- IIT-JEE Syllabus
Commercially important ores of iron, copper, lead, magnesium, aluminium , tin and silver . Carbon reduction process (iron and tin), Self reduction process (copper and lead), Electrolytic reduction process (magnesium and aluminium), Cyanide process (silver and gold).
The earth’s crust is the main source of metals. The occurrence of metal in native or in combined state in the earth’s crust along with a number of rocky and other impurities depends upon the chemical nature of metals. Metals having less electropositive character have less affinity for oxygen, moisture and occur in free or metallic or native state i.e., in uncombined state e.g. Au, Pt , Ag etc. On the other hand metals with higher electropositive character occurs in combined state i.e., as compounds.
The compound of a metal found in nature is called a mineral. A mineral may be a single compound or a complex mixture. Those minerals from which metal can be economically extracted are called ores. Thus all ores are minerals but all minerals are not ores. For e.g. copper occurs in nature in the form of several minerals like Cu2O, Cu2S, CuFeS2, but copper pyrites is considered as the most economical mineral for the extraction of the metal. Hence copper pyrites is the chief ore of copper.
Ores may be divided into four groups
- i) Native Ores: These ores contain the metal in free state Silver gold etc. These are usually formed in the company of rock or alluvial impurities like clay, sand etc.
- ii) Oxidised Ores: These ores consist of oxides or oxysalts (eg. carbonates, phosphate) and silicate of metal. Important oxide ore includes, Fe2O3, Al2O3.2H2O etc. and important cabonate ores are limestone (CaCO3), Calamine (ZnCO3) etc.
iii) Sulphurised Ores: These ores consist of sulfides of metals like iron, lead, mercury etc. Examples are iron pyrites (FeS2). galena (PbS), Cinnabar (HgS)
- iv) Halide ores: Metallic halides are very few in nature. Chlorides are most common examples include horn silver (AgCl) carnallite KCl. MgCl2.6H2O and fluorspar (CaF2) etc.
It is the process of extracting a metal from its ores. The following operations are carried out for obtaining the metal in the pure form.
- i) Crushing of the ore
- ii) Dressing or concentration of the ore.
iii) Reduction of metal.
- v) Purification or refining of the metal.
Ores usually contain soil, sand, stones and other useless silicates. These undesired impurities present in ores are called Gangue or Matrix. The removal of these impurities from the ores is known as concentration. The concentration process involve physical as well as chemical method.
- a) Gravity separation: The separation is based on the difference in the specific gravities of the gangue particles and ore particles. The powdered ores is agitated with water or washed with a running stream of water. The heavy ore particles of sand, clay etc. are washed away. For this either wilfley table or hydraulic classifier is used.
- b) Froth Floatation Process: Metallic sulphides are wetted by certain oil like pine oils and not by water.
The finely divided ore is introduced into water containing small quantity of oil (e.g. Pine Oil). The mixture is agitated violently with air a froth is formed which carries away along with it the metallic particles on account of the surface tension forces. The froth is transferred to another bath where gangue-free ore settles down. As the heavy metallic material is floated upward with the froth, this process is known as froth floatation process. The method is based upon preferential wetting of surfaces by liquids.
- c) Electro Magnetic Separator: When one component either ore or the impurity is magnetic in nature this method can be used for separation. A magnetic separator consists of a belt moving over two rollers, one of which is magnetic. The powdered ore is dropped on the belt at the other end. Magnetic portion of the ore is attracted by the magnetic roller and falls near to the roller while the non-magnetic impurities fall
- a) Calcination: Calcination is a process in which the ore are usually carbonate or hydrated oxide is subjected to the action of heat in order of expel water from hydrated oxide and carbon dioxide from a carbonate.
Examples: ZnCO3 ¾® ZnO + CO2
CaCO3 ¾® CaO + CO2
Al2O3×2H2O ¾® Al2O3 + 2H2O
2Fe2O3×3H2O ¾® 2Fe2O3 + 3H2O
Calcination is generally done in a reverberatory furnace.
- b) Roasting: Roasting is a process in which ores (usually sulphide ores) either alone or along with some other materials are subjected to the action of heat and air at temperatures below their melting points in order to bring about chemical changes in them. Calcination is also roasting but in this case we are concerned mainly with the changes due to the expulsion of some ingredients such as water, carbon dioxide and no other chemical change occurs. But during roasting chemical changes like oxidation, chlorination etc. takes places. The following equations represent roasting:
2PbS + 3O2 ¾® 2PbO + 2SO2
PbS + 2O2 ¾® PbSO4
2ZnS + 3O2 ¾® 2ZnO + 2SO2
ZnS + 2O2 ¾® ZnSO4
CuS + 2O2 ¾® CuSO4
2Cu2S + 3O2 ¾® 2Cu2O + 2SO2
Roasting is generally carried out in a reverberatory furnace or in a blast furnace.
- c) Leaching: It involves the treatment of the ore with a suitable reagent as to make it soluble while impurities remain insoluble. The ore is recovered from the solution by suitable chemical method. e.g. bauxite ore contains ferric oxide, titanium oxide and silica as impurities. When the powdered ore is digested with an aqueous solution of sodium hydroxide at about 150°C under pressure, the alumina dissolves forming soluble sodium meta aluminate while ferric oxide, TiO2 and silica remains as insoluble part.
