inorganic paper
TRANSCRIPT
INORGANIC PAPER
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P. JOYIIT-JEE
CHEMISTRY P. JOY
Q.1 Reactions of aluminium with
1. O2
2. N2
3. Cl2
4. Cr2O
3
5. Mn3O
46. HCl
7. H2SO
4(Dil.) 8. H
2SO
4 (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 Al2Cl
6 is prepared.
Q.19 How Al2O
3 can be converted into Al
2Cl
6
Q.20 In which conditions does Al2Cl
6 exist.
Q.21 What happens when Al2Cl
6 dimer is added to water.
Q.22 Are the bonding states of Al2Cl
6 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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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� -ions
Q.28 What happens when Al2Cl
6 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 Al
2O
3 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 ?
INORGANIC PAPER
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Q.59 What is the shape of C60
?
Q.60 Which acid anhydride is carbon sesquioxide C3O
2 ?
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. H2SO
4 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 SiO
2 is 3D network solid ?
Q.76 What are the nature of CO2, SiO
2, GeO
2, SnO
2, PbO
2 ?
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
(d) HF (e) Coke
Q.86 What type of glass is K2O.PbO.4SiO
2 ?
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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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 KNO
2 and O
2 but what happens when KNO
3 is heated with SiO
2 ?
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 Na2SiO
3. CaSiO
3.4SiO
2 ?
Q.104 What do you call K2O.CaO.4SiO
2 ?
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(SiH
3)
3 ?
Q.112 How the name silicone is derived for the polymer R2SiO ?
Q.113 Why CO2 is a gas while SiO
2 is a solid ?
Q.114 Why CCl4 does not hydrolyse but SiCl
4 ?
Q.115 How tin is purified ?
Q.116 Which oxide of tin (SnO, SnO2) is/are amphoteric ?
Q.117 Why heating of SnC2O
4 does not yield SnO instead of SnO
2 ?
Q.118 What happens when SnO2 is reacted with (i) H
2SO
4 (ii) NaOH
Q.119 What happens when SnCl2.2H
2O crystals are heated ?
Q.120 Which of the two SnCl2 or SnCl
4 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 & NH
3 ?
Q.123 What is the double salt of SnCl4 with NH
3 ?
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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Q.126 Which property of tin makes it useful for tinning of utensils ?
Q.127 What happens when AuCl3 is treated with SnCl
2 ?
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, SnBr
4, SnI
4 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 CF
62� 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 PbCl
4 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 What type of π bond is present in POX3.
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Q.156 What happens when Ca3N
2 and Ca
3P
2 are added to water ?
Q.157 What happens when Zn3As
2, Zn
3Sb
2, Zn
3Bi
2 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, PH
3, AsH
3, SbH
3
Q.160 Arrange following hydrides in the increasing order of their thermal stability NH3, PH
3, AsH
3, SbH
3, BiH
3
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 NH
3 has
higher b.p. than PH3 and AsH
3 ?
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, AsCl
3, SbCl
3, BiCl
3
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 ?
INORGANIC PAPER
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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. H
2SO
4, CuSO
4, AgNO
3 are reduced by white phosphorous ?
Q.190 What happens when white phosphorous is reacted with following nonmetals (a) Cl2, (b) S
8.
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) Ca3P
2, (b) Na
3P.
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 PF
5 are not hydrolysed ?
Q.200 Write the hydrolysis product of following compounds NCl3, PCl
3, AsCl
3, SbCl
3, BiCl
3.
Q.201 Why penlahalide like BiF5 does not exist ?
Q.202 B, Ga, Al, Tl, In [First Ionisation Energy]
Q.203 BF3, BBr
3, BCl
3, BI
3 [Lewis Acid Strength]
Q.204 BCl3, GaCl
3, AlCl
3, InCl
3 [Lewis Acid Strength]
Q.205 B2O
3, Al
2O
3, In
2O
3, Tl
2O
3, Ga
2O
3 [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, PbCl
2, PbBr
2, PbI
2 [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, AsH
3, BiH
3, PH
3, SbH
3 [Basic Strength]
Q.218 NH3, AsH
3, BiH
3, PH
3, SbH
3 [Reducing Character]
Q.219 NH3, PH
3, AsH
3, SbH
3 [Boiling point]
Q.220 NI3, NCl
3, NBr
3, NF
3 [Basic Character]
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Q.221 NH3, AsH
3, PH
3, BiH
3, SbH
3 [Bond Angle]
Q.222 PCl3, SbCl
3, AsCl
3 [Acid Strength]
Q.223 N2O
3, As
2O
3, P
2O
3 [Acidic Strength]
Q.224 N2O
5, As
2O
5, P
2O
5, Bi
2O
5, Sb
2O
5 [Acidic Strength]
Q.225 N2O, N
2O
3, NO, N
2O
4, N
2O
5 [Acidic Strength]
Q.226 P2O
5, Sb
2O
5, As
2O
5, Bi
2O
5, N
2O
5 [Stability]
Q.227 NCl3, AsCl
3, PCl
3, SbCl
3, BiCl
3 [Ease of hydrolysis]
Q.228 PF3, PBr
3, PCl
3, PI
3 [Acid Strength]
Q.229 PF3, PCl
3, PBr
3, PI
3 [Bond Angle]
Q.230 HNO3, H
3AsO
4, H
3PO
4, H
3SbO
4 [Strength and solubility]
Q.231 O, Se, S, Te [Electron Affinity]
Q.232 O, Se, S, Te, Po [Ionisation potential]
Q.233 H2O, H
2S, H
2Te, H
2Se [Reducing power]
Q.234 H2O, H
2S, H
2Te, H
2Se [Bond angles]
Q.235 H2O, H
2S, H
2Te, H
2Se [Stability]
Q.236 H2O, H
2S, H
2Te, H
2Se [Acidic nature]
Q.237 H2O, H
2S, H
2Te, H
2Se [Dipole moment]
Q.238 SO3, TeO
3, SeO
3 [Acidic nature]
Q.239 SO, SO2, SO
3 [Acidic nature]
Q.240 H2SO
3, H
2SeO
3, H
2TeO
3 [Acidic strength]
Q.241 F, Cl, Br, I [Electron affinity]
Q.242 F, Cl, Br, I [Electronegativity]
Q.243 Cl2, Br
2, F
2, I
2 [Bond energy]
Q.244 Cl2, Br
2, F
2, I
2 [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, HClO
3, HClO
4 [Thermal stability]
Q.250 HClO, HBrO, HIO [Thermal stability]
Q.251 HClO3, HBrO
3, HIO
3 [Thermal stability]
Q.252 HClO, HClO2, HClO
3, HClO
4 [Acidic strength]
Q.253 HClO, HBrO, HIO [Acidic strength]
Q.254 HClO, HClO2, HClO
3, HClO
4 [Oxidising power]
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Q.255 MF, MCl, MBr, MI [Ionic character]
Q.256 I3+, I
3�, H
5IO
6, I
2O
5, I� [Oxidation number]
Q.257 HClO3, HClO
4, HClO
2, HClO [Acidic strength]
Q.258 I2, HI, HIO
4, ICl [Oxidation number]
Q.259 He, Ar, Ne, Kr, Xe [Polarizability]
Q.260 He, Ar, Ne, Kr, Xe [Solubility in water]
Q.261 XeF2, XeF
4, XeF
6 [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.
