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Module 3 Chapter 7 (7.2 Ionisation energies (Period (Nuclear charge…

- - - - Same number of electrons in outer shell
    - - Sub-shells filled the same way across a period
    - - s,p,d and f- follow the order of sub-shell filling
- - - - High electrical conductivity- conduct when solid or molten- delocalised electrons move carrying charge through structure
      - High MP and BP- High temp. needed to break strong electrostatic attraction between cation and electrons
  - - - Properties
        
        Stable due to strong covalent bonds
        
        High melting and boiling points
        
        Insoluble
        
        Don't conduct- except graphite and graphene
    - - Graphite
        
        Parallel layers of hexagonally arranged carbon atoms
        
        Layers held together by weak London forces
        
        Spare electron delocalised so conducts
        
        Planar hexagonal layers- bond angle 110
      - Graphene
        
        Single layer of graphite
        
        Thinnest and strongest material- almost transparent
        
        Allotrope of carbon- 2D hexagonal lattice
        
        Conducts heat and electricity
        
        Base of graphite, charcoal, nanotubes and fullerenes
      - Diamond
        
        Very high melting point- very strong covalent bonds must be broken
        
        Doesn't conduct electricity- all electrons held tightly between atoms so can't move
        
        Insoluble in water and organic solvent as there aren't any possible attractions with the solvent molecules
      - Silicon dioxide
        
        High melting point- very strong silicon-oxygen covalent bonds
        
        Can't conduct electricity- no delocalised electrons and electrons aren't free to move
        
        Insoluble in water and organic solvents- No possible attractions that can occur between sovlent molecules and silicon or oxygen atoms which could overcome the covalent bonds in the giant structure