Important MCQs on The Solid State with Explanation

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Solids are a state of matter in which the constituent particles are packed together very closely. Solids have a very high intermolecular force due to the low intramolecular distance. They do have a rigid shape and are incompressible. Solids have fixed volume, size, and shape. The particles that make up a solid item are set in place and cannot freely move. For the components of solids, only motion along the mean position is possible.

Based on the type of order inherent in the arrangement of their constituent particles, solids can be categorized as crystalline and amorphous solids. Crystalline solids are anisotropic, have a high melting temperature, and have their component particles arranged in a long-range order. Since the organization of the component particles is short-range ordered, isotropic, and lacks a clearly defined melting temperature, amorphous solids behave like icy liquids.

Important MCQs on The Solid State for the students to test their knowledge on the given topic.

Ques 1. A crystalline solid:

Changes abruptly from solid-state to liquid upon heating
Has no definite melting point.
Undergoes deformation of its geometry easily
Has irregular 3-dimensional arrangements.

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Ans. (A) Changes abruptly from solid-state to liquid upon heating

Explanation: Even when heated, they do not undergo geometric deformation. Over a range of temperatures, they don't become softer. In actuality, when heated to their melting point, crystalline solids quickly transform from solid to liquid.

Ques 2. What will be the ratio of the number of atoms present in a simple cubic, body-centred cubic and face-centred cubic structure respectively?

8:1:6
1:2:4
4:2:1
4:2:3

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Ans. (B) 1:2:4

Explanation: The basic cube has eight atoms at each corner, the body-centred cube has one atom in the middle of the body and the face-centred cube has eight atoms at each corner and six atoms in the centre of each face. Each atom in the corner contributes 1/8, while each atom in the face's centre contributes 1/2. Now it is straightforward to determine the ratios of a body-centred cubic, a face-centred cubic, and a basic cube.

Ques 3. Na and Mg crystallize in crystals of bcc and fcc form respectively and then the amount of Na and Mg atoms present in their respective crystal unit cells is:

4 and 2
9 and 14
14 and 9
2 and 4

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Ans. (D) 2 and 4

Explanation: Eight atoms are located at the corners of the bcc cell, with one atom in the middle. The fcc cell has one atom on each of the six sides and eight atoms at each of the eight corners. Two unit cells share the atom at the face.

Ques 4. How many unit cells are divided equally in a face-centred cubic lattice?

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Ans. (C) 6

Explanation: It is evenly shared by 6 unit cells since the F.C.C. unit cells have 6 faces.

Ques 5. When is the Schottky defect in a crystal observed?

When the ion leaves its normal position and then, occupies an interstitial location
When the unequal number of cations and anions is missing from the lattice
When the density of the crystal increases
When an equal number of cations and anions are missing from the lattice

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Ans. (D) An equal number of cations and anions are missing from the lattice.

Explanation: When the lattice is missing an equal amount of cations and anions, this is known as a Schottky defect. The electrical neutrality of the crystal will be impacted if there are not an equal amount of missing cations and anions.

Ques 6. What is the total number of voids in 0.5 mol of a compound forming hexagonal close-packed structure?

6.022 × 10²³
3.011 × 10²³
9.033 × 10²³
4.516 × 10²³

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Ans. 9.033 × 10²³

Explanation: Z eff for HCP electrons = 6

Number of the unit cells in HCP = 0.5/6 × 6.022 ×10²³

= 6.022 ×10²³ / 12

There are 12 tetrahedral and 6 octahedral voids in a single unit cell. 18 total voids (in one unit cell)

Total Number of Voids = 18 × 6.022 ×10²³/12 = 9.033 × 10²³

Ques 7. The axial ratios for the orthorhombic system are a ≠ b ≠ c, what will be the axial angles?

α = β = γ ≠ 90
α ≠ β ≠ γ ≠ 90
α = β = γ = 90
α ≠ β ≠ γ = 90

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Ans. (C) α = β = γ = 90

Explanation: For the orthorhombic system, axial ratios are a ≠b≠ c and the axial angles are α=β=γ=90. Thus, all three edge lengths are unequal but all the angles are equal. They are equal to 90 degrees.

Ques 8. In NaCl structure

All octahedral and tetrahedral sites are occupied
Only octahedral sites are occupied
Only tetrahedral sites are occupied
Neither octahedral nor tetrahedral sites are occupied

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Ans. (B) Only octahedral sites are occupied

Explanation: Chlorine ions are found in every part of the NaCl molecule. The octahedral voids, on the other hand, are occupied by sodium ions. We can observe that in the structure, every octahedral vacuum is filled. We may infer from these facts that only octahedral sites are occupied in the NaCl structure.

Ques 9. Why do the Alkali halides not display or show the Frenkel defect?

Anions and Cations have almost equal sizes
There is a large difference in the size of cations and anions
Anions and Cations have a low coordination number
Anions cannot be accommodated in voids

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Ans. (A) Anions and Cations have almost equal sizes

Explanation: Because cations and anions are almost the same size and cannot fit in interstitial locations, alkali metals do not exhibit the Frenkel defect.

Ques 10. Silver halides generally show

Schottky defect
Frenkel defect
Both Frenkel and Schottky defects
Cation excess defect

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Ans. (C) Both Frenkel and Schottky defects

Explanation: Due to the strong ionic nature of silver halides, the Schottky defect is conceivable. So, option C is the right response. As an illustration, AgBr exhibits the Schottky and Frenkel defects. Ions absent from their lattice point cause the Schottky defect while missing ions occupying interstitial sites cause the Frenkel defect.

