class - xii chemistry solid state 1. equal no. of cation & anion
TRANSCRIPT
CLASS - XII CHEMISTRY
Solid State
1. Equal no. of cation & anion missing in the diagram is given. 2. What are these types of vacancy defects called? 3. How is the density of crystal affected by these defects? 4. Name one ionic compound which can show this type of defect in crystalline
state. 5. How is the stoichiometry of compound affected?
a. Analysis shows that M.O. has E.F.M 0.96 O 1.00 Calculate % M 2+ & M 3+
ions in the crystal 6. In an ionic compound N- form cubic close type packing while the cation M+
a. ions occupy one third of the tetrahedral voids. Deduce the formula of b. compound & the C.N. of M+ ions.
7. A compound contains 2 types of atoms X & Y . It crystallizes in a cubic
lattice with atom X at the corner & Y at body centres. What is the simplest possible formula of compound.
8. An element X with an at.mass 60 g/mol has density 6.23 g/cm3 If the edge
length of cubic unit cell is 400pm.Identify the type of cubic unit cell. Calculate the radius of an atom of this element.
9. What is the C.N. of each type of ions in a rock salt type crystal
structure? 10. what is a semiconductor? Describe the two main types of semiconductors & explain mechanism for their conduction. 11. What is the total no. of atoms per unit cell in a FCC structure? 12. What type of substance exhibits antiferromagnetism? 13. Reasons: (i) Frenkel defects are not found in alkali metal halides.
i. (ii)Schottky defects lower the density of related solids. ii. (iii) Impurity doped Si is a semiconductor.
14. Explain (i) Ferromagnetism (ii)Paramagnetism (iii) Ferrimagnetism.
15. What are F- centres? 16. Reason: (i) Fe3O4 is ferromagnetic at room temperature but becomes
1. paramagnetic at 850K. ii. (ii) ZnO on heating becomes yellow.
iii. (iii) Frenkel defect does not change the density of AgCl crystals
17. With the help of suitable diagram, on the basis of Band theory,explain the difference between (a)A conductor & an insulator (b) A conductor & semiconductor. 18. Why is glass considered a supercooled liquid 19. What is the two dimensional coordination no. of a sphere in square close packing?
Solid State - Numericals
20. Iron(II) oxide crystallize as Fe 0.93O. Find the %Fe2+ and Fe3+ in this
compound 21. A Solid AB has NaCl structure. If the radius of cation A+ is 100 pm, what
is the possible maximum and minimum radius of anion B- 22. If the radius of Mg2+, Cs+, O2-,S2- and Cl- ion are 0.65 A0, 1.69 A0, 1.40 A0,
1.84 A0 and 1.81 A0 respectively. Find the coordination number of MgO,MgS and CsCl.
23. In corundum, oxide ion are in hcp and aluminium ion occupy 2/3 of the octahedral void. What is the formula of aluminium oxide?
24. A cubic solid is made up of two elements P and Q. Q occupies corners of the cube and P occupies the body centre. What is the formula of the compound?
25. In a crystalline solid anion C occupies ccp, cation A occupies 50% tetrahedral void and cation B occupies 50% octahedral void. What is the formula of the compound?
26. If NaCl is doped with 10-3 mole % SrCl2 . What is the concentration of cation vacancies?
27. Sodium metal crystallizes in bcc with a cell edge of 4.3 A0. What is the radius of sodium atom?
28. Copper crystallizes in fcc with a density 9g/cm3.Calculate the radius of copper atom (Atomic mass of Cu=63)
29. . Cr crystallizes in bcc with atomic diameter 250pm. Determine the density of unit cell. (Atomic mass of Cr=52)
30. Calculate the value of Avagadro number. Given Density of unit cell of NaCl=2.165 g/cm3 Distance between Na+ and Cl- is 281pm. Atomic mass of NaCl= 58.5.
31. CsBr has bcc structure.a= 400pm Calculate the distance between Cs+ and Br-
32. . KF has NaCl structure. Find the distance between K+ and F-. Density of unit cell= 2.5 g/ cm3 ( Molar mass of KF = 58 )
33. An element crystallizes in bcc. a = 288 pm. How many atoms are there in 208 grams of this elements?
34. . An element crystallizes in fcc with a = 200 pm. Calulate its density if 200grams of this element contains 24x 1023 atoms.
35. Unit cell of an element has atomic mass 108. d= 10.5 g/cm3 a= 409 pm. Find the structure of the crystal lattice.
36. A compound has hexagonal close packing structure. Determine the total number of voids, number of tetrahedral void, and number of octahedral voids in 0.5 mole of this compounds.
37. Al crystallizes in a cubic close packing structure. Its metallic radius is 125 pm .Find the edge length of the unit cell. How many unit cells are there in 1cm3 of Al ? How many atoms are there in 1cm3 of Al ?
38. Silver chrysalises in FCC with an edge length 409 pm and density 10.5g/cm3. Calculate the Atomic mass of silver.
Solutions
39. What is van’t Hoff factor for a compound which undergoes tetramerization in an organic compound ?
40. Ethylene glycol (M.M. = 62 g/mol) is an antifreeze. Calculate F.P. of solution
containing 12.4 g of substance in 100 g of water. Would it be advisable to keep the substance in the car radiator during summer (kf for water = 1.86 KKg/mol , Kb for water= 0.512 KKg/mol) 41. Reason: (a) At higher altitude people suffer from a disease called anoxia.
In this disease they become weak & can’t think clearly. (b) When HgI2 is added to KI , the F.P. is raised? 42. (i) Benzoic acid completely dimerises in benzene. What will be the V.P. of a
solution containing 61 g of benzoic acid per 500 g benzene when the V.P. of pure benzene at the temp. of experiment is 66.6 Torr.
What would have been the V.P. in the absence of dimerization. 43. Derive a relationship between mole fraction & V.P. of a component of an
ideal solution in the liquid phase & vapour phase. Which aqueous solution has higher concentration 1M or 1 molal solution of
the same mole? Give reason. 44. 0.5 g KCl was dissolved in 100 g water & the solution originally at 20 0C,
froze at -0.24 0C Calculate % ionization of salt (Kf= 1.86 KKg /mol) 45. State Henry’s law correlating the pressure of a gas & its solubility in a
solvent & mention two applications for the law. 46. What is meant by negative deviation from Raoult’s law? Draw diagram to illustrate the relationship between V.P. & mole fraction of components in a solution to represent negative deviation. 47. The b.p. elevation of 0.3g of acetic acid in 100g benzene is 0.0633K.
a. Calculate the molar mass of acetic acid from this data.What conclusion can
b. you draw about the molecular state of the solute in solution? c. (Kb for benzene = 2.53KKg/mol)
48. Distinguish between the terms molality & molarity.Under what conditions are the molarity & molality of a solution nearly the same? 49. The F.P. of a solution containing 0.2 g of acetic acid in 20 g of benzene is
a. lowered by 0.450 Calculate (i) the mol.mass of acetic acid from this data.(ii) van’t Hoff factor
(Kf benzene = 5.12 K Kg/mol) What conclusion can you draw from the value of van’t Hoff factor obtained. 50. What are non ideal solutions? Give one example.Explain as to why non ideal
solution deviate from Raoult’s law. 51. Calculate the amount of KCl which must be added to 100 g of water so
that water freezes at –20C Assume that KCl undergoes complete dissociation. (Kf = 1.86KKg/mol , K=39,Cl=35.5)
52. Account for the following: a) intravenous injection is given by using 0.9%
NaCl (mass/volume) solution. b) Dried fruits and vegetables swell when kept in fresh water. c) The tanks used by scuba divers are diluted with helium. d) Mountain climbers sometimes get symptoms of a condition known as anoxia. e) Calcium chloride is added to clear the
roads covered by snow. f) Raw mango placed in concentrated salt solution shrivel in to pickle. g) People suffering from high blood pressure are advised to take minimum quantity of salty food. Concentration of solutions (Numerical)
53. A sample of drinking water contains 15 ppm of CHCl3 (by mass) Express this in % mass.Also find out the molality of the solution.
