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Related Concept Videos

Metal-Ligand Bonds02:51

Metal-Ligand Bonds

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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...
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Structural Isomerism02:34

Structural Isomerism

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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,...
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Valence Bond Theory02:42

Valence Bond Theory

11.9K
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...
11.9K
Valence Bond Theory02:45

Valence Bond Theory

52.0K
Overview of Valence Bond Theory
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Coordination Compounds and Nomenclature02:54

Coordination Compounds and Nomenclature

28.5K
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...
28.5K
Lewis Structures of Molecular Compounds and Polyatomic Ions02:54

Lewis Structures of Molecular Compounds and Polyatomic Ions

49.0K
To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:
49.0K

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Synthesis of a Thiol Building Block for the Crystallization of a Semiconducting Gyroidal Metal-sulfur Framework
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SO₂--yet another two-faced ligand.

Jingbai Li1, Andrey Yu Rogachev

  • 1Department of Biological and Chemical Sciences, Illinois Institute of Technology, Chicago, Illinois 60616, USA. andrey.rogachev@iit.edu andrey.rogachev@gmail.com.

Physical Chemistry Chemical Physics : PCCP
|December 6, 2014
PubMed
Summary

Sulfur dioxide (SO2) exhibits dual bonding roles in transition metal complexes, acting as an acceptor in d(8)/d(10) metals and a donor in others. This behavior dictates distinct adduct geometries and bonding interactions.

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Area of Science:

  • Inorganic Chemistry
  • Organometallic Chemistry
  • Computational Chemistry

Background:

  • Transition metal complexes form adducts with sulfur dioxide (SO2).
  • Experimentally observed adducts display varied geometries.
  • Understanding SO2's coordination behavior is key to predicting complex structures.

Purpose of the Study:

  • To analyze the bonding interactions between SO2 and transition metal complexes.
  • To elucidate the factors governing SO2's donor and acceptor roles.
  • To correlate bonding modes with observed adduct geometries.

Main Methods:

  • Bonding analysis using Natural Bond Orbital (NBO) analysis.
  • Energy Decomposition Analysis (EDA) to quantify interaction energies.
  • Computational modeling of SO2 adducts with d(8), d(10), and other transition metal complexes.

Main Results:

  • SO2 acts as an acceptor in square-planar d(8) and linear d(10) metal complexes, with Lewis Acidic Orbital (LAO) on sulfur accepting from metal's dz(2) orbital.
  • SO2 acts as a donor in paddle-wheel and square-pyramidal complexes, with its lone pair donating to metal-based acceptor orbitals.
  • Coordination geometry (bent vs. linear) is directly linked to SO2's donor/acceptor role.

Conclusions:

  • The bonding analysis explains the distinct geometries of SO2 transition metal adducts.
  • SO2's electronic properties allow it to function as both a Lewis acid and a Lewis base.
  • Computational methods provide insights into fundamental chemical bonding principles.