Bakliwal Tutorials-IIT p block practice

ONLY ONE ANSWER IS CORRECT

Group 13th
1. Which of the following facts regarding boron and silicon is not true :
(A) Boron and silicon are semiconductors.
(B) Boron and silicon form halides which are not hydrolysed.
(C) Boron and silicon react with magnesium to form magnesium boride and magnesium silicide which
are decomposed by acids to give volatile borane and silane, respectively.
(D) Both boron and silicon react with alkali to form borates and silicates containing BO4 and SiO4
tetrahedral units, respectively.
2. B3+ cannot exist in aqueous solution becuase of its :
(A) Strong reducing ability. (B) Strong oxidizing ability.
(C) Small size and large charge. (D) Large size and small charge.
3. The product obtained in the reaction of diborane with excess of ammonia is :
(A) B2H6. NH3 (B) B2H6. 2NH3 (C) (BN)x (D) Borazine
4. In the following reaction :
B (OH)3 + H2O → [B(OH)4]– + H+
(A) B(OH)3 is a Lewis acid (B) B(OH)3 is a Lewis base
(C) B(OH)3 is amphoteric (D) none is correct
5. The decrease stability of higher oxidation state in p–block with increasing atomic number is due to :
(A) Increase in bond energy as going down the group
(B) Energy required to unpair ns2 – electrons is not compensated by the energy released in forming the
two additional bonds
(C) Both are correct
(D) None is correct.
6. Pure boron is best prepared by
(A) Heating B2O3 with H2 (B) Heating B2O3 with Na or K
(C) Heating KBF4 with Na or K (D) Heating BBr3 with H2 in presence of a catalyst
7. Water softener is :
(A) Borax (B) Zeolite
(C) Both (A) and (B) (D) None of these
8. Which of the following statements regarding ortho boric acid (H3BO3) is false ?
(A) It acts as a weak monobasic acid (B) It is soluble in hot water
(C) It has a planar structure (D) It acts as a tribasic acid
9. When orthoboric acid is heated to red heat, the residue is :
(A) Boron (B) Boric oxide (C) Metaboric acid (D) Pyroboric acid
10. BF3 on hydrolysis forms :
(A) H3BO3 (B) HBF4 (C) Both (A) and (B) (D) None of these
11. From B2H6 all the following can be prepared except :
(A) H3BO3 (B) NaBH4 (C) B2(CH3)6 (D) B2O3
12. Boron nitride has the structure of the type :
(A) Both diamond and graphite (B) Graphite
(C) Diamond (D) NaCl
13. On passing CO2 into aqueous solution containing Al3+ :
(A) Al2(CO3)3 is formed (B) Al(OH)3 is precipitated
(C) Al2O3 is formed (D) Collodial Al(OH)3 is formed
14. Alum is found to contain hydrated monovalent cation [M(H2O)6]+ , trivalent cation [M′(H2O)6]3+ and SO42– in
the ratio of :
(A) 1 : 1 : 1 (B) 1 : 2 : 3 (C) 1 : 3 : 2 (D) 1 : 1 : 2
15. When orthoboric acid (H3BO3) is heated the residue left is:
(A) Boron (B) Metaboric acid (C) Boric anhydride (D) Borax

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16. Borax is:
(A) Na2B4O7 (B) Na2B4O7.4H2O (C) Na2B4O7.7H2O (D) Na2B4O7.10H2O
17. Borax on heating with cobalt oxide forms a blue bead of:
(A) Co(BO2)2 (B) CoBO2 (C) Co3(BO3)2 (D) Na3Co(BO3)2
18. The correct order of decreasing hardness of the follwing compound is:
(A) Diamond > Borazone > Carborundum > Corundum
(B) Borazone > Diamond > Carborunndum > Corundum
(C) Corundum > Carborundum > Borazone > Diamond
(D) None
19. Al dissolves in molten NaOH with the formation of:
(A) Sodium aluminate (Na3AlO3) (B) Sodium metaluminate (NaAlO2)
(C) Aluminium hydroxide (D) Alumina
20. Aqueous solution of potash alum is:
(A) Alkaline (B) Acidic (C) Neutral (D) Soapy
21. Alumina is ......... in nature:
(A) Acidic (B) Basic (C) Amphoteric (D) Neutral
22. The protective film of oxide on the surface of Al metal may be strengthened by:
(A) Galvanizing (B) Cathodizing (C) Sheradizing (D) Anodizing
23. The borax bead is chemically:
(A) B2O3 (B) Na2B4O7 (C) Na3BO3 (D) B2O3 + NaBO2
24. When Al is added to potassium hydroxide solution:
(A) No reaction takes place (B) Oxygen is evolved
(C) Water is produced (D) Hydrogen is evolved
25. Which reaction cannot give anhydrous AlCl3:
(A) Heating of AlCl3.6H2O
(B) Passing dry HCl over heated aluminium powder
(C) Passing dry Cl2 over heated aluminium powder
(D) Heating a mixture of alumina and coke in a current of dry Cl2
26. Alum is used by dyer of cloth:
(A) For fire-proofing fabrics (B) As first aid for cuts
(C) For softening hard water (D) As mordant
27. Stable compounds in +1 oxidation state is formed by:
(A) B (B) Al (C) Ga (D) Tl
28. Aluminium vessels should not be washed with materials containing washing soda because:
(A) Washing soda is expensive
(B) Washing soda is easily decomposed
(C) Washing soda reacts with aluminium to form soluble aluminate
(D) Washing soda reacts with aluminium to form insoluble aluminium oxide
29. Aluminium is more reactive than iron. But aluminium is less easily corroded then iron because:
(A) Aluminium is a noble metal (B) Oxygen forms a protective oxide layer
(C) Iron unergoes reaction easily with water (D) Iron forms both mono and divalent ions
30. The dissolution of Al(OH)3 by a solution of NaOH results in the formation of:
(A) [Al(H2O)4(OH)]2+ (B) [Al(H2O)2(OH)4]- (C) [Al(H2O)3(OH)3] (D) [Al(H2O)6(OH)3]
31. Which mixed sulphate is not an alum:
(A) K2SO4.Al2(SO4)3.24H2O (B) K2SO4.Cr2(SO4)3.24H2O
(C) Na2SO4.Fe2(SO4)3.24H2O (D) CuSO4.Al2(SO4)3.24H2O
32. Which of the following is pseudo alum:
(A) (NH4)2SO4.Fe(SO4)3.24H2O (B) K2SO4.Al2(SO4)3.24H2O
(C) MnSO4.Al2(SO4)3.24H2O (D) None
33. Aluminium does not react with:
(A) NaOH (B) HCl (C) N2 (D) HNO3
34. Borax bead test is responded by:
(A) Divalent metals (B) Heavy metals
(C) Light metals (D) Metal which forms coloured metaborates
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35. When a solution of sodium hydroxide is added in excess to the solution of potash alum, we obtain:
(A) A white precipitate (B) Bluish white precipitate
(C) A clear solution (D) A crystalline mass

36. Which of the following is a gas (at 0°C) :

(A) BF3 (B) BCl3 (C) BBr3 (D) BI3
37. Aluminium metal is corroded in coastal places near to the sea, beacause protective oxide film:
(A) Is removed by sea water (B) Reacts with sea water
(C) Is attacked by salt present in sea water (D) Reacts with sand particles

38. B2O3 is:

(A) Ionic (B) Basic (C) Acidic (D) Amphoteric
39. On the addition of mineral acid to an aqueous solution of borax, the compound formed is:
(A) Borodihydride (B) Orthoboric acid (C) Metaboric acid (D) Pyroboric acid

40. Pure H2S gas can be obtained by the action of water on:
(A) CuS (B) FeS (C) Flower of sulphur (D) Al2S3

41. Which cannot be prepared by B2H6:

(A) NaBH4 (B) H3BO3 (C) B2(CH3)6 (D) B2H6 . 2NH3
42. Which does not react with water:
(A) B2S3 (B) B4C (C) Al4C3 (D) Al2S3
43. Diborane reacts with water to form:
(A) HBO2 (B) H3BO3 (C) H3BO3 + H2 (D) H2
44. There are two H-bridge bonds in diborane molecule because there are:
(A) Only 12 electrons (B) 14 electrons
(C) 2 elecrons less required for bonding (D) Two electrons more than required for bonding
45. Borax is prepared by treating colemanite with:
(A) NaNO3 (B) NaCl (C) Na2CO3 (D) NaHCO3
46. An aqueous solution of BCl3 is:
(A) Weak acid (B) Weak base (C) Neutral (D) Strong base
47. Boric acid is polymeric because of:
(A) Its acidic nature (B) Presence of hydrogen bonds
(C) Its monobasic nature (D) Its geometry
48. The bonds present in borazole are:
(A) 12σ, 3π (B) 9σ, 6π (C) 6σ, 6π (D) 9σ, 9π
49. Reactivity of borazole is greater than that of benzene because:
(A) Borazole is non-polar compound (B) Borazole is polar compound
(C) Borazole has electrons in it (D) Of localized electrons in it
50. Aqueous ammonia is used as a precipitating reagent for Al3+ ions as Al(OH)3 rather than aqueous NaOH,
because:
(A) N H+
4 is a weak base (B) NaOH is a very strong base
(C) NaOH forms [Al(OH)4]- ions (D) NaOH forms [Al(OH)2]+ ions
51. BCl3 does not exist as dimer but BH3 exist as dimer (B2H6) because:
(A) Chlorine is more electronegative than hydrogen
(B) There is pπ-pπ back bonding in BCl3 but BH3 does not contain such multiple bonding
(C) Large sized chlorine atoms do not fit in between the small boron atoms whereas small sized
hydrogen atoms get fitted in between boron atoms
(D) None of the above
52. An aqueous solution of borax is
(A) netural (B) amphoteric (C) basic (D) acidic
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53. Boric acid is polymeric due to
(A) its acidic nature (B) the presence of hydrogen bonds
(C) its monobasic nature (D) its geometry
54. Aqueous solution containing 1 mol of borax reacts with 2 mol of acids. This is because of :
(A) formaiton of 2 mol of B(OH)3 only
(B) formation of 2 mol of [B(OH)4]– only
(C) formation of 1 mol each of B(OH)3 and [B(OH)4]–
(D) formation of 2 mol each of [B(OH)4]– and B(OH)3 , of which only [B(OH)4]– reacts with acid
55. Borax is used as a buffer since :
(A) Its aqueous solution contains equal amount of weak acid and its salt
(B) It is easily available
(C) Its aqueous solution contains equal amount of strong acid and its salt
(D) Statement that borax is a buffer, is wrong

Group 14th
56. Me2SiCl2 ⎯⎯ ⎯→ (A) ⎯⎯
H2 O
⎯ ⎯⎯→ (B).
condensati on

The nature of product (B) may be

(A) only linear polymers (B) cyclic products
(C) (A) and (B) both (D) none of these
57. Diamond and graphite are
(A) Isomers (B) Isotopes (C) Allotropes (D) None of the above
58. CO is isostructural with
(A) HgCl2 (B) SnCl2 (C) C2H2 (D) NO2
59. HCl is added to the following oxides. Which will give H2O2?
(A) MnO2 (B) PbO2 (C) BaO2 (D) NO2
60. Which of the following is a good conductor of electricity ?
(A) diamond (B) graphite (C) coal (D) none
61. CO forms a voltile compound with
(A) nickel (B) copper (C) sodium (D) aluminium

62. A colourless gas which burns with blue flame and reduces CuO to Cu is :
(A) N2 (B) CO (C) CO2 (D) NO2
63. H2SO4 is not used for the preparation of CO2 from marble chips because :
(A) it does not react (B) huge amount of heat is evolved
(C) the reaction is vigorous
(D) calcium sulphate is sparingly soluble and get deposited on marble chips and stops the reaction
64. Producer gas is the mixture of :
(A) CO and N2 (B) CO and H2 (C) N2 and NH3 (D) CO, H2 and N2
65. If CO2 is passed in excess into lime water, the milkiness first formed disappears due to
(A) reversal of the original reaction
(B) formation of volatile calcium derivative
(C) formation of water soluble calcium bicarbonate
(D) the solution getting heated by exothermic reaction
66. When steam is passed through red hot coke :
(A) CO2 and H2 are obtained (B) CO and N2 are formed
(C) CO and H2 are obtained (D) petrol gas is obtained
67. Glass is soluble in
(A) HF (B) H2SO4 (C) HClO4 (D) aqua-regia
68. Coal gas is a mixture of
(A) CO and H2
(B) H2, saturated and unsaturated hydrocarbons, CO, CO2, N2 and O2
(C) Saturated and unsaturated hydrocabons
(D) CO, CO2 and CH4

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69. Which of the following is not hydrolysed ?
(A) CCl4 (B) SiCl4 (C) SnCl4 (D) PbCl4
70. Red lead is
(A) PbO (B) PbO2 (C) Pb3O4 (D) Pb2O3
71. Which one of the oxides is netural ?
(A) CO (B) SnO2 (C) ZnO (D) SiO2
72. The formula of white lead is
(A) Pb(OH)2. PbCO3 (B) 2PbCO3.Pb(OH)2
(C) Pb(OH)2. Pb(CH3COO)2 (D) PbCO3 . PbO
73. The butter of tin is represented by
(A) SnCl2 . 5H2O (B) SnCl2 (C) SnCl4 (D) SnCl4 . 5H2O
74. The hydroxide of which metal ion is soluble in excess of sodium hydroxide solution
(A) Fe3+ (B) Cr3+ (C) Sn3+ (D) Cu2+
75. Which compound is called sugar of lead ?
(A) PbCl2 (B) Pb(NO3)2 (C) PbSO4 (D) Pb(CH3COO)2
76. The number and type of bonds between two carbon atoms in CaC2 are
(A) one sigma and one pi bond (B) one sigma and two pi bonds
(C) one sigma and one and a half pi bond (D) one sigma bond

77. Tin reacts with conc. HNO3 and gives

(A) stannic nitrate (B) stannous nitrate (C) metastannic acid (D) none of sigma bond