54. Concentrated H2SO4 is 49% by mass. Density of the solution is 1.5 g/ cm3.
Determine the molality and molarity of the solution.(Molar mass of H2SO4 = 98)
55. Concentated HNO3 is 68% by mass. Density of the solution is 1.5 g/ cm3.
Calculate the volume of the solution containing 20 grams of HNO3. 56. Na2CO3 and NaHCO3 mixture containing 1 gram is completely neutralised
by 0.1 M HCl. Determine the volume of HCl needed if the mixture contains equimolar mixture of Na2CO3 and NaHCO3.
57. Calulate the molality of 1M solution of NaNO3.Density of solution is 1.25 g/ cm3. Molar mass of NaNO3 = 85.
58. Calculate the number of moles of CH3OH in 5 litres of 2 molal solution. Density of the solution is 0.981 g/ cm3
59. Calculate the molality , molarity and mole fraction of KI if the density of 20% (mass/mass) aqueous solution of KI is 1.2 g/ cm3
Henry's law (Numerical)
60. Partial pressure of ethane over a saturated solution containing 6.56x10-2gram of ethane is 1 bar. What will be the partial pressure of the gas if it contains 5x 10-2 grams of ethane.
61. Solubility of H2S in water at STP is 0.195 m. Calculate KH. 62. KH for CO2 in water is 1.67x10
8 Pa at 298K. Calculate the mass of CO2that can be dissolved in 500 ml of water at a pressure of 2.5 atmosphere at 298K. ( 1 atm= 1.013 x105 Pa)
63. Air is a mixture gases. It contains 20% by volume of O2 gas and 79% by volume of N2 gas at 298K. Water is in quilibrium with air at a pressure of 10 atmospheres. KH for O2 and N2 at 298 K are 3.30x10
7mm and 6.51x 107mm respectively. Determine the composition of these gases in water.
Raoult's law and Colligative properties. (Numerical)
1. liquid mixture if the total pressure is 600 mm Hg. Also find the composition in vapour phase.
2. Calculate the mass of non volatile solute which should be dissolved in 114 g of octane to reduce its vapour pressure to 80% (Molar mass of solute=40, Molar mass of octane=114)
3. Benzene and naphthalene forms ideal solution at 300K. Vapour pressure of pure benzene and naphthalene are 50.71 and 32.06 mm Hg respectively at 300K. Find the mole fraction of each components in vapour phase if 80 g of benzene mixed with 100 g naphthalene.(Molar mass enzene = 78, naphthalene = 128)
4. Benzene and toluene forms an ideal solution at 300K Vapour pressure of pure benzene and pure toluene are 160 mm and 60 mm Hg respectively. Calculate the total pressure of the solution under the following conditions :
a) mixing equal number of moles of benzene and toluene. b) equal mass of benzene and toluene. Also find the composition of benzene and toluene in vapour phase in each case.
Electrochemistry -
64. Molar conductivity vs square root of conc. is given
a. What can you say about the nature of the two electrolytes A & B b. How do you account for the increases in molar conductivity for strong
electrolyte A & weak electrolyte B on dilution. (a) A current of 1.5 A was passed through an
electrolytic cell containing ii. AgNO3 soln. With an inert electrodes. The weight of Ag
deposited was iii. 1.5 g How long did the current flow?
c. (b)Write the reactions taking place at the anode & cathode in the above cell.
d. (c)Give reactions taking place at the two electrodes if these are made up of Ag.
(a) Two electrolytic cells containing AgNO3 solution and dil. HCl solution
e. were connected in series A steady current of 2.5 A was passed through
f. them till 1.078 g of Ag was deposited. [Ag = 107.8 g/mol, 1F = 96500 C]
65. How much electricity was consumed? 66. What was the weight of O2 gas liberated? 67. Give reasons: Rusting of iron pipe can be prevented by joining it with a piece of Mg Conductivity of an electrolyte solution decreases with the decrease in concentration.
(a) What is a fuel cell? What is the main advantage?
( b ) What are the reactions occurring at the cathode and anode of a b. Lachlanche cell?
68. In a button cell widely used for watches and other devices the following reactions takes place a. Zn(s)+Hg2O+H2O � 2Hg + 2OH- + Zn2+ b. Give the cell representation and determine the value of Kc for the
above reactions using the following data. Zn(s) � Zn2+ + 2 e E0Zn2+/Zn = - 0.76V)
c. Hg2O+H2O + 2e � 2Hg + 2OH- ( E0Hg+/Hg = - 0.344V) i. Zn2+ + 2 e � Zn(s) ( E0Zn2+/Zn = - 0.76V)
(a) Define molar conductivity of a substance & describe how far weak &
d. strong electrolyte,molar cond. Changes with conc. of solute . How is such
e. change. Explain. 69. (b) A voltaic cell is set up at 25 0C with the following half cells
a. Ag+ (0.001M)/Ag & Cu 2+ (0.1M)/Cu b. What would be the voltage of this cell? (E0cell. + 0.46V)
(a) State the relationship amongst cell const. of a cell,resistance of the soln.
c. in the cell & cond. Of soln. How is molar cond. Of a solute related to cond.
d. Of its soln. 70. (b) Calculate K for the reaction Fe+ Cd2+ � Fe2+ + Cd
a. (E0Fe2+/Fe = -0.44V, E0Cd2+/Cd = -0.40V) (a) Define molar conductivity.How is it related to
cond. Of the related soln. b. (b)One half cell in voltaiccell is constructedfrom a silver wire dipped
in AgNO3 soln. of unknown conc.Its other half cell consists of a Znelectrode dipping in 1.0 M soln. of Zn(NO3)2.A voltage of 1.48V is measured for this cell. Calculate [Ag+ ]
i. (E0Zn2+/Zn = -0.76V, E0Ag+/Ag = 0.80V) (a) Corrosion is essentially an electrochemical
phenomenon. Explain the c. reactions occurring during the corrosion of iron kept in an open
i. atmosphere. 71. (b) Calculate K for the reaction Fe+ Cd2+ � Fe2+ + Cd
a. (E0Fe2+/Fe = -0.44V, E0Cd2+/Cd = -0.40V) 72. . Explain the terms
a) resistance b) resistivity c) conductance d) conductivity e) molar conductivity
73. Give the products of electrolysis of a) NaCl (molten)
b) NaCl (aq) c) H2SO4(aq) d) CuSO4(aq) using inert electrode like Pt e) CuSO4(aq) using Cu electrodes f) AgNO3(aq) using Ag electrode g) AgNO3(aq) using Pt electrode.
