HBSE Class 11 Sample Paper 2027 Chemistry

FOR HARYANA CLASS 11 PREPARATION

HBSE Class 11 Sample
Paper 2027 Chemistry
EXAM YEAR TYPE SUBJECT

Haryana Class 11 2027 Sample Paper Chemistry

Notes · Sample Papers · Previous Year Papers · Mock Tests

m
m .co

m .co s e m
se g l a
th a
CLASS:11 (Sr. Secondary)
Roll No.

CHEMISTRY m
m [Hindi and English Medium] .co
m .co s e m
s e
[Time allowed: 3 hours] [Maximum Marks: 70] la
g l a ag
a
• d`I;k lqfuf”pr djsa fd bl iz”u i= esa eqfnzr i`’B la[;k esa 12 gS vkSj blesa
35 iz”u gSA
Please make sure that the printed pages in this question paper are 12 in
number and it contains 35 questions.
•
o m Nk= }kjk mÙkj iqfLrdk ds igys
iz”u i= ds nkbZ vksj fn, x, dksM uEcj dks
i`’B ij fy[kk tkuk pkfg,A .c
s em
la
The Code No. on the right side of the question paper should be written by
g
the candidate on the front a
page of the answerbook.
• fdlh iz”u dk mÙkj “kq: djus ls igys mldk Øekad fy[kuk gksxkA
Before beginning to answer a question, its Serial Number must be written.
• viuh mÙkj iqfLrdk esa [kkyh iUuk@iUus u NksM+sA
Don’t leave blank page/pages in your answer-book.
o m
m . c
c. o • mÙkj s e m
iqfLrdk ds vfrfjDr dksbZ vU; lhV ugha nh tk,xh vr% vko”;drkuq lkj
e m gh fy[ks o fy[ks mÙkj dks u dkVsaA
l a
l as g
a to the point and
ag
Except answer-book, no extra sheet will be given. Write
do not strike the written answer.
• ijh{kkFkhZ viuk jksy uEcj iz”u i= ij vo”; fy[ksaA
Candidates must write their Roll Number on the question paper.
• d`Ik;k iz”uksa dk mÙkj nsus ls iwoZ ;g lqfuf”pr dj ysa fd iz”u i= iw.kZ o lgh
gS] ijh{kk ds mijkUr bl laca/k esa dksbZ Hkh nkok Lohdkj ugha fd;k tk,xkA
m .
.co s e m
s em l a
g la ag
a For more Question Papers, Sample Papers, Notes & Syllabus visit Page 1 of 16

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 %
(i) lHkh iz”u vfuok;Z gSA
(ii) oLrqfu’B iz”uksa ds mÙkj lgh fodYi fy[ksaA
(iii) izR;sd iz”u ds vad mlds lkeus n”kkZ, x, gSaA
General Instructions:
i) All questions are compulsory.
ii) Write the correct option in objective type questions.
iii) Marks of each question are indicated against it.
1. Which of the following is independent of temperature? 1
(a) Molarity (b) Formality
(c) Normality (d) Molality
fuEufyf[kr esa ls dkSu rkieku ls Lora== gS\
(a) eksyfjVh (b) vkSipkfjdrk
(c) lk/kkj.k voLFkk (d) eksySfyVh
2. Number of significant figures in 2.005 are : 1
(a) 1 (b) 2

(c) 3 (d) 4
2-005 esa lkFkZd vadks dh la[;k gS %
(a) 1 (b) 2

(c) 3 (d) 4
3. Which series series of lines is the only series in the hydrogen spectrum
which appears in the visible region of electromagnetic spectrum ? 1
(a) Lymen (b) Balmer
(c) Paschen (d) Bracket

