CBSE Questions for Class 12 Engineering Chemistry The Solid State Quiz 10 - MCQExams.com

The maximum radius of sphere that can be fitted in the octahedral hole of cubical closed packing of sphere of radius $$r$$ is:
  • $$0.732\ r$$
  • $$0.225\ r$$
  • $$0.155\ r$$
  • $$0.414\ r$$
The unit cell length of $$NaCl$$ is observed to be $$0.5627$$ nm by X-ray difference studies; the measured density of $$NaCl$$ is $$2.164$$g $$cm^{-3}$$/ Calculate the difference of observed and calculated density. lso calculate $$\%$$ is missing $$Na^+$$ and $$Cl^-$$ ions:
  • $$0.031, 0.775\%$$
  • $$3.96, 0.031\%$$
  • $$0.0031, 7.75\%$$
  • $$1.7, 1.75\%$$
A crystalline solid $$AB$$ adopts sodium chloride type structure with edge length of the unit cell as 745 pm and formula mass of 74.5 a.m.u. The density of the crystalline compound is:
  • $$2.16 g cm^{-3}$$
  • $$0.99g cm^{-3}$$
  • $$1.88g cm^{-3}$$
  • $$1.97 g cm^{-3}$$
The fraction of octahedral voids filled by $$A{l^{3 + }}$$ ions in $$A{l_2}{O_3}\left( {{r_{Al^{3 \oplus }}}}/r_{O^{2 - }} = 0.43 \right)$$ is:
  • 0.43
  • 0.287
  • 0.667
  • 1
The pattern in Hexagonal close packing and cubic close packing are same.
Is the statement true or false?
  • True
  • False
Silver crystallizes in fcc structure with edge length of unit cell, $$408.7pm$$. Hence density of silver is $$(Ag = 108\ g\ mol^{-1})$$
  • $$10.5\ g \ cm^{-3}$$
  • $$9.82\ g \ cm^{-3}$$
  • $$12.06\ g \ cm^{-3}$$
  • $$8.86\ g \ cm^{-3}$$
Copper crystallizes in fcc structure and the edge length of the unit cell is $$3.61A^o$$. Hence the density of copper is:
(atomic mass of $$Cu = 63.5\ g \ mol^{-1}$$)
  • $$5.17\ g \ cm^{-3}$$
  • $$0.72\ g \ cm^{-3}$$
  • $$7.09\ g \ cm^{-3}$$
  • $$8.97\ g \ cm^{-3}$$
The side length of diamond unit cell is (in pm):
  • $$154$$
  • $$1422.63$$
  • $$711.32$$
  • $$355.66$$
The crystal system possess by $${K}_{2}{Cr}_{2}{O}_{7}$$ is:
  • Tetragonal
  • Cube
  • Hexagonal
  • Triclinic
The coefficient of linear expansion of crystal in x-direction is $$6\times {10}^{-5}/^{o}C$$ and that in y and z- directions is $$4\times {10}^{-5}/^{o}C$$. The coefficient of cubical expansion of the crystal is?
  • $$18\times {10}^{-5}/^{o}C$$
  • $$16\times {10}^{-5}/^{o}C$$
  • $$14\times {10}^{-5}/^{o}C$$
  • $$32\times {10}^{-5}/^{o}C$$
Number of unit cells in $$10\ g\ NaCl$$ is:
  • $$\dfrac {1.5}{58.5}\times 10^{24}$$
  • $$\dfrac {2.5}{58.5}\times 10^{23}$$
  • $$\dfrac {5.6}{58.5}\times 10^{20}$$
  • $$\dfrac {5.6}{58.5}\times 10^{21}$$
A metal $$M$$ is crystallised in $$F.C.C$$ lattice. The number of unit cells in it having $$2.4\times 10^{24}$$ atoms are:
  • $$6.023\times 10^{23}$$
  • $$\frac{6.023\times 10^{23}}{2}$$
  • $$2\times 6.023\times 10^{23}$$
  • $$4\times 6.023\times 10^{23}$$
$$NaBr$$ has same crystal structure as $$NaCl$$. If density is $$3.203g\ cm^{-3}$$. Calculate the unit cell side length. [$$Na=23, Br=79.9$$]
  • $$5.976A^{o}$$
  • $$6.976A^{o}$$
  • $$7.976A^{o}$$
  • $$4.976A^{o}$$
The rank of atoms in the hexagonal until cell is:
  • 4
  • 3
  • 5
  • 6
In fcc, the neighbouring number of atoms for any lattice points is:
  • 6
  • 8
  • 12
  • 14
If the edge length of a KCl cell is 488 pm, what is the length of KCl bond if it crystallizes in the fcc structure?
