inorganic paper

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INORGANIC PAPER CHEMISTRY P. JOYQ.1 Reactions of aluminium with

1. O

3. Cl

5. Mn O

2. N

4. Cr O

6. HCl

7. H2SO4(Dil.) 8. H2SO4 (Conc.)

9. HNO

11. AlCl

10. NaOH

Q.2 Reactions of Al(OH)3 with

1. Acid

2. NaOH

3. Heating Below 450°C

4. Heating above 450°C

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.1O 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 Al Cl is prepared.2 6

Q.19 How Al O can be converted into Al Cl2 3 2 6

Q.2O In which conditions does Al2Cl6 exist.

Q.21 What happens when Al Cl dimer is added to water.2 6

Q.22 Are the bonding states of Al Cl in vapour phase and in aqueous phase are different.2 6

Q.23 What is the nature of AlCl in aqueous state.

Q.24 Does AlCl3 on heating melts.

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INORGANIC PAPER CHEMISTRY P. JOYQ.25 Why is it difficult keep AlCl dry

Q.26 Comment on stability of AlCl

Q.27 What happens when AlCl reacted with Cl— -ions

Q.28 What happens when Al2Cl6 is reacted with LiH

Q.29 Which is the most stable compound of aluminium.

Q.3O What are the different forms of alumina.

Q.31 What is corundum.

Q.32 What is thermite reaction.

Q.33 What happens when AlCl vapours are passed over fused Al O at 1000°C.

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.4O 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.5O Which allotrope of carbon is insoluble solvent ?

Q.51 What are the oxides of carbon ?

Q.52 Which acid anhydride is CO ?

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 C in Toluene ?

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INORGANIC PAPER CHEMISTRY P. JOYQ.59 What is the shape of C ?

Q.6O Which acid anhydride is carbon sesquioxide C3O2 ?

Q.61 Which oxide of IV group is not solid ?

Q.62 Which monoxide of IV group does not exist ?

Q.63 Which monoxide of IV group is neutral ?

Q.64 What is the nature of IV group monoxides ?

Q.65 Which IV group oxides are network solids ?

Q.66 Why bicarbonates are alkaline in nature although they has H+ ?

Q.67 How calcium cyanamide can be prepared from CaC2 ?

Q.68 What happens when calcium cyanamide is hydrolysed ?

Q.69 What happens when calcium cyanamide is heated with Coke & NaCl

Q.7O What happens when K Fe(CN) is heated strongly ?4 6

Q.71 What happens when KCN & dil. H2SO4 reacts ?

Q.72 What is the nature of aqueous solution of KCN ?

Q.73 What happens when HCN is oxidised by O , Ag, Cu2+ ?

Q.74 Why (CN)2 is pseudohalide ?

Q.75 Why CO is molecule but SiO is 3D network solid ?

Q.76 What are the nature of CO , SiO , GeO , SnO , PbO ?2 2 2 2 2

Q.77 What happens when Pb(NO ) 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 KMnO ?

Q.8O 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 SiO is reacted (heated) with alkalis and alkali metal carbonates ?

Q.85 What happens when SiO2 is reacted with following ?

(a) KOH (b) CaCO (c) KNO (d) HF (e) Coke

Q.86 What type of glass is K O.PbO.4SiO ?2 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.9O 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 KNO2 and O2 but what happens when KNO3 is heated with SiO2 ?

Q.99 Name an acid which dissolves silica ?

Q.1OO What are corundum and carborundum ?

Q.1O1 What pseudo solids ?

Q.1O2 Which allotrope of Si is isomorphous with carbon ?

Q.1O3 What is Na SiO . CaSiO .4SiO ?2 3 3 2

Q.1O4 What do you call K O.CaO.4SiO ?2 2

Q.1O5 Which type of anions are present in pyrex glass ?

Q.1O6 Which type of glass are prisms and lenses are made up of ?

Q.1O7 What is Crookes glass ? What is its speciality ? Which metal compound is present in it ?

Q.1O8 Which type of glass has lane thermal expansion ?

Q.1O9 How borosilicate glass are obtained ?

Q.11O Why trimethyl amine is pyramidal but trisilyl amine is planar ?

Q.111 Which of two is more basic N(CH ) or N(SiH ) ?

Q.112 How the name silicone is derived for the polymer R SiO ?

Q.113 Why CO2 is a gas while SiO2 is a solid ?

Q.114 Why CCl does not hydrolyse but SiCl ?

Q.115 How tin is purified ?

Q.116 Which oxide of tin (SnO, SnO2) is/are amphoteric ?

Q.117 Why heating of SnC O does not yield SnO instead of SnO ?

Q.118 What happens when SnO is reacted with (i) H SO (ii) NaOH2 2 4

Q.119 What happens when SnCl .2H O crystals are heated ?2 2

Q.12O Which of the two SnCl2 or SnCl4 is a liq. at room temperature ?

Q.121 What is butter of Sn ? What is its major use.

Q.122 What are the addition compounds of SnCl & NH ?

Q.123 What is the double salt of SnCl with NH ?

Q.124 How calamel is produced by SnCl2 ?

Q.125 Which tin compound is used in tooth paste to help tooth decay ?


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INORGANIC PAPER CHEMISTRY P. JOYQ.126 Which property of tin makes it useful for tinning of utensils ?

Q.127 What happens when AuCl3 is treated with SnCl2 ?

Q.128 How PURPLE OF CASIUS is formed ?

Q.129 What happens when butter of tin is hydrolysed with excess of water ?

Q.13O What happens when tin metal is reacted with conc. HNO3 ?

Q.131 Which tin halide out of SnCl , SnBr , SnI is coloured ?4 4 4

Q.132 How Tin (II) fluoride is obtained ?

Q.133 Why Pb has higher I.E. than Sn ?

Q.134 What are various oxides of Pb ?

Q.135 Why do PbCl acts as strong oxidising agent ?

Q.136 SiF 2— exist but not CF 2— explain why ?6 6

Q.137 What is the order of ease of catenation ?

Q.138 How many allotropes of Sn exist ?

Q.139 Why PbCl is ionic where is PbCl is covalent.

Q.14O 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.15O 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 p — p 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 bond is present in POX3.

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Q.156 What happens when Ca3N2 and Ca3P2 are added to water ?

Q.157 What happens when Zn As , Zn Sb , Zn Bi are added to water ?3 2 3 2 3 2

Q.158 Which compound is formed when NH gas is passed into NaOCl solution.

Q.159 Arrange following hydrides in increasing bond angle NH3, PH3, AsH3, SbH3

Q.16O Arrange following hydrides in the increasing order of their thermal stability NH , PH , AsH , SbH , BiH

Q.161 Which hydride of group V is strongest reducing agent ?

3 3 3 3 3

Q.162 Which V group hydride is the weakest reducing agent.

Q.163 On moving down the group generally b.p. of group V hydrides increases except NH3. Why NH3 hashigher b.p. than PH and AsH ?

Q.164 What is order of Lewis base character of V group metal hydrides.

Q.165 Which trihalide of group V elements is not covalent but ionic ?

Q.166 What is the shape of group V trihalides ?

Q.167 Write hydrolysis product of following trihalides PCl3, AsCl3, SbCl3, BiCl3

Q.168 Why nitrogen trihalides cannot be hydrolysed ?

Q.169 Do fifth group trihalides work as Lewis acid ?

Q.17O 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 PCl in gaseous state and in solid state ?

Q.174 Draw the structure of PCl 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.18O 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 CS ?

Q.184 What happenes when phosphorous combine with metals like Ca and Mg, Na and K.

Q.185 Why white phosphorous is kept in water ?

Q.186 Which is formed by the combustion of phosphorous in air ?


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INORGANIC PAPER CHEMISTRY P. JOYQ.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 HNO , conc. H SO , CuSO , AgNO are reduced by white phosphorous ?3 2 4 4 3

Q.19O What happens when white phosphorous is reacted with following nonmetals (a) Cl , (b) S .2 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) Ca P , (b) Na P.

Q.193 How AlP can be decomposed into pH ?

3 2 3

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 PH ? Why these rings are formed ?

Q.197 How vortex rings of PH can be prepared in laboratory.

Q.198 Why NF is not hydrolysed ?

Q.199 Why PF3 and PF5 are not hydrolysed ?

Q.2OO Write the hydrolysis product of following compounds NCl , PCl , AsCl , SbCl , BiCl .

Q.2O1 Why penlahalide like BiF does not exist ?

3 3 3 3 3

Q.2O2 B, Ga, Al, Tl, In [First Ionisation Energy]

Q.2O3 BF , BBr , BCl , BI [Lewis Acid Strength]3 3 3 3

Q.2O4 BCl , GaCl , AlCl , InCl [Lewis Acid Strength]3 3 3 3

Q.2O5 B O , Al O , In O , Tl O , Ga O [Basic Stregnth]2 3 2 3 2 3 2 3 2 3

Q.2O6 B, Ga, Al, In, Tl [Stability of +3 oxidation state]

Q.2O7 Ga, Tl, In [Stability of +1 oxidation state]

Q.2O8 B, Ga, Al, In, Tl [Stability of hydride]

Q.2O9 Al, In, Ga, Tl [Reducing nature]

Q.21O C, Si, Sn, Ge, Pb [First Ionisation Energy]

Q.211 C, Si, Sn, Ge, Pb [Catenation]

Q.212 C, Si, Sn, Ge, Pb [Ionisation Energy]

Q.213 PbF2, PbCl2, PbBr2, PbI2 [Ionic Character]

Q.214 C, Si, Sn, Ge, Pb [Density]

Q.215 N, As, P, Sb, Bi [Melting Point]

Q.216 N, As, P, Sb, Bi [Boiling Point]

Q.217 NH3, AsH3, BiH3, PH3, SbH3 [Basic Strength]

Q.218 NH , AsH , BiH , PH , SbH [Reducing Character]3 3 3 3 3

Q.219 NH , PH , AsH , SbH [Boiling point]3 3 3 3

Q.22O NI , NCl , NBr , NF [Basic Character]3 3 3 3

E D U C A T I O N S


INORGANIC PAPER CHEMISTRY P. JOYQ.221 NH , AsH , PH , BiH , SbH [Bond Angle]3 3 3 3 3

Q.222 PCl , SbCl , AsCl [Acid Strength]3 3 3

Q.223 N2O3, As2O3, P2O3 [Acidic Strength]

Q.224 N O , As O , P O , Bi O , Sb O [Acidic Strength]2 5 2 5 2 5 2 5 2 5

Q.225 N O, N O , NO, N O , N O [Acidic Strength]2 2 3 2 4 2 5

Q.226 P2O5, Sb2O5, As2O5, Bi2O5, N2O5 [Stability]

Q.227 NCl , AsCl , PCl , SbCl , BiCl [Ease of hydrolysis]3 3 3 3 3

Q.228 PF , PBr , PCl , PI [Acid Strength]3 3 3 3

Q.229 PF , PCl , PBr , PI [Bond Angle]3 3 3 3

Q.23O HNO3, H3AsO4, H3PO4, H3SbO4 [Strength and solubility]

Q.231 O, Se, S, Te [Electron Affinity]

Q.232 O, Se, S, Te, Po [Ionisation potential]

