Properties of Ionic Compounds

• What should you be able to describe by the end of the video?

  How ionic compounds form giant ionic lattices
• Why do ionic compounds have high melting and boiling points?

  Because of the strong electrostatic forces of attraction between ions
• Why can't ionic compounds conduct electricity when solid?

  Because the ions are locked in place by strong electrostatic forces
• When can ionic compounds conduct electricity?

  When they are molten or dissolved in water
• What is an example of ionic bonding given in the video?

  The reaction between sodium and chlorine
• What happens to the sodium atom during the reaction with chlorine?

  One electron is transferred from sodium to chlorine
• What charge does the sodium ion have after the reaction?

  One positive charge
• What charge does the chloride ion have after the reaction?

  One negative charge
• What is the electronic structure of sodium and chloride ions after the reaction?

  They both have a full outer energy level
• What is the name of the compound formed from sodium and chlorine?

  Sodium chloride
• What is the structure of ionic compounds like sodium chloride?

  They form giant ionic lattices
• How are ions arranged in a giant ionic lattice?

  Every positive ion is surrounded by negative ions and vice versa
• What are the forces of attraction in a giant ionic lattice called?

  Electrostatic forces of attraction
• What do strong electrostatic forces of attraction do in ionic compounds?

  They hold the positive and negative ions in place
• What happens to ionic solids when heated?

  The particles vibrate and can eventually break the electrostatic forces
• What is the melting point of sodium chloride?

  Around 800°C
• Why does it take a great deal of heat energy to break ionic bonds?

  Because the electrostatic forces of attraction are very strong
• What is the difference between how ionic compounds conduct electricity in solid and molten states?

  In solids, ions cannot move; in molten states, they can move
• What is often confused in exams regarding ionic compounds conducting electricity?

  That it is the ions that are moving, not electrons
• What are the key properties of ionic compounds?

  • High melting and boiling points
  • Cannot conduct electricity when solid
  • Can conduct electricity when molten or dissolved in water
• How do ionic compounds form giant ionic lattices?

  • Metal reacts with non-metal
  • Electrons are transferred between atoms
  • Ions are arranged in a three-dimensional structure
  • Strong electrostatic forces hold the ions in place