Ionic bonding

• ionic bonding has giant lattice networks
• in an ionic solid, there's strong electrostatic interactions between the ions
• the smaller the ions the more energy is require to overcome the electrostatic attraction
• the strength of ionic bonding can be calculated by the amount of energy needed to break one mole of solid ( but in a gas state)
• when both cation and anion are doubly charged, the energy required to separate the ions is larger. (like Mg2+ and O2- making MgO)
• the smaller the ions and the larger charge makes ionic bonding stronger.
• ionic radii increases as you go down a group due to ions having more electron shells
• solid ionic compounds do not tend to conduct electricity as there are no delocalised electrons and the ions are not free to move under the force of potential difference
• molten ionic compounds can conduct electricity as there are ions free to move around and can travel to the electrodes of the opposite signs
• lithium nitrate can conduct electricity in the solid state
• aqeuous ionic compounds can also conduct electricty
• physical properties of ionic compounds:

  • brittle
  • high melting points
  • soluble in water
• if stress is applied to an ionic material, the ions may slide over each other, ions of the same charge now may be next to each other so it breaks off (brittle)
• a good example of the proof of ions is the fact that they can conduct electricity and electrolysis when molten this is because:

  • positive ions migrate to the anode where they gain electrons and become ___ atoms
  • negative ions migrate to the cathode where they lose electrons and become ___ atoms
• An ionic bond is the bond formed between a positively charged and negatively charged ion due to the electrostatic forces of attraction between them