Chemical Properties of Ionic Compounds
Chemistry: AQA GCSE Higher, topic 2.3.2
Properties of Ionic Compounds
The lattice structure of ionic compounds gives them certain properties.
High melting and boiling points
- To break ionic bonds, significant energy is needed to overcome the electrostatic forces between the ions and electrons in the lattice.
- Because of this, the melting and boiling points of ionic compounds is high.
Don't conduct electricity if solid
- When solid, the ions in the lattice are fixed in place.
- This means that charges cannot flow, so electricity cannot be conducted.
Conduct electricity if liquid or in solution
- When molten, or dissolved in water, the ions in the lattice can move freely.
- Because of this, charge can flow and electricity can be conducted.
Test yourself on Chemical Properties of Ionic Compounds
Why can a molten ionic compound conduct electricity when the same compound cannot conduct electricity as a solid?
What would happen to the melting point of an ionic compound if the electrostatic forces between its ions were weaker?
Why can't a solid ionic compound conduct electricity, even though it is made up of charged ions?
What does the high melting point of an ionic compound suggest about the electrostatic forces between its ions?