INORGANICCHEMISTRY
Daily Practice Problems
CLASS : XIII DPP. NO.1
Q1. Aninorganiccompound (A) shows thefollowing reactions
(i) It is white solid and exists as a dimer, gives fumes ofB with wet air.
(ii) It sublimes at 1800C and forms monomer ifheated to 4000C.
(iii) Itsaqueous solutionturns bluelitmus to red.
(iv)Addition ofNH4OH and NaOH separatelyto a solution of(A) gives white ppt. whichis however
soluble inexcess ofNaOH. [Ans: (A)AlCl3; (B) HCl]
Q2. Asubstance(X)dissolves inconc. andhot HClto givesolutionwhichwhentreatedwithNaOH solution
gives a white ppt. which however dissolves in excess of NaOH. On heating X with sulphur, a brown
powderYisformed whichdissolvedonwarming withyellowammoniumsulphidesolution.The solution
gives a greyprecipitate withHCl. WhenX is heated inair, a white powder Z is obtained whenZ is dues
withNaOH, extracted withhot water, thentreated with mineralacid, whiteprecipitate is obtained.
[Ans: X = Sn; Y = SnS2; Z = SnO2]
Q3. Acertain metal (A) is boiled in dil. HNO3 to give a salt (B) and an oxide of nitrogen (C).An aqueous
solutionof(B) whichNaClgives a precipitate(D) whichis soluble inNH4OH. Ona whiteprecipiate (E)
is obtained. (E) on standing turns to a black compound (F). Identify(A) to (F).
[Ans: (A)Ag; (B)AgNO3; (C) NO; (D)AgCl; (E)Ag2S2O3; (F)Ag2S]
Q4. Identifythe unknownalphabets and completethe following reactions:
(i) (A) + dil. H2SO4 + K2Cr2O7  B (green coloured)
A + dil. H2SO4 + C  MnSO4 A + O2 
 
 O
H2 D D + BaCl2  White ppt.
(ii) A(aq) + Zn 
 B  ; A(aq) + C 
 PH3 ; A(aq) + PH4Cl  D 
[Ans: (i)A: SO2; B : Cr2(SO4)3; C : KMnO4; D: H2SO4; (ii)A: NaOH/KOH; B : H2; C :P4; D: PH3]
Q5. Ametalchloride (C) shows the following reactions.
(i) When H2S is passed in an acidified aqueous solution of(X), a black ppt. is obtained.
(ii) The precipitate obtained in step(i) isnot soluble is yellowammoniumsulphide.
(iii) When asolution ofSnCl2 isadded to aqueous solutionof(X) a white ppt. is obtained whichturns grey
on addition ofmore ofSnCl2.
(iv) WhenaqueoussolutionofKI isadded to anaqueoussolutionofXared ppt. is obtainedwhichdissolves
in excess ofKI. Identify‘X’. [Ans: HgCl2]
Q6. An aqueous blue coloured solution ofa transition metal sulphate reacts with H2S inacidic mediumto
give black ppt. (A) which is insoluble in warm aq. KOH. The blue solution on treatment with KI in
weaklyacidic medium, turns yellow and producesa white ppt. B. Identifythe transitionmetalionandA
and B. [Ans: Cu2+, A= CuS, Cu2I2]
Q.7 A given metal(X) on heating stronglyinpresence ofO2 gives anoxide which is also a constitutent ofa
whitepaint. Metal(X)ontreatment withdil. H2SO4 evolvesthe lightest gas(Y)andtheresultant solution
oncrystallizationgivesvitriol(Z). The metalis also used asaprotective coating oniron.Identify(X), (Y)
and (Z). [Ans: (X) Zn, (Y) H2, (Z) ZnSO4.7H2O]
Q.8 Anunknowninorganiccompound(X)losesitswaterofcrystallizationonheatinganditsaqueoussolution
gives thefollowing reactions.
(a) It givesa white turbiditywithdil. HClsolution.
(b) It decolourises a solution ofI2 inKI solution.
(c) It gives a white ppt withAgNO3 solutionwhichturn black onstanding.
Identify(X)givechemicalequations. [A: (X) Na2S2O3.5H2O]

INORGANICCHEMISTRY
Daily Practice Problems
Q.1 Acompound(X) gives a goldenyellow flame and shows the following reactions.
(a) Zn powder whenboiled with a concentrated solution of(X) dissolves and H2 is evolved.
(b) When an aqueous solution of (X) is added to an aqueous solution of SnCl2, a white precipitate is
produced which becomes soluble when (X) is added in excess.
(c) Compound (X) is used for thepreparation ofwashing soap on reaction with fat and oils.
(d) (X) is not a primarystandard henceits standard solutionisprepared bytitrating against oxalic acid using
phenolphthaleinindicator.
(e) Aqueous solution of (X) precipitates hydroxides ofAl3+ and Cr3+, which dissolves in its excess, the
former giving colourless solution, while the latter a yellow solutionin presence ofBr2 water.
Identify(X)givingdifferent reactions. [A: NaOH]
Q.2 A black colouredcompound (A) on reactionwithdil. H2SO4 gives a gas (B) whichonpassing through
a solution ofanacid (C) givesa white turbidity(D). Gas(B) when passed throughan acidified solution
ofacompound (E) gives ppt (F) whichis solubleindil. Nitric acid.After boiling this solutionanexcess
of NH4OH is added a blue coloured compound (G) is produced. To this solution on addition of
CH3COOH and aqueous K4[Fe(CN)6] a chocolate ppt (H) is produced. On addition of an aqueous
solutionofBaCl2 toaqueoussolutionof(E),awhitepptinsolubleinHNO3 isobtained. Identifycompounds
(A) to (H).
[A: (A) FeS (B) H2S (C) HNO3 (D) S (E) CuSO4 (F) CuS (G) [Cu(NH3)4]SO4 (H) Cu2[Fe(CN)6]]
Q.3 Acertaininorganic compound (A)onheatingloseswaterofcrystallization. Onfurther heatingablackish
powder (B) and two oxides ofsulphur (C) and (D) are obtained. The powder (B) onboiling with HCl
gives a yellow solution (E). When H2S gas is passed in (E) a white turbidity (F) and an apple green
solution(G)is obtained. The solution(E) ontreatment withthiocyanate iongives bloodred compound
(H). Identify(A) to (H).
[A: (A) FeSO4.7H2O, (B) Fe2O3, (C) SO2, (D) SO3, (E) FeCl3, (F) S, (G) FeCl2, (H) Fe(CNS)3]
Q.4 Anunknowncompound(A)givesayellowppt.onpassingH2Sgas.Thepptdissolvesinyellowammonium
sulphide to give a soluble thiosalt (B) and turbidity(C). The compound (A) giveschromylchloride test
and oxideofits cationisa wellknownslowpoison. The soluble salt (B) ontreatment withdil. HClgives
a yellowppt (D) inwhichcationof(A)is presentinthepentavalent state. (D)is insolubleinhotconcHCl
but it onheating withconc HNO3 dissolves to produce onacid of(A) with the liberationofNO gas and
sulphur is set free. Addition of ammonium molybdate solutionto conc. HNO3 solutionof(D) gives a
yellow ppt of(E). What are (A) to (E)? Give balanced equationofthe reactions.
[A: (A)AsCl3, (B) (NH4)3AsS4, (C) S, (D)As2S5, (E) (NH4)3AsO4.12MoO3]
Q.5 Anaqueoussolutionofinorganic compound(X) gives the followingreactions :
(a) With an aqueoussolution ofBaCl2 a whiteppt insoluble in dil. HClis produced.
(b) Addition ofexcess ofKI gives a brown ppt which turns white on addition ofexcess ofhypo.
(c) With an aqueous solution ofK4[Fe(CN)6] a chocolate coloured ppt. is produced. What is (X)?
Explainthereactions involved. [Ans: CuSO4 ]]
Q.6 A scarlet compound (A) is treated with conc. HNO3 to give a chocolate brown. The precipitate (B). It
is filtered and the filterate is neutralised with NaOH. Addition ofKI to the resulting solution gives a
yellow ppt. (C). The precipitate(B)onwarmingwithconc. HNO3 inthepresenceofMn(NO3)2 produces
a pink coloured solution due to the formation of ‘D’. IdentifyA, B, C and D. Write the reaction in
sequence. [Ans: (A) Pb3O4; (B) PbO2; (C) PbI2; (D) Pb(MnO4)2]
CLASS : XIII DPP. NO.2

Q.7 A white substance (A) reacts with dil. H2SO4 to produce a colourless gas (B) and colourless solution
(C). The reaction between (B) and acidified K2Cr2O7 solution produces a green solution and slightly
coloured ppt. (D). The substance (D) burns in air to produce gas (E) whichreacts with B to yield (D)
and colourless liquid.Anhydrous copper sulphate is turned blue on addition ofthis colourless liquid.
Additionofaqueous NH3 orNaOH to Cproduces first appt., whichdissolvesinthe excessofrespective
reagent to produce a clear solution in each case. Identify A, B, C, D and E. Write equation of the
reactionsinvolved. [Ans: (A) ZnS; (B) H2S;(C) ZnSO4; (D) S; (E) SO2]
Q.8 Anaqueous solutionofa gas (X) showsthe following reactions:
(i) It turnsred litmus blue.
(ii) When added in excess to copper sulphate solution deep blue colour is obtained.
(iii) Onaddition to a ferricchloride a brown ppt. soluble in dilute nitric acid is obtained.
Identify(X) and give equations for the reactions at steps(ii) and (iii).

