Diamond as a Carbon Allotrope (Essay Sample)

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Carbon is atomic number six with an atomic arrangement of 2, 4. The arrangement carbon atoms in the lattice and the bonds formed determine the type of structure that result. Carbon exists in different forms called allotropes. (Carmichaelp p. 17) These include: graphite, diamond and amorphous carbon. The carbon form is determined by the type of bonds that exist between the atoms. In diamond, each atom shares electrons with four other atoms. Each atom has four electrons in the outermost energy level; it therefore requires four other electrons when bonding. By sharing an electron with each atom in the bond, the outer energy level is filled up with electrons (Holman et al p.77). The result is the formation of four single bonds as shown below:
Figure SEQ Figure \* ARABIC 1: Covalent bonds in diamond
Figure 1 shows only a small portion of the structure in diamond. This type of structure is referred to as a giant covalent bond. The structure continues indefinitely in three dimensions. Bonds joining the atoms are called covalent bonds. They are very strong bonds and very strong structures result from these bonds (Carmichaelp p. 17&37). The atoms in the lattice are arranged regularly giving the diamond crystals their regular shapes. Diamond has the following physical characteristics: Very high melting point (4000oC). The strong covalent bonds must be broken first for it to melt. Diamond is very hard and is insoluble in water and organic solvents (Carmichaelp p. 19). Diamond does not conduct electricity (there are no free electrons in the lattice which would conduct electricity) (Holman et al p.77). Diamond has several uses. Among them are:
* It is used to make drilling bits and precision and glas...