Q.270 Why NH3(l) is a better solvent for organic compounds but generally a poorer one for ionic inor-
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)
2Cr
2O
7 is heated.
Q.276 What are the gases produced when NH4NO
3(s) is dissociated.
Q.277 What are the gas as produced when NH4NO
3(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).
Q.281 Equimolar mixture of which two oxides of nitrogen on condensing at how temperature gives N2O
3,
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 N2O
4 is diamagnetic or paramagnetic.
Q.285 What is the anhydride of nitric acid.
Q.286 In which state (liquid, gas, vapour, solid) covalent N2O
5 molecules are present.
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Q.287 Complete the following reaction
Fe(CO)5 + NO
50º
Pr
C
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
P
OHH
Hypophosphorous acid
O
H
Ag+
Ag
Cr O2 72–
C r+3
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 H3PO
2.
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 NH2CONH
2 is treated with HNO
2. Write the balanced equa-
tion.
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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 N2O
4 is dissolved in water.
Q.314 When HNO3 is dissolved in pure H
2SO
4, an active agent is formed which has an important applica-
tion in organic chemistry. Name the agent.
Q.315 What are the two oxides of phosphorus.
Q.316 Which compound is formed when P2O
3 combines with oxygen.
Q.317 What happens when P2O
3
(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 N
2O
5 and H
2SO
4 to SO
3.
Q.321 What happens when P2O
5
(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 N
2, 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.
N2
H
Haber process
2 → NH3
O2 → NO O H O2 2+ → HNO
3(aq)
(I) (II) (III) (IV)
Name the process by which II is converted into III.
Q.325 Complete the following reaction
4NH3(g) + 3O
2(g) l
Q.326 At 750�900ºC 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.
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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 O
2.
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, O
2+, O
2�, O
22�
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 Na2O
2 ?
Q.351 Arrange the following oxides in increasing order of their acidic property.
ZnO, Na2O
2, P
2O
5, 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 O
2.
Q.362 Give two applications of ozone.
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Q.363 To which group of the periodic table, ozone belong ?
Q.364 Can ozone oxidises
(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 O�O 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� + H
2O →
Q.374 In which phase hydrogen bonded molecules of H2O
2 are found.
Q.375 Which is more associated via hydrogen bonding i.e. H2O or H
2O
2.
Q.376 What is the structure of the molecule of H2O
2.
Q.377 Which has more density H2O or H
2O
2
Q.378 What is the limitations of H2O
2 which inhibits its utility as an ionizing solvent.
Q.379 Is H2O
2 is more acidic than H
2O in dilute aq. solution.
Q.380 H2O
2 acts as oxidizing agent or reducing agent towards MnO
4�
Q.381 In which type of solution (acid or basic), oxidations with H2O
2 is slow.
Q.382 In which type of solution (acid or basic) disproportionation of H2O
2 occurs most rapidly
Q.383 Which free radicals are formed by metal ion catalysed decomposition of H2O
2.
Q.384 Identify the products of the following reaction
BaO O2 → BaO2 H SO2 4 → A + B.
Q.385 Give the structure and name of the reactant involved in the synthesis of H2O
2 by the reaction
given below.
Reactant O 2
H 2/Pd .
O
O
C H2 5
+ H2O
2
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Q.386 Consider the following reaction
H2O
2(l) → H
2O(l) + ½O
2∆G = � 121.4 kJ mol�1
Is water or oxygen is thermodynamically unstable with respect to H2O
2.
Q.387 Which acid on hydrolysis give H2O
2. Write a chemical equation.
Q.388 Arrange the following O2, H
2O and O
3 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 :
(i) 2S + Cl2 Boil →
(ii) 3S + P4 ∆ →
(iii) 2S + C 1200 1400− →K
Q.396 What compound is formed when sulphur reacts with NH3 in presence of H
2S 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 H2SO
4.
Q.402 What is oxidation state of sulphur in SO2 & SO
3 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 H
2S.
Q.408 Why coordination compounds of H2S are very rare.
Q.409 H2S in large doses prove fatal. What is antidote of H
2S.
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 H2SO
4 by contact process.
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Q.413 What is the strength of H2SO
4 produced by chamber process.
Q.414 By which process 100% pure H2SO
4 is obtained.
Q.415 Which removes impurities of arsenic in contact process.
Q.416 Why SO3 is never directly dissolved in H
2O to form H
2SO
4.
Q.417 Write down the chemical reactions taking place in contact process.
Q.418 H2SO
4 has low volatility. Why ?
Q.419 Name the two series of salts formed by H2SO
4.
Q.420 How many oxygen atoms in H2SO
4 are linked to sulphur by single covalent bonds.
Q.421 What is the oxidation state of sulphur in H2SO
4.
Q.422 Which type of bond is responsible for associated structure of H2SO
4.
Q.423 It is suggested that to dilute conc. H2SO
4, always add conc. H
2SO
4 to water and never water to
conc. H2SO
4. Why ?
Q.424 Why conc. H2SO
4 is used extensively to prepare other acids.
Q.425 Why H2SO
4 has great affinity for water.
Q.426 What are the functions of H2SO
4 in the reaction given below.
2Ag + H2SO
4 → Ag
2SO
4 + 2H
2O + SO
2
Q.427 Why sugar becomes black when it comes in contact with conc. H2SO
4.
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 Na2S
2O
3.
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 Na2S
2O
3.
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 + H
2SO
4 ∆ →
(ii) 2NaCl + H2SO
4 ∆ →
Q.441 Which hydrogen halide is liquid at room temperature.
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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 → H
2NO
3+ + 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 KHF
2.
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, HClO
3, HClO
4
Q.460 What is the oxidation state of chlorine in hypochlorous acid.
Q.461 Consider the following reaction
HClO2 → HOCl → ½Cl
2
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.
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Q.465 Salts (0.1 M solution) of which oxyacid of chlorine is most basic ?
Q.466 Consider the following reaction
NH3 + NaOCl → X + NaOH
X + NH3 + OH� Gum → H
2N � NH
2 + Cl� + H
2O
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, HClO
3, HBrO
3
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 + H
2O → Ca(OH)
2 + Cl
2
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 (H2SO
4, HCl, HNO
3) reacts with CaOCl
2.
Q.485 What do you mean by available Cl2.
Q.486 Why CaOCl2 uses as a disinfectant.
Q.487 Why CaOCl2 gives Cl
2 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 ?
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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. H2SO
4 is added on NaCl and MnO
2.
Q.505 What happens when K2MnF
6 is reacted with SbF
5.
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 Cl
2
(c) S8 reacted with F
2
(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 UF
4 ?
