Related Experiment Video
Updated: Jul 4, 2026

11:27
Synthesis and Characterization of Functionalized Metal-organic Frameworks
Published on: September 5, 2014
Robust metal-organic framework enforced by triple-framework interpenetration exhibiting high H2 storage density
Ming Xue1, Shengqian Ma, Zhao Jin
1State Key Laboratory of Inorganic Synthesis & Preparative Chemistry, Jilin University, Changchun, China.
Inorganic Chemistry
|June 28, 2008
Summary
A novel metal-organic framework, Zn2(CNC)2(DPT).G, was synthesized. This robust material demonstrates significant hydrogen uptake and storage capacity, making it promising for hydrogen storage applications.
Area of Science:
- Materials Science
- Chemistry
- Nanotechnology
Background:
- Metal-organic frameworks (MOFs) are porous materials with potential applications in gas storage.
- Developing robust MOFs with high storage capacity is crucial for practical applications.
Purpose of the Study:
- To synthesize and characterize a new microporous metal-organic framework.
- To evaluate the hydrogen uptake and storage properties of the synthesized MOF.
Main Methods:
- Synthesis of Zn2(CNC)2(DPT).G using 4-Carboxycinnamic (CNC) and 3,6-Di-4-pyridyl-1,2,4,5-tetrazine (DPT).
- Structural characterization using X-ray diffraction.
- Hydrogen gas uptake measurements at 1 atm and 77 K.
Main Results:
- The MOF features a triply interpenetrated primitive cubic net with 1D pores (approx. 3.7 A).
- The framework exhibits high robustness due to triple interpenetration.
- Activated MOF (1b) achieved 1.28 wt % hydrogen uptake.
- A high hydrogen storage density of 95.2% was observed.
Conclusions:
- The synthesized MOF, Zn2(CNC)2(DPT).G, is a robust and porous material.
- The MOF demonstrates excellent hydrogen storage capabilities, indicating its potential for practical hydrogen storage solutions.
Related Concept Videos
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...
Metal-Ligand Bonds
The hemoglobin in the blood, the chlorophyll in green plants, vitamin B-12, and the catalyst used in the manufacture of polyethylene all contain coordination compounds. Ions of the metals, especially the transition metals, are likely to form complexes.
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
Bonding in Metals
Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Drüde called the “Electron Sea Model”.
Properties of Organometallic Compounds
Organometallic compounds are compounds that contain a carbon–metal bond. Carbon belongs to an organyl group like alkyl, aryl, allyl, or benzyl groups. The metal can be from Group I or Group II of the periodic table, a transition metal, or a semimetal.
Electrophilic 1,2- and 1,4-Addition of HX to 1,3-Butadiene
The electrophilic addition of hydrogen halides such as HBr to alkenes and nonconjugated dienes gives a single product as per Markovnikov’s rule.
Network Covalent Solids
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...

