Final answer:
The student asks about transforming the carbon structure of diamond into graphene for its superior electrical conduction. The conversion from diamond to graphite (graphitization) occurs slowly at high temperatures and graphene can subsequently be isolated from graphite. Graphene is desired for many advanced technological applications due to its strength and electrical properties.
Step-by-step explanation:
Conversion of Carbon Allotropes
The student is inquiring about the possibility of converting the carbon atoms in diamond into graphene to utilize its excellent electricity conducting properties. Diamond and graphite are two well-known allotropes of carbon which have vastly different properties. Diamond has a three-dimensional network of strongly bonded carbon atoms making it extremely hard, while graphite is composed of layers of carbon atoms arranged in a hexagonal structure, which makes it soft and slippery. Graphene, a one-atom-thick layer of graphite, has been discovered to be an exceptional conductor of electricity and heat. It's also very strong and lightweight.
The process of transforming diamond into graphite is known as graphitization, which is spontaneous at ambient pressure but occurs at an immeasurably slow rate at low to moderate temperatures. To observe this process within a practical timeframe, temperatures in the range of 1000-2000 K are required. Once graphite is formed, it may potentially be converted to graphene by peeling off layers using methods such as the one developed by Nobel laureates Andre Geim and Konstantin Novoselov in 2004.
Graphene's potential applications include vastly improved computer chips, better batteries and solar cells, and stronger, lighter structural materials due to its impressive properties.