PAPER : CHEMISTRY-I

Reg. No. :

PART – A

Answer ALL the Questions: (20x1=20) Choose the correct Answer: Answer

1. Atomic number is represented by the symbol a) A b) N c) S d) Z 2. In the modern periodic table, second period consists of __________ elements. a) 2 b) 18 c) 8 d) 65 3. The bond order of

2He molecule is

a) 0 b) 1 c) 2 d) 3 4. Which one is a non-polar molecule? a) H Cl b) 2H O

c) NaCl d) 6 6C H

5. The unit for dipolemoment is

a) cm b) 2cm

c) Debye d) Pascal

6. The bond angle of 4CH molecule is

a) 129o b) 109.5o c) 139o d) 149o 7. The another name for Azimuthal quantum number is a) Principal Quantum number b) Magnetic Quantum number c) Spin Quantum number d) Subsidiary Quantum number 8. The shape of p-orbital is a) Linear b) Spherical c) Pentagonal d) Dumb-bell 9. Change in Entropy is represented by the symbol a) G b) S

c) H d) E 10. An example for covalent crystal is a) Diamond b) LiF

c) 2Co d) Agcl

11. If the value of H is negative, the process is a) Reversible b) Irreversible c) Exothermic d) Endothermic 12. The resistance of superconductors are a) Zero b) Very high c) High d) None

ST. XAVIER'S COLLEGE (AUTONOMOUS), PALAYAMKOTTAI - 627 002.

SEMESTER EXAMINATIONS – NOVEMBER – 2016 15UCHA31

B.Sc. PHYSICS SEMESTER - III

PAPER : CHEMISTRY-I Time : 3 Hrs. MAX. MARKS: 100

13. Which one is an example for semiconductor? a) Ag b) Cu c) Plastic d) Ge 14. 3AlCl is an example for

a) Lewis base b) Bronsted acid c) Bronsted base d) Lewis acid

15. Lewis bases are__________ doner. a) Proton b) Electron c) Electron pair d) None of the above 16. The oxidation of Manganese in 4KMnO is?

a) +6 b) +9 c) +10 d) +7 17. In flame test strontium give ___________ colour. a) Brick red b) Crimson red c) Apple green d) Bluish green 18. Which one is an interfering acid radical? a) Chloride b) Fluoride c) Bromide d) Nitrate 19. Chemicals used for removal of Ink spots and Ink stains an cotton is a) 2SO b) 3NH

c) Tartaric acid d) 6 6C H

20. An example for medicated soap is a) Dettol soap b) Sodium soap c) Potassium soap d) Sodium oleate

Reg. No. : PART – B

Answer ALL the Questions: (10x2=20) 21. State and explain Heisenberg's Uncertainty principle. 22. What are isotopes and isobars? Give example. 23. Define covalent bond. Give any two examples. 24. Distinguish between sigma and pi bonds.

25. Define pH and pOH. 26. What are oxidizing agent and reducing agent? Give examples. 27. What is mean by enthalpy and entropy? 28. What are crystals? How are they classified? 29. Distinguish between soap and detergents.

30. What are corrosive chemicals and explosive chemicals? Give example.

PART – C

Answer ALL the Questions: (5x6=30) 31. a) Explain the Bohr's theory of an atom.

(OR)

b) What is mean by ionization energy? Explain its periodic trend. 32. a) Draw and explain the M.O diagram of 2H and 2O molecules, calculate its bond

order and explain its magnetic behavior. (OR)

b) What are covalent compounds and ionic compounds? Explain their properties. 33. a) Define Lattice energy. Write a note on Born-Haber cyclic.

(OR) b) i) State and explain first law of thermodynamics.

ii) Explain about enthalpy of reactions. 34. a) Describe the Arrhenius, Bronsted-Lowry and Lewis concepts of acids and bases.

(OR)

b) Briefly explain about oxidation number rules with suitable examples. 35. a) Discuss the elimination of oxalate and phosphate.

(OR) b) Write a brief notes on hazardous chemicals and various first aids used in

chemistry laboratory.

PART – D

Answer ANY THREE Questions: (3x10=30) 36. a) What are quantum numbers? Explain its significance. (5) b) Discuss Modern periodic table. (5)

37. a) Explain VSEPR theory and its applications. (5) b) What is mean by dipolemoment? Mention its applications. (5) 38. a) What are super conductors? Give examples. Explain their applications. (4) b) Describe the various types of crystalline solids with suitable examples. (6)

39. a) What is mean by Buffer solution? How is it classified? (4) b) Explain about effect of solvents and substituent's on relative strengths of acid and bases. (6)

40. a) Explain the cleaning action of soap. (6) b) Explain group separation in inorganic qualitative analysis. (4)

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B.Sc. PHYSICS SEMESTER - III


Reg. No. :

PART – A Answer ALL the Questions: (20x1=20) Choose the correct Answer: Answer

1. The Conjugate base of 3H O

a) H b) 2H O

c) OH d) 2 2H O

2. Which of the following is a hard acid? a) Ag b) Au

c) Li d) Cu

3. The Shape of the 4XeF is

a) Tetrahedral b) Octahedral c) Square planar d) Pyramidal 4. __________ is used to produce sustain powerful superconducting magnets in MRI for clinical diagnosis. a) Helium b) Argon c) Xenon d) Krypton

