C2.3.3 Properties of Giant Covalent Structures

• Giant covalent structures form a continuous lattice where each atom is bonded to multiple neighbors


  True
• Giant covalent structures have high melting and boiling points due to the strong covalent bonds
• Match the giant covalent structure with its properties:

  Diamond ↔️ Extremely hard, thermal conductor, electrically insulating

  Graphite ↔️ Soft, good electrical conductor, lubricates surfaces

  Silicon Dioxide ↔️ Hard, chemically inert, high melting point
• The absence of free electrons in most giant covalent structures leads to electrical insulation
• All giant covalent structures are electrical insulators.

  False
• Giant covalent structures have a vast network of atoms held together by strong covalent bonds
• Giant covalent structures are hard because their strong covalent bonds require significant energy to break.


  True
• Diamond has a melting point above 3550
• Graphite is a good electrical conductor because it has mobile electrons between layers.


  True
• Common examples of giant covalent structures include diamond, graphite, and silicon dioxide
• What are the properties of diamond?

  Extremely hard, excellent thermal conductor, electrically insulating
• Why is graphite a good electrical conductor?

  Delocalized electrons
• Steps involved in explaining the high melting and boiling points of giant covalent structures:

  1️⃣ Strong covalent bonds form a continuous lattice

  2️⃣ Significant energy is required to break these bonds

  3️⃣ High temperatures are needed to melt or boil the substance
• Giant covalent structures have low melting and boiling points.

  False
• Why do giant covalent structures have high melting and boiling points?

  Strong covalent bonds
• Graphite conducts electricity due to delocalized electrons.


  True
• What type of bonds must be broken to melt or boil a giant covalent structure?

  Strong covalent bonds
• Silicon dioxide has a melting point of 1713°C.
• Why is graphite an exception to the electrical insulation rule in giant covalent structures?

  Delocalized electrons
• Match the giant covalent structure with its electrical conductivity:

  Diamond ↔️ Insulator

  Graphite ↔️ Conductor
• What are the uses of graphite?

  Pencils, lubricants, electrodes
• Giant covalent structures are substances with a large lattice composed of strong covalent bonds
• What is a key property of giant covalent structures regarding electrical conductivity?

  Most are insulators
• Name two real-life examples of giant covalent structures.

  Diamond and graphite
• Giant covalent structures have high melting and boiling points because strong covalent bonds require significant energy to break.


  True
• Why are the melting and boiling points of giant covalent structures high?

  Strong covalent bonds
• Arrange the following giant covalent structures in order of increasing electrical conductivity:

  1️⃣ Diamond

  2️⃣ Silicon Dioxide

  3️⃣ Graphite
• What is the primary reason for the hardness of giant covalent structures?

  Robust covalent networks
• What type of bonding is present in giant covalent structures that contributes to their high melting and boiling points?

  Strong covalent bonds
• Match the giant covalent structure with its structure:

  Diamond ↔️ Tetrahedral lattice

  Graphite ↔️ Layers of hexagonal rings

  Silicon Dioxide ↔️ Three-dimensional network
• What defines a giant covalent structure?

  Large lattice of strong bonds
• Diamond has a tetrahedral lattice structure.


  True
• Match the substance with its structure:

  Diamond ↔️ Tetrahedral lattice

  Graphite ↔️ Layers of hexagonal rings

  Silicon Dioxide ↔️ Three-dimensional network
• Silicon dioxide is used in the production of glass, ceramics, and electronic components
• What characteristic of giant covalent structures contributes to their thermal stability?

  High bond strength
• Giant covalent structures are generally electrical insulators, except for graphite
• What property of giant covalent structures requires significant energy to break bonds?

  High melting/boiling points
• Match the property of giant covalent structures with its description:

  Melting and Boiling Points ↔️ High due to strong covalent bonds

  Electrical Conductivity ↔️ Mostly insulating, except graphite

  Hardness ↔️ Very hard due to robust bonding
• Giant covalent structures are suitable for high-temperature applications due to their thermal stability.


  True
• Diamond is an electrical insulator, while graphite is a conductor.