Q.512 What happens when
(i) CaF2 + H
2SO
4 con. ∆ → (ii) NaCl + H
2SO
4 conc. ∆ →
(iii) H2 + Br
2 Pt as bijects)( → (iv) 2I
2(s) + N
2H
4
∆ →5731K
(v) I2 + H
2S ∆ →
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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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 H
2O
2 & ClO
2
Q.520 How HClO3 can be obtained by Ba(ClO
2)
2
Q.521 How Ba(ClO3)
2 can be prepared. [What happens when Cl
2 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 NH4ClO
4 ?
Q.524 How NH4ClO
4 can be obtained from NaClO
4
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, IF
5, BrF
3, ClF, IF
2, BrF
5, ClF
3
Q.541 Why ICl3 exist in form of dimers (I
2Cl
6). 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 :
(i) I2 + ICl
AlCl3 →∆
(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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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 226Ra. Write a chemical reaction.
Q.559 In which year real chemistry of noble gases began.
Q.560 Bartlett had noticed that PtF6 reacts with oxygen to form O
2+ [PtF
6]� & then he reasoned that
PtF6 would react with xenon to form Xe+[PtF
6]� 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) + 2H
2O(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-
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 :
(i) Xe + F2
Ni
K atm →673 1,
(ii) Xe + 2F2
Ni
K atm →
−673 5 7, (iii) Xe + 3F
2
Ni
K atm →
−673 60 70,
2 : 1 1 : 5 1 : 20
Q.570 Complete the following reaction : XeF6 + 3H
2O →
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.
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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) IBr
2� (c) BrO
3�
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 pur-
poses.
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 XeF
6
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 XeF
6
Q.592 Which species is formed when XeF4 react with SbF
5. Give a chemical reaction : XeF
4 + SbF
5 →.
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) Na2CO
3(d) Ca(NO
3)
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) C
2H
5OH (c) Diethyl ether (d) Acetone
Q.603 M(g) → M+(g)
+ e� is most favourable in
(a) Cs (b) Li (c) Na (d) K
Q.604 Which is a characteristic of alkali metal
(a) Conductivity (b) High I.P. (c) Low O.P. (d) High m.p., b.p.
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Q.605 It same molar amount of lithium, sodium & potassium are dissolved in water and the heat released
are measured Q1, Q
2 & Q
3. Which of the following relations are correct.
Li
Q 1
Na
Q 2
K
Q 3
(a) Q1 > Q
2 > Q
3(b) Q
1 < Q
2 < Q
3(c) Q
1 = Q
2 = Q
3(d) Q
2 > Q
1 > Q
3
Q.606 M + H2O → MOH + ½H
2
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) K
2O
2(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 ?
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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, Na
2O, K
2O, Rb
2O.
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 Na
2O
2. He dipped red litmus paper into freshely
prepared solution of water and found litmus decolouried, solid is
(a) Na2O
2(b) Na
2O (c) NaO
2(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) Na
2O (c) KO
2
Q.642 Which of following has highest bond order among O22�, O
2�, O
2, O2�
Q.643 Predict the magnetic nature of following ?
(a) Na2O
2(b) KO
2(c) O
2(d) Na
2O
Q.644 What is oxone chemically ?
Q.645 What is the order of basic strength of following oxides ?
Li2O, Na
2O, K
2O, Rb
2O, Cs
2O
Q.646 Why Na2O
2 & KO
2 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) CO
2 lost (c) Na
2O + CO
2 formed (d) None
Q.650 Why alkali metal carbonates are stable on heating ?
Q.651 Arrange following in order of stability H2CO
3, NaHCO
3, Na
2CO
3
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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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 Na
3N 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 Li2CO
3 is strongly heated till 500ºC.
(a) H2O vapours are formed (b) H
2O, Li
2O, CO
2
(c) Li2O, CO
2 only (d) None
Q.664 Why Li2CO
3 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 Na2CO
3 & CaCO
3 differenting react on heating ?
Q.669 How will you make distinction between Na2O and Na
2O
2.
Q.670 What happens. When Li2CO
3 & Na
2CO
3 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 Na2CO
3, NaHCO
3 ?
Q.674 What happens when Na2CO
3 . NaHCO
3.2H
2O 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
(c) Ammonated e�
(d) Ammonated metal ion (e) NaLi
Q.680 What organic application of Na in NH3(l) ?
Q.681 Na+NH3(l) observation are
(a) Blue colour (b) Strong reducing agent
(c) Produce NaNH2
(d) Produce H2
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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 (c) Diglyme
(d) RNH2
(e) Ethers
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 Cs2CO
3, Rb
2CO
3, K
2CO
3, Na
2CO
3, Li
2CO
3 (increasing order of stability of carbonates)
Q.707 CsHCO3, RbHCO
3, KHCO
3, NaHCO
3, LiHCO
3 (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, Na
2O, K
2O, Rb
2O < Cs
2O (Increasing order of basic nature)
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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 + P4O
10 →
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 + CO
2 → X
(excess) (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)
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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, MgCO
3, CaCO
3,SrCO
3, BaCO
3 (Thermal stability)
(ii) CaSO4, SrSO
4, BaSO
4 (Solubility)
(iii) Ca(C2O
4)
2, Sr(C
2O
4)
2, Ba(C
2O
4)
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.MgCO
3 + 2H
2SO
4 → CaSO
4 + MgSO
4 + 2H
2O + 2CO
2
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 contain-
ing CaSO4 & MgSO
4 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.
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CHEMISTRY P. JOY
Q.764 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 AgClO
4 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 MnO
4� 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 H2O
2 is added to an acidified solution of K
2Cr
2O
7
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(H
2O)
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� (b) [Cr(en)
3]3+ (c) Ni(CO)
4(d) [Fe(H
2O)
6]2+
Q.788 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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CHEMISTRY P. JOY
Q.789 One mol of the aqueous solution of the complex CoCl3.5H
2O 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(H
2O)
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+ (e) Ti2+
(f) V3+ (g) Mn2+ (h) Ni2+ (i) Na+ (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 MnO
4� 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, Cr
2O
3, CrO
3, CrO.
Q.802 What is oxidation number of Cr in CrO2Cl
2.
Q.803 What is oxidation number of Cr in CrO5 or CrO(O
2)
2
Q.804 What is oxidation number of Cr in (NH4)
2Cr
2O
7
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) Cr2O
72�
Q.807 H2O
2 can be oxidised to O
2 by MnO
4� in acidic as well as in basic medium. Write reactions
Q.808 What happens when CO2 gas is passed into MnO
42� 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 FeCl
3 solution, yellow colour of FeCl
3 changes to light green.
Explain
(b) Same behaviour is also observed when SnCl2 solution is observed. Explain.
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CHEMISTRY P. JOY
Q.811 Given chemical tests for making distinction between Fe2+ and Fe3+ ions.
Q.812 When K2HgI
4 reacts with NH
3, 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 K2Cr
2O
7 paper when it is treated with SO
2.
