Calcium hydride

Summary

Calcium hydride
Calcium hydride
Names
IUPAC name
Calcium hydride
Other names
Calcium(II) hydride
Calcium dihydride
Hydrolith
Identifiers
  • 7789-78-8 checkY
3D model (JSmol)
  • Interactive image
ChemSpider
  • 94784 checkY
ECHA InfoCard 100.029.263 Edit this at Wikidata
EC Number
  • 232-189-2
  • 105052
UNII
  • WY779SQ0XW checkY
  • DTXSID60894886 Edit this at Wikidata
  • InChI=1S/Ca.2H/q+2;2*-1 checkY
    Key: UUGAXJGDKREHIO-UHFFFAOYSA-N checkY
  • InChI=1/Ca.2H/q+2;2*-1
    Key: UUGAXJGDKREHIO-UHFFFAOYAG
  • [H-].[H-].[Ca+2]
Properties
CaH2
Molar mass 42.094 g/mol
Appearance gray powder (white when pure)
Density 1.70 g/cm3, solid
Melting point 816 °C (1,501 °F; 1,089 K)
reacts violently
Solubility reacts in alcohol
Structure
Orthorhombic, oP12
Pnma, No. 62
Thermochemistry
41.4 J·mol−1·K−1[1]
−181.5 kJ·mol−1
-142.5 kJ/mol
Hazards
GHS labelling:
GHS07: Exclamation markGHS05: CorrosiveWater-react. 1GHS09: Environmental hazard
Danger
H260
NFPA 704 (fire diamond)
3
3
2
Related compounds
Other cations
Sodium hydride,
Potassium hydride
magnesium hydride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Calcium hydride is the chemical compound with the formula CaH2, and is therefore an alkaline earth hydride. This grey powder (white if pure, which is rare) reacts vigorously with water liberating hydrogen gas. CaH2 is thus used as a drying agent, i.e. a desiccant.[2]

CaH2 is a saline hydride, meaning that its structure is salt-like. The alkali metals and the alkaline earth metals heavier than beryllium all form saline hydrides. A well-known example is sodium hydride, which crystallizes in the NaCl motif. These species are insoluble in all solvents with which they do not react. CaH2 crystallizes in the PbCl2 (cotunnite) structure.[3]

Preparation

Calcium hydride is prepared from its elements by direct combination of calcium and hydrogen at 300 to 400 °C.[4][5]

Uses

Reduction of metal oxides

CaH2 is a reducing agent for the production of metal from the metal oxides of Ti, V, Nb, Ta, and U. It is proposed to operate via its decomposition to Ca metal:[4]

TiO2 + 2 CaH2 → Ti + 2 CaO + 2 H2

Hydrogen source

CaH2 has been used for hydrogen production. In the 1940s, it was available under the trade name "Hydrolith" as a source of hydrogen:

'The trade name for this compound is "hydrolith"; in cases of emergency, it can be used as a portable source of hydrogen, for filling airships. It is rather expensive for this use.'[6]

The reference to "emergency" probably refers to wartime use. The compound has, however, been widely used for decades as a safe and convenient means to inflate weather balloons. Likewise, it is regularly used in laboratories to produce small quantities of highly pure hydrogen for experiments. The moisture content of diesel fuel is estimated by the hydrogen evolved upon treatment with CaH2.[4]

Desiccant

The reaction of CaH2 with water can be represented as follows:

CaH2 + 2 H2O → Ca(OH)2 + 2 H2

The two hydrolysis products, gaseous H2 and Ca(OH)2, are readily separated from the dried solvent.

Calcium hydride is a relatively mild desiccant and, compared to molecular sieves, probably inefficient.[7] Its use is safer than more reactive agents such as sodium metal or sodium-potassium alloy. Calcium hydride is widely used as a desiccant for basic solvents such as amines and pyridine. It is also used to dry alcohols.[2]

Despite its convenience, CaH2 has a few drawbacks:

  • It is insoluble in all solvents with which it does not react vigorously, in contrast to LiAlH4, thus the speed of its drying action can be slow.
  • Because CaH2 and Ca(OH)2 are almost indistinguishable in appearance, the quality of a sample of CaH2 is not obvious visually.

History

During the Battle of the Atlantic, German submarines used calcium hydride as a sonar decoy called bold.[8]

See also

References

  1. ^ Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A21. ISBN 978-0-618-94690-7.
  2. ^ a b Gawley, Robert E.; Davis, Arnold (2001). "Calcium Hydride". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rc005. ISBN 0471936235.
  3. ^ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
  4. ^ a b c Rittmeyer, Peter; Wietelmann, Ulrich (2000). "Hydrides". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a13_199.
  5. ^ P. Ehrlich (1963). "Calcium Strontium and Barium Hydrides". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. 1. NY,NY: Academic Press. p. 929.
  6. ^ Adlam G.H.J. and Price L.S., A Higher School Certificate Inorganic Chemistry, John Murray, London, 1940
  7. ^ Williams, D. Bradley G.; Lawton, Michelle (2010). "Drying of Organic Solvents: Quantitative Evaluation of the Efficiency of Several Desiccants". The Journal of Organic Chemistry. 75 (24): 8351–8354. doi:10.1021/jo101589h. PMID 20945830.
  8. ^ McNeil, Ian (2002-06-01). An Encyclopedia of the History of Technology. ISBN 9781134981649.