Benchmarking electronic structure calculations on the bare UO2(2+) ion: how different are single and multireference
Florent Réal1, André Severo Pereira Gomes, Lucas Visscher
1Université Lille1 (Sciences et Technologies), Laboratoire PhLAM, CNRS UMR 8523, CERLA, CNRS FR 2416, Villeneuve d'Ascq, France.
The Journal of Physical Chemistry. A
|November 6, 2009
Summary
Comparing computational methods for actinide molecules, this study finds that coupled cluster (CC) methods align well, while CASPT2 shows discrepancies. Electron correlation, not spin-orbit coupling, is the primary cause of differing results for uranyl ions.
Area of Science:
- Computational Chemistry
- Quantum Chemistry
- Spectroscopy of Actinides
Background:
- Discrepancies exist between CASPT2 and linear response coupled cluster (LRCC) methods for uranyl (UO22+) ion spectra.
- The reliability of these methods for actinide-containing molecules is questioned, particularly concerning spin-orbit coupling effects.
Purpose of the Study:
- To compare the accuracy of CASPT2 and LRCC methods for actinide spectroscopy.
- To evaluate the performance of these methods against the four-component intermediate Hamiltonian Fock-space coupled cluster (IHFSCC) method.
Main Methods:
- Utilized the four-component intermediate Hamiltonian Fock-space coupled cluster (IHFSCC) method as a benchmark.
- Compared CASPT2 and LRCC calculations for the uranyl (UO22+) ion.
- Analyzed the impact of electron correlation and spin-orbit coupling on spectral descriptions.
Main Results:
- Electron correlation, rather than spin-orbit coupling, is identified as the main source of discrepancies between methods.
- IHFSCC and LRCC show strong agreement in describing excited states, with minor blue-shifts in LRCC energies.
- CASPT2 agrees with IHFSCC on individual frequencies but less so on the overall spectrum due to differences in recovered correlation.
Conclusions:
- For uranyl ions, IHFSCC and LRCC provide reliable descriptions of electronic spectra.
- CASPT2 may be less suitable for comprehensive actinide spectral analysis compared to LRCC and IHFSCC.
- Accurate treatment of electron correlation is crucial for high-fidelity actinide spectroscopy.
Related Concept Videos
Electron Configurations
Electron configurations and orbital diagrams can be determined by applying the Aufbau principle (each added electron occupies the subshell of lowest energy available), Pauli exclusion principle (no two electrons can have the same set of four quantum numbers), and Hund’s rule of maximum multiplicity (whenever possible, electrons retain unpaired spins in degenerate orbitals).
The relative energies of the subshells determine the order in which atomic orbitals are filled (1s, 2s, 2p, 3s, 3p, 4s,...
The relative energies of the subshells determine the order in which atomic orbitals are filled (1s, 2s, 2p, 3s, 3p, 4s,...
Molecular Orbital Theory II
Molecular Orbital Energy Diagrams
Electronic Structure of Atoms
An atom comprises protons and neutrons, which are contained inside the dense, central core called the nucleus, with electrons present around the nucleus. Taking into account the wave–particle duality of electrons and the uncertainty in position around the nucleus, quantum mechanics provides a more accurate model for the atomic structure. It describes atomic orbitals as the regions around the nucleus where electrons of discrete energy exist, characterized by four quantum numbers: n, l, ml, and...
MO Theory and Covalent Bonding
The molecular orbital theory describes the distribution of electrons in molecules in a manner similar to the distribution of electrons in atomic orbitals. The region of space in which a valence electron in a molecule is likely to be found is called a molecular orbital. Mathematically, the linear combination of atomic orbitals (LCAO) generates molecular orbitals. Combinations of in-phase atomic orbital wave functions result in regions with a high probability of electron density, while...
The Aufbau Principle and Hund's Rule
To determine the electron configuration for any particular atom, we can build the structures in the order of atomic numbers. Beginning with hydrogen, and continuing across the periods of the periodic table, we add one proton at a time to the nucleus and one electron to the proper subshell until we have described the electron configurations of all the elements. This procedure is called the aufbau principle, from the German word aufbau (“to build up”). Each added electron occupies the subshell of...
Electron Orbital Model
Orbitals are the areas outside of the atomic nucleus where electrons are most likely to reside. They are characterized by different energy levels, shapes, and three-dimensional orientations. The location of electrons is described most generally by a shell or principal energy level, then by a subshell within each shell, and finally, by individual orbitals found within the subshells.The first shell is closest to the nucleus, and it has only one subshell with a single spherical orbital called the...


