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Rubidium permanganate
Identifiers
CAS Number	13465-49-1;
3D model (JSmol)	Interactive image;
ChemSpider	13389592;
PubChem CID	23674440;
CompTox Dashboard (EPA)	DTXSID00635477 ;
	InChI InChI=1S/Mn.4O.Rb/q;;;;-1;+1 Key: UJCOPKFKNRFWHO-UHFFFAOYSA-N;
	SMILES [Rb+].[O-][Mn](=O)(=O)=O;
Properties
Chemical formula	RbMnO4
Molar mass	204.404
Appearance	purple crystals
Density	3.325 g·cm−3
Melting point	295 °C (decomposes)
Solubility in water	10.6 g·l−1 （19 °C）
Structure
Crystal structure	orthorhombic
Space group	Pnma (Nr. 62)
Lattice constant	a = 954.11 pm, b = 573.926 pm, c = 763.63 pm
Related compounds
Other anions	rubidium perchlorate; rubidium periodate; rubidium pertechnetate
Other cations	lithium permanganate; sodium permanganate; potassium permanganate; ammonium permanganate; caesium permanganate
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references

Rubidium permanganate is the permanganate salt of rubidium, with the chemical formula RbMnO
₄.

Preparation

Rubidium permanganate can be formed by the reaction of potassium permanganate and rubidium chloride:^[4]^[5]

RbCl + KMnO₄ → KCl + RbMnO₄ ↓

Properties

Physical

Rubidium permanganate is soluble in water with a solubility of 6.03 g/L at 7 °C,^[3] 10.6 g/L at 19 °C,^[2] and 46.8 g/L at 60 °C.^[6] Its crystal structure is orthorhombic,^[1] the same as caesium permanganate, ammonium permanganate and potassium permanganate.

Chemical

Similar to potassium permanganate, the two-step decomposition of rubidium permanganate leads to the formation of rubidium manganate intermediates. It breaks down into manganese dioxide, rubidium oxide and oxygen.^[4] The decomposition temperature is between 200 and 300 °C.^[7] Drift-away oxygen caused an 8% mass loss in the product.^[7]

10RbMnO₄ → 3Rb₂MnO₄ + 7MnO₂ + 2Rb₂O + 6O₂ ↑

2Rb₂MnO₄ → 2MnO₂ + 2Rb₂O + O₂ ↑

Total reaction:

4RbMnO₄ → 4MnO₂ + 2Rb₂O + 3O₂ ↑

Uses

In qualitative analysis, rubidium permanganate is used as a reagent to detect perchlorate ions. It is produced as an intermediate from rubidium nitrate and potassium permanganate and precipitates with existing perchlorate ions as RbClO₄·RbMnO₄ mixed crystal.^[8]

References

^ ^a ^b 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, vol. 625, no. 7, pp. 1521–3749, doi:10.1002/(SICI)1521-3749(199907)625:7<1135::AID-ZAAC1135>3.0.CO;2-L{{citation}}: CS1 maint: multiple names: authors list (link)
^ ^a ^b ^c Dale L. Perry, Sidney L. Phillips: Handbook of inorganic compounds. CRC Press, 1995, ISBN 978-0-8493-8671-8, S. 336 ([1], p. 336, at Google Books).
^ ^a ^b Aterton Seidell (1940), Solubilities of Organic Compounds, vol. 1, p. 1438
^ ^a ^b Michael W. Beck, Michael E. Brown (1983), "Thermal analysis of antimony/potassium permanganate pyrotechnic compositions" (PDF), Thermochimica Acta, vol. 65, no. 2–3, pp. 197–212, doi:10.1016/0040-6031(83)80022-7, archived from the original (PDF) on 2013-10-29
^ P. J. Herley, E. G. Prout (1960), "The Thermal Decomposition of Rubidium Permanganate", The Journal of Physical Chemistry, vol. 64, no. 5, pp. 675–677, doi:10.1021/j100834a503
^ Austin M. Patterson (1906), "Solubilities of Permanganates of the Alkali Metals", Journal of the American Chemical Society, vol. 28, no. 12, pp. 1734–1736, doi:10.1021/ja01978a009
^ ^a ^b Z. Gontarz, B. Pisarska (September 1990), "Thermal decomposition stages of potassium, rubidium and caesium permanganates", Journal of Thermal Analysis and Calorimetry, vol. 36, no. 6, pp. 2113–2117, doi:10.1007/BF01914135, S2CID 95763664
^ E. Gerdes (2001), Qualitative anorganische Analyse (Ein Begleiter für Theorie und Praxis) (2 ed.), Springer, p. 139, ISBN 978-3-540-67875-5

[Hoppe-1] 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, vol. 625, no. 7, pp. 1521–3749, doi:10.1002/(SICI)1521-3749(199907)625:7<1135::AID-ZAAC1135>3.0.CO;2-L{{citation}}: CS1 maint: multiple names: authors list (link)

[Perry-2] Dale L. Perry, Sidney L. Phillips: Handbook of inorganic compounds. CRC Press, 1995, ISBN 978-0-8493-8671-8, S. 336 ([1], p. 336, at Google Books).

[Seidell-3] Aterton Seidell (1940), Solubilities of Organic Compounds, vol. 1, p. 1438

[Beck-4] Michael W. Beck, Michael E. Brown (1983), "Thermal analysis of antimony/potassium permanganate pyrotechnic compositions" (PDF), Thermochimica Acta, vol. 65, no. 2–3, pp. 197–212, doi:10.1016/0040-6031(83)80022-7, archived from the original (PDF) on 2013-10-29

[Herley-5] P. J. Herley, E. G. Prout (1960), "The Thermal Decomposition of Rubidium Permanganate", The Journal of Physical Chemistry, vol. 64, no. 5, pp. 675–677, doi:10.1021/j100834a503

[Patterson-6] Austin M. Patterson (1906), "Solubilities of Permanganates of the Alkali Metals", Journal of the American Chemical Society, vol. 28, no. 12, pp. 1734–1736, doi:10.1021/ja01978a009

[Gontarz-7] Z. Gontarz, B. Pisarska (September 1990), "Thermal decomposition stages of potassium, rubidium and caesium permanganates", Journal of Thermal Analysis and Calorimetry, vol. 36, no. 6, pp. 2113–2117, doi:10.1007/BF01914135, S2CID 95763664

[Gerdes-8] E. Gerdes (2001), Qualitative anorganische Analyse (Ein Begleiter für Theorie und Praxis) (2 ed.), Springer, p. 139, ISBN 978-3-540-67875-5

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