Properties of Ionic Compounds
Ionic compounds have unique properties due to their lattice structure:
Solid State Properties
In the solid state, ionic compounds have the following characteristics:
- High melting points due to the strong electrostatic forces in the lattice.
- Poor electrical conductivity because ions are fixed in the lattice and cannot move freely.
- Brittleness, as a sharp blow can disrupt the lattice structure.
Highlight: Why do ionic compounds not conduct electricity when solid? The ions are not free to move in the solid state, preventing electrical conduction.
Liquid State Properties
When melted or dissolved in water, ionic compounds behave differently:
- They conduct electricity because the ions are free to move.
- The lattice structure is broken down, allowing for ion mobility.
Highlight: Why do ionic compounds conduct electricity when molten? In the liquid state, ions are free to move and carry electrical charge.
Example: When sodium chloride is melted, the Na⁺ and Cl⁻ ions can move freely, allowing for electrical conduction.
Vocabulary: Electrolysis is the process of using electricity to drive a non-spontaneous chemical reaction, often performed with molten ionic compounds.
Understanding these properties is crucial for predicting the behavior of ionic compounds in various states and applications.
