AQA · GCSE · Chemistry
Course version: 8462 · Version from Sept 2018
The ions produced by metals in Groups 1 and 2 and by non-metals in Groups…
Full specification wording
Ionic bonding: The ions produced by metals in Groups 1 and 2 and by non-metals in Groups 6 and 7 have the electronic structure of a noble gas (Group 0).
Atoms form ions by transferring electrons so that their outer shell becomes full, giving the stable electronic structure of a noble gas.
Checked against the AQA 8462 specification (opens in a new tab) on .
- Point 4 of 7
- 3 key terms
Study notes
From the checked teaching notes for this specification point.
The idea
Atoms form ions by transferring electrons so that their outer shell becomes full, giving the stable electronic structure of a noble gas. A sodium atom (2,8,1) loses one electron to form Na⁺ (2,8), like neon. A magnesium atom (2,8,2) loses two electrons to form Mg²⁺ (2,8), also like neon. A chlorine atom (2,8,7) gains one electron to form Cl⁻ (2,8,8), like argon, and an oxygen atom (2,6) gains two electrons to form O²⁻ (2,8), like neon. In each case the ion has a full outer shell, which is why these ions are stable. For metals, the group number tells you how many electrons are lost; for non-metals, the number gained is 8 minus the group number. The resulting ion always matches the nearest noble gas.
What earns the marks
- Atoms lose or gain electrons so that their outer shell becomes full.
- Metal atoms in Groups 1 and 2 lose one or two electrons respectively to form positive ions.
- Non-metal atoms in Groups 6 and 7 gain two or one electrons respectively to form negative ions.
- The ion formed has the same electronic structure as the nearest noble gas in Group 0.
- Examples include Na⁺ and Mg²⁺ with the structure 2,8, and Cl⁻ with the structure 2,8,8.
Common mistakes and how to put them right
Thinking that the ion has the same number of electrons as the original atom.
Put it right: The number of electrons changes by the number lost or gained.
Confusing the noble gas matched by an ion, for example saying Mg²⁺ has the structure of argon when it is 2,8 like neon.
Writing the electron configuration of the atom instead of the ion, for example writing 2,8,7 for a chloride ion instead of the correct 2,8,8.
Exam tips
- Write the electron configuration of the atom first, then add or remove the outer electrons.
- Compare the ion configuration with the nearest noble gas to check it is correct.
Try the lesson
The start of the Ionic bonding: The ions produced by metals in Groups 1 and 2 and by non-metals in Groups 6 and 7 have the electronic structure of a noble gas (Group 0). lesson, made from checked teaching notes for this specification point.
Have a go first
A sodium atom has the electronic structure 2,8,1. When it forms an ion, which noble gas electronic structure does it achieve?
Listen
Atoms form ions by transferring electrons so that their outer shell becomes full, giving the stable electronic structure of a noble gas. A sodium atom (2,8,1) loses one electron to form Na⁺ (2,8), like neon. A magnesium atom (2,8,2) loses two electrons to form Mg²⁺ (2,8), also like neon. A chlorine atom (2,8,7) gains one electron to form Cl⁻ (2,8,8), like argon, and an oxygen atom (2,6) gains two electrons to form O²⁻ (2,8), like neon. In each case the ion has a full outer shell, which is why these ions are stable. For metals, the group number tells you how many electrons are lost; for non-metals, the number gained is 8 minus the group number. The resulting ion always matches the nearest noble gas. A strong answer earns marks for these points. Atoms lose or gain electrons so that their outer shell becomes full. Metal atoms in Groups 1 and 2 lose one or two electrons respectively to form positive ions. Non-metal atoms in Groups 6 and 7 gain two or one electrons respectively to form negative ions. The ion formed has the same electronic structure as the nearest noble gas in Group 0. Exam tip: Write the electron configuration of the atom first, then add or remove the outer electrons.
See it
Key words
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Stability and full outer shells
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Electronic structure of atoms and ions
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Group number and ion charge
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See every definition
- Stability and full outer shells
- When atoms lose or gain electrons so that their outer shell becomes full, the resulting ion is stable.
- Electronic structure of atoms and ions
- The arrangement of electrons in an atom changes by the number lost or gained when it forms an ion, so the ion's structure differs from the atom's.
- Group number and ion charge
- For metals the group number tells you how many electrons are lost, and for non-metals the number gained is 8 minus the group number.
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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