The Spark Institute / The Science Foundation (Solid State)

1. The state of matter without definite shape & 14. A crystal is most likely to have a low melting
volume: point if:
(a) Solid (b) Liquid (a) Is macro molecule
(c) Gas (d) All of these (b) Is a crystalline solid
2. The strongest attractive forces are present (c) Has a delacalized valence electron
between the particles of _______. (d) Has weak Vander weal’s force
(a) Gases (b) Liquids 15. Which of the following pair are isomerphous?
(c) Solids (d) All of these (a) CaCO3 and NaNO3 (b) NaF and NaNO3
3. A sample of sodium chloride is likely pure of it: (c) Zn SO4 and NaNO3 (d) None of these
(a) Is colourless 16. Naphthalene is an example of:
(b) Dissolve completely in water (a) Ionic crystal (b) Covalent crystal
(c) Melt at exact temperature (c) Molecular crystal (d) Atomic crystal
(d) Is crystalline 17. ZnSO4 and NiSO4 are:
4. ZnSO4 and NiSO4 are (a) Polymorphous (b) Isomorphous
(a) Cubic (b) Tetragonal (c) Allotropies (d) Isotopes
(c) Orthorhombic (d) Trigonal 18. Diamond is an example of:
5. Iodine is an example of (a) Atomic crystal (b) Network crystal
(a) Covalent crystal (b) Molecular crystal (c)Ionic crystal (d) Molecular crystal
(c) Ionic crystal (d) Atomic crystal 19. Crystals in which molecules are held together
6. Calcium carbonate exist in nature in two through Vander Waal’s force are called:
crystalline form calcite is trigonal and (a) Metallic crystals (b) Covalent crystals
Aragonite is (c) Molecular crystals (d) Ionic crystals
(a) Cubic (b) Orthorhombic 20. Ionic solids are characterized by:
(c) Monoclinic (d) Tetragonal (a) Low melting point
7. In which of the following solids sublimation (b) Good conductivity in solid state
occurs. (c) Solubility in polar solvent
(a) Graphite (b) Ice (d) High vapour pressure
(c) Iodine (d) Sodium chloride 21. The metallic solids are characterized by:
8. Which of the following pairs are Isomorphous (a) High vapour pressure
(a) Na F and NaNO3 (b) MgO and NiSO4 (b) Low electrical conductivity
(c) NaNO3 and CaCO3 (d) ZnSO4 and NaNO3 (c) High melting point
9. Which of the following crystal have low melting (d) All of these
point 22. When a = b ≠ cand ∝ 𝜷 = 𝜸 = 90, the crystalline
(a) Atomic crystal (b) Ionic crystal system is:
(c) Molecular crystal (d) Covalent crystal (a) Cubic (b) Hexagonal
10. Which of the following is hexagonal crystal? (c) Tetragonal (d) Triclinic
(a) Diamond (b) Graphite 23. A crystalline solid:
(c) Cane sugar (d) Washing soda (a) Changes abruptly from solid to liquid when
11. Which of the following is an example of heated.
covalent crystal? (b) Specific cleavage planes
(a) Iodine (b) Diamond (c) Undergoes deformation of its geometry
(c) Common salt (d) Alum easily
12. Which of the following solid does not have (d) All of these
sharp melting point? 24. For the orthorhombic system, axial ratios are a
(a) Silver (b) Sodium chloride ≠ b ≠ c and the axial angles are:
(c) Glass (d) Diamond (a) α = β = γ ≠ 90o (b) α ≠ β ≠ γ ≠ 90o
13. CaSO4 5H2O occurs in nature in two crystalline (c) α = β = γ = 90o (d) α ≠ β ≠ γ = 90o
form monoclinic and trigonal this property is 25. Which solid structure has a definite and sharp
called melting point?
(a) Isomorphism (b) Polymorphism (a) All types of solids (b) No type of solid
(c) Allotropies (d) Isomerism (c) Amorphous solids (d) Crystalline solids
26. Which one of the following is non-crystalline or
amorphous?
(a) Diamond (b) Graphite
(c) Glass (d) Common Salt

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 The Spark Institute / The Science Foundation (Solid State)

