Obtaining & Using Metals (Edexcel GCSE Chemistry)

Exam Questions

3 hours25 questions
1a1 mark

Unreactive metals are found as uncombined metals in the Earth’s crust.

Which of the following metals is found uncombined in the Earth’s crust?

  A aluminium
  B gold
  C sodium
  D zinc
1b3 marks

When iron oxide is heated with carbon, iron is produced.

i)
Complete the word equation for the reaction.

   iron oxide + carbon → ............................................ + .......................................

(2)

ii)
What happens to the iron oxide during this reaction?

(1)

  A the iron oxide burns
  B the iron oxide is neutralised
  C the iron oxide is oxidised
  D the iron oxide is reduced
1c1 mark

Copper ore contains copper carbonate, CuCO3.

In the first stage of the extraction process, the copper carbonate is decomposed by heating to form copper oxide, CuO, and carbon dioxide.

CuCO3 → CuO + CO2

When 100g of copper carbonate is decomposed completely in this way, it is found that the total mass of products is 100g.

Give a reason why the starting mass of copper carbonate is always the same as the mass of the products formed.

1d1 mark

Zinc can be extracted from its ore by electrolysis or by heating the ore with carbon.

Give a reason for the method that is used.

1e2 marks

Figure 2 gives information about aluminium and tin

Figure 2

metal cost of 1kg/£ amount in Earth’s crust/%
aluminium 1.31 8
tin 12.60 0.0002

Give two reasons why it could be more important to recycle tin than to recycle aluminium. Use the information in Figure 2.

Reason 1

............................................................

Reason 2

............................................................

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2a6 marks

The reactivity of copper, magnesium and zinc was investigated.
Each metal was placed separately in dilute hydrochloric acid.
The amount of effervescence was observed.

i)
The same mass of metal was used in each experiment.
Which piece of apparatus should be used to find the mass of metal used? 
(1)
  A a balance
  B a pipette
  C a stopwatch
  D a thermometer

ii)
State two variables, apart from the mass of the metals, that should be controlled in this investigation.  
(2)
iii)
Magnesium produces the most vigorous effervescence.
Copper does not produce any effervescence.

Give the reason why copper does not produce any effervescence. 
(1)

iv)
The magnesium reacts with dilute hydrochloric acid to form magnesium chloride solution and hydrogen gas.

The equation for the reaction is
Mg (s) + 2HCl (aq) → MgCl2 (.....) + H2 (.....)
 
Fill in the missing state symbols in the spaces provided. 
(2)
2b
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3 marks

Potassium carbonate reacts with dilute sulfuric acid to form potassium sulfate.

i)
Potassium sulfate contains potassium ions, K+, and sulfate ions, SO42–
Write the formula of potassium sulfate. 
(1)
ii)
Equal volumes of a solution of potassium carbonate were reacted separately with an excess of dilute sulfuric acid solution.
Pure dry samples of potassium sulfate were obtained from the resulting solutions.

The experiment was repeated three times using the same conditions.

The masses of potassium sulfate obtained were
experiment 1 = 5.22 g
experiment 2 = 5.24 g
experiment 3 = 5.21 g

Calculate the mean mass of potassium sulfate obtained, giving your answer to two decimal places.  
(2)

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3a1 mark

Part of the reactivity series is shown in Figure 1.

edx-4-1e-q3a-reactivity-series

Figure 1

Reactive metals are found combined with other elements as ores in the Earth’s crust.

Which of these metals is always found as an ore?

A Calcium
B Copper
C Gold
D Silver
3b2 marks

Iron ore contains iron oxide.
Iron is extracted from iron oxide by heating the oxide with carbon.

The word equation for the reaction is:

Iron oxide + carbon → iron + carbon dioxide

i)
Name the substance that has been oxidised.

[1]

ii)
Name the substance that has been reduced.

[1]

3c1 mark

Aluminium can’t be extracted from its ores using carbon.
Electrolysis has to be used instead.

State why.

3d1 mark

Iron can be extracted from its ores using electrolysis but this method is not used.

Suggest why.

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4a1 mark

Part of the reactivity series is shown in Figure 1.

edx-4-1e-q3a-reactivity-series

Figure 1

Name one metal from Figure 1 that is found pure in the Earth’s crust.

4b2 marks

When iron is added to dilute hydrochloric acid bubbles are formed slowly.

i)
Predict how the speed of bubbles forming is different when calcium is added to dilute hydrochloric acid.