5. The Hybridisation of 23CO is

a) 3sp b) 2sp

c) sp d) 2dsp

6. The bond order of 2O

a) 1.5 b) 2 c) 2.5 d) 3.5 7. Paramagnetic moment is expressed in a) Debye unit b) Kilojoules c) BM d) Ergs 8. VB theory does not explain the property of complex. a) Geometry b) Magnetic c) Nature of ligand d) All the these above 9. The most important ore of Titanium is a) Bauxite b) Ilmenite c) Zincite d) Azurite 10. The titanium can be purified by a) Froth floatation process b) Van Arkel-de Boer method c) Alumino thermite process d) Monds process 11. The most common oxidation state of lanthanides is a) +2 b) +3 c) +1 d) +4


SEMESTER EXAMINATIONS – NOVEMBER – 2016 12UCH52

B.Sc. CHEMISTRY SEMESTER - V

PAPER : INORGANIC CHEMISTRY-III Time : 3 Hrs. MAX. MARKS: 100

12. _______________ is used in gas lamp materials. a) 2 2CeO and ThO b) 2 3Fe O

c) 2 5N O d) 2MnO

13. Which is the technique to produce nanotube is sizeable quantities? a) Arc discharge b) Laser ablation c) Chemical vapour deposition d) All are correct

14. The chemical bonding of carbon nanotubes is composed entirely by a) sp bonds b) 2sp bonds

c) 3sp bonds d) none of the above

15. Carbon nanotubes are members of which structural family? a) Glycerol b) Polyanilines c) Fullerenes d) Amines 16. The process of synthesis of nano powders is a) Sol-gel process b) Electrodepostion c) Sputtering technique d) All the correct 17. The impurities get entrapped as imperfections within the crystals of the precipitate is called a) Sublimation b) Hydration c) Occlusion d) Post precipitation

18. The solubility product of 2 4Ag CrO is 121.9 10 and its solubility is

a) 57.8 10 moles/litre b) 452.3 10 mole/litre

c) 1253.8 10 moles/litre d) 1051.9 10 moles/litre

19. EDTA is a(an)____________. a) Oxidizing agent b) Reducing agent

c) Masking agent d) none of these above 20. The smaller particles tend to dissolve and reprecipitate one the surface of the larger particles is termed as a) Precipitation b) Agglomeration c) Digestion d) Co-precipitation

Reg. No. :

PART – B

Answer ALL the Questions: (10x2=20) 21. State Arrhenius concept of acids and bases. 22. Give the uses of Neon. 23. Draw the MO diagram of O2. 24. Why 2He is not formed?

25. Lanthanides have a poor tendency to form complexes. Explain. 26. Mention the uses of vanadium. 27. Define nanotechnology. 28. How are the nanoparticles used to eliminate pollutants from the environments? 29. What is meant by digestion of precipitate? 30. Describe the factors governing the solubility of a precipitate.

PART – C Answer ALL the Questions: (5x6=30) 31. a) Discuss Lux-Flood concept of acid and base.

(OR) b) Discuss the structure and bonding in 3XeO .

32. a) Explain the postulates of VB theory.

(OR)

b) Draw the geometry of 3CIF and 3CO . Explain their structure.

33. a) Explain Lanthanide contraction and its consequences.

(OR) b) How is titanium extracted from its ore? 34. a) How do you synthesis nanoparticles by aerosol method?

(OR) b) Explain the optical properties of nanomaterials. 35. a) Write short notes on Co-precipitation.

(OR) b) What are the factors affecting particle size in gravimetric estimation?

PART – D Answer ANY THREE Questions: (3x10=30) 36. Describe in detail how noble gases are isolated from air? 37. a) Distinguish between VBT and MOT. b) Explain the limitations of MO theory. 38. a) Compare the properties of lanthanides and actinides. b) List important uses of lanthanides and actinides. 39. a) Outline the working of TEM. b) Discuss the application of nanoparticles in the following fields. i) Medicine ii) Food

40. Give an account on the followings i) Post precipitation ii) Selective precipitants.

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PAPER : INORGANIC CHEMISTRY-III Time : 3 Hrs. MAX. MARKS: 100

Reg. No. : PART – A

Answer ALL the Questions: (20x1=20) Choose the correct Answer: Answer 1. p-Nitrotoluene undergoes reduction with 4LiAIH to give

a)O-toluene b) p-toluidine c) 2,3 diaminotoluene d) none of these 2. Nitrobenzene fused with KOH a) o-chloronitrobenzene b) o-bromonitrobenzene c) o-nitrophenol d) m-bromonitrobenzene

3. Acetamide reacts with Br2

NaOH to give

a) Methylamine b) Urea c) Ethylamine d) Acetyl bromide 4. Nitro ethane on hydrolysis with hydrochloric acid gives a) Oxalic acid b) Propionic acid c) Formic acid d) Acetic acid 5. Preparation of a diazonium salt from a primary aromatic amine is known as a) Coupling reaction b) Sandmeyer reaction c) Diazotization d) Corey-House synthesis

6. Benzenediazonium chloride reacts with hypophosphorus acid to form. a) Phenol b) Benzaldehyde c) Aniline d) Benzene 7. Diazomethane on reacts with phenol yields a) Methane b) Ethane c) Anisole d) Acetic acid 8. IUPAC name of methyl cyanide is a) acetonitrile b) Propionitrile c) Butyronitrile d) Pentinonitrile 9. 1,4-naphthaquinone on oxidation with acidified 4KMnO , gives

a) Phthalic acid b) Phthalonic acid c) Naphthionic acid d) Benzoinc acid 10. Naphthalene reacts with conc. 2 4H SO at 40oC gives____________

a) Phthlalic acid b) Naphthalenesulphonic acid

c) sulphonic acid d) Phenyl acetic acid

11. Naphthalene undergoes reduction with H2 in the presence of nickel catalyst at high temperature and pressure to give a) Phthalic Acid b) Decalin c) Both a and b d) Tetralin 12. Anthracene undergoes electrophilic substitution reactions mainly at a) C-1 b) C-2 c) C-9 d) C-1 and C-2




