JEE Main & Advanced Chemistry The Solid State / ठोस प्रावस्था Sample Paper

done Topic Test - Solid State Total Questions - 35    [Download]

• question_answer1)
  A solid AB has NaCl structure. If the radius of action \[{{A}^{+}}\] is 170 pm, calculate the maximum possible radius of the anion \[{{B}^{-}}\]
  A)
  210.3 pm
  done clear
  B)
  397.4 pm
  done clear
  C)
  410.6 pm
  done clear
  D)
  347.9 pm
  done clear
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• question_answer2)
  If NaCl is doped with mol% \[SrC{{l}_{2}},\] what is the concentration of cation vacancies?
  A)
   \[6.02\times {{10}^{18}}mo{{l}^{-1}}\]
  done clear
  B)
  \[6.02\times {{10}^{19}}mo{{l}^{-1}}\]
  done clear
  C)
  \[6.02\times {{10}^{23}}mo{{l}^{-1}}\]
  done clear
  D)
  \[6.02\times {{10}^{26}}mo{{l}^{-1}}\]
  done clear
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• question_answer3)
  In a cubic dosed packed structure of mixed oxides, the lattice is made up of oxide ions, one eighth of tetrahedral/voids are occupied by divalent ions \[({{A}^{2+}}),\] while one half of the octahedral voids are occupied by trivalent ions \[({{B}^{3+}})\]. What is the formula of the oxide?
  A)
  \[{{A}_{3}}{{B}_{2}}{{O}_{4}}\]
  done clear
  B)
  \[{{A}_{2}}{{B}_{2}}{{O}_{4}}\]
  done clear
  C)
  \[A{{B}_{2}}{{O}_{5}}\]
  done clear
  D)
  \[A{{B}_{2}}{{O}_{4}}\]
  done clear
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• question_answer4)
  The composition of sample of wustite is \[F{{e}_{0.93}}{{O}_{1.00}}\]. What percentage of the iron is present in the form of Fe (III)?
  A)
  14%
  done clear
  B)
  15.05%
  done clear
  C)
  17%
  done clear
  D)
  29%
  done clear
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• question_answer5)
  In fcc lattice, A, B, C, D atoms are arranged at corners, face centres, octahedral voids and tetrahedral voids respectively, then the body diagonal contains
  A)
  2A, C, 2D
  done clear
  B)
  2A, 2B, 2C
  done clear
  C)
  2A, 2B, D
  done clear
  D)
  2A, 2D
  done clear
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• question_answer6)
  Which of the following order is correct regarding size of the voids.
  A)
  Octahedral < tetrahedral < square planar < trigonal
  done clear
  B)
  trigonal < tetrahedral = square planar < octahedral
  done clear
  C)
  trigonal < tetrahedral < square planar = octahedral
  done clear
  D)
  tetrahedral < trigonal = square planar <octahedral
  done clear
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• question_answer7)
  In which of the following unit cells all sides and all angles are equal? Cubic (I), Tetragonal (II), Orthorhombic (III), Rhombohedra (IV)
  A)
  I and II
  done clear
  B)
  I            
  done clear
  C)
  I and III
  done clear
  D)
  I and IV
  done clear
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• question_answer8)
  Which of the following represents correct order of conductivity in solids?
  A)
  \[{{\kappa }_{\text{metals}}}>>{{\kappa }_{\text{insulators}}}<{{\kappa }_{\text{semiconductors}}}\]
  done clear
  B)
  \[{{\kappa }_{\text{metals}}}<<{{\kappa }_{\text{insulators}}}<{{\kappa }_{\text{semiconductors}}}\]
  done clear
  C)
  \[{{\kappa }_{\text{metals}}};{{\kappa }_{\text{semiconductors}}}<{{\kappa }_{\text{insulators}}}=\text{zero}\]
  done clear
  D)
  \[{{\kappa }_{\text{metals}}}<{{\kappa }_{\text{semiconductors}}}>{{\kappa }_{\text{insulators}}}\ne \text{zero}\]
  done clear
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• question_answer9)
  Match the type of packing given in Column-I with the items given in Column-II.

  Column-I	Column-II
  [a] Square close packing two dimensions	(1) Triangular voids
  [b] Hexagonal close packing in two dimensions	(2) Pattern of sphere is repeated in every fourth layer.
  [c] Hexagonal close packing in three dimensions	(3) Coordination number 4
  [d] Cubic close packing in three dimensions	(4) Pattern of sphere is repeated in alternate layers.

