Tris(bipyridine)ruthenium(II) chloride

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Tris(bipyridine)ruthenium(II) chloride
Other names

Ru-bpy
Ruthenium-tris(2,2’-bipyridyl) dichloride

Identifiers
CAS number 14323-06-9 (anhydrous) YesY, 50525-27-4 (hexahydrate)

 RTECS number VM2730000
Properties
Molecular formula C30H24N6Cl2Ru·6H2O
Molar mass 640.53 g/mol (anhydrous)
748.62 g/mol (hexahydrate)
Appearance red solid
Density solid
Melting point >300 °C
Solubility in water Soluble
Structure
Molecular shape Octahedral
Dipole moment 0 D
Hazards
R-phrases none
S-phrases S22 S24/25
Main hazards mildly toxic
Related compounds
Related compounds Ruthenium trichloride
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Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
Infobox references

Tris(bipyridine)ruthenium(II) dichloride is the coordination compound with the formula [Ru(bpy)3]Cl2. This red crystalline salt is obtained as the hexahydrate, although all of the properties of interest are in the cation [Ru(bpy)3]2+, which has received much attention because of its distinctive optical properties. The chlorides can be replaced with other anions, such as PF6−.

Synthesis and structure

Structure of [Ru(bpy)3]2+

This salt is prepared by treating an aqueous solution of ruthenium trichloride with 2,2'-bipyridine. In this conversion, Ru(III) is reduced to Ru(II), and hypophosphorous acid is typically added as a reducing agent.[1] [Ru(bpy)3]2+ is an octahedral coordination complex. The complex is chiral, with D3 symmetry. It has been resolved into its enantiomers, which are kinetically stable.


Photochemistry of [Ru(bpy)3]2+

[Ru(bpy)3]2+ absorbs UV light and visible light. An aqueous solution absorbs at 452 ± 3 nm with an extinction coefficient of 14,600 M−1cm−1. Solutions of the resulting excited state have a comparatively long lifetime of 890 nanoseconds in acetonitrile[2] and 650 ns in water.[2] The excited state relaxes to the ground state by emission of a photon at the wavelength of 620 nm. The long lifetime of the excited state is attributed to the fact that it is triplet, whereas the ground state is a singlet state and in part due to the fact that the structure of the molecule allows for charge separation. Singlet-triplet transitions are forbidden and therefore often slow.

The triplet excited state has both oxidizing and reducing properties. This unusual situation arises because the excited state can be described as an Ru3+ complex containing a bpy- ligand. Thus, the photochemical properties of [Ru(bpy)3]2+ are reminiscent of the photosynthetic assembly, which also involves separation of an electron and a hole.[3]

[Ru(bpy)3]2+ has been examined as a photosensitiser for both the oxidation and reduction of water. Upon absorbing a photon, [Ru(bpy)3]2+ converts to the aforementioned triplet state, denoted [Ru(bpy)3]2+*. This species transfers an electron, located on one bpy ligand, to a sacrificial oxidant such as peroxodisulfate (S2O82-). The resulting [Ru(bpy)3]3+ is a powerful oxidant and oxidizes water into O2 and protons via a metal oxide catalyst.[4] Alternatively, the reducing power of [Ru(bpy)3]2+* can be harnessed to reduce methylviologen, a recyclable carrier of electrons, which in turn reduces protons at a platinum catalyst. For this process to be catalytic, a sacrificial reductant, such as EDTA4- or triethanolamine is provided to return the Ru(III) back to Ru(II).

Derivatives of [Ru(bpy)3]2+ are numerous.[5][6] Such complexes are widely discussed for applications in biodiagnostics, photovoltaics and organic light-emitting diode, but no derivative has been commercialized. Application of [Ru(bpy)3]2+ and its derivatives to fabrication of optical chemical sensors is arguably one of the most successful areas so far.[7]

[Ru(bpy)3]2+ and photoredox catalysis

Photoredox catalysis using combination of [Ru(bpy)3]2+ catalyst and visible light has been considered as a tool for preparative organic chemistry since the 1970s.[8] However, only a few research groups dealt with this topic until the beginning of the 21st century. Since 2008, development of this bond-forming strategy for organic synthesis has gained considerable momentum due to the seminal studies by MacMillan,[9] Yoon,[10] and Stephenson[11] groups. Depending on the choice of suitable reductive or oxidative quencher, the [Ru(bpy)3]2+ catalyst can be used to trigger photoreduction or photooxidation, respectively. Current status of this field has been recently summarized in several review articles.[8][12][13][14] It can be anticipated that photoredox reactivity of complexes based on metals other than Ru (e.g. Ir, Re, and bimetallic photocatalysts) will also be intensively explored. Additionally, transformations triggered by purely organic photoredox catalysts start to attract attention as highlighted in the recent report by Zeitler group.[15]

Safety

Metal bipyridine as well as related phenanthroline complexes are generally bioactive, as they can act as intercalating agents.

