HBSE Class 11 Question Paper 2019 Chemistry

Code No. 1029
CLASS : 11th (Eleventh) Series : 11-M/2019
Roll No.











jlk;u foKku
CHEMISTRY
[ fgUnh ,oa vaxzsth ek/;e ]
[ Hindi and English Medium ]
(Only for Fresh/School Candidates)

le; : 3 ?k.Vs ] [ iw.kk±d : 70
Time allowed : 3 hours ] [ Maximum Marks : 70
• Ñi;k tk¡p dj ysa fd bl iz'u-i= esa eqfnzr i`"B 16 rFkk iz'u
34 gSaA
Please make sure that the printed pages in this
question paper are 16 in number and it contains
34 questions.
• iz'u-i= esa lcls Åij fn;s x;s dksM uEcj dks Nk= mÙkj-iqfLrdk
ds eq[;-i`"B ij fy[ksaA
The Code No. on the top of the question paper
should be written by the candidate on the front
page of the answer-book.
• Ñi;k iz'u dk mÙkj fy[kuk 'kq: djus ls igys] iz'u dk Øekad
vo'; fy[ksaA
Before beginning to answer a question, its Serial
Number must be written.
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• mÙkj-iqfLrdk ds chp esa [kkyh iUuk / iUus u NksMsa+A
Don’t leave blank page/pages in your answer-book.
• mÙkj-iqfLrdk ds vfrfjDr dksbZ vU; 'khV ugha feysxhA vr%
vko';drkuqlkj gh fy[ksa vkSj fy[kk mÙkj u dkVsaA
Except answer-book, no extra sheet will be given.
Write to the point and do not strike the written
answer.
• ijh{kkFkhZ viuk jksy ua0 iz'u&i= ij vo'; fy[ksaA
Candidates must write their Roll Number on the
question paper.
• d`i;k iz'uksa dk mÙkj nsus lss iwoZ ;g lqfuf'pr dj ysa fd iz'u-i=
iw.kZ o lgh gS] ijh{kk ds mijkUr bl lEcU/k esa dksbZ Hkh nkok
Lohdkj ugha fd;k tk;sxkA
Before answering the questions, ensure that you
have been supplied the correct and complete
question paper, no claim in this regard, will be
entertained after examination.

lkekU; funsZ'k %
General Instruction :
(i) lHkh iz'u vfuok;Z gSaA
All questions are compulsory.
(ii) çR;sd ç'u ds vad mlds lkeus n'kkZ, x, gSaA
Marks of each question are indicated against
it.

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(iii) ç'u Øekad 1 ls 14 rd cgqfodYih; ç'u gSaA çR;sd
ç'u 1 vad dk gaSA ftuds lgh mÙkj viuh mÙkj-iqfLrdk
esa fy[kus gSaA
Question Nos. 1 to 14 are multiple chocie
type questions carrying 1 mark each.
Candidate have to write the correct answer
in their answer-book.
(iv) ç'u Øekad 15 ls 24 rd vfr y?kwÙkjkRed ç'u gSaA
çR;sd ç'u 2 vadksa dk gSA çR;sd ç'u dk mÙkj yxHkx
30 'kCnksa esa nhft,A
Question Nos. 15 to 24 are very short
answer type questions carrying 2 marks
each. Answer these in about 30 words each.
(v) ç'u Øekad 25 ls 31 rd y?kwÙkjkRed ç'u gSaA çR;sd
ç'u 3 vadksa dk gSA çR;sd ç'u dk mÙkj yxHkx 40
'kCnksa esa nhft,A
Question Nos. 25 to 31 are short answer
type questions carrying 3 marks each.
Answer these in about 40 words each.
(vi) ç'u Øekad 32 ls 34 rd nh?kZ mÙkjkRed ç'u gSaA
çR;sd ç'u 5 vadksa dk gSA çR;sd ç'u dk mÙkj yxHkx
70 'kCnksa esa nhft,A

Question Nos. 32 to 34 are long answer type
questions of 5 marks each. Answer these in
about 70 words each.

