Electro chemistry1 Write the Chemical equations for the steps involved in rusting of iron. Give one method to prevent rusting of

iron.2 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?

3 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 atomic 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 + 2e 2Ag + S2- is –0.17V Al3+ +3e Al is -1.66V

4 (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

5 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.

6 (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 reaction s taking place at the anode & Cathode in the above Cell.(C)Give reaction s taking place at the two electrodes if these are made up of Ag.

7 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 its dissociation Constant?

8 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)

9 (a) What is primary Cell? Give one example(b) The Conductivity of a 0.2M soln. of KCl at 298 K is 0.0248 SCm-1. Calculate its molar Conductivity.

10 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.

11 (a)Express the relation between Conductivity & molar Conductivity of a soln.(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

12 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

13 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)

14 (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 Conductivity Cell Containing 0.05 M soln of an electrolyte X at 40 0C is 100 ohm The same Cell is filled with 0.01M soln. of electrolyte. Y has a resistance of 50 ohm . The Conductivity 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.

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

16 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.

17 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.

18 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)

19 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+/Al = -1.66V)

20 (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)

21 a) State the relationship amongst cell const. of a cell, resistance of the soln. in the cell & conductivity of soln. How is molar conductivity of a solute related to conductivity of its soln. (b) Calculate K for the reaction Fe+ Cd2+ Fe2+ + Cd (E0Fe2+/Fe = -0.44V, E0Cd2+/Cd = -0.40V)

22 (a) Define molar conductivity. How is it related to conductivity Of the related soln.(b)One half cell in voltaiccell is constructed from a silver wire dipped in AgNO3 soln. of unknown conc. Its other half cell consists of a Zn electrode 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)

23 (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)

24 (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]

25 (a)What is meant by Limiting molar conductivity? (b) 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.

26 Write the anode and cathode reactions occurring in a commonly used Hg – cell. How is the overall reaction represented?

27 One Half cell in a voltaic cell is constructed from Ag wire dipped in AgNO 3 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)

28 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)

29 (i) Write the product obtained at anode on electrolysis of conc. H2SO4 using Pt electrode. (ii) For a weak electrolyte molar conductance in dilute solution increases sharply as the concentration in solution is decreased. Give reason.(iii)Write overall cell reaction for lead storage battery when the battery is being charged.

30 (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 occur Zn(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 energy31 (a)Describe the construction of a H2 –O2 fuel cell and the reactions taking place in it.

(b) Define the terms given below- (a)Conductivity (b) molar conductivity What are their units?

32 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?

33 (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.

34 (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 place

Zn(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)

35 (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 = 1.33V

36 (a) How many moles of Hg 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)

37 (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.

38 (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)

39 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.

40 State and explain Kohlrausch law of independent migration of ions. How can the degree of dissociation of acetic acid be calculated from its molar conductivity data.

41 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.12 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)

43 (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.An electrochemical 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)

44 The standard electrode potential (E0) for Daniel cell is +1.1 V. Calculate the ∆G 0 for the reaction Zn(s) + Cu 2+ Zn2+ + Cu(s) ( 1F = 96500 C mol-1)

45 Calculate emf of the following cell at 250C Ag(s) /Ag+ (10-3M)// Cu2+ (10-1 M)/Cu (s) (Given E0 Cell= + 0.46 V and log 10 n = n)

Chemical Kinetics

1 For a chemical reaction variation in the [R] t ( 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

2 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 & B3 Consider the reaction AP (graph [R] t is given)

(i)Predict the order of reaction(ii)Derive expression for the integrated rate law for the reaction

4 (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

5 (i)The decomposition reaction ofNH3 gas on Pt surface has a rate const. K = 2.5x10-4 mol /L/s. What is the order of reaction?(ii) What is molecularity of the reaction Cl (g) ½ Cl2(g)

6 (i) Graph of log[Ro]/[R] t is given for a 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.7 (i)Define the term order of reaction for chemical reaction

(ii)A first order decomposition reaction takes 40 min. for 30% decomposition Calculate its t1/2 value.8 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 reaction9 (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 N 2 & H2

if k = 2.5x10-4 mol/L/s10 (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.