[1]

ii)
Give a reason for your answer.

[1]

4c1 mark

When zinc is added to copper sulfate the products are zinc sulfate and copper.

Write the word equation for this reaction.

4d1 mark

Which statement describes why this reaction happens?

A Copper is more reactive than zinc
B Copper sulfate is more reactive than zinc
C Zinc is more reactive than copper
D Zinc is more reactive than copper sulfate

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5a1 mark

The environmental impact of a product is assessed in a life-cycle assessment.

The stages of the life-cycle assessment of an aluminium can are shown below.
The stages are not in the correct order.

A     Using the cans

B     Disposal of the cans

C     Extracting aluminium from ores using electrolysis

D     Mining aluminium ores from the Earth’s crust

E     Manufacturing cans from aluminium

Write the stages in the correct order, using the letters A, B, C, D and E.

…………..   ……………   …………..   ………….   …………..

5b2 marks

Aluminium cans can be recycled.

Suggest how this is done.

5c1 mark

Give one advantage of recycling aluminium cans.

5d1 mark

Give one disadvantage of recycling aluminium cans.

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1a2 marks

A student carried out an experiment to see how reactive different metals are when they are placed in dilute hydrochloric acid.
A sample of each metal was placed in a separate test tube of acid.

When zinc reacts with dilute hydrochloric acid, a gas is given off and zinc chloride is formed.

i)
Which gas is given off?
(1)
  A carbon dioxide
  B chlorine
  C hydrogen 
  D oxygen 

ii)
What is the formula of zinc chloride?
(1)
  A ZnCl
  B Zn2Cl
  C ZnCl2 
  D Zn2Cl2 
1b2 marks

In the experiment, the student used the same amount of each metal in a finely powdered form.

State two factors, concerning the hydrochloric acid, which should also be controlled to produce valid results.

1c3 marks

Part of the reactivity series is shown in Figure 8.

most reactive magnesium
  aluminium
  iron
least reactive  silver

Figure 8

Iron is extracted from its ore by heating with carbon.
Aluminium is extracted from its ore using a different method.

i)
Give the name of the method used to extract aluminium.

(1)

ii)
Explain why aluminium is extracted by a different method rather than heating the ore with carbon.

(2)

1d2 marks

The extraction of iron involves the reduction of iron oxide, Fe2O3, by carbon monoxide, CO. During this reaction, the iron oxide is reduced to iron, Fe, and the carbon monoxide is oxidised to carbon dioxide.

Write the balanced equation for the reaction.

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21 mark

Some metals, such as aluminium, are extracted from their ores using electrolysis. 

Why are some metals extracted using electrolysis? 

  A They are native metals
  B They are more reactive than carbon
  C They have low melting points
  D They conduct electricity 

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3a
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4 marks

Most metals are extracted from ores found in the Earth’s crust.

The method used to extract a metal from its ore is linked to the reactivity of the metal.

Part of the reactivity series is shown in Figure 14.

fig-14-q9-1cho-1f-paper-1-june-2018

Figure 14

Iron ore contains iron oxide.

Iron is extracted from iron oxide by heating the oxide with carbon.

iron oxide + carbon → iron + carbon dioxide

i)
In this reaction
(1)
  A carbon is reduced
  B iron oxide is neutralised
  C iron oxide is reduced
  D iron is oxidised

ii)
The formula of the iron oxide is Fe2O3.
Calculate the maximum mass of iron that can be obtained from 240 tonnes of iron oxide, Fe2O3.
(relative atomic masses: O = 16, Fe = 56)
(3)
3b2 marks

Aluminium cannot be extracted by heating its oxide with carbon.

Aluminium has to be extracted from its oxide by electrolysis.

Explain why.

3c1 mark

Predict the method that will have to be used to extract calcium from its ore.

3d6 marks

Aluminium is extracted from its ore by electrolysis.

Iron is extracted from its ore by heating with carbon.

Both metals can also be obtained by recycling.

Explain the advantages of recycling aluminium and iron rather than extracting them from their ores.

3e2 marks

Higher Only

In recent years, researchers have been investigating alternative methods of extracting metals from soils.

Researchers have found that growing certain plants in appropriate areas can result in the phytoextraction of copper.

Describe how growing plants can result in the phytoextraction of copper.

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41 mark

Which of the following metals can not be extracted from its ore by reduction?

