Intermolecular Forces and Types of Solids Quiz PDF
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This quiz covers intermolecular forces and different types of solids, including ionic, covalent, and metallic bonding. It includes questions about properties and characteristics of each type of solid.
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Intermolecular Forces and Types of Solids Quiz 1. What is the primary bonding force in molecular (covalent) solids? A) Ionic bonds B) Covalent bonds C) Intermolecular forces D) Metallic bonds 2. Which property is characteristic of molecular solids? A) High melt...
Intermolecular Forces and Types of Solids Quiz 1. What is the primary bonding force in molecular (covalent) solids? A) Ionic bonds B) Covalent bonds C) Intermolecular forces D) Metallic bonds 2. Which property is characteristic of molecular solids? A) High melting points B) High electrical conductivity C) Low melting points D) Hardness and brittleness 3. What type of bonding holds ionic solids together? A) Covalent bonds B) Ionic bonds C) London dispersion forces D) Metallic bonds 4. Which of the following is true about ionic solids? A) They are excellent conductors of electricity in their solid state. B) They have low melting and boiling points. C) They conduct electricity when molten or dissolved in water. D) They are typically soft and malleable. 5. What is the defining feature of network covalent solids? A) They are made of large, interconnected networks of covalent bonds. B) They consist of metal atoms surrounded by free electrons. C) They are held together by London dispersion forces. D) They are composed of ions arranged in a lattice structure. 6. Which of these is an example of a network covalent solid? A) Sodium chloride (NaCl) B) Graphite C) Diamond D) Copper (Cu) 7. Which property is most associated with metallic solids? A) They have a low melting point. B) They are good conductors of electricity. C) They are brittle and easily broken. D) They are soluble in water. 8. Which of the following substances is an example of a metallic solid? A) Ice (H₂O) B) Sodium chloride (NaCl) C) Copper (Cu) D) Quartz (SiO₂) 9. What characteristic makes metallic solids good conductors of electricity? A) The presence of free electrons that can move easily through the structure. B) The covalent bonding between atoms. C) The ionic bonds that hold the atoms together. D) The low melting points of metals. 10. What is the reason ionic solids are typically hard and brittle? A) The ionic bonds between oppositely charged ions are very strong, but when force is applied, like charges can align and repel, causing the solid to break. B) The covalent bonds between molecules are weak and flexible. C) The metallic bonds allow the atoms to slide past each other without breaking. D) The molecules are arranged in a loose, flexible structure. 11. Which type of solid is characterized by a "sea of electrons" surrounding metal atoms? A) Ionic solids B) Molecular solids C) Network covalent solids D) Metallic solids 12. What is the most likely property of a substance that forms a network covalent solid? A) High electrical conductivity B) High solubility in water C) High hardness and high melting point D) Malleability and ductility 13. Which of the following solids would likely be the hardest? A) Ice (H₂O) B) Diamond (C) C) Sodium chloride (NaCl) D) Copper (Cu) 14. What type of solid has no free-moving electrons or ions and cannot conduct electricity? A) Ionic solids B) Molecular solids C) Network covalent solids D) Metallic solids 15. Which of these is true about network covalent solids like diamond or graphite? A) They are good conductors of electricity. B) They consist of atoms covalently bonded into large, continuous networks. C) They are soft and easily molded. D) They have low melting points.