INORGANICCHEMISTRY
Daily Practice Problems
Q.1 Draw theLewis structures ofthefollowing compounds
1. Fluorine F2
2. Dioxygen O2
3. Dinitrogen N2
4. Water H2O
5. Hydrogen peroxide H2O2
6. Hydroniumion H3O+
7. Sulphur dioxide SO2
8. Sulphur trioxide SO3
9. Sulphurous acid H2SO3
10. Sulphuric acid H2SO4
11. Hypochlorous acid HClO
12. Chlorous acid HClO2
13. Chloric acid HClO3
14. Perchloric acid HClO4
CLASS : XIII DPP. NO.3

15. Nitrous acid HNO2
16. Nitric acid HNO3
17. Chlorine heptaoxide Cl2O7
18. Hypophosphorous acid H3PO2
19. Phosphorus acid H3PO3
20. Pyrophosphorus acid H4P2O5
or disphosphorus acid
21. Metaphosphoric acid HPO2
22. Hypophosphoric acid H4P2O6
23. Orthophosphoric acid H3PO4
24. Phosphorus P4
25. Sulphur S8
26. Potassiumcyanide KCN
27. Sodiumnitrate NaNO3
28. Calciumcarbide CaC2
29. Copper Sulphate CuSO4
30. BariumCarbonate BaCO3

INORGANICCHEMISTRY
Daily Practice Problems
Q.1 Draw theLewis structures ofthefollowing compounds
1. Potassiumpermanganate KMnO4
2. Hyposulphurous acid H2SO4
3. Thiosulphuric acid H2S2O3
4. Pyrosulphuric acid H2S2O7
5. Peroxymonosulphuricacid (caro’s acid) H2SO5
6. Peroxydisulphuricacid (Marshall’s acid) H2S2O8
7. Dithionic acid H2S2O6
8. Trithionic acid H2S3O6
9. Tetrathionic acid H2S4O6
10. Pentathionic acid H2S5O6
11. Pyrophosphoric acid or diphosphoric acid H4P2O7
12. Triphosphoric acid H5P3O10
13. Tetraphosphoric acid H6P4O13
14. Peroxymonophosphoric acid H3PO5
CLASS : XIII DPP. NO.4

15. Peroxydiphosphoric acid H4P2O8
16. Chlorine monoxide Cl2O
17. Chlorine dioxide ClO2
18. Chlorine trioxide ClO3
19. Chlorate ion ClO3
–
20. Carbon sesqueoxide C3O2
21. Nitrosylchloride NOCl
22. Perchlorate ion ClO4
–
23. Iodate ion IO3
–
24.Azide ion N3
–
25. Iodine pentaoxide I2O5
26. Cynogen gas (CN)2
27. Xenontrioxide XeO3
28. Xenontetraoxide XeO4
29. Xenonoxydifluoride XeOF2
30. Xenonoxytetrafluoride XeOF4

INORGANICCHEMISTRY
Daily Practice Problems
Q1. Arrange inthe increasing order ofcovalent character (a) LiCl, LiBr, LiI (b) NaCl, MgCl2
, AlCl3
Q2. On the basis ofFajan’s Rule, arrange the following moleculesinincreasing order ofcovalent character.
(a) CuCl, NaCl (b) NaF, Na2
O, Na3
N
(c) NaCl, MgCl2
, AlCl3
, SiCl4
, PCl5
(d) NaF, NaCl, NaBr, NaI
Q3. Draw theLewis structures of
(a) C3
4–
(b) PF6
–
(c) ICl4
–
(d) PCl6
–
(e) [Fe(H2
O)6
]2+
Q4. Whydoes ammonia forms Co-ordinationcomplexes, whereas the isoelectronic species CH4
does not?
Q5. Aqueous solution ofa mixture contains LiCl, NaCland KCl. How is LiClseparated?
Q6. Compound withmaximumionic character isformed from
(A) Na and Cl (B) Cs & F (C) Cs & I (D) Na & F
Q7. Compound having highestMelting point is
(A) BeCl2
(B) MgCl2
(C) CaCl2
(D) SrCl2
Q8. Which ofthe following statements is correct for CsBr3
(A) It is a covalent compounds (B) It contains Cs+3
and Br–
ions
(C) It contains Cs+
and Br3
–
ions (D) It contains Cs+
, Br–
and Lattice Br2
molecule
Q9. The no. of(S–S) bonds in sulphur trioxide trimer (S3
O9
) is
(A) 3 (B) 2 (C) 1 (D)zero
Q10. Sulphide of phosphorus P4
S3
is a well known Chemical used in match industry. Phosphorus lies in
Trivalent and sulphur indivalent state. Draw the shape ofthe sulphide.
Q11. It is found that SnCl2
issoluble inwaterwhereas SnCl4
is aliquid itselfand is insolubleinwater. Explain.
Q12. Normallycertain metalsulphides are found to be precipitate in aqueous medium. Whereas their oxide
maybe soluble. Explain.
Q13. Explainthefollowing
(a) PCl5
is a stable molecule, but NCl5
is not.
(b) SF4
and SF6
are known, but OF4
and OF6
are not.
Q14. Discuss the hybridization and shapes ofthe following species–
(a) (NH3
)2+
(b) CH3
+
(c) NO2
–
(d) NO2
+
(e) H2
O2+
(f) ICl4
–
(g) OSF2
(h) O2
SF2
(i) OSF4
(j) TeCl4
(k) ClO3
+
Q15. Why?
CLASS : XIII DPP. NO.-5

Q16. Which one ofeach ofthe following pairs is expected to have the largerbond angle?
(A) H2
O & NH3
(B) SF2
& BeF2
(C) BF3
& BF4
–
(D) NH3
& NF3
Q17. Polarisation may be called as the distortion of the shape of an anion by an adjacently placed cation.
Whichofthe following statement(s) is(are) not correct?
(A) Minimumpolarisation is brought about bya cationoflow radius.
(B)Alarge cation is likelyto bring about a large degree ofpolarisation.
(C) Maximumpolarisation is brought about bya cation ofhigh charge
(D)Asmallanion is likelyto undergo a large degree ofpolarisation
Q18. Compare polarizing power ofthe following ions Li+
, Be2+
, B3+
& Na+
Q19. Whichcharge the following atoms would bearin the following ofanionic bond. Justify.
(a) Cs+
, Cs2+
(b) Ba+
, Ba2+
, Ba3+
(c)Al+
,Al3+
(d) O2–
, O4+
, O6+
(e) Pb2+
, Pb4+
Q20. At 1 atmpressure and300 K, densityofHFmolecules is3.25 gm/lt. NumberofHFmolecules associated
in a cluster is
(A) 2 (B) 3 (C) 4 (D) 6
Q21. What is uncertainityinlocationofaprotonofwavelength5000Åifwavelengthis knownto anaccuracy
of 1 pm?
(A) 8 × 10–14
m (B) 0.02 m (C) 3.9 × 10–8
m (D) none
Q22. (a) Increasing covalent character TiCl2
, TiCl3
,TiCl4
(b) Increasingionic character VCl2
, VCl3
, VCl4

INORGANICCHEMISTRY
Daily Practice Problems
CLASS : XIII DPP. NO.-6
Q.1 Whichofthe following compounds ofelementsin groupIV isexpected to be most ionic ?
(A) 2
PbCl (B) 4
PbCl (C) 4
CCl (D) 4
SiCl
Q.2 Which has the lowest anionto cationsize ratio :
(A) LiF (B) NaF (C) CsI (D) CsF
Q.3 Whichofthe following compounds contain/s bothionicand covalent bonds?
(A) NH4Cl (B) KCN (C) CuSO4·5H2O (D) NaOH
Q.4 Whichofthe following compound is/arepredominantlyionic?
(A) KCl (B) Na2S (C) H2 (D) CaO
Q.5 Onheatingto 400-500ºC, relativelyunstablehydridesandcarbonatesdecompose. Whichofthefollowing
may decompose when heated to 400-500ºC ?
(A) LiH (B) NaH (C) 3
2CO
Li (D) 3
2CO
Na
Q.6 Whether the following reactions are possibleor not :
(a) Tl+ +Al3+ Al+ + Tl3+ (b) Sn2+ + Pb4+  Sn4+ + Pb2+
Q.7 5
PCl exists but 5
NCl does not because :
(A) Nitrogen has no vacant 2d-orbitals (B) 5
NCl is unstable
(C) Nitrogenatomis much smallerthan P (D) Nitrogenis highlyinert
Q.8 3
AgNO gives a white precipitate withNaCl but not with 4
CCl . Why?
Q.9 Whichofthe following Lewis diagrams is(are) incorrect ?
(A) 










 l
C
O
Na (B)
Cl
Cl C Cl
Cl
(C)















2
|
|
H
H
H
N
H [ ] -
S 2
(D) H
H
N
H
N
H 






|
|
Q.10 The totalnumber ofvalence electrons in4.2g of 
3
N ionare :
(A) 2.2 NA (B) 4.2 NA (C) 1.6 NA (D) 3.2 NA
Q.11 Pick out among thefollowing species isoelectronic with 2
CO :
(A) 
3
N (B) 
)
(CNO (C) 
2
)
(NCN (D) 
2
NO
Q.12 Which ofthe followingoxyacids ofsulphur contain S
S  bonds ?
(A) 8
2
2 O
S
H (B) 6
2
2 O
S
H (C) 4
2
2 O
S
H (D) 5
2
2 O
S
H
Q.13 When magnesiummetalis burnt inair, it forms two productA& B.
Areacts withwater to forma basic solution. B reacts with water to forma similar solution as thatofA
with agas witha pungent odour. IdentifyAandB and write equations for the reaction.
Q.14 Fromthe following data calculate the bond energyofthe F2
– ion
F2 (g)  2F(g) H0 = 157 kJ/mol
F– (g)  F(g) + e H0 = 333 kJ/mol
F2
– (g)  F2(g) + e H0 = 290 kJ/mol
Explain the difference betweenthe bond energies ofF2 and F2
–.
Q.15 DrawLewisstructures for the followingorganic molecules:
(a) C2F4 (b) C3H8 (c) butadiene (C4H6) (d) Propyne (C3H4) (e) CH2O (f) C2H4O2