For more Question Papers, Sample Papers, Notes & Syllabus visit Page 2 of 16

m
m .co

m .co s em
se g la
a Js.kh gS tks fo|qr pqacdh;
gkbMªkstu LisVªe esa js[kkvksa dh dkSu&lh Js.kh ,dek=
LisVªe ds n`”;&{ks= esa izkIr gksrh gS\
(a) ykbeSu (b) ckej
(c) ik”pu (d) czsdVs
Out of isoelectronic ions 0 2- ,F - , Na + and Mg 2+ , which will have
4.
m
smallest radius ? m 1 .co
.co s e m
em
2-
(a) 0 (b) Na+
s l a
(c) la Mg
g
2+
(d) F- ag
alebys 2-
DVªkWfud vk;uksa 0 ,F , Na - +
vkSj Mg 2+ esa ls fdldh f=T;k U;wure
gS\
(a) 0 2- (b) Na+
(c) Mg 2+ (d) F-

m
.co
5. CH 2 = CH 2 + Br 2 ⎯ X
Here X is : e m 1
las
(a) CH 2 – CH 2
ag (b) CH 2 = CHBr
Br Br
(c) CH  CH (d) CH = CH
Br Br

CH 2 = CH 2 + Br 2 ⎯ X
m
m ;gk¡ mRikn gS% .co
m .co (a) CH 2 – CH 2 (b) s e
CH 2 = CHBr
m
s e g l a
g la Br Br a
a (c) CH  CH (d) CH = CH
Br Br
6. The repulsive interaction of electron pair decrease in the order
(Here lp = lone pair, bp = bond pair) 1
(a) bp – bp > lp – bp > lp – lp
m .
.co s e m
s em l a
g la ag
a For more Question Papers, Sample Papers, Notes & Syllabus visit Page 3 of 16

(b) lp – lp > lp – bp > bp - bp
(c) lp – lp > bp – bp > lp – bp
(d) bp – bp > lp – lp > lp – bp
bysDVªku ;qXeksa ds chp izfrd’kZ.k vU;ksU; fdz;k,¡ fuEufyf[kr Øe esa ?kVrh gSa
¼;gk¡ ,dkdh ;qXe] vkca/kh ;qXe½ %
(a) bp – bp > lp – bp > lp – lp
(b) lp – lp > lp – bp > bp - bp
(c) lp – lp > bp – bp > lp – bp
(d) bp – bp > lp – lp > lp – bp
7. State of hybridisation of carbon in HCHO is: 1
(a) sp (b) sp2
(c) sp3 (d) dsp 2
HCHO esa dkcZu dh ladj.k voLFkk gS %
(a) sp (b) sp 2
(c) sp3 (d) dsp 2
8. If concentration of hydrogen ion [H+ ] changes by a factor of 100, then
the value of pH changes by:- 1
(a) one unit (b) 2 unit
(c) 10 unit (d) 100 unit
;fn gkbMªkstu vk;u lkanzrk esa 100 xq.kd dk ifjorZu gks] rks ds eku esa
ifjorZu gksxk %
(a) ,d bdkbZ (b) 2 bdkbZ
(c) 10 bdkbZ (d) 100 bdkbZ
9. Which of the following species do not show disproportionation
reaction? 1
(a) 𝐶𝑙𝑂 (b) 𝐶𝑙𝑂
(c) 𝐶𝑙𝑂 (d) 𝐶𝑙𝑂

For more Question Papers, Sample Papers, Notes & Syllabus visit Page 4 of 16

m
m .co

m .co s em
se g la
fuEufyf[kr esa ls dkSu&lh Lih”kht vlekuqikruaizo`fr ugha n”kkZrh \
(a) 𝐶𝑙𝑂 (b) 𝐶𝑙𝑂
(c) 𝐶𝑙𝑂 (d) 𝐶𝑙𝑂
Fill in the blanks in following questions (10-12) :
fuEufyf[kr iz”uksa ¼10&12½ esa fjDr LFkku Hkjsa % m
m .co
10.
.co
Oxidation number of Sulphur (S) in H2S2O7 is …………………. 1
s e m
s em
H2S2O7 esa lYQj dh vkWDlhdj.k la[;k ------------------------ gSaA l a
g l a a1g
11. aTotal number of sigma (𝜎) and pi () bonds in C H is …………………. 2 2

C2H2 v.kq esa flXek (𝜎) rFkk ikbZ () vkca/kksa dh dqy la[;k ----------------------- gSA

