AS Chemistry Unit 1 Module 2

Shapes and Bond Angles
1. Tetrahedral
  1. 4 BPs, 0 LPs.
    1. 109.5'
  2. Example - Methane
2. Trigonal Planar
  1. 3 BPs, 0 LPs.
    1. 120'
  2. Example - Boron Trifluoride
3. Linear
  1. 2BPs, 0LPs.
    1. 180'
  2. Example - Beryllium Dichloride
4. Octahedral
  1. 6BPs, 0LPs.
    1. 90'
  2. Example - Sulfur Hexafluoride
5. Pyramidal
  1. 3BPs, 1 LP.
    1. 107'
  2. Example - Ammonia
6. Non - Linear
  1. 2BPs, 2 LPs.
    1. 104.5'
  2. Example - Water
Ionisation Energies
1. Orbitals
  1. Each shell contains three p orbitals, which hold 2 electrons each, so 6 altogether.
  2. Each shell contains 5 d orbitals, which hold 2 electrons each, so 10 altogether.
  3. Each shell contains one s orbital, which holds 2 electrons
Electron Configuration
1. Positive and negative ions
2. Dot and cross diagrams
3. Half equations
4. Fill orbitals seperately (seats on the bus)
  1. Arrow up then arrow down to fill orbital
Structure, Bonding and Properties
1. See Bonding Mind Map
  1. Dative Covalent Bond
  2. Expansion of the Octet
  3. Polar and Non Polar bonds
    1. If electronegativity is less than 0.4, NON POLAR, more than 0.4, POLAR!
    2. Symmetry cancels
    3. Delta Positive or Negative
  4. Permanent Dipole
Intermolecular Forces
1. The longer the chain, the more points of contact
  1. The more points of contact, the stronger the van der waals forces
    1. The more the van der waals forces, the higher the boiling point.
2. Van Der Waals X1
  1. Permanent Dipole-Dipole Forces 10X
    1. Hydrogen Bonds X50
    2. Any bond X1000

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AS Chemistry Unit 1 Module 2

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