The pictures below show the arrangement of the carbon atoms Key Stage 4 in diamond and graphite Carbon Copy In diamond, the carbon is arranged in a tetrahedral pattern, with Student worksheet each carbon being connected to four other carbons by covalent bonds. This is a very strong arrangement and explains why diamond is the hardest known natural substance. As a result, Spot the difference manufactured diamonds are used as hard-wearing coatings for The pictures above show diamond and graphite. Both of these drill bits and cutting blades. substances are made of the element CARBON. However they Although each layer of graphite has carbon atoms that are have very different properties. In the box below, list as many strongly covalently bonded to their neighbouring carbon atoms differences as you can between the two types of carbon. It may the bonds between the layers are weak. This means that the help to think about what they look like and how they are used. layers can slide over each other easily. This makes it ideal for its use in pencils where layers of graphite slide off the pencil onto the paper. It is also used in many lubricants. Because graphite only forms three covalent bonds rather than the four found in diamond, it contains electrons which are free to move within the graphite lattice. These free electrons, also found in the lattices of metal elements allow graphite to conduct electricity. Allotropes Some elements can exist in different structural forms. These Both diamond and graphite have a giant covalent structure in different forms are known as allotropes of that element. So which the carbon atoms are bonded with strong covalent bonds. graphite and diamond are allotropes of carbon. Molecular Structure Manufactured Allotropes of Carbon Although diamond and graphite are both made of carbon the way that the atoms are arranged in the two substances is Fullerenes completely different.
Key Stage 4 Carbon Copy Student worksheet Spot the difference The pictures above show diamond and graphite. Both of these substances are made of the element CARBON. However they have very different properties. In the box below, list as many differences as you can between the two types of carbon. It may help to think about what they look like and how they are used. Allotropes Some elements can exist in different structural forms. These different forms are known as allotropes of that element. So graphite and diamond are allotropes of carbon. Molecular Structure Although diamond and graphite are both made of carbon the way that the atoms are arranged in the two substances is completely different. The pictures below show the arrangement of the carbon atoms in diamond and graphite In diamond, the carbon is arranged in a tetrahedral pattern, with each carbon being connected to four other carbons by covalent bonds. This is a very strong arrangement and explains why diamond is the hardest known natural substance. As a result, manufactured diamonds are used as hard-wearing coatings for drill bits and cutting blades. Although each layer of graphite has carbon atoms that are strongly covalently bonded to their neighbouring carbon atoms the bonds between the layers are weak. This means that the layers can slide over each other easily. This makes it ideal for its use in pencils where layers of graphite slide off the pencil onto the paper. It is also used in many lubricants. Because graphite only forms three covalent bonds rather than the four found in diamond, it contains electrons which are free to move within the graphite lattice. These free electrons, also found in the lattices of metal elements allow graphite to conduct electricity. Both diamond and graphite have a giant covalent structure in which the carbon atoms are bonded with strong covalent bonds. Manufactured Allotropes of Carbon Fullerenes