Lithium aluminium hydride
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Names | |||
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Preferred IUPAC name
Lithium tetrahydridoaluminate(III) | |||
Systematic IUPAC name
Lithium alumanuide | |||
Other names
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Identifiers | |||
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3D model (
JSmol ) |
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Abbreviations | LAH | ||
ChEBI | |||
ChemSpider | |||
ECHA InfoCard
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100.037.146 | ||
EC Number |
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13167 | |||
PubChem CID
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RTECS number
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UNII | |||
UN number | 1410 | ||
CompTox Dashboard (EPA)
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Properties | |||
Li[AlH4] | |||
Molar mass | 37.95 g·mol−1 | ||
Appearance | white crystals (pure samples) grey powder (commercial material) hygroscopic
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Odor | odorless | ||
Density | 0.917 g/cm3, solid | ||
Melting point | 150 °C (302 °F; 423 K) (decomposes) | ||
Reacts | |||
Solubility in tetrahydrofuran | 112.332 g/L | ||
Solubility in diethyl ether | 39.5 g/(100 mL) | ||
Structure | |||
monoclinic
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P21/c | |||
Thermochemistry | |||
Heat capacity (C)
|
86.4 J/(mol·K) | ||
Std molar
entropy (S⦵298) |
87.9 J/(mol·K) | ||
Std enthalpy of (ΔfH⦵298)formation |
−117 kJ/mol | ||
Gibbs free energy (ΔfG⦵)
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−48.4 kJ/mol | ||
Hazards[2] | |||
GHS labelling: | |||
Danger | |||
H260, H314 | |||
P223, P231+P232, P280, P305+P351+P338, P370+P378, P422[1] | |||
NFPA 704 (fire diamond) | |||
Flash point | 125 °C (257 °F; 398 K) | ||
Safety data sheet (SDS) | Lithium aluminium hydride | ||
Related compounds | |||
Related hydride
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aluminium hydride sodium borohydride sodium hydride Sodium aluminium hydride | ||
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 aluminium hydride, commonly abbreviated to LAH, is an inorganic compound with the chemical formula Li[AlH4] or LiAlH4. It is a white solid, discovered by Finholt, Bond and Schlesinger in 1947.[4] This compound is used as a reducing agent in organic synthesis, especially for the reduction of esters, carboxylic acids, and amides. The solid is dangerously reactive toward water, releasing gaseous hydrogen (H2). Some related derivatives have been discussed for hydrogen storage.
Properties, structure, preparation
LAH is a colourless solid but commercial samples are usually gray due to contamination.
LAH violently reacts with water, including atmospheric moisture, to liberate dihydrogen gas. The reaction proceeds according to the following idealized equation:[5]
- Li[AlH4] + 4 H2O → LiOH + Al(OH)3 + 4 H2
This reaction provides a useful method to generate hydrogen in the laboratory. Aged, air-exposed samples often appear white because they have absorbed enough moisture to generate a mixture of the white compounds lithium hydroxide and aluminium hydroxide.[8]
Structure
LAH crystallizes in the
Preparation
Li[AlH4] was first prepared from the reaction between lithium hydride (LiH) and aluminium chloride:[4][5]
- 4 LiH + AlCl3 → Li[AlH4] + 3 LiCl
In addition to this method, the industrial synthesis entails the initial preparation of sodium aluminium hydride from the elements under high pressure and temperature:[10]
- Na + Al + 2 H2 → Na[AlH4]
Li[AlH4] is then prepared by a salt metathesis reaction according to:
- Na[AlH4] + LiCl → Li[AlH4] + NaCl
which proceeds in a high yield. LiCl is removed by filtration from an ethereal solution of LAH, with subsequent precipitation of LAH to yield a product containing around 1% w/w LiCl.[10]
An alternative preparation starts from LiH, and metallic Al instead of AlCl3. Catalyzed by a small quantity of TiCl3 (0.2%), the reaction proceeds well using
Solubility data
Solvent | Temperature (°C) | ||||
---|---|---|---|---|---|
0 | 25 | 50 | 75 | 100 | |
Diethyl ether | – | 5.92 | – | – | – |
THF
|
– | 2.96 | – | – | – |
Monoglyme | 1.29 | 1.80 | 2.57 | 3.09 | 3.34 |
Diglyme | 0.26 | 1.29 | 1.54 | 2.06 | 2.06 |
Triglyme | 0.56 | 0.77 | 1.29 | 1.80 | 2.06 |
Tetraglyme | 0.77 | 1.54 | 2.06 | 2.06 | 1.54 |
Dioxane
|
– | 0.03 | – | – | – |
Dibutyl ether | – | 0.56 | – | – | – |
LAH is soluble in many ethereal solutions. However, it may spontaneously decompose due to the presence of catalytic impurities, though, it appears to be more stable in tetrahydrofuran (THF). Thus, THF is preferred over, e.g., diethyl ether, despite the lower solubility.[12]
Thermal decomposition
LAH is
When heated LAH decomposes in a three-step reaction mechanism:[13][14][15]
-
3 Li[AlH4] → Li3[AlH6] + 2 Al + 3 H2
(R1)
-
2 Li3[AlH6] → 6 LiH + 2 Al + 3 H2
(R2)
-
2 LiH + 2 Al → 2 LiAl + H2
(R3)
R1 is usually initiated by the melting of LAH in the temperature range 150–170 °C,[16][17][18] immediately followed by decomposition into solid Li3[AlH6], although R1 is known to proceed below the melting point of Li[AlH4] as well.[19] At about 200 °C, Li3[AlH6] decomposes into LiH (R2)[13][15][18] and Al which subsequently convert into LiAl above 400 °C (R3).[15] Reaction R1 is effectively irreversible. R3 is reversible with an equilibrium pressure of about 0.25 bar at 500 °C. R1 and R2 can occur at room temperature with suitable catalysts.[20]
Thermodynamic data
The table summarizes thermodynamic data for LAH and reactions involving LAH,[21][22] in the form of standard enthalpy, entropy, and Gibbs free energy change, respectively.