74. Write the reactions involved at each electrode in Leclanche cell. Mention the disadvantage of this cell.
75. Write the reactions involved at each electrode in mercury cell. Why does the cell potential of this cell remains constant?
76. What are fuel cells? Write the reactions involved at each electrode in H2-O2 fuel cell.
77. Give one similarity and one difference between fuel cell and other primary cells.
78. For a chemical reaction variation in the [R] � t (first order graph ln log [R] � t )
What is the order of reaction What are the units of rate constant k Give the relationship between k & t ½ What does the slope of the above line indicate? Draw a plot log [R0]/[R] � t
79. The reaction A+2B� 2C+D
Expt. [A]0 [B]0 Initial rate
1 0.3 0.3 0.96
2 0.6 0.3 0.384
3 0.3 0.6 0.192
4 0.6 0.6 0.768
(i)Derive the order of reaction w.r.t.both reactants [A] & [B] (ii)Write the rate law (iii)Write the expression for the rate of reaction in terms of A & B
80. Define the term order of reaction for chemical reaction 81. A first order decomposition reaction takes 40 min. for 30% decomposition 82. Calculate its t1/2 value. 83. What is meant by the rate const.’k’of a reaction. If the concentration be 84. expressed in mol/L units & time in sec.What would be the units for k (i)
for a 85. zero order reaction (ii) for a first order reaction
(a) Derive the general form of the expression for the half life of a first order
ii. reaction b. ( b) The decomposition of NH3 on Pt surface is a zero order reaction
What are the rates of production of N2 & H2 if k = 2.5x10-4 mol/L/s
(a) List the factors on which the rate of a chemical reaction depends?
c. ( b) The half life for decay of radioactive C-14 is 5730 years An i. archeological artifact containing wood has only 80% of C-14
activity is found in living trees. Calculate the age of the artifact.
86. Explain the following terms: a) average rate of a reaction
b) instantaneous rate of a reaction.
c) rate constant of a reaction d) rate law of a reaction e) order of a reaction f) molecularity of a reaction.
87. Derive integrated rate law for a) zero order reaction
b) first order reaction. Show that t1/2 for c) zero order reaction is directly proportional to initial concentration of the reactant. d) first order reaction is independant initial concentration of the reactant.
88. Chemical kinetics (Numerical) 1. The decomposition ammonia on a platinum surface follows
zero order kinetics. 2NH3(g) N2(g)+3H2(g) K= 2.5x10
-4 mole/l/sec. Determine the rate of
a) disapperance of NH3 b) rate of formation of N2 c) rate of formation of H2.
2. The decomposition ammonia on a platinum surface follows zero order kinetics. Calculate the value of rate constant K and the half life of the reaction. Given
Time (seconds) Pressure of NH3(g) in Pascal 0 4x10-2 100 3.5 x10-2 200 3.0 x 10-2 300 2.5 x 10-2
89. A first order reaction is 20% complete in 10 minutes. Determine the time taken for 80% completion of the reaction.
90. 2A +B A2B K= 2.5 x10-4 M-2 sec-1 Find the rate when the initial
concentrations of [A] = 0.1M [B] = 0.2 M. Also find the rate when 0.04 moles/litre of A has reacted.Rate=K[A][B]2
91. For a certain chemical reaction variation in the concentration in [R ] versus time(s) plot is given below
i. what is the order of the reactions?
ii) what are the units of rate constant k? iii) give the relationship between k and t1/2 iv) what does the slope of the above line indicate? v) draw the plot [R ] 0 / [R] versus time(s)
92. Consider the reaction R → P. The change in the concentration of R with shown in the following plot.
93. Predict the order of the reaction. ii) Write the expression for half life of this reaction.
94. 2NO2+F2 _2NO2F Write the rate of reaction in terms of (a) rate of formation of NO2F
(b) rate of disappearance of NO2 (c) rate of disappearance of F2
95. The decomposition of NH3 follows zero order. 2 NH3 N2+3H2 Find the rate of production of N2 and H2.K=2.5x10
-4MS-1 −1 96. 2A+B+C_ A2B+C Rate=K(A)(B)2 K=2x10-6M-2S-1Calculate the initial
rate when 97. (A)=0.1M
(B)=0.2M (C)=0.6M Find the rate when 0.04mole of (A) is consumed.
98. 2NO2+F2 _2NO2F Experiment (NO2)M (F2) M Rate(M/S) 1 0.2 0.05 0.006 2 0.4 0.05 0.012 3. 0.8 0.10 0.048
99. Find the order with respect to NO2 and F2.Also find the overall order of the reaction. Deduce the mechanism of the reaction.
100. Show that(a) 2t½=t¾ (b)Half life of a reaction is 10seconds.Find t2/3 101. Hydrolysis of methyl acetate in aqueous solution has been studied by
titrating liberated acetic acid with NaOH 102. rate=K(CH3COOCH3) (H2O)
t/min 0 30 60 90 c/M 0.8500 0.8004 0.7538 0.7096
103. Show that it follows pseudo first order reaction as the concentration of water remains constant (1L of water=1000g) What is the value of K?
104. Give differences between a) adsorption and absorption
b) physisorption and chemisorption c) lyophillic and lyophobic sol.
105. Explain the terms a) extent of adsorption(x/m)
b) enthalpy of adsorption c) desorption d) adsorbent e) adsorbate
106. Mention the factors affecting the adsorption of gases on solids. 107. Explain Freundlich adsorption isotherm with suitable graphs. 108. Why is adsorption
a) exothermic process b) surface property
109. Explain the effect of temperature on physisorption and chemisorption with graphs.
110. Mention five applications of adsorption. 111. Explain activity and selectivity of a catalyst with suitable examples. 112. What are shape selective catalysts? Give one example. 113. Give three examples each of homogeneous and heterogeneous
catalysis. 114. Explain the mechanism of
a) homogeneous catalysis b) heterogeneous catalysis.
115. Give three examples of reactions involving enzyme as catalyst. Explain the mechanism of enzyme catalysed reaction.
116. Explain the terms a) zeta potential
b) Helmoltz electrical double layer c) coagulation d) Colloidion e) peptisation
117. Explain Hardy and Schulze rule with suitable examples. 118. What are emulsions? How are they classified? Give two examples
each. 119. Explain the terms
a) emulsification b) demulsification c) emulsifier.
120. Write two uses of emulsion. 121. List four applications of colloids. 122. What is coagulation value? 123. Out of ammonia and nitrogen which gas will be absorbed more readily
on the surface of Charcoal and why? 124. How does adsorption of a gas vary with
a) temperature b) pressure? Illustrate with graphs.
125. Describe some features of catalysis by zeloite. Mention one application of zeolite.
126. . What do you mean by activation of adsorbent? How is it achieved? 127. General principles and process of isolation of elements
128. Distinguish between mineral and ore. 129. Mention the steps involved in metallurgy. 130. Name the important ores of Al, Fe, Cu and Zn. 131. . Explain the principles of
a) Hydraulic washing b) agnetic separation c) Froth floatation.
