CH-270
Giant covalent structures
Chemistry · Secondary 3 · Hard · Giant covalent structures
Which statement explains why graphite conducts electricity but diamond does not?
A) Graphite has ions that can move; diamond has no ions.
B) Graphite has delocalised electrons between layers; all electrons in diamond are used in covalent bonds.
C) Graphite is a metal; diamond is a non-metal.
D) Graphite has weak covalent bonds; diamond has strong covalent bonds.
A) Graphite has ions that can move; diamond has no ions.
B) Graphite has delocalised electrons between layers; all electrons in diamond are used in covalent bonds.
C) Graphite is a metal; diamond is a non-metal.
D) Graphite has weak covalent bonds; diamond has strong covalent bonds.
- Graphite has ions that can move; diamond has no ions.
- Graphite has delocalised electrons between layers; all electrons in diamond are used in covalent bonds.
- Graphite is a metal; diamond is a non-metal.
- Graphite has weak covalent bonds; diamond has strong covalent bonds.
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