GUESS PAPER
CHEMISTRY
SOLID STATE
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Define the term amorphous solids. Give a few
examples of amorphous solids.
Ionic solids are hard and brittle. Explain.
What effect do mechanical pressure and electric field
have on a piezoelectric crystal?
Sodium chloride is doped with 102 mole percent of
SrCl2. Find the concentration of cation vacancies.
Why is the coordination number of 12 not found in ionic
crystals ?
Give reasons for non-stoichiometric sodium chloride is
a yellow solid.
Give reasons for Cation vacancies in some crystals
make them good catalysts.
Electrical conductivity of copper decreases with
increase in temperature, whereas of NaCl increases.
Explain.
Diamond and rhombic (solid) sulphur both are covalent
solids, the later has very low m.pt. in comparison to
diamond. Explain.
Covalent bonding occurs in the molecular and covalent
network solids. Why do these two kinds of solids differ
so greatly in their hardness and melting point ?
If NaCl a doped with 103 mol% of SrCl2, what is the
concentration of cation vacancies ?
The first order diffraction of X-rays from a certain set of
crystal planes occurs at an angle of 11.8o from the
planes. If the planes are 0.281 nm apart, what is the
wavelength of X-rays ?
Analysis shows that nickel oxide has formula Ni0.98O1.00.
What fractions of nickel exist as Ni+2 and Ni+3 ions ?
If the radius of the octahedral void is r and radius of the
atoms in close packing is R, derive relation between r
and R.
Ferric oxide crystallizes in hexagonal close packed
array of oxide ions with two out of every three
octahedral holes occupied by ferric ions. Derive the
formula of the ferric oxide.
Br ions form close packed structure. If the radius of Br 
ion is 195 pm, calculate the radius of the cation that just
fits in the tetrahedral hole.
Can a cation A+ having a radius of 82 pm be slipped
into the octahedral hole of the crystal A+ Br ?
Calcium chloride crystallizes as a body centred cubic
lattice and has a density of 4.0 g cm 3. Calculate the
length of the edge of the unit cell of calcium chloride
crystal
[Molar mass of
CaCl = 168.5 g mol1,
NA = 6.02  1023 mol1]
Account for the following :
(a) Silicon is an insulator but silicon doped with
phosphorus acts as a semiconductor
(b) Some of the glass objects recovered from ancient
monuments look milky instead of being
transparent?
State the difference between schottky and frenkel
defects. Which of these two changes the density of the
solid ?
FCC structure possesses the closest packing of atom
in it.
21. Aluminium crystallizes in a cubic close-packed
structure. Its metallic radius is 125 pm.
(a) What is the length of the side of the unit cell ?
(b) How many unit cells are there in 1.00 cm 3 of
aluminium ?
22. Explain the following terms with suitable examples
(a) F-centres
(b) Ge doped with in
(c) ferrimagnetism
(d) antifluorite structure (e) between a conductor and
a semiconductor
23. Which point defect may lower the density of an ionic
crystal?
24. What are the lattice imperfection found in crystals?
25. What is space lattice and crystal lattice?
26. What are the co-ordination numbers of each of the
ions present in the cubic close packed structure of
Na2O at ordinary temperature and pressure?
27. The ionic radii of Rb+ and Br- are 147 and 195 pm
respectively. Deduce the most probable coordination
number of Rb+ ion in RbBr.
28. If the radius of Cs+ is 169 pm and that of Cl- is 181
pm predict the structure of CsCl.
29. Why is the window glass of the old building thick at
the bottom?
30. What is Curie point and Neel’s point?
31. When excess of sodium is burnt in chlorine, we get
yellow sodium chloride instead of white sodium
chloride. Why?
32. Why
are
the
solids
containing
F-centres
paramagnetic?
33. Schottky defect lowers the density of the crystal but
frenkel defect does not. Discuss.
34. Discuss the main features of calcium fluoride
(Fluorite) structure.
35. Give four points of difference between crystalline
solids and amorphous solids.
36. With the help of electron spin, clearly distinguish
between Ferromagnets, Antiferromagnets and
Ferrimagnets.
37. What are pseudosolids? Give two examples.
38. CsCl has bcc arrangement and its unit cell edge
length is 400 pm. Calculate the interionic distance
(nearest neighbour distance) in CsCl.
