IGCSEChemistryEdexcelExam Questions2. Inorganic ChemistryReactivity Series

Reactivity Series (Edexcel IGCSE Chemistry)

Exam Questions

2 hours19 questions
Easy
Medium
Hard
1a4 marks

This question is about rusting.

A simplified formula for rust is Fe2O3 

 
i)
Name the two substances needed for iron to rust.
 
(2)
 
ii)
Give the chemical name for rust.
 
(1)
 
iii)
What type of reaction occurs in the rusting of iron?
 
(1)
 
A combustion
B neutralisation
C oxidation
D thermal decomposition

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1b5 marks

Some iron objects are coated with a layer of zinc to prevent rusting.

 
i)
Name this type of rust prevention.
 
(1)
 
ii)
Explain how this type of rust prevention continues to protect iron when the layer of zinc is damaged.
 
(2)
 
iii)
Give two other methods used to prevent iron from rusting.
 
(2)

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21 mark

What type of reaction occurs when iron rusts?

  ☐ A Oxidation
  ☐ B Neutralisation
  ☐ C Combustion
  ☐ D Displacement

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31 mark

Which metal is most suitable for galvanizing iron?

  ☐ A Lead
  ☐ B Copper
  ☐ C Sodium
  ☐ D Zinc

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4a2 marks

Two substances are needed to cause iron to rust.

Name these two substances.

1.......................................................................................................................................

2.......................................................................................................................................

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4b3 marks

The box gives the names of some substances.

calcium copper gold
iodine methane zinc

Use words from the box to answer these questions.

i)
Give the name of a non-metallic element.

(1)

ii)
Give the name of a compound.

(1)

iii)
Give the name of the metal that is lowest in the reactivity series.

(1)

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5a2 marks

The following reaction occurs when zinc is added to a solution of copper(II) sulfate.

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

i)
Name the type of reaction occurring.
(1)

ii)
Give one observation for this reaction. 
(1)

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5b3 marks

Zinc also reacts with hydrochloric acid to form a salt and a gaseous product.

i)
Write a word equation for this reaction.

zinc + hydrochloric acid → ___________ _____________ + _______________

(1)

ii)
Describe how to test for the gas formed in this reaction.
(2)

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5c2 marks

Metals, such as the alkali metals, which are more reactive than zinc react readily with water. State two observations for the reaction of an alkali metal and water.

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5d1 mark

When Group 1 metals react with water they are oxidised and form the metal hydroxide. What is the correct definition of oxidation.

  ☐ A Gain of electrons
  ☐ B Loss of electrons
  ☐ C Loss of oxygen
  ☐ D Gain of hydrogen

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1a3 marks

This question is about metals.

Metals can be arranged in a reactivity series based on their reactions with water and their reactions with dilute hydrochloric acid. 

The table shows how four metals, P, Q, R and S, react with water and with dilute hydrochloric acid.

 
Metal Reaction with water Reaction with dilute hydrochloric acid
P no reaction hydrogen gas forms very slowly
Q no reaction no reaction
R hydrogen gas forms very quickly not done
S hydrogen gas forms quickly hydrogen gas forms very quickly
 
i)
Identify which of the metals P, Q, R or S could be gold.
 
(1)
 
ii)
Suggest why the reaction between metal R and dilute hydrochloric acid was not done.
 
(1)
 
iii)
Use the information in the table to place the metals in order of reactivity from most reactive to least reactive.
 
(1)
 
reactivity-order-blank

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1b2 marks

Zinc is used to coat iron gates to prevent the iron from rusting.

 
i)
State the name of this method of preventing iron from rusting.
 
(1)
 
ii)
State another method of preventing iron from rusting.
 
(1)

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1c3 marks

A mixture of zinc powder and copper(II) oxide is heated. 

The chemical equation for the reaction that takes place is 

Zn + CuO → ZnO + Cu

 
i)
State how the reaction shows that zinc is more reactive than copper.
 
