Chemsitry 9th Class Model Papers

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2367
(I)





 2012-13











12 

Paper Code  
 15




	


























D 



 C , B , A







-





	




























	
	
Note:-  You have four choices for each objective type question as A, B, C and D.  The choice which you think is correct; fill 
that circle in front of that question number.  Use marker or pen to fill the circles. Cutting or filling two or more circles 
will result in zero mark in that question.
( D )
( C )
( B )
( A )
QUESTIONS
S.No
0.24
0.21
0.18
0.15
The number of     










	
CO2



8
moles in 8 grams of CO2 is equivlent to:
1
C2H5OH
CH3OH
C12H22O4
C6H12O6






	
CH2O
CH2O is the empirical formula of:
2
32
18
8
2











	
N-Shell
The maximum electrons in N-shell are:
3
Sr
Hg
Li
Zn






	
The lightest metal at room temperature is:
4
+ 3
+ 2
+ 1
Zero
The                  




	




18


Oxidation states of group 18 elements are
5

Five


Four

Three


Two
The number     





	 









	
C2H2
 of covalent bonds in C2H2 molecule are:
6

Nitrogen



Hydrogen





Boron


Flourine













	







	
A dative bond is formed between ammonia
and Boron triflourides, the donor atom is:
7
10.3 gcm-3
19.3 gcm-3
7.86 gcm-3
2.70 gcm-3







	
The density of gold is:
8



 






Methyl alcohol

Water



Liquid Ammonia




 






C2H5OH








	
The universal solvent in the following is:
9
+7
+5
+3
+1








	
HNO3
The oxidation state of Nitrogen in HNO3 is:
10











	
Which of the following is reduction  reaction?
11








Magnesium

Potassium


Silver


Gold
The most          
	
reactive metal 

 reactive metal among the following  is:
12
(I)





 2012-13





 




63 

 2.45

Part ------------------------ I

	
	
	
	
	
	
	
	
	
	
	
	
	
	
	



2. Answer briefly any FIVE parts from the following           5x2=10   











	
	2

	


	
Relative atomic mass
C-12
(i)  
       (i) Define relative atomic mass based on C-12 scale.
  (ii) Calculate the formula mass of Potassium Sulphate.                                   









	



	
(ii)
          The atomic mass of elements are;             K = 39 amu,           S = 32 amu,        O = 16 amu  
  (iii)  Differentiate between molecule and molecular ion.                                             





	 












	 













	
(iii)
(iv)  State four uses of isotope.                                                                                             



	








	
(iv)
(v)  Differentiate between shell and sub shell.                                                                













	
(v)
(vi)  Write the reaction of chlorine with hydrogen and water.                                






	



	
(vi)
(vii)  Compare two physical properties of metals and non-metals.                 






















	
(vii)
(viii) State two properties of positve rays                                                                       












	
viii
3. Answer briefly any SIX parts from the following           6x2=12   











	
	3
(i)  Define electron affinity with an example.                                             

	


	
Electron Afinity 


	
(i)
(ii)  Distinguish between period and group in periodic table.                                             











	
(ii)
(iii)  State the four salient features of Periodic Law.                                                              










	
(iii)
(iv)  Differentiate between lone pair and bond pair of electron.                        




 

 




	





(iv)
(v)  State the Octet and Duplet rules.                                                                        














	


	
(v)
(vi)  Define ionic bond with an example.                                                                  






	
	


	
(vi)
(vii)  Describe melting and boiling point of solids.                                             


















(vii)
(viii)  State the Charles's law.  Also write its mathematical representation.                







	










	




	
(viii)
(ix)  Describe two factors on which evaporation depneds upon.      









	



	
Evaporation
(ix)
4. Answer briefly any FIVE parts from the following         5x2=10    











	
	4


















	
(i)   
(i)  Justify with an example that the solubility of salt increases with the increase in temperature.
(ii)  Differentiate between true solution and colloidal solution.      







