2.1.3 Giant Covalent Structures

• Giant covalent structures are large lattices of atoms bonded by strong covalent
• Giant covalent structures are insoluble
• Giant covalent structures are poor conductors of electricity
• Diamond has a tetrahedral
• What are two prominent examples of giant covalent structures composed entirely of carbon atoms?

  Diamond and graphite
• Why are giant covalent structures poor conductors of electricity?

  Lack of free electrons
• What is the structure of simple covalent structures?

  Discrete molecules
• Graphite is extremely hard.

  False
• Giant covalent structures are usually soluble in water.

  False
• Why is graphite soft?

  Weak van der Waals
• Giant covalent structures are insoluble in water due to the strong bonds and lack of discrete molecules
• What type of bonding is present in giant covalent structures?

  Covalent bonds
• Match the giant covalent structure with its property:

  Diamond ↔️ Extremely hard

  Graphite ↔️ Electrical conductivity
• Giant covalent structures are poor conductors of electricity because they lack free-moving ions or electrons.
• Why are giant covalent structures insoluble in water?

  Strong bonds and discrete molecules
• What type of structure do giant covalent structures have?

  Large lattices
• What is the primary reason for the high melting points of giant covalent structures?

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

  Strong covalent bonds
• Match the structure type with its description:

  Large lattice ↔️ Giant covalent structures

  Crystalline lattice ↔️ Ionic structures
• Giant covalent structures are poor conductors of electricity due to the absence of free ions
• Graphite's conductivity allows it to be used in electrodes and batteries.


  True
• What is the structure of graphite?

  Hexagonal rings
• What type of melting and boiling points do giant covalent structures have?

  High
• Match the bonding type with the structure:

  Diamond ↔️ Covalent bonds between carbon atoms

  Graphite ↔️ Weak van der Waals between layers
• Giant covalent structures have high melting and boiling points because their strong covalent bonds require a lot of energy to break.


  True
• Giant covalent structures have a large lattice structure, unlike the discrete molecules of simple covalent structures.
• What type of structure do giant covalent structures have?

  Large lattice
• Ionic structures conduct electricity when molten or dissolved because their ions become mobile.
• The high melting and boiling points of giant covalent structures are due to their strong covalent bonds.


  True
• Giant covalent structures have high melting and boiling points because strong covalent bonds require a lot of energy to break.


  True
• Giant covalent structures dissolve in water because they are polar.

  False
• Giant covalent structures have strong covalent bonds throughout their lattice
• Giant covalent structures are good conductors of electricity because they have free-moving ions.

  False
• Giant covalent structures are poor conductors of electricity due to the absence of free-moving ions or electrons.


  True
• Ionic structures have higher melting and boiling points than giant covalent structures.

  False
• Graphite is used in lubricants due to its soft and slippery
• Simple covalent structures are usually soluble, while giant covalent structures are insoluble.


  True
• Ionic structures are usually soluble in polar solvents like water, whereas giant covalent structures are insoluble.


  True
• Order the properties of diamond and graphite based on their differences:

  1️⃣ Diamond has a tetrahedral structure.

  2️⃣ Graphite has a layered structure.

  3️⃣ Diamond is extremely hard.

  4️⃣ Graphite is soft.

  5️⃣ Diamond is non-conductive.

  6️⃣ Graphite is conductive.
• Why cannot giant covalent structures conduct electricity well?

  Lack of free-moving electrons