78. CCl4 is inert towards hydrolysis but SiCl4 is readily hydrolysed because
(A) carbon cannot expand its octet but silicon can expand its octet
(B) ionisation potential of carbon is higher than silicon
(C) carbon forms double and triple bonds
(D) electronegativity of carbon is higher than that of silicon
79. Carborundum is the commercial name of
(A) Al2O3 (B) SiC (C) CaCN2 (D) CaC2
80. Lead dissolves most readily in
(A) acetic acid (B) sulphuic acid (C) nitric acid (D) hydrochloric acid
81. Softening of lead’ means
(A) conversion of lead to PbO (B) conversion of lead to Pb3O4
(C) removal of impurities (metallic) from lead
(D) washing lead with HNO3 followed by a dil. alkali solution.
82. Which of the following is obtained on heating potassium ferrocyanide with H2SO4?
(A) CO2 (B) CO (C) C2H2 (D) (CN)2
83. Inert form of carbon is
(A) Diamond (B) Graphite (C) Coal (D) Charcoal
84. The carbide which gives propyne on hydrolysis is :
(A) Al4C3 (B) CaC2 (C) Fe3C (D) Mg2C3
85. Which of the following reactions is not correct ?
(A) CF4 + 2F– → [CF6]2– (B) SiF4 + 2F– → [SiF6]2–
(C) GeCl4 + 2Cl– → [GeCl6]2– (D) SnCl4 + 2Cl– → [SnCl6]2–
86. The ions present in Al4C3, CaC2 and Mg2C3 are respectively-
(A) C4–, C22–, C34– (B) C22–, C4–, C34– (C) C34–, C32–, C4– (D) C34–, C4–, C22–
87. Allylides are ionic carbides. They contains
(A) C4– ions (B) C2 2– (C) C33– ions (D) C34– ions
88. The structural unit pesent in pyro sillicates is
(A) Si3O96– (B) SiO44– (C) Si2O76– (D) (Si2O52–)n

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89. Fire extinguishers contain a bottle of H2SO4 and :
(A) CaCO3 (B) MgCO3 (C) NaHCO3 (D) any carbonate
90. Which substance is used as lubricant?
(A) SnCl2 (B) SiO2 (C) graphite (D) quartz
91. CO is absorbed by
(A) CHCl3 (B) pyrogallol
(C) CCl4 (D) ammonical solution of copper (I) chloride
92. Thermodynamically the most stable form of carbon is
(A) diamond (B) graphite (C) fullerenes (D) coal
93. Elements of group 14
(A) exhibit oxidation state of +4 only (B) exhibit oxidation state of +2 and +4
(C) form M–2 and M4+ ions (D) form M2+ and M4+ ions
94. Hot concentrated HNO3 converts graphite into :
(A) Graphite oxide (B) Benzene hexacarboxylic acid
(C) Both (A) and (B) (D) None of the above
95. Silicon reacts with hot solution of NaOH forming :
(A) Si(OH)4 (B) Si(OH)2 (C) SiO2 (D) Na4SiO4
96. When a mixture of carbon monoxide and chlorine is exposed to sunlight the product formed is :
(A) Thionyl chloride (B) Phosgene
(C) Phosphine (D) Carbon tetrachloride
97. CO2 in water behaves as :
(A) Weak dibasic acid H2CO3 (B) Weak monobasic acid HO – CO2H
(C) Weak diacid base CO(OH)2 (D) Weak monoacid base HO – CO2H
98. Methanides are :
(A) Mg2C3 , Be2C, Al4C3 and CaC2 (B) Mg2C3 , Be2C and Al4C3
(C) Be2C, Al4C3 and CaC2 (D) Be2C and Al4C3
99. Select incorrect statemen (s) :
(A) Interstitial carbides are formed by metalloids like Si and B
(B) Covalent carbides are formed by metalloids
(C) CO and CN– both are fatal due to complex formation with Fe(III) present in blood
(D) SiC is called carborundum
100. The oxide which is not a reducing agent is
(A) CO2 (B) NO2 (C) SO2 (D) CIO2
Group 15th
101. In group 15, the melting points of the elements
(A) increase regularly on moving down the group.
(B) decrease regularly on moving down the group.
(C) first decrease upto As and then increase to Bi
(D) first increase form N to As and then decrease to Bi.

102. N2 molecule is very stable because

(A) nitrogen is unreactive at ordinary temperatures
(B) the two nitrogen atoms are linked together through a double bond
(C) the two nitrogen atoms are linked together through a single bond
(D) the bond dissociation energy of N ≡ N bond is very high

103. The H–M--H bond angle in the hydrides of group 15 elements follows the order
(A) NH3 > PH3 > AsH3 > SbH3 (B) NH3 < PH3 < AsH3 < SbH3
(C) NH3 < PH3 = AsH3 = SbH3 (D) PH3 > NH3 > AsH3 > SbH3

104. The thermal stability of the hydrides of group 15 follows the order
(A) NH3 < PH3 < AsH3 < SbH3 < BiH3 (B) NH3 > PH3 > AsH3 > SbH3 > BiH3
(C) PH3 > NH3 > AsH3 > SbH3 < BiH3 (D) AsH3 < PH3 > SbH3 > BiH3 > NH3
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105. The hydrides of group 15 elements act as
(A) Lewis acids (B) Lewis bases (C) both (D) none
106. The basic strength of the hydrides of goup 15 elements
(A) decreases on moving down the group (B) increases on moving down the group
(C) first decreases upto AsH3 and then increases (D) first increases upto AsH3 and then decreases

107. When NH3 is oxidised with excess NaOCl, the compound formed is
(A) NCl3 (B) NH2OH (C) N3H (D) NO2
108. A gas is obtained on heating ammonium nitrate. The gas
(A) causes laughter (B) brings tears to the eyes
(C) is acidic in nature (D) basic in nature

109. The gas obtained on heating lead nitrate to 400ºC is

(A) N2O (B) NO (C) NO2 (D) N2O5
110. Which of the following oxides is amphoteric in nature ?
(A) N2O3 (B) P4O6 (C) Sb4O6 (D) Bi2O3
111. Which of the following acids is monobasic?
(A) H3PO2 (B) H3PO4 (C) H4P2O7 (D) H4P2O6 .
112. Which of the following is (are) paramagnetic in nature?
(A) NO (B) NO2 (C) N2O4 (D) A and B both

113. Which of the following compounds does give N2 on heating?

(A) NH4NO2 (B) NH4NO3 (C) NaN3 (D) Both (A) and (C)
114. A mixture of alumina and coke is heated in a current of nitrogen to about 1800ºC and the product obtained is
treated with water. A gas is evolved. The gas is
(A) N2 (B) N2O (C) NH3 (D) NO
115. When ammonia is oxidsed by oxygen in the presence of platinum at 800ºC, the gas obtained is
(A) N2O (B) NO (C) NO2 (D) N2O5

116. NO2 can be prepared by heating

(A) NH4NO3 (B) NaNO3 (C) Pb(NO3)2 (D) KNO3
117. Which of the following acids can form two types of salts?
(A) Hyponitrous acid (B) Nitrous acid (C) Nitric acid (D) Pernitric acid
118. Nitric acid usually turns yellow on standing. This is due to
(A) absorption of yellow wavelength (B) slow decomposition of HNO3 into NO2
(C) its oxidation by atmospheric air (D) absorption of moisture by it
119. Nitric acid oxidises P into
(A) PH3 (B) P2O5 (C) HPO3 (D) H3PO4

120. Which of the following metals does not dissolve in conc. HNO3?
(A) Pb (B) Cu (C) Au (D) Hg

121. The geometry of the phosphorus molecule (P4) is

(A) linear (B) angular (C) squar planar (D) tetrahedral
122. Which of the following is least reactive ?
(A) White phosphorus (B) Yellow phosphorus
(C) Red phosphorus (D) Black phosphorus

123. When P4O10 is dissolved in water, the acid formed finally is

(A) H3PO2 (B) H3PO4 (C) H3PO3 (D) H4P2O7

124. Phosphoric acid on heating above 300ºC gives

(A) hypophosphorus acid (B) orthophosphoric acid
(C) metaphosphoric acid (D) phosphorous acid

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125. Metaphosphoric acid exists in polymeric form and may have
(A) a linear structure (B) a cyclic structure
(C) both linear as well as cyclic structures (D) None
126. In the ostwald’s process, nitric acid is prepared by the catalytic oxidation of
(A) N2 (B) NH3 (C) N2O5 (D) NO2
127. Red phosphorus can be prepared from white phosphorus by
(A) adding red colour to white phosphorus
(B) heating white phosphorus to red heat
(C) heating white phosphorus with few crystals of iodine
(D) dissolving white phosphorus in NaOH
128. .... is obtained when ammonium dichromate is heated
(A) nitrogen (B) oxygen (C) ammonia (D) none
129. Superphosphate of lime is
(A) Ca3(PO4)2.CaSO4 (B) Ca(H2PO4)2
(C) Ca(H2PO4)2.CaSO4 (D) Ca(H2PO4)2.H2O.2CaSO4.2H2O
130. A hydride of nitrogen which is acidic in nature :
(A) N3H (B) N2H4 (C) NH3 (D) N4H4
131. Nitrolim is obtained by passing nitrogen over :
(A) heated mixture of Al2O3 and carbon (B) carborundum
(C) calcium carbide (D) heated aluminium
132. White phosphorus may be removed from red phosphorus by
(A) sublimation (B) distillation
(C) dissolving in CS2 (D) heating with an alkali solution
133. Which of the following will combine with Fe(II) ion to form a brown complex compound?
(A) N2O (B) NO (C) N2O3 (D) NO2
134. Which of the following dibasic acids shows geometrical isomerism ?
(A) Hyponitrous acid H2N2O2 (B) Maleic acid C4H4O4
(C) Both (a) and (b) (D) None of the above
135. 1 mol each of H3PO2, H3PO3 and H3PO4 will neutralise x mole of NaOH, y mol of Ca(OH)2 and z mol of
Al(OH)3 (assuming all as strong electrolytes) respectively. x,y,z are in the ratio of :
(A) 3 : 1 . 5 : 1 (B) 1 : 2 : 3 (C) 3 : 2 : 1 (D) 1 : 1 : 1
136. Glacial phosphoric acid is :
(A) HPO3 (B) H3PO3 (C) H3PO4 (D) H4P2O7
137. Holme's signals can be given by using
(A) CaC2 + CaCN2 (B) CaC2 + Ca3P2 (C) CaC2 + CaCO3 (D) Ca3P2 + CaCN2
138. Which is a set of acid salts and can react with base ?
(A) NaH2PO2, Na2HPO3, NaH2PO4 (B) Na2HPO3, NaH2PO3, Na2HPO4
(C) NaH2PO4, NaH2PO3, Na2HPO4 (D) All of these
139. NH3 can't be obtained by
(A) heating of NH4NO3 or NH4NO2 (B) heating of NH4Cl or (NH4)2 CO3
(C) heating of NH4NO3 with NaOH (D) reaction of AIN or Mg3N2 or CaCN2 with H2O
140. Red and white phosphorus will differ but not in :
(A) smell (B) solubility in CHCl3
(C) exhibiting phosphoresence (D) reaction with conc. HNO3
141. Choose correct statement
(A) Superphosphate is [3Ca(H2PO4)2 + 7CaSO4] (B) Triple superphosphate is [10Ca(H2PO4)2]
(C) Both (a) and (b) are correct (D) None is correct
142. N2O (laughing gas) finds use in the following except :
(A) as a propellant for whipped ice-cream (B) as an anaesthetic
(C) for the preparation of N3H (D) as fuel for rockets

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143. Select incorrect statement about N2O4 :
(A) It self ionises as NO+, NO3–
(B) N2O4 is paramagnetic
(C) Substance containing NO+ is said to be acid and that containing NO3– is said to be base
(D) NO2 dimerises to N2O4 with disappearance in paramagnetism
144. Compound used in safety matches is
(A) P4S3 (B) P4 (C) P2O5 (D) PCl3
145. The wrong statement about N2O is
(A) It is nitrous oxide (B) It is least reactive oxide of nitrogen
(C) It is not a linear molecule (D) It is known as laughing gas
146. The mixture of concentrated HCl and HNO3 made in 3 : 1 ratio contains :
(A) CIO2 (B) NOCl (C) NCI3 (D) N2O4
147. The true statement for the acids of phosphorus. H3PO2 H3PO3 and H3PO4 is.
(A) H3PO3 on heating does not disproportionate
(B) All of them are reducing in nature
(C) All of them are tribasic acids
(D) The geometry of phosphorus is tetrahedral in all the three
148. Nitrogen is obtained by the thermal decomposition of :
(A) NH4Cl (B) NH4NO3 (C) AgNO3 (D) None of these
149. The substance used as a fast drying agent in the laboratory is :
(A) Na3 PO4 (B) P2O5 (C) charcoal (D) anhydrous calcium chloride

150. 4HNO3 + P4O10 ⎯⎯→ 4HPO3 + X

in the above reaction the product X is :
(A) NO2 (B) N2O3 (C) N2O4 (D) N2O5
151. Cold solution of barium nitrite on mixing with sulphuric acid produces :
(A) BaSO4 + HNO2 (B) BaSO4 + HNO3 (C) BaSO4 + NO2 (D) BaSO4 + N2 + O2
152. Following are neutral oxides except :
(A) NO (B) N2O (C) CO (D) NO2
153. Pure N2 is prepared in the laboratory by heating a mixture of :
(A) NH4Cl and NaOH (B) NH4OH and NaCl (C) NH4Cl and NaNO2 (D) NH4Cl and NaNO3
154. Substances burn more readily in N2O than in air because N2O :
(A) is reactive at high temperature
(B) dissociates to give O2 that supports combustion
(C) the activation energy is increased on increasing temperature
(D) acts as a catalyst
155. NH4Cl (s) is heated in test tube. Vapours are brought in contact with red litmus paper, which changes to blue
and then to red. It is because of :
(A) formation of NH4OH and HCl (B) formation of NH3 and HCl
(C) greater diffusion of NH3 than HCl (D) greater diffusion of HCl than NH3
156. A gaseous substance dissolve in water giving a pale blue solution which decolourises KMnO4 and oxidised
KI to I2 .
(A) N2O5 (B) NH3 (C) N2O3 (D) HNO3
157. In the preparation of red phosphorus from white phosphorus :
(A) MnO2 is used as a catalyst (B) the white phosphorus is treated in an electric furnace
(C) a little iodine is used as catayst in absence of air (D) the gas P4 is released
158. Compound A undergoes hydrolysis to produce a colourless gas with rotten fish smell. The gas gives a vortex
ring. The gas is :
(A) PH3 (B) P2O3 (C) P2O5 (D) P2S5

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159. A substance which gives a yellow precipitate when boiled with an excess of nitric acid and ammonium
molydate, and yellow precipitate with AgNO3 is :
(A) orthophosphate (B) pyrophosphate (C) metaphosphate (D) hypophosphate
160. Calgon (sodium methphosphate) finds application as :
(A) artificial jewel (B) paint (C) a resin (D) washing powder
161. Phosphorus trichloride, PCl3 undergoes, hydrolysis at room temperature to produce an oxoacid. It has the
formula :
(A) HPO3 (B) H3PO3 (C) H3PO4 (D) H3PO2
162. The high reactivity and low volatility of white phosphorous is due to :
(A) tetrahedrally arranged P4 units (B) bond angle of 600 increases steric (strain) factor
(C) weak van der Waals forces of attraction (D) both (B) and (C)

