The extremely high melting point of diamond (carbon) may be explained by the
A
Network covalent bond
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B
Ionic bond
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C
Hydrogen bond
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D
Van der Waal's forces
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Solution
The correct option is A
Network covalent bond
Explanation for correct option:
A. Network covalent bond
Diamond has a crystalline structure.
Diamond has a covalent structure in which each carbon atom is bonded to four other carbon atoms via covalent bonds.
It has the highest hardness as well as high thermal conductivity.
A lot of energy is needed to detach the atoms in a diamond as there is strong covalent bonding due to which the melting, as well as the boiling point of the diamond, is very high.
The covalent bonding in diamonds is given below:
Explanation for incorrect options:
B. Ionic bonds are formed from the electrostatic attraction between oppositely charged ions in a chemical compound.
C. Hydrogen bond is the attraction between hydrogen and a more electronegative atom than hydrogen.
D. Van der Waal's forces are weak intermolecular attractions.
Thus, the other options B, C, and D stand incorrect.
Hence, the correct option is A. The extremely high melting point of diamond (carbon) may be explained by the network covalent bond.
