AQA · GCSE · Chemistry

    Course version: 8462 · Version from Sept 2018

    Students should be able to: explain how properties of the elements in…

    Full specification wording

    Group 0: Students should be able to: explain how properties of the elements in Group 0 depend on the outer shell of electrons of the atoms predict properties from given trends down the group.

    Group 0 elements are the noble gases: helium, neon, argon, krypton and xenon.

    Checked against the AQA 8462 specification (opens in a new tab) on .

    • Point 5 of 5
    • 4 key terms

    Study notes

    From the checked teaching notes for this specification point.

    The idea

    Group 0 elements are the noble gases: helium, neon, argon, krypton and xenon. Each has a full outer electron shell, so its atoms neither gain nor lose electrons easily. This stable arrangement means they exist as single atoms and have very weak forces between them, giving very low melting and boiling points that rise slowly down the group as atoms get larger and forces between them strengthen. They are chemically unreactive, so they are used where inertness matters, such as argon in lamps and helium in balloons. To predict trends, use the pattern: going down Group 0, relative atomic mass, atomic radius and boiling point increase, while reactivity stays very low.

    What earns the marks

    • States that Group 0 atoms have a full outer shell of electrons, which is a stable arrangement.
    • Explains that a full outer shell means the atoms do not readily lose or gain electrons, so they are chemically unreactive.
    • Links weak intermolecular forces between noble gas atoms to their very low melting and boiling points.
    • Describes the trend down the group: increasing relative atomic mass, larger atomic radius and higher boiling point.
    • Uses the trend to predict properties of a named noble gas, such as predicting that krypton boils at a higher temperature than argon.
    • Recognises that noble gases are monatomic because they do not need to bond to gain a full outer shell.

    Common mistakes and how to put them right

    • Saying noble gases have no electrons in their outer shell.

      Put it right by stating the outer shell is full, not empty.

    • Claiming noble gases are unreactive because they are too heavy.

      Put it right by linking unreactivity to the stable full outer shell.

    • Assuming boiling point decreases down the group.

      Put it right by stating that boiling point increases as atoms become larger and forces between them strengthen.

    Exam tips

    • When asked to explain, always name the full outer shell and link it to stability and lack of electron transfer.
    • For prediction questions, quote the trend first, then apply it to the named element to reach a conclusion.
    • Use comparative language such as higher, lower, larger or stronger when describing trends down the group.

    Try the lesson

    The start of the Group 0: Students should be able to: explain how properties of the elements in Group 0 depend on the outer shell of electrons of the atoms predict properties from given trends down the group. lesson, made from checked teaching notes for this specification point.

    Have a go first

    Why are the Group 0 elements unreactive?

    Listen

    Group 0 elements are the noble gases: helium, neon, argon, krypton and xenon. Each has a full outer electron shell, so its atoms neither gain nor lose electrons easily. This stable arrangement means they exist as single atoms and have very weak forces between them, giving very low melting and boiling points that rise slowly down the group as atoms get larger and forces between them strengthen. They are chemically unreactive, so they are used where inertness matters, such as argon in lamps and helium in balloons. To predict trends, use the pattern: going down Group 0, relative atomic mass, atomic radius and boiling point increase, while reactivity stays very low. A strong answer earns marks for these points. States that Group 0 atoms have a full outer shell of electrons, which is a stable arrangement. Explains that a full outer shell means the atoms do not readily lose or gain electrons, so they are chemically unreactive. Links weak intermolecular forces between noble gas atoms to their very low melting and boiling points. Describes the trend down the group: increasing relative atomic mass, larger atomic radius and higher boiling point. A common slip: Saying noble gases have no electrons in their outer shell. Instead, stating the outer shell is full, not empty. Exam tip: When asked to explain, always name the full outer shell and link it to stability and lack of electron transfer.

    See it

    A flowchart running from top to bottom. The first box states that Group 0 atoms have a full outer shell, which leads to a stable arrangement. From the stable arrangement, one arrow leads to atoms not readily losing or gaining electrons, which leads to being chemically unreactive. A second arrow from the stable arrangement leads to existing as single atoms (monatomic), which leads to very weak forces between atoms, which leads to very low melting and boiling points. Separately, a box reading 'Going down the group' branches into three: relative atomic mass increases, atomic radius increases, and forces between atoms strengthen; the last of these leads to boiling point increases.
    Shows how a full outer shell leads to stability, unreactivity and monatomic atoms with low boiling points, and how properties change down the group.

    Key words

    Say what each word means before you turn the card.

    Electronic structure and stability

    Try answering aloud or in your head before turning the card.

    Periodic trends

    Try answering aloud or in your head before turning the card.

    Intermolecular forces and physical properties

    Try answering aloud or in your head before turning the card.

    Structure and properties of monatomic gases

    Try answering aloud or in your head before turning the card.

    See every definition
    Electronic structure and stability
    Each Group 0 atom has a full outer electron shell, which is a stable arrangement, so its atoms neither gain nor lose electrons easily.
    Periodic trends
    Going down Group 0, relative atomic mass, atomic radius and boiling point increase, while reactivity stays very low.
    Intermolecular forces and physical properties
    Very weak forces between the atoms give very low melting and boiling points, which rise slowly down the group as atoms get larger and forces between them strengthen.
    Structure and properties of monatomic gases
    Because the stable arrangement means they do not need to bond to gain a full outer shell, they exist as single atoms and are chemically unreactive.

    Label the diagram

    Some boxes have lost their names. Pick the right name for each number.

    The diagram again, with 3 boxes numbered instead of named. A flowchart running from top to bottom. The first box states that Group 0 atoms have a full outer shell, which leads to a stable arrangement. From the stable arrangement, one arrow leads to atoms not readily losing or gaining electrons, which leads to being chemically unreactive. A second arrow from the stable arrangement leads to existing as single atoms (monatomic), which leads to very weak forces between atoms, which leads to very low melting and boiling points. Separately, a box reading 'Going down the group' branches into three: relative atomic mass increases, atomic radius increases, and forces between atoms strengthen; the last of these leads to boiling point increases.

    • 1Box 1

    • 2Box 2

    • 3Box 3

    0 of 3 labelled

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