AP Class 11 Model Paper Chemistry

FOR AP CLASS 11 EXAM PREPARATION

AP Class 11
Model Paper ·
Chemistry
EXAM YEAR TYPE SUBJECT

AP Class 11 — Model Paper Chemistry

Notes · Sample Papers · Previous Year Papers · Mock Tests

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Answers 396

BOARD OF INTERMEDIATE EDUCATION: ANDHRA PRADESH
INTERMEDIATE 1ST YEAR – CHEMISTRY

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MODEL QUESTION PAPER-1 (Effective from IPE MARCH 2026)
TIME : 3 HOURS]
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e m .
e m SECTION-A
l as
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l carries one mark. ag
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I. Answer ALL the following questions.

a
Each question 9 × 1 = 9 Marks
1. Which one of the following pairs of the compounds illustrate the law of multiple proportions?

(1) H2O & Na2O (2) MgO & Na2O (3) Na2O & BaO (4) SnCl2 & SnCl4

2. Increasing order for the values of e/m for electron (e), proton (p), neutron (n) and
-particles is

(1) e < p < n <  (2) n < < p < e (3) n < p < e <  (4) n < p < < e

o m
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3. Which of the following oxide, when dissolved in water form an acidic solution ?

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(1) Na O (2) CO (3) Al O (4) Cl O

a
2 2 3 2 7

l
agamount of heat is supplied to the system. What type of
4. What is the shape of NH ion ? +
4

5. Work is done by the system and ‘q’
system would it be ?

6. What is the value of Kw at 25ŗC ?

7. Reductant is the element which can reduce the other substances and itself undergoes_________.

8. Ethyl alcohol and methyl alcohol can be separated by _____________.

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9. The possible Isomers for C4H10 are ____________.

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c. oAnswer ALL the following questions. e m
SECTION-B

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e Each question carries two marks.
II.

l as
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la 10. How many moles of glucose are present in 540 g of glucose ? ag 14×2=28 Marks

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11. Calculate the volume of O2 at STP required to completely burn 100 mL of acetylene.

12. What is the frequency of radiation of wavelength 600nm ?

13. What is Hund’s rule ?

14. An element ‘X’ has atomic number 34. Give it’s position in the periodic table.

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Answers 397

15. Water is a liquid at room temperature, but hydrogen sulphide is a gas. Give reason.

16. What is meant by bond order ?

17. What are intensive and extensive properties ?

18. What is meant by dynamic equilibrium ?

19. What is disproportionation reaction? Give example.
20. What is the hybridization of carbon in CH3F ?
21. What is distillation ?
22. What is Friedel-Crafts alkylation ?
23. Explain the structural isomerism with one example.

SECTION-C
III. Answer ANY EIGHT of the following questions.
Each question carries four marks. 8×4=32 Marks
24. A carbon compound contains 12.8% carbon, 2.1% hydrogen and 85.1% bromine. The
molecular mass of the compound is 187.9 u. Calculate its molecular formula.
25. What is a nodal plane ? How many nodal planes are possible for 2p, and 3d orbitals ?
26. Give any four characteristic properties of transition elements.
27. Explain the structure of CH4 molecule.
28. Explain the hybridisation involved in PCl5 molecule.
29. Define heat capacity. What are Cp and Cv ? Show that Cp – Cv = R.
30. Define and explain the standard enthalpy of formation (f H).
31. State Le Chateliers's Principle. Discuss the application of Le Chatelier's principle for the
industrial synthesis of Ammonia by Haber's process.
32. Explain Lewis acids and bases with suitable examples. Classify the following species into
Lewis acids and Lewis bases.
a) OH– b) F– c) H+ d) BCl3
33. Balance the following redox reactions by ion-electron method (in acidic medium):
Cr2O72– (aq) + SO32– (aq)  Cr3+ (aq) + SO42– (aq)
34. What are different types of organic reactions ?
35. What is dehydrohalogenation ? Write the equation for the formation of alkene from alkyl
halide.

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Answers 398

SECTION-D
IV. Answer ANY TWO of the following questions.
Each question carries eight marks. 2×8=16 Marks
36. What are the postulates of Bohr's model of hydrogen atom ? Discuss the importance of this
model to explain various series of line spectra in hydrogen atom.
37. Write an essay on s,p,d, and f-block elements.
38. Describe two methods of preparation of Ethylene. How does it reacts with the following. Give
equations.
a) Ozone b) Cold and dil.alk KMnO4 c) Br2

v v v

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426  -I

  
  
m
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 (IPE )
]
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[  : 85
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e  l
  - A
l as a g
a g
I. 
 9 × 1 = 9 

1. 
(1) H2O & Na2O (2) MgO & Na2O (3) Na2O & BaO (4) SnCl2 & SnCl4
2.  (e),  (p), (n)  -e/m 
(1) e < p < n <  (2) n < < p < e (3) n < p < e <  (4) n < p < < e

m
 

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3.

m
(1) Na2O (2) CO (3) Al2O3 (4) Cl2O7

e
s    
a
4. NH4+  

l
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5.  ‘q’  
6. K 25ºC 
w

7. 
 
  _________  
8.      _____________.
9. C4H10  ____________.

om
  - B

m
 
c.14×2=28
co 
II.

m
m. s e 
s e 10. 540    g l a
g la 11. 100 mL    O 
a STP  
a 12. 600 nm  
 
2

13. 
14. ‘X’ 
   
15.    H2O  SO2  

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 427

16. 
17.  (extensive),  (intensive)  
18.  
19.       
20. CH3F   
21. 
22.     
23. 
  - C
III.   
  8×4=32 

24.   12.8% , 2.1% 85.1%  187.9 u. 

25. 2p, 3d 
26.      
27. CH4 

28. PCl5   
29.    Cp  Cv  Cp – Cv = R 
30.       (f H) 
31.     

32.  
 
a) OH– b) F– c) H+ d) BCl3
33.  
     
Cr2O72– () + SO32– ()  Cr3+ () + SO42– ()
34.  
35.      

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428  -I

  - D
IV.   
  2×8=16 

36.           

37. s,p,d, f-  

38.    
a)  b)    KMnO4 c) Br2

v v v

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