E.MUTHUSAMY MSc.(Che), MSc.(Psy), MEd., MPhil., MA(Eng)., MA(Soc).,MA(P.admin).,BLISc.,DMLT, PGDCA

CHEMISTRY REVISION EXAM - 1 A1 PART – I

Choose the most appropriate answer 15x1=15 1. The mass of a chlorine atom is ……..

(a) 5.90 х 1023

g (b) 5.90 х 10-23

kg (c) 5.90 х 10-23

g (d) 5.90 х 1023

kg

2. ….... is used as a foaming agent.

(a) water (b) Lignite (c) Pine oil (d) Caster oil

3. consider the following statements. (i) Fluorine has low electron affinity than chlorine.

(ii) I.E. decreases with increase in atomic size. (iii) Actinide elements are not radio active

Which of the following statements given above is / are not correct

(a) (i),(ii) and (iii) (b) only (ii) (c) only (iii) (d) (ii) and (iii)

4. Match the list I with list II and select the correct answer using the code given below the lists

List- I List – II

A C2H4 + D2 1 Deuterium Fluoride

B D2 + O2 2 Ethylene deuteride

C D2 + N2 3 Heavy water

D D2 + F2 4 Heavy ammonia

Code: A B C D

(a) 1 2 3 4

(b) 4 3 2 1

(c) 2 3 4 1

(d) 1 3 4 2

5. The basic character of oxides down the group…..

(a) increases (b) decreases (c ) remains same (d) no change

6. The plane is parallel to z-axis and makes unit intercept an X and Y axis its plane is designated as …..

(a) (111) (b)( 010) (c) (110) (d) (100)

7. Excluded volume per molecule is……

(a) 4Vm (b) 2Vm (c) Vm / 2 (d) 4Vm

8. The compound which contains both ionic and covalent is …….

(a) CH4 (b) H2 (c) KCN (d) KCl

9. Work done in the reversible expansion is…….

(a) Minimum (b) Maximum (c) Zero (d) Not predictable

10. The equilibrium constant for the reaction CO2(g) + C(s) ↔ 2CO(g). When the partial pressure of CO2 and CO are

0.04 atm and 0.2 atm respectively is…….

(a) 1.9 atm (b) 1 atm (c) 2 atm (d) 0.04 atm

11. IUPAC name of CH2 = CH – CH2Cl is……

(a) Allyl chloride (b) 3- chloro 1- propene (c) 1- chloro 2-propene (d) Vinyl chloride

12. In the detection of sulphur using Lassaigne’s test the purple colour is developed due to……..

(a) Na4[Fe(CNS)5NO] (b) Na4[Fe(CN)5NOS] (c) Fe(CNS)3 (d) Na(CNS)

13. Diels – Alder reaction is a reaction between……

(a) diene and dieneophile (b) electrophile and nucleophile(c) Oxidant and reductant (d) free radicals

14. The ortho and para directing groups are……

(a) activating groups (b) deactivating group (c) both (a) & (b) (d) No effect

15. Statement – I: Aryl halides do not readily undergo Nuclephilic substitution reactions under ordinary

Conditions. Statements – II: In Aryl halides C – X bond is short and strong.

a)Both the statements are individually true but statement – II is not the correct explanation of statement – I.

b)Both the statements are individually ture and statement – II is not correct explanation of

statement - I.

(a) Statement – I is ture but statement – II is false. b)Statement - I is false, but statement – II is ture.

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E.MUTHUSAMY MSc.(Che), MSc.(Psy), MEd., MPhil., MA(Eng)., MA(Soc).,MA(P.admin).,BLISc.,DMLT, PGDCA

PART- II

Answer any six Questions in which Question No. 21 is compulsory. 6 х 2 = 12 16. What is the molality of the solution containg 25 g of suger (C12H22O11) in 1000g of water ?

17. How many electrons can have S + ½ in a d-sub-shell?

18. Mention any two uses of ozone.

19. Define Boyle’s law and charle’s law.

20. Calculate the vapour pressure of the solution.The molefraction of the solute is 0.25.The vapour

pressure of the pure solvent is 0.8 atm.

21. Substantiate with reason NH3 is a Nucleophile and BF3 is a electrophile.

22.0.530g of an organic compound gave 0.90g of BaSO4 in carius determination of sulphur. Calculate the

percentage of sulphur.

23. Explain the term aromaticity.

24. Explain why AlCl3 is an ionic compound in aqueous solution while it is covalent in vapour phase. PART-III

Answer any Six Questions in which Question No. 30 is compulsory. 6 х 3 = 18 25. How is pure H2O2 manufractured?