132. What is the role of depressant in froth floatation process? Name the depressant used in case of ore containing ZnS and PbS.
133. Mention the principle of leaching. Write the reactions involved in leaching of aluminium.
134. Write the reactions involved in leaching of Ag and Au. 135. Mention the principles of refining the metals by
a) Distillation b) Liquation c) Electrolytic refining d) Zone refining e) Vapour phase refining
136. Explain the electrolytic refining of copper with the reactions involved at each electrode.
137. Mention the uses of Al, Cu, Zn , cast iron, wrought iron and steel. 138. Dand F block elements 139. Account for the following
1. Zn, Cd and Hg are not considered as transition metals. 2. Cu,Ag &Au are considered as transition metal though it
has 3d10 configuration. 3. Zn, Cd and Hg are volatile and Hg is a liquid metal. 4. Transition metals have high enthalpy of atomisation. 5. 4d and 5d elements have higher enthalpy of atomisation
than 3d elements. 6. Density of 3d elements increases from Sc to Ni. 7. Atomic and ionic radii generally decrease along the
period. 8. Zr and Hf have similar size. 9. Transition metals do not show regular variation of
ionisation enthalpies. 10. 5d elements have higher ionisation enthalpy than 3d and
4d elements. 11. Generally first ionisation enthalpy increases along the
period. 12. Cr &Cu has higher second ionisation enthalpy
(Cr=24,Cu=29) 13. Mn &Zn has higher 3rd ionisation enthalpy (Mn=25
Zn=30) 14. Cu, Ni and Zn normally do not exhibit oxidation state
higher than +2. 15. Transition metals show variable oxidation state.
140. What is lanthonoid contraction? What is the reason for lanthonoid contraction? Mention the consequences of lanthonoid contraction.
141. What is mischmetal? Mention two uses of mischmetal. 142. How is
a) KMnO4 prepared from pyrolusite ore? b) K2Cr2O7 prepared from chromite ore?
143. Write the ionic equations of the reactions involved when acidified KMnO4 is treated with
a) FAS solution b) oxalic acid solution c) hydrogen sulphide d) KI solution e) Sn2+solution f) SO3
2- g) NO2- h) SO2
144. Write the ionic equation of the reaction involved when alkaline KMnO4 is reacted with
a) KI solution. b) S2O3
2- 145. Write the ionic equation of the reaction involved when acidified
K2Cr2O7 reacts with a) Sn2+ solution
b) SO2 c) hydrogen sulphide d) Fe2+
146. What is the effect of PH on chromate and dichromate solutions? 147. Compare the chemistry of lanthonoids and actinoids with reference to
a) electronic configuration b) oxidation state c) ionization enthalpy d) chemical reactivity e) magnetic behaviour f) atomic size
148. Coordination compounds 1. Write IUPAC names of the following compounds
a) [Co (NH3 )5 Cl ] Cl2 b) [Cr(NH3 )6 ]
3+ c) [Ni(NH3 )6 ] Cl2 d) [CoCl(NO2)(NH3)4 ] Cl
e) [Co(en)2(ONO)2] Cl f) [Cr(NH3 )5(H2O)]
3+ g) K3 [Co(C2O4)3 ] h) Na3 [Cr(OH)2F4 ] i) [Co(NH3 )6] [Cr(CN)6 ] j) [Pt(NH3 )2Cl(NH2CH3)] Cl k) [Ni(CO)4 ] l) [CrCl3 (Py)3 ]
149. Write the IUPAC name of ionization isomer of [Co(NH3)5Br ]SO4. Write the IUPAC name of linkage isomer of [Co(en)2(ONO)2 ]Cl
150. Write the formula of the following coordination compounds: a) Tris (ethane-1,2-
diamine)cobalt(III)sulphate b) Amminebromidochloridonitrito-N- platinate(II) c) Pottasiumtetrachloridopalladate(II) d) Tetrahydroxozincate Explain the following with suitable examples
2. coordination entity b) ligand c) coordination number d) coordination polyhedron e) homoleptic f) heterolrptic
151. What is meant by unidentate, bidentate and ambidentate ligands? Give two examples each.
152. Give an example of hexadentate ligand. 153. Explain chelation with a suitable example. 154. Using valence bond theory, predict the structure and the magnetic
behavior of the below given complexes: a) [Fe(CN)6 ]
4- b) [Fe(CN)6 ]
3- c) [NiCl4]
2- d) [Ni(CN)4]
2- e) [Cr(NH3)6 ]
3+ f) [Co(NH3)6 ]
3+ g) [Ni(CO)4] h) [Fe(CO)5]
i) [MnCl4]2- j) [CoF6 ]
3- k) [Co(en)3]
3+ l) [Co(C2O4)3]
3- 155. Account for the following:
a) [Fe(CN)6]4- is diamagnetic while [Fe(CN)6]
3-
is paramagnetic. b) [NiCl4]
2 is tetrahedral while [Ni(CN)4]2- is
square planar. c) Hydrated copper sulphate is colored while
anhydrous copper sulphate is colorless. d) [Ti(H2O)6]
3+ become colorless on heating. e) [Ni(H2O)6]
2+ is green while [Ni(CN)4]2- is
colorless. f) [Fe(CN)6]
4- and [Fe(H2O)6]2+ show
different colors in aqueous solution.. g) [Cr(NH3)6]
3+ is paramagnetic while[Ni(CN)4]
2- is diamagnetic. 156. Draw the structure of optical isomers of
a) [Co(en)3]3+
b) [Cr(C2O4)3]3-
c) [PtCl2(en)2 ]2+
d) [Cr(NH3)2 Cl2(en)]+
157. Draw the structure of all the isomers (geometrical and optical) of a) [CoCl2(en)2]
+ b) [Co(NH3)2Cl2(en)]
+ c) [Co(NH3) Cl (en)2]
2+
Question Bank
(The p-Block Elements)
1. Account for the following:
Among the halogens F2 is the strongest O.A.
F exhibit only –1 oxidation state whereas other halogens exhibit higher positive oxidation state
also
2. Acidity of oxo acids of Cl is HOCl<HOClO<HOClO2<HOClO
3. A translucent white waxy solid A on heating in an inert atmosphere is converted to its
allotrope B. Allotrope A on reaction with very dil KOH liberates a highly poisonous gas C
having rotten fish smell. With excess of Cl2 forms D which hydrolyses to compound E Identify
A to E.Conc. H2SO4 is added to following chemicals in a test tube Identify the change observed
& support your answer with equation
(i)cane sugar(ii)NaBr(iii) Cu-pieces(iv) S powder (v) KCl
4. Complete hydrolysis of XeF6.Write equation
5. Predict the shape of ClF3 on the basis of VSEPR theory
6. Account for (a) Cl2 water has both oxidizing & bleaching properties
(b)H3PO2 &H3PO3 act as good R.A.while H3PO4 does not
(c)On oxidation of O3 gas to KI soln. violet vapours are obtained.
