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GCSE Chemistry · GCSEChapter 3 · Reactivity of metals and halogens
GCSE · Chapter 3

Reactivity of metals and halogens

By the end of this chapter you will be able to

  • Use the reactivity series to say which metal is more reactive
  • Predict whether a displacement reaction happens, and write a word equation for it
  • Describe how Group 1 metals react with water, and how the reactivity changes down the group
  • Describe the colours, states and melting points of the halogens, and their reactivity
  • Explain displacement of halide ions, and [H] explain the trends using electron shells

You should already know

  • Groups and outer electrons (Chapter 2)
  • The atomic number and electron shells (Chapters 1 and 2)

Where this leads

  • Ionic bonding of Group 1 and Group 7 ions (Chapter 4)
  • Acids, alkalis and salts (Chapter 10)
  • Electrolysis and displacement (Chapter 11)

GCSE Chemistry. Content follows the GCSE (9-1) subject content for England (Edexcel and AQA). Content references: Use the reactivity series of metals (potassium to gold) to predict displacement reactions, Describe reactions of metals with water and dilute acid, and the products, Carry out a displacement practical with metals and metal salt solutions, safely, Describe the trend in reactivity of Group 1 metals, and their reactions with water, Describe the trend in properties and reactivity of Group 7 halogens, and displacement reactions, [H] Explain the trends in reactivity using electron shells and outer electrons.

Exercise P  Do you remember?

1
FWhich group are the alkali metals in? Write the number.
2
FHow many outer electrons does a halogen have? Write the number.
3
FWhat is the chemical symbol for potassium? Write the symbol.
4
FWrite the word for the gas that is produced when some metals react with acid, and which burns with a squeaky pop. Write the word.
5
FWhat is 2 x 3 + 4? Write the number.
3.1

The reactivity series and reactions of metals

GCSE
Use the reactivity series of metals (potassium to gold) to predict reactions, Describe reactions of metals with water and dilute acid, and the products
Video lesson: The reactivity series and reactions of metalsComing soon
Context. A jeweller tells a customer that a ring will not tarnish in air. “Why is gold different from iron?” the customer asks. The answer is in the reactivity series: some metals react easily and some hardly react at all.

The reactivity series lists metals from the most reactive to the least reactive. Potassium is the most reactive in this list, and gold is the least. The more reactive a metal, the more readily it loses electrons to form positive ions. Reactive metals react faster with water and acids, and they form more stable compounds.

Metals above copper react with dilute acid to give a salt and hydrogen. Copper, silver and gold do not react with dilute acid.

Reactivity series (most reactive at the top)potassium (K)sodium (Na)lithium (Li)calcium (Ca)magnesium (Mg)aluminium (Al)zinc (Zn)iron (Fe)copper (Cu)silver (Ag)gold (Au)moreless
The reactivity series, most reactive at the top
MetalCold waterDilute acid
potassium, sodium, lithiumvigorous reaction; hydrogen forms (teacher demonstration only)very vigorous (not for pupils)
calciumsteady reaction, hydrogen formsvigorous
magnesiumvery slowvigorous
aluminium, zinc, ironalmost no reactionreacts, hydrogen forms
copper, silver, goldno reactionno reaction
Reactions of metals with water and dilute acid (general pattern)

Key ideas

  • The reactivity series ranks metals from most reactive (potassium) to least reactive (gold).
  • A metal above copper in the series (and so above hydrogen) reacts with dilute acid to give a salt and hydrogen.
  • Copper, silver and gold do not react with dilute acid.
  • Potassium, sodium and lithium react with cold water; calcium reacts steadily; magnesium reacts very slowly with cold water.
Worked example 3.1.1
Which is more reactive: zinc or copper? Write the name.

Method. Find both metals in the reactivity series.

  1. Find. Zinc is above copper in the reactivity series.
    zinc above copper
  2. Decide. So zinc is more reactive.
    zinc
  3. Write the answer.
    zinc

Check. Zinc reacts with dilute acid, and copper does not. ✓

Worked example 3.1.2
Magnesium is placed in dilute hydrochloric acid. What gas is produced? Write the word.