Al2O3 + 2NaOH ¾® + H2O
3.2 Reduction of Free Metal
- a) Smelting:The reduction of a metal from its ore by a process involving melting is known as smelting. It is generally done in a reverberatory furnace or a blast furnace in a controlled supply of air. Several reducing agents such as sodium, magnesium and aluminium are used for reduction. The calcinated or roasted ore is mixed with carbon (coal or coke) and heated in a reverberatory or a blast furnace. Carbon and carbon monoxide produced by incomplete combustion of carbon reduce the oxide to the metal.
- b) Flux:The ores even after concentration contain some earthy matter called gangue which is heated combine with this earthy matter to form an easily fusible material. Such a substance is known as flux and the fusible material formed during reduction process is called slag. Slag is usually lighter and floats on the surface of the molten metal.
Concentrated ore + gangue + reduction agent + flux
Metal + slag + gases
Fluxes are of the following two types:
- i) Acidic fluxes like silica, borax etc. These are used when the gangue is basic such as lime or other metallic oxides like MnO, FeO, etc. The chemical reaction which takes place in removing a basic gangue is as follows:
- ii) Basic fluxes like CaO, lime stone (CaCO3), magnesite (MgCO3), haematite (Fe2O3) etc. These fluxes are used when the gangue is acidic like silica, P4O10 For example
The other methods used for the reduction of metals are electrolytic reduction, hydro metallurgy and amalgamation method.
Illustration 1: Write short notes on
(a) Amalgamation (b) Hydrometallurgy
(c) Self reduction (d) Electrolytic reduction
Solution: a) This process is used for the extractioin of noble metals like gold and silver from the native ores. The finely crushed ore is brought into contact with mercury which combines with the metal forming its amalgam. The metal is then recovered by distilling the amalgam.
- b) Hydrometallurgy is the process of bringing the metal into solution by the action of suitable chemical reagents (e..g., sodium cyanide solution or chlorine in presence of water etc.) followed by recovery of the metal by the use of a proper precipitating agent which is a more electropositive metal. For example, poor ores of silver are suspended in a dilute solution of sodium cyanide and air is blown through it when the silver present goes into solution as the argentocyanide complex. From this solution the metal is precipitated by adding zinc turnigs.
4Ag + 8NaCN + O2 (air) + 2H2O ¾® 4Na [Ag(CN)2] + 4NaOH
or AgCl + 2NaCN ¾® Na[Ag(CN)2] + NaCl
2Na [Ag(CN)2] + Zn ¾® Na2[Zn(CN)4] + 2Ag¯
- c) In some cases no extra reducing agent is required. A part of the sulphide ore is changed to oxide or sulphate which then reacts with the remaining part to give the metal and sulphur dioxide. Copper and lead are obtained by this method.
2Cu2S + 3O2 ¾® 2Cu2O + 2SO2
Cu2S + 2Cu2O ¾® 6Cu + SO2
2PbS + 3O2 ¾® 2PbO + 2SO2
PbS + 2O2 ¾® PbSO4
PbSO4 + PbS ¾® 2Pb + 2SO2
- d) The carbon reduction methods are not applicable for the highly electropositive and chemically active metals such as alkali metals, alkaline earth metals, aluminium etc. The oxides of these metals are very stable and have to be heated very strongly with carbon in order to reduce them to metals. But at high temperatures these metals combine with carbon to form carbides, thus creating problem. Hence these metals are extracted by the electrolytic reduction of their fused halides. The metal is liberated at the cathode. Aluminium is however obtained by the electrolytic reduction of alumina (Al2O3) dissolved in molten cryolite (Na3AlF6).
3.3 Refining or purification
The metals obtained by the application of above reduction methods from the concentration ores are usually impure. The impure metal is thus subjected to some purifying process known as refining in order to remove undesired impurities. Various process for this are
- a) Liquation process b) Distillation process
- c) Cupellation d) Poling
- e) Elecrolytic refining f) Bessemerisation
This is a process in the metallurgy of copper. It involves the reduction of molten matte (mixture of cuprous and ferrous sulphide) obtained after smelting of copper pyrites ore in a Bessemer converter.
The molten matte is taken in Bessemer converter and heated by blowing hot blast of air and sand through tuyeres. The following reactions takes place in the converter.
- i) Air oxidizes iron sulphide to iron oxide and SO2
2FeS + 3O2 ¾® 2FeO + 2SO2
- ii) Sand reacts with iron oxide to form iron silicate
2FeO + SiO2 ¾® FeSiO3 (Slag)
iii) After the iron has been removed, hot blast of air converts a part of cuprous sulphide to cuprous oxide.
2Cu2S + 3O2 ¾® 2Cu2O + 2SO2
- iv) The cuprous oxide so formed reacts immediately with remaining cuprous sulphide to form metallic copper.
2Cu2O + Cu2S ¾® 6Cu + SO2
Since the reaction is exothermic, the heat liberated maintains the crude copper in the molten state. The completion of the reaction is indicated by the appearance of green flame produced by the vaporization of copper.
It is a device in which high temperature is produced either by burning a fuel or by using electricity. The important ones are described below.
- a) Blast Furnace: It is used for smelting iron, copper and lead ores. It has a tall structure made of steel plates rivetted together lined inside with fire bricks. The furnace is provided with an arrangement for blowing air near the base, a slag hole, a tapping hole for removing the molten metal and an exit for waste gases near the top. The charge is introduced at the top. The mouth of the furnace is closed by a special arrangement through which the charge is introduced.
