Question

(a) Write two points of difference in the structures of diamond and graphite.
(b) Explain why graphite can be used as a lubricant but diamond cannot.
(c) State the two properties of carbon which led to the huge number of carbon compounds.
(d) Both carbon and silicon belong to Group 14 of the periodic table.
But the tendency to exhibit catenation in carbon is much more than silicon. Explain.

Answer 1

3. It is used as lubricant because it's soft

Answer 2

a) The high quanity of bonds : surface area ratio makes both carbon and diamond very
strong. Differences 1. Diamond: each carbon atom bonds to 4 other carbon atoms, WHILST,
Graphite: each carbon atom bonds to 3 other carbon atoms. ... Therefore, diamond has a
higher boiling point.

b) Graphite is used as a lubricant due to its slippery nature. Graphite has layers of carbon
atoms, with weak forces, residing in between its layers because of which it is quite slippery.

c) The two features of carbon that give rise to a large number of compounds are as follows: (i)
Catenation − It is the ability to form bonds with other atoms of carbon. (ii) Tetravalency −
With the valency of four, carbon is capable of bonding with four other atoms.

d) Both carbon and silicon belong to group 14 of the periodic table. But the tendency to
exhibit catenation in carbon is much more than in silicon. ... As a result, any number of
carbon atoms can be linked to each other resulting in a large number of carbon
compounds.