NON-METALS - III : LONG ANSWERS

GIVE ANSWER IN DETAIL

*INDEX-TOPIC SEARCH

1. Mention physical properties of nonmetals.
   

   ANS :
   

   
   
   • Nonmetals occur in all three states : solid, liquid and gas.
     
   • They are neither malleable nor ductile.
     
   • They do not conduct heat and electricity because they do not have free electrons (graphite is an exception).
     
   • They are lustreless.
     
   • They are hard and brittle.
     
   • They generally have low melting points and boiling points.
     
   • They are light in weight.
     
   • Solid nonmetals do not produce ringing sound.
     

   
   

   
   
2. Explain chemical properties of nonmetals.
   

   ANS : Nonmetals are electronegative elements because they accept electrons and form negatively charged ions. For example, oxygen forms negative oxide ion O^-2 by accepting two electrons.
   

   1/2 O₂ + 2 e^- → O^-2
   1/2 Cl₂ + e^- → Cl^-
   

   
   
   REACTION WITH OXYGEN : Nonmetals form either acidic oxide or neutral oxide with oxygen.
   

   
   
   • When carbon burns in air, it forms carbon dioxide which is an acidic oxide.
     

     C_(s) + O_2(g) → CO_2(g)
     

     
     
     Carbon dioxide dissolves in water to form carbonic acid [H₂CO₃].
     

     CO_2(g) + H₂O_(l) → H₂CO_3(aq)
     

   
   
   
   • When sulphur burns in air, it reacts with oxygen to form sulphur dioxide which is an acidic oxide.
     

     S_(s) + O_2(g) → SO_2(g)
     

     
     
     Sulphur dioxide dissolves in water to form sulphurous acid [H₂SO₃]
     

     SO_2(g) + H₂O_(l) → H₂SO_3(aq)
     

   
   
   
   • Phosphorus forms phosphurus pentoxide (2P₂O₅) with oxygen which dissolves in water to form phosphoric acid [H₃PO_4(aq)].
     

     P_4(s) + 5O_2(g) → 2P₂O_5(g)
     
     2P₂O_5(g) + 6H₂O → 4H₃PO_4(aq)
     

   
   
   • Oxides like CO, N₂O, H₂O are neutral oxides as their aqueous solutions are neither acidic nor basic or they do not have any effect on any litmus paper.
   
   

   
   
   REACTION WITH ACIDS : Nonmetals do not react with dilute acids as they are not able to displace hydrogen from acids.
   
   REACTION WITH CHLORINE : Nonmetals form chlorides with chlorine. These chlorides are either liquid or gas.
   
   
   
   REACTION WITH HYDROGEN : Nonmetals form covalent hydrides with hydrogen.
   
   
   
   Methane (CH₄), hydrochloric acid (HCl), etc. are hydrides of nonmetals.
   



3. Describe the Importance of nonmetals.
   

   ANS :
   

   
   
   • Hydrogen gas reacts with nitrogen to form ammonia gas.
     
   • Carbon is used in the preparation of useful substances like gunpowder, sugar, cold drinks, dry ice, urea, etc.
     
   • Oxygen supports life on earth.
     
   • Nitrogen is used in the preparation of nitric acid, nitroglycerin(explosives) and nitrogenous fertilisers.
     
   • Sulphur is used in the preparation of paper pulp, fungicides, etc.
     
   • Phosphorus is used in making matchsticks, insecticides, etc.
     

   
   

   
   
4. Write a few sentences on Hydrogen.
   

   ANS :
   

   
   
   • Hydrogen was discovered in 1766 AD by English chemist Cavendish.
     
   • Its chemical symbol is H.
     
   • It is the lightest of all elements.
     
   • It is the first element of the periodic table.
     
   • Hydrogen does not occur in free state (monoatomic molecule) in the atmosphere.
     
   • It is a diatomic molecule.
     
   • it is a colourless, odourless gas.
     
   • It is present in outer space.
     
   • It is the main element present in sun.
     

   
   

   
   
5. Describe preparation of hydrogen in laboratory.
   

   ANS :
   
   
   AIM : To prepare hydrogen gas in laboratory.
   
   APPARATUS & MATERIAL : Conical flask, Thistle funnel, glass container, bee-hive shelf, glass jar, glass tube, zinc granules, hydrochloric acid, water, etc.
   
   PROCEDURE :

   
   
   • Zinc granules are taken in conical flask and the equipment is set up as shown in figure.
     
   • Dilute hydrochloric acid is added slowly to the flask through thistle funnel.
     

   
   
   OBSERVATION : The reaction between zinc granules and dilute hydrochloric acid produces hydrogen gas which is collected by downward displacement of water in an inverted jar.
   
   CHEMICAL REACTION :
   
   Zn_(s) + 2HCl_(aq) → ZnCl_2(aq) + H_2(g)
   
   NOTE : In place of dilute HCl we can also use dilute H₂SO₄.
   
   Zn_(s) + H₂SO_4(aq) → ZnSO_4(aq) + H_2(g)
   

   
   
6. Describe manufacture of hydrogen from natural gas.
   

   ANS :
   

   
   
   • Hydrogen gas is manufactured on large scale from natural gas by steam reforming process.
     
   • Methane (the main constituent of natural gas) is mixed with steam and passed over nickel catalyst at 800°C and 30 atm pressure.
     
   • The reaction produces carbon dioxide and hydrogen.
     
     
     
   • Hydrogen gas can also be obtained by the electrolysis of acidified water.
     

   
   

   
   
7. Describe chemical properties of hydrogen.
   

   ANS :
   

   
   
   1. Hydrogen gas burns in air (oxygen) with a blue flame forming watervapour.
      
      2H_2(g) + O_2(g) → 2H₂O_(g)
   
   
   
   2. It burns in chlorine to form white fumes of hydrogen chloride gas.
      
      H_2(g) + Cl_2(g) → 2HCl_(g)
      
      Similarly it forms hydrogen fluoride gas with fluorine.
      
      H_2(g) + F_2(g) → 2HF_(g)
      
   
   
   
   3. It forms hydrides with metals like lithium, sodium and calcium.
      
      H_2(g) + 2Li_(s) → 2LiH_(s)
      
      H_2(g) + 2Na_(s) → 2NaH_(s)
      
      H_2(g) + Ca_(s) → CaH_2(s)
   
   
   
   4. Hydrogen reduces oxides of those metals, which are less reactive, to free metals. Thus, when hydrogen is passed over hot copper oxide copper metal and water are produced.
      
      CuO_(s) + H_2(g) → Cu_(s) + H₂O_(l)
   
   

   
   



8. Write a detailed note on ammonia, its manufacture, properties and uses.
   

   ANS :
   AMMONIA : Ammonia is a very important industrial chemical as it is used for the manufacture of a wide range of chemicals. It is manufactured commercially by Haber's process.
   
   MANUFACTURE : A mixture of nitrogen and hydrogen in the ratio of 1 : 3 is heated under 200 - 300 atm pressure in presence of catalyst (finely divided iron + molybdenum) at about 450 °C. The reaction is reversible.
   
   
   
   PHYSICAL PROPERTIES :
   

   
   
   • It is a colourless gas.
     
   • It has characteristic pungent smell which irritates eyes and nose.
     
   • It is poisonous.
     
   • It is highly soluble in water.
     

   
   
   CHEMICAL PROPERTIES :
   

   
   
   • Ammonia reacts with hydrochloric acid to form ammonium chloride.
     
     NH_3(g) + HCl_(l) → NH₄Cl_(s)
     
     
   • Ammonia decomposes in presence of electric discharge.
     
     
     
     
   • Ammonia reacts with oxygen in presence of catalyst platinum at 1073 K to form nitric oxide.
     
     
     
     
   • Aqueous solution of ammonia acts as a base. [NOTE : This property is given as physical property in the text book]
     

   
   
   USES :
   

   
   
   • In the manufacture of fertilisers such as urea, ammonium nitrate and ammonium sulphate.
     
   • In the manufacture of nitric acid.
     
   • In the manufacture of baking soda and washing soda.
     
   • In the manufacture of some medicines such as para-aminobenzoic acid (PABA), folic acid, etc.
     
   • In the preparation of dyes and explosives.
     

   
   

   
   
9. Describe Extraction of Sulphur.
   

   ANS : Pure sulphur is obtained by (i)Frasch Process or (ii) from natural gas and oil by chemical process.
   
   FRASCH PROCESS : The process is used to obtain pure sulphur from the sulphur bed in the ground. It is based on the fact that sulphur has relatively low melting point.
   
   

   
   
   • A hole of about 30 cm diameter is bored upto the sulphur bed.
     
   • Three concentric pipes of different diameters are descended upto sulphur deposits.
     
   • Pressurised superheated water at about 170°C is forced down through the outermost pipe. The heat of water melts the underground sulphur.
     
   • Hot compressed air is passed through the innermost pipe.
     
   • A mixture of molten sulphur and water comes out through central pipe.
     
   • The sulphur-water emulsion is allowed to settle in settling tanks. Yellow solid sulphur separates from water after cooling. This sulphur is 99.5% pure.
     

   
   
   FROM NATURAL GAS AND OIL :
   

   
   
   • Sulphur compounds in natural gas and oil are first converted into hydrogen sulphide. (H₂S).
     
   • Hydrogen sulphide is heated in presence of oxygen to obtain sulphur dioxide.
     
   • This sulphur dioxide is then heated with additional hydrogen sulphide in the presence of catalyst Fe₂O₃ to obtain sulphur in free state.
     
