IIT-JEE
INORGANIC PAPER Q.1
CHEMISTRY
P. JOY
Reactions of aluminium with 1. O2
2. N2
3. Cl2
4. Cr2O3
5. Mn3O4
6. HCl
7. H2SO4(Dil.)
8. H2SO4 (Conc.)
9. HNO3
10. NaOH
11. AlCl3 Q.2
Reactions of Al(OH)3 with 1. Acid 2. NaOH 3. Heating Below 450ºC 4. Heating above 450ºC
Q.3
What is the general formula of alum.
Q.4
How many water molecules act as ligands about mono and trivalent metal cations.
Q.5
Which unipositive cations do form alum.
Q.6
Which tripositive cations do form alum.
Q.7
How do structures of all alums differ.
Q.8
Which alkali metal cation does not form alum.
Q.9
What happens when alums are heated.
Q.10
What are the major uses of alum.
Q.11
What is the nature of aqueous solution of alums.
Q.12
How are alums prepared.
Q.13
What are pseudo alums.
Q.14
Are pseudo alums isomorphous to alums.
Q.15
What is feather alum or hair salt.
Q.16
How can you prove that Al(OH)3 is amphoteric in nature.
Q.17
How Al(OH)3 ppt is different than Zn(OH)2 ppt
Q.18
How Al2Cl6 is prepared.
Q.19
How Al2O3 can be converted into Al2Cl6
Q.20
In which conditions does Al2Cl6 exist.
Q.21
What happens when Al2Cl6 dimer is added to water.
Q.22
Are the bonding states of Al2Cl6 in vapour phase and in aqueous phase are different.
Q.23
What is the nature of AlCl3 in aqueous state.
Q.24
Does AlCl3 on heating melts.
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P. JOY
CHEMISTRY
Q.25
Why is it difficult keep AlCl3 dry
Q.26
Comment on stability of AlCl
Q.27
What happens when AlCl3 reacted with Cl
Q.28
What happens when Al2Cl6 is reacted with LiH
Q.29
Which is the most stable compound of aluminium.
Q.30
What are the different forms of alumina.
Q.31
What is corundum.
Q.32
What is thermite reaction.
Q.33
What happens when AlCl3 vapours are passed over fused Al2O3 at 1000ºC.
Q.34
Which form of alumina is corundum.
Q.35
Which form of alumina is acid soluble.
Q.36
Why 'C' shows highest properties of catenation ?
Q.37
Which element of fourth group donot show allotropy ?
Q.38
Which allotrope of carbon is thermodynamically more stable ?
Q.39
Which of two has a dipole moment CO & CO2 ?
Q.40
Which element of group IV does not show allotropy ?
Q.41
Why graphite is good conductor of electricity ?
Q.42
Which is thermodynamically most stable ? Graphite, Diamond or fullerene ?
Q.43
Which element occurs in both very hard and very soft form ?
Q.44
In which form does silicon show its allotropy ?
Q.45
What are three crystalline modifications of tin ?
Q.46
How various allotropes of tin are related to temperature ?
Q.47
What is tin disease, tin pest or tin plague ?
Q.48
What is tin cry ?
Q.49
Which element of IV group has maximum number of Isotopes ?
Q.50
Which allotrope of carbon is insoluble solvent ?
Q.51
What are the oxides of carbon ?
Q.52
Which acid anhydride is CO2 ?
Q.53
Which acid anhydride is CO ?
Q.54
How fullerence was originally prepared ?
Q.55
Can fullerence be prepared by evaporation of graphite by electric arc ?
Q.56
How many 'C' atoms are there normally in fullerence ?
Q.57
What is the colour of C60 in toluene ?
Q.58
What is the colour of C70 in Toluene ?
-ions
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IIT-JEE
INORGANIC PAPER
CHEMISTRY
P. JOY
Q.59
What is the shape of C60 ?
Q.60
Which acid anhydride is carbon sesquioxide C3O2 ?
Q.61
Which oxide of IV group is not solid ?
Q.62
Which monoxide of IV group does not exist ?
Q.63
Which monoxide of IV group is neutral ?
Q.64
What is the nature of IV group monoxides ?
Q.65
Which IV group oxides are network solids ?
Q.66
Why bicarbonates are alkaline in nature although they has H+ ?
Q.67
How calcium cyanamide can be prepared from CaC2 ?
Q.68
What happens when calcium cyanamide is hydrolysed ?
Q.69
What happens when calcium cyanamide is heated with Coke & NaCl
Q.70
What happens when K4Fe(CN)6 is heated strongly ?
Q.71
What happens when KCN & dil. H2SO4 reacts ?
Q.72
What is the nature of aqueous solution of KCN ?
Q.73
What happens when HCN is oxidised by O2, Ag, Cu2+ ?
Q.74
Why (CN)2 is pseudohalide ?
Q.75
Why CO2 is molecule but SiO2 is 3D network solid ?
Q.76
What are the nature of CO2, SiO2, GeO2, SnO2, PbO2 ?
Q.77
What happens when Pb(NO3)2 is strongly heated ?
Q.78
Which dioxide of nonmetal C, S, N or Cl does not act as reducing agent ?
Q.79
What happens when graphite is heated with KMnO4 ?
Q.80
What is the general formula of organosilicone ?
Q.81
What happens when dialkyldichloro silanes of diaryl dichlorosilanes are subjected to hydrolysis ?
Q.82
What is the hybridisation state of Si in SiO2 ?
Q.83
What is the purest form of silicon ?
Q.84
What happens when SiO2 is reacted (heated) with alkalis and alkali metal carbonates ?
Q.85
What happens when SiO2 is reacted with following ? (a) KOH
(b) CaCO3
(c) KNO3
Q.86
What type of glass is K2O.PbO.4SiO2 ?
Q.87
What is the definition of glass ?
Q.88
Why HF acid is stored in plastic bottles and not glass bottles ?
Q.89
Which compound is formed when glass reacts with HF ?
Q.90
What is the formula of soda glass ?
Q.91
What is the formula of water glass
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(d) HF
(e) Coke
PAGE # 3
INORGANIC PAPER
IIT-JEE
CHEMISTRY
P. JOY
Q.92
What is silica Garden ?
Q.93
What are silanes and germanes ? What are their general formula.
Q.94
What happens when mixture of silane and H2 is bubbled through water ?
Q.95
What happens when Si is fused with NaOH in air ?
Q.96
Which acid is used for etching glass ?
Q.97
How silanes are different than alkanes ?
Q.98
KNO3 on heating produce KNO2 and O2 but what happens when KNO3 is heated with SiO2 ?
Q.99
Name an acid which dissolves silica ?
Q.100
What are corundum and carborundum ?
Q.101
What pseudo solids ?
Q.102
Which allotrope of Si is isomorphous with carbon ?
Q.103
What is Na2SiO3. CaSiO3.4SiO2 ?
Q.104
What do you call K2O.CaO.4SiO2 ?
Q.105
Which type of anions are present in pyrex glass ?
Q.106
Which type of glass are prisms and lenses are made up of ?
Q.107
What is Crookes glass ? What is its speciality ? Which metal compound is present in it ?
Q.108
Which type of glass has lane thermal expansion ?
Q.109
How borosilicate glass are obtained ?
Q.110
Why trimethyl amine is pyramidal but trisilyl amine is planar ?
Q.111
Which of two is more basic N(CH3)3 or N(SiH3)3 ?
Q.112
How the name silicone is derived for the polymer R2SiO ?
Q.113
Why CO2 is a gas while SiO2 is a solid ?
Q.114
Why CCl4 does not hydrolyse but SiCl4 ?
Q.115
How tin is purified ?
Q.116
Which oxide of tin (SnO, SnO2) is/are amphoteric ?
Q.117
Why heating of SnC2O4 does not yield SnO instead of SnO2 ?
Q.118
What happens when SnO2 is reacted with (i) H2SO4 (ii) NaOH
Q.119
What happens when SnCl2.2H2O crystals are heated ?
Q.120
Which of the two SnCl2 or SnCl4 is a liq. at room temperature ?
Q.121
What is butter of Sn ? What is its major use.
Q.122
What are the addition compounds of SnCl2 & NH3 ?
Q.123
What is the double salt of SnCl4 with NH3 ?
Q.124
How calamel is produced by SnCl2 ?
Q.125
Which tin compound is used in tooth paste to help tooth decay ?
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INORGANIC PAPER
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CHEMISTRY
P. JOY
Q.126
Which property of tin makes it useful for tinning of utensils ?
Q.127
What happens when AuCl3 is treated with SnCl2 ?
Q.128
How PURPLE OF CASIUS is formed ?
Q.129
What happens when butter of tin is hydrolysed with excess of water ?
Q.130
What happens when tin metal is reacted with conc. HNO3 ?
Q.131
Which tin halide out of SnCl4, SnBr4, SnI4 is coloured ?
Q.132
How Tin (II) fluoride is obtained ?
Q.133
Why Pb715 has higher I.E. than Sn707 ?
Q.134
What are various oxides of Pb ?
Q.135
Why do PbCl4 acts as strong oxidising agent ?
Q.136
SiF62 exist but not CF62 explain why ?
Q.137
What is the order of ease of catenation ?
Q.138
How many allotropes of Sn exist ?
Q.139
Why PbCl2 is ionic where is PbCl4 is covalent.
Q.140
How do following properties vary ? (a) Atomic radii (b) Melting point and boiling point (c) Density (d) I.E. (e) O.S.
Q.141
Why Group V elements have much higher I.E. than group IV elements.
Q.142
Which two elements of Group V are metalloids ?
Q.143
Why Bi has low melting point ?
Q.144
What are the important oxidation states exhibited by Group V elements ?
Q.145
Give an example of each of compound in which 'N' is having oxidation states 3 to +5
Q.146
Why Group V elements have poor catenation property ?
Q.147
What is the structure of hydrazoic acid ?
Q.148
Which elements of Group V do not show allotropy ?
Q.149
What are the allotropes of phosphorous ?
Q.150
What are the allotropes of Arsenic ?
Q.151
What are the allotropes of Antimony ?
Q.152
Which element of group V has tendency to form pπ pπ bond ?
Q.153
Why N2 is less reactive than other members of its family ?
Q.154
What is the formula of elemental state of group V elements.
Q.155
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CHEMISTRY
P. JOY
Q.156
What happens when Ca3N2 and Ca3P2 are added to water ?
Q.157
What happens when Zn3As2, Zn3Sb2, Zn3Bi2 are added to water ?
Q.158
Which compound is formed when NH3 gas is passed into NaOCl solution.
Q.159
Arrange following hydrides in increasing bond angle NH3, PH3, AsH3, SbH3
Q.160
Arrange following hydrides in the increasing order of their thermal stability NH3, PH3, AsH3, SbH3, BiH3
Q.161
Which hydride of group V is strongest reducing agent ?
Q.162
Which V group hydride is the weakest reducing agent.
Q.163
On moving down the group generally b.p. of group V hydrides increases except NH3. Why NH3 has higher b.p. than PH3 and AsH3 ?
Q.164
What is order of Lewis base character of V group metal hydrides.
Q.165
Which trihalide of group V elements is not covalent but ionic ?
Q.166
What is the shape of group V trihalides ?
Q.167
Write hydrolysis product of following trihalides PCl3, AsCl3, SbCl3, BiCl3
Q.168
Why nitrogen trihalides cannot be hydrolysed ?
Q.169
Do fifth group trihalides work as Lewis acid ?
Q.170
Which fifth group element does not form pentahalide ?
Q.171
Which of the two trihalide or pentahalide of fifth group is thermally more stable ?
Q.172
Do all pentahalides act as Lewis acids ?
Q.173
What are the formula of PCl5 in gaseous state and in solid state ?
Q.174
Draw the structure of PCl5 in solid state.
Q.175
How white phosphorous is obtained from calcium phosphate ?
Q.176
Which form of phosphorous has garlic smell ?
Q.177
Which form of phosphorous is toxic.
Q.178
Which form of phosphorous is soluble in CS2 but insoluble in water ?
Q.179
What is the structure of phosphorous in solid and vapour state ?
Q.180
Which form of phosphorous spontaneously burn in air with green flame ?
Q.181
What happens when (a) White phosphorous is heated upto 540 K in inert atmosphere. (b) White phosphorous is heated upto 450 K at 1200 atm pressure.
Q.182
What is the structure of Red phosphorous.
Q.183
Which form of phosphorous is insoluble in both water and CS2 ?
Q.184
What happenes when phosphorous combine with metals like Ca and Mg, Na and K.
Q.185
Why white phosphorous is kept in water ?
Q.186
Which is formed by the combustion of phosphorous in air ?
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INORGANIC PAPER
IIT-JEE
CHEMISTRY
P. JOY
Q.187
Which two products are formed by heating phosphorous with NaOH ?
Q.188
What white phosphorous is ? A good reducing agent or a good oxidising agent ?
Q.189
What are products when HNO3, conc. H2SO4, CuSO4, AgNO3 are reduced by white phosphorous ?
Q.190
What happens when white phosphorous is reacted with following nonmetals (a) Cl2, (b) S8.
Q.191
Which form of phosphorous red or white reacts with NaOH to produce pH3 ?
Q.192
What happenes when following are reacted with water (a) Ca3P2, (b) Na3P.
Q.193
How AlP can be decomposed into pH3 ?
Q.194
What happenes when phosphorous acid is strongly heated ?
Q.195
How phosphene is prepared in laboratory ?
Q.196
What are vortex rings formed by PH3 ? Why these rings are formed ?
Q.197
How vortex rings of PH3 can be prepared in laboratory.
Q.198
Why NF3 is not hydrolysed ?
Q.199
Why PF3 and PF5 are not hydrolysed ?
Q.200
Write the hydrolysis product of following compounds NCl3, PCl3, AsCl3, SbCl3, BiCl3.
Q.201
Why penlahalide like BiF5 does not exist ?
