Solid State PYQs Set 4 (PDF)

Set 4 of 6 · Questions 91-120 of 153

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NEET Chemistry · Solid State · Set 4 (Q91-120)

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91.
Which one of the following is a molecular crystal?
1. (1) $Rock salt$
2. (2) $Quartz$
3. (3) $Dry ice$
4. (4) $Diamond$
92.
If we mix a pentavalent impurity in a crystal lattice of germanium, what type of semiconductor formation will occur?
1. (1) $n ‐type semiconductor$
2. (2) $p ‐type semiconductor$
3. (3) $both (a) and (b)$
4. (4) $None of these.$
93.
The packing efficiency of simple cubic (sc), body centred cubic (bcc) and cubic close packing (ccp) lattices follow the order
1. (1) $bcc < ccp < sc$
2. (2) $ccp < bcc < sc$
3. (3) $sc < ccp < bcc$
4. (4) $sc < bcc < ccp$
94.
The correct statement regarding defect in solids is
1. (1) $Schottky defect has no effect on the physical properties of solids$
2. (2) $Frenkel defect is a dislocation defect$
3. (3) $Frenkel defect is usually favoured by a very small difference in the sizes of cations and anions$
4. (4) $trapping of proton in the lattice leads to the formation of F -centers.$
95.
A metal crystallises in face centred cubic structure with metallic radius $2 Å$ . The volume of the unit cell (in $m^{3}$ ) is
1. (1) $6.4\times 1 0^{- 29}$
2. (2) $4 \times 10^{- 29}$
3. (3) $6.4 \times 10^{- 30}$
4. (4) $4 \times 10^{- 10}$
96.
Vacant space in body centred cubic lattice unit cell is about
1. (1) $23 %$
2. (2) $46 %$
3. (3) $32 %$
4. (4) $10 %$
97.
Elements $A$ and $B$ have fcc and bcc structures respectively with a unit cell edge length of $3 A^{0}$ for both elements. The no. of atoms in $210 gm$ of $A$ is equal to $594 gm$ of $B$ . If density of $A$ is $7 g cm^{- 3}$ , what is the density of $B$ ?
1. (1) $9.9 g cm^{- 3}$
2. (2) $4.5 g cm^{- 3}$
3. (3) $6.8 g cm^{- 3}$
4. (4) $11.2 g cm^{- 3}$
98.
At 100ºC, copper (Cu) has FCC unit cell structure with cell edge length of x Å. What is the approximate density of Cu (in g $c m^{-3}$ ) at this temperature? [Atomic mass of Cu = 63.55 u]
1. (1) $\frac{205}{x ^{3}}$
2. (2) $\frac{105}{x ^{3}}$
3. (3) $\frac{422}{x ^{3}}$
4. (4) $\frac{211}{x ^{3}}$
99.
What is the packing efficiency of silver metal in its unit cell?
1. (1) $52.4 %$
2. (2) $68.0 %$
3. (3) $32.0 %$
4. (4) $74.0 %$
100.
What is the number of unit cells when one mole atom of a metal, that forms simple cubic structure?
1. (1) $6.022 \times 10^{23}$
2. (2) $1.204 \times 10^{24}$
3. (3) $9.033 \times 10^{23}$
4. (4) $3.011 \times 10^{23}$
101.
In chrysoberyl, a compound containing beryllium, aluminium and oxygen, oxide ions form cubic close packed structure. Aluminium ions occupy $\frac{1}{4}$ th of tetrahedral voids and Beryllium occupy $\frac{1}{4}$ th of octahedral voids. The formula of the compound is
1. (1) $BeAlO_{4}$
2. (2) $BeAl_{2} O_{4}$
3. (3) $Be_{2} AlO_{2}$
4. (4) $BeAlO_{2}$
102.
An element has a body centered cubic structure with a unit cell edge length of $400 pm$ . Atomic mass of an element is $24 g mol^{- 1}$ . What is the density of the element? $(N_{A} = 6 \times 10^{23} mol^{- 1})$
1. (1) $2.50 g cm^{- 3}$
2. (2) $1.80 g cm^{- 3}$
3. (3) $3.60 g cm^{- 3}$
4. (4) $1.25 g cm^{- 3}$
103.
An ionic compound has a unit cell consisting of A ions at the corners of a cube and B ions on the centers of the faces of the cube. The empirical formula for this compound would be
1. (1) $AB$
2. (2) $A_{2} B$
3. (3) $A B_{3}$
4. (4) $A_{3} B$
104.
Calculate the volume of unit cell if an element having molar mass $56 g mol^{- 1}$ that forms $bcc$ unit cells. $(ρ . N_{A} = 4.8 \times 10^{24} g cm^{- 3} mol^{- 1})$ ]
1. (1) $1.17 \times 10^{- 23} cm^{3}$
