Related Experiment Video
Updated: Jun 1, 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
Tris(2,2'-bipyridyl-κN,N')copper(II) sulfate 7.5-hydrate
1State Key Laboratory of Coordination Chemistry, Nanjing National Laboratory of Microstructures, School of Chemistry and Chemical Engineering, Nanjing University, Nanjing, 210093, People's Republic of China.
Summary
This study details a copper(II) complex with three bipyridyl ligands, revealing a non-planar structure and hydrogen bonding interactions in its crystalline form. The findings contribute to understanding coordination chemistry and crystal packing.
Area of Science:
- Coordination Chemistry
- Crystallography
- Materials Science
Background:
- Copper(II) complexes are widely studied for their diverse applications.
- Bipyridyl ligands are common in coordination chemistry due to their chelating ability.
- Understanding the structural nuances of metal complexes is crucial for predicting their properties.
Purpose of the Study:
- To synthesize and characterize a novel copper(II) complex with 2,2'-bipyridyl ligands.
- To investigate the coordination geometry and crystal structure of the [Cu(bipy)(3)]SO(4)·7.5H(2)O complex.
- To explore the intermolecular interactions within the crystal lattice.
Main Methods:
- Single-crystal X-ray diffraction was employed to determine the molecular and crystal structure.
- Spectroscopic methods were used for characterization.
- Analysis of bond lengths, angles, and hydrogen bonding networks.
Main Results:
- The title compound, [Cu(C(10)H(8)N(2))(3)]SO(4)·7.5H(2)O, was successfully synthesized and characterized.
- The copper(II) center exhibits a six-coordinate, slightly elongated octahedral geometry.
- The pyridyl rings of the bipyridyl ligands are non-planar, with observed dihedral angles.
- Extensive O-H⋯O and C-H⋯O hydrogen bonding interactions were identified in the crystal structure.
Conclusions:
- The structural analysis provides detailed insights into the coordination environment of copper(II) with bipyridyl ligands.
- The non-planar nature of the ligands and the presence of significant hydrogen bonding influence the crystal packing.
- This study contributes to the fundamental understanding of copper coordination complexes and their solid-state structures.
Related Concept Videos
02:57Coordination Number and Geometry
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.
01:18Aromatic Hydrocarbon Cations: Structural Overview
Cycloheptatriene is a neutral monocyclic unsaturated hydrocarbon that consists of an odd number of carbon atoms and an intervening sp3 carbon in the ring. The three double bonds in the ring correspond to 6 π electrons, which is a Huckel number, and therefore satisfies the criteria of 4n + 2 π electrons. However, the intervening sp3 carbon disrupts the continuous overlap of p orbitals. As a result, cycloheptatriene is not aromatic.
Removing one hydrogen from the intervening CH2 group with both...
Removing one hydrogen from the intervening CH2 group with both...
02:46Crystal 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,...
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,...
01:22EDTA: Chemistry and Properties
Polydentate ligands are most widely used in complexometric titrations because they form more stable complexes with the metal ions than mono- or bidentate ligands due to the chelate effect. Examples of polydentate ligands are ethylenediaminetetraacetic acid (EDTA), crown ethers, and cryptands. The most important feature of optimal polydentate ligands is the ability to form 1:1 complexes in a single-step process. Amino carboxylic acid derivatives are frequently used as complexing agents. EDTA is...
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.
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.