Q.202
B, Ga, Al, Tl, In [First Ionisation Energy]
Q.203
BF3, BBr3, BCl3, BI3 [Lewis Acid Strength]
Q.204
BCl3, GaCl3, AlCl3, InCl3 [Lewis Acid Strength]
Q.205
B2O3, Al2O3, In2O3, Tl2O3, Ga2O3 [Basic Stregnth]
Q.206
B, Ga, Al, In, Tl [Stability of +3 oxidation state]
Q.207
Ga, Tl, In [Stability of +1 oxidation state]
Q.208
B, Ga, Al, In, Tl [Stability of hydride]
Q.209
Al, In, Ga, Tl [Reducing nature]
Q.210
C, Si, Sn, Ge, Pb [First Ionisation Energy]
Q.211
C, Si, Sn, Ge, Pb [Catenation]
Q.212
C, Si, Sn, Ge, Pb [Ionisation Energy]
Q.213
PbF2, PbCl2, PbBr2, PbI2 [Ionic Character]
Q.214
C, Si, Sn, Ge, Pb [Density]
Q.215
N, As, P, Sb, Bi [Melting Point]
Q.216
N, As, P, Sb, Bi [Boiling Point]
Q.217
NH3, AsH3, BiH3, PH3, SbH3 [Basic Strength]
Q.218
NH3, AsH3, BiH3, PH3, SbH3 [Reducing Character]
Q.219
NH3, PH3, AsH3, SbH3 [Boiling point]
Q.220
NI3, NCl3, NBr3, NF3 [Basic Character]
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IIT-JEE
CHEMISTRY
Q.221
NH3, AsH3, PH3, BiH3, SbH3 [Bond Angle]
Q.222
PCl3, SbCl3, AsCl3 [Acid Strength]
Q.223
N2O3, As2O3, P2O3 [Acidic Strength]
Q.224
N2O5, As2O5, P2O5, Bi2O5, Sb2O 5 [Acidic Strength]
Q.225
N2O, N2O 3, NO, N2O4, N2O5 [Acidic Strength]
Q.226
P2O5, Sb2O5, As2O5, Bi2O5, N2O5 [Stability]
Q.227
NCl3, AsCl3, PCl3, SbCl3, BiCl3 [Ease of hydrolysis]
Q.228
PF3, PBr3, PCl3, PI3 [Acid Strength]
Q.229
PF3, PCl3, PBr3, PI3 [Bond Angle]
Q.230
HNO3, H3AsO4, H3PO4, H3SbO4 [Strength and solubility]
Q.231
O, Se, S, Te [Electron Affinity]
Q.232
O, Se, S, Te, Po [Ionisation potential]
Q.233
H2O, H2S, H2Te, H2Se [Reducing power]
Q.234
H2O, H2S, H2Te, H2Se [Bond angles]
Q.235
H2O, H2S, H2Te, H2Se [Stability]
Q.236
H2O, H2S, H2Te, H2Se [Acidic nature]
Q.237
H2O, H2S, H2Te, H2Se [Dipole moment]
Q.238
SO3, TeO3, SeO3 [Acidic nature]
Q.239
SO, SO2, SO3 [Acidic nature]
Q.240
H2SO3, H2SeO3, H2TeO3 [Acidic strength]
Q.241
F, Cl, Br, I [Electron affinity]
Q.242
F, Cl, Br, I [Electronegativity]
Q.243
Cl2, Br2, F2, I2 [Bond energy]
Q.244
Cl2, Br2, F2, I2 [oxidising power]
Q.245
HF, HCl, HBr, HI [Acidic strength]
Q.246
HF, HCl, HBr, HI [Reducing character]
Q.247
HF, HCl, HBr, HI [Boiling point]
Q.248
HF, HCl, HBr, HI [Thermal stability]
Q.249
HClO, HClO2, HClO3, HClO4 [Thermal stability]
Q.250
HClO, HBrO, HIO [Thermal stability]
Q.251
HClO3, HBrO3, HIO3 [Thermal stability]
Q.252
HClO, HClO2, HClO3, HClO4 [Acidic strength]
Q.253
HClO, HBrO, HIO [Acidic strength]
Q.254
HClO, HClO2, HClO3, HClO4 [Oxidising power]
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INORGANIC PAPER
IIT-JEE
CHEMISTRY
P. JOY
Q.255
MF, MCl, MBr, MI [Ionic character]
Q.256
I3+, I3, H5IO6, I2O5, I [Oxidation number]
Q.257
HClO3, HClO4, HClO2, HClO [Acidic strength]
Q.258
I2, HI, HIO4, ICl [Oxidation number]
Q.259
He, Ar, Ne, Kr, Xe [Polarizability]
Q.260
He, Ar, Ne, Kr, Xe [Solubility in water]
Q.261
XeF2, XeF4, XeF6 [Melting point]
Q.262
What is liquor ammonia ?
Q.263
Why decomposition temperature of NH3 will be highest ?
Q.264
What is the colour of the flame produced when NH3 burns in pure oxygen.
Q.265
Ammonia will burn in air ? Yes or No.
Q.266
Which factor is responsible for high boiling point of NH3.
Q.267
Name the process by which ammonia is made industrially.
Q.268
How liquid NH3 resembles water in its physical behaviour.
Q.269
Which factor is responsible for making liquid NH3 a fair ionizing solvent. Why NH3(l) is a better solvent for organic compounds but generally a poorer one for ionic inor-
Q.270
ganic compounds. Q.271
Why AgI is exceedingly insoluble in water but good soluble in NH3.
Q.272
Name the two species formed when liquid ammonia undergoes autodissociation.
Q.273
Which type of reaction occurs when liquid ammonia undergoes autodissociation.
Q.274
Sodium in liquid ammonia is most widely used as a reducing agent or oxidising agent.
Q.275
What are the gases produced when (NH4)2Cr2O7 is heated.
Q.276
What are the gases produced when NH4NO3(s) is dissociated.
Q.277
What are the gas as produced when NH4NO3(l) is decomposed when heated.
Q.278
What is the structure of N2O.
Q.279
How many unpaired electron(s) are present in NO.
Q.280
Which type of molecular orbital, is occupied by unpaired electron(s). Equimolar mixture of which two oxides of nitrogen on condensing at how temperature gives N2O3,
Q.281
as a blue solid. Q.282
Which gas is produced on thermal decomposition of lead nitrate.
Q.283
Which gas is produced on when copper dissolve in conc. HNO3
Q.284
Solid N2O4 is diamagnetic or paramagnetic.
Q.285
What is the anhydride of nitric acid.
Q.286
In which state (liquid, gas, vapour, solid) covalent N 2O5 molecules are present.
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INORGANIC PAPER Q.287
P. JOY
CHEMISTRY
Complete the following reaction 50ºC
→ Fe(CO)5 + NO Pr essure Whether the product formed is ionic or covalent. Q.288
Which compound is formed when NO is reacted with freshly prepared FeSO4 solution.
Q.289
What are the two classess in which phosphorus oxo acids can be divided.
Q.290
What are the formal oxidation states of two oxoacids of phosphorus.
Q.291
How many nonacidic hydrogen atoms are attached directly to phosphorus acids.
Q.292
Consider the following reaction
O
A g+
Ag
P H
OH
C r2 O 7
2–
H
C r +3
H ypophosphorous acid
In the above reaction hypophosphorous acid act as an oxidising agent or reducing agent. Q.293
Which allotropic form of phosphorous is used in preparing hypophosphorus acid from Ba(OH)2.
Q.294
How many acidic hydrogen(s) is/are present in H3PO2.
Q.295
Which phosphorus acid is formed on reaction between water and phosphorous trichloride at 0ºC.
Q.296
Is it possible to obtain polymeric phosphates with layer structures similar to those found in some of the polysilicates.
Q.297
Which phosphoric acid is prepared by treating phosphate rock with sulfuric acid.
Q.298
Which phosphoric acid on dehydration produces orthophosphoric acid.
Q.299
Which oxoacids of phosphorus are tetrabasic acid ?
Q.300
What is the general formula by which cyclic polymetaphosphates can be represented.
Q.301
What are the two main oxoacids of nitrogen.
Q.302
What are the properties possessed by HNO2.
Q.303
Which oxoacid of nitrogen act as both reducing and oxidising agent.
Q.304
What is fuming nitric acid.
Q.305
In which type of solution HNO2 is stable.
Q.306
What is Aqua fortis and what is its meaning.
Q.307
Name the two processess by which HNO3 can be prepared.
Q.308
Aqueous nitric acid is an oxidant, which ion is responsible for this property.
Q.309
What are the products formed when NH2CONH2 is treated with HNO2. Write the balanced equation.
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INORGANIC PAPER
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P. JOY
Q.310
Which two oxyacids of nitrogen are explosive in nature.
Q.311
How nitric acid is manufactured industrially.
Q.312
Which oxide is used to convert nitric acid to its anhydride.
Q.313
What are the oxides produced when N2O4 is dissolved in water.
Q.314
When HNO3 is dissolved in pure H2SO4, an active agent is formed which has an important application in organic chemistry. Name the agent.
Q.315
What are the two oxides of phosphorus.
Q.316
Which compound is formed when P2O3 combines with oxygen.
Q.317
What happens when P2O3 (i) Combines with cold water
(ii) Combines with hot water.
Write the corresponding reactions. Q.318
Which oxide of phosphorus acts as Dehydrating agent.
Q.319
Which oxide of phosphorus is highly, poisonous in nature.
Q.320
Which oxide of phosphorus converts HNO3 to N2O5 and H2SO4 to SO3.
Q.321
What happens when P2O5 (i) Combines with cold water.
(ii) Combines with hot water.
Write the corresponding reactions. Q.322
If ammonia in large excess is treated with Cl2 diluted with N2, what product is produced. Write the balanced equation.
Q.323
Which compound is formed when chloramine reacts with NH3.
Q.324
Consider the sequence for industrial utilization of atmospheric nitrogen. H
O2 +H2O O2 2 → NH3 → HNO3(aq) → NO N2
Haber process
(I)
(II)
(III)
(IV)
Name the process by which II is converted into III. Q.325
Complete the following reaction 4NH3(g) + 3O2(g) l
Q.326
At 750900ºC and in the presence of a platinum catalyst ammonia reacts with oxygen to give other product instead of O2. What is the product formed.
Q.327
How many allotropes of oxygen are present.
Q.328
Give the two laboratory methods for the preparation of oxygen.
Q.329
What are the gases produced on reaction of oxygen with carbon disulphide.
Q.330
Which oxide is present is the compound when Na(s) reacts O2(g).
Q.331
What is the colour of liquid dioxygen and solid dioxygen. VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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INORGANIC PAPER
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CHEMISTRY
P. JOY
Q.332
Name the compound in which the oxygen shows an oxidation state of + 2.
Q.333
Can oxygen show oxidation state beyond 2.
Q.334
Why OF6 is not known.
Q.335
How oxygen can be obtained from bleaching powder.
Q.336
What is an acidic oxide ? Give an example.
Q.337
What is an basic oxide ? Give an example.
Q.338
What is an amphoteric oxide ? Give an example.
Q.339
Which elements generally form amphoteric oxides.
Q.340
Which acid is produced on reaction of SO2 with water.
Q.341
Which type of solution (alkaline, acidic or neutral) is produced on reaction of BaO with water.
Q.342
Which gas is produced when ZnO reacts with an acid.
Q.343
Which factor is responsible for stability of an ionic metal oxide.
Q.344
Give an example of ionic oxides with some covalent character.
Q.345
What are the product(s) formed when H2S react with O2.
Q.346
How many lone pairs of electron are present in OF2 molecule.
Q.347
Arrange the following species in decreasing order of their bond strength. O2, O2+, O2, O22
Q.348
Which gas is produced when sodium nitrate decomposes above 800ºC.
Q.349
Is oxygen has highest electron affinity in group 16 ?
Q.350
What is the oxidation state of O in Na2O2 ?
Q.351
Arrange the following oxides in increasing order of their acidic property. ZnO, Na2O2, P2O5, MgO.
Q.352
What are the factors which are responsible for anomalous behaviour of oxygen.
Q.353
Who discovered oxygen.
Q.354
Which factor is responsible for existence of oxygen as discrete diatomic molecule.
Q.355
Is ozone linear or non linear molecule.
Q.356
How does oxygen and ozone differ in their magnetic nature ?
Q.357
Which ion is isoelectronic with ozone.
Q.358
How does oxygen is converted into ozone.
Q.359
What is the bond angle < O O O in ozone.
Q.360
What change occurs in volume of ozone when it is heated.
Q.361
Which is more powerful oxidizing agent O3 or O2.
Q.362
Give two applications of ozone. VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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IIT-JEE
INORGANIC PAPER
CHEMISTRY
Q.363
To which group of the periodic table, ozone belong ?
Q.364
Can ozone oxidises
P. JOY
(i) Lead sulphide. (ii) Potassium iodide (iii) Mercury Q.365
What is the oxidation state of oxygen in O3.
Q.366
What is the percentage of ozone in ozonised oxygen ?
Q.367
What is the change in the oxidation state of P occurs when ozone reacts with phosphorus. Give an chemical equation.
Q.368
There are two different values of OO bond length in ozone ? True or False.
Q.369
Which halogen (Chlorine or Fluorine) interacts with water to form ozone.
Q.370
Ozone has a dark blue colour. Absorption of which colour of light is responsible for its blue colour.
Q.371
Which type of radiation from the sun is absorbed by the ozone layer in the upper atmosphere.
Q.372
Which compounds are blamed for making holes in ozone layer.
Q.373
Complete the following reaction : O3 + 2K+ + 2I + H2O →
Q.374
In which phase hydrogen bonded molecules of H2O2 are found.
Q.375
Which is more associated via hydrogen bonding i.e. H2O or H2O2.
Q.376
What is the structure of the molecule of H2O2.
Q.377
Which has more density H2O or H2O2
Q.378
What is the limitations of H2O2 which inhibits its utility as an ionizing solvent.
Q.379
Is H2O2 is more acidic than H 2O in dilute aq. solution.
Q.380
H2O 2 acts as oxidizing agent or reducing agent towards MnO4
Q.381
In which type of solution (acid or basic), oxidations with H2O2 is slow.
Q.382
In which type of solution (acid or basic) disproportionation of H2O2 occurs most rapidly
Q.383
Which free radicals are formed by metal ion catalysed decomposition of H2O2.
Q.384
Identify the products of the following reaction O2 H2SO 4 BaO → BaO2 → A + B.
Give the structure and name of the reactant involved in the synthesis of H2O 2 by the reaction given below.
Q.385
O Reactant
C 2H 5
O2 H 2 /Pd .
+ H2 O 2
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INORGANIC PAPER Q.386
IIT-JEE
CHEMISTRY
P. JOY
Consider the following reaction H2O2(l) → H2O(l) + ½O2
∆G = 121.4 kJ mol1
Is water or oxygen is thermodynamically unstable with respect to H2O 2. Q.387
Which acid on hydrolysis give H2O2. Write a chemical equation.
Q.388
Arrange the following O2, H2O and O3 in increasing order of their O O bond length.
Q.389
How many atoms of sulphur are present in its free state.
Q.390
Which ore of sulphur is also called as Fool's gold.
Q.391
Name the process by which sulphur is generally extracted from underground sulphur bearing rocks.
Q.392
Which allotropic form of sulphur is considered as a supercooled liquid.
Q.393
How milk of sulphur is prepared.
Q.394
Below which temperature β-sulphur is converted into α-sulphur and what this temperature is called.
Q.395
Complete the following reactions : Boil (i) 2S + Cl2 → ∆ (ii) 3S + P4 → 1200 −1400K (iii) 2S + C →
Q.396
What compound is formed when sulphur reacts with NH3 in presence of H2S gas.
Q.397
Which oxide of sulfur is closely related structurally & electronically to ozone.
Q.398
What is the structure and bond angle of SO3.
Q.399
Which oxide of sulphur act as an antichlor for removing excess of chlorine.
Q.400
Which property of SO2 is responsible for its bleaching action.
Q.401
Which oxide of sulphur is used in the preparation of H2SO4.
Q.402
What is oxidation state of sulphur in SO2 & SO3 respectively.
Q.403
Give two methods for preparation of Hydrogen Sulphide.
Q.404
H2S is a dibasic acid or monobasic acid.
Q.405
Name the two series of salts formed by H2S.
Q.406
Which property of H2S is used for detection of various cations in laboratory.
Q.407
What happens when SO2 is passed through acidified solution of H2S.
Q.408
Why coordination compounds of H2S are very rare.
Q.409
H2S in large doses prove fatal. What is antidote of H2S.
Q.410
Which acid is called king of chemicals and why is it so called.
Q.411
Name the two processess by which sulphuric acid can be manufactured.
Q.412
What are the ideal conditions required for manufacturing of H2SO4 by contact process. VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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INORGANIC PAPER
IIT-JEE
CHEMISTRY
P. JOY
Q.413
What is the strength of H2SO4 produced by chamber process.
Q.414
By which process 100% pure H2SO4 is obtained.
Q.415
Which removes impurities of arsenic in contact process.
Q.416
Why SO3 is never directly dissolved in H2O to form H2SO4.
Q.417
Write down the chemical reactions taking place in contact process.
