Zinc: Inorganic & Coordination ChemistryBased in part on the article Zinc: Inorganic & Coordination Chemistry by Reg H. Prince which appeared in theEncyclopedia of Inorganic Chemistry, First Edition.

Abstract

Alloys and salts of zinc have been known for many centuries; commercial production of the metal dates from early in the eighteenth century. Of the several million tons now produced annually, by electrolytic and smelting processes, much is used in alloys, in batteries, in corrosion prevention, and in the manufacture of a range of compounds with various uses. In particular, zinc oxide and zinc chloride have a large number of uses, detailed in this article. Zinc sulfide is both one of the main zinc ores and the archetype for the two main structural forms of 4:4‐coordinated structures (zinc blende and wurtzite). Many zinc compounds and complexes have interesting structural, spectroscopic, optical, magnetic, and conductivity properties, some of which are of actual or potential value in technical and industrial applications. Zinc‐containing species have also proved valuable in synthesis and self‐assembly of a range of supramolecular structures. Both in the solid state and in solution zinc exhibits a range of coordination numbers, though tetrahedral and, especially in solution, octahedral stereochemistries dominate. Zinc forms a variety of complexes, especially with nitrogen, oxygen, sulfur, and halide donor ligands. Many of these complexes show high stability, but they are generally labile in solution. Zinc plays an essential role in biology, being a key constituent of at least 200 metalloproteins. It is an essential element in human nutrition, but toxic in large quantities. Many zinc complexes have been synthesized as biochemical models; a few zinc salts are used in dietary supplements.

Recovery of Pure Pd(II) from Spent Electroplating Solutions by Solvent Extraction with Ionic Liquids from Sulfuric Acid Leaching Solution of Cemented Pd

“…Since chloride ions are a hard base, Zn(II) has a stronger tendency to form chloro complexes than Pd(II). Compared to pure sulfuric acid solution, the extraction of Zn(II) is enhanced in the real leaching solution owing to the formation of Zn(II)-chloro complexes [34,42]. According to our results on the leaching of Pd and Zn metal, Pd metal would not be dissolved in the sulfuric acid solution when hydrogen peroxide is employed as an oxidizing agent [2], and thus the use of NaClO is necessary.…”

“…Compared to the complex formation constants of Pd(II) with sulfate/hydrogen sulfate ions, the complex formation constants with SCN − , I − and Br − are large, as represented in Table 2 [23,24,[30][31][32][33][34], and these complexes can be extracted by the ammonium cation of the corresponding ILs owing to their affinity. In addition, Pd(II) has a stronger tendency to form stable complexes with these inorganic anions than that of Zn(II), thus the selective separation could be obtained on the basis of the difference in formation of extracted complexes.…”

Comparison of force fields to study the zinc-finger containing protein NPL4, a target for Antabuse in cancer therapy

“…As observed for the minimal systems Npl4(Zn 2+ ) 129-151 , the non-bonded model in CHARMM36m showed a strong tendency to favor the entrance of additional water molecules in the coordination shell of Zn 2+ , increasing the coordination number to six and adopting octahedral coordination geometries. Octahedral geometries of Zn 2+ with six water molecules dominate in aqueous solution [102,103]. Thus, the performance of non-bonded parameters on our model systems using CHARMM36m reflects how the parameters have been developed, referring to complexes of Zn 2+ -water molecules [38].…”

Selective precipitation of ammonium hexachloropalladate from leaching solutions of cemented palladium with zinc

“…Zn(II) was not precipitated in these experimental conditions. Zn(II) has a strong tendency to form complex with chloride ions like ZnCl4 2 [23], which can react with NH4 + ion to form a soluble ammonium salt in solution [24]. The purity of Pd(IV) precipitate was over 99.99%.…”