Method. Recall what metals above copper produce with acid.

  1. Recall. Magnesium is above copper, so it reacts with dilute acid.
    reacts
  2. Product. Metals with dilute acid give a salt and hydrogen.
    hydrogen
  3. Write the answer.
    hydrogen

Check. Magnesium chloride is the salt. Hydrogen is the gas. ✓

Worked example 3.1.3
Which metal in the series reacts steadily with cold water? Write the name.

Method. Use the results table.

  1. Look. Calcium reacts steadily with cold water, and magnesium only very slowly.
    calcium steady
  2. Name. So calcium is the metal.
    calcium
  3. Write the answer.
    calcium

Check. Potassium and sodium react more vigorously. ✓

Watch out

Watch out: the reactivity series is about reactivity, not about the price or the density of a metal. Use the order only to predict reactions.

Exam tip

Exam tip. When you compare two metals, say which is higher in the reactivity series, not which is “stronger”.

Exercise 3A  The reactivity series and reactions of metals

1
FWhich metal is the most reactive in the series? Write the name.
2
FWhich metal is the least reactive in the list? Write the name.
3
FWhich metal is between zinc and copper in the reactivity series? Write the name.
4
FIs magnesium more or less reactive than zinc? Write the word.
5
FWrite the chemical symbol for sodium. Write the symbol.
6
FWhich metal in the list reacts steadily with cold water? Write the name.
7
FWhich metal does not react with dilute acid? Write the name.
8
FWhat gas is produced when zinc reacts with dilute hydrochloric acid? Write the word.
9
FWrite the name of the salt formed when magnesium reacts with dilute hydrochloric acid. Write the name.
10
PSPut these in order, from most reactive to least reactive: copper, magnesium, zinc. Write the three names.
11
RExplain why gold is used for jewellery, in one sentence. Accept any sentence that says gold is unreactive, so it does not corrode or tarnish.
12
RA pupil says, “Gold must react with dilute acid because gold is a metal.” Explain why this is wrong, in one sentence. Accept any sentence that says gold is below hydrogen in the series, so it does not react with dilute acid.
13
PSPredict which metal reacts more vigorously with dilute acid: calcium or copper. Write the name.
3.2

Displacement reactions: required practical

GCSE
Carry out a displacement practical with metals and metal salt solutions, safely, Predict whether a displacement reaction happens, and write a word equation
Video lesson: Displacement reactions: required practicalComing soon
Context. A class places pieces of four metals in copper sulfate solution and watches for changes. “Which metal will take the place of copper?” asks a pupil. The results show which metals are more reactive than copper, and the reactivity series explains the rest.

A displacement reaction happens when a more reactive metal takes the place of a less reactive metal in a compound. In the practical, pupils place a clean piece of a metal into a dilute copper sulfate solution. A reaction shows as a brown solid of copper forming, and the blue colour of the solution fading. Magnesium, zinc and iron displace copper; copper does not displace magnesium.

Displacement: magnesium in copper sulfate solutioncopper sulfateMgreactsmagnesium sulfatecopper solidMg + CuSO4 -> MgSO4 + Cu (the blue colour fades; brown copper forms)
Magnesium and copper sulfate solution (a displacement reaction)
MixtureObservationConclusion
Mg + CuSO4Copper forms; the blue colour fadesmagnesium is more reactive than copper
Zn + CuSO4Copper forms; the blue colour fadeszinc is more reactive than copper
Fe + CuSO4Copper forms slowlyiron is more reactive than copper
Cu + MgSO4No reactioncopper is less reactive than magnesium
Results of the displacement practical (typical)

Try it (with your teacher). Required practical: displacement of metals in copper sulfate solution. Use a fixed volume of dilute copper sulfate in each tube, and the same size of each metal piece. Wear goggles and gloves, keep copper sulfate off your skin, and wash your hands at the end. Copper sulfate is harmful if swallowed. Put the solids in the waste container that your teacher gives you. Record the colour change and the solid formed.

