Perruthenate
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| 2-D skeletal version of the perruthenate anion | |
| Ball-and-stick model of the perruthenate anion | |
| Identifiers | |
|---|---|
3D model (JSmol)
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| Properties | |
| RuO4- | |
| Molar mass | 165.07 g·mol−1 |
| Structure | |
| Tetrahedral | |
| Related compounds | |
Other cations
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Tetrapropylammonium perruthenate N(C3H7)4RuO4 |
Related compounds
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Ruthenium tetroxide RuO4 |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Perruthenate is an oxyanion of ruthenium in its +7 oxidation state. It is a mild oxidising agent useful in organic synthesis.[1]
Properties
Perruthenate can be considered as the partially reduced derivative of ruthenium tetroxide. It is a much milder oxidising agent than the unionised compound, but still capable of oxidising a number of compounds via its reduction to ruthenate RuO2−4.
Synthesis
Perruthenate can be produced as the sodium[2] or potassium[3] salt by reduction of ruthenium tetroxide with alkaline hydroxide:
4 RuO4 + 4 KOH → 4 KRuO4 + 2 H2O + O2
Both the concentration and temperature of the reduction must be controlled to avoid further reduction to ruthenate:[4]
4 KRuO4 + 4 KOH → 4 K2RuO4 + 2 H2O + O2
An alternative route can proceed from the oxidation of ruthenate salts by chlorine gas, .[3]
Perruthenate can also be produced in situ by the oxidation of aqueous ruthenium trichloride with sodium bromate; this method produces a dark green solution, which can be precipitated with an appropriate cation to yield the corresponding salt.[5]
Applications
Salts of perruthenate with permanently charged cations are used as catalytic reagents for the oxidation of primary and secondary alcohols to aldehydes and ketones respectively. While the perruthenate anion serves as the oxidising agent in this reaction, rather than a true catalyst, it is quickly restored by an appropriate cooxidant such as N-methylmorpholine N-oxide.[1]
Tetrapropylammonium perruthenate (TPAP) is the most widely used of these reagents, though some alternatives have been proposed which offer greater longevity and temperature stability.[6] Some notable alternate perruthenates are the triphenylphosphine derivatives, such as the salts of isoamyltriphenylphosphonium (ATP3), methyltriphenylphosphonium (MTP3), and tetraphenylphosphonium (TP3).[7]
References
- ^ a b Ley, Steven V.; Norman, Joanne; Griffith, William P.; Marsden, Stephen P. (1994). "Tetrapropylammonium Perruthenate, Pr4N+RuO4 -, TPAP: A Catalytic Oxidant for Organic Synthesis". Synthesis. 1994 (7): 639–666. doi:10.1055/s-1994-25538.
- ^ Lee, Donald G.; Congson, Ligaya N.; Spitzer, Udo A.; Olson, Merle E. (1984). "The oxidation of alcohols by sodium ruthenate". Canadian Journal of Chemistry. 62 (9): 1835–1839. doi:10.1139/v84-314.
- ^ a b Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 1082. ISBN 978-0-08-037941-8.
- ^ Lee, Donald G.; Hall, David T.; Cleland, James H. (1972). "The Oxidation of Organic Compounds by Sodium Ruthenate". Canadian Journal of Chemistry. 50 (22): 3741–3743. doi:10.1139/v72-592.
- ^ Langer, Peter (2000). "Tetra-n-propyl Ammonium Perruthenate (TPAP) - an Efficient and Selective Reagent for Oxidation Reactions in Solution and on the Solid Phase". Journal für Praktische Chemie. 342 (7): 728–730. doi:10.1002/1521-3897(200009)342:7<728::AID-PRAC728>3.0.CO;2-R.>
- ^ Moore, Peter W.; Read, Christopher D. G.; Bernhardt, Paul V.; Williams, Craig M. (2018). "ATP3 and MTP3: Easily Prepared Stable Perruthenate Salts for Oxidation Applications in Synthesis". Chemistry – A European Journal. 24 (18): 4556–4561. doi:10.1002/chem.201800531. PMID 29508453.
- ^ Dallaston, Madeleine A.; Bettencourt, Christian J.; Chow, Sharon; Gebhardt, Joshua; Spangler, Jordan; Johnston, Martin R.; Wall, Craig; Brusnahan, Jason S.; Williams, Craig M. (2019). "Ranking Oxidant Sensitiveness: A Guide for Synthetic Utility". Chemistry – A European Journal. 25 (41): 9614–9618. doi:10.1002/chem.201902036. PMID 31245899.