Graphite is a soft solid lubricant extremely difficult to melt. The reason for this anomalous behavior is that graphite:
A) has molecules of variable molecular masses like polymers.
B) has carbon atoms arranged in large plates of rings of strongly bound carbon atoms with weak inter plate bonds.
C) is a non-crystalline substance
D) is an allotropic form of diamond

Hint: In the given question graphite shows the anomalous behavior which can be described as a property of an element that shows the deviation from its original properties and shows the different behavior of an element from its normal behavior. One can use this concept for the graphite element and analyze the options which relate to the anomalous behavior of the graphite.

Complete step by step answer:
1) first of all we will learn about anomalous behavior and the reasons which lead a molecule to that behavior. Anomalous behavior can be described as a property of an element that shows the deviation from its original properties and shows the different behavior of an element from its normal behavior. The reasons for that behavior are the exceptionally small size of the elements atom and ion and another is high polarizing power.
2) Now let's analyze the element graphite in which the structure of graphite is a layered structure which is held by Van der Waals forces and each layer is formed due to planar hexagonal rings of a carbon atom which forms three sigma bonds with the three neighboring carbon atoms, the fourth electron contributes in $\pi - $bond.
3) The carbon atoms present in the graphite structure form a two-dimensional sheet-like structure. The graphite structure is less compact than the structure of the diamond. Hence, it is not an allotropic form of diamond which shows option D is incorrect.
4) The given options A and C are also incorrect as discussed above.

Option B is a correct choice which indicates the graphite has carbon atoms arranged in large plates of rings of strongly bound carbon atoms with weak inter plate bonds.

Note:
The graphite is made up of only carbon atoms and its structure depends on the arrangement of carbon atoms. The carbon atom in graphite is $s{p^2}$ hybridized and it is a thermodynamically more stable structure than diamond at an ordinary temperature. In graphite, the high electrical conductivity through its structure is due to the presence of delocalized $\pi - $ electron present.