Q.233 H O, H S, H Te, H Se [Reducing power]2 2 2 2

Q.234 H2O, H2S, H2Te, H2Se [Bond angles]

Q.235 H O, H S, H Te, H Se [Stability]2 2 2 2

Q.236 H O, H S, H Te, H Se [Acidic nature]2 2 2 2

Q.237 H2O, H2S, H2Te, H2Se [Dipole moment]

Q.238 SO , TeO , SeO [Acidic nature]3 3 3

Q.239 SO, SO , SO [Acidic nature]2 3

Q.24O H SO , H SeO , H TeO [Acidic strength]2 3 2 3 2 3

Q.241 F, Cl, Br, I [Electron affinity]

Q.242 F, Cl, Br, I [Electronegativity]

Q.243 Cl , Br , F , I [Bond energy]2 2 2 2

Q.244 Cl , Br , F , I [oxidising power]2 2 2 2

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, HClO , HClO , HClO [Thermal stability]

2 3 4

Q.25O HClO, HBrO, HIO [Thermal stability]

Q.251 HClO , HBrO , HIO [Thermal stability]

3 3 3

Q.252 HClO, HClO2, HClO3, HClO4 [Acidic strength]

Q.253 HClO, HBrO, HIO [Acidic strength]

Q.254 HClO, HClO , HClO , HClO [Oxidising power]

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Q.255 MF, MCl, MBr, MI [Ionic character]

CHEMISTRY P. JOY

Q.256 I +, I —, H IO , I O , I— [Oxidation number]3 3 5 6 2 5

Q.257 HClO , HClO , HClO , HClO [Acidic strength]3 4 2

Q.258 I2, HI, HIO4, ICl [Oxidation number]

Q.259 He, Ar, Ne, Kr, Xe [Polarizability]

Q.26O He, Ar, Ne, Kr, Xe [Solubility in water]

Q.261 XeF , XeF , XeF [Melting point]2 4 6

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 NH

Q.265 Ammonia will burn in air ? Yes or No.

burns in pure oxygen.

Q.266 Which factor is responsible for high boiling point of NH .

Q.267 Name the process by which ammonia is made industrially.

Q.268 How liquid NH resembles water in its physical behaviour.

Q.269 Which factor is responsible for making liquid NH a fair ionizing solvent.

Q.27O Why NH (I) is a better solvent for organic compounds but generally a poorer one for ionic inorganic compounds.

Q.271 Why AgI is exceedingly insoluble in water but good soluble in NH .

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 (NH ) Cr O is heated.

4 2 2 7

Q.276 What are the gases produced when NH NO (s) is dissociated.4 3

Q.277 What are the gas as produced when NH4NO3(I) is decomposed when heated.

Q.278 What is the structure of N O.

Q.279 How many unpaired electron(s) are present in NO.

Q.28O 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 N2O3, 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 N O is diamagnetic or paramagnetic.

Q.285 What is the anhydride of nitric acid.

Q.286 In which state (liquid, gas, vapour, solid) covalent N O

molecules are present.

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Q.287 Complete the following reaction

Fe(CO) + NO50°C

Pressure

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.29O What are the formal oxidation states of two oxoacids of phosphorus.

Q.291 How many nonacidic hydrogen atoms are attached directly to phosphorus acids.

Q.292 Consider the following reaction

O

PH OH

H

Ag+

Cr2 O 7

Ag

Cr+3

H yp oph os p ho rou s a c id

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) .

Q.294 How many acidic hydrogen(s) is/are present in H3PO2.

Q.295 Which phosphorus acid is formed on reaction between water and phosphorous trichloride at 0°C.

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.3OO What is the general formula by which cyclic polymetaphosphates can be represented.

Q.3O1 What are the two main oxoacids of nitrogen.

Q.3O2 What are the properties possessed by HNO2.

Q.3O3 Which oxoacid of nitrogen act as both reducing and oxidising agent.

Q.3O4 What is fuming nitric acid.

Q.3O5 In which type of solution HNO is stable.

Q.3O6 What is Aqua fortis and what is its meaning.

Q.3O7 Name the two processess by which HNO can be prepared.

Q.3O8 Aqueous nitric acid is an oxidant, which ion is responsible for this property.

Q.3O9 What are the products formed when NH CONH is treated with HNO . Write the balanced equa-tion.

2 2 2


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INORGANIC PAPER CHEMISTRY P. JOYQ.31O 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 N O is dissolved in water.

Q.314 When HNO is dissolved in pure H SO , an active agent is formed which has an important applica-3 2 4

tion in organic chemistry. Name the agent.

Q.315 What are the two oxides of phosphorus.

Q.316 Which compound is formed when P2O3 combines with oxygen.

Q.317 What happens when P O2 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.32O Which oxide of phosphorus converts HNO to N O and H SO to SO .

Q.321 What happens when P2O5

3 2 5 2 4 3

(i) Combines with cold water. (ii) Combines with hot water.

Write the corresponding reactions.

Q.322 If ammonia in large excess is treated with Cl2 diluted with N2, what product is produced. Write the balanced equation.

Q.323 Which compound is formed when chloramine reacts with NH3.

Q.324 Consider the sequence for industrial utilization of atmospheric nitrogen.

H2 NH2 Haber processO2 NO

O2 H2OHNO (aq)

(I) (II) (III) (IV)

Name the process by which II is converted into III.


4NH (g) + 3O (g) l3 2

Q.326 At 750—900°C and in the presence of a platinum catalyst ammonia reacts with oxygen to give other product instead of O . 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.33O Which oxide is present is the compound when Na(s) reacts O (g).

Q.331 What is the colour of liquid dioxygen and solid dioxygen.

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INORGANIC PAPER CHEMISTRY P. JOYQ.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 OF 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.34O Which acid is produced on reaction of SO 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 H S react with O .2

Q.346 How many lone pairs of electron are present in OF

2

molecule.

Q.347 Arrange the following species in decreasing order of their bond strength.

+ — 2—O2, O

2 , O

2 , O

2

Q.348 Which gas is produced when sodium nitrate decomposes above 800°C.

Q.349 Is oxygen has highest electron affinity in group 16 ?

Q.35O What is the oxidation state of O in Na O ?

Q.351 Arrange the following oxides in increasing order of their acidic property.

ZnO, Na2O2, P2O5, MgO.

Q.352 What are the factors which are responsible for anomalous behaviour of oxygen.

Q.353 Who discovered oxygen.

Q.354 Which factor is responsible for existence of oxygen as discrete diatomic molecule.

Q.355 Is ozone linear or non linear molecule.

Q.356 How does oxygen and ozone differ in their magnetic nature ?

Q.357 Which ion is isoelectronic with ozone. Q.358

How does oxygen is converted into ozone.

Q.359 What is the bond angle < O — O — O in ozone.

Q.36O What change occurs in volume of ozone when it is heated.

Q.361 Which is more powerful oxidizing agent O or O .

Q.362 Give two applications of ozone.


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INORGANIC PAPER CHEMISTRY P. JOYQ.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 O .

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.37O 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 :

O + 2K+ + 2I— + H2O

Q.374 In which phase hydrogen bonded molecules of H O are found.

Q.375 Which is more associated via hydrogen bonding i.e. H O or H O .

Q.376 What is the structure of the molecule of H O .

2 2 2

2 2

Q.377 Which has more density H2O or H2O2

Q.378 What is the limitations of H O which inhibits its utility as an ionizing solvent.

Q.379 Is H O is more acidic than H O in dilute aq. solution.

Q.38O H2O2 acts as oxidizing agent or reducing agent towards MnO4

Q.381 In which type of solution (acid or basic), oxidations with H2O2 is slow.

Q.382 In which type of solution (acid or basic) disproportionation of H O occurs most rapidly

Q.383 Which free radicals are formed by metal ion catalysed decomposition of H O .2 2

Q.384 Identify the products of the following reaction

BaO O2 BaO2H2SO4 A + B.

Q.385 Give the structure and name of the reactant involved in the synthesis of H2O2 by the reaction given below.

ReactantO 2

H 2 /Pd .

OC 2 H 5

O

+ H O

E D U C A T I O N S


—

3 2

3

3

2

2

2 2

2

INORGANIC PAPER CHEMISTRY P. JOYQ.386 Consider the following reaction

H2O2()) H2O()) + ½O2 G = — 121.4 kJ mol

Is water or oxygen is thermodynamically unstable with respect to H O .2 2

Q.387 Which acid on hydrolysis give H O . Write a chemical equation.2 2

Q.388 Arrange the following O , H O and O in increasing order of their O — O bond length.2 2 3

Q.389 How many atoms of sulphur are present in its free state.

Q.39O 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 -sulphur is converted into -sulphur and what this temperature is called.

Q.395 Complete the following reactions :

(i) 2S + Cl2Boil

(ii) 3S + P4

(iii) 2S + C 1200 1400K

Q.396 What compound is formed when sulphur reacts with NH in presence of H S gas.

Q.397 Which oxide of sulfur is closely related structurally & electronically to ozone.

Q.398 What is the structure and bond angle of SO .

Q.399 Which oxide of sulphur act as an antichlor for removing excess of chlorine.

Q.4OO Which property of SO2 is responsible for its bleaching action.

Q.4O1 Which oxide of sulphur is used in the preparation of H2SO4.

Q.4O2 What is oxidation state of sulphur in SO & SO respectively.

Q.4O3 Give two methods for preparation of Hydrogen Sulphide.

Q.4O4 H2S is a dibasic acid or monobasic acid.

Q.4O5 Name the two series of salts formed by H S.

Q.4O6 Which property of H S is used for detection of various cations in laboratory.

Q.4O7 What happens when SO is passed through acidified solution of H S.

Q.4O8 Why coordination compounds of H2S are very rare.

Q.4O9 H S in large doses prove fatal. What is antidote of H S.2 2

Q.41O Which acid is called king of chemicals and why is it so called.

Q.411 Name the two processess by which sulphuric acid can be manufactured.

Q.412 What are the ideal conditions required for manufacturing of H2SO4 by contact process.



Q.413 What is the strength of H SO produced by chamber process.2 4

Q.414 By which process 100% pure H SO is obtained.2 4

Q.415 Which removes impurities of arsenic in contact process.

Q.416 Why SO is never directly dissolved in H O to form H SO .3 2 2 4

Q.417 Write down the chemical reactions taking place in contact process.

Q.418 H SO has low volatility. Why ?2 4

Q.419 Name the two series of salts formed by H2SO4.

Q.42O How many oxygen atoms in H SO are linked to sulphur by single covalent bonds.2 4

Q.421 What is the oxidation state of sulphur in H SO .2 4

Q.422 Which type of bond is responsible for associated structure of H2SO4.

Q.423 It is suggested that to dilute conc. H2SO4, always add conc. H2SO4 to water and never water to conc. H2SO4. Why ?

Q.424 Why conc. H SO is used extensively to prepare other acids.2 4

Q.425 Why H SO has great affinity for water.2 4

Q.426 What are the functions of H SO in the reaction given below.2 4

2Ag + H2SO4 Ag2SO4 + 2H2O + SO2

Q.427 Why sugar becomes black when it comes in contact with conc. H SO .2 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.43O What are the oxidation number of both the S in Na2S2O3.

