Soluble magnesium hydrides, method of preparing them, and use thereof

The present invention relates to previously unknown highly reactive and soluble magnesium hydrides, a method of preparing them, and their use in chemical syntheses.
Magnesium dihydride, MgH.sub.2 (hereinafter "magnesium hydride") is known as a solid that is insoluble in all organic and inorganic solvents. This is true not only of the highly reactive magnesium hydride obtained from the elements at high temperatures and pressures (Ullmans Enzyklopadie der technischen Chemie, 4th Ed., Vol, 13, p. 116) but also of that obtained catalytically under mild conditions (B. Bogdanovic, EP 3564. Studiengesellschaft Kohle mbH, 1982).
According to European Patent 3564, hydridomagnesium halides that are soluble in tetrahydrofuran (THF) can be prepared by catalytically hydrogenating magnesium in the presence of magnesium halides. It accordingly becomes possible to prepare tetrahydrofuran solutions for example that are no more than 1.5 molar in terms of the hydride content, assuming the structural formula I (1<n<2) for the dissolved species (B. Bogdanovic & M. Schwickardi, Zeitschrf. f. Naturforsch. 39b [1984], 1001). This means that 2 moles of the soluble hydridomagnesium chloride (HMgCl) can be used to obtain in soluble form 1 mole of the per se insoluble magnesium hydride. The hydridomagnesium chloride solutions can then be concentrated to obtain solutions of Type I with n a maximum of 3. ##STR3##
It is of course possible to prepare the THF solutions of Type I only at the cost of low hydrogenation temperatures (0.degree. C.), long hydrogenation times (18-20 hours), and incomplete conversion, which is a considerable drawback on an industrial scale.
It is known from the literature that soluble magnesium hydrides of the formula HMgQ--wherein Q is an alkyl, aryl, dialkyl (or aryl) amino, alkoxy, or halide radical--can be obtained by reacting an especially reactive form of magnesium hydride (MgH.sub.2 *), obtainable from dialkylmagnesium compounds and LiAlH.sub.4, by reaction with MgQ.sub.2 compounds (E. C. Ashby & T. Smith, Chem. Comm. 30 [1978] for alkyl and aryl; E. C. Ashby et al, J. Org. Chem. 43 [1978], 1564 for amide; and E. C. Ashby & A. B. Goel, Inorg. Chem. 18 [1979], 1306 for alcoholate and 16 [1977], 2941 for halide).
Thus ##STR4##
None of the aforesaid instances resulted in the dissolution of more than 1 mole of MgH.sub.2 * per mole of MgQ.sub.2, meaning that solutions of Type II ##STR5## cannot be obtained in this way, and the method is not appropriate for obtaining soluble MgH.sub.2 hydrides on a technical scale.
Even the conversion of a stoichiometric excess of the active magnesium hydride (MdH.sub.2 **), insoluble in tetrahydrofuran, catalytically obtained as described in European Patent 3564 with different MgQ.sub.2 compounds in tetrahydrofuran, does not lead to compounds of Type II with n>1. The most that can be obtained is to bring an equimolar amount of MgH.sub.2 ** per mole of MgQ.sub.2 into solution.
Thus ##STR6##
It is accordingly an object of the present invention to provide magnesium hydrides (MgH.sub.2) that are soluble in the organic phase and a method of preparing them. The desired magnesium hydrides should, due to their satisfactory solubility in the organic phase, have a reactivity as good or better than magnesium hydrides from the state of the art and should also be stable for a long time when dissolved, with no loss of reactivity. The object also includes providing magnesium hydrides that are much easier to handle and especially to measure out than the known solid magnesium hydrides. The method should also make available such organic-soluble magnesium hydrides in yields appropriate for industrial-scale production.
It has now surprisingly been discovered that highly active magnesium hydrides (MgH.sub.2) can be prepared in a soluble form by preparing adducts of magnesium hydride on organomagnesium compounds, organoboron compounds, organoaluminum compounds, or even tertiary bicyclic amines. The preparation of such adducts leads, surprisingly even on an industrial scale, to highly active magnesium hydrides that are soluble in organic phase.
