The weak attractive forces present in graphite are called:
(A) gravitational forces
(B) van der waal forces
(C) coulombic forces
(D) repulsive forces

Hint:Solid carbon comes in different forms which are known as allotropes of carbon depending on the type of chemical bond between them. The most common of them are diamond and graphite.

Complete step by step answer:
Graphite occurs in crystalline form in which the arrangement of the atoms is hexagonal structure. It occurs naturally in this form and under the standard temperature and pressure conditions, it is the most stable form of carbon. Under high pressures and temperatures, Graphite transforms into diamond.
The carbon atoms in Graphite tend to have stable chemical bonds with the other three carbon atoms, hence making the sheets appear like a chicken wire, they are held together by the weak forces of the covalent bond.
The carbon atoms of Graphite show $s{p^2}$ hybridized and are arranged in the same plane hence they form hexagonal rings. The rings have many layers of particles. There are two forms of graphite $\alpha $ (alpha) and $\beta $ (beta).
These two forms are interconvertible and show the same physical properties. The short-range electrostatic attractive forces that are present between uncharged molecules, which arises from the interaction of permanent electric dipole moments. The weak forces between the covalent bonds in graphite are van der Waals forces.
Graphite is a good conductor of heat and electricity. Its high conductivity due to the presence of a free-electron that conducts electricity.
Hence, The weak attractive forces present in graphite are called Van der waal forces.

Therefore, Option (B) is correct.

Note:
The powder of Graphite is used as a lubricant in the form of dispersion material or powder. It is also widely used in lead pencils. It is used in the manufacture of electrodes of carbon employed in the electrolytic cells.