Q.431 Why hypo is used in iodometric titrations.

Q.432 Why hypo is used as a fixing agent in photography.

Q.433 What are the products formed when chlorine is passed through aqueous hypo solution.

Q.434 When hypo is heated to high temperatures, the products are.

Q.435 Sulphur disappears when it is boiled in a solution of sodium sulphite. This is due to formation of.

Q.436 Write the spring‘s reaction for formation of Na S O .2 2 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.44O Complete the reactions :

(i) CaF + H SO2 2 4

(ii) 2NaCl + H SO2 4

Q.441 Which hydrogen halide is liquid at room temperature.

E D U C A T I O N S


2

5

2 2

INORGANIC PAPER CHEMISTRY P. JOYQ.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 KHF .

Q.445 Why acidity of anhydrous HF is considerably increased in the presence of super acid, SbF . 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.45O 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.


HNO + HF H NO + + F—3 2 3

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 KHF . What are the species present in the KHF .2 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, HClO , HClO , HClO2 3 4

Q.46O What is the oxidation state of chlorine in hypochlorous acid.


HClO HOCl ½Cl

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.


3

3 2 2

2

2

2

2

2 2

2

2

INORGANIC PAPER CHEMISTRY P. JOYQ.465 Salts (0.1 M solution) of which oxyacid of chlorine is most basic ?


NH + NaOCl X + NaOH

X + NH + OH— Gum H N — NH + Cl— + H O

Identify the X & what is it called.

Q.467 What is the shape of ClO — & what is the hybridisation state of Cl.

Q.468 Draw the structure of ClO —.

Q.469 Which oxyacid of chlorine has highest oxidation number.

Q.47O 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

HIO , HClO , HBrO3 3 3

Q.473 BY which mechanism HOCl is formed from Cl 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.48O Name the type of reaction as given below

CaOCl + H O Ca(OH) + Cl2 2 2 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 (H SO , HCl, HNO ) reacts with CaOCl .

Q.485 What do you mean by available Cl .

Q.486 Why CaOCl2 uses as a disinfectant.

2 4 3 2

Q.487 Why CaOCl gives Cl like smell.

Q.488 Bleaching power is an example of ..... salt.

Q.489 What % of available Cl is present in a good quality of bleaching powder.

Q.49O 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 ?

E D U C A T I O N S


2

4

8

2

2

6

2

4

INORGANIC PAPER CHEMISTRY P. JOYQ.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.5OO Why diaphragm made of Teflon is used to separate anode from cathode in preparation of fluorine.

Q.5O1 How bromine is commercially obtained ?

Q.5O2 How iodides are converted into iodine.

Q.5O3 How iodates can be converted into I ?

Q.5O4 What is correct when conc. H SO is added on NaCl and MnO .2 4 2

Q.5O5 What happens when K MnF is reacted with SbF .2 6 5

Q.5O6 Halogen oxidises halide ions of higher atomic number. (True/False)

Q.5O7 In which state of halide ion F can act as an oxidising agent ?

Q.5O8 Which three elements do no reacts with hydrogen ?

Q.5O9 What happens when ?

(a) Mg reacted with Br2

(b) P

(c) S

reacted with Cl

reacted with F

(d) Xe(g) reacted with F2

Q.51O 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 UF or UF ?

Q.512 What happens when

(i) CaF + H SO con. (ii) NaCl + H SO conc.2 2 4 2 4

(iii) H + Br Pt (as bijects) (iv) 2I (s) + N H5731 K

2 2 2 2 4

(v) I2 + H2S

Q.513 How DCl can be prepared in laboratory.

Q.514 What do you call OCl—.

Q.515 How pure HOCl can be formed.

Q.516 What is house hold bleach.

Q.517 What happens when cold dil. NaCl is electrolysed ?


2

2 2 2

3 2 2

4

n

3

5

2 7

2

n

n


Q.518 What is the composition of bleaching powder when Cl is passed over slacked lime.

Q.519 What happens when Ba(OH) is reacted with H O & ClO

Q.52O How HClO3 can be obtained by Ba(ClO2)2

Q.521 How Ba(ClO ) can be prepared. [What happens when Cl is passed through hot Ba(OH) solution]

Q.522 What happens when NaClO is reacted with conc. HCl.

Q.523 What is the major use of NH ClO ?4 4

Q.524 How NH4ClO4 can be obtained from NaClO4

Q.525 Inter halogen compounds are more reactive then halogens. Explain.

Q.526 Interhalogen compounds are always diamagnetic. Explain.

Q.527 Why interhalogen compounds have covalent character.

Q.528 Interhalogen compounds are conducts electricity.

Explains. Q.529 Why IBr known but ClBr is not known ?

Q.53O 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 X (interhalogen compounds) can be 1, 3, 5 or 7. (T/F)

Q.534 A can never be F in A X (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 X (interhalogen compounds) (T/F)

Q.537 How many lone pairs are present on ClF molecule.

Q.538 What is Wij‘s reagent.

Q.539 What is Iodine number.

Q.54O Arrange the following interhalogen compounds in increasing order of reactivity

IF, IF , BrF, IF , BrF , ClF, IF , BrF , ClF3 5 3 2 5 3

Q.541 Why ICl3 exist in form of dimers (I2Cl6). Explain.

Q.542 What do you mean of cationic iodine. Give the examples of compounds showing existance of cationic iodine.

Q.543 Which acids are produced during hydrolysis of ICl.

Q.544 Which acids are produces during hydrolysis of BrF .

Q.545 Complete and balance the following reactions :

(i) I + IClAlCl3 (ii) CsF + IF

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.

E D U C A T I O N S


6

6

6

2 2 2

6


Q.548 Why group 18 elements exhibit low chemical reactivity.

Q.549 Why noble gases have very low melting and boiling points ?

Q.55O 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.56O Bartlett had noticed that PtF reacts with oxygen to form O + [PtF ]— & then he reasoned that6 2 6

PtF would react with xenon to form Xe+[PtF ]— what was the basis of his reasoning.

Q.561 Recent studies indicates that xenon reacts with PtF

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 : 2XeF (s) + 2H O(I)2 2

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 techniques.

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 + FNi

673K, 1atm (ii) Xe + 2FNi

673K, 5 7 atm (iii) Xe + 3FNi

673K, 60 70 atm

2 : 1 1 : 5 1 : 20

Q.57O Complete the following reaction : XeF6 + 3H2O

Q.571 Which oxyacids are formed when XeF 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.


6

6

6

(g)

+

+


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.58O Which noble gas species is isostructural with (a) ICl — (b) IBr — (c) BrO —4 2 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 purposes.

Q.583 Which noble gas is used in gas-cooled nuclear reactors.

Q.584 What are the three binary fluorides of xenon.

Q.585 Which fluoride of xenon has square planar structure.

Q.586 How many bonding pairs of e— are present in XeF .

Q.587 Which fluoride of xenon have a distorted octahedral structure.

Q.588 Which ion forms bridges between XeF5 units in the solid state of XeF6

Q.589 Which type of bridge is formed in solid state of XeF .

Q.59O Which type of units are present in solid state of XeF

Q.591 What is the shape of XeF5 units present in solid state of XeF6

Q.592 Which species is formed when XeF react with SbF . Give a chemical reaction : XeF

+ SbF .4 5 4 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) NaNO (b) CaCO (c) Na CO (d) Ca(NO )3 3 2 3 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.6OO Why Li is not stored in kerocene ?

Q.6O1 Bright metallic lister of freshely cut piece of Na is lost on exposure to air why ?

Q.6O2 Which of the following does not react with Na metal ?

(a) D O (b) C H OH (c) Diethyl ether (d) Acetone2 2 5

Q.6O3 M(g) M+ + e— is most favourable in

(a) Cs (b) Li (c) Na (d) K

Q.6O4 Which is a characteristic of alkali metal

(a) Conductivity (b) High I.P. (c) Low O.P. (d) High m.p., b.p.

E D U C A T I O N S


1 2 3 1 2 3 2 3 2 3

2

2

1 1

+

INORGANIC PAPER CHEMISTRY P. JOYQ.6O5 It same molar amount of lithium, sodium & potassium are dissolved in water and the heat

released are measured Q1, Q2 & Q3. Which of the following relations are correct.

Li Na K

Q 1 Q 2 Q 3

(a) Q > Q > Q (b) Q < Q < Q (c) Q = Q = Q (d) Q > Q > Q

Q.6O6 M + H2O MOH + ½H2

What is order of alkali metals reactivity.

Q.6O7 Li reacts with water slowly but when added to water explodes why ? How thermodynamic and kinetic terms can be related to above observation.

Q.6O8 Does during the reaction of K with water K solid evaporates ?

Q.6O9 When alkali metals are added to water how does it changes the pH of water ?

Q.61O 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) product is

(a) KO2 (b) K2O (c) K2O2 (d) None

Q.613 Which alkali metal can be used to absorb N .

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.62O 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.63O What are colours imparted in flame by alkali metals ?


2

2 2 2 2

2

2

2 2

INORGANIC PAPER CHEMISTRY P. JOYQ.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 Li O, Na O, K O, Rb O.2 2 2 2

Q.638 Why some alkali metals form oxide some form peroxide and other forms super oxide.

Q.639 A student wish to confirm a white solid as Na2O or Na2O2. He dipped red litmus paper into freshely prepared solution of water and found litmus decolouried, solid is

(a) Na2O2 (b) Na2O (c) NaO2 (d) None

Q.64O What would have happened if red litmus has brought in contact with Na O.

Q.641 What happens when following is added to water

(a) Na O (b) Na O (c) KO2 2 2

2— — 2—Q.642 Which of following has highest bond order among O2

Q.643 Predict the magnetic nature of following ?

, O2

, O2, O

(a) Na O (b) KO (c) O (d) Na O

Q.644 What is oxone chemically ?

Q.645 What is the order of basic strength of following oxides ?

Li O, Na O, K O, Rb O, Cs O2 2 2 2 2

Q.646 Why Na O & KO 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 Na2Ored hot

(a) H O lost (b) CO lost (c) Na O + CO formed (d) None2 2 2 2

Q.65O Why alkali metal carbonates are stable on heating ?

Q.651 Arrange following in order of stability H CO , NaHCO , Na CO2 3 3 2 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

E D U C A T I O N S


3

3

3

3

2 2

—

INORGANIC PAPER CHEMISTRY P. JOYQ.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.66O why Li N is stable where as Na N does not exist at 25°C.3 3

Q.661 Why lithium salts are commonly hydrated where as other alkali ions are anhydrous.

Q.662 For salts of strong acids the Li salt is usually the most soluble in water of the alkali metal salts, where as Li salts are usually less soluble than there of the other elements.

Q.663 What happens when Li2CO3 is strongly heated till 500°C.

(a) H O vapours are formed (b) H O, Li O, CO2

(c) Li O, CO

2 2 2

only (d) None2

Q.664 Why Li CO

2

decomposes on heating while other metal carbonates donot2 3

Q.665 Alkali metal carbonates are good soluble in water. Explain why ?

Q.666 Why alkali metal carbonates are alkaline in nature ?