12. The conjugate base of 𝑁𝐻 is ………………… 1
𝑁𝐻 dk la;qXeh {kkjd --------------------------------- gSA
Answer the following questions (13-15) in one word/sentence:
m
fuEufyf[kr iz”uksa ¼13&15½ ds mRrj ,d.co
“kCn@okD; esa nhft, %
e m
13.
las
Draw the Lewis structure for H2S. 1
g
H S v.kq dh ywbl lajpuk afyf[k,A
2

14. Write the formula of the compound Iron (III) sulphate. 1
vk;ju (III) lYQsV ;kSfxd dk lw= fyf[k,A
15. Given the standard electrode potentials, arrange these metals in their increasing
order of reducing power: 1
m
m K+ / K = -2.93 V, Ag+ / Ag = 0.80V .co
m .co Hg2+ / Hg = 0.79 V, Mg2+ / Mg = -2.37V s em
s e g l a
g la aksa dks mudh c<+rh
uhps fn, x, ekud bysDVªksM foHkoksa ds vk/kkj ij /kkrqv
a vipk;d {kerk ds Øe esa fyf[k,%
K+ / K = -2.93 V, Ag+ / Ag = 0.80V
Hg2+ / Hg = 0.79 V, Mg2+ / Mg = -2.37V
Note: In the following questions (Q. Nos. 16, 17 and 18 ) two statements are given for
each. Assertion (A) and Reason (R). Study both the statement carefully and
m .
.co s e m
s em l a
g la ag
a For more Question Papers, Sample Papers, Notes & Syllabus visit Page 5 of 16

decide which answer option is correct and write the correct answer by selecting
the given options (a), (b), (c), & (d):
Options:
(a) Both Assertion (A) and Reason (R) are true and Reason (R) is the correct
explanation of Assertion (A).
(b) Both Assertion (A) and Reason (R) are true, but Reason (R) is not the
correct explanation of Assertion (A).
(c) Assertion (A) is true, but Reason (R) is false.
(d) Assertion (A) is false, but Reason (R) is true.
uksV % fuEufyf[kr iz”uksa ¼iz0 la0 16] 17 ,oa 18½ esa nks dFku fn;s x;s gSaA
vfHkdFku(A) rFkk dkj.k(R) nksuksa dFkuksa dk /;kuiwoZd v/;;u djsa ,oa fu.kZ;
yhft, dh dkSu&lk mRrj fodYi lgh gS rFkk lgh mRrj dks fn;s x;s fodYi
(a), (b), (c), & (d) ,oa esa ls pqudj fyf[k, %

fodYi %
(a) vfHkdFku rFkk dkj.k nksuksa lR; gS vkSj dkj.k vfHkdFku dh lgh
O;k[;k gSA
(b) vfHkdFku rFkk dkj.k nksuksa lR; gS] ijUrq dkj.k vfHkdFku dh lgh
O;k[;k ugh gSA
(c) vfHkdFku lR; gS] ijUrq dkj.k vlR; gSA
(d) vfHkdFku vlR; gS] ijUrq dkj.k lR; gSA
16. Assertion (A) : Trans-But-2-ene has higher melting point than cis form. 1
Reason (R): Cis-But-2-ene is more polar than trans form.
vfHkdFku (A) % foi{k&C;wV&2&bZu dk xyukad lei{k C;wV&2&bZu ls mPp
gksrk gSA
dkj.k (R) % ,Ydhu dk lei{k :i] foi{k dh rqyuk esa vf/kd /kzqoh;
gksrk gSA
17. Assertion (A): Noble gases are highly reactive. 1
Reason (R): Noble gases have stable closed shell electronic configuration.
vfHkdFku (A) % mRd`’V xSlsa vf/kd fØ;k”khy gksrh gSA