26. Why the IE2 of the alkaline earth metals is much higher than the IE1?

27. Explain why is Na atom bigger than the atoms of both lithium and magnesium?

28. What are miller indices?

29. Write the expression for the equilibrium constant (kc) for the reaction and how is it related to kp for the

reaction.

30. What are the scope of chemical kinetics?

31. How would you convert the following.

32. Explain the following terms.

33. Complete the following reaction.

(a) CH2 = CH2 + KMnO4 →? (b) CH3CH = CH2 →? (c) C2H6 = C = CH2 + O3 → ? PART – IV

Anwser All the Questions. 5 х 5 = 25 34.(a) (i) 4.5g of urea (molecular mass = 63 g/mol) are dissolved in water and solution is made to 100 ml in a

volumetric flask. Calculate the molarity of solution. (2)

(ii) A flask contains 53.1 ml of 0.150M Ca(OH)2 solution . How many ml of 0.350 M Na2CO3 are

required to react completely with Ca(OH)2 in the following reaction. (3) (OR)

(b) What is roasting ? Explain different types of roasting with suitable example. (5)

35. (a) (i) Give the values for all quantum numbers for 2p electrons in nitrogen (z = 7) (2)

(ii) Distinguish between an orbit and orbital. (3) (OR)

(b) (i) Explain the liquefaction of gases by Linde’s method. (3)

(ii) Write the Limitations of Vanderwaal’s equation of state. (2)

36. (a) (i) Mention the general characteristics of resonance. (3)

(ii) Distinguish between sigma and pi bonds. (2) (OR)

(b) Describe the factors on which the rate of reaction depends. (5)

37. (a) (i) Write the differences between an exothermic and an endothermic process. (3)

(ii) Explain thermal and mechanical equilibrium process (2) (OR)

(b) (i) Explain the purification of compounds by using thin layer chromatography. (3)

(ii) Under what conditions, would you prefer steam distillation as a purification technique? (2)

38. (a) Give the structural formula for (i) pent-1-ene-3-one, (ii) prop (iii) 3-methyl butanoic acid,

(iv) Neopentane, (V) 3-ethyl-2-methyl hexane. (5) (OR)

(b)An organic compound ‘A’ having molecular formula C7H7Cl gives the following reactions.

(i) on reduction with Zn-Cu couple, it gives toluene.

(ii) on oxidation with alkaline KMnO4 it gives benzoic acid.

Identify the compound ‘A’ and write equation for reactions (i) and (ii). (5)

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E.MUTHUSAMY MSc.(Che), MSc.(Psy), MEd., MPhil., MA(Eng)., MA(Soc).,MA(P.admin).,BLISc.,DMLT, PGDCA

CHEMISTRY REVISION MODEL EXAM – 2 A2

PART-I MARKS :70

Choose the most appropriate answer

1.The oxidation number of M in MnSO4 …….

(a) +4 (b) +2 (c) +6 (d) 0 2. An example for platinum metal is…….. (a) Ge (b) Ir (c) As (d) Sb

3. Consider the following statements …….

(i) Transition metals have the ns1-2

(n-1)d1-10

electronic configuration

(ii) Second ionisation potential is lesser than the first ionisation potential

(iii) Cl- ion is bigger than Cl atom

Which of the following statement(s ) given above is / are not correct

(a) (i), (ii) and (iii) (b) only (ii) (c) only (iii) (d) (ii) and (iii)

4. Match the list-I with list-II and select the correct answer using the code given below the lists.

List-I List-II

A Li vapour 1. Bleaching agent

B Na + liq. NH3 2. Artificial rubber

C Isoprene 3. Intense blue solution

D H2O2 4. Calamin red colour

Code:

A B C D

(a) 1 2 3 4

(b) 4 3 2 1

(c) 2 3 4 1

(d) 1 2 4 2

5……… is known as inorganic benzene.