  A)
  A-3, B-1, C-4, D-2
  done clear
  B)
  A-1, B-2, C-3, D-4
  done clear
  C)
  A-3, B-2, C-1, D-4
  done clear
  D)
  A-4, B-3, C-2, D-1
  done clear
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• question_answer10)
  Ferrous oxide has a cubic structure and each edge of the unit cell is \[5.0\text{ }{{A}^{o}}\]. Assuming density of the oxide as \[4.0\text{ }g\text{ }c{{m}^{-3}}\] the number of \[F{{e}^{2+}}\] and \[{{O}^{2-}}\] ions present in each unit cell will be
  A)
  two \[F{{e}^{2+}}\] and four \[{{O}^{2-}}\]
  done clear
  B)
  three \[F{{e}^{2+}}\] and three \[{{O}^{2-}}\]
  done clear
  C)
  four \[F{{e}^{2+}}\] and two \[{{O}^{2-}}\]
  done clear
  D)
  four \[F{{e}^{2+}}\] and four \[{{O}^{2-}}\]
  done clear
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• question_answer11)
  Which solid will have the weakest intermolecular forces?
  A)
  Ice
  done clear
  B)
  Phosphorus
  done clear
  C)
  Naphthalene
  done clear
  D)
  Sodium fluoride
  done clear
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• question_answer12)
  In normal spinel structures \[MgA{{l}_{2}}{{O}_{4}},\] the percentage of tetrahedral void occupied is
  A)
  12.5%
  done clear
  B)
  25%      
  done clear
  C)
  50%
  done clear
  D)
  None of these
  done clear
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• question_answer13)
  \[ZnO\] is white when cold and yellow when heated. It is due to the development of
  A)
  Frenkel defect                
  done clear
  B)
  Schottky defect
  done clear
  C)
  Metal excess defect                     
  done clear
  D)
  Metal deficiency defect
  done clear
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• question_answer14)
  A ferromagnetic substance becomes a permanent magnet when it is placed in a magnetic field because
  A)
  all the domains get oriented in the direction of magnetic field
  done clear
  B)
  all the domains get oriented in the direction opposite to the direction of magnetic field
  done clear
  C)
  domains get oriented randomly
  done clear
  D)
  domains are not affected by magnetic field
  done clear
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• question_answer15)
  A metallic element has a cubic lattice. Each edge of the unit cell is \[2{{A}^{0}}\]. The density of the metal is \[2\text{ }g\text{ }c{{m}^{-3}}\]. The unit cells in 200 g of the metal are
  A)
  \[1\times {{10}^{25}}\]
  done clear
  B)
  \[1\times {{10}^{24}}\]
  done clear
  C)
  \[1\times {{10}^{22}}\]
  done clear
  D)
  \[1\times {{10}^{20}}\]
  done clear
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• question_answer16)
  Which of following is an example of ionic crystalline solid?
  A)
  Diamond
  done clear
  B)
  LiF
  done clear
  C)
  Li
  done clear
  D)
  Silicon
  done clear
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• question_answer17)
  Which of the following statements about amorphous solids
  A)
  They melt over a range of temperature
  done clear
  B)
  They are isotropic
  done clear
  C)
  There is no orderly arrangement of particles
  done clear
  D)
  They are rigid and incompressible
  done clear
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• question_answer18)
             

  DIRECTION: Read the passage given below and answer the questions that follows:

  In hexagonal systems of crystals, a frequently encountered arrangement of atoms is described as a hexagonal prism. Here, the top and bottom of the cell are regular hexagons and three atoms sandwiched in between them. A space-of this model of this structure, called hexagonal close-packed (HCP), is constituted of a sphere on a flat surface surrounded in the same plane by six identical spheres as closely as possible. There spheres are then placed over the first layer so that they touch each other and represent the second layer. Each one of these three spheres touches three spheres of the bottom layer. Finally, the second layer is covered with third layer that is identical to the bottom layer in relative position. Assume radius of every sphere to be 'r'.

  The number of atoms in the HCP unit cell is

  A)
  4
  done clear
  B)
  6
  done clear
  C)
  12
  done clear
  D)
  17
  done clear
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• question_answer19)
             

  DIRECTION: Read the passage given below and answer the questions that follows:

  In hexagonal systems of crystals, a frequently encountered arrangement of atoms is described as a hexagonal prism. Here, the top and bottom of the cell are regular hexagons and three atoms sandwiched in between them. A space-of this model of this structure, called hexagonal close-packed (HCP), is constituted of a sphere on a flat surface surrounded in the same plane by six identical spheres as closely as possible. There spheres are then placed over the first layer so that they touch each other and represent the second layer. Each one of these three spheres touches three spheres of the bottom layer. Finally, the second layer is covered with third layer that is identical to the bottom layer in relative position. Assume radius of every sphere to be 'r'.