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(vii) ç'u-i= esa lexz :i ls dksbZ fodYi ugha gSA rFkkfi 5
vadksa okys lHkh ç'uksa esa vkarfjd p;u çnku fd;k x;k
gSA ,sls ç'uksa esa ls vkidks dsoy ,d gh ç'u djuk gSA
There is no over all choice. However, internal
choice is given in all long answer type
questions of 5 marks each. You have to
attempt only one of the given choice in such
questions.

1. le-vk;uh Lih'kht gksrs gSa % 1

(A) Na + ,O − (B) F ,O 2 −
(C) Al 3 + ,P 3 + (D) F − ,O 2 −
Isoelectronic ions are :
(A) Na + ,O − (B) F ,O 2 −
(C) Al 3 + ,P 3 + (D) F − ,O 2 −

2. dkfLVd lksMk dk lw= gS % 1

(A) NaOH (B) Ca(OH )2
(C) Al (OH )3 (D) Na 2CO 3
Formula of Caustic Soda is :
(A) NaOH (B) Ca(OH )2
(C) Al (OH )3 (D) Na 2CO 3

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3. 22 xzke dkcZu MkbvkDlkbM esa fdrus eksy gS \ 1

(A) 1.0 (B) 1.5

(C) 2 (D) 0.5

Number of moles in 22 gram of carbondioxide
are :

(A) 1.0 (B) 1.5

(C) 2 (D) 0.5

4. d-CykWd ds rÙoksa dk bysDVªkWfud foU;kl gS % 1

(A) (n − 1)d1−10ns 2 (B) (n − 1)d 1−10ns 0 − 2
(C) (n − 1)d 1−10ns1− 2 (D) buesa ls dksbZ ugha
Electronic configuration of d-block elements is :
(A) (n − 1)d1−10ns 2 (B) (n − 1)d 1−10ns 0 − 2
(C) (n − 1)d 1−10ns1− 2 (D) None of these

80
5. 35
Br esa U;wVªkWuksa dh la[;k D;k gksxh \ 1

(A) 80 (B) 35
(C) 45 (D) 115
80
Number of Neutrons in 35 Br are :

(A) 80 (B) 35
(C) 45 (D) 115

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6. MnO 42 − esa Mn dh vkWDlhdj.k voLFkk gksxh % 1
(A) +7 (B) +6
(C) −2 (D) +2
Oxidation state of Mn in MnO 42 − is :
(A) +7 (B) +6
(C) −2 (D) +2

7. fdlesa f}/kzqo vk?kw.kZ 'kwU; gS \ 1

(A) SnCl 2 (B) SO 2
(C) H 2O (D) CCl 4
In which dipole moment is zero ?
(A) SnCl 2 (B) SO 2
(C) H 2O (D) CCl 4

8. lehdj.k 2 Cl (g) → Cl 2 (g) ds fy, ∆H o ∆S gksxh % 1

(A) +ve, −ve (B) +ve, +ve
(C) −ve, −ve (D) −ve, +ve
In equation 2 Cl (g) → Cl 2 (g) the value of ∆H and
∆S will be :
(A) +ve, −ve (B) +ve, +ve
(C) −ve, −ve (D) −ve, +ve

9. Hkkjh ty fdls dgrs gS \ 1

(A) H 2O 2 (B) H 2O
(C) D 2O (D) D 2O 2

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(7) 1029
Which is hard water ?
(A) H 2O 2 (B) H 2O

(C) D 2O (D) D 2O 2

10. gkbMªkstu dk ekud bysDVªksM foHko gS % 1

(A) 0.0V (B) −3.04V

(C) +2.85V (D) 1.0 V

Standard electrode potential of hydrogen is
taken as :