For more Question Papers, Sample Papers, Notes & Syllabus visit Page 6 of 16

m
m .co

m .co s em
se g la
a DVªkWfud foU;kl gksrk gSA
dkj.k (R) % mRd`’V xSalksa esa fLFkj cUn dks”k bys
18. Assertion (A) : The bond order of helium molecule is zero. 1
Reason (R) : The number of electrons in bonding molecular orbitals and
anti-bonding molecular orbitals are equal in helium
molecule.
m
.co
vfHkdFku (A) % ghfy;e v.kq dk vkca/k dksfV “kwU; gSA
om ghfy;e esa vkca/kh vkf.od d{kdksa ,oa izfr&vkca/kh vkf.od em
dkj.k (R) .% c
em d{kdksa esa mifLFkr bysDVªkWuksa dh la[;k cjkcj gksrh gSA gla
s
las a
ag Section – B
[k.M & c
(Very Short Answer Type Questions)
¼vfr&y?kwÙkjkRed iz”u½
19. What is law of multiple proportion? Explain with example. 2

.c lfgr Li’V dhft,A
xqf.kr vuqikr dk fu;e D;k gS\ mnkgj.k om
s em
20.
la
State and explain ‘Heisenberg Uncertainty Principle’.
g
2
^gkbtsucxZ dk vfuf”prrk afl)kUr* crkb, o le>kb,A
21. How do atomic radius vary in a period and in a group? How do you explain the
variation? 2
fdlh oxZ ;k vkorZ esa ijek.kq f=T;k fdl izdkj ifjofrZr gksrh gS\ bl
ifjorZu dh O;k[;k vki fdl izdkj djsax\s
m
.co
22. What is the basic difference between the terms ‘electron gain enthalpy’ and
m
m .co ‘electronegativity’?
s em 2

s e ^bysDVªkWu yfC/k ,UFkSYih* vkSj ^bysDVªkWu _.kkRedrk* esa D;klaewy vUrj gS\
la a g
ag 23. Describe the effect of : 2
(i) addition of H2 (ii) removal of CH3OH on the
equilibrium 2H2(g) + CO (g) ←⃑CH3OH(g)

lkE; 2H2(g) + CO (g) ←⃑CH3OH(g) ij fuEufyf[kr dk izHkko crkb, %
(i) H2 feykus ij (ii) CH3OH gVkus ij
m .
.co s e m
s em l a
g la ag
a For more Question Papers, Sample Papers, Notes & Syllabus visit Page 7 of 16

(OR)
vFkok
What are buffer solutions? Give example.
cQj&foy;u D;k gSa \ mnkgj.k nhft,A
24. Balance the following redox reaction by ion-electron method: 2
Mn𝑂 (𝑎𝑞) + 𝐼 (𝑎𝑞) → 𝑀𝑛𝑂 (𝑠) + 𝐼 (𝑠)
(In acidic medium)
vk;u&bysDVªkWu fof/k }kjk fuEufyf[kr jsMkWDl vfHkfØ;k dks larqfyr dhft, %
Mn𝑂 (𝑎𝑞) + 𝐼 (𝑎𝑞) → 𝑀𝑛𝑂 (𝑠) + 𝐼 (𝑠)
¼vEyh; ek/;e½
(OR)
vFkok
Consider the elements: Cs, Ne, I and F identify the element that:
(i) exhibits only negative oxidation state.
(ii) exhibits only positive oxidation state.
(iii) exhibits both negative and positive oxidation state.
(iv) exhibits neither negative nor positive oxidation state.
Cs, Ne, I rFkk F esa ,sls rRoksa dh igpku dhft,] tks %

(i) dsoy _.kkRed vkWDlhdj.k voLFkk iznf”kZr djrk gSA
(ii) dsoy /kukRed vkWDlhdj.k voLFkk iznf”kZr djrk gSA
(iii) _.kkRed rFkk /kukRed nksuksa vkWDlhdj.k voLFkk iznf”kZr djrk gSA
(iv) u _.kkRed vkSj u gh /kukRed vkWDlhdj.k voLFkk iznf”kZr djrk gSA
25. Explain ‘functional group isomerism’ with the help of suitable example. 2
^fØ;kRed lewg leko;ork* dks mi;qDr mnkgj.k dh lgk;rk ls Li’V dhft,A
(OR)

