Extraction of Metals and Iron from Hematite
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Questions and Answers

Which element is extracted from hematite?

  • Iron (correct)
  • Aluminium
  • Zinc
  • Copper

The least reactive element mentioned in the notes is gold.

True (A)

What is the primary purpose of a blast furnace in metal extraction?

To extract iron from its ore.

Iron is extracted from hematite using a large container called a ______.

<p>blast furnace</p> Signup and view all the answers

Match the following elements with their extraction methods:

<p>Copper = Heating with carbon or hydrogen Zinc = Heating with reducing agent such as carbon Iron = Blast furnace from hematite Gold = Found as pure element</p> Signup and view all the answers

What is the role of coke in the extraction of iron?

<p>To burn and produce heat (C)</p> Signup and view all the answers

Calcium carbonate decomposes to form calcium oxide and carbon monoxide.

<p>False (B)</p> Signup and view all the answers

What is formed when carbon monoxide reduces iron(III) oxide?

<p>iron</p> Signup and view all the answers

The process of removing impurities from iron ore using lime is called _____ .

<p>fluxing</p> Signup and view all the answers

Match the materials to their roles in the extraction of iron:

<p>Iron ore (Hematite) = Provides iron Coke = Fuel and reducing agent Limestone = Removes impurities Hot air = Supports combustion</p> Signup and view all the answers

Which chemical reaction occurs in Zone 2 of the blast furnace?

<p>Carbon + carbon dioxide → carbon monoxide (D)</p> Signup and view all the answers

The molten slag floats on top of the molten iron in the blast furnace.

<p>True (A)</p> Signup and view all the answers

What two substances react to form calcium silicate?

<p>calcium oxide and silicon dioxide</p> Signup and view all the answers

What is the purpose of dissolving aluminium oxide in molten cryolite?

<p>To lower the melting point and reduce energy consumption (A)</p> Signup and view all the answers

Carbon dioxide is produced at the cathode during aluminium extraction.

<p>False (B)</p> Signup and view all the answers

What is the formula for aluminium oxide?

<p>Al2O3</p> Signup and view all the answers

At the __________, aluminium ions gain electrons and molten aluminium forms.

<p>cathode</p> Signup and view all the answers

Which of the following equations correctly represents the oxidation process at the anode?

<p>2O2- → O2 + 4e- (D)</p> Signup and view all the answers

Match the following terms with their definitions:

<p>Reduction = Gaining electrons Oxidation = Losing electrons Cathode = Negative electrode Anode = Positive electrode</p> Signup and view all the answers

What happens to the anode during the extraction of aluminium?

<p>It wears away and needs to be replaced regularly.</p> Signup and view all the answers

The overall reaction for the extraction of aluminium can be summarized as __________.

<p>2Al2O3 → 4Al + 3O2</p> Signup and view all the answers

Which equation represents the burning of carbon to produce carbon dioxide?

<p>C (s) + O2 (g) → CO2 (g) (C)</p> Signup and view all the answers

Aluminium can be extracted from bauxite using carbon reduction.

<p>False (B)</p> Signup and view all the answers

What is the main ore of aluminium?

<p>bauxite</p> Signup and view all the answers

The reduction of iron(III) oxide by carbon monoxide produces ______.

<p>iron</p> Signup and view all the answers

What is produced when calcium carbonate decomposes?

<p>CaO and CO2 (A)</p> Signup and view all the answers

Match the reactions with their corresponding zones in iron extraction:

<p>C (s) + O2 (g) → CO2 (g) = Zone 1 CO2 (g) + C (s) → 2CO (g) = Zone 2 Fe2O3 (s) + 3CO (g) → 2Fe (I) + 3CO2 (g) = Zone 3 CaCO3 (s) → CaO (s) + CO2 (g) = Zone 3</p> Signup and view all the answers

Electrolysis is the method used to extract aluminium from its ore.

<p>True (A)</p> Signup and view all the answers

The formation of slag involves the reaction of CaO with ______.

<p>SiO2</p> Signup and view all the answers

What is a metal ore?

<p>A rock that contains enough metal to make extraction worthwhile (A)</p> Signup and view all the answers

Native metals are found in chemically combined forms.

<p>False (B)</p> Signup and view all the answers

Name two examples of native metals.

<p>Gold and Platinum</p> Signup and view all the answers

The extraction method for metals high in the reactivity series, such as potassium and sodium, involves __________.

<p>electrolysis</p> Signup and view all the answers

Match the following metals with their methods of extraction:

<p>Iron = Blast furnace Gold = Mined directly Aluminium = Electrolysis Copper = Heating with carbon</p> Signup and view all the answers

Which of the following metals requires extraction by electrolysis?

