Collins IGCSE Chemistry WB sample by Collins

Cambridge IGCSE™

GE S

Chemistry SA M

WORKBOOK

Chris Sunley

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Contents

Contents Section 1: States of matter

Solids, liquids and gases

Diffusion 7 Section 2: Atoms, elements and compounds

Elements, compounds and mixtures

Atomic structure and the Periodic Table

Isotopes 13 15

Simple molecules and covalent bonds

Giant covalent structures S Metallic bonding

GE S

Ions and ionic bonds

Section 3: Stoichiometry

23 25

Formulae 25

Section 4: Electrochemistry

The mole and the Avogadro constant

Relative masses of atoms and molecules

28 30 36

SA M

Electrolysis 36 Hydrogen–oxygen fuel cells

Section 5: Chemical energetics

Exothermic and endothermic reactions

Section 6: Chemical reactions

Physical and chemical changes; Rates of reaction

Reversible reactions and equilibrium

Redox 55 Section 7: Acids, bases and salts

The characteristic properties of acids and bases

Oxides 62 Preparation of salts

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Contents

Arrangement of elements

Group I properties

Group VII properties

Transition elements; Noble gases

Section 9: Metals

Properties of metals

Uses of metals; Alloys and their properties

Reactivity series

Corrosion of metals

Extraction of metals

Section 10: Chemistry of the environment

GE S

Section 8: The Periodic Table

Water; Fertilisers Air quality and climate

Section 11: Organic chemistry

88 90 93

Fuels 93

Alkanes 95

Alkenes 99 Carboxylic acids

SA M

Alcohols 102 104

Polymers 107 Section 12: Experimental techniques and chemical analysis

110

Experimental design

110

Acid–base titrations

112

Chromatography 115 Separation and purification

118

Identification of ions and gases

120

The Periodic Table of Elements

124

Answers for all the questions in this Workbook are available from http://www.collins.co.uk/internationalresources.

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Section 2: Atoms, elements and compounds | Atomic structure and the Periodic Table

Atomic structure and the Periodic Table Student’s Book pages 25–27 and 30–33 | Syllabus learning objectives 2.2.1–2.2.6

State whether the following statements are True or False. Statement

True or False

GE S

Protons are found in the nucleus In an atom, the numbers of protons and neutrons are always the same

Electrons are arranged in shells around the nucleus

A proton has a relative charge of +1

An electron has a relative mass of 1

The nucleon number gives the number of protons and neutrons in the nucleus

SA M

An element with an atomic number of 11 has three electron shells [7 ] TIP When answering questions about atomic structure, make sure to have a copy of the Periodic Table to hand (included on page 124 of this Workbook).

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Section 2: Atoms, elements and compounds | Atomic structure and the Periodic Table

Complete the following table.

Atom

Atomic number

Nucleon number

Number of neutrons

Number of electrons

Electron arrangement

7 Li 3

199F 28 Si 14

31 P 15 39 K 19

[5 ]

GE S

Look at the Periodic Table on page 124 and then answer questions a–e.

Which Group is nitrogen in?

Which Group is calcium in?

SA M

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[1 ]

Oxygen is in Group VI. How many electrons does it have in its outer electron shell?

[1 ]

Sodium is in the third Period. How many electron shells does it have?

What do the final electron shells of all the noble gases have in common?

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Section 2: Atoms, elements and compounds | Isotopes

The drawing below shows an atom diagram.

16p 16n

Taking information from the Periodic Table, on page 124 draw atom diagrams of the following elements: Aluminium

[2 ]

Magnesium

[2 ]

Neon

[2 ]

Isotopes

GE S

SA M

Student’s Book pages 27–30 | Syllabus learning objectives 2.3.1–2.3.2; SUPPLEMENT 2.3.3–2.3.4

TIP You need to be familiar with these terms: proton number/ atomic number and mass number/nucleon number.

Look at the atomic structures of these two atoms: 63 Cu Cu and 65 29 29

How do you know these atoms are isotopes?

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[1 ]

State one feature of the atoms that these isotopes have in common.

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Section 2: Atoms, elements and compounds | Isotopes

Chlorine has two common isotopes: 35 Cl and 37 Cl. 17 17

SUPPLEMENT

Explain why these isotopes of chlorine have the same chemical properties. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . ................................................................................................................................................

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[2 ]

Use the data in the following table to calculate the relative atomic mass of magnesium. Give your answer to 3 significant figures. SUPPLEMENT Relative abundance (%)

GE S

Nucleon number

10 11

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SA M

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Section 2: Atoms, elements and compounds | Ions and ionic bonds

Ions and ionic bonds Student’s Book pages 38–44 | Syllabus learning objectives 2.4.1–2.4.4; SUPPLEMENT 2.4.5–2.4.7

Chlorine forms the chloride ion Cl−.

Has the chlorine atom lost or gained an electron?

Why is only one electron lost or gained?

[1 ]

[2 ]

GE S

Is the chloride ion an anion or a cation?

SA M

Sodium chloride is a solid at room temperature.