16th Group
163. The oxide which on strong heating gives oxygen is :
(A) AgNO3 (B) BaO2 (C) Both (A) and (B) (D) Na2 O
164. In the reaction
O3 + Ι2 + H2O ⎯⎯→ (X) + O2
The compound (X) is
(A) HΙO3 (B) HΙ (C) HΙO4 (D) Ι2O5
165. When H2S is passed through acidified K2Cr2O7 solution, the solution turns,
(A) Yellow (B) Blue (C) Green (D) White
166. Which one of the following gives mixture of SO2 and SO3 on heating ?
(A) ZnSO4 (B) CuSO4 (C) Fe2 (SO4)3 (D) FeSO4
167. Which of the following statement is false.
(A) An acidified solution of titanium salt gives yellow or orange colour with H2O2.
(B) An acidified solution of K2Cr2O7 gives a bright blue coloured compound with H2O2 which is soluble in
ether.
(C) Reaction of HCHO with H2O2 in presence of pyrogallol in alkaline solution liberates hydrogen gas
(D) Anhydrous H2O2 is more stable and is kept in glass bottles.
168. The aqueous solution of hydrogen peroxide
(A) converts blue litmus pink (B) converts blue litumus white
(C) converts red litumus blue (D) None of these
169. Which is true about ozone ?
(A) It turns filter paper soaked in alcoholic benzidine to brown colour.
(B) It is used for detecting the position of double bond in unsaturated organic compound.
(C) It forms a solid Ι4O9 with dry iodine (Ι2)
(D) All of these
170. The following catalyst is used in the manufacturing of sulphuric acid by lead chamber process.
(A) NO (B) NO2 (C) Pt (D) V2O5
171. The gas respectively absorbed by alkaline pyrogallol and oil of cinnamon is
(A) O2, O3 (B) SO2, O3 (C) O3, CH4 (D) N2O, O3
172. Concentrated H2SO4 displaces hydrogen chloride from chlorides because :
(A) it is stronger than hydrochloric acid. (B) HCl is a gas while H2SO4 is a liquid.
(C) Sulphates are more soluble than chlorides (D) Sulphates are less soluble than chlorides
173. H2SO4 has very corrosive action on skin because :
(A) It reacts with proteins
(B) it acts as an oxidising agent
(C) It acts as a dehydrating agent
(D) It acts as a dehydrating agent and absorption of water is highly exothermic.
174. When H2S is passed through nitric acid and KMnO4 solution, the product formed is
(A) H2SO4 (B) colloidal sulphur (C) SO2 (D) plastic sulphur

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175. Which of the following hydrides of the oxygen family shows the lowets boiling point?
(A) H2O (B) H2S (C) H2Se (D) H2Te

176. Alkaline KΙ is oxidised by ozone to

(A) potassium iodate (B) potassium periodate (C) both (A) and (B) (D) None of these

177. Which of the following reactions depict the oxidising behaviour of H2SO4 ?
(A) 2PCl5 + H2SO4 ⎯⎯→ 2POCl3 + 2HCl + SO2 Cl2
(B) 2NaOH + H2SO4 ⎯⎯→ Na2SO4 + 2H2O
(C) NaCl + H2SO4 ⎯⎯→ NaHSO4 + HCl
(D) 2HΙ + H2SO4 ⎯⎯→ Ι2 + SO2 + 2H2O

178. Sulphur on oxidation with hot sulphuric acid gives :

(A) SO3 (B) SO2 (C) H2SO3 (D) H2S2O3
179. Which of the following statement is true for sulphur dioxide?
(A) it reacts with dry chlorine in absence of moisture to form sulphuryl chloride.
(B) it in acidic medium reduce halogens to corresponding halides.
(C) burning magnesium and potassium continue to burn in its atmosphere.
(D) All above are correct.
180. In the reaction
Δ
H2SO4 + P2O5 ⎯⎯→ (X) + SO3
the product (X) is :
(A) PH3 (B) H3PO4 (C) HPO3 (D) N4 P2 O7
181. The reaction between ferric salt and aqueous sodium thiosulphate produces pink colour which soon diminishes.
The pink colour is due to the formation of
(A) [Fe(S2O3)3]4– (B) [Fe(S2O3)2]– (C)
Δ Fe2 (S4O6)3 (D) None of these
⎯⎯→
182. Bleaching action of SO2 is due to
(A) its reducing nature (B) its oxidising nature
(C) its acidic nature (D) its both oxidising as well as reducing nature

183. KClO3 + H2SO4 KHSO4 + HClO4 + (X) + H2O

In above unbalanced chemical equation, the product (X) may be
(A) O2 (B) Cl2 (C) ClO2 (D) HCl
184. Which of the following statement is false ?
(A) Superoxides give hydrogen peroxide and oxygen with water
(B) CrO3 is an acidic oxide.
(C) PbO is an amphoteric oxide.
(D) Sub oxides contain more oxygen than expected from the normal valency of the element.
185. H2S is far more volatile than water because
(A) Sulphur atom is more electronegative than oxygen atom.
(B) Oxygen atom is more electronegative than sulphur atom.
(C) H2O has bond angle of nearly 105°.
(D) Hydrogen atom is loosely bonded with sulphur.
186. Which of the following has peroxy linkage ?
(A) H2S2O3 (B) H2SO5 (C) H2S2O7 (D) H2S4O6
187. The term 'thio' is used in the names of all of the following compounds except :
(A) Na2S2O3 (B) Na2S2O6 (C) NaSCN (D) Na2SO3
188. Which of the following product is formed by the reaction of sulphurdioxide with chlorine in presence of
sunlight ?
(A) SO2Cl (B) SO2Cl2 (C) SOCl2 (D) SO3Cl

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189. Consider the following compounds :
(i) Sulphur dioxide (ii) Hydrogen peroxide (iii) Ozone
Among these compounds, those which can act as bleaching agents would include :
(A) 1 and 3 (B) 2 and 3 (C) 1 and 2 (D) 1, 2 and 3
190. A considerable part of the harmful UV rays of the sun does not reach the surface of the earth. This is because
high above the earth's atmosphere , there is a layer of :
(A) O3 (B) CO2 (C) SO2 (D) NO
191. Which is true statement ?
(A) Sulphur trioxide exist as cyclic trimer in solid state, S3O9
(B) Selenium trioxide solid is a cyclic tetramer, Se4 O12
(C) TeO3 is a solid with a network structure in which TeO6 octahedra share all vertices.
(D) All are correct
192. Ozone layer is being depleted. This is due to :
(A) NO emission from supersonic jets (B) chloroflurocarbon used as aerosols
(C) both (A) and (B) (D) none of the above
193. Estimation of ozone can be made quantitatively by :
(A) decomposition into O2 and absorption of O2 into pyrogallol
(B) volumetric method using KI and titration of the liberated iodine using hypo solution
(C) oxidative ozonolysis method
(D) all methods given above
194. The process of obtaining sulphur by the borehole method is called :
(A) the Frasch process (B) the Lablanc process
(C) the Calcaroni process (D) the Mannheium process
195. SO2 behaves as a reducing agent when :
(A) passed over hot CuO (B) mixed with moist H2S
(C) passed through acidified KMnO4 solution (D) passed through FeSO4 solution
196. When an article is bleached by SO2 it loses its colour. The colour can be restored by :
(A) exposure to air (B) heating
(C) dilution (D) none of these
197. Out of H2S2O3 , H2S4O6 , H2SO5 and H2S2O8 peroxy acids are :
(A) H2S2O3 , H2S4O6 (B) H2S4O6 , H2SO5
(C) H2SO5 , H2S2O8 (D) H2S2O3 and H2S2O8
198. Which of the following can convert acidified Cr2O72– to green ?
(A) SO2 / H2SO3 / H2SO4 (B) SO3 / H2SO3 / H2S
(C) SO32– / H2S / Fe2+ (D) S2O32– / SO3 / Fe3+
199. Bleaching of a fabric cloth is done using A and excess of chlorine is removed using B. A and B are :
(A) CaOCl2 , Na2SO3 (B) Na2S2O3 , CaOCl2
(C) CaCl2 , Na2S2O3 (D) CaOCl2 , Na2S2O3
200. Aqueous hypo solution on reaction with aqueous AgNO3 gives :
(A) yellow precipitate changing to black (B) white precipitate changing to black
(C) orange precipitate to blue (D) no precipitate
201. SO2 can reduce :
(A) HClO3 to HCl (B) Cr2O72– / H+ to Cr3+ (C) MnO4– / H+ to Mn2+ (D) all of these

Group 17th
202. The most powerful oxidising agent is :
(A) fluorine (B) chlorine (C) bromine (D) iodine
203. Which one of the hydracid does not form any precipitate with AgNO3 ?
(A) HF (B) HCl (C) HBr (D) HI
204. The strongest reducing agent is :
(A) F– (B) Cl– (C) Br– (D) Ι–
205. Which one of the following has hydrogen bonding ?
(A) HI (B) HBr (C) HF (D) HCl

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206. Chlorine gas is dried over :
(A) CaO (B) NaOH (C) H2SO4 (D) HBr
207. On heating a mixture of NaCl, K2Cr2O7 and conc. H2SO4 .......... is obtained :
(A) chromic chloride (B) chromyl chloride (C) chlorine (D) none of the above
208. Elements of which one of the following groups will form anions most readily ?
(A) oxygen group (B) nitrogen group (C) halogens (D) alkali metals
209. Which statement is correct about halogen ?
(A) They are all diatomic and form univalent ions
(B) They are all capable of exhibiting several oxidation states
(C) They are all diatomic and form diatomic ions
(D) They are all reducing agents
210. Iodine vapours are violet in colour because :
(A) the molecules of iodine in vapour phase absorb green and yellow radiations
(B) the molecules of iodine absorb red and violet radiations and then emit them
(C) it is a solid
(D) it is easily volatile

211. The halogens are :

(A) transition elements (B) inner-transition elements
(C) noble elements (D) representative elements
212. Iodine is liberated from KI solution when treated with :
(A) ZnSO4 (B) CuSO4 (C) NiSO4 (D) FeSO4
213. Which of the following arrangements for the three halogesn CI, Br, I when placed in order of their increasing
electron affinity is correct ?
(A) Cl, Br, Ι (B) Ι, Br, Cl (C) Br, Cl, Ι (D) Ι, Cl, Br
214. Oxidising action increases in the following order :
(A) Cl < Br < Ι < F (B) Cl < Ι < Br < F (C) Ι < F < Cl < Br (D) Ι < Br < Cl < F
215. Which of the following is not oxidised by MnO2 ?
(A) F– (B) Cl– (C) Br– (D) I–
216. HBr and HI can reduce H2SO4, HCl can reduce KMnO4 and HF can reduce :
(A) K2Cr2O7 (B) KMnO4 (C) H2SO4 (D) none
217. Which of the following pairs is not correctly matched ?
(A) A halogen which is liquid at room temperature – Bromine
(B) The most electronegative element–Fluorine
(C) The most reactive halogen – Fluorine
(D) The strongest oxidising agent – Iodine
218. Fluorine reacts with water to give :
(A) hydrogen fluoride and oxygen (B) hydrogen fluoride and ozone
(C) hydrogen fluoride and oxygen fluoride (D) hydrogen fluoride, oxygen and ozone

219. When iodine is dissolved in CCl4, the colour that results is :

(A) brown (B) bluish green (C) violet (D) colourless
220. Hydrogen bonding does not play role in the boiling point of :
(A) NH3 (B) H2O (C) HI (D) HF
221. Hydrogen fluoride is a liquid unlike other hydrogen halides, because :
(A) H–F bond is strong (B) F atom is small in size
(C) Hydrogen bonding is present (D) HF is a weak acid
222. Which one of the halogen acids is a liquid under ordinary conditions ?
(A) HF (B) HCl (C) HBr (D) HI
223. Bleaching powder is obtained by the interaction of chlorine and :
(A) dilute solution of Ca(OH)2 (B) concentrated solution of Ca(OH)2
(C) dry calcium oxide (D) dry slaked lime

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224. Which amongst the following reactions cannot be used for the respective preparation ?
(A) 2KBr + H2SO4 (conc.) ⎯⎯→ K2SO4 + 2HBr (B) NaCl + H2SO4 (conc.) ⎯⎯→ NaHSO4 + HCl
(C) NaHSO4 + NaCl ⎯⎯→ Na2SO4 + HCl (D) CaF2 + H2SO4 ⎯⎯→ CaSO4 + 2HF
225. Which of the following possess the highest bond energy ?
(A) F2 (B) Cl2 (C) Br2 (D) I2
226. Astatine is the element below iodine in the group VIIA of the periodic table. Which of the following statements
is not true for astatine ?
(A) It is less electronegative than iodine
(B) It will exhibit only–1 oxidation state
(C) Intermolecular forces between the astatine molecules will be larger than between iodine molecules
(D) It is composed of diatomic moleucles
227. When thiosulphate ion is oxidised by iodine, the new product formed is :
(A) SO32– (B) SO42– (C) S4O62– (D) S2O62–
228. Which of the following is the strongest acid ?
(A) HBr (B) HF (C) H2S (D) PH3
229. Which of the following statements is correct ?
(A) all halogens form oxyacids (B) only chlorine and bromine form oxyacids
(C) all halogens except fluorine form oxyacids (D) only iodine forms oxyacid

230. On heating KClO3 we get :

(A) KClO2 + O2 (B) KCl + O2 (C) KCl + O3 (D) KCl + O2 + O3
231. The reaction
3CIO– (aq.) ⎯⎯→ CIO3– (aq.) + 2Cl– (aq.)
is an example of :
(A) oxidation reaction (B) reduction reaction (C) disproportionation (D) decomposition reaction
232. Which of the following has highest bond strength :
(A) HI (B) HCl (C) HF (D) HBr

233. Which of the following will displace the halogen from the solution of the halide ?
(A) Br2 added to NaI (B) Br2 added to NaCl
(C) Cl2 added to KCl (D) Cl2 added to NaF
234. The high oxidising power of fluorine is due to :
(A) high electron affinity
(B) high heat of dissociation and low heat of hydration
(C) low heat of dissociation and high heat of hydration
(D) high heat of dissociation and high heat of hydration
235. In the preparation of HBr or HI , NaX (X = Br, I) is treated with H3PO4 and not by concentrated H2SO4 since,
(A) H2SO4 makes the reaction reversible
(B) H2SO4 oxidises HX to X2 (Br2 , I2)
(C) Na2SO4 is water soluble and Na3PO4 is water insoluble
(D) Na3PO4 is water insoluble and Na2SO4 is water soluble
236. Bleaching powder is disinfectant for purification of water when water – born germs are killed. But disinfectant
activity is destroyed. It is due to its disproportionation into :
(A) CaCl2 and Cl2 (B) Ca–Cl2 and Ca(ClO3)2
(C) CaO and Cl2 (D) CaO, Cl2 and CaCl2
237. CaOCl2 + H2O + CO2 → CaCO3 + CaCl2– + HO–Cl+
This reaction is simply :
(A) oxidation (B) reduction (C) redox (D) hydrolysis in presence of CO2
238. Select correct statement :
(A) Cl2O and ClO2 are used as bleaching agents and as germicides
(B) I2O5 is used in the quantitative estimation of CO
(C) bond angle XOX varies in the order
FOF < ClOCl < BrOBr
(D) all are correct
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239. ClO2s is the anhydride of :
(A) HOCl (B) HClO2 (C) HClO3 (D) HClO2 and HClO3
240. ClO3 is the mixed anhydride of :
(A) HClO2 and HClO3 (B) HClO3 and HClO4 (C) HClO2 and HClO4 (D) HClO2 and HClO3
.
Group 18th
241. Of the following species, one which is non-existent :
(A) XeF6 (B) XeF5 (C) XeF4 (D) XeF2
242. The coloured discharge tube for advertisement mainly contains :
(A) xenon (B) helium (C) neon (D) argon
243. Maximum number of compounds are known in the case of :
(A) neon (B) xenon (C) krypton (D) argon