PAPER : ORGANIC CHEMISTRY-III Time : 3 Hrs. MAX. MARKS: 100

13. Which of the following is a chromophore? a) 2NO b) 3SO H

c) OH d) COOH

14. Which dyes becomes linked to the fibre by chemical reaction? a) Acid dyes b) Direct dyes c) Disperse dyes d) Vat dyes

15. Fats and Oils are a) Monoesters of glycerol b) Diesters of glycerol c) Triesters of glycerol d) Triesters of glycol 16. Sodium or Potassium salt of fatty acids a) Proteins b) Terpenes c) Alkaloids d) Soaps 17. Which of the following transitions is the highest energy transition?

a) *n to b) *n to

c) *to d) *to

18. ________________ is the IR lighting source for scanning the spectrum of organic compounds? a) Hydrogen lamp b) Cathode lamp c) Nernst glower d) Carbon lamp 19. The red shift is also known as a)Bathochromic effect b) Hypsochromic shift c) Hyperchromic effect d) Hypochromic effect 20. The number of vibrational degrees of freedom for carbondioxide molecule is a) 2 b) 3 c) 4 d) 5


Answer ALL the Questions: (10x2=20) 21. How will you synthesis p-amino phenol from Nitrobenzene? 22. How will you distinguish an aromatic primary amine and an aliphatic amine? 23. Why coupling reaction does not occur in stong alkaline medium? 24. Carry out the following conversions: Benzene diazonium salts to Benzene. 25. Write down the synthesis of Anthrone. 26. Why Electrophilic substitution reaction of Naphthalene occurs mainly at C-1? 27. Explain Oxidative rancidity? 28. What is disperse dyes? Give an example. 29. Write notes on fermiresonance. 30. Define the term 'Auxochrome'.

PART – C

Answer ALL the Questions: (5x6=30) 31. a) i) How will you synthesis o-Nitrophenol from di-nitro benzene? ii) How will you synthesis of azobenzene from nitrobenzene.

(OR) b)Write down the reactions of aniline with 3CH COCl acidified 2 2 7K Cr O and

/3CHCl KOH

32. a) What is proof for the presence of two fused rings in Naphthalene?

(OR) b) How is Anthracene isolated from coal-tar. 33. a) i) How will you convert diazomethane to methyl ether? ii) What happens when methyl isocyanate is treated with amines?

(OR) b) Predict the product and propose the mechanism of the followings: i) Acid chloride + diazomethane ?

ii) Methyl cyanide + / ?2H O H

34. a) Explain the following terms. i) Iodine value ii) Waxes. (OR)

b) i) RM value ii) Vat dyes. 35. a) Explain the Woodward-Fieser rules for calculating max .

(OR) b) Write short note on Finger print region.

PART – D Answer ANY THREE Questions: (3x10=30) 36. i) Why is Aniline more basic than p-nitroaniline? (2+8) ii) Discuss the effect of various substrituents on basic character of amines? 37. i) Outline the synthesis of Urea. (4+6) ii) Explain the synthetic applications of Benzene diazonium salts. 38. Describe the preparation and chemical properties of Anthracene and Alizarin. (5+5).

39. i) Explain the preparations and uses of Indigo dye. (6+4) ii) Write down the preparations of Malachite green and Methyl orange. 40. i) Discuss the principle of UV spectroscopy. (5+5) ii) Explain the different types electronic transition in IR frequency.

***************




PAPER : ORGANIC CHEMISTRY-III Time : 3 Hrs. MAX. MARKS: 100

Reg. No. : PART – A


1. The system that show lower CST only is a) phenol-water b) nicotine-water c) Tri ethylamine-water d) -picoline-water

2. The liquid pair which obeys Raoult's law is a) 2HCl H O b) 6 6 6 5 3C H C H CH

c) 2 5 2C H OH H O d) None

3. The critical solution temperature of phenol-water system is a) 66oC b) 167oC c) 49oC d) 59oC 4. The law which relates the solubility of gas to its pressure is a) Raoult's law b) Distribution law c) Henry's law d) Oswalds's law 5. The solution of sodium acetate in water a) Acidic b) Basic c) Neutral d) Called as a buffer

6. The pH of a solution is 4. Its H is

a) 4M b) 104M c) 10-10M d) 10-4M

7. The pH of the 0.1 M solution of sulphuric acid is a) 1 b) 0.3010 c) 0.699 d) 3.010 8. Ionic product of water is a) 49 b) 14 c) 10-14 d) 10-7 9. What is point group of CHCl3 molecule?

a) 3hD b) 2hD

c) 2vC d) 3vC

10. Point group of CO2 is

a) 2vC b) 2hD

c) 3hC d) 3hD

11. Which one of the following 3vC group?

a) 3POX b)

3CH X

c) 2H O d)

3CHX




PAPER : PHYSICAL CHEMISTRY-II Time : 3 Hrs. MAX. MARKS: 100

12. Which of the following possess identity element? a) 2H b b)

3CHCl

c) 6 6C H d) All the above

13. Wave characteristics of electron particle is due to

a) deBroglie's concept b) Heisenberg's concept c) Sommerfed's concept d) Bohr's concept 14. The Compton effect the scattered X-rays have a) Longer frequency b) Longer wave c) Same wave length d) Same frequency 15. The splitting energy level in the presence of a magnetic field is called a) Zeeman effect b) Stark effect c) Raman effect d) Photoelectric effect 16. The atomic orbital not allowed in quantum theory is a) 3f b) 4p c) 5s d) 4d 17. Number of Vibrational modes of H2O molecule is a) 2 b) 3 c) 4 d) 5 18. Rotational spectroscopy is studied in the region a) Microwave b) Visible c) UV d) UV 19. NMR spectrum is the studies in a) UV region b) Visible region

c) Radio frequency region d) Microwave region 20. ESR spectrum is shown by a) Benzene b) Methane c) Toluene d) Methyl radical

