Lithium aluminium hydride

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Lithium aluminium hydride
IUPAC name Lithium aluminium hydride
Other names LAH, lithium alanate,
lithium tetrahydridoaluminate
Lithal (UK slang)
CAS number 16853-85-3
RTECS number BD0100000
Molecular formula LiAlH4
Molar mass 37.95 g/mol
Appearance white crystals (pure samples)
grey powder (commercial material)
Density 0.917 g/cm3, solid
Melting point

150 °C (423 K), decomposing

Solubility in water reactive
Crystal structure monoclinic
Main hazards highly flammable
NFPA 704

NFPA 704.svg

R/S statement R: 15 S: 7/8, 24/25, 43
Related Compounds
Related hydride sodium borohydride
sodium hydride
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)

Infobox disclaimer and references

Lithium aluminium hydride (LiAlH4), commonly abbreviated to LAH, is a powerful reducing agent used in organic chemistry. It is more powerful than the related reducing agent sodium borohydride due to the weaker Al-H bond compared to the B-H bond. It will convert esters, carboxylic acids and ketones to alcohols; and nitro compounds into amines.

LAH violently reacts with water, including atmospheric moisture, and the pure material is pyrophoric. Commercial material is inhibited with mineral oil to allow handling in air.

Pure LAH (recrystallized from diethyl ether) is a white solid. Commercial samples are almost always grey due to trace contamination with aluminium metal. White air-exposed commercial samples of LAH have absorbed enough moisture to become a mixture of lithium hydroxide and aluminium hydroxide.


LAH is usually produced in industry[1] by first preparing sodium aluminium hydride from the elements

Na + Al + 2 H2 → NaAlH4

under high pressure and temperature. LAH is then prepared by salt elimination according to:

NaAlH4 + LiCl → LiAlH4 + NaCl

In the laboratory it is easily accessible by the reaction between lithium hydride (LiH) and aluminium chloride (AlCl3)

4 LiH + AlCl3 → LiAlH4 + 3 LiCl

which proceeds with a high yield of LAH (97% w/w). LiCl is removed by filtration from an ethereal solution of LAH, with subsequent precipitation of LAH to yield a product with around 1% w/w LiCl.

Inorganic reactions

LAH and NaH can be used to produce sodium aluminium hydride (NaAlH4) by metathesis in THF with a yield of 90.7% w/w

LiAlH4 + NaH → NaAlH4 + LiH

Potassium aluminium hydride (KAlH4) can be produced with a yield of 90% w/w by reaction in diglyme in a similar way

LiAlH4 + KH → KAlH4 + LiH

The reverse, i.e., production of LAH from either sodium aluminium hydride or potassium aluminium hydride can be obtained by reaction with LiCl in diethyl ether and THF with a yield of 93.5 and 91% w/w, respectively.

NaAlH4 + LiCl → LiAlH4 + NaCl
KAlH4 + LiCl → LiAlH4 + KCl

Magnesium alanate (Mg(AlH4)2) can be synthesized from LAH and MgBr2

2 LiAlH4 + MgBr2 → Mg(AlH4)2 + 2 LiBr

Use in organic chemistry

Lithium aluminium hydride is widely used in organic chemistry as a very powerful reducing agent. Despite handling problems associated with its reactivity, it is even used at the small-industrial scale, although for large scale reductions the related reagent sodium bis(2-methoxyethoxy)aluminium hydride, commonly known as Red-Al, is more often used. For such purposes it is usually used in solution in diethyl ether, and an aqueous workup is usually performed after the reduction in order to remove inorganic by-products.

LAH is most commonly used for the reduction of esters[2][3] and carboxylic acids[4] to primary alcohols; prior to the advent of LiAlH4 this was a difficult conversion involving sodium metal in boiling ethanol (the Bouveault-Blanc reduction). Aldehydes and ketones[5] can also be reduced to alcohols by LAH, but this is usually done using milder reagents such as NaBH4. α,β-Unsaturated ketones are reduced to allylic alcohols.[6] When epoxides are reduced using LAH, the reagent attacks the less hindered end of the epoxide, usually producing a secondary or tertiary alcohol. It reduces by progressive breakup of the complex AlH4 and transfer of hydride ions to the positive centre in an organic compound which may have a low density of electrons due to inductive or mesomeric effects.

Organic reactions of lithium aluminium hydride

Amines can be prepared by the LAH reduction of amides[7][8], oximes[9], nitriles, nitro compounds or alkyl azides. LAH is also able to reduce primary alkyl halides to alkanes.

Lithium aluminium hydride is not able to reduce simple alkenes or benzene rings, and alkynes are only reduced if an alcohol group is nearby.[10]

Thermal decomposition

At room temperature LAH is metastable. During prolonged storage it may slowly decompose to Li3AlH6 and LiH. This process can be accelerated by the presence of catalytic elements e.g. Ti, Fe, V.

When heated LAH decompose in a three step reaction mechanism.

LiAlH4 → ⅓ Li3AlH6 + ⅔ Al + H2 (R1)
⅓ Li3AlH6 → LiH + ⅓ Al + ½ H2 (R2)
LiH + Al → LiAl + ½ H2 (R3)

R1 is usually initiated by the melting of LAH around a temperature of 150-170oC immediately followed by decomposition into solid Li3AlH6. From 200-250oC Li3AlH6 decompose into LiH (R2) which subsequently decompose into LiAl above 400oC (R3). R1 is effectively irreversible, because LiAlH4 is metastable. The reversibility of R2 has not yet been conclusively established. R3 is reversible with an equilibrium pressure of about 0.25 bar at 500oC. R1 and R2 can occur at room temperature with suitable catalysts.

