Macrocyclic ligand

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In coordination chemistry, a macrocyclic ligand is a macrocyclic ring having at least nine atoms (including all hetero atoms) and three or more donor sites that serve as ligands that can bind to a central metal ion.[1] Crown ethers and porphyrins are prominent examples. Macrocyclic ligands exhibit high affinity for metal ions.

History[]

Porphyrins and phthalocyanines have long been recognized as potent ligands in coordination chemistry.

Binding of dioxygen to a heme (an iron macrocyclic complex) occurs in myoglobin and hemoglobin.

In the 1960s the synthesis of macrocylic ligands received much attention, beginning with the synthesis of the "Curtis macrocycles", in which a metal ion serves as a template for ring formation.[2] Porphyrins, which feature 16-membered central rings, form even in the absence of metal templates.

14-membered N4 macrocyclic ligands, called Curtis macrocycles, arise from the condensation of acetone and a nickel complex of ethylenediamine.

In 1967 a new series of macrocyclic compounds was reported by Pederson, who synthesized many cyclic polyethers or "crown" compounds with variety of ring sizes and substituent groups, and different numbers of ether oxygens that serve as ligands.[3] A few years later, three-dimensional analogs of crown ethers called "cryptands" were reported by Lehn and co-workers.[4]

Macrocyclic effect[]

Crystal structure of a Zn(II) ion coordinated to cyclen and ethanol.[5]

The macrocyclic effect is the high affinity of metal cations for macrocyclic ligands, compared to their acyclic analogues.[6][7] The high affinity of macrocyclic ligands is thought to be a combination of the entropic effect seen in the chelate effect, together with an additional energetic contribution that comes from the preorganized nature of the ligating groups (that is, no additional strains are introduced to the ligand on coordination).[8]

Synthesis[]

1,4,7-Triazacyclononane is a popular macrocyclic ligand, which is prepared without metal templating.

In general, macrocyclic complexes are synthesized by combining macrocyclic ligands and metal ions.[9]

In template reactions, macrocyclic ligands are synthesized in the presence of metal ions. In the absence of the metal ion, the same organic reactants may produce different, often polymeric, products. The metal ion may direct the condensation preferentially to cyclic rather than polymeric products (the kinetic template effect) or stabilize the macrocycle once formed (the thermodynamic template effect). The template effect makes use of the pre-organization provided by the coordination sphere of the metal. The coordination modifies the electronic properties such as the acidity and electrophilicity of the ligands. When the metal atom is not desired in the final product, a disadvantage of templated synthesis is the difficulty in removing the templating metal from the macrocyclic ligand.

18-Crown-6 can be synthesized by the Williamson ether synthesis using potassium ion as the template cation.

Phthalocyanines were the first macrocycles synthesized by template reaction. They bear strong structural resemblance to natural porphyrin systems.

The size of the metal cation used as the template has proved to be of importance in directing the synthetic pathway for the Schiff base systems. The compatibility between the radius of the template cation and the "hole" of the macrocycle contributes to the effectiveness of the synthetic pathway and to the geometry of the resulting complex.[10]

Uses and occurrence[]

Structure of an Fe-TAML complex.[11]

Phthalocyanines, as their metal complexes, are arguably the most commercially useful complex of a macrocyclic ligand. They are used as dyes and pigments such as phthalocyanine blue.[12]

Macrocyclic ligands occur in many cofactors in proteins and enzymes. Of particular interest are tetraazamacrocycles.[13]

Heme, the active site in the hemoglobin (the metalloprotein in blood that transports oxygen), is a porphyrin that contains iron. Chlorophyll, the green photosynthetic pigment found in plants, contains a chlorin ring. Vitamin B12 contains a corrin ring.

References[]

  1. ^ Melson, GA (1979). Coordination Chemistry of Macrocyclic Compounds. New York: Plenum Press. p. 2. ISBN 0-306-40140-1.
  2. ^ Curtis, N.F. (April 1968). "Macrocyclic coordination compounds formed by condensation of metal-amine complexes with aliphatic carbonyl compounds". Coordination Chemistry Reviews. 3 (1): 3–47. doi:10.1016/S0010-8545(00)80104-6.
  3. ^ Pedersen, Charles J. (December 1967). "Cyclic polyethers and their complexes with metal salts". Journal of the American Chemical Society. 89 (26): 7017–7036. doi:10.1021/ja01002a035.
  4. ^ Pedersen, C. J.; Frensdorff, H. K. (January 1972). "Macrocyclic Polyethers and Their Complexes". Angewandte Chemie International Edition in English. 11 (1): 16–25. doi:10.1002/anie.197200161. PMID 4622977.
  5. ^ Antje Schrodt, Anton Neubrand, Rudi van Eldik (1997). "Fixation of CO2 by Zinc(II) Chelates in Alcoholic Medium. X-ray Structures of {[Zn(cyclen)]3(μ3-CO3)}(ClO4)4 and [Zn(cyclen)EtOH](ClO4)2". Inorg. Chem. 36 (20): 4579–4584. doi:10.1021/ic961368t. PMID 11670124.CS1 maint: uses authors parameter (link)
  6. ^ Cabbines, D. K.; Margerum, D. W. (1969). "Macrocyclic effect on stability of copper(II) tetramine complexes". J. Am. Chem. Soc. 91 (23): 6540–6541. doi:10.1021/ja01051a091.
  7. ^ Melson, GA (1979). Coordination Chemistry of Macrocyclic Compounds. New York: Plenum Press. p. 166. ISBN 0-306-40140-1.
  8. ^ Weller M, Overton T, Rourke J, Armstrong F (2014). Inorganic Chemistry. OUP Oxford. p. 229. ISBN 978-0-19-964182-6.
  9. ^ L.F Lindloy, The Chemistry of Macrocylic Ligand Complexes, Cambridge University Press, 1989, 20-50 ISBN 0-521-25261-X
  10. ^ Alexander, V. (March 1995). "Design and Synthesis of Macrocyclic Ligands and Their Complexes of Lanthanides and Actinides". Chemical Reviews. 95 (2): 273–342. doi:10.1021/cr00034a002.
  11. ^ Collins, T. J. (2002), "TAML oxidant activators: a new approach to the activation of hydrogen peroxide for environmentally significant problems", Accounts of Chemical Research, 35 (9): 782–790, doi:10.1021/ar010079s, PMID 12234208
  12. ^ Milgrom, L.R (1997). The Colours of Life: An Introduction to the Chemistry of Porphyrins and Related Compounds. New York: Oxford University Press. ISBN 0-19-855380-3. (hardbound) ISBN 0-19-855962-3 (pbk.)[page needed]
  13. ^ S. J. Lippard, J. M. Berg “Principles of Bioinorganic Chemistry” University Science Books: Mill Valley, CA; 1994. ISBN 0-935702-73-3.[page needed]
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