- b) Reverberatory Furnace: It is used for calcination, roasting or for smelting. The charge in the powdered form along with a flux is placed on the hearth of the furnace. The fuel is placed on grate and the flames are deflected from its low sloping roof. This furnace is used in case of copper, tin, lead and wrought iron.
- c) Muffle Furnace: A furnace in which the charge container is heated from all sides is called muffle furnace. The burnt materials including the vapours of the metal are allowed to escape through the same opening. The metal is obtained by condensing the vapours. In Belgian process for extracting zinc, the retorts act as muffles and prolongs help in completing the condensation.
- d) Bassemer Converter: It is a pear-shaped furnace made of steel plates lined inside with lime or magnesium oxide. It is fixed on pivots and can be tilted in any direction. It is provided with pipes through which hot air can be blown for heating purposes.
- Extraction of Aluminium
4.1 Important ores of aluminium
- Bauxite Al2O3×2H2O
- Cryolite Na3AlF6
- Feldspar K2Oal2O3×6SiO2 or KalSi3O8
- Mica K2O×3Al2O3×6SiO2×2H2O
- Corundum Al2O3
- Alumstone or Alunite K2SO4×Al2(SO4)3×4Al(OH)3
Aluminium is mainly extracted from bauxite ore.
4.2 Purification of Bauxite
2Al(OH)3 (calcination of aluminium hydroxide)
4.3 Electrolysis of fused pure alumina (Hall & Herwlt Method)
The addition of cryolite (Na3AlF6) and fluorspar (CaF2) makes alumina a good conductor of electricity and lowers its Fusion temperature from 2323 to 1140 K. the reaction taking place during electrolysis.
Na3AlF6 3NaF + AlF3
AlF3 Al3+ + 3F–
Al3+ + 3e– ¾® Al
F– ¾® F + e–
2Al2O3 + 12 F ¾® 4AlF3 + 3O2
2C + O2 ¾® 2CO
2CO + O2 ¾® 2CO2
4.4 Refining of Aluminium
The aluminium metal obtained by the electrolysis of fused almina is about 99.5% pure. It can be further refined by Hoope’s electrolytic process.
The graphite rods dipped in pure aluminium and Cu–Al alloy rod at the bottom in the impure aluminium work as conductors. On electrolysis, aluminium is deposited at cathode from the middle layer and equivalent amount of aluminium is taken up by the middle layer from the bottom layer (impure aluminium). Therefore, aluminium is transferred from bottom to the top layer through middle layer while the impurities are left behind. Aluminium thus obtained is 99.98% pure.
Illustration -2: Aluminium cannot be prepared by the electrolysis of aqueous solution of its salts. Why?
Solution: Discharge potential of aluminium is higher then the discharge potential of hydrogen. Thus the aqueous solution containing Al+3 and H+ ion when electrolysed, the H+ ions rather than Al+3 ions are discharged at cathode and hydrogen is evolved.
- Extraction of Iron
5.1 Important Ores of Iron
- i) Haematite Fe2O3 (red oxide of iron)
- ii) Limonite Fe2O3×3H2O (hydrated oxide of iron)
iii) Magnetite Fe3O4 (magnetic oxide of iron)
5.2 Extraction of Cast Iron
Iron is usually extracted from the haematite. Concentrated ore after calcination is reduced with carbon i.e. smelted in the blast furnace.
|Reactions taking place in the blast furnace
i) Zone of combustion
ii) Zone of reduction
Fe2O3 + 3CO ¾® Fe + CO2
iii) Zone of reduction
Fe2O3 + 3CO ¾® 2Fe + 3CO2
FeO + CO ¾® Fe + CO2
iv) Zone of slag formation
v) Zone of fusion lower part of furnace
Molten iron is heavier than from molten slag. The two liquids are periodically tapped off. The molten iron tapped off from the furnace is solidifed into blocks called ‘pigs’.
5.3 Preparation of Wrought Iron
This is done by heating cast iron with haematite (Fe2O3) which oxidises C to CO, S to SO2, Si to SiO2, P to P4O10 & Mn to MnO
Fe2O3 + 3C ¾® 2Fe + 3CO
Where CO & SO2 escape, manganous oxide (MnO) and Silica (SiO2) combine to form slag.
MnO + SiO2 ¾® MnSiO3
Similarly phosphorus pentoxide combines with haematite to form ferric phosphate slag.
2Fe2O3 + P4O10 ¾® 4FePO4
Illustration 3: Cast iron is hard but pure iron is soft in nature. Explain why?
Solution: Cast iron contains 2.5 to 5% carbon which makes cast iron hard.