11 (i) 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(ii)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)

12 (i)Distinguish between order & molecularity of a reaction When could order & molecularity of a reaction be the same.(ii)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)

13 (i)Define order of reaction. How will you prove that a chemical reaction is of first order?(ii) 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

14 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 law15 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 hours?16 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)

17 (i)Why does the rate of a reaction not remain const. throughout the reaction process?(ii) Explain the term order of a reaction. Derive the unit for first order rate const.(iii) Show that for a first order reaction, the time required for half life period is independent of initial concentration.

18 (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 sample of PH3 remains behind after one minute.

19 (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)

20 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.

21 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 0.075M?

22 For the reaction N2 + 3H2 2NH3 If ∆[NH3]/ ∆t = 4 x 10 -8 mol/L/s what is the value of -∆[H2]/ ∆t?23 Sucrose decomposes in acid solution into glucose and fructose according to the first order rate law with t 1/2 = 3 hrs.

Calculate the fraction of sucrose which remains after 8 hrs.24 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)25 (a) For the reaction C12H22O11 + H2O C6H12O6 + C6H12O6

Write (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 0.6

Calculate the rate of reaction when total press. Is 0.65 atm.26 (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

27 Consider the decomposition of H2O2 in alkaline medium which is ctalysed by iodide ions. 2H2O2 2H2O + O2

This 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?

28 In a hydrolysis reaction 5 g ethyl acetate is hydrolysed in presence of dil. HCl in 300 min. If the reaction is of 1 st

order and the initial concentration of ethyl acetate 22 mol/L, Calculate the rate const. of the reaction.29 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 it will take for 3 /4th of initial quantity of HCOOH to decompose. (log 0.25 = -0.6021)(a) Distinguish between rate expression and rate constant of a reaction.(b)2N2O5 4NO2 +O2

The first order reaction was allowed to proceed at 400Cand 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.

30 (i)Why does rate of reaction not remain constant throughout the reaction Process?(ii)Explain the term order of reaction Derive the unit for first order rate constant.

(iii)Show that for the first order reaction the time required for half life period is independent of initial concentration.

31 (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.

Time 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.

32 (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)

33 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?

34 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)

35 (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.

SURFACE CHEMISTRY1 (a)Consider the adsorption isotherm given & interpret the variation in the extent of adsorption (x/m) when

(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.

(c) Why is FeCl3 preferred over KCl in case of cut leading to bleeding?2 (a)What are the physical states of dispersed phase & dispersion medium of froth?

(b) Explain: (i) Fe(OH)3 sol gets coagulated on addition of NaCl solution(ii) Cottrell’s smoke precipitator is fitted at the mouth of the chimney used in factories.(iii) Physical adsorption is multi layered while chemisorption is mono layered.

3 (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

4 A colloidal solution of AgI is prepared by two different methods shown below(A) By adding AgNO3 in excess KI & (B) By adding KI in excess AgNO3 (i) What is the charge of AgI colloidal particles in the two (A) & (B)(ii) Give reasons for the origin of charge (A)AgNO3 added to KI (B) KI added to AgNO3

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

(b) An electric current is passed through a colloidal solution. (c) A beam of strong light is passed through a colloidal solution.

6 (i)Differentiate between multi molecular & macromolecular colloids? Give one example of each. How are these two types of colloids different from associated colloids.(ii) Define electrophoresis briefly.

7 (i) Why does physisorption decrease with increase in temp.?(ii) What is observed when (a) a beam of light is passed through colloidal Solution (b)An electrolyte NaCl is added to hydrated Fe2O3 sol (c)An electric current is passed through a colloidal solution(iii) In chemisorption why x/m initially increases& then decreases with rise in temp.

8 (a)What is the difference between a colloidal solution & an emulsion? Give one example of each(b) What are emulsifiers?

9 How does adsorption of a gas on a solid surface vary with increase in Pressure?10 Explain with example: (a) Peptization (ii) gel (iii) dialysis11 Distinguish between homogeneous & heterogeneous catalysis?

What role does adsorption play in heterogeneous catalysis? 12 Distinguish between micelles & colloidal particles. Give one example of each.13 (i)What is the coagulation process?

(ii)What is the sign of ∆H & ∆S when a gas is adsorbed by an adsorbent?(iii) What are emulsions? State one application of emulsification

14 (i)Define the term Tyndall effect.(ii)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(iii) Write three special features of chemisorption which are not found in physisorption.