For more Question Papers, Sample Papers, Notes & Syllabus visit Page 8 of 16

m
m .co

m .co s e m
se g l a
vFkok a
Write IUPAC names of the following compounds: 2
(i) CH2 = CH – CH – COOH
OH
(ii) OH
m
m .co
.co s e m
s em Br l a
g la ;kSfxdksa ds vkbZ0;w0ih0,0lh0 uke fyf[k, % ag
a
fuEufyf[kr
(i) CH2 = CH – CH – COOH
OH
(ii) OH

m
Br
.co
s em
g la – C
Section
a
[k.M & l
(Short Answer Type Questions)
¼y?kwÙkjkRed iz”u½
26. (i) Define the term mole fraction. 1
m
m eksy&va”k dks ifjHkkf’kr dhft,A
.co
m .co (ii) s
Calculate the molarity of NaOH in the solution prepared by dissolving its e m
s e 5 gram in enough water to form 250ml of solution. g l
2 a
g la a
a NaOH ds ,sls foy;u dh eksyjrk dk ifjdyu dhft,] ftls 5 xzke
NaOH dks ty dh i;kZIr ek=k esa feykdj izkIr fd;k x;k gks] rkfd
foy;u 250 feyhyhVj gks tk;sA
27. (i) For the reaction 2𝐶𝑙(𝑔) → 𝐶𝑙 (𝑔), what are the sign of H and S? 1

vfHkfØ;k 2𝐶𝑙(𝑔) → 𝐶𝑙 (𝑔) ds fy, H ,o S ads fpg~u D;k gksaxs\
m .
.co s e m
s em l a
g la ag
a For more Question Papers, Sample Papers, Notes & Syllabus visit Page 9 of 16

(ii) On 300 K, the equilibrium constant for a reaction is 10. What will be the
value of G0? (R = 8.314 JK-1 mol-1) 2

300 K ij ,d vfHkfØ;k ds fy, lkE; fLFkjkad 10 gSA G0 dk eku D;k
gksxk\ (R = 8.314 JK-1 mol-1)
28. (i) What is pH? 1
pH D;k gS \
(ii) Assuming complete dissociation, calculate the pH of 0.002 M KOH. 2
iw.kZ fo;kstu ekurs gq, 0.002 M KOH foy;u dh pH Kkr dhft,A
29. (i) Identify the underlined reagent in the following equations as nucleophile
or elctrophile: 1
(a) CH3Br + HO-  CH3OH + Br- COCH3

(b) + 𝐶𝐻 𝐶𝑂 →

fuEufyf[kr lehdj.kksa esa js[kkafdr vfHkdeZdksa dh ukfHkdLusgh rFkk
bysDVªkWuLusgh ds rkSj ij igpku dhft, %
(a) CH3Br + HO-  CH3OH + Br- COCH3

(b) + 𝐶𝐻 𝐶 𝑂 →

(ii) Which of the following is expected to be more stable and why? 2
NO2CH2CH2O- and CH3CH2O-
fuEufyf[kr esa ls dkSu&lk vf/kd LFkk;h gS rFkk D;ks\a
NO2CH2CH2O- vkSj CH3CH2O-

(OR)
vFkok
What is resonance effect? Explain its types by giving one example of each.
vuqukn izHkko D;k gS \ izR;sd dk ,d mnkgj.k nsrs gq,] blds izdkjksa dks Li’V
dhft,A