  • 122 pm
  • 244 pm
  • 488 pm
  • 974 pm
If $$fcc$$ unit cell is converted in to End centred unit cell, then its packing efficiency will decrease by:
  • $$25\%$$
  • $$50\%$$
  • $$40\%$$
  • $$60\%$$
The unit cell cube length for $$LiCl$$ (just like $$NaCl$$ structure) is $$5.14 \ \mathring { A } $$. Assuming anion-anion contact, the ionic radius for chloride ion is:
  • $$1.815 \ \mathring { A } $$
  • $$2.8 \ \mathring { A } $$
  • $$3.8 \ \mathring { A } $$
  • $$4.815 \ \mathring { A } $$
A compound $$CuCl$$ has face centered cubic structure. Its density is $$3.4 \ g \ cm^{-3}$$. The length of unit cell is :
  • $$5.783 \ \mathring { A } $$
  • $$6.783 \ \mathring { A } $$
  • $$7.783 \ \mathring { A } $$
  • $$8.783 \ \mathring { A } $$
The Aluminium chloride crystallizes in BCC lattice with an edge length of unit cell equal to $$387\ pm $$. If the size of $$Cl^- $$ ion is $$181\ pm $$, the size of $$NH_4^{+} $$ ion would be:
  • $$ 116\ pm$$
  • $$ 154\ pm$$
  • $$174\ pm$$
  • $$206\ pm$$
How many unit cells are there in $$1.00$$ gm cube shaped ideal crystal $$AB (MF = 60)$$ having $$NaCl$$ type lattice?
  • $$6.02 \times 10^{23}$$
  • $$2.50 \times 10^{21}$$
  • $$1.00 \times 10^{22}$$
  • $$6.02 \times 10^{24}$$
In a cubic close packing of spheres in three dimensions, the co-ordination number of each sphere?
  • 6
  • 9
  • 3
  • 12
In a hypothetical solid, C atoms are found to form cubical close-packed lattice . A atoms occupy att tetrahedral voids and B atoms occupy all octahedral voids.
A and B atoms are of appropriate size, so that there is no distortion in the ccp lattice of C atoms .Now if a plane as shown in the following figure is cut, then the cross section of this plane will look like?
1092614_32ce49feb1534991a9339a33c6dc0fa2.png
For bcc structure, the coordination number and packing are ______  respectively.
  • $$8, \cfrac {\pi \sqrt 3}{8}$$
  • $$6, \cfrac {\pi \sqrt 2}{6}$$
  • $$8, \cfrac {\pi \sqrt 2}{6}$$
  • none of the above
 The number of unit cells in 58.5 g of $$NaCl$$ is approximately:
  • $$6 \times 10^{20}$$
  • $$1.5 \times 10^{23}$$
  • $$9 \times 10^{23}$$
  • None of these
Which is correct statement?
  • Schottky defect occurs when radius of cation is smaller
  • When temperature increases then number of defects decreases
  • Frenkel defect occurs when radius of cation is smaller
  • None of these
How many units cells are there in $$ 1.00 g $$ cube shaped ideal crystal of $$ AB (Mw = 60 ) $$ which has a $$NaCl$$ type lattice?
  • $$ 6.02 \times 10^{23} $$
  • $$ 1.00 \times 20^{22} $$
  • $$ 2.50 \times 10^{21} $$
  • $$6.02 \times 10^{24} $$
The density of crystalline sodium chloride is 5.85 g $${cm}^{-3}$$. What is the edge length of the unit cell?
  • $$4.04 \times 10^{-9}$$ cm
  • $$1.32 \times 10^{-14}$$ cm
  • $$7.8 \times 10^{-23}$$ cm
  • $$9.6 \times 10^{-24}$$ cm
An element X (At. wt. = 80 g / mol ) having fcc structure, calculate no. of unit cells in 8 gm of X:
  • $$0.4 \times N_A$$
  • $$0.1 \times N_A$$
  • $$4 \times N_A$$
  • None of these
Certain quantity of metal is crystallised $$60\%$$ in ccp structure $$40\%$$ in hcp structure. What is the ratio of number of unit cells in ccp and hcp?
  • $$3:2$$
  • $$1:1$$
  • $$9:4$$
  • $$4:9$$
The density of solid argon (Ar = 40 g / mol) is 1.68 g/mL at 40 K. If the argon atom is assumed to be a sphere of radius 1.50 x $$10^{-8}$$ cm, what % of solid Ar is apparently empty space? (use $$N_A = 6 \times10^{23}$$)
  • 35.64
  • 64.36
  • 74%
  • none of these
The compound $${ MX }_{ 4 }$$ is tetrahedral . The number of $$X-M-X$$ angles in the compound is:
  • three
  • four
  • five
  • six
Select the wrong statement (s) :-
  • A NaCl type AB crystal lattice can be interpreted to be made up of two individual fcc type unit lattice of $$A^+$$ and $$B^-$$ fused together in such a manner that the corner of one unit lattice becomes the edge centre of the other
  • In a fcc unit cell, the body center is an octahedral void
  • In an scc lattice, there can be no octahedral void
  • In an scc lattice, the body center is the octahedral void
Packing efficiency of body centred unit cell is:
  • 85%
  • 68%
  • 33.33%
  • 45%
$$A_2B$$ molecules (molar mass =259.8 g/mol) crystallises in a hexagonal lattice as shown in figure. The lattice constants were $$a = 5 \mathring{A}$$ and $$ b= 8 \mathring{A}$$. If density of crystal is 5 $$g/cm^3$$ then how many molecules are contained in given unit cell? (use $$N_A= 6 \times 10^{23}$$)
1119884_c7da2c1450374fe689d6bb517cc12153.GIF
  • 6
  • 4
  • 3
  • 2
Total number of unit cells present in a cube shaped ideal crystal of $$1g \ NaCl(s)$$ is (Avogdro's number = $$6\times10^{23}$$).
