Aqua[N-(2,5-dihydroxybenzyl)imino-diacetato]copper(II)
Xiu-Qing Zhang1, Fu-Ping Huang, He-Dong Bian
1Key Laboratory for the Chemistry and Molecular Engineering of Medicinal Resources (Ministry of Education of China), School of Chemistry and Chemical Engineering of Guangxi Normal University, Guilin 541004, People's Republic of China.
Summary
This study details a novel copper(II) complex with a distorted square-pyramidal structure. Intermolecular hydrogen bonding forms a 3D framework, revealing insights into coordination chemistry.
Area of Science:
- Inorganic Chemistry
- Crystallography
- Coordination Chemistry
Background:
- Copper(II) complexes are vital in catalysis and materials science.
- Understanding coordination geometry is key to designing functional metal complexes.
- Tetradentate ligands offer versatile coordination possibilities.
Purpose of the Study:
- To synthesize and characterize a new copper(II) complex.
- To elucidate the coordination geometry and crystal structure of the complex.
- To investigate the role of intermolecular interactions in structure formation.
Main Methods:
- Single crystal X-ray diffraction was used to determine the molecular and crystal structure.
- The coordination environment around the Cu(II) center was analyzed.
- Intermolecular hydrogen bonding networks were identified.
Main Results:
- A novel copper(II) complex, [Cu(C(11)H(11)NO(6))(H(2)O)], was synthesized.
- The Cu(II) atom adopts a distorted square-pyramidal geometry.
- The structure is stabilized by intermolecular hydrogen bonds involving hydroxyl and water groups, forming a 3D framework.
Conclusions:
- The synthesized copper(II) complex exhibits unique coordination geometry.
- Hydrogen bonding plays a crucial role in the self-assembly of a 3D supramolecular structure.
- This work contributes to the understanding of copper coordination complexes and their structural diversity.
Related Concept Videos
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.
02:54Coordination 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...
03:45Formation 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...
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...
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...
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.