27. How many chloride ions are surrounding 39. At Mount Everest, external pressure is 323 torr
sodium ion in sodium chloride crystal? and water boils at:
(a) 6 (b) 8 (a) 100 oC (b) 0 oC
(c) 2 (d) 12 (c) 69 oC (d) 98 oC
28. The shape in which crystals of a substances 40. Which of the following is not a molecular solid?
usually grow is called: (a) Boron Nitride (b) Solid Iodine
(a) Habit of crystal (b) Over –growth (c) Sugar (d) Ice
(c) Allotropy (d) Isotropy 41. The molecules of CO2 in dry ice form the:
29. Ionic solids are characterized by: (a) Covalent crystals (b) Any type of crystal
(a) High vapour pressures (c) Molecular crystals (d) Ionic crystals
(b) Good conductivity in solid state 42. London dispersion forces are also known as:
(c) Solubility in polar solvents (a) Instantaneous dipole-induced dipole forces
(d) Low melting points (b) ion-dipole forces
30. Amorphous solids: (c) dipole-dipole for
(a)Undergo clean cleavage when cut with knife (d) dipole-induced dipole forces
(b)Can possesses small regions of orderly 43. Strength of hydrogen bonding is:
arrangement of atoms (a) 20 times less than covalent bond
(c)Have perfect arrangement of atoms (b) 10 times less than covalent bond
(d)Have sharp melting points (c) 30 times less than covalent bond
31. Metallic luster shown by sodium metal is (d) 40 times less than covalent bond
explained by: 44. Amorphous solid among the following is:
(a) Excitation of free protons (a) Glass (b) Wax
(b) Diffusion of Na+ ion (c) Plastic (d) All of these
(c) Oscillation of loose electron 45. Temperature at which two or more crystalline
(d) Strong crystal lattice form of same substance co –exixts is called:
32. Which substance will conduct current in solid (a) Eutectic temperature
state? (b) Critical temperature
(a) Graphite (b) Nacl (c) Transition temperature
(c) Iodine (d) Diamond (d) Ideal temperature
33. Which of the following is a pseudo solid'? 46. Non –repetitive arrangement of particles is
(a) NaCl (b) CaF2 found in:
(c) Glass (d) All (a) Silver (b) Glass
34. The crystal formed due to London forces of (c) Wax (d) Both b & c
interaction are: 47. Unit cell of NaCl contains:
+1
(a) Covalent (b) Molecular
(a) 6 Na & 6Cl −1 (b) 6 Na
+1
& 4Cl −1
(c) Ionic (d) Metallic +1 −1 +1 −1
35. Dry ice belongs to: (c) 4 Na & 4Cl (d) 4 Na & 6Cl
(a) Molecular solid (b) Ionic solid 48. When water freezes at 0oC, its density
(c) Metallic solid (d) Covalent solid decreases due to:
36. London dispersion forces are the only forces (a) Empty spaces present in the structure of ice
present among the: (b) Change of bond angles
(a) Molecules of water in liquid state (c) Change of bond lengths
(b) Molecules of solid iodine (d) Cubic structure of ice
(c) Molecules of hydrogen chloride gas 49. A solid is likely to be pure if:
(d) None of these (a) It exists in a crystalline form
37. CuSO4.5H2O is an example of crystal system: (b) It dissolve completely in water
(a) Cubic (b) Triclinic (c) It is colourless
(c) Rhomohedral (d) Tetragonal (d) It melts at an exact temperature
38. The intermolecular forces between ions and 50. A crystal is most likely have a low melting
water are: point, if it:
(a) Dipole-induced dipole forces (a) Is a macro molecule
(b) Molecules of Methane (b) Is a crystal lattice
(c) Ion dipole force (c) Has a delocalized valence forces
(d) London dispersion forces (d) Has a weak Vander all’s forces

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 The Spark Institute / The Science Foundation (Solid State)