Reg. No. :

PART – B Answer ALL the Questions: (10x2=20) 21. Give examples for ideal and non-ideal solution? 22. Give any two reasons for water as good solvent for ionic crystal? 23. Differentiate strong and weak elecholytes. 24. What is buffer solution? Give examples? 25. What is meant by point groups? 26. Explain Cyclic groups with suitable example. 27. Explain dual characteristics of light. 28. What is orthogonally of wave functions? 29. 12C does not give NMR spectrum but 13C gives why? 30. In IR spectroscopy water is not used as solvent, why?

PART – C Answer ALL the Questions: (5x6=30) 31. a) What is meant by fractional distillation? Explain?

(OR) b) Write a note on steam distillation? 32. a) Differentiate strength and concentration. How will you choose a suitable

indicate TN a titration. (OR)

b) Derive the Henderson-Hasselbalch equation? 33. a) Prove that symmetry operations in water molecule form an abelian group.

(OR) b) Write note on axioms of a mathematical group. 34. a) Prove that linear momentum operator is hermitian

(OR) b) Explain Heisenberg uncertainty principle. 35. a) Describe the fundamental vibrations of carbon dioxide with the aid of diagrams.

(OR) b) What is the important criteria for a molecule to give rotational spectrum?

PART – D

Answer ANY THREE Questions: (3x10=30) 36. What is distribution law? Experimental verification of distribution law? Give limitation of distribution law? Explain the application of solvent extraction? 37. Explain the biological importance of buffer. 38. Write the flow chart to find out point group of a molecule. 39. Derive Plank's radiation Law and prove it is an interpolation of Ray Leigh Jean's Law and Wein's equation.

40. Explain the instrumentation and application of IR spectroscopy.

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PAPER : PHYSICAL CHEMISTRY-II Time : 3 Hrs. MAX. MARKS: 100

Reg. No. :


1. Carbohydrate can be represented by the formula____________. a) 2C H Om n

b) 2C H On m

c) 2 2C H Om n d) None of these

2. Approximately by what factor is the sweetness of saccharin greater than the sugar? a) 5 b) 50 c) 500 d) 1000 3. Which one of the following products is not derived from cellulose? a) Rayon b) Insulin c) Gun cotton d) Paper 4. A reducing sugar will a) Reduce Fehling's solution b) Oxidise Febbig solution c) Not precipitate Tolleri reagent d) A ketone 5. Pyridine is less basic than trimethylamine because the lone-pari of electrons on N-atom is pyridine resides in a) SP2 hybrid orbital b) SP hybrid orbital c) SP3 hybrid orbital d) p-orbital 6. Which one of the following heterocyclic compounds is not aromatic? a) Pyridine b) Pyrrole c) Furan d) Piperidine 7. Which one of the following is not a heterocyclic compound?

N

a)

N

b)

Oc)

s

d)

8. Furan reacts with ammonia in the presence of alumina at 400oC to give__________. a) Pyridine b) Furfural c) Pyrrole d) Furoic acid


SEMESTER EXAMINATIONS – NOVEMBER – 2016 12UCHE51


PAPER : BIOMOLECULES Time : 3 Hrs. MAX. MARKS: 100

9. Proteins are a) Polyamides b) Polymers of ethylene c) -amino carboxylic acid d) Polymers of propylene

10. Upon hydrolysis, proteins give, a) Amino acids b) Hydroxyl acids c) Fatty acids d) Alcohols

11. Precipitation or coagulation of proteins may be caused by a) Heat b) Changes in pH c) Heavy metal salts d) All of these 12. An example of pyridine alkaloid is a) Nicotine b) Coniine c) Quinine d) None of these 13. What is the formula of piperine? a) 17 19 3C H O N b) 19 17 3C H O N

c) 17 18 2C H O N d) none of these

14. On oxidation with chromic acid or nitric acid, the nicotine gives a) Nicotinic b) Nicotinonitrile c) Hygrinic acid d) None of these 15. Menthol heated with potassium hydrogen sulfate and gives a) Menthene b) Methane c) Mentone d) None of these 16. How many known vitamins are these? a) 6 b) 13 c) 19 d) 26 17. The vitamin known as thiamin is also known as a) Vitamin B1 b) Vitamin B2 c) Vitamin B6 d) Vitamin B12

18. Penicillin has_____________ thiazolidine structure. a) -lactam b) -lactam

c) -lactam d) -lactam

19. Sulpha drugs are used as a) Antimalarial b) Analgesic c) Antibacterial d) Antipyretics 20. Glycine results with nitrous acid to form a) Glycolic acid b) Diketo piperazine c) Methylamine d) Ethyl alcohol


Answer ALL the Questions: (10x2=20) 21. What are the main functions of carbohydrates? 22. Write a note on: Killiani Fischer synthesis. 23. How will you prepare quinolin from aniline? 24. Discuss the molecular structure of furan. 25. What are the physical properties of amino acids? 26. Define Zwitter ions. 27. Draw the structure of i) Dipentene and ii) Gernaniol 28. How is nicotine reacted with bromine? 29. Define chemotherapy. 30. What is the structural difference between water-soluble and fat-soluble vitamins?( any two)

PART – C Answer ALL the Questions: (5x6=30) 31. a) starting from glucose how will you Prepare. i) Sorbitol ii) Gluconic acid iii) Fructose

(OR) b) Explain the structure of lactose.

