Group 0: The Noble Gases
Get to grips with Group 0: The Noble Gases for GCSE Chemistry with this free worksheet and full mark scheme — Foundation and Higher exam-style questions with worked answers for AQA, Edexcel and OCR. The noble gases are unreactive because they have full outer shells, and their boiling points increase down the group.
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These worksheets and mark schemes are original, written for Virtus Academy and checked against the current AQA, Edexcel and OCR specifications. Every worksheet comes with a full mark scheme.
Topic overview
The noble gases in group 0 are unreactive and exist as single atoms rather than molecules. Their lack of reactivity is the defining feature and the key to every question on them.
They are unreactive because they have a full outer shell of electrons. Helium has 2 electrons, filling its only shell, and the others have 8 in their outer shell. Because the arrangement is already stable, they have no tendency to lose, gain or share electrons.
Boiling points increase going down the group, because the atoms get larger, the intermolecular forces between them become stronger, and more energy is needed to overcome those forces.
Revision notes
Why they are unreactive
Noble gases have a full outer shell of electrons — 2 for helium and 8 for the rest.
This is a stable arrangement, so they have no tendency to lose, gain or share electrons, and therefore do not react. They exist as single atoms, not molecules.
Trends down the group
The boiling points increase going down the group.
This is because the atoms become larger, so the intermolecular forces between them are stronger and more energy is needed to overcome them.
Uses
Helium is used in balloons and airships because it is less dense than air and unreactive, so it will not burn.
Argon is used in light bulbs and in welding to provide an unreactive atmosphere. Neon is used in advertising signs.
Key points
- Noble gases are in group 0.
- They are unreactive.
- They have a full outer shell of electrons.
- Helium has 2 outer electrons; the others have 8.
- They exist as single atoms.
- Boiling points increase down the group.
Worked examples
Example 1
Explain why the noble gases are unreactive. [2 marks]
Model answer
They have a full outer shell of electrons (1 mark), which is a stable arrangement, so they have no tendency to lose, gain or share electrons (1 mark).
Example 2
Explain why the boiling points of the noble gases increase down the group. [2 marks]
Model answer
The atoms become larger going down the group (1 mark), so the intermolecular forces between them are stronger and more energy is needed to overcome them (1 mark).
Example 3
Explain why helium is used in balloons. [2 marks]
Model answer
Helium is less dense than air, so the balloon rises (1 mark), and it is unreactive so it will not burn or explode (1 mark).
Common mistakes
Saying helium has 8 outer electrons.
Helium has only 2, which fills its single shell.
Saying noble gases form molecules.
They exist as single atoms because they do not bond.
Explaining boiling point trends using bond strength.
It is the intermolecular forces between atoms, not bonds within them.
Saying they are unreactive because they have no electrons.
They have a full outer shell, which is a stable arrangement.
Exam tips
- Always mention the full outer shell when explaining unreactivity.
- Say intermolecular forces, not bonds, for boiling point trends.
- Remember helium is the exception with 2 outer electrons.
- Link each use to the property that makes it suitable.
Key terms
- Noble gas
- An unreactive element in group 0.
- Full outer shell
- A stable electron arrangement preventing reaction.
- Intermolecular force
- A force of attraction between separate atoms or molecules.
- Inert
- Chemically unreactive.
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Written and reviewed against the current AQA, Edexcel and OCR specifications. Spotted an error? Let us know.