39. A sample of a crystalline solid scatters a beam of Xrays of wavelength 70.93 pm at an angle 2 of
14.660. If this is a second order reflection (n = 2),
calculate the distance between the parallel planes of
atoms from which the scattered beam appears to
have been reflected.
40. In a cubic close packed structure of mixed oxides, the
lattice is made of oxide ions, one eighth of tetrahedral
voids are occupied by divalent ions (A2+) while one
half of the octahedral voids are occupied by trivalent
ions (B3+). What is the formula of the oxide?
41. What is the distance between Na+ and Cl- ions in a
NaCl structure, if its density is 2.165 g cm -3? NaCl
crystallizes in fcc lattice.
42. Differentiate
n-type
and
p-type
extrinsic
semiconductors.
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43. The composition of a sample of wustite is Fe0.93O1. 0. 44. Derive the relationship between the radius (r) of the
What percentage of the iron is present in the 0form of
tetrahedral void and hcp structure”. Do you agree
Fe (III)?
atoms in close packing.
DILUTE SOLUTION
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How is it that alcohol and water are miscible in all
proportions?
What are isotonic solutions? Give example.
Differentiate between boiling point and normal boiling
point.
Name two natural semipermeable membranes.
After removing the outer shell of two eggs in dill. HCl,
one is placed in distilled water and the other is placed
in a saturated solution of NaCl. What will you observe
and why?
What do you expect to happen when Red Blood
Corpuscles (RBS’s) are placed in
(i) 1% NaCl solution
(ii) 0.5% NaCl solution?
What happens if pressure greater than osmotic
pressure is applied on the solution separated by a semi
permeable membrane from the solvent?
When fruits and vegetables that have dried are placed
in water, they slowly swell and return to the original
form. Explain why? Would a temperature increase
accelerate the process? Explain.
Why it is advised to add ethylene glycol to water in a
car radiator while driving in a hill station?
Why camphor is preferred as a solvent in finding the
molecular mass of naphthalene by Rast method?
Equimolal solutions of NaCl and BaCl2 are prepared in
water. Freezing point of NaCl is found to be –20C.
What freezing point you expect for BaCl2 solution?
What are azeotropic mixtures? What are its types?
Show how molecular mass of a solute can be
calculated from elevation in boiling point of the solution.
When fruits and vegetables that have dired are placed
in water, they swell and return to original form. Why?
Would a temperature increase accelerate the process?
Explain.
“Vapour pressure of the solution is less than the vapour
pressure of the pure solvent.” Comment on the
statement.
What care is generally taken during intravenous
injections and why?
Which solution is more concentrated 1 molal or 1
molar, why?
An antifreeze solution is prepared from 222.6 g of
ethylene glycol –C2H4(OH)2 and 200 g of water.
Calculate the molality of the solution. If the density of
the solution is 1.072 g mL-1, then what shall be the
molarity of the solution?
200 cm3 of an aqueous solution of a protein contains
1.26 g of the protein. The osmotic pressure of such a
solution at 300 K is found to be 2.57 × 10-3 bar.
Calculate the molar mass of the protein
The partial pressure of ethane over a saturated
solution containing 6.56 × 10-2 g of ethane is 1 bar. If
the solution contains 5.00 × 10-2 g of ethane, then what
shall be the partial pressure of the gas.
Why do you get sometimes abnormal molecular
masses of the substance by using colligative properties
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of the solution? State the factors with examples
which produce abnormality in the result.
(i) Which colligative property is preferred for the
molar mass determination of macromolecules and
why?
(ii) A solution containing 10.2 g glycerine per litre of
a solution is found to be isotonic with 2.0% solution of
glucose (molar mass 180). Calculate the molecular
mass of glycerine.
What is binary solution?
Define azeotropic mixture.
Define molal depression constant or cryoscopic
constant.
What helps in the existence of aquatic life?
Define saturated, unsaturated and suspersaturated
solution.
Do solids exert vapour pressure?
what will happen, when outer shell of an egg
dissolved in hydrochloric acid and then placed in
concentrated sodium chloride solution?
Why does chemist prefer to refer concentration of
solution in terms of molality?
Why is an increase in temperature observed on
mixing chloroform with acetone.
