"1. What are the factors influencing ionic bond formation?2. Out of MgO and NaCl, whech has higher lattice energy and why?3. BaSO being an electrovalent compound and still it does not pass into solution4 state in water.4. Why an ionic bond is formed between two elements having large difference intheir electronegativity?COVALENT BOND :6. Which compound has 3 carbon atoms, 4 double bonds and the total no. of atomsare five?7. Which compound has 3 carbon atoms. 4 ??and 4 ? bonds but not 4 double bondsand the total no. of atoms are 5. Writes its IUPAC 8. Element A has 3 electrons in the valency shell and its principal quantum no. forthe last electron is 3 and element B has 4 electrons in the valency shell and itsprincipal quantum to. For the last electrons is 2. Identify the compound and it‘snature of bonding.9. The compound X has 8 atoms, 4 ? bonds, no ? bonds, no. ionic bonds, nocoordinate bonds, no H-bond. Explain its structure.10. The compound X has 8 atoms, 0 ? bonds, no ionic or ? bonds. Explain itsstructure.11. SnCl has melting point –15ºC where as SnCl has melting point 535ºC. Why?4 2 12. Inorganic benzene is more reactive than organic benzene. Why?FAJAN’S RULE :13. SnCl is white but SnI is red. Why?2 2 14. Explain the least melting point and highest solubility in H O.2(i) LiCl NaCl KCl (ii) NaCl NaBr Nal (iii) LiCl BeCl BCl 2 3(iv) beSO MgSO CaSO SrSO4 4 4 4BaSO4(v) CaF CaCl CaBr2 2 2 15. Which one has highest and lowest melting point and why? NaCl KCl RbCl CsCl16. LiOH and carbonates decomposes on heating in I-group. Other hydroxides andcarbonates of this group will not. Why?LEWIS STRUCTURE AND FORMAL CHARGE :17. Draw the Lewis structures of the following molecules and ions.2 5-PH , H S, BeF , SiCl , N O , H SO , O , IO .3 2 2 4 2 4 2 4 2 6 V.B.T. & HYBRIDISATION :20. Explain hydrbidisation in (1) XeF (2) XeF (3) PCl (4) IF2 6 3 3(5) IF (6) IF (7) CCl (8)5 7 4 SiCl4(9) SlH (10) H O4 2 22. PH is not possible but PCI is possible. Why?5 536 VSEPR THEORY :24. Which one has highest and least bond angle in the following - (1) NH PH AsH SbH3 3 3 3(2) CH PH AsH SbH4 3 3 3(3) H O H S H Se H Te2 2 2 2(4) CH PH AsH H Te4 3 3 2(5) CH SiH CCl SiCl4 4 4 4(6) NCl PCl NBr PBr3 3 3 3(7) PF PH3 3(8) As F AsH3 3 3 MOT :29. Super oxide are coloured and paramagnetic why?30. Write the important conditions required for the linear combination of atomicorbitals to form molecular orbitals.+ 33. Exalain why NO is more stable towards dissociation into its atoms than NO,+ where as CO is less stable than CO.BACK BONDING AND HYDROLYSIS :40. Arrange the following boron trihalides in the increasing order of their ease ofhydrolysis. Also give the reason for the same. BF , BCl , BBr3 3 3 DIPOLE MOMENT :53. Why NH is having more dipole moment than NF .3 3 54. Whyis having more dipole moment than /55. Why p-dichloro benzene in having zero dipole moment while hydroquinone ishaving some dipole moment?56. Why CH Cl is having high dipole moment than CH F?3 3 57. Why ortho fluoro Phenol have greater dipole moment than ortho chloro phenol?58. Why trans–1, 2 sichloro ethene in having zero dipole moment than cis form?59. Write the order of dipole moments of 1, 2–1.3– and 1, 4–dichlorobenzene.60. Arrange in increasing order of dipole moment ; H O, H S, BF .2 2 3 61. BcF has zero dipole moment whereas H O has a dipole moment?2 2 62. CCl having zero dipole momnet but CHCl having some dipole moment?4 3 63. While down the resonance structure (S) for :–(i) N (ii) O (iii) CO3 3 2 2– (iv) N2O (v) SCO 4 2 1. Arrange the following in