APFIVE Electrical Conductivity of Network Covalent Solids
Pure network covalent solids, such as diamond, are known for their extremely high melting and boiling points. Which statement best explains the poor electrical conductivity of such network covalent solids?
A
The extended network structure forms a continuous sea of free electrons that are immobilized.
B
At high temperatures, network covalent solids become metallic despite their strong bonds.
C
The electrons are localized in strong, directional covalent bonds and are not free to move.
D
The presence of ionic impurities disrupts the conduction of electricity in network covalent solids.
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