What everyone needs to know:
Ionic bonds are formed between metals and non-metals in a compound. Covalent bonds are formed with non-metals only. Metallic bonding is present in metals and alloys. You need to explain these bonds in terms of electron transfer and sharing.
Ionic compounds have specific properties such as high melting points, they are usually soluble and only conduct electricity if they are melted or dissolved in water (as they need free moving ions to conduct). They are held together by strong electrostatic forces.
Covalent molecules are also called simple molecules. This is because despite having very strong covalent bonds between the atoms, they have very weak intermolecular forces between molecules giving them very low melting ad boiling points. You need to be able to draw dot and cross diagrams for their structures.
In metallic bonding, you need to describe the regular arrangement of ions (remember that there are no atoms in metal, they are all ions) surrounded by the delocalised electrons (sea of electrons). This explains why metals can conduct both heat and electricity.
You need to describe the properties of polymers, giant covalent structures including the allotropes of carbon and different alloys (how adding different sized atoms can change the strength etc).
Linking to these properties, you need to understand the models of solids, liquids and gases. Accurately sue state symbols.
Extra topics needed for the Higher papers:
For this, you need to be able to explain the limitations of the models we use for solids liquids and gases, for example, there are no forces between the molecules in this model and that the particles are shown as perfect spheres that do not change shape at all.
What is being taught week by week: