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A corrole is an aromatic organic chemical, the structure of which is similar to the corrin ring, which is also present in cobalamin (vitamin B12). The ring consists of nineteen carbon atoms, with four nitrogen atoms in the core of the molecule. In this sense, corrole is very similar to porphyrin, which is also an organic macrocycle but has twenty carbon atoms and is found in hemoglobin and chlorophyll.

Corroles can be prepared through organic synthesis by condensation reaction of a benzaldehyde with pyrrole in a water / methanol / hydrochloric acid mixture to an open-ring bilane (or tetrapyrrane) followed by oxidation and ring closure with p-chloranil:[1]

Corrole synthesis

Corrole has several important differences from porphyrin. The first is that it is normally a trianionic ligand with transition metals, while porphyrin is typically a dianionic ligand. As a result, corrole supports metals in higher oxidation states. The second difference from porphyrin is that, because the ring of corrole is smaller, there is slightly less space in the middle of it, which results in many metals sitting slightly out of the plane created by the four nitrogen atoms in the ring.

Corroles have been attached to a wide range of transition metals,[2][3] main group elements,[4] and more recently, lanthanides[5] and actinides.[6] Additionally, corroles and their metal complexes have been demonstrated to be useful as imaging agents in tumor detection,[7] for prevention of heart disease,[8] in synthetic chemistry as oxo, imido, and nitrido transfer agents,[9] and as catalysts for the catalytic reduction of oxygen to water,[10] and hydrogen production form water under aerobic conditions.


  1. ^ Efficient Synthesis of meso-Substituted Corroles in an H2O-MeOH Mixture Beata Koszarna and Daniel T. Gryko J. Org. Chem.; 2006; 71(10) pp 3707 - 3717. doi:10.1021/jo060007k
  2. ^ Aviv-Harel, I.; Gross, Z. Chem. Eur. J. 2009, 15, 8382–8394.
  3. ^ Buckley, H. L.; Chomitz, W. A.; Koszarna, B.; Tasior, M.; Gryko, D. T.; Brothers, P. J.; Arnold, J. Chem. Commun. 2012, 48, 10766–10768.
  4. ^ Aviv-Harel, I.; Gross, Z. Coord. Chem. Rev. 2010, 255, 717–736.
  5. ^ Buckley, H. L.; Anstey, M. R.; Gryko, D. T.; Arnold, J. Chem. Commun. 2013, 49, 3104–3106.
  6. ^ Ward, A. L.; Buckley, H. L.; Lukens, W. W.; Arnold, J. J. Am. Chem. Soc. 2013, 135, 13965–13971.
  7. ^ Agadjanian, H.; Ma, J.; Rentsendorj, A.; Valluripalli, V.; Youn, J.; Mahammed, A.; Farkas, D. L.; Gray, H. B.; Gross, Z.; Medina-Kauwe, L. K. PNAS 2009, 106, 6105–6110.
  8. ^ Adi Haber; Ali, A. A.-Y.; Aviram, M.; Gross, Z. Chem. Commun. 2013, 49, 10917–10919.
  9. ^ Palmer, J. H. Struct. Bond. 2012, 142, 49–90.
  10. ^ Dogutan, D. K.; Stoian, S. A.; McGuire, R.; Schwalbe, M.; Teets, T. S.; Nocera, D. G. J. Am. Chem. Soc. 2011, 133, 131–140.