Related Experiment Video
Updated: Jun 2, 2026
![[(DPEPhos)(bcp)Cu]PF6: A General and Broadly Applicable Copper-Based Photoredox Catalyst](/_next/image?url=https%3A%2F%2Fcloudfront.jove.com%2FCDNSource%2Fteasers%2F59739.jpg&w=3840&q=50)
09:12
[(DPEPhos)(bcp)Cu]PF6: A General and Broadly Applicable Copper-Based Photoredox Catalyst
Published on: May 21, 2019
Chlorido(2-{1-[(2-morpholino-eth-yl)imino]-eth-yl}phenolato-κN,N',O)copper(II)
Nurul Azimah Ikmal Hisham1, Nura Suleiman Gwaram, Hamid Khaledi
1Department of Chemistry, University of Malaya, 50603 Kuala Lumpur, Malaysia.
Acta Crystallographica. Section E, Structure Reports Online
|April 28, 2011
Summary
This study details the crystal structure of a copper(II) compound featuring a tridentate Schiff base ligand and a chloride ion. The copper ion exhibits a distorted square-planar geometry, with molecules forming layered structures through intermolecular interactions.
Area of Science:
- Coordination Chemistry
- Crystal Engineering
- Materials Science
Background:
- Schiff base ligands are versatile in coordinating with metal ions.
- Copper(II) complexes are of interest due to their diverse applications.
- Understanding crystal packing is crucial for designing new materials.
Purpose of the Study:
- To synthesize and characterize a novel copper(II) complex with a Schiff base ligand.
- To elucidate the coordination geometry and crystal structure of the title compound.
- To investigate intermolecular interactions driving crystal formation.
Main Methods:
- Single-crystal X-ray diffraction was employed to determine the molecular and crystal structure.
- The coordination environment around the Cu(II) ion was analyzed.
- Intermolecular interactions (C-H⋯Cl, C-H⋯O) were identified and studied.
Main Results:
- The copper(II) ion is four-coordinated in a distorted square-planar geometry by a deprotonated N,N',O-tridentate Schiff base and a chloride ion.
- Adjacent molecules self-assemble into infinite layers parallel to the (100) crystallographic plane.
- The crystal structure was successfully solved from a non-merohedrally twined crystal.
Conclusions:
- The study provides a detailed structural analysis of a new copper(II)-Schiff base complex.
- The observed crystal packing highlights the role of specific intermolecular interactions in directing self-assembly.
- This structural insight contributes to the broader understanding of coordination compounds and crystal engineering.
Related Concept Videos
00:56Extraction: 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...
02:54Coordination Compounds and Nomenclature
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...
03:02Colors and Magnetism
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 eye.
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.
02:36Acidity and Basicity of Alcohols and Phenols
Like water, alcohols are weak acids and bases. This is attributed to the polarization of the O–H bond making the hydrogen partially positive. Moreover, the electron pairs on the oxygen atom of alcohol make it both basic and nucleophilic. Protonation of an alcohol converts hydroxide, a poor leaving group, into water—a good one. The two acid–base equilibria corresponding to ethanol are depicted below.
03:34Ionic Compounds: Formulas and Nomenclature
An element composed of atoms that readily lose electrons (a metal) can react with an element composed of atoms that readily gain electrons (a nonmetal) to produce ions through complete electron transfer. The compound formed by this transfer is stabilized by the electrostatic attractions (ionic bonds) between the oppositely charged ions.
02:51Metal-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.
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...
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...