Ruthenium tetroxide

Ruthenium(VIII) oxide  |  |

|

Names
IUPAC name

Ruthenium(VIII) oxide

Identifiers

CAS Number

* 20427-56-9 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 106401

EC Number |

* 243-813-8

PubChem CID

* 119079

UNII |

* 97E960G9RP Y

InChI

* InChI=1S/4O.Ru

Key: GJFMDWMEOCWXGJ-UHFFFAOYSA-N

SMILES

* O=[Ru](=O)(=O)=O

Properties

Chemical formula

| RuO4
Molar mass | 165.07 g/mol
Appearance  | yellow easily melting solid
Odor | pungent ozone like
Density | 3.29 g/cm3
Melting point |  25.5[1] °C (77.9 °F; 298.6 K)
Boiling point |  129.6[2] °C (265.3 °F; 402.8 K)

Solubility in water

| 2% w/v at 20 °C
Solubility in other solvents  | Soluble in
Carbon tetrachloride
Chloroform
Structure

Molecular shape

| tetrahedral

Dipole moment

| zero
Hazards
GHS pictograms |
GHS Signal word | Danger

GHS hazard statements

| HH271Script error: No such module "Preview warning".Category:GHS errors, HH319Script error: No such module "Preview warning".Category:GHS errors

GHS precautionary statements

| PP210Script error: No such module "Preview warning".Category:GHS errors, PP220Script error: No such module "Preview warning".Category:GHS errors, PP264+P265Script error: No such module "Preview warning".Category:GHS errors, PP280Script error: No such module "Preview warning".Category:GHS errors, PP283Script error: No such module "Preview warning".Category:GHS errors, PP305+P351+P338Script error: No such module "Preview warning".Category:GHS errors, PP306+P360Script error: No such module "Preview warning".Category:GHS errors, PP337+P317Script error: No such module "Preview warning".Category:GHS errors, PP370+P378Script error: No such module "Preview warning".Category:GHS errors, PP371+P380+P375Script error: No such module "Preview warning".Category:GHS errors, PP420Script error: No such module "Preview warning".Category:GHS errors, PP501Script error: No such module "Preview warning".Category:GHS errors
NFPA 704 (fire diamond)  |

Related compounds

Related compounds

| Ruthenium dioxide
Ruthenium trichloride
Osmium tetroxide

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Y verify (what is YN ?)
Infobox references

Ruthenium tetroxide is the inorganic compound with the formula RuO4. It is a yellow volatile solid that melts near room temperature.[4] It has the odor of ozone.[5] Samples are typically black due to impurities. The analogous OsO4 is more widely used and better known. One of the few solvents in which RuO4 forms stable solutions is CCl4.[6]

## Contents

* 1 Preparation
* 2 Structure
* 3 Uses
* 3.1 Isolation of ruthenium from ores
* 3.2 Organic chemistry
* 3.3 Other uses
* 4 Gaseous release by nuclear accidents
* 5 References
* 6 Further reading

## Preparation

RuO4 is prepared by oxidation of ruthenium(III) chloride with NaIO4.[4] The reaction initially produces sodium diperiodo­dihydroxo­ruthenate(VI), which then decomposes in acid solution to the tetroxide:[7]

2 Ru3+(aq) + 5 IO4−(aq) + 3 H2O(l) → 2 RuO4(s) + 5 IO3−(aq) + 6 H+(aq)[8]

Due to its challenging reactivity, RuO4 is always generated in situ and used in catalytic quantities, at least in organic reactions.[6]

## Structure

RuO4 forms two crystal structures, one with cubic symmetry and another with monoclinic symmetry, isotypic to OsO4. The molecule adopts a tetrahedral geometry, with the Ru–O distances ranging from 169 to 170 pm.[9]

## Uses

### Isolation of ruthenium from ores

The main commercial value of RuO4 is as an intermediate in the production of ruthenium compounds and metal from ores. Like other platinum group metals (PGMs), ruthenium occurs at low concentrations and often mixed with other PGMs. Together with OsO4, it is separated from other PGMs by distillation of a chlorine-oxidized extract. Ruthenium is separated from OsO4 by reducing RuO4 with hydrochloric acid, a process that exploits the highly positive reduction potential for the [RuO4]0/- couple.[10][11]

### Organic chemistry

RuO4 is of specialized value in organic chemistry because it oxidizes virtually any hydrocarbon.[12] For example, it will oxidize adamantane to 1-adamantanol. Because it is such an aggressive oxidant, reaction conditions must be mild, generally room temperature. Although a strong oxidant, RuO4 oxidations do not perturb stereocenters that are not oxidized. Illustrative is the oxidation of the following diol to a carboxylic acid:

