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The Solid State -Important Questions & Preparation Tips

In this article you will get the clue that from where and how the questions are being framed from the chapter The Solid State

Aug 13, 2013 16:26 IST
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The experts of jagranjosh.com have full confidence that you will not miss any of the questions in the board exam as well as in competitive exams from this chapter if you will keep the following terms / question in your mind while studying

  • Why is study of structures of solid important?
  • Characteristic properties of the solid state
  • Difference between amorphous and crystalline solid
  • In the case of amorphous quartz glass there is no long range order. What do you understand by “long range order”
  • Crystalline solids are anisotropic in nature. Brief the term anisotropic
  • Why glass is considered a super cooled liquid?
  • Examples of amorphous and crystalline solids
  • Refractive index of a solid is observed to have the same value along all directions. Comment on the nature of this solid. Would it show cleavage property?
  • Basis to classify the crystalline solids and amorphous solid
  • Short notes and different properties of the following

               Molecular solids
               Ionic solids
               Metallic solids and
               Covalent solids

  • Short notes on the structure of graphite and diamond
  • Solid A is a very hard electrical insulator in solid as well as in molten state and melts at extremely high temperature. What type of solid is it?

           Get the study material for the chapter The Solid State

  • Ionic solids conduct electricity in molten state but not in solid state. Explain
  • Significance of lattice point
  • Characteristics of crystal lattice
  • Define unit cell and mention the points to characterize a unit cell
  • Basic definitions of center unit cells(bcc,fcc,ecc)
  • Name the crystal system found in the given compounds:

               Zinc blende
               TiO2
               KNO3
               HgS

  • Concept to calculate the total number of atoms per cell in bcc, fcc and ecc
  • Distinguish between

             (i) Hexagonal and monoclinic unit cells
             (ii) Face-centred and end-centred unit cells.

  • Explain square close packing and hexagonal close packing of spheres in 2D and 3D with diagram
  • Relation between number of tetrahedral voids and octahedral voids
  • Write the name of the packing according to the given pattern:

               ABAB…..
               ABCABC…

  • Derivation of formula to calculate the packing efficiency for hcp, ccp and bcc

           Get the complete solution for the chapter The Solid State

  • Formula to calculate the density of solids
  • Which of the following lattices has the highest packing efficiency (i) simple cubic (ii) body-centred cubic and (iii) hexagonal close-packed lattice?
  • Basic differences and 2 examples for the following  

               stoichiometric defects
               impurity defects and
               non-stoichiometric defects.

  • Why ionic solids show Frenkel and Schottky defects rather than vacancy or interstitial defects
  • Frenkel and Schottky defects with example and diagram
  • Why Frenkel defect is termed as dislocation defect
  • What is f-center?
  • Explain the following with suitable examples:

               Ferromagnetism
               Paramagnetism
               Ferrimagnetism
               Antiferromagnetism
               12-16 and 13-15 group compounds.

Q. Select the incorrect statement regarding crystalline and amorphous solids

a. Amorphous solids are of irregular shape
b. Crystalline solids are isotropic in nature
c. Amorphous solids soften over a range of temperature.
d. Crystalline solids have characteristic geometrical shape.

Q. Which of the following solid is covalent solid?

a. CCl4
b. SiO2
c. ZnS
d. CO2

Q. A compound is formed by two elements A and B. The atoms of element A form hcp lattice and those of element B occupy 1/3 of the tetrahedral voids. The formula of the given compound is

a. AB
b. AB2
c. A2B
d. A3B2

Q. X-ray diffraction shows that an element crystallizes in a bcc unit cell with the cell edge of 2.55 × 10−8 cm. The density of the element is found to be 5.4 g cm−3.

a. 9.04 x 1023
b. 18.07 x 1023
c. 36.14 x 1023
d. 72.28 x 1023

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