Q.418
H2SO4 has low volatility. Why ?
Q.419
Name the two series of salts formed by H2SO4.
Q.420
How many oxygen atoms in H2SO4 are linked to sulphur by single covalent bonds.
Q.421
What is the oxidation state of sulphur in H2SO4.
Q.422
Which type of bond is responsible for associated structure of H2SO4.
Q.423
It is suggested that to dilute conc. H2SO4, always add conc. H2SO4 to water and never water to conc. H2SO4. Why ?
Q.424
Why conc. H2SO4 is used extensively to prepare other acids.
Q.425
Why H2SO4 has great affinity for water.
Q.426
What are the functions of H2SO4 in the reaction given below. 2Ag + H2SO4 → Ag2SO4 + 2H2O + SO2
Q.427
Why sugar becomes black when it comes in contact with conc. H2SO4.
Q.428
Which acid is consumed when a lead storage battery is discharged.
Q.429
Which acid can be used as an oxidising agent, reducing agent and bleaching agent.
Q.430
What are the oxidation number of both the S in Na2S2O3.
Q.431
Why hypo is used in iodometric titrations.
Q.432
Why hypo is used as a fixing agent in photography.
Q.433
What are the products formed when chlorine is passed through aqueous hypo solution.
Q.434
When hypo is heated to high temperatures, the products are.
Q.435
Sulphur disappears when it is boiled in a solution of sodium sulphite. This is due to formation of.
Q.436
Write the spring's reaction for formation of Na2S2O3.
Q.437
Which ion is produced when thiosulphate is oxidised by iodine.
Q.438
What are hydrohalic acids ?
Q.439
Why halogen react very easily and yield hydrogen halide.
Q.440
Complete the reactions : ∆ (i) CaF2 + H2SO4 → ∆ (ii) 2NaCl + H2SO4 →
Q.441
Which hydrogen halide is liquid at room temperature.
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IIT-JEE
INORGANIC PAPER
CHEMISTRY
P. JOY
Q.442
What is the increasing order of acidic strength of hydrohalic acids.
Q.443
Give two reasons for weak acidic character of HF.
Q.444
Why fluorine forms salts of the type KHF2.
Q.445
Why acidity of anhydrous HF is considerably increased in the presence of super acid, SbF5. Write a chemical reaction involved.
Q.446
Which hydrohalic acids has the highest value of dipole moment.
Q.447
Which hydrohalic acid does not form precipitate with AgNO3.
Q.448
Write the increasing order of reducing power of halogen acids.
Q.449
Dilute solution of HF cannot be concentrated beyond 36% by distilling only. Why ?
Q.450
Why HF is not stored in glass bottles.
Q.451
Which acid is used for etching the glass.
Q.452
Which is the most volatile among the following compounds HI, HCl, HF, HBr
Q.453
Which hydrogen halide has the highest molar heat of vaporization.
Q.454
Consider the following reaction HNO3 + HF → H2NO3+ + F Which species act as base.
Q.455
Arrange the following compounds in increasing order of their bond strength HF, HCl, HBr, HI
Q.456
KF combines with HF to form KHF2. What are the species present in the KHF2.
Q.457
Which halogen forms least number of oxyacid.
Q.458
Arrange the following acids in decreasing acid strength. ClOH, BrOH, IOH
Q.459
Arrange the following in increasing order of acidity, HClO, HClO2, HClO3, HClO4
Q.460
What is the oxidation state of chlorine in hypochlorous acid.
Q.461
Consider the following reaction HClO2 → HOCl → ½Cl2 I
II
III
Conversion of II into III will increases or decreases the oxidation number of chlorine. Q.462
Give a method for preparing HClO2.
Q.463
What are the salts of HClO2 called ?
Q.464
Which oxyacids of chlorine is the least oxidizing in nature. VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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INORGANIC PAPER
IIT-JEE
CHEMISTRY
Q.465
Salts (0.1 M solution) of which oxyacid of chlorine is most basic ?
Q.466
Consider the following reaction
P. JOY
NH3 + NaOCl → X + NaOH Gum X + NH3 + OH → H2N NH2 + Cl + H2O
Identify the X & what is it called. Q.467
What is the shape of ClO2 & what is the hybridisation state of Cl.
Q.468
Draw the structure of ClO2.
Q.469
Which oxyacid of chlorine has highest oxidation number.
Q.470
Arrange the oxyacids of chlorine is increasing order of their thermal stability.
Q.471
Arrange the oxyacids of chlorine in increasing order of their thermal stability.
Q.472
Arrange the following compounds in increasing order of their thermal stability HIO3, HClO3, HBrO3
Q.473
BY which mechanism HOCl is formed from Cl2 in water write a chemical reaction.
Q.474
What is the hybridisation state of chlorine in oxyacids of chlorine.
Q.475
What are the natue of oxides of Halogens.
Q.476
Which halogens forms acidic oxides.
Q.477
Which oxide of chlorine is least acidic and which is most acidic.
Q.478
Which oxide of chlorine is paramagnetic is nature.
Q.479
Aqueous solution of bleaching power gives a test of which ions.
Q.480
Name the type of reaction as given below CaOCl2 + H2O → Ca(OH)2 + Cl2
Q.481
What products are obtained by auto oxidation of bleaching power.
Q.482
Bleaching powder loses its bleaching property when it is kept in open bottle for long time. Why.
Q.483
Write the chemical equation involed in Hasenclever method for preparation of CaOCl2.
Q.484
Which gas is liberated when excess of dil. acids (H2SO4, HCl, HNO3) reacts with CaOCl2.
Q.485
What do you mean by available Cl2.
Q.486
Why CaOCl2 uses as a disinfectant.
Q.487
Why CaOCl2 gives Cl2 like smell.
Q.488
Bleaching power is an example of ..... salt.
Q.489
What % of available Cl2 is present in a good quality of bleaching powder.
Q.490
Is bleaching power is priced according to its crystal size.
Q.491
What is the meaning of halogens ?
Q.492
Which group 17 element is radioactive ? VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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INORGANIC PAPER
IIT-JEE
P. JOY
CHEMISTRY
Q.493
What are chalcogens ?
Q.494
Which group elements have greater similarities within group than other group in periodic table.
Q.495
Why halogens do not occur in free elemental state ?
Q.496
What are the generally found form of iodine ?
Q.497
What are the generally found forms of other halogens ?
Q.498
Which halogen is most abundant ?
Q.499
What was moissan method of fluorine formation ?
Q.500
Why diaphragm made of Teflon is used to separate anode from cathode in preparation of fluorine.
Q.501
How bromine is commercially obtained ?
Q.502
How iodides are converted into iodine.
Q.503
How iodates can be converted into I2 ?
Q.504
What is correct when conc. H2SO4 is added on NaCl and MnO2.
Q.505
What happens when K2MnF6 is reacted with SbF5.
Q.506
Halogen oxidises halide ions of higher atomic number. (True/False)
Q.507
In which state of halide ion F2 can act as an oxidising agent ?
Q.508
Which three elements do no reacts with hydrogen ?
Q.509
What happens when ? (a) Mg reacted with Br2 (b) P4 reacted with Cl2 (c) S8 reacted with F2 (d) Xe(g) reacted with F2
Q.510
What is the nature of chemical bond when a metal halide is found in its higher oxidation state ?
Q.511
Which of two is more covalent UF6 or UF4 ?
Q.512
What happens when
→ (i) CaF2 + H2SO4 con. ∆
→ (ii) NaCl + H2SO4 conc. ∆
Pt (as bijects) (iii) H2 + Br2 →
(iv) 2I2(s) + N2H4 → ∆
5731 K
→ (v) I2 + H2S ∆ Q.513
How DCl can be prepared in laboratory.
Q.514
What do you call OCl.
Q.515
How pure HOCl can be formed.
Q.516
What is house hold bleach.
Q.517
What happens when cold dil. NaCl is electrolysed ?
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IIT-JEE
INORGANIC PAPER
CHEMISTRY
P. JOY
Q.518
What is the composition of bleaching powder when Cl2 is passed over slacked lime.
Q.519
What happens when Ba(OH)2 is reacted with H2O2 & ClO2
Q.520
How HClO3 can be obtained by Ba(ClO2)2
Q.521
How Ba(ClO3)2 can be prepared. [What happens when Cl2 is passed through hot Ba(OH)2 solution]
Q.522
What happens when NaClO4 is reacted with conc. HCl.
Q.523
What is the major use of NH4ClO4 ?
Q.524
How NH4ClO4 can be obtained from NaClO4
Q.525
Inter halogen compounds are more reactive then halogens. Explain.
Q.526
Interhalogen compounds are always diamagnetic. Explain.
Q.527
Why interhalogen compounds have covalent character.
Q.528
Interhalogen compounds are conducts electricity. Explains.
Q.529
Why IBr known but ClBr is not known ?
Q.530
Which halogen forms largest inter halogen compounds.
Q.531
Which interhalogen compound exists in pentagonal bipyramidal geometry.
Q.532
Which halogen shows maximum oxidation state informing interhalogen compounds.
Q.533
The value of n in A Xn (interhalogen compounds) can be 1, 3, 5 or 7.
(T/F)
Q.534
A can never be F in A Xn (interhalogen compound)
(T/F)
Q.535
X can never be I in A Xn (interhalogen compound)
(T/F)
Q.536
A X bond is weaker than A A or X X bond in A Xn (interhalogen compounds) (T/F)
Q.537
How many lone pairs are present on ClF3 molecule.
Q.538
What is Wij's reagent.
Q.539
What is Iodine number.
Q.540
Arrange the following interhalogen compounds in increasing order of reactivity IF, IF3, BrF, IF5, BrF3, ClF, IF2, BrF5, ClF3
Q.541
Why ICl3 exist in form of dimers (I2Cl6). Explain.
Q.542
What do you mean of cationic iodine. Give the examples of compounds showing existance of cationic iodine.
Q.543
Which acids are produced during hydrolysis of ICl.
Q.544
Which acids are produces during hydrolysis of BrF5.
Q.545
Complete and balance the following reactions : AlCl
3 → (i) I2 + ICl ∆
→ (ii) CsF + IF7 ∆
Q.546
What is the general electronic configuration of elements of group 18.
Q.547
How many d electrons are present in Ne, Ar, Kr & Xe.
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IIT-JEE
INORGANIC PAPER
P. JOY
CHEMISTRY
Q.548
Why group 18 elements exhibit low chemical reactivity.
Q.549
Why noble gases have very low melting and boiling points ?
Q.550
Which noble gas has the lowest boiling point.
Q.551
Which noble gas has the unusual property of diffusing through rubber or glass.
Q.552
Which noble gas does not occur in the atmosphere.
Q.553
What is the total abundance by volume of noble gases in dry air.
Q.554
Which noble gas is the major component of total abundance of noble gases in dry air.
Q.555
Which noble gases constitutes the byproducts in liquefaction of air.
Q.556
What is the main commercial source of Helium.
Q.557
Which element is the second most abundant element in the universe.
Q.558
Which noble gas is obtained as the decay product of
Q.559
In which year real chemistry of noble gases began.
Q.560
Bartlett had noticed that PtF6 reacts with oxygen to form O2+ [PtF6] & then he reasoned that PtF6 would react with xenon to form Xe+[PtF6] what was the basis of his reasoning.
Q.561
Recent studies indicates that xenon reacts with PtF6 to form above indicated compound but it is to be formulated differently. What is its formula.
Q.562
Which type of elements (electronegative or electropositive) forms compounds with xenon.
Q.563
What are the gases evolved in the following chemical reaction : 2XeF2(s) + 2H2O(l) →
Q.564
Which noble gases are used in light bulbs designed for special purposes.
Q.565
Compounds of which noble gas have not been isolated but only identified by radiotracer tech-
226
Ra. Write a chemical reaction.
niques. Q.566
Which noble gases do not form true compounds.
Q.567
Which compound of krypton has been studied in detail.
Q.568
Which oxygen compound of xenon is formed when XeF4 undergoes hydrolysis write a balanced chemical equation.
Q.569
Complete the following reactions : Ni → (i) Xe + F2 673K , 1atm
2:1
Ni Ni → (iii) Xe + 3F → (ii) Xe + 2F2 2 673K , 60 − 70 atm 673K , 5−7 atm
1:5
1 : 20
Q.570
Complete the following reaction : XeF6 + 3H2O →
Q.571
Which oxyacids are formed when XeF6 undergoes partial hydrolysis.
Q.572
Which oxide of xenon is a colourless explosive solid.
Q.573
Which oxyacid of xenon is a colourless volatile liquid.
Q.574
Which oxygen compounds of xenon has a square pyramidal and trigonal pyramidal molecular structure.
Q.575
Name the ion formed when XeO3 reacts with aq. alkali write a chemical reaction. VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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IIT-JEE
INORGANIC PAPER
CHEMISTRY
P. JOY
Q.576
Ion formed above slowly disproportionates to give another ion. Name the ion.
Q.577
What is the oxidation state of Xe in perxenate ion.
Q.578
What is the colour of the solution of perxenate solutions.
Q.579
Perxenate solutions are powerful oxidising or reducing agents.
Q.580
Which noble gas species is isostructural with (a) ICl4 (b) IBr2 (c) BrO3
Q.581
Which noble gas is used in filling balloons & why it is used.
Q.582
Which noble gas is used in discharge tubes and fluoresent bulbs for advertisement display purposes.
Q.583
Which noble gas is used in gas-cooled nuclear reactors.
Q.584
What are the three binary fluorides of xenon.
Q.585
Which fluoride of xenon has square planar structure.
Q.586
How many bonding pairs of e are present in XeF6.
Q.587
Which fluoride of xenon have a distorted octahedral structure.
Q.588
Which ion forms bridges between XeF5+ units in the solid state of XeF6
Q.589
Which type of bridge is formed in solid state of XeF6.
Q.590
Which type of units are present in solid state of XeF6
Q.591
What is the shape of XeF5+ units present in solid state of XeF6
Q.592
Which species is formed when XeF4 react with SbF5. Give a chemical reaction : XeF4 + SbF5 →.
Q.593
At which temperature liquid He is used as cryogenic agent.
Q.594
Which noble gas has its application in NMR spectrometers.
Q.595
Which noble gas is radioactive in nature.
Q.596
State whether xenone fluoride are powerful flurinating agent.
Q.597
A compound gives off odourless, colourless gas with dil. HCl and develops golden gellone colour to flame compound is (a) NaNO3
(b) CaCO3
(c) Na2CO3
(d) Ca(NO3)2
Q.598
Li has higher I.E. than Na which of two is a better reducing agent ? Explain which factor is most responsible for above results ?
Q.599
Why Na is kept or stored in kerocene ?
Q.600
Why Li is not stored in kerocene ?
Q.601
Bright metallic lister of freshely cut piece of Na is lost on exposure to air why ?
Q.602
Which of the following does not react with Na metal ? (a) D2O
(b) C2H5OH
(c) Diethyl ether
(d) Acetone
(c) Na
(d) K
(c) Low O.P.
(d) High m.p., b.p.
M(g) → M+(g) + e is most favourable in
Q.603
(a) Cs Q.604
(b) Li
Which is a characteristic of alkali metal (a) Conductivity
(b) High I.P.
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IIT-JEE
INORGANIC PAPER Q.605
P. JOY
CHEMISTRY
It same molar amount of lithium, sodium & potassium are dissolved in water and the heat released are measured Q1, Q2 & Q3. Which of the following relations are correct.
