Related Experiment Video
Updated: Aug 13, 2026

08:18
Microscopic Visualization of Porous Nanographenes Synthesized through a Combination of Solution and On-Surface Chemistry
Published on: March 4, 2021
Structure of Au8: planar or nonplanar?
1Computational Chemistry Laboratory, Corporate R&D, LG Chem Ltd., Research Park, Daejeon, 305-380, Korea. ykhan@lgchem.com
The Journal of Chemical Physics
|January 21, 2006
Summary
Density-functional theory and ab initio methods reveal the structures and stabilities of gold clusters. For gold 8 (Au8), ab initio calculations confirm the lowest energy isomer is planar.
Area of Science:
- Computational Chemistry
- Materials Science
- Quantum Chemistry
Background:
- Understanding the properties of small metal clusters is crucial for catalysis and nanomaterials.
- Gold clusters, in particular, exhibit unique electronic and structural characteristics.
- Previous studies have explored various gold cluster sizes using different theoretical approaches.
Purpose of the Study:
- To investigate the structural and stability properties of gold 6 (Au6) and gold 8 (Au8) clusters.
- To compare the results obtained from density-functional theory (DFT) and ab initio correlated methods.
- To determine the most stable isomeric structure for Au8.
Main Methods:
- Density-functional theory (DFT) calculations were employed.
- Ab initio correlated levels of theory were utilized for higher accuracy.
- Computational modeling was performed to analyze cluster geometries and energies.
Main Results:
- The study determined the lowest energy structures for Au6 and Au8 clusters.
- For Au8, ab initio calculations predict a planar lowest-energy isomer.
- DFT calculations also indicated a planar structure for the most stable Au8 isomer, showing agreement between methods.
Conclusions:
- Both DFT and ab initio methods provide valuable insights into gold cluster properties.
- The planar structure is predicted to be the most stable for the Au8 cluster.
- This work contributes to the fundamental understanding of gold cluster behavior.
Related Concept Videos
VSEPR Theory
Valence shell electron-pair repulsion theory (VSEPR theory) enables us to predict the molecular structure around a central atom from an examination of the number of bonds and lone electron pairs in its Lewis structure. The VSEPR model assumes that electron pairs in the valence shell of a central atom will adopt an arrangement that minimizes repulsions between these electron pairs by maximizing the distance between them. The electrons in the valence shell of a central atom form either bonding...
Structure of Amines
The hybridized nitrogen atom in amines possesses a lone pair of electrons and is bound to three substituents with a bond angle of around 108°, which is less than the tetrahedral angle of 109.5°. However, the C–N–H bond angle is slightly larger at 112°, with a carbon–nitrogen bond length of 147 pm. This carbon–nitrogen bond length of of amines is longer than the carbon–oxygen bond of alcohols (143 pm) but shorter than alkanes’ carbon–carbon bond (154 pm). These aspects are illustrated in Figure...
Crystal Field Theory - Tetrahedral and Square Planar Complexes
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,...
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,...
Metallic Solids
Metallic solids such as crystals of copper, aluminum, and iron are formed by metal atoms. The structure of metallic crystals is often described as a uniform distribution of atomic nuclei within a “sea” of delocalized electrons. The atoms within such a metallic solid are held together by a unique force known as metallic bonding that gives rise to many useful and varied bulk properties.
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability. Many...
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability. Many...
VSEPR Theory and the Basic Shapes
Overview of VSEPR Theory
Structures of Solids
Solids in which the atoms, ions, or molecules are arranged in a definite repeating pattern are known as crystalline solids. Metals and ionic compounds typically form ordered, crystalline solids. A crystalline solid has a precise melting temperature because each atom or molecule of the same type is held in place with the same forces or energy. Amorphous solids or non-crystalline solids (or, sometimes, glasses) which lack an ordered internal structure and are randomly arranged. Substances that...