When is the value of van’t Hoff factor more than one.
(i) State Henry’s law.
(ii) Mention some of its important applications.
Concentrated nitric acid used in the laboratory work
is 68% nitric acid by mass in aqueous solution. What
should be the molarity of such a sample of the acid if
the density of the solution is 1.504 g mL-1?
18 g of glucose C6H12O6 is dissolved in 1 kg of water
in a saucepan. At what temperature will the water boil
(1.013 bar pressure)? Kb for water is 0.52 K kg mol-1.
A 5% solution (by mass) of cane sugar in water has
freezing point of 271 K. Calculate the freezing point
of 5% glucose in water if freezing point of pure water
is 273.15 K.
The boiling point of benzene is 353.23 K. When 1.80
g of a non-valatile solute is dissolved in 90 g of
benzene, the boiling point is raised to 354.11K.
Calculate the molar mass of the solute. Kb for
benzene is 2.53 K kg mol-1.
What is antifreeze? Which substance is used as
antifreeze?
Give three examples of each for solutions
(i) Showing positive deviation
(ii) Showing negative deviation.
What are van’t Hoff laws? Derive van’t Hoff equation
for dilute solutions.
How will you determine the molecular mass of a
substance using osmotic pressure method?
Calculate the mole fraction of rectified spirit (95%
ethyl alcohol by mass).
A 5% solution of cane sugar (Mol. Wt. 342) is isotonic
with 0.877% solution of urea. Find the molecular wt.
of urea.
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44. (i) How will you determine the molecular mass from the
relative lowering of vapour pressure?
(ii) At 298 K, the vapour pressure of water is 23.75
mm Hg. Calculate the vapour pressure at the same
temperature over 5% aqueous solution of urea
[Co(NH2)2].
ELECTROCHEMISTRY
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Rusting of iron is quicker in saline water than in
ordinary water. Why is it so?
In operation of a galvainic cell, at one its electrodes
oxidation takes place. What is the name of this
electrode and what is its polarity?
Why is it that aluminium metal cannot be obtained by
the electrolysis of an aqueous solution of a salt of
aluminium?
What would happen if the protective tin coating cover
an iron bucket is broken in some places?
Give an example of “fuel cells”.
What is the relationship between cell potential and
equilibrium constant.
Give a brief account of corrosion and its mechanism.
State and explain Faraday’s law of electrolysis.
How much electricity is required in coulomb for the
oxidation of
(i) 1 mol of H2O to O2
(ii) 1 mol FeO to Fe2O3
What is over voltage?
What is mercury cell? Give the electrode reactions.
Three electrolytic cells A, B, C containing solution of
ZnSO4, AgNO3 and CuSO4, respectively are connected
in series. A steady current of 1.5 amperes was passed
through them until 1.45 g of silver deposited at the
cathode of cell B. How long did the current flow? What
mass of copper and of zinc were deposited?
Explain the difference between electromotive force and
potential difference.
Calculate the number of molecules of sulphuric acid in
300 cm3 solution whose resistance has been found to
be 30 ohms in a conductivity cell constant is 0.5 cm -1.
The equivalent conductance is 50 S cm 2 eq-1.
1
3

1
2

15. Given m  Al3   = 63 S cm2 mol-1 and m  SO24  = 80
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21.
m

S
Calculate
[ Al2 (SO4 )3 ] .
Calculate equilibrium constant for the reaction at 298 K:
4Br- + O2 + 4H+  2Br2 + 2H2O
Given that E0cell = 3.17 V.
Calculate G0 for the reaction
(i) Fe3+ + 3e-  Fe(s) ; E0 = 0.036 V
(ii) 1/3 Fe3+ + e-  1/3 Fe(s)
The conductivity of 0.001028 M acetic acid is 4.95 ×
10-5 S cm-1. Calculate its dissociation constant if 0 for
acetic acid is 390.5 S cm 2 mol-1.
A solution of CuSO4 is electrolyzed for 10 minutes with
(b) The molar conductivity of 0.02 M NaCl solution in
a current 1.5 amperes. What is the mass of copper
S m2 mol-1. Given that the conductivity of 0.1 M
deposited at the cathode.
KCl solution at 298 K is 1.29 S m -1.