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, SO
3�, Br�, I�, Cl� whose barium salts or silver salts are dissolved by dil. acids.
Q.834 In which case CrO2Cl
2 test can't be employed.
Q.835 Which cation should be absent when CrO2Cl
2 test is employes.
Q.836 Which anion other than halide should be absent when CrO2Cl
2 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. H2SO
4.
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.
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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 H2SO
4 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. H2SO
4 which vapor and gas are released.
Q.859 Which hydrogen halide among HCl, HBr, HI can reduce H2SO
4 into SO
2.
Q.860 When iodides are treated with H2SO
4 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 NH
3 gas.
Q.872 Which anions show brown ring complex with FeSO4.
Q.873 Which gas is evolved when NO3� is decomposed by conc. H
2SO
4
Q.874 What happens when NO2� are treated with dil. H
2SO
4.
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 Ba
3(PO
4)
2
Q.878 What happens when BaSO4 ppt is reduced by charcoal in presence of Na
2CO
3.
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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 C2O
42� is reacted with conc. H
2SO
4.
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 C2O
42�
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 O
2 catalysis.
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SOLUTIONS
Q.1
1. 2Al + 3O2 → Al
2O
3
2. 2Al + N2 → 2AlN
3. 2Al + 3Cl2 → 2AlCl
3
4. Al + Cr2O
3 → Al
2O
3 + Cr
5. Al + Mn3O
4 → Al
2O
3 + Mn
6. Al + HCl → AlCl3 + H
2
↓H2O
Al(OH)3 + 3HCl
7. 2Al + 3H2SO
4(dil) → Al
2(SO
4)
3 + 6H
2
8. 2Al + H2SO
4(conc.) → Al
2(SO
4)
3 + SO
2 + H
2O
9. Al + HNO3 → No reaction
10. Al + NaOH → Al(OH)3 +
3
2H
2
11. 2Al + AlCl3 High Temp. → 3AlCl
Q.2
1. Al(OH)3 + 3H+ → Al+3 + 3H
2O
acid
2. Al(OH)3 + NaOH → Na[Al(OH)
4] or NaAlO
2.2H
2O
base sodium meta aluminate
3. Al(OH)3 Below C450º → Al
2O
3 (α-form)
4. Al(OH)3 Above C450º → Al
2O
3 (γ-form)
Q.3 M(I) M'(III) (SO4)
2.12H
2O
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.
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Q.12 An aqueous solution containing equimolar amount of Al2(SO
4) and K
2SO
4 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 Al2SO
4.18H
2O
Q.16 Al(OH)3 + 3H+ → Al+3 + 3H
2O
acid
Al(OH)3 + NaOH → Na[Al(OH)
4] or NaAlO
2.2H
2O
base sodium meta aluminate
Q.17 Al(OH)3
→ Gelatinous white ppt.
Zn(OH)2 → white ppt.
Q.18 It is prepared by passing dry chlorine over aluminium powder.
Q.19 Al2O
3 + 3C + 3Cl
2 → 2AlCl
3 + 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 + 3H
2O → 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� → [AlCl
4]�
Q.28 Al2Cl
6 + LiH (excess) →Li[AlH
4]
Q.29 Al2O
3
Q.30 α-Al2O
3, β-Al
2O
3
Q.31 α-Al2O
3
Q.32 Al + Fe2O
3 → Al
2O
3 + Fe + heat
Q.33 2Al2O
3 + 2AlCl
3 → 6AlCl + 3O
2
Q.34 α-form
Q.35 γ-Al2O
3
Q.36 The strength of C�C bond is very high.
Q.37 Pb
Q.38 Graphite
Q.39 CO
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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 ⇔840
β-Quartz ⇔ Tridymite ⇔1600ºC
cristobalite
Q.45 α-Sn ⇔15ºC
β-Sn ⇔160ºC
Rhombic Sn
Q.46 α-Sn ⇔15ºC
β-Sn ⇔160ºC
Rhombic Sn
Q.47 The conversion of white tin (β-Sn) is accompainied by an increase in volume and the letter, being
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, C
3O
2
Q.52 H2CO
3
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 CaC2 + N
2 1300ºC → CaCN
2
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Q.68 CaCN2 HOH → Ca(OH)
2 + H
2N � CN
BH2O
H N C NH
O
2 2− −||
urea
Q.69 CaCN2 + 2NaCl
Coke →∆
CaCl2 + NaCN + N
2
Q.70 K4Fe(CN)
6 ∆ → 4KCN + Fe + N
2
Q.71 2KCN + H2SO
4 → 2HCN + 2K+ + SO
4�2
Q.72 Alkaline
Q.73 HCN O2 → N ≡ C � C ≡ N
HCN Cu2+ → Cu(CN)
2 + NaCN
HCN Ag →
Q.74 Cl2 + NaOH → OCl+ + Cl�
(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, SiO
2 Acidic
GeO2, SnO
2 Amphoteric
PbO2 Basic
Q.77 Pb(NO3)
2 ∆ → PbO + NO
2
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 → K
2SiO
3 + H
2O
CaCO3 + SiO
2 → CaSiO
3 + CO
2
2KNO3 + SiO
2 → K
2SiO
3 + 2NO
2 + ½O
2
SiO2 + 6HF → H
2SiF
6 + 2H
2O
C + SiO2 → CO
2 + Si
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Q.86 Flint
Q.87 Super cooled liquid, pseudo solid.
Q.88 SiO2 + 6HF → H
2SiF
6 + 2H
2O
Q.89 Fluoro siliclic acid.
Q.90 Na2SiO
3.CaSiO
3.HSiO
2
Q.91 Na2SiO
3.H
2O
Q.92 When transition metals are added into soda glass solution. Different type of colour are obtained.
Q.93 Silanes Sin H
2n + 2
German Gen H
2n + 2
Q.94 Vertex of silica is formed.
Q.95 Si + 2NaOH → NaSiO3 + H
2↑
Q.96 HF
Q.97 Silanes Alkanes
Toxic Not
Autocombust Not
Reducing agent Not
Unstable Stable
Q.98 KNO3 + SiO
2 → K
2SiO
3 + 2NO
2 + ½O
2
Q.99 HF
Q.100 Corundum (α−Al2O
3) and Carborundum (SiC)
Q.101 Glass
Q.102 SiO2
Q.103 Soda glass
Q.104 Hard glass
Q.105 SiO4�4, BO
3�3
Q.106 Flint glass
Q.107 Stops U.V. light
Q.108 Pyrex glass
Q.109 CaCO3 + Na
2CO
3 + SiO
2 + H
3BO
3 ∆ → borosilicate gass
Q.110 Trimethyl amines sp3, Trisilyl amine sp2 hybridization
Q.111 N(CH3)
3
Q.112 Polymeric organocompounds contain Si�O�Si bonds therefore known as silicones.
Q.113 SiO2 form
Q.114 C does not have 3d orbitals.