244. XeF6 on complete hydrolysis gives :

(A) Xe (B) XeO2 (C) XeO3 (D) XeO4
245. Which one of the following fluorides does not exist ?
(A) HeF4 (B) XeF4 (C) CF4 (D) SF6

246. In Kroll and I.C.I process of the production of titanium, the inert gas used is :
(A) Ne (B) Ar (C) Kr (D) Xe
247. Which of the following gaseous molecules is monoatomic ?
(A) chlorine (B) helium (C) oxygen (D) nitrogen
248. Which one of the following noble gases is not found in atmosphere ?
(A) Rn (B) Kr (C) Ne (D) Ar
249. Helium is added to oxygen used by deep sea divers because :
(A) It is less soluble in blood than nitrogen under high pressure
(B) It is lighter than nitrogen
(C) It is readily miscible with oxygen (D) It is less poisonous than nitrogen
250. The inert gas abundantly found in atomosphere is :
(A) Ar (B) Kr (C) He (D) Xe

251. The hybridization of Xe in XeF2 is :

(A) sp3 (B) sp2 (C) sp3d (D) sp2d (E) sp3d2
252. Select the correct matching :
List I List II
A : XeF4 1. Pyramidal
B : XeF6 2. T-Shape
C : XeO3 3. Distorted octahedral
D : XeO2F2 4. Square planar
A B C D
(A) 4 3 1 2
(B) 1 2 3 4
(C) 2 1 3 4
(D) 4 1 3 2
253. Which one of the following does not exist ?
(A) XeOF4 (B) NeF2 (C) XeF2 (D) XeF6
254. Consider following properties of the noble gases :
I : They readily from compounds which are colourless
II : They generally do not form ionic compounds
III : They have variable oxidation states in their compounds
IV : They generally do not form covalent compounds.
Select correct properties.
(A) I, II , III (B) II , III (C) I , III (D) I

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QUESTION FOR SHORT ANSWER :

Group 13th
1. Explain why aluminium, though an electropositive metal, finds extensive use as a structural material
2. Discuss the pattern of variation in oxidation states of the following :
(i) Al to TI (ii) Si to Pb (iii) P to Bi
3. How is LiAlH4 prepared ? What is its important uses ?
4. What happens when NaOH (aq) is added drop wise to a solution of GaCl3 in water ?
5. Give formula of the following :
(i) Felspar (ii) Cryolite (iii) Jeweller’s borax (iv) Corundum (v) Colemanite
6. Answer the following :
(i) What is the outer electronic configuration of group IIA elements ?
(ii) Name the first two elements of group IIIA.
(iii) What is Tincal ?
(iv) What is thermite mixture ?
(v) What is inorganic benzene ?
(vi) Name the two metals present in common alum.
(vii) Name the aluminium compound used in Friedel Craft’s reaction.

7. What happens when :

(i) Borax is heated strongly
(ii) Aluminium is heated with caustic soda solution.
(iii) A mixture of borax and cobalt oxide is heated in a flame.
(iv) Water is added to aluminium nitride.
(v) Aluminium reacts with HNO3.
8. Explain the following with relevent reason.
(i) Aluminium metal is frequently used as reducing agent for the extraction of metals such as Cr, Mn, Fe, etc.
(ii) AlCl3 forms a dimer but BCl3 does not form dimer.
(iii) The B ____ X distance is shorter than what is expected theoretically in BX3 molecule (X = Cl, F, Br, Ι) ?
(iv) Why boron does not form B3+ ion ?
(v) Although the ionisation potential of boron (8.30 eV) is less than gold (9.22 eV), yet former is a non-metal
while the latter is a metal.
(vi) Borazine is more reactive than benzene.
(vii) First ionisation potential of Al is lower than that of Mg.
9. How will you obtain.
(A) Sodium peroxo borate from borax (in two steps only)
(B) Borazole from sodiumboro hydride (in three steps only)
Refer text.
(C) Borax from Boron (in two steps)

Group 14th
10. What is the importance of ultra pure elemental silicon ? How is it obtained ?
11. Write balanced equations for the following reactions :
(A) SnO is treated with dil. HNO3
(B) Tin is treated with an excess of chlorine gas.
(C) Lead sulphide is heated in air.
12. What are silicates ? How are they classified ?
13. What are silicones ? How are they manufactured ?

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14. How far do you agree with the phenomenon concept of inert pair effect ? Justify your answer.
15. Why alkali metals should not be used for drying CCl4 and other chlorocarbons?
16. Why in reactions of HCl & SO2 , PbO2 shows oxidising nature? Explain.
17. Dilute HCl is preferred over dilute H2SO4 for the preparation of CO2 from lime stone. Explain.
18. PbCl4 is less stable than SnCl4 . Explain.
19. Why does not silicon form an analogue of graphite?
20. Like CO why its analogue of SiO is not stable.
21. Why CO2 is a gas and SiO2 is solid ?
22. What happens when,
(a) Mixture of R2 -SiCl2 and R3 - SiCl is subjected to hydrolysis.
(b) Malonic acid is heated in presence of P4O10 .
(c) Tin (IV) Chloride is exposed to moist air.
23. Explain the term "plumbosolvency".

24. Δ
CaO + C ⎯⎯→ (A) + (B)

(A) + N2 (C) + carbon

(C) + H2O (D) + NH3
Identify (A), (B), (C) and (D)
25. How carbonates and bicarbonates can be differentiated from one another ?
Group 15th
26. Give reasons for the following:
(a) Formation of NH3 from its elements at constant pressure is accompanied by a decrease in volume.
(b) Nitric oxide turns brown in air.
(c) Copper dissolves in HNO3 but not in HCl. Δ
(d)
⎯⎯→
⎯→
Pb(NO3)2 on heating produces a pale yellow gas which on strong heating produces brown gas.
27. Write down the electron dot formula of NO, N2, N2O5, NH3, HCN, NH4+, HNO3, HNO2, PH3
28. State the property of ammonia due to which it is used in refrigeration.
29. What happens when:
(a) NH4Cl & NaNO3 is heated strongly
(b) NH4NO3 is heated
(c) NH4NO2 is heated
(d) Mg3N2 reacts with water
(e) NaNO3 is heated with NaOH and Zn powder in water
(f) Mg is burnt in air and the product is treated with water
30. State the conditions under which NH3 is manufactured from N2 and H2.
31. How will you obtain N2 from a mixture of N2 and CO?
32. How will you obtain :
(A) Ammonia from quick lime (in three steps)
(B) H3PO4 from phosphorite (in two steps only)
(C) Meta phosphate from primary phosphate (one step)
(D) White phosphorus from red phosphorus (one step)
(E) Phosphine from hypophosphorus acid (one step)
33. Commercial nitrogen is passed through copper chips kept in ammonia solution for removing oxygen. Explain.
34. Nitric acid acts only as an oxidising agent while nitrous acid can act both as an oxidising and reducing
agent.
35. Write down a reaction showing action of N2O4(A) as non-aqeous solvent.
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36. A waxy crystalline solid (A) with a garlic odour is obtained by buring white P in a stream of air. (A) reacts
vigorously with hot water forming a gas (B) and an acid (C). Gas (B) has unplesant odour of rotten fish and is
neutral towards litmus. When passed through CuSO4 solution gas (B) produced a black ppt. (D) What are
(A) to (D) ? Give chemical equations of the reactions.
37. Why does H3PO3 act as a reducing agent but H3PO4 does not ?

Group 16th
38. Oxygen almost invariably exhibits an oxidation state of -2 but other members of the family exhibit negative as
well as positive oxidation state of +2, +4 and +6.
39. Sulphur dioxide acts as a strong reducing agent in alkaline medium.
40. Among the hydrides, H2O, H2S, H2Se which has highest bond angle.
41. Which of the following has highest boiling point and why
(a) H2O (b) H2S
42. What do you understand by tailing of mercury ?
43. An inorganic halide (A) reacts with water to form two acids (B) and (C). Also aqueous solution of (A) reacts
with KOH to form two salts (D) and (E) Which are soluble in water. The solution gives white precipitates with
both AgNO3 and BaCl2 solutions respectively. Identify (A) to (E) and write the chemical reactions involved.
44. From the reactions given below, identify (A), (B), (C) and (D) and write their formulae.
(A) + dil. H2SO4 + K2Cr2O7 → (B) Green Solution
(A) + dil. H2SO4 + (C) MnSO4
(A) + O2 (D)
(D) + BaCl2 → White ppt.
45. Arrange the following in increasing order
(a) H2O, CO2, SO3, N2O5, SiO2 - Acidic character
(b) H2O, H2S, H2Se, H2Te - Thermal stability
46. On heating rhombic sulpur it melts but viscosity of liquid increases upto 2000C and beyond that it decreases
why ?
→⎯⎯ H2 O
⎯→
47. O - O bond length is more in H2O2 than in O2F2 . Explain.
48. For drying H2S gas conc. H2SO4 can not be used why ?
49. Draw the structure of following acids.
(a) Marshall's acid (b) Dithionic acid (c) Caro's acid (d) Thiosulphuric acid
50. Complete the following equations
(i) I2 + O3 + H2O HIO3 + ................
(ii) NaHS + .............. Na2S2O3 + H2O
(iii) (NH4)2S2O8 + H2O + MnSO4 ..............+..................+.................
(iv) Sb2S3 + HCl ...............+...............
(v) Hg2Cl2 + SO2 + HCl .................+..................+.................

(vi) CaS + H2O + CO2 ................+.................

51. What happens when

(A) FeCl3 reacts with hypo solution
(B) Mn2O7 dissolves in water.
(C) CuCl2 reacts with aqueous Na2S2O3
(D) Sulphuric acid is heated with potassium.

Group 17th
52. What happens when ? (Give balanced equations)
(i) Sodium iodate is treated with sodium bisulphite solution.
(ii) Chlorine is passed through hot NaOH solution.

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(iii) Chlorine is passed into aqueous potassium hydroxide.

(iv) Chlorine gas is bubbled through a solution of ferrous bromide
(v) Iodine reacts with conc. HNO3.
(vi) Chlorine is passed over slaked lime.
(vii) Potassium iodide is heated with MnO2 and conc. H2SO4.
(viii) Chlorine reacts with Na2SO3 solution.
(ix) Iodine is added to acidified stannous chloride solution
53. Explain the following with proper reason :
(i) Fluorine cannot be prepared from fluorides by chemical oxidation.
(ii) Anhydrous HCl is a bad conductor of electricity while aqueous HCl is a good conductor.
(iii) Halogens are strong oxidising agents.
(iv) The bleaching action of chlorine is permanent while that of sulphur dioxide is temporary.
(v) Iodine dissolves more in KΙ solution than in water..
(vi) KHF2 is well known whereas KHCl2 or KHBr2 does not exist.
(vii) Ferric iodide is very unstable but ferric chloride is stable.
(viii) Fluorine does not form F3– (polyhalide) ion.
(ix) HF is not stored in glass bottles but kept in wax lined bottles.

(x) HF has a greater electronegativity difference and more ionic character than HCl, HBr and HI but it is
the weakest acid.
54. Arrange the following :
(i) Increasing order of thermal stability HOCl, HClO2, HClO3, HClO4.
(ii) Increasing acid strength HClO, HClO2, HClO3, HClO4.
(iii) Increasing oxidising power HClO, HClO2, HClO3 , HClO4.
(iv) Increasing reducing nature F–, Cl–, Br–, Ι–.
(v) Increasing oxidation number of iodine Ι2, HΙ, HΙO4. ΙCl.
(vi) Increasing acid strength HOF, HOCl, HOBr, HOΙ.
(vii) Increasing oxidising power F2, Cl2, Br2, Ι2.
(viii) Increasing acid strength HF, HCl, HBr, HΙ.
(ix) Increasing electronegativity or reactivity F, Cl Br, Ι.
(x) Increasing electron affinity F, Cl, Br, Ι.
55. HI can not be prepared by heating NaI with conc. H2SO4. Give the method which is preferred for the preparation
of HI.
56. Freshly distilled colourless HI (aqueous solution) gradually turns brown with time.
57. State what happens when super halogen reacts with a cold dilute solution of NaOH ?
58. Complete and balance the following reactions :
(A) – CH = CH – + ICl ⎯→ ; (B) HCl + KIO3 + 2KI ⎯→
(C) SiO2 + HF ⎯→ ; (D) Pb3O4 + HCl ⎯→ ; (E) H2O2 + ClO2 + OH– ⎯→

Group 18th
59. Answer the following with relevant reason.
(i) Why the zero group elements do not form compounds under ordinary conditions ?
(ii) Xenon has closed shell configuration but is known to give compounds with fluorine.
(iii) The boiling points of noble gases increase with increase in atomic number.
(iv) A mixture of He and O2 is used for respiration by sea divers.
(v) Why helium and neon do not form clathrate compounds with quninol ?

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60. Point out hybridisation and draw the structures of XeF4, XeF6, XeOF4, XeOF2, XeO3 and XeO4.