15 (a)Describe the following: (i) Tyndall effect (ii) Shape selective catalysis(b) What is meant by coagulation of a colloidal solution? Name any method by which the coagulation of lyophobic sol can be carried out.(c) Define the following terms:(i) Peptization (ii) Reversible sol

16 (i)Which of the following is most effective electrolyte in coagulation of Fe2O3.H2O/Fe3+ sol KCl,AlCl3,MgCl2,K4[Fe(CN)6](ii)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

17 (a)Name the type of potential difference produced between the fixed charged layer and diffused layer having opposite charges around the colloidal particles. (b) Heat of adsorption is greater for chemisorption than physisorption why?(c) What is colloidion?

(d) Differentiate between peptization and coagulation.18 (a) Give main difference between lyophilic and lyophobic colloids.

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

19 (a)What is meant by shape selective catalysis?(b) Classify colloids where the dispersion medium is water. State their characteristics and write an example of each of these classes(c) What is lyophobic colloid? Give one example for them.

20 Explain how the phenomenon of adsorption finds application in each of the Following(i) Production of vacuum(ii)Heterogeneous catalysis(iii)Froth floatation process

21 Define each of the following-(i) Micelles (ii)Peptization(iii)Desorption22 (i)What is the difference between adsorption and absorption?

(ii) What is an adsorption isotherm? Describe Freundlich adsorption isotherm.(iii) Why is adsorption always exothermic?(iv) Discuss the effect of pressure and temperature on adsorption of gases on solids. Describe the application adsorption in controlling humidity.

23 (i)Name the two groups into which phenomenon of catalysis can be divided. Give an example of each group with the chemical equation involved.(ii) What is meant by coagulation of a colloidal solution? Describe briefly any three methods by which coagulation of lyophobic sols can be carried out.

METALURGY1 Account for

(a)The reduction of metallic 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.2 An ore of sample Galena is contaminated with Zinc Blende. Name one chemical which is used to concentrate

galena selectively by froth floatation method.3 ∆Gf for MgO & CO at 1273K & 2273K are given

∆Gf [MgO] = -941KJ/mol at 1273K & ∆Gf [CO]= - 439KJ/mol ∆Gf [MgO] = -314 KJ/mol at 2273K & ∆Gf [CO]= - 628 KJ/mol Predict the temp. at which C can be used as a reducing agent for MgO(s).

4 (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.

5 State briefly the principles which serves as basis for the following operations in metallurgy(i)Froth floatation process (ii)Zone refining (iii )Refining by liquation (iv) Vapour phase reefing (v) Electrolytic refining

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

7 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.

8 (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.

9 (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

10 State the basis of refining of a substance by chromatographic method. Under what Circumstances is this method specially useful.

11 (a)What is meant by the term Pyrometallurgy?(b)Describe the underlying principle of the following metal refining methods. (i)Electrolytic refining of metals (ii) Vapour phase refining of metals(c) Describe the role of following:

(i) NaCN in the extraction of Ag from silver ore. (ii) Cryolite in the metallurgy of Al

12 (i)Why is the froth floatation method selected for the concentration of sulphide ores?(ii) Explain the role of (a) CO in purification of Ni (b ) Cryolite in the electrolytic reduction of alumina.

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

14 Give 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 15 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

16 Describe how the following changes are brought about.(i)Pig iron into steel (ii)ZnO into metallic zinc (iii)Impure Ti to pure Ti

17 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

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

19 (a)Name the method used for refining of copper metal.(b) Name the method used for removing gangue from sulphide ores.(c) How is wrought iron different from steel?

20 Name the principal ore of aluminium. Explain the significance of leaching in the extraction of aluminium21 Write the reaction involved in the extraction of silver after the silver ore has been leached with NaCN.22 (a)Name one chief ore each of copper and aluminium. Name the method used for the concentration of these two

ores.(b)What is the role of depressant in Froth Floatation process for the concentration of a sulphide ore?

23 (a)What is the role of graphite in the electrometallurgy of aluminium?(b)What is the role of depressant in Froth Floatation process for the concentration of a sulphide ore?

24 (a) Name the method used for removing gangue from sulphide ores.(b) How is wrought iron different from steel?

