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Colors and Magnetism

Colors 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.

Structural Isomerism

Structural 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...

Valence Bond Theory

Valence 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...

Coordination Compounds and Nomenclature

Coordination 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...

Formation of Complex Ions

Formation 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...

Coordination Number and Geometry

Coordination 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.

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Related Experiment Video

Updated: Jun 1, 2026

Preparation of SNS Cobalt(II) Pincer Model Complexes of Liver Alcohol Dehydrogenase

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Published on: March 19, 2020

Hexakis(dimethyl sulfoxide-κO)cobalt(III) trinitrate.

Qiuhong Li, Seik Weng Ng

Acta Crystallographica. Section E, Structure Reports Online

|May 18, 2011

Summary

This study details the crystal structure of a cobalt(III) complex where six dimethyl sulfoxide molecules octahedrally coordinate the metal atom. The crystal structure reveals specific symmetries for the metal atom and disordered nitrate ions.

Area of Science:

Coordination chemistry
Inorganic chemistry
Crystallography

Background:

Dimethyl sulfoxide (DMSO) is a versatile ligand in coordination chemistry.
Cobalt complexes exhibit diverse structural and electronic properties.
Understanding metal-ligand interactions is crucial for designing new materials.

Purpose of the Study:

To elucidate the crystal structure of the cobalt(III) complex with dimethyl sulfoxide.
To investigate the coordination geometry and symmetry of the complex.
To characterize the arrangement of nitrate counterions.

Main Methods:

Single-crystal X-ray diffraction was employed to determine the molecular and crystal structure.
Symmetry analysis was performed on the determined crystal structure.

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The coordination environment around the cobalt atom was analyzed.

Main Results:

The cobalt(III) ion is octahedrally coordinated by six dimethyl sulfoxide (DMSO) ligands.
The cobalt atom occupies a special position with specific site symmetry.
Nitrate anions exhibit distinct positional characteristics, with one showing disorder.

Conclusions:

The crystal structure provides detailed insights into the coordination behavior of DMSO with cobalt(III).
The observed symmetries highlight specific packing arrangements in the solid state.
The findings contribute to the understanding of metal-organic frameworks and coordination compounds.