Calculate 0 for CaCl2 and MgSO4 from the following 35. The conductivity of a solution containing 1 gram of
data:
anhydrous BaCl2 in 200 cm3 of water has been found
0Ca + 2 = 119.0 S cm2 mol-1
to be 0.0058 S cm-1. What are the molar conductivity
0Cl- = 76.3 S cm2 mol-1
and equivalent conductivity of the solution? (At. wt. of
0Mg+2 =106.0 S cm2mol-1
Ba = 137 and Cl = 35.5).
0SO2-2 160 S cm2mol-1
36. At 291 K, the molar conductivities at infinite dilution of
Calculate the potential (e.m.f.) of the cell
NH4Cl, NaOH and NaCl are 129.8, 217.4 and 108.9
Cd | Cd2+ (0.10 M) | | H+ (0.20M) | Pt, H2 (0.5 atm)
ohm-1 cm2 respectively. If the molar conductivity of a
cm2
16.

(Given E0 for Cd2+ | Cd = -0.403 V, R = 8.314 JK-1 , F
=
96,500 C mol-1)
22. Calculate the e.m.f. of the cell at 250C
Mg(s) | Mg2+ (0.10 M) | | Ag+ (1.00 × 10-4 M) | Ag (s)
Where E0cell = 3.17 V
23. What do you mean by disproportionation reaction?
24. What is the theoretical efficiency of fuel cell? What
value of if has practically attained?
25. Can we use direct current for experimental
determination of resistance of a solution?
26. How can the standard oxidation potential of an
electrode be raised up?
27. Why does voltage of calomel electrode remain
constant throughout its life time?
28. What happens to free energy during operation of a
cell?
29. Why a salt bride is not necessary in lead storage
cell?
30. What changes would be observed if
(a) Solution of NaCl is made acidic before
electrolysis?
(b) Copper anode in a Cu plating cell is replaced by
Zn?
31. Corrosion of motor cars is of greater problem in
winter when salts are spread on road to melt ice and
snow, why?
32. Colour of KI solution containing starch turns blue
when Cl2 water is added. Explain.
33. A cell utilizes the following reaction:
2Co3+(aq) + Zn(s)  2Co2+(aq) + Zn2+ (aq)
What is the effect on cell emf of each of the following
changes?
(a) Co(NO3)2
is
dissolved
in
the
cathodic
compartment
(b) Co(NO3)3
is
dissolved
in
the
cathodic
compartment
(c) The size of Zn(s) electrode is doubled
(d)Additional water is added to the anode
compartment
34. The resistance of a conductivity cell with 0.1 M KCl
solution is found to be 200 at 298 K. When the
same cell is filled with 0.02 M NaCl solution, the
resistance at the same temperature is found to be
1100. Calculate
(a) The cell constant of the cell in m -1
mol-1.
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BRILLIANT
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ohm -1
cm2,
centinormal solution of NH4OH is 9.33
what
(ii) Standard electrode potential
is the percentage dissociation of NH4OH at this 42. (i) Can a copper spoon be used to stir a solution of
dilution? Also calculate the dissociation constant of
zinc sulphate? Support your answer with reason:
NH4OH.
= + 0.34 V ; E 0  2
= -0.76 V
E 0 2
37. What is the difference between electrochemical cell
Cu / Cu
Zn / Zn
and electrolytic cell?
(ii) Why are Co3+ salts unstable in water?
38. Silver is electrodeposited on a metallic vessel of 43. A 100 watt, 110 volt incandescent lamp is connected
surface area 800 cm 2 by passing a current of 0.2
in series with an electrolytic cell containing cadmium
ampere for 3 hours. Calculate the thickness of silver
sulphate solution. What weight of cadmium will be
deposited (Density of Ag = 10.47 g/cm and atomic
deposited by the current flowing for 10 hours?
mass = 108 g mol-1)
44. (i) Derive a relationship between free energy change
39. In a dry cell, ammonia liberated by the reaction
and equilibrium constant for the redox reaction
Zn(s) + Cu2+ (aq)
Zn2+ (aq) + Cu(s)
Zn + MnO2 + 4NH 4 + 2e- zn2++ Mn2+ + 2H2O + 4NH3
(ii) Show that the equilibrium constant of a weak
does not build up a gas pressure. Why?
electrolyte is given by the expression
40. Why blocks of magnesium are often strapped to the
X2m
steel hulls of ocean-going ships?
