Electron acceptor

An electron acceptor is a chemical entity that accepts electrons transferred to it from another compound.^[1] Electron acceptors are oxidizing agents.

The electron accepting power of an electron acceptor is measured by its redox potential.^[2]

In the simplest case, electron acceptors are reduced by one electron. The process can alter the structure of the acceptor substantially. When the added electron is highly delocalized, the structural consequences of the reduction can be subtle. The central C-C distance in the electron acceptor tetracyanoethylene elongates from 135 to 143 pm upon acceptance of an electron.^[3] In the formation of some donor-acceptor complexes, less than one electron is transferred. TTF-TCNQ is an charge transfer complex.

Biology

Paraquat, the dication on the left, functions as an electron acceptor, disrupting respiration in plants.

In biology, a terminal electron acceptor often refers to either the last compound to receive an electron in an electron transport chain, such as oxygen during cellular respiration, or the last cofactor to receive an electron within the electron transfer domain of a reaction center during photosynthesis. All organisms obtain energy by transferring electrons from an electron donor to an electron acceptor.^{[citation needed]}

One practical illustration of the role of electron acceptors in biology is the high toxicity of the paraquat. The activity of this broad spectrum herbicide results from the electron acceptor property of N,N'-dimethyl-4,4'-bipyridinium.^[4]

Materials science

In some solar cells, the photocurrent entails transfer of electrons from a donor to an electron acceptor.^[5]

References

^ "Electron Acceptor". The IUPAC Compendium of Chemical Terminology. 2014. doi:10.1351/goldbook.E01976.
^ Connelly, N. G.; Geiger, W. E. (1996). "Chemical Redox Agents for Organometallic Chemistry". Chemical Reviews. 96 (2): 877–910. doi:10.1021/cr940053x. PMID 11848774.
^ Bock, H.; Ruppert, K. (1992). "Structures of charge-perturbed or sterically overcrowded molecules. 16. The cesium tetracyanoethylenide radical salt". Inorganic Chemistry. 31 (24): 5094–5099. doi:10.1021/ic00050a032.
^ Bockman, T. M.; Kochi, J. K. (1990). "Isolation and Oxidation-Reduction of Methylviologen Cation Radicals. Novel Disproportionation in Charge-Transfer Salts by X-ray Crystallography". The Journal of Organic Chemistry. 55 (13): 4127–4135. doi:10.1021/jo00300a033.
^ Stoltzfus, Dani M.; Donaghey, Jenny E.; Armin, Ardalan; Shaw, Paul E.; Burn, Paul L.; Meredith, Paul (2016). "Charge Generation Pathways in Organic Solar Cells: Assessing the Contribution from the Electron Acceptor". Chemical Reviews. 116 (21): 12920–12955. doi:10.1021/acs.chemrev.6b00126. PMID 27341081.

External links

[1] "Electron Acceptor". The IUPAC Compendium of Chemical Terminology. 2014. doi:10.1351/goldbook.E01976.

[Geiger-2] Connelly, N. G.; Geiger, W. E. (1996). "Chemical Redox Agents for Organometallic Chemistry". Chemical Reviews. 96 (2): 877–910. doi:10.1021/cr940053x. PMID 11848774.

[3] Bock, H.; Ruppert, K. (1992). "Structures of charge-perturbed or sterically overcrowded molecules. 16. The cesium tetracyanoethylenide radical salt". Inorganic Chemistry. 31 (24): 5094–5099. doi:10.1021/ic00050a032.

[4] Bockman, T. M.; Kochi, J. K. (1990). "Isolation and Oxidation-Reduction of Methylviologen Cation Radicals. Novel Disproportionation in Charge-Transfer Salts by X-ray Crystallography". The Journal of Organic Chemistry. 55 (13): 4127–4135. doi:10.1021/jo00300a033.

[5] Stoltzfus, Dani M.; Donaghey, Jenny E.; Armin, Ardalan; Shaw, Paul E.; Burn, Paul L.; Meredith, Paul (2016). "Charge Generation Pathways in Organic Solar Cells: Assessing the Contribution from the Electron Acceptor". Chemical Reviews. 116 (21): 12920–12955. doi:10.1021/acs.chemrev.6b00126. PMID 27341081.

[1]

[2]

[3]

[4]

[5]

Biology

Materials science

See also

References

External links