Question

Select the correct option from the following:
A.Graphene is the atomic layer of graphite
B.Graphene is the atomic layer of composed of $s{p^2}$- hybridised carbon
C.Chemical bonds in graphite are similar in strength to that of diamond
D.All of these

Answer 1

Hint: Hybridisation: It is defined as the process of combining two or more atomic orbitals from the same atom to form a new orbital having different components.
Allotropes: They are defined as the different structure of the same element which shows quite different physical properties and chemical properties i.e. the atoms of an element are bonded together in different manner.

Complete step by step solution:
Let us first talk about allotropes.
Allotropes: They are defined as the different structures of the same element which show quite different physical properties and chemical properties i.e. the atoms of an element are bonded together in different manner. For example: carbon has allotropes i.e. graphite, diamond, fullerene.
Hybridisation: It is defined as the process of combining two or more atomic orbitals from the same atom to form a new orbital having different components.
In $s{p^2}$ hybridisation the mixing of one $2s$ orbital with two $2p$ orbitals takes place to form three hybrid orbitals.
Diamond: It is an allotrope of carbon in which carbon atoms are linked to each other to form three dimensional structure. The diamond is the hardest element which is known to us.
Graphite is an allotrope of carbon. Graphene is also an allotrope of carbon which is made of a single layer of atoms arranged in a two-dimensional structure. Graphene is the atomic layer of graphite. One single layer of carbons i.e. graphene in graphite is in hexagonal lattice. In graphene as well as in graphite the carbon atoms are hybridised. Chemical bonds (the bonds by which the different atoms of an element are connected) in graphite and in diamond are the same and of similar strength. But diamond is stronger than that of graphite because diamond is three dimensional structure while graphite is a two dimensional structure.
So, all the statements given in the question i.e. graphene is the atomic layer of graphite, graphene is the atomic layer of composed of $s{p^2}$- hybridised carbon and chemical bonds in graphite are similar in strength to that of diamond all are correct.

Hence option D is correct.

Note: The number of hybrid orbitals after hybridisation is equal to the number of orbitals which takes part in the hybridisation. For example: in $s{p^3}$the orbitals which take part in the hybridisation is four. So the number of hybrid orbitals formed will be four.