The invention relates to magnesium hydrides that are soluble in the organic phase and have the general formulas ##STR7## wherein Q represents straight-chained or branched alkyl, alkenyl, alkoxy, dialkylamino, aralkyl, aryl or diarylamino groups with 1 to 18 carbon atoms in the alkyl group and 6 to 18 carbon atoms in the aryl group,
R represents alkenyl, aralkyl, or aryl groups with comparable numbers of atoms,
X is chlorine, bromine, or iodine, ##STR8## is a chelating ligand wherein E --CH.sub.2, --N(R)-- and --O--, and D represents a dialkylamino, diarylamino, or alkoxy group with comparable numbers of carbon atoms,
p is a whole number from 1 to 6,
M is aluminum or boron,
1<n.ltoreq.50, and
m is 1, 2, or 3.
The invention also relates to a method of preparing soluble magnesium hydride of the general formulas (II) through (VIII) characterized by catalytically hydrogenating finely powdered magnesium, optionally in the presence of magnesium halides, in an organic solvent in the presence of the compounds ##STR9## wherein Q, R, X, E is ##STR10## M, and m have the foregoing significance.
The invention also relates to the use of soluble magnesium hydrides of Formulas II through VIII, wherein Q, R, X, ##STR11## p, M, m, and n have the foregoing significance, to prepare organomagnesium compounds as reducing agents and as reagents for hydrogenating metals and non-metals.
The new magnesium hydrides that are soluble in the organic phase in accordance with the invention have the general formulas II through III, wherein Q represents straight-chained or branched alkyl, alkenyl, alkoxy, dialkylamino, aralkyl, aryl or diarylamino groups with 1 to 18 carbon atoms in the alkyl group and 6 to 18 carbon atoms in the aryl group. The n-alkyl groups accordingly include the series methyl, ethyl, propyl, butyl, pentyl, hexyl, heptyl, octyl, nonyl, decyl, undecyl, dodecyl, tridecyl, tetradecyl, pentadecyl, hexadecyl, heptadecyl,and octadecyl. Instead of the aforesaid n-alkyl groups, Q can also represent their branched-chain isomers with 1 to 18 carbon atoms. How many branches the alkyl has or at what points in the chain they occur makes no difference. Alkyls with 1 to 8 carbon atoms are preferred.
Instead of the alkyl groups, the Q in Formulas II and VII can represent alkenyl groups with 1 to 18 carbon atoms. These can also be straight-chained or branched and have one or more double bonds at any point on the chain or side chain. An alkenyl with 1 to 8 carbon atoms is preferred. One example is the allyl group.
The Q in the aforesaid general formulas can also stand for alkoxy groups with 1 to 18 carbon atoms in the alkyl. Any of the alkyl groups previously specified herein can also contain a hydroxy substituent, preferably at the terminal carbon atom. The preferred alkoxy groups that Q can represent are those with 1 to 6 carbon atoms.
The Q in the aforesaid formulas can also stand for aralkyl or aryl groups with comparable numbers of carbon atoms. Preferred are benzyl, phenylethyl and phenyl. Q as even higher aralkyl or aryl groups, however, is also possible in the general formulas II and VII.
Q can also stand for dialkylamino or diarylamino groups with comparable numbers of carbon atoms. Groups of this type have two alkyls or aryls of the previously specified series attached to their amino-nitrogen atom.
The R in general formulas III and VI stands for straight-chain or branched alkyl or alkenyl groups or aralkyl or aryl groups with numbers of carbon atoms that are comparable to those of the aforesaid Q groups. Especially preferred from the aforesaid series for R are straight-chain alkyls with 1 to 8 carbon atoms, allyl, benzyl or phenyl radicals. ##STR12## in the general formulas IV, V, and VII stands for chelating ligands wherein E represents --CH.sub.2 --, --N(R)-- or --O--, D represents a dialkylamino, diarylamino or alkoxy group, all from the previously specified series, and --(CH.sub.2).sub.p 13 is an alkylene group from the series methylene, ethylene, trimethylene, tetramethylene, pentamethylene, or hexamethylene. E and D are accordingly attached through an alkylene of that type.
n in the aforesaid Formulas II through VIII can be greater than 1 and less than or equal to 50. This means that more than 1 but no more than 50 molecules of magnesium hydride (MgH.sub.2) per molecule of the adductor are bonded in the compounds with the general formulas II through VIII in accordance with the invention. The structure of these compounds should essentially be depicted as previously herein in relation to the hydrid magnesium halides I or the 1:1 adducts of the organomagnesium hydrides II.
