ORG./INO. CHEMISTRY
TARGET : JEE (Main) 2017 NO. 39
Course : ABHINAV (EA)
This DPP is to be discussed in the week (21-12-2015 to 28-12-2015) ANSWER KEY DPP No. # 39 1. 8. 15.
(2) (1) (1)
2. 9. 16.
(4) (2) (3)
3. 10. 17.
(2) (4) (3)
4. 11. 18.
(2) (1) (4)
5. 12. 19.
(3) (2) (4)
6. 13. 20.
(2) (3) (3)
22.
(2)
23.
(4)
24.
(3)
25.
(2)
26.
(3)
27.
(1)
7. 14. 21.
(4) (1) (1)
DPP No. # 39 Total Marks : 86
Max. Time : 54 min.
Single choice Objective ('–1' negative marking) Q.1 to Q.22 ChemINFO : 5 Questions ('–1' negative marking) Q.23 to Q.27
1.
(3 marks, 2 min.) (4 marks, 2 min.)
[66, 44] [20, 10]
The following structures represent various silicate anions. Their formulas are respectively
fuEu lajpuk,¡ fofHkUu flfydsV _.kk;uksa dks iznf’'’kZr djrh gSA muds lw=k Øe’'k% fuEu gSa& O O = Oxygen = Silicon
O (1) SiO44– & Si3O88– (1) SiO44– o Si3O88– 2.
O (2*) SiO44– & Si3O108– (2*) SiO44– o Si3O108–
(3) SiO42– & Si3O92– (3) SiO42– o Si3O92–
(4) SiO34– & Si3O108– (4) SiO34– o Si3O108–
Select the correct statements (1) Oxides of boron (B2O3) and silicon (SiO2) are acidic in nature. (2) Oxides of aluminium (Al2O3) and gallium (Ga2O3) are amphoteric in nature. (3) Oxides of germanium (GeO2) and tin (SnO2) are acidic in nature. (4*) both (1) and (2)
lgh dFkuksa dk p;u dhft;sA (1) cksjksu (B2O3) rFkk flfydkWu (SiO2) ds vkWDlkbM vEyh; izd‘fr ds gksrs gSA (2) ,yqehfu;e (Al2O3) rFkk xsfy;e (Ga2O3) ds vkWDlkbM mHk;/kehZ izd‘fr ds gksrs gSA (3) tesZfu;e (GeO2) rFkk fVu (SnO2) ds vkWDlkbM vEyh; izd‘fr ds gksrs gSA (4*) (1) rFkk (2) nksuksa
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Sol.
gy % 3.
Sol. 4.
S1 and S2 are correct statements. S3 : GeO2 is acidic while SnO2 is amphoteric in nature. S1 o S2 lgh dFku gSaA S3 : GeO2 vEyh; gS tcfd SnO2 mHk;/kehZ izd‘fr dk gSA BC3 is more stable than TC3 because : (1) The difference between electronegativity of B and C is larger than that of T and C. (2*) The higher oxidation state of T (+ 3) is less stable than that of B (+ 3). (3) Thallium being larger in size is able to accomodate more C atoms around it. (4) B3+ is more easily formed than T3+. BC3, TC3 dh vis{kk vf/kd LFkk;h gksrk gS] D;kasfd : (1) B rFkk C dh fo|qr_.krk ds e/; vUrj T rFkk C dh vis{kk vf/kd gksrk gSA (2*) T (+ 3) dh mPpre vkWDLkhdj.k voLFkk B (+ 3) dh vis{kk de LFkk;h gksrh gSA (3) FkSfy;e vkdkj esa cM+k gksrk gS] rFkk blds pkjks vksj vf/kd C ijek.kq fLFkr gksrs gSA (4) B3+, T3+ dh vis{kk vf/kd ljyrk ls curk gSA Refer notes (uksV~l ns[ksa) The straight chain polymer is formed by : (1) hydrolysis of (CH3)3 SiCl followed by condensation polymerization. (2*) hydrolysis of (CH3)2 SiCl2 followed by condensation polymerization. (3) hydrolysis of (CH3) SiCl3 followed by condensation polymerization. (4) hydrolysis of (CH3)4 Si followed by condensation polymerization.