(A) 0.0V (B) −3.04V

(C) +2.85V (D) 1.0 V

11. LoPN ty esa BOD dk eku fdruk gksrk gS \ 1

(A) 5 ppm ls T;knk (B) 5 ppm ls de

(C) 17 ppm ls T;knk (D) buesa ls dksbZ ugha
Value of BOD in clean water will be :

(A) More than 5 ppm (B) Less than 5 ppm

(C) More than 17 ppm (D) None of these

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12. fLFkj nkc ij % 1
(A) ∆H = qV (B) ∆H = 0

(C) ∆H = ∆U − P∆V (D) ∆H = qp
At constant pressure :
(A) ∆H = qV (B) ∆H = 0

(C) ∆H = ∆U − P∆V (D) ∆H = qp

13. IykLVj vkWQ isfjl gksrk gS % 1
1
(A) CaSO 4 (B) CaSO 4 . H 2O
2
(C) CaSO 4 .2H 2O (D) CaOCl 2
Plaster of Paris is :
1
(A) CaSO 4 (B) CaSO 4 . H 2O
2
(C) CaSO 4 .2H 2O (D) CaOCl 2

14. fuEu esa ukfHkd Lusgh gS % 1
+
(A) OH − , H 2O (B) CH 3 , NC −
+
(C) C = O, CH 3 (D) OH − , R 3C +
In the following Nucleophiles are :
+
(A) OH − , H 2O (B) CH 3 , NC −
+
(C) C = O, CH 3 (D) OH − , R 3C +

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15. yqbl vEy o yqbl {kkjd fdls dgrs gSa \ çR;sd dk ,d-,d
mnkgj.k fyf[k,A 2

What are Lewis Acids and Lewis bases ? Give
one example for each.

16. vkoksxknzks ds fu;e dks le>kb,A 2

Discuss Avogadro's Law.

17. yhfFk;e o eSXusf'k;e esa dksbZ nks lekurk,¡ fyf[k,A 2

Write two similarities between Lithium and
Magnesium.

18. ty dh vLFkk;h dBksjrk nwj djus ds fy, DykdZ fof/k
(Clark's method) dh O;k[;k dhft,A 2

Explain Clark's method to remove temporary
hardness of water.

19. 0.01 M lksfM;e gkbMªkWDlkbM foy;u dk pH Kkr dhft,A 2

Calculate pH of 0.01 M solution of sodium
hydroxide.

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20. lehdj.kksa dks iwjk djsa % 2

(i) B 2H 6 + NH 3 →

(ii) BF3 + LiH →

Complete the reactions :

(i) B 2H 6 + NH 3 →

(ii) BF3 + LiH →

21. flfydkWu ds egÙoiw.kZ vuqç;ksx fyf[k,A 2

Write important applications of Silicons.

22. lehdj.k H 2 (g ) + I 2 (g ) º 2HI (g) ds fy, K o K
c p

dk eku D;k gksxk \ 2

For equation H 2 (g ) + I 2 (g ) º 2HI (g) give the
value of K c and K p .

23. vfrla;qXeu dks le>kb,A 2

Explain Hyperconjugation.

24. gdy fu;e (Huckel Rule) D;k gS \ le>kb,A 2

What is Huckel Rule ? Explain.

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25. fuEu dks ifjHkkf"kr dhft, % 3

(i) eksy va'k
(ii) eksyjrk
(iii) eksyyrk
Define the following :

(i) Mole fraction

(ii) Molarity

(iii) Molality

26. ,d oxZ o vkorZ esa fo|qr~ _.kkRedrk fdl çdkj ifjofrZr
gksrh gS \ O;k[;k dhft,A 3

How do electronegativity vary in a group and
period ? Explain.

27. 27°C rFkk 730 mm (Hg) nkc ij ,d xSl 300 ml
vk;ru ?ksjrh gSA STP ifjfLFkfr;ksa ¼rki o nkc½ ij bldk
vk;ru crkb,A 3

A gas has a volume of 300 ml at 27°C and
730 mm (Hg) pressure. What will be its volume
at standard conditions of temperature and
pressure ?

