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Related Concept Videos

Coordination Compounds and Nomenclature02:54

Coordination Compounds and Nomenclature

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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...
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Coordination Number and Geometry02:57

Coordination Number and Geometry

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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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Ionic Crystal Structures02:42

Ionic Crystal Structures

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Ionic crystals consist of two or more different kinds of ions that usually have different sizes. The packing of these ions into a crystal structure is more complex than the packing of metal atoms that are the same size.
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
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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...
20.6K
Structural Isomerism02:34

Structural Isomerism

19.1K
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...
19.1K
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Valence Bond Theory

8.5K
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...
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Related Experiment Video

Updated: Jun 10, 2025

Manganese Oxide Nanoparticle Synthesis by Thermal Decomposition of ManganeseII Acetylacetonate
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Manganese Oxide Nanoparticle Synthesis by Thermal Decomposition of ManganeseII Acetylacetonate

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N-Oxide Coordination to Mn(III) Chloride.

Ananya Saju1, Matthew R Crawley1, Samantha N MacMillan2

  • 1Department of Chemistry, University at Buffalo, State University of New York, Buffalo, NY 14260, USA.

Molecules (Basel, Switzerland)
|October 16, 2024
PubMed
Summary

Manganese(III) chloride complexes with N-oxide ligands are reactive and decompose to manganese(II). These complexes can chlorinate organic compounds like hexamethylbenzene, demonstrating unique reactivity influenced by N-oxide coordination.

Keywords:
C–H chlorinationMn(III)N-oxide ligandscoordination chemistry

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Area of Science:

  • Inorganic Chemistry
  • Organometallic Chemistry
  • Materials Science

Background:

  • Manganese(III) chloride (MnCl3) complexes are of interest due to their variable oxidation states and potential catalytic applications.
  • N-oxide ligands, such as trimethyl-N-oxide (Me3NO) and pyridine-N-oxide (PyNO), can influence the electronic and steric properties of metal complexes.
  • Understanding the reactivity of Mn(III) complexes is crucial for developing new synthetic methodologies and catalytic systems.

Purpose of the Study:

  • To synthesize and characterize Mn(III) chloride complexes coordinated with N-oxide ylide ligands.
  • To investigate the reactivity and decomposition pathways of these novel Mn(III) complexes.
  • To explore the influence of N-oxide coordination on the reduction potential and reactivity of Mn(III) complexes.

Main Methods:

  • Synthesis of Mn(III) chloride complexes with trimethyl-N-oxide and pyridine-N-oxide ligands.
  • Characterization of the synthesized compounds using spectroscopic and crystallographic techniques.
  • Reactivity studies involving decomposition pathways and reactions with organic substrates like hexamethylbenzene (HMB).

Main Results:

  • Novel Mn(III) chloride complexes with Me3NO and PyNO ligands were successfully synthesized and characterized.
  • These complexes exhibit significant reactivity, readily decomposing to Mn(II) species, such as the 2D polymeric network [MnII(µ-Cl)3MnII(µ-ONMe3)]n[MnII(µ-Cl)3]n·(Me3NO·HCl)3n.
  • Reaction with HMB yielded the chlorinated product 1-chloromethyl-2,3,4,5,6-pentamethylbenzene, indicating chlorinating capabilities.
  • In contrast, reaction with TEMPO resulted in electron transfer, forming a manganate species rather than an adduct.

Conclusions:

  • N-oxide ylide ligands play a crucial role in stabilizing and modulating the reactivity of Mn(III) chloride complexes.
  • The observed decomposition and chlorination reactions highlight the potential of these complexes as reactive intermediates or precursors.
  • The distinct reactivity observed with TEMPO suggests that the electronic properties imparted by N-oxide coordination significantly influence redox behavior.