Reaction | ΔH° (kJ/mol) |
ΔS° (J/(mol·K)) |
ΔG° (kJ/mol) |
Comment |
---|---|---|---|---|
Li (s) + Al (s) + 2 H2 (g) → Li[AlH4] (s) | −116.3 | −240.1 | −44.7 | Standard formation from the elements. |
LiH (s) + Al (s) + 3⁄2 H2 (g) → LiAlH4 (s) | −95.6 | −180.2 | 237.6 | Using ΔH°f(LiH) = −90.579865, ΔS°f(LiH) = −679.9, and ΔG°f(LiH) = −67.31235744. |
Li[AlH4] (s) → Li[AlH4] (l) | 22 | – | – | Heat of fusion. Value might be unreliable. |
LiAlH4 (l) → 1⁄3 Li3AlH6 (s) + 2⁄3 Al (s) + H2 (g) | 3.46 | 104.5 | −27.68 | ΔS° calculated from reported values of ΔH° and ΔG°. |
Applications
Use in organic chemistry
Lithium aluminium hydride (LAH) is widely used in organic chemistry as a
LAH is most commonly used for the reduction of
Partial reduction of
Lithium aluminium hydride also reduces
Lithium aluminium hydride does not reduce simple
Inorganic chemistry
LAH is widely used to prepare main group and transition
LAH also reacts with many inorganic ligands to form coordinated alumina complexes associated with lithium ions.[21]
- LiAlH4 + 4NH3 → Li[Al(NH2)4] + 4H2
Hydrogen storage
LiAlH4 contains 10.6 wt% hydrogen, thereby making LAH a potential hydrogen storage medium for future fuel cell-powered vehicles. The high hydrogen content, as well as the discovery of reversible hydrogen storage in Ti-doped NaAlH4,[41] have sparked renewed research into LiAlH4 during the last decade. A substantial research effort has been devoted to accelerating the decomposition kinetics by catalytic doping and by ball milling.[42] In order to take advantage of the total hydrogen capacity, the intermediate compound
Other tetrahydridoaluminiumates
A variety of salts analogous to LAH are known. NaH can be used to efficiently produce sodium aluminium hydride (NaAlH4) by metathesis in THF:
- LiAlH4 + NaH → NaAlH4 + LiH
Potassium aluminium hydride (KAlH4) can be produced similarly in diglyme as a solvent:[43]
- LiAlH4 + KH → KAlH4 + LiH
The reverse, i.e., production of LAH from either sodium aluminium hydride or potassium aluminium hydride can be achieved by reaction with
- NaAlH4 + LiCl → LiAlH4 + NaCl
- KAlH4 + LiCl → LiAlH4 + KCl
"Magnesium alanate" (Mg(AlH4)2) arises similarly using MgBr2:[44]
- 2 LiAlH4 + MgBr2 → Mg(AlH4)2 + 2 LiBr
See also
References
- ^ Sigma-Aldrich Co., Lithium aluminium hydride. Retrieved on 2018-06-1.
- ^ Index no. 001-002-00-4 of Annex VI, Part 3, to Regulation (EC) No 1272/2008 of the European Parliament and of the Council of 16 December 2008 on classification, labelling and packaging of substances and mixtures, amending and repealing Directives 67/548/EEC and 1999/45/EC, and amending Regulation (EC) No 1907/2006. OJEU L353, 31.12.2008, pp 1–1355 at p 472.
- ^ Lithium aluminium hydride
- ^ .
- ^ ISBN 978-1-86928-384-1.
- ISBN 0-470-02966-8.
- doi:10.1016/j.jssc.2005.09.027. Archived from the original(PDF) on 2016-03-03. Retrieved 2010-05-07.
- ISBN 978-0-8155-1553-1.
- .
- ^ ISBN 978-3-11-017770-1.)
{{cite book}}
: CS1 maint: multiple names: authors list (link - PMID 21863886.
- ^ .
