Calcium hydride
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| Names | |
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| IUPAC name
Calcium hydride
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| Other names
Calcium(II) hydride
Calcium dihydride |
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| Identifiers | |
7789-78-8  |
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| ChemSpider | 94784 |
| EC Number | 232-189-2 |
| Jmol 3D model | Interactive image |
| PubChem | 105052 |
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| 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 | |
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Std molar
entropy (S |
41.4 J·mol−1·K−1[1] |
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Std enthalpy of
formation (ΔfH |
−181.5 kJ·mol−1 |
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Gibbs free energy (ΔfG˚)
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-142.5 kJ/mol |
| Vapor pressure | {{{value}}} |
| Related compounds | |
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Other cations
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Sodium hydride, Potassium hydride |
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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. 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 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]
Contents
Preparation
Calcium hydride is prepared from its elements by direct combination of calcium and hydrogen at 300 to 400 °C.[4]
Uses
Reduction of metal oxides
CaH2 is a reducing agent for the production of metal powders from the 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"[5] 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, H2, a gas 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.
See also
References
- ↑ Lua error in package.lua at line 80: module 'strict' not found.
- ↑ 2.0 2.1 Gawley, R. E., Davis, A., "Calcium Hydride," in Encyclopedia of Reagents for Organic Synthesis, 2001, John Wiley & Sons, Ltd. doi:10.1002/047084289X.rc005
- ↑ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
- ↑ 4.0 4.1 4.2 Peter Rittmeyer, Ulrich Wietelmann “Hydrides” in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a13_199
- ↑ Hydrolith in thefreedictionary.com
- ↑ Adlam G.H.J. and Price L.S., A Higher School Certificate Inorganic Chemistry, John Murray, London, 1940
- ↑ Williams, D. B. G., Lawton, M., "Drying of Organic Solvents: Quantitative Evaluation of the Efficiency of Several Desiccants", The Journal of Organic Chemistry 2010, vol. 75, 8351. doi: 10.1021/jo101589h
