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CBSE Class 12 Chemistry Question Bank – Solid State

CBSE Class 12 Chemistry Question Bank – Solid State

  1. What is a crystal?
  2. What are the different types of crystalline solids?
  3. Define a unit cell
  4. Why do atoms /ions in a crystal pack closely? Give two examples of close-packed structures.
  5. What are the coordination numbers for hcp and ccp structures?
  6. What do you understand by the term “ packing efficiency” ?
  7. What is radius ratio? What is its significance?
  8. Why do different ionic compounds assume different geometries of arrangement?
  9. What are the two type of holes or voids found in the close-packed structure of ionic compounds?
  10. What do you undersatand by defects in solids/
  11. What is the difference between a stoichiometric and a nonstoichiometric defect?
  12. What is a dopant? How does it affect the conductivity of a semiconductor?
  13. What are ferrimagnetic materials?
  14. Why do some solids exhibit magnetic properties?
  15. What type (n or p) of a semiconductor is created by the addition of arsenic to a crystal of germanium?
  16. Gallium arsenide can be made an n-type or p-type semiconductor by replacing some of the arsenic by another element.Which of the elements Se , Sb or Sn will work?
  17. Does the addition of Al2O3 to ZnO create an n-type or p-type semiconductor?
  18. Does doping ZnO with Li2O create an n-type or p-type semiconductor?
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Class 12 CBSE Chemistry Test Paper

1

Blood cells collapse when suspended in saline water. Account for it.

(1)

2

Name any two neutral oxides.

(1)

3

a) What is the principle behind reverse osmosis?

b) Which substance is usually added into water in the car radiator to act as antifreeze?

(2)

4

State Raoult’s law for a solution containing non-volatile solute.

(2)

     

5

Complete the following equations and also balance them.

i) NH4Cl + Ca(OH)2 clip_image002

ii) Zn + HNO3 clip_image004

iii) P4 + SOCl2clip_image004[1]

iv) MnO4 + HClclip_image006

(2)

6

Draw the structures of the following compounds.

i) Peroxodisulphuric acid

ii) Phosphorous acid and account for the basicity of phosphorous acid.

(2)

7

45 g of ethylene glycol ( C2H6O2) is mixed with 600g of water. Calculate (a) the freezing point depression and (b) the freezing point of the solution.

(3)

8

2 g of benzoic acid (C6H5COOH) dissolved in 25 g of benzene shows a depression in freezing point equal to 1.62 K. Molal depression constant for benzene is 4.9 K Kgmol-1. What is the percentage association of acid if it forms dimer in solution?

(3)

9

Arrange the following in the order indicated.

i) MF, MCl, MBr, MI – Decreasing ionic character.

ii)HOCl, HOBr, HOI – increasing acidic strength

iii)NH3, AsH3, SbH3, PH3 – Decreasing bond dissociation enthalpy

(3)

10

Give reasons for the following observations.

i)Halogens are strong oxidizing agents

ii)Noble gases have large positive electron gain enthalpy.

iii)Sulphur shows paramagnetic character in vapour phase.

(3)

11

How do you prepare XeO3 from XeF4? Write equation. Draw the structure of XeF6. Mention any two applications of He gas.

(3)

12

i) How is O3 estimated quantitatively?

ii)H2SO4 is a moderately strong acid. Give evidence.

ii)Though N2 exhibits +5 oxidation state, it doesnot form pentahalide. Why?

iv)Mention the conditions required for the maximum yield of NH3.

v)What happens when Cl2 reacts with excess NH3 and NH3 reacts with excess Cl2. Give equations.

(5)

13

i) With the help of a graph explain positive deviation.

ii)The vapour pressure of pure liquids A & B are 450 & 700mm Hg respectively at 350K. Find out the composition of the liquid mixture if total vapour pressure is 600mm Hg. Also find the composition of the vapour phase.

(5)

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Categories: AISSCE CHEMISTRY, CBSE Chemistry, Chemistry Model Papers, Chemistry Sample Papers, OLD QUESTION PAPERS, Question bank   Tags: , ,

Selected Questions for Class XI Chemistry

  1. State Aufbau Principle
  2. State Hund’s Rule
  3. State Pauli’s Exclusion principle
  4. State Heisenberg’s uncertainty principle.
  5. What are the Limitations of Thomson Model of atom?
  6. What are the Limitations of Rutherford Model of atom?
  7. What are the Limitations of Bohr Model of atom?
  8. State Pauli’s Exclusion principle
  9. State Modern periodic law.
  10. Explain sp, sp2 and sp3 hybridisation
  11. State Boyle’s law, Charle’s law, Avogadro’s lawand   Gaylussac’s law
  12. Explain the empirical derivation of gas equation
  13. Explain the concept of entropy
  14. State Hess’ law of constant heat summation
  15. Show that chemical equilibrium is synamic in nature
  16. State and explain Le Chatlier’s principle
  17. Why hydrogen is sjhown saparately in the periodic table?

More will be posted soon. You can also add more questions as comments.

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