7. Give reasons: (a) CN- ion is known but CP- is not
(b) NO2 dimerises to form N2O4
(c) ICl is more reactive than I2
8. An element X exists as yellow solid in standard state It forms a volatile
hydride B which is a foul smelling gas & is extensively used in qualitative
analysis of salts when treated with oxygen B forms an oxide C which is
pungent smelling gas. This gas is passed through acidified KMnO4 soln.
decolourises it. C gets oxidized to another oxide D in the presence of
heterogeneous catalyst. Identify A,B,C,D & also give chem.. reaction of C
with acidified KMnO4 soln. & for conversion of C to D.
9. In the ring test for identification of NO3- ion what is the formula of the
compound responsible for the brown ring formed at the interface of two
liquids
What is the covalence of nitrogen in N2O5
Explain why both N & Bi do not form pentahalides while P does.
10. When conc. H2SO4 was added into an unknown salt present in a Test tube, a
brown gas A was evolved. This gas intensified when Cu turnings were also
added into this T.T. On cooling the gas A changed into a colourless gas B
Identify the gases A& B
(ii) Write the equations for the reactions involved.
Why does Cl2 water lose its yellow colour on standing
( b)What happens when Cl2 water reacts with cold dil soln. of NaOH. Write equation
only
11. Write down the equations for hydrolysis of XeF4 & XeF6.Which of these two
reactions is a redox reaction.
Describe the favourable conditions for the manufacture of
NH3 by Haber’s process
(ii) H2SO4 by Contact process
( b ) Draw the structures of (i) PCl5 (ii) S8 (iii) ClF3
12. Which is a stronger acid in aq. Soln. of HF or HCl
13. Reasons(i) P shows marked tendency for catenation but N shows little
tendency for catenation
( ii )The electron gain enthalpy with –ve sign for O (-141 KJ/mol) is less
than that for S(-200KJ/mol)
14. ( a) complete (repeated)
( b )Draw structures of (i) H2S2O7(ii) NO3-
15. (a)Reasons: (i) P4 is more reactive than N2
(ii) All bonds in PCl5 are not equal in length.
(iii) S in vapour state exhibits a paramagnetic behaviour
(b) Draw the structures of (i) BrF3 (ii) XeF2
***********************************************************************
LESSON 10 -- HALOALKANES AND HALOARENES
Q1. Why haloalkanes are more reactive than haloarenes.
(Q2. Why do haloalkenes under go nucleophillic substitution whereas haloarenes under go
electophillic substitution.
.
Q3. When an alkyl halide is treated with ethanolic solution of KCN, the major product is alkyl
cyanide where as if alkyl halide is treated with AgCN,the major product is alkyl isocyanide.
Q4. How do 10 20 30 alcohols differ in terms of dehydrogenation?
Q5. Why are the reaction of alcohol /phenol with acid chloride in the presence of pyridine ?
Q6. Explain why o-nitrophenol is more acidic than o-methoxy phenol ?
Q7. Aryl halides cannot be prepared by the action of sodium halide in the presence H2SO4
.Why?
Q8. Why Grignard reagent should be prepared under an hydrous conditions.?
Q9. Why is Sulphuric acid not used during the reaction of alcohols with KI ?
Q10 p- dichlorobenzene has highest m.p. than those of ortho and m-isomers.?
Q11. Although chlorine is an electron- withdrawing group, yet it is ortho and para directing in
electrophillic aromatic substitution reactions. Why
Q12. The treatment of alkyl chlorides with aqueous KOH lead to the formation of alcohols but
in presence of alcoholic KOH alkenes are major products. Explain?
Q13. Explain why vinyl chloride is unreactive in nucleophillic substitution reaction?
Q14. Arrange the following compounds according to reactivity towards nucleophillic
substitution reaction with reagents mentioned:-
4- nitro chloro benzene, 2,4 di nitro chloro bemzene, 2,4,6, trinitrochlorobenzene with CH 3ONa
Q15. Which compound will react faster in SN 2 reaction with OH ---?
Q16. Arrange in increasing order of boiling points.
(a) Bromobenzene, Bromoform, chloromethane,Dibromo-methane
(b) 1-chloropropane, Isopropyle chloride, 1-Chlorobutane.
Q 17. Predict the reactivity in SN1
(a) C 6H 5CH 2Br, C 6H 5CH (C 6H 5)Br,
C 6H 5CH(CH 3)Br, C 6H 5C(CH 3)( C 6H 5)Br
VERY SHORT ANSWER TYPE QUESTION
[1 MARKS]
Q.1. Write the formula & chemical name of DDT?
Q.2. An alkyl halide having molecular formula C 4H 9Cl is optically active. what is its
structure?
Q.3. Why is vinyl chloride less reactive than ethyl chloride?
Q.4. Write the structural isomers of C 3H 6Cl 2 which can exihibit enantiomerism ?
Q.5. Write down the structure of the following compounds;
(a) 1- chloro-4-ethyl cyclohexane
(b) 1,4-dibrone but-2-ene
(c) 4-tert,butyl-3-iodoheptane
(d) 1-bromo-4-secbutyl-2-methylbenzene
Q.6. Which compound (CH 3 ) 3 - C-Cl or ; CH 3Cl will react faster in SN 2 reaction with -
OH?
Q.7. A hydrocarbon C 5H 10 does not react with chlorine in dark but it gives a single
monobromo compound in bright sunlight . Identify the compound.
Q.8. Why is sulphuric acid not used during the reaction of alcohols with KI?
Q.9. Chloroform is stored in dark coloured & sealed bottle. Why?
Short answer type questions
Q,1. Why is chloroform not used as anesthetic these days? What is the commonly used
anesthetic?
Q2. What happens when benzalchloride is boiled with aqueous NaOH solution?
Q3. Iodoform gives a precipitate with silver nitrate upon heating while CHCl3 does not .
Assign a suitable reason.
Q4. Which one of the following has highest dipole moment?
( a) CHCl2 (b) CHCl3 ( c) CCl4
Q5 Wurtz reaction is not a good method for preparing propane. Justify
Q6 Give the IUPAC names of the following compounds?
a) ClCH 2C = CCH 2Br b) (CCl 3 ) 3 CCl c) CH 3CH(Cl)CH(Br)CH3
Q.2. Starting from methyl iodine, how will you prepare :
a) nitromethane b) methyl nitrite
Q.3. How can iodoform be prepared from ethanol ?
Q.4. Predict the product of the following reactions;
Q.5. Write the reaction involved in :
a) isocyanide test b) iodoform test
Q.6. Rearranging the following in order of increasing case of dehydro halogenations
CH 3CH 2CH 2Cl CH 3CHClCH3 , CH 3 - C- Cl(CH 3 2.)
Q.7. How will you distinguish between
(i) CH 3NH 2 and (CH 3 2) N H (ii) ethanol & 1-propanol
Q.8. Give the uses of (a) CCl 4 (b) iodoform
Q.9. Propose the mechanism of the following reaction :
CH 3-CH 2-Br + CH 3ONa CH 3-CH 2-OCH 3 + Br
Q.10. Which will have a higher boiling point 1-chloropentane or 2-chloro-2-methylbutane?
Q.11. How will you bring the following conversion?