Q.667 What are the only five solid bicarbonates :

Q.668 Why Na2CO3 & CaCO3 differenting react on heating ?

Q.669 How will you make distinction between Na2O and Na2O2.

Q.67O What happens. When Li CO & Na CO are heated upto 500°C.2 3 2 3

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 Na CO , NaHCO ?2 3 3

Q.674 What happens when Na CO . NaHCO .2H O is strongly heated ?2 3 3 2

Q.675 What happens when Na metal is added to highly pure liq. NH ?

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 NH (I) 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.68O What organic application of Na in NH (I) ?

Q.681 Na+NH (I) observation are

(a) Blue colour (b) Strong reducing agent

(c) Produce NaNH (d) Produce H


3

3

2

INORGANIC PAPER CHEMISTRY P. JOYQ.682 Blue solution of alkali metals in NH (I) is diamagnetic or paramagnetic ?

Q.683 How blue solution of alkali metal ion is decomposed ?

Q.684 What happens if NH3(I) is carefully evaporated from blue solution ?

Q.685 To blue solution of Na/NH (I) if more sodium is added it show metallic copper coloured solutionthen 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(I)

(a) THF (b) HMPA (c) Diglyme

(d) RNH (e) Ethers

Q.688 Which alkali metals is radioactive.

Q.689 Which isotope of Fr has longest life.

Q.69O 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.7OO Li, Na, K, Rb, Cs (Increasing order of metallic radius)

Q.7O1 Li, Na, K, Rb, Cs (Increasing order of ionic radius).

Q.7O2 Li, Na, K, Rb, Cs (Increasing order of melting point).

Q.7O3 Li, Na, K, Rb, Cs (Increasing order of boiling point).

Q.7O4 Li, Na, K, Rb, Cs (Increasing order of density)

Q.7O5 Li, Na, K, Rb, Cs (Increasing order of standard potential).

Q.7O6 Cs2CO

3, Rb

2CO

3, K

2CO

3, Na

2CO

3, Li

2CO

3 (increasing order of stability of carbonates)

Q.7O7 CsHCO3, RbHCO3, KHCO3, NaHCO3, LiHCO3 (increasing order of stability of bicarbonates)

Q.7O8 MCl, MBr, MF, MI (Increasing order of covalent character) (M = alkali metal)

Q.7O9 KCl, KBr, KI (Decreasing solubility in water)

Q.71O LiF, NaF, KF, RbF, CsF (Increasing order of lattice energy)

Q.711 Li, Na, K (Decreasing order of reducing nature in solution).

Q.712 LI O, Na O, K O, Rb O < Cs O (Increasing order of basic nature)2 2 2 2 2

E D U C A T I O N S


2

2

INORGANIC PAPER CHEMISTRY P. JOYQ.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 H O 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.72O Magnesium acts as a (oxidising or reducing agent) in the production of metals such as Ti, Zr and Hf.

Q.721 Which alkaline earth metal is used as a an oxygen scavenger and for cathodic protection of other metals.

Q.722 Why the temperature of 1273 k is maintained when lime stone is heated for the production of quicklime.

Q.723 What is another name of calcium oxide.

Q.724 What is slaking ?

Q.725 Quicklime slaked with soda gives a solid.

Q.726 Complete the following chemical reaction occuring at high temperature

(a) CaO + SiO2

(b) CaO + P4O10

Q.727 What is slaked lime & how it is produced.

Q.728 What is lime water ?

Q.729 Suspension of slaked lime in water is known as.

Q.73O What happens when CO is passed through lime water.

Q.731 Identify X in following reaction

Ca(OH)2 + CO2 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) , Sr(OH) , Ba(OH) , Ca(OH) (Solubility)2 2 2 2

(ii) Ca(OH)2, Ba(OH)2, Sr(OH)2, Mg(OH)2 (Basic character))

(iii) Mg(OH) , Co(OH) , Sr(OH) , Ba(OH) (Solubility)2 2 2 2


2

4 4

INORGANIC PAPER

Q.738 Name the ion formed when Be(OH)

CHEMISTRY P. JOYreacts with alkali. Give the chemical reaction

Q.739 How many halogen atoms are coordinated with Be in condensed phase of beryllium halides.

Q.74O Which halides of magnesium are soluble in organic solvents.

Q.741 Fluoride of which alkaline earth metal is known as fluorospar.

Q.742 Name the halide of the alkaline earth metal which is the only large scale source of fluorine.

Q.743 Arrange the following :

(i) BeCO3, MgCO3, CaCO3,SrCO3, BaCO3 (Thermal stability)

(ii) CaSO , SrSO , BaSO (Solubility)4 4 4

(iii) Ca(C O ) , Sr(C O ) , Ba(C O ) (Solubility)2 4 2 2 4 2 2 4 2

Q.744 Nitrate of which alkaline earth metal crystallizes as the anhydrous salt.


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.75O How Mg is obtained from magnesite or dolomite.


CaCO3.MgCO3 + 2H2SO4 CaSO4 + MgSO4 + 2H2O + 2CO2

How the two sulphates formed in above reaction can easily be separated.

Q.752 What is the chemical formula of magnesium sulphate which is obtained from the solution contain-ing CaSO & MgSO 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.76O 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.

E D U C A T I O N S


4

2

4 4

3

4

6

INORGANIC PAPER CHEMISTRY P. JOYQ.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 CuSO solution which complex is formed.

Q.768 Out of AgNO3, AgF and AgClO4 which salts are water soluble.

Q.769 Write the stability of Cu+ and Ag+ halide complexes are in increasing order.

Q.77O 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 = 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 H S gas is passed through this solution, which ofthe ppt out.

Q.776 Silver ornaments turn black in atmosphere. Which gas is responsible.

Q.777 In dilute alkaline KMnO solution MnO — changes to.

Q.778 What is d-d transition.

Q.779 AgCl and Nacl are colourless while AgBr and AgI are coloured. Explain.

Q.78O Why d-block element have ability of complexes formation.

Q.781 What happens when H O is added to an acidified solution of K Cr O2 2 2 2 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) 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) ]3— ion has magnetic moment of 1.73 B.M., while [Fe(H O) ]3+ has a magnetic moment of 6 2 6

5.92 B.M. Explain.

Q.787 What is the EAN (effective atomic number) of the underlined atoms in the following complexes ?

(a) [F e(CN) ]4— (b) [C r(en) ]3+ (c) N i(CO) (d) [Fe(H O) ]2+6 3 4 2 6

Q.788 Match the geometry (given in column A) with the complexes (given in column B) in :

A B

(I) Octahedral (a) [Ni(CN) ]2—

(II) Square planar (b) [Fe(CN) ]4—

(III) Tetrahedral (c) Ni(CO) 4


3

2 4

2 4

—

INORGANIC PAPER CHEMISTRY P. JOYQ.789 One mol of the aqueous solution of the complex CoCl .5H O when treated with excess of aqueous3 2

AgNO 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.79O Arrange [Fe(CN) ]4—, [Fe(CN) ]3—, [Ni(CN) ]2— and [Ni(H O) ]2+ in increasing order of magnetic6 6 4 2 4

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.8OO VO2+ is oxidised to VO + by MnO — in acidic medium, which in turn is reduced to Mn2+. Write2 4

balanced equation for this reaction.

Q.8O1 One of the following oxide is also called chromic acid. Select that one : CrO , Cr O , CrO , CrO.

Q.8O2 What is oxidation number of Cr in CrO Cl .

2 2 3 3

2 2

Q.8O3 What is oxidation number of Cr in CrO5 or CrO(O2)2

Q.8O4 What is oxidation number of Cr in (NH ) Cr O4 2 2 7

Q.8O5 What is oxidation number of Cr in [Cr(O ) ]3—

Q.8O6 Arrange the following ions in order of increasing strength as a reducing agent, and account for the trend :

(a) Cr2+ (b) Cr3+ (c) Cr O 2—2 7

Q.8O7 H2O2 can be oxidised to O2 by MnO4 in acidic as well as in basic medium. Write reactions

Q.8O8 What happens when CO gas is passed into MnO 2— solution ?

Q.8O9 Unreacted AgBr in photography is removed by hypo used as ‘fixer‘. What is the reaction ?

Q.81O (a) When H2S gas is passed into FeCl3 solution, yellow colour of FeCl3 changes to light green.Explain

(b) Same behaviour is also observed when SnCl2 solution is observed. Explain.

E D U C A T I O N S


2

2

3

3

2

2

3


Q.811 Given chemical tests for making distinction between Fe2+ and Fe3+ ions.

Q.812 When K2HgI4 reacts with NH3, brown ppt is formed. Explain the formation of brown ppt.

Q.813 What is brass.

Q.814 What is coinge metal

Q.815 What is nichrome.

Q.816 Name those anions which have high solubility

Q.817 Which anion has least ppt. test.

Q.818 Soda extract is prepared by which carbonate.

Q.819 Soda extract can‘t be used for which anion detection.

Q.82O 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 CO X is.

Q.825 Which gas has suffocating order and responds to litmus paper.

Q.826 What is the colour of K2Cr2O7 paper when it is treated with SO2.

Q.827 What is the oxidation state of chromium when it is reduced by SO .

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.83O Which type of substances are detected by potassium iodide starch paper.

Q.831 Which type of reagents are detected by KIO starch paper.

Q.832 What happens when white ppt. of Ba(CO ) is is treated with dil acid.

Q.833 Out of CO 2, SO —, Br—, I—, Cl— whose barium salts or silver salts are dissolved by dil. acids.3 3

Q.834 In which case CrO2Cl2 test can‘t be employed.

Q.835 Which cation should be absent when CrO Cl test is employes.2 2

Q.836 Which anion other than halide should be absent when CrO Cl chloride test is employed.2 2

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.84O What is the gas released when Cl— ions are added with conc. H SO .2 4

Q.841 What is the gas evolves with Cl— ions are reacted with MnO .

Q.842 Which of the 2 gases Cl 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 AgNo .


3

2

2

2

4

4

2

3

—

INORGANIC PAPER CHEMISTRY P. JOYQ.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 NH solution.

Q.849 Which halide ions on addition of concentration H SO does not evolve halogen.2 4

Q.85O 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 PbO .

Q.856 Name some reagents which can oxidise Br— into bromine.

Q.857 Which halogen can displace bromide from its salt.

Q.858 When iodide is added to conc. H2SO4 which vapor and gas are released.

Q.859 Which hydrogen halide among HCl, HBr, HI can reduce H SO into SO .2 4 2

Q.86O When iodides are treated with H SO acid, a yellow ppt. and rotten egg smell are produced, small2 4

is due to.

Q.861 Which halide ion can‘t be oxidised by MnO .

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 HgCl 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 FeSO to produce brown solution.

Q.87O What is oxidation state of Fe in brown ring test.

Q.871 Which metals or heating with NO — evolves NH gas.3 3

Q.872 Which anions show brown ring complex with FeSO .

Q.873 Which gas is evolved when NO3 is decomposed by conc. H2SO4

Q.874 What happens when NO — are treated with dil. H SO .2 2 4

Q.875 What is the colour of HNO .

Q.876 Which gas is evolved when NO — are reduced by Cu turning.