32. a) Discuss the nucleophilic substitution reaction of furfural. (OR)

b) Describe the preparation and its properties of furfural. 33. a) What are peptides? Explain the linkages.

(OR) b) Draw the structure and explain the primary and secondary structure of proteins. 34. a) How will you synthesize i) Piperine from piperic acid ii) Pyridine-2-carboxylic acid from coniine

(OR) b) Discuss the constitution structure of citral. 35. a) What are organic drug? How are they classified? Give an example with structure of each class?

(OR) b) What is an antimalarial? Give the synthesis of three representative antimalarials?

PART – D Answer ANY THREE Questions: (3x10=30) 36. a) Point out the structural difference between starch and cellulose. (5) b) Discuss the structure of sucrose. (5)

37. a) ? 22 2 3 2| |

heatH C C C C H NH H O

pressure

OH OH

(2 marks)


SEMESTER EXAMINATIONS – NOVEMBER – 2016 12UCHE51


PAPER : BIOMOLECULES Time : 3 Hrs. MAX. MARKS: 100

O

+ ?

O

C CH3

O

b)

(2 marks)

o

c) ?H2O

+ ?CHO

(2)

NaOH

s

d) + 4 H

?

?

?

(2 marks)

N

O

KMnO4

? + N

HOOC

HOOC

e)

(2 marks) 38. How the proteins are classified? Discuss the structure and properties of proteins? 39. What happen when: a) pinene is heated with dilute 2 4H SO .

b) Menthol is heated with 4KHSO .

c) Geraniol is oxidized with /2 2 7 2 4Na Cr O H SO .

d) Citral is treated with aq. 2 3Na Co .

40. Describe the synthesize and uses of i) Dettol ii) Burden iii) Penicillin iv) Tetracycline v) Morphine

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Reg. No. :


1. Which of the following has the highest ionization energy? a) Cu b) Ag c) Au d) Na 2. Electron affinity value of which of the following element is almost zero? a) Mg b) He c) Both d) I 3. An element belonging to P block of the periodic table is a) Sodium b) Nitrogen c) Iron d) Lanthanum 4. Which of the following has the smallest covalent radius? a) Be b) B c) C d) N 5. A Covalent bond is formed between two atoms by a) Electron nuclear attraction b) Electron sharing

c) Electron transfer d) Electrostatic attraction 6. An ionic solid is a poor conductor of electricity because a) the charge on ions is unequally distributed b) the charge on ions is small c) ions are not free to move in the solid d) ions do not conduct electricity 7. Which of the following is polar? a) KCl b) LiCl

c) 2CaCl d) HF

8. A covalent bond is present in a) KCl b) LiCl

c) 2CaCl d)

2N

9. Lithium resembles magnesium because their polarizing powers are same. a) Always true b) Always false c) True at high temperature d) True in frozen condition 10. Lithium imparts_________ colour to the flame. a) Golden yellow b) Violet c) Crimson red d) Green 11. Which of the following is not an ore of Lithium?

a) Petalite b) Beryl c) Lepidolite d) Triphyllite



B.Sc. CHEMISTRY SEMESTER - I

PAPER : INORGANIC CHEMISTRY-I Time : 3 Hrs. MAX. MARKS: 100

12. Which of the following is the weakest base? a) Mg(OH)2 b) Ca(OH)2 c) NaOH d) KOH 13. The commonest method for extraction of metals from oxide ores involves. a) Reduction with carbon b) Reduction with hydrogen c) Reduction with aluminium d) Electrolytic reduction

14. A naturally occurring substance from which a metal can be profitably extracted is known as a) Mineral b) Gangue c) Ore d) Flux 15. Suggest a purification method for obtaining ultra pure silicon is a) Zone refining b) Electro chemical refining c) Thermal refining d) Vapour phase refining 16. The element which is found in native state is a) Al b) Mg c) Au d) Fe 17. A reducing agent is a substance which can a) accept electron b) donate electron c) accept proton d) donate proton

18. The reaction e

Na Na is an example for a/an ________ reaction.

a) Oxidation b) Reduction c) Redox d) none 19. The oxidation number of manganese is 4KMnO is

a) 4 b) 6 c) 7 d) 5

20. Which of the following cannot be used as a standard substance? a) 2 2 7K Cr O b) 4KM On

c) 4CuSO d) 2 2 4H C O

Reg. No. :

PART – B Answer ALL the Questions: (10x2=20) 21. Define atomic radius. 22. Electron affinity values of noble gases are zero and those of N and P are very low. Why? 23. How is sigma bond formed? 24. Explain why barium chloride is ionic and beryllium chloride is covalent in nature. 25. Give an account of the preparation of 2 4K SO .

26. What happens when an alkali metal dissolves in ammonia? 27. What is the difference between calcinations and roasting? 28. What is the role of flux in extractive metallurgy? 29. Explain the electronic concept of oxidation with an example. 30. Define Molarity.

PART – C Answer ALL the Questions: (5x6=30) 31. a) i) Define electro negativity ii) How are electro negativity scales determined by (a) Sanderson and (b) Allred Rochow electrostatic method

(OR) b) Define ionization energy. How does it vary along periods and groups in periodic table why? 32. a) Explain the formation of and bonds in N2 .

(OR) b) Explain Fajan's rules with example. 33. a) Explain the role of Na+ and K+ ions in biological systems.

(OR) b) Explain the anomalous begaviour of Lithium. 34. a) Write a note on froth floatation process and leaching.