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Q.115 Tin is purifyed by electrolytic method
Q.116 Both SnO and SnO2
Q.117 SnC2O
4 ∆ → SnO + CO + CO
2
Oxidation of SnO to SnO2 is checked by CO
Q.118 SnO2 NaOH → Na
2SnO
3
SnO2 H SO2 4 → H
3SnO
3 stannic acid
Q.119 SnCl2.2H
2O ∆ → Sn(OH)Cl
Q.120 SnCl4
Q.121 SnCl4.5H
2O
Q.122 SnCl2.2NH
3
Q.123 SnCl4.4NH
3
Q.124 HgCl2 + SnCl
2 → Calamel
Q.125 SnF2
Q.126 Does not reacts with organic acids.
Q.127 3SnCl2 + 2AuCl
3 → 3SnCl
4 + 2Au
Q.128 3SnCl2 + 2AuCl
3 → 2Au+ + 3SnCl
4 H O2 → Sn(OH)
4
Q.129 SnCl4.5H
2O H O2 → Sn(OH)Cl
Butter of Tin
Q.130 Sn + HNO3 → H
3SnO
3
Q.131 SnI4 → yellow, SnCl
4 and SnBr
4 coloured
Q.132 SnO + 2HF → SnF2 + H
2O
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, Pb
2O
3, Pb
3O
4
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 Fajan's rule
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Q.140 (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)
Q.141 Group V elements have ns2-np
3 general configurator which is a half filled orbital having extra
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), NH
2-NH
2(�2), NH
2OH(�1), N
2(0), N
2O(+1), NO(+2), N
2O
3(+3), NO
2(+4), N
2O
5(+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 M
4
Q.155 pπ -dπ
Q.156 Ca3, N
2 H O2 → NH
3
Ca3P
2 : H O2 → PH
3
Q.157 Ca3P
2 + 6HOH → 3CO(OH)
2 + 2PH
3 phosphene
Ca3N
2 + 6H
2O → 3Ca(OH)
2 + 2NH
3
Zn3As
2 + 6H
2O → 3Zn(OH)
2 + 2AsH
3
Q.158 Hydrazine
Q.159 NH3 > PH
3 > AsH
3 > SbH
3
Q.160 NH3 > PH
3 > AsH
3 > SbH
3 > BiH
3
Q.161 BiH3
Q.162 NH3
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Q.163 NH3 has H-bonding.
Q.164 NH3 > PH
3 > AsH
3 > SbH
3 > BiH
3
Q.165 BiX3
Q.166 Pyramidal
Q.167 PCl3 + HOH → H
3PO
3 + 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 [PCl
4+] [PCl
6�]
Q.174
Q.175 Ca(PO4)
2 + C → CaCO
3 + 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 → Ca3P
2 or Mg
3P
2
P + Na or K → Na3P or K
3P
Q.185 Highly reactive, burshing into Hames when exposed to air.
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Q.186 P O2 → P2O
3
Q.187 PH3 & NaH
2PO
2
Q.188 Reducing agent
Q.189 P + HNO3 → H
3PO
4 + NO
2
P + Conc H2SO
4 → H
3PO
4 + SO
3
P + CuSO4 → Cu
3P
3
P + AgNO3 → Ag
3P
2 + HNO
3
Q.190 P PCl5 → PCl5
P S8 → P4S
3
Q.191 White
Q.192 (a) Ca3P
2 + 6H
2O → 3Ca(OH)
2 + 2PH
3
(b) Na3P + H
2O → NaOH + PH
3
Q.193 AlP H O2 → PH3 ↑ + Al(OH)
3
Q.194 H3PO
3 ∆ → PH
3 + H
3PO
4
Q.195 P4 + 3NaOH + 3H
2O → PH
3 + 3NaH
2PO
2
Q.196 Ring of N2O
5 are known as vertex ring. During formations of PH
3, PH
3 is oxidized by O
2 and forms
P2O
5
Q.197 P4 + NaOH → Na
2HPO
4 + PH
3↑
PH3 + O
2 → HPO
3
PH3 + O
2 → P
2O
5 + H
2O
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 NCl3 H O2 → X
PCl3 H O2 → H
3PO
3
AsCl3 H O2 → As
2O
3
SbCl3 H O2 → Sb OCl
BiCl3 H O2 → 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 < BCl
3 < BBr
3 < BI
3
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Q.204 BCl3 < AlCl
3 < GaCl
3 < InCl
3
Q.205 B2O
3 < Al
2O
3 < Ga
2O
3 < In
2O
3 < Tl
2O
3
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 > PbCl
2 > PbBr
2 > PbI
2
Q.214 Si < C < Ge < Sn < Pb
Q.215 N < P < As > Sb > Bi
Q.216 N < P < As < Sb > Bi
Q.217 NH3 > PH
3 > AsH
3 > SbH
3 > BiH
3
Q.218 NH3 < PH
3 < AsH
3 < SbH
3 < BiH
3
Q.219 PH3 < AsH
3 < NH
3 < SbH
3
Q.220 NI3 > NBr
3 > NCl
3 > NF
3
Q.221 NH3 > PH
3 > AsH
3 > SbH
3 > BiH
3
Q.222 PCl3 > AsCl
3 > SbCl
3
Q.223 N2O
3 > P
2O
3 > As
2O
3
Q.224 N2O
5 > P
2O
5 > As
2O
5 > Sb
2O
5 > Bi
2O
5
Q.225 N2O < NO < N
2O
3 < N
2O
4 < N
2O
5
Q.226 P2O
5 > As
2O
5 > Sb
2O
5 > N
2O
5 > Bi
2O
5
Q.227 NCl3 > PCl
3 > AsCl
3 > SbCl
3 > BiCl
3
Q.228 PF3 > PCl
3 > PBr
3 > PI
3
Q.229 PI3 > PBr
3 > PCl
3 > PF
3
Q.230 HNO3 > H
3PO
4 > H
3AsO
4 > H
3SbO
4
Q.231 O < S > Se > Te
Q.232 O > S > Se > Te > Po
Q.233 H2O < H
2S < H
2Se < H
2Te
Q.234 H2Te < H
2Se < H
2S < H
2O
Q.235 H2O > H
2S > H
2Se > H
2Te
Q.236 H2O < H
2S < H
2Se < H
2Te
Q.237 H2O > H
2S > H
2Se > H
2Te
Q.238 SO3 > SeO
3 > TeO
3
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Q.239 SO > SO2 > SO
3
Q.240 H2TeO
3 < H
2SeO
3 < H
2SO
3
Q.241 F < Cl > Br > I
Q.242 F > Cl > Br > I
Q.243 Cl2 > Br
2 > F
2 > I
2
Q.244 F2 > Cl
2 > Br
2 > I
2
Q.245 HI > HBr > HCl > HF
Q.246 HI > HBr > HCl > HF
Q.247 HF > HI > HBr > HCl
Q.248 H�F > H�Cl > H�Br > H�I
Q.249 HClO4 > HClO
3 > HClO
2 > HClO
Q.250 HClO > HBrO > HIO
Q.251 HClO3 < HBrO
3 < HIO
3
Q.252 HClO4 > HClO
3 > HClO
2 > HClO
Q.253 HClO > HBrO > HIO
Q.254 HClO4 < HClO
3 < HClO
2 < HClO
Q.255 MF > MCl > M�Br > MI
Q.256 I� < I3� < I
3+ < I
2O
5 < H
5IO
6
Q.257 HClO < HClO2 < HClO
3 < HClO
4
Q.258 HI < I2 < ICl < HIO
4
Q.259 He < Ne < Ar < Kr < Xe
Q.260 Xe > Kr > Ar > Ne > He
Q.261 XeF6 < XeF
4 < XeF
2
Q.262 Concentration solution of NH3 is water.
