Related Experiment Video
Updated: Jul 25, 2026
14:44
Structure and Coordination Determination of Peptide-metal Complexes Using 1D and 2D 1H NMR
Published on: December 16, 2013
DNA damage by copper(II) complexes: coordination-structural dependence of reactivities
1Department of Chemistry, Huazhong University of Science and Technology, Wuhan, China. L20919@public.wh.hb.cn
Journal of Inorganic Biochemistry
|September 4, 1999
Summary
Copper complexes bind DNA and cause double-strand breaks via hydroxyl radical generation. Their DNA damage capacity depends on structure and ligands, with specific complexes showing higher potency.
Area of Science:
- Coordination Chemistry
- Biophysical Chemistry
- Molecular Biology
Background:
- Copper complexes exhibit DNA-binding capabilities.
- Certain copper complexes can induce DNA damage.
- Understanding copper-DNA interactions is crucial for developing targeted therapies.
Purpose of the Study:
- To investigate the DNA binding and damage mechanisms of various copper complexes.
- To correlate the structural features of copper complexes with their DNA damaging potential.
- To identify the role of hydroxyl radical generation in copper-mediated DNA damage.
Main Methods:
- Spectroscopic analysis (UV-Vis, ESR) to study copper-DNA interactions and radical generation.
- Quantification of hydroxyl radical production using 2-deoxy-D-ribose assay.
- Assessment of double-strand DNA damage using lambda DNA as a model system.
Main Results:
- Copper complexes bind double-helical DNA with high affinity (10(4)-10(7) M-1).
- Hydroxyl radical generation was confirmed via Electron Spin Resonance (ESR) spectroscopy.
- DNA damage capacity varied among complexes, influenced by geometric structure and ligands.
- A decreasing order of DNA damage capacity was established for the tested complexes.
Conclusions:
- Copper complexes can effectively bind and damage DNA through hydroxyl radical generation.
- The structural and ligand environment of copper complexes dictates their DNA interaction and damage potency.
- These findings provide insights into the design of copper-based agents for DNA-targeting applications.
More Related Videos
11:04Ion Mobility-Mass Spectrometry Techniques for Determining the Structure and Mechanisms of Metal Ion Recognition and Redox Activity of Metal Binding Oligopeptides
Published on: September 7, 2019
11:38Quantifying the Binding Interactions Between Cu(II) and Peptide Residues in the Presence and Absence of Chromophores
Published on: April 5, 2022
Related Concept Videos
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...
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.
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.
01:19Complexation 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...
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...
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...