Chapter 6: Solid State — Online MCQ Test
CHEMISTRY · CLASS 12th · Tamil Nadu State Board
Practice Chapter 6: Solid State with a free chapter-wise online MCQ test.
This chapter covers: Exploring crystalline solids this chapter covers unit cells crystal lattices packing efficiency and density calculations. Students examine Bragg law point defects like Schottky and....
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Chapter 6: Solid State — Important Questions & Answers
Which of the following is an example of a crystalline solid?
- A. Glass
- B. Quartz
- C. Rubber
- D. Plastic
Answer: B. Quartz
Quartz is a crystalline solid with a regular and repeating arrangement of particles. Glass is amorphous, not crystalline.
Quartz is a crystalline solid with a regular and repeating arrangement of particles. Glass is amorphous, not crystalline.
The number of nearest neighbouring atoms in a body-centered cubic (bcc) unit cell is:
- A. 6
- B. 8
- C. 12
- D. 4
Answer: B. 8
In a bcc structure, each atom has 8 nearest neighbours. This is called the coordination number.
In a bcc structure, each atom has 8 nearest neighbours. This is called the coordination number.
Which of the following statements about hexagonal close packing (hcp) is correct?
- A. Packing efficiency is 52%
- B. Coordination number is 8
- C. Packing efficiency is 74%
- D. It has one atom per unit cell
Answer: C. Packing efficiency is 74%
Both hcp and ccp structures have a packing efficiency of 74%, which is the maximum for close packing.
Both hcp and ccp structures have a packing efficiency of 74%, which is the maximum for close packing.
Which of the following statements is NOT correct regarding a simple cubic lattice?
- A. Coordination number is 6
- B. Packing efficiency is about 52.4%
- C. Atoms touch each other along the edge
- D. There are 2 atoms per unit cell
Answer: D. There are 2 atoms per unit cell
A simple cubic unit cell has only 1 atom per unit cell, not 2. The other statements are correct for a simple cubic structure.
A simple cubic unit cell has only 1 atom per unit cell, not 2. The other statements are correct for a simple cubic structure.
A cubic solid has a density of 10.0 g cm⁻³, molar mass 120 g mol⁻¹ and edge length 400 pm. How many formula units are present per unit cell? [N_A = 6.02 × 10²³ mol⁻¹]
- A. 1
- B. 2
- C. 4
- D. 8
Answer: B. 2
Using d = ZM / (N_A a^3), the given values give Z approximately 2. Therefore, the unit cell contains 2 formula units.
Using d = ZM / (N_A a^3), the given values give Z approximately 2. Therefore, the unit cell contains 2 formula units.