Q.263 Hydrogen bonding.
Q.264 Yellow flame.
Q.265 Yes NH3 + O
2 → N
2 + H
2O
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 sub-
stances.
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Q.271 AgI has covalent bond so it is insoluble in water but it is soluble in NH3 due to complex formation.
AgI + 2NH3 l [Ag(NH
3)
2]+
Q.272 NH4+ + NH
2�
Q.273 Acid - base
Q.274 Reducing agent.
Q.275 N2 + H
2O
Q.276 NH3 + HNO
3
Q.277 N2O + H
2O
Q.278 Linear
Q.279 One
Q.280 2p
Q.281 NO + NO2
Q.282 NO2
Q.283 NO2
Q.284 Diamagnetic
Q.285 N2O
5
Q.286 Vapour
Q.287 Fe(CO)5 + NO
50º
Pr
C
essure → [Fe(CO)
2 (NO)
2]
Q.288 [Fe(H2O)
5NO]SO
4
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, HNO
3
Q.302 Oxidising, reducing, complex forming ability
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Q.303 HNO3
Q.304 NO2 dissolved in concentrated HNO
3
Q.305 aq. solution
Q.306 HNO3
Q.307 Birkeland Eyde & ostwald
Q.308 Nitrate ion.
Q.309 Urea.
Q.310 H4N
2O
4 & HNO
4
Q.311 By direct oxidation of NH3 using Pt as a catalyst.
Q.312 P2O
5
Q.313 HNO2 + HNO
3
Q.314 NO2+
Q.315 P2O
3, P
2O
5
Q.316 P2O
5
Q.317 (i) P2O
3 + 3H
2O → 2H
3PO
2
(ii) 2P2O
3 + 6H
2O → 3H
3PO
3 + PH
3
Q.318 P2O
5
Q.319 P2O
3
Q.320 P2O
5
Q.321 (i) P2O
5 + H
2O → 2HPO
3
(ii) P2O
5 + 3H
2O → 2H
3PO
4
Q.322 Chloramine NH2Cl [2NH
3 + Cl
2 → NH
4Cl + NH
2Cl]
Q.323 Hydrazine
Q.324 Ostwald Process.
Q.325 2N2(g) + 6H
2O(g)
Q.326 NO
Q.327 O2, O
3
Q.328 (i) 2KClO3(s)
∆ →MnO2
3O2(g) + 2KCl(s)
Q.329 CO2 + SO
2
Q.330 Sodium peroxide Na2O
2
Q.331 Pale Blue
Q.332 F2O
Q.333 NO
Q.334 No vacant d-orbital.
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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, B
2O
3
Q.345 2H2S + O
2 → 2H
2O + 2S O2 → SO
2
Q.346 8
Q.347 O2+ > O
2 > O
2� > O
2�2
Q.348 O2
Q.349 Yes
Q.350 � 1
Q.351 Na2O
2 > MgO > ZnO > P
2O
5
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, O
3 = 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 + O
3 + H
2O → H
3PO
4 Zero to + 5
Q.368 False
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Q.369 F2
Q.370 Red
Q.371 U.V. Rays
Q.372 Chlorofloro Carbon
Q.373 O3 + 2K+ + 2I� + H
2O → KOH + I
2 + O
2
Q.374 Solid
Q.375 H2O
2
Q.376 Skew, chain structure
Q.377 H2O or H
2O
2
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 + H
2O
Q.385
OH
OH
C H2 5
Q.386 No
Q.387 Peroxodisulfuric acid
Q.388 O2 > O
3 > H
2O
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 (i) 2S + Cl2 Boil → S
2Cl
2
(ii) 3S + P4 ∆ → P
4S
3
(iii) 2S + C 1200 1400− →K CS2
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Q.396 (NH4)
2 S
x
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 + H2SO
4(dil.) → FeSO
4 + H
2S
H2(g) + S(l) → H
2S(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 S�2. It's ligand ability is very weak.
Q.409 Dilute chlorine.
Q.410 H2SO
4, it is used in most of manufacturing process.
Q.411 Contact process, Lead chamber process.
Q.412 Fe(OH)3 remove As
2O
5 in contact process. They absorb As
2O
5 on their surface.
Q.413 95%
Q.414 Contact process.
Q.415 Fe(OH)3
Q.416 SO3 + H
2O → H
2SO
4 it is a violent reaction.
Q.417 S + O2 → SO
2
O
V O
2
2 5
→ SO3 H O2 → H
2SO
4.
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 H2SO
4 is an oxidizing agent thus it can easily oxidised elements in their oxyacids.
Q.425 H2SO
4 can form strong extensive H-bonds.
Q.426 Oxidising agent.
Q.427 C6(H
2O)
6 Conc H SO. 2 4 → 6C + 6H
2O
Black
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Q.428 H2SO
4
Q.429 H2SO
3
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 + H
2O + Na
2S
2O
3 → 2HCl + Na
2SO
4 + S
Q.434 Cl2 + H
2O + Na
2S
2O
3 → 2HCl + Na
2SO
4 + S
Hypo is thus used as an antichlore.
Q.435 Na2S
2O
3
Q.436 Na2S + Na
2S
2O
3 + I
2 → 2NaI + Na
2S
2O
3
Q.437 S4O
6�2 (Tetrathionate)
Q.438 aq. solution of hydrogen halides.
Q.439 Strong affinity for hydrogen.
Q.440 (i) CaSO4 + 2HF(g), (ii) Na
2SO
2 + 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 < HClO
3 < HClO
4
Q.460 +1
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Q.461 Increases.
Q.462 Ba(ClO2)
2 + H
2SO
4 → 2HClO
2 + BaSO
4
Q.463 Chlorites
Q.464 HClO4
Q.465 NaClO
Q.466 X = NH2Cl, chloramine
Q.467 Tetrahedral, sp3
Q.468 O Cl OΘ
− →. .
. .
Q.469 HClO4
Q.470 HClO4 > HClO
3 > HClO
2 > HClO
Q.471 HClO4 > HClO
3 > HClO
2 > HClO
Q.472 HClO3 < HBrO
3 < HIO
3
Q.473 Cl2 + H
2O → H+ + Cl� + HOCl
Q.474 +1 to +7
Q.475 Acidic
Q.476 Cl, Br, I
Q.477 Cl2O least and Cl
2O
7 most acidic.