61. What is quantum mechanical liquid i.e. helium (ii) ? Give its two important characteristics.

62. How does XeO3 reacts with aqueous alkali ?

63. Write down the formula of the noble gas species which are isostructural with (a) ICl4– (b) IBr2– (c) BrO3–.

64. Write the oxidation product when XeO3 oxidises Ι– in acidic medium.

65. XeF6 is not stored in glass or quartz vessels. Why ?

66. Write down the hydrolysis of XeF6 in strongly alkaline medium.

67. Arrange the XeF2, XeF4, XeF6 in decreasing order of Xe – F bond length, give reason also.

A Objective :
Group 13th

1. Statement : 1 Boron always forms covalent bond. because [IIT- 2007]

Statement : 2 The small size of B3+ favours formation of covalent bond.
(A) Statement : 1 is True, Statement-2 is True ; Statement -2 is a correct explanation for Statement-1
(B) Statement-1 is True, Statment-2 is True ; Statement-2 is NOT a correct explanation for Statement-1
(C) Statement-1 is True, Statement-2 is False
(D) Statement-1 is False, Statement-2 is True
2. Statement : 1 In water, orthoboric acid behaves as a weak monobasic acid. because [IIT- 2007]
Statement : 2 In water, orthoboric acid acts as a proton donor.
(A) Statement : 1 is True, Statement-2 is True ; Statement -2 is a correct explanation for Statement-1
(B) Statement-1 is True, Statment-2 is True ; Statement-2 is NOT a correct explanation for Statement-1
(C) Statement-1 is True, Statement-2 is False
(D) Statement-1 is False, Statement-2 is True

3. B(OH)3 + NaOH ⎯⎯→ Na[B(OH)4] (aq)

Then addition of which of the following proceeds the reaction in the forward direction. [JEE 2006]
(A) cis-1, 2 diol (B) Trans 1, 2 diol (C) Borax (D) Na2 HPO4

4. H3BO3 is : [JEE 2003]

(A) Monobasic and weak Lewis acid (B) Monobasic and weak Bronsted acid
(C) Monobasic and strong Lewis acid (D) Tribasic and weak Bronsted acid

5. The geometry and the type of hybrid orbital present about the central atom in BF3 is : [ JEE 1998]
(A) linear, sp (B) trigonal planar, sp2 (C) tetrahedral, sp3 (D) pyramidal, sp3

6. Which of the statements about anhydrous aluminium chloride is correct ? [ JEE 1981 ]
(A) It exists as AlCl3 molecule (B) It is not easily hydrolysed
(C) It sublimes at 100ºC under vacuum (D) It is a strong Lewis base

Group 14th
7. Name the structure of silicate in which three oxygen atoms of [SiO4]4– are shared. [JEE 2005]
(A) Pyrosilicate (B) Sheet silicate
(C) Linear chain silicate (D) Three dimensional silicate
8. Which one of the following oxides is neutral ? [JEE 2004]
(A) CO (B) SnO2 (C) ZnO (D) SiO2

9. (Me)2 SiCl2 on hydrolysis will produce : [JEE 2003]

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(A) (Me)2 Si(OH)2 (B) (Me)2 Si = O
(C) – [⎯O⎯(Me)2 Si ⎯O⎯]n⎯ (D) Me2SiCl(OH)
10. Identify the correct order of acidic strengths of CO2, CuO, CaO, H2O [JEE 2002]
(A) CaO < CuO < H2O < CO2 (B) H2O < CuO < CaO < CO2
(C) CaO < H2O < CuO < CO2 (D) H2O < CO2 < CaO < CuO

11. The correct order of increasing C–O bond length of CO, CO 23− , CO2 is : [JEE 1999]

(A) CO 23− < CO2 < CO (B) CO2 < CO 23− < CO

(C) CO < CO23 − < CO2 (D) CO < CO2 < CO23 −

12. Which of the following halides is least stable and has doubtful existence? [JEE 1996]
(A) CΙ4 (B) GeΙ4 (C) SnΙ4 (D) PbΙ4

Group 15th
13. A pale blue liquid is obtained by equimolar mixutre of two gases at –30ºC : [JEE 2005]
(A) N2O (B) N2O3 (C) N2O4 (D) N2O5
14. Which of the following isomers of phosphorous is thermodynamically most stable ? [JEE 2005]
(A) Red (B) White (C) Black (D) Yellow
15. (NH4)2 Cr2O7 on heating gives a gas which is also given by [JEE 2004]
(A) Heating NH4NO2 (B) Heating NH4NO3
(C) Mg3 N2 + H2O (D) Na(comp.) + H2O2
16. For H3PO3 and H3PO4 , the correct choice is : [JEE 2003]
(A) H3PO3 is dibasic and reducing (B) H3PO3 is dibasic and non-reducing
(C) H3PO4 is tribasic and reducing (D) H3PO3 is tribasic and non-reducing
17. Polyphosphates are used as water softening agents because they [JEE 2002]
(A) form soluble complexes with anionic species
(B) precipitate anionic species
(C) form soluble complexes with cationic species
(D) precipitate cationic species
18. The number of P⎯O⎯P bonds in cyclic metaphosphoric acid is : [JEE 2000]
(A) zero (B) two (C) three (D) four
19. The correct order of acidic strength is : [JEE 2000]
(A) Cl2O7 > SO2 > P4O10 (B) CO2 > N2O5 > SO3
(C) Na2O > MgO > Al2O3 (D) K2O > CaO > MgO
20. Ammonia can be dried by : [JEE 2000]
(A) Conc. H2SO4 (B) P4O10 (C) CaO (D) Anhydrous CaCl2
21. Ammonia, on reaction with hypochlorite anion, can form : [JEE 1999]
(A) NO (B) NH4Cl (C) N2H4 (D) HNO2
22. One mole of calcium phosphide on reaction with excess water gives : [JEE 1999]
(A) one mole of phosphine (B) two moles of phosphoric acid
(C) two moles of phosphine (D) one mole of phosphorus pentoxide
23. On heating ammonium dichromate, the gas evolved is : [JEE 1999]
(A) oxygen (B) ammonia (C) nitrous oxide (D) nitrogen
24. Evaluate the following Assertion & the Reason thereof [JEE 1998]
Assertion : HNO3 is stronger acid than HNO2 .
Reason : In HNO3 there are two nitrogen to oxygen bonds where as in HNO2 there is only one
(A) Both (A) and (R) are correct and (R) is the correct explanation of (A)
(B) Both (A) and (R) are correct and (R) is not the correct explanation of (A)
(C) (A) is correct but (R) is incorrect
(D) (A) is incorrect but (R) is correct
25. White phosphorus (P4) has : [JEE 1998]
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(A) six P–P single bonds (B) four P–P single bonds
(C) four lone pairs of electrons (D) PPP angle of 60°
26. The cyanide ion CN– and N2 are isoelectronic. But in constrast to CN–, N2 is chemically inert, because of :
(A) low bond energy
(B) absence of bond polarity
(C) unsymmetrical electron distribution
(D) presence of more number of electrons in bonding orbitals. [JEE 1992]
27. The reddish brown coloured gas formed when nitric oxide is oxidised by air is : [JEE 1979]
(A) N2O5 (B) N2O4 (C) NO2 (D) N2O3

Group 16th
28. Which of the following is not oxidised by O3 ? [JEE 2005]
(A) KΙ (B) KMnO4 (C) K2 MnO4 (D) FeSO4
29. Which gas is evolved when PbO2 is treated with concentrated HNO3 [JEE 2005]
(A) NO2 (B) O2 (C) N2 (D) N2O
30. Which of the following oxoacids of sulphur has –O–O– linkage [JEE 2004]
(A) H2 S2 O3 (B) H2 S2 O5 (C) H2 S2 O6 (D) H2 S2 O8
31. The number of S–S bonds, in sulpur trioxide trimer S3O9 is [JEE 2001]
(A) three (B) two (C) one (D) Zero
32. Which of the following does not have S–S linkage? [REE 2000]
(A) S2O82– (B) S2O62– (C) S2O52– (D) S2O32–
33. Hydrolysis of one mole of peroxy disulphuric acid produces [JEE 1996]
(A) two moles of sulphuric acid
(B) two moles of peroxymonosulphuric acid.
(C) one mole of sulphuric acid and one mole of peroxy monosulphuric acid.
(D) one mole of sulphuric acid, one mole of hydrogen peroxide.
34. The oxidation number of sulphur in S8, S2 F2, H2S respectively are :
(A) 0, +1 and –2 (B) +2, +1 and –2 (C) 0, +1 and +2 (D) – 2, +1 and –2
35. Sodium thiosulphate is prepared by [JEE 1996]
(A) reducing Na2 SO3 solution with H2S (B) Boiling Na2SO3 with S in alkaline medium.
(C) Neutralising H2S2O3 solution with NaOH (D) Boiling Na2SO3 with S in an acidic medium
36. Which statement about H2S is false ? [JEE 1996]
(A) It is a covalent compound (B) It is a gas with bad smell
(C) It is a weak base than water (D) It is a stronger reducing agent than H2O
37. There is no S–S bond in : [JEE 1991]
(A) S2O42– (B) S2O5 (C) S2O32– (D) S2O72–
38. Which compound acts as an oxidising as well as a reducing agent? [JEE 1991]
(A) SO2 (B) MnO2 (C) Al2O3 (D) CrO3
39. A gas that can not be collected over water is [JEE 1988]
(A) N2 (B) O2 (C) SO2 (D) PH3

Group 17h & 18th

40. Total number of lone pairs of electrons in XeOF4 is : [JEE 2004]
(A) 0 (B) 1 (C) 2 (D) 3
41. Which of the following contains maximum number of lone pairs of electrons on the central atom? [JEE 2004]
(A) ClO3– (B) XeF4 (C) SF4 (D) Ι3–
42. Molecular shapes of SF4, CF4 and XeF4 are : [JEE 2000]

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(A) six P–P single bonds (B) four P–P single bonds
(C) four lone pairs of electrons (D) PPP angle of 60°
26. The cyanide ion CN– and N2 are isoelectronic. But in constrast to CN–, N2 is chemically inert, because of :
(A) low bond energy
(B) absence of bond polarity
(C) unsymmetrical electron distribution
(D) presence of more number of electrons in bonding orbitals. [JEE 1992]
27. The reddish brown coloured gas formed when nitric oxide is oxidised by air is : [JEE 1979]
(A) N2O5 (B) N2O4 (C) NO2 (D) N2O3

Group 16th
28. Which of the following is not oxidised by O3 ? [JEE 2005]
(A) KΙ (B) KMnO4 (C) K2 MnO4 (D) FeSO4
29. Which gas is evolved when PbO2 is treated with concentrated HNO3 [JEE 2005]
(A) NO2 (B) O2 (C) N2 (D) N2O
30. Which of the following oxoacids of sulphur has –O–O– linkage [JEE 2004]
(A) H2 S2 O3 (B) H2 S2 O5 (C) H2 S2 O6 (D) H2 S2 O8
31. The number of S–S bonds, in sulpur trioxide trimer S3O9 is [JEE 2001]
(A) three (B) two (C) one (D) Zero
32. Which of the following does not have S–S linkage? [REE 2000]
(A) S2O82– (B) S2O62– (C) S2O52– (D) S2O32–
33. Hydrolysis of one mole of peroxy disulphuric acid produces [JEE 1996]
(A) two moles of sulphuric acid
(B) two moles of peroxymonosulphuric acid.
(C) one mole of sulphuric acid and one mole of peroxy monosulphuric acid.
(D) one mole of sulphuric acid, one mole of hydrogen peroxide.
34. The oxidation number of sulphur in S8, S2 F2, H2S respectively are :
(A) 0, +1 and –2 (B) +2, +1 and –2 (C) 0, +1 and +2 (D) – 2, +1 and –2
35. Sodium thiosulphate is prepared by [JEE 1996]
(A) reducing Na2 SO3 solution with H2S (B) Boiling Na2SO3 with S in alkaline medium.
(C) Neutralising H2S2O3 solution with NaOH (D) Boiling Na2SO3 with S in an acidic medium
36. Which statement about H2S is false ? [JEE 1996]
(A) It is a covalent compound (B) It is a gas with bad smell
(C) It is a weak base than water (D) It is a stronger reducing agent than H2O
37. There is no S–S bond in : [JEE 1991]
(A) S2O42– (B) S2O5 (C) S2O32– (D) S2O72–
38. Which compound acts as an oxidising as well as a reducing agent? [JEE 1991]
(A) SO2 (B) MnO2 (C) Al2O3 (D) CrO3
39. A gas that can not be collected over water is [JEE 1988]
(A) N2 (B) O2 (C) SO2 (D) PH3

Group 17h & 18th

40. Total number of lone pairs of electrons in XeOF4 is : [JEE 2004]
(A) 0 (B) 1 (C) 2 (D) 3
41. Which of the following contains maximum number of lone pairs of electrons on the central atom? [JEE 2004]
(A) ClO3– (B) XeF4 (C) SF4 (D) Ι3–
42. Molecular shapes of SF4, CF4 and XeF4 are : [JEE 2000]

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(A) the same with 2, 0 and 1 lone pairs of electrons respectively
(B) the same with 1, 1 and 1 lone pairs of electrons respectively
(C) different with 0, 1 and 2 lone pairs of electrons respectively
(D) different with 1, 0 and 2 lone pairs of electrons respectively
43. Which one of the following is not a pseudohalide ? [JEE 1997]
(A) CNO– (B) RCOO– (C) OCN– (D) NNN –

44. The following acids have been arranged in order of decreasing acid strength. Identify the correct order.
ClOH (Ι), BrOH (ΙΙ), IOH (ΙΙΙ) [IIT 1996]
(A) Ι > ΙΙ > ΙΙΙ (B) ΙΙ > Ι > ΙΙΙ (C) ΙΙΙ > ΙΙ > Ι (D) Ι > ΙΙΙ > ΙΙ
45. Which one of the following pairs of substances when mixed, produces chlorine gas at room temperature
[JEE 1995]
(A) NaCl and MnO2 (B) NaCl and HNO3 (conc.)
(C) NaCl and H2SO4 (conc.) (D) HCl (conc.) and KMnO4
46. Concentrated H2SO4 cannot be used to prepare HBr from NaBr, because it [JEE 1995]
(A) Reduces HBr (B) Oxidises HBr
(C) Disproportionates HBr (D) Reacts slowly with NaBr
47. Which one of the following configuration represents a noble gas [JEE 1993]
(A) 1s2 2s2 p6, 3s2 (B) 1s2 2s2 p6, 3s1 (C) 1s2 2s2 p6 (D) 1s2 2s2 p6, 3s2 p6 , 4s2
48. The type of hybrid orbitals used by chlorine atom in ClO2– is [JEE 1992]
(A) sp3 (B) sp2 (C) sp (D) None of these
49. Which of the following is strongest oxidising agent [JEE 1992]
(A) F2 (B) Cl2 (C) Br2 (D) Ι2
50. The strongest acid amongst the following is [JEE 1989]
(A) HClO4 (B) HClO3 (C) HClO2 (D) HClO
51. Concentrated HNO3 reacts with Ι2 to give [JEE 1989]
(A) HΙ (B) HOΙ (C) HΙO3 (D) HOΙO3
52. → of−6
Chlorine acts as a bleaching agent only in presence [JEE 1983]
Si 2O 7
(A) Dry air (B) Moisture (C) Sunlight (D) Pure oxygen

Section : (B) Subjective

Group 13th
1. AlF3 is insoluble in anhydrous HF but when little KF is added to the compound it becomes soluble. On
addition of BF3, AlF3 is precipitated. Write the balanced chemical equations. [JEE 2004]
2. Which one is more soluble in diethyl ether anhydrous AlCl3 or hydrous AlCl3? Explain in terms of bonding.
[JEE 2003]
3. Match the column : [JEE 2003]
Column I Column II
(A) Bi3+ → (BiO)+ (p) Heat
(B) [AIO2]– Al(OH)3 (q) Hydrolysis
(C) SiO44– (r) Acidification
(D) (B4O72–) → [B(OH)3] (s) Dilution by water

