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Diamonds & Graphite
Diamonds & Graphite


Comparing the properties of diamonds and graphite provides clues as to where diamonds originate. Graphite forms close to the surface of the earth. The fact that diamond’s crystalline structure is more compact than that of graphite implies that they form in deeper environments where pressure and temperature is higher.

Production of synthetic diamonds has aided geologists in determining the origin of the diamond. An experiment was done to prove the hypothesis that diamonds must have been formed in much deeper environments than graphite. As these synthetic diamonds were being produced, they were subjected to high pressure and temperature. The result was as follows:

In the production of diamond and graphite, pressure conditions must increase along with the increase of temperature. The difference between the two is that lower temperatures are more conducive for the formation of the diamond and higher temperatures are more conducive for the formation of graphite.

In truth, diamonds could actually be converted to graphite. If diamonds are subjected to heat where oxygen is not present, it will eventually convert into graphite. Such conditions only occur in a vacuum or in a lifeless atmosphere. Depending on the quality of diamond, this process of conversion should take place between 1073º - 1973º Kelvin. The process initially takes place at a slow course when only a thin layer of the diamond is affected. After this initial process, rapid conversion to graphite takes place and the whole diamond eventually become graphite in powdered form. This comes about at around 1973º Kelvin.

Graphite is known as the stable form of crystalline carbon and, conversely, diamond is the unstable form. Diamond’s instability is revealed in normal temperatures and pressure conditions. Thus, given the temperature of 1973º Kelvin, the rate of transition of diamond to graphite is quick. At room temperature, however, this process is not possible.

Furthermore, knowing the properties of both minerals, it should also be possible for graphite to be converted to diamonds. Graphite has a hexagonal internal structure with carbon found in flat hexagonal rings in sheets, with loose bonds between the sheets. On the other hand, diamond has a three-dimensional structure with no loose bonds. Therefore, in theory, creating a condition wherein the hexagonal rings of its carbon atoms take the arrangement like that of diamonds would create diamonds out of graphite since the internal structure is the only difference between the two. To make this possible, graphite has to be compressed for the rings of its carbon atoms to take the form of the three-dimensional atomic structure of diamonds. For the atoms to retain its new atomic structure even after the release of compressional pressure, it has to be subjected to high temperatures. After this, graphite should have turned into diamond. However, this is merely stated in theory. Performing it is not as simple as it is written.
By: boredumb
Published: 02/18/08


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