Question

Graphite is used in making electrodes because:
A.) It has high melting point
B.) It is soft and slippery
C.) It is a good conductor of electricity
D.) None of these

Answer 1

Hint: We know that graphite is an organic compound. The atomic structure of graphite results in a large number of electrons not being bonded.

Step by step solution:
Graphite is simply an allotrope of carbon.
We know that graphite has a large number of electrons which are not bonded, which migrate between the layers of graphite. And the large number of free electrons (electron delocalization) that give graphite its excellent conductive properties.
Another reason for using graphite as an electrode is that it is a good conductor, cheap, robust and easily accessible.
Graphite bonds are formed of only three out of the four valence electrons of carbon, leaving the fourth electron to move freely. These electrons enable the electrolysis process to progress smoothly.
It is stable at high temperature means it has a high melting point. Carbons in graphite create layers. And there is no covalent bond between the layers. The layers though have a van der waal’s attraction force between them, which is very weak and lets the layers slide over each other very easily.
So, from all above points we can conclude that option “C” is correct. All other options as a property of graphite are correct but not the reason for making electrodes, only reason is good conductor.

Note: There are other materials which can be formed from graphite are crucibles, which is a ceramic or metal container in which metals or other substances may be melted or subjected to very high temperature. There can be any number of carbons in graphite.