The compounds of the general formulas II through VIII are prepared in accordance with the invention by catalytically hydrogenating finely powdered magnesium in an organic solvent in the presence of the compounds IIa through VIIIa. The finely powdered magnesium is commercially available powdered magnesium obtained by technical synthesis. It will preferably have a particle size of 0.3 to 0.04 mm (50-325 mesh). Such finely powdered magnesium is listed for example on page 7 of the catalog of the Ventron Company 1983).
The reaction is carried out in an appropriate organic solvent. Preferred solvents are those that stabilize alkaline earth metals in the organic phase. Particularly appropriate are cyclic ethers, preferably tetrahydrofuran.
The catalytic hydrogenation is carried out in the presence of slight amounts of compounds IIa through VIII a. In the context of the aforesaid definitions of Q, R, X, ##STR13## M, and m, diorganomagnesium compounds, organomagnesium halides, bis(chelate)magnesium compounds, chelate-magnesium halides, quinuclidine or its organosubstituted homologues, which can be substituted with an R of the aforesaid series at any point of the bicyclic ring system, aluminum trialkyls, aluminumalkyl halides, boron trialkyls, boronalkyl halides, and aluminum-chelate halides or boron-chelate halides are appropriate.
The catalytic hydrogenation is carried out with molecular hydrogen, which is supplied to the system in a conventional way at normal or elevated pressure. Operating at an elevated molecular-hydrogen pressure of up to 60 bars is preferred.
Preferred catalysts are those described in European Patent 3564 and European Laid Open Application 157,297. This means halides of the metals of the IVth through VIII subgroups of the periodic system. Especially preferred are compounds or combinations of compounds from the halides of titanium, chromium and iron. Usually supplied to the system as co-catalysts are such polycyclic aromatics as anthracene or its magnesium adduct (magnesium anthracene).
It is also possible to add equimolar or preferably substoichiometric (catalytic) amounts of magnesium halides (MgX.sub.2) during the hydrogenation. Such magnesium halides, however, are, like the extra tertiary amine described as a co-catalyst in the aforementioned publications, unnecessary, although they can have a positive effect on the yield and purity of the reaction product.
The soluble magnesium hydrides II through VIII are formed in accordance with the reaction equations ##STR14##
In one preferred embodiment of the method in accordance with the invention it is possible to produce the reaction components RMgX (IIIa) or ##STR15## in situ from magnesium and RX or from chelating ligand ##STR16## instead of adding it already synthesized to the reaction batch to prepare compounds III or V.
The soluble magnesium hydrides prepared in accordance with the instant method can be used for, among other purposes, preparing organomagnesium compounds by adding them to 1-alkenes, as reducing agents, and to prepare metallic or elementary hydrides (SiH.sub.4) and intermetallic compounds and their hydrides and carbides (J. of the Less Common Metals 131 [1987], 163). They have the following advantages over the catalytically prepared suspensions and solid magnesium hydride:
Easy and safe handling and transportation in that the up-to-5 molar solution in tetrahydrofuran does not, in contrast to the suspension, ignite in air.
Higher reactivity in chemical reactions.
Better possibility for measuring out.
The stability of the MgH.sub.2 solutions in tetrahydrofuran at room temperature depends on the molarity and the type of complexing agent. Whereas it was possible to keep a solution with the composition (MgH.sub.2).sub.6.Mg(C.sub.8 H.sub.17).sub.2.(MgCl.sub.2).sub.0.3 (3.8 molar in terms of the MgH.sub.2) under argon for 4 weeks with a practically unaltered hydride concentration, a solution with the composition (MgH.sub.2).sub.30.n-C.sub.8 H.sub.17 MgCl (3.7 molar in terms of the MgH.sub.2) solidified after only one week at room temperature. Evaporating the tetrahydrofuran from a solution of MgH.sub.2 in tetrahydrofuran with the composition (MgH.sub.2).sub.6.5.Mg(n-C.sub.8 H.sub.17).sub.2.(MgCl.sub.2).sub.0.7 (1.9 molar in terms of the MgH.sub.2) yielded a viscous oil that it was possible to re-dissolve in the same volume of tetrahydrofuran to obtain the same hydride content.

