Which statement best explains why Graphite conducts electricity among giant covalent structures?

Which statement best explains why Graphite conducts electricity among giant covalent structures?

• A. Graphite conducts electricity
• B. Diamond conducts electricity
• C. Silicon Dioxide conducts electricity
• D. None conduct electricity

Answer: (A)

Graphite conducts electricity because of its layered structure with delocalised electrons. Each carbon in a sheet forms three covalent bonds to neighbors, using three of its four valence electrons. The remaining electron is not tied to a specific atom and becomes free to move across the layer, so electric charge can flow through the material. This movement happens mainly within the layers, giving graphite its conducting property. In contrast, diamond is a giant covalent network where each carbon bonds to four others in a rigid 3D lattice, so all electrons are localized in bonds and there are no free carriers to move. Silicon dioxide also forms a giant covalent lattice with electrons locked in bonds, so it does not conduct. Hence graphite is the one that can conduct electricity.

Graphite conducts electricity because of its layered structure with delocalised electrons. Each carbon in a sheet forms three covalent bonds to neighbors, using three of its four valence electrons. The remaining electron is not tied to a specific atom and becomes free to move across the layer, so electric charge can flow through the material. This movement happens mainly within the layers, giving graphite its conducting property.

In contrast, diamond is a giant covalent network where each carbon bonds to four others in a rigid 3D lattice, so all electrons are localized in bonds and there are no free carriers to move. Silicon dioxide also forms a giant covalent lattice with electrons locked in bonds, so it does not conduct. Hence graphite is the one that can conduct electricity.