Oxidation of epoxy alcohols also occurs without degradation of the epoxide ring:

Under milder conditions, oxidative reaction yields aldehydes instead. RuO4 readily converts secondary alcohols into ketones. Although similar results can be achieved with other cheaper oxidants such as PCC\- or DMSO-based oxidants, RuO4 is ideal when a very vigorous oxidant is needed, but mild conditions must be maintained. It is used in organic synthesis to oxidize internal alkynes to 1,2-diketones, and terminal alkynes along with primary alcohols to carboxylic acids. When used in this fashion, the ruthenium(VIII) oxide is used in catalytic amounts and regenerated by the addition of sodium periodate to ruthenium(III) chloride and a solvent mixture of acetonitrile, water and carbon tetrachloride. RuO4 readily cleaves double bonds to yield carbonyl products, in a manner similar to ozonolysis. OsO4, a more familiar oxidant that is structurally similar to RuO4, does not cleave double bonds, instead producing vicinal diol products. However, with short reaction times and carefully controlled conditions, RuO4 can also be used for dihydroxylation.[13]

Because RuO4 degrades the "double bonds" of arenes (especially electron-rich ones) by dihydroxylation and cleavage of the C-C bond in a way few other reagents can, it is useful as a "deprotection" reagent for carboxylic acids that are masked as aryl groups (typically phenyl or p-methoxyphenyl). Because the fragments formed are themselves readily oxidizable by RuO4, a substantial fraction of the arene carbon atoms undergo exhaustive oxidation to form carbon dioxide. Consequently, multiple equivalents of the terminal oxidant (often in excess of 10 equivalents per aryl ring) are required to achieve complete conversion to the carboxylic acid, limiting the practicality of the transformation.[14][15][16]

Although used as a direct oxidant, due to the relatively high cost of RuO4 it is also used catalytically with a cooxidant. For an oxidation of cyclic alcohols with RuO4 as a catalyst and bromate as oxidant under basic conditions, RuO4 is first activated by hydroxide, turning into the hyperruthenate anion:[17]

RuO4 \+ OH− → HRuO5−

The reaction proceeds via a glycolate complex.

### Other uses

Ruthenium tetroxide is a potential staining agent. It is used to expose latent fingerprints by turning to the brown/black ruthenium dioxide when in contact with fatty oils or fats contained in sebaceous contaminants of the print.[18]

## Gaseous release by nuclear accidents

Because of the very high volatility of ruthenium tetroxide (RuO4) ruthenium radioactive isotopes with their relative short half-life are considered as the second most hazardous gaseous isotopes after iodine-131 in case of release by a nuclear accident.[19][5][20] The two most important radioactive isotopes of ruthenium are 103Ru and 106Ru. They have half-lives of 39.6 days and 373.6 days, respectively.[5]

