Crystal structures of ZnCl(2)·2.5H(2)O, ZnCl(2)·3H(2)O and ZnCl(2)·4.5H(2)O

The formation of different complexes in aqueous solutions is an important step in understanding the behavior of zinc chloride in water. The structure of concentrated ZnCl(2) solutions is governed by coordination competition of Cl(−) and H(2)O around Zn(2+). According to the solid–liquid phase diagram, the title compounds were crystallized below room temperature. The structure of ZnCl(2)·2.5H(2)O contains Zn(2+) both in a tetra­hedral coordination with Cl(−) and in an octa­hedral environment defined by five water mol­ecules and one Cl(−) shared with the [ZnCl(4)](2−) unit. Thus, these two different types of Zn(2+) cations form isolated units with composition [Zn(2)Cl(4)(H(2)O)(5)] (penta­aqua-μ-chlorido-tri­chlorido­di­zinc). The trihydrate {hexa­aqua­zinc tetra­chlorido­zinc, [Zn(H(2)O)(6)][ZnCl(4)]}, consists of three different Zn(2+) cations, one of which is tetra­hedrally coordinated by four Cl(−) anions. The two other Zn(2+) cations are each located on an inversion centre and are octa­hedrally surrounded by water mol­ecules. The [ZnCl(4)] tetra­hedra and [Zn(H(2)O)(6)] octa­hedra are arranged in alternating rows parallel to [001]. The structure of the 4.5-hydrate {hexa­aqua­zinc tetra­chlorido­zinc trihydrate, [Zn(H(2)O)(6)][ZnCl(4)]·3H(2)O}, consists of isolated octa­hedral [Zn(H(2)O)(6)] and tetra­hedral [ZnCl(4)] units, as well as additional lattice water mol­ecules. O—H⋯O hydrogen bonds between the water mol­ecules as donor and ZnCl(4) tetra­hedra and water mol­ecules as acceptor groups leads to the formation of a three-dimensional network in each of the three structures.