Q.877 Which of the 2 is soluble in HCl on warming BaSO4 or Ba3(PO4)2

Q.878 What happens when BaSO ppt is reduced by charcoal in presence of Na CO .4 2 3

E D U C A T I O N S


4

3 2

3

3

3

4 2

INORGANIC PAPER CHEMISTRY P. JOYQ.879 Write some common sulphate which are insoluble.

Q.88O What is the formula of ppt. formed when SO 2— 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(NO ) 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 C O 2— is reacted with conc. H SO .2 4 2 4

Q.889 What is the colour of flame when CO is burnt.

Q.89O 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 C O 2—2 4

ion.

Q.892 Which anion has a smell of vinegar.

Q.893 What happens when CH COO— 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 CH COO— 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 CH COO— forms blood red coloration and then brown ppt on heating.

Q.9OO Which anion on reaction with KMnO undergoes O catalysis.


2

2 3

2 2

3 2

2

3

3

H

3

3

2

32

32

4

2 3

3 3

43

3

3

3


SOLUTIONSQ.1

1. 2Al + 3O Al O

2. 2Al + N2 2AlN

3. 2Al + 3Cl 2AlCl

4. Al + Cr O Al O + Cr

5. Al + Mn O Al O + Mn

6. Al + HCl AlCl3 + H2

H O

Al(OH) + 3HCl

7. 2Al + 3H SO (dil) Al (SO ) + 6H2 4 2 4 3 2

8. 2Al + H2SO4(conc.) Al2(SO4)3 + SO2 + H2O

9. Al + HNO No reaction

31O. Al + NaOH Al(OH) +

2 2

11. 2Al + AlCl High Temp. 3AlCl

Q.2

1. Al(OH) + 3H+ Al+3 + 3H O

acid

2. Al(OH) + NaOH Na[Al(OH) ] or NaAlO .2H O3 4 2 2

base sodium meta aluminate

3. Al(OH) Below 450°C Al O ( -form)

4. Al(OH) Above 450°C Al O ( -form)

Q.3 M(I) M‘(III) (SO ) .12H O4 2 2

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+, NH +

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.1O Alums are used as mordant in dyeing.

Q.11 Acidic due to cationic hydrolysis of trivalent cation.

E D U C A T I O N S


3 2

2

2

3

3 4

2

2

2

2

3 2

3

3

3

3

3

INORGANIC PAPER CHEMISTRY P. JOYQ.12 An aqueous solution containing equimolar amount of Al2(SO4) and K2SO4 crystallises as allums.

Q.13 Double dulphate of divalent ions and trivalent ions with 24 water molecules in their crystals are known as pseudo alums.

Q.14 No

Q.15 Al SO .18H O2 4 2

Q.16 Al(OH) + 3H+ Al+3 + 3H O

acid

Al(OH) + NaOH Na[Al(OH) ] or NaAlO .2H O3 4 2 2

base sodium meta aluminate

Q.17 Al(OH)3 Gelatinous white ppt.

Zn(OH) white ppt.

Q.18 It is prepared by passing dry chlorine over aluminium powder.

Q.19 Al O + 3C + 3Cl 2AlCl + 3CO

Q.2O In inert orgnic solvent and in vapour state.

Q.21 The high enthalpy of hydration is sufficient to break the covalent dimer into [M(H O) ]3+ and 3X—

ions.

Q.22 Yes

Q.23 Acidic, AlCl + 3H O Al(OH)

2 6

+ 3HCl3 2 3

Q.24 Yes

Q.25 It is hydroscopic in nature.

Q.26 AlCl is unstable below 800°C. It disproportionate below 800°C

3AlCl AlCl + 2Al

Q.27 AlCl + Cl— [AlCl ]—

Q.28 Al Cl + LiH (excess) Li[AlH ]2 6 4

Q.29 Al O2 3

Q.3O -Al O , -Al O2 3 2 3

Q.31 -Al2O3

Q.32 Al + Fe O Al O + Fe + heat

Q.33 2Al O + 2AlCl 6AlCl + 3O

Q.34 -form

Q.35 -Al2O3

Q.36 The strength of C—C bond is very high.

Q.37 Pb

Q.38 Graphite

Q.39 CO


2


Q.4O Pb

Q.41 Free electrons present in 2p orbitals of graphite

Q.42 Graphite

Q.43 C

Q.44 -Quartz840

-Quartz Tridymite1600°C

cristobalite

Q.45 -Sn15°C

-Sn160°C

Rhombic Sn

Q.46 -Sn15°C

-Sn160°C

Rhombic Sn

Q.47 The conversion of white tin ( -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.5O Diamond

Q.51 CO, CO2, C3O2

Q.52 H CO2 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.6O Malonic acid

Q.61 CO2

Q.62 SnO

Q.63 CO

Q.64 CO neutral, others acidic

Q.65 SiO

Q.66 Produce strong base by hydrolysis.

Q.67 CaC2 + N21300°C CaCN2

E D U C A T I O N S


2 2 2

2

2 2 2

2

2

2

2

3 2 3 2

2 2

—


Q.68 CaCN HOH Ca(OH) + H N — CN

B H O

H2N C NH2||O

urea

Q.69 CaCN + 2NaClCoke

CaCl + NaCN + N

Q.7O K Fe(CN) 4KCN + Fe + N4 6 2

Q.71 2KCN + H SO 2HCN + 2K+

Q.72 Alkaline

Q.73 HCN O2 N C — C N

+ SO4

HCN Cu2 Cu(CN) + NaCN

HCN Ag

Q.74 Cl + NaOH OCl+ + Cl—

(CN) + NaOH OCN+ + CN—

both produced similar type of ions.

Q.75 SiO2 does not have tendency of p -p overlapping.

Q.76 CO , SiO Acidic2 2

GeO , SnO Amphoteric2

PbO

2

Basic2

Q.77 Pb(NO3)2 PbO + NO2

Q.78 CO2

Q.79 Gives mellitic acid [C (COOH) ] and oxalic acid.6 6

Q.8O (R SiO)2 n

Q.81 Silicones are produced.

Q.82 sp3

Q.83 -Quartz

Q.84 Silicates are formed

Q.85 2KOH + SiO K SiO + H O2 2 3 2

CaCO + SiO CaSiO + CO

2KNO3 + SiO2 K2SiO3 + 2NO2 + ½O2

SiO2 + 6HF H2SiF6 + 2H2O

C + SiO CO + Si


n H

n H

3

2


Q.86 Flint

Q.87 Super cooled liquid, pseudo solid.

Q.88 SiO2 + 6HF H2SiF6 + 2H2O

Q.89 Fluoro siliclic acid.

Q.9O Na SiO .CaSiO .HSiO2 3 3 2

Q.91 Na SiO .H O2 3 2

Q.92 When transition metals are added into soda glass solution. Different type of colour are obtained.

Q.93 Silanes Si2n + 2

German Ge2n + 2

Q.94 Vertex of silica is formed.

Q.95 Si + 2NaOH NaSiO3 + H2

Q.96 HF

Q.97 Silanes Alkanes

Toxic Not

Autocombust Not

Reducing agent Not

Unstable Stable

Q.98 KNO3 + SiO2 K2SiO3 + 2NO2 + ½O2

Q.99 HF

Q.1OO Corundum ( Al O ) and Carborundum (SiC)2 3

Q.1O1 Glass

Q.1O2 SiO2

Q.1O3 Soda glass

Q.1O4 Hard glass

Q.1O5 SiO4—4, BO —3

Q.1O6 Flint glass

Q.1O7 Stops U.V. light

Q.1O8 Pyrex glass

Q.1O9 CaCO + Na CO + SiO + H BO borosilicate gass3 2 3 2 3 3

Q.11O 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 SiO form

Q.114 C does not have 3d orbitals.

E D U C A T I O N S


2 2

2

2 2

2

2 3 4

2 3 44

4 4 4

2 2

4


Q.115 Tin is purifyed by electrolytic method

Q.116 Both SnO and SnO2

Q.117 SnC O SnO + CO + CO

Oxidation of SnO to SnO is checked by CO

Q.118 SnO NaOH Na SnO2 2 3

SnO2 H2SO4 H3SnO3 stannic acid

Q.119 SnCl .2H O Sn(OH)Cl2 2

Q.12O SnCl4

Q.121 SnCl4.5H2O

Q.122 SnCl2.2NH3

Q.123 SnCl .4NH4 3

Q.124 HgCl + SnCl Calamel

Q.125 SnF

Q.126 Does not reacts with organic acids.

Q.127 3SnCl + 2AuCl 3SnCl + 2Au

Q.128 3SnCl + 2AuCl 2Au+ + 3SnCl H2O Sn(OH)

Q.129 SnCl4.5H2OH2O Sn(OH)Cl

Butter of Tin

Q.13O Sn + HNO H SnO3 3 3

Q.131 SnI yellow, SnCl and SnBr coloured

Q.132 SnO + 2HF SnF + H O

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, PbO , Pb O , Pb O2 2 3 3 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


-np

2

2

3

INORGANIC PAPER CHEMISTRY P. JOYQ.14O (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 3 general configurator which is a half filled orbital having extrastability. 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 NH (—3), NH -NH (—2), NH OH(—1), N (0), N O(+1), NO(+2), N O (+3), NO (+4), N O (+5)3 2 2 2 2 2 2 3 2 2 5

Q.146 Group V elements have poor bond strength between their atoms.

Q.147 H N N N

Q.148 N

Q.149 Red, yellow, black.

Q.15O White and yellow

Q.151 White and yellow

Q.152 Nitrogen

Q.153 N has high bond energy.

Q.154 Nitrogen N2 others M4

Q.155 p -d

Q.156 Ca3, N2H2O NH3

Ca3P2 :H2O PH3

Q.157 Ca3P2 + 6HOH 3CO(OH)2 + 2PH3 phosphene

Ca N + 6H O 3Ca(OH) + 2NH3 2 2 2 3

Zn As + 6H O 3Zn(OH) + 2AsH3 2 2 2 3

Q.158 Hydrazine

Q.159 NH3 > PH3 > AsH3 > SbH3

Q.16O NH > PH > AsH > SbH > BiH3 3 3 3 3

Q.161 BiH

Q.162 NH3

E D U C A T I O N S


3

3

3


Q.163 NH has H-bonding.

Q.164 NH3 > PH3 > AsH3 > SbH3 > BiH3

Q.165 BiX

Q.166 Pyramidal

Q.167 PCl3 + HOH H3PO3 + 3HCl

Q.168 NX

Q.169 Yes

Q.17O Nitrogen

Q.171 Trihalides are more stable

Q.172 Yes

Q.173 Gaseous state PCl and in solid state [PCl +] [PCl —]5 4 6

Q.174

Q.175 Ca(PO4)2 + C CaCO3 + P

Q.176

Q.177

Q.178

Yellow

Yellow P

Red P

Q.179 ,

Q.18O Yellow

Q.181 (a) White P converts into Red P

(b) White P appears yellow

Q.182 Polymeric structure.

Q.183 Insoluble Red water P

Q.184 P + Ca or Mg Ca3P2 or Mg3P2

P + Na or K Na P or K P3 3

Q.185 Highly reactive, burshing into Hames when exposed to air.