     
     

   
   

   
   
10. Write a note on Allotropes of sulphur.
    

    ANS :
    

    
    
    • Different arrangement of molecules in the crystals give rise to allotropes of sulphur.
      
    • There are two allotropes of crystalline sulphur. (i)Rhombic sulphur and (ii) Monoclinic sulphur.
      
    • Rhombic sulphur is stable below 96°C and its crystals have octahedral shape.
      
    • Monoclinic sulphur is stable above 96°C and its crystals are needle-shaped.
      
    • As one allotrope changes into another at 96°C, it is called TRANSITION TEMPERATURE for sulphur.
      
    • Both allotropes have similar chemical properties but their physical properties differ due to their different physical structures.
      
    • When solid sulphur is heated its molecular chain breaks which on further heating yields viscous liquid sulphur. This on heating starts boiling.
      

    
    

    
    
11. Mention Chemical properties of sulphur.
    

    ANS :
    

    
    
    • Sulphur burns with blue flame and produces sulphur dioxide.
      
      

      S_(s) + O_2(g) → SO_2(g)

      
      
      
    • REACTION WITH ACIDS : Sulphur is oxidised to sulphur dioxide when it reacts with hot and concentrated sulphuric acid.
      
      

      S_(s) + 2 H₂SO_4(aq) → 2H₂O_(l) 3SO_2(g)

      
      
      Sulphur is oxidised to sulphuric acid when it reacts with hot and concentrated nitric acid.
      
      

      S_(s) + 6HNO_3(aq) → H₂SO_4(aq) + 6NO_2(g) + 2H₂O_(g)

      
      
      
    • REACTION WITH CARBON : Sulphur reacts with carbon at high temperature to give carbon disulphide.
      

      C_(s) + 2S_(s) → CS_2(l)

      
      
      
    • REACTION WITH HYDROGEN : When hydrogen gas is passed through boiling sulphur, foul smelling hydrogen sulphide gas is formed.
      

      S_(s) + H_2(g) → H₂S_(g)

      
      

    
    

    
    
12. Mention uses of sulphur.
    

    ANS :
    

    
    
    • In the manufacture of sulphuric acid.
      
    • As an antiseptic in skin ointments for skin treatment and in cosmetics.
      
    • For making dyes, matches, gunpowder, pulp of paper and fireworks.
      
    • In vulcanisation of rubber.
      
    • For manufacturing carbon disulphide which is a solvent.
      
    • As a disinfectant, fungicide, germicide, etc. for destroying bacteria, fungi, insects, etc.
      
    • In printing (dyeing) of clothes.
      

    
    

    
    
13. Write a detailed note on sulphur dioxide.
    

    ANS : The reaction of sulphur with oxygen gives sulphur dioxide.
    
    

    S_(s) + O_2(g) → SO_2(g)

    
    
    PHYSICAL PROPERTIES :
    

    
    
    • It is a colourless gas.
      
    • It has a pungent smell.
      
    • It is a pollutant gas which causes acid rain due to dissolution in rain water.
      

    
    
    CHEMICAL PROPERTIES :
    

    
    
    • Sulphur dioxide dissolves in water to form sulphurous acid (H₂SO₃).
      
      

      SO_2(g) + H₂O_(l) ↔ H₂SO_3(aq)

      
      
      
    • Sulphur dioxide reacts with aqueous sodium hydroxide to form sodium sulphite (Na₂SO₃).
      

      SO_2(g) + 2NaOH_(aq) → Na₂SO_3(aq) + H₂O_(l)

      
      
      
    • When sulphur dioxide gas is passed through lime-water, the solution turns cloudy due to the formation of insoluble calcium sulphite (CaSO₃).
      
      

      SO_2(g) + Ca(OH)_2(aq) → CaSO_3(s) + H₂O_(l)
      

      
      
      
    • When sulphur dioxide gas is passed through an aqueous solution of hydrogen sulphide, it turns milky (turbid) due to formation of colloidal sulphur.
      
      

      SO_2(g) + 2H₂S_(aq) → 3S_(s) + 2H₂O_(l)

      
      
      
    • Sulphur dioxide combines with oxygen in presence of catalyst vanadium pentoxide [V₂O₅] at 450°C to form sulphur trioxide.
      
      
      

    
    
    USES :
    

    
    
    • For the manufacture of sulphuric acid.
      
    • As a preservative in orange and lemon squashes and jams.
      
    • For bleaching of wood pulp in paper industry.
      

    
    

    
    
14. Describe manufacture of sulphuric acid by Contact Process.
    

    ANS : The contact process is divided into different stages and uses various units such as sulphur burner, precipitator, steam scrubber, drying tower, arsenic purifier, contact chamber and absorption unit.
    
    PREPARATION OF SO₂ : SO₂ is obtained by burning sulphur or pyrites.
    

    Δ
    S_(s) + O_2(g) → SO_2(g)
    

    
    CONVERSION OF SO₂ into SO₃ IN CONTACT CHAMBER : The mixture of purified SO₂ and air is passed over catalyst vanadium pentoxide [V₂O₅] to produce SO₃.
    
    
    
    ABSORPTION OF SO₃ IN CONC. H₂SO₄ : SO₃ obtained from the contact chamber is dissolved in concentrated H₂SO₄ acid giving oleum, H₂S₂O₇. [Oleum is also known as 'fuming sulphuric acid'.]
    
    
    
    Sulphuric acid of any concentration can be obtained by diluting oleum with water.
    
    

    H₂S₂O_7(l) + H₂O_(l) → 2H₂SO_4(aq)

    
    
    Contact process yields sulphuric acid which is pure and of about 100% strength.
    

    
    
15. Write physical properties, chemical properties and uses of sulphuric acid.
    

    ANS :
    PHYSICAL PROPERTIES
    

    
    
    • Concentrated sulphuric acid is colourless viscous liquid containing 98% H₂SO₄ and 2% water.
      
    • Concentrated sulphuric acid is a powerful water-absorbing agent.
      
    • Dilute sulphuric acid contains 10% H₂SO₄ and 90% water.
      

    
    CHEMICAL PROPERTIES
    

    
    
    • Concentrated sulphuric acid dehydrates sugar to carbon. The black mass of carbon is called sugar charcoal and the reaction is called charring of sugar.
      
      
      
      
    • Dilute sulphuric acid reacts with metals like zinc and iron to form metal sulphates and hydrogen gas.
      
      Zn_(s) + H₂SO_4(aq) → ZnSO_4(aq) + H_2(g)
      
      Fe_(s) + H₂SO_4(aq) → FeSO_4(aq) + H_2(g)
      
      
    • Sulphuric acid is strong dibasic acid from which two hydrogen atoms can be displaced in solution.
      
      H₂SO_4(l) + 2H₂O_(l) → 2H₃O⁺_(aq) + SO_4(aq)^-2
      

    
    USES
    

    
    
    • In the preparation of fertilisers.
      
    • In the manufacture of pigments, dyes and paints.
      
    • In the preparation of detergents.
      
    • In storage batteries.
      

    
    

    
    
16. 
    

    ANS :
    

    
    

NON-METALS - II : BRIEF ANSWERS

ANSWER IN BRIEF

*INDEX-TOPIC SEARCH

1. Explain with example : Reaction of nonmetals with chlorine.
   

   ANS: Nonmetals form chlorides with chlorine. These chlorides are usually in gaseous state.
   
   
   



2. Explain with example : Reaction of nonmetals with hydrogen.
   

   ANS: Nonmetals form covalent hydrides with hydrogen.
   
   
   
   Methane (CH₄), hydrochloric acid (HCl), etc. are hydrides of nonmetals.
   



3. Mention physical properties of hydrogen.
   

   ANS:
   

   
   
   • It is lighter than air.
     
   • It is a colourless, tasteless and odourless gas.
     
   • It is insoluble in water.
     
   • It is neutral gas (it does not change the colour of litmus paper).
     

   
   

   
   
4. Mention uses of hydrogen.
   

   ANS:
   

   
   
   • Hydrogen Welding : When an electric arc is passed through hydrogen, it splits into atoms which release large amount of heat when they recombine to form molecules. This heat is used to melt and join (weld) the metals.
     
   • In the manufacture of ammonia by Haber's process.
     
   • In the manufacture of methanol and hydrochloric acid.
     
   • Liquid hydrogen is used as a fuel in space shuttles.
     
   • In the manufacture of vegetable ghee.
     

   
   

   
   
5. Mention physical properties of sulphur.
   

   ANS:
   

   
   
   • It is pale yellow solid crystalline substance which exists in different forms called allotropes.
     
   • It is odourless and tasteless.
     
   • It is insoluble in water.
     
   • It is soluble in organic solvents like carbon disulphide, toluene (methyl
     benzene), etc.
     

   
   

   
   
6. 
   

   ANS:
   

   
   

NON-METALS - I : MCQs & SHORT ANSWERS

*INDEX-TOPIC SEARCH

MULTIPLE-CHOICE QUESTIONS

SELECT THE CORRECT ALTERNATIVE:

1. There are ______ nonmetals.
   
   
   
   1. 20
   2. 22
   3. 24
   4. 25
      
   
   
2. How many nonmetals are in solid state ?
   
   
   
   1. 11
   2. 12
   3. 13
   4. 14
      
   
   
3. How many nonmetals are in gaseous state ?
   
   
   
   1. 7
   2. 8
   3. 9
   4. 10
      
   
   
4. The atomic number of sulphur is...
   
   
   
   1. 15
   2. 16
   3. 17
   4. 18
      
   
   
5. Which of the following is used as a fuel in space rockets ?
   
   
   
   1. Liquid hydrogen
   2. Liquid nitrogen
   3. Refined kerosene
   4. phenol
      
   
   
6. Sulphur belongs to _____ group in periodic table.
   
   
   
   1. Boron
   2. Carbon
   3. Oxygen
   4. Halogen
      
   
   
7. _____ ia a metalloid.
   