4. Write balanced equation for the reactions of the following compounds with water : [JEE 2002]
(i) Al4C3 (ii) CaNCN (iii) BF3 (iv) NCl3 (v) XeF4
5. How is boron obtained from borax. Give chemical equations with reaction conditions. Write the structure of
B2H6 and its reaction with HCl. [JEE 2002]
6. Compound (X) on reduction with LiAlH4 gives a hydride (Y) containing 21.72% hydrogen along with other
products. The compound (Y) reacts with air explosively resulting in boron trioxide. Identify (X) and (Y). Give
balanced reaction involved in the formation of (Y) and its reaction with air. Draw structure of (Y).
[ JEE 2001 ]
7. Write the chemical reactions associated with the ‘borax bead test’ of cobalt (ΙΙ) oxide. [ JEE 2000 ]

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8. Evaluate the following Assertion & the Reason there of :

Assertion : Al (OH)3 is amphoteric in nature.
Reason : Al–O and O–H bonds can be broken with equal ease in Al(OH)3. [ JEE 1998 ]
9. Identify A and B in the following reactions : [JEE 1989]
Colemanite + (A) ⎯→ Na2B4O7
Na2B4O7 + (B) ⎯→ H3BO3
10. Aluminium sulphide gives a foul odour when it becomes damp. Write a balanced chemical
equation for the reaction. [ JEE 1997 ]
11. Write balanced equation for the following :
Reaction of aluminium with aqueous sodium hydroxide. [ JEE 1997]
12. (i) A white precipitate (B) is formed when a mineral (A) is boiled with Na2CO3 solution. [REE 1995]
(ii) The precipitate is filtered and filtrate contains two compounds (C) and (D). The compound (C) is removed
by crystallisation and when CO2 is passed through the mother liquor left (D) changes to (C).
(iii) The compound (C) on strong heating gives two compounds (D) and (E).
(iv) (E) on heating with cobalt oxide produces blue coloured substances (F).
Identify (A) to (F) and gives chemical equations for the reactions at steps (i) to (iv).
13. The two types of bonds present in B2H6 are covalent and .......... [ JEE 1994 ]
14. Give reason for the following : [ JEE 1994 ]
Although aluminium is above hydrogen in the electrochemical series, it is stable in air and water.
15. An inorganic Lewis acid (X) shows the following reactions : [REE 1994]
(i) It fumes in most air. (ii) The intensity of fumes increases when a rod dipped in NH4OH is brought near it.
(iii) An acidic solution of (X) on addition of NH4Cl and NH4OH gives a precipitate which dissolves in NaOH
solution. (iv) An acidic solution of (X) does not give precipitate with H2S. Identify (X) and give chemical
equations for reactions at steps (i) to (iii).
16. The basic nature of the hydroxides of Group 13 decreases progressively down the group.
(True or False) [ JEE 1993 ]

17. A certain salt (X) gives the following tests : [REE 1991]
(i) Its aqueous solution is alkaline to litmus.
(ii) On strongly heating it swells to give glassy material.
(iii) When concentrated H2SO4 is added to hot concentrated solution of (X), white crystals of a weak acid
separate out. Identify (X) and write down the chemical equations for reaction at steps (i), (ii), (iii)

Group-14
18. Trimethyl [(CH3)3N] is pyramidal while trimethyl silane [(SiH3)3N] is planar. Explain ? [JEE 2005]
19. Starting from SiCl4, prepare the following in steps not exceeding the number given in parentheses
(give reactions only) : [JEE 2001]
(i) Silicon (1)
(ii) Linear silicone containing methyl groups only (4)
(iii) Na2SiO3 (3)
20. Complete the following reaction :
(i) SnCl4 + C2H5Cl + Na ⎯→ [IIT 1998]
(ii) C + HNO3(conc.) ⎯→ [Roorkee 1999]
21. Diamonds is very hard while graphite is soft. [IIT 1993]
22. Write down hydrolysis of
(i) Alkyl substituted chlorosilane [IIT 1991]
(ii) Trialkyl chlorosilane [IIT 1994]

Group 15th
23. Using VSEPR theory, draw the shape of PCl5 and BrF5 . [JEE 2003]
24. Write the balanced equation for the reaction of CaCN2 with water. [JEE 2002]
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25. (i) Sodium salt of an acid (A) is formed on boiling white phosphorus with NaOH solution.
(ii) On passing chlorine through phosphorus kept fused under water, another acid (B) is formed which on
heating gives metaphosphorus acid.
(iii) Phosphorus on treatment with conc. HNO3 gives an acid (C) which is also formed by the action of dilute
H2SO4 on powdered phosphorite rock.
(iv) (A) on treatmen with a solution of HgCl2 first gives a white precipitate of compound (D) and then a grey
precipitate of (E). Identify (A) to (E) and write balanced chemical equations for the reactions at steps (i) to
(iv). [Roorkee 2001]
26. Give reasons(s) why elemental nitrogen exists as a diatomic molecule whereas elemental phosphorus is a
tetraatomic molecule. [JEE 2000]
27. In the following reaction,
A + 2B + H2O ⎯→ C + 2D
(A = HNO2 , B = H2SO3, C = NH2OH). Identify D. [JEE 1999]
28. What happens when phosphoric acid reacts with Ca5(PO4)3F. [JEE 1998]
29. Complete and balance the following :
(i) P4O10 + PCl5 ⎯→ [JEE 1998]
(ii) NH3 + NaOCl ⎯→ [JEE 1993]
30. What happens when gold is treated with aquaregia. [JEE 1997]
31. Write balanced equation for the following : [JEE 1997]
(i) phosphorus is treated with concentrated nitric acid.
(ii) Manufacture of phosphoric acid from phosphorus.
32. Draw the structure of P4O10 and identify the number of single and double P–O bonds. [JEE 1996]
33. Account for the following : [JEE 1995]
(a) The experimentally determined N–F bond length in NF3 is greater than the sum of the single bond
covalent radii of N and F.
(b) Mg3 N2 when reacted with water gives off NH 3 but HCl is not obtained from MgCl 2 on
reaction with water at room temperature.
34. (i) An organic iodide (A) on heating with a solution of KOH gives a gas (B) and the solution of compound (C).
(ii) The gas (B) on ignition in air gives a compound (D) and water.
(iii) Copper sulphate is finally reduced to the metal on passing (B) through its solution.
(iv) Precipitate of compound (E) is formed on reaction of (C) with copper sulphate solution. Identify (A) to (E)
and give chemical equations for steps (i) to (iv). [REE 1994]
35. What happens when white phosphorus is boiled with a strong solution of NaOH in moist atmosphere.
[JEE 1993]
36. An orange solid (A) on heating gives a green residue (B), a colourless gas (C) and water vapour. The dry gas
(C) on passing over heated Mg gave a white solid (D). (D) on reaction with water gave a gas (E) which formed
dense white fumes with HCl. Identify (A) to (E) giving reactions. [JEE 1993]
37. What happens when : [JEE 1992]
(i) Red phosporus is treated with I2 and water.
(ii) Cu reacts with HNO3 to produce NO and NO2 in the ratio 2 : 1
38. In P4O10, the number of oxygen atoms bonded to each phosphorus atom is ............... [JEE 1992]
39. What happens when : [JEE 1991]
(i) Ammonia reacts with KMnO4
(ii) Phosphorus reacts with conc. HNO3.
(iii) A mixture of NO and NO2 is passed in Na2CO3 solution. [JEE 1991]
40. What happens when : [JEE 1990]
(i) Aqueous solution of NaNO3 is heated with zinc dust and caustic soda.
(ii) CaO in water reacts with phosphorus. [JEE 1990]

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Group 16 th

41. Aqueous solution of sodium thiosulphate turns milky white, on acidification. Why ? [JEE 2005]
42. In the contact process for industrical manufacture of sulphuric acid some amount of sulphuric acid is used as
a starting material. Explain briefly. What is the catalyst used in the oxidation of SO2? [JEE 1999]
43. Thionly chloride can be synthesized by chlorinating SO2 using PCl5. Thionly chloride is used to prepare
anhydrous ferric chloride starting from its hexahydrated salt. Alternatively, the anhydrous ferric chloride can
also be prepared from its hexahydrated salt by treating with 2, 2-dimethoxypropane. Discuss all this using
balanced chemical equations. [JEE 1998]
44. An aqueous solution of a gas (X) gives the following reactions :
(i) It decolourizes an acified K2Cr2O7 solution.
(ii) On boiling with H2O2 , cooling it and then adding an aqeuous solution of BaCl2 , a precipitate insoluble in
dil HCl is obtained.
(iii) On passing H2S gas in the solution, white turbidity is obtained. Identifty (X) and give equations for steps
(i), (ii) and (iii) [REE 1993]
45. Complete the following equation : [JEE 1993]
(NH4)2 S2 O8 + H2O + MnSO4 ⎯⎯→ ........ + ......... + ..........

46. Arrange the following in decreasing order of acidic character H2O, CO2 , SO3 , N2O5 , SiO2 [JEE 1988]

47. What happens when [JEE 1985]

(i) Sulphur dioxide is bubbled through aqueous solution of copper sulphate in presence of potassium
thiocyanate. [JEE 1982]
(ii) Hydrogen sulphide is bubbled through an aqueous solution of sulphur dioxide . [JEE 1985]

Group 17th & 18th

48. Write balanced equation for the reaction of XeF4 with water. Also name the reaction nature [JEE 2002]

49. Give an example of oxidation of one halide by another halogen. Explain the feasibility of reaction.

50. Bleaching of flowers by chlorine is permanent while after bleaching with SO2, the colour returns. Explain.
[REE 2000]
51. H2SO4 + HΙ ⎯⎯→ ________ + ___________ + ________ [REE 1998]

52. CaOCl2 + NaΙ + HCl ⎯⎯→ _________ + CaCl2 + H2O + NaCl [REE 1998]

53. A liquid A is treated with Na2CO3 solution. A mixture of two salts B and C are produced in the soluiton. The
mixture on acidification with sulphuric acid and distillation produces the liquid A again. Identify A, B and C
and write the equations involved. [JEE 1997]

54. Complete the following chemical equations and justify the formation of the products in these reactions.
KI + Cl2 ⎯→ ; KCIO3 + l2 ⎯→ [JEE 1996]

55. HBr is a stronger acid than HΙ because of hydrogen bonding (true/false). [JEE 1993]

56. K2Cr2O7 + HCl ⎯⎯→ KCl + CrCl3 + _________ + _________. [JEE 1992]
57. Iodine reacts with hot concentrated NaOH solution. The products are NaΙ and _________. [JEE 1990]

58. An inorganic compound (X) gives a brick red flames on performing flame test. This compound gives the
following tests also.
(a) smells of chlorine when placed in moist air.
(b) if KΙ and CH3COOH are added to the suspension in water, a brown colour is obtained. Identigy (X) and
write down equations for reactions at steps (a) and (b) [REE 1989]
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59. Arrange HClO, HClO2, HClO3, HClO4 in increasing order of acid strength.

60. Arrange HF, HCl , HBr, HΙ in order of increasing acid strength

61. A certain compound (X) shows the following reactions.

(i) When KI is added to an aqueous suspension of (X) containing acetic acid, iodine is liberated.
(ii) When the paste of (X) in water is heated with ethyl alcohol, a product of anesthetic use is obtained.
(iii) When CO2 is passed through an aqueous suspension of (X) the turbidity transforms to a precipitate.
Identify (X) and write down chemical equations for the step (i), (ii) & (iii) [REE 1989]

62. The increase in solubility of iodine in an aqueous solution of potassium iodide is due to the formation of
________. [JEE 1988]

63. Arrange Ι2 , HΙ , HΙO4, ΙCl in increasing order of oxidation number of of iodine [JEE 1986]

64. Chlorine is passed through hot NaOH Solution. Give chemical equation involved. [JEE 1983]

65. In the preparation of HI from KΙ , phosphoric acid is preferred to sulphuric acid. Explain. [JEE 1982]

66. Silver fluoride is fairly ____________ in water. [JEE 1982]

67. What happens when sodium iodate is treated with sodium bisulphite solution [JEE 1982]

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EXERCISE - 1
SECTION (A) :
Group 13th
1. B 2. C 3. C 4. A 5. B 6. B 7. C
8. D 9. B 10. C 11. C 12. A 13. B 14. D
15. C 16. D 17. A 18. A 19. B 20. B 21. C
22. D 23. D 24. D 25. A 26. D 27. D 28. C
29. B 30. B 31. D 32. C 33. D 34. D 35. C

36. A 37. C 38. C 39. B 40. D 41. C 42. B

43. C 44. C 45. C 46. A 47. B 48. A 49. B
50. C 51. B 52. C 53. B 54. D 55. A
Group 14th
56. A 57. C 58. C 59. C 60. B 61. A 62. B
63. D 64. A 65. C 66. C 67. A 68. B 69. A
70. C 71. A 72. B 73. D 74. C 75. D 76. B
77. C 78. A 79. B 80. C 81. C 82. B 83. A
84. D 85. A 86. A 87. D 88. C 89. C 90. C
91. D 92. B 93. B 94. B 95. D 96. B 97. A
98. D 99. B 100. A

Group 15th
101. D 102. D 103. A 104. B 105. B 106. A 107. A
108. A 109. C 110. C 111. A 112. D 113. D 114. C
115. B 116. C 117. A 118. B 119. D 120. C 121. D
122. D 123. B 124. C 125. C 126. B 127. C 128. A
129. D 130. A 131. C 132. D 133. B 134. C 135. D
136. C 137. B 138. C 139. A 140. D 141. C 142. D
143. B 144. A 145. C 146. B 147. D 148. D 149. B
150. D 151. A 152. D 153. D 154. B 155. C 156. C
157. C 158. A 159. A 160. D 161. B 162. B

16th Group
163. C 164. A 165. C 166. D 167. D 168. B 169. D
170. A 171. A 172. B 173. D 174. B 175. B 176. C
177. D 178. B 179. D 180. C 181. B 182. A 183. C
184. D 185. B 186. B 187. D 188. B 189. D 190. A
191. D 192. C 193. B 194. A 195. C 196. A 197. C
198. C 199. D 200. B 201. D

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Group 17th
202. A 203. A 204. D 205. C 206. C 207. B 208. C
209. A 210. A 211. D 212. B 213. B 214. D 215. A
216. D 217. D 218. D 219. C 220. C 221. C 222. A
223. D 224. A 225. B 226. B 227. C 228. A 229. C
230. B 231. C 232. C 233. A 234. C 235. B 236. B
237. D 238. D 239. D 240. B

Group 18th

241. B 242. C 243. B 244. C 245. A 246. B 247. B

248. A 249. A 250. A 251. C 252. A 253. B 254. B

EXERCISE - 2
Group 13th
1. (a) being electropositive reacts with air or oxygen to form protective layer of Al2O3 on its surface which
protects it form further action.
(b) Cheap and light metal and forms alloys with other metal which are not easily corrode.
2. (i) Al has no d-or f-electrons. Therefore, it does not exhibit inert pair effect and consequenty, it shows an
oxidation state of +3 only due to the presence of two electrons in the s-and one electron in the p-orbital of the
valence shell. As we move down the group from Ga to TI, the stability of +1 oxidation state increases while
that of =3 oxidation decreases due to inert pair effect. For
(ii) and
(iii) refer text.