## References

1. ↑ Nuta, Ioana; Virot, Francois; Fischer, Evelyne; Chatillon, Christian (March 2023). "Thermodynamic assessment of RuO4 oxide". Calphad 80: 1-2. doi:10.1016/j.calphad.2022.102508.
2. ↑ Koda, Yoshio (1986). "Boiling Points and Ideal Solutions of Ruthenium and Osmium Tetraoxides". Journal of the Chemical Society, Chemical Communications 1986 (17): 1347–1348. doi:10.1039/C39860001347.
3. ↑ PubChem. "Ruthenium tetroxide" (in en). https://pubchem.ncbi.nlm.nih.gov/compound/119079.
4. ↑ 4.0 4.1 H. L. Grube (1963). "Ruthenium (VIII) Oxide". in G. Brauer. Handbook of Preparative Inorganic Chemistry, 2nd Ed.. 1. NY: Academic Press. pp. 1599–1600.
5. ↑ 5.0 5.1 5.2 Backman, U., Lipponen, M., Auvinen, A., Jokiniemi, J., & Zilliacus, R. (2004). Ruthenium behaviour in severe nuclear accident conditions. Final report (No. NKS–100). Nordisk Kernesikkerhedsforskning.
6. ↑ 6.0 6.1 Martín, V. S.; Palazón, J. M.; Rodríguez, C. M.; Nevill, C. R. (2006). "Ruthenium(VIII) Oxide". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rr009.pub2. ISBN 978-0471936237.
7. ↑ Mercer, E. E.; Meyer, S. M. (1972). "A periodate complex of ruthenium(VI)". J. Inorg. Nucl. Chem. (Great Britain: Pergamon) 34 (2): 777–778. doi:10.1016/0022-1902(72)80466-4.
8. ↑ Verma, P. K.; Gujar, R. B.; Mohapatra, P. K.; Sharpless (2018). "An efficient method for radio-ruthenium separation from acidic feeds: Extraction, transport and spectroscopic studies." (in en). Journal of Environmental Chemical Engineering 6 (5): 5830-5836. doi:10.1016/j.jece.2018.08.062. ISSN 22133437. https://doi.org/10.1016/j.jece.2018.08.062.
9. ↑ Pley, M.; Wickleder, M. S. (2005). "Two Crystalline Modifications of RuO4". Journal of Solid State Chemistry 178 (10): 3206–3209. doi:10.1016/j.jssc.2005.07.021. Bibcode: 2005JSSCh.178.3206P.
10. ↑ Bernardis, Francesco L.; Grant, Richard A.; Sherrington, David C. (2005). "A review of methods of separation of the platinum-group metals through their chloro-complexes". Reactive and Functional Polymers 65 (3): 205–217. doi:10.1016/j.reactfunctpolym.2005.05.011.
11. ↑ Swain, P.; Mallika, C.; Srinivasan, R.; Mudali, U. K.; Natarajan, R. (2013). "Separation and recovery of ruthenium: a review". Journal of Radioanalytical and Nuclear Chemistry 298 (2): 781–796. doi:10.1007/s10967-013-2536-5.
12. ↑ Vincenzo, Piccialli (2014). "Ruthenium Tetroxide and Perruthenate Chemistry. Recent Advances and Related Transformations Mediated by Other Transition Metal Oxo-species". Molecules 19 (5): 6534–6582. doi:10.3390/molecules19056534. PMID 24853716.
13. ↑ Plietker, Bernd (2005). "Selectivity versus reactivity - recent advances in RuO4-catalyzed oxidations". Synthesis 5 (15): 2453–2472. doi:10.1055/s-2005-872172.
14. ↑ Nunez, M. Teresa; Martin, Victor S. (March 1990). "Efficient oxidation of phenyl groups to carboxylic acids with ruthenium tetraoxide. A simple synthesis of (R)-.gamma.-caprolactone, the pheromone of Trogoderma granarium". The Journal of Organic Chemistry 55 (6): 1928–1932. doi:10.1021/jo00293a044. ISSN 0022-3263.
15. ↑ Nasr, Khaled; Pannier, Nadine; Frangioni, John V.; Maison, Wolfgang (February 2008). "Rigid Multivalent Scaffolds Based on Adamantane". The Journal of Organic Chemistry 73 (3): 1056–1060. doi:10.1021/jo702310g. ISSN 0022-3263. PMID 18179237.
16. ↑ Mander, Lewis N.; Williams, Craig M. (2003-02-17). "Oxidative degradation of benzene rings". Tetrahedron 59 (8): 1105–1136. doi:10.1016/S0040-4020(02)01492-8. ISSN 0040-4020.
17. ↑ Singh, Ashok K.; Singh, Amar; Gupta, Ranjana; Saxena, Madhu; Singh, Bharat (1992-01-01). "Mechanism of ruthenium tetroxide-catalysed oxidation of aldoses by alkaline N-bromoacetamide". Transition Metal Chemistry 17 (5): 413–416. doi:10.1007/BF02910720. https://www.academia.edu/87381764.
18. ↑ Mashiko, K.; Miyamoto, T. (1998). "Latent Fingerprint Processing by the Ruthenium Tetroxide Method". Journal of Forensic Identification 48 (3): 279–290. doi:10.3408/jasti.2.21. https://www.ncjrs.gov/App/publications/abstract.aspx?ID=172645.
19. ↑ Ronneau, C.; Cara, J.; Rimski-Korsakov, A. (1995). "Oxidation-enhanced emission of ruthenium from nuclear fuel". Journal of Environmental Radioactivity 26: 63–70. doi:10.1016/0265-931X(95)91633-F. https://doi.org/10.1016/0265-931X(95)91633-F.
20. ↑ Beuzet, Emilie; Lamy, Jean-Sylvestre; Perron, Hadrien; Simoni, Eric; Ducros, Gérard (2012). "Ruthenium release modelling in air and steam atmospheres under severe accident conditions using the MAAP4 code". Nuclear Engineering and Design 246: 157–162. doi:10.1016/j.nucengdes.2011.08.025.

