Rubidium permanganate

Last updated
Rubidium permanganate
Caesiumpermanganat.png
Identifiers
3D model (JSmol)
ChemSpider
PubChem CID
  • InChI=1S/Mn.4O.Rb/q;;;;-1;+1
    Key: UJCOPKFKNRFWHO-UHFFFAOYSA-N
  • [Rb+].[O-][Mn](=O)(=O)=O
Properties
RbMnO4
Molar mass 204.404
Appearancepurple crystals [1]
Density 3.325 g·cm−3 [2]
Melting point 295 °C (decomposes) [2]
10.6 g·l−1 （19 °C） [3]
Structure
orthorhombic
Pnma (Nr. 62)
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).

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

Contents

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]

Related Research Articles

<span class="mw-page-title-main">Oxidizing agent</span> Chemical compound used to oxidize another substance in a chemical reaction

An oxidizing agent is a substance in a redox chemical reaction that gains or "accepts"/"receives" an electron from a reducing agent. In other words, an oxidizer is any substance that oxidizes another substance. The oxidation state, which describes the degree of loss of electrons, of the oxidizer decreases while that of the reductant increases; this is expressed by saying that oxidizers "undergo reduction" and "are reduced" while reducers "undergo oxidation" and "are oxidized". Common oxidizing agents are oxygen, hydrogen peroxide, and the halogens.

<span class="mw-page-title-main">Potassium permanganate</span> Chemical compound

Potassium permanganate is an inorganic compound with the chemical formula KMnO4. It is a purplish-black crystalline salt, which dissolves in water as K+ and MnO−
4 ions to give an intensely pink to purple solution.

Cuprates are a class of compounds that contain copper (Cu) atom(s) in an anion. They can be broadly categorized into two main types:

<span class="mw-page-title-main">Permanganate</span> Chemical compound

A permanganate is a chemical compound with the manganate(VII) ion, MnO−
4, the conjugate base of permanganic acid. Because the manganese atom has a +7 oxidation state, the permanganate(VII) ion is a strong oxidising agent. The ion is a transition metal ion with a tetrahedral structure. Permanganate solutions are purple in colour and are stable in neutral or slightly alkaline media. The exact chemical reaction depends on the carbon-containing reactants present and the oxidant used. For example, trichloroethane (C2H3Cl3) is oxidised by permanganate ions to form carbon dioxide (CO2), manganese dioxide (MnO2), hydrogen ions (H+), and chloride ions (Cl−).

<span class="mw-page-title-main">Sodium perchlorate</span> Chemical compound

Sodium perchlorate is an inorganic compound with the chemical formula NaClO4. It consists of sodium cations Na+ and perchlorate anions ClO−4. It is a white crystalline, hygroscopic solid that is highly soluble in water and ethanol. It is usually encountered as sodium perchlorate monohydrate NaClO4·H2O. The compound is noteworthy as the most water-soluble of the common perchlorate salts.

<span class="mw-page-title-main">Caesium perchlorate</span> Chemical compound

Caesium perchlorate or cesium perchlorate (CsClO4), is a perchlorate of caesium. It forms white crystals, which are sparingly soluble in cold water and ethanol. It dissolves more easily in hot water.

<span class="mw-page-title-main">Rubidium perchlorate</span> Chemical compound

Rubidium perchlorate, RbClO4, is the perchlorate of rubidium. It is an oxidizing agent, as are all perchlorates.

<span class="mw-page-title-main">Sodium oxalate</span> Chemical compound

Sodium oxalate, or disodium oxalate, is a chemical compound with the chemical formula Na2C2O4. It is the sodium salt of oxalic acid. It contains sodium cations Na+ and oxalate anions C2O2−4. It is a white, crystalline, odorless solid, that decomposes above 290 °C.

<span class="mw-page-title-main">Potassium manganate</span> Chemical compound

Potassium manganate is the inorganic compound with the formula K2MnO4. This green-colored salt is an intermediate in the industrial synthesis of potassium permanganate, a common chemical. Occasionally, potassium manganate and potassium permanganate are confused, but each compound's properties are distinct.

Potassium hypomanganate is the inorganic compound with the formula K3MnO4. Also known as potassium manganate(V), this bright blue solid is a rare example of a salt with the hypomanganate or manganate(V) anion, where the manganese atom is in the +5 oxidation state. It is an intermediate in the production of potassium permanganate and the industrially most important Mn(V) compound.

<span class="mw-page-title-main">Sodium permanganate</span> Chemical compound

Sodium permanganate is the inorganic compound with the formula NaMnO4. It is closely related to the more commonly encountered potassium permanganate, but it is generally less desirable, because it is more expensive to produce. It is mainly available as the monohydrate. This salt absorbs water from the atmosphere and has a low melting point. Being about 15 times more soluble than KMnO4, sodium permanganate finds some applications where very high concentrations of MnO4− are sought.

<span class="mw-page-title-main">Manganese(IV) fluoride</span> Chemical compound

Manganese tetrafluoride, MnF4, is the highest fluoride of manganese. It is a powerful oxidizing agent and is used as a means of purifying elemental fluorine.

<span class="mw-page-title-main">Ammonium permanganate</span> Chemical compound

Ammonium permanganate is the chemical compound NH4MnO4, or NH3·HMnO4. It is a water soluble, violet-brown or dark purple salt.

Barium permanganate is a chemical compound, with the formula Ba(MnO4)2. It forms violet to brown crystals that are sparingly soluble in water.

Perchloratoborate is an anion of the form [B(ClO4)4]−. It can form partly stable solid salts with heavy alkali metals. They are more stable than nitratoborate salts. K[B(ClO4)4] decomposes at 35 °C, Rb[B(ClO4)4] is stable to 50 °C, and Cs[B(ClO4)4] can exist up to 80 °C.

<span class="mw-page-title-main">Chemical chameleon</span>

The chemical chameleon is a redox reaction, well known from classroom demonstrations, that exploits the dramatic color changes associated with the various oxidation states of manganese.

<span class="mw-page-title-main">Rubidium oxalate</span> Chemical compound

Rubidium oxalate is a chemical compound with the chemical formula Rb2C2O4. It is a rubidium salt of oxalic acid. It consists of rubidium cations Rb+ and oxalate anions C2O2−4. Rubidium oxalate forms a monohydrate Rb2C2O4·H2O.

<span class="mw-page-title-main">Rubidium triiodide</span> Chemical compound

Rubidium triiodide is an inorganic compound with the chemical formula RbI3. It is composed of Rb+ and I−
3.

<span class="mw-page-title-main">Caesium permanganate</span> Chemical compound

Caesium permanganate is the permanganate salt of caesium, with the chemical formula CsMnO4.

References

  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 , 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)
  2. 1 2 3 Dale L. Perry, Sidney L. Phillips: Handbook of inorganic compounds. CRC Press, 1995, ISBN 978-0-8493-8671-8, S. 336 ( , p. 336, at Google Books).
  3. 1 2 Aterton Seidell (1940), Solubilities of Organic Compounds, vol. 1, p. 1438
  4. 1 2 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
  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
  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
  7. 1 2 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
  8. ↑ E. Gerdes (2001), Qualitative anorganische Analyse (Ein Begleiter für Theorie und Praxis) (2 ed.), Springer, p. 139, ISBN   978-3-540-67875-5
This page is based on this Wikipedia article
Text is available under the CC BY-SA 4.0 license; additional terms may apply.
Images, videos and audio are available under their respective licenses.