Question
Graphite is a soft solid lubricant extremely difficult to melt. The reason for this anomalous behaviour is that graphite
A.
is an allotropic form of diamond
B.
has molecules of variable molecular masses like
polymers
C.
has carbon atoms arranged in large plates of rings of
strongly bound carbon atoms with weak interplate
bonds
D.
is a non-crystalline substance
Answer :
has carbon atoms arranged in large plates of rings of
strongly bound carbon atoms with weak interplate
bonds
Solution :
In graphite, carbon is $$s{p^2}$$ hybridized. Each carbon is thus linked to three other carbon atoms forming hexagonal rings. Since only three electrons of each carbon are used in making hexagonal ring, fourth electron of each carbon is free to move. This makes graphite a good conductors of heat and electricity. Further graphite has a two dimensional sheet like structure. These various sheets are held together by weak van der Waal’s force of attraction. due to these weak forces of attraction, one layer can slip over the other. This makes graphite soft and a good lubricating agent.