Three-dimensional microporous and mesoporous covalent organic frameworks based on cubic building units
Li Liao1, Xinyu Guan1, Haorui Zheng1
1State Key Laboratory of Inorganic Synthesis and Preparative Chemistry, Jilin University Changchun 130012 P. R. China postlh@jlu.edu.cn xdyao@jlu.edu.cn qrfang@jlu.edu.cn.
Chemical Science
|September 12, 2022
Summary
Researchers developed novel cubic building units for covalent organic frameworks (COFs), creating JUC-588 and JUC-589. These materials exhibit tunable porosity and high stability for gas adsorption and dye removal.
Area of Science:
- Materials Science
- Chemistry
Background:
- Covalent organic frameworks (COFs) are gaining attention for their diverse applications.
- Limited structural diversity in COFs hinders material development.
Purpose of the Study:
- To introduce novel cubic building units for creating new 3D imine-linked COFs.
- To achieve tunable porosity and enhanced properties in COFs.
Main Methods:
- Synthesis of two unusual cubic (8-connected) building units.
- Construction of 3D imine-linked COFs with bcu nets (JUC-588 and JUC-589).
- Characterization of pore structures, surface areas, and stability.
Main Results:
- Successfully synthesized JUC-588 and JUC-589 with bcu topology.
- Achieved tunable microporous and mesoporous structures with high surface areas (2728 m² g⁻¹ and 2482 m² g⁻¹).
- Demonstrated high CO₂/N₂ and CO₂/CH₄ selectivity, excellent H₂ uptake, and efficient dye adsorption.
Conclusions:
- The study presents a general strategy for designing stable 3D COF architectures with adjustable pores.
- Improving the valency of rigid building blocks is key to enhancing COF properties.
- The developed COFs show significant potential in gas separation and environmental remediation.
More Related Videos
Related Concept Videos
Network Covalent Solids
13.7K
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...
13.7K
Molecular Models
40.0K
Physical models representing molecular architectures of chemical compounds play essential roles in understanding chemistry. The use of molecular models makes it easier to visualize the structures and shapes of atoms and molecules.
40.0K
Crystal Field Theory - Tetrahedral and Square Planar Complexes
43.9K
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,...
43.9K
Crystal Field Theory - Octahedral Complexes
27.3K
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...
27.3K
Structures of Solids
14.5K
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...
14.5K
Ionic Crystal Structures
14.6K
Ionic crystals consist of two or more different kinds of ions that usually have different sizes. The packing of these ions into a crystal structure is more complex than the packing of metal atoms that are the same size.
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
14.6K


