1. Mention the characteristic properties of solid.
2. Mention the differences between crystalline solid and amorphous solid.
3. Explain the terms a) anisotropy b) isotropy. Why is crystalline solid anisotropic while amorphous solid isotropic in nature?
4. What makes glass different from quartz? Under what condition quartz is converted to glass?
5. Why are amorphous solids called pseudo solids or super cooled liquids?
6. How are crystalline solids classified on the basis of intermolecular forces? Give two examples of each type and mention their properties.
7. Compare the properties of diamond and graphite on the basis of their structures.
8. Classify the following as ionic, metallic, molecular, covalent, or amorphous.
9. How are molecular solids subdivided further? Give two examples each and mention their properties.
10. Account for the following:
a) Glass panes fixed to windows of old buildings becomes slightly thicker at the bottom than at the top.
b) NaCl(s) does not conduct electricity but it conducts either in molten state or in aqueous solution.
c) Diamond is a non conductor while graphite is a conductor of electricity.
d) Diamond is hard while graphite is soft.
e) Graphite is a lubricant.
f) Ionic solids are hard and brittle.
g) MgO and NaCl are ionic solids but MgO has higher melting point than NaCl.
h) NaCl exhibit schottky defect and not frenkel defect.
11. Explain the terms
a) lattice point
b) crystal lattice
c) unit cell.
12. What are Bravis lattices? Mention the characteristics of a crystal lattice.
13. Mention the characteristics of a unit cell. Draw a neat diagram of a unit cell and show its parameters.
14. What is the difference between primitive and centered unit cell?
15. Calculate the number of atoms in
c) FCC unit cells.
16. Mention the characteristics of seven primitive unit cells and their possible variation as centered unit cells.
17. Name the centered unit cells and position of atoms in each centered unit cell.
18. What do you mean by coordination number? Give the coordination number of atoms in
a) one dimensional arrangement of atoms
b) square close packing in two dimension.
c) hexagonal close packing in two dimension
c) hexagonal close packing in three dimension
d) cubic close packing or fcc in three dimension
e) cation in triangular void.
f) cation in tetrahedral void
g) cation in cubic void
19. A compound has hexagonal close packing structure. Determine the total number of voids, number of tetrahedral void, and number of octahedral voids in 0.5 mole of this compounds.
20. Calculate the number of octahedral and tetrahedral voids in unit cells of a)SCC b)BCC c)FCC
21. Distinguish between
a) octahedral and tetrahedral voids
b) Schottky and Frenkel defect.
c) Hexagonal closed packing and cubic close packing
d) crystal lattice and unit cell.
e) para magnetism and ferro magnetism
f) hexagonal and monoclinic unit cell
g) face centered and end centered unit cell.
22. Calculate the % efficiency of packing in
23. If the radius of octahedral void is r and the radius of atoms in close packing is R, derive the relationship between r and R.
24. What are interstitial defects? Mention its effect on density of a solid.
25. What is the effect of adding
a) SrCl2 to NaCl
b) CdCl2 to AgCl?
26. Explain the terms with suitable examples
a) Stoichiometric and non stoichiometric defects
b) F centre
c) Metal deficiency defect
d) 12-16 and 13-15 compounds
27. What happens when
a) NaCl crystal is heated with Na vapors
b) ZnO is heated
c) Fe3O4 is heated.
28. Explain n type and p type conduction with suitable examples.
29. Classify the following as n type or p type semi conductors.
a) Ge doped with In
b) B doped with Si.
30. In terms of band theory explain the differences between conductor , insulator, and semi conductor. Draw a neat diagram to show the valence band and conduction band in conductor, insulator and semi conductor.
31. Derive the expression for determining the density of unit cell.
Submitted By : Mr. R. Srinivas Vasudevamurthy