- Extraction of Copper
6.1 Important Ores of Copper
- i) Copper glance (chalcocite) Cu2S
- ii) Copper pyrites (Chalopyrites) CuFeS2
iii) Malchite Cu(OH)2 ×CuCO3
- iv) Cuprite or Ruby copper Cu2O
- v) Azurite Cu(OH)2×2CuCO3
6.2 Metallurgy of Copper
Copper is extracted mainly from copper pyrites. The various steps involved are
Concentration by froth floatation
Powdered ore + water + pine oil + air ¾® sulphide ore in the froth
Rosting in reverberatory furnace in presence of air
S + O2 ¾® SO2; 2As + 3O2 ¾® 2As2O3
2CuFeS2 + O2 ¾® Cu2S + 2FeS + SO2
Smelting in blast furnace in presence of air
2FeS + 3O2 ¾® 2FeO + 2SO2; FeO + SiO2 ¾® FeSiO3 (slag)
Bessemerisation in bessemer converter in presence of air
2FeS + 3O2 ¾® 2FeO + 2SO2; FeO + SiO2 ¾® FeSiO3
2Cu2S + 3O2 ¾® 2Cu2O + 2SO2
2Cu2O + Cu2S 6Cu + SO2
Blister copper (98% Cu + 2% impurities)
Anode–impure copper plates
Cathode-pure copper plates
Electrolyte -CuSO4 + H2SO4
Pure copper at cathode (99.9% pure)
- Extraction of Silver
7.1 Important Ores of Silver:
- i) Argentite or silver glance, Ag2S
- ii) Horn Silver AgCl
iii) Pyragyrite (Ruby Silver), Ag2S, Sb2S3
7.2 Metallurgy of silver:
Silver is mainly extracted from argentite (Ag2S) by Cyanide Process
silver ore (Argentite)
Concentration by froth floatation
Powdered ore + water + pine oil + air ¾® sulphide ore in the froth
Concentrated ore + NaCN solution (0.4 – 0.6%) + Air
Ag2S + 4NaCN 2Na[Ag(CN)2] + Na2S
4Na2S + 5O2 + 2H2O ¾® 2Na2SO4 + 4NaOH + 2S
Precipitation of silver with zinc
2Na[Ag(CN)2] + Zn ¾® + Na2[Zn(CN)4]
Black ppt. of Ag + KNO3 compact mass silver metal
Anode–impure silver plates
Cathode-pure silver plates
Electrolyte -AgNO3 solution + HNO3
Pure silver at cathode
- Extraction of Tin
The chief ore of tin is cassiterite or tin stone, SnO2. It contains about 10% of tin. The crushed ore is washed with water to remove lighter impurities. The ore is then roasted to remove arsenic and sulphur as volatile oxides. Tin is obtained by reducing SnO2 with carbon at 1200- 13000C in an electric furnace.
SnO2 + 2C Sn + 2 CO
The product often contains traces of Fe, which make the metal hard. Fe is removed by blowing air through the molten mixture to oxidise the iron to FeO, which then floats to the surface.
- Extraction of Lead
The principal ore of lead is Galena, PbS. The ore is first concentrated by froth floatation process. The concentrated ore is roasted in air to convert it into lead oxide PbO and lead sulphate. Some galena is also left unchanged. If the air supply is now reduced, the unreacted PbS reacts with PbO and PbSO4 to produce metal
3PbS + 5O2 ¾® 2PbO + PbSO4 + SO2
2PbO + PbS ¾® 3Pb + SO2
PbSO4 + PbS ¾® 2Pb + 2SO2
- Extraction of Magnesium
Magnesium from sea-water is obtained by the Dow’s process. It consists of electrolysis of molten magnesium chloride using an iron cathode and a graphite anode. Following are the steps that involved during the process.
- a) Mg+2 is precipitated as magnesium hydroxide by the addition of slaked lime, Ca(OH)2 to the sea water.
Mg2+ + Ca(OH)2 ¾® Mg(OH)2 + Ca2+
- b) Magnesium hydroxide on treatment with hydrochloric acid is converted to chloride which is crystallised as MgCl2.6H2O
Mg(OH)2 + 2HCl ¾® MgCl2 + 2H2O
- c) Now for electrolysis, magnesium chloride is fused as follows:
On passing a current of dry HCl gas it get partially dehydrated and the chloride thus obtained is added to a molten mix. of sodium chloride and calcium chloride (temp. range 973 – 1023 K).Under this condition MgCl2 melt with the loss of water.
If magnesium chloride hydrate is heated strongly, it hydrolyses to yield magnesia (magnesium oxide ) which is a refractory.
MgCl2.6 H2O ¾® MgO + 2HCl + 5H2O
- d) Molten mixture of MgCl2 , NaCl and CaCl2 is electrolysed. Magnesium is formed at the cathode and chlorine is evolved at the anode. The chlorine is used to make HCl acid which in turn is required for making magnesium chloride.
Cathode : Mg2+ + 2e– ¾® Mg
Anode : 2Cl– ¾® Cl2 + 2e–
Illustration 4: NaCl is added during electrolysis of fused anhydrous MgCl2. Why?
Solution: NaCl is added as to lower the fusion temperature of MgCl2 and to make the mixture a good conductor of electricity.
- Some Other Important Compounds
|15.||ZnSO4×7H2O||White Vitriol||16.||SnCl2×5H2O||Butter of Iron|
|17.||CaO||Quick lime||18.||Na2SO4×10H2O||Glauber’s salt|
|19.||Pb3O4||Red lead||20.||Pb(OH)22PbCO3||White lead|
|21.||Na2CO3||Soda ash||22.||NaOH||Caustic Soda|
|23.||KOH||Caustic potash||24.||Ca(OH)2||Slaked lime|
|25.||CaSO42H2O||Gypsum||26.||(CaSO4)2H2O||Plaster of Paris|
|33.||HgS||Cinnabar||34.||BaSO4||Baryte or heavy spar|
- Some important Alloy
|1.||Stainless Steel||Fe, Cr, Ni|
|3.||Alnico||Fe, Al, Ni, Co|
|5.||Bronze||Cu, Zn, Sn|
|6.||Gun Metal||Cu, Sn|
|7.||Bell Metal||Cu, Sn|
|8.||German Silver||Cu, Zn, Ni|
- Solved Problems
Problem 1: A student suggested that calcium should be made if CaO is reacted with Aluminium powder. Was student correct?
