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Related Concept Videos

Complexation Equilibria: The Chelate Effect01:19

Complexation Equilibria: The Chelate Effect

In complexation reactions, metal atoms or cations interact with ligands to form donor-acceptor adducts called metal complexes. Ligands that bind through one donor site are monodentate, ligands with two donor sites are bidentate, and those with more than two donor sites are polydentate ligands. For example, ethylene diamine is a bidentate ligand that binds through two nitrogen donor atoms, forming a five-membered ring. EDTA is a polydentate ligand that binds through four oxygen and two nitrogen...
Complexation Equilibria: Factors Influencing Stability of Complexes01:09

Complexation Equilibria: Factors Influencing Stability of Complexes

In complexation reactions, metal cations are the electron pair acceptors, and the ligands are the electron pair donors. The stability of the metal complexes depends primarily on the complexing ability of the central metal ion and the nature of the ligands. Generally, the complexing ability of the metal ion depends on the size and charge of the ion. As the metal ion size increases, the stability of the metal complexes decreases, provided that the valency of the metal ion and the ligands remain...
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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.
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Metal ions can be separated from one another by complexation with organic ligands–the chelating agent– to form uncharged chelates. Here, the chelating agent must contain hydrophobic groups and behave as a weak acid, losing a proton to bind with the metal. Since most organic ligands used in this process are insoluble or undergo oxidation in the aqueous phase, the chelating agent is initially added to the organic phase and extracted into the aqueous phase. The metal-ligand complex is formed in...
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A type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called ligands. These ligands can be neutral molecules like H2O or NH3, or ions such as CN− or OH−. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called coordination...
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Valence Bond Theory

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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Synthesis and Characterization of Functionalized Metal-organic Frameworks
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Published on: September 5, 2014

When do molecular bowls encapsulate metal cations?

Jason R Green1, Robert C Dunbar

  • 1Department of Chemistry, Northwestern University, 2145 Sheridan Road, Evanston, Illinois 60208, United States.

The Journal of Physical Chemistry. A
|April 22, 2011
PubMed
Summary

Curved carbon surfaces, like buckybowls, show strong potential for chemical microencapsulation. Multiply charged metal cations are preferentially encapsulated inside these structures due to size and charge interactions.

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Area of Science:

  • Nanomaterials science
  • Computational chemistry
  • Physical chemistry

Background:

  • Curved carbon π surfaces offer unique properties for chemical microencapsulation and nanoscale material self-assembly.
  • Understanding host-guest interactions, particularly with metal cations, is crucial for advancing these applications.

Purpose of the Study:

  • To quantitatively predict metal cation binding to prototypical buckybowls (C(20)H(10), C(30)H(10), C(40)H(10)).
  • To determine favorable binding sites (inside vs. outside) and factors influencing preference.
  • To explore binding behavior of various monocations and multiply charged cations.

Main Methods:

  • Density functional theory (DFT) calculations were employed.
  • Investigated binding affinities and preferred sites for Na(+), Cs(+), NH(4)(+), Ba(+), Ba(2+), and La(3+).
  • Analyzed factors such as ion size, charge, Coulomb potentials, and polarization interactions.

Main Results:

  • Large ion size and high charge favor inside binding.
  • Monocations showed weak encapsulation tendency, while Ba(2+) and La(3+) exhibited strong encapsulation.
  • Coulomb potentials favor outside binding, but cation microsolvation via polarization can favor encapsulation.

Conclusions:

  • Ion size and charge are key determinants for preferential binding inside buckybowls.
  • Multiply charged cations are strongly driven towards encapsulation.
  • These findings are valuable for designing nanocontainers and diverse nanostructures.