Key ideas

  • A more reactive metal displaces a less reactive metal from its compound.
  • Copper forms as a brown solid; the blue colour of copper sulfate fades when zinc or magnesium is used.
  • Fair test: keep the volume, the concentration and the size of the metal pieces the same.
  • Word equation: magnesium + copper sulfate -> magnesium sulfate + copper.
Worked example 3.2.1
Zinc is placed in copper sulfate solution. Will a reaction happen? Write yes or no.

Method. Compare zinc and copper in the series.

  1. Compare. Zinc is above copper in the reactivity series.
    zinc above copper
  2. Decide. So zinc displaces copper, and a reaction happens.
    yes
  3. Write the answer.
    yes

Check. The copper forms as a brown solid. ✓

Worked example 3.2.2
Write the word equation for magnesium reacting with copper sulfate solution. Write the products.

Method. Magnesium takes the place of copper in the compound.

  1. Reactants. Magnesium and copper sulfate.
    magnesium + copper sulfate
  2. Products. Magnesium takes the sulfate, so the products are magnesium sulfate and copper.
    magnesium sulfate + copper
  3. Write the answer.
    magnesium sulfate and copper

Check. Copper is the solid that forms. ✓

Worked example 3.2.3
Copper is placed in magnesium sulfate solution. What do you observe? Write the words.

Method. Compare copper and magnesium in the series.

  1. Compare. Copper is below magnesium, so it is less reactive.
    copper below magnesium
  2. Observe. Copper cannot displace magnesium, so no reaction is seen.
    no reaction
  3. Write the answer.
    no reaction

Check. The solution stays the same colour. ✓

Watch out

Watch out: the displaced metal is the less reactive one. In magnesium + copper sulfate, copper is displaced, so copper is the product that forms as a solid.

Exam tip

Exam tip. For a displacement practical, write the three things you control (volume, concentration, size of metal), and the one thing you measure or observe (the colour change).

Exercise 3B  Displacement reactions

1
FWhat colour is copper sulfate solution? Write the colour.
2
FWhat is displaced when magnesium reacts with copper sulfate solution? Write the word.
3
FWhat is the colour of the solid that forms when zinc displaces copper? Write the colour.
4
FAfter zinc reacts with copper sulfate solution, what colour is the solution? Write the colour.
5
FName the product, other than copper, when magnesium reacts with copper sulfate solution. Write the name.
6
FDoes copper react with magnesium sulfate solution? Write yes or no.
7
FWhich piece of safety equipment must be worn in the copper sulfate practical? Write the name.
8
FIn the fair test, which variable must be kept the same? Write the word. Accept volume, concentration or size of the metal.
9
PSPredict whether zinc will displace magnesium from magnesium sulfate solution. Write yes or no.
10
PSPredict whether magnesium will displace zinc from zinc sulfate solution. Write yes or no.
11
PSWrite the word equation for magnesium reacting with zinc sulfate solution. Write the products.
12
RA pupil says, “Iron must displace magnesium because iron is a metal.” Explain why this is wrong, in one sentence. Accept any sentence that says iron is less reactive than magnesium, so it cannot displace magnesium.
13
RExplain why the practical should use the same volume of solution in each tube. Accept any sentence that says it keeps the test fair.
3.3

Group 1: the alkali metals

GCSE
Describe the trend in reactivity of Group 1 metals, and their reactions with water
Video lesson: Group 1: the alkali metalsComing soon
Context. A teacher drops a small piece of lithium into a dish of water and it fizzes gently. A piece of potassium, dropped in the same way, reacts much more violently. “Why do they behave differently?” asks a pupil. Both metals are in group 1, so the pattern should be the same. The difference is in the size of the atoms.

The alkali metals are the group 1 elements: lithium, sodium and potassium. Each has one outer electron. When an alkali metal reacts with water, it forms a metal hydroxide and hydrogen. The hydroxide dissolves, making the solution alkaline. Going down group 1, the reactions become more vigorous, so reactivity increases down the group.

