GCSE Chemistry Revision "Properties of Ionic Compounds"
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Ionic compounds form giant ionic lattices with positive and negative ions held by strong electrostatic forces called ionic bonds, leading to high melting points like sodium chloride melting at 800°. Although they can't conduct electricity when solid, they become conductive when melted or dissolved in water since the ions can move to carry electrical charge, not electrons.
Insights
- Ionic compounds have high melting and boiling points due to the strong electrostatic forces between positive and negative ions, requiring substantial energy input for bond breakage.
- The conductivity of ionic compounds is linked to the mobility of ions when in a molten or dissolved state, allowing them to carry electrical charge, highlighting the distinction that it is ions, not electrons, responsible for the movement of charge.
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Recent questions
How do ionic compounds bond?
Through strong electrostatic forces known as ionic bonds.