11 mark
Astatine is found below iodine in Group 7 of the periodic table.
What is its formula and state at room temperature?
| Formula | State at room temperature | |||
| ☐ | A | At | gas | |
| ☐ | B | At | solid | |
| ☐ | C | At2 | liquid | |
| ☐ | D | At2 | solid |
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Group 7 (Edexcel GCSE Chemistry: Combined Science)
Exam Questions
2 hours17 questions
2a2 marks
A chlorine atom contains 17 electrons, 18 neutrons and 17 protons.
i)
State the mass number of this chlorine atom.
(1)
ii)
Give the electronic configuration of this chlorine atom.
(1)
2b2 marks
Describe what you would see if damp, blue litmus paper is placed into chlorine gas.
2c5 marks
Chlorine exists as diatomic molecules.
In a molecule, two chlorine atoms are joined by a covalent bond.
i)
Describe what is meant by a covalent bond.
(2)
ii)
Explain why chlorine is a gas, rather than a liquid, at room temperature.
(3)
2d1 mark
When the gas hydrogen chloride, HCl, is dissolved in water, a solution forms.
Blue litmus paper dipped in this solution turns red.
State why the litmus paper turns red.
2e2 marks
i)
Figure 13 lists the halogens in the order in which they appear in group 7 of the periodic table.
The melting points of four of the halogens are given.
| halogen | melting point in °C |
| fluorine | −220 |
| chlorine | −101 |
| bromine | −7 |
| iodine | |
| astatine | 302 |
Figure 13
Estimate the melting point of iodine.
(1)
........................ °C
ii)
Bromine reacts with heated iron.
Give the name of one halogen that would react with iron more vigorously than bromine.
Give the name of one halogen that would react with iron more vigorously than bromine.
(1)
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31 mark
A student carried out a displacement reaction using an unknown halogen and a salt containing a halide ion.
As the reaction progressed they observed the formation of a dark brown solution.
Which halogen and salt did the students react together?
| ☐ | A | Potassium iodide + bromine | |
| ☐ | B | Potassium bromide + chlorine | |
| ☐ | C | Potassium chloride + bromine | |
| ☐ | D | Potassium chloride + iodine |
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41 mark
The boiling point of the halogens increases down Group 7.
Which statement explains why?
| ☐ | A | The covalent bonds get stronger going down the group and require more energy to overcome | |
| ☐ | B | The intermolecular forces get stronger going down the group and require more energy to overcome | |
| ☐ | C | The intermolecular forces get weaker going down the group and require less energy to overcome | |
| ☐ | D | The covalent bonds get weaker going down the group and require less energy to overcome |
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5a2 marks
Complete the following sentences.
i)
The name given to group 7 in the periodic table is ............................................... .
(1)
ii)
The name given to group 0 in the periodic table is ............................................... .
(1)
5b1 mark
Which of the following rows gives the colours of the group 7 elements chlorine and bromine at room temperature?
| chlorine | bromine | |||
| ☐ | A | red-brown | purple | |
| ☐ | B | yellow-green | grey | |
| ☐ | C | yellow-green | red-brown | |
| ☐ | D | grey | red-brown |
5c1 mark
Figure 2 shows the melting and boiling points of bromine and iodine.
| element | melting point in °C | boiling point in °C |
| bromine | –7 | 59 |
| iodine | 114 | 184 |
Figure 2
Using the information in Figure 2, which row shows the physical states of these elements at 50°C?
| bromine | iodine | ||
| ☐ | A | liquid | gas |
| ☐ | B | solid | liquid |
| ☐ | C | gas | solid |
| ☐ | D | liquid | solid |
5d
1 mark
1 markThe densities of some elements in group 0 are shown in Figure 3.
| name | density in g cm–3 |
| helium | 0.15 |
| neon | 1.2 |
| argon | 1.4 |
| krypton | |
| xenon | 3.5 |
Figure 3
Use the information in Figure 3 to suggest the density of krypton.
