Question Bank Based on Board Papers

Prepared By Mrs. S.Srivastava

(The Solid States) 4 marksSAMPLE PAPER- 1 (OLD)Q9) Equal no. of cation & anion missing in the diagram is given.

(i) What are these types of vacancy defects called?(ii) How is the density of crystal affected by these defects?(iii) Name one ionic compound which can show this type of defect in

crystalline state.(iv) How is the stoichiometry of compound affected?

Q10) Analysis shows that M.O. has E.F.M 0.96 O 1.00 Calculate % M 2+ & M 3+ ions in the crystalQ10) In an ionic compound N- form cubic close type packing while the cation M+ ions occupy one third of the tetrahedral voids. Deduce the formula of compound & the C.N. of M+ ions.

SAMPLE PAPER- 2 (OLD)Q5) 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.Q19) 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.

SAMPLE PAPER- 3 (OLD) Q1) Name the type of point defect that occurs in a crystal of ZnS.Q4) How many octahedral voids are there in one mole of a compound having cubic close packed Structure? Q9) An element crystallizes in BCC structure.If the edge length of the cell is 1.469 x 10 -10 m. & density is 19.3 g/cm3. Calculate the at. Mass of this element. Also calculate the radius of an atom of this element.

2008 D

Asdfghlfkjaklsjdf;lkaejrgtlkQ1)What is the C.N. of each type of ions in a rock salt type crystal structure?Q19) what is a semiconductor? Describe the two main types of semiconductors & explain mechanism for their conduction.Q1) What is the total no. of atoms per unit cell in a FCC structure?Q1) What is the total no. of atoms per unit cell in a FCC structure?Q1) What type of substance exhibits antiferromagnetism?Q19) Reasons: (i) Frenkel defects are not found in alkali metal halides. (ii)Schottky defects lower the density of related solids.

(iii) Impurity doped Si is a semiconductor.Q19) Explain (i) Ferromagnetism (ii)Paramagnetism (iii) Ferrimagnetism.

2008 AIQ1) What is the total no. of atoms per unit cell in a FCC structure?Q19) Ag crystallizes in FCC lattice. The edge length of its unit cell is 4.077 x 10 -8 cm. & its density is 10.5 g/cm3 Calculate the at. Mass of Ag.

2008 FQ1) What type of alignment in crystals make them ferromagneticQ19) Reasons: (i) Frenkel defects are not found in alkali metal halides. (ii)Schottky defects lower the density of related solids. (iii) Impurity doped Si is a semiconductor.Q19) Explain (i) F-centre (ii)Paramagnetism (iii) Frenkel defect

2008 D COMPTTQ1) Name an element with which Si should be doped to give n- type semiconductor.Q19) Explain (i) F-centre (ii) Schottky defect (iii) Ferromagnetism

2008 AI COMPTTQ1) What are F- centres?Q19)Reason: (i) Fe3O4 is ferromagnetic at room temperature but becomes paramagnetic at 850K. (ii) ZnO on heating becomes yellow. (iii) Frenkel defect does not change the density of AgCl crystalsQ19) 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.Q8) Why is glass considered a supercooled liquidQ4) What is the two dimensional coordination no. of a sphere in square close packing?

2009 AIQ1) How do metallic & ionic substance differ in conducting electricity?Q20) Ag crystallizes with FCC unit cells. Each side of the unit cell has a length of 409 pm what is the radius of an atom of Ag?Q1) Which point defect of its crystals decreases the density of a solid?Q19) Fe has a BCC unit cell with a cell edge of 286.65 pm. The density of Fe is 7.87 g/cm3. Calculate Avogadro’s no. (at. Mass Fe=56 g/mol)Q1) What is the total no. of atoms per unit cell in a FCC structure?

2009 DQ1) Which point defect in crystal does not alter the density of the relevant solid?Q1) Which point defect in crystal alter the density of solid?Q1) Which point defect in crystal increases the density of solid?

2009 FQ1) What is the no. of atoms in a BCC unit cell of a crystal

2009 D COMPTT

Q13) How are the following properties of crystals affected by Schottky & Frenkel defects?(i) density (ii) electrical conductivityQ13) (a) In reference to crystal structure, explain the meaning of C.N.(b) What is the no. of atoms in a unit cell of FCC & BCC structureQ14) Cu crystallizes into a FCC lattice with edge length 3.61 x 10 -8 cm. Calculate the density of Cu? (Cu = 63.5 g/mol)

2010 AIQ1) What type of interaction hold the molecules together in a polar molecular solid?Q19 ) The density of Cu metal is 8.95 g / cm3 If the radius of Cu atom be 127.8pm Is the unit cell simple cubic , BCC or FCC? ( Cu = 63.54 g /mol , NA = 6.02 x 10 23 mol-1)Q1) What type of semiconductor is obtained when Si is doped with As?Q19) Ag crystallizes in FCC cubic unit cell. Each side of the unit cell has a length of 409 pm. What is the radius of Ag atom. Q1)Write distinguishing feature of metallic solids. Q19) Ag crystallizes in FCC cubic unit cell. If the edge length of unit cell is 4.07 x 10-8 cm. and density 10.5 g/cm3. Calculate the atomic mass of Ag (NA = 6.02 x 10 23 mol-1)

2010 DQ1)Write distinguishing feature of metallic solids from an ionic solid.Q19)In one unit cell of CaF2 there are 4Ca2+ and 8 F- ions.Ca2+ are arranged in FCC lattice.The F- ions fill all tetrahedral holes in the FCC lattice of Ca2+

ions,The edge of the unit cell is 5.46 x 10 -8 cm in length,the density of solid is 3.18 g/cm3.Calculate Avogadro’s no. (M.M. of CaF2 =78.08 g/mol) Q1) Which point defect in crystal of solid does not change the density of solidQ1) Which point defect in crystal of solid decreases the density of solid

2010 FQ1) What is the no. of atoms in a unit cell of a simple cubic crystal?Q19) Fe has a BCC unit cell with a cell edge of 286.65 pm. The density of Fe is 7.87 g/cm3. Calculate Avogadro’s no. (at. Mass Fe=56 g/mol)

NEW SAMPLE PAPER IQ1) Why LiCl acquires pink colour when heated in Li vapours.Q17) Sodium crystallizes in BCC unit cell. Calculate the approximate no. of unit cells in 9.2 g of sodium (Na = 23)Q18) What is a semiconductor? Describe the two main types of semiconductors.

NEW SAMPLE PAPER IIQ10) KF has CCP structure. Calculate the radius of unit cell if the side of the cube or edge length is 400 pm.How many F- ions and octahedral voids are there in this unit cell.Q11) Give reasons:

(a) Why is Frenkel defect found in AgCl?(b)What is the difference between P doped and Ga doped semiconductors.

NEW SAMPLE PAPER IIIQ9) Au )at.mass 197 u , at, radius= 0.144 nm) crystallizes in a FCC unit cell. Determine the density of Au.(NA = 6.022 x 10 23 mol -1)Q10) Classify each as being either p-type or n-type semiconductor. Give reason.

(a)Si doped with In(b) Si doped with P

2011 AIQ9) Explain how you can determine the at.mass of an unknown metal if you know its mass, density and the dimensions of unit cell of its crystal.Q10) Calculate the packing efficiency of a metal crystal for a simple cubic lattice.Q9)Define the following terms in relation to crystalline solids

(a)Unit cell (b) co-ordination no.Give one example in each case.

2011 DQ1) Crystalline solids are anisotropic in nature. What does this statement mean?Q19) Ag crystallizes in FCC unit cell. Each side of this unit cell has a length of 400pm. Calculate the radius of Ag atom.Q1) Which stoichiometric defect in crystal increases density of solid?Q19) The density of lead is 11.35 g/cm3 and the metal crystallizes with FCC unit cell. Estimate the radius of lead atom. (Pb = 207 g/mol)

2011 FQ1) What is meant by an intrinsic semi conductors?Q19) Al crystallizes in CCP. Radius of atom in metal is 125 pm.

(a)What is the length of side of unit cell?(b)How many unit cells are there in 1cm3 of Al

Q1) How many atoms are there in one unit cell of BCC crystal?Q19) Ag crystallizes in FCC unit cell. Each side of this unit cell has a length of 409 pm. Calculate the radius of Ag atom.

2010 D COMPTTQ13) How are the following properties of crystals affected by Schottky and Frenkel defects (i) density (ii) Electrical conductivity.Q13) (a) In reference to crystal structure , explain the meaning of coordination number.

(b ) What is the number of atoms in a unit cell of (i) a FCC structure (ii) a BCC structure

Q14) Copper crystallizes into an FCC lattice with edge length 3.61 x 10 -8 cm. Calculate the density of copper (Cu= 63.5 g/mol ,NA = 6.022 x 1023 /mol)

2010 AI COMPTTQ1) Give an example of an ionic compound which shows Frenkel defect.Q19) Copper crystallizes into an FCC lattice and has a density of 8.930g/cm3 at 293 K . Calculate the radius of copper atom. (Cu= 63.5 g/mol , NA = 6.022 x 1023 /mol)

2012 AIQ1) how may the conductivity of an intrinsic semiconductor be increased?Q19) copper crystallizes with FCC unit cell. if the radius of Cu atom is 127.8 pm, calculate the density of Cu metal. (at.mass of Cu = 63.55 u and NA = 6.02 x 10 23 /mol)Q19)iron has BCC unit cell with cell dimension of 286.65 pm. Density of iron is 7.87 g/cm3.use this information to calculate Avogadro’s number. (at.mass of Fe = 56.0u)Q1) which stoichiometric defect increases the density of a solid?Q1) what are n-type semiconductors?

2012 DQ1) What is meant by doping?Q19) Tungsten crystallizes in body centred cubic unit cell.If the edge of the unit cell is 316.5 pm.What is the radius of tungsten atom?Q19) Iron has a body centred cubic unit cell with a cell dimension of 286.65 pm The density of iron is 7.874 g/cm3 Use this information to Calculate Avogadro’s number.(at. Mass of Fe = 55.845 u)Q1)Write a point of differences between a metallic solid and an ionic solid other than metallic luster.

2012FQ1)What is meant by the term ‘forbidden zone’ in reference to band theory of solids?Q19) Iron has a body centred cubic unit cell with a cell dimension of 286.65 pm The density of iron is 7.874 g/cm3 Use this information to Calculate Avogadro’s number.(at. Mass of Fe = 55.845 u)Q19) Silver crystallizes in FCC unit cell.If the radius of silver atom is 145 pm, what is the length of each side of unit cell?Q1)Write a point of differences between a metallic solid and an ionic solid other than metallic luster.Q1) Define paramagnetism with an example.

2013 AIQ9) account for the following:

(i) schottky defects lower the density related solids.(ii) Conductivity of silicon increases on doping it with phosphorus

Q10) aluminium crystallizes in a fcc structure .atomic radius of the metal is 125 pm. What is the length of the side of the unit cell of the metal?Q9) (a) why does presence of excess of lithium makes LiCl crystals pink?(b ) a solid with cubic crystal is made of two elements P and Q. atoms of Q are at the corners of the cube and P at the body centre . what is the formula of the compound.Q13) (a) what change occurswhen AgCl is doped with CdCl2?

( b ) what type of semiconductor is produced when silicn is doped with boron

Solid state

FORMULAE :LIMITING RADIUS RATIO r+/ r-FOR CsCl STRUCTURE r+ (CATION RADII) =0.732 (C.N.8) r- (ANION RADII)FOR NaCl STRUCTURE r+ (CATION RADII) =0.414-0.732 (C.N.6) r- (ANION RADII)FOR ZnS STRUCTURE r+ (CATION RADII) =0.225 – 0.414 (C.N.4) r- (ANION RADII)FORMULA OF ACOMPOUND: NO. OF OCTAHEDRAL VOID=N NO. OF TETRAHEDRAL VOID = 2NRELATIONSHIP BETWEEN RADIUS OF THE SPHERE AND UNIT CELL EDGE LENGTH SIMPLE a =2r F.C.C. a = 4 / √2 r B.C.C. a = 4 /√3 rDENSITY OF THE UNIT CELL d = z M / a3 NA = no. of atoms per unit cell x molar mass (cell edge length)3 x Avogadro’s No.Imp. Points to be noted:AS DENSITY OF ELEMENT IS GIVEN IN g/cm3 , THE EDGE LENGTH IS TO BE CHANGED IN cm.IF VALUE OF a IS GIVEN IN pm THEN IT SHOULD BE MULTIPLIED BY10 -30

FOR NaCl STRUCTURE CELL LENGTH = 2 X DISTANCE BETWEEN Na+ AND Cl- IONIN SOME NUMERICALS

d = wt. OF ELEMENT X NO. OF ATOMS PER UNIT CELL (CELL EDGELENGTH)3 X NO. OF ATOMS PRESENT IN ELEMENTM IS AT. MASS IN CASE OF ELEMENTS AND MOLAR MASS IN CASE OF IONIC MOLECULE LIKE NaClVALUE OF zSIMPLE CUBE = 1 B.C.C. = 2 F.C.C. = 4CsCl = 1 , NaCl = 4 ,ZnS = 4

Question Bank

(Solutions) 5 marks

SAMPLE PAPER- 1 (OLD)Q11) Diagram of R.O. given. (i)Name the process occurring in the above plant. (ii) To which container does the net flow of solvent take place? (iii) Name one SPM which can be used in this plant.

(i) Give the practical use of the plant. Q19) Heptane & Octane form an ideal solution at 373 K. The V.P. of the pure liquid at this temperature is 105.2 KPa & 46.8 KPa resp. if the solution contains 25g of heptanes & 28.5 g of octane. Calculate

(i) V.P. exerted by heptanes (ii) V.P. exerted by solution(iii)mole fraction of octane in theV.P.

SAMPLE PAPER- 2 (OLD)Q6) What is van’t Hoff factor for a compound which undergoes tetramerization in an organic compound ?Q9)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)Q18) 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?

SAMPLE PAPER- 3 (OLD)Q28) (a) Derive relationship between relative lowering of V.P. & mole fraction of the volatile liquid

(b)(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.

(ii) What would have been the V.P. in the absence of dimerization.(iii) Derive a relationship between mole fraction & V.P. of a component

of an ideal solution in the liquid phase & vapour phase.Q28) (a) Which aqueous solution has higher concentration 1M or 1 molal solution of the same mole? Give reason.

(b)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)

2008 DQ11) State Henry’s law correlating the pressure of a gas & its solubility in a solvent & mention two applications for the law.Q20) Calculate the temp. at which a solution containing 54 g of glucose (C6H12O6) in 250 g of water will freeze (Kf for water =1.86 KKg/mol)Q9) State Raoult’s law for solution of volatile liquids taking suitable examples. Explain the meaning of positive & negative deviations from Raoult’law.Q9) Define the term O.P. Describe how the mol.mass of a substance can be determined by a method based on measurement of O.P.

2008 AIQ20) A solution containing 8 g. of substance in 100 g of diethyl ether boils at 36.86 0C whereas pure ether boils at 35.6 0C Determine the mol.mass of solute.( Kb for ether = 2.02 KKg/mol)Q20) Calculate the temperature at which a solution containing 54 g of glucose (C6H12O6) in 250 g of water will freeze.(Kf for water = 1.86 KKg/mol)

2008 FQ3) (a) State how the V.P, of a solvent is affected when a non volatile is dissolved in it .

( b )A 5% solution ( by mass ) of cane sugar in water has a F.P. 271K Calculate the F.P. of 5% (by mass) solution of glucose in water.

(F.P. of water is 273.15K,M.M.of sugar = 342g/mol & M.M. of glucose = 180 g/mol)

Q4) (a) If density of water of a lake is 1.25 g/mol & 1 kg of lake water contains 92g of Na+ ions. Calculate the molarity of Na+ ions in this lake water.

(b)Calculate the mass of a non volatile solute ( mol mass 40 g/mol) which should be dissolved in 114 g of octane to reduce its V.P. to 80 % (M.M. of octane = 114 g /mol )

2008 D COMPTTQ28) (a) The depression of F.P. of water observed for the same molar concn

of acetic acid, trichloroacetic acid & triflouroacetic acid increases in the order as stated above .Explain .

( b )Calculate the depression in F.P. of water when 20 g of CH3CH2CH(Cl) COOH is added to 500 g of water.(Ka =1.4 x10-3, Kf= 1.86KKg /mol)

Q28) (a) State Henry’s law & mention its two important applications.(b)Henry’s law constant for CO2 dissolving in water is 1.67 x 10 8 Pa at

298 K. Calculate the quantity of CO2 in 1L of soda water when packed under 2.5 atm CO2 pressure at 298 K.

2008 AI COMPTTQ9) 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.Q20) The b.p. elevation of 0.3g of acetic acid in 100g benzene is 0.0633K. Calculate the molar mass of acetic acid from this data.What conclusion can you draw about the molecular state of the solute in solution? (Kb for benzene = 2.53KKg/mol) Q18) Distinguish between the terms molality & molarity.Under what conditions are the molarity & molality of a solution nearly the same?Q26) The F.P. of a solution containing 0.2 g of acetic acid in 20 g of benzene is 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.Q13) What are non ideal solutions? Give one example.Explain as to why non ideal solution deviate from Raoult’s law.Q21) 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)

2009 AIQ28) (a) Define (i) mole fraction (ii) van’t Hoff factor

(b)100mg of a protein is dissolved in enough water to make 10 ml of a solution.If this solution has an O.P. of 13.3 mm Hg at 250CWhat is the molar mass of protein? (R= 0.0821 Latm/mol/K & 760 mm Hg=1atm)

Q28) (a) What is meant by (i) Colligative property (ii) molality of solution(b)What concentration of N2 should be present in a glass of water at room temp.?Assume temp. of 250C , a total pressure of 1 atm & mole fraction of N2 in air of 0.78 (KH for N2 = 8.42 x 10 –7 M/mmHg)

2009 DQ13) Differentiate between molality & molarity of solution.What is the effect of change in temp. of a solution on its molality or molarity?Q19) Calculate F.P. depression expected for 0.0711 m aq.solution of Na2SO4. If this solution actually freezes at –0.320C What would be the value of van’t Hoff factor (Kf for water = 1.86KKg/mol)

2009 FQ2) What is reverse osmosis?

2009 D COMPTTQ5) Define the term Osmotic Pressure.Q6) State the main advantage of molality over molarity as the unit of ConcentrationQ27) Calculate the amount of NaCl which must be added to 1 kg of water is depressed by 3K. ( Kf = 1.86KKg/mol, Na=23,Cl=35.5)Q5) State Raoult’s law for solution of volatile liquid.Q6) Define ideal solution Q19) A solution of urea in water has a b.p. 373.128K Calculate the F.P. of the same solution. (Kf = 1.86Km-1 , Kb=0.52Km-1)Q23) 0.1 mole of acetic acid was dissolved in 1 kg of benzene. Depression in F.P. of benzene was determined to be 0.256K. What is the state of solution? (Kf for benzene = 5.12K/m)

2010 AIQ9) Define the term osmosis and osmotic pressure.What is the advantage of using O.P. as compared to other colligative properties for the determination of molar masses of solute in solution.Q20) What mass of NaCl ( M.M. = 58.5 g/mol) must be dissolved in 65 g of water to lower the F.P. by 7.5 0C ? The F.P. depression constant Kf for water is 1.86 Kkg/mol. Assume that van’t Hoff factor for NaCl is 1.87.Q20) What mass of ethylene glycol (M.M = 62 g/mol) must be added to 5.5 kg of water to lower the F.P. of water from 0 0 C to – 10 0C ? (Kf for water = 1.86 Kkg/mol)Q20) 15 g of an unknown molecular substance was dissolved in 450 g of water . The resulting solution freezes at – 0.340C What is the molar mass of substance? (Kf for water = 1.86 Kkg/mol)Q2) Differentiate between molarity and molality of a solution.

2010 DQ9)Non ideal solution exhibits either +ve or –ve deviation from Raoult’s law.What are these deviations and why they are caused?Explain with one example of each.Q20) A solution prepared by dissolving 1.25 g of oil of winter green in 99 g benzene has a b.p. of 80.31 0C.Determine the molar mass of this compound. ( b.p. of pure benzene = 80.10 0C. and Kb for benzene = 2.530C kg/mol.)Q20) A solution of glycerol(M.M. = 92 g/mol) in water was prepared by dissolving some glycerol in 500 g of water.This solution has a b.p. of 100.42 0C

What mass of glycerol was dissolved to make the solution. (Kb for water = 0.512 Kkg/mol)

2010 FAll questions repeated

NEW SAMPLE PAPER IQ28) (a)Menthol is a crystalline substance with peppermint taste. A 6.2% solutionOf menthol in cyclohexane freezes at-1.950 C. Determine the formula mass of menthol.The F.P. and molal depression constant of cyclohexane are 6.5 0C and 20.2 K m-1 respectively, (b) State Henry’law and mention its two important applications. ( c ) Which of the following has higher b.p. and why? 0.1M NaCl or 0.1M glucoseQ28)(a) Define azeotropes and explain briefly minimum boiling azeotrope by taking suitable example. ( b ) The V.P. of pure liquids A and B are 450 mm and 700 mm of Hg respectively at 350 K.Calculate the composition of liquid mixture if total V.P, is 600 mmHg.Also find th composition of the mixture in vapour phase.

NEW SAMPLE PAPER IIQ13) State Raoult’s law for a solution containing volatile liquids.Explain with suitable example the concept of max. boiling azeotrope.Q24)On dissolving 19.5 g of CH2FCOOH in 500 g of water a depression of 1 0C

in F.P. of water is observed. Calculate the van’t Hoff factor and dissociation constant of flouro acetic acid, Given Kf = 1.86Kkg/mol

NEW SAMPLE PAPER IIIQ1) A and B liquids on mixing produce a warm solution. Which type of deviation from Raoult’s law is there?Q11) Determine the molarity of an antifreeze solution containing 250 g water mixed with 222 g ethylene glycol. The density of the solution is 1.07 g/mlQ12)An aqueous solution containing urea was found to haveb.p. more than the normal b.p. of water(313.13K)When the same solution was cooled it was

found that its F.P, is les than the normal b.p. of water(273.13K) Explain these observations

2011 AIQ11)State the following.

(a)Raoult’s law in its general formin reference to solutions(b)Henry’s law about partial pressure of a gas in a mixture

Q19) A solution prepared by dissolving 8.95 mg of a gene fragment in 35 ml of Water has an O.P. of 0.335 Torr at 25 0 V Assuming that the gene fragment is a non electrolyte,calculate its molar mass.Q19)What mass of NaCl must be dissolved in 65 g of water to lower the F.P. of water by7.5 0C?TheKf for water is1.86 0C/m. Assume van’t Hoff factor for NaCl is1.87(M.M. of NaCl is 1.87(M.M. of NaCl=58.5 g)Q2)What is reverse osmosis?Q3)Differentiate between molarity and molality values for solution.What is the effect of change in temperature on molarity and molality values?2011 DQ28) (a) Differentiate between molarity and molality for a solution. How does a change in temperature influence their values. (b ) Calculate F.P. of aq. solution containing 10.5 g of MgBr2 in 200g of water (MM of MgBr2 = 184g) (Kf for water = 1.86 Kkg/mol)Q28) (a) Define osmosis and osmotic pressure. Is the O.P.of a solution a colligative property? Explain. (b )Calculate the b.p. of a solution prepared by adding 15 g of NaCl to 250 g of water.(Kf for water = 0.512 Kkg/mol , M.M. of NaCl = 58.44g)Q28) (a) repeated (b ) What would be the M.M. of a compound if 6.21 g of it dissolved in 24 g of chloroform a solution that has a b.p. of 68.04 0C. The b.p. of pure chloroform is 61.7 0C . ( Kb for chloroform = 3.63 0C/m)

2011 FQ2) State Henry’s law about partial pressure of a gas in a mixture.Q9) Differentiate between molarity and molality for a solution. Explain how molarity value of a solution can be converted into its molality.Q10) A 0.561 m solution of an unknown electrolyte depresses the F.P. of water by 2.93 0C. What is van’t Hoff factor for this electrolyte. (Kf = 1.86 0C/kg/mol)

2010 D COMPTTQ5) Define the term Osmotic Pressure.Q6) State the main advantage of molality over molarity as the unit of concentration.Q27) Calculate the amount of NaCl which must be added to one kg of water so that the F.P. of water is depressed by 3K. (Kf = 1.86 Kkg /mol,Na =23, Cl=35.5)Q4) State Raoult’s law for a solution of volatile liquids

Q19) A solution of urea in water has a b.p. of 373.128K.Calculate the F.P. of the Same solution.(Kf for water = 1.86K/m , Kb = 0.52 K/m)Q1) Define an ideal solution.Q23) 0.1 mole of acetic acid was dissolved in 1 kg of benzene. Depression in F.P. of benzene was determined to be 0.256 K . What conclusion can you draw about the state of the solute in solution (Kf for benzene = 5.12 K/m)

2010 AI COMPTTQ2) Define the term, mole fraction.Q9) State Henry’s law and mention its two important applications.Q10) Calculate the mass of ascorbic acid (C6H8O6) to be dissolved in 75 g of acetic acid to lower its melting point by 1.5 0C (Kf for acetic acid = 3.9 Kkg /mol)Q17) Find the b.p. of a solution containing 0.520 g of glucose (C6H12O6) dissolved in 80.2 g of water.(Kb for water =0.52 K/m)Q18)Define the term Molarity of a solution. State one disadvantage in using the molarity as the unit of concentration.Q13) Find the f.p. of a solution containing 0.520 g of glucose (C6H12O6) dissolved in 80.2 g of water.(Kf for water = 1.86 K/m)

2012 AIQ28) (a) define the following terms:

(i) Mole fraction(ii) Ideal solution

(b) 15 g of an unknown molecular material is dissolved in 450 g of water. the resulting solution freezes at -0.340 C. what is the molar mass of the material?(Kf for water = 1.86 Kkg /mol)

Q28) (a) explain the following:(i) Henry’s law about dissolution of gases in a liquid(ii) Boiling point elevation constant for a solvent

(b)a solution of glycerol (C3H8O3) in water was prepared by dissolving some glycerol in 500 g of water. this solution has b.p.of 100.420C.what mass of glycerol was dissolved to make this solution? (Kb for water = 0.512 K kg /mol. )

2012DQ9)A 1 molal aqueous solution of trichloroacetic acid is heated to its b.p. The solution has the b.p. of 100.18 0C.Determine the van’t Hoff factor for trichloroacetic acid.(Kb for water = 0.512Kkg/mol) Q20) Calculate the amount of KCl which must be added to 1kg of water so that the f.p. is depressed by 2K.(Kf for water = 1.86Kkg/mol)Q20) a solution of glycerol (C3H8O3) in water was prepared by dissolving some glycerol in 500 g of water. this solution has b.p.of 100.420C.what mass of glycerol was dissolved to make this solution? (Kb for water = 0.512 K kg /mol. )Q20) 15 g of an unknown molecular material is dissolved in 450 g of water.

the resulting solution freezes at -0.340 C. what is the molar mass of the material?(Kf for water = 1.86 Kkg /mol)

2012 FQ9) (a) Define the following terms:

(i) Van’t Hoff factor(ii) Mole fraction(iii) Ebullioscopic constant

(b)State Raoult’s lawQ9) the density of water of a lake is1.25 g/ml and 1kg of this water contains 92 g of Na+ ions.What is the molarity of Na+ ions in the water of the lake? (at.mass of Na = 23 u ) Q20) At 250C the saturated V.P. of water is 3.165 kPa (23.75 mm Hg). Find the saturated vapour pressure of a 5% aqueous solution of urea (carbamide) at the same temperature. ( molar mass of urea = 60.05 g/mol)Q20) Calculate the F.P. depression expected for 0.0711 m aqueous solution of sodium sulphate. If the solution actually freezes at -0.320 0C,what is the actual value of van’t Hoff factor at this temperature? (Kf for water =1.86Kkg/mol)

2013 AIQ28) (a) state Raoult’s law for a solution containing volatile components. How does Raoult’s law become a special case of Henry’s law?

