1. Draw all VE for each atom
   1. Stable structure if all electrons paired and each atom has 8 electrons around (8 electron rule)
   2. Split all bonds and count the electrons for each atom => if no = no of VE, then no charge
   3. Assign all bonding electrons to the atom with higher EN => we get the oxidation no
   4. Sometimes RESONANCE structures are possible which stabilize a charge, like in the nitrate ion
   5. Resonance structures stabilizes a molecule like ozone
2. All electrons repulse each other ("VSEPR") => we can estimate the 3D structure
   1. most common geometries
3. AO Hybridization to explain single and multiple bonds
   1. Example: Carbon has 4 electrons, but they are not equal ! => Combine 2s and 2p AO's together:
      1. For 4 single bonds in C, we need 4 equal AO's, half filled => sp3
      2. For 3 single bonds in C, we need to combine s+2xp, = sp2 one p-AO is left
   2. Common hybridisation and structures
4. sigma and pi bonds and lone pairs
5. 2 sigma, 2 pi bonds and l.p.