(a) Propene to Propyne (b) Toluene to Benzyle Alcohol (c) Aniline to Phenylisocyanide
Q.12. What happen when;
(a) n-butyl chloride is treated with alc.KOH.
(b) ethyl chloride is treated with aq.KOH.
(c) methyl chloride is treated with KCN.
3 MARKS QUESTIONS
Q1. How can we produce nitro benzene from phenol?
Q 2. Alcohols reacts with halogen acids to form haloalkenes but phenol does not form
halobenzene. Explain
Q 3. Explain why o-nitrophenol is more acidic than o-methoxy phenol?
Q4. Of benzene and phenol, which is more easily nitrated and why?
Q5. How will you account for the following? Ethers possess a net dipole moment even if they
are symmetrical in structure?
Q 6. How do 1°, 2° and 3° alcohols differ in terms of their oxidation reaction and
dehydrogenation.
Q7. How is diethyl ether prepared from ethyl alcohol?
Q8. Why are reactions of alcohol/phenol and with acid chloride in the presence of pyridine?
LONG ANSWER TYPE QUESTIONS
Q1) How the following conversions can be carried out?
(i) Propene to propan-1-ol
(ii) 1-Bromopropane to 2-bromopropane
(iii) Toluene to benzyl alcohol
(iv) Benzene to 4-bromonitrobenzene
(v) Benzyl alcohol to 2-phenylethanoic acid
Q2) How the following conversions can be carried out?
(i) Ethanol to propanenitrile
(ii) Aniline to chlorobenzene
(iii) 2-Chlorobutane to 3, 4-dimethylhexane
(iv) 2-Methyl-1-propene to 2-chloro-2-methylpropane
(v) Ethyl chloride to propanoic acid
Q3) How the following conversions can be carried out?
(i) But-1-ene to n-butyliodide
(ii) 2-Chloropropane to 1-propanol
(iii) Isopropyl alcohol to iodoform
(iv) Chlorobenzene to p-nitrophenol
(v) 2-Bromopropane to 1-bromopropane
Q4) How the following conversions can be carried out?
(i) Chloro ethane to butane
(ii) Benzene to diphenyl
(iii) tert-Butyl bromide to isobutyl bromide
(iv) Aniline to phenylisocyanide
LESSON 11 - ALCOHOL PHENOL ETHER
Q1 Sodium metal cannot be used for drying alcohol. Assign reason.
Q2. Ethanol and di methyl ether are iso meric but alcohol is a liquid at room temperature but
ether is a gas. Explain
Q3. Tertiary alcohol forms white turbidity faster withLucas reagent while primary alcohol
does not at room temperature. Why?
Q4. Hydration of 3 – phenyl but-1-ene in dilute H2SO4 forms 2-phenylbutan-2-ol and not 3
phenyl butan-2-ol.Why?
Q5. p-nitrophenol is a stronger acid than phenol while p-cresol is a weaker acid. Discuss.
Q6. How will you distinguish between CH3 ( CH2)3OH and CH3 CH ==== CH CH2 OH
by a chemical test?
Q7. How will you distinguish between Allyl alcohol and n propyl alcohol?
Q8. Preparation of ethers by acid dehydration of secondry or 30alcohols is not a suitable
method. Why
Q9 Phenols do not give protonation reactions readily. Why?
Q10 Ortho‐ nitrophenol is more acidic than ortho -methoxy phenol ? Why?
REASONING QUESTIONS
Q1. Explain why propanol has higher boiling point than that of the hydrocarbon, butane?
Q2. Alcohols are comparatively more soluble in water than hydrocarbons of comparable
molecular masses. Explain this fact.
Q3 . While separating a mixture of ortho and para nitrophenols by steam distillation, name the
isomer which will be steam volatile. Give reason.
Q4. Explain why is ortho nitrophenol more acidic than ortho methoxyphenol?
Q5. Preparation of ethers by acid dehydration of secondary or tertiary alcohols is not a suitable
method. Give reason.
Q6. What is meant by hydroboration‐oxidation reaction? Illustrate it with an example .
Q7. Give the equations of reactions for the preparation of phenol fromcumene.
Q8. Write chemical reaction for the preparation of phenol from chlorobenzene.
Q9 How is aspirin (Acetylsalicylic acid) prepared from salicylic acid?
Q10. Which out of propan-1-ol and propan-2-ol is stronger acid?
Q11. What is denaturation of an alcohol?
Q12. Give IUPAC name of CH3OCH 2OCH3
Q13. Diethyl ether does not react with sodium. Explain.
2 MARKS QUESTIONS
Q1. Give two reactions that show the acidic nature of phenol. Compare acidity of phenol with
that of ethanol.
Q2. How does phenol react with dilute and conc. HNO3?
Q3 How does phenol react with Br2 in CS2 and Bromine water?
Q4. How do you account for the fact that unlike phenol, 2, 4- dinitrophenol and 2, 4, 6-
trinitrophenol are soluble in aqueous solution of sodium carbonate?
Q5 . (i) Why is the Dipole moment of methanol higher than that of phenol?
(ii) . Explain why phenols do not undergo substitution of the -OH group like alcohols.
Q6. Account for the following
a). Boiling point of the C2H5OH is more than that of C2H5Cl
b). The solubility of alcohols in water decreases with increase in molecular mass.
Q7. Answer the following:-
a) What is the order of reactivity of 10, 20 and 30 alcohols with sodium metal?
b) How will you account for the solubility of lower alcohols in water?
Q8. Give reasons:-
i) Nitration of phenol gives ortho- and para- products only.
ii) Why do alcohols have higher boiling points than the haloalkanes of the same molecular
mass?
Q9. Account for the following:
i) Phenols has a smaller dipole moment than methanol
ii) Phenols do not give protonation reactions readily.
Q10. Explain the fact that in aryl alkyl ethers
(i) The alkoxy group activates the benzene ring towards electrophilic substitution
(ii) It directs the incoming substituents to ortho and para positions in benzene ring.
3 MARKS QUESTIONS
Q1 How are primary, secondary and tertiary alcohols prepared from Grignard Reagents?
Q2. Give the equations of oxidation of primary, secondary and tertiary alcohols by Cu at 573
K.
.
Q3 Give equations of the following reactions:
(i) Oxidation of propan-1-ol with alkaline KMnO4 solution.
(ii) Bromine in CS2 with phenol.
(iii) Dilute HNO3 with phenol.
Q4. Show how will you synthesize:
(i) 1-phenylethanol from a suitable alkene.
(ii) cyclohexylmethanol using an alkyl halide by an SN 2 reaction.
(iii) pentan-1-ol using a suitable alkyl halide?
Q5. How are the following conversions carried out?
(i)Propene → Propan-2-ol
(ii) Benzyl chloride → Benzyl alcohol
(iii) Ethyl magnesium chloride → Propan-1-ol.
Q6. Name the reagents used in the following reactions:
(i) Oxidation of a primary alcohol to carboxylic acid.
(ii) Oxidation of a primary alcohol to aldehyde.
(iii) Bromination of phenol to 2,4,6-tribromophenol.
Q7 How is 1-propoxypropane synthesised from propan-1-ol? Write mechanism of this
reaction.
