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Forms of Carbon/Carbon Altropes

Carbon is the 6th element in the periodic table, and it can form many different allotropes, these are 3 examples of them-Diamond,graphite and Buckminster Fullerene(C    ). All of these 3 carbon alltropes, the carbon atoms are joined together to form strong covalent bonds, however they are arranged differently which gives them different properties.

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Similarities (Diamond and Graphite):
-Both are made out of carbon
-Giant covalent structures
-High melting and boiling points
-Insoluble in water
                                      Differences: 
          Diamond                                         Graphite
-Each carbon atom is bonded   -Each carbon atom is bonded 
to 4 other carbon atoms            with 3 other carbon atoms
-Due to its tetrahedral and        -Layers of hexagonaly
rigid structure it is very hard     arranged carbon atoms can 
                                                    slide off each other easily-Soft
-Insulator, does not conduct     -Good conductor of heat and
heat and electricity(All 4            electricity(Only 3 carbon 
carbon atoms are used in the   atoms are used in the bond, 
covalent bond)                           the remaining electrons can
                                                    delocalize across the carbon
                                                    atom 
-Density:3.51 gm/cm                  -Density:2.266 g/cm
-Shiny and transparent              -Dull and opaque
-Tetrahedral arrangement         -Hexagonal arrangement

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Uses:
Diamond:
     -Because it is so hard, it is used in cutting tools
     -Drilling holes through rocky layers of the ground for oil
     -Surgeons use sharp ended diamonds to remove cataracts from the eyes 
Graphite:
     -It's used in pencil leads because it slips easily off the pencil onto the paper and leaves a black mark, this is because the layers can slide off each other easily
    -Due to its slippery nature it is also used in lubricants
    -Since it has a high melting point and is a good conductor of electricity, it is also used as electrodes in electrolysis
Diamond
Graphite
Inter-molecular Forces:
Diamond:There are no intermolecular forces acting on diamond because each carbon atom is linked to 4 other carbon atoms;It is bounded by strong intramolecular forces rather than inter-molecular forces.
Graphite:The graphite layers stack due to weak intermolecular forces(van de Waals force), this is because there are no bonds that hold the layers together
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