  A Iron
  B Zinc
  C Copper
  D Lithium

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5a1 mark

Metals are extracted from substances naturally occurring in the Earth’s crust.

Which of these metals is usually found uncombined in the Earth's crust? 

  A calcium
  B gold
  C iron
  D magnesium
5b3 marks

Zinc can be extracted by heating zinc oxide with carbon.

The products are zinc and carbon dioxide.

 
i)
Write the word equation for this reaction. 
(2)
ii)
In this reaction zinc oxide loses oxygen.

State the type of reaction taking place when an oxide loses oxygen. 
(1)
5c3 marks

Aluminium is extracted from aluminium oxide by electrolysis.

Aluminium oxide is made up of ions.

i)
The formula of aluminium oxide is Al2O3.

Give the number of ions in the formula Al2O3.  
(1)
ii)
Complete the balanced equation for the overall reaction by putting numbers in the spaces.  
(2)
2Al2O3 → ..........Al + ..........O2
5d4 marks
i)
The environmental impact of a product is assessed in a life-cycle assessment.

The stages in this assessment are given below.
They are not in the correct order.

  A disposal of the product
  B manufacturing the product
  C obtaining and processing the raw materials
  D using the product

List the stages of the life-cycle assessment, using letters A, B, C, D, in the correct order from start to finish. 
(2)
4-boxes
  
ii)
Aluminium can be obtained by recycling aluminium waste.

Give two advantages of obtaining aluminium by recycling aluminium waste rather than mining the raw material and extracting aluminium from that raw material.  
(2)

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61 mark

A student was investigating the reactivity of different metals in hydrochloric acid. 

q3-4-1-investigating-reactivity-of-different-metals

What must the student keep constant in this investigation to make it a fair experiment?

(1)

      Control variable 1 Control variable 2
  A mass of metal concentration of acid
  B volume of acid length of metal
  C size of metal temperature of acid
  D temperature of room type of acid

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7a
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4 marks

Higher Only

One way to extract metals from land contaminated with metal compounds is phytoextraction.

When plants grow they absorb metal ions through their roots.

The plants are harvested, dried and burned forming an ash.

The ash contains metal compounds.

Plants were grown in a piece of ground contaminated with nickel compounds.

 
i)
1 kg of the ash from these plants contained 142.0 g of nickel compounds.

Calculate the percentage by mass of nickel compounds in the ash.
 
(3)
 
percentage by mass = ...............................
 
ii)
Nickel is extracted from nickel compounds.
 
State an advantage of extracting nickel by phytoextraction rather than from its ore.
 
(1)
7b3 marks

Some nickel ores contain nickel sulfide.

i)
In the first stage of extracting nickel from nickel sulfide, the nickel sulfide, NiS, is heated in air to form nickel oxide, NiO, and sulfur dioxide.

Write the balanced equation for this reaction.

(2)

ii)
In the final stage of the extraction process, a nickel compound is electrolysed to produce pure nickel.

An advantage of producing a metal by electrolysis is that:

(1)

  A electrolysis uses a large amount of energy
  B the metal produced by electrolysis is very pure
  C electrolysis is a very cheap method of extraction
  D electrolysis is the only method of extracting unreactive metals
7c3 marks
In a different method of obtaining nickel, the process produces a mixture of the liquids nickel tetracarbonyl and iron pentacarbonyl.

The boiling point of nickel tetracarbonyl is 43 °C.
The boiling point of iron pentacarbonyl is 103 °C.
These two liquids mix together completely. 

Describe the process used to separate these two liquids.

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81 mark

Some metals are unreactive and exist on their own in the earth. 

What are these metals known as?

  A Transition metals
  B Native metals
  C Alkali metals
  D Alkali earth metals

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9a2 marks

Pieces of zinc react with copper sulfate solution.
Zinc sulfate solution is colourless.

Zn (s) + CuSO4 (aq) → Cu (s) + ZnSO4 (aq)

Describe what you would see when an excess of zinc is added to copper sulfate solution and the mixture left until the reaction is complete.
9b4 marks

Higher Only

This reaction is described as a redox reaction.

Explain, in terms of electrons, which particles have been oxidised and which particles have been reduced in this reaction.

9c
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3 marks

Higher Only

The copper sulfate solution used has a concentration of 15.95 g dm−3.


Calculate the number of moles of copper sulfate, CuSO4, in 50.00 cm3 of this solution.