4 3

5

4

3

3 2 3

3 2 2 2

3

3 2

3

3

3

3

3

5

3


Q.186 P O2 P2O3

Q.187 PH & NaH PO3 2 2

Q.188 Reducing agent

Q.189 P + HNO H PO + NO3 3 4 2

P + Conc H2SO4 H3PO4 + SO3

P + CuSO

P + AgNO

Cu P

Ag P + HNO3 3 2 3

Q.19O P PCl5 PCl

P S8 P S

Q.191 White

Q.192 (a) Ca P + 6H O 3Ca(OH) + 2PH3 2 2 2 3

(b) Na3P + H2O NaOH + PH3

Q.193 AlP H2O PH + Al(OH)

Q.194 H PO PH + H PO3 3 3 3 4

Q.195 P + 3NaOH + 3H O PH + 3NaH PO4 2 3 2 2

Q.196 Ring of N2O5 are known as vertex ring. During formations of PH3, PH3 is oxidized by O2 and formsP O2 5

Q.197 P4 + NaOH Na2HPO4 + PH3

PH + O HPO

PH + O P O + H O

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.2OO NCl H2O X

PCl3H2O H3PO3

AsCl H2O As O

SbCl H2O Sb OCl

BiCl H2O BiOCl

Q.2O1 Bi does not show +5 oxidation state due to inert pair effect.

Q.2O2 B > Al < Ga > In < Tl

Q.2O3 BF3 < BCl3 < BBr3 < BI3

E D U C A T I O N S


2 2 2 2 2

2 2 2

2

3

3

3

3

3

3

3

3

3

3

3 3 3 3

2 2 2

3 3 3 3 3

3

3

3

3

3

3

3

3

3 3

3 3 3 3 3

3 3 3

3

INORGANIC PAPER CHEMISTRY P. JOYQ.2O4 BCl3 < AlCl3 < GaCl3 < InCl3

Q.2O5 B O < Al O < Ga O < In O < Tl O

Q.2O6 B > Al > Ga > In > Tl

Q.2O7 Ga < In < Tl

Q.2O8 B > Al > Ga > In > Tl

Q.2O9 Al > Ga > In > Tl

Q.21O C > Si > Ge > Sn <

Pb

Q.211 C >> Si > Ge > Sn > Pb

Q.212 C > Si > Ge > Sn > Pb

Q.213 PbF > PbCl > PbBr > PbI

Q.214 Si < C < Ge < Sn < Pb

Q.215 N < P < As > Sb > Bi

Q.216 N < P < As < Sb > Bi

Q.217 NH

Q.218 NH

> PH

< PH

> AsH

< AsH

> SbH

< SbH

> BiH

< BiH

Q.219 PH3 < AsH3 < NH3 < SbH3

Q.22O NI

Q.221 NH

> NBr

> PH

> NCl

> AsH

> NF

> SbH > BiH3 3 3 3 3

Q.222 PCl3 > AsCl3 > SbCl3

Q.223 N O

Q.224 N O

> P O

> P O

> As O

> As O > Sb O > Bi O2 5 2 5 2 5 2 5 2 5

Q.225 N O < NO < N O < N O < N O2 2 3 2 4 2 5

Q.226 P2O5 > As2O5 > Sb2O5 > N2O5 > Bi2O5

Q.227 NCl > PCl > AsCl > SbCl > BiCl

Q.228 PF

Q.229 PI

> PCl

> PBr

> PBr

> PCl

> PI

> PF

Q.23O HNO3 > H3PO4 > H3AsO4 > H3SbO4

Q.231 O < S > Se > Te

Q.232 O > S > Se > Te > Po

Q.233 H2O < H2S < H2Se < H2Te

Q.234 H Te < H Se < H S < H O2 2 2 2

Q.235 H O > H S > H Se > H Te2 2 2 2

Q.236 H O < H S < H Se < H Te2 2 2 2

Q.237 H2O > H2S > H2Se > H2Te

Q.238 SO > SeO > TeO


2 3

2 2

2 2 2

4 3 2

3 3

2 4

3

3

2 2

2

3

INORGANIC PAPER CHEMISTRY P. JOYQ.239 SO > SO > SO

Q.24O H TeO < H SeO < H SO2 3 2 3 2 3

Q.241 F < Cl > Br > I

Q.242 F > Cl > Br > I

Q.243 Cl > Br > F > I

Q.244 F > Cl > Br > I

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 HClO > HClO > HClO > HClO

Q.25O HClO > HBrO > HIO

Q.251 HClO

Q.252 HClO

< HBrO

> HClO

< HIO

> HClO > HClO4 3 2

Q.253 HClO > HBrO > HIO

Q.254 HClO4 < HClO3 < HClO2 < HClO

Q.255 MF > MCl > M—Br > MI

Q.256 I— < I — < I + < I O < H IO3 3 2 5 5 6

Q.257 HClO < HClO2 < HClO3 < HClO4

Q.258 HI < I < ICl < HIO

Q.259 He < Ne < Ar < Kr < Xe

Q.26O Xe > Kr > Ar > Ne > He

Q.261 XeF6 < XeF4 < XeF2

Q.262 Concentration solution of NH is water.

Q.263 Hydrogen bonding.

Q.264 Yellow flame.

Q.265 Yes NH3 + O2 N2 + H2O

Q.266 Hydrogen bonding.

Q.267 Haber process.

Q.268 NH3 has hydrogen bonding like water.

Q.269 Good dielectric constant.

Q.27O NH has a tendency to form H-bond which helps to dissolve organic substances whereas itsrelatively low dielectric constant then water makes it a poor solvent for ionic inorganic substances.

E D U C A T I O N S


+

3

2

2

5 2 2

3

3


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(NH3)2]

Q.272 NH + + NH —4 2

Q.273 Acid - base

Q.274 Reducing agent.

Q.275 N2 + H2O

Q.276 NH + HNO

Q.277 N O + H O2 2

Q.278 Linear

Q.279 One

Q.28O 2p

Q.281 NO + NO

Q.282 NO2

Q.283 NO

Q.284 Diamagnetic

Q.285 N O2 5

Q.286 Vapour

Q.287 Fe(CO) + NO50°C

Pressure [Fe(CO) (NO) ]

Q.288 [Fe(H2O)5NO]SO4

Q.289 Phosphorous acid & phosphoric acids.

Q.29O +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.3OO (HPO )

Q.3O1 HNO , HNO2 3

Q.3O2 Oxidising, reducing, complex forming ability


3

3

2

2

3

2

2 2

2

INORGANIC PAPER

Q.3O3 HNO

Q.3O4 NO2 dissolved in concentrated HNO3

Q.3O5 aq. solution

Q.3O6 HNO

Q.3O7 Birkeland Eyde & ostwald

Q.3O8 Nitrate ion.

Q.3O9 Urea.

CHEMISTRY P. JOY

Q.31O H N O & HNO4 2 4 4

Q.311 By direct oxidation of NH3 using Pt as a catalyst.

Q.312 P2O5

Q.313 HNO

Q.314 NO +

+ HNO

Q.315 P2O3, P2O5

Q.316 P O2 5

Q.317 (i) P O + 3H O 2H PO2 3 2 3 2

(ii) 2P O + 6H O 3H PO + PH2 3 2

Q.318 P2O5

Q.319 P O

3 3 3

2 3

Q.32O P O2 5

Q.321 (i) P2O5 + H2O 2HPO3

(ii) P2O5 + 3H2O 2H3PO4

Q.322 Chloramine NH Cl [2NH + Cl NH Cl + NH Cl]2

Q.323 Hydrazine

3 2 4 2

Q.324 Ostwald Process.

Q.325 2N (g) + 6H O(g)2 2

Q.326 NO

Q.327 O , O2 3

Q.328 (i) 2KClO3(s) MnO 3O2(g) + 2KCl(s)

Q.329 CO + SO

Q.33O Sodium peroxide Na O2 2

Q.331 Pale Blue

Q.332 F O

Q.333 NO

Q.334 No vacant d-orbital.

E D U C A T I O N S


2

2 2

3

2 5

2


Q.335 Heating with a cobalt salt

Q.336 SO

Q.337 BaO

Q.338 ZnO

Q.339 Elements that are on the borderline between metals and non-metals

Q.34O Sulphurous acid (HSO3)

Q.341 Alkaline

Q.342 Hydrogen

Q.343 High lattice energy

Q.344 BeO, SiO2, B2O3

Q.345 2H2S + O 2 2H2O + 2S O2 SO2

Q.346 8

Q.347 O + > O > O — > O —22

Q.348 O

2 2 2

2

Q.349 Yes

Q.35O — 1

Q.351 Na O > MgO > ZnO > P O

Q.352 Small size, High EN, Absence of d orbitals.

Q.353 Priestley

Q.354 Strong covalent between two O atoms due to p -p overlapping.

Q.355 Non-linear

Q.356 O = paramagnetic, O = diamagnetic

Q.357 Nitrite ion

Q.358 By action of a silent electric discharge

Q.359 117°

Q.36O 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 P + O + H O H PO Zero to + 54 3 2 3 4

Q.368 False


2

4 2

3 2

2

2

2

2

INORGANIC PAPER CHEMISTRY P. JOYQ.369 F

Q.37O Red

Q.371 U.V. Rays

Q.372 Chlorofloro Carbon

Q.373 O + 2K+ + 2I— + H O KOH + I + O3

Q.374 Solid

Q.375 H O

2 2 2

2 2

Q.376 Skew, chain structure

Q.377 H O or H O2 2 2

Q.378 Its strong oxidizing nature ready decomposition

Q.379 Yes

Q.38O Reducing agent

Q.381 Acid

Q.382 Basic

Q.383 HO and OH

Q.384 BaSO + H O

Q.385

OH

C 2 H 5

OH

Q.386 No

Q.387 Peroxodisulfuric acid

Q.388 O > O

Q.389 8

> H O

Q.39O FeS

Q.391 Frasch process

Q.392 -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 + Cl Boil S Cl2 2 2

(ii) 3S + P4 P4S3

(iii) 2S + C 1200 1400K CS

E D U C A T I O N S


2

3

2

3 2 2

3

5 5

INORGANIC PAPER CHEMISTRY P. JOYQ.396 (NH ) S4 2 x

Q.397 SO

Q.398 Trigonal planner, 120°

Q.399 SO2

Q.4OO Reducing nature

Q.4O1 SO

Q.4O2 +4 and +6

Q.4O3 FeS + H SO (dil.) FeSO + H S2 4 4 2

H (g) + S(I) H S(g)2 2

Q.4O4 Dibasic acid

Q.4O5 Bisulphides and hydrogen sulphides.

Q.4O6 It reacts with cations and produced coloured insoluble sulphides.

Q.4O7 s is pricipatted.

Q.4O8 H S is readly oxidized into s or its disprotonation to SH— or S—2. It‘s ligand ability is very weak.

Q.4O9 Dilute chlorine.

Q.41O H SO , it is used in most of manufacturing process.2 4

Q.411 Contact process, Lead chamber process.

Q.412 Fe(OH) remove As O in contact process. They absorb As O on their surface.

Q.413 95%

Q.414 Contact process.

