Extraction of metals Flashcards
Explain why calcium has a higher melting point than strontium.(2)
Calcium has a higher melting point than strontium, because1.Correct reference to size of cations/proximity of electrons(For Ca) delocalised electrons closer to cations / positive ions / atoms / nucleusOR cations / positive ions / atoms are smallerOR cation / positive ion / atom or it has fewer (electron) shells / levels2. Relative strength of metallic bonding (Ca) has stronger attraction between the cations / positive ions / atoms / nucleus and the delocalised electronsORstronger metallic bonding
Magnesium is used in fireworks. It reacts rapidly with oxygen, burning with a bright white light. Magnesium reacts slowly with cold water.Write an equation for the reaction of magnesium with oxygen. Write an equation for the reaction of magnesium with cold water.Give a medical use for the magnesium compound formed in the reaction of magnesium with cold water.
2Mg + O2 ——>2MgOM2 Mg + 2H2O Mg(OH)2 + H2Magnesium hydroxide is used as an antacid / relieve indigestion (heartburn) / neutralise (stomach) acidity / laxative
State why the value for the standard enthalpy of formation of Mn(s) is zero
Because it is an element / elemental
Titanium is extracted in industry from titanium(IV) oxide in a two-stage process.Write an equation for the first stage of this extraction in which titanium(IV) oxide is converted into titanium(IV) chloride.
TiO2 + 2Cl2 + 2C ———>TiCl4 + 2CO
Write an equation for the second stage of this extraction in which titanium(IV) chloride is converted into titanium.
TiCl4 + 4Na ————->Ti + 4NaCl
Chromium is extracted in industry from chromite (FeCr2O4).In the first stage of this extraction, the FeCr2O4 is converted into Na2CrO4 Balance the equation for this reaction……….. FeCr2O4 + ………. Na2CO3 + ………. O2 ———> ………. Na2CrO4 + 2Fe2O3 + 8CO2
4FeCr2O4 + 8Na2CO3 + 7O2 ———->8Na2CrO4 + 2Fe2O3 + 8CO2
In the final stage, chromium is extracted from Cr2O3 by reduction with aluminium. Write an equation for this reaction.
Cr2O3 + 2Al ——–>Al2O3 + 2Cr
Metals can be extracted by different methods.Give one reason why titanium cannot be extracted directly from titanium(IV) oxide using carbon.
Ti is not producedORTiC / carbide is produced OR titanium reacts with carbonORProduct is brittleORProduct is a poor engineering material
Titanium steel is an alloy of titanium and iron. Titanium steel is extracted from the mineral ilmenite (FeTiO3) in a two-stage process.Purified FeTiO3 is first converted into a mixture of two metal chlorides. These two metal chlorides are then reduced simultaneously using sodium.Write an equation for the reaction of FeTiO3 with chlorine and carbon to produce iron(III) chloride (FeCl3), titanium(IV) chloride and carbon monoxide.
FeTiO3 + 31⁄2Cl2 + 3C ——>FeCl3 + TiCl4 + 3CO
Write an equation for the simultaneous reduction of the mixture of iron(III) chloride and titanium(IV) chloride to iron and titanium using sodium.
FeCl3 +TiCl4 +7Na —————>7NaCl+Fe+Ti
Scrap iron is used to extract copper from dilute aqueous solutions containing copper(II) ions.Explain, in terms of redox, what happens to the copper(II) ions in this extraction.
The Cu2+ / copper(II) ions / they have gained (two) electronsOR Cu2+ + 2e– ——>CuOR oxidation state / number decreases (or specified from 2to 0)ANDThe Cu2+ / copper(II) ions / they have been reduced
Aluminium is an expensive metal because it is extracted from molten aluminium oxide using electrolysis.Write the half-equation for the reaction that occurs at the positive electrode during this extraction.
2O2– ————>O2 + 4e–
Iron is extracted from iron(III) oxide using carbon at a high temperature.State the type of reaction that iron(III) oxide undergoes in this extraction.
reduction
Write a half-equation for the reaction of the iron(III) ions in this extraction.
