Solid state chapter 1 class 12 Mcqs with solutions || Chemistry ||

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 Q. 1. Which of the following is not true about the ionic solids? 

(A) Bigger ions form the close packed structure. 

(B) Smaller ions occupy either the tetrahedral or the octahedral voids depending upon their size. 

(C) Occupation of all the voids is not necessary. 

(D) The fraction of octahedral or tetrahedral voids occupied depends upon the radii of the ions occupying the voids.

 Ans. Option (B) is correct. 

Explanation: In ionic solids, smaller ions occupy the voids, and this depends on stoichiometry of the compounds not on the radius of ions. 

Q. 2. Solid A is very hard electrical insulator in solid as well as in molten state and melts at an extremely high temperature. What type of solid is it? 

(A) Ionic solid 

(B) Molecular solid 

(C) Covalent solid 

(D) Metallic solid 

Ans. Option (C) is correct. 

Explanation: Covalent solids are generally hard, act as insulators and melting points of such solids are extremely high. 

Q. 3. Which of the following is a network solid? 

(A) SO2 (solid) 

(B) I2 

(C) Diamond 

(D) H2O (ice) 

Ans. Option (C) is correct. 

Explanation: A network solid consists of a network atoms of same or different elements connected to each other by covalent bonds. So, diamond is a network solid as it contains network of carbon atoms . 

Q. 4. Graphite cannot be classified as __________. 

(A) Conducting solid 

(B) Network solid 

(C) Covalent solid 

(D) Ionic solid 

Ans. Option (D) is correct. 

Explanation: Graphite is a conducting solid, network or covalent solid but it cannot be classified as ionic solid. 

Q. 5. Which of the following statements is not true about amorphous solids? 

(A) On heating they may become crystalline at certain temperature. 

(B) They may become crystalline on keeping for long time. 

(C) Amorphous solids can be moulded by heating. 

(D) They are anisotropic in nature. 

Ans. Option (D) is correct. 

Explanation: Amorphous solids are isotropic in nature, i.e., there is no long-range order, and arrangement is irregular along all the directions. 

Q. 6. Which of the following is an amorphous solid? 

(A) Graphite (G) 

(B) Quartz glass (SiO2) 

(C) Chrome alum 

(D) Silicon carbide (SiC) 

Ans. Option (B) is correct. 

Explanation: Quartz glass (SiO2) is an amorphous solid as it has no long-range order. 

Q. 7. The sharp melting point of crystalline solids is due to ___________. 

(A) a regular arrangement of constituent particles observed over a short distance in the crystal lattice. 

(B) a regular arrangement of constituent particles observed over a long distance in the crystal lattice. 

(C) same arrangement of constituent particles in different directions. 

(D) different arrangements of constituent particles in different directions. 

Ans. Option (B) is correct. 

Explanation: The sharp melting point of crystalline solids is due to a regular arrangement of constituent particles observed over a long distance in the crystal lattice. 

Q. 8. Which of the following conditions favours the existence of a substance in the solid state? 

 (A) High temperature 

(B) Low temperature 

(C) High thermal energy 

(D) Weak cohesive forces 

Ans. Option (B) is correct. 

Explanation: At low temperature substance exists in solid state. It is due to the decrease in molecular movement which leads to strong cohesive force, that is, the force which tightly holds the constituent particles together. 

Q. 9. A compound is formed by two elements M and N. 

The element N forms ccp lattice and atoms of M occupy two atoms an Mercury 1/3rd of tetrahedral voids. What is the formula of the compound 

(A) MN2 

(B) M2N3 

(C) M3N2 

(D) M2N2 

Ans. Option (B) is correct. 

Explanation: Suppose the atoms N in the ccp = a \ No. of tetrahedral voids = 3a 

No. of atoms M = 2 3 a : a = 2: 3 

 Hence compound as M2: N3

Q. 10. Silver crystallises in f.c.c. Lattice. It edge length of the unit cells is 4.07 × 10–8 cm density and is 10.5g cm–3. Calculate the atomic mass of silver. 

(A) 144 g/mol 

(B) 125 g/mol 

(C) 106.6 g/mol 

(D) 213 g/mol



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