Network Solids and Carbon: Crash Course Chemistry

The video explores the differences between graphite and diamond, both made of carbon but with distinct properties due to their atomic structures. Graphite's layered structure allows it to conduct electricity and act as a lubricant, while diamond's rigid 3D network makes it extremely hard but brittle. The video also discusses how heat and pressure can transform graphite into diamond, highlighting the role of covalent bonds and atomic arrangements in determining material properties.

How do the electrical properties of diamond differ from those of graphite?

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In what ways do the covalent bonds in network solids affect their thermal conductivity?

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Discuss the significance of the arrangement of chemical bonds in determining the characteristics of materials.

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