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Questions and Answers
What are network solids?
What are network solids?
A covalent network solid is a chemical compound or element in which the atoms are bonded by covalent bonds in a continuous network extending throughout the material.
What is an example of a three-dimensional covalent network?
What is an example of a three-dimensional covalent network?
Diamond
Which of the following is a property of 3D network covalent solids?
Which of the following is a property of 3D network covalent solids?
Why do 3D network covalent solids have high melting points?
Why do 3D network covalent solids have high melting points?
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3D network covalent solids conduct electricity.
3D network covalent solids conduct electricity.
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Which of the following best describes the bonding in graphite?
Which of the following best describes the bonding in graphite?
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What is the solubility behavior of graphite?
What is the solubility behavior of graphite?
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Match the following properties with their corresponding 3D network covalent solid examples:
Match the following properties with their corresponding 3D network covalent solid examples:
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Study Notes
Covalent Network Solids
- Covalent network solids consist of atoms bonded in a continuous network without individual molecules, forming macromolecules.
- Types of structures: 1D chains (e.g., plastics like polyethene), 2D layers (e.g., graphite), and 3D networks (e.g., diamond, silica).
Properties of 3D Network Solids
- Example: Diamond exhibits strong covalent bonding with carbon atoms forming a rigid interlocking lattice.
- Extremely high melting point nearing 4000°C due to robust C-C bonds that require significant energy to break.
- Diamond is characterized as the hardest natural material, making it highly resistant to scratching.
- Insoluble in water and organic solvents because the strong attractive forces within the solid overpower potential solvation.
Electrical Conductivity
- 3D network solids like diamond do not conduct electricity as they lack free ions or electrons to carry an electric charge.
Characteristics of Graphite
- Graphite consists of layers of carbon atoms arranged in a hexagonal lattice, with strong covalent bonds within layers and weak interactions between layers.
- High melting point similar to diamond, requiring considerable heat to disrupt C-C bonds within its layers.
- Conducts electricity due to delocalized electrons that flow between layers, allowing it to function effectively in batteries as an electrode.
- Soft and slippery texture results from weak intermolecular forces allowing layers to slide easily, useful in applications like lubricants and pencil leads.
- Does not dissolve in polar or non-polar solvents due to strong C-C bonds resisting disruption by solvent interactions.
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Description
Test your knowledge on covalent network solids with this set of flashcards. Learn about their unique structures, including 1D chains, 2D layers, and 3D networks. This quiz is perfect for students studying chemistry or materials science.
