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Valence Bond Theory02:42

Valence Bond Theory

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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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Overview of Valence Bond Theory
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In complexation reactions, metal cations are the electron pair acceptors, and the ligands are the electron pair donors. The stability of the metal complexes depends primarily on the complexing ability of the central metal ion and the nature of the ligands. Generally, the complexing ability of the metal ion depends on the size and charge of the ion. As the metal ion size increases, the stability of the metal complexes decreases, provided that the valency of the metal ion and the ligands remain...
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Metal-Ligand Bonds02:51

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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.
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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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Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence shell, and an anion (a negative ion) forms when a neutral atom gains one or more electrons in its valence shell. Compounds composed of ions are called ionic compounds (or salts), and their constituent ions are held together by ionic bonds: electrostatic forces of attraction between oppositely charged cations and anions. 
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Author Spotlight: Experimental Approaches for the Synthesis of Low-Valent Metal-Organic Frameworks from Multitopic Phosphine Linkers
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Neutral zero-valent s-block complexes with strong multiple bonding.

Merle Arrowsmith1, Holger Braunschweig1, Mehmet Ali Celik1

  • 1Institut für Anorganische Chemie, Julius-Maximilians-Universität Würzburg, Am Hubland, 97074 Würzburg, Germany.

Nature Chemistry
|June 24, 2016
PubMed
Summary
This summary is machine-generated.

Researchers synthesized the first neutral zero-valent beryllium compounds using stabilizing ligands. These brightly colored complexes exhibit strong beryllium-carbon bonding and unusual stability due to a unique three-center π bond.

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Area of Science:

  • Inorganic Chemistry
  • Organometallic Chemistry
  • Main-Group Chemistry

Background:

  • S-block metals are typically strong electron donors, forming complexes with metals in high oxidation states.
  • Low-valent main-group compounds are gaining interest for their unique reactivities, comparable to transition metal complexes.

Purpose of the Study:

  • To isolate and characterize the first neutral compounds featuring a zero-valent s-block metal, specifically beryllium.
  • To investigate the bonding and stability of these novel low-valent beryllium complexes.

Main Methods:

  • Synthesis of novel beryllium complexes utilizing stabilizing cyclic (alkyl)(amino)carbene ligands.
  • Characterization through structural, spectroscopic (e.g., NMR, UV-Vis), and theoretical (e.g., DFT) analyses.

Main Results:

  • Isolation and characterization of the first neutral zero-valent beryllium compounds.
  • Observation of very short beryllium-carbon bond lengths and linear coordination geometries, indicating strong Be-C multiple bonding.
  • Confirmation of a closed-shell singlet configuration with a Be(0) center, stabilized by a three-center two-electron π bond.

Conclusions:

  • Neutral, low-valent beryllium compounds can be stabilized, challenging previous assumptions about beryllium chemistry.
  • The observed strong Be-C bonding and stability are attributed to significant π-backbonding and a unique C-Be-C three-center two-electron π system.
  • These findings open new avenues for exploring the chemistry of low-valent main-group elements.