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28. fuEu dks ifjHkkf"kr djsa % 3

(i) eksyj xyu ,aFkSYih (∆H° fus.)
(ii) gsl dk fu;e
(iii) ,UVªkWih
Define the terms :

(i) Molar enthalpy of fusion (∆H° fus.)
(ii) Hess's Law
(iii) Entropy

29. Fe 2 + (aq ) + Cr2O 72 − (aq ) → Fe 3 + (aq ) + Cr 3 + (aq )

lehdj.k dks vEyh; ek/;e esa v)Z vfHkfØ;k fof/k }kjk
larqfyr dhft,A 3

Balance the given equation in acidic medium
using Half reaction method :

Fe 2 + (aq ) + Cr2O 72 − (aq ) → Fe 3 + (aq ) + Cr 3 + (aq )

30. fdlh ;kSfxd esa lYQj ds vkdyu dh dsfjvl fof/k dh foospuk
dhft,A 3

Discuss the Carius method for the estimation of
sulphur in organic compound.

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31. vEyh; o"kkZ ls vki D;k le>rs gSa \ blds ifj.kke D;k gSa \ 3

What is meant by Acidic Rain ? What are its
consequences ?

32. (a) cksj ekWMy dh lhek,¡ D;k gSa \ O;k[;k dhft,A 3

(b) d 2
x −y 2
o dxy d{kdksa dh lajpuk,¡ cukb,A 2

(a) What are limitations of Bohr's model ?
Explain.

(b) Draw shapes of d 2 and dxy orbitals.
x −y 2

vFkok
OR

(a) ikmyh viotZu fl)kar dh O;k[;k dhft,A 3

(b) uhys jax dh rjaxnS?;Z 4800 Å gSA bldh vko`fÙk (V ) vkSj
rjaxla[;k (V ) dk ifjdyu dhft,A 2

(a) Explain Pauli's Exclusion Principle.

(b) Calculate the frequency (V ) and wavenumber
(V ) of blue light of wavelength 4800 Å.

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33. vkf.od d{kd fl)kar ds vk/kkj ij vkWDlhtu dh vkca/k dksfV
o pqacdh; xq.k dh O;k[;k dhft,A 5

Explain bond order and magnetic behaviour of
oxygen molecule on the basis of molecular
orbital theory.

vFkok
OR

ladj.k ls vki D;k le>rs gSa \ ladj.k ds vk/kkj ij C 2H 2
o NH 3 v.kqvksa dh lajpuk,¡ le>kb,A 5

What is Hybridisation ? On the basis of
hybridization explain shapes of C 2H 2 and NH 3
molecules.

34. fuEufyf[kr dk foLr`r o.kZu djsa % 5

(a) ekdksZuhdkWQ fu;e
(b) ÝhMsy Øk¶V ,sflyhdj.k
Explain the following in detail :

(a) Markovnikov rule

(b) Friedal Craft acylation

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vFkok

OR

fuEu vfHkfØ;kvksa dks iwjk dhft, % 5

UV
(i) + Cl 2 →
500 K

lkanz H SO4
(ii) +  2  →
∆

2 
(iii) CH 3CH 2OH   
lkaæ H SO
4 →
∆

3 → (i ) O
(iv) CH 3CH = CH 2  

(ii ) Zn , H 2O

(v)
,Ydks
s gkWy
CH 3CH 2Br    
→
KOH

Complete the following reactions :

UV
(i) + Cl 2 →
500 K

Conc . H SO
(ii)   2 
4 →

∆

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Conc . H SO
(iii) CH 3CH 2OH   2 
4 →

∆

(i ) O
3 →
(iv) CH 3CH = CH 2  

(ii ) Zn , H 2O

Alcoholic
(v) CH 3CH 2Br   →
KOH

S

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