Chemistry:Caesium hydride
 Caesium cation, Cs+ Hydrogen anion, H− | |
| Names | |
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| IUPAC name
Caesium hydride
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| Other names
Cesium hydride
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
PubChem CID
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| Properties[1] | |
| CsH | |
| Molar mass | 133.913 g·mol−1 |
| Appearance | White cubic crystals |
| Density | 3.42 g/cm3 |
| Melting point | 528 °C (982 °F; 801 K) |
| reacts | |
| Structure | |
| Face centered cubic | |
| Octahedral | |
| Thermochemistry[1] | |
Std enthalpy of
formation (ΔfH⦵298) |
−54.2 kJ⋅mol−1 |
Enthalpy of fusion (ΔfH⦵fus)
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15 kJ⋅mol−1 |
| Related compounds | |
Other anions
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Other cations
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
Caesium hydride or cesium hydride is an inorganic compound of caesium and hydrogen with the chemical formula CsH. It is an alkali metal hydride. It was the first substance to be created by light-induced particle formation in metal vapor, and showed promise in early studies of an ion propulsion system using caesium.[2][3] It is the most reactive stable alkaline metal hydride. It is a powerful superbase and reacts with water extremely vigorously.
The caesium nucleus in CsH can be hyperpolarized through interactions with an optically pumped caesium vapor in a process known as spin-exchange optical pumping (SEOP). SEOP can increase the nuclear magnetic resonance (NMR) signal of caesium nucleus by an order of magnitude.[4]
It is very difficult to make caesium hydride in a pure form. Caesium hydride can be produced by heating caesium carbonate and metallic magnesium in hydrogen at 580 to 620 °C (1,076 to 1,148 °F).[5]
Crystal structure
At room temperature and atmospheric pressure, CsH has the same structure as NaCl.[citation needed]
References
- ↑ 1.0 1.1 Template:RubberBible97th
- ↑ Tam, A.; Moe, G.; Happer, W. (1975). "Particle Formation by Resonant Laser Light in Alkali-Metal Vapor". Phys. Rev. Lett. 35 (24): 1630–33. doi:10.1103/PhysRevLett.35.1630. Bibcode: 1975PhRvL..35.1630T.
- ↑ Burkhart, J. A.; Smith, F. J. (November 1963). "Application of dynamic programming to optimizing the orbital control process of a 24-hour communications satellite". https://ntrs.nasa.gov/search.jsp?R=543868&id=2&qs=N%3D4294965816.
- ↑ Ishikawa, K.; Patton, B.; Jau, Y.-Y.; Happer, W. (2007). "Spin Transfer from an Optically Pumped Alkali Vapor to a Solid". Phys. Rev. Lett. 98 (18). doi:10.1103/PhysRevLett.98.183004. PMID 17501572. Bibcode: 2007PhRvL..98r3004I. https://zenodo.org/record/1059117.
- ↑ A. Jamieson Walker (1924). A Text Book Of Inorganic Chemistry Volume I The Alkali Metals And Their Congeners. https://archive.org/details/in.ernet.dli.2015.153684.
| Alkali metal (Group 1) hydrides |  Lithium hydride, LiH ionic metal hydride   Beryllium hydride Left (gas phase): BeH2 covalent metal hydride Right: (BeH2)n (solid phase) polymeric metal hydride   Borane and diborane Left: BH3 (special conditions), covalent metalloid hydride Right: B2H6 (standard conditions), dimeric metalloid hydride  Methane, CH4 covalent nonmetal hydride  Ammonia, NH3 covalent nonmetal hydride  Water, H2O covalent nonmetal hydride  Hydrogen fluoride, HF covalent nonmetal hydride | ||||||||||||||||||
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| Alkaline (Group 2) earth hydrides |
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| Group 13 hydrides |
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| Group 14 hydrides |
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| Pnictogen (Group 15) hydrides |
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| Hydrogen chalcogenides (Group 16 hydrides) |
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| Hydrogen halides (Group 17 hydrides) | |||||||||||||||||||
| Transition metal hydrides | |||||||||||||||||||
| Lanthanide hydrides |
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| Actinide hydrides |
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