Magnesium hydride
Chemical compound From Wikipedia, the free encyclopedia
Magnesium hydride is the chemical compound with the molecular formula MgH2. It contains 7.66% by weight of hydrogen and has been studied as a potential hydrogen storage medium.[2]
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| Names | |
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| IUPAC name
Magnesium hydride | |
| Identifiers | |
3D model (JSmol) |
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.028.824 |
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PubChem CID |
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| Properties | |
| MgH2 | |
| Molar mass | 26.3209 g/mol |
| Appearance | white crystals |
| Density | 1.45 g/cm3 |
| Melting point | 327 °C (621 °F; 600 K) decomposes |
| decomposes | |
| Solubility | insoluble in ether |
| Structure | |
| tetragonal | |
| Thermochemistry | |
Heat capacity (C) |
35.4 J/mol K |
Std molar entropy (S⦵298) |
31.1 J/mol K |
Std enthalpy of formation (ΔfH⦵298) |
−75.2 kJ/mol |
Gibbs free energy (ΔfG⦵) |
−35.9 kJ/mol |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards |
pyrophoric[1] |
| Related compounds | |
Other cations |
Beryllium hydride Calcium hydride Strontium hydride Barium hydride |
| Magnesium monohydride Mg4H6 | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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For comparison, one cubic meter can contain 45 kg of hydrogen pressurized at 700 atm, 70 kg of liquid hydrogen, or up to 106 kg of hydrogen bound in magnesium hydride.[3]
Magnesium hydride is also investigated for use in thermobaric weapons and incendiary weapons, standalone or as a mixture with a solid oxidizer; China tested a (non-nuclear) "hydrogen bomb" using the substance.[4] It can be also used in emulsion explosives as a source of bubbles and additional fuel.[5] It can be added to improve heat release of aluminized explosive compositions and to improve burn rate of propellants.[6][7]
Preparation
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 MgI2 catalyst:[8]
- Mg + H2 → MgH2
Lower temperature production from Mg and H2 using nanocrystalline Mg produced in ball mills has been investigated.[9] Other preparations include:
- the hydrogenation of magnesium anthracene under mild conditions:[10]
- Mg(anthracene) + H2 → MgH2
- the reaction of diethylmagnesium with lithium aluminium hydride[11]
- product of complexed MgH2 e.g. MgH2.THF by the reaction of phenylsilane and dibutyl magnesium in ether or hydrocarbon solvents in the presence of THF or TMEDA as ligand.[1]
Structure and bonding
The room temperature form α-MgH2 has a rutile structure.[12] There are at least four high pressure forms: γ-MgH2 with α-PbO2 structure,[13] cubic β-MgH2 with Pa-3 space group,[14] orthorhombic HP1 with Pbc21 space group and orthorhombic HP2 with Pnma space group.[15] Additionally a non stoichiometric MgH(2-δ) has been characterised, but this appears to exist only for very small particles[16]
(bulk MgH2 is essentially stoichiometric, as it can only accommodate very low concentrations of H vacancies[17]).
The bonding in the rutile form is sometimes described as being partially covalent in nature rather than purely ionic;[18] charge density determination by synchrotron x-ray diffraction indicates that the magnesium atom is fully ionised and spherical in shape and the hydride ion is elongated.[19] Molecular forms of magnesium hydride, MgH, MgH2, Mg2H, Mg2H2, Mg2H3, and Mg2H4 molecules identified by their vibrational spectra have been found in matrix isolated samples at below 10 K, formed following laser ablation of magnesium in the presence of hydrogen.[20] The Mg2H4 molecule has a bridged structure analogous to dimeric aluminium hydride, Al2H6.[20]
Reactions
MgH2 readily reacts with water to form hydrogen gas:
- MgH2 + 2 H2O → 2 H2 + Mg(OH)2
At 287 °C it decomposes to produce H2 at 1 bar pressure.[21] The high temperature required is seen as a limitation in the use of MgH2 as a reversible hydrogen storage medium:[22]
- MgH2 → Mg + H2
References
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