5e2 marks
For many years, argon was used to fill filament light bulbs.
A filament light bulb is shown in Figure 4.
Figure 4
When the bulb is in use the metal filament becomes extremely hot.
Explain why argon, rather than air, was used to fill filament light bulbs.
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61 mark
Higher Only
Chlorine reacts with potassium iodide to form potassium chloride and iodine.
Cl2 (g) + 2KI (aq) → 2KCl (aq) + I2 (aq)
Which species has been reduced?
| ☐ | A | Chlorine | |
| ☐ | B | Potassium | |
| ☐ | C | Potassium iodide | |
| ☐ | D | Potassium chloride |
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7a2 marks
Fluorine, chlorine, bromine, iodine and astatine are elements in group 7.
Describe the test to show that a gas is chlorine.
7b1 mark
Bromine reacts with hydrogen to form hydrogen bromide.
Hydrogen bromide dissolves in water to form a solution.
State the name of the solution formed.
7c2 marks
There is a trend in the colour and the state of the halogens at room temperature.
Predict the colour and state of astatine at room temperature.
colour ..............................
state ..............................
7d4 marks
Bromine, chlorine and iodine are dissolved in water to make aqueous solutions.
Potassium iodide solution is added to each of these solutions.
Figure 6 shows the observations.
Potassium iodide solution is added to each of these solutions.
Figure 6 shows the observations.
| halogen | initial colour of aqueous solution | final colour of mixture |
| bromine | orange | brown |
| chlorine | pale green | brown |
| iodine | brown | brown |
Figure 6
Explain the observations shown in the table.
7e2 marks
Fluorine reacts vigorously with iron to produce iron(III) fluoride, FeF3.
Write the balanced equation for this reaction.
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81 mark
Which test is used to confirm the presence of chlorine gas during a reaction?
| ☐ | A | Collect the gas and see if it extinguishes a glowing splint | |
| ☐ | B | Collect the gas and check if it is green | |
| ☐ | C | Collect the gas and see if it bleaches damp litmus paper | |
| ☐ | D | Collect the gas and check if it smells of swimming pools |
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9a4 marks
Fluorine, chlorine, bromine and iodine are elements in group 7 of the periodic table.
i)
State the name given to the group 7 elements.
(1)
ii)
Name one other element that is in group 7.
Use the periodic table on the back of this exam paper to help you.
Use the periodic table on the back of this exam paper to help you.
(1)
iii)
Which element is liquid at room temperature and pressure?
(1)
| ☐ | A | fluorine | |
| ☐ | B | chlorine | |
| ☐ | C | bromine | |
| ☐ | D | iodine |
iv)
Which element is dark-grey in colour at room temperature and pressure?
(1)
| ☐ | A | fluorine | |
| ☐ | B | chlorine | |
| ☐ | C | bromine | |
| ☐ | D | iodine |
9b3 marks
3 marksTin reacts with chlorine to form tin chloride. A sample of tin chloride contains 1.19 g of tin and 1.42 g of chlorine.
Calculate the empirical formula of this tin chloride.
(relative atomic masses: Cl = 35.5, Sn = 119.0)
You must show your working.
9c2 marks
Tin also reacts with fluorine. The reaction between fluorine and tin is much more vigorous than the reaction between chlorine and tin.
Figure 8 shows the electronic configurations of fluorine and chlorine.
Figure 8
Explain, in terms of their electronic configurations, why fluorine reacts with tin more vigorously than chlorine reacts with tin.
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101 mark
Bromine can react with hydrogen to form hydrogen bromide.
Which statement is not true about hydrogen bromide?
| ☐ | A | It is an acidic gas | |
| ☐ | B | It does not dissolve in water | |
| ☐ | C | It contains covalent bonds | |
| ☐ | D | It is more stable than hydrogen iodide |
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11a1 mark
This question is about some of the elements in group 7 of the periodic table.
