Lithium aluminium hydride

Lithium aluminium hydride
General
Systematic name	Lithium aluminium hydride
Other names	LAH, lithium alanate, lithium tetrahydridoaluminate Lithal (UK slang)
Molecular formula	LiAlH₄
Molar mass	37.95 g/mol
Appearance	white crystals (pure samples) grey powder (commercial material)
CAS number	^*
Properties
Density and phase	0.917 g/cm³, solid
Solubility in water	reactive
in diethyl ether, THF	5.92 and 2.96 mol/L
Melting point	150 °C (423 K), decomposing
Boiling point	n/a
Structure
Coordination geometry	?
Crystal structure	monoclinic
Dipole moment	? D
Hazards
MSDS	External MSDS
Main hazards	highly flammable
NFPA 704
Flash point	n/a
R/S statement	R: 15 S: 7/8, 24/25, 43
RTECS number	BD0100000
Supplementary data page
Structure & properties	n, ε_r, etc.
Thermodynamic data	Phase behaviour Solid, liquid, gas
Spectral data	UV, IR, NMR, MS
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) Chemical infobox

Lithium aluminium hydride (Li Al H₄), 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, recrystallized (from diethyl ether) LAH 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.

Preparation

LAH is usually produced by the reaction between lithium hydride (LiH) and aluminium chloride (AlCl₃)

4LiH + AlCl₃ $\rightarrow$ LiAlH₄ + 3LiCl

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 $\rightarrow$ 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 $\rightarrow$ 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 $\rightarrow$ LiAlH₄ + NaCl

KAlH₄ + LiCl $\rightarrow$ LiAlH₄ + KCl

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

'''2LiAlH₄ + MgBr₂

\rightarrow

Mg(AlH₄)₂ + 2LiBr

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 or Red-Al is more usual. 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. It is most commonly used for the reduction of esters and carboxylic acids 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 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. 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.

Amines can be prepared by the LAH reduction of amides, oximes, 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.

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 $\rightarrow$ 1/3Li₃AlH₆ + 2/3Al + H₂ (R1)

1/3Li₃AlH₆ $\rightarrow$ LiH + 1/3Al + 1/2H₂ (R2)

LiH + Al $\rightarrow$ LiAl + 1/2H₂ (R3)

R1 is usually initiated by the melting of LAH around a temperature of 150-170^oC immediately followed by decomposition into solid Li₃AlH₆. From 200-250^oC Li₃AlH₆ decompose into LiH (R2) which subsequently decompose into LiAl above 400^oC (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 500^oC. 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.

align="center" | **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 + 4H₂O

\rightarrow

Li⁺ + Al³⁺ + 4OH^- + 4H₂

Crystal structure

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.

align="center" | **Thermodynamic data for reactions involving LiAlH₄**
Reaction	ΔH^o (kJ/mol)	ΔS^o (J/(mol K))	ΔG^o (kJ/mol)	Comment
Li(s) + Al(s) + 2H₂(g) $\rightarrow$ LiAlH₄(s)	-116.3	-240.1	-44.7	Standard formation from the elements.
LiH(s) + Al(s) + 3/2H₂(g) $\rightarrow$ LiAlH₄(s)	-25.6	-170.2	23.6	Using ΔH^o_f(LiH) = -90.5, ΔS^o_f(LiH) = -69.9, and ΔG^o_f(LiH) = -68.3.
LiAlH₄(s) $\rightarrow$ LiAlH₄(l)	22	--	--	Heat of fusion. Value is probably unreliable.
LiAlH₄(l) $\rightarrow$ 1/3Li₃AlH₆(s) + 2/3Al(s) + 1/2H₂(g)	3.46	104.5	-27.68	ΔS^o calculated from reported values of ΔH^o and ΔG^o.

References

Reetz, M. T.; Drewes, M. W.; Schwickardi, R. Organic Syntheses, Coll. Vol. 10, p.256 (2004); Vol. 76, p.110 (1999). (Article)
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Koppenhoefer, B.; Schurig, V. Organic Syntheses, Coll. Vol. 8, p.434 (1993); Vol. 66, p.160 (1988). (Article)
Barnier, J. P.; Champion, J.; Conia, J. M. Organic Syntheses, Coll. Vol. 7, p.129 (1990); Vol. 60, p.25 (1981). (Article)
Elphimoff-Felkin, I.; Sarda, P. Organic Syntheses, Coll. Vol. 6, p.769 (1988); Vol. 56, p.101 (1977). (Article)
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)
Park, C. H.; Simmons, H. E. Organic Syntheses, Coll. Vol. 6, p.382 (1988); Vol. 54, p.88 (1974). (Article)
Chen, Y. K.; Jeon, S.-J.; Walsh, P. J.; Nugent, W. A. Organic Syntheses, Vol. 82, p.87 (2005). (Article)
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

on-line version
Chapter 5 in Full text version

External links

Lithium compounds | Aluminium compounds | Metal hydrides | Reagents for organic chemistry

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