51. Which of the following solid directly change 59. Select the incorrect statement from the
into vapour on heating? following option.
(a) Ice (b) Sodium chloride (a)Evry pure solid crystalline substance has a
(c) Naphthalene (d) Diamond characteristic and unique melting point
52. Which of the following solids has (have) sharp (b)Ipure sample of substance has different
melting point? melting point
(a) Glass (b) Sodium chloride (c)Two different pure substances have same
(c) Plastic (d) All of these melting points
53. When two substances have same crystal (d)Melting point serves as the criteria of purity of
structure, they are said to be: a solid substance
(a) Polymorphous (b) Isomorphous 60. When the solid and liquid phase are in
(c) Isotopes (d) Isomers equilibrium, the temperature ________
54. Heat energy required to change 1g of a solid (a) Increases gradually
into liquid at its melting is called: (b) Decreases gradually
(a) Molar heat (c) Remains constant
(b) Latent heat to vaporization (d) None of the mentioned
(c) Latent heat of fusion 61. Molar heat of fusion is defined as ________
(d) Ionization enthalpy (a) Energy required to melt one gram of solid
55. When pressure is applied on ice, its melting (b) Energy required to melt one mole of solid
point: (c) Energy required to melt one kilogram of
(a) Increases (b) Decrease solid
(c) Remains constant (d) Remain unchanged (d) Energy required to melt ten moles of solid
56. Identify the dimensional relation for the unit 62. The temperature remains constant during
cell illustrated below. phase change because:
(a) The increased kinetic energy is used to
overcome the cohesive forces in the liquid
(b) Solids always have sharp melting point
(c) In solids each particle is at same distance
along each axis
(d) None of these
63. What is the name of the phase transition that
occurs when a solid is converted directly into a
gas
(a) Melting (b) Boiling
(c) Condensing (d) Sublimation
64. A solid melts sharply just above 80°C & does
(a) a = b = c (b) a = b ≠ c
not conduct electricity even when molten. The
(c) a ≠ b ≠ c (d) a ≠ b = c solid is most likely to be:
57. Which of the following pairs are Isomorphous?
(a)An atomic crystal (b)An ionic crystal
(a) NaF and NaNO3 (b) MgO and NiSO4 (c)A molecular crystal (d)Metallic
(c) NaNO3 and CaCO3 (d) ZnSO4 and NaNO3
65. The crystals formed as a result of Vander
58. Select the correct statement from the following Waal’s interactions are:
options.
(a)Molecular crystals
(a)The transformation of solid to liquid is called (b)Covalent crystals
melting and the reverse process is called
(c)Metallic crystals
freezing (d)Ionic crystals
(b)The transformation of solid to liquid is called
66. When a solute particles accumulates on the
freezing and the reverse process is called surface of a solution the surface tension
melting
(a) Remains unaffected
(c)The transformation of liquid to solid is called (b) Increases
melting and the reverse process is called
(c) Decreases
freezing (d) Keeps on fluctuating
(d)None of the mentioned

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 The Spark Institute / The Science Foundation (Solid State)

67. Which of the following statements is incorrect 78. What is characteristic of amorphous solid?
about amorphous solids? (a) Definite and characteristic enthalpy of
(a) They are anisotropic fusion
(b) They are rigid and incompressible (b) Melt at sharp and characteristic meltin
(c) They melt over a wide range of temperature point
(d) There is no orderly arrangement of particles (c) A definite characteristic geometric shape
68. What is the total number of ions present in one (d) Gradual softening over range of
unit cell of sodium chloride lattice? temperature
(a) 2 (b) 6 (c) 12 (d) 8 79. Which of the following solid is generally volatile
69. ZnS is and have low melting points?
(a) Ionic crystal (b) Covalent crystal (a)Ionic solids (b)Covalent solids
(c) Metallic crystal (d) Molecular crystal (c)Molecular solids (d)Metallic solids
70. The structure of sodium chloride crystal is 80. Which of the following correct list of
(a) Body centered cubic amorphous solids?
(b) Face centered cubic (a) Glass, Wax & Copper sulphate
(c) Square planar (b) Wood, Copper & plastic
(d) Hexagonal (c) Glass, wax & plastic
71. Which of the following does not belong to cubic (d) Plastic, iron & glass
crystal system? 81. A sample of sodium chloride is likely pure of it:
(a) NaCl (b) ZnS (a) Is colorless
(c) Diamond (d) ZnO (b) Completely dissolves in water
72. Which of the following represents the plane of (c) Melt at exact temperature
symmetry? (d) Is crystalline
82. Which of the following is hexagonal crystal
(a) Diamond (b) Graphite
(c) Cane sugar (d) washing soda
83. The site labeled as ‘a’ in fcc arrangement is:

(a)1, 2 & 3 (b)2, 3 & 4

(c)3, 4 & 5 (d)4, 5 & 6
73. Which of the following crystalline solid have no
cleavage plane? (a) Face with ½ contribution
(a)Ionic solids (b)Molecular solids (b) Edge with ¼ contribution
(c)Covalent solids (d)Metallic solids (c) Corner with ¼ contribution
74. Which of the following is correct match? (d) Edge with ½ contribution
(a) Ice –ionic solid 84. Which one of the following statements is
(b) Naphthalene –molecular solids incorrect?
(c) Calcium carbonate –metallic solid (a) coordination number in bcc mode of
(d) Sulphur –network solid packing
75. Density of water is maximum at: is 8
(a)0oC (b)100 oC (c)4 oC (b) coordination number in hcp mode of
(d)25 oC packing
76. Melting point of ice is: is12
(a) Inversely proportional to pressure (c) void space in hcp mode of packing is 32%
(b) Directly proportional to pressure (d) void space in ccp mode of packing is 26%
(c) Independent of pressure 85. Which of the following set contains all network
(d) None of these covalent solids?
77. Which of the following pair shows anisotropy? (a) LiF, solid CO2, diamond
(a)CaF2 & ZnS (b)Glass & charcoal (b) ZnS, silicon, NaCl
(c)Plastic & graphite (d)Diamond & charcoal (c) Diamond, carborundum, NaCl
(d) SiC, graphite, diamond

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 The Spark Institute / The Science Foundation (Solid State)

86. Percent packing fraction of hcp is: 96. Match List I with List II and select the correct
(a) 74% (c) 68% answer:
(b) 26% (d) 78% List I List II
87. The cubic unit cell which possesses particles at shape Radius ratio
only corners is called: 1.BCC (I) 0.414
(a)simple cubic
2.Tetrahedral (II) 0.732
(b)body-centered cubic
3. Octahedral (III) 0.93
(c)face-centered cubic
(d)both body- and face-centered cubic 1 2 3
88. The positions of Cl- ions in NaCl structure are: (a) (I) (II) (III)
(a)corners of the cube (b) (III) (I) (II)
(b)face centers of the cube (c) (II) (III) (I)
(c)edge centers of the cube (d) (III) (II) (I)
(d)both a and b 97. In closest packing of atoms, the number of
89. The range of radius ratio (cationic to anionic) atoms surrounding an atom in one layer is
for an tetrahedral arrangement of ions in an (a) 2 (b) 4 (c) 6 (d) 8
ionic solid is 98. In an ionic structure, the radius ratio, rc/ra, is
(a) 0 – 0.155 (b) 0.155 – 0.225 0.66. The expected arrangement of anions
(c) 0.225 – 0.414 (d) 0.414 – 0.732 around a cation is
90. Which of the following exists as molecular (a) Cubic (b) Octahedral
crystals in the solid state? (c) Tetrahedral (d) Triangular
(a)Potassium nitrate (b)Coal 99. Which of the following statements is not
(c)Sulphur (d)Gold correct?
91. In general, a crystal shows cleavage in a (a)The molecular crystals are soft and possess
pattern, which is specific for that type of comparatively low melting points.
crystal. This is because the atoms and (b)The ionic crystals have high melting points.
molecules or ions in a crystal are: (c)Covalent crystals are good conductor of
(a)Arranged in planes heat and electricity.
(b)Spherically symmetrical (d)Metallic crystals are ductile and malleable.
(c)Bonded together strongly 100. Total number of sodium ions and chloride ions
(d)Bonded together weakly present in FCC structure of NaCl is:
92. Which of the following is not a characteristic of (a) 4 (b) 2 (c) 8 (d) 1
solids? 101. Which of the followings is incorrect statement?
(a)Definite shape (a)Isomorphs have same physical properties
(b)Definite mass and volume (b)Isomorphs possess different chemical
(c)Frequent fluidity composition
(d)Rigidity (c)Isomorphs have tendency of overgrowth
93. Which of the following is/are pseudo solids? (d)Isomorphs have same empirical ratio of
I. KCl atoms
II. Barium chloride dihydrate 102. Melting point of most of the solids increases
III. Rubber with:
IV. Solid cake left after distillation of coal tar (a)Decrease in pressure
(a) I, III (b) II, III (b)Decrease in intermolecular forces
(c) III, IV (d) only III (c)Increase in pressure
94. Which of the following pairs has non-metallic (d)None of these
crystalline solids? 103. Potassium dichromate exists in
(a) Copper, Chromium (a) Cubic system
(b) Chromium, Wood (b) Triclinic system
(c) Mercury, Calcium (c) Tetrahedral system
(d) Rock salt, Sodium nitrate (d) Monoclinic system
95. MgO is isomorph of 104.In which of the following crystal system one
(a) Sodium nitrate angle is always 120o?
(b) Zinc sulfate (a) Cubic (b) Tetragonal
(c) Calcium carbonate (c) Orthorhombic (d) Hexagonal
(d) Sodium fluoride