Q.478 ClO2
Q.479 Ca+2, Cl�, OCl�
Q.480 CaOCl2 + H
2O → Ca(OH)
2 + Cl
2Autooxidation
Q.481 Ca(OH)2, Cl
2
Q.482 It reacts with H2O and convert into Ca(OH)
2 and Cl
2 by auto oxidation.
Q.483 Ca(OH)2 + Cl
2 → Ca(OCl) Cl + H
2O
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 H2SO
4.
Q.487 Autooxidation
Q.488 Mixed salt.
Q.489 35 to 38%
Q.490 Yes
Q.491 Halogen means salt forming.
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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 F
2 otherwise these gases reacts explosively.
Q.501 By passing Cl2 gas into bromide salt solution
Q.502 6H+ + IO3� + I� → I
2 + 3H
2O
Q.503 6H+ + IO3� + I� → I
2 + 3H
2O
Q.504 When H2SO
4 is added to NaCl with MnO
2, Cl
2 is evolved.
Q.505 K2MnF
6 + SbF
5 → K
2SbF
7 + MnF
3 + ½F
2
Q.506 True
Q.507 When halogen has � 1 oxidation state.
Q.508 He, Ne, Ar
Q.509 (a) Mg + Br2(l) → MgBr
2
(b) P4 + Cl
2(g) → PCl
5
(c) S8 + F
2(g) → SF
6
(d) Xe(g)
+ F2(g) → XeF
6
Q.510 Covalent nature
Q.511 UF6
Q.512 (i) CaF2 + H
2SO
4 con. ∆ → CaSO
4 + HF
(ii) NaCl + H2SO
4 conc. ∆ → Na
2SO
4 + HCl
(iii) H2 + Br
2 Pt as bijects)( → HBr
(iv) 2I2(s) + N
2H
4
∆ →5731K
N2 + HI
(v) I2 + H
2S ∆ → HI + S
Q.513 PCl5 + D
2O → POCl
3 + 2DCl
Q.514 Hypochlorite ion
Q.515 Cl2 + H
2O + HgO → HOCl + HCl, HCl is absorbed by HgO
Q.516 NaOCl
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Q.517 Anode → Cl2 gas, Cathode → H
2 and OH� obtain.
Q.518 Ca(OH)2 Cl2 → Ca(OCl)
2. CaCl
2.Ca(OH)
2.2H
2O
Q.519 2Cl2O + 2NaOH + H
2O
2 → 2NaClO
2 + O
2 + 2H
2O
Q.520 Ba(ClO3)
2 + H
2SO
4 → BaSO
4 + 2HClO
3
Q.521 Ba(ClO3)
2 + Cl
2 → Ba(ClO
3)
2
Q.522 THCl.
Q.523 Used in rockets as fuels.
Q.524 NaClO4 + NH
4Cl → NH
4ClO
4 + 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 < IF
5 < BrF
3 < ClF < IF
2 < BrF
5 < ClF
3
Q.541 ICl3 is unstable.
Q.542 I+ → ICl, IBr, ICN, I+3 → ICl3, I(ClO
4)
3.IPO
4.
Q.543 HOI (Hypo iodous acid) HCl.
Q.544 HF, HBrO3 bromic acid.
Q.545 (i) [I3]+ [AlCl
4]�
(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.55888
Ra226 →
86Rn222 +
2He4
Q.559 1962
Q.560 Ionization enthalpies of O2 & Xe are close to each other.
Q.561 [XeF]+ [Pt2F
11]�
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 + 12H
2O → 4Xe + 2XeO
3 + 24HF + 3O
2
Q.569 XeF2, XeF
4, XeF
6
Q.570 XeO3� + 6HF
Q.571 XeOF4 & XeO
2F
2
Q.572 XeO3
Q.573 XeOF4
Q.574 XeO3 = Trigonal pyramidal, XeOF
4 = Square pyramidal.
Q.575 XeO3 + OH� → HXeO
4�
hydrogen xenate ion
Q.576 Perxenate ion XeO64�
Q.577 +8
Q.578 Yellow
Q.579 Oxidising
Q.580 (a) XeF4, (b) XeF
2, (c) XeO
3
Q.581 He non flammable & light gas
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Q.582 Neon
Q.583 He
Q.584 XeF2, XeF
4, XeF
6
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]+ [SbF
6]�
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 → M
2O
Q.611 H2O, Na
2O
2, KO
2, RbO
2, CsO
2
Q.612 (b)
Q.613 Li
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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 Na2SO
4.10H
2O, Na
2SO
4, NaNO
3
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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Q.641 Na2O
2 + H
2O → 2NaOH + H
2O
2
Na2O + H
2O → 2NaOH
KO2 + H
2O → 2KOH + H
2O
2 + O
2
Q.642 O2
Q.643 (a) Na2O
2 diamagnetic (b) KO
2 paramagnetic
(c) O2 paramagnetic (d) Na
2O paramagnetic
Q.644 Na2O
2 + HCl(dil.)
Q.645 Li2O < Na
2O < K
2O < Rb
2O < Cs
2O
Q.646 They easily liberates oxygen.
Q.647 Na2CO
3.10H
2O, Na
2CO
3.7H
2O, Na
2CO
3.H
2O, Na
2O
Q.648 s-block element.
Q.649 (d) Na2O
2 and Na vapour are formed.
Q.650 s-block elements have calculate with high thermal stability due to less polarizing power of cat-
ions.
Q.651 Na2CO
3 > NaHCO
3 > H
2CO
3
Q.652 Cs2CO
3 > ........... > Li
2CO
3
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 � C
5H
5)
2Co+
Q.659 Mg+2
Q.660 Na3N does not exist at room temperature N
3� 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 HClO4.3H
2O
Q.663 (c)
Q.664 Li2CO
3 is stable due to higher polarizing power of lithium.
Q.665 Hydration energy is greater then lattice energy.
Q.666 Due to anion hydrolysis.
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Q.667 LiHCO3, NaHCO
3, KHCO
3, RbHCO
3, NH
4HCO
3
Q.668 Na2CO
3 is stable.
Q.669 Na2O
2 + H
2O → 2NaOH + H
2O
2
Na2O + H
2O → 2NaOH
Q.670 Li2CO
3 decomposed into LiO and CO
2 but Na
2CO
3 does not decomposed.
Q.671 Because all bicarbonates passes H+ as an essential cation which polarises CO3�2 ions and decom-
poses into CO2.
Q.672 All bicarbonates all soluble in water.
Q.673 Na2CO
3 is more basic in aqueous state.
Q.674 Decomposed into 2Na2CO
3 + 2H
2O
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 e�s.
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 By addition T.M. ion Na + NH3(l) Fe3+
→ NaNH2 + ½H
2 ↑
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 223Fr
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.
Low solubility of CsI is due to smaller hydration energy.
