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Diamond

Which of the ...

Question

Which of the following types of forces bind together the carbon atoms in diamond?

A

Van der Waals forces

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B

Ionic

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C

Covalent

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D

Dipolar

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Solution

The correct option is C Covalent
Diamond is a covalent crystal. In diamonds, each carbon atom is $s p^{3}$ hybridized and strongly bonded to four adjacent carbon atoms located at the apices of a tetrahedron (a three-sided pyramid). The four valence electrons of each carbon atom participate in the formation of very strong covalent bonds. These bonds have the same strength in all directions. This gives diamonds their great hardness.

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Q. Forces that bind atoms in diamond are :

Q. Consider the following statements
I : In diamond, each carbon atom is linked tetrahedrally for four other carbon atoms by

{s p}^{3}

bonds.
II : Graphite has planar hexagonal layers of carbon atoms held together by weak Van der Waal's forces.
III : Silicon exists only in diamond structure due to its tendency to form

p π - p π

bonds to itself.

Q. Fullerene, an allotrope of carbon, has 60 carbon atoms joined together and no other element in it. There are various types of fullerenes.

C_{60}, C_{70}, C_{74}

C_{78}

are the members of the fullerene family. Identify the property due to which such large numbers of carbon atoms are joined together in this molecule :

Q. In a crystal of diamond:
(i) How many carbon atoms are present per unit cell?
(ii) What type of lattice does diamond crystallize in?
(iii) How many carbon atoms surround each carbon atom?
(iv) How are they arranged?

Q. Which of the following types of carbon atoms possess the highest electronegativity?

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