increasing order of property given- (i) O, F, S, Cl, N strength of H-bonding (X-H_X) (ii) N , O , F , Cl bond dissociation energy2 2 2 2(iii) MCl, MCl , MCl ionic nature2 3(iv) HI, HBr, HCl, HF dipole moment (v) AsH , PH , NH bond angle 3 3 337 5. Explain the structure hybridisation and oxidation state of S i sulphuric acid,marshall‘s acid, caro‘s acid, oleum.6. Boric acid is monobasic acid. Why?7. Boron has exceptionally high melting point. Why?8. BCl is more acidic than BF . Why?3 3 9. CCl is not dissolved in H O but SiCl dissolves. Why?4 2 4 10. Trimethylamine (CH ) N, is pyramidal but trisylyamine (SiH ) N is planer. Why?3 3 3 3 11. SnCl has melting point –15ºC Where as SnCl has melting point 535ºC.Why?4 2 12. PbCl is possible but PbBr and Pbl are not. Why?4 4 4 +4 +5 +3 13. Pb , Bi and Tl act as oxidising agent. Why?14. NCl & PCl on hydrolysis will give different products. Why?3 3 15. ClO does not forms dimer but NO forms. Why?2 2 16. How many ? and ? bonds are presents in hexacyanoethane and tetracyanoethylene?17. Explain the structure of ClF on the basis of bent rule.3 18. All bonds length of PCl are not equal but PF has same bond lengths. Why?5 5 19. The experimentally determined N – F bond length in NF is greater than sum of3 single bond covalent radii of N and F.24. The dipole moment of HBr is 7.95 debye and the intermolecular separation is-10 1.94 × 10 m Find the % ionic character in HBr molecule.-30 25. HBr has dipole moment 2.6 × 10 cm. If the ioninc character of the bond is11.5%, calculate the interatomic spacing.26. Dipole moment of LiF was experimentally determined and was found to be 6.32D. Calculate percentage ionic character in LiF molecule Li – F bond length is0.156 pm.27. A diatomic molecule has a dipole moment of 1.2 D. If bond length is 1.0 A, whatpercentage of an electronic charge exists on each atom.SECTION (B) FILL IN THE BLANKS :1. Two atoms of similar electronegativity are expected to form __________compound.2. When two atoms approach each other, potential energy ______ and a___________ is formed between them.3. Conversion of a neutral atom into a cation is _________ process.4. The strongest hydrogen bond is formed between _________ and hydrogen.5. Low ionization potential of electropositive element and high electron affinity ofelectronegative element favours the formation of __________ bond.6. NaCl is soluble in water due to its low ___________ energy.7. The ________ value of lattice energy of a crystal favours the formation of anionic compound.8. Solid NaCl ___________ conductor of electricity.9. For dissolution of an ionic solid, ________ energy should be low and hydrationenergy should be _________________.10. ___________ cation and ___________ anion favour covalency.11. Anhydrous AlCl is a _____________ compound while hydrated AlCl is3 3 ___________.12. Covalent compounds are generally _________ conductors of electricity.13. There are ___________? bonds in a nitroge molecule.14. A double bond is shorter than ___________ bond. 38 15. Axial overlapping of half-filled atomic orbitals results in __________ bond.16. ____________ and ___________ bonds are present in N O molecule.2 5 17. The angle between two covalent bonds is maximum in _________ (CH , H O,4 2 CO ).2 18. ___________ hybrid orbital of nitroger atom are involved in the formation ofammonium ion.19. The hybridization state of oxygen in water molecule is ___________.