Fe3+ + 3e– ————-> Fe
At a high temperature, carbon undergoes combustion when it reacts with oxygen. Suggest why it is not possible to measure the enthalpy change directly for the followingcombustion reaction.C(s,graphite) + 1/2 O2(g) —–> CO(g)
CO is not the only product OR(Some) complete combustion (also)occurs ORCO2 is (also) formedFurther oxidation occurs
This question is about the extraction of titanium from titanium(IV) oxide by a two-stage process.The first stage in the process produces titanium(IV) chloride. In the second stage, titanium(IV) chloride is converted into titanium.The enthalpy change for the second stage can be determined using Hess’s Law.Give one reason why titanium is not extracted directly from titanium(IV) oxide using carbon.
One from 1 Ti is not produced TiC / carbide is produced (NOT TITANIUM CARBONATE) OR titanium reacts with carbon Product is brittle Product is a poor engineering material
Give the meaning of the term enthalpy change.
Heat (energy) change at constant pressure
Define the term standard enthalpy of formation.
The enthalpy change / heat change at constant pressure when 1 mol of a compound / substance / product is formed from its (constituent ) elementswith all reactants and products / all substances in standardstates i.e. 100 kPa / 1 bar and any specified T (usually 298 K)
Metals are usually extracted from oxides.Some of these oxides occur naturally. Other oxides are made by roasting sulfide ores in air, producing sulfur dioxide as a by-product.For the extraction of some metals, the oxide needs to be converted into a chloride.The ore molybdenite contains molybdenum disulfide (MoS2).The first stage in the extraction of molybdenum is to roast the ore in air to form molybdenum oxide (MoO3) and sulfur dioxide.Write an equation for the first stage in this extraction.
2MoS2 + 7O2———->2MoO3 + 4SO2
The release of sulfur dioxide into the atmosphere causes environmental problems and wastes a valuable resource. Identify one environmental problem and identify one use for the sulfur dioxide.
Acid rain (NOT GREENHOUSE GASES)SO2 could be used to make H2SO4 / sulfuric acidORTo make CaSO4 or plaster of Paris / plaster board
Pure molybdenum is formed in the second stage by the reduction of MoO3 using hydrogen.Write an equation for this reaction.
MoO3 + 3H2 ————–>Mo + 3H2O
State one risk in using hydrogen gas in metal extractions.
Explosive or easily ignited
Calcium is an expensive metal. It is extracted by the electrolysis of molten calcium chloride.State why calcium chloride must be molten for electrolysis to occur.
To allow ions to move (when molten) ORIons cannot move in the solid
Write an equation for the reaction that takes place at the negative electrode during this electrolysis.
Ca2+ + 2e- ———–>Ca
Identify the major cost in this extraction of calcium.
electricity
Titanium and aluminium are both extracted from their oxides. Both extraction processes require high temperatures.5 (a) Outline the essential features of the extraction process used to obtain titanium from titanium(IV) oxide. Illustrate your answer with equations.Give three reasons why the manufacture of pure titanium is expensive(7)
React with carbon/coke and chlorineTiO2 +2C+2Cl2—–> TiCl4 +2COReact with Na (or Mg); TiCl4 + 4Na ——>Ti + 4NaClNa / sodium neededCl2 / chlorine neededArgon needed/ TiCl4 hydrolysedEnergy needed to give the high temp Batch process
here has been a great deal of research into finding cheaper methods of extracting pure titanium but so far none has been commercially successful.Give a reason why a cheaper method, using direct reduction of titanium(IV) oxide by carbon, has been unsuccessful.State one property of titanium which makes it more useful than aluminium
TiC /carbide forms Stronger/ higher melting point ./more resistant to corrosion
In the presence of cryolite, aluminium is extracted from its oxide by electrolysis. State the essential condition for this electrolysis and write half-equations for the reactions occurring at the electrodes. Give the main reason why this process is expensive
MoltenAl3+ + 3e- —–>Al2O2− —–>O2 +4e- A lot of electricity needed
Give two reasons why recycling aluminium is environmentally beneficial.