   
   
   1. Copper
   2. Sodium
   3. Bromine
   4. Silicon
      
   
   
8. When sulphur reacts with sulphuric acid _____ gas is produced.
   
   
   
   1. SO₂
   2. H₂S
   3. NO₂
   4. NH₃
      
   
   
9. Sulphuric acid is produced by ______.
   
   
   
   1. Ostwald process
   2. Frasch process
   3. Contact process
   4. Bessemer process
      
   
   
10. 
    
    
    
    4. 
       
    
    

ANSWERS TO MCQs

(1) B (2) A (3) D (4) B (5) A (6) C (7) D (8) A (9) C (10)

SHORT QUESTIONS

ANSWER IN SHORT:

1. Which nonmetal is in liquid state ?
   
        ANS : Bromine is the nonmetal in liquid state.
   


2. Give an example of a nonmetal which conducts heat and electricity.
   
        ANS : Graphite ( a form of carbon) conducts heat and electricity.
   


3. Why are nonmetals electronegative elements ?
   
        ANS : Nonmetals are electronegative elements because they accept electrons and form negatively charged ions.
   


4. Which type of oxides do nonmetals form ?
   
        ANS : Nonmetals form either acidic or neutral oxides.
   


5. Write formula of carbonic acid.
   
        ANS : The formula of carbonic acid is H₂CO₃.
   


6. Give examples of some neutral oxides.
   
        ANS : CO, N₂O, H₂O are examples of neutral oxides.
   


7. Why is carbon monoxide a neutral oxide ?
   
        ANS : Carbon monoxide (CO) is a neutral oxide because it forms neither acid nor base with water.
   


8. Why do nonmetals not react with dilute acids ?
   
        ANS : Nonmetals do not react with dilute acids because they are not able to displace hydrogen from acids.
   


9. Who discovered hydrogen ? When ?
   
        ANS : English chemist Cavendish discovered hydrogen in 1766 AD.
   


10. Why is ammonia a very important chemical ?
    
         ANS : Ammonia is a very important chemical because it is used in the preparation of fertilisers, nitric acid, explosives, nylon fibre, etc as well as household cleaners.
    


11. Why is ammonia not collected by downward displacement of water ?
    
         ANS : Ammonia is not collected by downward displacement of water because it is highly soluble in water.
    


12. What is the full form of PABA ?
    
         ANS : The full form of PABA is Para-Amino Benzoic Acid.
    


13. Mention important ores of sulphur.
    
         ANS : Important ores of sulphur are : Zinc blende (ZnS), gypsum (CaSO₄.2H₂O) and copper pyrites (CuFeS₂).
    


14. Write electronic configuration of sulphur ?
    
         ANS : The electronic configuration of sulphur is 2,8,6.
    


15. When SO₂ is heated with H₂S in the presence of catalyst ______, sulphur is obtained. [Fill up the blank].
    
         ANS : Fe₂O₃.
    


16. Mention two crystalline allotropes of sulphur.
    
         ANS : The crystalline allotropes of sulphur are (1) rhombic sulphur (2) monoclinic sulphur.
    


17. What is transition temperature ?
    
         ANS : The temperature at which one allotrope of an element changes into another allotrope is called TRANSITION TEMPERATURE of that element.
    


18. What is the transition temperature of sulphur ?
    
         ANS : The transition temperature of sulphur is 96°C.
    


19. What is the shape of the crystals of rhombic sulphur ?
    
         ANS : The shape of the crystals of rhombic sulphur is octahedral.
    


20. What is the shape of the crystals of monoclinic sulphur ?
    
         ANS : The shape of the crystals of monoclinic sulphur is needle-like.
    


21. What is known as the king of chemicals ?
    
         ANS : Sulphuric acid is known as the king of chemicals.
    


22. Why is sulphuric acid known as the king of chemicals ?
    
         ANS : Sulphuric acid is known as the king of chemicals because it is used to prepare many important chemical substances like fertilisers, dyes, soap, etc.
    


23. Which catalyst is used for conversion of SO₂ into SO₃ in contact chamber ?
    
         ANS : V₂O₅ is used as catalyst for conversion of SO₂ into SO₃ in contact chamber.
    


24. What is the strength of H₂SO₄ obtained by Contact process ?
    
         ANS : The strength of H₂SO₄ obtained by Contact process is about 100 %.
    


25. What is charring of sugar ?
    
         ANS : The process in which concentrated sulphuric acid converts sugar to a black mass of carbon (sugar charcoal) by dehydration is called charring of sugar.
    


26. Give names of some nonmetallic elements.
    
         ANS : Hydrogen, oxygen, nitrogen, chlorine, bromine, iodine, sulphur, phosphorus, etc. are nonmetallic elements.
    


27. Write an equation for the reaction of phosphorus pentoxide with water.
    
         ANS :

    2P₂O_5(g) + 6H₂O_(l) → 4H₃PO_4(aq)
    

    
    


28. Write the equation for the industrial production of hydrogen.
    
         ANS :

    Ni catalyst
    800°C
    30 atm
    CH_4(g) + 2H₂O -----> CO_2(g) + 4H_2(g)
    



29. By which method is ammonia gas produced ?
    
         ANS : Ammonia gas is produced by Haber's process.
    


30. Which nonmetallic element is obtained by Frasch process ?
    
         ANS : Sulphur is obtained by Frasch process.
    


31. Write chemical formula of Oleum (fuming sulphuric acid).
    
         ANS : The chemical formula of fuming sulphuric acid is H₂S₂O₇.
    


32. Which crystalline form of sulphur is most stable ?
    
         ANS : Rhombic sulphur is the most stable crystalline form of sulphur.
    


33. On which physical property of sulphur is Frasch process based ?
    
         ANS : Frasch process is based on the property of low melting point (388 K) of sulphur.
    


34. 
    
         ANS :
    

METALS - III : LONG ANSWERS

GIVE ANSWER IN DETAIL

*INDEX-TOPIC SEARCH

1. Write a note on minerals in India.
   
   ANS : [table to be posted]
   
   
2. Explain : Froth Floatation Process OR The process to concentrate sulphide ores.
   
   ANS : This method is used for the concentration of sulphide ores of copper, zinc, lead, etc.
   
   PRINCIPLE: This method is based on the principle of difference in the wetting properties of the ore and the gangue particles with water and oil.
   
   PROCESS:
   
   
   The powdered ore is mixed with water, containing small quantity of oil (pine oil or turpentine oil) in a large tank.
   The sulphide particles in the ore get wet with oil while dust and sand particles do not get wet with oil.
   The water containing ore is agitated violently by blowing air to form froth.
   Sulphide particles being lighter float along with the froth at the surface which is removed from the top of the tank and collected.
   Impurities being heavier collect at the bottom. The froth is then washed, filtered and dried.
   
   
3. Write a note on Magnetic Separation.
   
   ANS :
   
   PRINCIPLE:This method uses the principle of difference in the magnetic properties of the ore and the gangue (impurities).
   
   EQUIPMENT:
   
   
   
   A magnetic separator consists of a leather conveyer belt moving over two rollers. One of the rollers has a strong magnet in it.
   
   PROCESS: Powdered ore is dropped on the moving belt at one end through a hopper. When it reaches the other end , nonmagnetic impurities fall down first whereas the magnetic particles fall later forming a separate heap.
   
   This method is generally used for the concentration of iron ores.
   
   
4. Explain : Calcination with proper examples.
   
   ANS : Calcination is a process in which concentrated ore is heated strongly in absence of air. Calcination is generally used
   for conversion of metal carbonates and hydroxides in to their corresponding oxides and to remove volatile impurities.
   
   Examples:
   
   
   
   
5. Write a note on 'Chemical Reduction' method.
   
   ANS : The conversion of metal oxide into metal is called REDUCTION. When chemicals like carbon, carbon monoxide, aluminium, etc. are used as reducing agents, the process is called CHEMICAL REDUCTION.
   In the carbon-reduction process, the metal oxide is mixed with coke (a form of carbon) and heated in a furnace. Carbon reduces metal oxide to free metal. Oxides of zinc, iron, copper, nickel, tin and lead are reduced by this method.
   
       ZnO_(s) + C_(s) → Zn_(s) + CO_(g)
   
       Fe₂O_3(s) + 3C → 2Fe_(s) + 3CO_(g)
   
       MnO_2(s) + 2C_(s) → Mn_(s) + 2CO_(g)
   
   Carbon monoxide is also used as reducing agent.
   
       Fe₂O_3(s) + 3CO_(g) → 2Fe_(s) + 3CO_2(g)
   
   Aluminium is used as reducing agent for the reduction of certain oxides of metals like chromium, manganese and iron. A large amount of heat is produced during the process and the metal is obtained in liquid (molten) state. The process is known as THERMIT PROCESS.
   
       Cr₂O_3(s) + 2Al_(s) → 2Cr_(l) +Al₂O_3(s)
   
       3MnO_2(s) + 4Al_(s) → 3Mn_(l) + 2Al₂O_3(s)
   
       Fe₂O_3(s) + 2Al_(s) → 2Fe_(l) + Al₂O_3(s)
   
   Chemical reduction method cannot be used for highly reactive metals like sodium, potassium, aluminium, etc. Oxides of such metals are reduced by electrolytic reduction method.
   