Q.696 Due to their high electropositivity.
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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 Li2CO
3 < Na
2CO
3 < K
2CO
3 < Rb
2CO
3 < Cs
2CO
3
Q.707 CsHCO3 < RbHCO
3, KHCO
3 < NaHCO
3 < LiHCO
3
Q.708 MF < MCl < MBr < MI
Q.709 KI > KBr < KCl
Q.710 Li > K > Na
Q.711 Li2O, Na
2O < K
2O, Rb
2O < Cs
2O
Q.712 Li < Na < K < Rb < Cs
Q.713 BLi < Na < K < Rb < Cs
Q.714 BLi < Na < K < Rb < Cs
Q.715 MgSO4.7H
2O
Q.716 Due to the formation of a surface film of the oxide.
Q.717 H2
Q.718 MgO, Mg3N
2
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 + O
2
Q.723 Quick time
Q.724 Disintegration of lump of lime in limited amt. of water.
Q.725 Sodalime.
Q.726 (a) CaO + SiO2 → CaSiO
3
(b) CaO + P4O
10 → Ca(PO
4)
2
Q.727 Ca(OH)2 when water is added to slaked lime.
Q.728 Aq. solution of Ca(OH)2
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Q.729 Milk of lime.
Q.730 It turns milky.
Q.731 Ca(HCO3)
2
Q.732 Ca(ClO)2
Q.733 CaSO4.2H
2O
Q.734 When gypsum CaSO4.2H
2O 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
(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 & MgI
2
Q.741 Ca
Q.742 CaF2
Q.743 (i) BeCO3 < MgCO
3 < CaCO
3 < SrCO
3 < BaCO
3 (increasing thermal stability)
(ii) CaSO4 > SrSO
4 > BaSO
4 (Increasing solubility)
(iii) Ca(C2O
4)
2 > Sr(C
2O
4)
2 > Ba(C
2O
4)
2 (increasing solubility)
Q.744 Ba
Q.745 2Ca(NO3)
2 ∆ → 2CaO + 4NO
2 + O
2
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 MgSO4.2H
2O, MgSO
4.7H
2O
Q.750 By treating with H2SO
4
Q.751 By fractional crystallization
Q.752 MgSO4.7H
2O
Q.753 [Mg(H2O)
6]SO
4.H
2O
Q.754 Potash magnesis is a Fertilizer & Its chemical composition K2SO
4.MgSO
4.6H
2O.
Q.755 Purgative in medicine.
Q.756 Ca2SiO
4, Ca
3SiO
5, Ca
3Al
2O
6
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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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 < CrO
2(OH)
2 acid strength increases with increase in oxidation number.
Q.784 Cr(OH)3 + 3HCl → CrCl
3 + 3H
2O
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(H
2O)
6]3+ has five unpaired
electrons (sp3d2 hybridised Fe3+)
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Q.787 (a) 36 (b) 33 (c) 36 (d) 36
Q.788 I(b), II(a), III(c)
Q.789 [Co(H2O)
4Cl
2]Cl.H
2O
Q.790 [Ni(H2O)
4]2+ > [Fe(CN)
6]2� > [Fe(CN)
6]4� = [Ni(H
2O)
4]2+
Q.791 N N( )+ 2 = 35 ⇒ N = 5 (unpaired electrons) ⇒ x = 3(Fe3+)
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� + H
2O → 5VO
2+ + Mn2+ + 2H+
Q.801 CrO3
Q.802 VI
Q.803 VI (O = � 2 diperoxo = � 4)
Q.804 VI
Q.805 V
Q.806 Cr2O
72� < Cr3+ < Cr2+
Smaller the oxidation state of the element in the ion, greater the reducing nature.
Q.807 2MnO4� + 5H
2O
2 + 6H+ → 2Mn2+ + 5O
2 + 8H
2O
2MnO4� + 3H
2O
2 → 2MnO
2 + 3O
2 + 2OH� + 2H
2O
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Q.808 Aqueous CO2 releases H+ which can convert MnO
42� into MnO
2 and MnO
4� in a disproportionation
reaction.
CO2 + H
2O l H+ + HCO
3�
3MnO42� + 4H+ → MnO
2 + 2MnO
4� + H
2O
Q.809 AgBr + 2Na2S
2O
3 → Na
3[Ag(S
2O
3)
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 Fe3+ gives red brown ppt.
Q.812 2K2HgI
4 + NH
3 + 3NaOH →
Hg
Hg(Iodide of M illon’s base)
brown ppt
O NH 2 I + 4KI + 3NaI + 2H2O
Q.813 70% Cu + 30% Zn
Q.814 75% Cu + 25% Ni
Q.815 60% Ni + 20Fe + 20% Fe
Q.816 NO3�, HCO
3�, CH
3COO�
Q.817 NO3�
Q.818 Na2CO
3
Q.819 CO32�
Q.820 CO2
Q.821 S2� → SO2 and CO
32� → CO
2
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, Br
2, KIO
3, Cu4+, K
2Cr
2O
7, KMnO
4.
Q.831 Reducing agents.
Q.832 ppt dissolves through formation of CO2
Q.833 CO3� and SO
3�
Q.834 In presence of I� and Br�
Q.835 Pb, Ag, Sb, Sn
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Q.836 NO3�, NO
2�, chlorates.
Q.837 Cl2 is evolved as Cr
2O
72� are oxidising agent and oxidises Cl� into Cl
2
Q.838 HCl
Q.839 Cr2F
2, 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, SO
32� 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 H3PO
4�
Q.852 CCl4, CS
2
Q.853 Br� → Br2 (Red)
I� → I2 (violet / purple)
Q.854 Cl2 water, HOCl, NaOCl, conc. HNO
3
Q.855 Redox reaction take place and Br2 is liberated.
Q.856 H2SO
4, HNO
3, MnO
2, PbO
2, Cl
2 water, KMnO
2, NaOCl, HOCl
Q.857 Cl2 and F
2
Q.858 SO2 and I
2 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 Cu2I
2
Q.863 I2 is formed
Q.864 K2HgI
4
Q.865 HgI2 → K
2HgI
4
Q.866 I�
Q.867 It forms free iodine, which is detected by starch.
Q.868 NO
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Q.869 NO
Q.870 +1
Q.871 Al, Zn
Q.872 NO2�, NO
3�
Q.873 NO2
Q.874 HNO2 i.e. formed releasing NO.
Q.875 Pale, Blue
Q.876 NO2
Q.877 Ba3(PO
4)
2
Q.878 Sulphide
Q.879 PbSO4, BaSO
4, Ag
2SO
4, HgSO
4.HgO
Q.880 HgSO4.HgO
Q.881 (NH4)
2MO
4
Q.882 (NH4)
6Mg
7O
24.4H
2O
Q.883 (NH4)
3 [P(MO
3O
10)
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, H
2O 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(CH
3COO)
6}+
Q.898 Fe(OH)2 (CH
3COOH)
Q.899 Formate
Q.900 (C2O
42�)