Ques 11. The effect of the Frenkel defect on the density of ionic solids is that

The density of the crystal increases
The density of the crystal decreases
The density of the crystal remains unchanged
There is no relationship between the density of a crystal and the defect present in it.

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Ans. (C) The density of the crystal remains unchanged

Explanation: The Frenkel defect does not affect the density of ionic solids. This flaw simply causes the ions to move within the crystal, preserving both the volume and mass, hence it does not affect the solid's density.

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Important MCQs on The Solid State with Explanation

Important MCQs on The Solid State for the students to test their knowledge on the given topic.

CBSE CLASS XII Related Questions

1.
How would you account for the following:
Of the d⁴ species, Cr²⁺ is strongly reducing while manganese(III) is strongly oxidising.
Cobalt(II) is stable in aqueous solution but in the presence of complexing reagents it is easily oxidised.
The d¹ configuration is very unstable in ions.

2.
Define the term solution. How many types of solutions are formed? Write briefly about each type with an example.

3.
Write equations of the following reactions:
(i)Friedel-Crafts reaction–alkylation of anisole.
(ii)Nitration of anisole.
(iii)Bromination of anisole in ethanoic acid medium.
(iv)Friedel-Craft’s acetylation of anisole.

4.
Draw the structures of optical isomers of:
(i) \([Cr(C_2O_4)_3]^{3–}\)
(ii) \([PtCl_2(en)_2]^{2+}\)
(iii) \([Cr(NH_3)2Cl_2(en)]^{+}\)

5.
Give the IUPAC names of the following compounds:
(i)CH₃CH(Cl)CH(Br)CH₃
(ii)CHF₂CBrClF
(iii)ClCH₂C≡CCH₂Br
(iv)(CCl3)₃CCl
(v)CH₃C(p-ClC₆H₄)₂CH(Br)CH₃
(vi)(CH₃)₃CCH=CClC₆H₄I-p

6.
Depict the galvanic cell in which the reaction Zn(s) + 2Ag⁺(aq) → Zn²⁺(aq) + 2Ag(s) takes place. Further show:
(i) Which of the electrode is negatively charged?
(ii) The carriers of the current in the cell.
(iii) Individual reaction at each electrode.

Similar Chemistry Concepts

Comments

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Important MCQs on The Solid State with Explanation

Important MCQs on The Solid State for the students to test their knowledge on the given topic.

CBSE CLASS XII Related Questions

1. How would you account for the following: Of the d4 species, Cr2+ is strongly reducing while manganese(III) is strongly oxidising. Cobalt(II) is stable in aqueous solution but in the presence of complexing reagents it is easily oxidised. The d1 configuration is very unstable in ions.

2. Define the term solution. How many types of solutions are formed? Write briefly about each type with an example.

3. Write equations of the following reactions: (i)Friedel-Crafts reaction–alkylation of anisole.(ii)Nitration of anisole.(iii)Bromination of anisole in ethanoic acid medium.(iv)Friedel-Craft’s acetylation of anisole.

4. Draw the structures of optical isomers of: (i) \([Cr(C_2O_4)_3]^{3–}\)(ii) \([PtCl_2(en)_2]^{2+}\)(iii) \([Cr(NH_3)2Cl_2(en)]^{+}\)

5. Give the IUPAC names of the following compounds:(i)CH3CH(Cl)CH(Br)CH3(ii)CHF2CBrClF(iii)ClCH2C≡CCH2Br(iv)(CCl3)3CCl(v)CH3C(p-ClC6H4)2CH(Br)CH3(vi)(CH3)3CCH=CClC6H4I-p

6. Depict the galvanic cell in which the reaction Zn(s) + 2Ag+(aq) → Zn2+(aq) + 2Ag(s) takes place. Further show: (i) Which of the electrode is negatively charged? (ii) The carriers of the current in the cell. (iii) Individual reaction at each electrode.

Similar Chemistry Concepts

Comments

SUBSCRIBE TO OUR NEWS LETTER

1.
How would you account for the following:
Of the d⁴ species, Cr²⁺ is strongly reducing while manganese(III) is strongly oxidising.
Cobalt(II) is stable in aqueous solution but in the presence of complexing reagents it is easily oxidised.
The d¹ configuration is very unstable in ions.

2.
Define the term solution. How many types of solutions are formed? Write briefly about each type with an example.

3.
Write equations of the following reactions:
(i)Friedel-Crafts reaction–alkylation of anisole.
(ii)Nitration of anisole.
(iii)Bromination of anisole in ethanoic acid medium.
(iv)Friedel-Craft’s acetylation of anisole.

4.
Draw the structures of optical isomers of:
(i) \([Cr(C_2O_4)_3]^{3–}\)
(ii) \([PtCl_2(en)_2]^{2+}\)
(iii) \([Cr(NH_3)2Cl_2(en)]^{+}\)

5.
Give the IUPAC names of the following compounds:
(i)CH₃CH(Cl)CH(Br)CH₃
(ii)CHF₂CBrClF
(iii)ClCH₂C≡CCH₂Br
(iv)(CCl3)₃CCl
(v)CH₃C(p-ClC₆H₄)₂CH(Br)CH₃
(vi)(CH₃)₃CCH=CClC₆H₄I-p

6.
Depict the galvanic cell in which the reaction Zn(s) + 2Ag⁺(aq) → Zn²⁺(aq) + 2Ag(s) takes place. Further show:
(i) Which of the electrode is negatively charged?
(ii) The carriers of the current in the cell.
(iii) Individual reaction at each electrode.