   
6. Explain Electrochemical Reduction giving example.
   
   ANS : Oxides of highly reactive metals like sodium, potassium and aluminium cannot be reduced by using chemical reduction ( by carbon or aluminium). If carbon is used large amount of heat is required and metal carbide is formed. These metals are obtained by electrolysis of their fused (molten) salts. The cathode acts as the reducing agent as it supplies electrons to metal ions.
   
   ELECTROLYSIS OF SODIUM CHLORIDE
       In this process molten sodium chloride is taken as electrolyte in an electrolytic cell. The reactions taking place at the two electrodes are :
   

   NaCl_(l) → Na⁺ + Cl^-
   
   Na⁺ + e^- → Na_(s)
   (at cathode)
   
   Cl^- → Cl + e^-
   (at anode)
   
   Cl + Cl → Cl_2(g)

   
   
       If aqueous solution of sodium chloride is taken instead of molten sodium chloride, reduction of hydrogen ions (2H⁺) to hydrogen (H₂ gas) takes place instead of reduction of sodium ion(Na⁺) to sodium metal.
   
   
7. Explain : Reactivity Series of Metals.
   
   ANS : The series of metals in the decreasing order of their reactivities is called reactivity series of metals. Some metals like sodium and potassium are highly reactive whereas metals like copper, silver and gold have very low reactivity.
   
   The reactivities of metals can be compared by their reaction with dilute acid or by comparing their oxidation potential with the standard hydrogen potential. Based on their reaction with dilute acids the following series has been prepared :
   
   K > Na > Ca > Mg > Al > Zn > Fe > Pb > (H) > Cu > Hg > Ag > Au
   
   The metals on the left of the hydrogen in the series are more reactive and they can displace hydrogen from acids. Metals on the right side of hydrogen are less reactive and they cannot liberate hydrogen from dilute aqueous acids.
   
   similarly, a more reactive metal can displace a less reactive metal from its solution. Thus, a strip of more reactive zinc displaces less reactive copper from aqueous copper sulphate solution (Displacement reaction). The blue colour of copper sulphate solution disappears gradually and brown granules of copper are seen at the bottom.
   
   Zn_(s) + CuSO_4(aq) → ZnSO_4(aq) + Cu_(s)
   
   If a strip of copper is placed in the solution of ZnSO₄, no chemical reaction occurs as copper is less reactive than zinc.
   
   
8. Write two equations each for obtaining metal oxides and hydroxides.
   
   ANS :
   OXIDES
   
   
   
   1. When sodium reacts with oxygen it forms sodium oxide.
      

      4Na_(s) + O_2(g) → 2Na₂O_(s)

   
   
   2. Iron reacts with steam and forms iron oxide and hydrogen gas.
      

      3Fe_(s) + 4H₂O_(g) → Fe₃O_4(s) + 4H_2(g)

   
   
   
   HYDROXIDES
   
   
   
   1. Sodium oxide reacts with water and forms sodium hydroxide.
      

      Na₂O_(s) + H₂O_(l) → 2NaOH_(aq)

   
   
   2. Magnesium reacts slowly with cold water and forms magnesium hydroxide and hydrogen gas.
      

      Mg_(s) + 2H₂O_(l) → Mg(OH)_2(aq) + H_2(g)

   
   
   
   
   
9. Give names of different steps of metallurgy and write a brief note on each step.
   
   ANS : Different steps involved in metallurgy are :
   
   
   
   • Crushing and grinding of ore
     
   • Concentration or enrichment of ore
     
   • Roasting, calcination and smelting
     
   • Reduction
     
   • Refining and purification of metals
     
   
   
   CRUSHING AND GRINDING OF ORE : The ore in the form of big rocks is broken into small pieces with the help of crushers. These small pieces are then powdered with the help of a ball mill or stamp mill.
   
   CONCENTRATION OR ENRICHMENT OF ORE : The process of removal of impurities from an ore is called ' Ore Concentration'. Different methods are employed for concentration of ore depending on the nature of ore and the impurities in it.
   
   Froth Floatation Process is used for the concentration of sulphide ores.
   
   Magnetic Separation method is used for removal impurities present in an ore with magnetic properties or for concentration of a nonmagnetic ore containing magnetic impurities.
   
   Centrifugal method is used when there is a large difference in the densities of ore and impurities.
   
   Ores of highly reactive metals are concentrated by chemical method.
   
   ROASTING, CALCINATION,SMELTING :
   Roasting is used to convert sulphide ores into oxides by heating for a longer period.
   
   
   
   Calcination is the process of heating the ore strongly in absence of air to remove (i) volatile impurities (ii)water [from hydrated ore] or (iii) to convert carbonate ore into metal oxide.
   
   
   
   Smelting is used to get an ore reduced to metal by heating whereby the metal is obtained in molten state.
   
   REDUCTION : The conversion of metal oxide into metal is called 'Reduction'. For chemical reduction, reducing agents like carbon, carbon monoxide and aluminium are used. Metals like zinc, iron, copper, nickel, tin and lead are obtained by chemical reduction of their oxides.
   

   Fe₂O_3(s) + 3C_(s) → 2Fe_(s) + 3CO_(g)
   
   3MnO₂ + 4Al → 3Mn + 2Al₂O₃
   

   
   
   The oxides of highly reactive metals cannot be reduced by chemical reduction using carbon or aluminium. Such metals are extracted by electrolytic reduction of their molten salts. During electrolysis the cathode acts as reducing agent by supplying electrons to metal ions. Sodium, potassium and aluminium are obtained by this method.
   
   REFINING OF METALS : The metals obtained from their ores after several metallurgical processes still contain some impurities. The removal of these impurities is called refining of metals. Refining is done mainly by two processes.
   
   
   
   1. LIQUATION (Liquefaction) method is used to remove impurities from metals like tin, lead and bismuth whose melting points are low as compared to those of impurities.
      
   2. ELECTROLYTIC REFINING is used to refine metals like zinc, lead, aluminium, copper, silver, gold, etc. The impure metal works as anode, a strip of pure metal is taken as cathode and a suitable salt of the metal to be purified in aqueous solution is taken as an electrolyte. The impure metal enters the solution from anode and then gets deposited on cathode. The impurities remain in the solution.
      
      In addition, the metals (in fact, metalloids) like silicon, germanium, etc. which are needed in ultrapure state for certain applications are obtained by zone refining method.
      
   
   
   
10. Write a note in detail : Refining of Metals by Electrochemical Method.
    
    ANS : Metals like zinc, lead, aluminium, copper, silver, gold, etc. are refined by this process.
    
    
    
    A rod of impure metal is taken as anode and a strip of pure metal is taken as cathode. an aqueous solution of a simple or complex salt of the metal to be purified is taken as electrolyte. On passing electric current at suitable voltage, pure metal is deposited at the cathode. The impurities either remain in the solution or collect at the bottom of the anode as 'Anode Mud'.
    
    For example, to obtain pure copper, impure copper rod is taken as anode, a strip of pure copper is taken as cathode and aqueous solution of copper sulphate is taken as the electrolyte.
    
    The reactions taking place at both the electrodes are :
    
    
    
    Crude copper contains very small amounts of iron, silver and gold. Iron dissolves in the solution whereas silver and gold collect at anode as anode mud and are obtained in the native state.
    
    
11. Describe Extraction of aluminium from bauxite.
    
    ANS :
    CONCENTRATION OF BAUXITE [BAYER'S PROCESS] :
    
    bauxite is concentrated by Bayer's process to obtain pure aluminium oxide (alumina).
    Bauxite is first roasted by heating to convert ferrous oxide into ferric oxide. The ore is then dried, powdered and treated with 45% aqueous solution of caustic soda (sodium hydroxide) and is heated to about160°C in a closed vessel for 6 to 8 hours at 5 to 6 atmospheric pressure. Sodium aluminate is formed.
    
    
    
    The insoluble impurities are filtered. Sodium aluminate is soluble in water and is obtained as filtrate. Sodium aluminate is then hydrolysed by adding excess water and constantly stirring it whereby gelatinous precipitates of aluminium hydroxide are obtained. To enhance the formation of Al(OH)₃, some Al(OH)₃ is added from outside as seedling.
    
    
    
    The precipitates of Al(OH)₃ are then washed repeatedly with water, dried and heated up to 1200°C.
    
    
    
    Thus, 99.5% pure alumina (Al₂O₃) is obtained.
    
    ELECTROLYSIS OF ALUMINIUM OXIDE [HALL-HAROULT PROCESS] :
    
    A special electrolytic cell invented by 'Hall' and 'Haroult' is used to reduce alumina to aluminium metal.
    
    
    
    Pure aluminium oxide is mixed with cryolite (Na₃AlF₆). The mixture is then melted in iron tank lined with carbon from inside. The carbon lining acts as cathode. The anode consists of a number of carbon rods which are dipped into the molten mass of Al₂O₃ and cryolite.
    
    When electric current is passed, aluminium metal is obtained at the cathode and oxygen gas gets liberated at anode. This oxygen gas reacts with carbon anode to form carbon dioxide. Due to this the carbon anode is gradually consumed.
    
    Molten aluminium metal being heavier than the electrolyte, is collected at the bottom of the tank.
    