<p>Aluminium (C)</p> Signup and view all the answers

Reactive metals are typically found in their uncombined form.

<p>False (B)</p> Signup and view all the answers

What is the main process involved in the extraction of metals from oxide ores?

<p>Reduction</p> Signup and view all the answers

Flashcards

What is a metal ore?

A rock that contains enough of a metal to make it worthwhile extracting.

What is reduction in terms of metals?

The process of removing oxygen from a compound.

How are metals found in the Earth's crust?

Metals are often chemically combined with other substances in the Earth's crust.

How are metals above carbon extracted?

Metals placed above carbon in the reactivity series are extracted using electrolysis.

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How are metals below carbon extracted?

Metals placed below carbon in the reactivity series can be extracted by heating with carbon.

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What are the ores of iron and aluminium?

Hematite is the ore of iron and bauxite is the ore of aluminium.

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What are native metals?

Unreactive metals are often found as the uncombined element.

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How does the reactivity series affect metal extraction?

The extraction method of a metal depends on its position in the reactivity series.

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What is reduction?

The process of removing oxygen from a compound.

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How are metals more reactive than carbon extracted?

Metals that are more reactive than carbon can be extracted using electrolysis. This process uses electricity to break down the metal compound.

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How are metals less reactive than carbon extracted?

Metals that are less reactive than carbon can be extracted by heating their ores with carbon or carbon monoxide. The carbon acts as a reducing agent.

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How is iron extracted?

Iron is extracted from its ore, hematite, in a large container called a blast furnace. The process uses carbon monoxide to reduce the iron oxide to iron.

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What is the reactivity series?

The reactivity series is a list of metals arranged in order of their reactivity. Metals higher in the series are more reactive.

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What is reduction in terms of metal extraction?

The process of removing oxygen from a compound. During the extraction of iron, carbon monoxide acts as a reducing agent, removing oxygen from iron(III) oxide to produce iron.

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What is an exothermic reaction?

A chemical reaction that releases heat energy into the surroundings. In the blast furnace, the burning of coke in hot air is an exothermic reaction, which provides heat for the entire process.

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What is a flux?

A substance that is added to a reaction to remove impurities. Limestone is added to the blast furnace to remove impurities in the iron ore, specifically silicon dioxide.

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What is slag?

A molten mixture of impurities that forms in the blast furnace. Calcium oxide reacts with silicon dioxide (impurity in iron ore) to form calcium silicate, which melts and forms slag.

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What is thermal decomposition?

The process by which a compound breaks down into simpler substances when heated. In the blast furnace, limestone (calcium carbonate) thermally decomposes to form calcium oxide and carbon dioxide.

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What is the extraction of iron?

The process of extracting iron from its ore (hematite). It involves a series of chemical reactions in a blast furnace.

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What is coke?

A form of carbon used in the extraction of iron. Coke burns in the hot air, providing the heat for the process. It also reacts with carbon dioxide to form carbon monoxide, which is the reducing agent.

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What is hematite?

A type of iron ore containing iron(III) oxide. Other types of iron ores include magnetite and siderite, but hematite is the most common.

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What is reduction using carbon?

The process of extracting metals from their ores by using heat and a reducing agent, typically carbon.

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What is electrolysis?

The process used to extract metals that are more reactive than carbon, involving the passage of electricity through a molten electrolyte.

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What is bauxite?

The aluminium ore used in the extraction of aluminium.

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What is Zone 1 in iron extraction?

The first step in the extraction of iron from hematite, where carbon (coke) burns in the presence of oxygen to generate heat and produce carbon dioxide.

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What is Zone 2 in iron extraction?

The second step in the extraction of iron from hematite, where carbon dioxide reacts with carbon to form carbon monoxide.

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What is Zone 3 in iron extraction?

The third step in the extraction of iron from hematite, where carbon monoxide reduces iron(III) oxide to iron metal. Limestone is also decomposed to produce calcium oxide, which reacts with silica to form slag.

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Why is cryolite used in aluminium extraction?

Aluminium oxide (Al2O3) has a very high melting point, making it very expensive to melt. To solve this, it is dissolved in molten cryolite, which lowers the melting point without interfering with the electrolysis reaction.

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What are the electrodes in aluminium extraction?

In electrolytic extraction of aluminium, the graphite lining of the steel cell acts as the negative electrode (cathode), while large graphite blocks act as the positive electrodes (anode).

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What happens at the cathode during aluminium extraction?