25 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.

p-Block elements

1 Account for the following:(a)Among the halogens F2 is the strongest O.A.(b)F exhibit only –1 oxidation state whereas other halogens exhibit higher positive oxidation state also.(c)Acidity of oxo acids of Cl increases in order of HOCl<HOClO<HOClO2<HOClO3.

2 Account for (a) Cl2 water has both oxidizing & bleaching properties(b)H3PO2 &H3PO3 act as good reducing agent while H3PO4 does not(c)On oxidation of O3 gas to KI soln. violet vapours are obtained.

3 Give reasons: (a) CN- ion is known but CP- is not(b) NO2 dimerises to form N2O4 (c) ICl is more reactive than I2

4 (a) What is the covalence of nitrogen in N2O5?(b) Explain why both N & Bi do not form pentahalides while P does?

5 Why does Cl2 water lose its yellow colour on standing?6 Give Reasons: (i) NH3 is stronger base than PH3 (ii) S in vapour state exhibits a paramagnetic behaviour.7 (i)Why is the bond angle in PH3 molecule lesser than that in NH3 molecule?

(ii) Which neutral molecule would be isoelectronic with ClO-?(iii)Of Bi (V) & Sb(V) which may be stronger O.A.& why?

8 Give reasons: (i) S in vapour state exhibit 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.9 (a)Which is a stronger acid in aq. Soln. of HF or HCl and why?

(b) Give 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)

10 Give 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

11 Give reasons: (i) O2 molecule has formula O2 while S has S8 (ii) N does not form any pentahalide like P (iii) H2S is less acidic than H2Te

12 (a) Arrange HClO,HClO2,HClO3,HClO4 in order of acidic strength. Give reason.(b) Why do some noble gases form compounds with F & O only.

13 (i)Why is N2 very less reactive as compared to P4?(ii) When HCl reacts with finely powdered iron it forms FeCl2 & not FeCl3 why?

14 (a) How do Xe atom forms compounds even though the Xe atom has a closed shell electronic configuration?15 (i) Why are halogens mostly coloured?

(ii) Why is BiH3 the strongest R.A. among all the hydrides of gr 15 elements.(iii) H2O is liquid while H2S is a gas why?(iv)Why is Ka2<<Ka1 for H2SO4 in water?(v)Why is red P less reactive than white P?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.16 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

17 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.18 (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 (iv)Why is Bi(V) stronger O.A. than Sb(V)

19 Give 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 whereas SF6 is not

(vi)XeF2 has a linear structure & not a bent angular structure20 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

21 Explain (i) S in vap. State exhibit paramagnetism. (ii)+3 oxidation state becomes more & more stable from As to Bi in the group

22 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.23 Explain (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.

24 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 equipments25 Reason (i) PH3 is weaker base than NH3

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

26 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.27 Give reasons: (i) N2 is not particularly reactive

(i) X2 are strong O.A.(ii) SF6 is less reactive than SF4.

28 Account for the following:(i)F does not exhibit any + ve oxidation state Why? (ii) NCl3 is an endothermic compound while NF3 is an exothermic one (iii) XeF2 is a linear molecule without a bend.(iv)The electron gain enthalpy with – ve sign of F is less than that of Cl still F2 is strong O.A. than Cl2.(v)N2 is relatively inert as compared to P4 Why?

29 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.

30 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.(iv) Why does NO2 dimerise?

31 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.(iv) Which is stronger acid in aq. Solution HCl or HI and why?

32 Explain the following giving reason (i) S in vapour state exhibit paramagnetic behavior(ii)The stability of +3 state increases down the gr.in gr. 15 of the P.T.(ii)XeF2 has a linear shape and not a bent structure

33 Explain (i)H2S is less acidic thanH2Te ( ii) F2 is stronger O.A. thanCl2

( iii ) Noble gases are least reactive elements.34 Give reasons: (i) Solid PCl5 is an ionic compound.

(ii) Most of the reactions of F are exothermic.

(iii) O3 is thermodynamically unstable.35 Give reasons:

(a) Interhalogen compounds are more reactive thn halogens(b) PCl5 is known but NCl5 is not known.(c) Among all the noble gases only Xe is known to form compounds with O and F

36 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 F2

37 (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.?