INORGANICCHEMISTRY
Daily Practice Problems
Q.1 Draw theLewis structures ofthefollowing compounds
1. Hydrazine 2. Hyponitrous acid (H2N2O2) 3. Hydroxylamine (NH2OH)
4. Dithionate ion (S2O6
2–) 5. Trithionate ion (S3O6
2–) 6. Tetra thionate ion (S4O6
2–)
7. Pentathionate ion 8. Thionylchloride (SOCl2) 9. Sulphurylchloride (SO2Cl2)
10. Peroxymononitric acid (HNO4) 11. Calciumphosphite
12. Disodiumhydrogen phosphate 13. Sodiumdihydrogenphosphate
14. POCl3 15. S2F10 16. O2F2 17. N2O5 18. S2O7
2–
19. Inorganic Benzene 20. Inorganic graphite
Q.2 Out ofthe following whichone has thehighest covalent character
(A) ZnCl2 (B) CaCl2 (C) CdCl2 (D) CuCl
Q.3 Whichoneofthe following is anacetylide
(A)Al4C3 (B) BeC2 (C) CaC2 (D) Mg2C3
Q.4 Ifanatomhas emptyd-orbitalsavailable, thenit maybe able to usethemto accomodate morethaneight
electrons and hence to expand its octet to 10, 12 or even more electrons. That capacitymay
(A) not allow the centralatomto formadditionalmultiple bonds to the atomattached to it.
(B) allowthe centralatomto formadditionalmultiple bondsto the atoms attached to it.
(C) not allow to formadditionalsingle bondsto more atoms.
(D) allow to formadditionalsingle bonds to more atoms.
Q.5 The hydrationofionic compounds involves:
(A)Evolutionofheat (B) Dissociationofions
(C)Weakening ofattractive forces between the ionsoforiginalcompounds
(D)Allofthese
Q.6 Which ofthe following statement is(are) true for BaOand MgO?
(A) BaO is more ionic than MgO (B) MgO is more ionic than BaO
(C) BaO has a higher meltingpoint thanMgO (D) MgOhas a higher meltingpoint thanBaO
Q.7 Rotationaround the bond (betweenthe underlined atoms)is restricted in
(A) C2H4 (B) H2O2 (C)Al2Cl6 (D) I2Cl6
Q.8 To which ofthe following species octet ruleis not applicable:
(A) BrF5 (B) SF6 (C) IF7 (D) CO
Q.9 Which ofthe following species arehyper valent?
(1) ClO4
– (2) BF3 (3) SO4
2– (4) CO3
2–
(A) 1, 2, 3 (B) 1, 3 (C) 3, 4 (D) 1, 2
Q.10 Formationofwhichofthe following anionis not possible
(A) [AlF6]3– (B) [SiF6]2– (C) [BF6]3– (D) [BF4]–
CLASS : XIII DPP. NO.-7

INORGANICCHEMISTRY
Daily Practice Problems
Q.1 The formationofionic solids fromthe elements is anexothermic process. This isprimarilydue to
(A) The low values for vaporisationofthe metals (B) Theelectronaffinityterm
(C) The large values ofthe Latticeenergyofthese solids.(D) The low values for I.E. ofthe metals
Q.2 Given the electronegativities of three elements
x = 1.0 y = 2.5 z = 3.0
Type of bonding formed between xz and yz respectively would be:
(a) Covalent, ionic (b) Ionic, covalent
(c) Polar covalent, covalent (d) None of the above
Q.3 CO2
is isosteric with:
(1) HgCl2
(2) SnCl2
(3) C2
H2
(4) NO2
The correct answer is :
(a) 1, 2 (b) 2, 3 (c) 1, 3 (d) 2, 4
Q.4 Which of the following is not applicable-
(A) CO2
irregular geometry (B) BF3
regular geometry
(C) NH3
irregular geometry (D) SO2
irregular geometry
Q.5 C-C bond in C2
H6
undergoes heterolytic fission, the hybridisation of Carbon is/are 
(A) SP2
(B) SP3
(C) SP2
, SP3
(D) SP, SP2
Q.6 The halogen form compounds among thenselves with formula XX’, X '
3
X , X '
5
X , X '
7
X where X is
the heavier halogen. Which of the following pairs representing their structures and being polar and
non-polar are correct-
(A) XX’LinearPolar (B) X '
3
X T-shapedPolar
(C) X '
5
X Square PyramidalPolar (D) X '
7
X PBPNon Polar
Q.7 The value ofH0
forthe reactions Cu+
(g)+ I–
(g)  CuI(g)is –446 KI. Ifthe I.E. ofCu(g)is 745 kJ/mol
and the E.A. ofI (g) is –295 kJ/mol, thenthe value ofH0
for the formationofone mole ofCuI(g) ion–
pairs fromCu(g) and I(g) is
(A) –446 kH (B) 450 KI (C) 594 kJ (D) 4 kJ
Q.8 Whichofthe following reactions are not possible/possible?
(a) Sn2+
+ 2Hg2+
 Hg2
2+
+ Sn+4
(b) Ge2+
+ Pb4+
 Pb2+
+ Ge+4
(c) Tl+1
+ Ga3+
 Ga+
+ Tl3+
Q.9 Predict the shapes of (a) TeCl4
(b)ClO3
(c) Cl 
3
O
Q.10 Cl 
2
F is linear but the ion Cl 
2
F is bent explain.
Q.11 A compound ofchlorine and fluorine ClFn
reacts at about 75o
C with vranium metal to produce UF6
and ClF(g). A quantity of vranium produced 3.53 gm. UF6
and 343 ml ClF at 75o
C and 2.5atm.
What is the formula of the Compound Determine its shape.
Q.12 The common forms of N and P are N2
and P4
respectively.
:N N 946 ; P  P 481; N - N 160; P - P 215
Using these data explain why the stable forms are N2
and N4
; P4
and not P2
.
CLASS : XIII DPP. NO.-8

INORGANICCHEMISTRY
Daily Practice Problems
CLASS : XIII DPP. NO.-9
For Questions 1 to 3 :
When hybridisation involving ‘d’ orbitals are considered then allthe ‘5d’ orbitals are not ‘degenerate’
rather 2
2
y
x
d  , 2
z
d &dxy
, dyz
&dxz
formtwo different sets and the orbitalof‘appropriate’set is involved
inthehybridisation. Onthis informationanswer the question.
Q.1 In sp3
d2
hybridization whichorbitals are involved?
(A) 2
2
2
z
y
x
d
&
d  (B) xy
z
d
&
d 2 (C) dxy
& dyz
(D) xy
y
x
d
&
d 2
2

Q.2 In sp3
d3
hybridisationwhichorbitals are involved?
(A) 2
2
y
x
d  / 2
z
d /dxy
(B) dxy
/dxz
/dyz
(C) 2
2
y
x
d  /dxy
/dxz
(D) 2
z
d /dxz
/dyz
Q.3 Also ifit is known that in case lesser electrons are present in 2
2
y
x
d  & 2
z
d then ‘d’ orbitalinvolved in
sp3
d hybridisation
(A) dxy
(B) dxz
(C) dyz
(D) 2
z
d
Q.4 Explain whyI–I–I bond angle is higher in I3
–
as compared to I3
+
.
Q.5 Each ofthe following pairs ofchemicalspecies undergoes chemicalcombinationthrough a coordinate
bond?
(A) Ca+ ½ O2
(B) Ag+
+ 2NH3
(C) H2
+ ½O2
(D) Cl(g) + Na(g)
Q.6 F–As–F bond angle inAsF3
Cl2
can be
(A) 900
& 1800
only (B) 1200
only (C) 900
& 1200
only (D) 900
only
Q.7 Whichofthe following orbitals cannot undergo hybridizationamongst themselvesaccording to valence
bond theory
(i) 2px
, 2py
& 2pz
(ii) 3d & 4d (iii) 3d, 4s & 4p (iv) 3s, 3p & 4s
(A) only(ii) (B) (ii)&(iii) (C) (i), (ii) & (iv) (D) (ii)& (iv)
Q.8 Inthefollowingreaction
C2
H2 
 2
H C2
H4 
 2
H C2
H6
the state ofhybridisation ofcarbonchanges from
(A) sp  sp2
 sp3
(B) sp3
 sp2
 sp
(C) sp2
 sp3
 sp (D) sp3
 sp  sp2
Q.9 The bond present in [Cu(NH3
)4
]SO4
are
(A) Ionic (B) Coordinate (C) Covalent (D)All
Q.10 Amixture1,2–Dipropeneandhydrogengaswasplacedinarigidsteelcontainerataconstant temperature
of18°C. Initialpressure ofmixture was10 atm. Sparking the mixture caused hydrogenationreaction
C3H4 (g) + 2H2(g) C3H8 (g)
causing pressure to decrease by6 atm. Excess O2 was thenadded andonsparking thepressure further
decreased by11 atm. CalculatedecreaseinpressurebytreatingfinalmixturewithaqueousKOH solution.