For more Question Papers, Sample Papers, Notes & Syllabus visit Page 10 of 16

m
m .co

m .co s e m
se g l a
30. (i) Complete the reaction: a 1
/
CH3-C  CH + H2O ⎯⎯⎯⎯⎯
333k
vfHkfØ;k dks iwjk djsa %
/
CH3-C  CH + H2O ⎯⎯⎯⎯⎯
333k
m
(ii)
c o m
Explain ozonolysis with example. 2
m .co
tks.uh vi?kVu dh mnkgj.k lfgr O;k[;k dhft,A
vksm s e
s e l a
g l a (OR) ag
a vFkok
(i) Write the name and structural formula of the alkane used for the
preparation toluene by the process of ‘aromatization’. 1
^,sjkseSVhdj.k* izfØ;k }kjk VkWywbZu ds fojpu ds fy, iz;ksx fd;s tkus
okys ,Ydsu dk lajpukRed lw= o uke fyf[k,A
m
(ii) .co
What happened when 1, 2-Dichloroethane is treated with alcoholic KOH
em
followed by reaction with sodamide.
s
g la jksbFksu dks ,Ydksgfyd ds lkFk mipkfjr
D;k gksrk gS] tc 1] 2&MkbDyks
a
djds bldh vfHkfØ;k lksMkekbM ds lkFk dh tkrh gSA
Section – D
[k.M & n
(Case Study Type Questions)
m
.co
¼dsl v/;;u izdkj ds iz”u½
m
c. o31. The following questions (31 & 32) are case based. Read the case
s e mcarefully and
s em answer the questions that follow:
g l a
la a
ag fuEufyf[kr iz”u ¼31 ,oa 32½ dsl vk/kkfjr gSA dsl dks /;kuiwoZd i<+as vkSj
uhps fn;s x;s iz”uksa ds mRrj nsa %
Case :
Neither decrease in enthalpy nor increase in entropy alone can determine the
direction of spontaneous change for a system. For this purpose, a new
thermodynamic function is defined, which is Gibbs energy or Gibbs function. It
m .
.co s e m
s em l a
g la ag
a For more Question Papers, Sample Papers, Notes & Syllabus visit Page 11 of 16

is denoted by G and mathematically expressed as G = H – TS. Here H is
enthalpy and S is entropy of system. Gibbs function G is extensive property and
state function. If change in Gibbs energy G is negative, the process is
spontaneous. If G is positive, the process is non – spontaneous and if G is
zero, the process is in equilibrium.
Questions :
(i) Define the term extensive properties. 1
(ii) Write the unit of G. 1
(iii) For the reaction : 2
2 A(g) + B(g)  2 D(g)

𝑈 = -10.5 kJ and 𝑆 = -44.1 J𝐾 . Calculate 𝐺 for the reaction and
predict whether the reaction may occur spontaneously?
(R = 8.314 x 10-3 kJ K-1mol-1, T = 298K)
(OR)
Comment on the spontaneity of a reaction at constant temperature and
pressure in the following cases: 2
(i) H < 0 and S > 0 (ii) H > 0 and S < 0

(iii) H < 0 and S < 0 (iv) H > 0 and S > 0
dsl %
u rks dsoy ,UFkSYih esa deh vkSj] u gh ,UVªkWih esa o`f) Lor% izofrZr izdeksa dh
fn”kk fu/kkZfjr djrh gSA bl iz;kstu gsrq ge ,d u, Å’ekxfrdh Qyu dks
ifjHkkf’kr djrs gSaA tks fxCt ÅtkZ ;k fxCt Qyu gSA bls G }kjk fu:fir
fd;k tkrk gS vkSj xf.krh; :i ls G = H - TS ds :i esa O;Dr fd;k tkrk gSA
;gk¡ ,UFkSYih vkSj S fudk; dh ,UVªkWih gSA fxCt Qyu G foLrh.kZ xq.k ,oa ,d
voLFkk Qyu gSA ;fn fudk; dh fxCt ÅtkZ esa ifjorZu G _.kkRed gS] rc
izØe Lor% izofrZr gksrk gSA ;fn G /kukRed gS] rc vLor% izofrZr gksxk vkSj
;fn G “kwU; gS] rks izØe lkE; voLFkk esa gksxkA
iz”u %
(i) foLrh.kZ xq.k dks ifjHkkf’kr dhft,A
(ii) G dh bdkbZ fyf[k,A