According to reactions R1-R3 LiAlH4 contains 10.6 wt% hydrogen thereby making LAH a potential hydrogen storage medium for future fuel cell powered vehicles. Cycling only R2 would store 5.6 wt% in the material in a single step (comparable to the two steps of NaAlH4).

Solubility data

LAH is soluble in many etheral solutions. However, it may spontaneously decompose due to the presence of catalytic impurities, though, it appears to be more stable in THF. Thus, THF is preferred over e.g. diethyl ether even despite the lower solubility.

Solubility data for LiAlH4 (mol/l)
Temperature (oC)
Solvent 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 -- -- --

Note that water should not be used as a solvent for lithium aluminium hydride, which would react as in the following equation.

LiAlH4 + 4 H2O → Li+ + Al3+ + 4 OH- + 4 H2

Crystal structure

The crystal structure of LAH. Li atoms are blue and AlH4 tetrahedra are red. The unit cell border is marked by a black line.

The crystal structure of LAH belongs to the monoclinic crystal system and the space group is P21c. The crystal structure of LAH is illustrated to the right. The structure consists of Li atoms surrounded by five AlH4 tetrahedra. The Li atoms are bonded to one hydrogen atom from each of the surrounding tetrahedra creating a bipyramid arrangement. The side lengths of the unit cell are approx. a=4.82, b=7.81 and c=7.92, and the β angle is approx. 112 °. At high pressures (>2.2GPa) a phase transition into β-LAH occurs.

Thermodynamic data

The table summarizes thermodynamic data for LAH and reactions involving LAH, in the form of standard enthalpy, entropy and Gibbs free energy change, respectively.

Thermodynamic data for reactions involving LiAlH4
Reaction ΔHo (kJ/mol) ΔSo (J/(mol K)) ΔGo (kJ/mol) Comment
Li (s) + Al (s) + 2 H2(g) → LiAlH4 (s) -116.3 -240.1 -44.7 Standard formation from the elements.
LiH (s) + Al (s) + 3/2 H2 (g) → LiAlH4 (s) -25.6 -170.2 23.6 Using ΔHof(LiH) = -90.5, ΔSof(LiH) = -69.9, and ΔGof(LiH) = -68.3.
LiAlH4 (s) → LiAlH4 (l) 22 -- -- Heat of fusion. Value is probably unreliable.
LiAlH4 (l) → ⅓ Li3AlH6 (s) + ⅔ Al (s) + H2 (g) 3.46 104.5 -27.68 ΔSo calculated from reported values of ΔHo and ΔGo.


  1. Holleman, A. F., Wiberg, E., Wiberg, N. (2007). Lehrbuch der Anorganischen Chemie, 102nd ed. de Gruyter. ISBN 978-3-11-017770-1. 
  2. Reetz, M. T.; Drewes, M. W.; Schwickardi, R. Organic Syntheses, Coll. Vol. 10, p.256 (2004); Vol. 76, p.110 (1999). (Article)
  3. Oi, R.; Sharpless, K. B. Organic Syntheses, Coll. Vol. 9, p.251 (1998); Vol. 73, p.1 (1996). (Article)
  4. Koppenhoefer, B.; Schurig, V. Organic Syntheses, Coll. Vol. 8, p.434 (1993); Vol. 66, p.160 (1988). (Article)
  5. Barnier, J. P.; Champion, J.; Conia, J. M. Organic Syntheses, Coll. Vol. 7, p.129 (1990); Vol. 60, p.25 (1981). (Article)
  6. Elphimoff-Felkin, I.; Sarda, P. Organic Syntheses, Coll. Vol. 6, p.769 (1988); Vol. 56, p.101 (1977). (Article)
  7. Seebach, D.; Kalinowski, H.-O.; Langer, W.; Crass, G.; Wilka, E.-M. Organic Syntheses, Coll. Vol. 7, p.41 (1990); Vol. 61, p.24 (1983). (Article)
  8. Park, C. H.; Simmons, H. E. Organic Syntheses, Coll. Vol. 6, p.382 (1988); Vol. 54, p.88 (1974). (Article)
  9. Chen, Y. K.; Jeon, S.-J.; Walsh, P. J.; Nugent, W. A. Organic Syntheses, Vol. 82, p.87 (2005). (Article)
  10. Wender, P. A.; Holt, D. A.; Sieburth, S. Mc N. Organic Syntheses, Coll. Vol. 7, p.456 (1990); Vol. 64, p.10 (1986). (Article)

General references and further reading

  • Wiberg, Egon & Amberger, Eberhard (1971). Hydrides of the elements of main groups I-IV. Elsevier. ISBN 0-444-40807-X. 
  • Hajos, Andor (1979). Complex Hydrides and Related Reducing Agents in Organic Synthesis. Elsevier. ISBN 0-444-99791-1. 
  • Lide (ed.), David R. (1997). Handbook of chemistry and physics. CRC Press. ISBN 0-8493-0478-4. 
  • Carey, Francis A. (2002). Organic Chemistry with Online Learning Center and Learning by Model CD-ROM. McGraw-Hill. ISBN 0-07-252170-8.  on-line version
  • Chapter 5 in Andreasen, Anders (2005). Hydrogen Storage Materials with Focus on Main Group I-II Elements. Risoe National Laboratory. ISBN 87-550-3498-5.  Full text version
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