1. Which type of crystal is characterized by a lattice of positive ions in a "sea of delocalized electrons"?
A) Ionic
B) Metallic
C) Covalent
D) Molecular
Answer: B) Metallic
Explanation: Metallic crystals (e.g., copper, iron) consist of metal cations surrounded by delocalized electrons, explaining their conductivity and malleability.
2. Sodium chloride (NaCl) is an example of which type of crystal?
A) Metallic
B) Ionic
C) Molecular
D) Amorphous
Answer: B) Ionic
Explanation: Ionic crystals (e.g., NaCl) are formed by electrostatic attraction between cations and anions, arranged in a highly ordered lattice, giving high melting points and brittleness.
3. Which type of crystal has atoms bonded in a continuous 3D network, like diamond?
A) Metallic
B) Covalent
C) Ionic
D) Molecular
Answer: B) Covalent
Explanation: Covalent (network) crystals (e.g., diamond, silicon) feature strong covalent bonds in all directions, making them extremely hard and high-melting.
4. Dry ice (solid CO₂) is an example of which type of crystal?
A) Molecular
B) Ionic
C) Metallic
D) Amorphous
Answer: A) Molecular
Explanation: Molecular crystals (e.g., CO₂, I₂) consist of discrete molecules held by weak intermolecular forces (like van der Waals or hydrogen bonds), leading to low melting points.
5. Which material lacks a long-range ordered structure and is considered non-crystalline?
A) Quartz
B) Copper
C) Glass
D) NaCl
Answer: C) Glass
Explanation: Glass is an amorphous solid, meaning it has short-range order but no repeating crystalline lattice, unlike quartz (covalent) or copper (metallic).
6. What type of crystal is responsible for the shiny, ductile properties of gold?
A) Ionic
B) Molecular
C) Metallic
D) Covalent
Answer: C) Metallic
Explanation: Gold’s metallic crystal structure, with delocalized electrons, allows for luster (electron reflection) and ductility (electron mobility).
7. Which type of crystal typically has the highest melting point due to strong directional bonds?
A) Molecular
B) Ionic
C) Covalent
D) Metallic
Answer: C) Covalent
Explanation: Covalent network crystals (e.g., diamond, SiO₂) have strong covalent bonds throughout, requiring immense energy to break, unlike ionic or metallic bonds.
8. Sugar crystals belong to which crystal type?
A) Ionic
B) Molecular
C) Amorphous
D) Metallic
Answer: B) Molecular
Explanation: Sugar (sucrose) forms molecular crystals, where sugar molecules are held together by hydrogen bonds, making them soft and low-melting compared to ionic or covalent crystals.
9. Which of the following is an example of an amorphous solid?
A) Aluminum
B) Silicon carbide
C) Rubber
D) Potassium chloride
Answer:C) rubber
Explanation: Rubber is amorphous, lacking a crystalline structure. Aluminum (metallic), silicon carbide (covalent), and KCl (ionic) are crystalline.
10. Which crystal type conducts electricity in the solid state due to mobile electrons?
A) Ionic
B) Covalent
C) Metallic
D) Molecular
Answer: C) Metallic
Explanation: Metallic crystals (e.g., silver, copper) conduct electricity because their delocalized electrons are free to move, unlike ionic (conducts when molten) or covalent/molecular (insulators).
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