Diamond is a bad conductor of electricity because its bonding electrons are used in
crystal lattice formation
covalent bond formation
metallic bond formation
coordinate bond formation
Explanation
Video Explanation
Post your Contribution
Discussions (8)
As we know diamond is a giant covalent structure i.e. each carbon atom is covalently bonded with other carbon atoms. So the four outermost electrons, four carbon atoms, are engaged or trapped in the covalent bonds which means that there are no free electrons. ... So diamond is a bad conductor of electricity.
They are very correct because as we know diamond is a giant covalent structure where each carbon atoms are bounded to another carbon atoms and the have no free electrons
There should be a review of the question because in the Formation of the Carbon allotropes, Diamond cant conduct electricity based on its crystal lattice formation!