INORGANICCHEMISTRY
Daily Practice Problems
Q.1 Lithium among alkalimetals exhibits chemical properties different from the rest ofthe alkali metals.
Whichofthe following statements illustratesthis fact?
(A) Lialone among the alkalimetals displaces hydrogen fromC6
H5
–CCH
(B) LiOHis a stronger alkalithan the other alkalimetalhydrogen.
(C) LiH is thermallyless stable than NaH
(D) LiClissoluble in organic solvents
Q.2 An element is oxidised by fluorine and not by chlorine. Could the element be sodium?Aluminium?
Sulphur?Oxygen?Explainyour answer.
Q.3 Whichofthefollowing reaction would not proceed to R.H.S.
(a) F2
+ Cl–
 (b) Cl2
+ Br–
 (c) Br2
+ I–
 (d) I2
+ Cl–

Q.4 Agaseous reaction,A2
(g)  B(g)+ ½ C(g) shows increase in pressurefrom100 mmto 120 mmin
5 minutes. The rate of disappearance ofA2
is
(A) 4 mmmin–1
(B) 8 mmmin–1
(C) 16 mmmin–1
(D) 2 mmmin–1
Q.5 Whichiswrong statement?
(A) The decreasing order ofbond angle is H2
O > H2
S > H2
Se > H2
Te
(B) The decreasing order of bond angle is NH3
> PH3
>AsH3
> SbH3
(C) The decreasing order of bond angle is F2
> Cl2
> Br2
> I2
(D)The decreasing order of bond angle is CH4
> NH3
> H2
O
Q.6 Structure ofNa2
[B4
O5
(OH)4
]·8H2
O contains
(A)Two triangularand two tetrahedralunits
(B) Three triangularand one tetrahedralunits
(C)Alltetrahedralunits
(D)Alltraingular units
Q.7 A:Tetracyanomethane B: Carbondioxide C: Benzene D: 1, 3–buta–di–ene
Ratio of and  bonds is in order:
(A) A= B < C < D (B) A= B < D < C (C) A = B = C = D (D) C < D < A< A
Q.8 Number ofP–H, P–O–P, P–O–H & P= O bonds in sodium dihydrogen pyro phosphate respectively
are
(A) 1, 1, 1, 2 (B) 0, 1, 2, 2 (C) 0, 1, 1, 3 (D) 2, 0, 0, 2
Q.9 Amongst NO3
–
, AsO3
3–
, CO3
2–
, ClO3
–
, SO3
2–
and BO3
3–
the non-planar species are
(A) CO3
2–
, SO3
2–
, BO3
3–
(B) AsO3
3–
, ClO3
–
, SO3
2–
(C) NO3
–
, CO3
2–
, BO3
3–
(D) SO3
2–
, NO3
–
, BO3
3–
Q.10 The compound MX4
is tetrahedral. The number ofXMX angles inthe compound is
(A) three (B)four (C) five (D)six
Q.11 The nodalplane in the –bond ofethene is located in
(A) themolecular plane
(B) a plane parallelto the molecular plane
(C) aplane perpendicular to themolecular plane whichbisectsthe carbon–carbonbondat right angle.
(D) a plane perpendicualr to the molecular plane which contains the carbon carbon bond
Q.12 Azobenzene (C6
H5
)2
N2
: . Predict the hybridization for the atoms
marked with (*) and indicate the value ofthe bond angles labelled and .
CLASS : XIII DPP. NO.-10

INORGANICCHEMISTRY
Daily Practice Problems
Q.1 Which molecular geometryis least likelyto result froma trigonalbipyramidalelectrongeometry?
(A) trigonalplanar (B) see saw (C) linear (D) T-shaped
Q.2 Whichofthe following ions containsS–S linkage?
(A) pyrosulphite ion (B) peroxydisulphate ion
(C) pyrosulphate ion (D) peroxymonosulphate ion
Q.3 Whichhasmaximumdipole moment?
(A) (B) (C) (D)
Q.4 Which is not correctlymatched?
(A) XeO3
:Trigonalbipyramidal (B) ClF3
: bent T–shape
(C) XeOF4
: square pyramidal (D) XeF2
: Linear Shape
Q.5 Match list Iwith list II and select the correct answer:
List I List II
(i) NO2
+
1. 1800
(ii) NO2
2. 1320
(iii) NO2
–
3. 1200
(iv) NO2
–
4. 1150
5. 1090
(A) (i)  5; (ii)  4; (iii)  3; (iv)  2 (B) (i)  5; (ii)  2; (iii)  4; (iv)  3
(C) (i)  1; (ii)  2; (iii)  4; (iv)  3 (D) (i)  1; (ii)  4; (iii)  3; (iv)  2
Q.6 In a compound
the number ofsigma and pibonds respectivelyare
(A) 19, 11 (B) 19, 5 (C) 13, 11 (D) 7, 3
Q.7 In P4
, P2
O3
and P2
O5
have how many  bonds?
(A) 12, 6, 16 (B) 16, 6, 12 (C) 6, 12, 16 (D) 16, 16, 12
Q.8 Structure ofS2
Cl2
isanalogues to
(A) SOCl2
(B) CO2
(C) H2
S (D) H2
O2
Q.9 In whichofthe following compound B–Fbond lengthis shortest?
(A) BF4
–
(B) H3
N–BF3
(C) BF3
(D) (CH3
)3
N  BF3
Q.10 The correct sequence ofpolarityofthe following molecule
1. Benzene 2. Inorganic benzene 3. PCl3
F2
4. PCl2
F3
(P stands for polar and NP stands for non-polar)
1 2 3 4 1 2 3 4
(A) P NP NP P (B) NP NP NP P
(C) NP P NP P (D) NP P P NP
CLASS : XIII DPP. NO.-11

Q.11 The shapes of XeF4
, XeF5
–
and SnCl2
are
(A) octahedral, trigonalbipyramidaland bent
(B) square pyramidal, pentagonaland bent
(C) square planar, pentagonalplanar and bent
(D) see saw, T-shaped and linear
Q.12 The C–C singlebond distance is 1.54Å. What is the distance between the terminalcarbons in propane
(C3
H8
)?Assume that the four bonds ofanycarbon atoms are pointed towards the corners ofa regular
tetrahedron. [sin (540
44) = 0.758]

INORGANICCHEMISTRY
Daily Practice Problems
CLASS : XIII DPP. NO.-12
Q1. The HF2
–
ion exists in the solid state and also in liquid HF solution, but not indilute aqueous solution.
Explain.
Q2. Ortho chloro phenolis less polar thanortho fluoro phenol.
Q3. The forcesofattractionin liquidheliumare
(A) Ionic (B)Metallic (C) Vander Waals (D)covalent
Q4. The nature ofIntermolecularforces among benzene (C6
H6
)molecules is
(A) Dipole- dipole attraction (B) dispersion forces
(C) ion-dipole attraction (D) H–bonding
Q5. Identifythecorrect statements fromthegivenalternatives
(A) Intramolecular H–bonding is not found to occurin 2–hydroxybenzaldehyde
(B) The B.Pt. ofHI is more than HF
(C) The dipole moment ofCH3
Clis not equalto zero
(D) CH3
F has a smaller dipole moment than CH3
Cl
Q6. There is a large difference betweenB.Pt. ofButanoland Butanal, although theyhave almost the same
solubilityinwater. Explain.
Q7. The H–bondingin HF is stronger than in H2
O, but the B.Pt. ofwater is higher than that ofHF.
Q8. The two molecules indicated below are capable ofintramolecular H–bonding. Which is likelyto form
more stable H–bonds?
Q9. Explain why (maleate) is more stable than (Fumerate ion)
Q10. Consider the followinglist ofmolecules
(a) HNO3
(b) H2
SO4
(c) HClO4
(d) CH3
F (e) HF (f) HgCl2
(g) CCl2
F2
(h) CH3
OH (i) CH3
-O-CH3
(j) CH3
-CO-CH3
(k) CH3
CHO (l) HCOOH
(m) CH3
NH2
(n) C6
H5
NO2
(o) CH3
COOCH3
(p) OF2
(q) PCl3
(r) XeF4
(s) CH3
CONH2
(t)dichlobenzene (u) dichloropropane (v) C6
H5
COOH
(w)AceticAnhydride (x) 2,3-dichloro-2-butene (y) C2
H6
O
(i) Which ofthese are polar? (ii) Which ofthese exhibit H–bonding?
Q11. Arrange the following inthe increasingorder of
(a) C2
H5
OH, CH3
CHO, CH3
COOH (B.Pt.) (b) Pentane, Pentene, pentyne (B.Pt.)
(c) HF, HCl, HBr, HI (d) H2
O, H2
S, H2
Se (B.Pt.) (e) He, Ne, Ar, Kr (B.Pt.)
(f) F-
, O, N, F (H-bondingstrength) (g) F-
, S2-
, Cl–
, P3-
(Polarisability)
Q12. Account forthe following
(a) Benzene isalmost insoluble inwater, but pyridine is soluble.
(b) There iscantractionin valume as ice melts and the densityofwater is maxiumumat 4o
C.
(c) H2
O is lessbasic thenNH3
, eventhoughoxygenhas a greater number oflove pair ofe-
sthannitrogen
(d) The tendencyfor catenation decreases down the group inthe carbon family.

INORGANICCHEMISTRY
Daily Practice Problems
CLASS : XIII DPP. NO.-13
Q1. Select the species which is best decribed bythe statement in the brackett.
(a) CO2
, NH3
, CO( zero dipole moment) (b) CH4
, NH3
, HF(max. B.Pt.)
(c) Cl2
, Br2
, I2
(min. B.Pt.) (d) HOI, HOBr, HOCl (Weakest Acid)
Q2. Which threemolecules would you expect to be polar &which non-polar:
(Cl2
, ICl, BF3
, NO, SO2
, XeF4
, CH2
Cl2
, OCS)
Q3. Whichhasdipole moment
(A) [Ni(CN)4
]2–
(B) CHCl3
(C) CO2
(D)
Q4. Dipole moment is shown by
(A) 1, 4–dicholorobenzene (B) Cis–1–2, dichloroethene
(C) Trans–1, 2–Dichloroethene (D) Trans–2, 3–Dichloro–2–Pentene
Q5. Whichofthefollowing has dipole moment
(A) Nitrobenzene (B)P–chloronitrobenzene
(C) m–di–chlorobenzene (D) O–di–chloro–benzene
Q6. The dipole moment ofCH2
Cl2
is greater than that of CHCl3
. Why?
Q7. Which isomer ofthe molecule PBr2
Cl3
isexpected to have maximumdipole moment value?
Q8. NH3  BF3
adduct can be easily separated into its component:
(a) Usually the coordinate compounds are unstable.
(b) BF3
and NH3
have their independent existence.
(c) Difference in the number of electrons between N and B is 2.
(d) BF3
and NH3
possess no resultant dipole moment.
Q9. Type of bonding exists in HCl(gaseous state):
(a) Pure covalent (b) Polar covalent (c) Pure ionic (d) Dative
Q10. Species containing no peroxide ion would be:
(a) PbO (b) H2
O2
(c) SrO2
(d) BaO2
Q11. Conside the following energies
I : Covalent single bond energy
II :Average translational kinetic energy of gases at room temperature
III: Rotational barrier energy in ethane between eclipsed and staggered forms.
IV : Ionisation energy of hydrogen atom
The order of magnitude of these energies is
(A) I > II > III > IV (B) IV > III > II > I (C) IV > I > III > II (D) IV > II > I > III
Q12. The dipole moments of the given molecules are such that
(A) BF3
> NF3
> NH3
(B) NF3
> BF3
> NH3
(C) NH3
> NF3
> BF3
(D) NH3
> BF3
> NF3

