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Graphene And Fullerenes (GCSE Chemistry)

The following is a GCSE Chemistry test covering 'Graphene And Fullerenes' from the broader topic Bonding, Structure, And The Properties Of Matter. The test is geared towards the AQA exam board style syllabus.
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In a single layer of graphene each carbon atom is sp2 hybridised. What does sp2 hybridisation mean for the bonding?
Compared with diamond, graphene and graphite conduct electricity while diamond does not. What is the correct explanation?
Graphene is a single layer of carbon atoms arranged in a hexagonal (honeycomb) lattice. Which statement best describes its bonding and structure?
Which property of graphene is mainly due to the delocalised electrons in its structure?
Which property of fullerenes makes them useful as molecular cages in nanotechnology?
Fullerenes can be chemically modified by attaching other atoms or groups to the carbon cage. What is a likely effect of such functionalisation?
Which description best distinguishes graphene from graphite?
How does the strength-to-weight ratio of graphene compare to many conventional materials?
Why can graphene be used to make very thin, flexible electronic components?
How does the electrical conductivity of a single graphene sheet compare to that of bulk graphite?
Fullerenes such as C60 (buckminsterfullerene) are best described as: