1. Chemical bonds: -
1. Ionic – between separate ions
2. Covalent: divided into 2 types
o polar covalent where the bonding pair of electrons is nearer to one atom
o Pure covalent where the bonding pair of electrons is shared equally
o Metallic- bonding caused by electrons delocalised throughout the solid
2. Intermolecular forces (BETWEEN covalent molecules)
o Hydrogen bonds: Between δ+ H in one molecule and δ- F,O or N in another molecule
o Dispersion forces: between all molecules. Their strength depends upon the number of electrons in the molecule.
o Dipole/dipole forces (aka Van Der Waals): between δ+ in one molecule and δ- in another molecule.