Li
Na
K
Q1
Q2
Q3
(a) Q1 > Q2 > Q3
(b) Q1 < Q2 < Q3
(c) Q1 = Q2 = Q3
(d) Q2 > Q1 > Q3
M + H2O → MOH + ½H2
Q.606
What is order of alkali metals reactivity. Q.607
Li reacts with water slowly but when added to water explodes why ? How thermodynamic and kinetic terms can be related to above observation.
Q.608
Does during the reaction of K with water K solid evaporates ?
Q.609
When alkali metals are added to water how does it changes the pH of water ?
Q.610
How does alkali metals react with limited quantity of oxygen ?
Q.611
What happens when alkali metal are reacted with excess of oxygen
Q.612
K(excess) + O2 → product is (a) KO2
(b) K2O
(c) K2O2
(d) None
Q.613
Which alkali metal can be used to absorb N2.
Q.614
Which elements are called S block elements ?
Q.615
Why I A group elements are called alkali metals ?
Q.616
Which alkali metal is most abundant in earth crust ?
Q.617
Why alkali metals are not found in free state ?
Q.618
What are Globular salt, salt cake, chilisalt peter ?
Q.619
What you call an element if it has 18e in Penultimate shell and 1 electron in outer most shell ?
Q.620
What you call an element if it has 8e in Penultimate shell and one e in outermost shell ?
Q.621
Why do alkali metals show mealability, ductility, etc.
Q.622
Why alkali metal have weak metallic bond ?
Q.623
Why alkali metal have low m.p. as compared to Transition metals.
Q.624
Which alkali metal is a liq. at room temperature.
Q.625
What is unit cell type of alkali metals ?
Q.626
Why Cs is used in photoelectric cells ?
Q.627
Why general analytical techniques like coloured ppt, titrations optical rotation are not useful for alkali metal analysis ?
Q.628
Why alkali metals do not form coloured compounds.
Q.629
How do alkali metals are qualitatively identified ?
Q.630
What are colours imparted in flame by alkali metals ? VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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PAGE # 22
IIT-JEE
INORGANIC PAPER
P. JOY
CHEMISTRY
Q.631
Why alkali metals impart colour to bunsen flame.
Q.632
Why different alkali metals impart different colours to bunsen flames ?
Q.633
In flame why alkali metals or metal salt is added to HCl to prepare paste ?
Q.634
Why in flame test Cu wires cannot be used in place of Pt wire ?
Q.635
What is the reliability of flame test ?
Q.636
How the formation of various oxides of alkali metals can be related to their size ?
Q.637
What is structure of Li2O, Na2O, K2O, Rb2O.
Q.638
Why some alkali metals form oxide some form peroxide and other forms super oxide.
Q.639
A student wish to confirm a white solid as Na2O or Na2O2. He dipped red litmus paper into freshely prepared solution of water and found litmus decolouried, solid is (a) Na2O 2
(b) Na2O
(c) NaO2
(d) None
Q.640
What would have happened if red litmus has brought in contact with Na2O.
Q.641
What happens when following is added to water (a) Na2O
(b) Na2O
(c) KO2
Q.642
Which of following has highest bond order among O22, O2, O2, O2
Q.643
Predict the magnetic nature of following ? (a) Na2O 2
(b) KO2
(c) O2
Q.644
What is oxone chemically ?
Q.645
What is the order of basic strength of following oxides ?
(d) Na2O
Li2O, Na2O, K2O, Rb2O, Cs2O Q.646
Why Na2O2 & KO2 are used in space ships.
Q.647
What are washing soda, heptahydrated sod. carbonate and crystalline carbonate, soda ash.
Q.648
Which elements of P.T. forms most stable carbonates ?
Q.649
→ What happens when Na2O ∆
red hot
(a) H2O lost
(b) CO2 lost
(c) Na2O + CO2 formed (d) None
Q.650
Why alkali metal carbonates are stable on heating ?
Q.651
Arrange following in order of stability H2CO3, NaHCO3, Na2CO3
Q.652
What is the order of thermal stability of alkali metal carbonates ?
Q.653
Arrange following ions in order as indicated Li+, Na+, K+, Rb+, Cs+ (a) Ionic radii
(b) Hydrated radii
(c) Hydration number
(d) Hydration enthalpy
(e) Ionic mobility
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IIT-JEE
INORGANIC PAPER
CHEMISTRY
P. JOY
Q.654
What is the primary co-ordination of Li+ ion.
Q.655
In what order M+ ions eluted from cation exchange resins ?
Q.656
How would you make LiH ? Why is it more stable than NaH.
Q.657
How does change radius of Li+ differ from other alkali metal ion ?
Q.658
What other ion has properties similar to alkali metal ion ?
Q.659
The solubility of Li+ cation matches to which other cation.
Q.660
why Li3N is stable where as Na3N does not exist at 25ºC.
Q.661
Why lithium salts are commonly hydrated where as other alkali ions are anhydrous.
Q.662
For salts of strong acids the Li salt is usually the most soluble in water of the alkali metal salts, where as Li salts are usually less soluble than there of the other elements.
Q.663
What happens when Li2CO3 is strongly heated till 500ºC. (a) H2O vapours are formed
(b) H2O, Li2O, CO2
(c) Li2O, CO2 only
(d) None
Q.664
Why Li2CO3 decomposes on heating while other metal carbonates donot
Q.665
Alkali metal carbonates are good soluble in water. Explain why ?
Q.666
Why alkali metal carbonates are alkaline in nature ?
Q.667
What are the only five solid bicarbonates :
Q.668
Why Na2CO3 & CaCO3 differenting react on heating ?
Q.669
How will you make distinction between Na2O and Na2O2.
Q.670
What happens. When Li2CO3 & Na2CO3 are heated upto 500ºC.
Q.671
Why all bicarbonates decompose on heating.
Q.672
Comment on the solubility of bicarbonates ?
Q.673
Which of the two is more basic in Na2CO3, NaHCO3 ?
Q.674
What happens when Na2CO3 . NaHCO3.2H2O is strongly heated ?
Q.675
What happens when Na metal is added to highly pure liq. NH3 ?
Q.676
How does the blue colour of Na in NH3Cl, changes when Na is added in high concentration.
Q.677
Why solution of Na in NH3(l) appears Blue.
Q.678
Why do all alkali metals form same blue colour.
Q.679
Blue colour of solution of alkali metal in NH3 is due to (a) Na metal
(b) NaNH2
(d) Ammonated metal ion Q.680
What organic application of Na in NH3(l) ?
Q.681
Na+NH3(l) observation are
(c) Ammonated e (e) NaLi
(a) Blue colour
(b) Strong reducing agent
(c) Produce NaNH2
(d) Produce H2
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IIT-JEE
INORGANIC PAPER
P. JOY
CHEMISTRY
Q.682
Blue solution of alkali metals in NH3(l) is diamagnetic or paramagnetic ?
Q.683
How blue solution of alkali metal ion is decomposed ?
Q.684
What happens if NH3(l) is carefully evaporated from blue solution ?
Q.685
To blue solution of Na/NH3(l) if more sodium is added it show metallic copper coloured solution then its paramagnetism is (a) Increased
(b) Decreased
(c) The same
(d) No change
Q.686
Why paramagnetism of blue solution decreases on increasing concentration.
Q.687
Which other liq. form blue colour other than NH3(l) (a) THF
(b) HMPA
(d) RNH2
(e) Ethers
(c) Diglyme
Q.688
Which alkali metals is radioactive.
Q.689
Which isotope of Fr has longest life.
Q.690
What is the half life of longest lived isotope of francium.
Q.691
How many valence electron(s) are present in the alkali metal.
Q.692
Which type of ion (monovalent or bivalent) are formed by the alkali metal.
Q.693
Superoxides are paramagnetic or diamagnetic is nature.
Q.694
Which oxide of alkali metal is widely used as an oxidizing agent in inorganic chemistry.
Q.695
Give the reason for the low solubility of LiF & CsI in water.
Q.696
Why alkali metals forms salts with all the oxoacids.
Q.697
Which alkali metal have thermally unstable carbonate.
Q.698
Li, Na, K, Rb, Cs (increasing order of occurence in lithosphere)
Q.699
Li, Na, K, Rb, Cs (increasing order of ionization enthalpy).
Q.700
Li, Na, K, Rb, Cs (Increasing order of metallic radius)
Q.701
Li, Na, K, Rb, Cs (Increasing order of ionic radius).
Q.702
Li, Na, K, Rb, Cs (Increasing order of melting point).
Q.703
Li, Na, K, Rb, Cs (Increasing order of boiling point).
Q.704
Li, Na, K, Rb, Cs (Increasing order of density)
Q.705
Li, Na, K, Rb, Cs (Increasing order of standard potential).
Q.706
Cs2CO3, Rb2CO3, K2CO3, Na2CO3, Li2CO3 (increasing order of stability of carbonates)
Q.707
CsHCO3, RbHCO3, KHCO3, NaHCO3, LiHCO3 (increasing order of stability of bicarbonates)
Q.708
MCl, MBr, MF, MI (Increasing order of covalent character) (M = alkali metal)
Q.709
KCl, KBr, KI (Decreasing solubility in water)
Q.710
LiF, NaF, KF, RbF, CsF (Increasing order of lattice energy)
Q.711
Li, Na, K (Decreasing order of reducing nature in solution).
Q.712
LI2O, Na2O, K2O, Rb2O < Cs2O (Increasing order of basic nature) VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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IIT-JEE
INORGANIC PAPER
CHEMISTRY
P. JOY
Q.713
Li, Na, K, Rb, Cs (Increasing order of reactivity with water)
Q.714
Li, Na, K, Rb, Cs (Increasing order of electropositive character).
Q.715
Write the chemical formula of epsomite.
Q.716
Why Mg does not react with oxygen & water.
Q.717
Which gas is liberated from H2O by magnesium amalgam.
Q.718
Which oxide and nitride are formed when Mg burns in air.
Q.719
Which organometallic compound is formed when alkyl & aryl halides react with Mg.
Q.720
Magnesium acts as a (oxidising or reducing agent) in the production of metals such as Ti, Zr and Hf.
Q.721
Which alkaline earth metal is used as a an oxygen scavenger and for cathodic protection of other metals.
Q.722
Why the temperature of 1273 k is maintained when lime stone is heated for the production of quicklime.
Q.723
What is another name of calcium oxide.
Q.724
What is slaking ?
Q.725
Quicklime slaked with soda gives a solid.
Q.726
Complete the following chemical reaction occuring at high temperature (a) CaO + SiO2 → (b) CaO + P4O10 →
Q.727
What is slaked lime & how it is produced.
Q.728
What is lime water ?
Q.729
Suspension of slaked lime in water is known as.
Q.730
What happens when CO2 is passed through lime water.
Q.731
Identify X in following reaction Ca(OH)2 + CO2 (excess)
→
X (soluble)
Q.732
Milk of lime reacts with chlorine and forms a compound A which is a constituent of bleaching powder. Identify the compound A.
Q.733
What is gypsum.
Q.734
How plaster of paris is obtained.
Q.735
Why compounds of alkaline earth metal are less ionic than the corresponding compounds of the alkali metals.
Q.736
Which type of bond (ionic or covalent) is found in BeO.
Q.737
Arrange the following in order of their indicated property. (i) Mg(OH)2, Sr(OH)2, Ba(OH)2, Ca(OH)2 (Solubility) (ii) Ca(OH)2, Ba(OH)2, Sr(OH)2, Mg(OH)2 (Basic character)) (iii) Mg(OH)2, Co(OH)2, Sr(OH)2, Ba(OH)2 (Solubility) VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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PAGE # 26
INORGANIC PAPER
IIT-JEE
CHEMISTRY
P. JOY
Q.738
Name the ion formed when Be(OH)2 reacts with alkali. Give the chemical reaction
Q.739
How many halogen atoms are coordinated with Be in condensed phase of beryllium halides.
Q.740
Which halides of magnesium are soluble in organic solvents.
Q.741
Fluoride of which alkaline earth metal is known as fluorospar.
Q.742
Name the halide of the alkaline earth metal which is the only large scale source of fluorine.
Q.743
Arrange the following : (i) BeCO3, MgCO3, CaCO3,SrCO3, BaCO3 (Thermal stability) (ii) CaSO4, SrSO4, BaSO4 (Solubility) (iii) Ca(C2O4)2, Sr(C2O4)2, Ba(C2O4)2 (Solubility)
Q.744
Nitrate of which alkaline earth metal crystallizes as the anhydrous salt.
Q.745
Complete the following reaction ∆ 2Ca(NO3)2 →
Q.746
Name the nitrate of alkaline earth metal which is used in pyrotechnics for giving red flame.
Q.747
Why the sulphates of Be & Mg are readily soluble.
Q.748
Except Be, remaining members of the group 2 can have a coordination number of six. Why it is so ?
Q.749
Name the minerals in which Mg occurs in earth's crust.
Q.750
How Mg is obtained from magnesite or dolomite.
Q.751
Consider the following reaction CaCO3.MgCO3 + 2H2SO4 → CaSO4 + MgSO4 + 2H2O + 2CO2 How the two sulphates formed in above reaction can easily be separated.
Q.752
What is the chemical formula of magnesium sulphate which is obtained from the solution containing CaSO4 & MgSO4 is the temperature range 273-320K.
Q.753
What is the correct formulation of the heptahydrate form of magnesium.
Q.754
What is pottash magnesis & what is its chemical composition.
Q.755
Give an medical application of magnesium sulphate.
Q.756
What are the important compounds present in portland cement.
Q.757
Why portland cement was named so ?
Q.758
Who firstly used the name portland cement ?
Q.759
Chemically explain the setting of cement.
Q.760
Which element of group 2 is not known as the alkaline earth metal.
Q.761
How many valence electrons are present in Mg.
Q.762
Which shell occupies valence electrons in Ba.
Q.763
Which metals (alkali or alkaline earth) have smaller atomic radii. Give reason in support of your answer. VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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PAGE # 27
IIT-JEE
INORGANIC PAPER Q.764
P. JOY
CHEMISTRY
The first ionization enthalpies of alkaline earth metals are higher than these of alkali metals but second ionization enthalpies of the alkaline earth metals are smaller than those of corresponding alkali metals why.
Q.765
Which alkaline earth metals do not give flame test & why.
Q.766
Which alkaline earth metal imparts apple green colour to the flame.
Q.767
When KCN is added to CuSO4 solution which complex is formed.
Q.768
Out of AgNO3, AgF and AgClO4 which salts are water soluble.
Q.769
Write the stability of Cu+ and Ag+ halide complexes are in increasing order.
Q.770
Most commen oxidation state of lanthanides is.
Q.771
The purest form of Fe is
Q.772
Cu+ is diamagnetic explain.
Q.773
Paramagnetism is given by the relation µ = 2 s(s + 1) megnetons where 's' is the total spin. On the this basis what is the paramagnetism of Cu+ ion.
Q.774
What is gun metal.
Q.775
An acidic solution contain Cu+2, Pb+2, Zn+2. If H2S gas is passed through this solution, which of the ppt out.
Q.776
Silver ornaments turn black in atmosphere. Which gas is responsible.
Q.777
In dilute alkaline KMnO4 solution MnO4 changes to.
Q.778
What is d-d transition.
Q.779
AgCl and Nacl are colourless while AgBr and AgI are coloured. Explain.
Q.780
Why d-block element have ability of complexes formation.
Q.781
What happens when H2O2 is added to an acidified solution of K2Cr2O7
Q.782
Which metal of 3d transition series have maximum oxidation state.
Q.783
Arrange the following hydroxy compounds in order of increasing acid strength, and account for the trend : (a) CrO2(OH)2
(b) Cr(OH)2
(c) Cr(OH)3
Q.784
Explain how Cr(OH)3 can act both as an acid and as a base.