Alkali metalSymbolAtomic numberReaction with water (teacher demonstration)
LithiumLi3fizzes steadily
SodiumNa11melts and moves about, faster
PotassiumK19very vigorous; hydrogen may ignite
Group 1 metals: reactions with water (teacher demonstration only)

Key ideas

  • Alkali metals have one outer electron.
  • Reactivity increases down group 1: potassium is more reactive than sodium, which is more reactive than lithium.
  • The word equation: metal + water -> metal hydroxide + hydrogen.
  • Alkali metal reactions with water are done by a teacher only. They are vigorous and can be dangerous.
Worked example 3.3.1
Write the word equation for sodium reacting with water. Write the products.

Method. Use the general pattern for group 1 with water.

  1. Reactants. Sodium and water.
    sodium + water
  2. Products. Sodium forms sodium hydroxide, and hydrogen is released.
    sodium hydroxide + hydrogen
  3. Write the answer.
    sodium hydroxide and hydrogen

Check. Sodium hydroxide is a strong alkali. ✓

Worked example 3.3.2
Which is more reactive: lithium or potassium? Write the name.

Method. Reactivity increases down group 1.

  1. Position. Potassium is below lithium in group 1.
    below
  2. Decide. So potassium is more reactive.
    potassium
  3. Write the answer.
    potassium

Check. Potassium reacts more vigorously with water. ✓

Worked example 3.3.3
Name the product, other than hydrogen, when lithium reacts with water. Write the name.

Method. Name the metal hydroxide.

  1. Metal. The metal is lithium.
    lithium
  2. Hydroxide. Lithium with water forms lithium hydroxide.
    lithium hydroxide
  3. Write the answer.
    lithium hydroxide

Check. The solution is alkaline. ✓

Watch out

Watch out: a group 1 metal reacts with water to make a hydroxide (for example sodium hydroxide), not an acid. The solution made is alkaline.

Exam tip

Exam tip. When you describe a trend, say the direction: reactivity increases down group 1. Do not write “gets bigger” without saying what changes.

Exercise 3C  Group 1: the alkali metals

1
FWhich group are the alkali metals in? Write the number.
2
FHow many outer electrons does a group 1 atom have? Write the number.
3
FWhat is the symbol for lithium? Write the symbol.
4
FWhat is the name of the group 1 metal with atomic number 11? Write the name.
5
FWhat is formed, with hydrogen, when a group 1 metal reacts with water? Write the word.
6
FIs potassium more or less reactive than sodium? Write the word.
7
FWrite the word equation for lithium reacting with water. Write the products.
8
FWhich metal in group 1 reacts most vigorously with water: lithium, sodium or potassium? Write the name.
9
FWhy are the alkali metals kept away from water in the lab? Write one reason. Accept any reason that says they react vigorously with water.
10
PSPredict how rubidium, which is below potassium in group 1, will react with water. Write the word. Accept more vigorous, or more reactive.
11
PSExplain why the reactions of group 1 metals become more vigorous down the group, in one sentence. Accept any sentence that says the outer electron is further from the nucleus, so it is lost more easily.
12
RExplain why a teacher should carry out the group 1 reaction with water, not a pupil. Write one reason. Accept any reason that says the reaction is vigorous and can be dangerous.
13
RIs it true that all group 1 metals react with water in the same way? Write yes or no, then give a reason in one sentence.
3.4

Group 7: the halogens

GCSE
Describe the trend in properties and reactivity of Group 7 halogens, and displacement reactions
Video lesson: Group 7: the halogensComing soon
Context. At a school open day, a technician shows visitors four bottles of halogens. “Why is one a gas, one a liquid and one a solid?” asks a visitor. The answer is in the melting points: they increase as you go down group 7.

The halogens are group 7: fluorine, chlorine, bromine and iodine. Going down the group, their melting points increase, so they change from gases, to liquids, to solids. Their reactivity decreases down the group. A more reactive halogen displaces a less reactive halide ion from solution.

