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Module 2 Chapter 6 (6.1 Shapes of molecules and ions (Shapes (2 regions-…

- - - - Lone pairs= one region
      - Bond angle for number of regions
      - Subtract 2.5 for every lone pair
- - - - Polar molecules can form strong enough bonds to permit dissolving
      - Water can dissolve most but not all ionic substances
- - - - Electrons and atoms constantly mobbing, temporary uneven distribution of electrons occurs. Creates a dipole induces dipole in neighbour= attraction
      - Occurs for an instant
      - Non-polar- Only London forces, as molecules get larger number of electrons increase so size of dipoles increase- stronger forces
      - All atoms and molecules are able to exert attractive forces
    - - Between molecules that are polar- do not come and go so exert full time forces which are stronger= higher melting point
      - Opposite dipoles attract
      - Have London forces as well
  - - - Solid state= Simple molecular lattice, with only London forces holding them together
      - When heated intermolecular forces overcome- melting some overcome- boiling all overcome Doesn't break covalent
      - Low melting and boiling points, Don't conduct no charged particles
      - Solubility
        
        Non-polar substances
        
        Polar- Insoluble- Intermolecular bonds in solvent to strong
        
        Non-polar- Soluble in non-polar solvents as similar strength form between solute and solvent
        
        Polar substances
        
        Dissolve in polar solvents due to strong attraction
        
        Depends on strength of dipole- very difficult to predict