lh/kh J‘a[kyh; cgqyd dk fuekZ.k fd;k tk ldrk gS % (1) (CH3)3 SiCl dk ty&vi?kVu rRi’pkr~ la?kuu cgqydhdj.k }kjk (2*) (CH3)2 SiCl2 dk ty&vi?kVu rRi’pkr~ la?kuu cgqydhdj.k }kjk (3) (CH3) SiCl3 dk ty&vi?kVu rRi’pkr~ la?kuu cgqydhdj.k }kjk (4) (CH3)4 Si dk ty&vi?kVu rRi’pkr~ la?kuu cgqydhdj.k }kjk 5.
Sol.
Which gas is formed when CaC2 is allowed to react with dilute HCl ? (1) Ethane (2) Ethene (3*) Ethyne tc CaC2 dks ruq HCl ds lkFk vfHkёr fd;k tkrk gS] rks dkSulh xSl curh (1) ,sFksu (2) ,Fkhu (3*) ,Fkkbu
(4) Methane
gS \
CaC2 + 2HCl CaCl2 + HCCH
(4) esFksu
Ethyne
,Fkkbu 6.
The function of fluorspar in the electrolytic reduction of alumina dissolved in fused cryolite (Na3AlF6) is (1) as a catalyst (2*) to lower the temperature of the melt and to make the fused mixture very conducting (3) to decrease the rate of oxidation of carbon at the anode (4) none of these above laxfyr Øk;ksykbV (Na3AlF6) esa ?kqfyr ,sY;qfeuk ds oS|qr vi?kVuh; viPk;u esa ¶yksjLikj dk dk;Z gksrk gSA (1) mRizsjd ds :i esa gSA (2*) xfyr dk rki de djuk rFkk laxfyr feJ.k dks vfrpkyd cukuk (3) ,uksM+ ij dkcZu dh vkWDlhdj.k dh nj dks ?kVkuk (4) buesa ls dksbZ ugha
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7.
Which of the following is bauxite?
fuEu esa ls dkSulk ckWDlkbV gS\ (1) Al(NO3)3 8.
(2) AlCl3
(3) Al2(SO4)3. xH2O
(4*) Al2O3. xH2O
Which of the following oxidation states are the most characterstics for lead and tin, respectively ?
ySM o fVu ds fy, fuEu esa ls dkSulh vkWDlhdj.k voLFkk Øe’'k% lokZf/kd :i ls vfHkyk{kf.kd gSa \ (1*) + 2 , + 4 9.
(2) + 4 , + 4
(3) + 2 , + 2
(4) + 4 , + 2
Which of the following anions is present in the chain structure of silicates ?
flfydsV dh J`‘a[kyk lajpuk esa fuEu esa ls dkSulk _.kk;u mifLFkr gksrk gS \ (1) (Si2 O52– )n 10.
11.
(2*) (SiO32– )n
Glass reacts with HF to produce Xykl] HF ds lkFk fØ;k dj fuEu mRikn (1) H2SIO3 (2) SiF4
curk gSA
(3) SiO 4– 4
(4) Si2 O76–
(3) Na3AlF6
(4*) H2SiF6
The oxide which is not a reducing agent is :
og vkWDlkbM tks fd vipk;d ugha gS] fuEu gS % Sol.
gy12.
Sol.