INORGANICCHEMISTRY
Daily Practice Problems
Q.1 Which bond angle,  would result in the maximum dipole moment for the triatomic molecule XY2 shown
below:
(A)  = 900 (B)  = 1200 (C)  = 1500 (D)  = 1800
Q.2 The correct increasing bond angle among BF3, PF3 and ClF3 follows the order
(A) BF3 < PF3 < ClF3 (B) PF3 <BF3 < ClF3 (C) ClF3 < PF3 < BF3 (D) BF3 = PF3 = ClF3
Q.3 Which one of the following compounds has bond angle close to 90°?
(A) NH3 (B) H2S (C) H2O (D) CH4
Q.4 Which is the correct Lewis arrangement of 
2
2
S ion?
(A) [ = ]2– (B) [ – ]2– (C) [S S]2– (D) none of these
Q.5 Which one of the following is the correct structure of XeOF4?
(A) (B)
Square pyramid with Xe = O in the square plane Trigonal bipyramid with equatorial Xe = O
(C) (D)
Trigonal bipyramid with axial Xe = O Square pyramid with axial Xe = O
Q.6 The pressure in a container of some volume at some temperature is found to be P atm when it contained 1
mole of NH3 gas. What would be final pressure if 2 mole of H2, 2 moles of HCl gas & 1 mole of O2 is
introduced into the containers under same condition.
(A) 6 P (B) 3 P (C) 4 P (D) P
Q.7 Which of the following options are written with correct order of polar nature of bonds.
(i) NH3 > PH3 > SbH3 > AsH3 (ii) NH3 > AsH3 > SbH3 > PH3 (iii) NH3 > SbH3 > AsH3 > PH3
(iv) H2O > H2S > H2Se > H2Te (v) H2O > H2Te > H2Se > H2S
(A) (i) & (iv) (B) (iii) & (iv) (C) (iii) & (v) (D) (ii) & (iv)
Q.8 Two element X and Ycombined together to form a molecule in which X is a central atom. In the surrounding
of nucleus X the % of p character is found to be 80% then the hybridised state in molecule is :
(A) sp2 (B) sp3 (C) sp4 (D) sp5
Q.9 A perfect gas of a given mass is heated first in a small vessel and then in a large vessel, such that their
volume remains unchanged. The P–T curves are
(A) parabolic with same curvature (B) parabolic with different curvature
(C) linear with same slope (D) linear with different slope
Q.10 100 ml of phosphine when decomposed produces phorsphorus and H2. The change in volume is
(A) 50 ml increase (B) 500 ml decrease (C) 900 ml decrease (D) none of these
Q.11 Which of the following solid(s) consists of molecules held together by vander Waals’ forces
(A) Calcium carbonate (B) Calcium dioxide (C) Sugar (D) Iodine
Q.12 Calculate the percentage ionic character of C-Cl bond in CCl4, if the electronegativities of C & Cl are 3.5
& 3.0 respectively.Using Hanny & smith equation [16 (XA – XB) + 3.5 (XA – XB)2]. If this % ionic
character can be equated to one calculated using dipole moment than calculate the bond length of C–Cl
bond if bond dipole of C–Cl is 1.5 D. Also calculate total charge on C & Cl atoms.
CLASS : XIII DPP. NO.-14

INORGANICCHEMISTRY
Daily Practice Problems
Q.1 Whichofthe following molecules areexpected to exhibit intermolecularH – bonding.
I :Acetic acid II :o-nitrophenol III: m-nitrophenol IV : o-boric acid
Select correct alternate?
(A) I, II, III (B) I, II, IV (C*) I, III, IV (D) II, III, IV
Q.2 What is not true about ice?
(A) It hasopencage like structure. (B) It has less densitythan water
(C) EachOatomis surroundedby4 Hatoms (D*) EachO atom has 4–H bonds around it
Q.3 Assuming the bond direction to be z-axis, whichofthe overlapping ofatomic orbitals oftwo atom(A)
and (B) willresult inbonding?
(I) s-orbital ofAand px orbitalof B (II) s-orbital ofAand pz orbitalofB
(III) py-orbital ofAand pz orbitalofB (IV) s-orbitals ofboth (A) and (B)
(A) I and IV (B) I and II (C) III and IV (D*) II and IV
Q.4 GivethecorrectorderofinitialsTorFforfollowingstatements. UseTifstatementistrueandFifitisfalse.
(i) The order of repulsion between different pair ofelectrons is lp – lp > lp – bp > bp – bp
(ii)Ingeneral, as thenumberoflone pair ofelectrons oncentralatomincreases, value ofbondanglefrom
normalbond angle also increases.
(iii) The number of lone pair onO in H2O is 2 while on N in NH3 is 1.
(iv) The structures ofXenon-fluorides and Xenon-oxyfluorides could not be explained onthe basis of
VSEPR theory.
(A)TTTF (B*) TFTF (C) TFTT (D) TFFF
Q.5 The bond length ofthe S–O bond is maximuminwhichofthe givencompound :SOBr2,SOCl2, SOF2
(A) SOCl2 (B*) SOBr2 (C) SOF2 (D)Allhave same length
Q.6 The diagrambelowshows part ofthe skeletonofthe PeriodicTable in which elementsare indicated by
letters whichare not their usualsymbols
Q
H L R
J T
M
Whichone ofthe following statementsis correct?
(A) Thegreatest ionic character ofcompounds formed byreactionofpairs ofthelisted elements would
be exhibitedbythe compound withthe formula, M2Q
(B*) The J2+ ionis coloured in aqueous solution
(C) The carbonate ofelement H isinsoluble inwater
(D) Element R is a gasat roomtemperature
Q.7 The ground state electronic configurations of the elements, U, V, W, X and Y(these symbols do not
have anychemicalsignificance) are as follows
U 1s22s22p3 V 1s22s22p63s1 W 1s22s22p63s23p2
X 1s22s22p63s23p63d54s2 Y 1s22s22p63s23p63d104s24p6
Determine whichsequence ofelements satisfythe following statements
(i) element-forms a carbonate which is not decomposed byheating
(ii) element-ismost likelyto formcoloured ionic compounds
(iii) element-haslargest atomic radius
(iv) element-formsonlyacidic oxide
(A) V WY U (B*) V X Y W (C) V WY X (D) V X W U
CLASS : XIII DPP. NO.-15

Q.8 Give the correct order ofinitialsT or F for followingstatements. Use T ifstatement is true and F ifit is
false.
(I) Br–P–Br bond angle in PCl3Br2 is 180°.
(II) 
2
NO , NO2 & 
2
NO species have O–N–O bond angle order,
, 
2
NO < NO2 < 
2
NO .
(III) Oxyacid is not produced, when NCl3 undergoes hydrolysis.
(IV) In complete combustionofmethane, change in hybridisation ofcarbon atomundergoes sp3 to sp.
(A) TTTF (B) TFTT (C) FTFF (D*) FTFT
Q.9 Whichofthe following compounds havethe same number oflone pairs withtheir centralatom
(I) XeF5
– (II) BrF3 (III) XeF2 (IV) H3S+ (V)Triplet methylene
(A) IV & V (B) I & III (C) I & II (D) II, IV & V
Q.10 When ice melts to formliquid water at 00C, there is a contractionin volume. This is due to
(A) the moleculecontracting insize
(B) a partialdisruption ofthe hydrogenbonded network ofice onmelting
(C) the absorptionofheat during themelting process
(D) thedissolving ofair into the water during themelting process
Q.11 Whichisomer ofhydroxyacetophenone steamdistills?
(A) O–isomer (B)m–isomer (C) p–isomer (D)all
Q.12 Which statement is correct?
(A) Boiling point ofH2O, NH3, HFaremaximumin their respective groupdue to intermolecular
H–bonding.
(B) Boiling point ofCH4 out of CH4, SiH4, GeH4 and SnH4 is least due to intermolecular force of
attraction
(C) Formic acid forms dimer byH–bonding
(D*)Allare correct

