Question

Which of the following models best describes the bonding within a layer of the graphite structure?
A. Metallic bonding
B. Ionic bonding
C. Non-metallic covalent bonding
D. Van der Waals forces

Answer 1

Graphite is a compound which is purely made from only carbon atoms. In graphite, each carbon is attached to three different carbon atoms. Carbon is a non-metallic compound and will bond with itself as the non-metal does.

Complete step by step answer:
- Graphite is used widely in every area, it is used in our household as well. It is a compound purely made of a carbon atom. It is a network of giant covalent structures. In its structure, where there is only carbon involved, each carbon atom is bonded with three different carbon atoms due to covalent bonding. Now, going on the carbon atom on joining with each other forms hexagonal arrangements, producing layers of hexagonal structures. Now, in between the layers, there is a weak force of attraction which holds them together.
- Since each carbon atom has four electrons in its valence shell, and we have connected each carbon atom with only three carbon atoms, hence one electron remains non-bonded. Now, this non bonded electron becomes delocalised.
- This delocalized electron acts the same as the free electrons in metal resulting in conductivity of electricity through graphite. Therefore, graphite is used as an electrode in electrolysis and batteries. We also observe that when you touch graphite it feels slippery, this is because the weak force of attraction between the layers of graphite which leads them to become slippery.
Now from the above explanation of graphite, we can say that graphite has non-metallic covalent bonding.

So option C is correct.

Note:
There is a huge range of compounds made only out of carbon atoms, this is because carbon can bond to four monovalent atoms or four other carbon. Therefore changing the arrangement of these carbons leads to forming various compounds such as diamond, coal etc.