1.6: Giant Covalent Structures – Graphite, Diamond, and Silicon Dioxide Flashcards
Q: What is the structure of diamond?
A: Diamond has a 3D lattice where each carbon atom is covalently bonded to four others.
Q: Why is diamond extremely hard?
A: The strong covalent bonds in its rigid structure make diamond very hard.
Q: Why doesn’t diamond conduct electricity?
A: Diamond lacks free electrons or ions to carry an electric current.
Q: Why is graphite a good conductor of electricity?
delocalized
A: Graphite has delocalized electrons that move freely between layers.
Q: What is the structure of graphite?
A: Graphite has layers of carbon atoms arranged in hexagonal rings, with one free electron per atom.
Q: Why is graphite a good lubricant?
slide due to…
A: The layers in graphite can slide over each other due to weak forces between them.
Q: What is silicon dioxide (SiO₂)?
A: Silicon dioxide is a giant covalent structure where each silicon atom is bonded to four oxygen atoms.
Q: How is the structure of SiO₂ similar to diamond?
tetrehedral arrangement of… and strong…
A: Both have a tetrahedral arrangement of atoms and strong covalent bonds.
Q: Why do both diamond and SiO₂ have high melting points?
A: The strong covalent bonds in their structures require a lot of energy to break.
Q: Why is SiO₂ used in glass-making?
A: Its hardness and high melting point make it ideal for durable materials like glass.