## Further reading

* Cotton, S.A. (1997). Chemistry of Precious Metals. London: Chapman and Hall. ISBN 978-0-7514-0413-5.
* Farmer, V.; Welton, T. (2002). "The oxidation of alcohols in substituted imidazolium ionic liquids using ruthenium catalysts". Green Chemistry 4 (2): 97. doi:10.1039/B109851A.
* Singh, B.; Srivastava, S. (1991). "Kinetics and mechanism of ruthenium tetroxide catalysed oxidation of cyclic alcohols by bromate in a base". Transition Metal Chemistry 16 (4): 466. doi:10.1007/BF01129466.
* Courtney, J.L.; Swansbor, K.F. (1972). "Ruthenium tetroxide oxidation". Reviews of Pure and Applied Chemistry 22: 47.

* v
* t
* e

Ruthenium compounds

Ru(0)|

* Ru3(CO)12
* Ru(P(C6H5)3)3(CO)2

Ru(I)|

* (C5(C6H5)4O)2H(Ru(CO)2)2H

Ru(II)|

* RuB2
* Na4Ru(N2C12H6(C6H4SO3)2)3
* (Ru((NC5H4)2)3)Cl2
* Ru(P(C6H5)3)3Cl2
* Ru(SO(CH3)2)4Cl2
* (RuCl2C6H4CH3CH(CH3)2)2
* RuClC5H5(P(C6H5)3)2
* C43H72Cl2P2Ru
* (C5H5)2Ru

Ru(III)|

* RuCl3

Ru(IV)|

* RuO2
* Sr2RuO4

Ru(V)|

* RuF5

Ru(VI)|

* RuF6

Ru(VII)|

* N(C3H7)4RuO4

Ru(VIII)|

* RuO4

* v
* t
* e

Oxides

Mixed oxidation states|

* Antimony tetroxide (Sb2O4)
* Cobalt(II,III) oxide (Co3O4)
* Europium(II,III) oxide (Eu3O4)
* Iron(II,III) oxide (Fe<sub>3O4)
* Lead(II,IV) oxide (Pb3O4)
* Manganese(II,III) oxide (Mn3O4)
* Silver(I,III) oxide (Ag2O2)
* Triuranium octoxide (U3O8)
* Carbon suboxide (C3O2)
* Mellitic anhydride (C12O9)
* [[Chemistry:Praseodymium(III,IV) Praseodymium(III,IV) oxide]] (Pr6O11)
* Terbium(III,IV) oxide (Tb4O7)

+1 oxidation state|

* Copper(I) oxide (Cu<sub>2O)
* Caesium oxide (Cs2O)
* Dicarbon monoxide (C2O)
* Dichlorine monoxide (Cl2O)
* Gallium(I) oxide (Ga2O)
* Lithium oxide (Li2O)
* Potassium oxide (K2O)
* Rubidium oxide (Rb2O)
* Silver oxide (Ag2O)
* Thallium(I) oxide (Tl2O)
* Sodium oxide (Na2O)
* Water (hydrogen oxide) (H2O)

+2 oxidation state|

* Aluminium(II) oxide (AlO)
* Barium oxide (BaO)
* Beryllium oxide (BeO)
* Cadmium oxide (CdO)
* Calcium oxide (CaO)
* Carbon monoxide (CO)
* Chromium(II) oxide (CrO)
* Cobalt(II) oxide (CoO)
* Copper(II) oxide (CuO)
* Europium(II) oxide (EuO)
* Germanium monoxide (GeO))
* Iron(II) oxide (FeO)
* Lead(II) oxide (PbO)
* Magnesium oxide (MgO)
* Manganese(II) oxide (MnO)
* Mercury(II) oxide (HgO)
* Nickel(II) oxide (NiO)
* Nitric oxide (NO)
* Palladium(II) oxide (PdO)
* Silicon monoxide (SiO)
* Strontium oxide (SrO)
* Sulfur monoxide (SO)
* Disulfur dioxide (S2O2)
* Thorium monoxide (ThO)
* Tin(II) oxide (SnO)
* Titanium(II) oxide (TiO)
* Vanadium(II) oxide (VO)
* Zinc oxide (ZnO)

