Types Of Structures
Simple Covalent (Ammonia NH3)
Properties
Don't conduct electricity because they don't have delocalized electrons that can flow through the structure.
They have low melting and boiling points as they have weak intermolecular forces which lets them break down easily
Giant Covalent
Proporties
Very high melting point because of the strong covalent bonds within the atoms in the structure.
Some conduct electricity if they contain delocalized electrons. For example, graphite has them but diamond doesn't so graphite can conduct electricity
Graphite
Diamond
Diamond is one of the forms of carbon as each carbon atom is connected to four other carbon atoms.
Diamond doesn't conduct electricity and is a very hard material.
Diamond is used for cutting tools at it is so hard. It's also used for jewelry as it is very nice and shiny and almost can't break.
It does conduct electricity and is used for penciles as when the layers slide over each other they can slide off and that's how the graphite rubs off on the paper.
Each carbon atom in a layer is joined to only three other carbon atoms.
Graphite is one of the forms of carbon as the layers can slide over each other since it has delocalized electrons.
Sand (Silicon Dioxide)
Very similar properties to diamond but is not as hard or strong.
Its is made up of silicon and oxygen which isn't like diamond which has only carbon.