(1)
 
ii)
Explain which substance is the oxidising agent.
 
(2)

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21 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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3a2 marks

A metal is added to copper(II) sulfate solution. A displacement reaction only occurs if the metal added is more reactive than copper.

metal + copper(II) sulfate → metal sulfate + copper

Displacement reactions are exothermic. The more reactive the metal added, the greater the temperature rise. A student uses the following method in an experiment to compare the reactivities of different metals:

  • Pour some copper(II) sulfate solution into a boiling tube and record its temperature using a thermometer
  • Add some metal to the tube and stir with the thermometer
  • Record the maximum temperature of the contents of the tube.

He repeats the method using the same amount, in moles, of different metals.

To make the experiment valid, he starts with the copper(II) sulfate solution and the added metal at the same temperature.

State two other variables that must be controlled if the experiment is to be valid.

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3b6 marks

Another student uses the same method three times for each of the metals E, F, G and H. The table shows her results for these metals.

screen-shot-2022-10-10-at-13-50-45

i)
The student calculates the mean temperature increase for metals E and F. She does not include anomalous values in her calculations. Calculate the mean temperature increase for metals G and H, ignoring any anomalous values. Write your answers in the table.
(2)
ii)
Explain which metal is the most reactive.
(2)
iii)
Explain which metal is less reactive than copper.
(2)

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4a1 mark

The reactions of metals with water and with dilute sulfuric acid can be used to determine the order of reactivity of the metals.

The table shows the reactions of four metals, W, X, Y and Z, with water and with dilute sulfuric acid.

Metal Reaction with water Reaction with dilute sulfuric acid
W no reaction  no reaction
X very slow reaction reacts quickly
Y no reaction reacts slowly
Z reacts quickly reacts violently

 

What is the order of reactivity of these metals?

 
 
  most reactive     least reactive
A W X Y Z
B Z X Y W
C W Y X Z
D Z Y X W

How did you do?

4b2 marks
 i)
State which metal, W, X, Y or Z, could be copper.
 
(1)
 
ii)
State which metal, W, X, Y or Z, could be magnesium.
 
(1)

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4c2 marks

A displacement reaction can also be used to decide the order of reactivity of two metals. 

State two observations made when an excess of magnesium powder is added to an aqueous solution of copper(ll) sulfate.

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5a1 mark

The diagram shows two samples of iron, A and B.

Diagram to show coating of iron with zinc

Sample B is coated with a thin layer of zinc.

Name the process used to coat iron with zinc.

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5b3 marks

The two samples of iron are left outside for several weeks.

A brown solid containing hydrated iron(III) oxide forms on sample A.

i)
Give the common name for the brown solid.

(1)

ii)
Give the names of the two substances that react with the iron to form the brown solid.

(2)

1.......................................................................................................................

2.......................................................................................................................

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5c6 marks

Iron can be formed by reacting aluminium powder with iron(III) oxide.

The diagram shows how this reaction can be demonstrated.

2020-ja1c-q3c

When the magnesium fuse is lit, a very exothermic reaction occurs.

i)
State the meaning of the term exothermic.

(1)

ii)
The equation for the reaction between aluminium and iron(III) oxide is

2Al + Fe2O3 → 2Fe + Al2O3

Explain what this reaction shows about the relative reactivities of aluminium and iron.

(2)

iii)
Explain why the reaction between aluminium and iron(III) oxide is a redox reaction.

(3)

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6a1 mark

A student uses this method to investigate the reaction of dilute hydrochloric acid with zinc.

  • pour some dilute hydrochloric acid into a glass beaker
  • record the initial temperature of the acid
  • add a piece of zinc and stir the mixture
  • record the temperature of the mixture after one minute

Write a word equation for the reaction of dilute hydrochloric acid with zinc.

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6b
Sme Calculator3 marks

The diagram shows the thermometer readings for this reaction.

2020-ja1c-q6b

Complete the table, giving all values to the nearest 0.1 °C.

 temperature in °C after adding zinc  
 temperature in °C before adding zinc  
 temperature change in °C  

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6c5 marks

Another student repeats the method using five different metals to compare their reactivity.

i)
This student uses a polystyrene cup instead of a glass beaker.

Explain why a polystyrene cup is better than a glass beaker in this investigation.

(2)

ii)
Give three factors that the student should keep constant in this investigation.

(3)

1...............................................................................................................................
2...............................................................................................................................
3...............................................................................................................................

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6d3 marks

The table shows some of the student’s results.

Metal added Observation Temperature change in °C
 copper  no bubbling 0.0
 iron  slow bubbling  
 magnesium  rapid bubbling 8.7
 tin  very slow bubbling 1.4
 zinc  moderate bubbling 5.1

i)
State why there is no temperature change for copper.

(1)

ii)
Predict the temperature change for iron.

(1)

temperature change = ...................................................................... °C

iii)
Deduce the order of reactivity of the five metals.

(1)

most reactive ......................................................................
  ......................................................................
  ......................................................................
  ......................................................................
least reactive ......................................................................

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7a3 marks

When iron is left in damp air, rust forms on its surface.

i)
State the chemical name for rust.
(1)
ii)
Explain how a barrier method prevents rusting.
(2)

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7b
Sme Calculator3 marks

A student uses this apparatus to find the approximate percentage by volume of oxygen in air.

1cr-q4

This is the student’s method:

  • Place a graduated glass tube in a beaker of water
  • Place some damp iron wool and a rubber bung in the top of the tube
  • Record the reading of the water level in the tube
  • Leave the apparatus for a few days
  • Record the reading of the water level again

The diagram shows the readings at the start and at the end of the experiment.

1cr-q42

i)
Use the readings to complete the table, giving all values to the nearest 0.5 cm3

reading at start in cm3  20.5
reading at end in cm3  
volume of oxygen used in cm3  
(2)
ii)
The student uses these results to calculate the percentage by volume of oxygen in air.

Suggest why her calculated value is lower than the expected value.

(1)

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7c3 marks

The student repeats the experiment using the same apparatus.

These are her results for the second experiment.

volume of air in tube at start = 80.0 cm3

reading at start = 20.0 cm3

reading at end = 35.5 cm3

Use the results to calculate the percentage by volume of oxygen in air.

percentage = ............................................... %

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8a2 marks

A student investigates the rusting of iron.

She places an iron nail in a test tube of water and leaves it for several days.


Rusting nail experiment 1
i)
Predict the appearance of the iron nail after several days.

(1)

ii)
Name the main compound in rust.

(1)

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8b4 marks

The student then sets up two more test tubes containing iron nails.

Rusting nail experiment 2


Explain why the iron nail in tube 1 and the iron nail in tube 2 do not rust.

tube 1

tube 2

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91 mark

A reactivity series can be deduced by observing the reactions of metals with water and sulfuric acid. 

Four metals were added to water and sulfuric acid and the results recorded below. 

Metal Reaction with water Reaction with dilute sulfuric acid
W no reaction no reaction
X very slow reaction reacts quickly
Y no reaction reacts slowly
Z reacts quickly reacts violently

What is the order of reactivity starting with the least reactive? 

  ☐ A W, Y, X, Z
  ☐ B Y, W, X, Z
  ☐ C W, Y, Z, X
  ☐ D Z, X, Y, W

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1a
Sme Calculator3 marks

This question is about rusting.

When iron rusts, it reacts with oxygen in the air.

A student uses the rusting of iron to find the percentage of oxygen in a sample of air.

The diagram shows the apparatus.

2021-ja1c-q4a

These are the student’s results.
   volume of air in conical flask and connecting tube = 265 cm3
   volume of air in gas syringe at start = 100 cm3
   volume of air in gas syringe at end = 25 cm3

Calculate the percentage of oxygen in the sample of air using the student’s results.



percentage of oxygen = .............................................................. %

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1b4 marks
i)
Cars are painted to prevent the iron in car bodies from rusting.

