Explain why elements and compounds can be classified as:

a) ionic
b) simple molecular (covalent)
c) giant covalent
d) metallic

and how the structure and bonding of these types of substances results in different physical properties, including relative melting point and boiling point, relative solubility in water and ability to conduct electricity (as solids and in solution)

Explain the properties of ionic compounds limited to:

a) high melting points and boiling points, in terms of forces between ions
b) whether or not they conduct electricity as solids, when molten and in aqueous solution

Explain the properties of typical covalent, simple molecular compounds limited to:

a) low melting points and boiling points, in terms of forces between molecules (intermolecular forces)
b) poor conduction of electricity

Recall that graphite and diamond are different forms of carbon and that they are examples of giant covalent substances

Describe the structures of graphite and diamond

Explain, in terms of structure and bonding, why graphite is used to make electrodes and as a lubricant, whereas diamond is used in cutting tools

Explain the properties of fullerenes including C₆₀ and graphene in terms of their structures and bonding

Describe, using poly(ethene) as the example, that simple polymers consist of large molecules containing chains of carbon atoms

Explain the properties of metals, including malleability and the ability to conduct electricity

Describe the limitations of particular representations and models, to include dot and cross, ball and stick models and two- and three-dimensional representations

Describe most metals as shiny solids which have high melting points, high density and are good conductors of electricity whereas most non-metals have low boiling points and are poor conductors of electricity