Which row in the table correctly shows the colours and physical states of the elements at room temperature?
| ☐ | A | iodine: purple gas | bromine: yellow liquid | |
| ☐ | B | chlorine: pale green gas | iodine: brown solid | |
| ☐ | C | bromine: red-brown liquid | chlorine: yellow liquid | |
| ☐ | D | iodine: dark grey solid | bromine: red-brown liquid |
11b2 marks
2 marksThe compound phosphorus oxychloride has the formula POCl3.
Calculate the percentage by mass of chlorine in phosphorus oxychloride.
(relative atomic masses: O = 16.0, P = 31.0, Cl = 35.5)
percentage by mass of chlorine = .......................................
11c3 marks
3 marksHigher Only
When iron reacts with chlorine, iron chloride is formed.
Two possible equations for this reaction are
A Fe + Cl2→ FeCl2
B 2Fe + 3Cl2→ 2FeCl3
In an experiment, 8.40 g iron reacts with chlorine to form 19.05 g iron chloride.
Show, using a calculation, which reaction, A or B, is taking place.
You must show your working.
(relative atomic masses: Cl = 35.5, Fe = 56.0)
11d6 marks
Group 1 metals react with the elements from group 7 to form salts.
Some examples of these reactions are shown in Figure 10.
Some examples of these reactions are shown in Figure 10.
| reaction | word equation |
| W | lithium + chlorine → lithium chloride |
| X | potassium + fluorine → potassium fluoride |
| Y | rubidium + iodine → rubidium iodide |
| Z | potassium + bromine → potassium bromide |
Figure 10
You will find the position of these elements in their groups on the periodic table.
Explain, in terms of their electronic configurations and the relative reactivity of these elements, which of the reactions shown in Figure 10 would be the most violent.
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121 mark
A student adds some drops of bromine water to a solution of potassium iodide.
Which statement is correct?
| ☐ | A | The solution turns brown | |
| ☐ | B | A yellow precipitate forms | |
| ☐ | C | The bromine water turns the solution orange | |
| ☐ | D | The bromine water decolourises the solution |
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1a1 mark
The elements chlorine, bromine and iodine are part of group 7 in the periodic table.
The appearances of chlorine, bromine and iodine at room temperature are shown in Figure 10.
| halogen | appearance |
| chlorine | green gas |
| bromine | red-brown liquid |
| iodine | grey solid |
Figure 10
Astatine is the element below iodine in group 7.
Predict the appearance of astatine.
1b6 marks
The order of reactivity of chlorine, bromine and iodine can be determined by carrying out displacement reactions.
Explain how displacement reactions can be used to show the reactivity of these three elements.
Explain how displacement reactions can be used to show the reactivity of these three elements.
1c6 marks
6 marksHigher Only
When iron wool is heated in bromine vapour, it reacts to form iron bromide.
i)
In an experiment, 5.60 g of iron reacted exactly with 24.0 g of bromine, Br2
[relative atomic masses: Fe = 56.0, Br = 80.0]
Determine, using this information, the balanced equation for the reaction between iron and bromine.
You must show your working.
(4)
ii)
When iron reacts with bromine, bromide ions are formed.
Explain the type of reaction bromine atoms undergo when they are converted to bromide ions.
(2)
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2a6 marks
Sodium thiosulfate solution, Na2S2O3, reacts with dilute hydrochloric acid.
Na2S2O3 (aq) + 2HCl (aq) → 2NaCl (aq) + H2O (l) + SO2 (g) + S (s)
i)
When dilute hydrochloric acid is mixed with sodium thiosulfate solution, the mixture turns cloudy.
Explain why the mixture turns cloudy.
(2)
ii)
In an investigation, different concentrations of hydrochloric acid are reacted with sodium thiosulfate solution.
The mixture goes cloudy at different rates.
Describe how the rate at which the mixture goes cloudy can be measured.
(3)
iii)
You are provided with some dilute hydrochloric acid which has a concentration of 50 g dm-3.
