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Chapter-wise Objective Questions: General Principles and Processes Of Isolation Of Elements
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Multiple Choice Questions
(a) Na
(b) Au
(c) Ag
(d) Pb
Show Answer & Explanation
Answer: (a) Na
Explanation:
1. Gold and silver occur native because they are unreactive.
2. Lead occurs mostly as galena, but traces of native lead have been reported.
3. Sodium is so reactive that it is found only in combined form such as NaCl.
Teacher's Note:
1. Native state is typical of the least reactive metals.
2. Alkali metals occur only as compounds.
(a) Magnesium silicate
(b) Sodium borofluoride
(c) Sodium aluminium fluoride
(d) Magnesium aluminium silicate
Show Answer & Explanation
Answer: (c) Sodium aluminium fluoride
Explanation:
1. Cryolite has the formula Na3AlF6.
2. It is sodium hexafluoroaluminate, used as the solvent for alumina in the electrolytic extraction of aluminium.
Teacher's Note:
1. Remember cryolite and fluorspar as the two additives in the Hall-Heroult cell.
(a) Anhydrite
(b) Bauxite
(c) Corundum
(d) Diaspore
Show Answer & Explanation
Answer: (a) Anhydrite
Explanation:
1. Bauxite is Al2O3.2H2O, corundum is Al2O3 and diaspore is Al2O3.H2O.
2. Anhydrite is anhydrous calcium sulphate, CaSO4.
Teacher's Note:
1. Match each mineral with its metal by its formula.
(a) Cryolite
(b) Mica
(c) Fluorspar
(d) Feldspar
Show Answer & Explanation
Answer: (c) Fluorspar
Explanation:
1. Cryolite Na3AlF6, mica K2O.3Al2O3.6SiO2.2H2O and feldspar KAlSi3O8 all contain Al.
2. Fluorspar is CaF2.
Teacher's Note:
1. Fluorspar (calcium fluoride) is used as a flux and as the additive in aluminium electrolysis.
(a) ZnSO4
(b) ZnO
(c) Zn(NO3)2
(d) ZnCO3
Show Answer & Explanation
Answer: (d) ZnCO3
Explanation:
1. Zinc ores: zinc blende ZnS, calamine ZnCO3 and zincite ZnO.
2. Calamine is the carbonate ore of zinc.
Teacher's Note:
1. Calamine is a carbonate, zincite is an oxide, and blende is a sulphide.
(a) Silver glance mainly contains silver sulphide
(b) Gold is found in the native state
(c) Zinc blende mainly contains zinc chloride
(d) Copper pyrites contains iron along with copper and sulphur
Show Answer & Explanation
Answer: (c) Zinc blende mainly contains zinc chloride
Explanation:
1. Silver glance (argentite) is Ag2S, so (a) is correct.
2. Gold is native, so (b) is correct.
3. Zinc blende is ZnS, a sulphide, not a chloride, so (c) is incorrect.
4. Copper pyrites is CuFeS2, so (d) is correct.
Teacher's Note:
1. Zinc blende is the sulphide ore ZnS.
(a) Calamine and siderite are carbonates
(b) Argentite and cuprite are oxides
(c) Zinc blende and pyrites are sulphides
(d) Malachite and azurite are ores of copper
Show Answer & Explanation
Answer: (b) Argentite and cuprite are oxides
Explanation:
1. Calamine ZnCO3 and siderite FeCO3 are carbonates: correct.
2. Argentite is Ag2S (a sulphide) and cuprite is Cu2O (an oxide), so (b) is wrong.
3. Blende ZnS and pyrites FeS2 are sulphides; malachite and azurite are basic copper carbonates.
Teacher's Note:
1. Learn the anion class of each common ore.
(a) Cuprite
(b) Chalcocite
(c) Chalcopyrite
(d) Malachite
Show Answer & Explanation
Answer: (c) Chalcopyrite
Explanation:
1. Cuprite is Cu2O, chalcocite is Cu2S and malachite is CuCO3.Cu(OH)2.
2. Chalcopyrite (copper pyrites) is CuFeS2.
Teacher's Note:
1. Chalcopyrite is the chief ore of copper.
(a) Cs
(b) Ag
(c) Zn
(d) Mg
Show Answer & Explanation
Answer: (a) Cs
Explanation:
1. Reactivity order: Cs > Mg > Zn > Ag.
2. The more electropositive the metal, the more stable its oxide and the harder it is to reduce.
3. Ag2O decomposes on heating, whereas Cs requires electrolysis of a fused salt, so Cs is hardest.
Teacher's Note:
1. Ellingham lines of very reactive metals lie lowest on the diagram.
(a) Au
(b) Ag
(c) Both Au and Ag
(d) Cu
Show Answer & Explanation
Answer: (c) Both Au and Ag
Explanation:
1. Gold and silver dissolve in dilute NaCN solution in the presence of air to form [Au(CN)2]- and [Ag(CN)2]-.
2. The metals are then displaced with zinc dust.
Teacher's Note:
1. Cyanide leaching suits noble metals.
(a) Oxide ores
(b) Silicate ores
(c) Sulphide ores
(d) Carbonate ores
Show Answer & Explanation
Answer: (c) Sulphide ores
Explanation:
1. Roasting is heating in excess air.
2. Sulphide ores are converted into oxides with release of SO2, for example 2ZnS + 3O2 gives 2ZnO + 2SO2.
Teacher's Note:
1. Carbonates are calcined, sulphides are roasted.
(a) CaCO3
(b) Lime
(c) SiO2
(d) CaO
Show Answer & Explanation
Answer: (c) SiO2
Explanation:
1. Basic fluxes (CaO, CaCO3, MgO) remove acidic impurities such as silica.
2. SiO2 is acidic and is used as an acidic flux for basic impurities.
Teacher's Note:
1. Choose the flux opposite in nature to the gangue.
(a) Calcination
(b) Roasting
(c) Smelting
(d) Ore dressing
Show Answer & Explanation
Answer: (a) Calcination
Explanation:
1. CaCO3 gives CaO + CO2 on heating in limited air or no air.
2. Heating a carbonate to drive off CO2 is calcination.
Teacher's Note:
1. Roasting needs excess air; calcination does not.
(a) An acidic flux is needed
(b) A basic flux is needed
(c) Both acidic and basic fluxes are needed
(d) Neither is needed
Show Answer & Explanation
Answer: (b) A basic flux is needed
Explanation:
1. Silica is an acidic oxide.
2. A basic flux such as CaO combines with it to form fusible slag, CaSiO3.
Teacher's Note:
1. Acid + base gives slag.
(a) FeO
(b) FeSiO3
(c) MgSiO3
(d) CaSiO3
Show Answer & Explanation
Answer: (d) CaSiO3
Explanation:
1. Limestone gives CaO on heating.
2. CaO + SiO2 gives CaSiO3, which melts and floats as slag on molten iron.
Teacher's Note:
1. For copper the slag is FeSiO3, for iron it is CaSiO3.
(a) 4Cu2O + FeS gives 8Cu + FeSO4
(b) Cu2S + 2Cu2O gives 6Cu + SO2
(c) 2Cu2O + FeS gives 4Cu + Fe + SO2
(d) Cu2S + 2FeO gives 2Cu + 2FeCO + SO2
Show Answer & Explanation
Answer: (b) Cu2S + 2Cu2O gives 6Cu + SO2
Explanation:
1. In the converter, part of Cu2S is oxidised to Cu2O.
2. Cu2O then reacts with the remaining Cu2S in self-reduction: 2Cu2O + Cu2S gives 6Cu + SO2.
Teacher's Note:
1. Self-reduction needs no carbon.
2. Check that the equation balances: Cu 4 + 2 = 6, O 2, S 1.
(a) Pb
(b) Al
(c) Hg
(d) Zn
Show Answer & Explanation
Answer: (b) Al
Explanation:
1. Carbon reduces oxides of Pb and Zn (ZnO + C gives Zn + CO), and HgO decomposes thermally.
2. The oxide of Al is far too stable, so aluminium is obtained by electrolysis.
Teacher's Note:
1. Al2O3 lies below the carbon line on the Ellingham diagram up to very high temperatures.
(a) Cu2O, K2O
(b) Fe2O3, ZnO
(c) CaO, K2O
(d) PbO, Fe3O4
Show Answer & Explanation
Answer: (c) CaO, K2O
Explanation:
1. Oxides of Cu, Fe, Zn and Pb are reduced by carbon.
2. Oxides of calcium and potassium are very stable, so carbon cannot reduce them.
Teacher's Note:
1. Alkali and alkaline earth metals are obtained by electrolysis.
(a) Bauxite into aluminium
(b) Cuprite into copper
(c) Zinc oxide into zinc
(d) Haematite into iron
Show Answer & Explanation
Answer: (a) Bauxite into aluminium
Explanation:
1. Cuprite, zinc oxide and haematite are reduced by carbon or CO.
2. Alumina cannot be reduced chemically with carbon; electrolytic reduction is used.
Teacher's Note:
1. Think of the Ellingham diagram.
(a) Oxidising agent
(b) Reducing agent
(c) Flux
(d) Solder
Show Answer & Explanation
Answer: (b) Reducing agent
Explanation:
1. Aluminium has a very high affinity for oxygen, for example Cr2O3 + 2Al gives Al2O3 + 2Cr.
2. So it acts as a reducing agent (it gets oxidised).
Teacher's Note:
1. Thermite is a mixture of Al powder and a metal oxide.
(a) Heating cryolite in a limited air supply
(b) Reducing aluminium oxide with coke
(c) Reducing aluminium oxide with sodium
(d) Electrolysing aluminium oxide dissolved in a fused electrolyte
Show Answer & Explanation
Answer: (d) Electrolysing aluminium oxide dissolved in a fused electrolyte
Explanation:
1. Alumina is dissolved in molten cryolite with a little fluorspar and electrolysed at about 1233 K.
2. Carbon cannot reduce Al2O3, and sodium is far too costly.
Teacher's Note:
1. Hall-Heroult process.
(a) Alumino-thermic process
(b) Electrolytic reduction
(c) Carbon reduction
(d) Carbon monoxide reduction
Show Answer & Explanation
Answer: (a) Alumino-thermic process
Explanation:
1. Carbon reduction of Cr2O3 gives chromium carbide impurities.
2. Reduction by aluminium is used: Cr2O3 + 2Al gives 2Cr + Al2O3.
Teacher's Note:
1. Aluminothermy gives carbon-free metals such as Cr and Mn.
(a) To expel the dissolved gases
(b) To bring the impurities to the surface and oxidise them
(c) To increase the carbon content of copper
(d) To reduce the metal oxide impurities with hydrocarbon gases liberated from the wood
Show Answer & Explanation
Answer: (d) To reduce the metal oxide impurities with hydrocarbon gases liberated from the wood
Explanation:
1. Green wood releases hydrocarbons and reducing gases on heating.
2. They reduce the dissolved Cu2O to copper (poling).
Teacher's Note:
1. Poling is used for blister copper and tin.
(a) Silver
(b) Copper
(c) Aluminium
(d) Zinc
Show Answer & Explanation
Answer: (c) Aluminium
Explanation:
1. Ag, Cu and Zn can be deposited from aqueous solutions of their salts.
2. Aluminium is more electropositive than hydrogen's discharge potential in water, so water is reduced instead of Al3+.
Teacher's Note:
1. Al is refined by Hoope's process using molten salts, not aqueous solution.
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