(a) BF3 (b) B2O4N7 (c) C2H2 (d) Diborane

6. Crystalline solids that exhibit different physical properties in all directions are called as ……..

(a) anisotropic (b) isotropic (c) symmetric (d) differential

7. The rate of diffusion of gas is ……. To square root of molecular mass.

(a) inversely proportional (b) directly proportional (c) is equal (d) not related

8. The molecule which has two bond pairs and two lone pairs of electrons……

(a) NH4+ (b) PCl5 (c) SO2 (d) H2O

9. Freezing of a liquid at the freezing point is an…… process.

(a) reversible (b) endothermic (c) exothermic (d) spontaneous

10. Kp ≠ Kc for equilibrium…….

(a) PCl5↔ PCl3 + Cl2 (b) H2 + I2 ↔ 2HI (c) N2O4 ↔ 2NO2 (d) N2 + O2 ↔ 2NO

11. The unsaturated hydrocarbon which contains one C – C sigma bond and one C – C pi bond are known as……..

(a) alkanes (b) alkynes (c) alkenes (d) alkyls

12. 0.12g of an organic compound gave on combustion 0.11g of CO2. Calculate the percentage of carbon is …….

(a) 23% (b) 25% (c) 27% (d) 28%

13. CH3C ≡ CH A:A is …….

(a) CH3CHO (b) CH3COCH3 (c) CH3CH2CHO (d) CH3CH2COCH3

14. Benzene does not decolourise alkaline ……. Solution

(a) KMnO4 (b) FeSO4 (c) NaCl (d) K2Cr2O7

15. Statement – I: Organic halides are insoluble in water

Statement – II: Organic halides are unable to form strong H- bond with water

(a) Both the statements are individually true but statement – II is not the correct explanation

Of statement – I

(b) Both the statements are individually true and statement – II is the correct explanation of statement – I

(c) Statement – I is true but statement – II is false

(d) Statement – I is false, but statement – II is true

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E.MUTHUSAMY MSc.(Che), MSc.(Psy), MEd., MPhil., MA(Eng)., MA(Soc).,MA(P.admin).,BLISc.,DMLT, PGDCA

PART – II Answer any six Questions in which Question No. 21 is compulsory

16. Calculate the oxidation number of underlined elements in the following species.

(a) Cr2O7-2

(b) K2MnO4

17. Write the electronic configuration of chromium and copper.

18. Why NH3 has high boiling point than PH3.?

19. What are the units of vanderwaal’s constants ‘a’ and ‘b’?

20. 10g of an organic substance when dissolved in two litres of water gave an osmotic pressure of .59 atm at 7 C.

Calculate the molecular weight of the substance.

21. Explain the term “Catenation”.

22. 0.36g of a nitrogeneous organic compound was kejldahilised and the ammonia liberated was exactly neutralized by

20ml of 0.3N H2SO4. Calculate the percentage of nitrogen in compound.

23. Convent sodium benzoate Benzene.

24. Give the electron dot representation for PH3 and ethane.

PART – III Answer any six Questions in which Question No. 30 is compulsory.

25. Explain why alkali metals possess only +1 oxidation state.

26. Bring out the relationship between Be and Al.

27. Out of fluorine and chlorine, which has greater electron gain enthalpy?

28. Calculate the miller indices of crystal planes which cut through the crystal axes at

(i) (2a, 3b, c) (ii) (a, b, c) (iii) (6a, 3b, 3c)

29. The value of the equilibrium constant for the reaction H2 + I2 ↔ 2HI is 54 at 7 k. In one experiment the equilibrium

concentrations of iodine and hydrogen iodide are 1.3 х 1 -3

and 1.6 х 1 -2

moles respectively. Calculate the equilibrium

concentrations of hydrogen.

30. (i) Explain why the rate of a reaction increases with the increase in temperature.

(ii) Write the rate law of pA + pB → lC + mD reaction.

31. Write note on Wurtz – Fitting reaction.

32. Give an example of monohydric, dihydric and trihydric alcohols. Write their IUPAC name.

33. Complete the following reactions.

(i) CH ≡ CH ? (ii) CH3 – CHBr – CH2Br - ? iii) C6H5COONa ?

PART – IV Answer All the Questions.

34. (a) (i) Identify oxidized and reduced species in H2S + Cl2 2HCl + S. (2)

(ii) Balance the following redox reaction. (3)

MnO2 + Cl- Mn

2+ Cl2 + H2O (acid medium) (OR)

34. (b) (i) What is the principle involved in Bessemer process. (2)

(ii) Explain the froth flotation process with neat diagram. (3)

35. (a) (i) Describe Aufbau principle. Explain its significance in the electronic build up of atoms. (3)

(ii) Using s, p, d, f notations. Describe the orbital with the following quantum numbers

(a) n= 2, l = 1 (b) n = 4, l = 0 (c) n = 5, l = 3 (c) n = 3, l = 2 (2)

(OR)

35. (b) (i) Describe Claude’s process of liquefaction of gases with neat diagram. (3)

(ii) Define Joule – Thomson effect. (2)

36. (a) Explain how the valence bond theory accounts for

(i) a carbon – carbon double (C = C) (ii) a carbon - carbon triple bond (5) (OR)

36. (b) Compare and contrast the terms, order and molecularity of a reaction. (5)

37. (a) (i) Calculate the heat of formation of ethylene from the following data: (3)

H2(g) + ½ O2 (g) H2O ; (l) ΔH1 = - 65,000 cal. C(g) + O2 (s) CO2 ; (g) ΔH2 = - 97,000 cal.

