在低指数CeO2表面上吸附的弱结合的CO分子:使用嵌入式集群模型进行CCSD (T) 基准研究的一个案例
1Institut für Nanotechnologie, Karlsruher Institut für Technologie (KIT), Kaiserstraße 12, 76131 Karlsruhe, Germany.
The Journal of chemical physics
|January 13, 2026
概括
本研究使用先进的计算方法对二氧化 (CeO2) 表面的一氧化碳 (CO) 吸附进行了基准测试. 结果显示,理论和实验振动频率之间有很好的一致性,证实了低指数CeO2表面的物理吸收.
科学领域:
- 计算化学计算化学
- 表面科学是一门学科.
- 材料科学 材料科学 材料科学
背景情况:
- 了解像一氧化碳 (CO) 这样的探头分子在金属氧化物表面上的吸附对于催化和表面科学至关重要.
- 二氧化 (CeO2) 是由于其独特的氧化还原特性和催化中的应用而被广泛研究的材料.
研究的目的:
- 为了对低指数 CeO2 表面上吸附的 CO 的结合能和振动拉伸频率进行基准测试 [(100), (110) 和 (111) ].
- 为了比较理论计算与实验数据对CO吸附在CeO2.
- 为了研究这些表面上CO的吸附特性 (物理吸附与化学吸附).
主要方法:
- 采用结合集群单,双,扰动三重 [CCSD(T] 方法与嵌入式集群方法.
- 使用了def2-TZ/QZVPP基础集进行高精度计算.
- 计算的振动频率,包括无声调整和吸附能量.
主要成果:
- 在CeO2{100}和CeO2{111}表面上的理论CO振动频率与实验值相一致 (分别有17厘米-1和12厘米-1的差异).
- 对于CeO2(110) 表面,理论值低于实验特征 (-7 cm-1和-21 cm-1).
- 吸附能量证实了CO在所有三个低指数CeO2表面的物理吸附特性,其值从-0.17到-0.40 eV不等.
结论:
- 该CCSD (T) 方法可提供可靠的预测,用于低指数CeO2表面的CO吸附.
- 这项研究证实了CO在CeO2{100}, (110) 和 (111) 表面上的物理吸收性质.
- 在 (110) 表面的差异可能表明复杂的吸附动态或多个配置.
相关概念视频
Crystal Field Theory - Octahedral Complexes
30.6K
Crystal Field Theory
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...
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...
30.6K
MO Theory and Covalent Bonding
13.5K
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...
13.5K
Noncovalent Attractions in Biomolecules
19.2K
19.2K
Noncovalent Attractions in Biomolecules
63.0K
Noncovalent attractions are associations within and between molecules that influence the shape and structural stability of complexes. These interactions differ from covalent bonding in that they do not involve sharing of electrons.
Four types of noncovalent interactions are hydrogen bonds, van der Waals forces, ionic bonds, and hydrophobic interactions.
Hydrogen bonding results from the electrostatic attraction of a hydrogen atom covalently bonded to a strong-electronegative atom like oxygen,...
Four types of noncovalent interactions are hydrogen bonds, van der Waals forces, ionic bonds, and hydrophobic interactions.
Hydrogen bonding results from the electrostatic attraction of a hydrogen atom covalently bonded to a strong-electronegative atom like oxygen,...
63.0K
Lattice Centering and Coordination Number
11.4K
The structure of a crystalline solid, whether a metal or not, is best described by considering its simplest repeating unit, which is referred to as its unit cell. The unit cell consists of lattice points that represent the locations of atoms or ions. The entire structure then consists of this unit cell repeating in three dimensions. The three different types of unit cells present in the cubic lattice are illustrated in Figure 1.
Types of Unit Cells
Imagine taking a large number of identical...
Types of Unit Cells
Imagine taking a large number of identical...
11.4K
Network Covalent Solids
16.0K
Network covalent solids contain a three-dimensional network of covalently bonded atoms as found in the crystal structures of nonmetals like diamond, graphite, silicon, and some covalent compounds, such as silicon dioxide (sand) and silicon carbide (carborundum, the abrasive on sandpaper). Many minerals have networks of covalent bonds.
To break or to melt a covalent network solid, covalent bonds must be broken. Because covalent bonds are relatively strong, covalent network solids are typically...
To break or to melt a covalent network solid, covalent bonds must be broken. Because covalent bonds are relatively strong, covalent network solids are typically...
16.0K


