MgH2 contains 7.66% by weight of hydrogen and has
been studied as a potential hydrogen-storage medium. It
was discovered in 1912, during the pyrolysis of ethyl
magnesium iodide (a Grignard reagent), which produced
small amount of MgH2. In 1951, preparation from the
elements was first reported involving direct hydrogenation
of Mg metal at high pressure and temperature (200 atmospheres, 500°C)with magnesium iodide as a catalyst:
Mg＋H2→MgH2
Lower temperature production from Mg and H2
using nano-crystalline Mg produced in ball mills has
been investigated. Other preparations include:
1. The hydrogenation of magnesium anthracene under
mild conditions:
Mg(anthracene)＋H2→MgH2＋C14H10
2. The reaction of diethyl magnesium with LiAlH4
3. An adduct of complexed MgH2, e.g. MgH2·THF by
the reaction of phenylsilane (C6H8Si) and dibutyl
magnesium in ether or hydrocarbon solvents in the
presence of THF (C4H8O) using TMEDA
(Tetramethylethylenediamine＝(CH3)2NCH2CH2N
(CH3)2) as a ligand.
Pure magnesium hydride is a white, nonvolatile powder. Although its properties are predominantly salt-like, it shows signs of a transition towards the covalent polymeric hydride structure of compounds such as beryllium and aluminum hydride. Magnesium hydride decomposes without melting at 280 ℃. Its reactivity depends on the method of preparation. The product obtained by direct synthesis from the elements is stable in air. Nevertheless, if it is prepared by pyrolysis of dialkyl magnesium or by reaction of lithium aluminum hydride with dimethyl magnesium, the product is very pure and finely divided and ignites spontaneously on contact with air.
Magnesium hydride contains a high
proportion of hydrogen (7.65 wt %), which can
be liberated by heat. The catalytically produced
compound displays rapid rates of hydrogenation
and dehydrogenation and it is therefore of interest as a hydrogen reservoir. The high activity
of catalytically produced magnesium hydride
also enables it to take part in an addition reaction
with 1-alkenes to form organomagnesium compounds:
MgH2+2 CH2 = CHR→Mg（CH2CH2R）2
These dialkylmagnesium compounds have
become industrially important in the production
of very active Ziegler catalysts.
The Mg – H2 system can also be used for the
simultaneous removal and purification of pure
hydrogen from gas mixtures. Magnesium
hydride is also used as a drying agent for organic
solvents and gases and in chemical syntheses.
Magnesium hydride is synthesized industrially from the elements at 300 – 400 ℃ and 10 – 15 MPa hydrogen pressure in a rotary autoclave provided with steel grinding balls:
Mg+H2→MgH2
The commercial product is gray due to the presence of impurities, being about 97 % pure (Ventron). Less drastic reaction conditions are required when a homogeneous catalyst is used. The hydrogenation can be carried out at 60 – 70 ℃and 8 MPa in THF in the presence of halides of chromium, titanium, or iron and magnesium – anthracene complex. In contrast to the product from an uncatalyzed synthesis, this has a high specific surface area (90 m2 /g compared with 0.5 m2 /g), and is very reactive and pyrophoric.
Magnesium hydride is a white crystalline solid. Magnesium hydride reacts violently with water and may ignite upon contact with air. Magnesium hydride is used to make other chemicals.
Highly flammable. Pyrophoric, ignites spontaneously in air and forms magnesium oxide and water [Merck 11th ed. 1989]. Reacts with water to form caustic solution of magnesium hydroxide and hydrogen gas (H2) and heat sufficient to ignite the evolved hydrogen [Merck 11th ed. 1989].
Hydrides, such as Magnesium hydride, are reducing agents and react rapidly and dangerously with oxygen and with other oxidizing agents, even weak ones. Thus, they are likely to ignite on contact with alcohols. Hydrides are incompatible with acids, alcohols, amines, and aldehydes.
Inhalation or contact with vapors, substance or decomposition products may cause severe injury or death. May produce corrosive solutions on contact with water. Fire will produce irritating, corrosive and/or toxic gases. Runoff from fire control may cause pollution.
Produce flammable gases on contact with water. May ignite on contact with water or moist air. Some react vigorously or explosively on contact with water. May be ignited by heat, sparks or flames. May re-ignite after fire is extinguished. Some are transported in highly flammable liquids. Runoff may create fire or explosion hazard.
Used in hydrogen production and in
production of magnesium alcoholates.
If this chemical gets into the eyes, remove anycontact lenses at once and irrigate immediately for at least15 min, occasionally lifting upper and lower lids. Seek medical attention immediately. If this chemical contacts theskin, remove contaminated clothing and wash immediatelywith soap and water. Seek medical attention immediately. Ifthis chemical has been inhaled, remove from exposure,begin rescue breathing (using universal precautions, including resuscitation mask) if breathing has stopped and CPR ifheart action has stopped. Transfer promptly to a medicalfacility. When this chemical has been swallowed, get medical attention. Give large quantities of water and inducevomiting. Do not make an unconscious person vomit.
Color Code—Red Stripe: Flammability Hazard:Store separately from all other flammable materials. Storeunder nitrogen in tightly closed containers in cool (decomposes .250℃), well-ventilated area. Keep containers dry atall times. Magnesium hydride reacts violently with water,releasing caustic material, heat, and flammable gas. Sourcesof ignition, such as smoking and open flames, are prohibited where magnesium hydride is handled, used, or stored.
UN2010 Magnesium hydride, Hazard Class: 4.3;
Labels: 4.3-Dangerous when wet material.
A strong reducing agent. Pyrophoric:
the powder or dust may ignite spontaneously in air, or
in the presence of moisture. Contact with water or steam
forms magnesium hydroxide, flammable hydrogen gas,
and enough heat to ignite the hydrogen. Violent reaction
with oxidizers, alcohols, halogens, chlorinated solvents.
Incompatible with strong acids, acid chlorides, alcohols,
amines and aldehydes. Store under nitrogen. Decomposes
@ 280C in high vacuum