(OR)

b) Write a note on i) Hydrometallurgy ii) Electrometallurgy. 35. a) Describe the theory of complexometric titrations.

(OR)

b) Balance the following equation by the oxidation number method. 3 2 2CuO NH Cu N H O

PART – D

Answer ANY THREE Questions: (3x10=30) 36. i) Define electron affinity. How do the electron affinity values of elements vary on moving a) Down a group and b) Across a period. Give reasons for the variations. (6) ii) Fluorine has lower electron affinity than chlorine-Explain. (2)



B.Sc. CHEMISTRY SEMESTER - I

PAPER : INORGANIC CHEMISTRY-I Time : 3 Hrs. MAX. MARKS: 100

iii) Electron affinity of beryllium is zero and that of nitrogen is very low- Explain. (2) 37. i) Write a note on dative bond. (4) ii) Compare the properties of covalent and ionic compounds. (6) 38. i) How beryllium is extracted from its ores? ii) Justify the position of Beryllium in II A group of the periodic table.(6)

39. Describe in detail the following general methods of purification of metals with example. i) Electrolytic method ii) Zone refining iii) Vapour phase refining iv) Van Arkel process. (10) 40. i) Describe the theory of dichrometry. (5) ii) Explain the terms oxidizing agent and reducing agent in terms of oxidation number. (2) iii) What is the oxidation number of S in H2SO4. (1) iv) Calculate the normality of oxalic acid solution containing 1.26 gm per liter. (2)

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Reg. No. :

PART – A


1. 2713Al is a stable isotope. 29

13Al is expected to disintegrate by

a) Alpha emission b) Beta emission c) Positron emission d) Proton emission 2. If Uranium (A=238, Z=92) emit an alpha particle, the product has mass number and atomic no. a) 236 & 92 b) 234 & 90 c) 238 & 90 d) 236 & 90 3. Positron has nearly the same weight as that of a) Alpha particle b) Neutron c) Proton d) Electron 4. Geiger-Muller counter is suitable for a) Fast counting b) Extremely fast counting c) Slow counting d) All situation 5. 1 a.m.u= _________ MeV. a) 931.5 b) 900.5 c) 920.5 d) 950.5

6. The most commonly used moderator in nuclear plants is a) Heavy water b) Graphite c) Concrete and brick d) Deuterium 7. Which one of the following isotope has been used for the treatment of leukemia?

a) 3015P b) 14

6C

c) 23892

U d) 13153I

8. What is the principle of a hydrogen bomb? a) Nuclear fission b) Nuclear fusion c) Radioactive decay d) None of the above 9. Inorganic benzene is a) Zeolite b) Silicon c) Carborandum d) Borazine 10. In graphite, carbon atoms are arranged in _______ shape. a) Hexagon b) Trigonal c) Square d) Elliptical 11. Find out the chemical formula of carborandum. a) SiO2 b) SiC

c) SiCl4 d) SiO4



B.Sc. CHEMISTRY SEMESTER - III

PAPER : INORGANIC CHEMISTRY-II Time : 3 Hrs. MAX. MARKS: 100

12. Diboran gives boric acid during________. a) Hydrolysis b) Action with oxygen c) Action with metals d) Action with metals 13. In which reaction does SO4 act as oxidizing agent?

a) Acidified 4KMnO b) Acidified 2 2 7K Cr O

c) Acidified 2 5C H OH d) 2H S

14. There is no S-S bond in

a) 22 4S O b) 2

2 5S O

c) 22 3S O d) 2

2 7S O

15. Ammonia can be dried by

a) 2 4conc.H SO b) 4 10P O

c) CaO d) anhydrous CaCl2

16. Which is the most thermodynamically stable allotropic form of phosphorus? a) Red b) White c) Black d) Yellow 17. What is the colour change observed in flame test for Borate? a) Crimson red b) Apple green c) Bright green d) Bluish green 18. Find out the interfering anion in qualitative inorganic analysis. a) Borate b) Carbonate c) Chloride d) Nitrate 19. Sodium sulphide reacts with sodium nitroprusside to form purple coloured compound. During the reaction, oxidation state of iron

a) Changes from +2 to +3 b) Changes from +3 to +2 c) Changes from +2 to +4 d) Remains unchanged 20. Which of the following sulphides has lowest solubility product? a)FeS b) MnS

c)PbS d) ZnS


Answer ALL the Questions: (10x2=20) 21. Define nuclear fission reaction with suitable example. 22. Write any two differences between chemical reaction and nuclear reaction. 23. Explain the term K-electron capture.

24. A piece of wood was found to have 14

12

c

c ratio 0.7 times that in a living plant.

Calculate the period when the plant died. Hslf-life of C14=5760 years. 25. BF3 exists but BH3 does not exist. Account for that. 26. CCl4 resists hydrolysis while SiCl4 gets readily hydrolysis. Account for that.

27. How do you prepare hydrazine?

28. Write an equation for auto ionization of liquid 3NH and 2SO .

29. Write sodium nitroprusside test with equation for sulphide.

30. Define common ion effect with example.

PART – C

Answer ALL the Questions: (5x6=30) 31. a) Define the following term with suitable example. (2+2+2)

i) Isotope ii) Isobar iii) Isotone (OR)

b) Calculate the mass defect and the binding energy of the helium nucleus having a mass of 4.0039 a.m.u. given that masses of proton and neutron are 1.00758 & 1.00893 a.m.u respectively.

32. a) What are harmful effects of radiation hazards? How do you prevent that?

(OR)

b) Give a detailed description of induced radioactivity.

