Solid State
1. A metal crystallizes with a face-centered cubic lattice. The edge length of the unit cell is 408 pm. The
diameter of the metal atom is :
1) 288 pm
2) 408 pm
3) 144 pm
4) 204 pm
2. Glass is a
1) micro-crystalline solid
2) supercooled liquid
3) gel
4) polymeric mixture
3. A solid compound XY has NaCl structure. If the radius of the cation is 100 pm, the
radius of the anion (Y–) will be :
1) 275.1 pm
2) 322.5 pm
3) 241.5 pm
4) 165.7 pm
4. A body centric cubic lattice is made up of two different types of atoms A and B. Atom A occupies the
body centre and B occupying the corner positions. One of the corners is left unoccupied per unit cell.
Empirical formula of such a solid is
1) AB
2) A2B3
3) A5B7
4) A8B7
5. When molten zinc is converted into solid state, it acquires hcp structure. The number of nearest
neighbours will be
1) 6
2) 12
3) 8
4) 4
6. A solid has a structure in which, atoms of W, O and Na are located respectively at the corners, centre of
edge and at the centre of the cubic lattice. The compound is
1) NaWO2
2) NaWO3
3) Na2 WO3
4) NaWO4
7. In the solid state, MgO has the same structure as that of sodium chloride. The number of oxygens
surrounding each magnesium in MgO is
1) 6
2) 1
3) 2
4) 4
8. A metal has a fcc lattice. The edge length of the unit cell is 404 pm. The density of the metal is 2.72 g
cm–3. The molar mass of the metal is : (NA, Avogadro’s constant = 6.02 × 1023 mol-1)
1) 30 g mol-1
2) 27 g mol-1
3) 20 g mol-1
4) 40 g mol-1
9. Structure of a mixed oxide is cubic close-packed (c.c.p). 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 :
1) ABO2
2) A2BO2
3) A2B3O4
4) AB2O2
10. Total volume of atoms present in a face centred cubic unit cell of a metal is (r = atomic radius)
1) 20/3 πr3
2) 24/3 πr3
3) 12/3 πr3
4) 16/3 πr3
11. A metallic element has a cubic lattice. Each edge of the unit cell is 2 Å. The density of the metal is 2.5
g cm-3. The unit cells in 200 g of metal are
1) 1 × 1024
2) 1 × 1020
3) 1 × 1022
4) 1 × 1025
12. Which one of the following defects in the crystals lowers its density ?
1) F-centres defect
2) Interstitial defect
3) Frenkel defect
4) Schottky defect
13. Schottky defects occurs mainly in electrovalent compounds where
1) positive ions and negative ions are of different size
2) positive ions and negative ions are of same size
3) positive ions are small and negative ions are big
4) positive ions are big and negative ions are small
14. Schottky defect generally appears in
1) NaCl
2) KCl
3) CsCl
4) All of these
15. The flame colours of metal ions are due to
1) Frenkel defect
2) Schottky defect
3) Metal deficiency defect
4) Metal excess defect
16. Which one of the following is a covalent crystal?
1) Rock salt
2) Ice
3) Quartz
4) Dry ice
17. Silver (atomic weight = 108 g mol-1 ) has a density of 10.5 g cm-3. The number of silver atoms on a
surface of area 10-12 m2 can be expressed in scientific notation as y × 10x . The value of x is
1) 3
2) 5
3) 7
4) 9
18. How many unit cells are present in a cube shaped ideal crystal of NaCl of mass 1.00 g?
(Atomic masses Na = 23, Cl = 35.5)
1) 2.57 × 1021
2) 5.14 × 1021
3) 1.28 × 1021
4) 1.71 × 1021
19. Experimentally it was found that a metal oxide has formula M0.98 O. Metal M, present as M2+ and
M3+ in its oxide. Fraction of the metal which exists as M3+ would be
1) 7.01%
2) 4.08%
3) 6.05%
4) 5.08%
20. A compound MPXq has cubic close packing (ccp) arrangement of X. Its unit cell
structure is shown below. The empirical formula of the compound, is
1) MX
2) MX2
3) M2X
4) M5X14