( b) 1.00 g of a non electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene by 0.40 K. Find the molar mass of the solute. (Kf for benzene = 5.12 Kkg mol -1)

Q28) (a) define the following trms:(i) Ideal solution(ii) Azeotrope(iii) Osmotic pressure

( b) a solution of glucose (C6H12O6) in water is labeled as 10 % by weight. What would be the molality of the solution?(molar mass of glucose = 180 g mol -1)

SOLUTION:

FORMULAE

∆Tb = Kb. wB .1000 MB .wA

∆Tf = Kf. wB .1000 MB .wA Π . V = wB . R T MB

FOR IONIC SOLUTE:

∆Tb = i Kb * m

∆Tf = i Kf * m

Π = i C R T

THE VALUE OF i MAY BE CONSIDERED 100% IF IONIZATION IS NOT GIVEN

NOTE: DON’T CHANGE THE UNIT OF ∆Tb OR ∆Tf FROM 0C TO K

OSMOTIC PRESSURE

IF THE VALUE OF R IS GIVEN 0.083 Lbar /mol.K , Π SHOULD BE IN bar

VOLUME OF SOLUTION WOULD BE IN LITRES.

WEIGHT OF SOLUTE SHOULD BE IN gm.

TEMP. SHOULD BE IN KELVIN

3% SOLUTION MEANS w = 3g & Vol. is 100 ml.

RAOULT’S LAW :

FOR VOLATILE COMPONENT:

P1 = P01 *X1 P2 = P02 * X2

TOTAL V.P. OF SOLUTION P = P1 + P2

FOR NON VOLATILE COMPONENT:

FOR DILUTE SOLUTION

EXPRESSION OF CONCENTRATION:

MOLE FRACTION XA = nA/nA +nB

Molality (m) = wB * 1000 (no. of moles present in 1kg solvent) MB *wA

Molarity (M) = = wB * 1000 ((no. of moles present in 1L solution) MB *Vol (ml)

RELATION SHIP BETWEEN MOLARITY AND MOLALITY

m = M____________ d-MB/100

HENRY’S LAW:

P = KH * X

VAN’T HOFF FACTOR:

i = NORMAL M.M./ ABNORMAL M.M. = OBSERVED /CALCULATED

i < 1 (ASSO) i > 1 (DISSO) i = 1 (NO ASSO OR DISSO)

FOR COMPLETE DISSOCIATION i for KCl = 2 ,for CH3COOH = ½ ,for K2SO4 =3

DEGREE OF DISSOCIATION

α = i - 1 / n -1

DEGREE OF ASSOCIATION

α = i - 1 / 1/n -1

Question Bank

(Electrochemistry) 5 marks

SAMPLE PAPER- 1 (OLD)Q12) Write the chemical equations for the steps involved in rusting of iron. Give one method to prevent rusting of ironQ20) For the galvanic cell Mg(s) + 2Ag+ (0.0001M Mg2+ (0.1M) + 2Ag(s) E0Mg2+/Mg = -2.36V, E0Ag+/Ag = 0.81V Calculate Ecell,E0cell. Write cell representation.Will the reaction be spontaneous?

SAMPLE PAPER- 2 (OLD)Q29)(a)Calculate the eq. Const. for the reaction Zn + Cd2+ Zn2+ + Cd E0Cd2+/Cd = -0.403V, E0Zn2+/Zn = -0.763V (b) When a current of 0.75A is passed through a CuSO4 solution for 25 min. 0.369 g of Cu is deposited at the cathode. Calculate at. mass of Cu

(c ) Tarnished Ag contains Ag2S Can this tarnish be removed by placing tarnished Ag ware in an Al pan containing an electrolytic solution such as NaCl.The E0 for half reactions are Ag2S Ag2S + 2e 2Ag + S2- is –0.17V Al3+ +3e Al is -1.66VQ29) (a) Calculate ∆G0 for the following reaction at 250C Au + Ca2+(0.1M) Au3+(1M) + Ca E0Au3+/Au = +1.5V, E0Cd2+/Cd = -0.403V Predict whether the reaction will be spontaneous or not at 250C Which of the above two half cells will act as an O.A. & which one will be a R.A.(b)The conductivity of 0.001M acetic acid is 4 x 10 –5 S/cm Calculate the dissociation const. of acetic acid if limiting molar conductivity for acetic acid is 390.5 Scm2/mol

SAMPLE PAPER- 3 (OLD)Q10) 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.Q19) (a) A current of 1.5 A was passed through an electrolytic cell containing AgNO3 soln. With an inert electrodes. The weight of Ag deposited was 1.5 g How long did the current flow?

(b)Write the reactions taking place at the anode & cathode in the above cell. (c)Give reactions taking place at the two electrodes if these are made up of Ag.

2008 D Q28) Conductivity of 0.00241M acetic acid solution is 7.896x10 –5 S cm-1 Calculate its molar conductivity in this soln. If limiting molar conductivity for acetic acid be 390.5Scm2mol-1 What would be the its dissociation const?Q28) Three electrolytic cells A,B,C containing soln. of ZnSO4,AgNO3,CuSO4 resp. are connected in series A steady current of 1.5 A was passed through them until 1.45 g of Ag was deposited at the cathode of cell B How long did the current flow? What mass of Cu & what mass of Zn were deposited in the concerned cell?(Ag = 108, Zn = 65.4 ,Cu =63.5)Q2) What is primary cell? Give one exampleQ10) The conductivity of a 0.2M soln. of KCl at 298 K is 0.0248 Scm -1. Calculate its molar conductivity.Q11) Formulate the galvanic cell in which the following reaction tale place Zn + 2Ag+ Zn2+ + 2Ag

(i) Which one of its electrodes is negatively charged?(ii) The reaction taking place at each of its electrode(iii) The carriers of current within & out side this cell.

Q2) Express the relation between conductivity & molar conductivity of a soln.Q10) The resistance of cond. Cell containing 0.001 M KCl soln. at 298 K is 1500

ohm What is the cell const. if the conductivity of 0.001 M soln. at 298 K is 0.146 x 10 –3 S cm-1

2008 AIQ10) Depict the Galvanic cell for the reaction Zn + 2Ag+ Zn 2+ + 2Ag What are the carriers of current inside and outside the cell.State the reactions at each electrode.

2008 FRepeated Questions.

2008 D COMPTTQ6) Illustrate with the help of diagram how the molar conductivities of a

(i) strong electrolyte (ii) weak electrolyte vary with dilution of soln. Give reason for this variation

Q20) Calculate E0cell for the following. 2Cr + 3Cd2+ 2Cr3+ + 3Cd Calculate ∆G0 & eq. Const. K of the above reaction at 25 0C (E0Cd2+/Cd = -0.40V, E0Cr3+/Cr = -0.74V)

2008 AI COMPTTQ28) (a) Explain why electrolysis of an aq. Soln. of NaCl gives H2 at cathode & Cl2 at anode. (E0Na+/Na = -2.71V, E0H2O/H2 = -0.83V, E0Cl2/2Cl- = +1.36V E02H+/1/2O2/H2O = +1.23V)

(b)The resistance of cond. Cell containing 0.05 M soln of an electrolyte X at 400C is 100 ohm The same cell is filled with 0.01M soln. of electrolyte. Y has a resistance of 50 ohm The cond. of 0.05 M soln of electrolyte X is 1.0 x 10 –4 Scm-1 Calculate

(i)cell const. (ii) conductivity of 0.01 M Y soln.(iii) molar conductivity of 0.01M Y soln.

Q28) (a) State Kohlrausch law of independent migration of ions. How can the degree of dissociation of acetic acid in a soln. to be calculated from its molar conductivity data. (b)(i) Formulate the galvanic cell 2Cr + 3Fe2+ 2Cr3+ + 3Fe

(ii)Calculate E0cell. (iii)Calculate Ecell at 250C if [Cr3+] = 0.1M , [Fe2+] = 0.01 M (E0Cr3+/Cr = -0.74V , E0Fe2+/Fe = -0.44V)

2009 AIQ9) What type of cell is a lead storage battery? Write the anode & cathode reaction & the overall reactions occurring in the use of a lead storage battery.Q9)Two half cell reactions of an electrochemical cells are given below. MnO4- + 8H++ 5 e Mn 2+ + 4H2O E0 = +1.51V Sn2+ Sn 4+ + 2e E0 = +0.15V Construct the redox equation from the two half cell reactions & predict if this reaction favours formation of reactants or product shown in the equation.Q21) A Cu-Ag cell is set up. The Cu 2+ concentration in it is 0.1M The Ag+

concentration is not known. The cell potential measured 0.422V Determine concentration of Ag+ in the cell. Given: (E0Ag+/Ag = 0.80V,E0Cu2+/Cu = +0.80V)Q21) A voltaic cell is set up at 25 0C with the following half cells Al/Al 3+ (0.001M) & Ni/Ni 2+ (0.5M) Write the equation for the cell reaction that occurs when the cell generates an electric current & determine the cell potential. (E0Ni2+/Ni = -0.25V, E0Al3+/AlCr = -1.66V)

2009 DQ28) (a) Define molar conductivity of a substance & describe how far weak & strong electrolyte,molar cond. Changes with conc. of solute . How is such change. Explain. (b) A voltaic cell is set up at 25 0C with the following half cells Ag+ (0.001M)/Ag & Cu 2+ (0.1M)/Cu What would be the voltage of this cell? (E0cell. + 0.46V)Q28)(a) State the relationship amongst cell const. of a cell,resistance of the soln. in the cell & cond. Of soln. How is molar cond. Of a solute related to cond. Of its soln. (b) Calculate K for the reaction Fe+ Cd2+ Fe2+ + Cd (E0Fe2+/Fe = -0.44V, E0Cd2+/Cd = -0.40V)Q28) (a) Define molar conductivity.How is it related to cond. Of the related soln.

(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+ ]

(E0Zn2+/Zn = -0.76V, E0Ag+/Ag = 0.80V)Q28)(a) Corrosion is essentially an electrochemical phenomenon. Explain the reactions occurring during the corrosion of iron kept in an open atmosphere. (b) Calculate K for the reaction Fe+ Cd2+ Fe2+ + Cd (E0Fe2+/Fe = -0.44V, E0Cd2+/Cd = -0.40V)

2009 FRepeated Questions

2009 D COMPTTQ28 ) (a) Explain why electrolysis of an aq. Soln. of NaCl gives H2 at cathode & Cl2 at anode. (E0Na+/Na = -2.71V, E0H2O/H2 = -0.83V, E0Cl2/2Cl- = +1.36V E02H+/1/2O2/H2O = +1.23V)

(b)The resistance of cond. Cell containing 0.001 M KCl soln. at 298 K is

1500 ohm What is the cell const. if the conductivity of 0.001 M soln. at 298 K is 0.146 x 10 –3 S cm-1

Q28) (a)Calculate emf for the given cell at 5 0C Cr/Cr3+(0.1M)//Fe2+

(0.01M)/Fe (E0Fe2+/Fe = -0.44V, E0Cr3+/Cr = -0.74V) (b)Calculate the strength of current required to deposit 1.2 g Mg from molten MgCl2 in 1 hour. [1F =96500C/mol at.mass Mg =24]

2010 AIQ2) What is meant by Limiting molar conductivity? Q11) Given that E0 of metals are K+/K = -2.93V,Ag+/Ag = 0.80V, Cu2+/Cu = 0.34V,Mg2+/Mg = -2.37V,Cr3+/Cr = -0.74V,Fe2+/Fe = -0.44V. Arrange these metals in increasing order of their reducing power.Q11) Two half reactions of an electrochemical cells are given below MnO4- + 8H+ + 5e Mn2+ + 4 H2O E0 = +1.51V Sn2+ Sn4+ + 2e E0 = +0.15V Costruct the redox reaction equation from the two half reactions and calculate the cell potentials and predict if the reaction is reactant or product favoured?Q10) Express the relation among cell constant, the resistance of the solution in the cell and conductivity of solution.How is the conductivity of solution related to its molar conductivity?

2010 DQ28)(a)State Kohlrausch law of independent migration of ions.Write an expression for the molar conductivity of acetic acid at infinite dilution according to Kohlrausch law.(b)Calculate limiting molar conductivity for acetic acid. Given that limiting molar conductivity of HCl,NaCl,CH3COONa are 426,126,91 Scm2 mol-1 respectively. Q28)(a) Write the anode and cathode reactions and overall reactions occurring in a lead storage battery. (b )A Cu-Ag cell is set up [Cu2+]=0.1M [Ag+] is not known. The cell potential when measured was 0.422V.Determine the concentration of Ag+ ions in the cell.(Given E0Ag+/Ag = 0.80V, E0Cu2+/Cu = 0.34V)

2010 FQ9) Write the anode and cathode reactions occurring in a commonly used Hg – cell. How is the overall reaction represented?Q20)One Half cell in a voltaic cell is constructed from Ag wire dipped in AgNO3 solution of unknown concentration .The other half cell consists of Zn electrode in 0.1M solution of Zn(NO3)2.A voltage of 1.48V is measured for this cell.Calculate concentration of AgNO3 solution. (Given E0Ag+/Ag = 0.80V, E0Zn2+/Zn = - 0.763V)Q20) A voltaic cell is set up at 250C with the following half cells Al3+ (0.001M) and Ni2+ (0.5M) Write equation and determine Ecell. (Given E0Al3+/Al = -1.66 V, E0Ni2+/Ni = - 0.25V)

NEW SAMPLE PAPER IQ2) Write the product obtained at anode on electrolysis of conc. H2SO4 using Pt electrode.Q9) (i) For a weak electrolyte molar conductance in dilute solution increases sharply as the concentration in solution is decreased . Give reason.

(ii) Write overall cell reaction for lead storage battery when the battery is being charged.

Q19)(a)Calculate the charge in Coulombs required for oxidation of 2 moles of water to oxygen.(1 F = 96500 C/mol)

( b ) Zn/Hg oxide cell is used in hearing aids and electric watches.The following reactions occurZn(s) Zn2+ + 2 e E0Zn2+/Zn = - 0.76V)Hg2O+H2O + 2e 2Hg + 2OH- E0Hg+/Hg = - 0.344V)Calculate (i) standard potential of the cell(ii ) standard Gibb’s energy

NEW SAMPLE PAPER IIQ12) Describe the construction of a H2 –O2 fuel cell and the reactions taking place in it.Q12) Define the terms given below.

(a)Conductivity (b) molar conductivity Wh at are their units?

Q19) Give reasons: (a)Why does an alkaline medium inhibit the rusting of iron? (b) Why does a dry cell become dead after a long time even if it has not been used? ( c ) Why is Zn better than Sn in protecting iron from corrosion? NEW SAMPLE PAPER IIIQ28) (a) Two electrolytic cells containing AgNO3 solution and dil. HCl solution were connected in series A steady current of 2.5 A was passed through them till 1.078 g of Ag was deposited. [Ag = 107.8 g/mol, 1F = 96500 C]

(i) How much electricity was consumed?(ii) What was the weight of O2 gas liberated?

(b)Give reasons:(i) Rusting of iron pipe can be prevented by joining it with a piece

of Mg(ii) Conductivity of an electrolyte solution decreases with the

decrease in concentration.Q28)(a) What is a fuel cell? What is the main advantage?

( b ) What are the reactions occurring at the cathode and anode of a Lachlanche cell?(c) In a button cell widely used for watches and other devices the

following reactions takes placeZn(s)+Hg2O+H2O 2Hg + 2OH- + Zn2+

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)Hg2O+H2O + 2e 2Hg + 2OH- ( E0Hg+/Hg = - 0.344V) Zn2+ + 2 e Zn(s) ( E0Zn2+/Zn = - 0.76V)

2011 AIQ28) (a) What type of cell is a lead storage battery? Write the anode & cathode reaction & the overall reactions occurring in the use of a lead storage battery.(b ) Calculate the potential for half cell containing 0.1M K2Cr2O7 (aq) , 0.2M Cr3+(aq)and 1.0 x 10 -4 M H+.The half cell reaction is Cr2O7 2- (aq) + 14 H+(aq) + 6 e 2 Cr3+(aq) + 7 H2O(l)

And the standard electrode potential is given as E0 = 1.33VQ28) (a) How many moles ofHg will be produced by electrolyzing 1M Hg(NO3)2 solution with a current of 2 A for 3 hours? [Hg(NO3)2 = 200.6 g/mol](b) A voltaic cell is set up at 250C with the following half cells Al3+ (0.001M) and Ni2+ (0.5M) Write equation and determine Ecell. (Given E0Al3+/Al = -1.66 V, E0Ni2+/Ni = - 0.25V)2011 DQ2) Express the relation between conductivity and molar conductivity of a solution held in a cell’Q9) The chemistry of corrosion of iron is an electrochemical phenomenon. Explain the reactions occurring in the corrosion of iron in the atmosphere.Q10) Determine the value of Kc and ∆ G0 for Ni + 2Ag + Ni2+ + 2Ag (E0 cell = 1.05V)

2011 FQ11) Determine the value of Kc and ∆ G0 for Ni + 2Ag + Ni2+ + 2Ag (E0 cell = 1.05V)Q20) A voltaic cell is set up at 25 0C with the following half cells Al 3+ (0.001 M) and Ni2+ (0.5 M) Write the cell reaction and determine the cell potential. (E0 Ni2+/Ni = 0.258V , E0 Al3+ /Al = -1.66 V)

2010 D COMPTTQ28)(a) Explain why electrolysis of aq. solution of NaCl gives H2 at cathode and Cl2 at anode.Write overall reaction. ( E0 Na+/Na = - 2.71 V,E0 H2O/H2 = - 0.83 V, E0 Cl2/Cl- = + 1.36V, E0 H+/H2/H2O = + 1.23V)(b ) The resistance of a conductivity cell containing 0.001 M KCl solution at 298K is 1500 Ω Calculate the cell constant if conductivity of 0.001M KCl solution at 298 K is 0.146 x 10 -3 S/cm.Q28) (a) Calculate the emf for the given cell at 250C. Cr/Cr 3+ (0.1M)//Fe2+(0.01M)/Fe (E0 Cr3+/Cr = -0.74V , E0 Fe2+ /Fe = -0.44 V)(b ) Calculate the strength of the current required to deposit 1.2 g of Mg from molten MgCl2 in 1 hour.( 1F = 96500 C / mol , Mg = 24)

2010 AI COMPTTQ11) The molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9 S cm2 /mol Calculate the conductivity of solution.Q20)What is nickel-cadmium cell? State its one merit and one demerit over lead storage cell. Write the overall reaction that occurs during discharging of this cell.Q20)State and explain Kohlrausch law of independent migration of ions. How can the degree of dissociation of acetic acid be calculated from its molar conductance data.

2012 AI

Q9) express the relation among cell constant, resistance of the solution in the cell and conductivity of the solution. How is molar conductivity of a solution related to its conductivity?Q9) the molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9 Scm2 /mol. Calculate the conductivity of this solution.Q20) the electrical resistance of a column of 0.05 M NaOH solution of diameter 1 cm length 50 cm is 5.55 x 10 3 ohm. Calculate its resistivity, conductivity and molar conductivity.Q20) A voltaic cell is set up at 25 0C with the following half cells Al 3+ (0.001 M) and Ni2+ (0.5 M) Write the cell reaction and determine the cell potential. (E0 Ni2+/Ni =- 0.258V , E0 Al3+ /Al = -1.66 V)

2012DQ28)(a) What type of battery is the lead storage battery ?Write the anode and cathode reaction and the overall reaction occurring in a lead storage battery when current is drawn from it. (b)In the button cell, widely used in watches, the following reaction takes place. Zn +Ag2O + H2O Zn2+ + 2Ag + 2OH-

Determine E0 and ∆G0 for the reaction (E0 Ag+/Ag = +0.80V , E0 Zn2+ /Zn = -0.76 V)Q28)(a) Define molar conductivity of a solution and explain how molar conductivity changes with change in concentration of a solution for a weak and a strong electrolyte. (b)The resistance of a conductivity cell containing0.001M KCl solution at 298 K is 1500Ω.What is the cell constant if the conductivity of 0.001M KCl Solution at 298 K is 0.146 x 10 -3 Scm-1?

2012FQ28) (a) What type of battery is the lead storage battery ?Write the anode and cathode reaction and the overall reaction occurring in a lead storage battery when current is drawn from it. (b) A voltaic cell is set up at 250C with the Half cells Ag+ (0.001M)/Ag and Cu2+(0.1M)/Cu What should be its cell potential?(E0cell = 0.46V) Q28) (a) Define molar conductivity of a solution and explain how molar conductivity changes with change in concentration of a solution for a weak and a strong electrolyte.

(b)A strip of nickel metal is placed in a 1 molar solution of Ni(NO3)2 and a strip of silver metal is placed in a 1 molar solution of AgNO3.Anelectrochemical cell is created when the two solutions are

connected by a salt bridge and the two strips are connected by wires to volt meter.(i) Write the balanced equation for the overall reaction occurring in

the cell and calculate the cell potential.(ii)Calculate the cell potential,E at 250C for the cell, if the initial concentration of Ni(NO3)2 is 0.1 molar and the initial concentration of AgNO3 is 1 molar.