38 Account for the following:(i) NF3 is an exothermic compound but NCl3 is not(ii) The acidic strength of compounds increases in the order PH3 < H2S< HCl(iii) SF6 is kinetically inert.

39 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.

40 Which is stronger reducing agent , SbH3 or BiH3, and why?41 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.

42 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?

43 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.

44 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.

45 What is the basicity of H3PO2 acid and why?46 Which one of PCl4 + and PCl4 – is not likely to exist and why?47 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 cannot be explained by Valence Bond approach.

48 Which is stronger acid in aqueous solution, HF or HCl, and why?49 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.

50 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.51 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 amongst the hydrides of group 15 elements.

52 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.

53 What is the basicity of H3PO3 and why?

1 Write equation for the complete hydrolysis of XeF6.2 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) KCl3 What happens when Cl2 water reacts with cold dil soln. of NaOH? Write equation only4 Write down the equations for hydrolysis of XeF4 & XeF6.Which of these two reactions is a redox reaction.5 Write equations (i)Cl2 reacts with hot conc. soln. of NaOH ii)orthophosphorous acid is heated (iii)PtF 6 & Xe

are mixed together6 Complete the equation: (i) Ca3P2 + H2O (ii) Cu2+ + NH3 (aq) (excess) (iii) F2 (g) + H2O (l)

(iv)XeF4 + H2O (v)O3 + I- + H2O7 Write equation for Cl2 water reacts with conc. soln. of NaOH Justify that this is a disproportionation reaction.8 How are the following compounds prepared fro XeF6 - (i) XeOF4 (ii)XeO3

9 Complete XeF4 + H2O10 Complete (i) XeF2 + H2O (ii) PH3 + HgCl2 11 Complete : (i)P4 + NaOH + H2O (ii) O3 + I- + H2O 12 Complete (i) XeF2 + PF5 (ii)Cl2 + NaOH (hot& conc.) 13 Complete (i)PCl5 + H2O (excess) (ii) F2 + H2O 14 Complete (i) SO2 + MnO4- + H2O (ii) HgCl2+ PH3 15 Complete (a) : P4 + NaOH + H2O (b) Cu + HNO3 (dil) 16 Write equation: (i) Cl2 + NaOH (hot & conc.) (ii)XeF6 + H2O (iii) NaOH +SO2(excess) 17 Complete (i) I2 + HNO3 (conc) (ii) HgCl2 + PH3 18 Complete (i) NaOH (cold & dil.) + Cl2 (ii) XeF6 + H2O (excess) 19 Complete the following: 1.NaOH (hot and conc.) + Cl2 2. XeF6 + H2O20 Complete the following: ( i) P4 + SOCl2 (ii) XeF4 + H2O21 (a) Complete (i) AgCl + NH3 (ii) P4 + NaOH + H2O 22 Write equation for the following reaction

( a) thermal decomposition of (NH4)2Cr2O7

( b) reaction of Cl2 with cold and hot dil.NaOH( c) when phosphine is passed through HgCl2 solution

23 Give chemical reaction in support of the following observations ( a) H2SO4 has low volatility. ( b) I- can be oxidized by O2 in acidic medium

24 Complete the following equations (i)HgCl2 + PH3 (ii)SO3 + H2SO4 (iii)XeF4 + H2O 25 Write balanced chemical equation for the following observations

(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

26 Complete-(i)C + conc. H2SO4 (ii)P4 + NaOH + H2O (iii)Cl2 + F2(excess) 27 Complete the following equations:(i) P4 + SO2Cl2 (ii) XeF2 + H2O (iii)I2 + HNO3 (conc.) 28 Complete the following chemical equations (i)NaOH (hot and conc.)+ Cl2 (ii)XeF4 + O2F2 at 143 K

(iii)Br2 + F2 (excess) 29 Complete the following chemical equations(i)P4 + SO2Cl2 (ii)Fe3+ + SO2 + H2O

(iii)XeF6 + H2O (excess) 30 complete the following observations(i) Cu + HNO3 (dilute) (ii)XeF4 + O2F2 31 Complete the following chemical reaction equations:

(i) P4 + SO2Cl2 (ii) XeF6 + H2O

32 Complete the following chemical equation (i) NaOH + Cl2 (hot and conc.) (ii)XeF4 + O2F2 33 Complete the following chemical equations:

(i) XeF4 + SbF5 (ii) Cl2 + F2 (excess)

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

35 Complete the following chemical equations:(i) Sn + 2PCl5 (heat) (ii) Fe3+ + SO2 +H2O (iii) XeF2 + H2O

1 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 Cl 2

forms D which hydrolyses to compound E Identify A to E.2 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.