The process will now be described with reference to examples which are not to be considered as limiting the scope of the invention in any way.
EXAMPLE 1
The reaction vessel was a 250 ml two-necked cylindrical flask equipped with a magnetic stirrer, a tailkey stopcock, and stoppers, and was an appropriate glass insert for a 50 ml autoclave. 10.00 g (411 mmoles) of powdered magnesium (with a mean particle size of 0.050 mm or appr. 270 mesh) and 0.73 g (4.1 mmoles) of anthracene were added to 20 ml of absolute tetrahydrofuran. 0.05 ml of ethyl bromide were added and the suspension was stirred at room temperature. The solution turned green, and orange magnesium anthracene.tetrahydrofuran precipitated out about 20 minutes later. 0.72 g (4.5 mmoles) of anhydrous CrCl.sub.3 was added to the batch, which was simultaneously cooled (with water at 15.degree. C.) and stirred, whereupon magnesium anthracene went into solution in an exothermic reaction accompanied by a color change to deep brown. The solution was then treated with, first, 30 ml of tetrahydrofuran and, second, 22 ml of a 1.18 molar di-n-octylmagnesium solution in tetrahydrofuran (26 mmoles) (B. Bogdanovic, M. Schwickardi, & P. Sikorski, Angew. Chem. Suppl. [1982], 457). The glass vessel was placed in a flat-bottomed 500 ml stainless-steel autoclave and the suspension hydrogenated while simultaneously being powerfully agitated with the magnetic stirrer at 22.degree. to 26.degree. C. and an initial hydrogen pressure of 60 bar. The hydrogen pressure dropped to 40 bar within 33/4 hours. The volume of the resulting magnesium hydride mixture was 77 ml. 10 ml was centrifuged for 1 hour at 10 000 rpm. 2.0 ml of the clear residual solution was subjected to pyrolysis with ethanol (cooled with water), yielding 318 ml of gas (20.degree. C. at 1 bar) composed (by MS analysis) of H.sub.2 97.6, C.sub.2 H.sub.5 OH 1.8, and THF 0.6% (another sample of the solution was centrifuged for 2.5 hours with the same result). The amount of H.sub.2 that formed was equivalent to a total magnesium hydride in solution of 249 mmoles or a yield of 61% soluble magnesium hydride in terms of the initial powdered magnesium. The composition of the soluble magnesium hydride is determined from the amount of di-n-octylmagnesium employed (26 mmoles) to be (MgH.sub.2).sub.9.6.Mg(n-C.sub.8 H.sub.17).sub.2. The concentration of the tetrahydrofuran solution was 3.25 molar in terms of the soluble magnesium hydride. IR analysis of a centrifuged magnesium-hydride solution revealed the broad absorption band at 1100 cm.sup.-1 typical of MgH.sub.2 and another magnesium-hydride band at 670 cm.sup.-1.
EXAMPLES 2 TO 17
These tests were carried out analogously to Example 1 and with the same amounts of magnesium, anthracene, CrCl.sub.3, and tetrahydrofuran. The details and results of the tests are listed in Table 1. Example 17 was a comparison example, with no complexing agents.