(E0 Ag+/Ag = +0.80V , E0 Ni2+/Ni = - 0.25V)

2013 AIQ11) the standard electrode potential (E0) for Daniell cell is +1.1 V. Calculate the ∆G 0 for the reaction Zn(s) + Cu 2+ Zn2+ + Cu(s) ( 1F = 96500 C mol-1)Q26 ) Calculate emf of the following cell at 25 0C Ag(s) /Ag + (10 -3M)// Cu 2+ (10 -1 M)/Cu (s) (Given E 0 Cell= + 0.46 V and log 10 n = n

Formulae

ELECTROCHEMISTRY:

NERNST EQUATION FOR HALF CELL:

E = E0 – 2.303RT log 1 nF [Mn+]

E = E0 – 0.059 log 1 nF [Mn+]

NERNST EQUATION FOR CELL POTENTIAL OR e.m.f. OF THE CELL:

E0cell = E0cathde - E0 anode

Zn / Zn 2+ // Cu 2+ / Cu R P R P Zn Zn 2+ + 2e Cu 2+ + 2e Cu Ecell = E0cell – 2.303RT log [Zn2+] 2F [Cu2+] Zn + Cu 2+ Zn 2+ + Cu

Mg / Mg 2+ // Cr3+ / Cr R P R P Mg Mg 2+ + 2e Cr 3+ + 3e Cr Ecell = E0cell – 2.303RT log [Mg 2+ ] 3

6F [Cr3+] 2 3Mg + 2Cr 3+ 3Mg2++2Cr

Pt /Br2 /Br- // H+ / H2 / Pt 2 Br - Br2 + 2e

P R R P 2H+ + 2e H2 Ecell = E0cell – 2.303RT log 1 2 Br- + 2H+ Br2 + H2 2 F [Br - ] [H+]2

Pt / I2 / I- // Cl - / Cl2 / Pt 2I - I2 + 2e

P R P R Cl2 + 2e 2Cl -

Ecell = E0cell – 2.303RT log [Cl - ] 2 2I- + Cl2 I2 + 2Cl- 2 F [I - ]2

EQUILIBRIUM CONSTANT Kc

Ecell = E0cell – 2.303RT log Kc nF

log Kc = E 0 cell x nF 2.303RT

∆G 0 = - n F E 0 cell

Λm = K x 1000 / C

K = CELL CONSTANT / RESISTANCE

CELL CONSTANT G* = CONDUCTIVITY x RESISTANCE

CELL CONSTANT = l /A

KOHLRAUSCH LAW: Λ 0

Λ 0 Al2(SO4)3 = 2 λ0 Al 3+ + 3 λ0 SO4 2-

Λ 0 CH3COOH = Λ 0 CH3COONa + Λ 0HCl - Λ 0NaCl DEGREE OF DISSOCIATION:

α = Λ / Λ 0

K = C α 2 / (1 – α)FARADAY’S LAW

ELECTRIC CHARGE REQUIRED IN F = 1F FOR Na+ , 2 F FOR Ca2+

MnO4 - Mn 2+ NEEDS 5 F .

Q = I * t

Question Bank

(Chemical Kinetics) 5 marks

SAMPLE PAPER- 1 (OLD)Q28) For a chemical reaction variation in the [R] t (first order graph ln log [R] t )

(i) What is the order of reaction(ii) What are the units of rate constant k(iii) Give the relationship between k & t ½(iv) What does the slope of the above line indicate? (v) Draw a plot log [R0]/[R] t

Q28) The reaction A+2B 2C+DExpt. [A]0 [B]0 Initial rate1 0.3 0.3 0.962 0.6 0.3 0.3843 0.3 0.6 0.1924 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

SAMPLE PAPER- 2 (OLD)Q10) Consider the reaction AP The change in concentration of A with time is shown (i)Predict the order of reaction(ii)Derive expression for the completion of the reaction

Q24) (a) 2N2O5 4NO2 + O2 is first order reaction with rate constant of 5x10-4 s-1.If initial concentration of N2O5 is 0.25M. Calculate its concentration after 2 min. Also calculate half life for decomposition of N2O5 (b)2A +B 3C The rate of appearance of C at time t is 1.3x10-4 mol/L/s Calculate at this time (i)rate of reaction (ii) rate of disappearance of A

SAMPLE PAPER- 3 (OLD)Q2) The decomposition reaction ofNH3 gas on Pt surface has a rate const. K = 2.5x10-4 mol /L/sWhat is the order of reaction?Q5) What is molecularity of the reaction Cl (g) ½ Cl2(g)Q20)(i) Graph of log[Ro]/[R] t is given for first order reaction (a) What is the relation between slope of this line & rate const. (b) Calculate the rate const. Of the above reaction if the slope is2x10 -4 s-1

(ii) Derive the relation between half life of a first order reaction & its rate

const.

2008 DQ2) Define the term order of reaction for chemical reactionQ12) A first order decomposition reaction takes 40 min. for 30% decomposition Calculate its t1/2 value.Q13) What is meant by the rate const.’k’of a reaction. If the concentration be expressed in mol/L units & time in sec.What would be the units for k (i) for a zero order reaction (ii) for a first order reactionQ28) (a) Derive the general form of the expression for the half life of a first order reaction

( 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

Q28) (a) List the factors on which the rate of a chemical reaction depends?( b) The half life for decay of radioactive C-14 is 5730 years An

archeological artifact containing wood has only 80% of C-14 activity is found in living trees. Calculate the age of the artifact.

2008 AIQ4) Define order of a reaction.Q9) List the factors which influence the rate of chemical reaction.

2008 FQ11) A reaction is second order w.r.t. A How is the rate of this reaction altered if the concentration of A is (i) doubled (ii) reduced to halfQ20) The rate of reaction increases to four times when the temp. is raised from 300K to320K Calculate Ea of this reaction (R = 8.314J/mol/K)

2008 D COMPTTQ10) Distinguish between order & molecularity of a reaction When could order & molecularity of a reaction be the same.Q21) The decomposition of PH3 4PH3 P4 + 6H2 has the rate law r = 6.0x10-4 s-1 & Ea is 3.05 x 105 J/mol Calculate k at 310 K (R = 8.314J/mol/K)Q17) List four factors which affect the rate of reaction.

2008 AI COMPTTQ11) Define order of reaction.How will you prove that a chemical reaction is of first orderQ10) For a chemical reaction what is the effect of catalyst on the following

(i) activation energy of the reaction(ii) rate const. of the reaction

Q21) For the reaction 2N2O5 4NO2 + O2 at 298 K

Sr.no. [N2O5] mol/L Rate of disappearance of N2O5(mol/L/min)

1 1.13 x10-2 34 x 10-5

2 0.84 x10-2 25 x 10-5

3 0.62 x10-2 18 x 10-5

Determine (i) order of reaction(ii)rate const.(iii) rate law

2009 AIQ10) Define (a) elementary step in a reaction

( b) rate of reactionQ19) A first order reaction has a rate const. of 0.0051 min-1 If we begin with 0.10 M concentration of reactant.What concentration of reactant will be left over after 3 hoursQ20) For a decomposition reaction the values of rate const. k at two different temp. are given below K1 = 2.15 x 10-8 L /mol/s at 650K K2= 2.39 x 10-7 L/mol/s at 700K Calculate Ea for this reaction (R = 8.314J/mol/K)Q14) Define activation energy of a reaction and order of reaction

2009 DQ9) A reaction is second order w.r.t. A How is the rate of this reaction altered if the concentration of A is (i) doubled (ii) reduced to half

2009 FAll Questions are repeated

2009 D COMPTTQ4) Why does the rate of a reaction not remain const. throughout the reaction ProcessQ16) Explain the term order of a reaction.Derive the unit for first order rate const.Q17) Show that for a first order reaction,the time required for half life period is independent f initial concentration.

2010 AIQ28) (a) Explain the terms: (i) Rate of reaction (ii) Activation energy of a reaction (b) The decomposition of PH3 proceeds according to the following equation. 4PH3 P4 + 6H2 It is found that the reaction follows the following rate equation Rate = k [PH3] The half life of PH3 is 39.9 s at120 0C

(i) How much time is required for 3/4th of PH3 to decompose? (ii) What fraction of the original sampeof PH3 remain behind after one minute.Q28) (a) Explain the terms: (i) Order of reaction (ii) molecularity of a reaction

( b) The rate of reaction increases four times when the temperature changes from 300K to 320 K Calculate Ea ,assuming that it does not change with temperature . ( R = 8.314J/K/mol)

2010 D

Q2) Define order of reactionQ10) A reaction is of first order in reactant A and second order in reactant B.How is the rate of this reaction affected when (i) [B] alone is increased to three times (ii) [A] as well as [B] are doubled.Q11)The rate constant for a reaction of zero order is 0.003mol/L/s.How long will it take for the initial concentration of A to fall from 0.1M to 0.075MQ2) Define rate of reaction.

2010 F Q2) Identify the order of reaction from the unit for rate constant L/mol/sQ10) Define (i) elementary reaction

NEW SAMPLE PAPER IQ3) For the reaction N2 + 3H2 2NH3 If ∆[NH3]/ ∆t = 4 x 10 -8 mol/L/s what is the value of -∆[H2]/ ∆tQ10)Sucrose decomposes in acid solution into glucose and fructose according to the first order rate law with t/2 = 3 hrs.Calculate the fraction of sucrose which remains after 8 hrs.Q10) The rate constant of a reaction at 500K and 700K are 0.02 /s and 0.07 /s resp.Calculate value of activation energy for the reaction (R = 8.314 J/mol/K)Q11) For a chemical reaction variation in the [R] t (first order graph ln [R] t )

(i) What is the order of reaction(ii) What are the units of rate constant k(iii) If the initial concentration of reactant is half of the original

concentration how will t/2 change? (iv) Draw a plot log [R0]/[R] t (s)

NEW SAMPLE PAPER IIQ30) (a) For the reaction C12H22O11 + H2O C6H12O6 + C6H12O6Write (i) Rate of reaction expression

( ii) Rate law equation( iii) molecularity

( iv) order of reaction( b) The following data were obtained during the first order thermal decomposition of SO2Cl2 at const. volume.SO2Cl2 (g) SO2(g) + Cl2(g)experiment Time (s) Total press. (atm)1 0 0.52 100 0.6Calculate the rate of reaction when total press. Is 0.65 atm.Q30) (a) Illustrate graphically the effect of catalyst on activation energy

( b ) Catalysts have no effect on equilibrium const. why?( c) The decomposition of A into product has value of K as 4.5 x 10 3

/s at 10 0 C and activation energy is 60 KJ/mol.Calculate the temp. at which the value of K be 1.5 x 10 4 /s

NEW SAMPLE PAPER III

Q13) Consider the decomposition of H2O2 in alkaline medium which is ctalysed by iodide ions. 2H2O2 2H2O + O2This reaction takes place in two steps as given belowStep I H2O2 + I- H2O + IO-

Step II H2O2 + IO- H2O + I- +O2(a)Write the rate law expression and determine the order of reaction w.r.t.

H2O2 (b)What is the molecularity of each individual step.

Q20)In a hydrolysis reaction 5 g ethyl acetate is hydrolysed in presence of dil. HCl in 300 min. If the reaction is of 1st order and the initial concentration of ethyl acetate 22 mol/L,Calculate the rate const. of the reaction.

2011 AIQ1)Define order of reaction.Q12) What do you understand by the rate law and the rate const. of a reaction?Identify the order of reaction if the units of its rate const. are

(i) mol/L/s (ii) L/mol/sQ13)The thermal decomposition of HCOOH is first order reaction with a rate const. of 2.4x10 -3 /s at a certain temp. Calculate how long will it take for 3/4th of inititial quantity of HCOOH to decompose. (log 0.25 = -0.6021)Q12)A reaction is of second order with respect to a reactant.How is the rate of reaction affected if the concentration of the reactant is reduced to half? What is the unit of rate const. for such a reaction?Q1)Define activation energy of a reaction.2011 DQ11)Distinguish between rate expression and rate constant of a reaction.Q20)2N2O5 4NO2 +O2The first order reaction was allowed to proceed at 40 0Cand the data below were collected.

[N2O5] M 0.4 0.289 0.209 0.151 0.109Time (min) 0 20 40 60 80

(a)Calculate the rate constant. Include units with your answer.(b)What will be the concentration of N2O5 after 100 min.(c) Calculate the initial rate of reaction.

2011FQ28) Repeated questionsQ28) Repeated questions

2010 D COMPTTQ4) Why does rate of reaction not remain constant throughout the reaction Process?Q16)Explain the term order of reaction Derive the unit for first order rate constant.Q17)Show that for the first order reaction the time required for half life period is independent of initial concentration.

2010 AI COMPTT

Q28) (a) Explain difference between the average rate and instantaneous rate of Reaction.(b ) In pseudo first order hydrolysis of ester in water, the following results are obtained.

T in seconds 0 30 60 90[Ester] M 0.55 0.31 0.17 0.085

(i) Calculate the average rate of reaction between time interval 30 to 60 seconds

(ii) Calculate the pseudo first order rate constant for the hydrolysis of ester.

Q28) (a) Distinguish between molecularity and order of reaction(b )The activation energy for the reaction 2 HI H2 + I2 is 209.5 kJ/mol at 581K.Calculate the fraction of molecules having energy equal to or greater than activation energy (R= 8.31 J/mol/K)

2012 AIQ10) A reaction is of second order with respect to a reactant.how is the rate affected if the concentration of the reactant is (i) doubled (ii) reduced to half?Q21) the reaction N2 + O2 ↔ 2 NO contributes to air pollution whenever a fuel is burnt in air at high temperature. At 1500 K, equilibrium constant K for it is

1.0 x 10 -5 . Suppose in a case [N2] = 0.80 mol/L and [O2] = 0.20 mol/L before any reaction occurs. Calculate the equilibrium concentrations of the reactants and the product after the mixture has been heated to 1500K.

2012 DQ10) What do you understand by the ‘order of a reaction’ ? Identify the reaction order from each of the following units of reaction rate constant:

(i) L-1mol s-1

(ii) L mol -1 s-1

Q21)For the reaction 2NO + Cl22NOClThe following data were collected .All the measurements were taken at 263K

Expt no. Initial [NO](M) Initial [Cl]2 (M) Initial rate of disappearance of Cl2 (M/min)

1 0.15 0.15 0.602 0.15 0.30 1.203 0.30 0.15 2.404 0.25 0.25 ?

(a)Write the expression for rate law.(b)Calculate the value of rate constant and specify its units.(c) What is the initial rate of disappearance of Cl2 in expt.4?

2012FQ10) Define the following terms:

(i) Order of reaction(ii) Activation energy of a reaction

Q21) Consider the reaction 2A + B C+ D

Following results were obtained in experiments designed to study the rate of reaction .

Expt. No. Initial concentration (mol/L) Initial rate of formation

[A] [B] [D] (M/min)1 0.1 0.1 1.5 x 10 -3

2 0.2 0.2 3.0 x 10-3

3 0.2 0.4 6.0 x 10 -3

(a)Write the rate law for the reaction(b)Calculate the value of rate constant for the reaction.(c) Which of the following possible reaction mechanism is consistent with

the rate law found in (a)?(i) A + B C + E (slow)

A + E D (fast)(ii) B C + E (slow)

A + E F (fast)A + F D (fast)

2013 AIQ12) (a) For a reaction A + B P , the rate law is given by, R = k [A]1/2[B]2 What is the order of this reaction?

( b ) A first order reaction is found to have a rate constant k=5.5 x 10 -14s-1 Find the half life of the reaction.

Q19) The rate of reaction becomes four times when the temperature changes from293 K to 313 K.Calculatethe energy of activation (Ea) of thereaction assuming that it does not change with temperature.[R = 8.314 J K -1, log4 = 0.6021]

FORMULAE:

i. Rate Expression: ii. rav = - ∆[R] / ∆t = + ∆ [P] / ∆tiii. r ins = - d[R] / ∆t = + d [P] / ∆tiv. RATE = - ∆[R] / ∆t = + ∆ [P] / ∆tv.

In aqueous solution change in concentration of H2O is not considered.vi. Rate law:

x and y are order of reaction7) order of reaction through initial rate method

r0) I = k [A]a [B]b [C]c

(r0)II = k [A]a [B]b [C]c

If [B ] and [C] kept constant value of a can be calculated. Similarly value of b and c can be calculated.

vii. Integrated rate equation :

For zero order reaction :

Unit of k = mol/l/s

For first order reaction :

Unit of k = /s

For nth order reaction :

Unit of k = (mol/L)1- n s -1

Activation Energy:

K = A e –Ea/RT

Question Bank

(Surface Chemistry) 4 marks

SAMPLE PAPER- 1 (OLD)Q21) Consider the adsorption isotherm given & interpret the variation in the extent of adsorption (x/m) when (a) (i) temp.increases at constant pressure ( ii) pressure increases at constant temp. (b)Name the catalyst& promoter used in Haber’s process for manufacture of NH3. Q1) Why is FeCl3 preferred over KCl in case of cut leading to bleeding?

SAMPLE PAPER- 2 (OLD)Q2) What are the physical states of dispersed phase & dispersion medium of froth?Q22) Explain: (a) Fe(OH)3 sol gets coagulated on addition of NaCl solution

( b) Cottrell’s smoke precipitator is fitted at the mouth of the chimney

used in factories. (c ) Physical adsorption is multi layered while chemisorption is mono layered

SAMPLE PAPER- 3 (OLD)Q11) (a) Adsorption of a gas on the surface of solid is generally accompanied by a decrease in entropy. Still it is a spontaneous process.Explain.

( b) How does an increase in temp. affect both physical as well as chemical adsorption

Q12) A collidal solution of AgI is prepared by two different methods shown below

(i) What is the charge of AgI colloidal particles in the two T.T.(A) & (B)

(ii) Give reasons for the origin of charge (A)AgNO3 added to KI (B) KI added to AgNO3

2008 DQ3) What causes Brownian movement in a colloidal solution?Q21) What are lyophilic & lyophobic sols? Give one example of each type which one of these two types of sols is easily coagulated & why?Q3) Which has a higher enthalpy of adsorption,physisorption or chemisorption?Q22) What is observed when (i) an electrolye KCl is added to hydrated ferric oxide sol.

(ii)an electric current is passed through a colloidal solution (iii)a beam of strong light is passed through a colloidal solution

2008 AIQ21) Differntiate between multimolecular & macromolecular colloids? Give one example of each. How are these two types of colloids different from associated colloids.Q3) Define electrophoresis briefly.

2008 .FAll question repeated

2008 D COMPTTQ2)Why does physisorption decrease withincrease in temp.?Q22) What is observed when (i) a beam of light is passed through colloidal Solution (ii)An elctrolyte NaCl is added to hydrated Fe2O3 sol

(iii) An electric current is passed through a colloidal solutionQ7) In chemisorption why x/m initially increases& then decreases with rise in temp.Q24) (a)What is the difference between a colloidal solution & an emulsion? Give one example of each (b) What are emulsifiers?

2008 AI COMPTTQ3) How does adsorption of a gas on a solid surface vary with increase in Pressure?Q20) Explain with example: (a) Peptization (ii) gel (iii) dialysisQ11) Distinguish between homogeneous & heterogeneous catalysis?What role does adsorption play in heterogeneous catalysis? Q12) Distinguish between micelles & colloidal particles. Give one example of each.

2009 AIQ2) What is the coagulation process?Q22)What happens in the following activities & why?

(i) An electrolyte is added to a hydrate ferric oxide sol in water(ii) A beam of light is passed through a colloidal solution(iii) An electric current is passed through a colloidal solution

2009 DQ2) Define the term Tyndall effect.Q22)How are the following colloids different from each other with respect of

dispersion medium & dispersed phase?Give one example of each type(i) an aerosol (ii) a hydrosol (iii) an emulsion

Q21) Differntiate between multimolecular & macromolecular colloids? Give one example of each. How are these two types of colloids different from associated colloids.

2009 FQ21) Write three special features of chemisorption which are not found in physisorption.

2009 D COMPTTQ3) Name two types of adsorption phenomenonQ18) How are associated colloids different frommacro molecular colloids? Give one example of each type.Q1) What is the sign of ∆H & ∆S when a gas is adsorbed by an adsorbent?Q9) What are emulsions? State one application of emulsificationQ14) What is the difference between a colloidal solution & emulsion? What is the role of emulsifier in forming emulsion

2010 AIQ12) Describe the following: (i) Tyndall effect (ii) Shape selective catalysisQ13) What is meant by coagulation of a colloidal solution? Name any method by which the coagulation of lyophobic sol can be carried out.Q13) Define the following terms:

(i) Peptization (ii) Reversible sol

2010 DQ3) What is an emulsion?Q21) Differntiate between multimolecular & macromolecular colloids? Give one example of each. How are these two types of colloids different from associated colloids.Q3) Give an example of shape selective catalyst.Q20) How are the following colloids different from each other in respect of their dispersion medium and dispersion phase?Give one example of each

(i) aerosol (ii) emulsion (iii) hydrosol

2010 FQ21)State what is observed when (i) an electrolyte NaCl is added to hydrated ferric oxide sol (ii) an electric current is passed through a colloidal solution

( iii )a beam of light is passed through colloidal solutionQ21) Write three features of chemisorptions which is not found in physisorption.Illustrate your answer with suitable example.

NEW SAMPLE PAPER IQ4) Which of the following is most effective electrolyte in coagulation of Fe2O3.H2O/Fe3+ sol KCl,AlCl3,MgCl2,K4[Fe(CN)6]Q20)Give reasons for the following observations:

(a)Peptizing agent is added to convert ppt into colloidal solution

(b)Cottrell’s smoke precipitator is fitted at the mouth of chimney used in factories

(c) Colloidal gold is used for intramuscular injection

NEW SAMPLE PAPER IIQ2) Name the type of potential difference produced between the fixed charged layer and and diffused layer having opposite charges around the colloidal particles.Q26) (a) Heat of adsorption is greater for chemisorption than physisorption why?

( b) What is colloidion( c) Differentiate betweenpeptization and coagulation.

NEW SAMPLE PAPER IIIQ2)Why is FeCl3 preferred over KCl in case of a cut leading to bleeding?Q27) (a) Give main difference between lyophilic and lyophobic colloids.

( b) Explain (i) sky appears blue in colour (ii) Afreshly formed ppt of Fe(OH)3 can be converted to a colloidal sol by shaking it with a small quantity of FeCl3.

20 11 AI Q2) What is meant by shape selective catalysis?Q20) Classify colloids where the dispersion medium is water.State their characteristics and write an example of each of these classesQ2) What is lyophobic colloid? Give one example for them.Q20) Explain what is observed when

(i) An electric current is passed through a sol(ii) A beam of light is passed through a sol(iii) An electrolyte (NaCl) is added to Fe(OH)3 sol.

20 11 D Q3) Define electrophoresis.Q21) Explain how the phenomenon of adsorption finds application in each of the Following

(i) Production of vacuum(ii) Heterogeneous catalysis(iii) Froth floatation process

Q21) Define each of the following(i) Micelles(ii) Peptization(iii) Desorption

20 11 F Q12) Repeated question.Q13) Repeated question.

2010D COMPTTQ7) What is the sign of ∆H and ∆S when gas is adsorbed by adsorbent?Q18) How are associated colloids different from macro molecular colloids? Give example of each type.Q9) What are emulsions? State one application of emulsificationQ14) What is the difference between colloidal solution and emulsion? What is the role of emulsifier in forming emulsion?

2010AI COMPTTQ3) What is the difference between adsorption and absorption ?Q21) Explain the following terms

(i) Electrophoresis(ii) Coagulation(iii) Tyndall effect

Q6) Distinguish between physisorption and chemisorptions.Q25) What is an adsorption isotherm? Describe Freundlich adsorption isotherm.Q3) Why is adsorption always exothermic?Q22) Discuss the effect of pressure and temperature on adsorption of gases on solids.Describe the application adsorption in controlling humidity.

2012 AIQ22) explain the following terms giving suitable example for each:

(i) Aerosol(ii) Emulsion(iii) Micelle

Q22) write three distinct features of chemisorptions which are not found in physisorptions.2012 DQ11) Name the two groups into which phenomenon of catalysis can be divided. Give an example of each group with the chemical equation involved.Q12) What is meant by coagulation of a colloidal solution? Describe briefly any three methods by which coagulation of lyophobic sols can be carried out.Q11) Describe a conspicuous change observed when

(a)A solution of NaCl is added to a sol of hydrated ferric oxide.(b)A beam of light is passed through a solution of NaCl and then through a

solQ12) Explain the following terms giving one example of each:

(i) Micelles(ii) Aerosol.

2012 FQ2)Why is the adsorption phenomenon always exothermic?Q22) Define the following terms giving one suitable example for each:

(i) Electrophoresis(ii) Micelles(iii) Peptization

Q2) What is meant by ‘shape selective catalysis’?Q22) Differentiate among a homogeneous solution, a suspension and a colloidal solution, giving a suitable example of each.Q22)Present a classification of colloids where dispersion medium is water.State the chatacteristics and one example of each of these classes.

2013 AIQ1) Of physisorption or chemisorptions , which has a higher enthalpy of formation?Q20) What are the characteristics of the following colloids? Give one example of each.

(i) Multimolecular colloids

(ii) Lyophobic sols(iii) Emulsions

Q19) define the following terms giving an example of each:(i) Associated colloids(ii) Lyophilic sol(iii) Adsorption

Q1) what is especially observed when a beam of light is passed through colloidal solutionQ19) define the following terms giving an example of each:

(i) Macromolecular sol(ii) Peptization(iii) Emulsion

Question Bank(General Principles & Processes of Isolation of Elements) 3 marksSAMPLE PAPER- 1 (OLD)Q22) Account for (a) the reduction of metalic oxide is easier if the metal formed is in liquid state at the temp. of reduction.

(b)the reduction of Cr2O3 with Al is thermodynamically feasible,yet it does not occur at room temp.

