Related Experiment Video
Updated: Jun 1, 2026

Synthesis of a Water-soluble Metal–Organic Complex Array
Published on: October 8, 2016
Poly[[aqua-bis(μ(3)-isonicotinato-κO:O':N)tris-(μ(2)-isonicotinato-κO,O':N)(nitrato-κO)bis-(μ(4)-oxalato-κO,O:O:O,O:O
Abstract:
In the title coordination polymer, {[Ag(4)Er(2)(C(6)H(4)NO(2))(5)(C(2)O(4))(2)(NO(3))(H(2)O)]·4H(2)O}(n), each Er(III) atom is coordinated in a bicapped trigonal-prismatic coordination geometry by three O atoms from two isonicotinate (IN) ligands, four O atoms from two oxalate ligands and one O atom from either a nitrate ion or a water mol-ecule, both of which are half-occupied over the same site. One Ag(I) atom has a Y-shaped geometry defined by one N atom from one IN ligand, one O atom from another IN ligand and one O atom from an oxalate ligand. The other Ag(I) atom is coordinated by two IN ligands and one O atom from an oxalate ligand. One of the IN ligands is disordered over an inversion center and forms a bridge between two centrosymmetric Ag(I) ions. Due to the disorder, this IN ligand coordinates to the Ag atom through either the pyridyl N or the carboxyl-ate O atoms. The IN and oxalate ligands link the Er and Ag atoms into a three-dimensional coordination framework. O-H⋯O and C-H⋯O hydrogen bonds are observed in the crystal structure.
Related Concept Videos
Structural Isomerism
Isomers are different chemical species that have the same chemical formula. Structural isomerism of coordination compounds can be divided into two subcategories, the linkage isomers and coordination-sphere isomers.
Linkage isomers occur when the coordination compound contains a ligand that can bind to the transition metal center through two different atoms. For example, the CN− ligand can bind through the carbon atom or through the nitrogen atom. Similarly, SCN− can be...
Coordination Compounds and Nomenclature
Valence Bond Theory
Formation of Complex Ions
Crystal Field Theory - Tetrahedral and Square Planar 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,...
Coordination Number and Geometry

