Chemisty Revision

Chemisty Revision

1. Periodic table

   • Elements
     • Electons
       • mass;very small (0.0005)
       • Charge;negative
       • location;outer shells
     • Neutron
       • Location;inside the nucleus
       • Charge;neutral
       • Mass; 1
     • Protons
       • Mass; 1
       • Charge;positive
       • Location;inside the nucleus
   • Ordered in atomic mass
   • Columns going across; groups
   • Rows going across;periods
   • Group 0;noble gases

2. Isotops

   • Atoms with the same number of protons but different number of neutrons

3. Maxium number of electrons in each shell;

   • 2,8,8,12

4. Colvent compounds

   • Covenlent bonds
     • Bonds ocurring between non-metals
     • Electrons shared between atoms
   • Three different types;
     • simple molecules(very small)
       • very low boiling point.
       • Intermolecluar forces are weak (force between molecules)
       • Chlorine has a low boiling point as it contains simple covent molecules
       • Nitrogen has a low boiling point as it contains simple colvent molecules
     • Giant covelent (giant cluster structures)
     • Polymers(long, straight lines)
       • long chains of covalently bound molecules.
         • Along chains are many weak intermolealur forces
   • Covalent;sharing metals= always lose electrons.

5. diamond

   • Structure;each carbon atoms is bonded to other of their own
   • Melting points;high melting points because of large repeating structures
   • Electrical conductivity;Doesn't conduct as all carbon electrons are bonded

6. Graphite

   • Structure;each carbon in every layer is bonded to three others.
     • Between the layers are very weak forces meaning they can slide
       • Used in pemcils
   • Melting points;high melting points because of large repeating structures
   • Electrical conductivity;from free delocalised electron it can conduct

7. Delocalised=negative

8. Fullerene

   • Structure;carbon bonded with three other carbons.
     • hollow, cage like structure.
   • Properties;
     • Used in nanotubes
     • can be used for drug delivery

9. Graphene

   • Structure;one graphite layer

10. Ion;metal=non-metal=electrostatic

    • Ionic bonds
      • Formed by the transfer of electrons to form ions. These are attracted to each other by electronic forces.
      • Ionic structures
        • Giant repeating lattices
          • With strong electostatic forces in all directions
            • Meaning high melting&Boiling points
          • Lattices;
        • When dissolved or molten(melted) the ions can move=create electrons
        • Higher boiling points from giant repeating lattices with strong electrostatic forces in all directions.

11. Metallic bonding

    • losing electrons to gain a full outer shell
    • Electrons form a 'sea of delocalisation'
      • flows around the positive metals

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