(c) Pine oil is used in froth floatation method

SAMPLE PAPER- 2 (OLD)Q1) An ore of sample Galena is contaminated with Zinc Blende.Name one chemical which is used to concentrate galena selectively by froth floatation methodQ11) ∆Gf for MgO & CO at 1273K & 2273K are given ∆Gf [MgO] = -941KJ/molat 1273K & ∆Gf [CO]= - 439KJ/mol ∆Gf [MgO] = -314 KJ/molat 2273K & ∆Gf [CO]= - 628 KJ/mol Predict the temp. at which C can be used as a reducing agent for MgO(s).

SAMPLE PAPER- 3 (OLD)Q21) (a) Name the method used for refining of (i) Ni (ii) Zr (b) The extraction of gold by leaching with NaCN involves both Oxidation & Reduction. Justify giving equation

2008 DQ22) State briefly the principles which serves as basis for the following operations in metallurgy

(I)Froth floatation process(ii)Zone refining

(iii )Refining by liquationQ21) Explain the basic principles(i) Vapour phase reefing(ii) Electrolytic refining(iii) Zone refining

2008 AIQ22) What chemical principle is involved in choosing a R.A. for getting the metal from its oxide ore? Consider the metallic oxide,Al2O3 & Fe2O3 & Justify the choice of R.A. in each case

2008 FQ23) Describe the role of (a) Depressant in Froth floatation process. (b) silica in the extraction of Cu from copper pyrite ore ( c ) Cryolite in the metallurgy of Al

2008 D COMPTTQ23) (a) The reaction Cr2O3 + 2Al Al2O3 + 2Cr , ∆G = -421KJ is thermodynamically feasible as is apparent from the Gibb’s energy value .Why does it not take place at room temp. (b) Write all the reactions involved in the extraction of Al from bauxite ore.Q22) (a)Write the reactions involved in the extraction of Fe from iron oxide ore in the blast furnace.

( b) What criterion is followed for the selection of stationary phase in Chromatography

2008 AI COMPTTQ13) State the basis of refining of a substance by chromatographic method. Under what Circumstances is this method specially useful.

2009 AIQ3)What is meant by the term Pyrometallurgy.Q11)Describe the underlying principle of the following metal refining methods.

(i) Electrlytic refining of metals(ii) Vapour phase refining of metals

Q13) Describe the role of following: (i) NaCN in the extraction of Ag from silver ore. (ii) Cryolite in the metallurgy of Al

2009 DQ3) Why is the froth floatation method selected for the concentration of sulphide ores.Q10) ( i) Explain the role of CO in purification of Ni (ii ) cryolite in the electrolytic reduction of alumina

2009 FQ9) Name two metals which occur in nature as oxides. Why is it that sulphide ores are concentrated by froth floatation process

2009 D COMPTTQ26) Reasons: (a) Alumina is dissolved in cryolite for electrolysis instead of being electrolysed directly (b)ZnO can be reduced to metal by heating with carbon but not Cr2O3( c ) Extraction of Cu directly from sulphide ore is less favourable than that from its oxide ore through reduction .

2010 AIQ21) Describe the role of following: (i) NaCN in the extraction of Ag from silver ore. (ii) I2 in the refining of Ti. (iii) Cryolite in the metallurgy of Al

Q21) Describe the principle involved in each of the following processes of metallurgy. (i) Froth floatation process (ii) Electrolytic refining of metals(iv) Zone refining of metals.

2010 DQ22) Describe how the following changes are brought about.

(i) Pig iron into steel(ii) ZnO into metallic zinc(iii) Impure Ti to pure Ti

Q22) Describe the role of (i) NaCN in the extraction of Au from Au ore(ii) SiO2 in the extraction of Cu from Cu matte(iii) I2 in the refining of Zr

Write equation for the involved reactions

2010 FQ21) Describe the method (i) Bauxite into pure alumina (ii)Impure Cu into pure Cu

NEW SAMPLE PAPER IQ21) (a) Extraction of gold by leaching with NaCN involves both oxidation and reduction.Justifying by giving equations for the reactions involved.

( b) Why is the froth floatation method selected for the concentration of sulphide ore?

Q21) outline the principle of the method used for refining of (a) Ni (b) Zr (c) TinQ5) Write the overall reaction taking place in the process used for electrolysis of alumina by Hall’s process.

NEW SAMPLE PAPER IIQ7) Write a non exothermic reaction taking place in the blast furnace during extraction of ironQ16) What is flux?What is the role of flux in the metallurgy of Fe and Cu.

NEW SAMPLE PAPER IIIQ14) (a) What is the role of depressant in the froth floatation process ( b ) Out of C and CO which is better R.A. for FeO

(i) In the lower part of blast furnace(high temp.)(ii) In the upper part of blast furnace (lower temp.)

2011 AIQ3) Differentiate between a mineral and an ore.Q14) Describe the principle controlling each of the following processes ( i) Vapour phase refining of Ti metal ( ii) Froth floatation method of concentration of a sulphide oreQ3) Why is that only sulphide ores are concentrated by Froth floatation process Q14) Describe the principle controlling each of the following processes(i) Zone refining of metals(ii) Electrolytic refining of metalsQ3) What type of ores can be concentrated by the magnetic separation methodQ14) Describe the principle controlling each of the following processes ( i) Preparation of cast iron from pig iron ( ii ) preparation of pure alumina from bauxite ore.

2011 DQ22) Repeated questionsQ22) Repeated questions

2011 FQ21) Repeated questionsQ21) Repeated questions

2010 D COMPTTQ26)Give reasons for the following

(i) Alumina is dissolved in cryolite for electrolysis instead of being electrolysed directly

(ii) Zinc oxide can be reduced to the metal by heating with carbon but not Cr2O3.

(iii) Extraction of copper directly from sulphide ores is less favourable tha that from its oxide ore through reduction.

2010 AI COMPTTQ4) Copper matte is charged into a silica lined convertor in extraction of copper. What is the role of silica lining there.Q12) How is the chemical reduction different from electrolytic reduction? Name a metal each which is obtained by

(i) Electrolytic reduction (ii) Chemical reduction.

Q12) How can you obtain pure alumina from bauxite ore? Write the chemical Equations involved.

2012 AIQ3) how is copper extracted from a low grade ore of it? Q11) which methods are usually employed for purifying the following metals:

(i) Nickel (ii) GermaniumMention the principle behind each one of them .

Q3) what is the role of collectors in Froth Floatation process?Q11) explain the role of each of the following:

(i) NaCN in the extraction of silver(ii) SiO2 in the extraction of copper.

2012 D Q2) What is the role of graphite in the electrometallurgy of aluminium?Q13) Describe the principle involved in each of the following processes.

(i) Mond process for refining of Nickel.(ii) Column chromatography for purification of rare elements.

Q13) Describe the following:(i) The role of cryolite in electrometallurgy of aluminium(ii) The role of CO in the refining of crude nickel.

Q3) Write the reaction involved in the extraction of silver after the silver ore has been leached with NaCN.Q11) Name one chief ore each of copper and aluminium. Name the method used for the concentration of these two ores.Q3)What is the role of depressant in Froth Floatation process for the concentration of a sulphide ore?

2013AIQ2) Name the method used for refining of copper metal.Q13) (a) Name the method used for removing gangue from sulphide ores.( b) How is wrought iron different from steel?Q18) outline the principles of refining of metals by the following methods:

(i) Zone refining(ii) Vapour phase refining

Q18) name the principal ore of aluminium. Explain the significance of leaching in the extraction of aluminium

Question Bank(The p-Block Elements) 8 marks

SAMPLE PAPER- 1 (OLD)Q25) Account for the following:

(i) Among the halogens F2 is the strongest O.A.(ii) F exhibit only –1 oxidation state whereas other halogens exhibit

higher positive oxidation state also(iii) Acidity of oxo acids of Cl is HOCl<HOClO<HOClO2<HOClO3

Q29)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.Q29) 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

SAMPLE PAPER- 2 (OLD)Q3) Complete hydrolysis of XeF6.Write equationQ8)Predict the shape of ClF3 on the basis of VSEPR theoryQ23) 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.

Q26) Give reasons: (a) CN- ion is known but CP- is not (b) NO2 dimerises to form N2O4 (c) ICl is more reactive than I2Q26) 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.

SAMPLE PAPER- 3 (OLD)Q7) 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

Q13) (a) What is the covalence of nitrogen in N2O5 (b) Explain why both N & Bi do not form pentahalides while P does.Q13) 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 (i) Identify the gases A& B (ii) Write the equations for the reactions involved.Q16) (a) 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

Q22) Write down the equations for hydrolysis of XeF4 & XeF6.Which of these two reactions is a redox reaction.

2008 DQ4) In which one of the two structures NO2+ & NO2-, the bond angle has a higher value? Q16) Reasons: (i) NH3 is stronger base than PH3 (ii) S in vapour state exhibits a paramagnetic behaviourQ17) Draw structures of (i) SF4 (ii) XeF4Q23) Write equations (i) Cl2 reacts with hot conc. soln. of NaOH

(ii)orthophosphorous acid is heated (iii)PtF6 & Xe are mixed together

Q23) Complete the equation: (i) Ca3P2 + H2O (ii) Cu2+ + NH3 (aq) (excess) (iii) F2 (g) + H2O (l) (iv)XeF4 + H2O (v)O3 + I- + H2O

2008 AIQ4) Why is the bond angle in PH3 molecule lesser than that in NH3 moleculeQ12) (i) which neutral molecule would be isoelectronic with ClO-

(ii)Of Bi (V) & Sb(V) which may be stronger O.A.& why?Q29) Reasons: (i) S in vapour state exhibits a paramagnetic behaviour (ii) NH3 has greater affinity for protons than PH3 (iii) The –ve value of electron gain enthalpy of F is less than that of Cl

(iv)SF6 is much less reactive than SF4 (v)Of the noble gases only Xe is known to form well established chemical compounds.

Q29) (a) Describe the favourable conditions for the manufacture of (i) NH3 by Haber’s process (ii) H2SO4 by Contact process

( b ) Draw the structures of (i) PCl5 (ii) S8 (iii) ClF3Q4) Which is a stronger acid in aq. Soln. of HF or HClQ12) 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)

Q30) ( a) complete (repeated) ( b )Draw structures of (i) H2S2O7(ii) NO3-

Q30) (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

(c) Draw the structures of (i) BrF3 (ii) XeF22008 FQ4)Which is stronger acid in aq.soln. HCl or HI?Q29) ( a )Complete : (repeated)

O3 + I- + H2O ( b )Draw the structures of (i) XeF4 (ii) H2S2O7( c ) Draw the structures of (i) HClO4 (ii)BrF32008 D COMPTTQ3) N does not form any pentahalide like P why?Q11) Reasons:(i) O2 molecule has formula O2 while S has S8

(ii) H2S is less acidic than H2TeQ29) (a) Arrange HClO,HClO2,HClO3,HClO4 in order of acidic strength. Give reason. (b)Write equation for Cl2 water reacts with conc. soln. of NaOH Justify that this is a disproportionation reaction. (c) Give one use of ClF3Q29) (a) Why do some noble gases form compounds with F & O only. (b) How are the following compounds prepared fro XeF6

(i) XeOF4 (ii)XeO3 (c) Draw structure of BrF3Q3) Why is N2 very unreactive as compared to P4Q4) When HCl reacts with finely powdered iron it forms FeCl2 & not FeCl3 why?Q22) (a) How are interhalogen compounds formulated & how are they prepared? (b) which neutral molecule would be isoelectronic with ClO-

Q23) (a) How does Xe atom forms compounds even though the Xe atom has a closed shell electronic configuration (b) Draw structures of XeOF4 (c) Complete XeF4 + H2O

2008 AI COMPTTQ5) F exhibits only –1 oxidation state in its compound whereas other halogens exhibit many other oxidation state why?Q24) (i) Draw structure of SO2 molecule .Comment. On the nature of two S-O bonds formed in it Are the two S-O bonds in this molecule equal?

( ii ) What happens when white P is heated with conc. NaOH soln.in an inert

gas atmosphere.Q1) Why are halogens mostly coloured?Q20) (i) Why is BiH3 the strongest R.A. among all the hydrides of gr 15 elements. (ii) H2O is liquid while H2S is a gas why? (iii) Why is Ka2<<Ka1 for H2SO4 in water

2009 AIQ4) Why is red P less reactive than white PQ12) Complete (i) XeF2 + H2O (ii) PH3 + HgCl2 Q29) (a)Draw structures of (i) H2S2O8(ii) HClO4 (b) How would you account for the following :

(i) NH3 is stronger base than PH3 (ii) F2 is a stronger O.A. than Cl2 (iii)S shows greater tendency for catenation than O.Q29) (a)Draw structures of (i) H2S2O7(ii) HClO3 (b) How would you account for the following :

(i) In the structure of HNO3 the N-O bond (121pm) is shorter than N-OH bond (140pm)

(ii) All P-Cl bonds in PCl5 are not equivalent.(iii) ICl is more reactive than I2

Q29)(a)Draw structures of (i) H3PO2(ii) BrF3 (b) How would you account for the following :

(i) No chemical compound of He is known(ii) Bond dissociation energy of F2 is less than that of Cl2(iii) P shows greater tendency for catenation than N.

Q30) (a)Draw structures of (i) H2S2O7(ii) XeF4 (b) How would you account for the following : (i) The –ve value of electron gain enthalpy is less for F than that for Cl (ii) F2 is a stronger O.A. than Cl2 (iii)HF has a much higher b.p. than HCl

2009 DQ21)(i)Why is Bi(V) stronger O.A. than Sb(V) (ii)Complete : P4 + NaOH + H2O

O3 + I- + H2O (iii)Draw structure of XeF4 , BrF3

Q23) Reasons:(i) NH3 is stronger base than PH3

(ii)S shows greater tendency for catenation than O.(iii)Bond dissociation energy of F2 is less than that of Cl2(iv) In the structure of HNO3 the N-O bond (121pm) is shorter than N-OH bond (140pm)

(v) SF4 is easily hydrolysed wheras SF6 is not(vi)XeF2 has a linear sructure & not a bent angular structure

Q24) Explain :(i) F does not exhibit any +ve oxidation state(ii) The majority of known noble gas compounds are those of Xe(iii) P is much more reactive than N

2009 FQ29) (a) Complete (i) XeF2 + PF5

(ii)Cl2 + NaOH (hot& conc.) (b) Explain(i) S in vap. State exhibit paramagnetism

(ii)+3 oxidation state becomes more & more stable from As to Bi in the group

Q29) Complete (i)PCl5 + H2O (excess) (ii) F2 + H2O

Reasons: (i) No chemical compound of He is known (ii)In soln of H2SO4 in water Ka2 is less than Ka1 (iii)P shows greater tendency for catenation than N.

Q30) Complete (i) SO2 + MnO4- + H2O (ii) HgCl2+ PH3Explain (i) S shows greater tendency for catenation than O. (ii) F is stronger O.A. than Cl

(iii)The + 5 oxidation state becomes less stable down the group in gr.15 of the Periodic Table.

Q30) (i) Complete (a) : P4 + NaOH + H2O (b) Cu + HNO3 (dil) (ii) Explain (a) H2O is liquid while H2S is a gas (b) Fe dissolves in HCl to form FeCl2 & not FeCl3 (c) He is used in diving equipments

2009 D COMPTTQ15) Write the formula & structure of noble gas species which are iso structural with ICl4- & BrO3- Q24)Reason (i) PH3 is weaker base than NH3

(ii)OF6 copound is not known (iii)F provides the largest variety of interhalogen compounds amongst the halogen

Q25) Write equation: (i) Cl2 + NaOH (hot & conc.) (ii)XeF6 + H2O (iii) NaOH +SO2(excess)

Q22) Reason : (i)In the solid state PCl5 behaves as an ionic species (ii) H2S is more acidic than water

(iii)N2 is not particularly reactive (iv)Halogens are stronger O.A. (v)SF6 is less reactive than SF4

(vi )F forms largest no. of interhalogen compounds amongst halogens.

Q26) Give reasons: (i) N2 is not particularly reactive(i) X2 are strong O.A.(ii) SF6 is less reactive than SF4.

2010 AIQ3) F does not exhibit any + ve oxidation state Why?Q14) Complete (i) I2 + HNO3 (conc) (ii) HgCl2 + PH3 Q15) Draw structures of (i) H4P2O5 (ii) XeF4Q25) Account for the following: (i) NCl3 is an endothermic compound while NF3 is an exothermic one (ii) XeF2 is a linear molecule without a bend.

(iii) The electron gain enthalpy with – ve sign of F is less than that of Cl still F2 is strong O.A. than Cl2.

Q2)N2 is relatively inert as compared to P4 Why?Q15) Complete (i) NaOH (cold & dil.) + Cl2 (ii) XeF6 + H2O (excess) Q22) Account for the following:

(i) The electron gain enthalpy with – ve sign is less for O than that of S.

(ii) P shows greater tendency for catenation than N(iii) F never acts as a central atom in polyatomic interhalogen

compounds.

2010 DQ4)Why does NO2 dimerise?Q12 )Draw the structure of white and red phosphorous.Which one of these two types of phosphorous is more reactive and why?Q29) ( a )Complete the following:

1. NaOH (hot and conc.) + Cl2 2. XeF6 + H2O( b ) How would you account for the following:( i ) The value of EGE with –ve sign of S is higher than that of O( ii ) NF3 is exothermic but NCl3 is endothermic.

( iii ) ClF3 molecule has T shaped structure and not a triangular planar one.

Q29) ( a) Complete the following: ( i) P4 + SOCl2 (ii) XeF4 + H2O ( b ) Explain the following giving reason ( i ) The stability of +5 oxidation state decreases down the group in gr. 15 of the P.T. ( ii ) Solid PCl5 behaves as an ionic compound. ( iii ) Halogens are strong oxidizing agent.Q4)What is O.N. of P in H3PO2 moleculeQ12) Draw structure of ( i) BrF3 ( ii ) XeF4Q4) Draw structure of O3 molecule.

2010 FQ4) Which is stronger acid in aq. Solution HCl or HI and why?Q12) Draw structures of (i) BrF3 (ii) XeOF4Q29) (a) Complete (i) HgCl2 +PH3 (ii) SiO2 + HF ( b) Explain (i) S in vapour state exhibit paramagnetic behavior

(ii) The stability of +3 state increasesdown the gr.in gr. 15 of the P.T.(iii) XeF2 has a linear shape and not a bent structure

Q29 ) (a) Complete (i) AgCl + NH3 (ii) P4 + NaOH + H2O ( b ) Explain (i)H2S is less acidic thanH2Te ( ii) F2 is stronger O.A. thanCl2( iii ) Noble gases are least reactive elements.Q9) Draw structures of O3 and S8 molecules.Q12) Draw structures of XeF2 and HClO4 molecules.

NEW SAMPLE PAPER IQ6) Which Xe compound is isostructural with ICl4- ?

Q12)(i) Draw structure of phosphinic acid(H3PO2)( ii) Write a chemical reaction for its use as a reducing agent.

Q13) ( a) Suggest a quantitative method for estimation of gas which protect us from uv rays of the sun

( b)Nitrogen oxides emitted from the exhaust system of supersonic jet aeroplanes slowly deplete the concentration of O3 layer in the upper atmosphere.Comment.

Q22) Write equation for the following reaction( a) thermal decomposition of (NH4)2Cr2O7( b) reactionof Cl2 with cold and hot dil.NaOH( c) when phosphine is passed through HgCl2 solution

NEW SAMPLE PAPER IIQ4) Which of the following compounds has a lone pair of electron at the central atom? H2S2O8,H2S2O7,H2SO3,H2SO4Q14) Give chemical reaction in support of the following observations ( a) H2SO4 has low volatility. ( b) I- can be oxidized by O2 in acidic mediumQ28)(a) An orange solid A on heating gives a colourless gas B.The gas B in dry condition is passed over heated Ca to give a solid C.The solid C further reacts with water to produce a gas D which forms a blue coloured

compound E on reaction with CuSO4 solution.Identify A,B,C,D,E and give the sequence of reactions involved. ( b) Arrange the following in order of property indicated for each set ( i) HCl,HI,HBr,HF (decreasing thermal stability) ( ii) Xe,He,Kr,Rn,Ne (decreasing order of EGE)Q28) (a) Give reasons: ( i) solid PCl5 is an ionic compound.

(ii ) Most of the reactions of F are exothermic.( iii) O3 is thermodynamically unstable.

( b) Draw the structure of the following. ( i) XeOF4 ( ii) H4P2O7

NEW SAMPLE PAPER IIIQ15) Complete the following:(a)(NH4)2Cr2O7 on heat (b)I- + O3 +H2O Q19) Draw the structures (a) H2S2O8 (b)XeO3 ( c) HOClO2Q26) Give reasons: ( a) Interhalogen compounds are more reactive thn halogens( b) PCl5 is known but NCl5 is not known.( c) Among all the noble gasesonly Xe is known to form compounds with O and F

2011 AIQ21) How would you account for the following: ( i) H2S is more acidic than H2O. ( ii) The N-O bond in NO2– is shorter than N-O bond in NO3-

(iii ) Both O2 and F2 stabilize high oxidation states but the ability of O2 to stabilize the higher oxidation state exceeds that of F2Q29) ( a) Draw the structures of the following molecules.

(i) (HPO3)3 (ii) BrF3( b) Complete the following equations(i) HgCl2 + PH3 (ii) SO3 + H2SO4 (iii) XeF4 + H2O

Q29) ( a) (i) Cl2 gas is passed through a hot concentrated solution of NaOH (ii ) SO2 gas is passed through an aqueous solution of a Fe 3+ salt( b) Answer thefollowing:(i) What is the basicity of H3PO3 and why?(ii) Why does F not play the role of central atom in interhalogen

compounds(iii) Why do noble gases have very low b.p.?

Q21) Account for the following:(i) NF3 is an exothermic compound but nCl3 is not(ii) The acidic strength of compounds increasesin the order PH3 < H2S<

HCl(iii) SF6 is kinetically inert.

2011 DQ4) Draw the structure of XeF2 moleculeQ12) Repeated questionQ12) Repeated questionQ30) (a) Explain

(i) NF3 is an exothermic compound whereas NCl3 is not(ii) F2 is more reactive of all the four common halogens

(b ) Complete

(i) C + conc. H2SO4 (ii) P4 + NaOH + H2O (iii) Ci2 + F2(excess)

Q30)(a) Account for the following:(i) The acidic strength decreases in the order HCl>H2S>PH3(ii) Tendency to form pentahalides decreases down the group in group

15 of the periodic table(b) Complete the following equations:(i) P4 + SO2Cl2 (ii) XeF2 + H2O (iii) I2 + HNO3 (conc.)

Q4) draw the structure of XeF4 molecule.Q4) draw the structure of BrF3 molecule.

2011 FQ14) how would you account for the following:

(i) The following order of increase in strength of acids:PH3<H2S<HCl

(ii) The oxidizing power of oxoacids of chlorine follows the order:HClO4 < HClO3 <HClO2 <HClO

Q22)complete the following chemical equations:(i) NaOH (hot and conc.)+ Cl2 (ii) XeF4 + O2F2 at 143 K (iii) Br2 + F2 (excess)

Q23) (a) Mention the optimum conditions for the industrial manufacture of ammonia by Haber’s process.(b) Explain the following giving appropriate reasons: (i)sulphur vapour exhibits paramagnetic behavior. (ii) red phosphorus is less reactive than white phosphorus.Q23)draw the structures of the following molecules:

(i) NF3(ii) H2S2O8(iii) H3PO3

Q22) Complete the following chemical equations:(i) P4 + SO2Cl2 (ii) Fe3+ + SO2 + H2O (iii) XeF6 + H2O (excess)

Q14) Explain giving a reason each for the following situation:(i) In aqueous medium HCl is stronger acid than HF(ii) White phosphorus is more reactive than red phosphorus.

Q22) complete the following chemical equations:(i) C + H2SO4 (conc.) (ii) P4 + NaOH +H2O (iii) Cl2 + F2 (excess)

2010 D COMPTTQ15)write the formulae and the structures of noble gas species which are isostructural with (i)ICl4- (ii) BrO3-

Q24) give reasons for the following:(i) PH3 is weaker base than NH3 (ii) OF6 compound is not known(iii) Fluorine provides the largest variety of interhalogen compounds

amongst the halogens.Q25) Write the balanced equations for the following reactions.

(i) Chlorine is passed through hot concentrated NaOH solution.(ii) XeF6 is hydrolysed.(iii) Excess of SO2 reacts with NaOH solution

Q25) arrange the following in order of the property mentioned:(i) PH3 ,NH3,SbH3,AsH3 (increasing basic strength)(ii) HCl,HBr,HI,HF (increasing acidic strength)(iii) HClO4,HClO, HClO2 (increasing oxidizing power)

Q12) draw structure and predict the shape of (i) H3PO3 (ii) XeOF4Q22) suggest the possible reason for the following observations:

(i) In the solid state , PCl5 behaves as an ionic species.(ii) H2S is more acidic than water(iii) Fluorine forms the largest number of interhalogen compounds

amongst the halogens.Q17) draw the structure and predict the shape of (i) XeO3 (ii) BrF3Q26) give reasons for the following:

(i) N2 is not particularly reactive(ii) Halogens are strong oxidizing agents(iii) SF6 is less reactive thanSF4

2010 AI COMPTT:Q5) what is the covalence of nitrogen in N2O5?Q6) why are the two S –O bonds in SO2 molecule of equal strength?Q22) answer the following:

(a)Complete the equation XeF6 + H2O (excess) (b)What happens when H3PO3 is heated?(c) Why is ICl more reactive than I2?

