa</a> and 600 °C (1,112 °F). The reaction between the liquified hydrogen produces α-AlH3 which could be recovered under ambient conditions.<a class="footnote-ref" id="fnref:31" href="#fn:31"><sup>31</sup></a> </p> <h2 id="reactions">Reactions</h2> <h3>Formation of adducts with Lewis bases</h3> <p>AlH3 readily forms adducts with strong <a href="/facts/Lewis_acids_and_bases/qlLqRvg2">Lewis bases</a>. For example, both 1:1 and 1:2 complexes form with <a href="/facts/Trimethylamine/cj1dWmJq">trimethylamine</a>. The 1:1 complex is tetrahedral in the gas phase,<a class="footnote-ref" id="fnref:32" href="#fn:32"><sup>32</sup></a> but in the solid phase it is dimeric with bridging hydrogen centres, [(CH3)3NAlH2(μ-H)]2.<a class="footnote-ref" id="fnref:33" href="#fn:33"><sup>33</sup></a> The 1:2 complex adopts a <a href="/facts/Trigonal_bipyramid_molecular_geometry/fTayDtlN">trigonal bipyramidal structure</a>.<a class="footnote-ref" id="fnref:34" href="#fn:34"><sup>34</sup></a> Some adducts (e.g. dimethylethylamine alane, (CH3CH2)(CH3)2N·AlH3) thermally decompose to give aluminium and may have use in <a href="/facts/MOCVD/Ldg0BICo">MOCVD</a> applications.<a class="footnote-ref" id="fnref:35" href="#fn:35"><sup>35</sup></a> </p><p>Its complex with <a href="/facts/Diethyl_ether/Ep20vEdj">diethyl ether</a> forms according to the following stoichiometry: </p> AlH3 + (CH3CH2)2O → (CH3CH2)2O·AlH3 <p>Similar adducts are assumed to form when alane is generated in THF from lithium aluminium hydride. </p><p>The reaction with <a href="/facts/Lithium_hydride/uWCl2pST">lithium hydride</a> in ether produces <a href="/facts/Lithium_aluminium_hydride/QMMhdqEy">lithium aluminium hydride</a>: </p> AlH3 + LiH → Li[AlH4] <p>Various alanates have been characterized beyond lithium aluminium hydride. They tend to feature five- and six-coordinate Al centers: Na3AlH6, Ca(AlH4))2, SrAlH5).<a class="footnote-ref" id="fnref:36" href="#fn:36"><sup>36</sup></a> </p> <h3>Reduction of functional groups</h3> <p>Alane and its derivatives are <a href="/facts/Redox/Pyd5RVcj">reducing</a> reagents in <a href="/facts/Organic_synthesis/aprl6Iq7">organic synthesis</a> based around <a href="/facts/Group_13_hydride/05HHDu0R">group 13 hydrides</a>.<a class="footnote-ref" id="fnref:37" href="#fn:37"><sup>37</sup></a> In solution—typically in ethereal solvents such <a href="/facts/Tetrahydrofuran/P5t6SkMK">tetrahydrofuran</a> or <a href="/facts/Diethyl_ether/Ep20vEdj">diethyl ether</a>—aluminium hydride forms complexes with <a href="/facts/Lewis_base/qlLqRvg2">Lewis bases</a>, and reacts selectively with particular organic <a href="/facts/Functional_group/GXkSPsjM">functional groups</a> (e.g., with <a href="/facts/Carboxylic_acid/U4xuMosy">carboxylic acids</a> and <a href="/facts/Ester/FoUAIIw4">esters</a> over <a href="/facts/Organic_halide/FTmWVdPT">organic halides</a> and <a href="/facts/Nitro_group/pem2BhMY">nitro groups</a>), and although it is not a reagent of choice, it can react with carbon-carbon multiple bonds (i.e., through <a href="/facts/Alkenylaluminium_compounds/oz2DgmKK">hydroalumination</a>). Given its density, and with hydrogen content on the order of 10% by weight,<a class="footnote-ref" id="fnref:38" href="#fn:38"><sup>38</sup></a> some forms of alane are, as of 2016,<a class="footnote-ref" id="fnref:39" href="#fn:39"><sup>39</sup></a> active candidates for storing hydrogen and so for power generation in fuel cell applications, including electric vehicles.[<i>not verified in body</i>] As of 2006 it was noted that further research was required to identify an efficient, economical way to reverse the process, regenerating alane from spent aluminium product. </p><p>In organic chemistry, aluminium hydride is mainly used for the reduction of functional groups.