Given DGf0 (CaO) = – 604.2 kJ/mol
DGf0 (Al2O3) = –1582 kJ/mol
Solution: 2Al + 3CaO ¾¾® Al2O3 + 3Ca
DG° = (Al2O3) – 3 (CaO)
–1582 – 3 ´ (–604.2)
= –1582.0 + 1812.6 = + 130.6
DG° = +ve Þ reaction is non spontaneous hence not possible. So student was wrong.
Problem 2: Cinnabar (HgS) and galena (PbS) on roasting often gives their respective metals but zinc blende (ZnS) does not. Explain.
Solution: On roasting all these sulphides ores are partly converted into their respective oxides. Since the oxides of Hg and Pb are unstable. While that of zinc is stable, therefore, oxides of Hg and Pb bring about the reduction of their sulphides to metals, but zinc oxides does not reduce ZnS to Zn metal
HgS + 3Hg + SO2
PbS + 3Pb + SO2
Problem 3: Explain the following
- a) Although Au is soluble in aqua-regia, Ag is not
- b) Zinc and hot copper is used for recovery of Ag from the complex [Ag(CN)2]–
- c) Aluminium metal is frequently used as a reducing agent for extraction of metal such as chromium manganese etc.
- d) Partial roasting of sulphide ore is done in the metallurgy of copper.
Solution: a) Au dissolved in aquaregia forming soluble HAuCl4 but Ag forms insoluble AgCl
Au + 4HCl + 3HNO3 ¾¾® + 3NO2 + 3H2O
Ag + HCl + HNO3 ¾¾® + NO2 + H2O
- b) zinc is powerful reducing agent in comparison to copper and zinc is cheaper also than copper.
- c) Auminium metal is frequently used as a reducing agent for the extraction of metals. Such as Cr and Mn from their respective oxides because aluminium is more electropositive than Cr or Mn. The process of reduction is called alumino thermy.
Cr2O3 + 2Al ¾¾® Al2O3 + 2Cr
3Mn3O4 + 8Al ¾¾® 4Al2O3 + 9 Mn
- d) Partial roasting of sulphide ore forms some oxide. The oxide then reduces the remaining sulphide ore into metal.
2CuS + 3O2 ¾¾® 2CuO + 2SO2
2CuO + CuS ¾¾® 3Cu+ + SO2
Problem 4: Copper pyrites, CuFeS2, is the important source of copper. 10g of it was leached with dil. H2SO4 and solution diluted to 1 L.
- a) 10 ml of this solution required 10 ml of 0.02 M KMnO4 in acidic solution
- b) 10 ml of this solution was treated with excess of KI and liberated iodine required 10 ml of 0.02 M hypo solution. What is percentage of Cu and Fe in copper pyrites?
Solution: CuFeS2 + 2H2SO4 ¾¾® CuSO4 + FeSO4 + 2H2S
- a) Equivalent of Fe+2 º equivalent of KMnO4
10 ´ N = 10 ´ 0.02 ´ 5 ´ 10–3
Þ N = 0.1N
Strength = Normality ´ equivalent wt. = 0.1 ´ 56 = 5.6 gm/ litre
% of Fe+2 = 56%
- b) CuSO4 + 4KI ¾¾® Cu2I2 + 2K2SO4 + I2
Equivalent of Cu+2 = equivalent of I2 = equivalent of Na2S2O3
Equivalent of Cu+2 in 10 ml = 10 ´ 0.02 ´ 1 ´ 10–3
Equivalent of Cu+2 in 1000 ml = 100 ´ 10 ´ 0.02 ´ 10–3 = 0.02
Strength = Normality ´ equivalent weight
= 0.02 ´ = 12.7 g
or percentage of Cu = 12.7%
Problem 5: a) MgO is used for the lining in steel making furnace.
- b) Which of the metals Na, Ag and Fe are extracted by
- i) Complex formation
- ii) Reduction with carbon
iii) Electrolysis of fused salts
Solution: a) Magnesium oxide acts as a flux to remove impurities of Si, P and S through slag formation
- b) (i) Ag, (ii) Fe, (iii) Na
Problem 1: The material used in semiconductors
(A) Si (B) Sn
(C) Ti (D) Cs
Problem 2: Electrolytic bath electrolytic refining of lead contains
(a) H2SiF6 only
(b) PbSiF6 only
(c) H2SiF6 in presence gelatin
(d) H2SiF6 and PbSiF6 in presence of gelatin
Problem 3: Which of the following is manufactured by Siemens Martin process?