    At Cathode
    
    2Al⁺³_(aq) + 6e^- → 2Al_(l)
    
    At Anode
    
    C_(s) + O^-2 → CO_(g) + 2e^-
    
    C_(s) + 2O^-2 → CO_2(g) + 4e^-
    

    
    
    
12. Describe extraction of iron using Blast Furnace.
    
    ANS : Blast furnace is used to obtain iron metal from haematite (Fe₂O₃). A proper mixture of haematite, coke and calcium carbonate is added to the blast furnace from the top and hot air is blown from the bottom of the blast furnace.
    
    
    
    [Diagram of blast furnace is only for information]
    
    
    
    1. At the bottom of the furnace coke burns in air to form carbon dioxide and large amount of heat is produced.
       

       C_(s) + O_2(g) → CO_2(g) + Heat

       
       
    2. In the center of the furnace carbon dioxide reacts with hot coke and forms carbon monoxide.
       

       CO_2(g) + C_(s) → 2CO_(g)
       

       
       
    3. In the upper part of the furnace the temperature is 400°C to 700°C. Here the reaction between iron oxide and carbon monoxide takes place in three stages and iron oxide is reduced to iron.
       

       3Fe₂O_3(s) + CO_(g) → 2Fe₃O_4(s) + CO_2(g)
       
       Fe₃O_4(s) + CO_(g) → 3FeO_(s) + CO_2(g)
       
       FeO_(s) + CO_(g) → Fe_(s) + CO_2(g)
       

       
       
    
    Due to large amount of heat produced in the furnace, limestone (CaCO₃) decomposes to calcium oxide. Calcium oxide reacts with sand (SiO₂) present as impurity in the ore and forms calcium silicate known as SLAG.
    

    CaO_(s) + SiO_2(s) → CaSiO_3(l)[slag]

    
    
    Both slag and iron ore are in molten state due to very high temperature in the lower part of the furnace. Both are collected separately from the bottom of the furnace. Once started, the blast furnace works for many months.
    
    
13. Mention physical properties of metals.
    
    ANS :
    
    
    
    • Metals have lustrous surface which can be polished.
      
    • Metals are solid (exception : gallium and mercury are in liquid state).
      
    • Metals are heavy (exception : sodium, potassium, magnesium and aluminium are comparatively lighter).
      
    • Metals are hard and cannot be cut with knife (exception : sodium, potassium and lead are soft and can be cut with knife).
      
    • Metals are good conductors of heat and electricity (exception : lead and mercury are bad conductors of heat).
      
    • Metals are ductile, i.e., they can be drawn in to wires.
      
    • Metals are malleable, i.e., they can be hammered and sheets can be prepared from them.
      
    • Metals have high melting points and boiling points. The melting point of iron is 1539°C.
      
    • Metals possess high tensile strength.
      
    • Most of the metals are sonorous, i.e., they produce sounding noise on collision.
      
    • Metals can be mixed with other metals and nonmetals to form alloys.
      
    
    
    
14. Write a note on chemical properties of metals OR Explain how metals react with oxygen, water, dilute acids, chlorine and hydrogen giving examples.
    
    ANS : Metals are electropositive elements since they have a tendency to lose electrons and form positively charged ions.
    
    REACTION WITH OXYGEN : Metals form oxides with oxygen. These oxides are basic in nature because when dissolved in water they form alkaline solutions. For example, sodium reacts with oxygen to give sodium oxide.
    

    4Na_(s) + O_2(g) → 2Na₂O_(s)

    
    
    Sodium oxide reacts with water to form sodium hydroxide ( an alkali).
    

    Na₂O_(s) + H₂O_(l) → 2NaOH_(aq)

    
    
    Oxides of metals like aluminium and zinc are called AMPHOTERIC OXIDES as they exhibit both acidic and basic behaviour.
    
    REACTION WITH WATER : Metals form either metal oxides or hydroxides when they react with water. Hydrogen gas is evolved in both cases.
    Highly reactive metals like sodium and potassium react violently with cold water.
    

    2Na_(s) + 2H₂O_(l) → 2NaOH_(aq) + H_2(g)

    
    
    Magnesium reacts slowly with cold water but rapidly with hot boiling water.
    

    Mg_(s) + 2H₂O_(l) → Mg(OH)_2(aq) + H_2(g)

    
    
    Zinc and iron react with steam only (i.e., they do not react with cold or warm water).
    

    Zn_(s) + H₂O_(g) → ZnO_(s) + H_2(g)
    
    3Fe_(s) + 4H₂O_(g) → Fe₃O_4(s) + 4H_2(g)
    

    
    
    Less reactive metals like lead, copper, silver and gold do not react with water at all.
    
    REACTION WITH DILUTE ACIDS : Depending on their reactivity, metals react with dilute acids at different rates and liberate hydrogen gas.
    

    Mg_(s) + 2HCl_(aq) → MgCl_2(aq) + H_2(g)
    
    2Al_(s) + 6HCl_(aq) → 2AlCl_3(aq) + 3H_2(g)
    

    
    
    Copper does not react with dilute acids.
    
    REACTION WITH CHLORINE : Metals react with chlorine to form metal chlorides which are ionic compounds.
    

    2Na_(s) + Cl_2(g) → 2NaCl_(s)
    

    
    
    REACTION WITH HYDROGEN : All metals do not combine with hydrogen. Only reactive metals like sodium, potassium and calcium form their hydrides with hydrogen.
    

    2Na_(s) + H_2(g) → 2NaH_(s)
    
    Ca_(s) + H_2(g) → CaH_2(s)
    
    2K_(s) + H_2(g) → 2KH_(s)
    

    
    
    
15. Write a note on Corrosion.
    
    ANS :
    
    
    
    • Corrosion is a process in which rust is formed on metal surface when it is exposed to air, water or moisture. Oxygen of air, carbon dioxide and moisture(water) are mainly responsible for corrosion.
      
    • Some of the metals undergo corrosion. For example : (i) Green coloured salt is formed on copper and brass vessels.
      (ii) Iron becomes rusted because of its reaction with oxygen of air. Iron rust is mainly iron oxide (Fe₂O₃.xH₂O) which is red in colour.
      
    • Corrosion results in wastage of billions of rupees. Therefore, it is better to prevent corrosion.
    
    
    PREVENTION OF CORROSION :
    
    
    
    • Rusting of iron can be prevented by covering its surface with a paint. This method is less effective because rusting starts again if the paint is removed from some part.
      
    • Iron is galvanised by applying a thin layer of more active zinc on its surface. Zinc prevents rusting effectively. Even if a small amount of zinc is removed from the surface, rusting does not start again because zinc spreads to cover the surface and prevents corrosion.
      
    • To prevent corrosion of iron plates of steamers, blocks of more reactive metals like magnesium or zinc are combined with iron plates and then allowed to come in contact with seawater. Here iron plates act as cathode and magnesium(or zinc) act as anode because the oxidation potential of iron is less. The magnesium/zinc blocks get corroded in seawater so they are replaced periodically.
      
    • Corrosion can also be prevented by using suitable chemical inhibitors which form a chemical bond with the metal surface and prevent corrosion.
      
    • A layer of enamel applied on the metal can prevent corrosion.
      
    
    
    
16. Write a note on Alloys.
    
    ANS : An alloy is a homogeneous solid solution of two or more metals or a metal and a nonmetal. An alloy is generally prepared by heating the mixture of its constituents to molten state and then cooling it at room temperature. An alloy is prepared to obtain material with desired properties because the properties of constituents of an alloy are modified to some extent. Sometimes the melting point of an alloy is lower than that of the constituents. For example, solder is an alloy of lead and tin. Its melting point is lower than that of lead and tin and it is used in soldering of electrical wires. [Table to be posted]
    
    Pure gold cannot be used to make jewellery as it is very soft. To make it hard, it is generally alloyed with copper or silver. The purity of gold is expressed in CARATS. Pure gold is 24 carats. 18 carat gold means it contains 18 parts of gold in 24 parts by weight of the alloy.
    
    
17. Distinguish between metals and nonmetals based on physical properties.
    ANS :
    
    
    
18. Distinguish between metal and nonmetal based on chemical properties.
    
    ANS:
    
    

METALS - II : BRIEF ANSWERS

ANSWER IN BRIEF

*INDEX-TOPIC SEARCH

1. Explain : 'Earth - A treasure of Elements'.
   
   ANS:
   
   
   
   • Elements necessary for life are available in the form of minerals [native state or compound form] from all three main spheres of earth.
     
   • LITHOSPHERE consists of rocks and sand. It provides elements like aluminium, sodium, iron, calcium, copper, etc. in the form of their oxides and sulphides.
     
   • HYDROSPHERE consists of all water sources like seas, rivers, lakes, etc. It supplies elements like chlorine, bromine, sodium, potassium, magnesium, etc. in the form of their compounds.
     
   • ATMOSPHERE is the envelope of gases surrounding the earth. It provides nitrogen, oxygen, carbon dioxide, etc.
     
   
   Hence the earth is a treasure of elements for us.
   
   
2. Explain : Roasting giving examples.
   
   ANS: Roasting is a process in which the concentrated ore is heated for a longer period. This process is used to convert sulphide ore into oxide by removing sulphur. The volatile impurities are removed by roasting.
   
   
   
   
3. Describe the importance of Ultrapure metals.
   
   ANS: Modern science and technology require ultrapure elements for several specific applications. Elements like silicon, boron and germanium used as semiconductors, in space and in technology must be ultrapure. Elements like uranium used in nuclear field must also be ultrapure. Amount of boron in uranium is 1 ppm. Neutron produced during nuclear fission breaks boron atom and the chain reaction stops. A similar problem arises when germanium is used as semiconductor because it contains 1 ppm of copper. Such ultrapure elements are obtained by zone refining method or 'van Arkel' method.
   