HalogenSymbolColour and state at room temperatureMelting point (degrees C)
FluorineFpale yellow gas-220
ChlorineClgreen gas-101
BromineBrred-brown liquid-7
IodineIgrey-black solid114
Astatine (predicted)Atdark solid (predicted)higher than iodine (predicted)
Group 7 halogens: colour, state and melting point

Key ideas

  • Halogens are diatomic molecules: Cl2, Br2, I2.
  • Melting points increase down group 7; fluorine is a pale yellow gas, iodine is a grey-black solid.
  • Reactivity decreases down group 7: fluorine is the most reactive.
  • Displacement: chlorine displaces bromide and iodide ions; bromine displaces iodide ions.

Try it (with your teacher). Teacher demonstration only: a teacher may add a little chlorine water to potassium bromide solution. Chlorine is toxic, so pupils watch from a safe distance in a fume cupboard. The solution turns orange-brown because bromine is displaced.

Worked example 3.4.1
Which halogen is a pale yellow gas at room temperature? Write the name.

Method. Use the table.

  1. Look. Fluorine is a pale yellow gas at room temperature.
    pale yellow gas
  2. Name. So the halogen is fluorine.
    fluorine
  3. Write the answer.
    fluorine

Check. Fluorine has the lowest melting point of the group. ✓

Worked example 3.4.2
Chlorine is added to potassium bromide solution. Write the name of the element that forms. Write the name.

Method. A more reactive halogen displaces a less reactive one.

  1. Compare. Chlorine is above bromine in group 7, so it is more reactive.
    more reactive
  2. Displace. Chlorine displaces bromine from potassium bromide.
    bromine forms
  3. Write the answer.
    bromine

Check. Potassium chloride is the other product. ✓

Worked example 3.4.3
Name the halogen that is a grey-black solid at room temperature. Write the name.

Method. Use the melting point and state.

  1. Look. Iodine has the highest melting point of the four.
    highest melting point
  2. Name. It is a grey-black solid at room temperature.
    iodine
  3. Write the answer.
    iodine

Check. Iodine melts at 114 degrees C. ✓

Watch out

Watch out: a more reactive halogen displaces a less reactive halide ion, not a metal. Iodide is displaced by bromine, and bromide is displaced by chlorine.

Exam tip

Exam tip. For halogen displacement, say which halogen is more reactive (the one higher up group 7) and what forms.

Exercise 3D  Group 7: the halogens

1
FWhich group are the halogens in? Write the number.
2
FWhat colour is chlorine gas? Write the colour.
3
FWhat state is bromine at room temperature? Write the word.
4
FWhat state is iodine at room temperature? Write the word.
5
FWhich halogen has the highest melting point? Write the name.
6
FWhich halogen is the most reactive? Write the name.
7
FWhich halogen displaces bromide ions from solution? Write the name.
8
FIn the reaction of chlorine with potassium bromide solution, which product is red-brown? Write the name.
9
FIs bromine more reactive or less reactive than iodine? Write the word.
10
PSPredict whether iodine will displace chloride ions from potassium chloride solution. Write yes or no.
11
PSPredict whether bromine will displace iodide ions from potassium iodide solution. Write yes or no.
12
PSWrite the word equation for chlorine displacing bromine from potassium bromide. Write the products.
13
RExplain why the displacement of halogens is a teacher demonstration only, in one sentence. Accept any sentence that says chlorine is toxic, so pupils must not handle it.
3.5

Explaining the trends and predicting [H]

GCSE
[H] Explain the trends in reactivity using electron shells and outer electrons, Predict the properties of an element from its position in its group
Video lesson: Explaining the trends and predicting [H]Coming soon
Context. A student says, “Potassium has one electron on its outside, just like sodium. Why is it more reactive?” The answer is in the number of shells: the outer electron of potassium is further from the nucleus, and it is held more weakly.

