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Supramolecular structures of metronidazole and its copper(II), cobalt(II) and zinc(II) coordination compounds

Nadeshda Galván-Tejada1, Sylvain Bernès, Silvia E Castillo-Blum

  • 1Departamento de Química Inorgánica, Facultad de Química, Universidad Nacional Autónoma de México, Cuidad Universitaria, México D.F. 04510, Mexico.

Journal of Inorganic Biochemistry
|July 18, 2002
PubMed

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Metal-Ligand Bonds

The hemoglobin in the blood, the chlorophyll in green plants, vitamin B-12, and the catalyst used in the manufacture of polyethylene all contain coordination compounds. Ions of the metals, especially the transition metals, are likely to form complexes.
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In most main group element compounds, the valence electrons of the isolated atoms combine to form chemical bonds that satisfy the octet rule. For instance, the four valence electrons of carbon overlap with electrons from four hydrogen atoms to form CH4. The one valence electron leaves sodium and adds to the seven valence electrons of chlorine to form the ionic formula unit NaCl (Figure 1a). Transition metals do not normally bond in this fashion. They primarily form coordinate covalent bonds, a...
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Valence Bond Theory

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When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human eye.