INORGANICCHEMISTRY
Daily Practice Problems
CLASS : XIII DPP. NO.-16
Q.1 Which ofthe following sets ofcharacteristics leads to the increase insolubilityofionic substances?
(A) Highdipole moment, strong attractionbyan ion andlarge solvation energy.
(B) Lowdipole moment, weak attractionbyan ion and highsolvationenergy.
(C) Highdipole moment, strong attractionbyan ion and low solvation energy.
(D) Highdipole moment, weak attractionbyanionand large solvationenergy.
Q.2 The dipolemoment ofChlorobenzene is 1.5 D. The dipole moment of1, 2, 3, 5–tetrachlorobenzene is:
(A) 0 (B) 1.5 D (C) 2.86 D (D) 2.25 D
Q.3 Dipole moment of H2O is 1.85 D. If bond angle is 1050 and O–H bond length is 0.94 Å, determine
magnitude ofthe charge on the oxygenatomin the water molecule. (Given: cos 52.5 Å = 0.609)
Q.4 Draw the Lewis dot structure of azide ion (N3
–), such that all nitrogen atoms have complete octet.
Calculate formalcharge onallthe nitrogen atom.
Q.5 NO2 gas isparamagnetic at roomtemperature. Whena sample ofgas iscooled below 00C, its molecular
weight increases and it looses paramagnetism. When it is reheated the behaviour is reversed. Using
electron dot structures, write anequation which accountsfor these observation.
Q.6 Explain the hybridisation in solid formofPCl5 , PBr5 , N2O5 and XeF6.
Q.7 Which ofthe following species do you expect to be planar :
NH3, NH3
2+, CH3
+, 
3
NO , 
2
3
CO ? Give reasons.
Q.8 Whichofthe following species do you expect to be linear :
CO2, NO2, NO2
+, 
2
NO , SO2, H2O ? Give reasons.
Q.9 Discuss the hybridisation ofC – atoms in allene (C3H4) and CH2CCHCH2CHCCH2 and show the
–orbitaloverlap.
Q.10 Estimate the lengthand width ofthe carbonskeleton inNaphthacene
Given : SBCR ofcarbon is 0.7 Å.
Q.11 “Strike anywhere matchsticks” containa layer ofKClO3 and a layer ofP4S3. The heat produced bythe
friction of striking the match causes these two compounds to react and to inflames setting fire to the
wooden stemofthe matchstick. P4S3 is an unusualmolecule withthe skeleton structure.
(a) Name the geometryabout the P atoms, about the S atoms, and about the Clatomis there species.
(b) Assign a hybridizationto the P atoms to the S atoms, and to the Clatom, in there species.
(c) Determine the oxidation states ofthe atoms in P4S3 &inthe 
3
ClO ion.
HYBRIDISATION :
Q.12 Explain type ofhybridisation shape, bondangle and geometryofthe following compounds.
(1) XeF2 (2) XeF4 (3) XeF6 (4) XeOF4
(5) PCl3 (6) PCl5 (7) SF2 (8) SF6
(9) IF3 (10) IF5 (11) IF7 (12) OF2
(13) 
3
NO (14) 
5
2
3
O
P
H (15) 
4
ClO (16) SF4
(17) 
3
I (18) N2O5 (19) 
3
ClO (20) OCl2
(21) Cl2O7 (22) 
4
8
2O
P (23) H2SO5 (24) 
2
3
2O
S
(25) Na2[B4O5(OH)4]· 8H2O

INORGANICCHEMISTRY
Daily Practice Problems
CLASS : XIII DPP. NO.-17
Q.1 What is true for resonance?
(A) Canonicalforms differ onlyinelectronic arrangement.
(B) Canonicalforms differ inatomic as wellas inelectronic arrangement.
(C) Canonicalforms have same number ofunpaired electrons.
(D) Canonicalforms are hypotheticaland do not have actualexistence.
Q.2 Which ofthe following is not a preferred resonating structure ofazide ion N3
–?
(A) (B) (C) (D)
Q.3 Amolecule may be represented by three structures having energies E1, E2and E3, respectively. The
energies of these structures follow the order E3 < E2 < E1 , respectively. If actual energy content of
molecule is E0, the resonance energyis
(A) (E1 + E2 + E3) – E0 (B) E3 – E0
(C) E3 – E1 (D) E0 – E2
Q.4 Whichofthefollowing has maximumnumberofresonatingstructures?
(A) CO (B) CH2=CH–OH (C) C6H5–O– (D) CH3COO–
Q.5 Compare the extent ofdelocalisation oflone pair in (a) chlorobenzene (b) phenoland comment about
comparison inresonance energy.
Q.6 The carbon–chlorine bondis the shortest in
(A) CH3–Cl (B) C6H5–Cl (C) CH3–CH2–Cl (D) CH2=CH–CH2–Cl
Q.7 Which ofthefollowing solid(s) consists ofmolecules held together byvander Waal’s forces
(A) molecules carbonate (B) carbondioxide
(C) sugar (D) iodine
Q.8 Compare which would be more stable and why?
(a) CH2=CH–CH=CH–CH3 (b) CH2=CH–CH2–CH=CH2
Q.9 Identifythecorrect sequenceofincreasingnumberof-bondsinthestructuresofthefollowingmolecules:
(I) H2S2O6 (II) H2S2O3 (III)H2S2O5
(A) I, II, III (B) II, I, III (C) II, III, I (D) I, III, II
Q.10 In whichexample vacant orbitaltakepart inhybridisation
(A) B2H6 (B)AlCl3 (C) C2H5Cl (D) H3BO3
Q.11 Number of S–S bond in H2SxO6
(A) x (B) (x – 1) (C) x – 2 (D) x + 1
Q.12 Draw the structuresofthe following compounds
1. H2SeO4 2. HSO3Cl 3. HNC 4. N2F4 5. H2P2O6 6. B4Cl4
7. K4[Fe(CN)6] 8. Na6P6O18 9. H5P3O10 10. H6P4O13 11. P4S10 12. RbIO2
13. CsH2PO2 14. CuSiO3 15. NH4OCN 16. KHSO5 17. H2P2O5
2–
18. Na[B3O3(OH)4] 19. Na2[B3O5(OH)4]·8H2O 20. Hexachloro cyclotriphosphazene (N3P3Cl6)

INORGANICCHEMISTRY
Daily Practice Problems
CLASS : XIII DPP. NO.-18
Q.1 Explainwhy
(i) The dipole moment ofwater is higher thanthat ofNH3
.
(ii) SiCl4
is hydrolysed bywater, but not CCl4
.
(iii) BeCl2
shows a high degree ofcovalencyin its reactions, whereas BaCl2
is predominantlyionic.
(iv) The H–P–H angle in PH3
is smaller than that H–N–H angle in NH3
.
(v) The molecule ofmagnesiumchloride is linear, whereas that ofstannouschloride is angular.
(vi) The hydrogen bonding in HFis stronger thanin H2
O but the boiling point ofwater is 1000
C, while that
of HF is only 19.50
C.
(vii) Carbon–oxygen bond lengths in formic acid are 1.23 Å and 1.36 Å and both oxygen bonds in sodium
formate have the same value, i.e. 1.27 Å.
(viii) Valencyofoxygenis generallytwo whereassulphur shows valencyoftwo, four and six.
(ix) Three carbon oxygenbonds are having equallengthin carbonate ion.
(x) Amongst LiFand Lilwhich has more covalent character.
(xi) BaO has a lower melting point than CaO.
(xii) F2
is a gas while I2
is a solid.
(xiii) Phosphine hasa lower boiling point than ammonia.
(xiv) AlthoughClhassame electronegativityas nitrogenbut it does not formeffective H–bonding.
(xv) Ammoniumsaltsare more soluble inwater thanthe corresponding sodiumsalts.
(xvi) AlCl3
is covalent in nature whereasAlCl3
. 6H2
O is ionic.
(xvii) BaSO4
beinganelectrovalent compound and stillit does not pass into solutionstateinwater.
(xviii) In between MgO and BaO, which has high melting point.
(xix) Iodine is more soluble in CCl4
but less soluble in H2
O
(xx) Alkalimetalsimpart flame colour.
(xxi) Thio ethershave higher boiling point thanethers.
(xxii) Compared to p-nitrophenol, o–nitrophenolis more soluble in benzene andless in water.
(xxiii) The super oxides KO2
, RbO2
and CsO2
are paramagnetic.
(xxiv) Lead prefers to formdivalent compounds.
(xxv) BeF2
and BF3
are stable though Be and B have less than 8 electrons? Which one is more stable?
(xxvi) The repulsions betweennon-bonded orbitals are greater than that ofbetweenthe bonded orbitals?
(xxvii) SnCl2
is ionic but SnCl4
is covalent.
(xxviii) NF3
is weaker base than NH3
, NCl3
, NBr3
and NI3
.
(xxix) NO molecule is paramagnetic
(xxx) A bond order of3 is computed for the diatomic molecule. It is possible that in the absence of further
information, this triple bond bond maybe made up of one and two -bonds.
(xxxi) Wood pieces are used to hold ice-cream. Why?
(xxxii) Drywood burns but not wet wood. Why?
(xxxiii) The experimentalmolecular weight ofacetic acid in just double than theoreticalmolecular weight of
acetic acid. Why?
(xxxiv) (H3
Si)2
NH is planar while (H3
C)2
NH is pyramidal. Why?
(xxxv) AlCl3
hydratedor anhydrous which is soluble inether.
(xxxvi) CCl4
is not dissolved in H2
O but SiCl4
dissolves. Why?
(xxxvii) Pb+4
, Bi+5
and Tl+3
act as oxidising agent. Why?
(xxxviii)NCl3
& PCl3
onhydrolysis willgive different products. Why?
(xxxix) (CH3
)3
C–OH is less acidic than (CH3
)3
Si–OH.
(xxxx) Trimethylamine (CH3
)3
N, is pyramidalbut trisylamine (SiH3
)3
N is planer. Why?

Q.2 N2 and O2 are converted to monocations 
2
N and 
2
O respectively, whichis wrong statement
(A) In 
2
N , the N–N bond weakens (B) In 
2
O , the O–O bond order increases
(C) In 
2
O , the paramagnetismdecreases (D) 
2
N becomes diamagnetic
Q.3 Linear structure is assumed by
(I) NCO– (II) CS2 (III) 2
NO

(IV) Soild BeH2
(A) allfour (B) (II), (III) & (IV) (C) (I), (II) & (III) (D) (II) & (III)
Q.4 Correct order ofbond angle in CH2F2
(A)  H C H >  H C F >  F C F (B)  F C F >  H C F >  H C H
(C)  H C H >  F C F >  H C F (D)  H C F >  F C F >  H C H
Q.5 Assuming pure 2s and 2p orbitals ofcarbon are used in forming CH4 molecule, whichofthe following
statement is false?
(A) Three C–H bonds willbe at right angle
(B) One C–H bond willbe weaker than other three C–H bonds
(C) The shape ofmolecule willbe tetrahedral
(D) The angle ofC–H bond formed by s–s overlapping willbe uncertain with respect to other three
bonds.
Q.6 Whichofthefollowing order is correct ofthe givenproperty.
(A) NaCl > KCl > RbCl > CsCl > LiCl : melting point order
(B) BeF2 < MgF2 < CaF2 < SrF2 < BaF2 : solubilityorder
(C) NO2– > NO— > NO = NO2+ > NO+ : bond lengthorder
(D) BaO > SrO > CaO > BeO > MgO : basic character order
Q.7 Inthefollowingseries ofelectronicallysaturatedandisoelectronicionsthe observedX–Obonddistances
have beendetermined.
ION X–O bond length (Å)
SiO4
4– 1.63
PO4
3– 1.54
SO4
2– 1.49
ClO4
– 1.46
The order of p-d bond character is
(A) SiO4
4– < PO4
3– < SO4
2– < ClO4
– (B) SiO4
4– > PO4
3– > SO4
2– > ClO4
–
(C) SiO4
4– > SO4
2– > PO4
3– > ClO4
– (D) ClO4
– > PO4
3– > SO4
2– > SiO4
4–
Q.8(a) The O2
F2
molecule has the same shape as that ofH2
O2
but the O–O bond distance in O2
F2
is only122
ppmas compared with that in H2
O2
(148 pm). What explanation can you provide for this difference ?
(b) For ozone  OOO = 1170
. For sulphur dioxide,  OSO = 1200
. Explain.