- ^ a b c Dymova T. N.; Aleksandrov, D. P.; Konoplev, V. N.; Silina, T. A.; Sizareva; A. S. (1994). Russian Journal of Coordination Chemistry. 20: 279.
{{cite journal}}
: Missing or empty|title=
(help) - .
- ^ .
- .
- .
- ^ .
- .
- .
- ^ ISBN 978-0-07-049439-8.
- .
- ISBN 0-471-26418-0.
- ^ Seebach, D.; Kalinowski, H.-O.; Langer, W.; Crass, G.; Wilka, E.-M. (1991). "Chiral Media for Asymmetric Solvent Inductions. (S,S)-(+)-1,4-bis(Dimethylamino)-2,3-Dimethoxybutane from (R,R)-(+)-Diethyl Tartrate". Organic Syntheses; Collected Volumes, vol. 7, p. 41.
- ^ Park, C. H.; Simmons, H. E. (1974). "Macrocyclic Diimines: 1,10-Diazacyclooctadecane". Organic Syntheses. 54: 88; Collected Volumes, vol. 6, p. 382.
- ^ Chen, Y. K.; Jeon, S.-J.; Walsh, P. J.; Nugent, W. A. (2005). "(2S)-(−)-3-exo-(Morpholino)Isoborneol". Organic Syntheses. 82: 87.
- ^ "Red-Al, Sodium bis(2-methoxyethoxy)aluminumhydride". Organic Chemistry Portal.
- ^ Reetz, M. T.; Drewes, M. W.; Schwickardi, R. (1999). "Preparation of Enantiomerically Pure α-N,N-Dibenzylamino Aldehydes: S-2-(N,N-Dibenzylamino)-3-Phenylpropanal". Organic Syntheses. 76: 110; Collected Volumes, vol. 10, p. 256.
- ^ Oi, R.; Sharpless, K. B. (1996). "3-[(1S)-1,2-Dihydroxyethyl]-1,5-Dihydro-3H-2,4-Benzodioxepine". Organic Syntheses. 73: 1; Collected Volumes, vol. 9, p. 251.
- ^ Koppenhoefer, B.; Schurig, V. (1988). "(R)-Alkyloxiranes of High Enantiomeric Purity from (S)-2-Chloroalkanoic Acids via (S)-2-Chloro-1-Alkanols: (R)-Methyloxirane". Organic Syntheses. 66: 160; Collected Volumes, vol. 8, p. 434.
- ^ Barnier, J. P.; Champion, J.; Conia, J. M. (1981). "Cyclopropanecarboxaldehyde". Organic Syntheses. 60: 25; Collected Volumes, vol. 7, p. 129.
- ^ Elphimoff-Felkin, I.; Sarda, P. (1977). "Reductive Cleavage of Allylic Alcohols, Ethers, or Acetates to Olefins: 3-Methylcyclohexene". Organic Syntheses. 56: 101; Collected Volumes, vol. 6, p. 769.
- .
- ISBN 0-13-147871-0.
- ISBN 978-0-321-81139-4.
- PMID 18121883.
- .
- ISBN 0-521-31117-9.
- ^ Wender, P. A.; Holt, D. A.; Sieburth, S. Mc N. (1986). "2-Alkenyl Carbinols from 2-Halo Ketones: 2-E-Propenylcyclohexanol". Organic Syntheses. 64: 10; Collected Volumes, vol. 7, p. 456.
- PMID 25347383.
- .
- ^ ISBN 978-0-387-77711-5.
- ^ .
- ISBN 0-12-352651-5.
- .
Further reading
- Wiberg, E.; Amberger, E. (1971). Hydrides of the Elements of Main Groups I-IV. Elsevier. ISBN 0-444-40807-X.
- Hajos, A. (1979). Complex Hydrides and Related Reducing Agents in Organic Synthesis. Elsevier. ISBN 0-444-99791-1.
- Lide, D. R., ed. (1997). Handbook of Chemistry and Physics. CRC Press. ISBN 0-8493-0478-4.
- Carey, F. A. (2002). Organic Chemistry with Online Learning Center and Learning by Model CD-ROM. McGraw-Hill. ISBN 0-07-252170-8.
- Andreasen, A. (2005). "Chapter 5: Complex Hydrides" (PDF). Hydrogen Storage Materials with Focus on Main Group I-II Elements. Risø National Laboratory. ISBN 87-550-3498-5. Archived from the original(PDF) on 2012-08-19.
External links
- "Usage of LiAlH4". Organic Syntheses.
- "Lithium Tetrahydridoaluminate – Compound Summary (CID 28112)". PubChem.
- "Lithium Tetrahydridoaluminate". WebBook. NIST.
- "Materials Safety Data Sheet". Cornell University. Archived from the original on March 8, 2006.
- "Hydride Information Center". Sandia National Laboratory. Archived from the original on May 7, 2005.
- "Reduction Reactions" (PDF). Teaching Resources – 4th Year. University of Birmingham. Archived from the original (PDF) on May 23, 2016.