   
4. Write in brief about the Fractional Refining Process (Zone Refining Process).
   
   ANS: The fractional refining process [zone refining process] is used to obtain ultrapure elements [metals with almost 100% purity] used in some specific applications like semiconductors, space technology, nuclear energy, etc. During the process impurities are removed on the basis of fractional crystallization. The impurities being more volatile remain in solution in molten state and their solubility decreases as the molten metal cools and can be separated in the form of crystals. This gives ultrapure element. Silicon, boron, germanium, etc.are obtained in ultrapure form by this method and are used in semiconductor technology.
   
   
5. Give the names of different steps of metallurgy.
   
   ANS: Different steps involved in metallurgy are :
   
   
   
   • Crushing and grinding of ore
     
   • Concentration or enrichment of ore
     
   • Roasting, calcination and smelting
     
   • Reduction
     
   • Refining and purification of metals
     
   
   
6. Distinguish between roasting and calcination.
   
   ANS:
   
   

METALS - I : MCQs & SHORT ANSWERS

*INDEX-TOPIC SEARCH

MULTIPLE-CHOICE QUESTIONS

SELECT THE CORRECT ALTERNATIVE:

1. ______ is the formula of cuprite.
   
   
   
   1. Cu₂O
   2. Cu₂S
   3. CuCO₃
   4. CuCl₂
      
   
   
2. Siderite is an ore of ______.
   
   
   
   1. Copper
   2. Silver
   3. Calcium
   4. Iron
      
   
   
3. ______ is an ore of calcium.
   
   
   
   1. Magnetite
   2. Siderite
   3. Malachite
   4. Gypsum
      
   
   
4. During electrolytic reduction, ______ acts as reducing agent.
   
   
   
   1. anode
   2. cathode
   3. electrolyte
   4. the metal
      
   
   
5. Liquefaction method is used for the purification of metals with ______.
   
   
   
   1. high melting point
   2. low melting point
   3. high boiling point
   4. low boiling point
      
   
   
6. The formula of cryolite is ______.
   
   
   
   1. Cr₂O₃
   2. Na₃AlF₆
   3. Na₂AlF₆
   4. Na₂Cr₂O₇
      
   
   
7. Which of the following is a liquid metal at room temperature ?
   
   
   
   1. Sodium
   2. Cobalt
   3. Bromine
   4. Mercury
      
   
   
8. ______ is the best conductor of heat and electricity.
   
   
   
   1. Gold
   2. Silver
   3. Copper
   4. Iron
      
   
   
9. ______ is a poor conducting metal for heat.
   
   
   
   1. Copper
   2. Silver
   3. Aluminium
   4. Lead
      
   
   
10. The melting point of iron is ______ °C.
    
    
    
    1. 1539
    2. 1639
    3. 1359
    4. 1369
       
    
    
11. The true order of reactivity of metals with dil. HCl is ______.
    
    
    
    1. Mg>Al>Zn>Fe
    2. Mg>Zn>Fe>Al
    3. Al>Mg>Zn>Fe
    4. Zn>Mg>Al>Fe
       
    
    
12. Pure gold is ______ carats.
    
    
    
    1. 22
    2. 23
    3. 24
    4. 25
       
    
    
13. Which of the following is used as a semi-conductor ?
    
    
    
    1. Copper
    2. Silver
    3. Gold
    4. Germanium
       
    
    
14. The main constituent of bauxite is ______.
    
    
    
    1. Al₂O₃
    2. Al₂(SO₄)₃
    3. CaSO₄
    4. Na₃AlF₆
       
    
    
15. Which method is used for the purification of more reactive metals ?
    
    
    
    1. Chemical reduction
    2. Roasting
    3. Calcination
    4. Electrochemical reduction
       
    
    
16. Which reaction takes place at anode in an electrolytic process ?
    
    
    
    1. Oxidation
    2. Reduction
    3. Oxidation-reduction
    4. None of above
       
    
    
17. Which metal is obtained in liquid state (during extraction) ?
    
    
    
    1. Sodium
    2. Gallium
    3. Tin
    4. Uranium
       
    
    
18. Which substance is used to decrease the melting point of alumina in Hall - Haroult process ?
    
    
    
    1. CuSO₄
    2. Cryolite
    3. Gypsum
    4. Limonite
       
    
    
19. ______ is used in manufacturing scientific balance.
    
    
    
    1. Steel
    2. Brass
    3. Stainless steel
    4. Magnalium
       
    
    

ANSWERS TO MCQs

(1) A (2) D (3) D (4) B (5) B (6) B (7) D (8) B (9) D (10) A (11) A (12) C (13) D (14) A (15) D (16) A (17) C (18) B (19) D (20)

SHORT QUESTIONS

ANSWER IN SHORT:

1. Which metals are available in free state in nature ?
   
        ANS : Less reactive metals like gold, silver and copper are available in free state in nature.
   
2. Why are metals like sodium, potassium and aluminium not available in free state in nature ?
   
        ANS : Metals like sodium, potassium and aluminium are not available in free state in nature because they are more reactive metals.
   
3. Define : Mineral.
   
        ANS :Elements as well as elements in the form of their compounds which are available in earth's crust are known as minerals. OR A naturally occuring compound in which the metal exists either in native state or combined state is called mineral.
   
4. Define : Ore.
   
        ANS : A metal in the form of its compounds with other elements and/or their compounds is known as an ore. OR A mineral from which a metal can be extracted economically and conveniently is called an ore.
   
5. In what form are ores/minerals generally found in nature ?
   
        ANS : Generally, ores/minerals are found in the form of oxides, silicates, sulphides, carbonates, phosphates, etc.
   
6. Write names of two ores of copper.
   
        ANS : Cuprite and malachite are two ores of copper.[Also, copper pyrite and copper glance are ores of copper.]
   
7. Write the formula of siderite and gypsum.
   
        ANS : The formula of siderite is FeCO₃ and that of gypsum is CaSO₄.2H₂O.
   
8. Mention three main spheres of earth.
   
        ANS : Three main spheres of earth are : Lithosphere, Hydrosphere and Atmosphere.
   
9. Which elements are found in lithosphere ?
   
        ANS : Lithosphere mainly consists of oxides and sulphides of elements like aluminium, sodium, iron, copper, calcium, etc.
   
10. Which elements are found in the liquid sphere (hydrosphere) of the earth ?
    
         ANS : Hydrosphere contains elements like chlorine, bromine, sodium, potassium, magnesium in the form of their compounds.
    
11. Define : Metallurgy.
    
         ANS : The process of extracting pure metals from their ores and refining them for commercial use is called metallurgy.
    
12. What is gangue (or matrix) ?
    
         ANS : The impurities such as sand, stones, earthy matter, etc. present in the ore are called gangue (or matrix).
    
13. On what does the process of metallurgy depend ?
    
         ANS : The process of metallurgy depends on (i) the nature of the metal to be extracted (ii) the type of impurity present in the ore.
    
14. Mention the equipment used for grinding of ore.
    
         ANS : Ball mill and Stamp mill are equipment used for grinding ore.
    
15. What is concentration of ore ?
    
         ANS : The process of removal of impurities from an ore is called concentration of ore.
    
16. Mention the methods employed for concentration of ore.
    
         ANS : Methods employed for concentration of ore are :
    
    
    • Froth floatation process
      
    • Magnetic Separation method
      
    • Centrifugal method
      
    • Chemical method.
      
    
    
17. What is the principle of froth floatation process ?
    
         ANS : The froth floatation process is based on the principle of difference in wetting properties of the ore and the gangue particles with water and oil.
    
18. What is the principle of magnetic separation method ?
    
         ANS : Magnetic separation method uses the principle of difference in the magnetic properties of the ore and the gangue.
    
19. What is the principle of centrifugal method ?
    
         ANS : The principle of centrifugal method is the difference in the densities of ore and the impurities.
    
20. Which type of ores are concentrated by chemical method ?
    
         ANS : Ores of highly reactive metals are concentrated by chemical method.
    
21. Define : Roasting.
    
         ANS : Heating a substance (concentrated ore) in presence of oxygen under controlled atmospheric pressure is called roasting.
    
22. What is the purpose of roasting in metallurgy ?
    
         ANS : In metallurgy, the purpose of roasting is the conversion of sulphide ore into oxide besides the removal of volatile impurities.
    
23. What is calcination ?
    
         ANS : Calcination is the process in which the concentrated ore is heated strongly in absence of air.
    
24. What is smelting ?
    
         ANS : Smelting is a process of heating an ore strongly to obtain metal in molten state by reduction.
    
25. What is reduction ?
    
         ANS : The conversion of metal oxide into metal is called reduction.
    
26. On what does the method of reduction depend ?
    
         ANS : The method of reduction depends on the nature and reactivity of the metal.
    
27. Mention some reducing agents.
    
         ANS : Carbon, carbon monoxide, alumunium, etc are examples of reducing agent.
    
28. What is taken as anode in electrolytic refining of a metal ?
    
         ANS : A rod of impure metal is taken as anode in electrolytic refining of a metal.
    
29. By which method are ultrapure elements obtained ?
    
         ANS : Ultrapure elements are obtained by Zone refining (fractional separation) method.
    
30. What is the use of van Arkel's method ?
    
         ANS : van Arkel's method is used for obtaining ultrapure elements like germanium and uranium.
    
