AQA · GCSE · Chemistry
Course version: 8462 · Version from Sept 2018
Students should be able to explain chemical bonding in terms of…
Full specification wording
Chemical bonds: Students should be able to explain chemical bonding in terms of electrostatic forces and the transfer or sharing of electrons.
All chemical bonding is fundamentally driven by electrostatic forces, which are the attractions between positive and negative charges.
Checked against the AQA 8462 specification (opens in a new tab) on .
- Point 6 of 6
- 3 key terms
Study notes
From the checked teaching notes for this specification point.
The idea
All chemical bonding is fundamentally driven by electrostatic forces, which are the attractions between positive and negative charges. In ionic bonding, electrons are transferred from a metal to a non-metal, creating oppositely charged ions (e.g., Na⁺ and Cl⁻) that are held together by strong electrostatic attraction. In covalent bonding, non-metal atoms share pairs of electrons; the electrostatic attraction occurs between the positive nuclei of the atoms and the negative shared electrons. In metallic bonding, the attraction is between a lattice of positive metal ions and a sea of negative delocalised electrons. Understanding these electrostatic interactions is key to explaining bond strength.
What earns the marks
- Explain that ionic bonding involves the transfer of electrons to form oppositely charged ions attracted by electrostatic forces.
- Explain that covalent bonding involves sharing electron pairs, with electrostatic attraction between nuclei and shared electrons.
- Explain that metallic bonding involves electrostatic attraction between positive metal ions and delocalised electrons.
- Identify electrostatic forces as the fundamental attraction between positive and negative charges in all bond types.
Common mistakes and how to put them right
Failing to mention electrostatic forces when explaining why bonds are strong.
Put it right: State that strong electrostatic attraction holds the particles together.
Confusing the particles involved in the electrostatic attraction for different bonds.
Put it right: Specify ions for ionic, nuclei and shared electrons for covalent, and positive ions and delocalised electrons for metallic.
Using the term 'intermolecular forces' when describing the bonds within a molecule or lattice.
Put it right: Use 'electrostatic forces' or 'covalent bonds' for intramolecular attraction.
Exam tips
- Whenever a question asks why a bond is strong or requires a lot of energy to break, explicitly mention 'strong electrostatic forces'.
- Be specific about what is attracting what: positive ions and negative ions (ionic), positive nuclei and shared electrons (covalent), or positive ions and delocalised electrons (metallic).
- Do not mix up the concepts of electron transfer (ionic) and electron sharing (covalent).
Try the lesson
The start of the Chemical bonds: Students should be able to explain chemical bonding in terms of electrostatic forces and the transfer or sharing of electrons. lesson, made from checked teaching notes for this specification point.
Have a go first
Which force holds oppositely charged ions together in an ionic compound?
Listen
All chemical bonding is fundamentally driven by electrostatic forces, which are the attractions between positive and negative charges. In ionic bonding, electrons are transferred from a metal to a non-metal, creating oppositely charged ions (e.g., Na⁺ and Cl⁻) that are held together by strong electrostatic attraction. In covalent bonding, non-metal atoms share pairs of electrons; the electrostatic attraction occurs between the positive nuclei of the atoms and the negative shared electrons. In metallic bonding, the attraction is between a lattice of positive metal ions and a sea of negative delocalised electrons. Understanding these electrostatic interactions is key to explaining bond strength. A strong answer earns marks for these points. Explain that ionic bonding involves the transfer of electrons to form oppositely charged ions attracted by electrostatic forces. Explain that covalent bonding involves sharing electron pairs, with electrostatic attraction between nuclei and shared electrons. Explain that metallic bonding involves electrostatic attraction between positive metal ions and delocalised electrons. Identify electrostatic forces as the fundamental attraction between positive and negative charges in all bond types. A common slip: Failing to mention electrostatic forces when explaining why bonds are strong. Instead, state that strong electrostatic attraction holds the particles together. Exam tip: Whenever a question asks why a bond is strong or requires a lot of energy to break, explicitly mention 'strong electrostatic forces'.
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Key words
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Electrostatic forces
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Electron transfer
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Electron sharing
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See every definition
- Electrostatic forces
- The attractions between positive and negative charges, which fundamentally drive all chemical bonding.
- Electron transfer
- The movement of electrons from a metal to a non-metal in ionic bonding, creating oppositely charged ions.
- Electron sharing
- The sharing of pairs of electrons by non-metal atoms in covalent bonding.
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