Question

Explain the difference in the properties of diamond and graphite on the basis of their structure.

Answer 1

Hint: Diamond is formed due to covalent bonds which forms a strong three-dimensional network whereas graphite is formed due to cohesive forces like Van der Waals force which is a weak force of attraction. Thus, graphite is formed of flat carbon atoms layers one upon another. These carbon atoms layers form a slippery surface over each other, giving graphite its soft nature.

Complete answer:
Graphite is a crystalline form of the element carbon with its atoms arranged in a hexagonal structure. It occurs naturally in this form and is the most stable form of carbon under standard conditions. Under high pressures and temperatures it converts to diamond. Graphite is used in pencils and lubricants. It is a good conductor of heat and electricity. Its high conductivity makes it useful in electronic products such as electrodes, batteries, and solar panels.
Diamond is a solid form of the element carbon with its atoms arranged in a crystal structure called diamond cubic. At room temperature and pressure, another solid form of carbon known as graphite is the chemically stable form of carbon, but diamond almost never converts to it. Diamond has the highest hardness and thermal conductivity of any natural material, properties that are utilized in major industrial applications such as cutting and polishing tools.

Note:
Graphite occurs in metamorphic rocks as a result of the reduction of sedimentary carbon compounds during metamorphism. It also occurs in igneous rocks and in meteorites. Natural, synthetic and imitation diamonds are most commonly distinguished using optical techniques or thermal conductivity measurements.