At the cathode (negative electrode), aluminium ions (Al3+) gain electrons and are reduced to form molten aluminium. This aluminium collects at the bottom of the cell and is siphoned off periodically.

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What happens at the anode during aluminium extraction?

At the anode (positive electrode), oxide ions (O2-) lose electrons, undergoing oxidation to form oxygen gas (O2). The oxygen then reacts with the carbon of the anode, forming carbon dioxide (CO2).

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What is the overall reaction for aluminium extraction?

The overall reaction in aluminium extraction can be represented by the equation: 2Al2O3 → 4Al + 3O2 This equation shows that aluminium oxide breaks down into aluminium and oxygen gas.

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Why does the anode need to be replaced in aluminium extraction?

The reaction of oxygen with the carbon of the anode (C + O2 → CO2) results in the gradual wearing away of the anode. This means the anode needs to be replaced regularly.

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What is the main expense in aluminium extraction?

The process of aluminium extraction requires a significant amount of electricity, which is a major cost factor.

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What does the acronym OIL RIG represent?

OIL RIG stands for 'Oxidation Is Loss (of electrons), Reduction Is Gain (of electrons).'

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Study Notes

Extraction of Metals

  • Metals are often chemically combined with other substances in ores
  • Metal ores contain enough metal to make extraction worthwhile
  • Extraction methods include electrolysis, blast furnaces, and reacting with more reactive materials
  • Many ores are metal oxides, requiring reduction processes to remove oxygen
  • Common oxide ores include iron (hematite) and aluminium (bauxite)
  • Unreactive metals (e.g., gold, platinum) are often found in their elemental form (native metals)
  • Metal reactivity influences extraction method
  • Higher reactivity metals require electrolysis; lower reactivity metals require heating with carbon

Extraction of Iron from Hematite

  • Iron is extracted from its ore, hematite, in a blast furnace
  • Modern blast furnaces produce approximately 10,000 tonnes of iron per day
  • Raw materials include iron ore (hematite), coke (carbon), and limestone
  • The blast furnace is a large container
  • Three zones are crucial in the extraction process

Blast Furnace Zones

  • Zone 1: Coke burns in hot air, producing heat and carbon dioxide (CO2)
  • Zone 2: Carbon dioxide is reduced to carbon monoxide (CO) at high temperatures
  • Zone 3: Carbon monoxide reduces iron(III) oxide in the iron ore to form iron
  • Limestone (calcium carbonate) removes impurities (e.g., silicon dioxide) to form slag (calcium silicate)
  • Molten iron is collected at the bottom of the furnace and tapped off
  • Molten slag floats on top of the molten iron and is also tapped off

Equations for Iron Extraction (Extended Tier Only)

  • Zone 1: C + Oâ‚‚ → COâ‚‚
  • Zone 2: COâ‚‚ + C → 2CO
  • Zone 3: Feâ‚‚O₃ + 3CO → 2Fe + 3COâ‚‚
  • Limestone Decomposition: CaCO₃ → CaO + COâ‚‚
  • Slag Formation: CaO + SiOâ‚‚ → CaSiO₃

Extraction of Aluminium from Bauxite

  • Aluminium is extracted by electrolysis, as it's higher in the reactivity series than carbon
  • The main ore is bauxite, which contains aluminium oxide (Alâ‚‚O₃)
  • Bauxite is purified to produce aluminium oxide (Alâ‚‚O₃)
  • Aluminium oxide is dissolved in molten cryolite to lower the melting point for electrolysis
  • Electrolysis uses graphite anodes and a steel case lined with graphite as the cathode
  • Molten aluminium forms at the bottom of the cell and is tapped off
  • Oxide ions lose electrons at the anode producing oxygen
  • Aluminium ions gain electrons at the cathode forming aluminium metal
  • Requires a large amount of electricity
  • During electrolysis, carbon in the graphite anodes reacts with oxygen, producing carbon dioxide

Electrochemical Principles (Extended Tier Only)

  • OIL RIG: Oxidation Is Loss, Reduction Is Gain of electrons
  • Cathode: Negative electrode where reduction occurs (electrons gained)
  • Anode: Positive electrode where oxidation occurs (electrons lost)
  • Overall Equation (for aluminium): 2Alâ‚‚O₃ → 4Al + 3Oâ‚‚

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Cambridge (CIE) IGCSE Chemistry Extraction of Metals PDF

Description

This quiz explores the processes involved in the extraction of metals from ores, focusing specifically on iron extraction from hematite using blast furnaces. It delves into the various extraction methods and the role of metal reactivity in determining the appropriate approach for different metals.

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