Electrosynthesis

Electrosynthesis in chemistry is the synthesis of chemical compounds in an electrochemical cell.[1][2][3][4] Compared to ordinary redox reaction, electrosynthesis sometimes offers improved selectivity and yields. Electrosynthesis is actively studied as a science and also has industrial applications. Electro-oxidation has potential for wastewater treatment as well.

Experimental setupEdit

The basic setup in electrosynthesis is a galvanic cell, a potentiostat and two electrodes. Typical solvent and electrolyte combinations minimizes electrical resistance.[5] Protic conditions often use alcohol-water or dioxane-water solvent mixtures with an electrolyte such as a soluble salt, acid or base. Aprotic conditions often use an organic solvent such as acetonitrile or dichloromethane with electrolytes such as lithium perchlorate or tetrabutylammonium salts. The choice of electrodes with respect to their composition and surface area can be decisive.[6] For example, in aqueous conditions the competing reactions in the cell are the formation of oxygen at the anode and hydrogen at the cathode. In this case a graphite anode and lead cathode could be used effectively because of their high overpotentials for oxygen and hydrogen formation respectively. Many other materials can be used as electrodes. Other examples include platinum, magnesium, mercury (as a liquid pool in the reactor), stainless steel or reticulated vitreous carbon. Some reactions use a sacrificial electrode that is consumed during the reaction like zinc or lead. Cell designs can be undivided cell or divided cell type. In divided cells the cathode and anode chambers are separated with a semiporous membrane. Common membrane materials include sintered glass, porous porcelain, polytetrafluoroethene or polypropylene. The purpose of the divided cell is to permit the diffusion of ions while restricting the flow of the products and reactants. This separation simplifies workup. An example of a reaction requiring a divided cell is the reduction of nitrobenzene to phenylhydroxylamine, where the latter chemical is susceptible to oxidation at the anode.

ReactionsEdit

Organic oxidations take place at the anode. Compounds are reduced at the cathode. Radical intermediates are often invoked. The initial reaction takes place at the surface of the electrode and then the intermediates diffuse into the solution where they participate in secondary reactions.

The yield of an electrosynthesis is expressed both in terms the chemical yield and current efficiency. Current efficiency is the ratio of Coulombs consumed in forming the products to the total number of Coulombs passed through the cell. Side reactions decrease the current efficiency.

The potential drop between the electrodes determines the rate constant of the reaction. Electrosynthesis is carried out with either constant potential or constant current. The reason one chooses one over the other is due to a trade off of ease of experimental conditions versus current efficiency. Constant potential uses current more efficiently because the current in the cell decreases with time due to the depletion of the substrate around the working electrode (stirring is usually necessary to decrease the diffusion layer around the electrode). This is not the case under constant current conditions however. Instead as the substrate's concentration decreases the potential across the cell increases in order to maintain the fixed reaction rate. This consumes current in side reactions produced outside the target voltage.

Anodic oxidationsEdit

  • A well-known electrosynthesis is the Kolbe electrolysis, in which two carboxylic acids decarboxylate, and the remaining structures bond together:
 
  • A variation is called the non-Kolbe reaction when a heteroatom (nitrogen or oxygen) is present at the α-position. The intermediate oxonium ion is trapped by a nucleophile, usually solvent.
 
  • Anodic electrosynthesis oxidize primary aliphatic amine to nitrile.[7]
  • Amides can be oxidized to N-acyliminium ions, which can be captured by various nucleophiles, for example:
 
This reaction type is called a Shono oxidation. An example is the α-methoxylation of N-carbomethoxypyrrolidine[8]
 

Cathodic reductionsEdit

 
 
 

and the reduction of 2-methoxynaphthalene:

 
 
 
  • Cathodic reduction of a nitroalkene can give the oxime in good yield. At higher negative reduction potentials, the nitroalkene can be reduced further, giving the primary amine but with lower yield.[16]
 
 
2 CH2=CHCN + 2 e + 2 H+ → NCCH2CH2CH2CH2CN
 
HCO
3
+ H
2
O
+ 2eHCO
2
+ 2OH

or

CO
2
+ H
2
O
+ 2eHCO
2
+ OH

If the feed is CO
2
and oxygen is evolved at the anode, the total reaction is:

CO
2
+ OH
HCO
2
+ 1/2 O2

RedoxEdit

ElectrofluorinationEdit

In organofluorine chemistry, many perfluorinated compounds are prepared by electrochemical synthesis, which is conducted in liquid HF at voltages near 5–6 V using Ni anodes. The method was invented in the 1930s.[25] Amines, alcohols, carboxylic acids, and sulfonic acids are converted to the perfluorinated derivatives using this technology. A solution or suspension of the hydrocarbon in hydrogen fluoride is electrolyzed at 5–6 V to produce high yields of the perfluorinated product.