TABLE 1 Preparing soluble magnesium hydrides by catalytically hydrogenating magnesium in the presence of various complexing agents (see text for amounts) Vol. Vol. H.sub.2.sup.c Hydride mmoles Yield.sup.d Complexing Hydr. Pressure.sup.b of from content MgH.sub.2 of sol. Composition Ex. MgCl.sub.2.sup.a agent time, drop, susp. protol. moles in MgH.sub.2 of soluble No. added mmoles/ml THF hours bar ml ml H/l sol. (%) MgH.sub.2 1 - Mg(-n-C.sub.8 H.sub.17).sub.2 3.75 20 77 310 6.5 249 61 (MgH.sub.2).sub.9.6.Mg(-n-C.su b.8 H.sub.17).sub.2 26/22 2 + Mg(CH.sub.3 C.sub.6 H.sub.5).sub.2 2.5 25 72 343 7.15 257 63 (MgH.sub.2).sub.10.Mg(CH.sub.2 C.sub.6 H.sub.5).sub.2.(MgCl.sub.2).sub.0.6 26/20 3 - -n-C.sub.8 H.sub.17 MgCl 4.5 24 76 345 7.2 273 66 (MgH.sub.2).sub.15.-n-C.sub.8 H.sub.17 MgCl 18/15 4 - -n-C.sub.8 H.sub.17 MgCl 5.33 23 75 359 7.5 280 68 (MgH.sub.2).sub.30.8.-n-C.sub.8 H.sub.17 MgCl 9/8 5 - -n-C.sub.8 H.sub.17 Cl.sup.e 3.66 23 77 307 6.4 246 63 (MgH.sub.2).sub.12.3.-n-C.sub.8 H.sub.17 MgCl 20/-- 6 - -nC.sub.4 H.sub.9 MgCl 4.25 23 72 236 4.9 177 43 (MgH.sub.2).sub.10.-n-C.sub.4 H.sub.9 MgCl 18/14 7 + Mg[(CH.sub.2).sub.4 OCH.sub.3 ].sub.2 1 11 64 196 4.1 130 32 (MgH.sub.2).sub.6.5.Mg[(CH.sub.2).sub.4 OCH.sub.3 ].sub.2 (MgCl.sub.2).sub.0.7 20/10 8 - Cl(CH.sub.2).sub.3 OCH.sub.3.sup.e 5.66 24 77 361 7.5 290 75 (MgH.sub.2).sub.11.6.ClMg(CH.sub.2).sub.3 OCH.sub.3 25/-- 9 - Mg[(CH.sub.2).sub.4 OCH.sub.3 ].sub.2 7.25 23 75 305 6.35 238 58 (MgH.sub.2).sub.10.Mg[(CH.sub.2).sub.4 OCH.sub.3 ].sub.2 24/9 10 + Mg[(CH.sub.2).sub.3 N(CH.sub.3).sub.2 ].sub.2 3.33 17 75 163 3.4 127 31 (MgH.sub.2).sub.4.5.Mg[(C.sub.3 H.sub.6 N(CH.sub.3).sub.2 ].sub.2.(MgCl.sub.2).sub.0.5 28.4/-- 11 + Mg[O(CH.sub.2).sub.2 CH(CH.sub.3)OCH.sub.3 ].sub.2 6 10 .sup. 73.sup.f 85 1.7 64 15 (MgH.sub.2).sub.2.5.Mg[O(CH.sub.2).sub.2 CH(CH.sub.3)OCH.sub.3 ].sub.2.(MgCl.sub.2).sub.0.6 26/25 12 - C.sub.7 H.sub.13 N.HCl.sup.g 5 22 55 436 9.1 250 62 (MgH.sub.2).sub.12.7.C.sub.7 H.sub.13 N.(MgCl.sub.2).sub.0.5 19.6/-- 13 - C.sub.7 H.sub.13 N.HCl.sup.g & h 5 22 100 228 4.7 237 58 (MgH.sub.2).sub.46.C.sub.7 H.sub.13 N.(MgCl.sub.2).sub.0.5 5.2/-- 14 + Al(-n-C.sub.8 H.sub.17).sub.3 7.5 23 80 237 4.9 197 48 (MgH.sub.2).sub.7.6.Al(C.sub.8 H.sub.17).sub.3.(MgCl.sub.2).sub.0.6 26/20 15 + Al(-n-C.sub.4 H.sub.9).sub.3 3.5 16.5 75 127 2.65 99 24 (MgH.sub.2).sub.4.Al(C.sub.4 H.sub.9).sub.3.(MgCl.sub.2).sub.0.6 25/-- 16 + B(CH.sub.2 C.sub.6 H.sub.5).sub.3 6.75 23 70 169 3.5 123 30 (MgH.sub.2).sub.4.9.B(CH.sub.2 C.sub.6 H.sub.5).sub.3.(MgCl.sub.2).sub.0.6 25/-- .sup. 17.sup.i + -- 3.25 22 69 32 0.67 Notes to Table .sup.a 15 mmoles of MgCl.sub.2 in 30 ml of tetrahydrofuran, added subsequent to the addition of CrCl.sub.3, in each case. .sup.b The pressure drop is 23 to 24 bar for the quantitative hydrogenation of magnesium. .sup.c 2.0 ml of the centrifuged solution; ml H.sub.2 (20.degree. C./1 bar). .sup.d Total yield of soluble magnesium hydride (in terms of Mg) due to protolysis. .sup.e The Grignard bond occurs here in situ from magnesium and alkyl halide, added subsequent to the addition of CrCl.sub.3. .sup.f The solution is highly viscous. .sup.g Quinuclidine hydrochloride. .sup.h 2% molar of CrCl.sub.3 or anthracene (in terms of the magnesium) were employed in this case. .sup.i Comparison example without complexing agent.
