• Lewis (electron dot) structures show all the valence electrons in a covalently bonded species.

• The “octet rule” refers to the tendency of atoms to gain a valence shell with a total of 8 electrons.

• Some atoms, like Be and B, might form stable compounds with incomplete octets of electrons.

• Resonance structures occur when there is more than one possible position for a double bond in a molecule.

• Shapes of species are determined by the repulsion of electron pairs according to VSEPR theory.

• Carbon and silicon form giant covalent/network covalent structures.

• Deduction of Lewis (electron dot) structure of molecules and ions showing all valence electrons for up to four electron pairs on each atom.

• The use of VSEPR theory to predict the electron domain geometry and the molecular geometry for species with two, three and four electron domains.

• Prediction of bond angles from molecular geometry and presence of non-bonding pairs of electrons.

• Prediction of molecular polarity from bond polarity and molecular geometry.

• Deduction of resonance structures, examples include but are not limited to C₆H₆, CO₃^2- and O₃.

• Explanation of the properties of giant covalent compounds in terms of their structures.

• The term “electron domain” should be used in place of “negative charge centre”.

• Electron pairs in a Lewis (electron dot) structure can be shown as dots, crosses, a dash or any combination.

• Allotropes of carbon (diamond, graphite, graphene, C60 buckminsterfullerene) and SiO2 should be covered.

• Coordinate covalent bonds should be covered.