Related Experiment Video
Updated: Jul 14, 2026
16:11
Thermochemical Studies of Ni(II) and Zn(II) Ternary Complexes Using Ion Mobility-Mass Spectrometry
Published on: June 8, 2022
Ligand-controlled nuclearity in nickel bis(benzimidazolyl) complexes
Way-Zen Lee1, Huan-Sheng Tseng, Ting-Shen Kuo
1Department of Chemistry, National Taiwan Normal University, Taipei, 11650, Taiwan. wzlee@ntnu.edu.tw
Dalton Transactions (Cambridge, England : 2003)
|June 15, 2007
Summary
This study synthesized novel nickel(II) complexes using tripodal ligands. The ligand structure and coordinating groups influenced the nickel center
Area of Science:
- Coordination Chemistry
- Organometallic Chemistry
- Materials Science
Background:
- Nickel complexes are crucial in catalysis and materials science.
- Tripodal ligands offer unique coordination geometries.
- Understanding ligand effects on metal complex structure is key.
Purpose of the Study:
- Synthesize and characterize novel nickel(II) complexes with two distinct tripodal ligands.
- Investigate the influence of ligand structure on the geometry and nuclearity of nickel complexes.
- Explore the coordination behavior of sulfonamide-containing ligands.
Main Methods:
- Synthesis of nickel(II) complexes.
- Full characterization using spectroscopic and analytical techniques.
- X-ray crystallography for structural determination.
Main Results:
- Synthesized octahedral and tetrahedral nickel complexes.
- Demonstrated that ligand coordination mode (tridentate vs. bidentate) depends on ligand structure and co-ligands.
- Showed that nickel complex nuclearity is controllable via ligand design.
Conclusions:
- Tripodal ligand structure significantly dictates nickel complex geometry.
- Sulfonamide group's weak coordination and steric bulk affect ligand binding.
- Ligand design offers control over nickel complex nuclearity and properties.
More Related Videos
Related Concept Videos
02:51Metal-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...
01:09Complexation Equilibria: Factors Influencing Stability of Complexes
In complexation reactions, metal cations are the electron pair acceptors, and the ligands are the electron pair donors. The stability of the metal complexes depends primarily on the complexing ability of the central metal ion and the nature of the ligands. Generally, the complexing ability of the metal ion depends on the size and charge of the ion. As the metal ion size increases, the stability of the metal complexes decreases, provided that the valency of the metal ion and the ligands remain...
02:42Valence Bond Theory
Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...
01:19Complexation Equilibria: The Chelate Effect
In complexation reactions, metal atoms or cations interact with ligands to form donor-acceptor adducts called metal complexes. Ligands that bind through one donor site are monodentate, ligands with two donor sites are bidentate, and those with more than two donor sites are polydentate ligands. For example, ethylene diamine is a bidentate ligand that binds through two nitrogen donor atoms, forming a five-membered ring. EDTA is a polydentate ligand that binds through four oxygen and two nitrogen...
03:02Colors and Magnetism
Color in Coordination Complexes
When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human eye.
When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human eye.
01:07Ladder Diagrams: Complexation Equilibria
Ladder diagrams are useful for evaluating equilibria involving metal-ligand complexes. The vertical scale of the ladder diagram represents the concentration of unreacted or free ligand, pL. The horizontal lines on the scale depict the log of stepwise formation constants for metal-ligand complexes and indicate the dominant species in all the regions.
The formation constant, K1, for the formation of Cd(NH3)2+ complex from cadmium and ammonia is 3.55 × 102. Log K1 (i.e. pNH3) is 2.55, and...
The formation constant, K1, for the formation of Cd(NH3)2+ complex from cadmium and ammonia is 3.55 × 102. Log K1 (i.e. pNH3) is 2.55, and...