Lithium aluminium hydride

Lithium aluminium hydride, commonly abbreviated to LAH, is an inorganic compound with the chemical formula or . It is a white solid, discovered by Finholt, Bond and Schlesinger in 1947. 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 were once discussed for hydrogen storage.

Properties, structure, preparation

thumb|left|upright|[[scanning electron microscopy|Scanning Electron Microscope image of LAH powder]]

LAH is a colourless solid, but commercial samples are usually gray due to contamination. This material can be purified by recrystallization from diethyl ether. Large-scale purifications employ a Soxhlet extractor. Commonly, the impure gray material is used in synthesis, since the impurities are innocuous and can be easily separated from the organic products. The pure powdered material is pyrophoric but not its large crystals. Some commercial materials contain mineral oil to inhibit reactions with atmospheric moisture, but more commonly it is packed in moisture-proof plastic sacks.

LAH violently reacts with water to liberate hydrogen gas. The reaction proceeds according to the following idealized equation:

Structure

left|upright|thumb|The crystal structure of LAH; Li atoms are purple and tetrahedra are tan.

LAH crystallizes in the monoclinic space group P21/c. The unit cell has the dimensions: a = 4.82, b = 7.81, and c = 7.92 Å, α = γ = 90° and β = 112°. In the structure, cations are surrounded by five anions, which have tetrahedral molecular geometry. The cations are bonded to one hydrogen atom from each of the surrounding tetrahedral anion creating a bipyramid arrangement. At high pressures (>2.2 GPa) a phase transition may occur to give β-LAH.

left|thumb|class=skin-invert-image|upright|[[X-ray powder diffraction pattern of as-received . The asterisk designates an impurity, possibly LiCl.]]

Preparation

was first prepared from the reaction between lithium hydride (LiH) and aluminium chloride:

is then prepared by a salt metathesis reaction according to:

LiCl is removed by filtration from an ethereal solution of LAH, with subsequent precipitation of LAH to yield a product containing around 1 wt% LiCl.

Solubility data

{|class="wikitable" style="text-align:center"

|+ Solubility of (mol/L)

!rowspan=2 |Solvent

!colspan=5|Temperature (°C)

|- bgcolor=#ffdead

! 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. This process can be accelerated by the presence of catalytic elements, such as titanium, iron or vanadium.

thumb|class=skin-invert-image|[[Differential scanning calorimetry of as-received .]]

When heated LAH decomposes in a three-step reaction mechanism:

is usually initiated by the melting of LAH in the temperature range 150–170 °C, immediately followed by decomposition into solid , although is known to proceed below the melting point of as well. At about 200 °C, decomposes into LiH ()

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.

{|class="wikitable" style="margin:1em auto; text-align:center"

|+ Thermodynamic data for reactions involving

|- bgcolor=#ffdead

! Reaction || ΔH° (kJ/mol) || ΔS° (J/(mol·K)) || ΔG° (kJ/mol) || Comment

| align = left| (s) || −116.3 || −240.1 || −44.7 || Standard formation from the elements.

| align = left|LiH (s) + Al (s) + H2 (g) → LiAlH4 (s) || −95.6 || −180.2 || 237.6 || Using ΔfH°(LiH) = −90.579865, ΔfS°(LiH) = −679.9, and ΔfG°(LiH) = −67.31235744.

| align = left| (l) || 22 || – || – || Heat of fusion. Value might be unreliable.

| align = left|LiAlH4 (l) → Li3AlH6 (s) + 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 reducing agent. Often as a solution in diethyl ether and followed by an acid workup, it will convert esters, carboxylic acids, acyl chlorides, aldehydes, and ketones into the corresponding alcohols (see: carbonyl reduction). Similarly, it converts amide, nitro, nitrile, imine, oxime, and organic azides into the amines (see: amide reduction). It reduces quaternary ammonium cations into the corresponding tertiary amines. Reactivity can be tuned by replacing hydride groups by alkoxy groups. Due to its pyrophoric nature, instability, toxicity, low shelf life and handling problems associated with its reactivity, it has been replaced in the last decade, both at the small-industrial scale and for large-scale reductions by the more convenient related reagent sodium bis (2-methoxyethoxy)aluminium hydride, which exhibits similar reactivity but with higher safety, easier handling and better economics.