Q.785
Why does chromium seem to be less reactive than its standard reduction potential suggests ?
Q.786
[FeIII(CN)6]3 ion has magnetic moment of 1.73 B.M., while [Fe(H2O)6]3+ has a magnetic moment of 5.92 B.M. Explain.
Q.787
What is the EAN (effective atomic number) of the underlined atoms in the following complexes ? (a) [Fe(CN)6]4
Q.788
(b) [Cr(en)3]3+
(c) Ni(CO)4
Match the geometry (given in column A) with the complexes (given in column B) in : A
B
(I)
Octahedral
(a) [Ni(CN)4]2
(II)
Square planar
(b) [Fe(CN)6]4
(III)
Tetrahedral
(c) Ni(CO)4
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(d) [Fe(H2O)6]2+
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PAGE # 28
IIT-JEE
INORGANIC PAPER Q.789
CHEMISTRY
P. JOY
One mol of the aqueous solution of the complex CoCl3.5H2O when treated with excess of aqueous AgNO3 solution gave one mol of white ppt of AgCl. What is the complex ? (For this you should know that how many Cl ions are not coordinated to Co3+ - naturally one which is precipitated as AgCl)
Q.790
Arrange [Fe(CN)6]4, [Fe(CN)6]3, [Ni(CN)4]2 and [Ni(H2O)4]2+ in increasing order of magnetic moment.
Q.791
Magnetic of Fex+ ion is
35 B.M. Determine number of unpaired electrons. Also write its elec-
tronic configuration. Q.792
s- and p-block elements form coloured/colourless ? (a) Zn2+
(b) Cu+
(c) Cu2+
(d) Sc3+
(f) V3+
(g) Mn2+
(h) Ni2+
(i) Na+
(e) Ti2+ (j) Ca2+
Q.793
Hg2+ salts are colourless. Explain.
Q.794
Compounds, containing the Sc3+ ion are colourless, whereas those containing the Ti3+ ion are coloured. Explain.
Q.795
Explain the term 'Lanthanide contraction'.
Q.796
Due to 'lanthanide contraction', second and third row transition elements (called 4d and 5d series respectively) have similar radii. What are the other properties do you think would be similar ?
Q.797
Reduction using Lindlar catalyst converts 2-butyne into ....
Q.798
TiCl4 is used as ........... catalyst in polymerisation of ethylene.
Q.799
Cracking of hydrocarbons in presence of hydrogen is done by ............ catalysts.
Q.800
VO2+ is oxidised to VO2+ by MnO4 in acidic medium, which in turn is reduced to Mn2+. Write balanced equation for this reaction.
Q.801
One of the following oxide is also called chromic acid. Select that one : CrO2, Cr2O3, CrO3, CrO.
Q.802
What is oxidation number of Cr in CrO2Cl2.
Q.803
What is oxidation number of Cr in CrO5 or CrO(O2)2
Q.804
What is oxidation number of Cr in (NH4)2Cr2O7
Q.805
What is oxidation number of Cr in [Cr(O2)4]3
Q.806
Arrange the following ions in order of increasing strength as a reducing agent, and account for the trend : (a) Cr2+
(b) Cr3+
(c) Cr2O72
Q.807
H2O 2 can be oxidised to O2 by MnO4 in acidic as well as in basic medium. Write reactions
Q.808
What happens when CO2 gas is passed into MnO42 solution ?
Q.809
Unreacted AgBr in photography is removed by hypo used as 'fixer'. What is the reaction ?
Q.810
(a) When H2S gas is passed into FeCl3 solution, yellow colour of FeCl3 changes to light green. Explain (b) Same behaviour is also observed when SnCl2 solution is observed. Explain.
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INORGANIC PAPER
IIT-JEE
CHEMISTRY
P. JOY
Q.811
Given chemical tests for making distinction between Fe2+ and Fe3+ ions.
Q.812
When K2HgI4 reacts with NH3, brown ppt is formed. Explain the formation of brown ppt.
Q.813
What is brass.
Q.814
What is coinge metal
Q.815
What is nichrome.
Q.816
Name those anions which have high solubility
Q.817
Which anion has least ppt. test.
Q.818
Soda extract is prepared by which carbonate.
Q.819
Soda extract can't be used for which anion detection.
Q.820
Name effervetive gas.
Q.821
Which anions release gases which turns lime water milky.
Q.822
The milkiness of lime water is due to.
Q.823
Formula of lime water is.
Q.824
Mikiness of lime water dissappears due to formation of x on passage of excess CO2 X is.
Q.825
Which gas has suffocating order and responds to litmus paper.
Q.826
What is the colour of K2Cr2O 7 paper when it is treated with SO2.
Q.827
What is the oxidation state of chromium when it is reduced by SO2.
Q.828
In which medium di-chromate ions are converted into chromate ion.
Q.829
Which of the 2 has more oxidising action dichromate or chromate.
Q.830
Which type of substances are detected by potassium iodide starch paper.
Q.831
Which type of reagents are detected by KIO3 starch paper.
Q.832
What happens when white ppt. of Ba(CO3) is is treated with dil acid.
Q.833
Out of CO32, SO3, Br, I, Cl whose barium salts or silver salts are dissolved by dil. acids.
Q.834
In which case CrO2Cl2 test can't be employed.
Q.835
Which cation should be absent when CrO2Cl2 test is employes.
Q.836
Which anion other than halide should be absent when CrO2Cl2 chloride test is employed.
Q.837
What happens when NaCl is treated with potassium dichromate ?
Q.838
Chromyl chloride formation indicates formation of which gas.
Q.839
What is formula of chromyl chloride and its color.
Q.840
What is the gas released when Cl ions are added with conc. H2SO4.
Q.841
What is the gas evolves with Cl ions are reacted with MnO2.
Q.842
Which of the 2 gases Cl2 or HCl is coloured.
Q.843
What happens when chromyl chloride gas is passed into alkaline water.
Q.844
What happens when chlorides are added to AgNo3. VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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INORGANIC PAPER
IIT-JEE
CHEMISTRY
P. JOY
Q.845
Name some substances in which AgCl is soluble.
Q.846
Which of the Ag halide is most colored.
Q.847
Which theory explains colour of Ag halides.
Q.848
Which Ag halide is most easy to break by NH3 solution.
Q.849
Which halide ions on addition of concentration H2SO4 does not evolve halogen.
Q.850
How does solubility of PbCl2 depends on the temp. of water.
Q.851
Name one acid which on added to Br and I does not evolves halogen.
Q.852
Which liq. can be used for organic layer test.
Q.853
What is the colour of organic layer when Br and Cl are tested separately.
Q.854
Which oxidising agent can theoretically employed as for organic layer test of halides.
Q.855
What happens when Br ions are reacts PbO2.
Q.856
Name some reagents which can oxidise Br into bromine.
Q.857
Which halogen can displace bromide from its salt.
Q.858
When iodide is added to conc. H2SO4 which vapor and gas are released.
Q.859
Which hydrogen halide among HCl, HBr, HI can reduce H 2SO4 into SO2.
Q.860
When iodides are treated with H2SO4 acid, a yellow ppt. and rotten egg smell are produced, small is due to.
Q.861
Which halide ion can't be oxidised by MnO2.
Q.862
What happens when CuSO4 is added to iodide.
Q.863
What happens when hypo is added to I ion.
Q.864
What is formula of Nesslers reagent.
Q.865
What happens when HgCl2 is added to excess of KI.
Q.866
Which halide ion catalyses reaction between Ce4+ and aresnate ion.
Q.867
What happens when I ions are treated with acidified potassium nitrite solution.
Q.868
Which gas is coorless but on exposure to air turns brown.
Q.869
Which gas is complexed by FeSO4 to produce brown solution.
Q.870
What is oxidation state of Fe in brown ring test.
Q.871
Which metals or heating with NO3 evolves NH3 gas.
Q.872
Which anions show brown ring complex with FeSO4.
Q.873
Which gas is evolved when NO3 is decomposed by conc. H2SO4
Q.874
What happens when NO2 are treated with dil. H2SO4.
Q.875
What is the colour of HNO2.
Q.876
Which gas is evolved when NO3 are reduced by Cu turning.
Q.877
Which of the 2 is soluble in HCl on warming BaSO4 or Ba3(PO4)2
Q.878
What happens when BaSO4 ppt is reduced by charcoal in presence of Na2CO3. VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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INORGANIC PAPER
IIT-JEE
CHEMISTRY
P. JOY
Q.879
Write some common sulphate which are insoluble.
Q.880
What is the formula of ppt. formed when SO42 are treated with mercuric nitrates.
Q.881
What is the formula of ammonium molybdate.
Q.882
What is the formula of ammonium molybdate that is commercially available.
Q.883
Formula of ammonium phosphomolybdate.
Q.884
What is the color of ammonium phosphomolybate.
Q.885
What happens when disodium hydrogen phosphate is added to FeCl3.
Q.886
What happens when ZrO(NO3)2 is added to phosphate ions.
Q.887
Which ions on treatment with ammonium molybdate produce canary yellow colour.
Q.888
What are the gases produced when C2O42 is reacted with conc. H2SO4.
Q.889
What is the colour of flame when CO is burnt.
Q.890
What happens when drops of potassium per mangnate is added to oxalate ion solution.
Q.891
What is the colour change produce when potassium dichromate is added to aq. solution of C2O42 ion.
Q.892
Which anion has a smell of vinegar.
Q.893
What happens when CH3COO are rubbed with oxalic acid.
Q.894
Name one substance which is an acetate and insoluble.
Q.895
Which anion show fruity ester test.
Q.896
Which reagent or addition to CH3COO forms blood red calouration.
Q.897
What is the formula of blood red coloration formed in above test.
Q.898
What is the formula of basic ferric acetate.
Q.899
Which anion other than CH3COO forms blood red coloration and then brown ppt on heating.
Q.900
Which anion on reaction with KMnO4 undergoes O2 catalysis.
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IIT-JEE
INORGANIC PAPER
CHEMISTRY
P. JOY
SOLUTIONS Q.1 1. 2Al + 3O2 → Al2O3 2. 2Al + N2 → 2AlN 3. 2Al + 3Cl2 → 2AlCl3 4. Al + Cr2O3 → Al2O3 + Cr 5. Al + Mn3O4 → Al2O3 + Mn 6. Al + HCl → AlCl3 + H2 ↓H2O Al(OH)3 + 3HCl 7. 2Al + 3H2SO4(dil) → Al2(SO4)3 + 6H2 8. 2Al + H2SO4(conc.) → Al2(SO4)3 + SO2 + H2O 9. Al + HNO3 → No reaction 10. Al + NaOH → Al(OH)3 +
3 H 2 2
High Temp. 11. 2Al + AlCl3 → 3AlCl
Q.2 1. Al(OH)3 + 3H+ → Al+3 + 3H2O acid 2. Al(OH)3 + NaOH → Na[Al(OH)4] or NaAlO2.2H2O base
sodium meta aluminate
Below 450º C 3. Al(OH)3 → Al2O3 (α-form) Above 450º C 4. Al(OH)3 → Al2O3 (γ-form)
Q.3
M(I) M'(III) (SO4)2.12H2O
Q.4
6 water molecule act as ligands about mono valent metal cations and 6 water molecule act as ligands about trivalent metal cations.
Q.5
Almost any unipositive cations (except Li+) most commen alums have K+, NH4+
Q.6
Al+3, Ti+3, V3+, Cr3+, Fe3+, Mn3+, Co3+, Ga3+, Re3+, Ir3+
Q.7
Due to different type of ions.
Q.8
Li+
Q.9
It loses water of crystallisation and swell up.
Q.10
Alums are used as mordant in dyeing.
Q.11
Acidic due to cationic hydrolysis of trivalent cation. VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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P. JOY
Q.12
An aqueous solution containing equimolar amount of Al2(SO4) and K2SO4 crystallises as allums.
Q.13
Double dulphate of divalent ions and trivalent ions with 24 water molecules in their crystals are known as pseudo alums.
Q.14
No
Q.15
Al2SO4.18H2O
Q.16
Al(OH)3 + 3H+ → Al+3 + 3H2O acid Al(OH)3 + NaOH → Na[Al(OH)4] or NaAlO2.2H2O base
sodium meta aluminate
Al(OH)3 → Gelatinous white ppt.
Q.17
Zn(OH)2 → white ppt. Q.18
It is prepared by passing dry chlorine over aluminium powder.
Q.19
Al2O3 + 3C + 3Cl2 → 2AlCl3 + 3CO
Q.20
In inert orgnic solvent and in vapour state.
Q.21
The high enthalpy of hydration is sufficient to break the covalent dimer into [M(H2O)6]3+ and 3X ions.
Q.22
Yes
Q.23
Acidic, AlCl3 + 3H2O → Al(OH)3 + 3HCl
Q.24
Yes
Q.25
It is hydroscopic in nature.
Q.26
AlCl is unstable below 800ºC. It disproportionate below 800ºC 3AlCl → AlCl3 + 2Al
Q.27
AlCl3 + Cl → [AlCl4]
Q.28
Al2Cl6 + LiH (excess) →Li[AlH4]
Q.29
Al2O3
Q.30
α-Al2O3, β-Al2O3
Q.31
α-Al2O3
Q.32
Al + Fe2O3 → Al2O3 + Fe + heat
Q.33
2Al2O3 + 2AlCl3 → 6AlCl + 3O2
Q.34
α-form
Q.35
γ-Al2O3
Q.36
The strength of CC bond is very high.
Q.37
Pb
Q.38
Graphite
Q.39
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Q.40
Pb
Q.41
Free electrons present in 2p orbitals of graphite
Q.42
Graphite
Q.43
C
Q.44
α-Quartz ⇔ β-Quartz ⇔ Tridymite
Q.45
α-Sn ⇔ β-Sn
Q.46
α-Sn ⇔ β-Sn
Q.47
The conversion of white tin (β-Sn) is accompainied by an increase in volume and the letter, being
840
15ºC
160ºC
15ºC
160ºC
⇔
⇔
1600ºC
⇔
cristobalite
Rhombic Sn
Rhombic Sn
very brittle, easily crumbles down to powder, this phenomenon is known as tin disease. Q.48
When bent the metal produces a cracking sound due to rubbing of crystals over one another is known as tin cry.
Q.49
Sn
Q.50
Diamond
Q.51
CO, CO2, C3O2
Q.52
H2CO3
Q.53
HCOOH
Q.54
Fullerens are produced by evoparation of graphite by lesser.
Q.55
Yes
Q.56
60
Q.57
Purple colour
Q.58
Red orange colour
Q.59
Socker's ball
Q.60
Malonic acid
Q.61
CO2
Q.62
SnO
Q.63
CO
Q.64
CO → neutral, others → acidic
Q.65
SiO2
Q.66
Produce strong base by hydrolysis.
Q.67
1300ºC CaC2 + N2 → CaCN2
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INORGANIC PAPER Q.68
CHEMISTRY
P. JOY
HOH CaCN2 → Ca(OH)2 + H2N CN
BH O 2
H2N − C − NH2 || O urea Coke
Q.69
→ CaCl + NaCN + N CaCN2 + 2NaCl 2 2 ∆
Q.70
∆ K4Fe(CN)6 → 4KCN + Fe + N2
Q.71
2KCN + H2SO4 → 2HCN + 2K+ + SO42
Q.72
Alkaline
Q.73
O2 HCN → N ≡ C C ≡ N 2+
Cu HCN → Cu(CN)2 + NaCN Ag HCN →
Cl2 + NaOH → OCl+ + Cl
Q.74
(CN)2 + NaOH → OCN+ + CN both produced similar type of ions. Q.75
SiO2 does not have tendency of pπ-pπ overlapping.
