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Metal-Ligand Bonds02:51

Metal-Ligand Bonds

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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.
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
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Valence Bond Theory02:42

Valence Bond Theory

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Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...
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Coordination Number and Geometry02:57

Coordination Number and Geometry

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For transition metal complexes, the coordination number determines the geometry around the central metal ion. Table 1 compares coordination numbers to molecular geometry. The most common structures of the complexes in coordination compounds are octahedral, tetrahedral, and square planar.
19.9K
Structural Isomerism02:34

Structural Isomerism

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Isomerism in Complexes
Isomers are different chemical species that have the same chemical formula. Structural isomerism of coordination compounds can be divided into two subcategories, the linkage isomers and coordination-sphere isomers.
Linkage isomers occur when the coordination compound contains a ligand that can bind to the transition metal center through two different atoms. For example, the CN− ligand can bind through the carbon atom or through the nitrogen atom. Similarly, SCN− can...
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Colors and Magnetism03:02

Colors and Magnetism

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Color in Coordination Complexes
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...
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Coordination Compounds and Nomenclature02:54

Coordination Compounds and Nomenclature

28.3K
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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Amide Coupling Reaction for the Synthesis of Bispyridine-based Ligands and Their Complexation to Platinum as Dinuclear Anticancer Agents
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Dipyridinophane ligands - synthesis and coordination study.

Lucie Kuncová1, Jana Lazarová1, Jan Kotek1

  • 1Department of Inorganic Chemistry, Faculty of Science, Charles University in Prague Hlavova 2030 128 40 Prague Czech Republic kubicek@natur.cuni.cz.

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|April 9, 2026
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Summary

New dipyridinophane ligands with acetate or methylphosphonate arms show low basicity, leading to stable metal complexes in acidic conditions. Metal ion size dictates complex structure, accommodating larger divalent ions poorly but smaller trivalent ions well.

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Area of Science:

  • Coordination Chemistry
  • Supramolecular Chemistry
  • Organic Synthesis

Background:

  • Macrocyclic ligands are crucial in coordination chemistry.
  • Dipyridinophanes offer unique structural and electronic properties.
  • Understanding ligand basicity and metal ion interactions is key.

Purpose of the Study:

  • To synthesize novel twelve-membered dipyridinophane ligands.
  • To investigate the coordination properties of these ligands with transition metal ions.
  • To determine the influence of ligand structure and metal ion size on complex stability and geometry.

Main Methods:

  • Potentiometry for protonation and stability constants.
  • Spectroscopic measurements for characterization.
  • Single-crystal X-ray diffraction for solid-state structural analysis.

Main Results:

  • Synthesized dipyridinophane ligands with acetate/methylphosphonate pendant arms.
  • Determined lower basicity of dipyridinophanes compared to tetraazamacrocycles.
  • Observed high conditional stabilities of metal complexes in acidic media.
  • Divalent ions (NiII, CuII, ZnII) showed distorted octahedral geometry due to poor fit in the ligand cavity.
  • Trivalent ions (CoIII, FeIII, GaIII) exhibited favorable octahedral or pentagonal bipyramidal arrangements.

Conclusions:

  • Dipyridinophane ligands exhibit tunable coordination properties.
  • Low macrocycle basicity enhances complex stability in acidic environments.
  • Ligand cavity size significantly influences the coordination geometry and stability of metal complexes.