3 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.4 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.

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

6 Give one use each of ClF3, O2F2,I2O5

7 (a) How are interhalogen compounds formulated & how are they prepared?(b) Which neutral molecule would be isoelectronic with ClO-?

8 Draw the structure of white and red phosphorous. Which one of these two types of phosphorous is more reactive and why?

9 ( 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.

10 Which of the following compounds has a lone pair of electron at the central atom? H2S2O8,H2S2O7,H2SO3,H2SO4

11 (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)

12 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)

13 Name two poisonous gases which can be prepared from chlorine gas.Q14)

14 How are interhalogen compounds formed? What general compositions can be assigned to them?15 Which aerosol depletes ozone layer?

1 Predict the shape of ClF3 on the basis of VSEPR theory2 Draw structures of (i) SF4 (ii) XeF4 (iii) XeOF4 (iv)XeO3

3 Draw the structures of (i) PCl5 (ii) S8 (iii) ClF3

4 Draw structures of (i) H2S2O7(ii) NO3-

5 Draw the structures of (i) BrF3 (ii) XeF2

6 Draw the structures of (i) HClO4 (ii)BrF3

7 Draw structures of (i) H2S2O8(ii) HClO4

8 Draw structures of (i) H2S2O7(ii) HClO3

9 Draw structures of (i) H3PO2(ii) BrF3

10 Draw structures of (i) H2S2O7(ii) XeF4

11 Draw structure of XeF4 , BrF3 12 Write the formula & structure of noble gas species which are iso structural with ICl4- & BrO3- 13 Draw structures of (i) H4P2O5 (ii) XeF4

14 (i)What is O.N. of P in H3PO2 molecule(ii)Draw structure of ( i) BrF3 ( ii ) XeF4

(iii)Draw structure of O3 molecule.15 Draw structures of O3 and S8 molecules.

16 Draw structures of XeF2 and HClO4 molecules.17 Which Xe compound is isostructural with ICl4

- ?18 (i) Draw structure of phosphinic acid(H3PO2)

( ii) Write a chemical reaction for its use as a reducing agent.19 Draw the structure of the following- ( i) XeOF4 ( ii) H4P2O7

20 Draw the structures of the following molecules.(i)(HPO3)3 (ii) BrF3

21 Predict the shape of ClF3 on the basis of VSEPR theory22 Draw the molecular structures of the following compounds: N2O5, XeOF4

23 Predict the shape and angle(900 or more or less) in each of the following cases:(i) SO3

2- and the angle O-S-O(ii) ClF3 and the angle F-Cl-F(iii)XeF2 and the angle F- Xe –F

24 Draw the structures of the following molecules:(i ) H3PO2 (ii) H2S2O7 (iii) XeOF4

25 Draw molecular structures of following compounds: XeF6 , H2S2O8

26 Draw the structures of the following molecules: XeOF4 , H3PO3

d &f – Block elements

1 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.

2 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

3 (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 some time? Give the equation involved What is this type of reaction called?

4 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.

5 (a) Out of Ag2SO4,CuF2,MgF2& CuCl. Which compound will be coloured & why? (b) Explain: (i) CrO4 2- is strong O.A. while MnO4

2- 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.

6 (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

7 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, Cr 2+

act as a R.A. but Mn3+ acts as an O.A.8 (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

9 Complete the equations(i) oxidation of Fe2+ by Cr2O72-in acidic medium

(ii) oxidation of S2O32- by MnO4

- in neutral aq. medium10 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.

