Photochemical reduction of carbon dioxide

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Photochemical reduction of carbon dioxide harnesses solar energy to convert CO2 into higher-energy products. Environmental interest in producing artificial systems is motivated by recognition that CO2 is a greenhouse gas. The process has not been commercialized.


Photochemical reduction involves chemical reduction (redox) generated from the photoexcitation of another molecule, called a photosensitizer. To harness the sun's energy, the photosensitizer must be able to absorb light within the visible and ultraviolet spectrum. [1] Molecular sensitizers that meet this criterion often include a metal center, as the d-orbital splitting in organometallic species often falls within the energy range of far-UV and visible light. The reduction process begins with excitation of the photosensitizer, as mentioned. This causes the movement of an electron from the metal center into the functional ligands. This movement is termed a metal-to-ligand charge transfer (MLCT). Back-electron transfer from the ligands to the metal after the charge transfer, which yields no net result, is prevented by including an electron-donating species in solution. Successful photosensitizers have a long-lived excited state, usually due to the interconversion from singlet to triplet states, that allow time for electron donors to interact with the metal center. [2] Common donors in photochemical reduction include triethylamine (TEA), triethanolamine (TEOA), and 1-benzyl-1,4-dihydronicotinamide (BNAH).

An example of photoexcitation using Ru(bpy)3 and triethylamine. The net result is a lone electron, originating from the metal, residing in the aromatic bipyridine moiety of Ru(bpy)3.

After excitation, CO2 coordinates or otherwise interacts with the inner coordination sphere of the reduced metal. Common products include formic acid, carbon monoxide, and methanol. Note that light absorption and catalytic reduction may occur at the same metal center or on different metal centers. That is, a photosensitizer and catalyst may be tethered through an organic linkage that provides for electronic communication between the species. In this case, the two metal centers form a bimetallic supramolecular complex. And, the excited electron that had resided on the functional ligands of photosensitizer passes through the ancillary ligands to the catalytic center, which becomes a one-electron reduced (OER) species. The advantage of dividing the two processes among different centers is in the ability to tune each center for a particular task, whether through selecting different metals or ligands.

An example of a supramolecular complex capable of photochemical reduction. Notice the photosensitizer on left tethered to the catalytic complex on the right. [3]


In the 1980s, Lehn observed that Co(I) species were produced in solutions containing CoCl2, 2,2'-bipyridine (bpy), a tertiary amine, and a Ru(bpy)3Cl2 photosensitizer. The high affinity of CO2 to cobalt centers led both him and Ziessel to study cobalt centers as electrocatalysts for reduction. In 1982, they reported CO and H2 as products from the irradiation of a solution containing 700ml of CO2, Ru(bpy)3 and Co(bpy).[4]

Since the work of Lehn and Ziessel, several catalysts have been paired with the Ru(bpy)3 photosensitizer.[5] When paired with methylviologen, cobalt, and nickel-based catalysts, carbon monoxide and hydrogen gas are observed as products. Paired with rhenium catalysts, carbon monoxide is observed as the major product, and with ruthenium catalysts formic acid is observed. Some product selection is attainable through tuning of the reaction environment. Other photosensitizers have also been employed as catalysts. They include FeTPP (TPP=5,10,15,20-tetraphenyl-21H,23H-porphine) and CoTPP, both of which produce CO while the latter produces formate also. Non-metal photocatalysts include pyridine and N-heterocyclic carbenes. [6] [7]

A reaction scheme for the catalytic reduction of CO2 by Re(bpy)CO3Cl. CT is an abbreviation for Charge-Transfer. [8]

See also[edit]


  1. ^ Crabtree, R.-H.; “The Organometallic Chemistry of the Transition Metals, 4th ed.” John Wiley & Sons: New York, 2005. ISBN 978-0-471-66256-3
  2. ^ Whitten, David G (1980). "Photoinduced Electron-Transfer Reactions of Metal Complexes in Solution". Accounts of Chemical Research. 13 (3): 83–90. doi:10.1021/ar50147a004.
  3. ^ Gholamkhass, Bobak; Mametsuka, Hiroaki; Koike, Kazuhide; Tanabe, Toyoaki; Furue, Masaoki; Ishitani, Osamu (2005). "Architecture of Supramolecular Metal Complexes for Photocatalytic CO2 Reduction: Ruthenium-Rhenium Bi- and Tetranuclear Complexes". Inorganic Chemistry. 44 (7): 2326–2336. doi:10.1021/ic048779r. PMID 15792468.
  4. ^ Lehn, Jean-Marie; Ziessel, Raymond (1982). "Photochemical Generation of Carbon-Monoxide and Hydrogen by Reduction of Carbon-Dioxide and Water Under Visible-Light Irradiation". Proceedings of the National Academy of Sciences USA. 79 (2): 701–704. Bibcode:1982PNAS...79..701L. doi:10.1073/pnas.79.2.701. PMC 345815. PMID 16593151.
  5. ^ Fujita, Etsuko (1999). "Photochemical carbon dioxide reduction with metal complexes". Coordination Chemistry Reviews. 185–186: 373–384. doi:10.1016/S0010-8545(99)00023-5.
  6. ^ Cole, Emily; Lakkaraju,Prasad; Rampulla,David; Morris, Amanda; Abelev, Esta; Bocarsly, Andrew (2010). "Using a One-Electron Shuttle for the Multielectron of CO2 to Methanol: Kinetic, Mechanistic, and Structural Insights". Journal of the American Chemical Society. 132 (33): 11539–11551. doi:10.1021/ja1023496. PMID 20666494.
  7. ^ Huang, Fang; Lu,Gang; Zhao,Lili; Wang,Zhi-Xiang (2010). "The Catalytic Role of N-Heterocyclic Carbene in a Metal-Free Conversion of Carbon Dioxide into Methanol: A Computational Mechanism Study". Journal of the American Chemical Society. 132 (35): 12388–12396. doi:10.1021/ja103531z. PMID 20707349.
  8. ^ Hawecker, Jeannot; Lehn,Jean-Marie; Ziessel, Raymond (1983). "Efficient Photochemical Reduction of CO2 to CO by Visible-Light Irradiation of Systems Containing Re(bipy)(CO)3X or Ru(bipy)32+-Co2+ Combinations as Homogeneous Catalysts". Journal of the Chemical Society, Chemical Communications. 9 (9): 536–538. doi:10.1039/c39830000536.