Copper:

Types of Ores

-          Copper pyrites (chalcopyrite) CuFeS₂, 

-          Cuprite (ruby copper) Cu₂O,

-          The Copper glance Cu₂S ,

-          Malachite [Cu(OH)₂.CuCO₃],

-          Azurite [Cu(OH)₂.2CuCO₃]

Extraction of Copper 

Most of the copper which is approximately 75% is extracted from the sulphide ore, copper pyrites of it.

Concentration of ore: Froth floatation procedure.

Roasting: Main reaction of this is as follow: 

.

Side reaction:

The reaction for it is as follow:

.

Smelting:  

Smelting is explained like this:

Mixture of the copper and iron sulphides melt jointly to make 'matte' (Cu₂S + FeS) and the slag floats on its surface.

Conversion of matte into Blister copper (Bessemerisation)

Silica is added to matte and a hot blast of air is passed FeO + SiO₂ → FeSiO₃ (slag). After that the Slag is removed. By this time most of iron sulphide is eliminated.  Cu₂S + 2Cu₂O→6Cu + SO₂

Blister copper

 Blister copper consists of approximately 98% pure copper and the rest that is only 2% impurities (Ag, Au, Ni, Zn etc.)

Physical Properties of copper: 

The properties of copper are as follow:

(1)   Copper has reddish brown colour.

(2)   Copper is very malleable and ductile.

(3)   Copper as well has high electrical conductivity and high thermal conductivity.

(4)   Copper is the second most helpful metal because the first is iron.

(5)   Copper goes through the displacement reactions with lesser reactive metals example for this is, with Ag.

(6)   Copper can displace Ag from AgNO₃ . The at last divided Ag so acquired is black in colour.

Copper exhibit oxidation states of +1 and +2. While copper (I) salts are colorless, copper (II) in color salts are blue. Cu (I) salts are very much less stable and therefore are simply oxidized to Cu (II) salts (2Cu → Cu²⁺ + Cu). This reaction is termed as disproportionation.

(A) In existence of atmospheric CO₂ and moisture, copper gets covered with a green layer of basic copper carbonate (green layer) that protects the rest of the metal from additional action.

Equation that explained it is as follow:

(B) In existence of oxygen or air, copper heated to the redness (beneath temperature 1370 Kelvin) very firstly forms red cuprous oxide that alters to black cupric oxide on further heating. If the temperature is extremely high, cupric oxide (Cu₂O) changes back to the cuprous oxide

Equation:

(C) Action of acids. Non oxidising dil. acids like HCl, H₂SO₄ have no action on copper. Even though, copper dissolves in these acids in existence of air.

With dilute HNO₃, Cu liberates NO (nitric oxide) the equation is:

With concentrated HNO₃, copper gives NO₂ the equation is:

With hot concentrated H₂SO₄, copper gives SO₂ the equation is:

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