GENERAL KNOWLEDGE

DIAMOND IS A BAD CONDUCTOR OF ELECTRICITY BECAUSE ITS BONDING ELECTRONS ARE USED IN

  • A. crystal lattice formation
  • B. covalent bond formation ✓
  • C. metallic bond formation
  • D. coordinate bond formation

 

The answer to the question is: B. covalent bond formation

In diamond, each carbon atom forms four strong covalent bonds with its neighboring atoms, creating a rigid three-dimensional structure known as a crystal lattice. In this structure, all the valence electrons are involved in forming these strong covalent bonds, leaving no free electrons to conduct electricity.

In contrast to metals, where the delocalized electrons are free to move and conduct electricity, diamond’s covalent bonds hold its electrons tightly in place within the crystal lattice. As a result, diamond does not conduct electricity under normal conditions.

In conclusion, diamond’s inability to conduct electricity is due to the utilization of its bonding electrons in covalent bond formation within the crystal lattice.

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