3. 4LiH + AlCl3 ⎯⎯ ⎯→ Li [AlH4] + 3LiCl.

Dry ether
⎯⎯
+ –

Reducing agent in organic chemistry.

4. GaCl3 + 3NaOH ⎯→ Ga(OH)3 ↓ + 3NaCl
Ga(OH)3 + NaOH ⎯→ NaGaO2 + 2H2O
5. (i) KAISi3O8 (ii) Na3AIF6 (iii) Na2B4O7.5H2O (iv) Al2O3 (v) Ca2B6O11.5H2O
6. (i) ns2 np1
(ii) Boron and aluminium
(iii) It is a mineral of boron. Its composition is Na2B4O7.10H2O
(iv) Mixture containing 1 part Al powder and 3 parts Fe2O3 or Cr2 O3
(v) Borazole or borazine, B3N3H6 is known as inorganic benzene
(vi) Common alum is the double sulphate of potassium and aluminium. Its composition is,
K2SO4.Al2(SO4)3.24H2O
(vii) Anhydrous aluminium chloride, AlCl3.
−10H O
7. (i) Na2B4O7.10H2O ⎯⎯ ⎯2⎯→ Na2B4O7 ⎯⎯→ 2NaBO2 + B2O3

(ii) 2AI + 2NaOH + 2H2O ⎯⎯→ 2NaAIO2 + 3H2

−10H O
(iii) Na2B4O7.10H2O ⎯⎯ ⎯2⎯→ Na2B4O7 ⎯⎯→ 2NaBO2 + B2O3

B2O3 + CoO ⎯⎯→ Co(BO2)2

(iv) AIN + 3H2O ⎯⎯→ AI(OH)3 + NH3

(v) Nitric acid whether dilute or concentrated hardly affects aluminium at all. Aluminium is rendered passive.
A thin film of Al2O3 is formed on the surface of the metal.
8. Refer text and chemical bonding sheet.

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9. (A) Refer text.
ether
3NaBH4 + 4BF3 ⎯⎯ ⎯→ 3NaBF4 + 2B 2H6

100
B 2H6 + 2NH3 ⎯⎯⎯→ B 2H6 .2NH3
tempt .

200 o C
B 2H6 .2NH3 ⎯⎯ ⎯
⎯→ B 3N3H 6 + H 2
(C) Borax from Boron (in two steps)

2B + 6HNO 3 (or H2SO 4 ) ⎯⎯→ 2H3BO 3 + 6NO 2

4H3BO3 + Na 2CO 3 ⎯⎯→ Na 2B 4O 7 + 6H2O + CO 2

Group 14th
10. Ultra pure elemental silicon is used for making semiconductors.
Δ
SiCl 4 (pure ) + 2H2 (g) ⎯⎯→ Si(s) + 4HCl (g)
Δ
SiHCl3 (s) + H2 (g) ⎯⎯→ Si(s) + 3HCl(g)

675 K
SiH 4 (g) ⎯⎯ ⎯⎯→ Si(s) + 2H2 (g)
Pyrolysis

11. (A) SnO + 2HNO3 ⎯→ Sn(NO3)2 + H2O

Δ
(B) Sn + 2Cl2 ⎯⎯→ SnCl4
Δ
(C) 2PbS + 3O2 ⎯⎯→ 2PbO + 2SO2 ; PbS + 2O2 ⎯→ PbSO4

12. Refer text. 13. Refer text.

14. Inert pair effect is due to the ineffectively shielding of the s-electrons of the valence shell by the d-and
f-electrons of the inner shells. IV II
P bO2 + 4HCl ⎯⎯→ P bCl2 + Cl2
15. They violently react with alkali metals according to following reactions.

CCl 4 (A ) + 4Na(s) ⎯⎯→ 4NaCl(s) + C(s)

IV II
16. ; P bO2 + SO2 ⎯⎯→ P bSO 4

17. CaSO4 formed with H2SO4 forms a protective layer over lime stone and then reaction slowly ceases and stop.
But CaCl2 is soluble.
18. PbCl4 is less stable than SnCl4 due to more effective inert pair effect in lead. Pb–Cl bond length is more then
that of Sn–Cl.
19. Due to bigger atomic size of silicon, its reluctance for pp – pp bond does not allow to form graphite like
structure.
20. Low electronegativity and bigger size, Si does not have tendency to form pπ-pπ bonds like carbon.
21. Refer text.

COOH
P4 O10
22. (a) Refer text. (b) CH2 ⎯⎯ ⎯
⎯→ C3O2 (Carbon suboxide) + 2H2O (c) Refer text.
Δ
COOH

23. Lead dissolves in water containing dissolved air due to the formation of lead hydroxide (a poisonous substance).
This solvent action of water is called plumbo solvency. It increases if water contains nitrates, ammonium
salts and organic acids, and decreases if water contains phosphates, sulphates, bicarbonates and carbonates.
24. (A) CaC2 (B) CO (C) CaCN2 (D) CaCO3 .

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25. Carbonates evolve CO2 with phenol but bicarbonate do not.
Soluble carbonates give pink colour with phenolphthalein but soluble bicarbonates do not.

Group 15th
26. (a) Refer text
(b) 2NO + O2 ⎯→ 2NO2 (Brown)
(c) Copper is placed below hydrogen in electrochemical series and does not liberate H2 from acid. However,
HNO3 oxidises copper due to its strong oxidant nature.
3Cu + 8HNO3 (dil.) ⎯→ 3 Cu(NO3)2 + 4H2O + 2NO
Δ Δ
(d) Pb(NO 3 )2 ⎯⎯→ N2O 4 ⎯⎯→ NO 2 ↑ (Brown)

27. Refer chemical bonding sheet. 28. Due to its high heat of vaporisation.

29. Refer text. 30. Refer text. 31. Refer text.

800 −1000 º C
32. (A) CaO + 3C ⎯⎯ ⎯⎯ ⎯ ⎯→ CaC 2 + CO ↑

CaC 2 + N2 ⎯⎯→ CaCN2 + C

CaCN2 + 3H2O ⎯⎯→ CaCO 3 + 2NH3

(B) 2Ca3 (PO4)2 + 6SiO2 ⎯→ 6CaSiO3 + P4O10

P4O10 + 6H2O ⎯→ 4H3PO4

Δ Δ
(C) NaH2PO 4 ⎯⎯→ NaPO 3 + H2O (D) Refer text (E) 3H3PO 2 ⎯⎯→ PH3 + 2H3PO 3

33. 2Cu + 8NH3 + O2 + 2H2O ⎯⎯→ 2[Cu(NH3)4 (OH)2 ; O2 is removed in the form of cupra-ammonium hydroxide
complex.

35. N2O4(A) NO+ (acid) + NO3– (base)

ZnCl2 + 2N2O4(A) ⎯⎯→ Zn(NO3)2 + 2NOCl.

36. (A) P4O6 ; (B) PH3 ; (C) H3PO4 ; (D) Cu3P2

The given changes are :
P + 3O2 (s) (air) ⎯⎯→ P4O6 (Garlic odour) ; P4O6 + 6H2O (hot) ⎯⎯→ 3H3PO4 + PH3
(A) (C) (B)
(B) is PH3 having rotten fish smell and neutral towards litmus
3CuSO4 + 2PH3 ⎯⎯→ Cu3P2 + 3H2SO4 (Cu3P2 is black substance insoluble in water)

37. H3PO3 contains one P–H bond and hence acts as a reducing agent but H3PO4 does not contain a P–H bond.
Group 16th
38. Oxygen has no d-orbitals while other have d-orbitals. Therefore, the paired electrons can be made unpaired
by exciting electrons to d-orbitals.

39. SO2 + 2OH- SO42- + 2H+ + 2 e : reaction proceeds in forward direction as OH- concentration increases

SO2 + 2H2O SO42- + 4H+ + 2 e : as H+ concentration increases the reaction proceeds in backward
direction.
40. H2O = 104.50 ; H2S = 92.50 ; H2Se = 910
41. H2O ; intermolecular hydrogen bonding.
42. Mercury is a mobile liquid but in presence of ozone it loses its mobility due to the formation of mercury
suboxide and starts sticking to the glass. This is called as tailing of mercury. 2Hg + O3 → Hg2O + O2 .
43. (A) SO2Cl2 ; (B) H2SO4 ; (C) HCl ; (D) K2SO4 ; (E) KCl

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44. (A) Na2SO3 ; (B) Cr2(SO4)3 ; (C) KMnO4 ; (D) Na2SO4
45. (a) H2O < SiO2 < CO2 < N2O5 < SO3 (b) H2Te < H2Se < H2S < H2O
46. On heating, S8 rings are broken and long chain polymers are formed up to 2000C. Thus due to polymerisation,
liquid becomes viscous but beyond 2000C long chains are broken into short chains and ultimately S2 molecules
are formed in the vapour phase, so viscosity of liquid decreases.

0
47. repulsions ∴ B.L 1.48 A

48. H2SO4 acts as strong oxidising agent and, therefore, following reaction takes place.
H2S + H2SO4 SO2 + S + 2H2O

49. (a) (b)

S
(c) (d) H O S O H
O
55. (i) I2 + 5O3 + H2O → 2HIO3 + 5O2
(ii) 2NaHS +4NaHSO3 3Na2S2O3 + 3H2O
(iii) (NH4)2S2O8 + 2H2O + MnSO4 (NH4)2SO4 + MnO2 + 2H2SO4
(iv) Sb2S3 + 6HCl 2SbCl3 + 3H2S
(v) 2Hg2Cl2 + SO2 + 4HCl 4HgCl2 + 2H2O + S

(vi) CaS + H2O + CO2 CaCO3 + H2S

51. (A) Refer text (B) Refer text (C) Refer text (D) Refer text.

Group 17th →
↑
⎯⎯→
52. (i) 2NaΙO3 + 5NaHSO3 3 NaHSO4 + 2Na2SO4 + H2O + Ι2

(ii) 3Cl2 + 6 NaOH(conc) ⎯⎯⎯→ 5 NaCl + NaClO3 + 3H2O

Hot

(iii) Cl2 + 2KOH (aq) ⎯⎯→ KCl + KClO + H2O

(iv) 2FeBr2 + 3Cl2 ⎯⎯→ 2FeCl3 + 2Br2
(v) Ι2 + 10HNO3 ⎯⎯→ 2HΙO3 + 10NO2 + 4H2O
(vi) Ca(OH)2 + Cl2 ⎯⎯→ Ca(OCl)Cl + H2O
(vii) 2KΙ + MnO2 + 3H2SO4 ⎯⎯→ 2KHSO4 + MnSO4 + 2H2O + Ι2
(viii) Cl2 + Na2SO3 + H2O ⎯⎯→ 2HCl + Na2 SO4
acidified
(ix) SnCl2 + 2HCl + Ι2 ⎯⎯ ⎯⎯→ SnCl4 + 2HΙ

53. (i) The standard reduction potential of fluorine is maximum.

+ e– ⎯⎯→
Thus, it cannot be oxidised by any other reagent. F– ion is very stable due to small size and high
electronegativity of fluorine atom.
(ii) In anhydrous state, HCl is a covalent molecule. In aqueous solution, HCl combines with water
molecule to form H3O+ and Cl– ions.
HCl + H2O ⎯⎯→ H3O+ + Cl–

(iii) Halogens act as strong oxidising agents because they have high tendency to accept electron, i.e.,
they have high electron affinity values. Their reduction potentials are high (positive) and decrease from F to Ι.
Thus, oxidising nature decreases from F to Ι.

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(iv) Chlorine bleaching action is due to oxidation while that of sulphur dioxide is due to reduction. Hence,
the substance bleached by SO2 is reoxidised by the oxygen of the air to its original state.
(v) Ι2 is a covalent molecule. thus, its solubility is less in polar solvent, i.e., water. Potassium iodide
combines with iodine and forms a polyhalide which is an ionic compound. Being ionic, KΙ3 is more
soluble.
KΙ + Ι2 ⎯⎯→ KΙ3 (K+ Ι3–)
(vi) Hydrofluoric acid exists as dimeric molecule (H2 F2) due to hydrogen bonding. It, thus, exhibits
dibasic nature and forms two series of salts, KHF2 as [K+ and F– --- H –– F] and KF[K+ and F–]. HCl
and HBr exists as monomeric molecules as hydrogen bonding is not present.
(vii) Ι– ions is a strong reducing agent. Iodide thus reduces ferric into ferrous, Cl– ion is a weak reducing
agent and does not reduce Fe3+ to Fe2+ .

(viii) No d-orbitals are present in fluorine while d-orbitals are present in other halogens. The formation of
X3– ions involves sp3 d-hybrizaion.
(ix) HF attacks glass bottles. The sodium and potassium silicates are converted into flurosilicates
Na2 SiO3 + 6HF ⎯⎯→ Na2 SiF6 + 3H2O
(x) The weakest acidic nature of HF is due to following three factors :
(i) Strong H–F bond as the dissociation energy is high.
(ii) Large heat of dehydration dues to hydrogen bonding.
(iii) Low value of electron affinity.
54. (i) HClO < HClO2 < HClO3 < HClO4 (ii) HClO < HClO2 < HClO3 < HClO4
(iii) HClO4 < HClO3 < HClO2 < HClO (iv) F– < Cl– < Br – < Ι–
(v) HI < Ι2 < ΙCl < HΙO4 (vi) HOI < HOBr < HOCl < HOF
(vii) Ι2 < Br2 < Cl2 < F2 (viii) HF < HCl < HBr < HΙ
(ix) Ι < Br < Cl < F (x) Ι < Br < F < Cl
55. HI is a strong reducing agent and, therefore, reduces H2SO4 to SO2 and itself get oxidised to Ι2.
3NaΙ + H3PO4 ⎯⎯→ K3PO4 + HΙ

56. 4HΙ + O2 (air) ⎯ ⎯ ⎯ ⎯ ⎯→ 2H2O + Ι2

on s tan ding

liberation of Ι2 turns HΙ solution brown.

57. 2F2 + 2NaOH ⎯⎯→ OF2 + 2NaF + H2O 58. Refer text.