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

12 (a) Complete (i) Cr2O72- + H+ + Fe2+ (ii)MnO4

- + I- + H+ (b) How many unpaired electrons are present in Mn2+ ion? How does it influence magnetic behavior of Mn2+

ions?13 Reasons(i)There are irregularities in the e.c. of actinoids.(ii) Compounds of T.E. are often coloured14 (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.15 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. Radii16 Why do d block elements generally exhibit large no. of oxidation states than those exhibited by the f block

elements?17 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 K2 Cr2O7 is prepared from chromate (ii)The colour of K2 Cr2O7 solution changes with change in pH of solution

18 (a) On what ground can you say that Sc(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?

19 Complete the following reactions: (i) MnO4- + C2O4

2- + H+ (ii) Cr2O72- + H+ + Fe2+

20 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.21 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.

22 Complete the equations: (i) Cr2O72- + H+ +H2S (ii)MnO4

- + S2O32- + H2O

23 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.

24 ( 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. is quite high. 3. T.E. form coloured compounds 4. T.E. exhibit variable oxidation state.

25 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

26 (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.

27 Reason (i)The enthalpy of atomization of T,E. are quite high’ (ii) There is a greater horizontal similarity in the property of T.E. than that of the main gr. Elements.

28 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.

29 Complete: (i)MnO4- + Fe2+ + H+ (ii)Cr2O7

2- + C2O42- + H+

30 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 ore

31 (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.

32 (a)Complete the equations: (i) Cr2O7 2- + H2S + H+ (ii) Cu2+ + I - ( b) Account for the following:

(i) The oxidizing power of oxoanions 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+

33 (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.

34 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.

35 How would you account for the following(i) The at. Radii of elements of the 5 d series of T.E. are virtually 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 a metal is exhibited in its oxide or fluoride

36 Explain: (i) The T.E. generally form coloured compounds (ii) Zn is not regarded as a T.E.37 Describe preparation of (i) K2Cr2O7 from Na2CrO4 (ii) KMnO4 from K2MnO4

38 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.39 Explain: (i) The T.E. have great tendency for 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)

40 (a) (i) Which is stronger R.A.Cr2+ or Fe2+ and why? (ii)Explain why Cu+ ion is not stable in aq. soln. (iii) Explain why Ce4+ is a strong O.A.(b) Describe the oxidizing property of KMnO4 in neutral or faintly alkaline medium for its reaction with I- ions and S2O3

2- ions41 (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.

42 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 information answer the following:(i)Which is the most stable oxidation state for Ni and Pt? Why?(ii)Out of the two, name the metal which can easily form compounds in +4 oxidation state and why?

43 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

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

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

46 (a) Give two consequences of lanthanoid contraction.(b)Complete the following reactions: (i) MnO4

- + S2O32- + H2O (ii) Cr2O7

2- + H+ + Sn2+ (c)Which of the following has maximum number of unpaired electrons? Ti3+,V2+,Fe2+,Mn2+

(d)Based on the data arrange Fe2+,Mn2+ and Cr2+ in the increasing order of stability of +2 oxidation state. E0Cr3+/Cr2+ = -0.4V,E0Mn3+/Mn2+ = 1.5V,E0Fe3+/Fe2+ = 0.80

47 What is meant by Lanthanoid contraction?48 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

49 Complete the following: (i) MnO4- + S2O3

2- + H2O (ii) Cr2O72- + H+ + Fe2+

50 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 4d and the 5d series metals generally do not form stable cationic species.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 transition metals than that of the 3d series.

51 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.

52 (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

53 (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 amongst 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.

54 (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 oxidized.

55 (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 as a transition element but Zn(30) is not.(ii)E0(M2+/M) value for copper is +ve.

56 Complete the following chemical equations: (i) Cr2O72- + I- + H+ (ii) MnO4 - + NO2 - +H+

57 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 E0

M2+ /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.

58 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.

59 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.

60 Complete the following equations: (i) Cr2O72- + I- + H+ (ii) MnO4 - + NO2 - +H+

61 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.

62 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.

63 Explain the following observations giving an appropriate reason for each.(i) The enthalpies of atomization of transition elements are quite high.(ii) There occurs much more frequent metal-metal bonding in compounds of heavy transition metals.(iii) Mn2+ is much more resistant than Fe2+ towards oxidation.

64 (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.

65 (a)Calculate the number of unpaired electrons in the following gaseous state ions: Mn 2+,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.(iii)The highest oxidation state of a transition metal is exhibited in its oxide or fluoride.