INORGANICCHEMISTRY
Daily Practice Problems
Q1. The correct order ofbond energies for the C–H bond is
(A) H3C–H < H3C–CH2–H < (CH3)2CH–H < (CH3)3C–H
(B) (CH3)3C–H < (CH3)2CH–H < CH3–CH2–H < H3C–H
(C) H3C–H < (CH3)3C–H < CH3–CH2–H < (CH3)2CH–H
(D) (CH3)3C–H < (CH3)3CH–H < H3C–H < CH3–CH2–H
Q2. Indicate thecorrect statement
(A) Manysalts of[PCl4
+] are obtained when PCl5 reacts with Chloride ion acceptors such as TiCl4.
(B)Allthe trihalides ofthenitrogen group elements undergo easyhydrolysis bywaterto yield acidic
compounds.
(C)Allthe elements ofthe nitrogen groupformpenta halides.
(D) Inalloxo-acids ofsulphurcontaining two sulphur atoms per molecule there is an S–O–S likage.
Q3. At 373 K, a gaseous reactionA 2B+ C isfound to be offirst order. Starting withpureA, the total
pressure at the end of10 minutes was 176 mmand after a longtime whenAwascompletelydissociated,
it was 270 mm. The pressure ofAat the end ofthe 10 minutes was
(A) 94 mm (B) 47 mm (C) 43 mm (D) 90 min
Q4. Draw Lewis structuresfor the following speciesand arrange theminorderofincreasing carbon-oxygen
bond lengthand then byincreasing carbon-oxygenbond strength.
(A) CO (B) CO3
2– (C) H2CO (D) CH4O (E) HCO3
–
Q5. An atmospheric chemist, studying the reactions ofthe pollutant SO2, places a mixture ofSO2 and O2 in
a 2 litre container at 900 K and an initialpressure of1.95 atm. When the reaction occurs, gaseousSO3
forms and the pressure eventuallyfalls to 1.65 atm. How manymoles ofSO3 form?
Q6. Carbon has maximumcovalencyoffour. Explainthe covalencyofcarboningivencompound
Q7. Describle and compare the geometries ofthe molecules and the hybridization ofthe carbonand boron
atoms in F2C = C=C=CF2 and F2B –CC–BF2. Compare the relative orientation ofthe sets offluorine
atoms in the two cases. In whichcase is it possible for allfour fluorine atoms to lie inthe sameplane.
Q8. Manganese isa keycomponent ofextremelyhard steel. Theelement occurs naturallyinmanyoxides.A
542.3 gm sample of a manganese oxide has an Mn : O ratio of 1:00 : 1.42 and consists of braunite
(Mn2O3) andmanganosite (MnO).
(a) What masses ofbraunite and manganosite are in the givenmass ofore?
(b) What is the ratio Mn3+ : Mn2+ inthe ore?
CLASS : XIII DPP. NO.-19

Q9. In addition ofAl2
Cl6
, aluminiumforms other specieswithbridging halide ions to two aluminiumatoms.
One such species is the ionAl2
Cl2
–
. The ionis symmetrical, with a linearAl–Cl–Albond.
(a) What hybrid orbitaldoesAluse to bond with the Clatoms?
(b) What is the shape around eachAl?
(c) What is the hybridization ofthe centralCl?
Q10. The bond angle for H2
Omolecule (104.45o
) is closer to the tetrahedralangle whereas for H2
S, the bond
angle (92.2o
) is closer to the angle between two pure ‘P’orbitals. Explain with the assumptionthat the
‘S’charge ofthehybridisationis givenby
1
cosθ
cosθ

, where θ isthe bond angle. Extendthis conclusion
to the hydrides ofthe elements ofthe nitrogen family. How willyou use this to explain the decreasing
basicityofthese hydrides down the corp.?
Q11. There are two structuralisomers ofC2H4I2
(a) In the isomer in which bothiodine atoms are attached to the one carbon atom, find iodine -iodine
distance.
(b) In theother isomer find theminimumand maximumdistancesbetweenthe two iodine atoms as one
CH2I group rotates about the C–C bond as an axis.
Q12. Using0.102nmfortheradiusofaneutralsulphuratom.What maximumdiameter
sphere could you pass throughthe centre ofthe S8
moleculeshowninthe figure.
The S–S bond length is 0.207 nm, and the S–S–S bond angle is 1050
.

INORGANICCHEMISTRY
Daily Practice Problems
(Choose the correct option, their may be one or more than one correct options)
Question No. Q.1 to Q.5 (5 questions)
Polar covalent molecules exhibit dipole moment. Dipole moment is equal to the product of charge
separation, q and the bond lengthd for the bond. Unit ofdipole moment is Debye. One Debye is equal
to 10–18 esu cm.
Dipole moment is a vector quantity. It has both magnitude and direction. Hence, dipole moment ofa
molecule depends upon the relative orientationof the bond dipoles, but not on the polarity of bonds
alone. Asymmetricalstructure shows zero dipole moment. Thus, dipole moment helps to predict the
geometryofamolecules.Dipolemoment valuescanbeusedto distinguishbetweencis-andtrans-isomers;
ortho-, meta- and para-forms of a substance, etc.
Q.1 Whichis a polar molecule?
(A) XeF4 (B) BF3 (C) I2Cl6 (D) PCl2F3
Q.2 Adiatomic moleculehas a dipole moment of1.2 D. Ifthe bond lengthis 1.0 × 10–8 cm, what fractionof
charge does exist on each atom?
(A) 0.1 (B) 0.2 (C) 0.25 (D) 0.3
Q.3 Arrange the following compounds in increasing order of dipole moments, toluene (I),
o-dichlorobenzene (II), m-dichlorobenzene (III) and p-dichlorobenzene (IV)
(A) IV < I < II < III (B) I < IV < II < III (C) IV < I < III < II (D) IV < II < I < III
Q.4  oftheAX4 type ofmolecule is zero. The geometryofit can be
(A)Tetrahedral (B) Sq. planar (C)Aor B (D) None
Q.5 Whichofthe following statement is correct regarding C2H2F2 molecule.
(A) One isomer is polar, one is non polar (B) Two isomers are polar, one is non polar
(C) Two isomers are planar, one is non planar (D) Two isomers are onlypossible and planar
Q.6 The geometrywithrespect to thecentralatomofthefollowing molecules are:
N(SiH3)3 ; Me3N ; (SiH3)3P
(A) planar, pyramidal, planar (B) planar, pyramidal, pyramidal
(C) pyramidal, pyramidal, pyramidal (D) pyramidal, planar, pyramidal
Q.7 Whichofthefollowing order is correct?
(A) Thermalstability : LiOH > NaOH > KOH > RbOH
(B) Dipole moment : BF3 < H2O < H2S
(C) Polarityofthe bonds : SbH3 < AsH3 < PH3 < NH3
(D)Meltingpoint : CaF2 > CaCl2 > CaBr2 > CaI2
Q.8 Whichofthefollowing set ofspecieshave planar structures
(A) 
3
I , · 3
CH , 
3
ClO , 
2
6
SiF (B) 
3
I , 
4
ICl ,Al
Al2Cl6, TeCl4
(C) SCl2, N2O5, SF4, XeOF4 (D) I2Cl6, XeF2, 
4
BrF , 
5
XeF
Q.9 Matchthe column-Iwithcolumn-II. Notethat column-Imayhave more thanonematching options in
column-II.
Column-I Column-II
(P) Hypo phosphoricAcid (A)Allhydrogenare ionizable inwater
(Q) Pyro phosphorousAcid (B) LewisAcid in water
(R) BoricAcid (C) Monobasic in water
(S) Hypo phosphorousAcid (D) sp3 hybridised centralatom
CLASS : XIII DPP. NO.-20

Q.10 Which is the correct order between below three bond angles
(A) 1 < 2 < 3 (B) 1 < 3 < 2 (C) 3 < 1 < 2 (D) 1 = 2 = 3
Q.11 Select thecorrect statement
(A) 
5
HSO ion has one S–O–H linkage
(B) Number ofB–O–B linkages in Borax is equalto number ofP–O–P linkages in P4O10
(C) Hybridisation ofboth sulphur in H2S2O5 (pyrosulphurousAcid)is same but oxidationstate ofboth
sulphur are different
(D) Tetra PolyphosphoricAcid has four P–O–Pand no P–Plinkage
Q.12 Select the incorrect statement about N2F4 and N2H4.
(I) In N2F4 , d-orbitalsare contracted byelectronegative flourine atoms, but d-orbitalcontractionis not
possible byH-atom in N2H4.
(II) The N–N bond energy in N2F4 is more than N–N bond energyin N2H4.
(III) The N–N bond length in N2F4 is more than that ofin N2H4.
(IV) The N–N bond length in N2F4 is less than that ofin N2H4.
Choose the correct code
(A) I, II & III (B) I & III (C) II & IV (D) II & III
Q.13 ICN undergoes selfdissociation initsmelt as follows:
3ICN [I2CN]+ + [I(CN)2]–
Which ofthefollowing geometrywould be suggested for the anionic part ofliq. ICN
[Skeletononlyshowninthe diagram]
(A) Zigzag ; (B) Zigzag ;
(C) Linear ; [N–C–I–C–N] (D) Linear ; [N–C–C–N–I]
Q.14 Whichofthe following statements is/are not correct for following compounds.
(I) SCl2 (OCH3)2 and (II) SF2 (OCH3)2
(A) –OCH3 groups in both cases occupythe same position.
(B) Cl-atoms occupyequitorialposition incase of(I) andF-atoms occupyequitorialpositionin case of
(II).
(C) Cl-atoms occupyaxialposition in case of(I) and F-atoms occupyequitorialposition incase of(II)
(D) Cland F-atomoccupyeither axialor equitorial positionin case of(I) and (II) respectively.
Q.15 Arrange the following inorder ofdecreasing O
N  bond length: 


