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Related Concept Videos

Ionic Crystal Structures02:42

Ionic Crystal Structures

Ionic crystals consist of two or more different kinds of ions that usually have different sizes. The packing of these ions into a crystal structure is more complex than the packing of metal atoms that are the same size.
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
Metallic Solids02:37

Metallic Solids

Metallic solids such as crystals of copper, aluminum, and iron are formed by metal atoms. The structure of metallic crystals is often described as a uniform distribution of atomic nuclei within a “sea” of delocalized electrons. The atoms within such a metallic solid are held together by a unique force known as metallic bonding that gives rise to many useful and varied bulk properties.
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability. Many...
Valence Bond Theory02:42

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...
Extraction: Advanced Methods00:56

Extraction: Advanced Methods

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...
Formation of Complex Ions03:45

Formation of Complex Ions

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...
Crystal Field Theory - Tetrahedral and Square Planar Complexes02:46

Crystal Field Theory - Tetrahedral and Square Planar Complexes

Tetrahedral Complexes
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...

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Design, Synthesis, and Photochemical Properties of Clickable Caged Compounds
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An expanded cavity hexaamine cage for copper(II).

Paul V Bernhardt1, Richard Bramley, Rodney J Geue

  • 1Department of Chemistry, University of Queensland, Brisbane, Qld 4072, Australia. P.Bernhardt@uq.edu.au

Dalton Transactions (Cambridge, England : 2003)
|March 14, 2007
PubMed
Summary

The crystal structure of a novel copper complex reveals a compressed octahedral geometry, stabilized by a unique bicyclic hexaamine ligand. This complex exhibits a stable Cu(I) state, highlighting the ligand's protective cage effect.

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Area of Science:

  • Coordination Chemistry
  • Inorganic Chemistry
  • Crystallography

Background:

  • Bicyclic hexaamine ligands offer unique coordination environments for metal ions.
  • Copper complexes with cage ligands are of interest for their electronic and redox properties.
  • Understanding the structural dynamics and stability of such complexes is crucial for potential applications.

Purpose of the Study:

  • To determine the crystal structure of the [Cu(fac-Me5-tricosane-N6)](ClO4)2.H2O complex.
  • To investigate the structural dynamics and fluxional behavior of the complex.
  • To evaluate the electrochemical stability of the copper ions within the ligand cage.

Main Methods:

  • X-ray crystallography at 100 K to elucidate the static structure.
  • Electron Paramagnetic Resonance (EPR) spectroscopy to study dynamic behavior from 60 K upwards.
  • Aqueous cyclic voltammetry to assess redox properties and stability.

Main Results:

  • The crystal structure at 100 K shows a tetragonally compressed octahedral geometry around copper.
  • Dynamic interconversion and static disorder between elongated structures were identified.
  • The complex exhibits fluxional behavior at 60 K and above, confirmed by EPR.
  • Electrochemical studies revealed a remarkably stable Cu(I) state, attributed to the ligand's encapsulating effect.

Conclusions:

  • The bicyclic hexaamine ligand enforces a specific, albeit dynamic, coordination geometry around the copper ion.
  • The ligand's structure effectively stabilizes the reduced Cu(I) state, suggesting potential for redox-active applications.
  • The combination of structural rigidity and dynamic fluxionality in this complex offers insights into ligand design for metal stabilization.