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

67 (a) Why do transition elements show variable oxidation states?(b)Name the element showing maximum number of oxidation states among the first series of transition metals from Sc (Z=21) to Zn (Z = 30)(c)Name the element which shows only +3 oxidation state.(d) What is lanthanoid contraction? Name an important alloy which contains some of lanthanoid metals.

Co-ordination compounds

1 Why does a tetrahedral complex of type [MA2B2] not show geometrical isomerism?2 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 terms of t2g & eg.(iii)What type of hybridization will Mn+ ion have?(iii)Name the type of isomerism exhibited by this complex.

3 (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 shown by the following complexes [Co(NH3)5Br]SO4 & [Co(NH3)5 SO4]Br Give the chemical test to distinguish between these two compounds.

4 (a) Give the e.c. of the 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?

5 (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]

6 (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]+

7 Describe the limitations of V.B. theory.8 Write IUPAC name of[CoCl(NO2)(NH3)4]Cl9 Using V.B. approach , deduce the shape & magnetic character of [Co(NH3)6]3+ ion (Co =27)10 Write IUPAC name of[Co(NH3)6] [Cr(CN)6] & [Cu(NH3)4] [PtCl4]11 (a)Draw the structure & write the hybridization of Co in cis-[Co(NH3)4Cl2]+

(b)Write IUPAC name of[Co(NH3)4Cl(ONO)]Cl12 Giving example for each, explain the following-(i) Crystal field splitting (ii) Linkage isomerism

(iii)Ambidentate ligand13 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)14 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.15 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-

16 For the complex [Fe(en)2Cl2]Cl Identify- (a)Oxidation no. of Fe.(b) Hybrid orbitals & shape of complex (c) Magnetic behaviour of complex (d) No. of geometrical isomers (e) Whether there is an optical isomer also (f) Name of the complex

17 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-

18 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 chiral.

19 Compare with respect to molecular shape and magnetic behavior(i) [Cr(NH3)6]3+ (ii)[Fe(CN)6]4- (iii) [NiCl4]2-

20 Explain giving example ( i ) Linkage isomerism (ii) Outer orbital complex (iii) A bidentate ligand21 (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)

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.

23 Write the name , the state of hybridization , shape and the magnetic behaviour of the following :(i) [CoCl 4] 2- , [Ni(CN)4] 2- ,[Cr(H2O)2 (C2O4)2 ] – (at. No. Co = 27 , Ni = 28 , Cr = 24)

24 Give an example of linkage isomerism.25 Name the following coordination compounds according to IUPAC system of nomenclature:

(i )[Co(NH3)4(H2O)Cl]Cl2 (ii)[CrCl2(en)2]Cl26 Give an example of ionization isomerism.

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

27 What is an ambidentate ligand? Give an example.28 Describe the state of hybridization, shape and magnetic behaviour of

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

29 Give an example of coordination isomerism.30 What happens to the colour of coordination compound [Ti(H2O)6]Cl3 when heated gradually?31 (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

32 (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]

33 Using Valence bond theory, predict the geometry and magnetic character of [NiCl4]2-.34 Explain the following terms giving suitable example in each case- (i) Ambident ligand

(ii)Denticity of ligand (iii)Crystal splitting in an octahedral field35 Write the structures and name of all the stereo isomers of the following compounds.

(i)[Co(en)3]Cl3 (ii)[Pt(NH3)2Cl2] (iii)[Fe(NH3)4Cl2]Cl36 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]37 Name the following coordination compounds and draw their structures: (i) [CoCl2(en)2]Cl

(ii) [Pt(NH3)2Cl(NO2)] (Co=27,Pt=78)38 Why is CO a stronger ligand than Cl- ?39 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)40 Name the following coordination compound: K3[CrF6]41 Give the name ,the stereochemistry and the magnetic behavior of the following complexes:

(i)[Co(NH3)5Cl]Cl2 (ii) K2[Ni(CN)4]42 (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

43 write the IUPAC name and deduce the geometry and magnetic behavior of the complex K 4[Mn(CN)6] (Mn=25)

44 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)

45 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)46 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)

47 State reasons for each of the following situations:(i) Co2+ is easily oxidized to Co3+ in presence of 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-

48 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]

49 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.

50 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]+

51 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)

52 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