Graphite consists of planes of carbon atoms. Between atoms in the planes there are only weak forces. What kind of elastic properties do you expect from graphite ?

What is the state of hybridisation of carbon atoms in graphite ?

Graphite has h.c.p arrangements of carbon atoms and the parallel planes are 3.35 Å apart . Determine density of graphite :

Consider following statements: (I): In diamond, each carbon atom is linked tetrahedrally to four other carbon atoms by sp^(3) bonds. (II): Graphite has planar hexagonal layers of carbone atoms held together by weak Van der Waals forces. (III): Silicon exists only in diamonds structure due to its tendacy to form p pi- p pi bonds to itself. In this.

Consider following statements : I: In diamond, each carbon atom by sp^(3) bonds II : Graphite has planar hexagonal layers of carbon atoms held together by weak van der Walls forces III: Silicon exists only in diamond structure due to its tendency to from p pi-p pi bonds to itself. In this:

Conidier following statements : I : In diamond, each carbon atom is linked tetrahedrally to four other carbon atoms by sp_(3) bonds. II : Graphite has planer hexagonal layers of carbon atoms held together by weak vander Walls forces III : Silicon exists only in diamond structure due to its tendency to form p_(p)-p_(p) bonds to itself. In this :

PASSAGE-I : Diamond and graphite are two allotropic forms of carbon which are crystalline in nature. They differ physically but chemically they are similar. Diamond is the hardest crystalline form of carbon. In diamond each carbon atom is linked to four other carbon atoms by covalent bonds. In graphite, each carbon atom is linked to three other carbon atoms by covalent bond. Graphite is relatively soft and greasy. It is a good conductor or electricity. Which of the folowing types of forces bind together the carbon atoms in diamond?

In which of the following structures the pair of starred carbon atoms do not lie in the same plane?