++ 2 20. In the ion [Cu (H O) ] , copper is in dsp state of hybridization. The shape of the2 4 ion is ________.TRUE OR FALSE :5. A diatomic molecule has a dipole moment of 1.2 D. If bond length is 1.0 a, whatpercentage of an electronic charge exists on each atom.6. The size of negative ion decreases with increasing magnitude of negativecharge.2+ + 7. Ca is smaller in size than K because the effective nuclear charge is greater.8. The higher the latteice energy of an ionic solid, the greater will be its stability.9. Molten sodium chloride conducts electricity due to the presence of free ions.10. Linear overlap of two atomic p-rbitals leads to a ?-bond.11. The H-N bond angle in NH is greater than the H-AS-H bond angle in AsH .3 3 2 12. sp hybrid orbitals have equal s and p-character.3 13. The tetrahedral geometry in SiF is due to sp hybridization of Si atom.4 14. SnCl is a non-linear molecule.2 15. There are seven electron bond pairs in lF molecules.7 16. Dipole moment of CHF is greater than CHCl .3 3 17. Dipole moment of NF is lesser than NH .3 3 18. Among HF, HCl, HBr and HI, HF has highest dipole moment.19. All molecules with polar bonds have dipole moment.20. The presence of polar bonds in a polyatomic molecule suggests that themolecule has non zero dipole moment.21. AgCl is more covalent than NaC.REASONING AND ASSERTION :Direction: These quaestions consist of two statements each printed as Assertion andReason.While answering these questions you are required to choose any one ofthe following four responses to encircle (A, B, C, D) as per instructions givenbelow: (A) If both Assertion and Reason are true and Reason is a correct explanation ofAssertion. (B) If both Assertion and Reason are true and Reason is not a correctexplanation of Assertion. (C) If Assertion is true but Reason is false. (D) If Assertion is false but Reason is true.3. Assertion : Na SO is soluble in water while BaSO is insoluble.2 4 4Reason :Lattice energy of BaSO exceeds its hydration energy.4(a) A (b) b (c) C (d) D4. Assertion : p and p cannot combine to give molecular orbital.y zReason :Both p and p are dumb-bell shaped.y z39(a) A (b) b (c) C (d) D7. Assertion : Although PF , PCl and PBr are known, the pentahalides of nitrogen5 5 5 have not been observed. Reason :Phosphorus has lower electronegativity than nitrogen. (a) A (b) b (c) C (d) D– 9. Assertion : NO is planar while NH is pyramidal.3 3 – 2 3Reason :N in NO is sp and in NH it is sp hybridized.3 3(a) A (b) b (c) C (d) D11. Assertion : s-orbital cannot accommodate more than two electrons. Reason :s-orbitals are extremely poor shielders. (a) A (b) b (c) C (d) DMATCH THE FOLLOWING :1. Column - IColumn - II (A) Size of secondary layer of hydrated ions (P)Maximum in solid andminimum in gaseous state. (B) Magnitude of hydrogen bonding (Q) Strength of ion - dipoleattraction (C) Mobility of ions in water (R) Inversely proportional to thesize of metal ion (D) Degree of polarity of a bond (S) Dipole moment (T) Directly proprotional to thesize of metal ion2. Column - IColumn - II (A) SO3 (gas)(P)Polar with p ? - d ? bonds andidentical S – O bond, lengths. (B) OSF(Q) One lone pair and p ? – d ?4 bond.–(C) SO F(R) non - polar with p ? –p ? and3 p ? – d ? bonds. Identical S–Obod lengths. (D) ClOF(S) Polar with p ? – d ? bond.3(T) Hybridisation of central atomin ClO F .2 3 3. Column - IColumn - II Molecule/ionHybridisation of central atom– 3(A) IO F(P) sp d2 2 3(B) F SeO(Q)sp2 2(C) ClOF(R)sp3 + 2(D) XeF(S) sp5 ONLY ONE ANSWER CORRECT:1. In which molecule (s) is/are the vander waals force likely to be most important indetermining m.p. and b.p.2(a) ICI (b) Br(c) H S (d) CO2 2. Which is the most ionic 40 "