Q.76
CO2, SiO2 Acidic GeO2, SnO2 Amphoteric PbO2 Basic
Q.77
∆ Pb(NO3)2 → PbO + NO2
Q.78
CO2
Q.79
Gives mellitic acid [C6(COOH)6] and oxalic acid.
Q.80
(R2SiO)n
Q.81
Silicones are produced.
Q.82
sp3
Q.83
β-Quartz
Q.84
Silicates are formed
Q.85
2KOH + SiO2 → K2SiO3 + H2O CaCO3 + SiO2 → CaSiO3 + CO2 2KNO3 + SiO2 → K2SiO3 + 2NO2 + ½O2 SiO2 + 6HF → H2SiF6 + 2H2O C + SiO2 → CO2 + Si
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P. JOY
Q.86
Flint
Q.87
Super cooled liquid, pseudo solid.
Q.88
SiO2 + 6HF → H2SiF6 + 2H2O
Q.89
Fluoro siliclic acid.
Q.90
Na2SiO3.CaSiO3.HSiO2
Q.91
Na2SiO3.H2O
Q.92
When transition metals are added into soda glass solution. Different type of colour are obtained.
Q.93
Silanes Sin H2n + 2 German Gen H2n + 2
Q.94
Vertex of silica is formed.
Q.95
Si + 2NaOH → NaSiO3 + H2↑
Q.96
HF
Q.97
Silanes
Alkanes
Toxic
Not
Autocombust
Not
Reducing agent
Not
Unstable
Stable
Q.98
KNO3 + SiO2 → K2SiO3 + 2NO2 + ½O2
Q.99
HF
Q.100
Corundum (α−Al2O3) and Carborundum (SiC)
Q.101
Glass
Q.102
SiO2
Q.103
Soda glass
Q.104
Hard glass
Q.105
SiO44, BO33
Q.106
Flint glass
Q.107
Stops U.V. light
Q.108
Pyrex glass
Q.109
∆ CaCO3 + Na2CO3 + SiO2 + H3BO3 → borosilicate gass
Q.110
Trimethyl amines sp3, Trisilyl amine sp2 hybridization
Q.111
N(CH3)3
Q.112
Polymeric organocompounds contain SiOSi bonds therefore known as silicones.
Q.113
SiO2 form
Q.114
C does not have 3d orbitals. VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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Q.115
Tin is purifyed by electrolytic method
Q.116
Both SnO and SnO2
Q.117
∆ SnC2O4 → SnO + CO + CO2
P. JOY
Oxidation of SnO to SnO2 is checked by CO NaOH SnO2 → Na2SnO3
Q.118
H2SO 4 SnO2 → H3SnO3 stannic acid
Q.119
∆ SnCl2.2H2O → Sn(OH)Cl
Q.120
SnCl4
Q.121
SnCl4.5H2O
Q.122
SnCl2.2NH3
Q.123
SnCl4.4NH3
Q.124
HgCl2 + SnCl2 → Calamel
Q.125
SnF2
Q.126
Does not reacts with organic acids.
Q.127
3SnCl2 + 2AuCl3 → 3SnCl4 + 2Au
Q.128
H2O 3SnCl2 + 2AuCl3 → 2Au+ + 3SnCl4 → Sn(OH)4
Q.129
H2O SnCl4.5H2O → Sn(OH)Cl
Butter of Tin Q.130
Sn + HNO3 → H3SnO3
Q.131
SnI4 → yellow, SnCl4 and SnBr4 coloured
Q.132
SnO + 2HF → SnF2 + H2O
Q.133
Pb has more value of ionization energy then Sn due to poor shielding of the valence shell electrons by the electrons present in d and f subshells.
Q.134
PbO, PbO2, Pb2O3, Pb3O4
Q.135
Because Pb+2 is more stable than Pb+4
Q.136
Absence of d-orbitals in C
Q.137
C > > Si > Ge > Sn > Pb
Q.138
Three
Q.139
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INORGANIC PAPER Q.140
IIT-JEE
CHEMISTRY
P. JOY
(a) C < Si < Ge < Sn < Pb (b) M.P., C > Si > Ge > Pb > Sn B.P., C > Si > Ge > Sn > Pb (c) Si < C < Ge < Sn < Pb (d) C > Si > Ge > Pb > Sn (e) C(+4), Si(+4), Ge(+4), Sn(+4), Pb(+2) Group V elements have ns2-np3 general configurator which is a half filled orbital having extra
Q.141
stability. So they have high I.E. Q.142
As and Sb
Q.143
The bond strength between Bi-Bi is quite poor and secondly due to inert pair effect, it has poor tendency to form more no. of bonds with other Bi atoms.
Q.144
+3 and +5
Q.145
NH3(3), NH2-NH2(2), NH2OH(1), N2(0), N2O(+1), NO(+2), N2O3(+3), NO2(+4), N2O5(+5)
Q.146
Group V elements have poor bond strength between their atoms.
Q.147
H−N=N=N
Q.148
N2
Q.149
Red, yellow, black.
Q.150
White and yellow
Q.151
White and yellow
Q.152
Nitrogen
Q.153
N2 has high bond energy.
Q.154
Nitrogen N2 others M4
Q.155
pπ -dπ
Q.156
H2O Ca3, N2 → NH3
+
−
H2O Ca3P2 : → PH3
Ca3P2 + 6HOH → 3CO(OH)2 + 2PH3 phosphene
Q.157
Ca3N2 + 6H2O → 3Ca(OH)2 + 2NH3 Zn3As2 + 6H2O → 3Zn(OH)2 + 2AsH3 Q.158
Hydrazine
Q.159
NH3 > PH3 > AsH3 > SbH3
Q.160
NH3 > PH3 > AsH3 > SbH3 > BiH3
Q.161
BiH3
Q.162
NH3
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Q.163
NH3 has H-bonding.
Q.164
NH3 > PH3 > AsH3 > SbH3 > BiH3
Q.165
BiX3
Q.166
Pyramidal
Q.167
PCl3 + HOH → H3PO3 + 3HCl
Q.168
NX3
Q.169
Yes
Q.170
Nitrogen
Q.171
Trihalides are more stable
Q.172
Yes
Q.173
Gaseous state PCl5 and in solid state [PCl4+] [PCl6]
P. JOY
Q.174
Q.175
Ca(PO4)2 + C → CaCO3 + P
Q.176
Yellow
Q.177
Yellow P
Q.178
Red P
,
Q.179
Q.180
Yellow
Q.181
(a) White P converts into Red P (b) White P appears yellow
Q.182
Polymeric structure.
Q.183
Insoluble Red water P
Q.184
P + Ca or Mg → Ca3P2 or Mg3P2 P + Na or K → Na3P or K3P
Q.185
Highly reactive, burshing into Hames when exposed to air. VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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INORGANIC PAPER Q.186
O2 P → P2O3
Q.187
PH3 & NaH2PO2
Q.188
Reducing agent
Q.189
P + HNO3 → H3PO4 + NO2
IIT-JEE
CHEMISTRY
P. JOY
P + Conc H2SO4 → H3PO4 + SO3 P + CuSO4 → Cu3P3 P + AgNO3 → Ag3P2 + HNO3 Q.190
PCl5 P → PCl5 S8 P → P4S3
Q.191
White
Q.192
(a) Ca3P2 + 6H2O → 3Ca(OH)2 + 2PH3 (b) Na3P + H2O → NaOH + PH3
Q.193
H2O AlP → PH3 ↑ + Al(OH)3
Q.194
∆ H3PO3 → PH3 + H3PO4
Q.195
P4 + 3NaOH + 3H2O → PH3 + 3NaH2PO2
Q.196
Ring of N2O5 are known as vertex ring. During formations of PH3, PH3 is oxidized by O2 and forms P2O5
Q.197
P4 + NaOH → Na2HPO4 + PH3↑ PH3 + O2 → HPO3 PH3 + O2 → P2O5 + H2O vertex ring
Q.198
N has no d-orbital thus it can't accept H2O as a ligand for hydrolysis.
Q.199
Due to high P F bond strength
Q.200
H2O NCl3 → X H2O PCl3 → H3PO3 H2O AsCl3 → As2O3 H2O SbCl3 → Sb OCl H2O BiCl3 → BiOCl
Q.201
Bi does not show +5 oxidation state due to inert pair effect.
Q.202
B > Al < Ga > In < Tl
Q.203
BF3 < BCl3 < BBr3 < BI3 VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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INORGANIC PAPER Q.204
BCl3 < AlCl3 < GaCl3 < InCl3
Q.205
B2O3 < Al2O3 < Ga2O3 < In2O3 < Tl2O3
Q.206
B > Al > Ga > In > Tl
Q.207
Ga < In < Tl
Q.208
B > Al > Ga > In > Tl
Q.209
Al > Ga > In > Tl
Q.210
C > Si > Ge > Sn < Pb
Q.211
C >> Si > Ge > Sn > Pb
Q.212
C > Si > Ge > Sn > Pb
Q.213
PbF2 > PbCl2 > PbBr2 > PbI2
Q.214
Si < C < Ge < Sn < Pb
Q.215
N < P < As > Sb > Bi
Q.216
N < P < As < Sb > Bi
Q.217
NH3 > PH3 > AsH3 > SbH3 > BiH3
Q.218
NH3 < PH3 < AsH3 < SbH3 < BiH3
Q.219
PH3 < AsH3 < NH3 < SbH3
Q.220
NI3 > NBr3 > NCl3 > NF3
Q.221
NH3 > PH3 > AsH3 > SbH3 > BiH3
Q.222
PCl3 > AsCl3 > SbCl3
Q.223
N2O3 > P2O3 > As2O3
Q.224
N2O5 > P2O5 > As2O5 > Sb2O5 > Bi2O5
Q.225
N2O < NO < N2O3 < N2O4 < N2O5
Q.226
P2O5 > As2O5 > Sb2O5 > N2O5 > Bi2O5
Q.227
NCl3 > PCl3 > AsCl3 > SbCl3 > BiCl3
Q.228
PF3 > PCl3 > PBr3 > PI3
Q.229
PI3 > PBr3 > PCl3 > PF3
Q.230
HNO3 > H3PO4 > H3AsO4 > H3SbO4
Q.231
O < S > Se > Te
Q.232
O > S > Se > Te > Po
Q.233
H2O < H2S < H2Se < H2Te
Q.234
H2Te < H2Se < H2S < H2O
Q.235
H2O > H2S > H2Se > H2Te
Q.236
H2O < H2S < H2Se < H2Te
Q.237
H2O > H2S > H2Se > H2Te
Q.238
SO3 > SeO3 > TeO3
IIT-JEE
CHEMISTRY
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CHEMISTRY
P. JOY
Q.239
SO > SO2 > SO3
Q.240
H2TeO3 < H2SeO3 < H2SO3
Q.241
F < Cl > Br > I
Q.242
F > Cl > Br > I
Q.243
Cl2 > Br2 > F2 > I2
Q.244
F2 > Cl2 > Br2 > I2
Q.245
HI > HBr > HCl > HF
Q.246
HI > HBr > HCl > HF
Q.247
HF > HI > HBr > HCl
Q.248
HF > HCl > HBr > HI
Q.249
HClO4 > HClO3 > HClO2 > HClO
Q.250
HClO > HBrO > HIO
Q.251
HClO3 < HBrO3 < HIO3
Q.252
HClO4 > HClO3 > HClO2 > HClO
Q.253
HClO > HBrO > HIO
Q.254
HClO4 < HClO3 < HClO2 < HClO
Q.255
MF > MCl > MBr > MI
Q.256
I < I3 < I3+ < I2O5 < H5IO6
Q.257
HClO < HClO2 < HClO3 < HClO4
Q.258
HI < I2 < ICl < HIO4
Q.259
He < Ne < Ar < Kr < Xe
Q.260
Xe > Kr > Ar > Ne > He
Q.261
XeF6 < XeF4 < XeF2
Q.262
Concentration solution of NH3 is water.
Q.263
Hydrogen bonding.
Q.264
Yellow flame.
Q.265
Yes NH3 + O2 → N2 + H2O
Q.266
Hydrogen bonding.
Q.267
Haber process.
Q.268
NH3 has hydrogen bonding like water.
Q.269
Good dielectric constant.
Q.270
NH3 has a tendency to form H-bond which helps to dissolve organic substances whereas its relatively low dielectric constant then water makes it a poor solvent for ionic inorganic substances.
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INORGANIC PAPER Q.271
CHEMISTRY
P. JOY
AgI has covalent bond so it is insoluble in water but it is soluble in NH3 due to complex formation. AgI + 2NH3 l [Ag(NH3)2]+
Q.272
NH4+ + NH2
Q.273
Acid - base
Q.274
Reducing agent.
Q.275
N2 + H2O
Q.276
NH3 + HNO3
Q.277
N2O + H2O
Q.278
Linear
Q.279
One
Q.280
2p
Q.281
NO + NO2
Q.282
NO2
Q.283
NO2
Q.284
Diamagnetic
Q.285
N2O5
Q.286
Vapour
Q.287
50ºC → [Fe(CO) (NO) ] Fe(CO)5 + NO Pr 2 2 essure
Q.288
[Fe(H2O)5NO]SO4
Q.289
Phosphorous acid & phosphoric acids.
Q.290
+1 or +3 in phosphorous acid, +4 or +5 in phosphoric acid.
Q.291
Either one or two.
Q.292
Reducing agent
Q.293
White.
Q.294
One
Q.295
Orthophosphorous acid.
Q.296
NO
Q.297
Orthophosphoric acid.
Q.298
Pyrophosphoric acid.
Q.299
HPO3
Q.300
(HPO3)n
Q.301
HNO2, HNO3
Q.302
Oxidising, reducing, complex forming ability VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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Q.303
HNO3
Q.304
NO2 dissolved in concentrated HNO3
Q.305
aq. solution
Q.306
HNO3
Q.307
Birkeland Eyde & ostwald
Q.308
Nitrate ion.
Q.309
Urea.
Q.310
H4N2O4 & HNO4
Q.311
By direct oxidation of NH3 using Pt as a catalyst.
Q.312
P2O5
Q.313
HNO2 + HNO3
Q.314
NO2+
Q.315
P2O3, P2O5
Q.316
P2O5
Q.317
(i) P2O3 + 3H2O → 2H3PO2
P. JOY
(ii) 2P2O3 + 6H2O → 3H3PO3 + PH3 Q.318
P2O5
Q.319
P2O3
Q.320
P2O5
Q.321
(i) P2O5 + H2O → 2HPO3 (ii) P2O5 + 3H2O → 2H3PO4
Q.322
Chloramine NH2Cl [2NH3 + Cl2 → NH4Cl + NH2Cl]
Q.323
Hydrazine
Q.324
Ostwald Process.
Q.325
2N2(g) + 6H2O(g)
Q.326
NO
Q.327
O2, O3
Q.328
∆ → 3O (g) + 2KCl(s) (i) 2KClO3(s) MnO 2
Q.329
CO2 + SO2
Q.330
Sodium peroxide Na2O2
Q.331
Pale Blue
Q.332
F2O
Q.333
NO
Q.334
No vacant d-orbital.
