Related Experiment Video
Updated: Nov 9, 2025

07:57
Author Spotlight: A Rapid, Microwave-Assisted Hydrothermal Synthesis Of Nickel Hydroxide Nanosheets
Published on: August 18, 2023
2.2K
Nickel(II) Complex with a Flexidentate Ligand Derived from Acetohydrazide: Synthesis, Structural Characterization and
Acta Chimica Slovenica
|April 15, 2021
Summary
A new mononuclear Nickel(II) complex, [Ni(Lp)2(CH3OH)2]Cl2, was synthesized and characterized. X-ray crystallography revealed a distorted octahedral geometry, with detailed analysis of intermolecular interactions.
Area of Science:
- Coordination Chemistry
- Inorganic Synthesis
- Crystallography
Background:
- Nickel(II) complexes are crucial in catalysis and materials science.
- Understanding ligand behavior in metal complex formation is key.
- Pyrazole ligands offer versatile coordination modes.
Purpose of the Study:
- To synthesize and characterize a novel mononuclear Nickel(II) complex.
- To elucidate the coordination environment and geometry of the Nickel(II) center.
- To investigate intermolecular interactions within the crystal structure.
Main Methods:
- Synthesis of the Nickel(II) complex via reaction of a pyrazole precursor with NiCl2·6H2O.
- Structure determination using single-crystal X-ray crystallography.
- Analysis of intermolecular contacts using Hirshfeld surface analysis.
Main Results:
- Formation of the mononuclear complex [Ni(Lp)2(CH3OH)2]Cl2.
- The Ni(II) ion exhibits a six-coordinate, distorted octahedral geometry.
- Pyrazole ligands act as bidentate neutral ligands.
- Hirshfeld surface analysis identified H/H and Cl/H as dominant intermolecular interactions.
Conclusions:
- The study successfully synthesized and structurally characterized a novel Nickel(II) complex.
- The coordination chemistry and crystal packing of the complex were elucidated.
- Hirshfeld surface analysis provided insights into the nature of intermolecular forces governing crystal structure.
Related Concept Videos
Valence Bond Theory
10.0K
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...
10.0K
Crystal Field Theory - Tetrahedral and Square Planar Complexes
45.8K
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,...
45.8K
Crystal Field Theory - Octahedral Complexes
28.7K
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...
28.7K
Complexometric Titration: Ligands
1.6K
Different monodentate and polydentate ligands are used as complexing agents in complexometric titration reactions. The formation of complexes by mono- and bidentate ligands involves two or more intermediate steps, limiting their use as complexing agents. In comparison, polydentate ligands can form complexes with metal ions in a single-step process, facilitating sharper end points. This means polydentate ligands, such as amino carboxylic acid derivatives, are most commonly employed in...
1.6K
Metal-Ligand Bonds
22.6K
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...
22.6K
Coordination Number and Geometry
17.3K
For transition metal complexes, the coordination number determines the geometry around the central metal ion. Table 1 compares coordination numbers to molecular geometry. The most common structures of the complexes in coordination compounds are octahedral, tetrahedral, and square planar.
17.3K