(relative atomic masses: O = 16, S = 32, Cu = 63.5)
 
 
number of moles of copper sulfate = ............................... mol
9d
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2 marks

In another experiment, 0.043 mol of copper sulfate, CuSO4, is used.

 

Calculate, to one decimal place, the minimum mass of zinc that must be added to react with all the copper sulfate.

(relative atomic mass: Zn = 65)
  
mass = ............................... g

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101 mark

Zinc is extracted from zinc oxide by reduction.

Which element is oxidised during this process?

  A Hydrogen
  B Oxygen
  C Carbon
  D Zinc

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11a1 mark

Some metals are found in the Earth’s crust as uncombined elements.
Reactive metals are found in ores.

In ores, metals are combined with other elements.

Which of these metals is found as the uncombined element in the Earth’s crust?

  A aluminium
  B gold 
  C potassium 
  D zinc 
11b2 marks

Give two advantages of recycling metals rather than extracting metals from their ores.

11c1 mark

An ore of iron is mostly iron oxide, Fe2O3.
Iron can be extracted from this iron oxide by heating it with carbon.

Balance this equation for the reaction that takes place.

2Fe2O3 + ................C → ................Fe + ................CO2
11d
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2 marks

Most copper ores are described as low grade.
This means that the percentage of copper in the ore is very small.

5000 kg of one copper ore was found to contain 42.5 kg of copper.

Calculate the percentage of copper in this ore.

percentage of copper in ore = ...........................................
11e2 marks

In one stage of the extraction of lead from its ore, lead oxide is heated strongly with carbon.

The equation for the reaction is 

2PbO + C → 2Pb + CO2 
 

Explain, using this equation, which substance has been oxidised in this reaction.

11f
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3 marks

A titanium ore was analysed and found to contain 12 g of titanium atoms combined with 8.0 g of oxygen atoms.

Calculate the empirical formula of this titanium compound.
(relative atomic masses: Ti = 48, O = 16)

You must show your working.

empirical formula = ............................................

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121 mark

Coffee cups are usually made from ceramic, glass, paper, plastic or metal.

Some of these materials are recyclable. In a Life Cycle Assessment (LCA) where would this information be given?

  A During the extraction and processing of the raw materials needed to make the cup
  B Disposing of the cup at the end of its useful life
  C When the cup is manufactured and packaged
  D During the use and lifetime of the cup

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13a4 marks

When chromium reacts with oxygen, chromium oxide is formed.

i)
Write the word equation for this reaction.

(1)

............... + ................ → ..............

ii)
What type of reaction occurs when chromium reacts with oxygen?

  A condensation
  B evaporation
  C neutralisation
  D oxidation

(1)

iii)

Calculate the relative formula mass of chromium oxide, Cr2O3.

(relative atomic masses: O = 16, Cr = 52)

(2)

relative formula mass = .............................................................

13b3 marks

Three different metals are added to separate test tubes of acid.

The observations are shown in Figure 4.

metal observation
silver no change is seen
iron very slow bubbling
magnesium steady bubbling


Figure 4

i)
Place the metals in order of reactivity from most to least reactive.

(1)
most reactive .............................................................

least reactive .............................................................

ii)

Hydrogen is given off when magnesium reacts with acid.
The hydrogen is tested by collecting the gas in a test tube and igniting it.

What is the safest way to ignite the gas?

  A add fuel to the test tube
  B heat the test tube with a Bunsen burner
  C put a lighted splint at the open end of the test tube
  D put the test tube in an oven

(1)

iii)

State the observation made in this test that shows that the gas is hydrogen.

(1)

13c2 marks

Iron is extracted by heating iron oxide with carbon.

Electrolysis of molten iron oxide is not used to extract iron.

i)
State why iron can be extracted by heating iron oxide with carbon.
(1)
ii)
State why electrolysis is not used to extract iron.

(1)

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141 mark

Higher Only 

Copper can be extracted from low grade ores using bioleaching. 

A leachate solution is produced.

Which process is used to extract the copper from the leachate solution?

  A Distillation
  B Cracking
  C Displacement
  D Fermentation

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151 mark

A reaction took place between iron sulfate and magnesium. 

iron(II) sulfate + magnesium  →    magnesium sulfate + iron 

Which species has been oxidised?

  A Iron
  B Magnesium
  C Sulfur
  D None of the above

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1a3 marks

The order of reactivity of copper, magnesium and zinc can be determined by the displacement reactions between these metals and solutions of their salts.