Group 18th
59. (i) Zero group elements have complete electronic configuration of their outer shells, i.e. ns2 np6 (except
helium which has 1s2), hence they do not have any tendency either to lose or accept electron/
electrons or share electrons with other atoms.
(ii) Xe has relatively lower ionisation energy among inert gases and thus the outermost shell electrons
of Xe are excited to d-subshell and thereby showing unpaired electronic structure. Therefore Xe
shows covalent bonding with fluorine showing sharing of electron pair.
(iii) Van der Waal’s forces of attraction among molecules increase with the increase of atomic masses.
Thus, higher energy is required to separate these molecules as to get gaseous state. Hence, the
boiling points increase with increase of atomic masses.
(iv) Unlike nitrogen, helium is not soluble in blood even under high pressure.
(v) The size of cavities formed during crystallisation of quinol is more than the size of helium and neon
atoms.
60. XeF4 : sp3 d2 (Square planar structure)
XeF6 : sp3d3 (Distorted octahedral)
XeOF4 : sp3d2 (Square pyramidal structure)
XeOF2 : sp3d (T-shaped structure)
XeO3 : sp3 (Trigonal pyramidal structure)
XeO4 : sp3 (Tetrahedral structure)

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F
Ione pair ..
Xe O
Ione pair ..
F
T-shaped
(sp3d)

61. Refer text. 62. Refer text. 63. (a) XeF4 (b) XeF2 (c) XeO3

64. XeO3 + 6H+ + 9Ι– ⎯⎯→ Xe + 3H2O + 3Ι3– ; XeO3 + 6H+ + 6Ι– Xe + 3H2O + 3Ι2

65. 2XeF6 + 3SiO2 3SiF4 + 2XeO3

66. 2XeF6 + 16OH– XeO64– + Xe + O2 + 12F– + 8H2O

67. XeF2 > XeF4 > XeF6
2.00 Å 1.94 Å 1.89 Å (due to increse in number of fluorine atoms on xenon atom)

⎯⎯→
EXERCISE - 3
A Objective :
Group 13th
1. A 2. C 3. A 4. A 5. B 6. C

Group 14th
7. B 8. A 9. C 10. A 11. D 12. D
Group 15th

13. B 14. C 15. A 16. A 17. C 18. C 19. A

20. C 21. C 22. C 23. D 24. C 25. ACD 26. B
27. C

Group 16th
28. B 29. B 30. D 31. D 32. A 33. C 34. A
35. B 36. C 37. D 38. A 39. C

Group 17h & 18th

40. B 41. D 42. D 43. B 44. A 45. D 46. B
47. C 48. A 49. A 50. A 51. C 52. B

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SECTION : (B)
Group 13th
1. AlF3 dissolves in KF due to the formation of complex K3[AlF6]
AlF3 + 3KF ⎯⎯→ [AlF6]3– + 3K+
Anhydrous HF being weak acid does not dissociate to appreciable extent and so AlF3 does not form H[AlF4].
Because BF3 is more acidic than AlF3, so AlF3 is precipitated when BF3 is added in K3[AlF6].
K3 [AlF6] + 3 BF3 ⎯⎯→ 3 K [BF4] (soluble) + AlF3 (s)

2. Anhydrous AlCl3 is electron deficient. Therefore, moer soluble in diethyl ether because the oxygen atom of
ether donates a pair of electrons to vacant p-orbital on the Al atom forming a co-ordinate bond, hydrate AlCl3
is not electron deficient since H2O has already donated a pair of electrons to it.

3. A: Bi3+ + H2O → BiO+ + 2H+ thus (Q) and (S) B: Al + H3O+ → Al(OH)3 thus (R)

2Si O 44− + 2H+ → Si2 B4 O 27 − ⎯⎯→

+
C: thus (R) D: ⎯ B(OH)3
H

B4 O 27 − ⎯⎯⎯→ B(OH)3 Thus, (Q) and (R)

H2 O

4. (i) Al4C3 + H2O ⎯⎯→ 4 Al(OH)3 + 3CH4 ↑ (ii) CaNCN + 3H2O ⎯⎯→ CaCO3 ↓ + NH3 ↑

(iii) 4BF3 + 6H2O ⎯⎯→ H3BO3 + 3 [BF4]– + 3H3O+ (iv) NCl3 + 3H2O ⎯⎯→ NH3 + 3HOCl

(v) 2XeF4 + 3H2O ⎯⎯→ Xe + XeO3 + F2 + 6HF

Δ
5. Na 2B 4O 7 .10H2 O ⎯⎯→ Na 2B 4O 7 ; Na 2B 4 O 7 + 2HCl ⎯⎯→ 2NaCl + H2B 4 O 7 (tetra boric acid)

red hot
H2B 4 O 7 + 5H2 O ⎯⎯→ 4H3BO3 2H3BO3 ⎯⎯ ⎯ ⎯→ B 2O 3 + 3H2O
;
Boric acid Boric anhydride

−
6−
Fusion
B 2O 3 + 3Mg ⎯⎯ ⎯⎯→ 2B + 3MgO ; ↓
Reaction 7with HCl : B2H6 + HCl ⎯→ B2H5Cl + H2
⎯⎯→
O 2

Structure of B2H6 :

H................ B ................ H is hydrogen bridge i.e, 3 centre two electron bond

6. X = BF3 ; Y = B2H6
Δ
7. Na2 B4 O7 . 4H2O ⎯⎯ ⎯ ⎯ ⎯⎯→ B2O3 + 2Na+ + BO2– ; B2O3 + CoO Co(BO2)2
− 10 H2O
8. A (both assertion & reason are correct and explanation also correct)
9. A = Na2CO3 ; B = H2SO4 or HCl

10. Al2S3 + 6H2O ⎯⎯→ 2 Al(OH)3 + 3H2 S 11. 2Al + 2NaOH + 2H2O ⎯⎯→ 2NaAlO2 + 3H2

12. (A) Ca2B6O11.5H2O ; (B) CaCO3 ; (C) Na2B4O7 ; (D) NaBO2 ; (E) B2O3 ; (F) Co(BO2)2
13. Two electron three centre bond
14. Protective layer of Al2O3 is formed over Al metal.
15. X = AlCl3 16. False 17. X = Na2B4O7

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Group-14
18. In trimethyl silane, N-atom forms 3 Si-N σ bonds and lone pair of electron occupy a p-orbital which forms
pπ-dπ bond (a bond formed between full p-and empty d-orbital). pπ-dπ bonding is not possible in (CH3)3N
because N-does not contain d-orbitals and so molecule is pyramidal.

Si(CH3)3

(CH3)3Si Si(CH3)3

pπ-πd bonding in (SiH3)3N (CH3)3N (D)

19. (i) 3SiCl4(V) + 4Al(molten) ⎯→ 4AlCl3 + 3Si

Cu powder
(ii) (a) 3SiCl4 + 4Al ⎯→ 4AlCl3 + 3Si (b) Si + 2CH3Cl ⎯⎯⎯ ⎯⎯→ (CH ) SiCl
570 3 2 2

CH3
|
(c) OH–
(CH3)2 SiCl2 ⎯⎯⎯→ HO – Si – OH
|
CH3

CH3 CH3 CH3

|
(d) polymerisa tion
nHO – Si – OH ⎯ ⎯ ⎯ ⎯ ⎯⎯→ HO Si O Si O
|
CH3 CH3 CH3 n
linear silicone
(thermoplastic polymer)

(iii) (a) SiCl4 + 4H2O ⎯→ H4SiO4 (ortho silicic acid ) + 4HCl

Δ
(b) H4SiO4 ⎯⎯→ SiO2 + 2H2O (c) SiO2 + Na2CO3 ⎯→ Na2SiO3 + H2O
20. (i) SnCl4 + 4C2H5Cl + 8Na ⎯→ (C2H5)4Sn + 8NaCl (ii) C + 4HNO3 ⎯→ CO2 + 4NO2 + 2H2O
21. Diamond has giant three dimensional polymeric structure in which each carbon is sp3 hybridized and linked
to four carbon atoms. This structure makes diamond as hardest. On account of small radii of carbon atoms,
the various atoms are closely packed in the crystal lattice. Graphite possesses layer structure in which each
carbon atoms is sp2 hybridized. There is wide separation between various layers. One layer can slide easily
on the other. This makes graphite soft in nature.
R R R
| | |
22. (i) RSiCl3 + 3H2O ⎯⎯→ RSi(OH)3 ⎯⎯Polymerisation
⎯ ⎯ ⎯⎯→ HO − Si − O − Si − O − Si − OH
of 8 moles – 3H 2O | | |
OH OH OH

R R
| |
− O − Si − O − Si − O − Si − O −
| | | Further polymerisation
O O O of two moles
| | | –H2O
− O − Si − O − Si − O − Si − O −
| | |
R R R

Cross linked silicon

H2O Dimerisation
(ii) R 3 SiCl ⎯⎯⎯→ R 3 SiOH ⎯⎯ ⎯ ⎯ ⎯→ R 3Si − O − SiR 3
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Group 15 th

23. Refer chemical bonding sheet. 24. CaNCN + 3H2O ⎯→ CaCO3 + 2NH3
25. (A) NaH2PO2 ; (B) H3PO3 ; (C) H3PO4 ; (D) Hg2Cl2 ; (E) Hg

26. Refer chemical bonding sheet.

27. HNO2 + 2H2SO3 + H2O ⎯→ NH2OH + 2H2SO4
(A) (B) (C) (D)
28. Ca5(PO4)3F + 7H3PO4 + 5H2O ⎯→ 5Ca(H2PO4)2.H2O + HF
29. (i) P4O10 + 6PCl5 ⎯→ 10POCl3 (ii) 2NH3 + NaOCl ⎯→ NH2.NH2 + NaCl + H2O
30. 2Au + 3HNO3 + 11HCl ⎯→ 2HAuCl4 + 3NOCl + 6H2O
31. Refer text.
32. Single bonds = 12 and double bonds = 4
33. Refer chemical bonding and s-block sheet.
34. (A) PH4I ; (B) PH3; (C) KI; (D) P2O5; (E) Cu2I2
35. P4 + 3NaOH + 3H2O ⎯→ 3NaH2PO2 + PH3 ↑
36. (A) (NH4)2 Cr2O7 ; (B) Cr2O3 ; (C) N2 ; (D) Mg3N2 ; (E) NH3
37. (i) 2P + 3I2 + 3H2O ⎯→ H3PO3 +3HI
(ii) 7Cu + 20HNO3 ⎯→ 7Cu(NO3)2 + 4NO + 2NO2 + 10H2O
38. Four
39. (i) 2NH3 + 2KMnO4 ⎯→ 2KOH + 2MnO2 + N2 + 2H2O
(ii) P4 + 20HNO3 ⎯→ 4H3PO4 + 20NO2 + 4H2O (iii) Na2CO3 + NO + NO2 ⎯→ 2NaNO2 + CO2
40. 4Zn + 7NaOH + NaNO3 ⎯→ NH3 + 4Na2ZnO2 + 2H2O
3CaO + 8P + 9H2O ⎯→ 3Ca(H2PO2)2 + 2PH3

Group 16th
41. Colloidal sulphur is formed :
Na2S2O3 + 2H+ ⎯→ 2Na+ + H2SO3 + S ↓ (Colloidal sulphur)

42. The SO2 is obtained by buring sulphur in air as,

S + O2 ⎯→ SO2
The SO2 so obtained is impure. Dust present in sulphur is removed by allowing the gas to expand, when
some dust settles down by passage through electrostatic precipitator and finally washing with water. The
moistened gas is now treated with conc. H2SO4 to dry it which is ketp in use until its concentration falls to
94%.The SO2 so obtained then catalytically converted to SO3 which is absorbed in conc. H2SO4 to form
H2S2O7 .
Pt. asbestors
2SO2 + O2 ⎯⎯ ⎯ ⎯ ⎯⎯ ⎯⎯⎯ ⎯ ⎯→ 2SO3
Finely divided Pt deposited on MgSO 4
or Fe 2O3 and CuO
or Pt − silica gel

43. SO2 + PCl5 ⎯→ SOCl2 + POCl3

FeCl3. 6H2O + 6SOCl2 ⎯→ FeCl3 + 6SO2 + 12HCl
FeCl3. 6H2O + 6CH3C(OCH3)2 . CH3 ⎯→ FeCl3 + 12CH3OH + 6CH3COCH3
44. X = SO2
45. (NH4)2 S2 O8 + 2H2O + MnSO4 ⎯⎯→ (NH4)2 SO4 + MnO2 + 2H2SO4

46. SO3 > N2O5 > CO2 > SiO2 > H2O

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47. 2CuSO4 + 2KCN + SO2 + 2H2O ⎯⎯→ 2CuCNS + K2SO4 + 2H2SO4

(ii) SO2 (moist) + 2H2S ⎯⎯→ H2O + 3S ↓

Δ
(iii) 4NaCl + 2SO2 + O2 + 2H2O ⎯⎯→ 2Na2SO4 + 4HCl.
(iv) 2FeCl3 + H2S 2FeCl2 + 2HCl + S

Group 17th & 18th

48. Xe F4 + 6H2O 2Xe + XeO3 + 12HF + 3/2 O2

Disproportionation reaction (+ 4 to + 6 in XeO3 and 0 in Xe)

49. 2KΙ(aq.) + Cl2 ⎯→ 2KCl(aq.) + Ι2

In the reaction Cl2 oxidises iodide ion (–1 oxidation state) to Ι2 (0 oxidation state). Cl2 has higher reduction
potential then Ι2 and thus oxidises iodide to iodine getting itself reduced to chloride ion. Similarly,
2KΙ + X2 ⎯→ 2KX + Ι2 ; (X = Cl, Br, F)

50. Cl2 bleaches coloured material by oxidation and thus bleaching is permanent.
Cl2 + H2O ⎯→ 2HCl + [O]
Coloured material + [O] ⎯→ Colourless
On the other hand beaching by SO2 is by reduction and thus temporary because colourless articles are
further oxidised by air.
SO2 + 2H2O ⎯→ 2H2SO4 + 2[H]

51. Ι2 + SO2 + H2O 52. Ι2

53. (A) Br2 ; (B) NaBr ; (C) NaBrO3

54. 2KI + Cl2 ⎯→ 2KCI + l2 ; (Cl2 placed below I2 and thus replaces I2 from its solution)
⎯⎯→
2KCIO3 (Oxidant) + I2 (Reductant) ⎯→ 2KIO3 +⎯
⎯⎯→
⎯→
Cl2

55. False 56. Cl2 , H2O 57. NaΙO3

58. (X) = CaOCl2 59. HClO < HClO2 < HClO3 < HClO4

60. HF < HCl < HBr < HΙ 61. (X) CaOCl2 . 62. KΙ3

63. HΙ < Ι2 < ΙCl < HΙO4 64. 3Cl2 + 6KOH 5KCl + KClO3 + 3H2O.

65. H2SO4 being strong oxidising agent oxidises HΙ to Ι2.

66. Soluble 67. 2NaIO3 + 5NaHSO3 ⎯⎯→ 3 NaHSO4 + 2Na2SO4 + H2O + Ι2

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