(A) Pig iron (B) Cast iron
(C) wrought iron (D) steel
Problem 4: The process of producing a hard coating of iron nitride on the surface of steel is called
(A) Annealing (B) Quenching
(C) Tempering (D) Nitriding
Problem 5: Bordeaux mixture is
(A) CuSO4 +MgSO4 (B) FeSO4 + CuSO4
(C) CuSO4 and lime (D) NiSO4 + lime
Problem 6: The main function of roasting is
(A) to remove the volatile impurities
(B) oxidation of metal
(C) reduction of metal
(D) to make slag
Problem 7: Which method of purification is represented by the following equation
Ni + 4CO Ni(CO)4 Ni + 4CO
(A) van Arkel (B) zone refining
(C) mond process (D) cupellation
Problem 8: The process of converting hydrated alumina into anhydrous alumina is called
(A) roasting (B) calcination
(C) smelting (D) dressing
Problem 9: Zone refining is a method to obtain
(A) Very high temperature (B) Ultra pure Al
(C) Ultra pure metal (D) Ultra pure oxides
Problem 10: Thomas slag is –
(A) Ca3(PO4)2 (B) MnSiO3
(C) CaSiO3 (D) FeSiO3
- Assignments (Subjective Problems)
Level – I
- Complete the following reactions:
- a) Al(OH)4– + CO2 ¾® ? + ? + ?
- b) Ag+ + Na2S2O3 ¾® ? + ?
- c) + H2S ? + ?
- A sulfide ore (A) on roasting leaves a residue (B). (B) on heating with chlorine gives (C), soluble in water, addition of excess potassium iodide to a solution of (C) gives a solution (D). A brown precipitate (E)is formed when a solution of ammonium sulfate is added to an alkaline solution of (D). Identify (A) to (E).
- Write the balanced chemical equations for the following
- a) Pb3O4 is treated with nitric acid
- b) Zinc oxide is treated with excess of sodium hydroxide solution
- c) Dilute nitric acid is slowly reacted with metallic tin
- d) Gold is dissolved in aqua regia
- e) Iron reacts with cold dilute nitric acid
- f) Sodium thiosulphate is added slowly to silver nitrate
- g) Heating of ZnCl2×2H2O
- In moist air copper corrodes to produce a green layer on the surface. Explain.
- Why does AgNO3 produce a black stain on the skin.
- How is ferrochrome produced? What are its application?
- State the composition of Cu alloys used for coinage.
- State the composition and use of
- i) Monel metal
- ii) German silver
- Complete the following reactions
- i) Zn + conc. HNO3 ¾®
- ii) Zn + 2NaOH ¾®
- How does the composition of cast iron differ from wrought iron and steel?
level – ii
- What is solvent extraction
- What is Goldsmidt Thermite Process:?
- What is the main differences between cupellation and poling?
- Complete and balance the following equations
- a) Zn + Fe2(SO4)3 ¾® ? + ?
- b) CuSO4 ? + ?
- c) Al + conc. H2SO4 ¾® ? + ? + ?
- d) Al2O3 + C + N2 ? + ?
- e) Pb + O2 + H2O ?
- a) Egg shell is made up of a chemical. In which of the two ores this chemical is present.
- b) How we can remove impurity of Pb in silver and impurity of Cuprous oxide in copper.
- Explain the following terms
- i) Zone refining (Fractional crystallization)
- ii) Electro-refining:
iii) Van-Arkel Method:
- What is meant by passivity of iron.
- List the reaction which occur at the various part of the blast furnace during manufacture of cast iron.
- The most stable chlorides of Cu, Ag and Au have the stoichiometric composition CuCl2 AgCl and AuCl3 in which the oxidation states are +2, +1, +3 respectively. Justify.
- Complete the reaction
- i) 3Cu + conc. 4HNO3 ¾®
- ii) Cu + conc. 2H2SO4 ¾®
iii) Cu2O + 4NH4OH ¾®
- iv) 2CuSO4 + 4KI ¾®
- Assignments (Objective Problems)
Level – I
- Cupric oxide is reduced to copper by
(A) H2 (B) C
(C) CO (D) All of these
- Cupric chloride is converted into cuprous chloride by
(A) Zinc (B) SO2
(C) copper (D) All of these
- White lead is –
(A) Pb(OH)2.PbCO3 (B) 2PbCO3.Pb(OH)2
(C) Pb(OH)2.Pb(CH3COO)2 (D) PbCO3.PbO
- Cerussite is
(A) PbS (B) PbCO3
(C) PbSO4 (D) SnO2
- Which alloy of aluminium is used in aircraft industry
(a) duralumin (b) Magnalium
(c) Nickeloy (d) alunico
- The common impurities present in the bauxite ore are
(A) Fe2O3 and CuO (B) Fe2O3 and PbO
(C) Fe2O3 and SiO2 (D) SiO2 and CuO
- Froth floatation process is based on
(a) specific gravity of the ore particle
(b) magnetic properties of the ore particle
(c) wetting properties of the ore particle
(d) electrical property o the ore particle
- The iron manufactured by pudding process is called as
(A) Pig iron (B) cast iron
(C) wrought iron (D) white cast iron
- Which of the following is a highly deliquescent solid?
(A) FeCl3 (B) FeSO4
(C) CuSO4 (D) All of these
- The compound undergoing photoreduction is
(A) AgCl (B) AgF
(C) AgNO3 (D) AgBr
- In aluminotermic process aluminium acts as
(A) an oxidising agent (B) a reducing agent
(C) a flux (D) a solder
- Poling process is used
(A) for the removal of Cu2O from Cu (B) for the removal of Al2O3 from Al
(C) for the removal Fe2O3 from Fe (D) in all the above
- Calcination is used in metallurgy to remove
(A) H2O and H2S (B) H2O and CO2
(C) CO2 and H2S (D) H2O and H2S
- Mac-Aurthur forrest process is used for the extraction of
(A) Zn (B) Cu
(C) Fe (D) Ag
- Duralumin is an alloy of
(A) Al and Mg (B) Al, Mg, Ni
(C) Al, Mg, Mn, Cu (D) Al and Ni
Level – II
- Which of the following precipitates Ag from AgNO3?