<a class="footnote-ref" id="fnref:40" href="#fn:40"><sup>40</sup></a> In many ways, the reactivity of aluminium hydride is similar to that of <a href="/facts/Lithium_aluminium_hydride/QMMhdqEy">lithium aluminium hydride</a>. Aluminium hydride will reduce <a href="/facts/Aldehyde/xSIRkW03">aldehydes</a>, <a href="/facts/Ketone/BqQXpLo4">ketones</a>, <a href="/facts/Carboxylic_acid/U4xuMosy">carboxylic acids</a>, <a href="/facts/Anhydride/9YnWCsJo">anhydrides</a>, <a href="/facts/Acid_chloride/R4ppUXre">acid chlorides</a>, <a href="/facts/Ester/FoUAIIw4">esters</a>, and <a href="/facts/Lactone/UMgRUFtj">lactones</a> to their corresponding <a href="/facts/Alcohol_(chemistry)/Y0SCTDkh">alcohols</a>. <a href="/facts/Amide/C6kCzYEA">Amides</a>, <a href="/facts/Nitrile/Gz7RCnC6">nitriles</a>, and <a href="/facts/Oxime/xRlPfB6K">oximes</a> are reduced to their corresponding <a href="/facts/Amine/JvfYJfP6">amines</a>. </p><p>In terms of functional group selectivity, alane differs from other hydride reagents. For example, in the following cyclohexanone reduction, <a href="/facts/Lithium_aluminium_hydride/QMMhdqEy">lithium aluminium hydride</a> gives a trans:cis ratio of 1.9 : 1, whereas aluminium hydride gives a trans:cis ratio of 7.3 : 1.<a class="footnote-ref" id="fnref:41" href="#fn:41"><sup>41</sup></a> </p> <p>Alane enables the hydroxymethylation of certain ketones (that is the replacement of C−H by C−CH2OH at the <a href="/facts/Alpha_carbon/E44SeQ1L">alpha position</a>).<a class="footnote-ref" id="fnref:42" href="#fn:42"><sup>42</sup></a> The ketone itself is not reduced as it is "protected" as its enolate. </p> <p><a href="/facts/Organohalide/FTmWVdPT">Organohalides</a> are reduced slowly or not at all by aluminium hydride. Therefore, reactive functional groups such as <a href="/facts/Carboxylic_acid/U4xuMosy">carboxylic acids</a> can be reduced in the presence of halides.<a class="footnote-ref" id="fnref:43" href="#fn:43"><sup>43</sup></a> </p> <p>Aluminium hydride reduces <a href="/facts/Ester/FoUAIIw4">ester</a> in the presence of nitro groups.<a class="footnote-ref" id="fnref:44" href="#fn:44"><sup>44</sup></a> </p> <p>Aluminium hydride reduces acetals to half protected diols.<a class="footnote-ref" id="fnref:45" href="#fn:45"><sup>45</sup></a> </p> <p>Aluminium hydride reduces epoxide to the corresponding alcohol:<a class="footnote-ref" id="fnref:46" href="#fn:46"><sup>46</sup></a> </p> <p>The allylic rearrangement reaction carried out using aluminium hydride is a <a href="/facts/SN2_reaction/0N06Ra0R">SN2</a> reaction, and it is not sterically demanding:<a class="footnote-ref" id="fnref:47" href="#fn:47"><sup>47</sup></a> </p> <p>Aluminium hydride will reduce <a href="/facts/Carbon_dioxide/xGzpppEp">carbon dioxide</a> to <a href="/facts/Methane/kBHneYnh">methane</a> with heating: </p> 4 AlH3 + 3 CO2 → 3 CH4 + 2 Al2O3 <h3>Hydroalumination</h3> <p class="note">See also: <a href="/facts/Carbometalation/PPA3WdMv">Carbometalation § Carboalumination</a></p> <p>Akin to <a href="/facts/Hydroboration/Wm7v7Inr">hydroboration</a>, aluminium hydride can, in the presence of <a href="/facts/Titanium_tetrachloride/bGS32SsD">titanium tetrachloride</a>, add across <a href="/facts/Multiple_bond/Tdb1zgTc">multiple bonds</a>.<a class="footnote-ref" id="fnref:48" href="#fn:48"><sup>48</sup></a><a class="footnote-ref" id="fnref:49" href="#fn:49"><sup>49</sup></a> When the multiple bond in question is a <a href="/facts/Propargylic_alcohol/VgKsePpM">propargylic alcohols</a>, the results are <a href="/facts/Alkenylaluminium_compounds/oz2DgmKK">Alkenylaluminium compounds</a>.