  The volume of  this HCP units cell is-

  A)
  \[24\sqrt{2}{{r}^{3}}\]
  done clear
  B)
  \[16\sqrt{2}{{r}^{3}}\]
  done clear
  C)
  \[12\sqrt{2}{{r}^{3}}\]
  done clear
  D)
  \[\frac{64}{3\sqrt{3}}{{r}^{3}}\]
  done clear
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• question_answer20)
             

  DIRECTION: Read the passage given below and answer the questions that follows:

  In hexagonal systems of crystals, a frequently encountered arrangement of atoms is described as a hexagonal prism. Here, the top and bottom of the cell are regular hexagons and three atoms sandwiched in between them. A space-of this model of this structure, called hexagonal close-packed (HCP), is constituted of a sphere on a flat surface surrounded in the same plane by six identical spheres as closely as possible. There spheres are then placed over the first layer so that they touch each other and represent the second layer. Each one of these three spheres touches three spheres of the bottom layer. Finally, the second layer is covered with third layer that is identical to the bottom layer in relative position. Assume radius of every sphere to be 'r'.

  The empty space in this HCP unit cell is

  A)
  74%
  done clear
  B)
  47.6%
  done clear
  C)
  32%
  done clear
  D)
  26%
  done clear
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• question_answer21)
  Iron crystallizes in several-modifications. At about \[910{}^\circ C\] 'bcc' form (called \[\alpha -\]form) undergoes transitions, to \[\gamma -\]form with 'fcc' lattice. Assuming that the distance between the nearest neighbors is the same in the two forms at the transition temperature, calculate the ratio of the density of \[\gamma -\]ron to that of \[\alpha -\]iron at the transition temperature.
  A)
  0.0887
  done clear
  B)
  1.0887
  done clear
  C)
  1.546
  done clear
  D)
  1.544
  done clear
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• question_answer22)
  How many unit cells are present in a cube-shaped ideal crystal of \[NaCl\] of mass 1.00g? [Atomic masses: Na = 23, Cl = 35.5]
  A)
  \[2.57\times {{10}^{21}}\] unit cells      
  done clear
  B)
  \[5.14\times {{10}^{21}}\] unit cells
  done clear
  C)
  \[1.28\times {{10}^{21}}\] unit cells
  done clear
  D)
  \[1.71\times {{10}^{21}}\] unit cells
  done clear
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• question_answer23)
  A metal crystallizes into two cubic phases, face centred cubic (fee) and body centred cubic (bcc) whose unit cell lengths are 3.5 and \[3.0\,\overset{o}{\mathop{A}}\,\] respectively. Calculate the ratio of the densities of fee and bee.
  A)
  1.67
  done clear
  B)
  1.26
  done clear
  C)
  6.23
  done clear
  D)
  1.04
  done clear
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• question_answer24)
  A compound formed by elements A and B has a cubic structure in which A atoms are at the comers of the cube and B atoms are at the face centres. The formula for the compound is
  A)
  \[{{A}_{2}}{{B}_{3}}\]
  done clear
  B)
  \[A{{B}_{3}}\]
  done clear
  C)
  \[{{A}_{3}}B\]
  done clear
  D)
  \[{{A}_{3}}{{B}_{2}}\]
  done clear
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• question_answer25)
  When heated above \[916{}^\circ C,\] iron changes its bcc crystalline form to fcc without the change in the radius of atom. The ratio of the density of the crystal before heating and after heating is:
  A)
  1.069
  done clear
  B)
  0.918
  done clear
  C)
  0.725
  done clear
  D)
  1.231
  done clear
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• question_answer26)
  The first three nearest neighbor distance for primitive cubic lattice are respectively (edge length of unit cell = a):
  A)
  \[a,\,\sqrt{2}a,\sqrt{3}a\]
  done clear
  B)
  \[\sqrt{3}a,\,\sqrt{2}a,\,a\]
  done clear
  C)
  \[a,\,\sqrt{2}a,2\,a\]
  done clear
  D)
  \[a,\,\sqrt{3}a,2\,a\]
  done clear
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• question_answer27)
  A crystal is made of particles A and B. A forms fcc packing and B occupies all the octahedral voids. If all the particles along the plane as shown in the figure are removed, then the formula of the crystal would be:
  A)
  \[AB\]
  done clear
  B)
  \[{{A}_{5}}{{B}_{7}}\]
  done clear
  C)
  \[{{A}_{7}}{{B}_{5}}\]
  done clear
  D)
  none of these 
  done clear
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• question_answer28)
  Schottky defect in crystals is observed when
  A)
  unequal number of cations and anions are missing from the lattice.
  done clear
  B)
  equal number of cations and anions are missing from the lattice.
  done clear
  C)
  an ion leaves its normal site and occupies an interstitial site.
  done clear
  D)
  density of the crystal is increased
  done clear
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• question_answer29)
  List-I and List-II contains four entries each. Entries of List-I are to be matched with some entries of List-II. One or more than one entries of List-I may have the matching with the same entries of List-II.