Q.415 Fe(OH)

Q.416 SO + H O H SO it is a violent reaction.3 2 2 4

Q.417 S + O2 SO2

O2

V2O5SO

3H2O H2SO4.

Q.418 Intermolecular hydrogen bonding.

Q.419 Bisulphate and sulphate.

Q.42O 2

Q.421 +6

Q.422 H-bonding.

Q.423 Sparting of acid due to evolution of great amount of heat.

Q.424 H SO is an oxidizing agent thus it can easily oxidised elements in their oxyacids.2 4

Q.425 H SO can form strong extensive H-bonds.2 4

Q.426 Oxidising agent.

Q.427 C6(H2O)6Conc. H2SO4 6C + 6H2O

Black


5

2

2

2 3 4

2

INORGANIC PAPER CHEMISTRY P. JOYQ.428 H SO2 4

Q.429 H SO2 3

Q.43O Zero and +4

Q.431 It can be reduce I

Q.432 It dissolves unreacted AgBr from the photographic emulsion by complexation.

Q.433 Cl2 + H2O + Na2S2O3 2HCl + Na2SO4 + S

Q.434 Cl2 + H2O + Na2S2O3 2HCl + Na2SO4 + S

Hypo is thus used as an antichlore.

Q.435 Na S O2 2 3

Q.436 Na2S + Na2S2O3 + I2 2NaI + Na2S2O3

Q.437 S O —2 (Tetrathionate)4 6

Q.438 aq. solution of hydrogen halides.

Q.439 Strong affinity for hydrogen.

Q.44O (i) CaSO4 + 2HF(g), (ii) Na2SO2 + 2HCl(g)

Q.441 HF

Q.442 HI > HBr > HCl > HF

Q.443 High bond dissociation energy intermolecular hydrogen bonding.

Q.444 Due to high EN & small size of F.

Q.445 SbF 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.45O It reacts with SiO 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 [HF ]—

Q.457 Fluorine

Q.458 ClOH > BrOH > IOH

Q.459 HClO < HClO < HClO < HClO

Q.46O +1

E D U C A T I O N S


2

4

3

3

3

2

3

2 2

2

2

2


Q.461 Increases.

Q.462 Ba(ClO ) + H SO 2HClO + BaSO2 2 2 4 2 4

Q.463 Chlorites

Q.464 HClO4

Q.465 NaClO

Q.466 X = NH Cl, chloramine

Q.467 Tetrahedral, sp3

. .

Q.468 O Cl O. .

Q.469 HClO4

Q.47O HClO4 > HClO3 > HClO2 > HClO

Q.471 HClO

Q.472 HClO

> HClO

< HBrO

> HClO

< HIO

> HClO

Q.473 Cl + H O H+

Q.474 +1 to +7

Q.475 Acidic

+ Cl— + HOCl

Q.476 Cl, Br, I

Q.477 Cl2O least and Cl2O7 most acidic.

Q.478 ClO

Q.479 Ca+2, Cl—, OCl—

Q.48O CaOCl + H O Ca(OH) + Cl Autooxidation2 2 2 2

Q.481 Ca(OH) , Cl2 2

Q.482 It reacts with H2O and convert into Ca(OH)2 and Cl2 by auto oxidation.

Q.483 Ca(OH)2 + Cl2 Ca(OCl) Cl + H2O

Q.484 Cl2

Q.485 The amount of Cl obtained from a sample of bleaching powder by treatment with excess of diluteacids or CO .

Q.486 It produce nascent O by treatment with H SO .2 4

Q.487 Autooxidation

Q.488 Mixed salt.

Q.489 35 to 38%

Q.49O Yes

Q.491 Halogen means salt forming.


3

2

2

2

(g 2

6

2

2 2

2 2

2

6

2

INORGANIC PAPER CHEMISTRY P. JOYQ.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 IO —

Q.497 X—

Q.498 Cl

Q.499 Electrolysis of mixture of molten KF and HF

Q.5OO Diaphragm is used to separate the two gases H and F otherwise these gases reacts explosively.

Q.5O1 By passing Cl gas into bromide salt solution

Q.5O2 6H+ + IO — + I— I + 3H O3 2 2

Q.5O3 6H+ + IO — + I— I + 3H O3 2 2

Q.5O4 When H SO is added to NaCl with MnO , Cl is evolved.2 4 2 2

Q.5O5 K MnF + SbF K SbF + MnF + ½F2 6

Q.5O6 True

5 2 7 3 2

Q.5O7 When halogen has — 1 oxidation state.

Q.5O8 He, Ne, Ar

Q.5O9 (a) Mg + Br (I) MgBr2 2

(b) P4 + Cl2(g) PCl5

(c) S + F (g) SF8 2 6

(d) Xe + F (g) XeF

Q.51O Covalent nature

Q.511 UF

Q.512 (i) CaF2 + H2SO4 con. CaSO4 + HF

(ii) NaCl + H SO conc. Na SO + HCl2 4 2 4

(iii) H + Br Pt (as bijects) HBr

(iv) 2I (s) + N H5731 K

N + HI2 2 4 2

(v) I + H S HI + S

Q.513 PCl + D O POCl + 2DCl5 2 3

Q.514 Hypochlorite ion

Q.515 Cl + H O + HgO HOCl + HCl, HCl is absorbed by HgO

Q.516 NaOCl

E D U C A T I O N S


2 2

3 5 3

2

5

3

3

3 4

8


Q.517 Anode Cl gas, Cathode H and OH— obtain.

Q.518 Ca(OH)2Cl2 Ca(OCl)2. CaCl2.Ca(OH)2.2H2O

Q.519 2Cl2O + 2NaOH + H2O2 2NaClO2 + O2 + 2H2O

Q.52O Ba(ClO ) + H SO BaSO + 2HClO3 2

Q.521 Ba(ClO )

2

+ Cl

4 4 3

Ba(ClO )3 2 2 3 2

Q.522 THCl.

Q.523 Used in rockets as fuels.

Q.524 NaClO + NH Cl NH ClO + NaCl4 4 4 4

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.53O 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.54O IF < IF < BrF < IF < BrF < ClF < IF < BrF < ClF

Q.541 ICl3 is unstable.

Q.542 I+ ICl, IBr, ICN, I+3 ICl , I(ClO ) .IPO .3

Q.543 HOI (Hypo iodous acid) HCl.

4 3 4

Q.544 HF, HBrO bromic acid.

Q.545 (i) [I ]+ [AlCl ]—

(ii) Cs+ [IF ]—

Q.546 ns2 np6

Q.547 Ne = 0, Ar = 0, Kr = 10, Xe = 10

Q.548 Gain or loss of electrons requires high energies.


226 Rn

2

2

2

3

3 4

3

6

+ 2

—

INORGANIC PAPER CHEMISTRY P. JOYQ.549 Due to weak dispersion interactions between atoms.

Q.55O He

Q.551 He

Q.552 Rn

Q.553 “ 1%

Q.554 Ar

Q.555 Ne, Ar, Kr, Xe

Q.556 Natural gas

Q.557 He

Q.558 88

Ra

Q.559 1962

22286 He4

Q.56O Ionization enthalpies of O & Xe are close to each other.

Q.561 [XeF]+ [Pt F ]—2 11

Q.562 Electronegative

Q.563 Xe, O

Q.564 Xenon, krypton

Q.565 Radon

Q.566 Ar, Ne, He

Q.567 KrF

Q.568 6XeF4 + 12H2O 4Xe + 2XeO3 + 24HF + 3O2

Q.569 XeF , XeF , XeF2 4 6

Q.57O XeO — + 6HF

Q.571 XeOF & XeO F4 2 2

Q.572 XeO3

Q.573 XeOF

Q.574 XeO

4

= Trigonal pyramidal, XeOF = Square pyramidal.

Q.575 XeO + OH— HXeO4

hydrogen xenate ion

Q.576 Perxenate ion XeO 4—

Q.577 +8

Q.578 Yellow

Q.579 Oxidising

Q.58O (a) XeF , (b) XeF , (c) XeO4 2 3

Q.581 He non flammable & light gas

E D U C A T I O N S


6

2

2 2

6

+

INORGANIC PAPER CHEMISTRY P. JOYQ.582 Neon

Q.583 He

Q.584 XeF2, XeF4, XeF6

Q.585 XeF4

Q.586 6

Q.587 XeF

Q.588 F—

Q.589 Pyramidal

Q.59O Tetrameric & hexameric

Q.591 Square pyramidal

Q.592 [XeF3]

Q.593 4.2 K

Q.594 Helium

Q.595 Rn

Q.596 True

Q.597 (b)

[SbF ]—

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.6OO Li is lighter than kerosense so it float over kerosene surface there if reacts with atmosphereic oxygen.

Q.6O1 The O of atmosphere tarnishes metallic surface by reacting with metal.

Q.6O2 (a, b)

Q.6O3 (a)

Q.6O4 (c)

Q.6O5 (a)

Q.6O6 Cs > Rb > K > Na > Li

Q.6O7 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.6O8 Yes

Q.6O9 Solution become alkaline

Q.61O 2M + ½O M O

Q.611 H O, Na O , KO , RbO , CsO2

Q.612 (b)

Q.613 Li

2 2 2 2 2



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 Na SO .10H O, Na SO , NaNO2 4 2 2 4 3

Q.619 d-block element

Q.62O 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.63O 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.64O It would have turned blue.

E D U C A T I O N S


2

2 2

22

2

2

2

INORGANIC PAPER CHEMISTRY P. JOYQ.641 Na O + H O 2NaOH + H O2 2 2 2 2

Na O + H O 2NaOH2 2

KO + H O 2KOH + H O + O2 2

Q.642 O

2 2 2

Q.643 (a) Na O diamagnetic (b) KO paramagnetic

(c) O paramagnetic (d) Na O paramagnetic

Q.644 Na2O2 + HCl(dil.)

Q.645 Li O < Na O < K O < Rb O < Cs O2 2 2 2 2

Q.646 They easily liberates oxygen.

Q.647 Na2CO3.10H2O, Na2CO3.7H2O, Na2CO3.H2O, Na2O

Q.648 s-block element.

Q.649 (d) Na O and Na vapour are formed.

Q.65O s-block elements have calculate with high thermal stability due to less polarizing power of cat-ions.

Q.651 Na CO > NaHCO > H CO2 3 3 2 3

Q.652 Cs2CO3 > ........... > Li2CO3

Q.653 (a) Li+ < Na+ < Rb+ < Cs+ (b) Li+ > Na+ > Rb+ > Cs+

(c) Li+ > Na+ > Rb+ > Cs+ (d) Li+ > Na+I > 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 NH +, substituted ammonium ions, Ti+, Ag+, spherical + 1 complex (n5 — C H ) Co+4

Q.659 Mg+2

5 5 2

Q.66O Na N does not exist at room temperature N — has high —ve charge & prefers covalent bonding3 3

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 HClO .3H O4 2

Q.663 (c)

Q.664 Li CO is stable due to higher polarizing power of lithium.2 3

Q.665 Hydration energy is greater then lattice energy.

Q.666 Due to anion hydrolysis.