31. What acts as cathode in electrolytic reduction of Al₂O₃ ?
    
         ANS : Carbon (graphite) lining inside the iron tank acts as cathode in electrolytic reduction of Al₂O₃.
    
32. What works as electrolyte in Hall-Haroult cell ?
    
         ANS : The mixture of molten Al₂O₃ and Na₃AlF₆ works as electrolyte in Hall-Haroult cell.
    
33. What is slag ?
    
         ANS : Calcium silicate formed from sand present in iron ore and calcium oxide produced by decomposition of calcium carbonate is called SLAG.
    
34. Which metals can liberate H⁺ ions from aqueous solutions of acids ?
    
         ANS : More reactive metals or the metals on the left side of hydrogen in the reactivity series can liberate H⁺ ions from aqueous solutions of acids.
    
35. What is emf (electromotive force) ?
    
         ANS : The cell potential of an electrochemical cell measured in comparison to standard hydrogen electrode is known as electromotive force (emf) of that cell.
    
36. What is emf series ?
    
         ANS : The series prepared by arranging oxidation potentials (emfs) of half cells (electrodes) in descending order is called emf series.
    
37. What is reactivity series of metals ?
    
         ANS : The arrangement of metals in order of their decreasing reactivities is called reactivity series of metals.
    
38. Mention the most malleable and ductile metals.
    
         ANS : Gold and silver are the two most malleable and ductile metals.
    
39. What do we mean by malleability ?
    
         ANS : Malleability means capacity to be hammered into very thin sheet without being broken.
    
40. What do we mean by ductility ?
    
         ANS : Ductility is a property of a substance (metal) by which it can be drawn into thin wires.
    
41. Mention three metals having low density.
    
         ANS : Sodium, potassium and magnesium are metals with low density.
    
42. Why are metals electropositive ?
    
         ANS : Metals are electropositive because their atoms can lose electrons easily to form positively charged ions.
    
43. What is the nature of the oxides of metals ?
    
         ANS : Oxides of metals are basic in nature.
    
44. Why are the oxides of metals basic ?
    
         ANS : Oxides of metals are basic because they form alkaline solutions with water.
    
45. What do we mean by amphoteric oxides ?
    
         ANS : Those oxides of metals which show both acidic as well as basic behaviour in aqueous solutions are called amphoteric oxides.
    
46. Mention some metals that do not react with water at all.
    
         ANS : Lead, copper, silver and gold are the metals that do not react with water at all.
    
47. Why are metals reducing agents ?
    
         ANS : Metals are reducing agents because they give electrons to other element and in turn get oxidised to respective positive ion.
    
48. What is corrosion ?
    
         ANS : The destruction of metal due to its exposure to environmental factors like air and moisture is called corrosion of metals.
    
49. What is rust chemically ?
    
         ANS : Chemically rust is a mixture of ferric oxide and ferric hydroxide.[Fe₂O₃.xH₂O].
    
50. What is galvanization ?
    
         ANS : The process of depositing a thin layer of zinc metal on iron is called galvanization.
    
51. What is an alloy ?
    
         ANS : An alloy is a homogeneous solid solution (mixture) of two or more metals or a metal and a nonmetal.
    
52. Mention the constituents of stainless steel.
    
         ANS : Iron, nickel and chromium are the constituents of stainless steel.
    
53. Which unit is used to express the purity of gold ?
    
         ANS : Carat is used to express the purity of gold.
    
54. Write the classification of elements.
    
         ANS : Elements are classified as metals, nonmetals amd semimetals (metalloids).
    
55. How can special type of steel be obtained ?
    
         ANS : Special type of steel can be obtained by heating iron red hot in absence of air with pieces of leather (animal skin).
    
56. In which forms of compounds is an ore obtained in nature ?
    
         ANS : An ore is obtained in the form of oxide, carbonate, sulphide, silicate, sulphate, etc in nature.
    
57. Dolomite is a mineral of which metal ?
    
         ANS : Dolomite is a mineral of calcium.
    
58. From where in India is the mineral of aluminium obtained ?
    
         ANS : The mineral of aluminium (bauxite) is obtained from the states of Bihar, Gujarat, Madhya Pradesh and Rajasthan.
    
59. What is the importance of turpentine oil in froth floatation process ?
    
         ANS : In froth floatation process the importance of turpentine oil is that it selectively wets ore particles making them lighter and it forms lather (froth) containing those particles which can be easily taken out.
    
60. Which metals are obtained in their molten state ?
    
         ANS : Metals obtained in molten state are tin, lead, bismuth, iron and aluminium.
    
61. Mention the type of electric charge on anode.
    
         ANS : The electric charge on anode is positive.
    
62. Write the equation of the reaction taking place on inert anode during electrolysis of molten NaCl.
    
         ANS :
    
         Cl^-_(l) → Cl + e^-
    
         Cl + Cl → Cl_2(g)
    
63. Which metals are used as semiconductors ?
    
         ANS : Silicon, boron and germanium are used as semiconductors.
    
64. Which metals are obtained in ultrapure condition by van Arkel's method ?
    
         ANS : Metals like germanium and uranium are obtained in ultrapure condition by van Arkel's method.
    
65. Write the principle of zone refining (fractional ultrapurification) method.
    
         ANS : The zone refining process uses the principle of fractional crystallization.
    
66. Which method is used to obtain pure aluminium from alumina ?
    
         ANS : Hall-haroult electrolytic method is used to obtain aluminium from alumina.
    
67. How can the comparison of reactivity of metals be done ?
    
         ANS : The comparison of reactivity of metalscan be done by the reaction of dilute HCl with different metals and observing the rate of evolution of hydrogen gas.
    
68. What will be the reaction when zinc metal is placed in a solution of copper sulphate ?
    
         ANS : When zinc metal is placed in a solution of copper sulphate the more reactive zinc displaces copper from its solution forming colourless solution of zinc sulphate containing brown granules of copper metal.
    
69. Write the equation of the reaction of sodium oxide with water.
    
         ANS :
    
              Na₂O_(s) + H₂O_(l) → 2NaOH_(aq)
    
70. Write an equation of the reaction between a metal and hydrochloric acid.
    
         ANS :
    
               Mg_(s) + 2HCl_(aq) → MgCl_2(aq) + H_2(g)
    
    OR
    
               2Al_(s) + 6HCl_(aq) → 2AlCl_3(aq) + 3H_2(g)
    
71. What is the chemical formula of rust ?
    
         ANS : The chemical formula of rust is Fe₂O₃,Fe(OH)₃ OR Fe₂O₃.xH₂O
    
72. What is galvanised iron ?
    
         ANS : Iron with its surface covered by a thin layer of zinc metal to protect it from being rusted is called galvanised iron.
    
73. What is anode (anodic) mud ?
    
         ANS : The impurities(less reactive metals) that settle down at the bottom of the anode during electrolytic refining of a metal are collectively called anode mud.
    

SOME IMPORTANT CHEMICAL COMPOUNDS-III : LONG ANSWERS

GIVE ANSWER IN DETAIL

*INDEX-TOPIC SEARCH

1. Describe Solvay's Ammonia-soda process (manufacture of sodium carbonate or washing soda).
   
   ANS : AMMONIA-SODA PROCESS
   
   
   
   • A cold and concentrated solution of sodium chloride (brine) is saturated with ammonia to obtain ammoniacal brine.
     
   • Ammoniacal brine is allowed to drop from the top of the reactor called carbonating tower.
     
   • Simultaneously, carbon dioxide gas is introduced into the tower from the bottom.
     
   • Following reaction takes place :
     
     
     
   • Sodium hydrogen carbonate is separated from ammonium chloride.
     
   • When sodium hydrogen carbonate is heated, it decomposes to give sodium carbonate.
     
     
     
   • The sodium carbonate obtained in this process is anhydrous and is called 'Soda Ash'.
     
   • Soda ash is dissolved in water and crystallized to get washing soda.
     
     
     
   • RE-USE OF BY-PRODUCTS:
     
     
     
     • The chief attraction of Solvay's process is that the by-products can be re-used.
       
     • The carbon dioxide used in the process is obtained by decomposition of CaCO₃ in a lime-kiln (furnace).
       
       
       
     • Lime is heated with water to obtain slaked lime.
       
       
       
     • When this slaked lime is heated with ammonium chloride (also a by-product), it yields ammonia, which is recycled to the process.
       
       
       
     
     
   
   
2. Mention the properties of washing soda.
   
   ANS:
   
   
   
   • It is a colourless, crystalline solid.
     
   • When exposed to air, the crystals of washing soda lose 9 molecules of water of crystallization to give sodium carbonate monohydrate. This process is called 'EFFLORESCENCE'.
     
     
     
   • On strong heating it loses all the water of crystallization and forms anhydrous sodium carbonate (soda ash).
     
   • As it is a salt of weak acid and strong base, the aqueous solution of washing soda is alkaline. It turns red litmus to blue.
     
   • Its reaction with acid solution produces carbon dioxide gas.
     
     
     
   
   
3. Mention the properties of baking soda.
   
   ANS:
   
   
   
   • It is a colourless crystalline solid.
     
   • It is soluble in water.
     
   • It is a salt of weak acid and strong base. Therefore, its aqueous solution is slightly alkaline.
     
   • On heating it decomposes to give sodium carbonate.
     
     
     
   • It reacts with acid to form carbon dioxide.
     
     
     
   
   
4. Write a note on bleaching powder.
   
   ANS:
   MANUFACTURE : Bleaching powder is manufactured by Hesenclever process. In this process, chlorine gas is passed over slaked lime, Ca(OH)₂, to obtain bleaching powder.
   
