Diamond is a giant covalent network structure, having each Carbon atom sharing electrons with four other Carbon atoms, therefore having four single covalent bonds formed. These Carbon covalent bonds are extremely strong and account for two of diamond’s most prominent physical properties among all elements, hardness and a high melting point.

Diamond has a high melting point due to the fact that diamond is a covalent lattice, hence, melting this covalent lattice involves breaking many strong covalent bonds. This melting process requires a large amount of energy and, as a result, melting diamond requires a high temperature, approximately around 35500C.

Having strong covalent bonds, diamond also has a high level of hardness due to the fact that it is extremely difficult to break the strong covalent bonds within the covalent lattice. In fact, diamond is the hardest natural substance on earth, and for this reason it is used industrially to polish drill, cut or wear away any......

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Title: Account For The Different Physical Properties And Uses Of Diamond, Graphite And The Fullerene You Have Chosen, In Terms Of Bonding.
Approximate Word Count: 869
Approximate Pages: 4 (250 words per double-spaced page)

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