Q23) account for the following:(i) Halogens are coloured(ii) Nitrogen shows weaker tendency for catenation than phosphorus(iii) H2S is less acidic than H2Te

Q4) why are pentahalides of metals more covalent than its trihalides?Q23) account for the following:

(i) Halogensare strong oxidizing agents.(ii) NH3 is clearly basic while PH3 is feebly basic.(iii) Oxygen is involved in hydrogen bondingwhile chlorine is not.

Q1) why is BiH3 the strongest reducing agent amongst the hydrides of group 15 elements?Q20) account for the following:

(i) Unlike other halogens , fluorine forms only one oxoacid ,HOF(ii) Nitrogen exist as a diatomic molecule whereas phosphorus exist as

P4(iii) the two S –O bonds in SO2 molecule are equal .

2012 AIQ4) which is stronger reducing agent , SbH3 or BiH3, and why?Q12) explain the following facts giving appropriate reason in each case:

(i) NF3 is an exothermic compound whereas NCl3 is not.(ii) All the bonds in SF4 are not equivalent.

Q29) (a) Draw the molecular structures of the following compounds:(i) N2O5(ii) XeOF4(b) explain the following observations:(i) sulphur has a greater tendency for catenation than oxygen.(ii) ICl is more reactive than I2.(iii) Despite lower value of its electron gain enthalpy with negative

sign,F2 is a stronger oxidizing agent than Cl2.Q29)(a) complete the following observations:

(i) Cu + HNO3 (dilute) (ii) XeF4 + O2F2 (b) explain the following observations:

(i) phosphorus has a greater tendency for catenation than nitrogen.(ii) oxygen is a gas but sulphur is a solid(iii) The halogens are coloured. Why?

Q30) (a) Draw the molecular structures of the following compounds:(i) H3PO2(ii) ClF3(b) explain the following observations:(i) nitrogen is much less reactive than phosphorus.(ii) despite having greater polarity,HF boils at a lower temperature than water.(iii) sulphur has a greater tendency for catenation than oxygen in the

same group.Q30) (a) Draw the molecular structures of the following compounds:

(i) N2O5(ii) HClO4(b) explain the following observations:(i) H2S is more acidic than H2O.(ii) Fluorine does not exhibit any positive oxidation state.(iii) Helium forms no real chemical compound.

Q4) what is the basicity of H3PO2 acid and why?

2012 DQ3) Which one of PCl4 + and PCl4 – is not likely to exist and why?Q14) Explain the following giving an appropriate reason in each case.

(i) O2 and F2 both stabilize higher oxidation states of metals but O2 exceeds F2 in doing so.

(ii) Structures of Xenon fluorides can not be explained by Valence Bond approach.

Q29) (a) Complete the following chemical reaction equations:(i) P4 + SO2Cl2 (ii) XeF6 + H2O (b) Predict the shape and angle(900 or more or less) in each of the following cases:(i) SO32- and the angle O-S-O(ii) ClF3 and the angle F-Cl-F(iii) XeF2 and the angle F- Xe –F

Q29) (a) Complete the following chemical equation:(i) NaOH + Cl2

(hot and conc.)(ii) XeF4 + O2F2

(b) Drawthe structures of the following molecules:(i) H3PO2(ii) H2S2O7(iii) XeOF4

Q3) Of PH3 and H2S which is more acidic and why?Q30)(a) Draw molecular structures of following compounds:

(i) XeF6 (ii) H2S2O8

(b) Explain the following observations:(i) The molecules NH3 and NF3 have dipole moments which are of opposite direction.(ii) All the bonds in PCl5 molecules are not equivalent.(iii) S in vapour state exhibits paramagnetism.

Q30) (a) Complete the following chemical equations:(i) XeF4 + SbF5 (ii) Cl2 + F2 (excess)

(b) Explain each of the following:

(i)Nitrogen is much less reactive than phosphorus(ii) The stability of +5 oxidation state decreases down group 15

(iii) The bond angles (O-N-O) are not of the same value in NO2- and NO2+

Q4) Although the H –bonding in HF is much stronger than that in water,yet water has a much higher b.p. than HF. Why?Q12) Explain the following:

(i) The chemical reactivity ofnitrogen is much less thanthat of phosphorus.

(ii) SF6 is kinetically inert.Q13) Draw the molecular structures of the following:

(i) H3PO3(ii) BrF3

Q23) Complete the following chemical equations:(i) NH4Cl + NaNO2 (ii) P4 + NaOH + H2O (iii) Xe + F2 (at 673K,1bar)

Q4)Which is more acidic and why,H2O or H2S?Q13)Draw the molecular structures of the following:(i) H2S2O8(ii) XeF2Q23)Complete the following chemical equations:(i) HgCl2 + PH3 (ii) NaOH + Cl2

(hot and conc.)(iii) XeF4 + O2F2 Q4)Which is stronger acid in aqueous solution,HF or HCl, and why?Q12) State a reason for each of the following:(i) F never exhibits any positive oxidation state.(ii) He does not form any real chemical compound.Q23) Complete the following chemical equations:

(i) Sn + 2PCl5 (heat) (ii) Fe3+ + SO2 +H2O (iii) XeF2 + H2O

2013 AIQ2) Name two poisonous gases which can be prepared from chlorine gas.Q14) Draw the structures of the following molecules:

(i) XeOF4 (ii) H3PO3Q15) How are interhalogen compounds formed? What general compositions can be assigned to them?Q21) give reasons for the following:

(i) Where R is an alkyl group,R3P = O exist but R3N=O does not(ii) PbCl4 is more covalent than PbCl2(iii) At room temperature , N2 is much less reactive.

Q2) which aerosol depletes ozone layer?Q14) Draw the structures of the following molecules:

(i) XeF6 (ii) H2S2O7Q27) give reasons for the following:

(i) Oxygen is a gas but sulphur is a solid(ii) O3 acts as a powerful oxidizing agent (iii) BiH3 is the strongest reducing agent amongstall the hydrides of

group 15 elements.Q2) what is the basicity of H3PO3 and why?Q21) give reasons for the following:

(i) Though nitrogen exhibits +5 oxidation state, it does not form pentahalide.

(ii) Electron gain enthalpy with negative sign of fluorine is less than that of chlorine.

(iii) The two oxygen-oxygen bond length in ozone molecule are identical.

Question Bank

(The d & f – Block elements) 5 marksSAMPLE PAPER- 1 (OLD)Q14) A mixed oxide of Fe & Cr,Cr2O3 is fused with Na2CO3 in the presence of air to form a yellow compound (A), On acidification the compound (A) forms an orange coloured compound (B) which is strong O.A. Identify ( i ) the compounds (A) & (B)(ii)Write balanced equation for each step.Q23) Explain (a) Transition metals act as catalyst (b) Cr group elements have highest m.p. in their respective series. (c ) Transition metals form coloured complexes

SAMPLE PAPER- 2 (OLD)Q30) (a)A blackish brown coloured solid A when fused with alkali metal hydroxide in presence of air produces a dark green coloured compound B which on electrolytic oxidation in alkaline medium gives a dark purple compound C.Identify A,B,C& write the reactions involved. (b) What happens when an acidic solution of green compound B is allowed to stand for sometime? Give the equation involved What is this type of reaction called?Q30) Reasons: (a) T.E. have high enthalpy of atomization (b) Among the lanthanoids,Ce(III) is easily oxidized to Ce(IV) (c ) Fe 3+ /Fe 2+ redox couple has less +ve electrode potential than Mn 3+ / Mn 2+ couple (d)Cu (I) has d10 configuration while Cu (II) has d 9 configuration ,still Cu (II) is more stable in aq. solution than Cu (I).

(e)The second & third transition series elements have almost similar atomic radii.

SAMPLE PAPER- 3 (OLD)Q29) (a) Out of Ag2SO4,CuF2,MgF2& CuCl. Which compound will be coloured & why? (b) Explain: (i) CrO4 2- is strong O.A.while MnO42- not.

(ii) Zr & Hf have identical sizes (iii)The lowest oxidation state of Mn is basic while the highest is acidic (iv)Mn (II) shows maximum paramagnetic character amongst the divalent ions of the first transition series.

Q29) (a) In the titration of FeSO4 withKMnO4 in the acidic medium,why is dil. H2SO4used instead of HCl? ( b) Reasons: (i) Among transition metals the highest oxidation state is

exhibited in oxoanions of a metal (ii)T.E. form a no. of interstitial compounds. (iii)Zn2+ salts are white while Cu2+ salts are blue (iv)Ce4+ is used as an O.A. in volumetric analysis

2008 DQ29)Reasons: (i) T.E. & many of their compounds act as a good catalyst. (ii)Actinoid contraction is greater than lanthanoid contraction (iii)The E0 value for Mn 3+ / Mn 2+ couple is much more +ve than that for

Cr 3+ / Cr 2+. (iv)Sc(21) does not exhibit variable oxidation state & yet it is regarded as a T.E. (v) With d4 configuration , Cr2+ act as a R.A. but Mn3+ acts as an O.A.

Q29)(a) What may be the possible oxidation state of T.E. with the following d electronic configuration in the ground state of their atoms 3d34S2,3d54S2& 3d64S2.Indicate relative stability of oxidation state in each case.(b) Write the steps involved in the preparation of (i)Na2CrO4 from chromite ore (ii) K2MnO4 from pyrolusite ore

2008 AIQ13) Complete the equations(i) oxidation of Fe2+ by Cr2O72-in acidic medium (ii) oxidation of S2O32- by MnO4- in neutral aq. mediumQ23) Reason: (i) The T.E.generally form coloured compounds (ii) With 3d4 configuration,Cr2+ act as a R.A.but Mn3+ act as an O.A. (at. Mass Cr=24, Mn=25) (iii )The actinoids exhibit a larger no. of oxidation state than the corresponding lanthanoids.

2008 FQ13) Compare the relative stability of +2 oxidation state in aq. Solution for the metals having their atoms the outer configuration 3d34S2,3d54S2& 3d64S2

Q23) (a) Complete (i) Cr2O72- + H+ + Fe2+ (ii)MnO4- + I- + H+ (b) How many unpaired electrons are present in Mn2+ ion?How does it influence mag.behaviourof Mn2+ ions?

2008 D COMPTTQ12) Reasons(i)There are irregularities in the e.c. of actinoids.

(ii) Compounds of T.E. are often colouredQ24) (a) Describe the commercial preparation of KmnO4 from pyrolusite ore.

( b ) Write ionic equation to represent the reaction of acidified KmnO4 solution with oxalic acid.

Q15)Reasons: (a) T.E. are well known to form complex compounds ( b )The second & third members in Each group of T.E. have very similar at. RadiiQ12) Reasons: Why do d block elements generally exhibit large no. of oxidation states than those exhibited by the f block elements

2008 AI COMPTTQ29) Reasons: (i) The actinoids exhibit a larger no. of oxidation state as compared to Lanthanoids in general.

( ii) Though a T.E. (Sc=21) does not exhibit variable oxidation state.( b) (i) Describe how K2Cr2O7 is prepared from chromate

(ii)The colour of K2 Cr2O7 solution changes with change in pH of solution Q29) (a) On what ground can you say thatSc(21) is a T.E. but Zn(30) is not?

( b)Use Hund’s rule to derive the e.c. of Ce3+ ion & calculate its magnetic moment by using ‘spin only’formula (Ce=58)

( c )What is lanthanoid contraction & what are its consequences?

2009 AIQ13) Complete the following reactions:

(i) MnO4- + C2O42- + H+ (ii) Cr2O72- + H+ + Fe2+

Q25) How would you account for the following(i) Many of the T,E. and their compounds can act as good catalyst.(ii) The metallic radii of the5 d series of T.E. are virtually the same as

those of the corresponding members of the 4 d series.(iii) There is greater range of oxidation state among the actinoids than the

lanthanoids.

2009 DQ29) (a)Complete the equations:

(i) MnO4- + C2O42- + H+ (ii) Cr2O72- + H+ + Fe2+( b) Explain

(i)There is general increase in the density of elements from Ti to Cu

(ii)There occurs much more frequent M-M bonding in compounds of T.E. (3rd series)

(iii) The members in the actinoid series exhibit a large no. of oxidation states than the corresponding members in the lanthanoid series.

Q29) (a)Complete the equations: (i) Cr2O72- + H+ +H2S (ii)MnO4- + S2O32- + H2O ( b) Explain: (i)The gradual decrease in size in actinoid contraction from element to element is greater among the actinoids than that among the lanthanoids

(ii)The greatest no. of oxidation states are exhibited by members in the middle of a transition series.

(iii) With the same d orbitals (d4) Cr2+ Is a R.A. but Mn3+ ion is an O.A.Q28)( a) Complete the equations: (i) Cr2O72- + H+ + I-

(ii)MnO4- + Fe2+ + H+ ( b) Explain 1.T.E. are known to form many interstitial compounds 2. The enthalpy of atomization of T.E. are quite high. 3. T.E. formcoloured compounds 4. T.E. exhibit variable oxidation state.

Q28) Explain : (i) In general the atomic radii of T.E. decrease with at.no. in a given series. (ii ) E0 M 2+/ M for Cu is 0.34V It is the only metal in 3 d series showing this type of behaviour. ( iii) E0 value for Mn3+/Mn2+ couple is much more +ve than for Cr3+/Cr2+ or Fe3+/Fe2+ couple

Q28) (a ) What is meant by lanthanoid contraction?what is it due to and what consequences does it have on the chemistry of elements following lanthanoid in the P.T. ( b) Explain (i) Cu+ ion is unstable in aq.solution

(ii)although Co2+ ion appears to be stable ,it is oxidized to Co3+ ion in presence of strong ligand. (iii)E0Mn 2+ / Mn value for Mn is much more than expected from the trend for other elements in the series.

2009 FQ13) Reason:

(i) The enthalpy of atomization of T,E. are quite high’(ii) There isa greater horizontal similarity in the property ofT.E. than that of the main gr.

Elements.Q23) Explain :

(i) With the same d orbitals (d4) Cr2+ Is a R.A. but Mn3+ ion is an O.A.(ii) Cu+ ion is unstable in aq.solution(iii) Among 3d series of T.E. the largest no. of oxidation states are

exhibited by Mn

Q13) Complete:(i)MnO4- + Fe2+ + H+ (ii)Cr2O72- + C2O42- + H+

2009 D COMPTTQ29)Reasons:

( a) (i) Cu+ ion is unstable in aq.solution (ii)Mn2+ ion shows maximum paramagnetic character amongst the bivalent ions of 3d series (iii)Sc salts are white.( b) Describe the reactions involved in the preparation of K2Cr2O7 from chromite oreQ29)(a) Describe the following for first series of T.E. and their trends (i) at.radii (ii) oxidation states ( iii) I.E.( b) Name an important alloy which contains some of the lanthanoid metals.Mention its two uses.

2010 AIQ29) (a)Complete the equations: (i) Cr2O7 2- + H2S + H+ (ii) Cu2+ + I - ( b) Account for the following:(i) The oxidizing power of oxoanins are in the order VO2 + < Cr2O7 2- <

MnO4-

(ii) The third ionization enthalpy of Mn (25) is exceptionally high.(iii) Cr 2+ is a stronger R.A. than Fe 2+

Q29) (a)Complete the equations: (i) Cr2O7 2- + Fe 2+ + H+ (ii) ( b) Explain the following:

(i) La 3+ (57) and Lu 3+ (71) do not show any colour in solution(ii) Among the divalent cations in the first series of T.E. , Mn exhibits

the maximum paramagnetism.(iii) Cu + is not known in aqueous solution.

2010 DQ13) Explain

(i) Generally there is increase in density of elements from Ti-22 to Cu-29 in the first series of T.E.

(ii) T.E. and their compounds are generally found to be good catalysts in chemical reaction.

Q23) How would you account for the following(i) The at. Radii of elements of the 5 d series of T.E. arevirtually the

same as those of the corresponding members of 4 d series.(ii) E0 value for Mn3+/Mn2+ couple is much more +ve than for

Cr3+/Cr2+ or Fe3+/Fe2+ couple(iii) The highest oxidation state of ametal is exhibited in its oxide or

fluorideQ13) Explain:

(i) The T.E. generally form coloured compounds(ii) Zn is not regarded as a T.E.

2010 FQ13)Describe preparation of (i) K2Cr2O7 from Na2CrO4(ii) KMnO4 from K2MnO4Q22)Explain:

(i) The enthalpy of atomization of transition metals are quite high(ii) There is close similarity in physical and chemical property of 4d and

5 d series of the T.E. much more than expected on the basis of usual family relationship.

(iii)The members in the actinoid series exhibit large no. of oxidation state than the corresponding member in the lanthanoid series.

Q22) Explain:(i) The T.E. have great tendencyfor complex formation(ii) There is a gradual decrease in the atomic size of T.E. in a series with

increasing at.no.(iii)La and Lu do not show colouration in the solution.(at.no La = 57,Lu = 71)

NEW SAMPLE PAPER IQ29) (a) (i) Which is stronger R.A.Cr2+ or Fe2+ and why? (ii)Explain why Cu+ ion is not stable in aq. soln.

(iii) Explai why Ce4+ is a strong O.A.( b) Descrb the oxidizing property of KMnO4 in neutral or faintly alkaline medium for its reaction with I- ions and S2O32- ions

Q29) (a) Account for the following(i) Oxidising power in the series VO2+ <Cr2O72-<MnO4-(ii) Actinoid contraction is greater from element to element than

lanthanoid contraction(iii) Oxoanions of a metal show higher oxidation state. ( b) What is Misch metal?Give its one use.

NEW SAMPLE PAPER IIQ17)The sum of IE1 and IE2 ,IE3 and IE4 of Ni and Pt are

IE1+IE2 (MJ/mol) IE3+IE4 (MJ/mol)Ni 2.49 8.80Pt 2.66 6.70

Based on the above informations answer the following:(a)Which is the most oxidation state for Ni and Pt?Why?(b)Out of the two,name the metal which can easily form compounds in +4

oxidation state and why?Q22)Write chemical equation for the following reactions:

(a)Oxidation of NO2- ion by MnO4- in acidic medium(b)Acidification ofK2Cr2O7 solution(c) Disproportionation of Mn(VI) in acidic solution

Q22)Account for the followinh:(a)Eu(II) is more stable than Ce(II)(b)T.E. have high enthalpy of atomization(c) Actinoids are generally coloured.

Q29) Explain:(a)Actinoids show large number of oxidation states(b)T.E. form large number of complexes(c) Cr is typical hard metalwhile He is liquid(d)MnO is basic while Mn2O3 is acidic in nature(e)Ag is transition metal but Zn is not

Q29)(a) Give two consequences of lanthanoid contraction.(b)Complete the following reactions:

(i) MnO4- + S2O32- + H2O(ii) Cr2O72- + H+ + Sn2+ (c)Which of the following has maximum number of unpaired electrons? Ti3+,V2+,Fe2+,Mg2+

(d)Based on the data arrange Fe2+,Mn2+ and Cr2+ in the increasing order of stability of +2 oxidation stateE0Cr3+/Cr2+ = -0.4V,E0Mn3+/Mn2+ = 1.5V,E0Fe3+/Fe2+ = 0.80

2011 AIQ4) What is meant by Lanthanoid contraction?Q15)How would you account for the following:

(i) Cr2+ is reducing in nature while with the same d orbital configuration (d4) Mn3+ is an O.A.

(ii) In a transition series of metals,the metal which exhibits the greatest no. of oxidation state occurs in the middle of the series.

Q16) Complete the following:(i) MnO4- + S2O32- + H2O(ii) Cr2O72- + H+ + Fe2+

Q16) State reasons(i) Cu(I) ion is not stable in an aq. solution.(ii) Unlike Cr3+,Mn2+,Fe3+ and the subsequent other M2+ ions of the

3d series of elements,the rd and the 5d seriesmetals generally do not form stable cationic species.

Q15) Give reasons:(i) Transition metals and their compounds are generally found to be

good catalyst(ii) Metal-Metal bonding is more frequent for the 4d and the 5d series of

treansition metals than that of the 3d series.Q5)What is meant by lanthanoid contraction?Q15)Explain giving reasons:

(i) Transition metals and their compounds generally exhibit a paramagnetic behavior

(ii) The chemistry of actinoids is not smooth as that of lanthanoids.Q16)Complete the following equations

(i)MnO4- + S2O32- + H2O (ii) Cr2O72- + H+ + Fe2+

Q16)Reasons:(i) Cu(I) ion is not stable in an aq. solution.(ii) Unlike Cr3+,Mn2+,Fe3+ and the subsequent other M2+ ions of the

3d series of elements,the rd and the 5d series metals generally do not form stable cationic species.

2011DQ13)assign reason for the following:

(i) Copper(I) ion is not known in aqueous solution(ii) Actinoids exhibit greater range of oxidation states than lanthanoids.

Q23) complete the following chemical equations:(i) Cr2O7 2- + H2S + H+ (ii) KMnO4 (heated)(iii) MnO4- + C2O42- + H+

Q13)assign reason for each of the following:(i) Transition metals generally form coloured compounds.(ii) Mn exhibits the highest oxidation state of +7 among the 3d series of

transition elements.

2011 FQ29) (a) complete the following Reactions in aqueous medium:

(i) Cr2O7 2- + H2S + H+ (ii) MnO4- + C2O42- + H+ (b ) how would you account for the following:(i) Metal-metal bonding is more extensive in the 4d and 5d series of

transition elements than the 3d series.(ii) Mn(III) undergoes disproportionation reaction easily(iii) Co(II) is easily oxidised in the presence of strong ligands.

Q29)(a) complete the following chemical equations:(i) Fe3+ + I - (ii) CrO42- + H+ (b ) explain the following:(i) Copper(I) ion is not known in aqueous solution(ii) With d4 configuration Cr(II) is reducing whereas Mn(III) is oxidizing(iii) Transition metals in general act as good catalysts

2010D COMPTTQ29)(a) give reasons for the following observations:

(i) Copper(I) ion is not known in aqueous solution(ii) Mn(II) ion shows maximum paramagnetic character amonst the

bivalent ions of first transition series.(iii) Sc(21) salts are white.(b ) Describe the reactions involved in the preparation of K2Cr2O7 from chromite ore

Q29) (a) Describe the following characteristics of the first series of the transition metals and their trends in the series (Sc to Zn)(i) Atomic radii (ii) oxidation states (iii) ionization enthalpies(c) Name the important alloy which contains some of the lanthanoid

metals. Mention its two uses.2010 AI COMPTT:Q29) (a) write the electronic configuration of Ce3+ion,and calculate the magnetic moment on the basis of spin – only formula.(Ce = 58)(b) account for the following:(i) the enthalpy of atomization of the transition metals are high.(ii) the lowest oxide of a transition metal is basic, the highest is amphoteric /acidic.

(iii) Co(II) is stable in aqueous solution but in the presence of complexing agents,it is easily oxidizedQ29)(a) how does the acidified potassium permanganate solution react with (i)iron (II) ions and

(ii) Oxalic acid?Write the ionic equations for the reactions.(b )name the oxometal anion of the transition metals in which the metal exhibits the oxidation state equal to group number.(c ) account for the following:(i) Sc (21) is regarded asa transition element but Zn(30) is not.(ii) E0(M2+/M) value for copper is +ve.

2012 AIQ13) complete the following chemical reaction equations:

(i) Cr2O72- + I- + H+ (ii) MnO4 - + NO2 - +H+

Q23)how would you account for the following:(i) Among lanthanoids, Ln (III) compounds are predominant.

However,occasionally in solutions or in solid compounds, +2 and +4 ions are obtained.

(ii) The E0M2+ /M for copper is positive (0.34V). copper is the only metal in the first series of transition elements showing this behavior.

(iii) The metallic radii of the third (5d) series of transition metals are nearly the same as those of the corresponding members of the second series.

Q23) explain the following observations:(i) Many of the transition elements are known to form interstitial

compounds.(ii) There is a general increase in density from Ti (Z=22)to

copper(Z=29)(iii) The members of the actinoid series exhibit a larger number of

oxidation states than the corresponding members of the lanthanoid series.

Q23) explain the following observations:(i) With the same d- orbital configuration (d4) , Cr2+ is a reducing agent

while Mn3+ is an oxidizing agent.(ii) Actinoids exhibit a much larger number of oxidation states than the

lanthanoids.(iii) There is hardly any increase in atomic size with increasing atomic

numbers in a series of transition metals.2012 DQ15) Complete the following equations:

(i) Cr2O72- + I- + H+ (ii) MnO4 - + NO2 - +H+

Q22) How would you account for the following:(i) Many of T.E. are known to form interstitial compounds.(ii) The metallic radii of the third (5d) series of transition metals are

virtually the same as those of the corresponding group members of the second (4d) series.

(iii) Lanthanoids form primarily +3 ions , while the actinoids usually have higher oxidation states in their compounds,+4 or even +6 being typical.