For this experiment, dilute hydrochloric acid with a concentration of 20 g dm-3 is required.
How much water must be added to 100 cm3 of 50 g dm-3 hydrochloric acid to make dilute hydrochloric acid with a concentration of 20 g dm-3?
(1)
| ☐ | A | 200 cm3 | |
| ☐ | B | 150 cm3 | |
| ☐ | C | 100 cm3 | |
| ☐ | D | 50 cm3 |
2b3 marks
Higher Only
Sodium iodide solution is colourless.
When a solution of bromine is added to sodium iodide solution, a reaction occurs.
2NaI + Br2 → 2NaBr + I2.
i)
The mixture turns brown.
Give the name of the substance causing the brown colour.
(1)
ii)
Explain which substance has been reduced in this reaction.
(2)
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3a2 marks
Describe what is seen when chlorine water is added to potassium bromide solution and the mixture shaken.
3b4 marks
Higher Only
Chlorine reacts with potassium bromide to form potassium chloride and bromine.
In this reaction chlorine forms chloride ions
Cl2 + 2KBr format('truetype')%3Bfont-weight%3Anormal%3Bfont-style%3Anormal%3B%7D%3C%2Fstyle%3E%3C%2Fdefs%3E%3Ctext%20font-family%3D%22math12bba9f4124283edd644799e0ce%22%20font-size%3D%2216%22%20text-anchor%3D%22middle%22%20x%3D%2210.5%22%20y%3D%2216%22%3E%26%23x2192%3B%3C%2Ftext%3E%3C%2Fsvg%3E)
2KCl + Br2
i)
In this reaction, chlorine has been reduced.
Explain, using the equation, how you know that chlorine has been reduced.
(2)
ii)
Write the half equation for the formation of bromine from bromide ions.
(2)
3c3 marks
Aluminium reacts with chlorine to form aluminium chloride.
Write the balanced equation for this reaction.
3d3 marks
A solid ionic compound is dissolved in water to form a solution.
Describe a simple experiment to show that charged particles are present in this solution.
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4a2 marks
Group 7 elements are known as the halogens.
Chlorine is a Group 7 element with an atomic number of 17.
Complete Figure 1 show the number of neutrons, protons and electrons in the two isotopes of chlorine.
| chlorine-35 | chlorine-37 | |
| number of neutrons | ||
| number of protons | ||
| number of electrons |
Figure 1
4b2 marks
A regular sample of chlorine contains only chlorine-37 and chlorine-35 atoms.
Explain why the relative atomic mass of chlorine is 35.5.
4c2 marks
Chlorine can react with non-metals to form covalent compounds
It reacts with carbon to form tetrachloromethane, CCl4.
Draw a dot and cross diagram to show the bonding in one molecule of this compound.
Show outer shell electrons only.
4d3 marks
Higher Only
Chlorine also reacts with potassium bromide in a displacement reaction.
Cl2 + 2Kl ⟶ 2KCl + l2
i)
Explain which species which has been reduced.
(1)
ii)
Write the half equation for the oxidation reaction that occurs here.
(2)
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5a1 mark
The elements in Group 7 are known as the halogens.
Name the halogen in Period 5 of the Periodic Table.
5b3 marks
Explain why chlorine is more reactive than iodine.
5c1 mark
A piece of burning sodium is placed into a gas jar containing chlorine gas.
This can be seen in Figure 1.
White crystals can be seen coating the inside of the gas jar at the end of the reaction.
Identify the white crystals.
5d5 marks
Higher Only
Bromine is also located in Group 7.
It can react with sodium.
i)
Write the balanced equation for the reaction between bromine and sodium.
(2)
ii)
A student adds sodium bromide solution to chlorine water.
State what you would see in this reaction.
(1)
iii)
The ionic equation for the reaction between sodium bromide and chlorine is:
2Br– + Cl2 → 2Cl– + Br2
Explain which species has been oxidised in this reaction.
(2)
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