<a class="footnote-ref" id="fnref:50" href="#fn:50"><sup>50</sup></a> </p> <h3>Fuel</h3> <p>In its passivated form, alane is an active candidate for storing hydrogen, and can be used for efficient power generation via fuel cell applications, including fuel cell and electric vehicles and other lightweight power applications.<a class="footnote-ref" id="fnref:51" href="#fn:51"><sup>51</sup></a> AlH3 contains up 10.1% hydrogen by weight (at a density of 1.48 grams per milliliter),<a class="footnote-ref" id="fnref:52" href="#fn:52"><sup>52</sup></a> or twice the hydrogen density of liquid H2. As of 2006, AlH3 was described as a candidate for which "further research w[ould] be required to develop an efficient and economical process to regenerate [it] from the spent Al powder".<a class="footnote-ref" id="fnref:53" href="#fn:53"><sup>53</sup></a>[<i>needs update</i>] </p><p>Alane is also a potential additive to solid <a href="/facts/Rocket_fuel/IyFhQEA2">rocket fuel</a> and to explosive and pyrotechnic compositions due to its high hydrogen content and low dehydrogenation temperature.<a class="footnote-ref" id="fnref:54" href="#fn:54"><sup>54</sup></a> In its unpassivated form, alane is also a promising <a href="/facts/Rocket_fuel/IyFhQEA2">rocket fuel</a> additive, capable of delivering impulse efficiency gains of up to 10%.<a class="footnote-ref" id="fnref:55" href="#fn:55"><sup>55</sup></a> However, AlH3 can degrade when stored at room temperature, and some of its crystal forms have "poor compatibility" with some fuel components.<a class="footnote-ref" id="fnref:56" href="#fn:56"><sup>56</sup></a> </p> <h3>Deposition</h3> <p>Heated alane releases hydrogen gas and produces a very fine thin film of aluminum metal.<a class="footnote-ref" id="fnref:57" href="#fn:57"><sup>57</sup></a> </p> <h2 id="further-reading">Further reading</h2> <ul><li>Schmidt, Eckart W. (2022). "Aluminum Hydride". <i>Metals of the 2nd and 3rd Row and their Hydrides</i>. <i>Encyclopedia of Liquid Fuels</i>. De Gruyter. pp. 3799–3827. <a href="/facts/Doi_(identifier)/muM9Etpq">doi</a>:<a href="https://doi.org/10.1515%2F9783110750287-032">10.1515/9783110750287-032</a>. <a href="/facts/ISBN_(identifier)/15AdSPa9">ISBN</a> 978-3-11-075028-7.</li></ul> <h2 id="external-links">External links</h2> <ul><li><a href="http://EnvironmentalChemistry.com/yogi/chemicals/cn/Aluminum%A0hydride.html">Aluminium Hydride</a> on EnvironmentalChemistry.com Chemical Database</li> <li><a href="https://web.archive.org/web/20060823192048/http://www.bnl.gov/est/erd/hydrogenStorage/">Hydrogen Storage</a> from Brookhaven National Laboratory</li> <li><a href="http://www.webelements.com/compounds/aluminium/aluminium_trihydride.html">Aluminum Trihydride</a> on WebElements</li></ul> <h2 id="references">References</h2> <ol> <li id="fn:1"><p>Galatsis, P; Sintim, Herman O.; Wang J. (15 September 2008). "Aluminum Hydride". Encyclopedia of Reagents for Organic Synthesis (online ed.). New York, N.Y.: John Wiley & Sons. doi:10.1002/047084289X.ra082.pub2. ISBN 978-0471936237. Retrieved 28 July 2022. <a href="978-0471936237" target="_blank">978-0471936237</a> <a href="#fnref:1" class="footnote-back-ref">↩</a></p></li> <li id="fn:2"><p>Kurth, F. A.; Eberlein, R. A.; Schnöckel, H.-G.; Downs, A. J.; Pulham, C. R. (1993). "Molecular Aluminium Trihydride, AlH3: Generation in a Solid Noble Gas Matrix and Characterisation by its Infrared Spectrum and ab initio Calculations". Journal of the Chemical Society, Chemical Communications. 1993 (16): 1302–1304. doi:10.1039/C39930001302. (Abstract) Broad-band photolysis of a solid noble gas matrix containing Al atoms and H2 gives rise to the planar, monomeric AlH3 molecule. