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.

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Summary

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"Giant Ionic Lattices: Strong Bonds, Conductivity"

  • Ionic compounds form giant ionic lattices where positive ions are surrounded by negative ions and vice versa, held together by strong electrostatic forces of attraction known as ionic bonds.
  • The strong electrostatic forces in ionic compounds result in high melting and boiling points, requiring significant heat energy to break the bonds, such as sodium chloride melting at around 800°.
  • While ionic compounds cannot conduct electricity when solid due to locked ions, they can conduct when melted or dissolved in water as the ions gain mobility to carry electrical charge, emphasizing that it's the ions moving, not electrons.
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