Poly[di-μ(2)-chlorido-μ(2)-(1,4-dioxane-κO:O')-cadmium(II)]
Jian-Qiang Wang1, Ren-Jun Du, Wei Wang
1Department of Applied Chemistry, College of Science, Nanjing University of Technology, Nanjing 210009, People's Republic of China.
Summary
This study reveals a novel 3D coordination network of cadmium chloride and 1,4-dioxane. The structure features infinite linear chains formed by bridging chloride anions and interconnected by dioxane ligands.
Area of Science:
- Inorganic Chemistry
- Crystal Engineering
- Materials Science
Background:
- Coordination polymers and metal-organic frameworks are of interest for their diverse structures and potential applications.
- Cadmium(II) complexes with halide and oxygen-donor ligands offer tunable properties based on coordination environment.
Purpose of the Study:
- To synthesize and characterize a novel coordination network of cadmium(II) with 1,4-dioxane and chloride.
- To elucidate the structural features and dimensionality of the resulting complex.
Main Methods:
- Single-crystal X-ray diffraction was used to determine the molecular and crystal structure.
- Infrared spectroscopy may have been used for ligand identification.
Main Results:
- A 1D coordination polymer, [CdCl(2)(C(4)H(8)O(2))](n), was synthesized, featuring two distinct Cd(II) coordination environments.
- Cd(II) ions exhibit distorted octahedral geometry, coordinated by oxygen atoms from 1,4-dioxane and chloride anions.
- Infinite linear chains along the a-axis are formed by bridging chloride anions.
- These chains are further linked by bridging 1,4-dioxane ligands, creating a 3D network structure.
Conclusions:
- The study successfully demonstrates the formation of a 3D coordination network from cadmium(II), chloride, and 1,4-dioxane.
- The bridging nature of both chloride and 1,4-dioxane ligands is crucial for achieving the extended network architecture.
- This structural motif provides insights into the design of novel cadmium-based coordination materials.
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...
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.
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...
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...