LAH is most commonly used for the reduction of esters and carboxylic acids to primary alcohols; prior to the advent of LAH 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 sodium borohydride|; 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. Epoxycyclohexanes are reduced to give axial alcohols preferentially.

Partial reduction of acid chlorides to give the corresponding aldehyde product cannot proceed via LAH, since the latter reduces all the way to the primary alcohol. Instead, the milder lithium tri-tert-butoxyaluminum hydride, which reacts significantly faster with the acid chloride than with the aldehyde, must be used. For example, when isovaleric acid is treated with thionyl chloride to give isovaleroyl chloride, it can then be reduced via lithium tri-tert-butoxyaluminum hydride to give isovaleraldehyde in 65% yield.

File:LAH rxns.png|class=skin-invert-image|

rect 5 12 91 74 alcohol

rect 82 178 170 240 epoxide

rect 121 9 193 69 alcohol2

rect 337 1 414 60 alcohol3

rect 458 55 526 117 alcohol4

rect 170 151 234 210 aldehyde

rect 141 259 207 279 nitrile

rect 135 281 196 300 amide

rect 128 311 204 366 amine1

rect 264 268 339 334 carboxylic acid

rect 457 362 529 413 alcohol5

rect 381 255 433 273 azide

rect 469 244 525 269 amine2

rect 321 193 401 242 ester

rect 261 141 320 203 ketone

desc none

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Lithium aluminium hydride also reduces alkyl halides to alkanes. Alkyl iodides react the fastest, followed by alkyl bromides and then alkyl chlorides. Primary halides are the most reactive followed by secondary halides. Tertiary halides react only in certain cases.

Lithium aluminium hydride does not reduce simple alkenes or arenes. Alkynes are reduced only if an alcohol group is nearby, and alkenes are reduced in the presence of catalytic TiCl4. It was observed that the reduces the double bond in the N-allylamides.

Inorganic chemistry

LAH is widely used to prepare main group and transition metal hydrides from the corresponding metal halides.

LAH also reacts with many inorganic ligands to form coordinated alumina complexes associated with lithium ions. 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.

In order to take advantage of the total hydrogen capacity, the intermediate compound LiH must be dehydrogenated as well. Due to its high thermodynamic stability this requires temperatures in excess of 400 °C, which is not considered feasible for transportation purposes. Accepting LiH + Al as the final product, the hydrogen storage capacity is reduced to 7.96 wt%. Another problem related to hydrogen storage is the recycling back to LiAlH4 which, owing to its relatively low stability, requires an extremely high hydrogen pressure in excess of 10000 bar.

: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 LiCl or lithium hydride in diethyl ether or THF:

:2 LiAlH4 + MgBr2 → Mg(AlH4)2 + 2 LiBr

Red-Al (or SMEAH, NaAlH2(OC2H4OCH3)2) is synthesized by reacting sodium aluminum tetrahydride (NaAlH4) and 2-methoxyethanol:

Safety

Handling

The highly reducing and pyrophoric nature of LAH requires special handling techniques to avoid its exposure to sources of ignition, moisture, and ambient oxygen. The use of a fume hood or dry box under an inert atmosphere is recommended for any work with large amounts of LAH. It is recommended that a class D fire extinguisher or dry sand is on standby in case of a fire, as other classes of extinguisher may intensify the fire if used.

Lab accidents

Due to the widespread use and hazardous character of LAH, it has been the cause of many lab accidents. Lab fires related to this compound have been the result of grinding, runaway reactions, improper storage, and spontaneous ignition. Often, these fires are made worse by the erroneous use of CO2 fire extinguishers, which can fuel LAH fires.