33. a) Discuss the structure and bonding of Diborane. (OR)

b) Discuss the structure of borazine. 34. a) How do you prepare the following compounds?

i) Cyanogens ii) Dithionic acid iii) Hydroxylamine. (OR)

b) Discuss the chemical action of nitric acid with the following metals. i) Zinc ii) Copper iii) Gold (2+2+2)

35. a) Write a note on the following tests. (1.5x4=6) i) Boron trifluoride test ii) Ethyl borate test iii) Ammonium molybate test iv) Chromyl chloride test

(OR) b) i) What is solubility product? (2+4)

ii) Calculate the solubility of silver chromate, 2 4Ag CrO in mole per liter if

the solubility product of 2 4Ag CrO is 121.9 10

PART – D Answer ANY THREE Questions: (3x10=30) 36. a) Describe the properties of alpha ray. (3)

b) How do you detect radioactive ray by using Geiger-Muller counter. (7) 37. Describe important application of radio isotopes. 38. Classify silicate into different types. Give the composition and structure of each type silicate.

39. Discusses the structure of the following interhalogens. (1+3+3+3)

a) CIF b) CIF3 c) IF5 d) 4ICl 40. How the following radicals are responding to 2 4dil.H SO test? Explain with

equation. a) Carbonate b) Bicarbonate c) Sulphide d) Sulphite e) Nitrite

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B.Sc. CHEMISTRY SEMESTER - III

PAPER : INORGANIC CHEMISTRY-II Time : 3 Hrs. MAX. MARKS: 100

Reg. No. :

PART – A


1. The valency of Aluminium is a) 4 b) 2 c) 3 d) 1 2. A co-ordinate bond is formed by a) Complete transfer of electrons b) Sharing of electrons contributed by both the atoms. c) Sharing of electrons contributed by one atom only d) None of the above 3. The axial overlap between the two orbitals leads to the formation of a a) Sigma bond b) Pi bond c) Multiple bond d) Triple bond 4. According to VSEPR theory, the structure of 2H Omolecule has_______

structure. a) Tetrahedral b) Pyramidal c) Bent or angular d) Linear 5. The oxidation number of chromium in 2 7K CrO is

a) +6 b) +5 c) +3 d) +4 6. Oxidation means a) Gain of electrons b) Loss of electrons c) Loss of neutrons d) Loss of protons 7. According to Lewis concepts acids are a) Proton donors b) Proton acceptors c) Electron pair acceptors d) Electron pair donors

8. H OHp p ?

a) 13 b) 15 c) 14 d) 19 9. Which one is polar molecule? a) H-Cl b) Chloroform c) Acetone d) Benzene 10. London forces are present ins a) 2H b) 2N

c) ,He Ar and Ne ect d) All the above

11. The unit of equivalent conductance is

a) 1 2 1ohm cm equv b) 2 1ohm cm

c) 1 2ohm cm d) 1 2 1ohm cm mole



B.Sc. BOTANY & ZOOLOGY SEMESTER - I


12. Charge is measured in a) Coulomb b) Ampere c) ohm and volt d) All the above 13. The IUPAC name of 3CH CHO is

a) Pentanal b) Propanal

c) Ethanal d) Methanal 14. What happens when acetaldehyde is treated with moist chlorine at ordinary temperature? a) Trichloro acetone is formed b) Chloral is formed c) Semi carbazone is formed d) Diacetone alcohol is formed 15. Formalin is nothing but ___________ % aqueous solution of formal dehyde. a) 50% b) 70% c) 40% d) 90% 16. 6 5 2C H CONH is

a) Methanamide b) Benzamide c) Ethanamide d) Propananmide 17. The functional groups present in amino acids are a) Amine and alcohol b) amine and ester c) Aldehyde and ketone d) Amine and carboxylic acid 18. When two amino acids combine, the product formed is called? a) Monopeptide b) Polypeptide c) Tripeptide d) Dipeptide 19. 1o amine reacts with nitrous acid to form a) Alcohols and N2 gas b) Alcohols and O2 gas c) Alcohols and Cl2 gas d) Yellow oils 20. ______________ amine answer carbylamines reaction. a) Quarternary ammonium salts b) Primary c) Secondary d) Tertiary

Reg. No. :

PART – B Answer ALL the Questions: (10x2=20) 21. What is meant by variable valency? Give two examples 22. What is meant by covalent compound? 23. What is the oxidation number of Cl in

i) 4HClO ii) 2 7Cl O iii) 3ClO

24. Define the term solubility product. 25. What is mean by electrolysis? 26. Define the term specific conductance and equivalent conductance. Mention their units. 27. What happens when aldehyde and ketones are treated with i) HCN and ii)

Phynyl hydrazine? 28. What do you mean by cannizzaro reaction? 29. What are amines? How are they classified? Give an example for each type. 30. What is mean by carbylamines reaction and Diazotization?

PART – C Answer ALL the Questions: (5x6=30) 31. a) State and explain Fajan's rule.

(OR) b) What is mean by hybridization? Explain sp3 hybridization that exists in CH4 molecule.

32. a) Discuss Redox process in terms of oxidation number and in terms of electron transfer.

(OR) b) Explain the Arrhenius concepts, Lowry-Bronsted concepts of acids and bases with suitable examples.

33. a) What is mean by hydrogen bonding? How is it classified? Give an example for each type.

(OR) b) Explain the influence of hydrogen bonding on boiling points and

solubility. 34. a) What are amides? How are they classified? Distinguish between benzamide and acetamide.

(OR) b) Compare Benzaldehyde with Acetaldehyde.

35. a) Explain any five reactions of aniline. (OR)

b) What are peptides and polypeptides?