(1*) CO2 (2) CO (3) SO2 (4) Both (1) & (3) nksuks (1) CO2 can not act as reducing agent because carbon is in its highest oxidation state, i.e., +4. CO2 vipk;d ds :i esa dk;Z ugha djrk gS D;ksafd dkcZu bldh mPpre vkWDlhdj.k voLFkk +4 esa gSaA Aqueous solution of potash alum is : (1) alkalline (2*) acidic
(3) neutral
(4) soapy
iksVk'’k ,sye~ dk tyh; foy;u gksrk gS % (1) {kkjh; (2*) vEyh;
(3) mnklhu (4) lkcquhd‘r It is acidic because of the hydrolysis of Al2(SO4)3 according to the following reaction. Al2 (SO4)3 + 6H2O 2Al(OH)3 + 3H2SO4.
gy-
fuEufyf[kr vfHkfØ;k ds vuqlkj Al2(SO4)3 ds ty vi?kVu ds dkj.k ;g vEyh; gSA
13.
gy-
From B2H6, all the following can be prepared except : B2H6 ls fuEu esa ls fdl ,d ds vfrfjDr lHkh dks cuk;k tk ldrk gS % (1) H3BO3 (2) [BH2(NH3)2]+ [BH4]– (3*) B2(CH3)6 (4) NaBH4 (3) CH3 group being larger can not form a bridge between two small sized boron atoms. (3) CH3 lewg dk cM+k vkdkj gksus ds dkj.k ;g nks NksVs vkdkj ds cksjkWu ijek.kqvksa ds e/; lsrq ugha
14.
The species that does not contain peroxide ion is :
Sol. z
rFkk (3)
Al2 (SO4)3 + 6H2O 2Al(OH)3 + 3H2SO4.
cuk ldrk gSA
fuEUk esa ls dkSulh Lih'’kht ijkWDlkbM vk;u ;qDr ugh gS% (1*) PbO 2 15.
(3) SrO 2
(4) BaO 2
In the reaction B 2 O 3 C Cl 2 A CO . The A is
vfHkfØ;k 16.
(2) H 2 O 2 B 2 O 3 C Cl 2 A CO . esa A
gS %
BCl 3 (1*) (2) BCl 2 (3) B 2 Cl 2 (4) CCl 2 Which of the following is formed when aluminium oxide and carbon is strongly heated in dry chlorine gas
(1) Aluminium chloride
(2) Hydrate aluminium chloride
(3*)Anhydrous aluminium chloride
(4) None of these
Tkc ,Y;qfefu;e vkWDlkbM rFkk dkcZu dks '‘kq"”d Dyksjhu xSl dh mifLFkfr esa izcy :Ik ls xeZ djrs gS rks fuEu esa ls D;k curk gS \ (1)
,Y;qfefu;e DyksjkbM
(3*) futZy
(2) ty
,Y;qfefu;e DyksjkbM
(4) buesa
;ksftr ,Y;qfefu;e DyksjkbM ls dksbZ ugh
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17.
Aluminium hydroxide is soluble in excess of sodium hydroxide forming the ion
,Y;qfefu;e gkbMªksDlkWbM] lksfM;e gkbMªksDlkWbM ds vkf/kD; esa foys; gksdj vk;u cukrk gS % ? (1) AlO 2 3 18.
(2) AlO 23
(3*) AlO 2
(4) AlO 3
Aluminium chloride exists as dimer, Al 2 Cl6 in solid state as well as in solution of non-polar solvents such as benzene. When dissolved in water, it gives
,Y;qfefu;e DyksjkbM Bksl vOkLFkk ds lkFk&lkFk v/kzqoh; foyk;d tSls csUthu ds foy;u esa f}yd , Al 2 Cl 6 ds :Ik esa jgrk gSA tc bls ty esa ?kksyk tkrk gS rks ;g nsrk gS % (1) 19.
[ Al(OH )6 ]3 3 HCl
(2) [ Al(H 2 O)6 ]3 3 Cl
(4*) Al 2 O3 6 HCl
(3) Al 3 3 Cl
Which of the following does not exist in free form
fuEu es ls dkSulk eqDr voLFkk esa fo|eku ugh gksrk gS \ (1) 20.