3
2
2 ,
, NO
NO
NO
(A) 



 2
2
3 NO
NO
NO (B) 



 2
2
3 NO
NO
NO
(C) 



 2
3
2 NO
NO
NO (D) 



 2
3
2 NO
NO
NO

INORGANICCHEMISTRY
Daily Practice Problems
(Choose the correct option, only one is correct)
Question No. 1 to 4 (4 questions)
Inprinciple, Schrondinger equationcan bewrittenfor anymolecule. However, since it cannot be solved
exactlyfor anysystemcontaining more than one electron, molecular orbitals which are one electron
wavefunctionsformoleculesaredifficultto obtaindirectlyfromthesolutionoftheSchrondingerequation.
This difficultyisovercome byresorting to anapproximationmethod called linearcombinationofatomic
orbitals (LCAO) method to formmolecular orbitals.
The molecular orbitalformed bythe addition ofatomic orbitals is called the bonding molecular orbital
and the molecular orbitalformed bythe subtraction ofatomic orbitals is called antibonding molecular
orbital. Qualitatively, theformationofmolecular orbitals canbe understood interms ofthe constructive
or destructive interference ofthe electronwaves ofthe combiningatoms. In the formationofbonding
molecular orbital, the two electron waves of the bonding atoms reinforce each other (constructive
interference) while inthe formationofantibondingmolecular orbital, these electronwaves canceleach
other (destructive interference). The result is that in a bonding molecular orbitalmost ofthe electron
densityis located betweenthe nucleiofthe bonded atoms and hence the repulsionbetweenthe nucleiis
verylow whileinanantibonding molecularorbital, most oftheelectrondensityis locatedawayfromthe
space between the nuclei, as a matter of fact there is a nodal plane (i.e., plane in which the electron
densityis zero)
Q.1 How manynodalplaneis/are present in sp
 bondingmolecular orbital?
(A) zero (B) 1 (C) 2 (D) 3
Q.2 Whichofthe following combinationoforbitals is correct?
(A) + 
(B) + 
(C) + 
(D) — 
Q.3 Whichofthe following statements isnot correct regarding bonding molecular orbitals?
(A) Bondingmolecular orbitals possess lessenergythanthe atomicorbitals fromwhichtheyare formed
(B) Bondingmolecular orbitals have low electrondensitybetween thetwo nuclei
(C) Everyelectron inbonding molecularorbitals contributes to the attraction betweenatoms
(D) Theyare formed when thelobes ofthe combiningatomic orbitals have the same sign
Q.4 IfX-axis is the molecular axis, then-molecular orbitals are formed bythe overlap of
(A) s + pz (B) px + py (C) pz + pz (D) px + px
Q.5 Find out the bond order of:
(a) 2
H (b) 
2
H (c) 2
He (d) 2
Li (e) 2
Be (f) 2
B
Q.6 Inanantibonding MO, electrondensityis minimum
(A) around one atomofthe molecule (B) betweenthe two nucleiofthe molecule
(C) at the region awayfromthe nucleiofthe molecule (D) at no place.
CLASS : XIII DPP. NO.-21

Q.7 Which have odd bond order
(A) O2
+
(B) O2
–
(C) NO (D)all
Q.8 Whichofthefollowing has maximumbond strength
(A) O2
(B) O2
+
(C) O2
–
(D) O2
2–
Q.9 Number ofnon bonding electrons in 2
N is :
(A) 4 (B) 10 (C) 12 (D) 14
Q.10 Pick out the incorrect statement?
(A) N2 has greater dissociation energy than N2
+ (B) O2 has lower dissociation energy than O2
+
(C) Bond length in N2
+ is less than N2 (D) Bond length in NO+ is less than in NO.
Q.11 Bond order of 2
Be is :
(A) 1 (B) 2 (C) 3 (D) 0
Q.12 The bond order depends on the number ofelectrons inthebonding and nonbondingorbitals. Which of
the followingstatements is /are correct about bond order?
(A) Bondorder cannot have a negative value.
(B) It always has anintegralvalue.
(C) It is a nonzero quantity.
(D) It canassume anyvalue-positiveor negative, integralorfractional, including zero.
Q.13 In the formation of 
2
N from 2
N , the electronis removed from:
(A) orbital (B)  orbital (C) *
 orbital (D) *
 orbital
Q.14 Duringtheformationofa molecularorbitalfromatomic orbitalsofthe same atom,probabilityofelectron
densityis:
(A) minimuminthe nodalplane (B) maximuminthe nodalplane
(C) zero inthe nodalplane (D) zero on the surface ofthe lobe
Q.15 Whichofthe following has fractionalbond order :
(A) 
2
2
O (B) 
2
2
O (C) 
2
2
F (D) 
2
H
Q.16 How manyunpaired electrons are present in 
2
N :
(A) 1 (B) 2 (C) 3 (D) 4
Q.17 Which have odd-order bond?
(A) O2
+ (B) O2
 (C) NO (D) H2
+
Q.18 Whichofthe following have identicalbond order?
(A) 
2
2
O (B) 
NO (C) 
CN (D) 
CN
Q.19 Whichofthefollowing statement is/are correct
(A) Theperoxideionhasabondorder of1whilethe oxygenmoleculehas abondorderof2
(B) The peroxide ion has a weaker bond than the dioxygenmolecule has.
(C) The peroxide ion as wellas the dioxygenmolecules are paramagnetic
(D) The bond length ofthe peroxide ion is greater than that ofthe dioxygenmolecule
Q.20 Whichofthe following have unpaired electron(s)
(A) 
2
O (B) 
2
O (C) NO (D) 
2
H
Q.21 Whichofthe following are diamagnetic ?
(A) 2
C (B) 
2
2
O (C) 2
Li (D) 
2
N
Q.22 Whichofthefollowing are paramagnetic ?
(A) 2
B (B) 2
O (C) 2
N (D) 2
He
Q.23 Given the species : N2, CO, CN– and NO+. Which ofthe following statements are true for these
(A)Allspecies are paramagnetic (B) The species are isoelectronic
(C)Allthe species have dipole moment (D)Allthe species are linear

Q.24 Which ofthe following species is paramagnetic ?
(A) 
NO (B) 
2
2
O (C) 
CN (D) CO
Q.25 Asimplified applicationofMO theoryto the hypothetical‘molecule’OFwould giveits bond orderas :
(A) 2 (B) 1.5 (C) 1.0 (D) 0.5
Q.26 Which ofthe following species have a bond order of3 ?
(A) CO (B) 
CN (C) 
NO (D) 
2
O
Q.27 Among the following, the species with one unpaired electronare :
(A) 
2
O (B) NO (C) 
2
O (D) 2
B
Q.28 Which ofthe following pairs have identicalvalues ofbond order ?
(A) 
2
N and 
2
O (B) 2
F and 2
Ne (C) 2
O and 2
B (D) 2
C and 2
N
Q.29 Whichofthefollowing is correct ?
(A) During 
2
N formation, one electron each isremoved fromthe bonding molecular orbitals
(B) During 
2
O formation, one electroneachisremoved fromthe antibondingmolecular orbitals
(C) During 
2
O formation, one electron eachisadded to the bonding molecular orbitals
(D) During 
CN formation, one electron each is added to the bondingmolecular orbitals
Q.30 A complex compound like K2[Pt Cl6] is found to exist & also similar species like O2 [Pt F6]. Which
statement is trueofthe following.
(A) O – O bond length in O2[Pt F6] is less than that in KO2.
(B) O – O bond length in O2[Pt F6] is more than that in KO2.
(C) O – O bond length in O2[Pt F6] is more than that in O2.
(D) O – O bond length in O2[Pt F6] is more than that in O3.
Q.31 Based upon M.O. theorystate reason for the paramagneticcharacter ofCN, the diamagnetic character
of 
CN , the stabilityof 
CN and calculate their respective bond orders.
Q.32 Identifythe moleculesor atoms or ionsfromthe following molecular orbitalenergylevelformulations.
The species should be selected from (B2, C2, O2
2+, O2, F2, N2)
(a) 1
1
2
*
2
)
2
(
)
2
(
)
2
(
)
2
( y
x p
p
s
s
KK 



(b) 2
2
2
*
2
)
2
(
)
2
(
)
2
(
)
2
( y
x p
p
s
s
KK 



(c) 2
2
2
2
*
2
)
2
(
)
2
(
)
2
(
)
2
(
)
2
( y
x
z p
p
p
s
s
KK 




(d) 1
*
1
2
2
2
*
2
)
2
(
)
2
(
)
2
(
)
2
(
)
2
(
)
2
(
)
2
( y
x
y
x
z p
p
p
p
p
s
s
KK 






(e) 2
*
2
2
2
2
2
*
2
)
2
(
)
2
(
)
2
(
)
2
(
)
2
(
)
2
(
)
2
( y
x
y
x
z p
p
p
p
p
s
s
KK 






(f) 2
z
2
x
2
y
2
*
2
)
p
2
σ(
)
p
2
(
)
p
2
π(
s)
2
(
σ
s)
2
(
σ
KK 