bonding

• Ionic bonding


  The electrostatic force of attraction between oppositely charged ions formed by electron transfer
• Formation of ions


  1. Metal atoms lose electrons to form +ve ions

  2. Non-metal atoms gain electrons to form -ve ions
• Mg ion formation


  • Mg goes from 1s2 2s2 2p63s2 to Mg2+ 1s2 2s2 2p6
• O ion formation


  • O goes from 1s2 2s2 2p4 to O2- 1s2 2s2 2p6
• Covalent bond


  A shared pair of electrons
• Dative covalent bond


  The shared pair of electrons in the covalent bond come from only one of the bonding atoms
• Dative covalent bond examples

  • NH4+
  • H3O+
  • NH3BF3
• Metallic bonding


  The electrostatic force of attraction between the positive metal ions and the delocalised electrons
• Factors affecting metallic bonding strength

  • Number of protons/ Strength of nuclear attraction
  • Number of delocalised electrons per atom
  • Size of ion
• The more protons, the stronger the metallic bond
• The more delocalised electrons, the stronger the metallic bond
• The smaller the ion, the stronger the metallic bond
• The dative covalent bond acts like an ordinary covalent bond when thinking about shape, so in NH4+ the shape is tetrahedral