Each step down group 1 adds a shell. The outer electron is further from the nucleus, and the inner shells shield it from the attraction of the nucleus, so it is lost more easily. In group 7, each step down adds a shell, so the nucleus is further from the outer shell. An extra electron is attracted less strongly, so the halogens become less reactive down the group.

Group 1: more shells, the outer electron is further awayLi: 2 shellsouter electron in shell 2Na: 3 shellsouter electron in shell 3K: 4 shellsouter electron in shell 4
Electron shells of lithium, sodium and potassium (not to scale)

[H] Higher tier only. Explanation for the trends. In group 1, the outer electron is lost when the atom reacts; a larger atom with more shells loses its outer electron more easily, so reactivity increases down the group. In group 7, the outer shell needs one electron to be full; a larger atom attracts that electron less strongly, so reactivity decreases down the group.

Key ideas

  • Group 1: more shells, the outer electron is further from the nucleus and is lost more easily.
  • Group 7: more shells, the nucleus attracts an extra electron less strongly, so reactivity decreases.
  • The trends are in opposite directions for groups 1 and 7.
  • Predictions use the trend; check them with evidence.
Worked example 3.5.1
Which has more shells: lithium or potassium? Write the name.

Method. Count the shells of each atom.

  1. Lithium. Lithium is 2,1, which has 2 shells.
    2 shells
  2. Potassium. Potassium is 2,8,8,1, which has 4 shells.
    4 shells
  3. Decide. Potassium has more shells.
    potassium
  4. Write the answer.
    potassium

Check. Potassium is in period 4. ✓

Worked example 3.5.2
Explain, using shells, why astatine is predicted to be less reactive than iodine. Write one sentence.

Method. Compare the number of shells.

  1. Shells. Astatine is below iodine, so it has one more shell.
    more shells
  2. Conclude. A larger atom attracts an extra electron less strongly, so it is less reactive.
    less reactive
  3. Write the answer.
    Astatine has more shells, so the nucleus attracts an extra electron less strongly.

Check. Reactivity decreases down group 7. ✓

Worked example 3.5.3
In group 7, which is more reactive: chlorine or iodine? Write the name.

Method. Use the trend in group 7.

  1. Position. Chlorine is above iodine.
    above
  2. Decide. Reactivity decreases down the group, so chlorine is more reactive.
    chlorine
  3. Write the answer.
    chlorine

Check. Chlorine is the stronger attractor of an extra electron. ✓

Watch out

Watch out: the trends run in opposite directions. In group 1, reactivity increases down the group; in group 7, it decreases. Do not use the same reason for both.

Exam tip

Exam tip. Link the trend to shells and the outer electron in one sentence: more shells, the outer electron is further away, so it is lost or attracted differently.

Exercise 3E  Explaining the trends and predicting

1
FHow many shells does a lithium atom have? Write the number.
2
FHow many shells does a potassium atom have? Write the number.
3
FWhich atom has the outer electron further from the nucleus: sodium or potassium? Write the name.
4
FWhich metal in group 1 loses its outer electron most easily: lithium, sodium or potassium? Write the name.
5
R[H] Explain, using shells, why potassium is more reactive than sodium. Write one sentence. Accept any sentence that says the outer electron is further from the nucleus and is more shielded, so it is lost more easily.
6
R[H] Explain why chlorine gains one electron when it reacts. Write one sentence. Accept any sentence that says it has 7 outer electrons and gains one to fill its outer shell.
7
R[H] Explain why iodine is less reactive than chlorine. Write one sentence. Accept any sentence that says iodine has more shells, so the nucleus attracts an extra electron less strongly.
8
PSPredict whether astatine is more reactive or less reactive than iodine. Write the word.
9
PSPredict the state of astatine at room temperature. Write the word.
10
PSWhich is more reactive: sodium or caesium? Write the name.
11
R[H] Explain why the trends in reactivity are in opposite directions for group 1 and group 7, in one or two sentences. Accept any answer that says group 1 loses an outer electron more easily further down, while group 7 gains one less easily.

