1. States of matter

1.1 Solids, liquids and gases

1.2 Diffusion

2. Atoms, elements and compounds

2.1 Elements, compounds and mixtures

2.2 Atomic structure and the Periodic Table

2.3 Isotopes

2.4 Ions and ionic bonds

2.5 Simple molecules and covalent bonds

2.6 Giant covalent structures

2.7 Metallic bonding

3. Stoichiometry

3.1 Formulae

3.2 Relative masses of atoms and molecules

3.3 The mole and the Avogadro constant

4. Electrochemistry

4.1 Electrolysis

4.2 Hydrogen–oxygen fuel cells

5. Chemical energetics

5.1 Exothermic and endothermic reactions

6. Chemical reactions

6.1 Physical and chemical changes

6.2 Rate of reaction

6.3 Reversible reactions and equilibrium

6.4 Redox

7. Acids, bases and salts

7.1 The characteristic properties of acids and bases

7.2 Oxides

7.3 Preparation of salts

8. The Periodic Table

8.1 Arrangement of elements

8.2 Group I properties

8.3 Group VII properties

8.4 Transition elements

8.5 Noble gases

9. Metals

9.1 Properties of metals

9.2 Uses of metals

9.3 Alloys and their properties

9.4 Reactivity series

9.5 Corrosion of metals

9.6 Extraction of metals

10. Chemistry of the environment

10.1 Water

10.2 Fertilisers

10.3 Air quality and climate

11. Organic chemistry

11.1 Formulae, functional groups and terminology

11.2 Naming organic compounds

11.3 Fuels

11.4 Alkanes

11.5 Alkenes

11.6 Alcohols

11.7 Carboxylic acids

11.8 Polymers

12. Experimental techniques and chemical analysis

12.1 Experimental design

12.2 Acid–base titrations

12.3 Chromatography

12.4 Separation and purification

12.5 Identification of ions and gases

IGCSE Chemistry 9.4 Reactivity series Question Bank

[Maximum number: 5]

Some elements are shown in the order they appear in the reactivity series. The most reactive element is at the top.
> sodium calcium magnesium aluminium zinc iron hydrogen copper

(a)

Name the main ores of:

[ 2 ]

(i)

zinc [1]

[ 1 ]

(ii)

aluminium.

[ 1 ]

(b)

In an experiment, a sample of aluminium appeared less reactive than expected.

Explain why.

[ 1 ]

(c)

When zinc granules are added to aqueous copper(II) sulfate, a reaction occurs. During the reaction, a red-pink solid is formed and the solution becomes colourless.

[ 2 ]

(i)

Name the red-pink solid.

[ 1 ]

(ii)

Name the colourless solution.

[ 1 ]

[Maximum number: 1]

A list of oxides, A to H, is shown.

A calcium oxide
B aluminium oxide
C silicon(IV) oxide
D sulfur dioxide
E carbon dioxide
F iron(III) oxide
G silver oxide
H carbon monoxide

Answer the following questions about the oxides, A to H. Each letter may be used once, more than once or not at all.

State which of the oxides, A to H:

(a)

can be reduced by heating with copper.

[ 1 ]

[Maximum number: 2]

Rubidium, Rb, is a Group I element. It has similar physical and chemical properties to the other elements in Group I.

(a)

When rubidium is added to cold water a reaction occurs.

[ 2 ]

(i)

Suggest two observations that would be made when rubidium is added to cold water.

[ 2 ]

[Maximum number: 2]

Period 3 contains the elements sodium to argon. This question asks about the chemistry of each of the Period 3 elements or their compounds.

(a)

Magnesium reacts slowly with warm water to form a base, magnesium hydroxide.

[ 2 ]

(i)

Write a chemical equation for the reaction between magnesium and warm water.

[ 2 ]

[Maximum number: 2]

Boron and aluminium are Group III elements.

(a)

Explain the apparent unreactivity of aluminium.

[ 2 ]

(a)

When a piece of zinc metal is added to copper(II) sulfate solution there is an immediate reaction.

\mathrm{Zn}+\mathrm{CuSO}_{4} \rightarrow \mathrm{ZnSO}_{4}+\mathrm{Cu}

When a piece of aluminium metal is added to copper(II) sulfate solution the initial reaction is very slow.

[ 3 ]

(i)

Explain why zinc metal reacts with copper(II) sulfate.

[ 1 ]

(ii)

What type of reaction is this?

[ 1 ]

(iii)

Explain why the initial reaction between aluminium metal and copper(II) sulfate is very slow.

[ 1 ]

[Maximum number: 3]

Magnesium, calcium and strontium are Group II elements.

(a)

Calcium reacts with cold water to form two products:
- a colourless gas, P, which 'pops' with a lighted splint
- a weakly alkaline solution, Q, which turns milky when carbon dioxide is bubbled through it.

[ 3 ]

(i)

Name gas P.

[ 1 ]

(ii)

Write a chemical equation for the reaction of calcium with cold water.

[ 2 ]

[Maximum number: 4]

A list of five metals is shown.

A list of five metals is shown.

\title{
copper \\ iron \\ magnesium \\ potassium \\ silver
}

(a)

All metals form positive ions.

[ 1 ]

(i)

State which of the five metals in the list has the greatest tendency to form positive ions.

[ 1 ]

(b)

A student adds a sample of a metal to an aqueous metal salt in a beaker to see if a displacement reaction takes place.

Complete Table 2.1 to show the colour of the solution in the beaker at the start and at the end of the experiment.

Table 2.1

[ 3 ]

[Maximum number: 1]

The reactivity series for a number of different metals is shown.

The diagram shows different metal strips dipped into an electrolyte.

Which pair of metals produces the highest voltage?

copper and magnesium

magnesium and platinum

magnesium and zinc

silver and platinum

[Maximum number: 1]

Which metal combination produces the highest voltage reading in the cells shown?

0 selected

Question 1

Question 1(b)

Question 1(b)(i)

Question 1(b)(ii)

Question 1(c)

Question 1(e)

Question 1(e)(i)

Question 1(e)(ii)

Question 1

Question 1(f)

Question 2

Question 2(d)

Question 2(d)(i)

Question 2

Question 2(b)

Question 2(b)(ii)

Question 2

Question 2(e)

Question 2

Question 2(c)

Question 2(c)(i)

Question 2(c)(ii)

Question 2(c)(iii)

Question 2

Question 2(c)

Question 2(c)(i)

Question 2(c)(iv)

Question 2

Question 2(a)

Question 2(a)(ii)

Question 2(b)

Question 10

Question 10