AQA · GCSE · Combined Science
Course version: 8464 · Version from Sept 2018
The elements in Group 0 of the periodic table are called the noble gases.…
Full specification wording
Group 0: The elements in Group 0 of the periodic table are called the noble gases. They are unreactive and do not easily form molecules because their atoms have stable arrangements of electrons. The noble gases have eight electrons in their outer shell, except for helium, which has only two electrons.
Group 0 elements are the noble gases: helium, neon, argon, krypton, xenon and radon.
Checked against the AQA 8464 specification (opens in a new tab) on .
- Point 1 of 4
Study notes
From the checked teaching notes for this specification point.
The idea
Group 0 elements are the noble gases: helium, neon, argon, krypton, xenon and radon. Their atoms have full outer electron shells, which is a stable arrangement. Helium has two electrons in its only shell; the others have eight electrons in their outer shell. Because they already have a stable arrangement, noble gases do not need to gain, lose or share electrons. Consequently, they are unreactive and exist as single atoms rather than forming molecules easily. For example, neon (2,8) and argon (2,8,8) are chemically inert and are used where a non-reactive atmosphere is needed, such as in filament lamps or welding shields. This stable electron arrangement explains their lack of compounds under normal conditions.
What earns the marks
- Group 0 elements are called the noble gases and include helium, neon, argon, krypton, xenon and radon.
- Noble gases are unreactive because their atoms have stable, full outer electron shells.
- Helium has only two electrons in its outer shell; the other noble gases have eight electrons in their outer shell.
- Noble gases do not easily form molecules because they do not need to gain, lose or share electrons.
- The stable electron arrangement explains why noble gases exist as single atoms under normal conditions.
- The unreactive nature of noble gases makes them useful in applications such as inert atmospheres and lighting.
Common mistakes and how to put them right
Stating that all noble gases have eight outer electrons, forgetting helium's two.
Put it right by naming helium as the exception with two electrons.
Saying noble gases never form any compounds.
Put it right by explaining they are unreactive under normal conditions but some compounds can be made under extreme conditions.
Confusing noble gases with Group 1 or Group 7 elements.
Put it right by linking Group 0 to full outer shells and lack of reactivity.
Exam tips
- Quote the electron arrangements of neon (2,8) and argon (2,8,8) to show full outer shells.
- Explain unreactivity by referring to the stable arrangement rather than simply saying 'they are stable'.
- Use a named noble gas and a real use, such as argon in welding, to support your answer.
Try the lesson
The start of the Group 0: The elements in Group 0 of the periodic table are called the noble gases. They are unreactive and do not easily form molecules because their atoms have stable arrangements of electrons. The noble gases have eight electrons in their outer shell, except for helium, which has only two electrons. lesson, made from checked teaching notes for this specification point.
Have a go first
What name is given to the elements in Group 0 of the periodic table?
Listen
Group 0 elements are the noble gases: helium, neon, argon, krypton, xenon and radon. Their atoms have full outer electron shells, which is a stable arrangement. Helium has two electrons in its only shell; the others have eight electrons in their outer shell. Because they already have a stable arrangement, noble gases do not need to gain, lose or share electrons. Consequently, they are unreactive and exist as single atoms rather than forming molecules easily. For example, neon (2,8) and argon (2,8,8) are chemically inert and are used where a non-reactive atmosphere is needed, such as in filament lamps or welding shields. This stable electron arrangement explains their lack of compounds under normal conditions. A strong answer earns marks for these points. Group 0 elements are called the noble gases and include helium, neon, argon, krypton, xenon and radon. Noble gases are unreactive because their atoms have stable, full outer electron shells. Helium has only two electrons in its outer shell; the other noble gases have eight electrons in their outer shell. Noble gases do not easily form molecules because they do not need to gain, lose or share electrons. A common slip: Stating that all noble gases have eight outer electrons, forgetting helium's two. Instead, naming helium as the exception with two electrons. Exam tip: Quote the electron arrangements of neon (2,8) and argon (2,8,8) to show full outer shells.
See it
Label the diagram
Some boxes have lost their names. Pick the right name for each number.
1Box 1
2Box 2
3Box 3
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Test your understanding of Group 0: The elements in Group 0 of the periodic table are called the noble gases. They are unreactive and do not easily form molecules because their atoms have stable arrangements of electrons. The noble gases have eight electrons in their outer shell, except for helium, which has only two electrons.
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