3

2

INORGANIC PAPER CHEMISTRY P. JOYQ.667 LiHCO3, NaHCO3, KHCO3, RbHCO3, NH4HCO3

Q.668 Na CO is stable.2 3

Q.669 Na2O2 + H2O 2NaOH + H2O2

Na2O + H2O 2NaOH

Q.67O Li CO decomposed into LiO and CO but Na CO does not decomposed.2 3 2 2 3

Q.671 Because all bicarbonates passes H+ as an essential cation which polarises CO —2 ions and decom-poses into CO .

Q.672 All bicarbonates all soluble in water.

Q.673 Na CO is more basic in aqueous state.2 3

Q.674 Decomposed into 2Na CO + 2H O2 3 2

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.68O Strong reducing agent.

Q.681 (All)

Q.682 Paramagnetic

Q.683 By addition T.M. ion Na + NH (I) Fe3 NaNH + ½H3 2 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.69O 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.

E D U C A T I O N S


2

3

2

3

2

4 4 2

2

2

2

3

10

INORGANIC PAPER CHEMISTRY P. JOYQ.697 Li

Q.698 Na < K < Rb < Li <

Cs Q.699 Cs < Rb < K < Na

< K Q.7OO Li < Na < K < Rb

< Cs Q.7O1 Li < Na < K < Rb

< Cs Q.7O2 Cs < Rb < K < Na

< Li Q.7O3 Cs < Rb < K < Na

< Li Q.7O4 Li < Na < K < Rb

< Cs

Q.7O5 Li > Na > K > Rb > Cs

Q.7O6 Li CO < Na CO < K CO < Rb CO < Cs CO2 3 2 3 2 3 2 3 2 3

Q.7O7 CsHCO < RbHCO , KHCO < NaHCO < LiHCO3 3 3 3 3

Q.7O8 MF < MCl < MBr < MI

Q.7O9 KI > KBr < KCl

Q.71O Li > K > Na

Q.711 Li O, Na O < K O, Rb O < Cs O2 2 2 2 2

Q.712 Li < Na < K < Rb < Cs

Q.713 BLi < Na < K < Rb <

Cs Q.714 BLi < Na < K < Rb

< Cs

Q.715 MgSO4.7H2O

Q.716 Due to the formation of a surface film of the oxide.

Q.717 H

Q.718 MgO, Mg N

Q.719 Grignard Reagent

Q.72O Reducing agent.

Q.721 Mg

Q.722 Reaction is reversible & proceeds efficiently when CO is escaped which is only above 1100 K.

CaCO C CaO + O

Q.723 Quick time

Q.724 Disintegration of lump of lime in limited amt. of water.

Q.725 Sodalime.

Q.726 (a) CaO + SiO CaSiO

(b) CaO + P O Ca(PO )

Q.727 Ca(OH)2 when water is added to slaked lime.

Q.728 Aq. solution of Ca(OH)

2

2

4 4 4

3 2 22

INORGANIC PAPER CHEMISTRY P. JOYQ.729 Milk of lime.

Q.73O It turns milky.

Q.731 Ca(HCO3)2

Q.732 Ca(ClO)

Q.733 CaSO .2H O4 2

Q.734 When gypsum CaSO4.2H2O is heated to 393 K.

Q.735 Due to increased nuclear charge & smaller size.

Q.736 Covalent

Q.737 (i) Mg(OH) < Ca(OH) < Sr(OH)

< Ba(OH)2 2 2 2

(ii) Mg(OH)2 < Ca(OH)2 < Sr(OH)2 < Ba(OH)2

(iii) Mg(OH) < Ca(OH) < Sr(OH)

< Ba(OH)2 2 2 2

Q.738 Beryllate ion.

Q.739 Four

Q.74O MgBr2 & MgI2

Q.741 Ca

Q.742 CaF

Q.743 (i) BeCO3 < MgCO3 < CaCO3 < SrCO3 < BaCO3 (increasing thermal stability)

(ii) CaSO > SrSO > BaSO (Increasing solubility)

(iii) Ca(C O ) > Sr(C O ) > Ba(C O ) (increasing solubility)

Q.744 Ba

2 4 2 2 4 2 2 4 2

Q.745 2Ca(NO ) 2CaO + 4NO + O

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 MgSO .2H O, MgSO .7H O4 2 4 2

Q.75O By treating with H SO2 4

Q.751 By fractional crystallization

Q.752 MgSO .7H O4 2

Q.753 [Mg(H O) ]SO .H O2 6 4 2

Q.754 Potash magnesis is a Fertilizer & Its chemical composition K2SO4.MgSO4.6H2O.

Q.755 Purgative in medicine.

Q.756 Ca SiO , Ca SiO , Ca Al O2 4 3 5 3 2 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.

E D U C A T I O N S


2

2

2 2

3 3 2

INORGANIC PAPER CHEMISTRY P. JOYQ.758 J. Aspdin in 1824.

Q.759 It is the hydration of the molecules of the constituents and their rearrangement.

Q.76O 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.77O + 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 H S

Q.777 MnO

Q.778 Transition of electrons between d-orbitals of a metal.

Q.779 Ag+ polarises Br— and I—

Q.78O 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(O ) is formed.

Q.782 Mn

Q.783 Cr(OH)2 < Cr(OH)3 < CrO2(OH)2 acid strength increases with increase in oxidation number.

Q.784 Cr(OH) + 3HCl CrCl + 3H O

base

Cr(OH)3 + NaOH Na[Cr(OH)4]

acid

Q.785 Because of formation of oxide layer.

Q.786 [Fe(CN) ]3— has one unpaired electron (d2sp3 hybridised Fe3+) while [Fe(H O) ]3+ has five unpaired6 2 6

electrons (sp3d2 hybridised Fe3+)


62+ 4 2+

INORGANIC PAPER CHEMISTRY P. JOYQ.787 (a) 36 (b) 33 (c) 36 (d) 36

Q.788 I(b), II(a), III(c)

Q.789 [Co(H2O)4Cl2]Cl.H2O

Q.79O [Ni(H2O)4] > [Fe(CN) ]2— > [Fe(CN)6] = [Ni(H2O)4]

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.8OO 5VO2+ + MnO — + H O 5VO + + Mn2+ + 2H+4 2 2

Q.8O1 CrO3

Q.8O2 VI

Q.8O3 VI (O = — 2 diperoxo = — 4)

Q.8O4 VI

Q.8O5 V

Q.8O6 Cr O 2— < Cr3+ < Cr2+2 7

Smaller the oxidation state of the element in the ion, greater the reducing nature.

Q.8O7 2MnO — + 5H O + 6H+ 2Mn2+ + 5O + 8H O4 2 2 2 2

2MnO — + 3H O 2MnO + 3O + 2OH— + 2H O4 2 2 2 2 2

E D U C A T I O N S


3

2

3

2

2

2

3

—

— —


Q.8O8 Aqueous CO releases H+ which can convert MnO 2— into MnO and MnO — in a disproportionation2

reaction.4 2 4

CO + H O C H+ + HCO —2 2 3

3MnO4 + 4H+ MnO2 + 2MnO4 + H2O

Q.8O9 AgBr + 2Na S O2 2 3 Na [Ag(S O ) ] + NaBr3 2 3 2

Q.81O 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 2K2HgI4 + NH3 + 3NaOHHg

O NH 2 I + 4KI + 3NaI + 2H2OHg

(Iodide of M il lo n’s ba s e)

b row n p pt

Q.813 70% Cu + 30% Zn

Q.814 75% Cu + 25% Ni

Q.815 60% Ni + 20Fe + 20% Fe

Q.816 NO —, HCO —, CH COO—3 3 3

Q.817 NO —

Q.818 Na CO

Q.819 CO 2—

Q.82O CO

Q.821 S2— SO and CO 2— CO2 3 2

Q.822 CaCO3

Q.823 Ca(OH)

Q.824 Ca(HCO )3 2

Q.825 SO2

Q.826 Green.

Q.827 Cr+3

Q.828 Basic.

Q.829 Dichromate or chromate.

Q.83O Oxidising agents Cl , Br , KIO , Cu4+, K Cr O , KMnO .2 2 3

Q.831 Reducing agents.

2 2 7 4

Q.832 ppt dissolves through formation of CO2

Q.833 CO3 and SO3

Q.834 In presence of I— and Br—

Q.835 Pb, Ag, Sb, Sn


2

2

3 3

3 4

2

2

2 2

2

2

INORGANIC PAPER CHEMISTRY P. JOY— —Q.836 NO3 , NO

2 , chlorates.

Q.837 Cl is evolved as Cr O 2— are oxidising agent and oxidises Cl— into Cl2 2 7 2

Q.838 HCl

Q.839 Cr F , violet2 2

Q.84O HCl

Q.841 Cl

Q.842 Cl

Q.843 CrO4 (yellow colored ion) is formed.

Q.844 White ppt of AgCl

Q.845 NH

Q.846 AgI

solution, SO 2— solution, cyanide solution, hypo solution, amine solution.

Q.847 Fazan‘s theory.

Q.848 AgCl

Q.849 Cl—

Q.85O Soluble in hot water.

Q.851 H PO —

Q.852 CCl , CS4 2

Q.853 Br— Br (Red)

I— I (violet / purple)

Q.854 Cl2 water, HOCl, NaOCl, conc. HNO3

Q.855 Redox reaction take place and Br2 is liberated.

Q.856 H SO , HNO , MnO , PbO , Cl water, KMnO , NaOCl, HOCl2

Q.857 Cl

4 3

and F

2 2 2 2

Q.858 SO2 and I2 vapour is released.

Q.859 HCl, HBr and HI

Q.86O H S

Q.861 All can be oxidised.

Q.862 Formation of white ppt of Cu2I2

Q.863 I is formed

Q.864 K HgI2 4

Q.865 HgI K HgI2 2 4

Q.866 I—

Q.867 It forms free iodine, which is detected by starch.

Q.868 NO

E D U C A T I O N S


2

2

4 3 3 )

3

3

2 3

INORGANIC PAPER

Q.869 NO

Q.87O +1

Q.871 Al, Zn

Q.872 NO —, NO —

CHEMISTRY P. JOY

2

Q.873 NO2

Q.874 HNO

3

i.e. formed releasing NO.

Q.875 Pale, Blue

Q.876 NO

Q.877 Ba3(PO4)2

Q.878 Sulphide

Q.879 PbSO , BaSO , Ag SO , HgSO .HgO4 4 2 4 4

Q.88O HgSO4.HgO

Q.881 (NH ) MO4 2 4

Q.882 (NH ) Mg O .4H O4 6 7 24 2

Q.883 (NH ) [P(MO O10 4

Q.884 Canery yellow

Q.885 Yellow ppt of ferric phosphate is formed.

Q.886 White gelatinous ppt of zirconyl phosphate is formed.

Q.887 Phosphate and arsenate

Q.888 CO, CO2, H2O vapours

Q.889 Blue

Q.89O Redox takes place.

Q.891 Orange Green

Q.892 CH COO—

Q.893 Smell of vinegar is evolved.

Q.894 Silver acetate

Q.895 CH COO—

Q.896 FeCl3

Q.897 {Fe (OH) (CH COO) }+3 2 3 6

Q.898 Fe(OH)

Q.899 Formate

Q.9OO (C O 2—)

(CH COOH)

2 4


inorganic paper

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