Q23)How would you account for the following :(i) With the same d- orbital configuration (d4) Cr2+ is a reducing agent

while Mn3+ is an oxidizing agent.

(ii) The actinoids exhibit a large no. of oxidation states than the corresponding members in the lanthanoid series.

(iii) Most of the transition metal ions exhibit characteristic in colours in aq. solution.

Q22)Explain the following observations giving an appropriate reason for each.

(i) The enthalpies of atomization of transition elements are quite high.(ii) There occur much more frequent metal-metal bonding in

compoundsof heavy transition metals.(iii) Mn2+ is much more resistant than Fe2+ towards oxidation.

2012FQ29)(a) Complete and balance the following chemical equation:

(i) Cr2O72- + I- + H+ (ii) MnO4 - + SO3 2- +H+

(b) Explain the following observations:(i) The transition elements and their compounds are known to act as catalyst.(ii) The higher oxidation states are usually exhibited by the members in the middle of a series of transition elements.

(iii) The metal-metal bonding is more frequently found with the second and third series of transition elements.

Q29) Calculate the number of unpaired electrons in the following gaseous state ions: Mn2+,Cr3+,V3+ and Fe2+. Which one of these is the most stable in aqueous solution? (at.no. V=23,Cr=24,Mn=25,Fe=26)(b) Explain the following observations:

(i)The transition metal ions are usually coloured in aq. solution. (ii) Cu(I) is not stable in an aq.solution.

(iv) The highest oxidation state of a transition metal is exhibited in its oxide or fluoride.

2013 AIQ29) (a) give reasons for the following:

(i) Mn3+ is a good oxidizing agent.(ii) E0 M2+/M values are not regular for first row transition metals (3d

series)(iii) Although F is more electronegative than O , the highest Mn fluoride

is MnF4, whereasthe heist oxide is Mn2O7.( b ) Complete the following equations:(i) 2CrO4 2- + 2 H+ (ii) KMnO4 on heating

Q29) (a) Why do transition elements show variable oxidation states?(i) Name the element showing maximum number of oxidation states

among the first series of transition metals from Sc (Z=21) to Zn (Z = 30)

(ii) Name the element which shows only +3 oxidation state.( b ) What is lanthanoid contraction? Name an important alloy which contains some of lanthanoid metals.

Question Bank

(Co ordination compounds ) 3 marks

SAMPLE PAPER- 1 (OLD)Q2) Why dos a tetrahedral complex of type [MA2B2] not show geometrical isomerism?Q13) A metal ion Mn+ having d4 valence electronic configuration combines with three didentate ligands to form a complex compound Assuming ∆o >P

(i) Draw diagram showing d orbital splitting during this complex formation

(ii) Write the electronic configuration of valence electron of metal Mn+ in in terms of t2g & eg.

(iii) What type of hybridization will Mn+ ion have?(iv) Name the type of isomerism exhibited by this complex.

SAMPLE PAPER- 2 (OLD)Q21) (a) Give IUPAC name of [CrCl2(H2O)4]Cl (b) Give the no. of unpaired electrons in [FeF6]4- & [Fe(CN)6]4-

(c ) Name the isomerism. [Co(NH3)5Br]SO4 & [Co(NH3)5 SO4]Br Give the chemical test to distinguish between these two compounds.

SAMPLE PAPER- 3 (OLD)Q23) Give the e.c. of the

(a)d orbitals of Ti in[Ti(H2O)6]3+ ion in an octahedral crystal field.(b)Why is this complex coloured? Explain on the basis of distribution of

electron in the d orbitals?(c) How does he colour change on heating [Ti(H2O)6]3+ ion?

2008 DQ24) (a) What is a ligand? Give an example of bidentate ligand. (b) Explain as to how the two complexes of Ni, [Ni(CN)4]2- & Ni(CO)4 have different structures but do not differ in their magnetic behaviour.[Ni = 28]

2008 AIQ24) (a)What is the basis of formation of the electrochemical series? (b) Draw the structures of the geometrical isomers of following [Co(NH3)3Cl3] & [CoCl2(en)2]+

2008 FQ24) Describe the limitations of V.B. theory.

2008 D COMPTTQ4) Write IUPAC name of[CoCl(NO2)(NH3)4]ClQ13) Using V.B. approach , deduce the shape & magnetic character of [Co(NH3)6]3+ ion (Co =27)

2008 AI COMPTTQ5) Write IUPAC name of[Co(NH3)6] [Cr(CN)6]Q1) Write IUPAC name of[Cu(NH3)4] [PtCl4]Q24) (a)Draw the structure & write the hybridization of Co in cis-[Co(NH3)4Cl2]+

(b)Write IUPAC name of[Co(NH3)4Cl(ONO)]Cl

2009 AIQ23) Giving example for each, explain the following

(i) Crystal field splitting

(ii) Linkage isomerism(iii) Ambidentate ligand

Q23) Compare the following complexes with respect to structural shapes of units,magnetic behaviour & hybrid orbitals involved in units [Co(NH3)6]3+ , [Cr(NH3)6]3+,Ni(CO)4 (Co=27,Cr=24,NI=28)Q23) Explain (i) Low spin octahedral complexes of Ni are not known. (ii) The∏ complexes are known for transition elements only

(iii)CO is stronger ligand than NH3 for many metals.Q23) Compare the following complexes with respect to structural shapes of units,magnetic behaviour & hybrid orbitals involved in units (i) [Ni(CN)4]2- (ii) [NiCl4]2- (iii) [CoF6]3-

2009 DQ23) For the complex [Fe(en)2Cl2]Cl Identify

a) Oxidation no. of Fe.b) Hybrid orbitals & shape of complexc) Magnetic behaviour of complexd) No. of geometrical isomerse) Whether there is an optical isomer alsof) Name of the complex

Q24) Compare the following complexes with respect to structural shapes,magnetic behavior & hybridization (i) [CoF4]2- (ii) [Cr(H2O)2(C2O4)]- (iii) [Fe(CN)6]4-

2009 FQ24) Three geometrical isomers are possible for [Co(en)(H2O)2(NH3)2]3+. Draw molecular structures of these three isomers & indicate which one of them is chiralQ24) Compare with respect to molecular shape and magnetic behavior(i) [Cr(NH3)6]3+ (ii)[Fe(CN)6]4- (iii) [NiCl4]2-

Q24) Explain giving example( i ) Linkage isomerism (ii) Outer orbital complex (iii) A bidentate ligand

2009 D COMPTTQ24)(a) Square planar complexes of (MX2L2Type) with C.N. of 4 exhibit geometrical isomerism whereas tetrahedral complexes with similar composition do not why? (b)Describe the type of structural shapes ,magnetic behaviour & hybridization of [Co(NH3)4Cl2]Cl (at.no of Co =27)

2010 AIQ 22) Reasons : (i) Ni does not form low spin octahedral complexes. (ii) The∏ complexes are known for the T.E. only. (iii) Co 2+ is easily oxidized to Co 3+ in the presence of strong ligand.Q25 ) Write the name , the state of hybridization , shape and the magnetic behaviour of the following :(i) [CoCl4] 2- , [Ni(CN)4] 2- ,[Cr(H2O)2 (C2O4)2 ] –

(at. No. Co = 27 , Ni = 28 , Cr = 24)

2010 DQ5)Give an example of linkage isomerism.

Q14)Name the following coordination compounds according to IUPAC system of nomenclature:

(i) [Co(NH3)4(H2O)Cl]Cl2(ii) [CrCl2(en)2]Cl

Q5)Describe the shape and magnetic behavior of following complexes:(i) [Co(NH3)6]3+(ii) [Ni(CN)4]2-

Q5)Give an example of ionization isomerism.

2010 FQ5) What is an ambidentate ligand? Give an example.Q14)Describe the state of hybridization,shape and magnetic behaviour of

(i) [Cr(H2O)2(C2O4)2]-(ii) [Co(NH3)2(en)2]3+

Q4) Give an example of coordination isomerism.

NEW SAMPLE PAPER IQ7)What happens to the colour of coordination compound [Ti(H2O)6]Cl3 when heated gradually?Q14)(a) Give e.c. of d orbitals of Ti in [Ti(H2O)6]3+ ion and explain why this complex is coloured? (Ti = 22)(b) Write IUPAC name of [Cr(NH3)3(H2O)3]Cl3

NEW SAMPLE PAPER IIQ27)(a) State the hybridization and magnetic behavior of [Cr(CO)6]( b)What are the factors affecting crystal field splitting energy?(c) Which of the two is more stable and why? K4[Fe(CN)6] or K3[Fe(CN)6]NEW SAMPLE PAPER IIIQ16) Using Valence bond theory, predict the geometry and magnetic character of [NiCl4]2-. (Ni = 28)

2011 AIQ22)Explain the following terms giving suitable example in each case.

(i) Ambident ligand(ii) Denticity of ligand(iii) Crystal splitting in an octahedral field

Q22)Write the structures and name of all the stereoisomers of the following compounds.

(i) [Co(en)3]Cl3 (ii)[Pt(NH3)2Cl2] (iii)[Fe(NH3)4Cl2]ClQ22) Write the state of hybridization,the shape and magnetic behavior of(i) [Cr(NH3)4Cl2]Cl(ii) [Co(en)3]Cl3(iii) K2[Ni(CN)4]

2011 DQ24) write the name,stereochemistry and magnetic behavior of the following:(Mn =25,Co=27,Ni=28)

(i) K4[Mn(CN)6](ii) [Co(NH3)5Cl]Cl2(iii) K2[Ni(CN)4]

Q24) for the complex [Fe(en)2Cl2]Cl , identify the following:(i) Oxidation number of iron(ii) Hybrid orbitals and shape of the complex(iii) Magnetic behavior of the complex(iv) Number of its geometrical isomers

(v) Whether there may be optical isomer also(vi) Name the complex.

2011 FQ3)what do you understand by denticity of a ligand?Q15) name the following coordination compounds and draw their structures:

(i) [CoCl2(en)2]Cl(ii) [Pt(NH3)2Cl(NO2)]

(Co=27,Pt=78)Q3) why is CO a stronger ligand than Cl- ?Q17) draw the structures of isomers ,if any, and write the names of the following complexes:

(i) [Cr(NH3)4Cl2]+

(ii) [Co(en)3]3+

(Cr=24,Co=27)Q3)name the following coordination compound: K3[CrF6]Q15) give the name ,the stereochemistry and the magnetic behavior of the following complexes:

(i) [Co(NH3)5Cl]Cl2(ii) K2[Ni(CN)4]

2010DCOMPTTQ23)(a) square planar complexes(of MX2L2 type) with coordination number of 4 exhibit geometrical isomerism whereas tetrahedral complexes with similar composition, do not. why?(b)describe the type of hybridization,shape and magnetic property of [Co(NH3)4Cl2]Cl (Co=27)2010AICOMPTTQ24) write the IUPAC name and deduce the geometry and magnetic behavior of the complex K4[Mn(CN)6] (Mn=25)2012 AIQ24) name the following coordination entities and draw the structures of their stereo isomers:

(i) [Co(en)2Cl2]+(ii) [Cr(C2O4)3]3-(iii) [Co(NH3)3Cl3]( atomic no. Cr = 24 , Co = 27)

Q24) name the following coordination entities and draw the structures :(i) [Fe(CN)6]4 –(ii) [Cr(NH3)4Cl2]+(iii) [Ni(CN)4]2-

(atomic no. Fe = 26, Cr = 24, Ni = 28)2012DQ23) Give the formula of each of the following coordination entities.

(i) Co3+ ion is bound to one Cl- , one NH3 molecule and two bidentate ethylene diamine molecules

(ii) Ni2+ ion is bound to two water molecules and two oxalate ions.Write the name and magnetic behavior of each of the above coordination entities.(at.no.Co=27,Ni=28)

Q22) State reasons for each of the following situations:(i) Co2+ is easily oxidized to Co3+ in presenceof strong ligand(ii) CO is a stronger complexing reagent than NH3

(iii) The molecular shape of Ni(CO)4 is not same as that of [Ni(CN)4]2-Q23) write the name,the structure and the magnetic behavior of each one of the following complexes:

(i) [Pt(NH3)2Cl(NO2)](ii) [Co(NH3)4Cl2]Cl(iii) [Ni(CO)4]

(at.no. Co=27,Ni=28,Pt=78)2012FQ24) Explain the following:

(i) The ∏ complexes are known for transition elements only.(ii) Nickel(II) does not form low spin octahedral complexes.(iii) [Fe(CN)6]4- and [Fe(H2O)6]2+ are of different colours in dilute

solutions.Q24) Name the following complexes and draw the structures of one possible isomer of each:

(i) [Cr(C2O4)3]3-(ii) [Pt(NH3)2Cl2](iii) [Co(en)2Cl2]+

2013 AIQ22) For the complex [NiCl4]2- , write

(i) The IUPAC name.(ii) The hybridization type.(iii) The shape of the complex

(Atomic no. of Ni =28)Q22) what is meant by crystal field splitting energy? On the basis of crystal field theory ,write the electronic configuration of d4 in terms of t2g and eg in an octahedral field when

(i) ∆o > P(ii) ∆o < P

Question Bank

(Haloalkanes & Haloarenes) 4 marksIUPACQ1) IUPAC name of CH3CH=C(CH3)CH(Br)CH3Q2) IUPAC name of CH3CH=C(CH3)CH2BrQ3) IUPAC name of CH3C(CH3)=C(Br)CH2OHQ4) IUPAC name of CH3CH=CHCH2BrQ5) IUPAC name of

Q6) Draw the structure of following compound. 4-Bromo-3-methylpent-2-eneQ7) Draw the structure of following compound. 1-Bromo-4-sec-butyl-2-methyl benzeneQ8) IUPAC name of CH2=CHCH2BrQ9)CH3CH=C(CH3)CH2Br

MECHANISMQ1) An optically active compound having M.F.C7H5Br reacts with aq.KOH to give racemic mixture of products. Write the mechanism.Q2) Discuss the mechanism of SN1 reaction of haloalkanes Q3) Suggest a possible mechanism for the following

n-BuBr + KCN (ethanol/H2O n-BuCNQ4) How would you differentiate between SN1 and SN2 mechanism of substitution reaction ? Give one example of each.Q5)Propose mechanism of the reaction taking place when

(i) (-)-2-Bromooctane reacts with NaOH to form(+)-octan-2-ol(ii) 2- Bromopentane is heated with alc. KOH to form alkenes

REASONSQ1) Explain as to why haloarenes are much less reactive than haloalkanes Towards Nucleophilic substitution reaction.Q2) Which compound in the following pairs will react faster in SN2 reaction with –OH & why?(i)CH3Br or CH3I (ii) (CH3)3CCl or CH3ClQ3) Which compound in the following pairs will undergo SN2 reaction faster why?C6H11CH2Cl or C6H11Cl Q4) (i)Why is it that haloalkanes are more reactive than haloarenes towards nucleophile. (ii) Which one of the following reacts faster in SN1 reaction & why? CH3CH2C(Cl)CH2CH3 or CH3CH2CH2CH2Cl, Q5)Reason: (a) The order of reactivity of haloalkane is RI > RBr>RCl (b)Neopentylchloride does not follow SN2 mechanismQ6)(a)Which of the following compounds would react faster by SN2 path (1-Bromobutane or 2-Bromobutane) &why? (b)Allyl chloride is more reactive than n- propyl chloride towards nucleophilic substance reaction explain why? ( c ) Haloalkanes react with KCN to give alkyl cyanide as main product while with AgCN they form isocyanide as main product. Give reason.Q7) (a) Which will have a higher b.p. 1-chloropentane or 2-chloro-2-methyl butane

(b)Give reason:p- nitrochlorobenzene undergoes nucleophilic substitution faster than chlorobenzene.Explain giving the resonating structures as well.

Q8)Answer(i)Identify chiral in CH3CHOHCH2CH3 and CH3CHOHCH3(ii)Among the following compounds which one is more easily hydrolysed and why?CH3CHClCH2CH3 or CH3CH2CH2CH2Cl(iii)Which of these will react faster in SN2 displacement and why? 1-Bromopentane or 2-BromopentaneQ9)Which is more easily hydrolysed by KOH and why? CH3CHClCH2CH3 or CH3CH2CH2CH2ClQ10)Account for the following:

(i)Chloromethane reacts with AgCN to form methyl isocyanide as chief product(ii) Use of DDT was banned in United States in 1973(iii)Benzyl halides show high reactivity towards SN1 reaction

Q11)Iodoform has antiseptic property.Give reason to support this.

CONVERSION/WORD PROBLEMQ1)How will you bring about following conversion Methyl bromide to methyl iodide.

COMPLETE EQUATIONSQ1) Complete C6H5 CH=CH2 + HBrQ2)Write the main product

(i) (CH3)2CHCl + Na (dry ether ) (ii)CH3Br + AgF + Heat

(i) CH3CH2Br + NaI (dry acetone)(ii) C6H5N2Cl + Cu/HCl (iii)Complete CH3CH2CH=CH2 + HBr (peroxide)

Q3) Complete the reaction: (i) C6H5N2Cl + KI (ii) CH2=CH2 + Br2 (CCl4)

(i) C6H11OH + SOCl2 Q4) Write the major product

(i)CH3CH=C(CH3)2 + HBr (ii) C6H5ONa + C2H5Cl

Q5)Complete the reaction CH3CH=CH2 + HBr (peroxide) X +NaI(acetone)Y

QUESTIONQ1) In each of the following pairs of organic compounds. Identify the compound which will undergo SN1 reaction faster? (a) (CH3)3Cl & CH3CH2CH(Cl)CH3

(a)C6H5Cl & C6H5CH2ClQ2) The treatment of an alkyl chloride with aq. KOH leads to the formation of an Alcohol whereas in the presence ofalc.KOH , alkene is the major product.Q3) A solution of KOH hydrolyses CH3CHClCH2CH3 and CH3CH2CH2CH2Cl Which will be hydrolysed easily?Q4)(i) State one use of each DDT and Iodoform

(ii) Which couple reacts faster in SN2 displacement and why?(a)1-Bromopentane or 2-Bromopentane(b) 1-Bromo-2-methyl butane or 2-Bromo-2-methyl butane

Q5) Explain:(i)G.R. should be prepared under anhydrous condition.(ii)C6H5CHClCH3 is hydrolysed more easily with KOH than C6H5CH2Cl.

Q6)Arrange the following in the decrease order of reactivity towards SN2 displacement reaction and give reason in support of your answer.(i) C2H5Br ,C2H5I ,C2H5Cl.(ii)(CH3)3CBr ,CH3CH2CHBrCH3 , CH3CH2CH2CH2BrQ7)Rearrange the compounds of each of following set in order of reactivity towards SN2 displacement(i)2-Bromo-2-methylbutane , 1-Bromopentane ,2-Bromopentane(ii) 1-Bromo-3-methyl butane , 2-Bromo-2-methyl butane , 3-Bromo-2-methyl Butane(iii)1-Bromo butane ,1-Bromo-2,2-dimethyl propane ,1-Bromo-2-methyl butane

NAME REACTIONS

DISTINGUISHING TEST

2011 DQ5) write the IUPAC name of (CH3)3CCH2BrQ25) answer the following:

(i) Haloalkanes easily dissolve in organic solvent, why?(ii) What is known as a racemic mixture? give an example.(iii) Of the two bromoderivatives,C6H5CH(CH3)Br and C6H5CH(C6H5)Br

which on is more reactive in SN1 substitution reaction and why?

2011 FQ4) which will react faster in SN2 displacement,1-bromopentane or

2- Bromopentane and why?Q24) complete the following reaction equation:

(i) 1-Methylcyclohexene + HI (ii) C6H5 CH = CH2 + HBr (iii) CH3CH2CH =CH2 + HBr

2010 D COMPTTQ12) suggest a possible mechanism for the following reaction: n-BuBr + KCN (ETOH , H2O ) n- BuCNQ19) suggest a possible reason for the following observations:

(i) The orderof reactivity of haloalkanes is RI > RCl > RBr.(ii) Neopentyl chloride does not follow SN2 mechanism.(iii) Ethers have low boiling points.

2010 AI COMPTTQ7) write the structure of the compound 4-tert.Butyl-3-iodoheptane.Q25) explain why

(i) The dipole moment of chlorobenzene is lower than that of cyclohexyl chloride.

(ii) Alkyl halides though polar are immiscible with water.(iii) In the pair, (CH3)3CCl and CH3Cl,CH3Cl will react faster in SN2

reaction with –OH.Q1)write IUPAC name of neopentyl chlorideQ2) write the structure of 1-Chloro-4-ethylcyclohexane.Q6)write the structure of 1,4-Dibromobut-2-ene

2012 AIQ5) What happens when bromine attacks CH2 = CH-CH2-C ≡ CHQ25)Answer the following questions:

(i) What is meant by chirality of a compound?give an example.(ii) Which one of the following compounds is more easily hydrolysed by KOH and why?

CH3CHClCH2CH3 or CH3CH2CH2Cl(iii) Which one undergoes SN2 sustitution reaction faster and why?

CH3CH2CH2CH2CH2I or CH3CH2CH2CH2CH2Cl Q5) write IUPAC name of following. CH2 = C(CH3)-CH2Br2012 DQ4) write IUPAC name of following. CH2 = C(CH3)-CH2BrQ24) Although chlorine is an electron withdrawing group, yet it is ortho,para- directing in electrophilic aromatic substitution reactions.Explain why it is so.

2012 FQ14) What are ambident nucleophiles? Explain giving an example.Q15) Explain as to why

(i) Alkyl halides,though polar,are immiscible with water.(ii) Grignard reagent should be prepared under anhydrous conditions.

2013 AI Q5) Write IUPAC name of the following: CH3 C (CH3)2 CH (Cl) CH3Q23) Give reason for the following:

(i) Ethyl iodide undergoes SN2 reaction faster than ethyl bromide.(ii) (+_) 2- Butanol is optically inactive.

(iii) C-X bond length in halobenzene is smaller than C-X bond length in CH3-X

Q5) write the IUPAC name of the following compound: CH3CH(Br)CH2CH(Cl)CH3Q3) write the IUPAC name of the following compound: Benzene ring 1and 4 position Cl and 3 position CH3 gr.

Question Bank(Organic compounds – Alcohols , Phenols , Ethers) 4 marksIUPAC

1) (CH3)2CH-CH2-CH(OH)-CH(CH3)-CH2OH2) CH3-O-CH2-CH(CH3)-CH2-CH33) 4-Chloropentan-2-one4) CH2=CH-CH(OH)-CH2-CH2-CH35) (CH3)2C(OH)-CH2-CO-CH36) 2-Methyl-2-ethoxy pentane7) Write structure of 1- Phenylpropan – 2- ol8) Write the structure of phenyl isopentyl ether9) Draw the structure of 2,6-Dimethyl phenol

MECHANISM1) Formation of diethyl ether from ethyl alcohol.2) Alcohols reacts both as electrophile & as nucleophiles in their reactions3) Acid catalysed dehydration of an alcohol forming an alkene4) Acid catalysed hydration of an alkene forming an alcohol5) Preparation of ethoxyethane from ethanol.Does the reaction follow SN1

or SN2 pathway.

REASONS1) Ethoxy ethane is soluble in water?2) Phenol is more acidic than ethanol3) Which is stronger acid phenol or cresol? Why?4) Phenols do not give protonation reaction readily?5) m- amino phenol is stronger acid than o- aminophenol6) Alcohols act as weak base.7) Propanol has higher b. p. than that of hydrocarbon Butane.8) Preparation of ether by acid dehydration of 20 &30 alcohol is not a

suitable method9) Ethanol has higher b.p. than methoxy methane.10) Alcohols are comparatively more soluble in water than

hydrocarbon of comparable M.M11) O- & p- nitrophenols are more acidic than phenol12) Ethers have low b.p.13) The b.p. of ethanol is higher than that of methoxy methane14) O-nitrophenol is more acidic than o-methoxy phenol

CONVERSION/WORD PROBLEM1) Ethyl alcohol to acetaldehyde2) Butan-2-one to Butan-2-ol3) Phenol to 2,4,6-tribromophenol4) phenol to benzoquinone5) Propanone to 2- Methyl propan-2-ol6) Propene to Propan- 2- ol7) Benzyl chloride to Benzyl alcohol8) Methyl Mg Bromide to 2-Methyl propan-2-ol9) Ethyl Mg Bromide to propan-1-ol

10) Ethenol to ethene

COMPLETE EQUATIONS1) Write the products obtained when benzyl phenyl ether is heated with

HI

QUESTION1) Name the reagents & write chemical equation for preparation of

(a)ethoxy benzene(b)2- Methyl-2-methoxy propane

2) Addition of G.R. to a carbonyl group of a comp. forming an adduct followed by hydrolysis?