EXAMPLE 18
The reaction vessel was a 250 ml two-necked cylindrical flask equipped with a magnetic stirrer, a tailkey stopcock, and stoppers, and was an appropriate glass insert for a 50 ml autoclave. 10.00 g (411 mmoles) of powdered magnesium (with a mean particle size of 0.050 mm or appr. 270 mesh) and 0.73 g (4.1 mmoles) of anthracene were added to 20 ml of absolute tetrahydrofuran. 0.05 ml of ethyl bromide were added and the suspension was stirred at room temperature. The solution turned green, and orange magnesium anthracene.tetrahydrofuran precipitated out about 20 minutes later. 0.57 g (4.5 mmoles) of anhydrous FeCl.sub.2 was added to the batch, which was simultaneously cooled (with water at 15.degree. C.) and stirred, upon which magnesium anthracene went into solution in an exothermic reaction accompanied by a color change to deep brown. The solution was then treated with, first, 40 ml of tetrahydrofuran and, second, 11.8 ml of a 1.74 molar n-octylmagnesium chloride solution in tetrahydrofuran (20.5 mmoles).
The glass vessel was placed in a flat-bottomed 500 ml stainless-steel autoclave and the suspension hydrogenated while simultaneously being powerfully agitated with the magnetic stirrer at 20.degree. C. and an initial hydrogen pressure of 60 bar. The hydrogen pressure dropped to 40 bar within 4 hours. The volume of the resulting magnesium hydride mixture was 78.5 ml. 10 ml was centrifuged for 1 hour at 10,000 rpm. 2.0 ml of the clear residual solution was subjected to pyrolysis with ethanol (cooled with water), yielding 433 ml of gas (20.degree. C. at 1 bar) composed (by MS analysis) of H.sub.2 95.3, C.sub.2 H.sub.5 OH 2.8, and THF 1.9%. The amount of H.sub.2 that formed was equivalent to a total magnesium hydride in solution of 337 mmoles or a yield of 82% soluble magnesium hydride in terms of the initial powdered magnesium. The composition of the soluble magnesium hydride is determined from the amount of n-octylmagnesium chloride employed to be (MgH.sub.2).sub.16.4.n-C.sub.8 H.sub.17 MgCl. The concentration of the tetrahydrofuran solution was 4.3 molar in terms of the soluble magnesium hydride.
EXAMPLE 19
The reaction vessel was a 250 ml two-necked cylindrical flask equipped with a magnetic stirrer, a tailkey stopcock, and stoppers, and was an appropriate glass insert for a 50 ml autoclave. 10.00 g (411 mmoles) of powdered magnesium (with a mean particle size of 0.050 mm or appr. 270 mesh) and 0.73 g (4.1 mmoles) of anthracene were added to 20 ml of absolute tetrahydrofuran. 0.05 ml of ethyl bromide were added and the suspension was stirred at room temperature. The solution turned green, and orange magnesium anthracene tetrahydrofuran precipitated out about 20 minutes later. 0.56 g (4.4 mmoles) of anhydrous FeCl.sub.2 was added to the batch, which was simultaneously cooled (with water at 15.degree. C.) and stirred, upon which magnesium anthracene went into solution in an exothermic reaction accompanied by a color change to deep brown. The solution was then treated with, first, 10 ml of tetrahydrofuran and, second, 11 ml of a 1.86 molar quinuclidine solution in tetrahydrofuran (20.5 mmoles) and 30 ml of a 0.49 molar MgCl.sub.2 solution in tetrahydrofuran (14.7 mmoles).