What holds the solid structure together?

Why does solid sodium chloride not conduct an electric current?

Would you expect sodium chloride to have a high or low melting point? Explain your answer.

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Section 2: Atoms, elements and compounds | Ions and ionic bonds

Use the atomic numbers in the Periodic Table on page 124 to help you complete the table below.

Element

Electron arrangement of the atom

Electron arrangement of the ion

Charge on the ion

Sodium Fluorine Potassium [9 ]

Draw dot-and-cross diagrams to show the formation of the ionic bonds between the following elements. In each case, write the formulae of the ions formed.

GE S

TIP

Potassium fluoride

SA M

You will need to use the atomic numbers of the elements as shown in the Periodic Table on page 124.

[2 ] b

Lithium chloride

[2 ]

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Section 2: Atoms, elements and compounds | Ions and ionic bonds

The following diagram represents the structure of lithium chloride.

SUPPLEMENT

chloride ion a

lithium ion

What does the diagram show about the structure of lithium chloride?

GE S

[3 ]

[2 ]

Explain why lithium chloride conducts electricity when molten or in solution.

SA M

Explain why lithium chloride has a high melting point.

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Section 2: Atoms, elements and compounds | Ions and ionic bonds

Draw dot-and-cross diagrams to show the ionic bonding in the following compounds. In each case, write the formulae of the ions formed. SUPPLEMENT TIP Use the same approach as in Chapter 2 of the Student’s Book.

Calcium oxide (proton numbers Ca = 20; O = 8)

GE S

[2 ]

Aluminium chloride (proton numbers Al = 13; Cl = 17)

SA M

[2 ]

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Section 2: Atoms, elements and compounds | Simple molecules and covalent bonds

Simple molecules and covalent bonds Student’s Book pages 47–52 | Syllabus learning objectives 2.5.1–2.5.3; SUPPLEMENT 2.5.4–2.5.5

TIP

Use a dot-and-cross diagram to show how the covalent bond is formed in fluorine, F2. The proton number of fluorine is 9.

SA M

GE S

For dot-and-cross diagrams, use the same approach as in Chapter 2 of the Student’s Book.

[2 ] 2 a

Use a dot-and-cross diagram to show the covalent bonds in phosphine, PH3. The proton number of hydrogen is 1 and the proton number of phosphorus is 15.

[2 ]

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Section 2: Atoms, elements and compounds | Simple molecules and covalent bonds

Will phosphine conduct electricity? Give a reason for your answer.

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[2 ]

Would you expect phosphine to have a low or high boiling point? Give a reason for your answer.

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GE S

3 SUPPLEMENT

Draw a dot-and-cross diagram to show the electron configuration of propene, C3H6. The proton number of hydrogen is 1 and the proton number of carbon is 6.

SA M

[3 ] b

Explain, in terms of structure and bonding, the reasons for this simple molecule having a low melting point and poor electrical conductivity.

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[2 ]

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Section 2: Atoms, elements and compounds | Giant covalent structures

Giant covalent structures Student’s Book pages 52–55 | Syllabus learning objectives 2.6.1– 2.6.2; SUPPLEMENT 2.6.3–2.6.4

Use the diagram showing the structure of graphite to answer the questions below.

GE S

Structure of graphite

What do the complete lines in each layer represent?

SA M

[1 ]

[2 ]

Explain why graphite can be used as a lubricant.

[1 ]

What do the broken lines between the layers represent?

What property of diamond makes it useful as a cutting tool?

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Section 2: Atoms, elements and compounds | Giant covalent structures

Use the diagram showing the structure of silicon(IV) oxide to answer the questions below.

SUPPLEMENT

Si O Si O

Si O

O O Si O Si

O O

O Si

Si O

O O

Would you expect silicon(IV) oxide to have a low or high melting point? Explain your answer.

GE S

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[3 ]

SA M

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Would you expect silicon(IV) oxide to act as an electrode in the same way that graphite does? Explain your answer.

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Section 2: Atoms, elements and compounds | Metallic bonding

SUPPLEMENT

Metallic bonding Student’s Book pages 58–60 | Syllabus learning objectives SUPPLEMENT 2.7.1–2.7.2

The diagram below represents the structure of a metal.

GE S

SUPPLEMENT

TIP

What are represented by the circles with + signs inside?

SA M

Check you know the meaning of ‘delocalised’ – refer to Chapter 2 in the Student’s Book.

[1 ]

[2 ]

What are represented by the − signs?

Use the diagram to explain why metals have good electrical conductivity.

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Section 2: Atoms, elements and compounds | Metallic bonding

This question is about the properties of metals.

SUPPLEMENT a

Metals are ductile. Explain what this means.

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[1 ]

[2 ]

Metals are malleable. Explain what this means.

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Look at the information in the following table.

SUPPLEMENT

3550

660

801

GE S

Electrical conductivity

When solid

When molten

Poor

Good

Poor

Good

Melting point (°C)

Which of the substances is a metal?

SA M

Substance

Explain the reasons for your choice.

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