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 The Spark Institute / The Science Foundation (Solid State)

105. Iron is an example of 113. Which of the following is true about the value of
(a) Crystalline solid (b) Pseudo solid refractive index of quartz glass?
(c) Amorphous solid (d) All of these (a) Same in all directions
106. When substance moves from a solid to a liquid (b) Different in different directions
state all of the following changes occur except. (c) Cannot be measured
(a)Molecules becomes more disordered (d) Always zero
(b)K.E of molecule decrease 114. AB ABA… represents an arrangement of layers
(c)Intermolecular force becomes weaker called
(d)Molecule becomes further separated (a) Cubic closed packing
107. The sharp melting point of crystalline solids is (b) Fluorite closed packing
due to (c) Hexagonal closed packing
(a) A regular arrangement of constituent (d) Body-centred cubic packing
particles observed over a short distance in the 115. The melting point of most of the solid
crystal lattie. substances increase with an increase of
(b) A regular arrangement of constituent pressure. However, ice melts at a temperature
particles observed over a long distance in the lower than its usual melting point when the
crystal lattice. pressure is increase(d)This is because:
(c) Same arrangement of constituent particles (a) Ice is less dense than water
in different directions. (b) Pressure generates heat
(d) Different arrangement of constituent (c) The chemical bonds break under pressure
particles in different directions. (d) Ice is not a true solid
108. Iodine molecules are held in the crystals lattice 116. Amount of heat added at the melting point of
by liquid
(a) London forces (a)Increases the temperature of liquid
(b) Dipole-dipole interactions (b)Increases the kinetic energy of molecules
(c) Covalent bonds (c)Decreases the intermolecular forces between
(d) Coulombic forces the molecules
109. Which of the following is not the characteristic (d)Increases the intermolecular forces between
of ionic solids? the molecules
(a) Electrical conductivity in the molten state. 117. Which of the following is Isomorph of NaNO3?
(b) Brittle nature. (a) NaCl
(c) Very strong forces of interactions. (b) ZnSO4
(d) Anisotropic nature. (c) CaCO3
110. The lattice site in a pure crystal cannot be (d) MgO
occupied by : 118. BaSO4.4H2O is exists in
(a) Molecule (b) Ion (a)Cubic system
(c) Electron (d) Atom (b)Triclinic system
111. Which of the following conditions favours the (c)Monoclinic system
existence of a substance in the solid state? (d)None of these
(a) High temperature
(b) Low temperature
(c) High thermal energy
(d) Weak cohesive forces
112. Which of the following is not a characteristic of
a crystalline solid?
(a)Definite and characteristic heat of fusion.
(b)Isotropic nature
(c)A regular periodically repeated pattern of
arrangement of constituent particles in the
entire crystal
(d)A true solid

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 The Spark Institute / The Science Foundation (Solid State)

1 C 31 C 61 - 91 A

2 C 32 A 62 A 92 C

3 C 33 C 63 D 93 C

4 C 34 B 64 C 94 D

5 B 35 B 65 A 95 D

6 B 36 C 66 C 96 -

7 C 37 C 67 A 97 C

8 C 38 A 68 D 98 B

9 C 39 C 69 A 99 C

10 B 40 A 70 B 100 A

11 B 41 C 71 D 101 A

12 C 42 A 72 D 102 C

13 B 43 B 73 D 103 B

14 D 44 D 74 B 104 D

15 A 45 C 75 C 105 A

16 C 46 D 76 A 106 B

17 B 47 A 77 A 107 B

18 B 48 A 78 D 108 A

19 C 49 D 79 C 109 A

20 C 50 D 80 C 110 C

21 C 51 C 81 C 111 B

22 A 52 B 82 B 112 B

23 D 53 B 83 B 113 B

24 C 54 B 84 C 114 C

25 D 55 B 85 D 115 A

26 C 56 C 86 A 116 C

27 A 57 C 87 A 117 C

28 A 58 A 88 D 118 C

29 C 59 C 89 C

30 B 60 - 90 C

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