C5 - Chemicals of the Natural Environment

Ionic Bonding
1. Giving/Takeing Electrons
  1. Form positive/negative ions
2. Hydroshphere
  1. Where water is formed
3. Salt Formulae
  1. Magnesium Chloride
    1. Mg2+Cl-
  2. Sodium Chloride
    1. Na+Cl-
  3. Magnesium Sulphate
    1. Mg2+SO2-
  4. Sodium Sulpahte
    1. Na2+SO42-
  5. Potassium Bromide
    1. K+Br-
  6. Potassium Chloride
    1. K+Cl-
4. Tests
  1. Ions have distinct properties
  2. Tell you what ions are present
  3. Positive
    1. Add sodium hydroxide
      1. The metal will form metal hydroxide
        Forms precipitate
        Colour may tell you ion
  4. Negative
    1. Add reagent eg: silver nitrate
      1. Forms precipitate
        May tell you ion
  5. Positive losses ion
  6. Negative gains one for full outer shell
  7. Opposite charged attract
  8. Chrystals
    1. Forces push on layer to move across
      1. Two negative/positive it repels
        Chrystal breaks before bends
    2. High melting/boiling point
      1. Large Structure
      2. Strong bonds
Covalent Bonding
1. Simple
  1. Air
    1. Oxygen
      1. Double covalent bond
      2. Weak intermolecular bonds
        Between moelcules
      3. Strong intramolecular bonds
        Bonds within the molecule
    2. Nitrogen
      1. Triple Bond
    3. Carbon Dioxide
    4. Low melting/boiling point
  2. Molecules
    1. Florine
      1. One Bond
  3. Sharing electrons
    1. Held together by negative electron
  4. 2- = 2 Bonds
  5. 1- = 1 Bond
  6. 3- = 3 Bonds
2. Giant
  1. Minerals from lithosphere
  2. Minerals
    1. Diamond
      1. High melting/boiling point
      2. Hard
      3. Insoluble
      4. Insulator
    2. Graphite
      1. High melting/boiling point
      2. Soft
      3. Conductor
      4. Can't break Carbon apart
        Can break layers
    3. Silicon Dioxide
3. Electrostatic attractions
  1. Between Nuclei and electrons
    1. Electrons are shared
4. Don't conduct when pure
5. Usually non-metal
Extraction Metals
1. Metallic Bonding
  1. Giant Structure
  2. Strong metallic bonds
2. Metals attract to free negative electrons
  1. Sea of electrons
  2. Strong Structure
  3. Can conduct electricity
    1. Flow through substance carrying charge
  4. If force is applied
    1. Ions slip over eachother
      1. Malleable
        unlike chrystals
3. Reduction/Oxidation (Redox)
  1. Use Carbon to pull away metal ion
  2. Copper+Carbon=Carbon Dioxide+Copper
4. Electrolosis
  1. Positive electrode
    1. Attracts Oxygen
      1. Forms Carbon Dioxide
        Replaced Regularly
        Runs out of Carbon
    2. Anode
    3. Graphite (Carbon)
  2. Negative electrode
    1. Attracts Aluminium
      1. Forms molten aluminium
        Used
    2. Cathode
  3. Aluminium
  4. Aluminium dissolved in molten crydite
    1. Half the energy
      1. Melts at 1000 degrees not 2000
  5. Properties of metals
    1. Malleable
    2. High melting/boiling point
    3. Conductor

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C5 - Chemicals of the Natural Environment

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