1. OIL RIG
   1. oxidation is loss
   2. reduction is gain
2. Experiments
   1. Magnesium oxide
      1. 2.4g magnesium
         1. makes 4g Magnesium Oxide
         2. therefore uses 1.6g oxygen
      2. RAM
         1. 24g magnesium + 16goxygen = 4g Magnesium Oxide
         2. 1 mole Mg + 1mole O = 1 mole MgO
   2. Copper (II) Oxide
      1. burn in hydrogen
         1. copper + water
      2. 16g Cu3O makes 12.8g Cu
         1. 16-12.8 = 3.2g oxygen used to make water
         2. 2moles oxygen combine with 2 moles copper
            1. CuO
   3. Formula of Water
      1. current passed through water (dilute sulphuric acid)
      2. cathode = Hydrogen
         1. 2 units
      3. annode = oxygen
         1. 1 unit
      4. one mole any gas at RTP same volume
         1. 2moles hydrogen + 1 mole oxygen = water H2O
   4. moles
      1. know number moles combining element
         1. formula of compound deduced
3. Percentage Yield
   1. chemical reaction
      1. products formed
      2. yield
         1. amount of product
   2. percentage yield = (actual yield / predicted yield) x 100
4. Percentage Purity
   1. percentage purity = (amount of pure substance / total amount of substance) x 100
5. Chemical Equation
   1. steps
      1. write word equation
         1. hydrogen + oxygen ---> water
         2. sulphur + oxygen ---> sulphur dioxide
      2. write symbols (elements) & formulae (compounds)
      3. Balance Equation
         1. same number of each type atom on both sides
            1. 2H2 +O2 ---> H2O
            2. S + O2 ---> SO2
         2. balance numbers ONLY infront of formulae
   2. Diatomic Elements
      1. hydrogen H2
      2. Oxygen O2
      3. Nitrogen N2
      4. Chlorine Cl2
      5. Bromide Br2
      6. Iodine I2
   3. radicals
      1. An atom or group of atoms that has at least one unpaired electron and is therefore unstable and highly reactive. In animal tissues, free radicals can damage cells and are believed to accelerate the progression of cancer, cardiovascular disease, and age-related diseases.
      2. Words
         1. lead(II) nitrate + potassium iodide ---> lead (II) iodide + potassium nitrate
      3. symbols
         1. Pb(NO3)2 + KI ---> PbI2 + KNO3
      4. Balance the nitrates
         1. Pb(NO3)2 + KI ---> PbI2 + 2KNO3
      5. balance the iodides
         1. Pb(NO3)2 + 2KI ---> PbI2 + 2KNO3
6. Ionic Equations
   1. state symbols
      1. solid s
      2. liquid l
      3. gas g
      4. solution aq
   2. reactions involving ions
      1. atoms
      2. radicals
      3. lost or gained electrons
   3. only shows ions that change
   4. spectator ions
      1. do not take part in reation
      2. not shown in the ionic equation
   5. examples
      1. Pb2+ (aq) + 2I- (aq) ---> PbI2 (s)
      2. Cu2+ (aq) + 2OH- (aq) ---> Cu(OH)2 (s)
7. Linking Reactants and Products
   1. balanced equation
      1. 2Mg (s) + O2 (g) ---> 2MgO (s)
   2. number of moles
      1. 2 + 1 ---> 2
   3. Convet moles to mass
      1. 48g + 32g ---> 80g
      2. magnesium Ar=24
      3. oxygen Ar = 16
   4. 6g magnesium = 0.25 moles
      1. 0.25 moles magnesium oxide = 10g
   5. example
      1. N2 (g) + 3H2 (g) ---> 2NH3 (g) ammonia
8. Moles of solution
   1. solute
      1. The substance that is dissolved in a solution. For solutions of fluids, the solvent is present in greater amount than the solute.
         1. 1mole dm-3 solution
            1. 1 mole solute
            2. 1dm3 (1000cm3) solvent
            3. 1dm3 (1000cm3) solution
   2. moles = mol dm3 x volume (litres)