2. (2) $3.31 \times 10^{- 23} cm^{3}$
3. (3) $4.79 \times 10^{- 23} cm^{3}$
4. (4) $2.33 \times 10^{- 23} cm^{3}$
105.
At $T (K)$ , copper (atomic mass $= 63.5 u$ ) has fcc structure with an edge length of $x Å$ .The density of copper (in $g cm^{- 3}$ ) at that temperature approximately is $(N_{A} = 6.0 \times 10^{23} mol^{- 1})$
1. (1) $\frac{423}{x}$
2. (2) $\frac{4.23}{x ^{3}}$
3. (3) $\frac{423}{x ^{3}}$
4. (4) $\frac{212.5}{x ^{3}}$
106.
A compound $M_{P}$ $X_{q}$ has cubic close packing (ccp) arrangement of X. Its unit cell structure is shown below. The empirical formula of the compound is:
1. (1) $MX$
2. (2) $M X_{2}$
3. (3) $M_{2} X$
4. (4) $M_{5} X_{14}$
107.
An element crystallises in a face-centred cubic $(fcc)$ unit cell with cell edge a. The distance between the centres of two nearest octahedral voids in the crystal lattice is
1. (1) $a$
2. (2) $2 a$
3. (3) $\frac{a}{2}$
4. (4) $\frac{a}{2}$
108.
The arrangement of $X^{-}$ ions around $A^{+}$ ion in solid AX is given in the figure (not drawn to scale). If the radius of $X^{-}$ is 250 pm, the radius of $A^{+}$ is :
1. (1) $104 pm$
2. (2) $125 pm$
3. (3) $183 pm$
4. (4) $57 pm$
109.
How many of the following compounds show ferrimagnetism?
$Fe_{3} O_{4}; MgFe_{2} O_{4}; NiFe_{2} O_{4}; MnO; CrO_{2}$
1. (1) $1$
2. (2) $2$
3. (3) $3$
4. (4) $4$
110.
Consider the bcc unit cells of the solids 1 and 2 with the position of atoms as shown below. The radius of atom B is twice that of atom A. The unit cell edge length is 50% more in solid 2 than in 1. What is the approximate packing efficiency in solid 2?
1. (1) $45%$
2. (2) $75%$
3. (3) $90%$
4. (4) $65%$
111.
Which among the following solids is a non polar solid?
1. (1) $Hydrogen chloride$
2. (2) $Sulphur dioxide$
3. (3) $Water$
4. (4) $Carbon dioxide$
112.
At $10 0^{\circ} C$ , copper (Cu) has FCC unit cell structure with cell edge length of $x A ˚$ . What is the approximate density of Cu (in $g c m^{- 3}$ ) at this temperature ?
[Atomic Mass of Cu = 63.55 u]
1. (1) $\frac{205}{x ^{3}}$
2. (2) $\frac{105}{x ^{3}}$
3. (3) $\frac{211}{x ^{3}}$
4. (4) $\frac{422}{x ^{3}}$
113.
The correct statement(s) regarding defects in solids is(are)
1. (1) $Frenkel defect is usually favoured by a very small difference in the sizes of cation and anion.$
2. (2) $Frenkel defect is a dislocation defect.$
3. (3) $Trapping of an electron in the lattice leads to the formation of F-center.$
4. (4) $Schottky defects have no effect on the physical properties of solids.$
114.
Total volume of atoms present in a face-center cubic unit cell of a metals (r is atomic radius).
1. (1) $\frac{20}{3} π r^{3}$
2. (2) $\frac{24}{3} π r^{3}$
3. (3) $\frac{12}{3} π r^{3}$
4. (4) $\frac{16}{3} π r^{3}$
115.
$Match List I with List II (defects) (Examples)$
$List I$ $List II$
$A. Frenkel defects$ $1. FeO$
$B. Schottkey defects$ $2. NaCl$
$C. Vacancy defects$ $3. AgCl$
$D. Metal deficiency$ $4.Crystals with vacant$
$defects lattice sites. A B C D$
1. (1) $4321$
2. (2) $3241$
3. (3) $1234$
116.
Silicon doped with gallium forms
1. (1) $both n and p type semiconductor$
2. (2) $an intrinsic semiconductor$
3. (3) $p -type semiconductor$
4. (4) $n-type semiconductor.$
117.
Metallic lustre is due to
1. (1) $high density of metals$
2. (2) $high polish on the surface of metals$
3. (3) $reflection of light by mobile electrons$
4. (4) $chemical inertness of metals.$
118.
An example for network solid is
1. (1) $SiO_{2}$
2. (2) $MgO$
3. (3) $CaF_{2}$
4. (4) $ZnS$
119.
Pure silicon doped with phosphorus is
1. (1) $amorphous$
2. (2) $p-type semiconductor$
3. (3) $n-type semiconductor$
4. (4) $insulator$
120.
An example of covalent solid is
1. (1) $MgO$
2. (2) $Mg$
3. (3) $SiC$
4. (4) $CaF_{2}$