Related Experiment Video
Updated: Jun 1, 2026

Combining Solid-state and Solution-based Techniques: Synthesis and Reactivity of Chalcogenidoplumbates(II or IV)
Published on: December 29, 2016
Sesquicaesium hemisodium tetra-cyanidoplatinate(II) sesquihydrate
Andrew P Weber1, Milorad Stojanovic, Matthew R Pischek
1Department of Chemistry, University of South Alabama, Mobile, AL 36688-0002, USA.
Abstract:
The title compound, Cs(1.5)Na(0.5)[Pt(CN)(4)]·1.5H(2)O, was isolated from solution as a salt. The tetra-cyanidoplatinate (TCP) anions are stacked in a linear quasi-one-dimensional arrangement along the b axis, with Pt⋯Pt inter-actions of 3.6321 (5) Å. The mixed alkali metal TCP contains three distinct alkali metal positions in the structure that do not show any mixed occupancy: Cs1 (site symmetry 2), Cs2 (general position) and Na1 (site symmetry ). The Na(+) ion contains an octa-hedral coordination environment composed of two water mol-ecules and four N-terminal cyanides, which serve to bridge TCP anions. The Cs(+) cations contain mono- and bicapped square-prismatic environments, where the square prisms are formed from cyanide N atoms with water mol-ecules capping the faces. The 1.5 water mol-ecules per formula unit are a result of two fully occupied sites, one on a general position and one on a twofold rotation axis. Weak hydrogen-bonding inter-actions are observed between one water mol-ecule and terminal N-atom acceptors from TCP, while the second water mol-ecule is not involved in hydrogen bonding.
Related Concept Videos
Ionic Crystal Structures
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...
Unit Cells
Ionic Compounds: Formulas and Nomenclature
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,...
Ionic Bonding and Electron Transfer
Valence Bond Theory

