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In its compounds, Zn 2+ ions have an electronic configuration [Ar] 3d 10.As such, Zn 2+ tends to have a symmetrical coordination geometry in both its complexes and compounds. In both ZnO and ZnS, zinc is bound tetrahedrally bound to four ligands (oxide and sulfide, respectively).
Zinc nitrate is usually prepared by dissolving zinc metal, zinc oxide, or related materials in nitric acid: Zn + 2 HNO 3 → Zn(NO 3) 2 + H 2 ZnO + 2 HNO 3 → Zn(NO 3) 2 + H 2 O. These reactions are accompanied by the hydration of the zinc nitrate.
Zinc hydroxide Zn() 2 is an inorganic chemical compound.It also occurs naturally as 3 rare minerals: wülfingite (orthorhombic), ashoverite and sweetite (both tetragonal). Like the hydroxides of other metals, such as lead, aluminium, beryllium, tin and chromium, Zinc hydroxide (and Zinc oxide), is amphoteric.
[25] [137] Another alloy, marketed under the brand name Prestal, contains 78% zinc and 22% aluminium, and is reported to be nearly as strong as steel but as malleable as plastic. [ 25 ] [ 138 ] This superplasticity of the alloy allows it to be molded using die casts made of ceramics and cement.
The name of the metal was first documented in the 16th century, [40] [41] and is probably derived from the German zinke for the needle-like appearance of metallic crystals. [42] Alchemical symbol for the element zinc. The isolation of metallic zinc in the West may have been achieved independently by several people in the 17th century. [43]
Solutions of sodium zincate may be prepared by dissolving zinc, zinc hydroxide, or zinc oxide in an aqueous solution of sodium hydroxide. [2] Simplified equations for these complex processes are:
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Zn(CN) 2 is easy to make by combining aqueous solutions of cyanide and zinc ions, for example via the double replacement reaction between KCN and ZnSO 4: [5] ZnSO 4 + 2 KCN → Zn(CN) 2 + K 2 SO 4