   
   
   PROPERTIES OF BLEACHING POWDER :
   
   
   
   • It is yellowish white powder with strong smell of chlorine.
     
   • In moist air it liberates chlorine gas.
     
   • When it reacts with carbon dioxide or dilute sulphuric acid or dilute hydrochloric acid, it produces chlorine gas.
     
     
   
   
   USES OF BLEACHING POWDER :
   
   
   
   • For making drinking water germ-free.
     
   • As an oxidising agent in industry.
     
   • For bleaching of cotton, linen and wood-pulp.
     
   • For bleaching (removing stains from ) washed clothes in laundry.
     
   
   
5. Write a note on Plaster of Paris.
   
   ANS:
   
   
   
   • The chemical formula of Plaster of Paris is CaSO₄.1/2 H₂O.
     
     [ONLY FOR INFORMATION: The formula of Plaster of Paris should be written as (CaSO₄)₂.H₂O because a molecule never exists in fraction. Here 1/2 molecule is written only for convenience.]
     
   • Its chemical name is calcium sulphate hemihydrate.
     
   • Plaster of Paris derived its name from the fact that it was made from gypsum which was found mainly in Paris.
     
   • PREPARATION : Plaster of Paris is prepared by heating gypsum[CaSO₄.2H₂O] in a kiln to 100°C.
     
     
     
     The gypsum should be heated carefully under controlled condition because if it is heated above 100°C, then anhydrous calcium sulphate (CaSO₄) called 'dead burnt plaster' is formed which does not set like Plaster of Paris on adding water.
     
   • PROPERTIES :
     
     
     
     • It is a white powder.
       
     • On addition of 1/3 parts of water, it forms crystals of gypsum and sets into a hard mass.
       
       
       
     • Its setting time increases if NaCl is added to it.
       
     • If gypsum is heated above 200°C, it forms dead burnt plaster which does not set like Plaster of Paris on adding water.[NOTE : This point is given in the text book as a property of Plaster of Paris. Actually, it is not the property of Plaster of Paris].
       
     
     
   • USES :
     
     
     
     • In making toys, idols and casts for statues.
       
     • In preparation of denture castings.
       
     • In bone-setting, i.e. fixing fractured limbs, bone joints, etc.
       
     • For sealing air-gaps in laboratory apparatus during experiments.
       
     • For making black-board chalks,decorative materials,POP false ceilings, cosmetics, etc.
       
     
     
   
   
6. Write a note on lime.
   
   ANS:
   
   
   
   • Lime is calcium oxide ( also called slaked lime).
     
   • MANUFACTURE :
     
     
     
     • Lime is manufactured by heating lime stone (CaCO₃) to 1000°C in a lime kiln.
       
     • Limestone decomposes to form lime and carbon dioxide gas.
       
       
       
     • The above reaction is reversible. Therefore to convert all the limestone into lime, carbon dioxide is allowed to escape from the kiln.
       
     • The process is known as CALCINATION (calcining) of limestone.
       
     
     
   • PROPERTIES :
     
     
     
     • It is a colourless amorphous solid.
       
     • Its melting point is 2000°C.
       
     • When lime is heated in an oxy-hydrogen flame, it produces bright white light called "limelight".
       
     • Lime reacts with water vigorously releasing a lot of heat. Slaked lime is produced.
       
       
       
     • Lime forms calcium chloride with wet (moist) hydrogen chloride gas but it does not react with dry HCl gas.
       
       
       
     • When lime is heated at 2000°C in an electric arc furnace with carbon, it forms calcium carbide.
       
       
       
     
     
   • USES :
     
     
     
     • As a drying agent for drying of gases like ammonia and alcohols.
       
     • In the manufacture of glass and cement.
       
     • In the manufacture of dyes.
       For preparing basic lining in furnaces.
       
     • For white washing of walls.
       
     
     
   
   
7. Write a note on cement.
   
   ANS:
   
   
   
   • Cement is an important building material.
     
   • Cement was discovered by Joseph Aspdin of England in 1824.
     
   • It is called 'Portland Cement' as the hardness obtained by mixing cement with water resembles Portland rock of England.
     
   • MANUFACTURE :
     
     
     
     • A finely powdered mixture of limestone and clay is heated at 1500°C in a rotary kiln to form clinker (cement).
       
     • After cooling, the clinker is mixed with 2 to 5 % gypsum.
       
     • The mixture is then ground to obtain finely powdered cement (Portland Cement).
       
     • Dicalcium silicate, tricalcium silicate and tricalcium aluminate are the major constituents of Portland cement.
       
     
     
   • PROPERTIES :
     
     
     
     • Cement is fine gray powder.
       
     • If water is mixed to it , it sets to a very hard mass.
       
     • If kept open in moist air, it becomes hard like a rock.
       
     
     
   • USES :
     
     
     
     • For making roads, bridges, dams and other building materials.
       
     • For the manufacture of concrete/R.C.C.[Reinforced Concrete Cement].
       
     
     
   • R.C.C. : The concrete having an iron framework inside it is called Reinforced Concrete Cement or Reinforced Cement Concrete (R.C.C.). RCC is used for making structures like pillars, roofs (floors), bridges, tunnels, dams, etc.
     
   
   
8. Write the chemical formula of ordinary glass and describe its manufacture.
   
   ANS: The approximate composition of ordinary glass is Na₂O.CaO.6SiO₂.
   
   MANUFACTURE :
   
   
   
   • A mixture of sodium carbonate, calcium carbonate and silica (sand) is heated at 1400°C in a furnace.
     
   • The silica decomposes carbonate compounds into silicates and releases carbon dioxide.
     
   • A mixture of sodium silicate and calcium silicate along with silica is obtained in molten state.
     
     
     
   • This mixture is molten glass which on cooling forms solid glass.
     
   • The hot molten glass is cooled carefully, i.e. neither very quickly nor very slowly.
     
   • If it is cooled very quickly it becomes very brittle and cracks easily.
     
   • If it is cooled very slowly it becomes opaque.
     
   
   
9. Describe different types of glass briefly.
   
   ANS:
   
   
   
   1. Soda Glass (Soft Glass) :
      
      
      
      • Soda glass is the ordinary glass also called soft glass.
        
      • It is made by melting soda ash, sand and quick lime.
        
      • It is used for making glass tumblers, dishes, bottles, mirrors, window panes, light bulbs, etc.
        
      
      
   2. Potash Glass (Hard Glass) :
      
      
      
      • Hard glass is prepared by melting a mixture of potassium carbonate, calcium carbonate and silica.
        
      • It is more resistant to acids.
        
      • It is used for making hard glass laboratory apparatus.
        
      
      
   3. Lead Crystal Glass :
      
      
      
      • Lead crystal glass is made by melting potassium carbonate, lead oxide and silica.
        
      • It is used for making costly glass apparatus and for producing flashes by reflection of light.
        
      
      
   4. Pyrex Glass (Heat Resistant Glass) :
      
      
      
      • Pyrex glass is made by melting a mixture of sand, quick lime, borax and alkali carbonate.
        
      • It is also known as Borosilicate glass.
        
      • It is used for making ampoules and laboratory apparatus.[An ampoule is used to store liquid medicines, usually for injections.]
        
      
      
   5. Optical Glass :It is used for making lenses for spectacles, cameras, microscopes, telescopes and similar optical instruments.
      
   6. Photochromatic Glass :
      
      
      
      • Photochromatic glass is the one which darkens temporarily when exposed to bright light.
        
      • Silver bromide in the glass gives it its property of automatic darkening.
        
      • It is used for making spectacles to protect eyes from sun's heat(sunglass).
        
      
      
   7. Safety Glass :
      
      
      
      • It is prepared by placing a thin sheet of transparent plastic between two layers of glass.
        
      • It is safe as it does not break easily.
        
      • It is used for making the windscreens of automobiles, trains and aeroplanes.
        
      • It is also used in making bullet-proof glass.
        
      
      
   8. Glass Fibre :
      
      
      
      • It is heat resistant.
        
      • It is used in refrigerators, ovens, etc.
        
      • Optical fibres are used in telecommunication because their efficiency is more than copper cables.
        
      • Optical fibres are also used in endoscopy to examine the internal organs of human body.
        
      
      
   9. Coloured Glass :
      
      
      
      • Coloured glass is obtained by adding small amounts of colouring material like certain metal oxides in molten state during preparation of glass.
        
      • For example, Ferric oxide for brown glass, chromium oxide for green glass, manganese dioxide for purple(violet) glass and cobalt oxide for blue glass.
        
      • Coloured glass is used for making fancy articles, artificial gems and window panes.
        
      
      
   
   
10. What is steel ? Describe its manufacture using Bessemer convertor.
    
    ANS: Steel is an alloy of iron and carbon containing 0.1 to 1.5 % carbon. Different elements like nickel,manganese and silicon are added to it in different proportion to obtain steel of desired characteristics.
    
    MANUFACTURE :
    
    
    
    • Bessemer convertor is used to produce steel from pig iron.
      
    • Bessemer convertor is lined with heat-resistant bricks from inside.
      
    • First, the Bessemer convertor is turned sideways and molten pig iron is poured in to it.
      
    • It is then brought back to vertical position.
      
    • A blast of hot air with pressure is passed into the convertor from the bottom.
      
    • This removes oxides of manganese, silicon, phosphorus, etc present as impurities in pig iron in the form of slag or gases.
      
    • After the rem,oval of impurities, required amount of carbon is added to pure molten iron to obtain desired steel.