CBSE Questions for Class 12 Engineering Chemistry The Solid State Quiz 4 - MCQExams.com

An atomic soild has hexagonal arrangement of unit cell with height of hexagonal as $$h$$. The radius of atom terms of height is?
  • $$4\sqrt { \dfrac { 2 }{ 3 } } h$$
  • $$\dfrac { h }{ 4 } \sqrt { \dfrac { 2 }{ 3 } } $$
  • $$\dfrac { h }{ 2 } \sqrt { \dfrac { 3 }{ 2 } } $$
  • $$\dfrac { h }{ 4 } \sqrt { \dfrac { 3 }{ 2 } } $$
Ammonium chloride crystallizes in a body centred cubic lattice with edge length of unit cell of 390 pm. If the size of chloride ion is 180 pm, the size of ammonium ion would be :
  • 158 cm
  • 174 cm
  • 142 cm
  • 126 cm
The physical dimension of unit cells in a crystal lattice:
  • lattice parameter
  • packing factor
  • atomic radius
  • number of constituent particles
  • Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
  • Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
  • Assertion is correct but Reason is incorrect
  • Both Assertion and Reason are incorrect
Packing fraction in face-centered cubic unit cell is :
  • $$0.7406$$
  • $$0.6802$$
  • $$0.5236$$
  • none of the above
Percentage of empty space in body centered cubic unit cell is nearly:
  • $$52.36$$
  • $$68$$
  • $$32$$
  • $$26$$
Of the three cubic lattices, the one that has the largest mass of empty space is the :
  • simple cubic
  • ccp
  • bcc
  • both simple cubic and bcc
When a viscous liquid is cooled rapidly, _________ solid is formed.
  • eutectic
  • liquid crystal
  • super-cooled
  • amorphous
Sodium chloride crystal has a ________ shape.
  • Definite
  • Regular
  • Irregular
  • None of these
Which of the following is amorphous?
  • Sodium chloride
  • Quartz glass
  • Powdered marble
  • Cane sugar
Crystals can be classified into .......... basic crystal habits.
  • $$7$$
  • $$4$$
  • $$14$$
  • $$3$$
Hexagonal close packing is found in crystal lattice of:
  • $${\text{Na}}$$
  • $${\text{Mg}}$$
  • $${\text{Al}}$$
  • None of these
In a solid "AB" having $$NaCl$$ structure "A" atoms occupy the corners of the cubic unit cell. If all the face-centred atoms one of the axes are removed, then the resultant stoichiometry of the solid
  • $$AB_{2}$$
  • $$A_{2}B$$
  • $$A_{4}B_{3}$$
  • $$A_{3}B_{4}$$
$$f-centre$$ is
  • Anion vacancy occupied by unpaired electron
  • Anion vacancy occupied by electron
  • Cation vacancy occupied by electron
  • Anion present in interstitial site
Mostly crystals show  good cleavage because their atoms, ions or molecules are:
  • Wealky bonded together
  • Strongly bonded together
  • Spherically symmetrical
  • Arranged in planes
Edge length of a cube is $$300\ pm$$. Its body diagonal would be
  • $$600\ pm$$
  • $$423\ pm$$
  • $$519.6\ pm$$
  • $$450.5\ pm$$
Which of the following statements about the interstitial compounds is incorrect? 
  • They have higher melting points than the pure metal
  • They retain metallic conductivity
  • They are chemically reactive
  • They are much harder than the pure metal
In a BCC packing, the nearest neighbours lie along the _______________.
  • edges of the cube
  • face diagonal
  • line joining the two opposite corners of the face
  • cube diagonal
A certain ionic compound is formed in the Spinel structure in nature in which  $${O^{2 - }}$$ ionic constitute CCP lattice $${A^{2 + }}$$ ions occupy  $$1/{8^{th}}$$ of the  tetrahedral voids and  $$B{^{3 + }}$$ ions occupy $$1/2$$ of the octahedral voids . Find out total +ve charge contained in two-unit cell of given ionic structure.
  • +8 electronic charge
  • +12 electronic charge
  • +16 electronic charge
  • +24 electronic charge
Packing efficiency of $$NaCl$$ is almost
  • $$72\%$$
  • $$74\%$$
  • $$79\%$$
  • $$75\%$$
How many unit cells are present in $$0.1$$ moles of rock salt?
  • $$0.1{N}_{0}$$
  • $$0.25{N}_{0}$$
  • $$0.4{N}_{0}$$
  • $$0.025{N}_{0}$$
What forms a crystal of $$NaCl$$?
  • NaCl molecules
  • $$Na^+$$ and $$Cl^-$$ ions
  • $$Na$$ and $$Cl$$ atoms
  • None
In normal spinel structure there is a closed packed array of $${O}^{2-}$$ ions. The trivalent cations are present in:
  • $$75$$% of octahedral voids
  • $$50$$% of octahedral voids
  • $$12.5$$% of tetrahedral voids
  • $$25$$% of octahedral voids
Density of Nickel ($$M=59$$) metal is $$8.9\ g/cc$$ and it is known to crystallize in cubic unit cell. If edge length of the unit cell is $$3.5\ \mathring { A } $$, atomic radius of the metal is?
  • $$1.25\ \mathring { A } $$
  • $$12.5\ \mathring { A } $$
  • $$6.25\ \mathring { A } $$
  • $$25\ \mathring { A } $$
Tungsten ($$M=184$$) crystallises in cubic lattice structures and its density is $$19.26\ g/cc$$. If edge length of the unit cell is $$3.165\ \mathring { A } $$, the type of unit cell is?
  • simple cubic
  • BCC
  • FCC
  • edge-centred cubic lattice
Which of the following is true about the voids formed in 3 dimensional hexagonal close-packed structure?
  • A tetrahedral void is formed when a sphere of the second layer is present above triangular void in the first layer.
  • All the triangular voids are not covered by the spheres of the second layer.
  • Tetrahedral voids are formed when the triangular voids in the second layer lie above the triangular voids in the first layer and the triangular shapes of these voids do not overlap.
  • Octahedral voids are formed when the triangular voids in the second layer exactly overlap with similar voids in the first layer.
If silver iodide crystallizes in a zinc blende structure with $${I}^{-}$$ ion forming the lattice, the fraction of tetrahedral void occupied by $${Ag}^{+}$$ ion is
  • $$25$$%
  • $$50$$%
  • $$40$$%
  • $$60$$%
$$\alpha  \ne \beta  \ne \gamma  \ne {90^ \circ };$$  $$a \ne b \ne c$$, crystal system can have 
  • Primitive, end centered unit cells
  • Primitive, body centered unit cells
  • Primitive only
  • face centered and primitive
The empty space between the shaded balls and hollow balls as shown in the diagram is called
1402403_3072a0ac7c3346c585b823b67742572e.png
  • hexagonal void
  • octahedral aoid
  • tetrahedral void
  • double triangular void
Select the incorrect statement:
  • Atom present at the corner of HCP prism is shared by 6 such prisms
  • HCP is more close packing than FCC
  • Size of the octahedral void is bigger than tetrahedral void
  • If $$ \cfrac { r _ { + } } { r _ { - } } = 0.5 $$, then most probable co-ordination number of cation will be 6.
The crystalline structure of $$NaCl$$ is:
  • hexagonal close packing
  • face centred cubic
  • square planar
  • body centred cubic
Which of the following represents true statement?
  • Force of attraction between the molecules (inter molecular forces) in solids is very strong.
  • Force of attraction between the molecules (inter molecular forces) in solids is very weak.
  • Force of attraction between the molecules (inter molecular forces) in solids is either very strong or very weak.
  • There is no force of attraction between the molecules (inter molecular forces) in solids.
Interstitial hole is called tetrahedral because:
  • it is formed by four spheres
  • it is formed by four spheres and the centre of which forms a regular tetrahedron
  • coordination number of hole is 3
  • none of the above
If the distance between $$Na^+$$ and $$Cl^-$$ in $$NaCl$$ crystal is $$265 pm$$, the edge length of the unit cell will be:
  • 265 pm
  • 795 pm
  • 132.5 pm `
  • 530 pm
Polonium crystallizes in a simple cubic structure. The edge of the unit cell is $$0.236$$ nm. What is the radius of the polonium atom?
  • $$0.144$$ nm
  • $$0.156$$ nm
  • $$0.118$$ nm
  • $$0.102$$ nm
There are three cubic unit cells $$A, B$$ and $$C$$. $$A$$ is FCC and all of its tetrahedral voids are also occupied. $$B$$ is also FCC and all of its octahedral voids are also occupied. $$C$$ is simple cubic and all of its cubic voids are also occupied. If voids in all unit cells are occupied by the spheres exactly at their limiting radius, then the order of packing efficiency would be
  • $$A< B< C$$
  • $$C< A< B$$
  • $$C< B< A$$
  • $$A< C< B$$
The number of tetrahedral and octahedral voids in the hexagonal primitive unit cell is?
  • $$8,4$$
  • $$2,1$$
  • $$12,6$$
  • $$6,12$$
A solid contains $${ A }^{ n+ }$$ and $${ B }^{ m- }$$ ions. The structure of solid is FCC for $${ B }^{ m- }$$ ions and $${ A }^{ n+ }$$ ions are present in one-fourth of tetrahedral voids as well as in one fourth of octahedral voids. What is the simplest formula of solid?
  • $${ A }_{ 3 }{ B }_{ 4 }$$
  • $${ A }_{ 4 }{ B }_{ 3 }$$
  • $$A{ B }_{ 2 }$$
  • $${ A }_{ 2 }B$$
Crystalline solids are:
  • Glass
  • Rubber
  • Plastic
  • Sugar
The correct statement in the following is
  • The ionic crystal of $$AgBr$$ has Schottky defect
  • The unit cell having crystal parameters, $$a = b \neq c, \alpha = \beta = 90^{\circ}, \gamma = 120^{\circ}$$ is hexagonal
  • In ionic compounds having Frenkel defect the ratio $$\dfrac {\gamma +}{\gamma -}$$ is high
  • The coordination number of $$Na^{+}$$ ion in $$NaCl$$ is $$4$$
Under which category, iodine crystals are placed among the following?
  • Ionic crystal
  • Metallic crystal
  • Molecular crystal
  • Covalent crystal
In chromium chloride $$(CrCl_3)$$, $$Cl^-$$ ions have cubic close packed arrangement and $$Cr^{3+}$$ ions are present in the octahedral holes. The fraction of the total number of holes occupied is:
  • $$1/3$$
  • $$1/6$$
  • $$1/9$$
  • $$1/12$$
If metallic radius of metal having $$fcc$$ structure is $$127\ pm$$, then the length of edge of its unit cell will be.
  • $$288\ pm$$
  • $$359\ pm$$
  • $$576\ pm$$
  • $$432\ pm$$
Salt Ab has a zinc blende structure. The radius of $$A^{2+}$$ and $$B^{2-}$$ ions are $$0.7\mathring{A}$$ and $$1.8\mathring{A}$$ respectively. The edge length of AB unit cell is:
  • $$2.5 \mathring{A}$$
  • $$5.0.9\mathring{A}$$
  • $$5 \mathring{A}$$
  • $$5.77 \mathring{A}$$
The compound with the largest lattice energy would be:
  • NaF
  • KBr
  • $${ MgF }_{ 2 }$$
  • All have equal
Oxygen atom forms FCC unit cell with 'A' atoims occupying all tetrahedral voids and 'B' atoms occupying all octahedral voids. If atoms are removed from two of the body diagonals then determine the formula of resultant compound formed.
  • $$A_{4}B_{4}O_{7}$$
  • $$A_{8}B_{6}O_{7}$$
  • $$A_{8}B_{8}O_{7}$$
  • $$A_{6}B_{8}O_{6}$$
How many unit cell of $$NaCl$$ are present in $$7.02\ gm$$ of $$NaCl?$$
  • $$12\times 10^ {-2}N_{A}$$
  • $$3\times 10^ {-2}N_{A}$$
  • $$6\times 10^ {2}N_{A}$$
  • $$1.5\times 10^ {-2}N_{A}$$
$$PQ$$ is $$NaCI$$ type solid $$P$$ occupies corners of cubic unit cell. If all the atoms present along face centered axis are removed, the resultant stoichiometry and $$%$$ decrease in the total number of atoms per unit cell are
  • $$PQ_{2}$$ and $$25\%$$
  • $$P_{2}Q$$ and $$25\%$$
  • $$P_{4}Q_{3}$$and $$12.5\%$$
  • $$P_{3}Q_{4}$$ and $$12.5\%$$
According to recent studies which of the following interstitial hydrides have simi-lattices that of their parent metals
  • $$La, Yb, W$$
  • $$Yb, W, V$$
  • $$V, I, a$$
  • $$N, Pd, Ce, Ac$$
The pycnometric density of sodium chloride crystal is $$2.165 \times 10^3$$ $$kg m^{-3}$$ while its X-ray density is $$2.178 \times 10^3 kg m^{-3}$$. The fraction of the unoccupied sites in sodium chloride crystal is 
  • $$5.96$$
  • $$5.96 \times 10^{-2}$$
  • $$5.96 \times 10^{-1}$$
  • $$5.96 \times 10^{-3}$$
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