+3 oxidation state|

* Aluminium oxide (Al<sub>2O3)
* Antimony trioxide (Sb2O3)
* Arsenic trioxide (As2O3)
* Bismuth(III) oxide (Bi2O3)
* Boron trioxide (B2O3)
* Cerium(III) oxide (Ce2O3)
* Dibromine trioxide (Br2O3)
* Chromium(III) oxide (Cr2O3)
* Dinitrogen trioxide (N2O3)
* Dysprosium(III) oxide (Dy2O3)
* Erbium(III) oxide (Er2O3)
* Europium(III) oxide (Eu2O3)
* Gadolinium(III) oxide (Gd2O3)
* Gallium(III) oxide (Ga2O3)
* Holmium(III) oxide (Ho2O3)
* Indium(III) oxide (In<sub>2O3)
* Iron(III) oxide (Fe2O3)
* Lanthanum oxide (La2O3)
* Lutetium(III) oxide (Lu2O3)
* Manganese(III) oxide (Mn2O3)
* Neodymium(III) oxide (Nd2O3)
* Nickel(III) oxide (Ni2O3)
* Phosphorus trioxide (P4O6)
* Praseodymium(III) oxide (Pr2O3)
* Promethium(III) oxide (Pm2O3)
* Rhodium(III) oxide (Rh2O3)
* [[Chemistry:Samarium(III) Samarium(III) oxide]] (Sm2O3)
* Scandium oxide (Sc2O3)
* Terbium(III) oxide (Tb2O3)
* Thallium(III) oxide (Tl2O3)
* Thulium(III) oxide (Tm2O3)
* Titanium(III) oxide (Ti2O3)
* Tungsten(III) oxide (W2O3)
* Vanadium(III) oxide (V2O3)
* Ytterbium(III) oxide (Yb2O3)
* Yttrium(III) oxide (Y2O3)

+4 oxidation state|

* Americium dioxide (AmO2)
* Carbon dioxide (CO2)
* Carbon trioxide (CO3)
* Cerium(IV) oxide (CeO2)
* Chlorine dioxide (ClO2)
* Chromium(IV) oxide (CrO<sub>2)
* Dinitrogen tetroxide (N2O4)
* Germanium dioxide (GeO<sub>2)
* [[Chemistry:Hafnium(IV) Hafnium(IV) oxide]] (HfO2)
* Lead dioxide (PbO2)
* Manganese dioxide (MnO2)
* Neptunium(IV) oxide (NpO2)
* Nitrogen dioxide (NO2)
* Osmium dioxide (OsO2)
* Plutonium(IV) oxide (PuO2)
* Praseodymium(IV) oxide (PrO2)
* Protactinium(IV) oxide (PaO2)
* Rhodium(IV) oxide (RhO2)
* Ruthenium(IV) oxide (RuO<sub>2)
* Selenium dioxide (SeO2)
* Silicon dioxide (SiO2)
* Sulfur dioxide (SO2)
* Tellurium dioxide (TeO<sub>2)
* [[Chemistry:Terbium(IV) Terbium(IV) oxide]] (TbO2)
* Thorium dioxide (ThO2)
* Tin dioxide (SnO2)
* Titanium dioxide (TiO<sub>2)
* Tungsten(IV) oxide (WO2)
* Uranium dioxide (UO2)
* Vanadium(IV) oxide (VO2)
* Zirconium dioxide (ZrO2)

+5 oxidation state|

* Antimony pentoxide (Sb2O5)
* Arsenic pentoxide (As2O5)
* Dinitrogen pentoxide (N2O5)
* Niobium pentoxide (Nb2O5)
* Phosphorus pentoxide (P2O5)
* Protactinium(V) oxide (Pa2O5)
* Tantalum pentoxide (Ta2O5)
* Vanadium(V) oxide (V2O5)

+6 oxidation state|

* Chromium trioxide (CrO3)
* Molybdenum trioxide (MoO3)
* Rhenium trioxide (ReO3)
* Selenium trioxide (SeO3)
* Sulfur trioxide (SO3)
* Tellurium trioxide (TeO3)
* Tungsten trioxide (WO3)
* Uranium trioxide (UO3)
* Xenon trioxide (XeO3)
* Iridium trioxide (IrO3)

+7 oxidation state|

* Dichlorine heptoxide (Cl2O7)
* Manganese heptoxide (Mn2O7)
* [[Chemistry:Rhenium(VII) Rhenium(VII) oxide]] (Re2O7)
* Technetium(VII) oxide (Tc2O7)

+8 oxidation state|

* Osmium tetroxide (OsO4)
* Ruthenium tetroxide (RuO4)
* Xenon tetroxide (XeO4)
* Iridium tetroxide (IrO4)
* Hassium tetroxide (HsO4)

Related|

* Oxocarbon
* Suboxide
* Oxyanion
* Ozonide
* Peroxide
* Superoxide

Oxides are sorted by oxidation state. Category:Oxides

0.00

(0 votes)

Original source: https://en.wikipedia.org/wiki/Ruthenium tetroxide. Read more

|

Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:Ruthenium_tetroxide&oldid=4437644"
*[CID]: Compound ID
*[v]: View this template
*[t]: Discuss this template
*[e]: Edit this template