Zinc under normal conditions is fragile transition metal of bluish white color (tarnishes in air, becoming covered with a thin oxide layer). For a long time it was not possible to allocate it in a pure form. In 1738 in England by William Champion was patented distillation method for the preparation of zinc.

Zinc under normal conditions is fragile transition metal of bluish white color

Very pure zinc is almost insoluble in acids. But if it be connected with copper wire or to the reaction mixture, pour a few drops of SuSO4, as the hydrogen begins to stand fast. What if this happens? First, the more active zinc displaces copper:

Cu2+ + Zn = Cu + Zn2+.

Copper is deposited on its surface and thus there is a miniature electrochemical cell, wherein the zinc is quickly dissolved in the acid. Hydrogen is not released on its surface, and at least the surface of the active metal - copper.

66 is known zinc minerals, particularly zinc, sphalerite, willemite, calamine, smithsonite, franklinite. The most common mineral - sphalerite, or zinc blende. The main component of the mineral - sulfide ZnS, and a variety of impurities give this matter all kinds of colors.

Zinc is an important biogenic element in living organisms contain an average of 5x10-4% zinc. But there are exceptions - the so-called hubs organisms, for example, some violets.

In air, zinc is covered with a thin film of ZnO oxide. A strong heating burned to a white oxide ZnO. Oxide reacts with both the acid solutions and alkali. Zinc reacts normal purity with acid solutions and alkaline solutions. With solutions of acids and alkalis very pure Zn, as mentioned above, it does not react. With hydrogen, nitrogen, carbon, boron and silicon, it does not immediately react. Nitride Zn3N2 Zn obtained by reacting with ammonia at 550-6000 C.