Zinc:

 (1) Occurrence of zinc: Since zinc is a reactive metal so it does not occur in the native form. The chief ores of zinc are

(a) Zinc blende (ZnS)

(b) Calamine or zinc spar (ZnCO₃) and

(c) Zincite (ZnO)

(2) Extraction of zinc: Zinc blende, while the concentration through Froth floatation method zinc is roasted in air to convert it into ZnO. With the case of calamine, ore is calcined to get ZnO. The oxide thus acquired is heated with the temperature of 1673 K and mixed with the crushed coke and in fire clay retorts (Belgian Process) while ZnO gets decreased to metallic zinc. It being volatile at this temperature, a metal distils over and is condensed leaving behind Cd or Pb, Fe as impurities. Crude metal is also known as spelter metal. The metal could be refined either through the electrolysis or else by fractional distillation.

Properties of Zn:

As compare to the mercury Zinc is more reactive. This is a fine conductor of electricity and heat. Zinc simply merges along with the oxygen to form ZnO. A pure zinc do not react with the non-oxidising acids (HCl or H₂SO₄) but impure metal reacts forming Zn²⁺ ions and evolving H₂ gas.

Hot and conc. H₂SO₄ attacks zinc liberating SO₂ gas in the given equation

Zinc also reacts with both conditions (hot and cold) conc and HNO₃. HNO₃ liberating nitrous oxide (N₂O), ammonium nitrate (NH₄NO₃) and nitrogen dioxide (NO₂) correspondingly.

Zinc dissolves in hot concentrated NaOH creating the soluble sod. Zincate the reaction of zincate is given below:

Or

(3) Special varieties of zinc.

These both varieties of zinc are used as the reducing agents within laboratory.

(i) Granulated zinc: It could be prepared through pouring molten zinc within the cold water.

(ii) Zinc dust: It is prepared through melting zinc and then atomizing it with a blast of air.

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