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Types of Chemical Bonds02:37

Types of Chemical Bonds

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Chemical bonding theories were pioneered by American chemist Gilbert N. Lewis. He developed a model called the Lewis model to explain the type and formation of different bonds. Chemical bonding is central to chemistry; it explains how atoms or ions bond together to form molecules. It explains why some bonds are strong and others are weak, or why one carbon bonds with two oxygens and not three; why water is H2O and not H4O. 
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Atoms participate in a chemical bond formation to acquire a completed valence-shell electron configuration similar to that of the noble gas nearest to it in atomic number. Ionic, covalent, and metallic bonds are some of the important types of chemical bonds. Bond energy and bond length determine the strength of a chemical bond.
Types of Chemical Bonds
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Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual attraction of atoms for a “shared” pair of electrons.
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Chemical Bonds
The electrons of the outermost energy level determine the energetic stability of the atom and its tendency to form chemical bonds with other atoms. The innermost electron shell has a maximum capacity of two electrons, but the next two electron shells can each have a maximum of eight electrons. This is known as the octet rule, which states that, with the exception of the innermost shell, atoms are most stable energetically when they have eight electrons in their valence shell, the...
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Olefins, which are unsaturated hydrocarbons containing one or more carbon–carbon double bonds, are broadly divided into alkenes and cycloalkenes. The general chemical formula of an alkene is CnH2n.
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Uranocenium: Synthesis, Structure, and Chemical Bonding.

Fu-Sheng Guo1, Yan-Cong Chen2, Ming-Liang Tong2

  • 1Department of Chemistry, University of Sussex, Falmer, Brighton, BN1 9QR, UK.

Angewandte Chemie (International Ed. in English)
|April 30, 2019
PubMed
Summary
This summary is machine-generated.

Researchers synthesized a cationic uranium(III) metallocene, revealing significant covalent bonding due to uranium 5f orbital mixing. This covalency influences its magnetic properties, causing quenched anisotropy and fast relaxation.

Keywords:
chemical bondingelectronic structuremagnetic propertiesmetallocenesuranium

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Area of Science:

  • Organometallic Chemistry
  • Inorganic Chemistry
  • Uranium Chemistry

Background:

  • Uranium metallocenes are key compounds for studying uranium's electronic structure and bonding.
  • Understanding the nature of metal-ligand interactions in actinide complexes is crucial for predicting their properties.

Purpose of the Study:

  • To synthesize and characterize a cationic uranium(III) metallocene.
  • To investigate the electronic structure and bonding characteristics of the uranium center.
  • To explore the dynamic magnetic properties influenced by electronic structure.

Main Methods:

  • Synthesis of [(η⁵-C₅ⁱPr₅)₂UI] and subsequent abstraction of iodide.
  • Structural analysis of the resulting cationic uranium(III) metallocene, [(η⁵-C₅ⁱPr₅)₂U]⁺.
  • Computational analysis of uranium 5f orbital mixing with ligand orbitals.
  • Investigation of dynamic magnetic properties, including magnetic relaxation.

Main Results:

  • Successful synthesis of the cationic uranium(III) metallocene [(η⁵-C₅ⁱPr₅)₂U]⁺[B(C₆F₅)₄]⁻.
  • Structural determination revealed unsymmetrical cyclopentadienyl bonding and a bent uranium core.
  • Analysis showed significant uranium 5f orbital mixing with ligand orbitals, indicating covalent contributions.
  • Dynamic magnetic studies demonstrated partially quenched anisotropy and fast magnetic relaxation in zero field due to 5f covalency.

Conclusions:

  • The cationic uranium(III) metallocene exhibits significant covalency in its U-ligand bonding.
  • 5f orbital covalency plays a critical role in the observed magnetic properties, including anisotropy and relaxation.
  • Magnetic field application alters relaxation mechanisms, highlighting the complex interplay of electronic structure and magnetism.