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Predicting Molecular Geometry02:27

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Tetrahedral Complexes
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...
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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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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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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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To explain the observed behavior of transition metal complexes (such as colors), a model involving electrostatic interactions between the electrons from the ligands and the electrons in the unhybridized d orbitals of the central metal atom has been developed. This electrostatic model is crystal field theory (CFT). It helps to understand, interpret, and predict the colors, magnetic behavior, and some structures of coordination compounds of transition metals.
CFT focuses on...

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β-Technetium trichloride: formation, structure, and first-principles calculations.

Frederic Poineau1, Erik V Johnstone, Philippe F Weck

  • 1Department of Chemistry, University of Nevada at Las Vegas, Las Vegas, Nevada 89154, USA. poineauf@unlv.nevada.edu

Inorganic Chemistry
|April 11, 2012
PubMed
Summary

A new form of technetium trichloride, beta-technetium trichloride, was discovered. This technetium compound exhibits metal-metal bonding and transforms into a more stable form over time.

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Area of Science:

  • Solid-state chemistry
  • Inorganic chemistry
  • Materials science

Background:

  • Technetium trichloride (TcCl3) exists in multiple forms.
  • Understanding the structural and bonding properties of technetium halides is crucial for materials science.

Purpose of the Study:

  • To identify and characterize a new polymorph of technetium trichloride.
  • To investigate the structural features and stability of the newly identified phase.

Main Methods:

  • Synthesis of beta-technetium trichloride (β-TcCl(3)) via reaction of technetium metal with chlorine gas.
  • Structural analysis of the resulting compound.

Main Results:

  • Identification of a second polymorph of technetium trichloride, β-TcCl(3).
  • The structure features infinite layers of edge-sharing octahedra with a Tc-Tc distance of 2.861(3) Å, indicating metal-metal bonding.
  • β-TcCl(3) was found to be less stable than the alpha polymorph, slowly transforming into α-TcCl(3) (Tc(3)Cl(9)) at elevated temperatures.

Conclusions:

  • The discovery of β-TcCl(3) expands the known structural diversity of technetium halides.
  • The observed metal-metal bonding in β-TcCl(3) provides insights into the electronic properties of technetium compounds.
  • The lower stability of β-TcCl(3) compared to α-TcCl(3) is consistent with theoretical predictions and highlights the importance of polymorph stability in chemical synthesis.