Q8. Write the equation of the reaction of hydrogen iodide with:
(i) 1-propoxypropane (ii) Methoxybenzene and (iii) Benzyl ethyl ether
Q9. Name Reactions
a) Reimer Tiemann Reaction
b) Williamson Synthesis
c) Kolbes Reaction
d) Friedelcraft Reaction
5 MARKS QUESTIONS
Q1. Write equations of the following reactions:
(i) Friedel-Crafts reaction−alkylation of anisole.
(ii) Nitration of anisole.
(iii) Bromination of anisole in ethanoic acid medium.
(iv) Friedel-Craft's acetylation of anisole.
(v) Reaction of phenol with Zn dust.
ALDEHYDES,KETONES AND CARBOXYLIC ACID
1. NOMENCLATURE
a). CH 3CH CH 3 CH 2CH 2CHO
b). (CH 3)2C == CHCOCH3
c). CH 3CH=CHCHO
d). CH 3COCH 2COCH3
e). OHCC 6H 4CHO-p
f). CH 3C === CCH ===CHCOOH
2. Draw the structures of the following compounds;
(i) p-Methylbenzaldehyde
(ii) 4-Methypent-3-en-2-one
iii) 3‐Bromo‐4‐phenylpentanoic acid
iv) Hex‐2‐en‐4‐ynoic acid
(v) 2,6 – dimethyl phenol
Q1:-Distinguish between the following:-
(a) Phenol and alcohol
(b) Benzaldehyde and Propanal
(c) Acetic acid and formic acid
(d) Benzophenone and acetophenone
(e) Ethanal and propanal
(f) Propanol and ethanol
(g) Pentanone-2 and pentanone-3
(h) 2 Alcohol and 3 alcohol
(i) 1,2,3 amine
(j) Benzoic acid and benzene
(k) Phenol and benzoic acid
(l) Aniline and ethyl amine
(m) Aniline and nitrobenzene
(n) Benzaldehyde and acetophenone
(o) Methanol and benzaldehyde
(p) Chloro benzene and benzyl chloride
CONCEPTUAL QUESTIONS
Q1 Although phenoxide ion has more no. of resonating structures than carboxylate ion , even
though carboxylic acid is a stronger acid why ?
Q2 Why Carboxylic acid have higher boiling point than alcohols?
Q3 There are two-NH 2 group in semicarbazide . However only one is involved in formation
of semicarbazones. Why?
Q4 Why does solubility decreases with increasing molecular mass in carboxytic acid?
Q.5 Why are aldehydes are more reactive than ketones when undergo nucleophillic addition
reaction?
Q6 Why PCC cannot oxidise methanol to methanoic acid and while KMNO 4 can?
Q.7 During preparation of esters from a carboxylic acid and an alcohol in the presence of acid
catalyst water or ester formed should be removed as soon as it is formed.
Q8 Why HCOOH does not give HVZ ( Hell – Volhard – Zelinsky) reaction while CH
3COOH does?
Q.9 Suggest a reason for the large difference in the boling point of butanol and butanal
although they have same solubility in water.
Q.10 Would you expect benzaldehyde to be more reactive or less reactive in nuderophillic
addition reaction than propanol. Explain.
Q11 Why does methanal not give aldol condensation while ethanol gives?
Q12 Why does methanal undergo cannizaro's reaction?
Q13 Which acid is stronger and why?
F 3C-C 6H 4COOH and CH 3C 6H 4COOH
Q14 Explain why O-hydroxy benzaldehyde is a liquid at room temperature while p-
hydroxy benzaldehyde is a high melting solid.
Q15 Why is the boiling point of an acid anhydride higher than the acid from which it is
derived?
Q.16 Why do Carboxylic acids not give the characteristic reactions of a carbonyl group?
Q17 Cyclohexanone forms cyanohydrin in good yield but 2,2,6 trimethyle cyclo-hexanone
does not. Why
Q18 Why is carboxyl group in benzoic acid meta directing?
Q19 Treatment of Benzaldehyde with HCN gives a mixture of two isomers which cannot be
separated even by careful fractional distillation. Explain why?
Q20 Sodium Bisulphite is used for the purification of aldehydes and Ketones. Explain.
Q21 Why pH of reaction should be carefully controlled while preparing ammonia derivatives
of carbonyl compound?
Q22 Why formic acid is stronger acid than acetic acid?
Q23 Why is oxidation of alcohals to get aldehydes carried out under controlled conditions?
Q24 Why the oxidation of toluene to benzaldehyde with CrO3 is carried out in the presence of
acetic anhydride.
Q25 Melting point of an acid with even no. of carbon atoms is higher than those of its
neighbour with odd no. of carbon atoms
Q26 Why do aldehydes have lower boiling point than corresponding alcohals?
Q27 Why do aldehydes behave like polar compounds?
Q28 Most aromatic acids are solids while acetic acid and others of this series are liquids.
Explain why?
Q29 ethers possess a dipole moment ever if the alkyl radicals in the molecule are identical.
Why?
Q30 Why does acyl chorides have lower boling point than corresponding acids?
Q31 Why ethers are stored in coloured bottles?
Q.32 Why formaldehyde cannot be prepared by Rosenmund's reduction?
Name Reactions
a) Cannizaro’s Reaction
b) Aldol Condensation
c) Cross Aldol Condensation
d) Decarboxylation
e) Hell – Volhard – Zelinsky Reaction
f) Clemmenson Reaction
Long Answer Type Questions
Q1 : An organic compound (A) C8H16O2 was hydrolysed with dilute sulphuric acid to give
carboxylic acid (B) and an alcohol (C). Oxydation of (C) with chromic acid produced (B). (C)
on dehydration gives but – 1 – ene. Identify A,B, C
Q2. An organic compound with the molecular formula C9 H10 O forms 2,4 DNP
derivative reduces tollens reagent and undergoes . cannizaro reaction , on vigorous oxidation
it gives 1,2 benzenecarboxylic acid . identify the compound .
Q3. An organic compound (A) with molecular formula C 8H 8O forms an orange‐red
precipitate with 2,4 DNP reagent and gives yellow precipitate on heating with iodine in the pres
ence of sodium hydroxide. It neither reduces tollen's or fetiling's reagent , nor does it decolourise
bromine water or baeyer's reagents .On drastic oxidation with chromic acid .it gives a carboxylic
acid (B) having molecular formula C 7H 6O2. Identify the compounds (A)
and (B).
Q4. Two moles of organic compound A on treatment with a strong base gives two
compounds B and C. Compound B on dehydration with cu gives A while acidification of C
yields carboxylic acid D having molecular formula of CH 2O2 Identify the compounds A
,B,C,D
Q5. An aliphatic compound _A'with a molecular formula of C 3H 6O reacts with
phenylhydrazine to give compound _B' .Reaction of _A' with 2I in alkalene medium
on warming gives a yellow precipitate _C'. Identify the component A,B,C
Q6 . A compnent _A' with molecular formula C5 H10 O gave a positive 2,4 DNP test
but a negative tollen's reagents test . It was oxidised to carboboxylic acid _B' with molecular for
mula C 3H 6O 2 when treated with alkalines KMnO4 under vigrous condition . Sodium
salt of _B' gave hydrocarbon _C' on kolbe eletrolysis reduction . Identify A,B,C and D.