2
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Q.335
Heating with a cobalt salt
Q.336
SO2
Q.337
BaO
Q.338
ZnO
Q.339
Elements that are on the borderline between metals and non-metals
Q.340
Sulphurous acid (HSO3)
Q.341
Alkaline
Q.342
Hydrogen
Q.343
High lattice energy
Q.344
BeO, SiO2, B2O3
Q.345
O2 2H2S + O 2 → 2H2O + 2S → SO2
Q.346
8
Q.347
O2+ > O2 > O2 > O22
Q.348
O2
Q.349
Yes
Q.350
1
Q.351
Na2O2 > MgO > ZnO > P2O5
Q.352
Small size, High EN, Absence of d orbitals.
Q.353
Priestley
Q.354
Strong covalent between two O atoms due to pπ-pπ overlapping.
Q.355
Non-linear
Q.356
O2 = paramagnetic, O3 = diamagnetic
Q.357
Nitrite ion
Q.358
By action of a silent electric discharge
Q.359
117º
Q.360
Increases to 3/2 times.
Q.361
O3
Q.362
(i) Oxidation of organic compound, (ii) Water purification
Q.363
Group 16
Q.364
Yes it can be oxidise all of them
Q.365
Zero
Q.366
10%
Q.367
P4 + O3 + H2O → H3PO4 Zero to + 5
Q.368
False VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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Q.369
F2
Q.370
Red
Q.371
U.V. Rays
Q.372
Chlorofloro Carbon
Q.373
O3 + 2K+ + 2I + H2O → KOH + I2 + O2
Q.374
Solid
Q.375
H2O2
Q.376
Skew, chain structure
Q.377
H2O or H2O2
Q.378
Its strong oxidizing nature ready decomposition
Q.379
Yes
Q.380
Reducing agent
Q.381
Acid
Q.382
Basic
Q.383
HO2 and OH
Q.384
BaSO4 + H2O
P. JOY
OH C 2H 5 Q.385
OH Q.386
No
Q.387
Peroxodisulfuric acid
Q.388
O2 > O3 > H2O
Q.389
8
Q.390
FeS2
Q.391
Frasch process
Q.392
γ-sulphur
Q.393
It is prepared by boiling milk of lime with sulphur and decomposing the product with HCl.
Q.394
369 K, transition temperature.
Q.395
Boil (i) 2S + Cl2 → S2Cl2 ∆ (ii) 3S + P4 → P4S3 1200 −1400K (iii) 2S + C → CS2
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CHEMISTRY
Q.396
(NH4)2 Sx
Q.397
SO2
Q.398
Trigonal planner, 120º
Q.399
SO2
Q.400
Reducing nature
Q.401
SO3
Q.402
+4 and +6
Q.403
FeS + H2SO4(dil.) → FeSO4 + H2S
P. JOY
H2(g) + S(l) → H2S(g) Q.404
Dibasic acid
Q.405
Bisulphides and hydrogen sulphides.
Q.406
It reacts with cations and produced coloured insoluble sulphides.
Q.407
s is pricipatted.
Q.408
H2S is readly oxidized into s or its disprotonation to SH or S2. It's ligand ability is very weak.
Q.409
Dilute chlorine.
Q.410
H2SO4, it is used in most of manufacturing process.
Q.411
Contact process, Lead chamber process.
Q.412
Fe(OH)3 remove As2O5 in contact process. They absorb As 2O5 on their surface.
Q.413
95%
Q.414
Contact process.
Q.415
Fe(OH)3
Q.416
SO3 + H2O → H2SO4 it is a violent reaction.
Q.417
2 → SO H2O S + O2 → SO2 VO H2SO4. 3 → 2 5
Q.418
Intermolecular hydrogen bonding.
Q.419
Bisulphate and sulphate.
Q.420
2
Q.421
+6
Q.422
H-bonding.
Q.423
Sparting of acid due to evolution of great amount of heat.
Q.424
H2SO4 is an oxidizing agent thus it can easily oxidised elements in their oxyacids.
Q.425
H2SO4 can form strong extensive H-bonds.
Q.426
Oxidising agent.
Q.427
Conc. H2SO 4 C6(H2O)6 → 6C + 6H2O
O
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Q.428
H2SO4
Q.429
H2SO3
Q.430
Zero and +4
Q.431
It can be reduce I2
Q.432
It dissolves unreacted AgBr from the photographic emulsion by complexation.
Q.433
Cl2 + H2O + Na2S2O3 → 2HCl + Na2SO4 + S
Q.434
Cl2 + H2O + Na2S2O3 → 2HCl + Na2SO4 + S Hypo is thus used as an antichlore.
Q.435
Na2S2O3
Q.436
Na2S + Na2S2O3 + I2 → 2NaI + Na2S2O3
Q.437
S4O62 (Tetrathionate)
Q.438
aq. solution of hydrogen halides.
Q.439
Strong affinity for hydrogen.
Q.440
(i) CaSO4 + 2HF(g), (ii) Na2SO2 + 2HCl(g)
Q.441
HF
Q.442
HI > HBr > HCl > HF
Q.443
High bond dissociation energy intermolecular hydrogen bonding.
Q.444
Due to high EN & small size of F.
Q.445
SbF5 is a strong e pair acceptor.
Q.446
HF
Q.447
HF
Q.448
HF < HCl < HBr < HI
Q.449
HF forms a constant boiling mixture.
Q.450
It reacts with SiO2 of the glass.
Q.451
HF
Q.452
HCl
Q.453
HF
Q.454
HNO3
Q.455
HF > HCl > HBr > HI
Q.456
K+ and [HF2]
Q.457
Fluorine
Q.458
ClOH > BrOH > IOH
Q.459
HClO < HClO2 < HClO3 < HClO4
Q.460
+1
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Q.461
Increases.
Q.462
Ba(ClO2)2 + H2SO4 → 2HClO2 + BaSO4
Q.463
Chlorites
Q.464
HClO4
Q.465
NaClO
Q.466
X = NH2Cl, chloramine
Q.467
Tetrahedral, sp3
Q.468
O− Cl → O
Q.469
HClO4
Q.470
HClO4 > HClO3 > HClO2 > HClO
Q.471
HClO4 > HClO3 > HClO2 > HClO
Q.472
HClO3 < HBrO3 < HIO3
Q.473
Cl2 + H2O → H+ + Cl + HOCl
Q.474
+1 to +7
Q.475
Acidic
Q.476
Cl, Br, I
Q.477
Cl2O least and Cl2O7 most acidic.
Q.478
ClO2
Q.479
Ca+2, Cl, OCl
Q.480
CaOCl2 + H2O → Ca(OH)2 + Cl2
Q.481
Ca(OH)2, Cl2
Q.482
It reacts with H2O and convert into Ca(OH)2 and Cl2 by auto oxidation.
Q.483
Ca(OH)2 + Cl2 → Ca(OCl) Cl + H2O
Q.484
Cl2
Q.485
The amount of Cl2 obtained from a sample of bleaching powder by treatment with excess of dilute acids or CO2.
Q.486
It produce nascent O by treatment with H2SO4.
Q.487
Autooxidation
Q.488
Mixed salt.
Q.489
35 to 38%
Q.490
Yes
Q.491
Halogen means salt forming.
Θ
.. ..
Autooxidation
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P. JOY
Q.492
At
Q.493
16th group elements
Q.494
Alkali metals and halogens
Q.495
Due to higher EN and their reactivity.
Q.496
I and IO3
Q.497
X
Q.498
Cl2
Q.499
Electrolysis of mixture of molten KF and HF
Q.500
Diaphragm is used to separate the two gases H2 and F2 otherwise these gases reacts explosively.
Q.501
By passing Cl2 gas into bromide salt solution
Q.502
6H+ + IO3 + I → I2 + 3H2O
Q.503
6H+ + IO3 + I → I2 + 3H2O
Q.504
When H2SO4 is added to NaCl with MnO2, Cl2 is evolved.
Q.505
K2MnF6 + SbF5 → K2SbF7 + MnF3 + ½F2
Q.506
True
Q.507
When halogen has 1 oxidation state.
Q.508
He, Ne, Ar
Q.509
(a) Mg + Br2(l) → MgBr2 (b) P4 + Cl2(g) → PCl5 (c) S8 + F2(g) → SF6 (d) Xe(g) + F2(g) → XeF6
Q.510
Covalent nature
Q.511
UF6
Q.512
→ CaSO + HF (i) CaF2 + H2SO4 con. ∆ 4 → Na SO + HCl (ii) NaCl + H2SO4 conc. ∆ 2 4 Pt (as bijects) (iii) H2 + Br2 → HBr
5731 K
(iv) 2I2(s) + N2H4 → N2 + HI ∆
→ HI + S (v) I2 + H2S ∆ Q.513
PCl5 + D2O → POCl3 + 2DCl
Q.514
Hypochlorite ion
Q.515
Cl2 + H2O + HgO → HOCl + HCl, HCl is absorbed by HgO
Q.516
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Q.517
Anode → Cl2 gas, Cathode → H2 and OH obtain.
Q.518
Cl2 Ca(OH)2 → Ca(OCl)2. CaCl2.Ca(OH)2.2H2O
Q.519
2Cl2O + 2NaOH + H2O2 → 2NaClO2 + O2 + 2H2O
Q.520
Ba(ClO3)2 + H2SO4 → BaSO4 + 2HClO3
Q.521
Ba(ClO3)2 + Cl2 → Ba(ClO3)2
Q.522
THCl.
Q.523
Used in rockets as fuels.
Q.524
NaClO4 + NH4Cl → NH4ClO4 + NaCl
Q.525
x-x bond is stronger due to effective overlaping.
Q.526
Absence of unpaired electrons.
Q.527
Lower electronegativity difference.
Q.528
These are self ionizes
Q.529
Cl does not show +ve o.s. due to higher I.P.
Q.530
Fluorine
Q.531
I
Q.532
True
Q.533
True
Q.534
True
Q.535
True
Q.536
11
Q.537
IF7
Q.538
ICl is used as Wij's reagent in the estimated of the iodine number of fats and oils
Q.539
Iodine no. is a measure of the number of double bonds i.e. the degree of unsaturation of the fats.
Q.540
IF < IF3 < BrF < IF5 < BrF3 < ClF < IF2 < BrF5 < ClF3
Q.541
ICl3 is unstable.
Q.542
I+ → ICl, IBr, ICN, I+3 → ICl3, I(ClO4)3.IPO4.
Q.543
HOI (Hypo iodous acid) HCl.
Q.544
HF, HBrO3 bromic acid.
Q.545
(i) [I3]+ [AlCl4] (ii) Cs+ [IF8]
Q.546
ns2 np6
Q.547
Ne = 0, Ar = 0, Kr = 10, Xe = 10
Q.548
Gain or loss of electrons requires high energies.
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Q.549
Due to weak dispersion interactions between atoms.
Q.550
He
Q.551
He
Q.552
Rn
Q.553
~ 1%
Q.554
Ar
Q.555
Ne, Ar, Kr, Xe
Q.556
Natural gas
Q.557
He
Q.558
88
Q.559
1962
Q.560
Ionization enthalpies of O2 & Xe are close to each other.
Q.561
[XeF]+ [Pt2F11]
Q.562
Electronegative
Q.563
Xe, O2
Q.564
Xenon, krypton
Q.565
Radon
Q.566
Ar, Ne, He
Q.567
KrF2
Q.568
6XeF4 + 12H2O → 4Xe + 2XeO3 + 24HF + 3O2
Q.569
XeF2, XeF4, XeF6
Q.570
XeO3 + 6HF
Q.571
XeOF4 & XeO2F2
Q.572
XeO3
Q.573
XeOF4
Q.574
XeO3 = Trigonal pyramidal, XeOF4 = Square pyramidal.
Q.575
XeO3 + OH → HXeO4
P. JOY
Ra226 → 86Rn222 + 2He4
hydrogen xenate ion Q.576
Perxenate ion XeO64
Q.577
+8
Q.578
Yellow
Q.579
Oxidising
Q.580
(a) XeF4, (b) XeF2, (c) XeO3
Q.581
He non flammable & light gas
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P. JOY
Q.582
Neon
Q.583
He
Q.584
XeF2, XeF4, XeF6
Q.585
XeF4
Q.586
6
Q.587
XeF6
Q.588
F
Q.589
Pyramidal
Q.590
Tetrameric & hexameric
Q.591
Square pyramidal
Q.592
[XeF3]+ [SbF6]
Q.593
4.2 K
Q.594
Helium
Q.595
Rn
Q.596
True
Q.597
(b)
Q.598
Li is better reducing agent. Because the big size of Na+ releases smaller heat of hydration.
Q.599
Na can reacts with air and water.
Q.600
Li is lighter than kerosense so it float over kerosene surface there if reacts with atmosphereic oxygen.
Q.601
The O2 of atmosphere tarnishes metallic surface by reacting with metal.
Q.602
(a, b)
Q.603
(a)
Q.604
(c)
Q.605
(a)
Q.606
Cs > Rb > K > Na > Li
Q.607
The hydration energy of Li is greater therefore a large amount of heat is evolved. Heat of hydration (Thermodynamic factor) is highest for Li but kinetic order of reactivity is Cs > Rb > K > Na > Li.
Q.608
Yes
Q.609
Solution become alkaline
Q.610
2M + ½O2 → M2O
Q.611
H2O, Na2O2, KO2, RbO2, CsO2
Q.612
(b)
Q.613
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Q.614
Elements which have (noble gas) ns1, ns2 configuration.
Q.615
Hydroxides and oxides of these metals are highly alkaline in nature.
Q.616
Na
Q.617
Alkali metals are highly reactive.
Q.618
Na2SO4.10H2O, Na2SO4, NaNO3
Q.619
d-block element
Q.620
s-block element
Q.621
Alkali metals forms metallic bond by valency e s.
Q.622
This is due to lesser no. of electrons used by the elements to form electronic sea of metallic bond.
Q.623
This is due to covalent bond developed by the d-block elements in its metallic bond.
Q.624
Cs
Q.625
BCC
Q.626
Very low I.E.
Q.627
Alkali metal ion in aqueous state in alkali metal salts are colourless due all e's is paired state.
Q.628
Alkaly metals have inert gas configuration in ionic form.
Q.629
By flame test.
Q.630
Li Crimson red Na Yellow gold K Green (pale) Rb Blue Cs Blue
Q.631
Because photons or light energy of invisible part of bunsen flame is absorb by e s of alkali metal and get excited into higher energy shell. When electrons transite back it radiates light of visible region.
Q.632
Because energy gap of electron shells are different in different elements. Thus energy needed to transition and consecutive radiations are also different.
Q.633
To prepare volutile chlorides.
Q.634
Cu wire themselves in blue colour.
Q.635
Highly reliable
Q.636
Smaller ions forms oxide medium size ions form peroxide and larger ion forms superoxide.
Q.637
Antifluorite structure
Q.638
Depends upon the reactivity of metal toward oxygen.
Q.639
(a)
Q.640
It would have turned blue.
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IIT-JEE
CHEMISTRY
P. JOY
Na2O2 + H2O → 2NaOH + H2O2 Na2O + H2O → 2NaOH KO2 + H2O → 2KOH + H2O2 + O2
Q.642
O2
Q.643
(a) Na2O2 diamagnetic
(b) KO2 paramagnetic
(c) O2 paramagnetic
(d) Na2O paramagnetic
Q.644
Na2O2 + HCl(dil.)
Q.645
Li2O < Na2O < K2O < Rb2O < Cs2O
Q.646
They easily liberates oxygen.
Q.647
Na2CO3.10H2O, Na2CO3.7H2O, Na2CO3.H2O, Na2O
Q.648
s-block element.
Q.649
(d) Na2O2 and Na vapour are formed.