(A) Phosphine (B) Arsine
(C) Stibine (D) All of these
- Schwitzer’s reagent has the composition of
(A) [Ag(NH3)2]Cl (B) Fe4[Fe(CN)6]3
(C) [Cu(NH3)4]SO4 (D) K2[HgI4]
- The moleten matte obtained after the treatment of copper pyrites in the blast furnace, has the composition of –
(A) Cu2S (B) Cu2S + FeS
(B) Cu2S + Fe2S3 (D) CuS + Fe2S3
- Green coloured ore among the following is
(A) Cu2O (B) CuFeS2
(C) CuCO3.(Cu(OH)2 (D) 2CuCO3. Cu(OH)2
- Bromine is added to cold dilute aqueous solution of sodium hydroxide. The mixture is boiled. Which of the following statements is not true?
(A) During the reaction bromine is present in four different oxidation states.
(B) The greatest difference between the different oxidation states of bromine is 5.
(C) On acidification of the final mixture, bromine is formed
(D) Disproportionation of bromine occurs during the reaction
- Zeolite, which shows ion exchange ability –
(A) is an ion exchange resin
(B) is a closed packed assemblage of Si and O – atoms
(C) can provide H+ ions in place of Na+ ions
(D) is a sodium aluminum silicate
- Stainless steel contains –
(A) Fe, Cr, Cu (B) Fe, Cr, Ni
(C) Fe, Ni, C (D) Fe, Ni, Cu
- Books, periodicals, magazines and calendars are printed in large numbers. Type metal used in printing presses as alphabet letter printing contains –
(A) sulphur (B) chromium
(C) lead (D) copper
- The metallic lustre exhibited by sodium is explained by the presence of –
(A) Na+ ions (B) conducting electrons
(C) free protons (D) a body centred cubic lattice
- During Hoope’s process for electrolytic refining of Al, the middle layer is of –
(A) Pure aluminum (B) impure aluminum
(C) cryolite and BaF2 (D) alloys of Al, Ca, Si
- The silver halide, which is least soluble in NH4OH is
(A) AgF (B) AgCl
(C) AgBr (D) AgI
- Complex formation method is used for the exraction of
(A) Zn (B) Ag
(C) Hg (D) Cu
- Auto reduction process is used in the extraction of
(A) Cu and Hg (B) Zn and Hg
(C) Cu and Al (D) Fe and Pb
- Van Arkel method of purification of metals involves converting the metal to a
(A) Volatile stable compound (B) Volatile unstable compound
(C) non volatile stable compound (D) none of the above
- Which of the following is not a basic flux?
(A) CaCO3 (B) CaO
(C) SiO2 (D) MgO
- Answers to Objective Assignments
Level – I
- D 2. D
- B 4. B
- A 6. C
- C 8. C
- D 10. D
- B 12. A
- C 14. D
Level – II
- D 2. C
- B 4. C
- A 6. D
- B 8. C
- C 10. C
- D 12. B
- A 14. A
Ores and Metallurgy
LEVEL – I
- b) Ag+ + 2Na2S2O3 Na3[Ag(S2O3)2] + Na+
- c) + H2S Mn2++ SO2 + 2OH–
- a) Pb3O4 is a mixed oxide, 2PbO, PbO2, with nitric acid PbO is converted to Pb(NO3)2 while PbO2 remains as such
Pb3O4 + 2HNO3 ¾¾® PbO2 + Pb(NO3)2 + H2O
- b) ZnO is dissolved as Zincate ion
ZnO + 2NaOH ¾® Na2ZnO2 + H2O
- c) Tin reduces nitric acid (dilute) to ammonia
4Sn + + 10H+ ¾® 4Sn2+ + + 3H2O
- d) Gold dissolves in aqua regia as HAuCl4
Au + 4HCl + 3HNO3 ¾® HAuCl4 + 3NO2 + 3H2O
- e) 4Fe + 10HNO3 ¾® 4Fe (NO3)2 + NH4NO3 + 3H2O
- f) White precipitate changes to yellow, brown and finally becomes black
- g) ZnCl2×2H2O ZnCl(OH) + HCl + H2O
- In presence of moist air a thin film of green basic copper carbonate is formed on its surface and hence copper corrodes
2Cu + O2 + H2O + CO2 ¾®
- In presence of organic matter (skin) and light, AgNO3 decomposes to produce a black stain of metallic silver
2AgNO3 ¾® 2Ag + 2NO2 + O2
- FeOCr2O3 + 4C 2Cr + Fe + HCO
Ferrochrome (Fe 35%, Cr 65%) is used in steel industry.
- Ni coins = Cu 75% + Ni 25%
Guinea gold = Au 91%, Cu 9%
- i) Monel metal: Cu30% + Ni 67% + Fe, Mn 3% used for acid pumps and acid container.
- ii) German silver: Cu 50% + Zn 25% + Ni 25% used for utensils, resistance coils.
