Copper(II), a Peculiar Metal Ion for Complexation With Monensin A Ionophore.
Máté Levente Kis1, Bálint Hajdu1,2, Tamás Jakusch1
1Department of Molecular and Analytical Chemistry, University of Szeged, Szeged, Hungary.
Chemistry (Weinheim an Der Bergstrasse, Germany)
|January 25, 2026
Summary
The antibiotic monensin A forms unique dinuclear copper(II) complexes, unlike other metal ions. These novel coordination compounds are EPR-active, offering new insights into drug-metal interactions.
Area of Science:
- Coordination Chemistry
- Biophysical Chemistry
- Medicinal Chemistry
Background:
- Monensin A is an ionophore that transports sodium ions across cell membranes.
- Monensin A can also bind divalent metal ions, potentially altering its biological activity.
- Previous studies explored monensin A interactions with various metal ions.
Purpose of the Study:
- To investigate the interaction between copper(II) ions and monensin A.
- To characterize the coordination compounds formed between Cu(II) and monensin A.
- To explore the formation of novel dinuclear copper(II) species.
Main Methods:
- Circular dichroism (VIS- and NIR-CD) spectroscopy
- Visible light absorption spectroscopy
- Electron paramagnetic resonance (EPR) spectroscopy
- Electrospray ionization mass spectrometry (ESI-MS)
Main Results:
- Monensin A forms both mono- and bis-Cu(II) complexes.
- Excess Cu(II) salt leads to the formation of previously unobserved dinuclear Cu(II) complexes.
- The dinuclear Cu(II) complex is EPR-active, a rare characteristic for such compounds.
- Counterion origin influences the spectral properties of the dinuclear species.
Conclusions:
- Monensin A forms distinct dinuclear copper(II) complexes.
- These complexes exhibit unique EPR activity.
- Drug-metal ion interactions are significant and should be considered in understanding drug mechanisms.
Related Concept Videos
03:45Formation of Complex Ions
25.8K
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...
25.8K
03:11Precipitation of Ions
30.0K
Predicting Precipitation
The equation that describes the equilibrium between solid calcium carbonate and its solvated ions is:
The equation that describes the equilibrium between solid calcium carbonate and its solvated ions is:
30.0K
02:32Bonding in Metals
52.2K
Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Drüde called the “Electron Sea Model”.
52.2K
02:51Metal-Ligand Bonds
24.1K
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...
24.1K
02:37Metallic Solids
20.5K
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....
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability....
20.5K
03:06Alkali Metals
24.3K
Group 1 elements are soft and shiny metallic solids. They are malleable, ductile, and good conductors of heat and electricity. The melting points of the alkali metals are unusually low for metals and decrease going down the group, while the density increases going down the group with the exception of potassium (Table 1).
Table 1: Properties of the alkali metals
Table 1: Properties of the alkali metals
24.3K