Study Notes
Metallic bonding involves the electrostatic attraction between positive ions in a giant metallic lattice and a 'sea' of delocalized electrons. This unique structure gives metals their characteristic properties.
- Metallic Bonding — the strong electrostatic attractions between positively charged metal ions and the surrounding delocalized electrons. Example: Metal atoms lose their outer-shell electrons to form positive ions, creating a 'sea' of electrons around them.
- Electrical Conductivity — the ability of metals to conduct electricity due to free electrons that move and carry charge. Example: Electrons entering one end of the metal cause a delocalized electron to displace from the other end, allowing electricity to flow.
- Malleability and Ductility — the ability of metals to be hammered into shapes or drawn into wires without breaking. Example: Layers of positive ions can slide over one another while delocalized electrons move with them, maintaining metallic bonds.
Exam Tips
Key Definitions to Remember
- Metallic Bonding: Electrostatic attraction between positive ions and delocalized electrons.
- Malleability: Ability to be hammered into shapes.
- Ductility: Ability to be drawn into wires.
Common Confusions
- Confusing metallic bonding with ionic bonding.
- Misunderstanding why metals conduct electricity compared to ionic compounds.
Typical Exam Questions
- What is metallic bonding? Electrostatic attraction between positive ions and delocalized electrons.
- Why do metals conduct electricity? Due to the presence of free electrons that can move and carry charge.
- How does metallic bonding contribute to malleability? Layers of ions can slide over each other without breaking bonds.
What Examiners Usually Test
- Understanding of metallic bonding structure.
- Explanation of properties like conductivity and malleability.
- Differences between metallic and other types of bonding.