For more Question Papers, Sample Papers, Notes & Syllabus visit Page 12 of 16

m
m .co

m .co s em
se g la
(iii) a 𝑈 = -10.5 kJ ,oa 𝑆 = -
vfHkfØ;k 2 A(g) + B(g)  2 D(g) ds fy,
44.1 J𝐾 gSA vfHkfØ;k ds fy, 𝐺 dh x.kuk dhft, vkSj crkb, fd
D;k vfHkfØ;k Lor% izofrZr gksxh \
(R = 8.314 x 10-3 kJ K-1mol-1, T = 298K)
vFkok
m
o m a esa fLFkj rki o nkc ij fdlh vfHkfØ;k dh Lor%
fuEufyf[kr ifjfLFkfr;ks
c fVIi.kh dhft, % m .co
izofrZr gksus .ij e
e m l as
l s
(i) a H < 0 vkSj S > 0 (ii) H > 0 vkSj S < 0
ag
g
a(iii) H < 0 vkSj S < 0 (iv) H > 0 vkSj S > 0
32. During the organic reaction, a covalent bond between two carbon atoms or a
carbon atom and some other atom is broken and a new bond is formed. The
fission of bonds may be homolytic or heterolytic forming free radicals,
carbocations, carbanions etc. This depends upon the displacement of electron in
a bond and is governed by inductive effect, eletromeric effect, resonance effect
m
hyperconjugation.
.co
(i)
s em
Give correct order of relative stability of the following carbanions: 1

g la 𝐶𝑙, 𝐶𝐻𝐶𝑙 , 𝐶𝐶𝑙
a
𝐶𝐻 , 𝐶𝐻 , 𝐶𝐻 , 𝐶𝐻
(ii) What happened when 𝐶𝐻 𝐶𝑙 undergo homolytic fission? 1
(iii) Do (𝐶𝐻 ) 𝐶 and (𝐶𝐻 ) 𝐶 have same structure? Explain. 2
(OR)
Which of the two Pℎ 𝐶 or (𝐶𝐻 ) 𝐶 is more stable and why? 2
m
m dsl % .co
m .co dkcZfud vfHkfØ;kvksa ds nkSjku nks dkcZu ijek.kqvksa vFkok ,dsedkcZu vkSj ,d
m
s e vU; ijek.kq ds chp lgla;kstd vkca/k VwVdj ,d u;k gvkca la/k curk gSA vkca/kksa
g la a
a dk fonyu leki?kVuh vFkok fo’ke vi?kVuh gks ldrk gSA ftlesa eqDr ewyd]
dkcZ/kuk;u] dkcZ_.kk;u bR;kfn curs gSaA ;g ,d vkca/k esa foLFkkiu ij fuHkZj
djrk gS vkSj izsjf.kd izHkko] bysDVªksesjh izHkko] vuqukn izHkko vkSj vfrla;qXeu
}kjk fu;af=r gksrk gSA
iz”u %
(i)
m
fuEufyf[kr dkcZ_.kk;uksa ds LFkkf;Ro dk lgh Øe nhft, %
.
.co s e m
s em l a
g la ag
a For more Question Papers, Sample Papers, Notes & Syllabus visit Page 13 of 16

𝐶𝐻 , 𝐶𝐻 , 𝐶𝐻 , 𝐶𝐻 𝐶𝑙, 𝐶𝐻𝐶𝑙 , 𝐶𝐶𝑙
(ii) D;k gksrk gS tc 𝐶𝐻 𝐶𝑙 dk leki?kVuh fonyu gksrk gS\
(iii) D;k (𝐶𝐻 ) 𝐶 vkSj (𝐶𝐻 ) 𝐶 dh lajpuk leku gS \ Li’V dhft,A
vFkok
nksuksa Pℎ 𝐶 vFkok (𝐶𝐻 ) 𝐶 esa ls dkSu&lk vf/kd LFkk;h gS\ vkSj
D;ks\a
Section – E
[k.M & ;
(Long Answer Type Questions)
¼nh?kZ mÙkjkRed iz”u½
33. (i) Write de – Broglie equation. 1
ns&czkWXyh lehdj.k fyf[k,A
(ii) The mass of an electron is 9.1 x 10-31kg. If its kinetic energy is 3.0 x 10-25J
Calculate its wavelength. 2
,d bysDVªkWu dk nzO;eku 9.1 x 10-31 fdxzk0 gSA ;fn bldh xfrt ÅtkZ
3.0 x 10-25 twy gS] rks bldk rjax&nS/;Z D;k gksxk \
(iii) State and explain Aufbau Principle. 2
vkWQckÅ fl)kUr crkb, vkSj le>kb,A
(OR)
vFkok
(i) What is the significance of the square of wave function (𝜑 )? 1
rjax Qyu ds oxZ (𝜑 ) dk D;k egRo gS \
(ii) What are the reasons for the failure of the Bohr model of hydrogen atom?
gkbMªkstu ijek.kq ds cksj ekWMy dh foQyrk ds D;k dkj.k gSa \ 2
(iii) What will be the wavelength of light emitted when the electron in H –
atom undergoes transition from an energy level n = 4 to n = 2? 2