3) Acid catalysed dehydration of an alcohol forming an alkene4) Acid catalysed hydration of an alkene forming an alcohol5) How do you account for the miscibility of ethoxy ethane with water?6) Which is a stronger acid phenol or cresol?Explain7) Give possible explaination for the following

(a)O-nitrophenol is more acidic than o-methoxy phenol(b)Alcohols are easilyprotonated in comparison to phenol.(c) The relative ease of dehydration of alcohol is 30>20>10

NAME REACTIONS1) Reimer Tiemann reaction2) Williamson’s synthesis3) Kolbe’s reaction4) Friedel Crafts reaction

DISTINGUISHING TEST1) phenol & cyclohexanol2) Propan-2-ol & benzyl alcohol3) Phenol & benzyl alcohol4) Butan-2-ol & 2-Methyl propan-2-ol5) Ethanol & phenol6) 1- propanol & 2- propanol7) Phenol & benzoic acid8) Isopropyl alcohol and n-propyl alcohol9) Methyl ethanoate and ethyl methanoate

2011DQ14) Explain the following giving one example for each:

(i) Reimer Tiemann reaction(ii) Friedel Craft acetylation of anisole

Q15) How would you obtain (i) Picric acid (2,4,6 – Trinitrophenol) from phenol(ii) 2-Methylpropene from 2- Methylpropanol

2011FQ5) write IUPAC name of (CH3)2C = C(Br) CH2OHQ26) How would you obtain

(i) Benzoquinone from phenol(ii) Propan-2-ol from propene(iii) 2-Methylpropan-2-ol from methyl magnesium bromide

2010DCOMPTTQ1) write IUPAC name of (CH3)2C(OH)CH2 CO CH3Q2) write structure of 2-Methyl-2-thoxypentaneQ11) give one chemical test to distinguish between the following pairs of compounds:

(i) Phenol and benzoic acid(ii) 1-Propanol and 2-Propanol

2010 AI COMPTTQ13)Describe the mechanism of hydration of ethane to yield ethanolQ14) write chemical equation each to illustrate the following reactions:

(i) Reimer tiemann reaction(ii) Williamson’s synthesis

2012 AIQ14) Explain the following behaviours:

(i) Alcohols are more soluble in water than the hydrocarbons of comparable molecular masses.

(ii) Ortho nitrophenol is more acidic than ortho methoxyphenol.Q15) explain the mechanism of acid catalysed hydration of an alkene to form corresponding alcohol.

2012 DQ5) Draw structural formula of 2-methylpropan-2-ol.Q25) Draw the structure and name the product formed if the following alcohols are oxidized. Assume that an excess of oxidizing agent is used.Q5) Draw the structure of hex-1-en-3-ol.

2012 FQ5) Write the IUPAC name of CH3 CH=CH-CH(OH)CH2CH3.Q25) State the products of the following reactions:

(i) CH3CH2CH2OCH3 + HBr (ii) C6H5OC2H5 + HBr (iii) (CH3)3COC2H5 + HI

Q5) Of the two alcohols:(a)CH2=CHCH2OH (b)CH2=CHCH2CH2OH,

Which one will react more easily with conc. HCl in the presence of ZnCl2?Q5) Write the IUPAC name of CH3O CH2CH(CH3)2

2013 AIQ16) Explain the mechanism of the following reaction:CH3-CH2-OH (H+ and 443 K) CH2=CH2 + H2OQ17) Write the equations involved in the following reactions:

(i) Reimer – Tiemann reaction(ii ) Williamson’s ether synthesis.

Question Bank

(Organic compounds containing aldehydes, ketones & carboxylic acids) 6marks IUPAC(i) (CH3)2C=CHCOCH3 (ii) 4-Methylpent-3-en-2-one(iii)CH3COCH2COCH3(iv) CH3COCH2CH(Cl)CH3(v)CH3C≡CCH=CHCOOH

(vi)OH)C6H5COC6H5OH(vii)C6H5CON(CH3)2(viii)1-Phenylpentan-1-one(ix)3-Oxopentanal(x)(CH3)2CHCOCH(CH3)2(xi)CH3CH2COC6H5(xii)2-Methylcyclopent-3-enecarboxylic acid(xiii)(CH3)2C=CHCOCH3(xiv)4-Chloropentan-2-one(xv) 2,6-Dimethyl phenol

MECHANISM1)Explain the mechanism of a nucleophilic attack on the carbonyl gr. Of an aldehyde or a ketone.

REASONS (i)Aldehydes are more reactive than ketones towards nucleophile

(i) The b.p. of aldehydes & ketones are lower than corresponding acids.(ii) The aldehydes & ketones undergo a no. of addition reactions (iii) Monochloroethanoic acid has a higher pKa value than

dichloroethanoic acid(iv) Ethanoic acid is weaker acid than benzoic acid(v) Benzoic acid does not undergo F/C reaction.(vi) pKa value of chloroacetic acid is lower than pKa value of acetic acid.(vii) P-nitrobenzoic acid has higher Ka value than benzoic acid(viii) Acetone is highly soluble in water but benzophenone is not.

CONVERSION/WORD PROBLEMQ1) An organic compound (A)having M.F. C8H8O forms an orange red ppt (B) with 2,4-DNP reagent. Compound (A) gives a yellow ppt (C) when heated in presence of I2 & NaOH alongwith a colourless compound (D).(A) does not reduce Tollen’s reagent or Feh. Soln. nor does it decolourise Br2 water. On drastic oxidation of (A) with chromic acid,a carboxylic acid (E) of M.F. C7H6O2 is formed. Deduce the structures of org. compds. (A) to(E).Q2) An organic compound A with M.F. C5H8O2is reduced to n-pentane on treatment with Zn-Hg/HCl. A forms a dioxime with hydroxylamine &gives a positive iodoform test & Tollen’s test Identify the compound A & deduce its structure.Q3) An unknown aldehyde A on reacting with alkali gives β-hydroxyaldehyde which loses water to form an unsaturated aldehyde , 2- butenal.Another aldehyde B undergoes disproportionation reaction in presence of conc.alkali to form products C & D. C is aryl alcohol with the formula C7H8O.

(i) Identify A & B(ii) Wrute the sequence of reactions involved.(iii) Name the product when B reacts with Zn/Hg & HCl.

Q4) A compound X (C2H4O) on oxidation gives Y (C2H4O2). X undergoes haloform reaction. On treatment with HCN , X forms a product Z which on hydrolysis gives 2- hydroxyl propanoic acid

(i)Write structures of X & Y (ii)Name the product when X reacts with dil. NaOH(iii)Write the equation for the reactions involved.

Q5) An organic compound contains 69.77% C ,11.63% H ,& rest is O. The molar mass of the compound is 86.It does not reduce Tollen’s reagent but forms an addition compound with NaHSO3 & gives a positive iodoform test. On vigorous oxidation it gives ethanoic & propanoic acid.Deduce the possible structure of org. compd.

Q6)An org.compd.A(C7H6Cl2) on treatment with NaOH soln. gives another compd. B (C7H6O). B on oxidation gives an acid C (C7H6O2) which on treatment with a mixture of conc. HNO3 & conc.H2SO4 gives a compd. D (C7H5NO4). B on treatment with conc. NaOH gives a compd E (C7H8O) & C6H5COONa. Deduce structures of A,B,C,D,E.Q7) An org.compd.A having M.F. C8H16O2 was hydrolysed with dil. H2SO4 to give a carboxylic acid B& an alcohol C. Oxidation of C with chromic acid produces B.C on dehydration gives But-1-ene.Write equations for the reactions involved.Q8) An org. comp.A (C3H6O) is resistant to oxidation but forms comp. B(C3H8O) on reduction reacts with HBr to form the comp. C. C with Mg forms G.R. D which reacts with a to form a product whichon hydrolysis gives E. Identify A to EQ9) Identify A to E. A [O] B + Ca(OH)2 C +DistlD +LiAlH4[H]E + HBrCH3CH(Br)CH3Q10) An org.comp. A on treatment with acetic acid in presence ofH2SO4 produces an ester B. A on mild oxidation gives C.C with 50% KOH followed by acidification with dil HClgenerates A & D D with PCl5followed by reaction withNH3 gives E. E on dehydration produces HCN Identify the comp. A,B,C,D,E.Q11) Identify the comp. A,B,C,D,E. A +Cl2 CHCl3+NaOH B+ C6H5COCl C C6H6/AlCl3D + EQ12)An organic compound (A) which has characteristic odour.On treatment with NaOH it forms two compounds (b) and (C).Compound(B) has M.F. C7H8O which on oxidation gives back (A).The compound (C) is a sodium salt of an acid.When (C)is treated with sodalime it yields an aromatic hydrocarbon (D).Deduce the structure o A,B,C,D.Write the sequence of reactions involved.Q13)An organic compound X undergoes acid hydrolysis to form two compounds Y and Z.Y reacts with Na2CO3 to form A, A is heated with sodalime to form B(CH4). Y on reduction with LiAlH4 forms Z.Identify X,Y,Z,A,B and write the reactions involved.Q14) An organic compound A hasM.F. C5H10O.It does not reduce Tollen’s reagent but forms an orange ppt.with 2,4-DNP reagent.It forms a carboxylic acid B with M.F. C3H6O. When treated with alk. KMnO4. Yellow ppt. on treatment with NaOH and I2 under vigorous conditions.On oxidation it gives ethanoic acid and propanoic acid.Sodium salt of B gave a H.C. C in Kolbe’s electrolytic reduction.Identiy A,B,C and write the reactions involved.Q15) Predict the products formed:(i)A reacts with phMgBr and is then hydrolysed(ii)A reacts with hydrazine and then heated with KOH and ethylene glycol.

Identify Q1) (A) to (E) (i) (***) +O3 (A) +(B)

(ii) (A) + (B) +dil NaOH (C) + H2O(iii) (C) + O3 /Zn/H2O (A) + (D) (iv) (D) +H2/Ni&Heat (E)

Q2) A,B,C(iii) A + H2 + Pd /BaSO4 (CH3)2CHCHO(iv) (CH3)3C-CO-CH3 + NaOI B + C

Q3) Identify A,B and C in the following C2H2 + (dil.H2SO4/HgSO4)A (dil.NaOH) B on heatingC

Conversions: (i) Ethyl benzene to benzene (ii) acetaldehyde to Butan-1,3-diol (iii) acetone to propene

(iv)ethanol to acetone(v) benzene to acetophenone(vi) benzoic acid to benzaldehyde(vii) Propanone to Propene(viii) Bromobenzene to 1-Phenylethanol(ix) Benzoic acid from ethylbenzene(x) Benzaldehyde from Toluene(xi) Ethanol to 3- Hydroxybutanal(xii) Bezaldehyde to Benzophenone(xiii) Cyclohexanol to cyclohexan-1-one(xiv) Ethyl benzene to benzoic acid(xv) Bromobenzene to benzoic acid(xvi) Ethyl cyanide to ethanoic acid(xvii) Butan-1-ol to butanoic acid(xviii) Methyl benzoic acid to benzoic acid(xix) Ethanal to but-2-enal(xx) Benzene to bezaldehyde(xxi) Benzene to acetophenone(xxii) Ethyl cyanide to 1-phenyl propanone(xxiii) Butanoic acid from butanol

COMPLETE EQUATIONS1)C6H5COCl +H2(Pd-BaSO4) 2) C6H6+ ----------- (anhy.AlCl3)C6H5COCH33) C6H6 + ------------ C6H5COC6H54)Fill the missing X,Y,Z.(i)C6H5CHO + CH3CH2CHO +(NaOH) X(ii)Ch3CH2CH2CH2OH + (Y) CH3CH2CH2COOH(iii)CH3(CH2)9COOC2H5 + (Z) CH3(CH2)9CHO5)HOOCC6H4COOH + SOCl26)C6H5CHO + (H2NCONHNH2 )7) C6H10=CH2 C6H11CHO

QUESTION1) Arrange in increasing order of their acid strength(CH3)2CHCOOH ,CH3CH2CH(Br)COOH , CH3CH(Br)CH2COOHBenzoic acid , 4-Nitrobenzoic acid,3,4-Dintrobenzoic acid , 4- Methoxy benzoic acidCH3CH2CH(Br)COOH ,CH3CH(Br)CH2COOH ,(CH3)2CHCOOH ,CH3CH2CH2COOH(reactivity towards HCN)-acetaldehyde,acetone,Di-terbutylketone,methyl ter butyl ketone

2) What is Tollen’s Reagent?Write one usefulness of the reagent3)Write two important uses of formalin

NAME REACTIONS(i) Cannizaro’s reaction (ii) Cross aldol condensation (iii) Decarboxylation (iv) Acetylation(v) Hell VolHard Zelinsky reaction (vi) Clemmenson’s Reduction (vii) Rosenmund’s reduction(viii) Wolf Kishner reduction reaction (ix) Aldol condensation

Distinguishing Tests: acetaldehyde & benzaldehyde

(i) propanone & propanol(ii) Propanal & propanone(iii) Phenol & benzoic acid(iv) Acetophenone & benzophenone(v) Ethanal & propanal(vi) Benzoic acid & Ethyl benzoate(vii) Formic acid and acetic acid(viii) Benzaldehyde and acetophenone

2011 DQ6) 3-Methylbutanal (IUPAC)Q29) (a) give chemical test to distinguish between:

(i) Propanal and propanone(ii) Benzaldehyde and acetophenone(b)How would you obtain:

(i) But-2-enal from ethanol(ii) Butanoic acid from butanol(iii) Benzoic acid from ethyl benzene

Q29) (a) describe the following chemical equation(i) Cannizaro’s reaction(ii) decarboxylation (b) Complete

(i) Ethyl benzene (KMnO4/KOH ) and heat (ii) phthalic acid (SOCl2) and heat (iii) Benzamide (H3O+) and heat

2011 FQ6) Write the structure of following 3-oxopentanalQ30) (a) give chemical test to distinguish between:

(i) Propanal and propanone(ii) Benzaldehyde and acetophenone(b) How would you obtain:

(i) But-2-enal from ethanol(ii) Butanoic acid from butanol(iii) Benzoic acid from ethyl benzene

Q30) (a) describe the following chemical equation(i) Cannizaro’s reaction(ii) decarboxylation

(b) Complete(i) Ethyl benzene (KMnO4/KOH ) and heat (ii) phthalic acid (SOCl2) and heat (iii) Benzamide (H3O+) and heat

2010 DCOMPTTQ1) write IUPAC name of (CH3)2C(OH)CH2COCH3Q30)An organic compound (A) on treatment with acetic acid in the presence of sulphuric acid produces an ester (B). (A) on mild oxidation gives (C) (C) with 50%KOH followed by acidification with dilute HCl generates (A) and (D).(D)with PCl5 followed by reaction wit ammonia gives (E).(E) on dehydration produces hydrocyanic acid.Identify the compoundsA,B,C,D,E.Q30)Identify A,B,C,D,E in the following sequence of reactions: A (Cl2) CHCl3 (NaOH) B (C6H5COClC (C6H6 /AlCl3D + EQ8) write the IUPAC name of the following (CH3)2CH CO CH(CH3)2

Q5) write the IUPAC name of the following CH3CH2COC6H5

2010AI COMPTTQ8) write the IUPAC name of the following CH2CH2CH2CHCHO(cyclic structure)Q30)An organic compound A on treatment with ethyl alcohol gives a carboxylic acid B and compound. Hydrolysis of C under acidified condition gives B and D.Oxidation of D with KMnO4 also givesB. B on heating with Ca(OH)2 gives E having molecular formula C3H6O. E does not give Tollen’s test and does not reduce Fehling’s solution but forms a 2,4-dinitrophenyl hydrazone. Identify A,B,C,D and E.Q30) Identify A,B,C,D and E. C6H5CH3 + CrO3 + (CH3CO)2O (273-283K) A (heat,H2O) B (conc.NaOH) C+ C6H5COONa C6H5CH3(KMnO4,KOH ,HEAT) D ( H3O+) EQ7)C6H4Cl COCH3 (IUPAC name)

2012 AIQ6) CH3-CH2-CH = CH- CHO (IUPAC name)Q6) Ph-CH = CH –CHO (IUPAC name)Q30)(a) write a suitable chemical equation to complete each of the following Transformations:

(i) Butan-1-ol to butanoic acid(ii) 4-Methylacetophenone to benzene-1,4-dicarboxylic acid(b) An organic compound with molecular formula C9H10O forms 2,4-DNP

derivative,reduces Tollen’s reagent and undergoes Cannizaro’s reaction.On vigorous oxidation it gives 1,2-benzenedicarboxylic acid.Identify the compound.

Q30) (a) give chemical tests to distinguish between(i) Propanol and propanone(ii) Benzaldehyde and acetophenone

(b) arrange the following compounds in an increasing order of their property as indicated:(i) Acetaldehyde,acetone,methyl tert-butyl ketone (reactivity

towards HCN)(ii) Benzoic acid,3,4-dinitro benzoic acid ,4-methoxy benzoic acid

(acid strength)(iii) CH3CH2CH(Br)COOH,CH3CH(Br)CH2COOH,(CH3)2CHCOOH (acid

strength)2012 DQ6) Arrange the following compounds in an increasing order of their reactivity in nucleophilic addition reactions: ethanol,propanal,propanone,butanone.Q30) (a) Illustrate the following name reactions giving suitable example in each case:

(i) Clemmensen reduction(ii) Hell-Volhard Zelinsky reaction

(b) How are the following conversions carried out?(i) ethyl cyanide to ethanoic acid(ii)Butan-1-ol to butanoicacid

(iii) Benzoic acid to m-bromobenzoic acid

Q30) (a) Illustrate the following reactions giving suitable example for each.(i) Cross-Aldol condensation (ii) Decarboxylation

(b)Give simple test to distinguish between the following pairs of compounds.(i) Pentan-2-one and Pentan-3-one(ii) Benzaldehyde and acetophenone

(iii) Phenol and benzoic acid .

2012 FQ6) Draw the molecular structureof the compound,4-methylpent-3en-2-one.Q30) (a) Describe the mechanism of the addition of Grignard reagent to the carbonyl group of a compound to form an adduct which on hydrolysis yields an alcohol.(b) Draw thestructures of the following compounds:(i) 3-Methylbutanal(ii)Hexane-1,6-dioic acid(iii) p-NitropropiophenoneQ30) (a) Illustrate the following rections giving a suitable chemical equation for each:

(i) Cannizaro reaction(ii) Hell-Volhard-Zelinsky reaction(b) How would you bring about the following conversions?Write the complete equation in each case:(i) Ethanal to 3-Hydroxybutanal(ii)Benzoic acid to m-nitrobenzyl alcohol(iii)Benzaldehyde to Benzophenone

2013 AIQ5) Rearrange the following compounds in the increasing order of their b.p.CH3CHO ,CH3CH2OH , CH3CH2CH3Q30) (a) How will you convert the following:(i) Propanone to Prpan-2-ol(ii) Ethanal to 2-hydroxy propanoic acid(iii) Toluene to benzoic acid

( b ) give simple chemical test to distinguish between:(i) Pentan-2-one and Pentan-3-one(ii) Ethanal and Propanal

Q30) ( a) Write products of the following reactions:(i) CH3 CO CH3 (Zn-Hg , conc. HCl)(ii) CH3 CO Cl + H2 (Pd –BaSO4) (iii) C6H5COOH (Br2/FeBr3)

( b) Which of each pair shown here would you expect to e stronger?(i) F-CH2-COOH or Cl-CH2-COOH(ii) C6H5OH or CH3COOH

Q4) ethanal is soluble in water.why?

Question Bank

(Organic compounds containing nitrogen) 4 marks

IUPAC1) Write IUPAC name of CH3-N(C2H5)-CO-CH3

2) Write IUPAC name of H2NCH2CH2CH=CH2

MECHANISM1)Show the mechanism of acylation of ethanamine and write the IUPAC name of the product formed.

REASONS1) Direct nitration of aniline is not carried out. Explain why?2) Predict giving reason the order of basicity (i) gaseous phase (ii) in

aqueous solution (CH3)3N , (CH3)2NH , CH3NH2,NH33) pKb for aniline is more than methylamine4) Methyamine solution reacts with FeCl3 solution to give ppt of Fe(OH)35) Primary amines have higher b.p. than tertiary amine.6) AgCl dissolves in aq. Methylamine solution7) Presence of a base is needed in the ammonolysis of alkyl halide.8) Aromatic primary amines can not be prepared by Gabriel Phthalimide

synthesis.9) Alkyl amines are stronger bases than ammonia.10) Aliphatic amines are stronger bases than aromatic amines.11) B.P. of methyl amine is lower than that of methanol12) Aniline does not undergo Friedel Craft alkylation reaction13) Although -NH2 gr. Is –o & -p directing ,nitration of aniline give –m

derivative alongwith –o & -p derivatives.14) Ethyl amine is soluble in water whereas aniline is insoluble.15) Amines act as nucleophiles.16) Gabriel phthalimide synthesis is preferred for synthesizing

primary amines.

CONVERSION/WORD PROBLEM1) How can you convert an amide into an amine having one C less than the starting compound?

(a)Name the reaction(b)Give IUPAC name & structure of amine obtained by the above method if tha amide is 3-chlorbutanamide.

2) (i) Benzene diazonium chloride to nitro benzene (ii)aniline to Benzene diazonium chloride (iii)Ethylamide to methyl amine (iv)Aniline to nitro benzene (v)Ethanamine to N-ethyl ethanamide (vi)Chloroethane to propan-1-amin(vii) aniline to iodobenzene

3) Identify A and B (i) CH3CH2Cl (NaCN) → A (reduction Ni/H2) → B (ii) C6H5NH2 (NaNO2/HCl) → A (C6H5NH2 , OH-) → B4)Aniline to sulphanilic acid5)An organic compound (A) on treatment with NH3 followed by heating forms compound (B) which on heating with Br2 and KOH forms a compound (C) having M.F. (C6H7N).Give the structures of A,B and C.and write the reactions involved.

COMPLETE EQUATIONS1) Complete & name the reaction.

(i) RNH2 + CHCl3 + 3KOH →(ii) RCONH2+Br2+4NaOH →

2) (i) LiALH4/H2O RCONH2 →(iii) C6H5N2Cl + H3PO2 + H2O →(iv) C6H5NH2 + HNO2 →

(v) C6H5N2Cl + CH3COCl →(vi) C2H5NH2 + C6H5SO2Cl →(vii)C2H5NH2 + HNO2 → (viii) C6H5NH2 + CHCl3 + 3KOH →3)Identify A and B(i) CH3CH2Cl + NaCN A ( redNi/H2) B(ii)C6H5NH2 + NaNO2+HCl A ( C6H5NH2) OH- B

QUESTION1) Write the equation in which iodide ion replaces the diazonium gr. in

diazonium salt2) (i) Arrange the following in an increasing order of basic strength in

water C6H5NH2, (C2H5)2NH ,(C2H5)3N & NH3

(ii) Arrange the following in an increasing order of basic strength in gas

Phase C2H5NH2, (C2H5)2NH ,(C2H5)3N & CH3NH23) Explain

(i) Presence of base is needed in the ammonolysis of alkyl halide(ii) Aromatic primaryamines can not be prepared by

GabrielPhthalimide synthesis. 4)In the following rearrange (i) In an increasing order of basic strength C6H5NH2, C6H5N(CH3)2 ,(C2H5)2NH and CH3NH2

(ii)In a decreasing order of basic strengthAniline ,p-nitroaniline and p-toluidine(iii)In an increasing order of pKb valuesC2H5NH2 ,C6H5NHCH3,(C2H5)2NH and C6H5NH2

5) Rearrange in an increasing order of their basic strength. C6H5NH2,C6H5N(CH3)2,(C6H5)2NH and CH3NH2

6 ) Arrange the following compounds in an increasing order of their solubility in water

C6H5NH2,(C2H5)2NH and C2H5NH2

NAME REACTIONS(i) Hofmann Bromamide reaction(ii) Gabriel Phthalimide synthesis.(iii) Carbylmine reaction (iv) Diazotization(v) Acetylation (vi) Coupling reaction of diazonium salt(vii) Gattermann reaction (viii) Ammonolysis of alkyl halide(ix) Write the name associated with the following reactions:

(c) RCONH2+Br2+4NaOHRNH2+Na2CO3+2NaBr+2H2O(d)ArN2X- (CuCN/KCN)ArCN + N2(e)RNH2+CHCl3+3KOH (heat)RNC+3KCl+3H2O(f) ArN2X- (Cu/HCl) ArCl+N2+CuCl

DISTINGUISHING TEST(i) aniline & ethyl amine (ii) Dimethyl amine & Trimethylamine(iii) Methylamine & dimethylamine.(iv) aniline & N-methylaniline (v) aniline & benzylamine(vi) aniline and N-ethyl aniline(vii) N-methyl propan-2-amine and N-ethyl-N-methyl ethanamine

2011 DQ7) Arrange the following compounds in an increasing order of their solubility in water C6H5NH2,(C2H5)2NH,C2H5NH2.Q26) (a) Explain why an alkyl amine is more basic than ammonia?

(c) How would you convert(i) Aniline to nitro benzene(ii) Aniline to iodobenzene.

2011 FQ7) Why is an alkyl amine more basic than ammoniaQ25) Illustrate the following reactions giving a chemical equation in each case.

(i) Gabriel phthalimide synthesis(ii) A coupling reaction(iii) Hoffman bromamide reaction

2010 D COMPTTQ9) Reasons: (i) ethyl amine is soluble in water whereas aniline is insoluble.

(ii ) The pKb of aniline is higher than that of methyl amine.(iii ) methyl amine reacts with FeCl3 solution to precipitate hydrated Fe2O3.(iv ) Aliphatic amines are stronger bases than aromatic amines.