The glass vessel was placed in a flat-bottomed 500 ml stainless-steel autoclave and the suspension hydrogenated while simultaneously being powerfully agitated with the magnetic stirrer at 20.degree.-26.degree. C. and an initial hydrogen pressure of 60 bar. The hydrogen pressure dropped to 40 bar within 4 hours. The volume of the resulting magnesium hydride mixture was 78 ml. 10 ml was centrifuged for 1 hour at 10,000 rpm. 2.0 ml of the clear residual solution was subjected to pyrolysis with ethanol (cooled with water), yielding 462 ml of gas (20.degree. C. at 1 bar) composed (by MS analysis) of H.sub.2 96.3, C.sub.2 H.sub.5 OH 2.2, and THF 1.5%. The amount of H.sub.2 that formed was equivalent to a total magnesium hydride in solution of 361 mmoles or a yield of 88% soluble magnesium hydride in terms of the initial powdered magnesium. The composition of the soluble magnesium hydride is determined from the amount of quinuclidine employed (20.5 mmoles) to be (MgH.sub.2).sub.17.6.quinuclidine. The concentration of the tetrahydrofuran solution was 4.6 molar in terms of the soluble magnesium hydride.
EXAMPLE 20
The reaction vessel was a 250 ml two-necked cylindrical flask equipped with a magnetic stirrer, a tailkey stopcock, and stoppers, and was an appropriate glass insert for a 50 ml autoclave. 10.00 g (411 mmoles) of powdered magnesium (with a mean particle size of 0.050 mm or appr. 270 mesh) and 0.73 g (4.1 mmoles) of anthracene were added to 20 ml of absolute tetrahydrofuran. 0.05 ml of ethyl bromide were added and the suspension was stirred at room temperature. The solution turned green, and orange magnesium anthracene tetrahydrofuran precipitated out about 20 minutes later. 0.59 g (4.7 mmoles) of anhydrous MnCl.sub.2 was added to the batch, which was simultaneously cooled (with water at 15.degree. C.) and stirred, upon which magnesium anthracene went into solution in an exothermic reaction accompanied by a color change to deep brown. The solution was then treated with, first, 10 ml of tetrahydrofuran and, second, 11 ml of a 1.86 molar quinuclidine solution in tetrahydrofuran (20.5 mmoles) and 30 ml of a 0.49 molar MgCl.sub.2 solution in tetrahydrofuran (14.7 mmoles).
The glass vessel was placed in a flat-bottomed 500 ml stainless-steel autoclave and the suspension hydrogenated for 3 days while simultaneously being powerfully agitated with the magnetic stirrer at 20.degree.-25.degree. C. and an initial hydrogen pressure of 60 bar. The hydrogen pressure dropped to 40 bar within 4 hours. The volume of the resulting magnesium hydride mixture was 75 ml. 10 ml was centrifuged for 1 hour at 10,000 rpm. 2.0 ml of the clear residual solution was subjected to pyrolysis with ethanol (cooled with water), yielding 275 ml of gas (20.degree. C. at 1 bar) composed (by MS analysis) of H.sub.2 97.1, C.sub.2 H.sub.5 OH 2.0, and THF 0.9%. The amount of H.sub.2 that formed was equivalent to a total magnesium hydride in solution of 209 mmoles or a yield of 51% soluble magnesium hydride in terms of the initial powdered magnesium. The composition of the soluble magnesium hydride is determined from the amount of quinuclidine employed (20.5 mmoles) to be (MgH.sub.2).sub.10.2.quinuclidine. The concentration of the tetrahydrofuran solution was 2.8 molar in terms of the soluble magnesium hydride.
It is understood that the specification and examples are illustrative but not limitative of the present invention and that other embodiments within the spirit and scope of the invention will suggest themselves to those skilled in the art.

Number	Name	Date
4731203	Bogdanovic	Mar 1988
4835316	Corriu et al.	May 1989
5091536	Bogdanovic et al.	Feb 1992
5093046	Kober et al.	Mar 1992

	Number	Date	Country
Parent	686727	Apr 1991
Parent	153857	Feb 1988

Soluble magnesium hydrides, method of preparing them, and use thereof

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