Q.650
s-block elements have calculate with high thermal stability due to less polarizing power of cations.
Q.651
Na2CO3 > NaHCO3 > H2CO3
Q.652
Cs2CO3 > ........... > Li2CO3
Q.653
(a) Li+ < Na+ < Rb+ < Cs+
(b) Li+ > Na+ > Rb+ > Cs+
(c) Li+ > Na+ > Rb+ > Cs+
(d) Li+ > Na+| > Rb+ > Cs+
(e) Li+ < Na+ < Rb+ < Cs + Q.654
4
Q.655
Cs > Rb > K > Na > Li
Q.656
When lithium is reacted with pure hydrogen lithium hydride is formed. Small size of lithium ion better balances hydride ion.
Q.657
Lithium charge to size ratio is very high as compared other alkali metal ion therefore this leads to covalent property in lithium compounds.
Q.658
NH4+, substituted ammonium ions, Ti+, Ag+, spherical + 1 complex (n5 C5H5)2Co+
Q.659
Mg+2
Q.660
Na3N does not exist at room temperature N3 has high ve charge & prefers covalent bonding which can only be developed by lithium ions among alkali metal ion.
Q.661
Due to small size of lithium ions the energy released by reaction of Li+ with water is greater than the energy needed to wides the crystal lattice.
Q.662
HClO4.3H2O
Q.663
(c)
Q.664
Li2CO3 is stable due to higher polarizing power of lithium.
Q.665
Hydration energy is greater then lattice energy.
Q.666
Due to anion hydrolysis. VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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CHEMISTRY
Q.667
LiHCO3, NaHCO3, KHCO3, RbHCO3, NH4HCO3
Q.668
Na2CO3 is stable.
Q.669
Na2O2 + H2O → 2NaOH + H2O2
P. JOY
Na2O + H2O → 2NaOH Q.670
Li2CO3 decomposed into LiO and CO2 but Na2CO3 does not decomposed.
Q.671
Because all bicarbonates passes H+ as an essential cation which polarises CO32 ions and decomposes into CO2.
Q.672
All bicarbonates all soluble in water.
Q.673
Na2CO3 is more basic in aqueous state.
Q.674
Decomposed into 2Na2CO3 + 2H2O
Q.675
It forms a blue coloured solution of ammonated electrons and ammonated alkali metal ions.
Q.676
Blue colour turns to colour of metallic Cu.
Q.677
Due to ammonated es.
Q.678
Because blue colour is exihibited by ammonated electrons, and electrons obtained from all alkali metals are same.
Q.679
(c)
Q.680
Strong reducing agent.
Q.681
(All)
Q.682
Paramagnetic
Q.683
Fe By addition T.M. ion Na + NH3(l) → NaNH2 + ½H2 ↑
Q.684
Residual deposition of alkali metal.
Q.685
(b)
Q.686
Due to pairing of electrons.
Q.687
(a, b, c, d)
Q.688
Fr
Q.689
223
Q.690
21 min.
Q.691
One
Q.692
Monovalent
Q.693
Paramagnetic
Q.694
Sodium peroxide
Q.695
Low solubility of LiF is due to its high lattice energy.
3+
Fr
Low solubility of CsI is due to smaller hydration energy. Q.696
Due to their high electropositivity. VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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P. JOY
Q.697
Li
Q.698
Na < K < Rb < Li < Cs
Q.699
Cs < Rb < K < Na < K
Q.700
Li < Na < K < Rb < Cs
Q.701
Li < Na < K < Rb < Cs
Q.702
Cs < Rb < K < Na < Li
Q.703
Cs < Rb < K < Na < Li
Q.704
Li < Na < K < Rb < Cs
Q.705
Li > Na > K > Rb > Cs
Q.706
Li2CO3 < Na2CO3 < K2CO3 < Rb2CO3 < Cs2CO3
Q.707
CsHCO3 < RbHCO3, KHCO3 < NaHCO3 < LiHCO3
Q.708
MF < MCl < MBr < MI
Q.709
KI > KBr < KCl
Q.710
Li > K > Na
Q.711
Li2O, Na2O < K2O, Rb2O < Cs2O
Q.712
Li < Na < K < Rb < Cs
Q.713
BLi < Na < K < Rb < Cs
Q.714
BLi < Na < K < Rb < Cs
Q.715
MgSO4.7H2O
Q.716
Due to the formation of a surface film of the oxide.
Q.717
H2
Q.718
MgO, Mg3N2
Q.719
Grignard Reagent
Q.720
Reducing agent.
Q.721
Mg
Q.722
Reaction is reversible & proceeds efficiently when CO2 is escaped which is only above 1100 K. CaCO3 l CaO + O2
Q.723
Quick time
Q.724
Disintegration of lump of lime in limited amt. of water.
Q.725
Sodalime.
Q.726
(a) CaO + SiO2 → CaSiO3 (b) CaO + P4O10 → Ca(PO4)2
Q.727
Ca(OH)2 when water is added to slaked lime.
Q.728
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CHEMISTRY
Q.729
Milk of lime.
Q.730
It turns milky.
Q.731
Ca(HCO3)2
Q.732
Ca(ClO)2
Q.733
CaSO4.2H2O
Q.734
When gypsum CaSO4.2H2O is heated to 393 K.
Q.735
Due to increased nuclear charge & smaller size.
Q.736
Covalent
Q.737
(i) Mg(OH)2 < Ca(OH)2 < Sr(OH)2 < Ba(OH)2
P. JOY
(ii) Mg(OH)2 < Ca(OH)2 < Sr(OH)2 < Ba(OH)2 (iii) Mg(OH)2 < Ca(OH)2 < Sr(OH)2 < Ba(OH)2 Q.738
Beryllate ion.
Q.739
Four
Q.740
MgBr2 & MgI2
Q.741
Ca
Q.742
CaF2
Q.743
(i) BeCO3 < MgCO3 < CaCO3 < SrCO3 < BaCO3 (increasing thermal stability) (ii) CaSO4 > SrSO4 > BaSO4 (Increasing solubility) (iii) Ca(C2O4)2 > Sr(C2O4)2 > Ba(C2O4)2 (increasing solubility)
Q.744
Ba
Q.745
∆ 2Ca(NO3)2 → 2CaO + 4NO2 + O2
Q.746
Strontium nitrate.
Q.747
Greater hydration energies of Be2+ & Mg2+ ions overcome the lattice energy factor.
Q.748
Be have no vacant d-orbital while other have it.
Q.749
MgSO4.2H2O, MgSO4.7H2O
Q.750
By treating with H2SO4
Q.751
By fractional crystallization
Q.752
MgSO4.7H2O
Q.753
[Mg(H2O)6]SO4.H2O
Q.754
Potash magnesis is a Fertilizer & Its chemical composition K2SO4.MgSO4.6H2O.
Q.755
Purgative in medicine.
Q.756
Ca2SiO4, Ca3SiO5, Ca3Al2O6
Q.757
When it is mixed with water & send the powder herdered into a block that resembled the natural limestone quairried in the Isle of portland.
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P. JOY
Q.758
J. Aspdin in 1824.
Q.759
It is the hydration of the molecules of the constituents and their rearrangement.
Q.760
Be
Q.761
2
Q.762
7th
Q.763
Alkaline earth metals due to increased nuclear charge.
Q.764
After first ionization alkali metals aquired inert gas configuration therefore their second I.P. is very higher.
Q.765
Be, Mg : electron are too strongly bound to get excited by flame.
Q.766
Ba
Q.767
K3[Cu(CN)4]
Q.768
All
Q.769
I > Br > Cl > F
Q.770
+3
Q.771
Cast iron
Q.772
3d10 4s0 configuration
Q.773
Zero
Q.774
Mixture of Cu + Sn + Zn
Q.775
Cu+2 and pb+2
Q.776
H2S
Q.777
MnO2
Q.778
Transition of electrons between d-orbitals of a metal.
Q.779
Ag+ polarises Br and I
Q.780
Small and highly charged ions and have vacant orbitals to accept lone pair of electrons from ligand.
Q.781
A deep blue voilet coloured compound CrO(O2)2 is formed.
Q.782
Mn
Q.783
Cr(OH)2 < Cr(OH)3 < CrO2(OH)2 acid strength increases with increase in oxidation number.
Q.784
Cr(OH)3 + 3HCl → CrCl3 + 3H2O base Cr(OH)3 + NaOH → Na[Cr(OH)4] acid
Q.785
Because of formation of oxide layer.
Q.786
[Fe(CN)6]3 has one unpaired electron (d2sp3 hybridised Fe3+) while [Fe(H2O)6]3+ has five unpaired electrons (sp3d2 hybridised Fe3+) VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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IIT-JEE
INORGANIC PAPER Q.787
(a) 36
Q.788
I(b), II(a), III(c)
Q.789
[Co(H2O)4Cl2]Cl.H2O
Q.790
[Ni(H2O)4]2+ > [Fe(CN)6]2 > [Fe(CN)6]4 = [Ni(H2O)4]2+
Q.791
N(N + 2) =
P. JOY
CHEMISTRY
(b) 33
(c) 36
(d) 36
3+ 35 ⇒ N = 5 (unpaired electrons) ⇒ x = 3(Fe )
Fe3+ = [Ar] 3d5 Q.792
The s- and p-block elements do not have a partially filled d-shell so there cannot be any d-d* transition. The energy to promote as s- or p-electron to a higher energy level is much greater and corresponds to ultraviolet light being absorbed. Thus compound will not be coloured.
Q.793
Hg2+ has all filled 5d orbitals (no unpaired electron is 5d), hence no d-d* transition, hence colourless.
Q.794
Sc(21) : [Ar] 3d! 4s2 Sc3+ : [Ar] 3d0 no unpaired electron in d-orbital, hence no (d-d*) transition hence colourless. Ti(22) : [Ar] 3d2 4s2 Ti3+ : [Ar] 3d1 due to unpaired electron in d-orbital (d-d*) transition possible hence coloured.
Q.795
There is a steady decrease in the radii as the atomic number of the lanthanide element increases. It is because, for every additional proton in a nucleus, the corresponding electron goes into 4f shell which is too diffused to screen the nucleus as effectively as more localised inner shell. Hence the attraction of the nucleus for the outermost electrons increases steadily with the atomic number of the lanthanides. This contraction in size is quite regular. This is called Lanthanide Contraction.
Q.796
Lattice energies, solvation energies and ionisation energies would be similar.
Q.797
cis-2-butene
Q.798
Natta
Q.799
Zeolite
Q.800
5VO2+ + MnO4 + H2O → 5VO2+ + Mn2+ + 2H+
Q.801
CrO3
Q.802
VI
Q.803
VI (O = 2 diperoxo = 4)
Q.804
VI
Q.805
V
Q.806
Cr2O72 < Cr3+ < Cr2+ Smaller the oxidation state of the element in the ion, greater the reducing nature.
Q.807
2MnO4 + 5H2O2 + 6H+ → 2Mn2+ + 5O2 + 8H2O 2MnO4 + 3H2O2 → 2MnO2 + 3O2 + 2OH + 2H2O
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IIT-JEE
INORGANIC PAPER Q.808
CHEMISTRY
P. JOY
Aqueous CO2 releases H+ which can convert MnO42 into MnO2 and MnO4 in a disproportionation reaction. CO2 + H2O l H+ + HCO3 3MnO42 + 4H+ → MnO2 + 2MnO4 + H2O
Q.809
AgBr + 2Na2S2O3 → Na3[Ag(S2O3)2] + NaBr
Q.810
In both cases Fe2+ ions are formed due to reduction. Hence solution appears light green.
Q.811
Fe2+ gives green ppt with NaOH and Fe 3+ gives red brown ppt.
Q.812
2K2HgI4 + NH3 + 3NaOH →
Hg O Hg
NH 2
I + 4KI + 3NaI + 2H2O
(Iodide of M illo n’s ba se) b row n p pt
Q.813
70% Cu + 30% Zn
Q.814
75% Cu + 25% Ni
Q.815
60% Ni + 20Fe + 20% Fe
Q.816
NO3, HCO3, CH3COO
Q.817
NO3
Q.818
Na2CO3
Q.819
CO32
Q.820
CO2
Q.821
S2 → SO2 and CO32 → CO2
Q.822
CaCO3
Q.823
Ca(OH)2
Q.824
Ca(HCO3)2
Q.825
SO2
Q.826
Green.
Q.827
Cr+3
Q.828
Basic.
Q.829
Dichromate or chromate.
Q.830
Oxidising agents Cl2, Br2, KIO3, Cu4+, K2Cr2O7, KMnO4.
Q.831
Reducing agents.
Q.832
ppt dissolves through formation of CO2
Q.833
CO3 and SO3
Q.834
In presence of I and Br
Q.835
Pb, Ag, Sb, Sn VISION KOTA, 608-A, TALWANDI KOTA (RAJ.) Ph. 0744 - 6450883, 2405510
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CHEMISTRY
P. JOY
Q.836
NO3, NO2, chlorates.
Q.837
Cl2 is evolved as Cr2O72 are oxidising agent and oxidises Cl into Cl2
Q.838
HCl
Q.839
Cr2F2, violet
Q.840
HCl
Q.841
Cl2
Q.842
Cl2
Q.843
CrO42 (yellow colored ion) is formed.
Q.844
White ppt of AgCl
Q.845
NH3 solution, SO32 solution, cyanide solution, hypo solution, amine solution.
Q.846
AgI
Q.847
Fazan's theory.
Q.848
AgCl
Q.849
Cl
Q.850
Soluble in hot water.
Q.851
H3PO4
Q.852
CCl4, CS2
Q.853
Br → Br2 (Red) I → I2 (violet / purple)
Q.854
Cl2 water, HOCl, NaOCl, conc. HNO3
Q.855
Redox reaction take place and Br2 is liberated.
Q.856
H2SO4, HNO3, MnO2, PbO2, Cl2 water, KMnO2, NaOCl, HOCl
Q.857
Cl2 and F2
Q.858
SO2 and I2 vapour is released.
Q.859
HCl, HBr and HI
Q.860
H2S
Q.861
All can be oxidised.
Q.862
Formation of white ppt of Cu2I2
Q.863
I2 is formed
Q.864
K2HgI4
Q.865
HgI2 → K2HgI4
Q.866
I
Q.867
It forms free iodine, which is detected by starch.
Q.868
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CHEMISTRY
Q.869
NO
Q.870
+1
Q.871
Al, Zn
Q.872
NO2, NO3
Q.873
NO2
Q.874
HNO2 i.e. formed releasing NO.
Q.875
Pale, Blue
Q.876
NO2
Q.877
Ba3(PO4)2
Q.878
Sulphide
Q.879
PbSO4, BaSO4, Ag2SO4, HgSO4.HgO
Q.880
HgSO4.HgO
Q.881
(NH4)2MO4
Q.882
(NH4)6Mg7O24.4H2O
Q.883
(NH4)3 [P(MO3O10)4]
Q.884
Canery yellow
Q.885
Yellow ppt of ferric phosphate is formed.
Q.886
White gelatinous ppt of zirconyl phosphate is formed.
Q.887
Phosphate and arsenate
Q.888
CO, CO2, H2O vapours
Q.889
Blue
Q.890
Redox takes place.
Q.891
Orange → Green
Q.892
CH3COO
Q.893
Smell of vinegar is evolved.
Q.894
Silver acetate
Q.895
CH3COO
Q.896
FeCl3
Q.897
{Fe3(OH)2(CH3COO)6}+
Q.898
Fe(OH)2 (CH3COOH)
Q.899
Formate
Q.900
(C2O42)
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