Q10) Write the chemical reaction (i)Carbyl amine reaction

(ii) Hoffman bromamide reactionQ17) Write the reaction.

(i) Coupling reaction(ii) Ammonolysis

Q12) Write the reaction.(i) Acetylation(ii) Gabriel phthalimide synthesis

2010 AI COMPTTQ15) Reasons: (i) The pKb of aniline is higher than that of methyl amine. (ii)Aniline does not undergo Friedel Craft reaction (III) Gabriel phthalimide synthesis is preferred for synthesizing primary amines.Q16) Distinguishing test:

(I) Ethyl amine and aniline(II) Methyl amine and dimethyl amine.

Q26) (i) CH3CH2Cl ( NaCN) A (red.Ni/H2) B (ii ) benzene diazonium chloride +H3PO2 + H2O (iii ) RCONH2 (LAH/H2O)

2012 AIQ16) describe the following giving the relevant chemical equation in each case.

(i) Carbylamines reaction(ii) Hofmann’s bromamide reaction

Q17) complete the following reaction equation:(i) C6H5N2Cl + H3PO2 + H2O (ii) C6H5 NH2 + Br2 (aq)

2012 DQ7 )Arrange the following in the decreasing order of their basic strength in aqueous solutions: CH3NH2,(CH3)2NH,(CH3)3N and NH3.Q26) Write chemical equations for the following conversions:

(i) Nitrobezene to benzoic acid(ii) Benzyl chloride to 2- phenylethanamine(iii) Aniline to benzyl alcohol

2012 FQ16) Describe the following giving the chemical equation in each case:

(i) Carbylamines reaction(ii) Hoffmann’s bromamide reaction

Q17)Complete the following reactions equations:(i) C6H5N2Cl + H3PO2 + H2O (ii) C6H5NH2 + Br2(aq)

2013 AIQ6) Write the structure of n-methyl ethanamine.Q24) Complete the following reactions:

(i) CH3CH2NH2 + CHCl3 + alc.KOH (ii) C6H5N2 +Cl- (H2O Room Temp.)

(iii) C6H5NH2 + HCl (aq) Q1)write the structure of 2-aminotoluene.Q22) Complete the following reactions:

(i) C6H5N2 +Cl- (H3PO2 + H2O)

(ii) C6H5NH2 + Br2(aq) (iii) CH3CONH2 ( NaOH + Br2)

Q8) write the structure of prop-2-en-1-amine.Q27) write the main products of following reactions:

(i) CH3CH2NH2 (HNO2 , 00C)(ii) C6H5SO2Cl + C2H5NH2 (iii) C6H5NH2 + CH3COCl (base)

QUESTION BANK

(BIOMOLECULES)4 MARKSSAMPLE PAPER- 1 (OLD)Q8) What type of linkage holds together the monomers of DNA?Q27) An optically active compound having M.F.C6H12O6 is found in two isomeric forms (A) & (B) are dissolved in water they show the following equilibrium (A) ↔ Equilibrium Mixture ↔ (B) 1110 52.20 19.20

(i) What are such isomers called?(ii) Can they be called enantiomers ? Justify your answer.(iii) Draw the cyclic structure of isomer (A)

Q27)An optically active amino acid (A) can exist in 3 forms depending on the pH of the medium.if the M.F. of (A) is C3H7NO2 write

(i) Structure of compound (A) in aqueous medium. What are such ions called?

(ii)In which medium will the cationic form of compound (A) exist?(ii) In alkaline medium, towards which electrode will the

compound (a) migrate in electric field?

SAMPLE PAPER- 2 (OLD)Q12) Name the two components of starch. How do they differ from each other structurally?Q13)(a) What changes occur in nature of egg protein on boiling?

(a)Name the type of bonding which stabilizes α- helix structure in proteins.

SAMPLE PAPER- 3 (OLD)Q8) Except for vit.B12, all other vitamins of group B should be supplied regularly in diet. Why?Q25) Despite having a -CHO gr.

(a)Glucose does not give 2,4 –DNP test. What does this indicate?(b)Draw the Haworth structure of α-D-(+) glucopyranose(c) What is the significance of D & (+) here.

2008 DQ14) Define in relation to protein(i) peptide linkage(ii) denaturationQ15)List the reactions of glucose which can not be explained by its open structure.

2008 AIQ7) Write two main functions of carbohydrate in plants.Q26) What happens when D-glucose is treated with the following reagents(i)HI(ii)Br2 water (iii)HNO3

Q16) How are vitamins classified? Mention the chief sources of vit.A & vit. C.Q17) Describe with example (i) Glycosidic linkage(ii)peptide linkageQ17)Describe with reference to protein (i)Primary structure of Protein (ii)Denaturation

2008 FQ17)List any four vitamins. Mention the chief sources & functions of two of themQ7) Write two main functions of carbohydrate in plants.Q26)What are nucleic acids? Mention two of their important functions

2008 D COMPTTQ7) Why are carbohydrates generally optically active?Q26) What are amino acids? On electrolysis in an acidic solution, the relevant anions migrate towards the cathode while in alkaline solution they migrate towards the anode. Give reason.

Q16) What are essential & non essential amino acids? Give one example of each type.Q17)Mention the type of linkages responsible for formation of (i)Primary structure of protein(ii)cross linking of polypeptide chains(iii)α- helix formation(iv)β – sheet structure

2008 AI COMPTTQ11) When RNA is hydrolysed, there is no relationship among the quantity of different bases formed. What does this fact suggest about the structure of RNA?Q16) Explain the amphoteric behaviour of amino acid.Q26) (a) Which forces are involved in holding the substrate molecule to the active site of enzymes?(b) Name the receptor macromolecules that are chosen as drug targets.

2009 AIQ16) Name the four bases present in DNA. Which one of these is not present in RNA?Q17) Name two fat soluble vitamins ,their sources & the diseases caused due to Their deficiency in diet

2009 DQ16) Describe with example (i) Glycosidic linkage(ii)peptide linkageQ17 ) Name two water soluble vitamins ,their sources & the diseases caused due to their deficiency in diet

2009 FQ17) What are (i) Invert sugar (ii) Poly peptideQ18) State what are the following & how they differ from each other. (i) Nucleotide (ii)nucleoside

2009 D COMPTTQ8) What is the structural feature characterising reducing sugar?Q20) (a) What is the structural difference between a nucleoside & a nucleotide? (b) The two strands in DNA are not identical but are complementary .Explain.Q26)(a)Write the important structural difference between DNA & RNA?

( b )Mention the names of bases produced on hydrolysis of DNA.Q22) Name the chemical component which constitute nucleotide. Write any four functions of nucleotides in a cell

2010 AIQ7) What is meant by reducing sugars?Q26) Amino acids may be acidic ,alkaline , or neutral.How does this happens? What are essential and non essential amino acids? Name one of each type.Q6) What are mono saccharides?Q26) Differentiate between fibrous protein and globular protein.What is meant by denaturation of protein?Q8) What are the products of hydrolysis of sucrose?

2010 DQ17)Explain the following:

(i) Invert sugar (ii) poly peptidesQ17) Name the products of hydrolysis of sucrose.Why is sucrose not a reducing sugar?Q18) What are essential and non essential amino acids in human food? Give one example of each type.Q18) State clearly what are known as nucleosides and nucleotides?

2010 FQ8) What happens when glucose is treated with Br2 water?Q25) Explain the following:

(i) Invert sugar (ii) poly peptides (iii) Denaturation of proteinQ25) Mention three such facts/ reactions about glucose which can not be explained by its open chain structure .What is meant by pyranose structure of glucose?

NEW SAMPLE PAPER IQ25) (a) Give one reaction of D-glucose which can not be explained by its open chain structure.(b) Give one example of each for essential and non essential amino acids.( c) Differentiate between keratin and insulin.

NEW SAMPLE PAPER IIQ5) What type of linkage holds together the monomers of DNA?Q21) (a) Write the zwitter ion structure of glycine.(b) What is meant by inversion of sugar( c ) Name the vitamin in each case whose deficiency causes (i) Nightblindness

(ii) Poor coagulation of blood

NEW SAMPLE PAPER IIIQ8) What are the ultimate products of digestion of protein ?Q21) (a) Give reasons: (i) glucose does not give 2,4-DNP test and Sciff’s test(ii) Amino acids have high m.p. and are soluble in water.

(b)What is meant by the secondary structure of protein.

2011 AIQ17) Explain what is meant by the following:

(i) Peptide linkage(ii) Pyranose structure of glucose

Q18) Write the main structural difference between DNA and RNA.Of the four bases ,name those which are common to both DNA and RNA.Q18) Write such facts/ reactions about glucose which can not be explained by its open chain structure .

2011DQ16) What is essentially the difference between alpha form and beta form of Glucose?

Q17) Describe what do you understand by primary and secondary structure of protein.

2011 FQ16) Explain what is meant by

(i) Peptide linkage(ii) Pyranose structure of glucose.

Q17)Name the products of hydrolysis of (i) sucrose (ii) lactoseQ17) Mention three such properties of glucose which can not be explained by its open chain structure.

2010 D COMPTTQ8)What is the structural feature characterizing reducing sugar?Q20) (a) What is the structural difference between a nucleoside and nucleotide?

(b ) The two strands in DNA arenot identical but are complementary. Explain.

Q1) What are the expected products of hydrolysis of lactose?Q26) (a) Write the important structural difference between DNA and RNA.(b ) Mention the names of bases produced on hydrolysis of DNA.Q6) Give an example of the following

(a)Reducing sugar (b)Non reducing sugar

Q22) Name the chemical components which constitute nucleotides. Write any four functions of nucleotides in a cell.

2010 AI COMPTTQ17) What are vitamins? Deficiency of which vitamin causes

(i) pernicious anaemia (ii) convulsionsQ18) Enumerate the reactions of D-glucose which can not be explained by its open chain structure.Q9)What happens when D-glucose is treated with the following:

(i) HI (ii) Bromine water.Q15) What are the products of hydrolysis of the following

(i) Lactose(ii) A nucleotide from DNA containing thymine.

2012AIQ7) write the structure of the product obtained when glucose is oxidized with nitric acid.Q26) what is essentially the difference between ∞ - glucose and ß-glucose?what is meant by pyranose structure of glucose?Q7) write a reaction which shows that all the carbon atoms in glucose are linked in a straight chain.Q26)define the following as related to proteins:

(i) Peptide linkage(ii) Primary structure(iii) Denaturation.

2012 DQ16) What is meant by

(i) Peptide linkage(ii) Biocatalyst

Q17) Write any two reactions of glucose which can not be explained by the open chain structure of glucose molecule.Q18) Write the main structural difference between DNA and RNA. Of the two bases, thymine and uracil,which one is preset in DNA?

2012 FQ7) Write the full forms of DNA and RNA.Q26) What is glycogen? How is it different from starch? How is starch structurally different from cellulose?Q8) Of the two bases named below,which one is present in RNA and which one is present in DNA

(i) Thymine(ii) Uracil

Q26) Explain the meaning of the following terms:(i) Invert sugar(ii) Polypeptides(iii) Enzymes

Q26) Write three such behavior of glucose which can not be explained by the open chain structure of glucose molecule. What alternative structure has been proposed for the glucose molecule?

2013 AIQ7) what are the products of hydrolysis of sucrose?27) Shanti, a domestic helper of Mrs. Anuradha, fainted while mopping the floor.mrs. Anuradha immediately took her to a nearby hospital where she was diagnosed to be severely anaemic.The doctor prescribed an iron rich diet and multivitamins supplement to her. Mrs.Anuradha supported her financially to get the medicines. After a month, Shanti was diagnosed to be normal.After reading the above passage,answer the following questions:

(i) What values are displayed by Mrs.Anuradha?(ii) Name the vitamin whose deficiency causes pernicious anaemia.(iii) Give an example of water soluble vitamin.

Q7) write the name of linkage joining two amino acids.Q5) what are the products of hydrolysis of lactose?

Question Bank

(Polymers)

3 marks

SamplePaper – I (Old)Q5) Name the monomers of Nylon-2-Nylon-6 polymerQ17) Differentiate the following pair of polymers based on the property mentioned against each. a) Novolac & Bakelite (structure) b) Buna-S & Terylene (intermolecular force of attraction)

SamplePaper – II (Old)Q20) Write the names of monomers & classify them as addition or condensation polymers.

(a)Teflon (b) Bakelite (c) Natural rubber

SamplePaper – III (Old)Q26) (a)What is the role of Benzoyl peroxide in the polymerization of ethane? (b)What are LDPE & HDPE? How are they prepared?

2008 – DQ27)Write the names & structures of the monomers of given polymers.

(a)Buna-S (b) Neoprene (c) Nylon-6

2008 – AI Q8) Define polymerization.Q18) What are thermosetting & thermoplastic polymers? Give one example of eachQ18) Distinguish between homopolymer & copolymer & give an example of each class.

2008 – FQ8) What is the repeating structural unit in polythene polymer?

2008 – comptt DQ27) (b)Is –(CH2CHC6H5)n-- a homopymer or copolymer? Why?Q8) What is the difference two notations Nylon-6 & Nylon-6,6 ?Q18) What is step growth polymerization? Explain the steps involved in the process.Q18)What is the difference between elastomers & fibres ? Give one example of each.

2009 – AI Q8) What does 6,6 indicate in the name Nylon -6,6 ?Q18) Differentiate between molecular structure & behaviour of thermoplastic & thermosetting polymers.Give one example of each type.Q8) What is the primary structural feature necessary for a molecule to make it useful in condensation polymerization reaction?Q17) Differentite between condensation and addition polymerization.Give one example of each of the resulting polymers.

2009 – DQ7) Give an example of elastomers.Q18) Draw monomers of Teflon & polythene.Q18) What is the repeating unit in the condensation polymer obtained by combing HOOC-CH2-CH2-COOH (succinic acid) & H2N-CH2-CH2-NH2 (ethylene diamine)

2009 – FQ27) Differentite between mode of formation of condensation &addition polymerization.Give one example of each of these formation. Q27) Draw molecular structure of monomers of (i) PVC (ii) Teflon(iii) Neoprene

2009 – D(COMPTT)Q21) What are biodegradable polymers? Give an example of such polymer & mention its uses

2010 - AIQ8) What does the designation 6,6 mean in the name of nylon – 6,6?Q18) Draw molecular structure of monomers of (i) PVC (ii) Teflon

2010 - AIQ8) What is meant by coplymerisation?Q18) Draw molecular structure of monomers of (i) Bakelite (ii) Nylon -6

2010 – DQ26) Give one example of each (i) Addition polymers (ii) Condensation polymers (iii) CopolymersQ25) Write the name and structure of monomers of each polymer

(i) Neoprene (ii) Buna-S (iii) TeflonQ26) Differentiate between thermoplastic and thermosetting polymers .Give example of each

2010 – FQ26) Identify the four groups into which the polymers are classified on the basis of the magnitude of intermolecular forces present in them.To which group or groups do polythene and Bakelite belong?Q27) Write the name and structure of monomers of each polymer

(i) Polyvinyl chloride (ii)Bakelite (iii) Teflon

Sample Paper - I-(New)Q25) (a)Identify aliphatic biodegradable polyester which is used in packaging and orthopedic devices.

(i) Write its full form(ii)Give the structures of monomers from which it is formed.(iii) Show the formation of polymer

(b)Write the name and structure of monomer of nylon-6

Sample Paper - II-(New)Q20)(a)Write a reaction involved in the preparation of a biodegradable polyester. (b) Monomer unit of synthetic rubber (neoprene)( c )One use of Nylon-6,6

Sample Paper - III-(New)Q22) (a)Give an example of synthetic rubber and mention its one example.( b) Write the structures of monomers of Dacron( c ) Arrange the following in increasing order of their tensile strength.Nylon 6 ,Buna-S ,Polythene

A I-2011Q26)Draw the structures of monomers of (i) Polythene(ii) PVC(iii)TeflonQ26) Write the name and structures of the following polymers:

(i) Buna-S (ii)Dacron (iii) Neoprene

2011 DQ8) What are biodegradable polymers?Q18) Mention two important uses of each

(i) Bakelite(ii) Nylon – 6

Q8) In nylon 6,6 what does the designation 6,6 mean?Q18) Name the subgroups into which polymers are classifiedon the basis of magnitude of intermolecular forces.

2011 FQ27) Mention two important uses of each

(i) Bakelite(ii) Nylon-6,6(iii) PVC

Q27) (a)What does the designation 6,6 mean in Nylon 6,6 polymer? (b ) Which polymer is obtained when free radical polymerization of chloroprene occurs? Write the structure of polymer thus obtained.Q27) What are addition polymers? How are the two types of addition polymers different from each other? Give one example of each type.

2010 D COMPTTQ21) What are biodegradable polymers? Give an example of such a polymer and mention its uses.

2010 AI COMPTTQ26) Write the (i) structure and (ii) one use of each of the following polymers

(a)PVC(b)Urea-formaldehyde resin(c) Bakelite

2012AIQ27) differentiate between thermoplastic and thermosetting polymers. Give one example of each type.Q27) Explain the following terms giving example for each:

(i) Elastomers(ii) Condensation polymers(iii) addition polymers

2012 DQ8) Define the term, ‘homopolymerisation’ giving an example.Q18) Draw the structure of monomers for each of the following polymers:

(i) Nylon-6(ii) Polypropene.

2012 FQ18) Draw the structure of monomers for each of the following polymers:

(i) Nylon-6(ii) Teflon(iii) Neoprene

2013 AIQ8) Is (-CH2-CH)-n a homopolymer or a copolymer? I ClQ18) Define thermoplastic and thermosetting polymers. Give one example of each.

Q18) What is a biodegradable polymer? Give an example of a biodegradable aliphatic polyester.Q8) Give one example of a condensation polymer.Q6) Is (-CH2-CH)-n a homopolymer or a copolymer? I C6H5

Question Bank

(Chemistry in Everyday life)

3 marks

SamplePaper – I (Old) Q6) Give one example of artificial sweetener used by diabetic patients.Q18) In order to wash clothes with water containing dissolved calcium bicarbonate, which cleaning agent will you prefer & why, soap or synthetic detergent? Give one advantage of soap over synthetic detergent.

SamplePaper – II (Old)Q27) Reasons: a)Aspirin drug helps in prevention of heart attack.

b) Diabetic patients are advised to take artificial sweetener instead of natural sweeteners.

c) Detergents are non biodegradable while soaps are biodegradable

SamplePaper – III (Old)Q27) Classify synthetic detergents giving an example in each case.Q27) What are antihistamine? Give two examples. Explain how they act on the human body.

2008 - D Q8) Name a substance that can be used as an antiseptic as well as disinfectantQ18) What are biodegradable & non biodegradable detergents? Give one example of each class.

2008 – AIQ27) Mention one use of each:

a) Ranitidine b) Paracetamol c) Tincture of iodine

2008 – FQ27) a) What is the problem with hard water for washing with soap?

a) Explain (i) Broad spectrum antibiotics (ii) non ionic detergents

2008 –D –COMPTTQ8) What is meant by Broad Spectrum Antibiotics?Q18) Discuss the two ways in which drug prevent attachment of natural substrate on active site of enzyme.Q18) Explain with example: a) cationic detergent b) Tranqulizers

2008 –AI –COMPTTQ27) (a) What are antihistamine? Give two examples. Explain how they act on the human body.Give an example.

(b)Name a substance that can be used as an antiseptic as well as disinfectant

2008 –AI –COMPTTQ19) What are antibiotics? Distinguish between narrow spectrum & broad spectrum antibiotics.Classify the following into Bactericidal& Bacteriostatic antibiotics Tetracycline , Penicillin.

2009- AIQ27) Explain with example: a) Food preservatives b) Disinfectants c) Non ionic detergentQ27) Explain with example : a) Enzymes b) Sweetening agents c) cationic detergent.

2009 – DQ27) Explain with example: Analgesic ,Disinfectants, Antacid, Antiseptic.Q27) How do antiseptics differ from disinfectants ? Give one example of each

2009 –FQ1)Write the name of an antacid which is often used as a medicine.Q18) Reasons: (i) Soap do not do the cleansing in hard water. (ii) Synthetic detergents are preferred to soap in washing machine.Q8) What is meant by Broad Spectrum Antibiotics?Q17) Explain with example: a) Food preservatives b) cationic detergent

2009 – D-COMPTTQ22) What are anionic detergents ?How are they prepared ?Write their two uses.Q24) What are artificial sweetening agents ?Give two examples .Name the sweetening agents used in the preparation of sweets for diabetic patient.Q20)(a) Define the term chemotherapy. (b)While antacid & antiallergic drugs interfere with the function of histamine ,why do these not interfere with the function of each other.

2010- AI (I)Q27)Explain the following with one example : (i) Food Preservation (ii) Enzymes (iii) Detergents

2010 – AI (II)Q27) What are analgesic drugs?How are they classified and when are they usually recommended for use?

2010 – AI (III)Q27)Explain the following with one example : (i) Antibiotics (ii) Antiseptics (iii) Analgesic

2010 –DQ27) What are analgesic medicines?How are they classified and when are they commonly recommended for use?Q27) Explain with one suitable example

(i) Cationic detergent(ii) Enzymes(iii) Anti fertility drugs

2010 –FQ27) How do antiseptics differ from disinfectants? Name a substance that can be used as an antiseptic as well as disinfectant Q26) What are biodegradable and non biodegradable detergents? Give one example of each. Is there any structural difference between the two

Sample Paper - I-(New)Q26) (a) Justify the following:

(i) Sleeping pills are recommended to patients suffering from sleeplessness but it is not advisable to take them without consulting the doctor.

(ii) Why do we require artificial sweetening agents?(b)Write the composition of Dettol.

Sample Paper -II-(New)Q(25) (a)Name a substance which can act as both(i) analgesic and antipyretics (ii) antiseptic and disinfectant

(d)Explain the following with suitable example:(i) Broad spectrum antibiotics(ii) Anionic detergents

Sample Paper -III -(New)Q(23) Give one example of each

(g)An artificial sweetener whose use is limited to cold drink(h)A non ionic detergent(i) A pain reliever used for relief from severe pain like postoperative

or pain due to terminal cancer.

2011 AIQ27) What are the following substances?Give one example of each.

(i) Food preservatives(ii) Synthetic detergents(iii) Antacid

Q27)(a) Differentiate between a disinfectant and an antiseptic. Give one example of each.

(c) What is tincture of iodine and what is it used for? 2011 DQ27) Describe the following giving one example for each. (I ) detergent (ii) food preservative (iii) antacidQ27) Explain the following with suitable example. (I ) sweetening agent for diabetic patients (ii ) enzymes (iii ) analgesicsQ27) (I ) Why do soap not work in hard water?

(ii ) What are the main constituents of dettol? (iii )How do antiseptics differ from disinfectant?

2011 FQ8) What is meant by a Broad spectrum antibiotics?Q18) Give reasons:

(a)Soap do not work well in hard water.(b)Synthetic detergents are better than soap.

Q8) What are antiseptics? Give one example.Q18) Explain with example.

(a)Antacid(b) Sweetening agent.

2010 D comptt.Q22) What are anionic detergents? How are they prepared? Write their two main uses.Q24) What are artificial sweetening agents? Give two examples. Name the sweetening agent used in the preparation of sweets for a diabetic patients.Q20) (a) define the term chemotherapy.

(b ) While antacid and antiallergic drugs interfere with the function of histamines,why do these not interfere with the function of each other?

2010 AI COMPTT.Q27) Explain the following terms with suitable examples.

(d)Cationic detergent(e)Broad spectrum antibiotics(f) Tranquilizer

Q19) Explain the following terms:(j) Anionic detergent(k)Chemotherapy(l) Analgesics

Q26) Explain the following terms with one suitable example.(i) Non ionic detergent(j) Antiseptic(k)Antibiotic

2012AIQ8) Differentiate between disinfectants and antiseptics.Q18) what are food preservatives?Name two such substances.Q17) explain the cleansing action of soap.why do soap not work in hard water?Q8) what is the cause of a feeling of depression in human beings?Name a drug which can be useful in treating this depression.Q18) differentiate between disinfectants and antiseptics. give example of each group.

2012 DQ27)What are the following substances? Give one example of each one of them.

(i) Tranqilizers(ii) Food preservatives(iii) Synthetic detergent

Q27) Explain the following terms giving one example of each type:

(i) antacid (ii) disinfectants(iii) enzymes

2012 FQ8) What is meant by ‘narrow spectrum antibiotics’ ?Q18) State a reason for each of the following statements:

(i) soap does not work in hard water.(ii) The use of the sweetner aspartame is limited to cold foods

and drinks Q18) What are biodegradable and non biodegradable detergents? Give one example of each.

2013 AIQ25) (i) What class of drug is Ranitidine?(ii ) If water contains dissolved Ca2+ ions, out of soaps and synthetic detergents,which will you use for cleaning clothes?(iii ) Which of the following is an antiseptic? 0.2 % phenol , 1% phenol

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