Allotropes of carbon Flashcards
Describe the element of carbon
Carbon has 4 electrons in its outer shell, therefore it can form up to 4 covalent bonds, which makes it a very versatile element
What are allotropes
Different structural forms of the same element. The structure and bonding in different allotropes influences their properties and uses.
State some allotropes of carbon
Graphite and diamond
Describe the structure of diamonds
Each carbon atom is joined to four other carbon atoms by strong covalent bonds. the carbon atoms form a regular tetrahedral network structure. there are no free electrons.
What are the properties of diamonds
The rigid network of carbon atoms, held together by strong covalent bonds, makes diamond very hard. This makes it useful for cutting tools, such as diamond-tipped glass cutters and oil rig drills.
Do diamonds conduct electricity and do they have a high melting/ boiling point
Diamond has a very high melting point and it does not conduct electricity.
Describe the structure of graphite
each carbon atom forms three covalent bonds with other carbon atoms
the carbon atoms form layers of hexagonal rings
there are no covalent bonds between the layers
there is one delocalised electron from each atom
What are the properties of graphite
Graphite has delocalised electrons, just like metals. These electrons are free to move between the layers in graphite, so graphite can conduct electricity. This makes graphite useful for electrodes in batteries and for electrolysis.
The forces between the layers in graphite are weak. This means that the layers can slide over each other. This makes graphite slippery, so it is useful as a lubricant.
Can graphite conduct electricity
Graphite has delocalised electrons, just like metals. These electrons are free to move between the layers in graphite, so graphite can conduct electricity.