  • $$2.56\times10^6$$
  • $$2.56\times10^{21}$$
  • $$2.56\times10^{23}$$
  • $$4.2\times10^{22}$$
The magnitude of the lattice energy of a solid increases if:
  • the ions are large
  • the ions are small
  • the ions are of equal size
  • charges on the ions are large
Which forms a crystal of NaCl?
  • $$NaCl\ molecules$$
  • $$Na^{+}$$ and $$Cl^{-}ions$$
  • $$Na\ and\ Cl\ atoms$$
  • $$None\ of\ these$$
A metallic crystal has the bcc type stacking pattern. What percentage of volume of this lattice is empty space?
  • 68% 
  • 32%
  • 26%
  • 74%
In a unit cell, atoms A, B, C and D are present at half of total corners, all face-centres, body-centre and one third of all edge-centres respectively. Then formula of unit cell is ?
  • $$ AB_{3}CD_{3} $$
  • ABCD
  • $$ AB_{6}C_{2}D_{4} $$
  • $$ AB_{6}C_{2}D_{2} $$
If the radius of $${Cl}^{-}$$ ion is $$181pm$$, and the radius of $${Na}^{+}$$ ion is $$101pm$$ then the edge length of unit cell is:
  • $$282pm$$
  • $$285.71pm$$
  • $$512pm$$
  • $$564pm$$
How many molecules are there in the unit cell of sodium chloride?
  • $$2$$
  • $$4$$
  • $$6$$
  • $$8$$
(i) Frenkel defect create a vacancy defect at its original site and an interstitial defect at its new position.
(ii) Frenkel defect is stoichiometric point defect.
(iii) Frenkel defect is also called dislocation defect.
(iv) Silver halide shows Frenkel defect 
Select the correct statements :
  • $$(ii),(iii),(iv)$$ only
  • $$(i),(ii),(iii)$$ only
  • $$(i),(ii),(iii),(iv)$$
  • $$(i),(ii),(iv)$$ only
Lattice energy of an ionic compound depends upon?
  • Charge on the ion and size of the ion
  • Packing of Ions only
  • Size of the ion
  • Charge on the Ion only
An element having a face-centered cubic structure has a density of $$6.23g\ cm^{-3}$$. The atomic mass of elements is $$60$$. The edge length of the unit cell is:
  • $$400\ pm$$
  • $$300\ pm$$
  • $$425\ pm$$
  • $$370\ pm$$
Lattice energy of $$NaCl$$ is $$'X'$$. If the ionic size of $$A^{ +2 }$$ is equal to that of $$Na^{ + }$$ and $$B^{ -2 }$$ is equal to $$Cl^{ - }$$, then lattice energy associated with the crystal $$AB$$ is:
  • $$X$$
  • $$2X$$
  • $$4X$$
  • $$8X$$
Which of the following expression is correct for packing fraction of $$NaCI$$ if the ions along with face are diagonally removed ?
  • $$\dfrac{\dfrac{13}{3} \pi r^{3}_{-}+\dfrac{16}{3} \pi r_{+}^{3}}{8(r_{+}+r_{-})^{3}}$$
  • $$\dfrac{\dfrac{13}{3} \pi r^{3}_{-}+\dfrac{4}{3} \pi r_{+}^{3}}{8(r_{+}+r_{-})^{3}}$$
  • $$\dfrac{\dfrac{16}{3} \pi r^{3}_{-}+\dfrac{13}{3} \pi r_{+}^{3}}{8(r_{+}+r_{-})^{3}}$$
  • $$\dfrac{\dfrac{3}{4} \pi r^{3}_{-}+\dfrac{13}{3} \pi r_{+}^{3}}{8(r_{+}+r_{-})^{3}}$$
Which of the following pairs have layer lattice structure in solid state chemistry-
  • $$Sr{Cl}_{2}$$ and $$C{dI}_{2}$$
  • Diamond and Graphite
  • Graphite and $$Cd{I}_{2}$$
  • $$Mg{SO}_{4}.7{H}_{2}O$$ and $$Fe{SO}_{4}.7{H}_{2}O$$
In the given crystal what should be the cation $$X$$ which replaces to create a $${ Na }^{ + }$$ cation vacancy?

1141048_1fbc8458df494399a961785d6e8e6ddb.png
  • $${ Sr }^{ 2+ }$$
  • $${ K }^{ + }$$
  • $${ Li }^{ + }$$
  • $${ Br }^{ - }$$
Which of the following solid substance(s) will have the same refractive index when measured in different directions?
  • Rubber
  • $$NaCl$$
  • Plastic
  • Graphite
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