JEE Chemistry The Solid State MCQs Set 27

Chemistry Objective Questions and Answers: The Solid State

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Multiple Choice Questions

Question 1: What will be the value of rNa+ + rCl− in an NaCl crystal having edge length 'a'?
(a) a√3/2
(b) √2 a
(c) a/2
(d) a/(2√2)
Show Answer & Explanation

Answer: (c) a/2

Explanation:
1. In NaCl the ions touch along the cell edge: Na+ and Cl− alternate with a gap of a/2 between neighbours.
2. So r+ + r− = a/2.
3. Answer: (c)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 2: Which of the following can show both Schottky and Frenkel defects?
(a) NaCl
(b) AgCl
(c) AgBr
(d) KCl
Show Answer & Explanation

Answer: (c) AgBr

Explanation:
1. Schottky needs similar cation and anion sizes; Frenkel needs a small cation.
2. AgBr satisfies both conditions and shows both defects.
3. Answer: (c)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 3: The incorrect statement regarding defects in crystalline solids is:
(a) density of the crystal decreases in a Schottky defect
(b) Frenkel defect is a dislocation defect
(c) defects increase the conductivity of a solid
(d) density of the crystal increases in a Frenkel defect
Show Answer & Explanation

Answer: (d) density of the crystal increases in a Frenkel defect

Explanation:
1. In a Frenkel defect the ion only moves to an interstitial site; no ions leave the crystal.
2. So the density stays the same, not increases.
3. Answer: (d)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 4: Select the incorrect statement:
(a) stoichiometry of the crystal remains unaffected due to Schottky defect
(b) Frenkel defect is usually shown by ionic compounds having low coordination number
(c) F-centre generation is responsible for imparting colour to the crystal
(d) density of the crystal always increases due to a substitutional impurity defect
Show Answer & Explanation

Answer: (d) density of the crystal always increases due to a substitutional impurity defect

Explanation:
1. A substituted atom may be lighter or heavier, so the density may rise or fall.
2. The other three statements are correct.
3. Answer: (d)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 5: When AgCl is doped with 0.01 mole of CdCl2, what is the number of cationic vacancies?
(a) 0.02 NA
(b) 0.01 NA
(c) 0.01
(d) 0.02
Show Answer & Explanation

Answer: (b) 0.01 NA

Explanation:
1. Each Cd2+ replaces two Ag+ and leaves one vacancy.
2. Vacancies = 0.01 NA.
3. Answer: (b)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 6: The distance between Na+ and Cl− in NaCl is 281 pm. What is the edge length of the cubic unit cell?
(a) 1405 pm
(b) 562 pm
(c) 843 pm
(d) 281 pm
Show Answer & Explanation

Answer: (b) 562 pm

Explanation:
1. Na+–Cl− distance = a/2.
2. a = 2 × 281 = 562 pm.
3. Answer: (b)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 7: The nearest distance between a tetrahedral void and an octahedral void in an FCC unit cell is:
(a) a/2
(b) a/√2
(c) √3a/4
(d) √3a/2
Show Answer & Explanation

Answer: (c) √3a/4

Explanation:
1. A tetrahedral void is at (1/4, 1/4, 1/4) and an octahedral void at (1/2, 1/2, 1/2).
2. Distance = √3 × (a/4) = √3a/4.
3. Answer: (c)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 8: The coordination number of F− ion in the CaF2 crystalline structure is:
(a) 8
(b) 2
(c) 4
(d) 6
Show Answer & Explanation

Answer: (c) 4

Explanation:
1. In fluorite, Ca2+ has CN 8 and F− occupies tetrahedral voids.
2. So each F− has CN 4.
3. Answer: (c)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 9: A face centred cubic lattice is made up of two types of atoms A and B, in which A occupies the corner positions and B the face centres. If the atoms along one body diagonal are removed, the empirical formula of the remaining solid will be:
(a) AB2
(b) A2B
(c) A7B3
(d) AB4
Show Answer & Explanation

Answer: (d) AB4

Explanation:
1. A body diagonal passes through two corners (the body centre has no atom in fcc).
2. A left = 6 × 1/8 = 3/4; B = 6 × 1/2 = 3.
3. A : B = 3/4 : 3 = 1 : 4, so AB4.
4. Answer: (d)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 10: In the rock salt structure AB, if C is introduced into the tetrahedral voids such that no distortion occurs, the formula of the resulting compound is:
(a) ABC
(b) ABC2
(c) A4B4C
(d) ABC8
Show Answer & Explanation

