Question

With reference to graphite and diamond, which of the statement(s) given below is (are) correct? (This question has multiple correct options)
a.) Graphite is hard than diamond
b.) Graphite has higher electrical conductivity than diamond
c.) Graphite has higher thermal conductivity than diamond
d.) Graphite has higher $C-C$ bond order than diamond

Answer 1

Hint: As the formation of graphite and diamond tells about allotropes. Where Allotropy is the property of an entity that appears in more than one physical form with identical chemical properties but different physical properties. Carbon occurs in both crystalline and amorphous allotropic forms. Crystalline allotropic carbon: diamond, graphite and fullerene. Amorphous allotropic carbon: coal, coke, lamp black, gas and coke.

Complete step by step answer:
Here is the reason for all the option mentioned in the question:
(A) Diamond is harder than graphite.
(B) In graphite, each atom is joined to 3 others $C$ atoms leaving one free valence which ends up in electrical conductance. In diamond, all four valences of carbon are satisfied thanks to which diamond is an insulator.
Thus, graphite has higher electrical conductivity than diamond.
(C) Diamond has higher thermal conductivity than graphite because of the transfer of thermal vibrations from atom to atom. Diamond incorporates a compact and precisely aligned crystal which helps within the fast movement of warmth.
(D) Graphite includes a higher $C-C$ bond order than diamond.
Graphite contains $C=C~$ covalent bond whereas diamond contains $C-C$ single bond only.
So, the correct answer is “Option B and D”.

Note: As Allotropes are different structural varieties of the identical element and might exhibit quite different physical properties and chemical behaviours. The change between allotropic forms is triggered by the identical forces that affect other structures, i.e., pressure, light, and temperature.