Explain how painting prevents the iron in car bodies from rusting.

(2)

ii)
Some car manufacturers use paint containing tiny particles of zinc.

Explain how particles of zinc prevent iron in car bodies from rusting even when this paint is scratched.

(2)

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21 mark

A displacement reaction occurs between zinc and copper chloride.

Which half equation correctly shows the change that zinc undergoes? 

  ☐ A Zn2+(aq) + 2e-  →    Zn (s)
  ☐ B Zn (s) + 2e-  →    Zn2+ (aq)
  ☐ C Zn2+ (aq)  → Zn (s) + 2e-
  ☐ D Zn (s)  →    Zn2+ (aq) + 2e-

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3a1 mark

Zinc metal is obtained from sulfide ores. The most common ore of zinc is sphalerite, which contains zinc sulfide (ZnS) and a small amount of cadmium sulfide (CdS). The stages involved in the extraction of zinc from sphalerite are:

Stage 1: Sphalerite is strongly heated in air.

2ZnS (s) + 3O2 (g) → 2ZnO (s) + 2SO2 (g)

2CdS (s) + 3O2 (g) → 2CdO (s) + 2SO2 (g)

Stage 2: The mixture of oxides is reacted with sulfuric acid.

ZnO (s) + H2SO4 (aq) → ZnSO4 (aq) + H2O (l)

CdO (s) + H2SO4 (aq) → CdSO4 (aq) + H2O (l)

Stage 3: Zinc dust is added to the solution containing zinc sulfate and cadmium sulfate to remove the cadmium ions.

Cd2+ (aq) + Zn (s) → Cd (s) + Zn2+ (aq)

Stage 4: The solid cadmium is filtered off and the pure zinc sulfate solution is electrolysed.

State how the reaction in stage 3 shows that zinc is more reactive than cadmium.

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3b4 marks

Separate: Chemistry Only

 

i)
During the electrolysis in stage 4, zinc is deposited on the cathode.
Write an ionic half-equation for the reaction that occurs.
(1)
ii)
Complete the ionic half-equation for the reaction occurring at the anode.

.................... H2O → .....................H+ + O2 + ..................... e−
(1)
iii)
Explain how the pH of the solution surrounding the anode changes during the electrolysis.

(2)

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3c3 marks

Separate: Chemistry Only

 

Zinc is mixed with copper to make the alloy brass. Explain why brass is harder than pure copper.

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4a3 marks

Manganese is extracted from manganese oxide, MnO2 , by heating with aluminium powder. Molten manganese and a solid product are formed in this reaction.

Write a balanced symbol equation for this reaction. Include state symbols in your answer.

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4b2 marks

Use your answer to part a) to write the ionic equation for the reaction of manganese oxide with aluminium powder. You do not need to include state symbols in your answer.

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4c3 marks

In terms of electrons, explain why this reaction is classed as a redox reaction

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4d
Sme Calculator3 marks

Calculate the mass of aluminium that was required to react with manganese oxide, MnO2, to form 200 g of manganese. 

(Ar: O = 16, Mn = 55, Al = 27)

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5a3 marks

Tin can be extracted by smelting tin(IV) oxide with carbon. This reaction forms molten tin and carbon monoxide. 

Write a balanced symbol equation for this reaction. Include state symbols in your equation.

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5b2 marks

Separate: Chemistry Only

i)
In terms of electrons explain why tin ions have been reduced. 
(1)
ii)
Write the half equation for the reduction of tin ions.
(1)

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5c1 mark

Which is the correct formula of a compound that contains the tin(IV) ion?

  ☐ A SnCl2
  ☐ B Sn3(PO4)4
  ☐ C SnSO4
  ☐ D Sn(NO3)2

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5d2 marks

Zinc is a more reactive metal than tin. It can reduce tin(IV) oxide to tin when they are heated together. 

Write a ionic equation for this reaction.

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