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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...

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...

Valence Bond Theory

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Overview of Valence Bond Theory

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.

Noncovalent Attractions in Biomolecules

Noncovalent Attractions in Biomolecules

Noncovalent attractions are associations within and between molecules that influence the shape and structural stability of complexes. These interactions differ from covalent bonding in that they do not involve sharing of electrons.
Four types of noncovalent interactions are hydrogen bonds, van der Waals forces, ionic bonds, and hydrophobic interactions.
Hydrogen bonding results from the electrostatic attraction of a hydrogen atom covalently bonded to a strong-electronegative atom like oxygen,...

Noncovalent Attractions in Biomolecules

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Noncovalent attractions are associations within and between molecules that influence the shape and structural stability of complexes. These interactions differ from covalent bonding in that they do not involve sharing of electrons.
Four types of noncovalent interactions are hydrogen bonds, van der Waals forces, ionic bonds, and hydrophobic interactions.
Hydrogen bonding results from the electrostatic attraction of a hydrogen atom covalently bonded to a strong-electronegative atom like oxygen,...

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Construction and Systematical Symmetric Studies of a Series of Supramolecular Clusters with Binary or Ternary Ammonium Triphenylacetates

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Coordination chemistry beyond Werner: interplay between hydrogen bonding and coordination.

¹Leiden Institute of Chemistry, Gorlaeus Laboratories, Leiden University, P.O. Box 9502, 2300 RA Leiden, The Netherlands. reedijk@chem.leidenuniv.nl

Chemical Society Reviews

|August 21, 2012

Summary

Hydrogen bonding plays a crucial role in coordination compounds. This review explores its impact on molecular structure, reactivity, and crystal lattice stabilization in various coordination systems.

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Area of Science:

Coordination Chemistry
Supramolecular Chemistry
Chemical Bonding

Background:

Hydrogen bonding is a fundamental interaction in chemistry.
Coordination compounds exhibit diverse structural and reactive properties.
Understanding non-covalent interactions is key to designing functional materials.

Purpose of the Study:

To provide a tutorial review on the significance of hydrogen bonding in coordination chemistry.
To highlight the role of hydrogen bonds in stabilizing unusual coordination geometries and reactive species.
To discuss the influence of intermolecular hydrogen bonds on crystal lattices, including coordination polymers.

Main Methods:

Literature review of key studies on hydrogen bonding in coordination compounds.
Analysis of specific examples illustrating intramolecular and intermolecular hydrogen bonding.
Discussion of case studies involving coordination entities, anions, and crystal structures.

Main Results:

Intramolecular hydrogen bonding can stabilize unique coordination geometries and reactive intermediates.
Intermolecular hydrogen bonds between coordination complexes and anions are important for structural organization.
Hydrogen bonding significantly contributes to the stability of crystal lattices in coordination polymers.

Conclusions:

Hydrogen bonding is a versatile tool for controlling the structure, stability, and reactivity of coordination compounds.
The principles discussed are applicable to the design of novel coordination materials and supramolecular assemblies.
This review emphasizes the pervasive and critical role of hydrogen bonding across coordination chemistry.