C2H4 (g) + 3O2 (g) 2CO2 (g) + 2H2O ; (l) ΔH3 = - 340,000 cal.

(ii) ΔH for the reaction at 298 k CO (g) + ½ O2 (g) CO2 (g) is 282.85 kJ mol-1.Calculate ΔU of the reaction. (2) (OR)

37. (b) Define and explain the types of paper chromatography. (5)

38. (a) Give equations for the following reactions of acetylene with (i) H2 / Ni (ii) Br2 (iii) HBr

(iv) H2SO4 and HgSO4 (v) HOCl (vi) O3 (5) (OR)

38. (b) An element occupies group No. 16 and period number 2. This element on passing through silence electric

discharge forms (A). (A) also reacts with lead sulphide and forms (B) . (A) also reacts with BaO2 and forms (C). It

reacts with H2O2 and forms (D). Identify the element (A), (B), (C) and (D) (5)

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E.MUTHUSAMY MSc.(Che), MSc.(Psy), MEd., MPhil., MA(Eng)., MA(Soc).,MA(P.admin).,BLISc.,DMLT, PGDCA

CHEMISTRY MODEL EXAM – 3 A3

PART – I

Choose the most appropriate answer.

1. The total number of moles present in 111 g of CaCl2 is

a) One mole b) Two moles c) Three moles d) Four moles

2. Highly pure metals are obtained by ….. process.

(a) Gravity separation (b) Calcination (c) Zone refining (d) Froth floatation

3. Consider the following statements…….

(i) Inner transition metals have the (n-2)f1-14

(n-1)d0-10

ns2 electronic configuration

(ii) Electron affinity of fluorine is greater than chlorine.

(iii) E.A decreases with decreases in size.

Which of the following statement(s) given above is / are not correct.

(a) (i), (ii) and (iii) (b) only (ii) (c) only (iii) (d) (ii) and (iii)

4. Match the list-I with list – II and select the correct answer using the code given below the list.

List – I List – II

A D2O 1 Neutron moderator

B H2O2 2 Tetra ethyl lead

C LiAlH4 3 Rocket Propellant

D Na 4 Reducing agent

Code : A B C D

(a) 1 2 3 4

(b) 4 3 2 1

(c) 2 3 4 1

(d) 1 3 4 2

5. Boracite is……

(a) 2 Mg3 B8 O15 MgCl2 (b) 2 Mg3B8 O15 MgSO4 (c) 2 Mg3 B8 O15 MgCl2 (d) 2 Mg3 B8 O8 MgSO4

6. The Weiss indices of a plane are ½, ½,½. Its miller indices will be---------

a) (0,1,1) b) (1,0,1) c) (2,2,2) d) (½, ½,½)

7. Mole fraction of the gas---------

a) Ratio of the partial pressure to the total pressure of the gas.

b) Multiplication of the partial pressure with the total pressure of the gas

c) Sum of the partial pressure and total pressure of the gas. d) None of the above.

8. The compound which contains both ionic and covalent is

a) CH4 b) H2 c) KCl d) KCN

9. Enthalpy of neutralization of a strong and by a strong base

i) Has a constant value of -57.32KJ

ii) Is independent of the nature of strong acid and strong base.

iii) Is heat change accompanies the reaction H+

(aq)+OH-→H2O

a) (i) and (ii) b) (i) and( iii) c) (i) only d) (i) ,(ii) and (iii)

10. In endothermic equilibrium reaction the increase in temperature --------- the reaction.

a) Increases the Keq value b) Does not change the Keq value. c) Increases the Keq value d)constant unity

11. which one among the following is a heterocyclic compound?

a) cyclopentane b) antracene c) neopentane d) thiopene

12. percentage of sulphur is calculated by--------------

a) 14V1N1 /100 b) 14V1N1 /1000 c) 32/233xwt of B2SO4 formed/wt of organic compoundx100 d)none

13. witting reaction is used to prepare

a) an alkene b)an alkyne c) an alkane d) none of the above

14. which among the following substituents increase the rate of electrophilic substitution reaction compared to that of

benzene? CH3 b) NO2 c) NH2 d) both a and c

15. Statement – I : Arylhalide do not readily undergo nucleophilic substitution reaction under ordinary conditions.

Statement - II : In Arylhalides C – X bond is short and weak.

