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Questions and Answers
What is the primary bonding force in molecular solids?
What is the primary bonding force in molecular solids?
Which property is characteristic of molecular solids?
Which property is characteristic of molecular solids?
What type of bonding holds ionic solids together?
What type of bonding holds ionic solids together?
Which of the following is true about ionic solids?
Which of the following is true about ionic solids?
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What is the defining feature of network covalent solids?
What is the defining feature of network covalent solids?
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Which property is most associated with metallic solids?
Which property is most associated with metallic solids?
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What characteristic makes metallic solids good conductors of electricity?
What characteristic makes metallic solids good conductors of electricity?
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What is the reason ionic solids are typically hard and brittle?
What is the reason ionic solids are typically hard and brittle?
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Study Notes
Intermolecular Forces and Types of Solids
- Molecular (Covalent) Solids: Held together by intermolecular forces. These forces are weaker than the bonds within a single molecule.
- Property of Molecular Solids: Characterized by low melting points and poor electrical conductivity.
- Ionic Solids: Held together by ionic bonds. These are strong electrostatic forces between oppositely charged ions. Ionic solids have high melting points.
- Ionic Solids Conductivity: Conduct electricity when molten or dissolved in water, as the ions become free to move.
- Network Covalent Solids: Characterized by large, interconnected covalent bonds. These bonds are very strong, resulting in high melting points and hardness.
- Network Covalent Solid Example: Diamond and graphite are noteworthy examples.
- Metallic Solids: Consist of metal atoms surrounded by a "sea of electrons." This electron sea allows for good electrical conductivity and malleability (ability to be hammered into sheets) and ductility (ability to be drawn into wires).
- Metallic Solid Example: Copper is a prime example of a metallic solid.
- Metallic Solids Conductivity: Metallic solids are excellent electrical conductors due to the free-moving electrons.
- Ionic Solids Hardness: Ionic solids are usually hard and brittle. Strong ionic bonds resist deformation, but applied force can cause like charges to align and repel, causing breakage.
- Defining Characteristic of Network Covalent Solids: They feature large networks of atoms joined by covalent bonds.
- Solids that Do Not Conduct Electricity: Molecular solids and network covalent solids generally do not conduct electricity in their solid state because there are no free electrons or ions that can move.
- Hardness Comparison: Diamond (network covalent) is generally the hardest of the listed solids.
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Description
Explore the different types of solids, including molecular, ionic, network covalent, and metallic solids. Learn about their properties, bonding types, and conductivity. This quiz will test your understanding of how intermolecular forces influence solid materials.