BF3
(2) BCl 3
(3) BBr3
(4*) BH 3
(2)Basic
(3*) Amphoteric (4) None of these
Alumina is (1) Acidic
,yqfeuk gS % (1) vEyh; 21.
(2) {kkjh;
(3*) mHk;/kehZ
(4) buesa
ls dksbZ ugh
Which metal is protected by a layer of its own oxide
fuEu es ls dkSulh /kkrq dks Lo;a dh vkWDlkbM ijr }kjk ifjjf{kr fd;k tkrk gS % (1*) Al 22.
(2)
Ag
(3) Au
(4) Fe
Aluminium is more reactive than iron. But aluminium is less easily corroded than iron because (1) Aluminium is a noble metal (2*) Oxygen forms a protective oxide layer (3) Iron undergoes reaction easily with water (4) Iron forms mono and divalent ions
,Y;qfefu;e] vk;ju dh vis{kk vf/kd fØ;k’'khy gksrk gS fdUrq ,Y;qfefu;e] dk la{kkj.k vk;ju dh vis{kk ljyrk ls ugh gksrk gS D;ksfd& (1) ,Y;qfefu;e (2*) vkWDlhtu (3) vk;ju (4)
,d vfØ; /kkrq gS ,d ifjjf{kr vkWDlkbM ijr cukrk gSA
ty ds lkFk ljyrk ls vfHkfØ;k djrk gSA
vk;ju ,dy rFkk f}la;ksth vk;u cukrk gSA
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ChemINFO-1.4
HYDROGEN
Daily Self-Study Dosage for mastering Chemistry
Group 13 & 14 Elements
Properties of Hydrogen (1) It is colourless, odourless and taste less gas. (2) It is only slightly soluble in water. (3) It is lightest of all elements. (4) certain metals like palladium, platinum etc can adsorb large quantities of hydrogen. The adsorbed hydrogen is called occluded hydrogen and is more active than ordinary hydrogen. Combustion : Hydrogen is flammable or combustible gas it burn with blue flame in oxygen atmosphere. 2H2 + O2 2H2O Combination reaction : Due to very high bond dissociation energy (436 KJ mol–1) hydrogen is not a very active. (A) Except Beryllium all alkali and alkaline earth metal directly combine with hydrogen and ionic hydride is formed. 2Li + H2 2LiH 2Na + H2 2NaH
Ca + H2 CaH2 Ba + H2 BaH2
(B) Halogens directly combine with Hydrogen to form covalent compounds. H2 + X2 2HX
X F , Cl , Br , I
The reactivity of Halogen : F2 > Cl2 > Br2 > I2 (C) Synthesis of methyl alcohol : In presence of ZnO and CrO3 catalyst at 200 atmosphere CO and H2 combine to form CH3OH. catalyst CO + 2H2 CH3OH 300 C
(D) Unsaturated fats are changed to saturated fats in presence of nickel . Ni
Unsaturated fat + H2 Saturated Fat catalyst
(Oil)
(vanaspati ghee)
(E) Synthesis of Ammonia (Haber’s Process) : A mixture of N2 and H2 in ratio of 1 : 3 at 200 atm, 500°C in presence of Fe catalyst NH3 is formed. N2 + 3H2
2NH3
H = –22.4 Kcal mol–1
Memorize this theory as soon as you get the DPP. Revise it regularly and master this concept by practice. 23.
24.
25.
The colour of hydrogen is : (1) Yellow (2) Orange
(3) Red
(4*) None
Which of the following is the lightest gas ? (1) Nitrogen (2) Helium
(3*) Hydrogen
(4) Oxygen
Which of the following metal adsorb hydrogen ? (1) Zn (2*) Pd
(3) Al
(4) K
26.
Which of the following react with Hydrogen very fast : (1) Br2 (2) Cl2 (3*) F2
(4) I2
27.