Q7 An organic compound _A' has the molecular formula C5 H10 O .It
does not reduse fehling's solution but forms a bisulphite compound .It also gives positive Iodofor
m test. What are possible structure of A' ?Explain your reasoning.
Q8. An organic compound _A' which has characterstic odour , on
treatment with NaOH forms two compounds _B' and _C'.
Compound _B' has the molecular formula C 7H 8O which on oxidation
gives back compound _A'. Compound 'C' is the sodium salt of an
acid which when heated with soda lime yields an aromatic
hydrocarbon _D'. Deduce A,B,C,D
Q9. An organic compound _A' is resistant to oxidation forms an oxidation forms a
compound 'B_(C 3H 8O) on reduction ._B'reacts with HBr to form a bromide _C'
which on treatment with alkoholic KOH forms an alkene _D' (C 3H 6). Deduce A,B,C,D.
Q10. Eherial solution of an organic compound 'A' when heated with magnesium gave 'B'
on treatment with ethanal followed by acid hydrolysis gave 2‐propanol . Identify the
compound 'A_ . What is 'B' known as?
Q12. Primary alkyl halide C 4H 9Br (A) reacted with alcoholic KOH to give compound
(B) is reacted with HBr to give (C) which is an isomer of (A). When (A) is reacted with
sodium metal it gives compound (D) C8 H18 that was different from the compound formed
when n‐butyl bromide is reacted with sodium . Give the formula of (A) and
write equations.
Q13 . An organic compound 'A' having molecular formula C 4H 8 on treatment with dil.H
2SO 4 gives 'B_ . _B_on treatment with conc. HCL and anhydrous ZnCl2
gives C and on treatment with sodium ethoxide gives back A.Identify A,B,C.
Q14. An aromatic compound A on treatment with aqueous ammonia and heating forms
compound B which on heating with Br 2 and KOH forms a compound C of molecular
formula C 6H 7N .Identify A,B,C .
Q15 . Two isomeric compound A and B having molecular formula C H N , both lose N 2
on treatment with HNO and gives compound C and D. C is resistant to oxidation
but immediately responds to oxidation to lucas reagent after 5 minutes and gives a positive
Iodoform test. Identify A and B
Q16. An organic compound _A' having molecular formula C 2H 5O 2N reacts with
HNO 2 and gives C 2H 4O 3N 2. On reduction _A' gives a compound 'B' with molecular
formula C 2H7N._C' on treatment with HNO 2 gives _C' which gives positive
idoform test . Identify A,B,C
Q17 An organic compound _A' having molecular formula C 3H 5N reduction gave
another compound _B'. The compound B on treatment with HNO2 gave propyl alcohol. B on w
arming with CHCl 3 and alcohalic caustic potash give the offensive smelling C.
Identify A,B,C
Q18 . Idomethane reacts with KCN to form a major product A .Compound _A' on
reduction in presence of LiAlH 4 forms a higher amine 'B'. Compound B on treatm
ent with CuCl 2 forms a blue colur complex C . Identify A,B,C
Q19. An aliphatic compound A with molecular formula C 2H 3Cl on treatment with
AgCN gives two isomeric compounds of unequal amount with the molecular formula C 3H3N
.The minor of these two products on complete reduction with H in the presence of Ni gives 2
compound 'B' with molecular formula C 3H 9N.Identify the compounds.
Q20. A compound 'X' having molecular formula C 3H 7NO reacts with Br 2 in presence
of KOH to give another compound Y. the compound Y reacts with HNO to form ethanol N
gas. Identify X,Y,
Q21. A compound _A' of molecular formula C 3H 7O 2N reaction with Fe and conc, HCl
gives a compound _B' OF molecular formula C 3H 9N. Compound _B' on treatment
with NaNO and HCl gives another compound _C' of molecular formula C 3H8O .
The compound _C'gives effervescences with Na on oxidation with CrO 3.The compound
C' gives a saturated aldehyde containing three carbon atom deduce A,B,C.
Q22. A Chloro compound _A' on reduction with Zn - Cu and alcohol gives the hydro carbon
(B) with five carbon atom.When _A' is dissolved in ether and treated
with sodium 2,2,5,5 tetramethyl hexhane is formed structure of A and B?
1 MARK QUESTIONS
Q1 Name the reaction and the reagent used for the conversion of acid chlorides to the
corresponding aldehydes.
Q2 Suggest a reason for the large difference in the boiling points of butanol and butanal,
although they have same solubility in water
Q3 What type of aldehydes undergo Cannizaro reaction ?
Q 4. Out of acetophenone and benzophenone, which gives iodoform test ?
Write the reaction involved. (The compound should have CH 3CO-group to show the iodoform
test.)
Q5 Give Fehling solution test for identification of aldehyde gp (only equations). Name
thealdehyde which does not give Fehling's soln. test.
Q6 What makes acetic acid a stronger acid than phenol ?
Q7 Why HCOOH does not give HVZ (Hell Volhard Zelinsky) reaction but CH 3COOH
does?
Q. 8 During preparation of esters from a carboxylic acid and an alcohol in
the presence of an acid catalyst, water or the ester formed should be removed as
soon as it is formed.
Q9. Arrange the following compounds in increasing order of their acid strength.
Benzoic acid, 4‐Nitrobenzoic acid, 3, 4‐dinitrobenzoic acid, 4‐methoxy benzoic acid.
Q10. How is tert‐butyl alcohol obtained from acetone?
2 / 3 MARKS QUESTIONS
Q1. Arrange the following compounds in increasing order of their boiling points. Explain by
giving reasons.
Q2. Which acid of each pair shown here would you expect to be stronger?
CH 3CO 2H or FCH 2CO 2H
Q3. Which acid is stronger and why?
F 3C — C 6H 4 — COO H, CH 3 — C 6H 4 — COOH
Q4. Arrange the following compounds in increasing order of their reactivity towards HCN.
Explain it with proper reasoning.
Acetaldehyde, Acetone, Di-tert-butyl ketone,
Methyl tert-butyl ketone.
Q5. Explain why o‐hydroxybenzaldehyde is a liquid at room temperature while p‐hydroxybenzal
dehyde is a high melting solid.
5 MARKS QUESTIONS
Q1 Arrange the following compounds in order ot their property as indicated-
i) Acetaldehyde, Acetone, di-tert-butyl ketone,
Methyl tert-butyl ketone reactivity towards HCN
IDENTIFY A B C
HCl
Q1. CH3COOH NH3 A NaOBr B NaNO2 C
Fe/HCl NaNO2/HCl H2O/H
Q2 C6H5NO2 A B C
Q3. A + H2 + Pd / BaSO4 (CH3)2CH CHO
Q4. (CH3)3C – CO-CH3 + NaOI B + C
Q5 C2H2 + (dil H2SO4 / HgSO4) A( dil NaOH) B on Heating C
H/H2O LiAlH4l
Q6 CH3CN A B
NaCN OH-- NaOH
Q7 CH3CH2I A B C
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