Ionic Bonding

• Ionic bond occurs between metal and non-metal electrostatically attracted to each other. Very strong attraction.
• Solubility of Ionic Compounds: The ionic compound is attracted to the polar water molecules and binds with water molecule ion called hydration, the water releases the compound's energy, and water overcomes the ionic bonding.
• The melting and boiling points of Ionic compounds are strong and required a lot of heat energy to break them.
• Ionic compounds cannot conduct electricity in their solid form because the ions are held together in the lattice and can't freely move.

  When molten, the ion can break free from the lattice and is able to freely move, and can carry an electric current.

  
• Ionic Compound are Brittle meaning they shatter when they are hit.

  
• The structure of ionic compounds is a Giant Ionic Lattice

  
• Dot-and-cross diagrams of Ionic compounds

  • outer-shell electrons from a metal atom are transferred to the outer shell of a non-metal
  • Positive and negative ions are formed.

  
• Solubility of ionic compound requires two main processes:

  1. Ionic lattice must be broken
  2. Water molecules must attract and surround the ions
• Ionic Bond has:

  • High melting point because strong ionic bonds throughout the giant ionic lattice – all of which have to be broken hence needs high energy
  • High and low Conductivity
  • -> Low conductor when solid as the ions cannot freely move.
  • -> Good conductor when molten or when dissolved in water because the ions are free to move
• The ions have a regular, repeating arrangement called an ionic lattice. The lattice is formed because the ions attract each other and form a regular pattern with oppositely charged ions next to each other.