Ionic bonding

• Electrons

  Exist in energy levels or shells
• Maximum electrons per energy level

  • First energy level: 2
  • Second energy level: 8
  • Third energy level: 8
• Noble gases (group 0)

  • Have a full outer energy level
  • Are stable
  • Are unreactive
• Ionic bonding

  Occurs when a metal reacts with a non-metal
• Ionic bonding between lithium and fluorine

  1. Lithium atom loses outer electron

  2. Fluorine atom gains electron

  3. Both atoms achieve full outer energy level
• Lithium ion

  Atom with 3 protons and 2 electrons, overall +1 charge
• Fluoride ion

  Atom with 9 protons and 10 electrons, overall -1 charge
• During ionic bonding, group 1 metals lose 1 electron forming a +1 ion, and group 7 non-metals gain 1 electron forming a -1 ion
• Ionic bonding

  • Sodium and chlorine
• Ionic bonding between sodium and chlorine

  1. 1 electron passes from sodium atom to chlorine atom

  2. Both atoms achieve full outer energy level
• Ionic bonding

  Occurs when a metal reacts with a non-metal
• Electron transfer in ionic bonding between group two metals and group six non-metals

  1. Group two metal loses two electrons

  2. Electrons transferred to group six non-metal

  3. Group two metal forms positive ion

  4. Group six non-metal forms negative ion

  5. Both ions have full outer energy level (stable electronic structure of noble gas)
• Ionic bonding

  • Group two metals lose two electrons
  • Group six non-metals gain two electrons
  • Both ions have full outer energy level (stable electronic structure of noble gas)
• In dot and cross diagrams, only the outer energy levels are shown as they are involved in the reaction
• In exams, you could be asked to show ionic bonding between any metal in group 1 or 2 and any non-metal in group 6 or 7