Chemistry:Caesium permanganate
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| File:Crystals CsMnO4.png | |
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Other names
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3D model (JSmol)
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| Properties | |
| CsMnO4 | |
| Molar mass | 251.8406 |
| Appearance | purple powder, bronze crystals[1] |
| Density | 3.6[1] |
| Melting point | 200-300 °C (decomposes) |
| 2.3 g·l−1 (19 °C)[2] | |
| Structure | |
| orthorhombic | |
| Pnma (Nr. 62) | |
a = 1006 pm, b = 580.1 pm, c = 794.4 pm
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| Related compounds | |
Other anions
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caesium perchlorate caesium periodate caesium pertechnetate |
Other cations
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lithium permanganate sodium permanganate potassium permanganate rubidium permanganate ammonium permanganate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Caesium permanganate is the permanganate salt of caesium, with the chemical formula CsMnO
4.
Preparation
Caesium permanganate can be formed by the reaction of potassium permanganate and caesium chloride in aqueous solution, followed by concentrating the solution.[1]
- CsCl + KMnO
4 → KCl + CsMnO
4
Properties
Physical
It solubility in water is low: 0.97 g/L at 1 °C,[2] 2.3 g/L at 19 °C, and 12.5 g/L at 59 °C.[3] Its crystal structure is orthorhombic,[4] the same as rubidium permanganate, ammonium permanganate and potassium permanganate.
Thermal degradation
Similar to the behavior of potassium permanganate, the two-step decomposition of caesium permanganate leads to caesium manganate, which further breaks down into manganese dioxide, caesium oxide, and oxygen.[5] The decomposition temperature is between 200 and 300 °C.[6] Drift-away oxygen caused an 8% mass loss in the product.[6]
- 10CsMnO
4 → 3Cs
2MnO
4 + 7MnO
2 + 2Cs
2O + 6O
2 - 2Cs
2MnO
4 → 2MnO
2 + 2Cs
2O + O
2
Total reaction:
- 4CsMnO
4 → 4MnO
2 + 2Cs
2O + 3O
2
Further reading
- Fanning, James C. (1995). "The Solubilities of the Alkali Metal Salts and the Precipitation of Cs+ from Aqueous Solution". Coordination Chemistry Reviews 140: 27–36. doi:10.1016/0010-8545(94)01123-S.
References
- ↑ 1.0 1.1 1.2 R. Hoppe, D. Fischer, J. Schneider (1999), "Zur Kenntnis von Oxyden A[MO4]: Über LiMnO4, KMnO4, RbMnO4, CsMnO4 sowie RbIO4 und CsIO4. (– Was heißt eigentlich "Die Kristallstruktur von …"? –)", Zeitschrift für anorganische und allgemeine Chemie 625 (7): 1521–3749, doi:10.1002/(SICI)1521-3749(199907)625:7<1135::AID-ZAAC1135>3.0.CO;2-L
- ↑ 2.0 2.1 Aterton Seidell (1940), Solubilities of Organic Compounds, 1, pp. 1438, http://www.archive.org/stream/solubilitiesofor023311mbp#page/n933/mode/2up%20Volltext
- ↑ Austin M. Patterson (1906), "Solubilities of Permanganates of the Alkali Metals", Journal of the American Chemical Society 28 (12): 1734–1736, doi:10.1021/ja01978a009, https://zenodo.org/record/1428880
- ↑ Groth, P. (Paul) (1877). Zeitschrift für Krystallographie und Mineralogie. New York Public Library. Leipzig : Wilhelm Engelmann. http://archive.org/details/zeitschriftfrkr19grotgoog.
- ↑ Beck, Michael W.; Brown, Michael E. (Jul 1983). "Thermal analysis of antimony/potassium permanganate pyrotechnic compositions" (in en). Thermochimica Acta 65 (2–3): 197–212. doi:10.1016/0040-6031(83)80022-7. https://linkinghub.elsevier.com/retrieve/pii/0040603183800227.
- ↑ 6.0 6.1 Z. Gontarz, B. Pisarska (September 1990), "Thermal decomposition stages of potassium, rubidium and caesium permanganates", Journal of Thermal Analysis and Calorimetry 36 (6): 2113–2117, doi:10.1007/BF01914135
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