(a) Both the statements are individually true but statement – II is not the correct explanation of statement –I

(b) Both the statements are individually true but statement – II is the correct explanation of statement –I

(c) Statement –I is true but statement – II is false (d) Statement –I is false but statement – II is ture .

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E.MUTHUSAMY MSc.(Che), MSc.(Psy), MEd., MPhil., MA(Eng)., MA(Soc).,MA(P.admin).,BLISc.,DMLT, PGDCA

PART – II : Answer any six Questions in which Question No. 21 is compulsory

16. What is the simplest formula of the compound which has the following percentage composition.C = 80%, H =20%

17. How many orbitals are there in the second orbit? How are they designated?

18. How does ozone react with the following (a) Pbs (b) K2MnO4

19. Define Graham’s law of diffusion.

20. A stream of try air was passed through an aqueous solution containing 25.17g m-3

of a on – volatile solute. The loss

in mass of the solution was 3.0322 g and of the water 0.0188 g Calculate the water mass of the solute .

21. Give equations for the synthesis of urea in the laboratory.

22. 0.301g of an organic compound gave 0.282g of AgBr by carius method. Find the percentage of bromine.

23. Mention the uses of benzene.

24. Give reason. CCl4 is insoluble in H2O while NaCl is soluble? PART – III :Answer any six Questions in which Question No. 30 is compulsory.

25. How do you convert para hydrogen to ortho hydrogen?

26. Why there is increase in the ionization potential for forming M3+

ion for group 2 metals.

27. Lanthanides and actinides are placed in separate rows at the bottom of the periodic table. Explain the reason for

this arrangement.

28. How do this spacing of the three planes (100), (110) and (111) of cubic lattice vary?

29. Calculate the active mass of nitrogen if 56g of nitrogen is held in a 200ml container?

30. (i) How does a catalyst influence a chemical reaction?

(ii) Powered zinc reacts with dil. H2SO4 acid faster than the zinc rod. Explain why?

31. Explain the mechanism of sulphonation of benzene.

32. What are carbonium ions? How are they produced? Outline the geometry of carbonium ions.

33. Account for the following: (i) he boiling point of butane C is more than - methyl propane - . C).

(ii) he melting point of n- pentane - . C) is less than neopentane - C)

PART – IV :Answer All the Questions.

34. (i) Calculate the molarity of a solution by dissolving 0.850g of ammonia (NH3) in 100g of water. (2)

(ii)An acid of molecular formula mass 104 contains 34.6% carbon 3.85% hydrogen and the rest oxygen.

Calculate molecular formula of the acid. (OR) (3)

(i) What is anode mud? (2)

(ii) What is smelting? Explain the process with example (3)

35. Explain the various quantum numbers which completely specify the electron of an atom (5)

(OR)

Explain the causes for deviation for real from ideal behavior. (5)

36. (i) Draw the Lewis structures for the following: (a) PCl5 (b) SF6 (2)

(ii) Discuss the shape of following molecules: (a) NH3 (b) SO2 (OR) (3)

(i) What are the characteristics of a zero order reaction ? (2)

(ii)Mention the characteristics of a first order reaction. (3)

37. (i) Compare the enthalpy changes that occur between the neutralization of a strong acid and a week acid by sodium

hydroxide. Explain the differences seen. (3)

ii Distinguish between a “state function “ and “path function” with an example. (OR) (2)

(i)Give the advantages of distillation under reduced pressure (2)

(ii)Describe the procedure involved in TLC and explain how it is used to separate the components of a mixture.(3)

38. i Explain Markovnikov’s rule or addition of hydrogen bromide to propene gives -bromopropane. Explain the

mechanism of the reaction. (3)

(ii)Explain why direct fluorination is not favour to fluorinate alkanes (2)

(OR)

An organic compound (A) of molecular formula C6H6 on treatment with Cl2 in presence of catalyst as FeCl3 to give

compound (B)of molecular formula C6H5Cl. Compound (B) further undergo alkylation with CH3Cl and anhyd.

AlCl3 to give isomers C and D of molecular formula C7H7Cl. Identify A,B,C and D. Explain the reaction. (5)

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