Chapter summary

SkillMethod
Reactivity seriesPotassium (most reactive) to gold (least reactive); metals above copper react with dilute acid.
DisplacementA more reactive metal displaces a less reactive metal from its compound (copper sulfate practical).
Group 1 with waterMetal + water -> metal hydroxide + hydrogen; reactivity increases down the group.
Group 7 propertiesMelting points increase down the group; fluorine is a pale yellow gas; iodine is a grey-black solid.
Halogen displacementA more reactive halogen displaces a less reactive halide ion (teacher demonstration).
[H] ExplanationShells and outer electrons decide reactivity; the trends run in opposite directions in groups 1 and 7.

Can you…?

  • I can use the reactivity series to predict whether a displacement happens
  • I can carry out the copper sulfate displacement practical safely and record results
  • I can describe the reactions of Group 1 metals with water, and the trend down the group
  • I can describe the colours, states and melting points of the halogens
  • I can write word equations for displacement reactions
  • [H] I can explain the trends using electron shells and outer electrons

Key terms

reactivity series
the list of metals from most reactive to least reactive
displacement
a reaction where a more reactive element takes the place of a less reactive one in a compound
alkali metal
a Group 1 metal, such as lithium, sodium or potassium
hydroxide
a compound containing OH- ions, such as sodium hydroxide
halogen
a Group 7 element, such as chlorine or iodine
halide ion
an ion of a halogen, such as chloride (Cl-) or bromide (Br-)
shielding
[H] the effect of inner electrons reducing the attraction of the nucleus for outer electrons

Exercise 3Z  Check-up

1
Which metal is between zinc and copper in the reactivity series? Write the name.
2
What is the product, other than copper, when magnesium reacts with copper sulfate solution? Write the name.
3
Which is more reactive: magnesium or copper? Write the name.
4
Which group 1 metal reacts most vigorously with water: lithium or potassium? Write the name.
5
Write the word equation for sodium reacting with water. Write the products.
6
What colour is chlorine gas? Write the colour.
7
Which halogen is a liquid at room temperature? Write the name.
8
Will zinc displace magnesium from magnesium sulfate solution? Write yes or no.
9
Write the word equation for chlorine reacting with potassium bromide solution. Write the products.
10
[H] Explain, using shells, why reactivity decreases down group 7. Write one sentence. Accept any sentence that says more shells mean the nucleus attracts an extra electron less strongly.

Total 24 marks. Allow about 24 minutes.

Exercise 3X  Exam-style questions

1
FPlace these metals in order, most reactive first: calcium, copper, zinc. Write the three names.[2 marks]
2
FA pupil places zinc in copper sulfate solution. Describe two observations. Accept any two of: copper forms, a brown solid, the blue colour fades.[2 marks]
3
FName the gas produced when magnesium reacts with dilute hydrochloric acid. Write the name.[1 mark]
4
FDescribe the trend in reactivity of the group 1 metals down the group. Write one sentence. Accept any sentence that says reactivity increases down the group.[2 marks]
5
FWrite the word equation for sodium reacting with water. Write the products.[2 marks]
6
FDescribe the colour and state of bromine at room temperature. Write two words.[2 marks]
7
PSPredict whether iodine will displace bromide ions from potassium bromide solution. Write yes or no, then give a reason in one sentence.[3 marks]
8
RExplain why a teacher should carry out the reaction of chlorine with potassium bromide solution, not a pupil. Write one sentence. Accept any sentence that says chlorine is toxic.[3 marks]
9
RName the metal that does not react with dilute hydrochloric acid, and say why in one sentence. Accept copper, silver or gold, with a reason that they are below hydrogen in the reactivity series.[3 marks]
10
R[H] Explain, using shells, why fluorine is more reactive than chlorine. Write one or two sentences. Accept any answer that says fluorine has fewer shells, so the nucleus attracts an extra electron more strongly.[4 marks]
← Chapter 2: Electron arrangement and the periodic tableChapter 4: Ionic bonding and ionic compounds →

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