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:2" class="footnote-back-ref">↩</a></p></li> <li id="fn:3"><p>Andrews, Lester; Wang Xuefeng (2003). "The Infrared Spectrum of Al2H6 in Solid Hydrogen". Science. 299 (5615): 2049–2052. Bibcode:2003Sci...299.2049A. doi:10.1126/science.1082456. JSTOR 3833717. PMID 12663923. S2CID 45856199. See also emendations at doi:10.1126/science.300.5620.741a. <a href="/wiki/Bibcode_(identifier)" target="_blank">/wiki/Bibcode_(identifier)</a> <a href="#fnref:3" class="footnote-back-ref">↩</a></p></li> <li id="fn:4"><p>Pulham, C. R.; Downs, A. J.; Goode, M. J.; Rankin D. W. H.; Robertson, H. E. (1991). "Gallane: Synthesis, Physical and Chemical Properties, and Structure of the Gaseous Molecule Ga2H6 as Determined by Electron Diffraction". Journal of the American Chemical Society. 113 (14): 5149–5162. doi:10.1021/ja00014a003. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:4" class="footnote-back-ref">↩</a></p></li> <li id="fn:5"><p>Housecroft, Catherine (2018). Inorganic Chemistry (5th ed.). Pearson. p. 397. ISBN 978-1-292-13414-7. <a href="978-1-292-13414-7" target="_blank">978-1-292-13414-7</a> <a href="#fnref:5" class="footnote-back-ref">↩</a></p></li> <li id="fn:6"><p>Graetz, J..; Reilly, J..; Sandrock, G..; Johnson, J..; Zhou, W.-M.; Wegrzyn, J. (2006). Aluminum Hydride, A1H3, As a Hydrogen Storage Compound (Report). Washington, D.C.: Office of Science and Technical Information [OSTI]. doi:10.2172/899889. OSTI 899889. Retrieved 28 July 2022. <a href="https://www.osti.gov/biblio/899889-UGd8IT/" target="_blank">https://www.osti.gov/biblio/899889-UGd8IT/</a> <a href="#fnref:6" class="footnote-back-ref">↩</a></p></li> <li id="fn:7"><p>Turley & Rinn 1969. (Abstract) "The final Al⋯H distance of 1.72 Å, the participation of each Al in six bridges, and the equivalence of all Al⋯H distances suggest that 3c-2e bonding occurs." Angle is lasted as "Al(6)-H(5)-Al(4)" in Table IV. - Turley, J. W.; Rinn, H. W. (1969). "The Crystal Structure of Aluminum Hydride". Inorganic Chemistry. 8 (1): 18–22. doi:10.1021/ic50071a005. <a href="https://doi.org/10.1021%2Fic50071a005" target="_blank">https://doi.org/10.1021%2Fic50071a005</a> <a href="#fnref:7" class="footnote-back-ref">↩</a></p></li> <li id="fn:8"><p>Turley, J. W.; Rinn, H. W. (1969). "The Crystal Structure of Aluminum Hydride". Inorganic Chemistry. 8 (1): 18–22. doi:10.1021/ic50071a005. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:8" class="footnote-back-ref">↩</a></p></li> <li id="fn:9"><p>Galatsis, Sintim & Wang 2008, which describes the phenomenon using the synonym "inflammable". - Galatsis, P; Sintim, Herman O.; Wang J. (15 September 2008). "Aluminum Hydride". Encyclopedia of Reagents for Organic Synthesis (online ed.). New York, N.Y.: John Wiley & Sons. doi:10.1002/047084289X.ra082.pub2. ISBN 978-0471936237. Retrieved 28 July 2022. <a href="https://onlinelibrary.wiley.com/doi/10.1002/047084289X.ra082.pub2" target="_blank">https://onlinelibrary.wiley.com/doi/10.1002/047084289X.ra082.pub2</a> <a href="#fnref:9" class="footnote-back-ref">↩</a></p></li> <li id="fn:10"><p>Galatsis, P; Sintim, Herman O.; Wang J. (15 September 2008). "Aluminum Hydride". Encyclopedia of Reagents for Organic Synthesis (online ed.). New York, N.Y.: John Wiley & Sons. doi:10.1002/047084289X.ra082.pub2. ISBN 978-0471936237. Retrieved 28 July 2022. <a href="978-0471936237" target="_blank">978-0471936237</a> <a href="#fnref:10" class="footnote-back-ref">↩</a></p></li> <li id="fn:11"><p>Paquette, L. A.; Ollevier, T.; Desyroy, V. (15 October 2004). "Lithium Aluminum Hydride". Encyclopedia of Reagents for Organic Synthesis (online ed.). 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