Questions on Classes of Crystalline Solids
20 Multiple-Choice Questions on Classes of Crystalline Solids
1. Which of the following is NOT a class of crystalline solids?
A) Ionic solids
B) Metallic solids
C) Molecular solids
D) Polymer solids
E) Covalent network solids
2. Which class of crystalline solids is typically held together by electrostatic forces between ions?
A) Metallic solids
B) Ionic solids
C) Molecular solids
D) Covalent network solids
E) Amorphous solids
3. Which type of crystalline solid usually has high melting points and is hard and brittle?
A) Molecular solids
B) Metallic solids
C) Ionic solids
D) Covalent network solids
E) Liquid crystals
4. Which crystalline solids have atoms connected by covalent bonds in a continuous network?
A) Molecular solids
B) Metallic solids
C) Ionic solids
D) Covalent network solids
E) Van der Waals solids
5. Which class of crystalline solids has delocalized electrons allowing electrical conductivity?
A) Ionic solids
B) Metallic solids
C) Molecular solids
D) Covalent network solids
E) Hydrogen bonded solids
6. Which crystalline solids are usually soft and have low melting points?
A) Covalent network solids
B) Ionic solids
C) Metallic solids
D) Molecular solids
E) Amorphous solids
7. Which of the following is a typical example of a covalent network solid?
A) Sodium chloride (NaCl)
B) Diamond
C) Ice
D) Copper
E) Sugar
8. What is the primary intermolecular force in molecular solids?
A) Covalent bonds
B) Metallic bonds
C) Ionic bonds
D) Van der Waals forces and hydrogen bonds
E) Nuclear forces
9. Which crystalline solid class generally has poor electrical conductivity in solid form but may conduct in molten or dissolved state?
A) Molecular solids
B) Ionic solids
C) Metallic solids
D) Covalent network solids
E) Polymer solids
10. Which of the following solids is an example of a metallic solid?
A) Ice
B) Quartz
C) Aluminum
D) Sodium chloride
E) Sucrose
11. Which crystalline solid class is characterized by atoms bonded in a 3D network, making it extremely hard?
A) Molecular solids
B) Ionic solids
C) Metallic solids
D) Covalent network solids
E) Amorphous solids
12. Which class of crystalline solids can be malleable and ductile?
A) Ionic solids
B) Covalent network solids
C) Metallic solids
D) Molecular solids
E) Ionic liquids
13. Ice is classified as which type of crystalline solid?
A) Molecular solid
B) Ionic solid
C) Metallic solid
D) Covalent network solid
E) Amorphous solid
14. Which class of crystalline solids tends to be poor conductors of electricity both as solids and liquids?
A) Molecular solids
B) Ionic solids
C) Metallic solids
D) Covalent network solids
E) Amorphous solids
15. Which of the following is a common property of ionic solids?
A) Low melting point
B) Conduct electricity as solids
C) Brittle
D) Malleable
E) Poor solubility in water
16. Which class of crystalline solids is held together primarily by metallic bonding?
A) Covalent network solids
B) Molecular solids
C) Ionic solids
D) Metallic solids
E) Van der Waals solids
17. Which of the following is NOT typically a characteristic of molecular solids?
A) Low melting points
B) Held together by intermolecular forces
C) Good electrical conductivity
D) Soft texture
E) Often volatile
18. Silicon dioxide (quartz) belongs to which class of crystalline solids?
A) Molecular solids
B) Ionic solids
C) Metallic solids
D) Covalent network solids
E) Amorphous solids
19. Which class of solids would likely have the highest melting point?
A) Molecular solids
B) Ionic solids
C) Metallic solids
D) Covalent network solids
E) Polymer solids
20. What is the main bonding force in metallic solids?
A) Ionic bonds
B) Covalent bonds
C) Metallic bonds (delocalized electrons)
D) Hydrogen bonds
E) Van der Waals forces
Answers and Explanations
1. D – Polymer solids are generally amorphous or semi-crystalline, not a main class of crystalline solids.
2. B – Ionic solids are held together by electrostatic attraction between positive and negative ions.
3. C – Ionic solids tend to be hard, brittle, and have high melting points.
4. D – Covalent network solids have atoms connected by covalent bonds in a continuous 3D network.
5. B – Metallic solids have delocalized electrons that enable conductivity.
6. D – Molecular solids have weak intermolecular forces, leading to low melting points and softness.
7. B – Diamond is a classic example of a covalent network solid.
8. D – Molecular solids are held mainly by Van der Waals forces and hydrogen bonds.
9. B – Ionic solids conduct electricity only when molten or dissolved due to mobile ions.
10. C – Aluminum is a metallic solid.
11. D – Covalent network solids are extremely hard due to strong covalent bonds in a 3D network.
12. C – Metallic solids are malleable and ductile due to the mobility of delocalized electrons.
13. A – Ice is a molecular solid held together by hydrogen bonds.
14. A – Molecular solids are poor conductors both as solids and liquids.
15. C – Ionic solids are brittle due to rigid ionic lattices.
16. D – Metallic solids are held together by metallic bonding.
17. C – Molecular solids are poor conductors of electricity.
18. D – Quartz is a covalent network solid.
19. D – Covalent network solids generally have the highest melting points.
20. C – Metallic bonding involves delocalized electrons allowing for conductivity and malleability.
Share Online!