References

  1. ↑ Broomhead, J. A.; Young, C. G. “Tris(2,2’-bipyridine)Ruthenium(II) Dichloride Hexahydrate” Inorganic Syntheses, 1990, volume 28, pp. 338-340. doi:10.1002/9780470132593.ch86
  2. ↑ 2.0 2.1 Montalti, Marco; Alberto Cedi, Luca Prodi, M. Teresa Gandolfi (2006). Handbook of Photochemistry 3rd edition. 6000 Broken Sound Prkway NW, Suite 200 Boca Raton, FL: CRC press Taylor & Francis Group. pp. 379–404. ISBN 0-8247-2377-5. 
  3. ↑ A. J. Bard and M. A. Fox (1995). "Artificial Photosynthesis: Solar Splitting of Water to Hydrogen and Oxygen". Acc. Chem. Res. 28 (3): 141–145. doi:10.1021/ar00051a007. 
  4. ↑ M. Hara, C. C. Waraksa, J. T. Lean, B. A. Lewis and T. E. Mallouk (2000). "Photocatalytic Water Oxidation in a Buffered Tris(2,2'-bipyridyl)ruthenium Complex-Colloidal IrO2 System". J. Phys. Chem. A 104 (22): 5275–5280. doi:10.1021/jp000321x. 
  5. ↑ A. Juris, V. Balzani, F. Barigelletti, S. Campagna, P. Belser and A von Zelewsky (1988). "Ru(II) polypyridine complexes - photophysics, photochemistry, electrochemistry, and chemiluminescence". Coord. Chem. Rev. 84: 85–277. doi:10.1016/0010-8545(88)80032-8. 
  6. ↑ S. Campagna, F. Puntoriero, F. Nastasi, G. Bergamini and V. Balzani (2007). "Photochemistry and photophysics of coordination compounds: ruthenium". Top. Curr. Chem. Topics in Current Chemistry 280: 117–214. doi:10.1007/128_2007_133. ISBN 978-3-540-73346-1. 
  7. ↑ G. Orellana* and D. Garcia-Fresnadillo (2004). "Environmental and Industrial Optosensing with Tailored Luminescent Ru(II) Polypyridyl Complexes". Springer Ser. Chem. Sens. Biosens. 1: 309–357. doi:10.1007/978-3-662-09111-1_13. 
  8. ↑ 8.0 8.1 F. Teply (2011). "Photoredox catalysis by [Ru(bpy)3]2+ to trigger transformations of organic molecules. Organic synthesis using visible-light photocatalysis and its 20th century roots". Collect. Czech. Chem. Commun. (Free access article) 76 (7): 859–917. doi:10.1135/cccc2011078. 
  9. ↑ D. A. Nicewicz, D. W. C. MacMillan (2008). "Merging photoredox catalysis with organocatalysis: The direct asymmetric alkylation of aldehydes". Science 322 (5898): 77–80. doi:10.1126/science.1161976. 
  10. ↑ M. A. Ischay, M. E. Anzovino, J. Du, T. P. Yoon (2008). "Efficient visible light photocatalysis of [2+2] enone cycloadditions". J. Am. Chem. Soc. 130 (39): 12886–12887. doi:10.1021/ja805387f. 
  11. ↑ J. M. R. Narayanam, J. W. Tucker, C. R. J. Stephenson (2009). "Electron-transfer photoredox catalysis: Development of a tin-free reductive dehalogenation reaction". J. Am. Chem. Soc. 131 (25): 8756–8757. doi:10.1021/ja9033582. 
  12. ↑ J. M. R. Narayanam, C. R. J. Stephenson (2011). "Visible light photoredox catalysis: applications in organic synthesis". Chem. Soc. Rev. 40: 102–113. doi:10.1039/b913880n. 
  13. ↑ T. P. Yoon, M. A. Ischay, J. Du (2010). "Visible light photocatalysis as a greener approach to photochemical synthesis". Nat. Chem. 2 (7): 527–532. doi:10.1038/nchem.687. 
  14. ↑ K. Zeitler (2009). "Photoredox catalysis with visible light". Angew. Chem. Int. Ed. 48 (52): 9785–9789. doi:10.1002/anie.200904056. 
  15. ↑ M. Neumann, S. Füldner, B. König, K. Zeitler (2011). "Metal-free, cooperative asymmetric organophotoredox catalysis with visible light". Angew. Chem. Int. Ed. 50 (4): 951–954. doi:10.1002/anie.201002992. 
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