Related Experiment Video
Updated: May 31, 2026
10:42
Combining Solid-state and Solution-based Techniques: Synthesis and Reactivity of Chalcogenidoplumbates(II or IV)
Published on: December 29, 2016
Aqua-bromidobis(dimethyl-glyoximato)cobalt(III)
Parthasarathy Meera1, Madhavan Amutha Selvi, Pachaimuthu Jothi
1Loyola College (Autonomous), Chennai 600 034, Tamil Nadu, India.
Summary
This study details the crystal structure of a cobalt(III) complex, revealing an approximately octahedral geometry. The complex features glyoximate ligands, a bromide ion, and a water molecule, forming hydrogen bonds and supramolecular chains.
Area of Science:
- Coordination Chemistry
- Crystallography
- Supramolecular Chemistry
Background:
- Cobalt complexes are vital in catalysis and materials science.
- Understanding coordination geometry is key to predicting chemical properties.
- Glyoximate ligands offer unique coordination possibilities.
Purpose of the Study:
- To elucidate the crystal structure and coordination environment of a novel cobalt(III) complex.
- To investigate the role of glyoximate ligands in complex formation.
- To analyze the hydrogen bonding and supramolecular assembly.
Main Methods:
- Single-crystal X-ray diffraction analysis was performed.
- The molecular and crystal structure was determined and refined.
- Hydrogen bonding interactions and supramolecular architecture were analyzed.
Main Results:
- The cobalt(III) complex, [CoBr(C(4)H(7)N(2)O(2))(2)(H(2)O)], exhibits approximate octahedral geometry.
- A crystallographic mirror plane bisects the molecule, with glyoximate N atoms forming the base.
- Intramolecular hydrogen bonds and intermolecular O-H⋯O bonds generate supramolecular chains.
Conclusions:
- The determined structure provides insights into cobalt(III) coordination chemistry with glyoximate ligands.
- Hydrogen bonding plays a crucial role in the supramolecular organization of the complex.
- The findings contribute to the understanding of crystal engineering and materials design.
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.
02:42Valence Bond Theory
Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...
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...
02:34Structural Isomerism
Isomerism in Complexes
Isomers are different chemical species that have the same chemical formula. Structural isomerism of coordination compounds can be divided into two subcategories, the linkage isomers and coordination-sphere isomers.
Linkage isomers occur when the coordination compound contains a ligand that can bind to the transition metal center through two different atoms. For example, the CN− ligand can bind through the carbon atom or through the nitrogen atom. Similarly, SCN− can be...
Isomers are different chemical species that have the same chemical formula. Structural isomerism of coordination compounds can be divided into two subcategories, the linkage isomers and coordination-sphere isomers.
Linkage isomers occur when the coordination compound contains a ligand that can bind to the transition metal center through two different atoms. For example, the CN− ligand can bind through the carbon atom or through the nitrogen atom. Similarly, SCN− can be...
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...
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...