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.

What is the primary reason for the difference in hardness between diamond and graphite?

• The arrangement of their atomic networks

• The temperature at which they are formed

• The type of carbon atoms they contain

• The presence of impurities

How do network solids differ from other types of atomic solids?

• They are made of molecules

• They are made of ions

• They consist of atoms linked in a network

• They are not stable

What role do atomic orbitals play in the properties of network solids?

• They determine the color of the solid

• They affect the hybridization and bonding properties

• They influence the melting point

• They have no effect

Which type of hybridization is found in the carbon atoms of graphite?

• sp3 hybridization

• sp2 hybridization

• sp hybridization

• sp4 hybridization

Why is graphite a good conductor of electricity?

• It has free-moving electrons in pi bonds

• It contains metal atoms

• It has a crystalline structure

• It has a high density

What conditions are required to transform graphite into diamond?

• High temperature and high pressure

• High temperature and low pressure

• Low temperature and low pressure

• Low temperature and high pressure

Why is it difficult for diamonds to naturally transform into graphite?

• The activation energy required is too high

• Graphite is unstable

• Diamonds are not made of carbon

• Graphite cannot exist on Earth