carbon electrode is made by using graphite explain
Answers
Answer:
In graphite, the carbon atoms are arranged in layers, retaining their structure through the use of covalent bonds. ... These electrons enable graphite to exhibit a high level of conductivity, explaining why the material is frequently used for electrodes.
Answer:
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.