Solved papers for NEET Chemistry NEET PYQ-The Solid State

done NEET PYQ-The Solid State Total Questions - 34

• question_answer1) Schottky defect in crystals is observed when: [AIPMT 1998]
  A)
  an ion leaves its normal site and occupies an interstitial site
  done clear
  B)
  unequal number of cations and anions are missing from the lattice
  done clear
  C)
  density of the crystal is increased
  done clear
  D)
  equal number of cations and anions are missing from the lattice
  done clear
  View Answer play_arrow

• question_answer2) The edge length of face centred unit cubic cell is 508 pm. If the radius of the cation is 110 pm, the radius of the anion is:                [AIPMT 1998]
  A)
  288 pm
  done clear
  B)
  398 pm
  done clear
  C)
  144 pm
  done clear
  D)
  618 pm
  done clear
  View Answer play_arrow

• question_answer3) The second order Bragg diffraction of X-rays with \[\lambda =1.0\,\overset{\text{o}}{\mathop{\text{A}}}\,\]  from a set of parallel planes in a metal occurs at an angle \[60{}^\circ \]. The distance between the scattering planes in the crystals is: [AIPMT 1998]
  A)
  \[0.575\,\overset{o}{\mathop{A}}\,\]
  done clear
  B)
  \[1.00\,\overset{o}{\mathop{A}}\,\]
  done clear
  C)
  \[2.00\,\overset{o}{\mathop{A}}\,\]
  done clear
  D)
  \[1.17\,\overset{o}{\mathop{A}}\,\]
  done clear
  View Answer play_arrow

• question_answer4) In crystals of which of the following ionic compounds would you expect maximum distance between centres of cations and anions? [AIPMT 1998]
  A)
  LiF
  done clear
  B)
  CsF
  done clear
  C)
  Csl
  done clear
  D)
  Lil
  done clear
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• question_answer5) A compound formed by elements A and B crystallises in the cubic structure where A atoms are at the comers of a cube and B atoms are at the face centres. The formula of die compound is: [AIPMT 2000]  
  A)
  \[{{A}_{2}}{{B}_{2}}\]
  done clear
  B)
  \[A{{B}_{3}}\]
  done clear
  C)
  AB 
  done clear
  D)
  \[{{A}_{3}}B\]
  done clear
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• question_answer6) Zn convert its melted state to its solid state, it has hcp structure then find out number of nearest atom:[AIPMT 2001]
  A)
  6
  done clear
  B)
  8
  done clear
  C)
  12
  done clear
  D)
  4
  done clear
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• question_answer7) The pyknometric density of sodium chloride crystal is \[2.165\times {{10}^{3}}kg{{m}^{-3}}\] while its X-ray density is \[2.178\times {{10}^{3}}kg\text{ }{{m}^{-3}}\]. The fraction of unoccupied sites in sodium chloride crystal is: [AIPMT 2003]
  A)
        \[5.96\times {{10}^{-1}}\]
  done clear
  B)
  \[5.96\times {{10}^{-3}}\]
  done clear
  C)
  5.96
  done clear
  D)
  \[5.96\times {{10}^{-2}}\]
  done clear
  View Answer play_arrow

• question_answer8) A compound formed by elements X and Y crystallizes in a cubic structure in which the X atoms are at the comers of a cube and the Y atoms are at the face-centres. The formula of the compound is:
  A)
  \[X{{Y}_{3}}\]
  done clear
  B)
  \[{{X}_{3}}Y\]
  done clear
  C)
  XY
  done clear
  D)
  \[X{{Y}_{2}}\]
  done clear
  View Answer play_arrow

• question_answer9) In a face-centered cubic lattice, a unit cell is shared equally by how many unit cells? [AIPMT (S) 2005]
  A)
  8
  done clear
  B)
  4         
  done clear
  C)
  2
  done clear
  D)
  6
  done clear
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• question_answer10) CsBr crystallises in a body centred cubic lattice. The unit cell length is 436.6 pm. Given that the atomic mass of Cs = 133 and that of Br = 80 amu and Avogadro number being \[6.02\times {{10}^{23}}\]\[mo{{l}^{-1}}\], the density of CsBr is:[AIPMT (S) 2006]
  A)
  \[42.5\text{ }g/c{{m}^{3}}\]
  done clear
  B)
  \[0.425\text{ }g/c{{m}^{3}}\]
  done clear
  C)
  \[8.25\text{ }g/c{{m}^{3}}\]
  done clear
  D)
  \[4.25\text{ }g/c{{m}^{3}}\]
  done clear
  View Answer play_arrow

• question_answer11) The fraction of total volume occupied by the atoms present in a simple cube is: [AIPMT (S) 2007]
  A)
  \[\frac{\pi }{6}\]
  done clear
  B)
  \[\frac{\pi }{3\sqrt{2}}\]
  done clear
  C)
  \[\frac{\pi }{4\sqrt{2}}\]
  done clear
  D)
   \[\frac{\pi }{4}\]
  done clear
  View Answer play_arrow

• question_answer12) If NaCl is doped with \[{{10}^{-4}}mol\text{ }%\] of \[SrC{{l}_{2}},\] the concentration of cation vacancies will be \[({{N}_{A}}=6.02\times {{10}^{23}}mo{{l}^{-1}})\]:                [AIPMT (S) 2007]
  A)
  \[6.02\times {{10}^{15}}mo{{l}^{-1}}\]
  done clear
  B)
  \[6.02\times {{10}^{16}}mo{{l}^{-1}}\]
  done clear
  C)
  \[6.02\times {{10}^{17}}mo{{l}^{-1}}\]
  done clear
  D)
  \[6.02\times {{10}^{14}}mo{{l}^{-1}}\]
  done clear
  View Answer play_arrow

• question_answer13) Which of the following statements is not correct? [AIPMT (S) 2008]
  A)
  The fraction of the total volume occupied by the atoms in a primitive cell is 0.48
  done clear
  B)
  Molecular solids are generally volatile
  done clear
  C)
  The number of carbon atoms in an unit cell of diamond is 4
  done clear
  D)
  The number of Bravais lattices in which a crystal can be categorized is 14
  done clear
  View Answer play_arrow

• question_answer14) If ‘a’ stands for the edge length of the cubic systems: simple cubic, body centred cubic and face centred cubic, then the ratio of radii of the spheres in these systems will be respectively, [AIPMT (S) 2008]
  A)
  \[\frac{1}{2}a;\frac{\sqrt{3}}{4}a:\frac{1}{2\sqrt{2}}a\]
  done clear
  B)
  \[\frac{1}{2}a;\sqrt{3}a:\frac{1}{\sqrt{2}}a\]
  done clear
  C)
  \[\frac{1}{2}a:\frac{\sqrt{3}}{2}a:\frac{\sqrt{2}}{2}a\]
  done clear
  D)
  \[1a:\sqrt{3}a:\sqrt{2}a\]
  done clear
  View Answer play_arrow

• question_answer15) Percentage of free space in a body centred cubic unit cell is                   [AIPMT (S) 2008]
  A)
  30%
  done clear
  B)
  32%     
  done clear
  C)
  34%
  done clear
  D)
  28%
  done clear
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• question_answer16) With which one of the following elements silicon should be doped so as to give p-type of semiconductor?                            [AIPMT (S) 2008]
  A)
  Germanium
  done clear
  B)
  Arsenic
  done clear
  C)
  Selenium
  done clear
  D)
  Boron
  done clear
  View Answer play_arrow

• question_answer17) 

  Consider the following reaction     [AIPMT (S) 2009]

  \[\text{Phenol}\,\xrightarrow[{}]{\text{Zndust}}X\xrightarrow[\text{Anhydrous }AlC{{l}_{3}}]{C{{H}_{3}}Cl}Y\xrightarrow[{}]{\text{Alkaline }KMn{{O}_{4}}}Z,\]     the product Z is

  A)
  toluene
  done clear
  B)
  benzaldehyde
  done clear
  C)
  benzoic acid
  done clear
  D)
  benzene
  done clear
  View Answer play_arrow

• question_answer18) With a unit cell length of 361 pm. What is the radius of copper atom in pm? [AIPMT (S) 2009]
  A)
  128
  done clear
  B)
  157
  done clear
  C)
  181
  done clear
  D)
  198 
  done clear
  View Answer play_arrow

• question_answer19) Lithium metal crystallises in a body centred cubic crystal. If the length of the side of the unit cell of lithium is 351 pm, the atomic radius of the lithium will be                                       [AIPMT (S) 2009]
  A)
  240.8pm
  done clear
  B)
  151.8pm
  done clear
  C)
  75.5pm
  done clear
  D)
  300.5pm
  done clear
  View Answer play_arrow

• question_answer20) AB crystallizes in a body centred cubic lattice with edge length 'a' equal to 387 pm. The distance between two oppositively charged ions in the lattice is                                       [AIPMT (S) 2010]
  A)
  335 pm
  done clear
  B)
  250 pm
  done clear
  C)
  200 pm
  done clear
  D)
  300 pm
  done clear
  View Answer play_arrow

• question_answer21) A solid compound XY has \[NaCl\] structure. If the radius of the cation is 100 pm, the radius of the anion \[({{Y}^{-}})\] will be             [AIPMT (M) 2011]
  A)
  275.1pm
  done clear
  B)
  322.5 pm
  done clear
  C)
  241.5 pm
  done clear
  D)
  165.7 pm
  done clear
  View Answer play_arrow

• question_answer22) A metal crystallizes with a face-centered cubic lattice. The edge of the unit cell is 408 pm. The diameter of the metal atom is [AIPMT (S) 2012]
  A)
  288 pm
  done clear
  B)
  408 pm
  done clear
  C)
  144 pm
  done clear
  D)
  204 pm
  done clear
  View Answer play_arrow

• question_answer23) The number of octahedral void(s) per atom present in a cubic close-packed structure is [AIPMT (S) 2012]
  A)
  1
  done clear
  B)
  3
  done clear
  C)
  2
  done clear
  D)
  4
  done clear
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• question_answer24) Structure of a mixed oxide is cubic close packed (ccp). The cubic unit cell of mixed oxide is composed of oxide ions. One fourth of the tetrahedral voids are occupied by divalent metal A and the octahedral voids are occupied by a monovalent metal B. The formula of the oxide is                                 [AIPMT (M) 2012]
  A)
  \[AB{{O}_{2}}\]
  done clear
  B)
  \[{{A}_{2}}B{{O}_{2}}\]
  done clear
  C)
  \[{{A}_{2}}{{B}_{3}}{{O}_{4}}\]
  done clear
  D)
  \[A{{B}_{2}}{{O}_{2}}\]
  done clear
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• question_answer25) A metal has a fee lattice. The edge length of the unit cell is 404 pm. The density of the metal is 2.72 g \[c{{m}^{-3}}\]. The molar mass of the metal is            (\[{{N}_{A}}\]Avogadro's constant \[=6.02\times {{10}^{23}}mo{{l}^{-1}}\])                                       [NEET 2013]
  A)
                    \[40\,g\,mo{{l}^{-1}}\]
  done clear
  B)
  \[30\,g\,mo{{l}^{-1}}\]
  done clear
  C)
  \[27\,g\,mo{{l}^{-1}}\]
  done clear
  D)
  \[20\,g\,mo{{l}^{-1}}\]
  done clear
  View Answer play_arrow

• question_answer26) If a is the length of the side of a cube, the distance between the body centered atom and one corner atom in the cube will be                        [AIPMT 2014]
  A)
  \[\frac{2}{\sqrt{3}}a\]
  done clear
  B)
  \[\frac{4}{\sqrt{3}}a\]
  done clear
  C)
  \[\frac{\sqrt{3}}{4}a\]
  done clear
  D)
  \[\frac{\sqrt{3}}{2}a\]
  done clear
  View Answer play_arrow

• question_answer27) A given metal crystallises out with a cubic structure having edge length of 361 pm. If there are four metal atoms in one unit cell, what is the radius of one atom?          [NEET 2015 ]
  A)
  40 pm
  done clear
  B)
  127 pm
  done clear
  C)
  80 pm
  done clear
  D)
  108 pm
  done clear
  View Answer play_arrow

• question_answer28) The vacant space in bcc lattice cell is [NEET 2015 (Re)]
  A)
  26%
  done clear
  B)
  48%     
  done clear
  C)
  23%
  done clear
  D)
  32%
  done clear
  View Answer play_arrow

• question_answer29) Lithium has a bcc structure. Its density is \[530\,kg\,{{m}^{-3}}\] and its atomic mass is \[6.94\text{ }g\text{ }mo{{l}^{1~}}\]. Calculate the edge length of a unit cell of Lithium metal. \[({{N}_{A}}=\text{ }6.02\text{ }\times \text{ }{{10}^{23}}\text{ }mo{{l}^{1}})\][NEET - 2016]
  A)
  154 pm
  done clear
  B)
  352 pm
  done clear
  C)
  527 pm
  done clear
  D)
  264 pm
  done clear
  View Answer play_arrow

• question_answer30) The ionic radii of \[{{A}^{+}}\] and \[{{B}^{-}}\] ions are \[0.98\times {{10}^{-10}}m\] and \[1.81\times {{10}^{10}}\text{ }m\]. The coordination number of each ion in AB is :-      [NEET - 2016]
  A)
        6
  done clear
  B)
  4
  done clear
  C)
  8
  done clear
  D)
  2
  done clear
  View Answer play_arrow

• question_answer31) Which is the incorrect statement?  [NEET-2017]
  A)
        Frenkel defect is favoured in those ionic compounds in which sizes of cation and anions are almost equal
  done clear
  B)
  \[Fe{{O}_{0.98}}\] has non stoichiometric metal deficiency defect
  done clear
  C)
  Density decreases in case of crystals with Schottky's defect
  done clear
  D)
  \[NaCl(s)\] is insulator, silicon is semiconductor, silver is conductor, quartz is piezo electric crystal
  done clear
  View Answer play_arrow

• question_answer32) Iron exhibits bcc structure at room temperature. Above\[\text{900 }\!\!{}^\circ\!\!\text{ C}\], it transforms to fcc structure. The ratio of density of iron at room temperature to that at \[\text{900 }\!\!{}^\circ\!\!\text{ C}\](assuming molar mass and atomic radii of iron remains constant with temperature) is [NEET - 2018]
  A)
  \[\frac{3\sqrt{3}}{4\sqrt{2}}\]
  done clear
  B)
  \[\frac{4\sqrt{3}}{3\sqrt{2}}\]
  done clear
  C)
  \[\frac{\sqrt{3}}{\sqrt{2}}\]  
  done clear
  D)
  \[\frac{1}{2}\]
  done clear
  View Answer play_arrow

• question_answer33) A compound is formed by cation C and anion A. The anions form hexagonal close packed (hcp) lattice and the cations occupy 75% of octahedral voids. The formula of the compound is: [NEET 2019]
  A)
  \[{{C}_{3}}{{A}_{4}}\]
  done clear
  B)
  \[{{C}_{4}}{{A}_{3}}\]
  done clear
  C)
  \[{{C}_{2}}{{A}_{3}}\]
  done clear
  D)
  \[{{C}_{3}}{{A}_{2}}\]
  done clear
  View Answer play_arrow

• question_answer34) An element has a body centered cubic (bcc) structure with a cell edge of 288 pm. The atomic radius is                                       [NEET 2020]
  A)
  \[\frac{\sqrt{2}}{4}\times 288\,\,pm\]
  done clear
  B)
  \[\frac{4}{\sqrt{3}}\times 288\,\,pm\]
  done clear
  C)
  \[\frac{4}{\sqrt{2}}\times 288\,\,pm\]
  done clear
  D)
  \[\frac{\sqrt{3}}{4}\times 288\,\,pm\]
  done clear
  View Answer play_arrow