The forms of carbon
Diamond and graphite are both made of carbon, however, their structure are really different, below are the difference and similarities between them.
physical & chemical
properties
diamond
-Shiny
-Colorless (Transparent)
-Hard
-High melting/boiling point
-Insoluble
-Doesn't conduct electricity
Diamond has a giant molecular structure. Every atom is link to each other, and doesn't conduct electricity because there is no space for electrons to move since all atoms are linked together, it also makes it hard so it can be a useful cutting tool, such as drill.
graphite
-Shiny
-Black (Not Transparent)
-Soft
-High melting/boiling point
-Insoluble
-Conducts electricity
Graphite has a giant molecular structure, it is made of layers of carbon atoms, which is not really strong compared to diamond, and so it is easier to break down. Within these layers, they contain free electrons, therefore it conducts electricity. Since it can be broken down easily, it can be a writing tool such as pencil.
inter-molecular force
Diamond doesn't have any intermolecular forces because all atoms are linked together and no distance between molecules.
Graphite has weak intermolecular force, it is because it is made of layers of atoms, and the force of attraction is weak.
sources:
-Nanochemistry. (n.d.). Retrieved December 31, 2016, from http://www.bbc.co.uk/schools/gcsebitesize/science/add_gateway_pre_2011/chemical/nanochemistryrev1.shtml
-Allotropes of carbon and nanochemistry. (n.d.). Retrieved December 31, 2016, from http://www.bbc.co.uk/schools/gcsebitesize/science/add_ocr_gateway/chemical_economics/nanochemistryrev1.shtml