Less CO2 / greenhouse gas given off; No unsightly landfills;Conserves earth resources;Less mining;Avoids fluoride pollution
Pure manganese is extracted from the ore pyrolusite (MnO2) by reduction using carbon monoxide.Write an equation for the reduction of MnO2 to manganese using carbon monoxide.
MnO2 + 2CO  ——> Mn + 2CO2
Impure manganese is extracted by reduction of Mn3O4 using powdered aluminium according to the following equation.3Mn3O4 + 8Al → 9Mn + 4Al2O3Deduce the redox half-equation for aluminium in this extraction process
Al  ——> Al3+ + 3e―
Copper can be extracted by the high-temperature carbon reduction of copper(II) oxide. Write an equation for this reaction.
2CuO + C  ——->2Cu +CO2 ORCuO + C  ———>Cu + CO
Scrap iron is used in a low-cost process to extract copper from aqueous solutions containing copper(II) ions.Give 3 reasons, other than the cost of scrap iron, why this method is low-cost.
Low(er) energy requirementLow(er) temperatureCopper is obtained from low grade ore
Write the simplest ionic equation for the reaction of iron with copper(II) ions in aqueous solution
Fe + Cu2+  ———>Fe2+ + Cu
Sea water contains large amounts of dissolved magnesium compounds. Approximately 1 kg of magnesium can be extracted from 1000 dm3 of sea water.The first step in the extraction process is to react the magnesium ions in sea water with hydroxide ions to produce a precipitate of magnesium hydroxide.Write the simplest ionic equation for this reaction.
Mg2+ + 2OH– ——-> Mg(OH)2
The second step in the extraction process is to react magnesium hydroxide with hydrochloric acid to give magnesium chloride. Write an equation for this reaction.
Mg(OH)2 + 2HCl  ———> MgCl2 + 2H2O
In the final step, molten magnesium chloride is electrolysed to form magnesium and chlorine. This is similar to the method used to extract aluminium.Deduce an equation for the reaction that occurs at the negative electrode in the electrolysis of magnesium chloride.
Mg2+ +2e– ——–> Mg
Magnesium is used in the extraction of titanium.Write an equation for the conversion of titanium(IV) oxide into titanium(IV) chloride.
TiO2 + 2Cl2 + 2C  ——–> TiCl4 + 2COorTiO2 + 2Cl2 + C  ———> TiCl4 + CO2
Write an equation for the extraction of titanium from titanium(IV) chloride using magnesium.
TiCl4 + 2Mg ———>  Ti + 2MgCl2
State the role of magnesium in this extraction.
Reducing agent OR reduces TiCl4 ORElectron donor
Use your knowledge of the reactions of Group 2 metals with water to explain why water should not be used to put out a fire in which magnesium metal is burning
Hydrogen / H2 producedcausing an risk of explosion
In the first stage of zinc extraction process the following equilibrium is established when zinc carbonate is heated in a closed container.ZnCO3(s) ZnO(s) + CO2(g)Use Le Chatelier’s principle to suggest and explain the effect on the yield of zinc oxide of allowing the carbon dioxide to escape from the container
The yield of zinc oxide increases / greaterthe removal of the carbon dioxide results in the equilibrium either shifting / moving / goes to the right(By Le Chatelier’s principle) the reaction/equilibrium will respond so asto replace the CO2 / lost product
Hydrogen gas is used in the chemical industry. Tungsten is extracted by passing hydrogen over heated tungsten oxide (WO3). State the role of the hydrogen in this reaction.Write an equation for this reaction.
Reducing agent 1ORReduce(s) (WO3 / tungsten oxide)ORelectron donorORto remove oxygen (from WO3 / tungsten oxide or to form water)WO3 +3H2 ——-> W+3H2O
State one risk of using hydrogen gas in metal extractions.
H2 is• explosive• flammable or inflammable• easily ignited
