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Magnesium hydride

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"Magnesium dihydride" redirects here. Not to be confused with magnesium monohydride.
Magnesium hydride
Names
IUPAC name
Magnesium hydride
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.028.824 Edit this at Wikidata
EC Number
  • 231-705-3
  • InChI=1S/Mg.2H checkY
    Key: RSHAOIXHUHAZPM-UHFFFAOYSA-N checkY
  • InChI=1/Mg.2H/rH2Mg/h1H2
    Key: RSHAOIXHUHAZPM-HZAFDXBCAG
  • [MgH2]
Properties
MgH2
Molar mass 26.3209 g/mol
Appearance white crystals
Density 1.45 g/cm3
Melting point 285 °C (545 °F; 558 K) decomposes
decomposes
Solubility insoluble in ether
Structure
tetragonal
Thermochemistry
35.4 J/mol K
31.1 J/mol K
-75.2 kJ/mol
-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).
checkY verify (what is checkY☒N ?)

Magnesium hydride is the chemical compound MgH2, making it an alkaline earth hydride. It contains 7.66% by weight of hydrogen and has been studied as a potential hydrogen storage medium.[2]

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:[3]

Mg + H2 → MgH2

Lower temperature production from Mg and H2 using nano crystalline Mg produced in ball mills has been investigated.[4] Other preparations include:

  • the hydrogenation of magnesium anthracene under mild conditions:[5]
Mg(anthracene) + H2 → MgH2

Structure and bonding

The room temperature form α-MgH2 has a rutile structure, which is similar to TiO2[7] There are at least four high pressure forms: γ-MgH2 with α-PbO2 structure, cubic β-MgH2 with Pa-3 space group, orthorhombic HP1 with Pbc21 space group and orthorhombic HP2 with Pnma space grouAdditionally a non stoichiometricetric MgH(2-δ) has been characterised, but this appears to exist only for very small particles[8]
(bulk MgH2 is essentially stoichiometric, as it can only accommodate very low concentrations of H vacancies[9]).

The bonding in the rutile form is sometimes described as being partially covalent in nature rather than purely ionic;[10] 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.[11] 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.[12] The Mg2H4 molecule has a bridged structure analogous to dimeric aluminium hydride, Al2H6.[12]

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,[13] the high temperature required is seen as a limitation in the use of MgH2 as a reversible hydrogen storage medium:[14]

MgH2 → Mg + H2

Potential use for hydrogen storage

Its potential as a reversible "storage" medium for hydrogen has led to interest in improving the hydrogenation and dehydrogenation reaction kinetics.[14][15] This can be partially achieved by doping or by reducing the particle size using ball milling.[16][17][18] An alternative approach under investigation is the production of a pumpable slurry of MgH2 which is safe to handle and releases H2 by reaction with water, with reprocessing of the Mg(OH)2 into MgH2.[1] An application (yet to be examined) for a US Patent (US 2010/0163434 A1) [2] has been made in respect of a hydrogen energy storage system using laser excitation to assist desorption of hydrogen gas from magnesium hydride.