PART – D Answer ANY THREE Questions: (3x10=30) 36. a) Discuss VSEPR theory with suitable examples. (5) b) What are the important properties of ionic compounds and covalent compounds? (5) 37. a) What is mean by common ion effect? (4)

b) What are interfering acid radicals? Give any four examples. How are they eliminated? (6) 38. a) State and explain Faradays laws of electrolysis. (4) b) What are polar and non-polar molecules? Explain With suitable examples. (6)

39. a) Distinguish between Benzoic acid and Acetic acid. (5)

b) What is mean by Hell-Volhard-Zelinsky reaction and Perkin reaction? (5) 40. a) Explain the basic nature of amines. (5)

b) What are amino acids? How are they classified? Explain the terms: Zwitter ions and isoelectric. (5)

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B.Sc. BOTANY & ZOOLOGY SEMESTER - I


Reg. No. :


1. Average velocity of a gas molecule is inversely proportional to a) Temperature b) Molecular weight c) Mass d) Density 2. The pressure cooker reduces cooking time because a) The higher pressure tenderizes the distributed b) The boiling point of the water inside is elevated c) The heat is more evenly distributed d) A larger flame is used 3. Van der Waals proposed two corrections a) Pressure correction, volume correction b) Pressure correction, temperature correction c) Concentration, temperature d) Pressure, concentration 4. Kinetic theory of gases was proposed by a) Andrews b) Joule

c) Bernoulli d) Van der Waals 5. Tyndall effect is shown by a) Water b) KCl solution c) FeCl3 d) milk

6. The difference between crystalloid and colloid is of a) Solubility b) Diffusion c) Particle size d) Chemical composition 7. Peptization refers a) Digestion of food b) Hydrolysis of protein c) Breaking and dispersion into the colloidal state d) None of these 8. Which is used for producing artificial rain a) Silver nitrate b) Silver chloride mercury c) Chloride d) Silver iodide 9. Which of the following compounds will not have zero dipole moment value? a) 2SO b) 4CH

c) 3BF d) 2CO

10. Iron and Cobalt are examples of a) Diamagnetic b) Paramagnetic

c) Ferromagnetic d) Antiferri magnetic




PAPER : PHYSICAL CHEMISTRY-I Time : 3 Hrs. MAX. MARKS: 100

11. Identify the molecule having dipole moment? a) 4CCl b) 3CHCl

c) 2CO d) all the above

12. The magnetic moment of a molecule is expressed a) Magnetic tons b) Magnetons

c) Debye unit d) 1.secg

13. Number of phases in a mixture of He and H2 gas is a) 1 b) 2 c) many d) zero 14. Mathematical formation of phase rule is a) F=C+P+2 b) F=C+P+1 c) F=C-P+1 d) F=C-P+2 15. Sodium chloride-water system is an example of a) Binary system b) Freezing mixture c) Eutectic mixture d) All of these 16. The degree of freedom at triple point of water is a) 1 b) 2 c) 0 d) 3 17. The equation shows the homogenous equilibrium is a) 5( ) 3 2PCl PCl Clg g b) 4 ( ) 3( ) (1)( )NH Cl NH HCs g g

c) 3( ) ( ) 2( )CaCO CaO COs s g d) 4 ( ) 3 2 ( )2NH S NH H Ss g g

18. The equation that shows the relative between Kp and Kc is

a) Kp 1/Kc b) Kp Kc( ) nRT

c) Kp 1/RT Kc d) None

19. The equation that shows heterogeneous equilibria is a) ( ) ( ) 2 ( )2 2H g I g HI g b) ( ) 2 ( )2 4N O g NO g

c) 2 ( ) ( ) 2 ( )2 2 3SO g O g SO g d) ( ) ( ) ( )4 3NH Cl s NH g HCl g

20. The value of Kc for the equilibrium 22 2H I Hl is 40 at 1 atm. What is the

Kp value of the equilibrium at 2 atm pressure? a) 80 b) 20 c) 60 d) 40

Reg. No. :

PART – B Answer ALL the Questions: (10x2=20) 21. Define collion frequency. 22. Calculate the RMS velocity of O2 at 25oC. 23. Mention any two application of liquid crystal. 24. Define gel. Mention its uses. 25. What is polarisibility of molecules? 26. Define dipole moment. Give its unit. 27. Give examples of simple eutectic system of two components. 28. Draw the phase diagram of Ag-Pb system. 29. Define equilibrium constant. 30. Explain reversible reaction with suitable examples.

PART – C Answer ALL the Questions: (5x6=30) 31. a) State Maxwell's distribution law. Give its applications.

(OR) b) Write briefly on principle of equipartition of energy. 32. a) Discuss theory of liquid crystals?

(OR) b) Distinguish between colloid sol, suspension and emulsion? 33. a) Write a note on pare, dia and ferro magnetism?

(OR) b) Write briefly on magnetic permeability and magnetic susceptibility? 34. a) Draw and explain the phase diagram of water system?

(OR) b) Discuss any one two component phase diagram? 35. a) State and explain Lechatelier's principle with suitable examples.

(OR) b) Derive thermodynamically the law of mass action.

PART – D Answer ANY THREE Questions: (3x10=30) 36. Write a note on i) viscosity of gases ii) Distinguish between collision number and collision frequency? 37. Write note on i) Tyndall effect ii) Brownian motion iii) Hardy-Schulz law iv) gold number. 38. Derive Clauseius mosotti equation? How will you determined the dielectric constant? 39. Draw the phase diagram of

2KI H O system and explain? What are the

principles involved in freezing mixture?

40. Derive Vant Hoff isochore and discuss the applications.

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PAPER : PHYSICAL CHEMISTRY-I Time : 3 Hrs. MAX. MARKS: 100

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