H2 cannot combine directly with which metal : (1*) Be (2) Ca
(4) Na
(3) Ba
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PAGE NO.- 5
ChemINFO-1.4
HYDROGEN
Daily Self-Study Dosage for mastering Chemistry
Group 13 & 14 Elements
gkbMªkstu ds xq.k/keZ
(1) ;g jaxghu] xa/kghu rFkk Loknghu xSl gSA (2) ;g dsoy ty esa de ?kqyu’'khy gksrh gSA (3) ;g lHkh rRoksa ls gYdh gksrh gSA (4) fuf’pr /kkrq,sa tSls isysfM;e] IysfVue bR;kfn gkbMªkstu dks vf/kdre la[;k esa vf/k’'kksf"”kr dj ldrh gSA vf/k'’kksf"”kr gkbMªkstu vo:) gkbMªkstu (occluded hydrogen) dgykrh gS rFkk ;g lkekU; gkbMªkstu dh vis{kk vf/kd fØ;k'’khy gksrh gSaA ngu : gkbMªkstu Toyu’'khy ;k ngu’'khy xSl gS ;g vkWDlhtu;qDr ok;qe.My esa uhyh Tokyk ds lkFk tyrh gSA 2H2 + O2 2H2O la;kstu vfHkfØ;k : cgqr vf/kd cU/k fo;kstu ÅtkZ (436 KJ mol–1) ds dkj.k gkbMªkstu vf/kd lfØ; ugh gksrh gSA (A) csjhfy;e dks NksM+dj lHkh {kkjh; rFkk {kkjh; e‘nk /kkrq,sa gkbMªkstu ds lkFk izR;{k :i ls tqMrh gS rFkk vk;fud gkbMªkbM
cukrh gSA
2Li + H2 2LiH 2Na + H2 2NaH (B)
Ca + H2 CaH2 Ba + H2 BaH2
gsykstu gkbMªkstu ds lkFk izR;{k :i ls tqMdj lgla;kstd ;kSfxd cukrs gSA
H2 + X2 2HX
X F , Cl , Br , I
gsykstu dh fØ;k'’khyrk : F2 > Cl2 > Br2 > I2 (C) esfFky ,Ydksgy CH3OH cukrs gSA
dk la’ys”k.k : ZnO rFkk CrO3 mRizsjd dh mifLFkfr esa 200 ok;qe.Myh; nkc ij CO rFkk H2 tqM+dj
mRizsjd CO + 2H2 CH3OH 300 C
(D)
vlar‘Ir olk fudy dh mifLFkfr esa lar‘Ir olk esa cnyrh gSA Ni vlar‘Ir olk + H2 lar‘Ir olk mRizsjd
(rsy)
(ouLifr
?kh)
veksfu;k dk la’ys”k.k (gscj izØe) : N2 rFkk H2 dk feJ.k 200 atm rFkk 500°C ij Fe mRiszjd dh mifLFkfr esa 1 : 3 ds vuqikr esa fØ;k djds NH3 cukrk gSA (E)
N2 + 3H2 23.
24.
25.
(3) yky
fuEu esa ls dkSu gYdh xSl gS ? (1) ukbVªkstu (2) ghfy;e
(3*) gkbMªkstu
(4*) dksbZ
fuEu es ls dkSulh /kkrq gkbMªkstu dks vf/k’'kksf"”kr djrh gS ? (2*) Pd
(3) Al
gkbMªkstu fuEu es ls fdl ds lkFk lokZf/kd fØ;k’'khy gS& (1) Br2
27.
H = –22.4 Kcal mol–1
gkbMªkstu dk jax gksrk gS& (1) ihyk (2) ukjaxh
(1) Zn 26.
2NH3
(2) Cl2
(3*) F2
fuEu esa ls fdl /kkrq ds lkFk gkbMªkstu izR;{k :i ls ugh tqM+rh gS& (1*) Be
(2) Ca
(3) Ba
ugh (4) vkWDlhtu (4) K
(4) I2
(4) Na
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PAGE NO.- 6