  List-I	List-II
  [a] Rock salt structure	(p) General formula is AB
  [b] Zinc blende structure	(q) General formula is \[A{{B}_{3}}\]
  [c] Fluorite structure	(r) General formula is \[{{A}_{2}}B\]
  [d] Anti fluorite structure	(s) General formula is \[A{{B}_{2}}\]

  A)
  A-p, B-p, C-s, D-r                
  done clear
  B)
  A-q, B-q, C-p, D-s
  done clear
  C)
  A-r, B-p, C-r, D-s               
  done clear
  D)
  A-s, B-s, C-p, D-q
  done clear
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• question_answer30)
  In hexagonal close packing of sphere in three dimensions, which of the following statements is correct.
  A)
  In one unit cell there are 12 octahedral voids and all are completely inside the unit cell.
  done clear
  B)
  In one unit cell there are six octahedral voids and all are completely inside the unit cell.
  done clear
  C)
  In one unit cell there are six octahedral void and of which three are completely inside the unit cell and other three are partially inside the unit cell.
  done clear
  D)
  In one unit cell there are 12 tetrahedral voids, all are completely inside the unit cell.
  done clear
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• question_answer31)
  Percent of octahedral voids vacant in a perfect crystal of ZnS is
  A)
  0%
  done clear
  B)
  50%
  done clear
  C)
  100%
  done clear
  D)
  25%
  done clear
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• question_answer32)
  Lithium borohydride crystallizes in an orthorhombic system with 4 molecules per unit cell. The unit cell dimensions are \[a=6.8\text{ }\overset{o}{\mathop{A}}\,,\,b=4.4\overset{o}{\mathop{A}}\,\] and \[c=7.2\overset{o}{\mathop{A.}}\,\] If the molar mass is 21.76, then the density of crystals is:
  A)
  \[0.6708\text{ }g\text{ }c{{m}^{-2}}\]
  done clear
  B)
  \[1.6708\text{ }g\text{ }c{{m}^{-3}}\]
  done clear
  C)
  \[2.6708\text{ }g\,\,c{{m}^{-3}}\]
  done clear
  D)
  None of these.
  done clear
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• question_answer33)
  Column A describes nature of bonding and Column B the solid having that type of bonding:

  A (Nature of bonding)	B (solid)
  I. Van der Waals	P. Al, Cd
  II. Ionic	Q. \[C{{O}_{2}},{{H}_{2}}\]
  III. Metallic	R. Si diamond
  IV. Covalent	S. \[MgO,NaCl\]

  Correct matching of A and B is in alternate:
  A)
  I-P, II-Q, III-R, IV-S                 
  done clear
  B)
  I-Q, II-S, III-P, IV-R
  done clear
  C)
  I-Q, II-P, III-R, IV-S                 
  done clear
  D)
  I-S, II-P, III-Q, IV-R
  done clear
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• question_answer34)
  A crystalline solid:
  A)
  changes abruptly from solid to liquid when heated
  done clear
  B)
  has no definite melting point
  done clear
  C)
  undergoes deformation of its geometry easily
  done clear
  D)
  has an irregular three-dimensional arrangements
  done clear
  E)
  softens slowly
  done clear
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• question_answer35)
  Select the right expression for determining packing fraction (PF) of \[NaCl\] unit cell (assume ideal), if ions along an edge diagonal are absent
  A)
  \[PF=\frac{\frac{4}{3}\pi \left( r_{+}^{3}+r_{-}^{3} \right)}{16\sqrt{2}r_{-}^{3}}\]
  done clear
  B)
  \[PF=\frac{\frac{4}{3}\pi \left( \frac{5}{3}r_{+}^{3}+4r_{-}^{3} \right)}{16\sqrt{2}r_{-}^{3}}\]
  done clear
  C)
  \[PF=\frac{\frac{4}{3}\pi \left( \frac{5}{2}r_{+}^{3}+r_{-}^{3} \right)}{16\sqrt{2}r_{-}^{3}}\]
  done clear
  D)
  \[PF=\frac{\frac{4}{3}\pi \left( \frac{7}{2}r_{+}^{3}+r_{-}^{3} \right)}{16\sqrt{2}r_{-}^{3}}\]
  done clear
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