	
Colliodal Solution 



 True Solution (ii)
(iii)  Define aqueous solution with an example.                                          



	
	


	
Aqueous Solution(iii)
(iv)  Calculate the oxidation number of chlorine in KClO3 .                                      









	
KClO3 (iv)
 (v)  Differentiate between electrolytic cell and galvanic cell.           







	
Galvanic Cell



 Electrolytic Cell (v)
(vi)  Differentiate between valency and oxidation state.                                              





 












	
(vi)
(vii)  Differentiate between oxidizing and reducing agents.                         














	
(vii)
           (viii) Define Saturated solution and give example                                                                                      



	




 

	
	


	





viii
P.T.O.
( 2 )
Part ------------------------------- II

	
	
	
	
	
	
	
	
	
	
	
	
	
	
	
	
	
	



Note: Attempt any THREE questions.  
 7x3=21
 









	

	
4















	
6











	 





	


	
(a) 	5
5.  (a)  Define mole and molecule.  Calculate  number of moles, and number of molecules in 6 g of water.(1+1+1+1)
3           
                            























	
(b)
(b)  Describe Rutherford's atomic model . Also state two Observations  made by Rutherford. (1+1+1)           
4




	














	
a
	6
6.  (a) Define covalent bond. Explain single, double and triple covalent bond with example. (2+1+1+1)
3

	


	







Experimental






	


	




(b)
(b)   Define the Boyle's law. Explain the experimental verification of Boyle's law.  (1+2)
7.  (a)  Describe four rules for assigning oxidation number.          ( 1 x 4 )                  








	
(a) 	7
3


!
"










	

















	
(b)
(b)  Compare and contrast three chemical properties of Alkali metal and Alkaline earth metal.     ( 1 x 3 )
4







#







	









	









	
a 	
 8
(a)   Define electron affinity. why it increases in a period and decrease in a group in the Periodic Table   (1+1.5+1.5)



	
NaOH
	













500Cm3 , 0.4M








b
(b)   How much NaOH  is required to prepare its 500cm3 of 0.4M solution.
(a)  Differentiate between the following                                                     4                                                                










a
	9














 ii










 i
(i)    Molecular  Mass and Molar Mass                                (ii)     Chemical formula and Gram formula
   (b) Find out the Oxidration Numbers of the following:                                                 3                                                           










	
b
 (i)  S in Na2 SO4                 (ii) Mn in K Mn O4            (iii)      Cr in K2 Cr2 O7
Part ------------------------------- III

	
	
	
	
	
	
	
	
	
	
	
	
	
	
	
	
	
	


Note:- Attempt any TWO questions.                         (Practical)                                 










	
2
	

	
cm3







a
	10
8. i) What is the volume of liquid, to the nearest cm3  in the measuring cylinder.(2)














	
	
(ii)
ii) Which materials are attracted by a magnet?1x3=(3)
          Material
              Attracted by magnet or not    Yes/ No
            Plastic
          Copper
           Iron nails











	
	


(i
	11
	







	

1
2
	

















2
i) You are preparing crystals of pure Copper  Sulphate  from impure Copper Sulphate. What will be the:-                                                                                                                                                            
 1- Colour  of  pure Copper  Sulphate  crystals?
2- Shape of crystals & draw the diagram of crystals.           2                                                                                                                                
3 
	 Non conductor

Conductor















	
HCl



 NaOH NaCl



(ii
ii) You are provided solution of NaCl , NaOH, HCl, demonstrate the conductivity of different given solution by filling the
following table:     3  
Observations
Name of Solution
Bulb glows/Not glows
Result
1
NaCl
2
NaOH
3
HCl
2


	
	
Vapour Pressure















 i 	
 12
i)  Vapour pressure of which liquid will be higher at normal temperature , alcohol or water .
3










 

















	










 ii
(ii)  If you are provided few sugarcrystals and first heat gently and then strongly. Record your observations in the following table         1x3
Before Heating
After Gentle Heating
After Strong Heating
Colour of Sugar
Physical  state of Sugar