- i) Zn + conc. HNO3 ¾® Zn(NO3)2 + 2H2O + 2NO2
- ii) Zn + 2NaOH ¾® Na2ZnO2 + H2
|C %||Si %||S %||Mn%||P%|
|Cast iron||2 – 4.5||0.7 – 3.5||0.1 – 0.3||0.5 – 1.0||0 – 0.3|
|Steel||0.1 – 1.5||0.03 – 2.0||0.02 – 0.2||0.1 – 4.0||0.04 – 0.07|
|Wrought iron||0.04 – 0.25||0 – 0.14||0.02 – 0.15||Up to 0.25%||0.04 – 0.2|
level – ii
- Solvent extraction is the latest separation technique and has become popular because of its elegance, simplicity and speed. The method is based on preferential solubility principles.
Solvent or liquid-liquid extraction is based on the principle that a solute can distribute itself in a certain ratio between two immiscible solvents, one of which is usually water and the other an organic solvent such as benzene, carbon tetrachloride or chloroform. In certain cases, the solute can be more or less completely transferred into the organic phase. The technique can be used for purpose of preparation, purification, enrichment, separation and analysis.
- Certain oxides are not satisfactorily reduced by carbon. In such cases aluminium is used as a reducing agent. A mixture of metallic oxide and aluminium powder is ignited in a closed crucible by means of lighted magnesium ribbon. Metals like chromium, manganese etc. are extracted by thermite process as illustrated below.
Cr2O3 + 2Al ¾® Al2O3 + 2Cr
3Mn3O4 ¾® 4Al2O3 + 9Mn
The reaction is highly exothermic and the heat produced is sufficient to melt the metal.
- Both cupellation and poling are used for refining of metals, cupellation is contain impurities of other metals with traces of lead are removed from silver by heating impure silver with a blast of air in a cupel (an oval shaped pan made up of bone ash) in which lead is oxidised to lead oxide (PbO) which being volatile escapes leaving behind pure silver.
Poling is used for refining of such metals which contain impurities of its own oxide. In this process, the molten impure metal is stored with green wooden poles. At the high temperature of the molten metal, wood liberates methane which reduces the oxide of the metal to free metal.
3Cu2O + CH4 ¾® 6Cu + 2H2O + CO
- a) Zn + Fe2(SO4)3 ZnSO4 + 2FeSO4
- b) CuSO4 CuO +SO3
- c) 2Al + conc. 6H2SO4 ¾® Al2(SO4)3 + 3SO2 + 6H2O
- d) Al2O3 + 2C + N2 2AlN + 3CO
- e) 2Pb + O2 + 2H2O 2Pb (OH)2
- a) Limestone CaCO3
- b) Impurity of lead in silver can be removed by cupellation method and impurity of cuprous oxide in copper can be removed by poling.
- i) Zone refining (Fractional crystallization) This method is employed for preparing extremely pure metals. This method is based upon the principle that when a molten solution of the impure metal is allowed to cool, the pure metal crystallizes out while the impurities remain in the melt.
- ii) Electro-refining: In this method, the impure metal is converted into a block which forms the anode while cathode is a rod or plate of pure metal. These electrodes are suspended in an electrolyte which is the solution of a soluble salt of the metal usually a double salt of the metal. When electric current is passed, metal ions from the electrolyte are deposited at the cathode in the form of pure metal while an equivalent amount of metal dissolves from the anode and goes into the electrolyte solution as metal ion. The soluble impurities present in the crude metal anode go into the solution while the insoluble impurities settle down below the anode as anode mud.
iii) Van-Arkel Method: In this method, the metal is converted into it volatile unstable compound such as iodide leaving behind the impurities. The unstable compound thus formed is decomposed to get the pure metal.
Ti(s) + 2I2(s) + TiI4(g) Ti + 2I2(g)
- When iron is treated with concentrated HNO3 it stops showing its normal behaviour such as liberation of H2 from dil. H2SO4 and precipitation of Cu from CuSO4 solution. This phenomenon, when iron shows chemical inertness, is called passivity.
If iron is treated with certain oxidizing agents such as H2CrO4, KMnO4 etc., then also it becomes passive. In fact passivity of iron is suggested as formation of thin protective layer of Fe2O3 which prevents reaction of iron at room temperature.
- Zone of fusion (1200°C – 1500°C)
C + O2 ¾® CO2
CO2 + 2CO
Top section (4000°C – 900°C)
Fe2O3 + 3CO 2Fe + 3CO2
3Fe2O3 + CO 2Fe3O4 + CO2
Fe3O4 + CO 3FeO + CO2
FeO + CO Fe + CO2
Fe2O3 + 3C
Middle section (900°C)
CaCO3 CaO + CO2
CaO + SiO2 CaSiO3 (slag)
2Ca3(PO4)2 + 6SiO2 + 10C ¾® 6CaSiO3 + 10CO + 4P
3Fe + P ¾® Fe3P
- The (+1) state is expected to be the common and most stable for Cu, Ag and Au as they posses table d10 configuration. But only Ag+ is stable both in solid state and solution, which Cu+ and Au+ disproportionate very fast in H2O
2Cu+ Cu2+ + Cu K = = 1.6 ´ 106
3Au+ Au3+ + 2Au K = = 1 ´ 1010
- i) 3Cu + conc. 4HNO3 ¾®Cu(NO3)2 + 2NO2 + 2H2O
- ii) Cu + conc. 2H2SO4 ¾® CuSO4 + SO2 + 2H2O
iii) Cu2O + 4NH4OH ¾® 2[Cu(NH3)2]OH + 3H2O
- iv) 2CuSO4 + 4KI ¾® 2CuI2 + 2K2SO4