Answer: (b) ABC2

Explanation:
1. Rock salt has 4 AB units per unit cell and 8 tetrahedral voids.
2. C = 8 per 4 AB, so A : B : C = 1 : 1 : 2.
3. Answer: (b)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 11: A compound forms a hexagonal close packed structure. How many octahedral voids are present in 0.3 mol of it?
(a) 1.08 × 1023
(b) 1.80 × 1023
(c) 5.4 × 1023
(d) none of these
Show Answer & Explanation

Answer: (b) 1.80 × 1023

Explanation:
1. In close packing, octahedral voids equal the number of atoms.
2. Voids = 0.3 × 6.022 × 1023 = 1.80 × 1023.
3. Answer: (b)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 12: For graphite, which of the following unit cell parameters is possible?
(a) a = b = c, α = β = γ = 90°
(b) a = b ≠ c, α = β = γ = 90°
(c) a = b ≠ c, α = β = 90°, γ = 120°
(d) a ≠ b ≠ c, α = β = γ = 90°
Show Answer & Explanation

Answer: (c) a = b ≠ c, α = β = 90°, γ = 120°

Explanation:
1. Graphite has layers of hexagonally arranged carbon.
2. Its crystal system is hexagonal: a = b ≠ c, α = β = 90°, γ = 120°.
3. Answer: (c)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 13: Due to an excess of lithium, LiCl crystals appear:
(a) yellow
(b) violet
(c) pink
(d) white
Show Answer & Explanation

Answer: (c) pink

Explanation:
1. Excess metal creates F-centres (anion vacancies holding electrons).
2. These absorb light, and LiCl then appears pink.
3. Answer: (c)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 14: A metal crystallises in an FCC lattice. If the edge length of the unit cell is 4 × 10−8 cm and the density is 10.5 g cm−3, the atomic mass of the metal is:
(a) 101.2
(b) 50.6
(c) 202.3
(d) none
Show Answer & Explanation

Answer: (a) 101.2

Explanation:
1. M = dNAa3/Z = 10.5 × 6.022 × 1023 × 6.4 × 10−23/4.
2. = 101.2.
3. Answer: (a)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 15: Which of the following is a non-crystalline solid?
(a) CsCl
(b) NaCl
(c) CaF2
(d) glass
Show Answer & Explanation

Answer: (d) glass

Explanation:
1. Glass is an amorphous (supercooled liquid) solid with no long-range order.
2. The others have regular crystal lattices.
3. Answer: (d)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 16: Solid CO2 is an example of:
(a) ionic crystal
(b) covalent crystal
(c) metallic crystal
(d) molecular crystal
Show Answer & Explanation

Answer: (d) molecular crystal

Explanation:
1. Solid CO2 consists of discrete CO2 molecules held by weak van der Waals forces.
2. Answer: (d)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 17: The density of KBr is 2.82 g cm−3. The length of the unit cell is 654 pm. Atomic masses: K = 39, Br = 80. Then the solid is:
(a) face centred cubic
(b) simple cubic system
(c) body centred cubic system
(d) none of these
Show Answer & Explanation

Answer: (a) face centred cubic

Explanation:
1. Z = dNAa3/M = 2.82 × 6.022 × 1023 × (6.54 × 10−8)3/119.
2. = 3.99 ≈ 4 formula units per cell, which is the fcc (rock salt) arrangement.
3. Answer: (a)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

Question 18: Which statement is correct for the antifluorite structure of Na2O?
(a) O2− ions have a CCP arrangement
(b) Na+ ions occupy all the tetrahedral sites
(c) it has 4 : 8 coordination
(d) all are correct
Show Answer & Explanation

Answer: (d) all are correct

Explanation:
1. O2− forms ccp, Na+ fills all 8 tetrahedral voids.
2. Coordination numbers are 4 (Na+) and 8 (O2−).
3. Answer: (d)

Teacher's Note:
1. Recall the geometry of the lattice first, then count atoms per unit cell. Check the result against the known limiting values.

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Practice MCQs for JEE Chemistry The Solid State

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