For more Question Papers, Sample Papers, Notes & Syllabus visit Page 14 of 16

m
m .co

m .co s em
se g la
tc gkbMªkstu ijek.kq n = 4 ds ÅtkZ Lrjals n = 2 ÅtkZ Lrj esa
bysDVªkWu tkrk gS] rks fdl rjaxnS/;Z dk izdk”k mRlftZr gksxk \
34. (i) Explain why BeH2 molecule has zero dipole moment although the Be –H
bonds are polar. 1
;|fi vkca/k ?kzqoh; gS] rFkkfi v.kq dk f}/kzqo vk?kw.kZ “kwU; gSA Li’V
m
dhft,A
c o m m .co
. e
em stability of following species and indicate their magnetic glas
(ii) By writing molecular orbital electronic configuration, compare the
srelative
la properties: 𝑂 , 𝑂 , 𝑂 (Peroxide) a4
a g
vkf.od d{kd bysDVªkWfud foU;kl fyf[krs gq,] fuEufyf[kr Lih”kht ds
vkisf{kd LFkkf;Ro dh rqyuk dhft, rFkk muds pqacdh; xq.k bafxr
dhft, %
𝑂 ,𝑂 ,𝑂 ¼ijvkWDlkbM½

o m(OR)
vFkok. c
s em
(i) lain case of 𝑃𝐶𝑙 . Why are axial bonds longer as
Describe the hybridisation
g
a bonds?
compared to equatorial 3
𝑃𝐶𝑙 v.kq esa ladj.k dk o.kZu dhft,A buesa v{kh; vkca/k] fo’kqorh;
vkca/kksa dh vis{kk vf/kd yacs D;ksa gksrs gSa \
(ii) Distinguish between Sigma () and Pi () bond. 2

flXek () vkSj ikbZ () vkca/k esa vUrj dhft,A
m
m
35. (i) How will you convert benzene in to: .co
m .co s e m
s e csthu dks fuEufyf[kr esa dSls ifjofrZr djsaxs \
g l a
g la (a) p – nitrochlorobenzene a
a p – ukbVªksDyksjks csathu
(b) m – nitrochlorobenzene 2
m – ukbVªksDyksjks csathu
(ii) Write chemical equations for the preparation of Butane by following
reactions:
m .
.co s e m
s em l a
g la ag
a For more Question Papers, Sample Papers, Notes & Syllabus visit Page 15 of 16

fuEufyf[kr vfHkfØ;kvksa }kjk C;wVsu cukus ds jklk;fud lehdj.k
fyf[k, %
(a) Wurtz reaction
oqVZt vfHkfØ;k
(b) Decarboxylation reaction 2
fodkcksZfDlyhdj.k vfHkfØ;k
(iii) What is Huckel Rule? 1
gdy fu;e D;k gS \
(OR)
vFkok
What is peroxide effect? Explain with the help of suitable example by giving
mechanism. Why peroxide effect is not observed in addition of HCl and HI? 5
ijkWDlkbM izHkko D;k gS \ mi;qDr mnkgj.k dh lgk;rk ls fØ;kfof/k nsdj Li’V
dhft,A ijkWDlkbM izHkko HCl rFkk HI ladyu esa iznf”kZr D;ksa ugha gksrk\

For more Question Papers, Sample Papers, Notes & Syllabus visit Page 16 of 16