References

  1. ^ a b Synthesis of magnesium hydride by the reaction of phenylsilane and dibutylmagnesium , Michalczyk M.J., Organometallics; (1992); 11(6); 2307-2309. doi:10.1021/om00042a055
  2. ^ Catalytic Synthesis of Organolithium and Organomagnesium Compounds and of Lithium and Magnesium Hydrides - Applications in Organic Synthesis and Hydrogen Storage, Bogdanovic B., Angewandte Chemie International Edition in English, 24, 4, 262–73, doi:10.1002/anie.198502621
  3. ^ "Synthese von Magnesiumhydrid aus den Elementen (Synthesis of Magnesium Hydride from the Elements)" (PDF). Zeitschrift für Naturforschung B. 6b: 394. 1951. {{cite journal}}: Unknown parameter |authors= ignored (help)
  4. ^ Nanocrystalline magnesium for hydrogen storage, A Zaluska, L Zaluski, JO Ström–Olsen, Journal of Alloys and Compounds, 288, 1-2, 1999, 217-225, doi:10.1016/S0925-8388(99)00073-0
  5. ^ Catalytic Synthesis of Magnesium Hydride under Mild Conditions, Bogdanovic B., Liao S-T, Schwickardi M, Sikorsky P., Spliethoff B., Angewandte Chemie International Edition in English, 19,(1980), 10, 818 – 819, doi:10.1002/anie.198008181
  6. ^ The Preparation of the Hydrides of Zinc, Cadmium, Beryllium, Magnesium and Lithium by the Use of Lithium Aluminum Hydride, Barbaras G.D., Dillard C., Finholt A. E., Wartik T, Wilzbach K. E., Schlesinger H. I., J. Am. Chem. Soc.; 1951; 73(10); 4585-4590, doi:10.1021/ja01154a025
  7. ^ Neutron diffraction study of magnesium deuteride, Zachariasen W.H., Holley C.E, Stamper J.F. Jnr, Acta Crystallogr. (1963) 16, 352-353, doi:10.1107/S0365110X63000967
  8. ^ Hydrogen Cycling of Niobium and Vanadium Catalyzed Nanostructured Magnesium,Schimmel, H. G.; Huot, J.; Chapon, L. C.; Tichelaar, F. D.; Mulder, F. M.,J. Am. Chem. Soc.; (Article); 2005; 127(41); 14348-14354. doi:10.1021/ja051508a
  9. ^ Grau-Crespo, R.; K. C. Smith; T. S. Fisher; N. H. de Leeuw; U. V. Waghmare (2009). "Thermodynamics of hydrogen vacancies in MgH2 from first-principles calculations and grand-canonical statistical mechanics". Physical Review B. 80 (17): 174117. doi:10.1103/PhysRevB.80.174117.
  10. ^ Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, ISBN 0-471-19957-5
  11. ^ Charge density measurement in MgH2 by synchrotron X-ray diffraction, T. Noritake, S. Towata, M. Aoki, Y. Seno, Y. Hirose, E. Nishibori, M. Takata and M. Sakata, Journal of Alloys and Compounds, 356-357, (2003), 84-86, doi:10.1016/S0925-8388(03)00104-X
  12. ^ a b Infrared Spectra of Magnesium Hydride Molecules, Complexes, and Solid Magnesium Dihydride, Xuefeng Wang and Lester Andrews, J. Phys. Chem. A, 108 (52), 11511 -11520, 2004. doi:10.1021/jp046410h
  13. ^ McAuliffe, T. R. (1980). Hydrogen and Energy (illustrated ed.). Springer. p. 65. ISBN 978-1-349-02635-7. Extract of page 65
  14. ^ a b Hydrogen-storage materials for mobile applications, L. Schlapbach and A. Züttel, Nature 414, 353 (2001).doi:10.1038/35104634 https://web.archive.org/web/20050115181834/http://www.iea.org/textbase/work/2003/linking/Schlapbach%20Paper.PDF. Archived from the original (PDF) on January 15, 2005. Retrieved August 9, 2008. {{cite web}}: Missing or empty |title= (help); Unknown parameter |deadurl= ignored (|url-status= suggested) (help)
  15. ^ J Huot Hydrogen in Metals (2002) in New Trends in Intercalation Compounds for Energy Storage, Christian Julien, J. P. Pereira-Ramos, A. Momchilov, Springer, ISBN 1-4020-0594-6
  16. ^ Sakintuna, B.; F. Lamaridarkrim; M. Hirscher (2007). "Metal hydride materials for solid hydrogen storage: A review". International Journal of Hydrogen Energy. 32: 1121–1140. doi:10.1016/j.ijhydene.2006.11.022.
  17. ^ Smith, Kyle; Fisher, Timothy; Waghmare, Umesh; Grau-Crespo, Ricardo (2010). "Dopant-vacancy binding effects in Li-doped magnesium hydride". Physical Review B. 82 (13). doi:10.1103/PhysRevB.82.134109. ISSN 1098-0121.
  18. ^ Liang, G.; Huot, J.; Boily, S.; Van Neste, A.; Schulz, R. (1999). "Catalytic effect of transition metals on hydrogen sorption in nanocrystalline ball milled MgH2–Tm (Tm=Ti, V, Mn, Fe and Ni) systems". Journal of Alloys and Compounds. 292 (1–2): 247–252. doi:10.1016/S0925-8388(99)00442-9. ISSN 0925-8388.
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