You are provided with

  • samples of the three metals
  • solutions of copper sulfate, magnesium sulfate and zinc sulfate.

Describe the experiments that can be done to determine the order of reactivity of these metals by displacement reactions.

1b2 marks

Metals can be extracted from ores found in the Earth’s crust.


Explain why aluminium cannot be extracted from its ore by heating with carbon but can be extracted by electrolysis.

1c1 mark

Titanium is extracted from its ore in several stages.

In the first stage, titanium chloride is formed as a gas.

The gas is cooled to form liquid titanium chloride containing dissolved impurities.

Suggest how pure titanium chloride could be separated from the impurities.

1d
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3 marks

Higher Only

In another stage, the pure titanium chloride, TiCl4 , is reacted with 500 moles of magnesium, an excess.

TiCl4 + 2Mg → Ti + 2MgCl2

i)

Calculate the number of moles in 45 000 grams of titanium chloride.
(relative atomic masses: Cl = 35.5, Ti = 48.0)

(2)
number of moles titanium chloride = ...............................................................

ii)
Show that the 500 moles of magnesium added is an excess.

(1)

1e2 marks

After this reaction, there is a mixture of the solids magnesium, titanium and magnesium chloride.

Titanium does not react with dilute hydrochloric acid.

Suggest a simple method to separate titanium from the mixture.

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2a1 mark

Phytomining can be used to extract copper compounds from the soil.

Plants are grown on the soil and they absorb the copper compounds through their roots.
The plants are then harvested, dried and burnt to form an ash.
The ash contains the copper compounds.

One example of a copper compound extracted this way is copper oxide.
The copper oxide is added to acid where it reacts to form copper sulfate solution.
Give the formula of the acid used in this reaction.

2b1 mark

Higher Only

Copper is extracted from copper sulfate solution using scrap iron.

Explain why it is economical to use scrap iron for this function.

2c1 mark

Explain why scrap iron can be used to extract copper from copper sulfate.

2d1 mark

Higher Only

Describe one advantage of extracting copper by phytoextraction rather than from its ore.

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3a3 marks

Lead is found in the Earth’s crust in ores.
In ores, the lead is combined with other elements.

5000 kg of lead ore was found to contain 48 200 g of lead.

Calculate the percentage of lead in the ore.
Give your answer to 2 significant figures.

3b2 marks

The lead ore contains lead oxide (PbO).
To extract lead from lead oxide it is heated strongly with carbon.

Write the balanced symbol equation for this reaction.

3c2 marks

Explain which substance is oxidised, and which is reduced.

3d2 marks

Figure 1 shows the reactivity series of metals.

A non-metal - carbon - has also been included.

edx-4-1h-q3d-reactivity-series

Figure 1

Use Figure 1 to explain why:

i)
Lead can be extracted from its ores by heating with carbon.

[1]

ii)
Aluminium can only be extracted from its ores using electrolysis.

[1]

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4a1 mark

Calcium is added to a beaker of silver nitrate solution.

A reaction takes place.

The symbol equation for the reaction is:

Ca(s) + 2AgNO3(aq) → Ca(NO3)2 (aq) + 2Ag(s)

Explain why this reaction happens in terms of reactivity.

4b2 marks

Higher Only

Write the ionic equation for this reaction.

4c2 marks

Higher Only

Explain why this reaction is an example of a redox reaction.

4d2 marks

Potassium is more reactive than calcium.

Use the electronic structure of these elements to suggest why.

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5a2 marks

Figure 1 shows how five different metals - A, B, C and D react when heated in oxygen.

The same size and shape piece of metal was used for each.

Metal Heated in oxygen
A Glows and changes colour slowly
B No change
C Bursts into flames and colour change happens quickly
D No glowing or bursting into flames. Colour changes slowly

Figure 1

Most of the metals undergo a chemical reaction.

i)
Give one sign from Figure 2 that is evidence that a chemical reaction has happened.

[1]

ii)
Name this reaction.

[1]

5b1 mark

Order the metals in terms of reactivity, starting with the least reactive.

5c2 marks

The same metals are added to dilute hydrochloric acid.

Write the balanced symbol equation when magnesium reacts with hydrochloric acid.

5d2 marks

Predict what would be observed when:

i)
Metal C is added to the acid.

[1]

ii)
Metal B is added to the acid.

[1]

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