See alsoEdit

External linksEdit

  • Electrochemistry Encyclopedia Link

ReferencesEdit

  1. ^ Sperry, Jeffrey B.; Wright, Dennis L. (2006). "The application of cathodic reductions and anodic oxidations in the synthesis of complex molecules". Chem. Soc. Rev. 35 (7): 605–621. doi:10.1039/b512308a. PMID 16791332.
  2. ^ Topics in current chemistry. Electrochemistry, Vol. 3 (Topics in Current Chemistry, Vol. 148) E. Steckhan (Ed), Springer, NY 1988.
  3. ^ Yan, M.; Kawamata, Y.; Baran, P. S. (2017). "Synthetic Organic Electrochemistry: Calling All Engineers". Angewandte Chemie International Edition. 57 (16): 4149–4155. doi:10.1002/anie.201707584. PMC 5823775. PMID 28834012.
  4. ^ Utley, James (1997). "Trends in Organic Electrosynthesis". Chemical Society Reviews. 26 (3): 157. doi:10.1039/cs9972600157.
  5. ^ a b Grimshaw, James (2000). Electrochemical Reactions and Mechanisms in Organic Chemistry. Amsterdam: Elsevier Science. pp. 1–7, 282, & 310. ISBN 9780444720078.
  6. ^ Heard, D. M.; Lennox, A.J.J. (6 July 2020). "Electrode Materials in Modern Organic Electrochemistry". Angewandte Chemie International Edition. 59 (43): 18866–18884. doi:10.1002/anie.202005745. PMID 32633073.
  7. ^ Schäfer, H. J.; Feldhues, U. (1982). "Oxidation of Primary Aliphatic Amines to Nitriles at the Nickel Hydroxide Electrode". Synthesis. 1982 (2): 145–146. doi:10.1055/s-1982-29721.
  8. ^ Organic Syntheses, "Coll. Vol. 7, p.307 (1990); Vol. 63, p.206 (1985)". Archived from the original on 26 September 2007.
  9. ^ Organic Syntheses, "Coll. Vol. 7, p.482 (1990); Vol. 60, p.78 (1981)". Archived from the original on 26 September 2007.
  10. ^ Hampson, N; Lee, J; MacDonald, K (1972). "The oxidation of amino compounds at anodic silver". Electrochimica Acta. 17 (5): 921–955. doi:10.1016/0013-4686(72)90014-X.
  11. ^ a b Barba, Fructuoso; Batanero, Belen (2004). "Paired Electrosynthesis of Cyanoacetic Acid". The Journal of Organic Chemistry. 69 (7): 2423–2426. doi:10.1021/jo0358473. PMID 15049640.
  12. ^ Wilhelm Riemenschneider (2002). "Carboxylic Acids, Aliphatic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a05_235. ISBN 3527306730.
  13. ^ "Electrochemistry Encyclopedia – Tafel: his life and science". Archived from the original on 6 February 2012.
  14. ^ Tafel, Julius; Hahl, Hans (1907). "Vollständige Reduktion des Benzylacetessigesters". Berichte der deutschen chemischen Gesellschaft. 40 (3): 3312–3318. doi:10.1002/cber.190704003102.
  15. ^ Krishnan, V.; Muthukumaran, A.; Udupa, H. V. K. (1979). "The electroreduction of benzyl cyanide on iron and cobalt cathodes". Journal of Applied Electrochemistry. 9 (5): 657–659. doi:10.1007/BF00610957. S2CID 96102382.
  16. ^ Wessling, M.; Schäfer, H.J. (1991). "Cathodic reduction of 1-nitroalkenes to oximes and primary amines". Chem. Ber. 124 (10): 2303–2306. doi:10.1002/cber.19911241024.
  17. ^ a b Cardoso, D. S.; Šljukić, B.; Santos, D. M.; Sequeira, C. A. (17 July 2017). "Organic Electrosynthesis: From Laboratorial Practice to Industrial Applications". Organic Process Research & Development. 21 (9): 1213–1226. doi:10.1021/acs.oprd.7b00004.
  18. ^ Sakakura, Toshiyasu; Choi, Jun-Chul; Yasuda, Hiroyuki (13 June 2007). "Transformation of Carbon dioxide". Chemical Reviews. American Chemical Society. 107 (6): 2365–2387. doi:10.1021/cr068357u. PMID 17564481.
  19. ^ Tafel, Julius; Friedrichs, Gustav (1904). "Elektrolytische Reduction von Carbonsäuren und Carbonsäureestern in schwefelsaurer Lösung". Berichte der Deutschen Chemischen Gesellschaft. 37 (3): 3187–3191. doi:10.1002/cber.190403703116.
  20. ^ Cohen, Julius (1920) [1910]. Practical Organic Chemistry (PDF) (2nd ed.). London: Macmillan and Co. Limited. pp. 102–104.
  21. ^ A. W. Ingersoll (1929). "Hydrocinnamic acid". Organic Syntheses. 9: 42.; Collective Volume, 1, p. 311
  22. ^ Bouwman, Elisabeth; Angamuthu, Raja; Byers, Philip; Lutz, Martin; Spek, Anthony L. (15 July 2010). "Electrocatalytic CO2 Conversion to Oxalate by a Copper Complex". Science. 327 (5393): 313–315. Bibcode:2010Sci...327..313A. doi:10.1126/science.1177981. PMID 20075248. S2CID 24938351.
  23. ^ B. Innocent; et al. (February 2009). "Electro-reduction of carbon dioxide to formate on lead electrode in aqueous medium". Journal of Applied Electrochemistry. 39 (2): 227–232. doi:10.1007/s10800-008-9658-4. S2CID 98437382.
  24. ^ Lee, Byungik; Naito, Hiroto; Nagao, Masahiro; Hibino, Takashi (9 July 2012). "Alternating-Current Electrolysis for the Production of Phenol from Benzene". Angewandte Chemie International Edition. 51 (28): 6961–6965. doi:10.1002/anie.201202159. PMID 22684819.
  25. ^ Simons, J. H. (1949). "Production of Fluorocarbons I. The Generalized Procedure and its Use with Nitrogen Compounds". Journal of the Electrochemical Society. 95: 47–52. doi:10.1149/1.2776733. See also related articles by Simons et al. on pages 53, 55, 59, and 64 of the same issue.