Zinc coordination compounds materials

The first brief review on ° Zn SSNMR spectroscopy was written by Wu in 1998 [11]. Two overviews of Zn SSNMR later appeared in 2001 [12] and 2002 [13]. These reviews were mainly focused on the applications of Zn SSNMR spectroscopy to several inorganic materials and coordination compounds. EUis and Lipton later pubfished a review with particular attention being paid to the low-temperature SSNMR experimental methods designed for Zn and Mg [14]. In the book of The Chemistry of Organozinc Compounds, Zn NMR spectroscopy ofboth solution and sofids was briefly reviewed [15]. The research paper by Power and co-worker pubfished in 2010 provides a survey of Zn NMR parameters in sofids [16]. Very recently, Zn SSNMR spectroscopy of zinc-binding proteins was briefly summarized [17]. Here, we set out to provide a concise, but complete, overview of the literature relevant to Zn SSNMR spectroscopy up to early 2013. It is our hope that the article will encourage more people to choose Zn SSNMR spectroscopy as a tool for solving the problems encountered in their research. 

Zinc phosphates and phosphonates can form highly interesting coordination networks, some in the presence of additional ligands. A number of compounds that have useful properties for the formation of zinc phosphate materials will also be discussed. 

When 2-cyanoethylzinc iodide is recrystallized from THF, a crystalline material is obtained. This material appeared to be the mono-THF adduct of 2-cyanoethylzinc iodide which exists in the solid state as a coordination polymer via coordination of the cyanide functionality to an adjacent zinc atom. Coordination saturation at zinc is reached by the coordination of an additional THF molecule. No further structural data have been given for this compound . 

Cadmium is a member of Group 12 (Zn, Cd, Hg) of the Periodic Table, having a filled d shell of electrons 4valence state of +2. In rare instances the +1 oxidation state may be produced in the form of dimeric Cd2+2 species [59458-73-0], eg, as dark red melts of Cd° dissolved in molten cadmium halides or as diamagnetic yellow solids such as (Cd2)2+ (AlCl [79110-87-5] (2). The Cd + species is unstable in water or other donor solvents, immediately disproportionating to Cd2+ and Cd. In general, cadmium compounds exhibit properties similar to the corresponding zinc compounds. Compounds and properties are listed in Table 1. Cadmium(TT) [22537 48-0] tends to favor tetrahedral coordination in its compounds, particularly in solution as complexes, eg, tetraamminecadmium(II) [18373-05-2], Cd(NH3)2+4. However, solid-state cadmium-containing oxide or halide materials frequently exhibit octahedral coordination at the Cd2+ ion, eg, the rock-salt structure found for CdO. 

Thermogravimetric analyses show that the cobalt, nickel, and zinc complexes lose all six water molecules within the temperature range 100-130°. The copper and iron complexes lose four of the water molecules in this temperature range, and the remaining two coordinated water molecules are lost at 230°. The zinc-saccharin complex shows the largest thermal stability. For this compound pyrolysis of the carbonaceous material begins at —400°. The iron complex decomposes at - 300°, the cobalt complex at 350°, the nickel complex at 370°, and the copper complex at 270° the end product in each case is the corresponding metal oxide. 

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