K=
41. Define (i) Reference electrode
m ( m   m )
CHEMICAL KINETICS
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7.
The reaction A + B  C has zero order, write its rate
equation.
For the assumed reaction X2 + 3Y2  2XY3, write the
rate equation in terms of the rate of disappearance of
Y2.
How is rate constant related to concentration of the
reactants?
Express the relationship between the rate of production
of water and the rate of disappearance of oxygen in the
following reaction : 2H2 + O2  2H2O.
For the reaction : 2A + B + C  A2B + C
the rate = k [A] [B]2 with k = 2.0 × 10-6 M-2 s-1.
Calculate the initial rate of the reaction when [A] = 0.1
M, [B] = 0.2 M and [C] = 0.8 M.
A reaction is second order with respect to a reactant.
How is the rate of reaction affected if the concentration
of the reactant is doubled?
How can you study/measure the rate of following
reaction?
CH3COOH (aq) + CH3OH (aq)  CH3COOCH3 (aq) + H2O(l)
8.
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Out of the two, temperature and intensity of light, which
affects the rate of photochemical reaction?
What is photosensitizer? Name the photosensitizer in
photosynthesis by plants.
For
certain
photochemical
reactions
(e.g.,
Photosynthesis in plants) G is positive. Why?
What aspect of a reaction is influenced by presence of
catalyst which increases the rate or possibility of the
reaction?
In a reaction between A and B, the initial rate of
reaction
was
measured
for
different
initial
concentrations of A and B as given below: What is the
order of reaction with respect to A and B?
A/M
0.20
0.20
0.40
B/M
0.30
0.10
0.05
r0/Ms-1
5.07 × 10-5 5.07 × 10-5
7.6 × 10-5
The decomposition of dimethyl ether leads to the
formation of CH4, H2 and CO and the reaction rate is
given by Rate = k[CH3OCH3]3/2
The rate of reaction is followed by increase in pressure
in a closed vessel and the rate can also be expressed
in terms of the partial pressure of dimethyl ether i.e.,
rate = k(pCH3OCH3)3/2.
14. What are pseudounimolecular or psedo first order
reaction? Give two examples.
15. Define Quantum yield or Quantum efficiency. Why
Quantum yield of H2 and Cl2 reaction is very high
while that H2 + Br2 reaction is very low?
16. Give
the
points
of
difference
between
thermochemical
reactions
and
photochemical
reactions.
17. Give reasons for the following:
(a) On the basis of heat of combustion values,
graphite is more stable than diamond. However,
diamond does not change into graphite for years
together.
(b) Explosives release a lot of energy on heating or
when hit, yet they can be stored confidently for
long time.
18. How does a photosensitizer differ from a catalyst in
action?
19. Show that time taken to complete 99.9% of a first
order reaction is 10 times the time taken to complete
half of the reaction.
20. The thermal decomposition of 1 mol of ditert-butyl
peroxide in gaseous phase 2 moles of acetone and
one mole of ethane at constant volume. If the
reaction is of first order, write the equation relating
rate constant, initial pressure.
21. In the Arrhenius equation for a certin reaction, the
values of A and Ea are 4 × 1013s-1 and 98.6 kJ/mol
respectively? If the reaction is of first order, at what
temperature will its half life period be 10 min.?
22. The reaction A + 2 B  C + D obeys the rate equation:
Rate = k [A]x [B]y
What would be the order of this reaction?
23. Calculate the half life period of a first order reaction
when the rate constant is 5 year-1.
24. What is the difference between average rate and
instantaneous rate of a chemical reaction ?
26. Express the relationship between the rate of
production of iodine and the rate of disappearance
of hydrogen iodide in the following reaction :
2HI  H2 + I2
27. A reaction is 50% complete in 2 hours and 75%
complete in 4 hours. What is the order of reaction ?
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28. Define activation energy of a reaction.
29. The rate of decomposition of a substance A becomes
eight times when its concentration is doubled. What is
the order of this reaction ?
30. For the reaction A  B, deduce the integrated form of
rate of law.
31. Differentiate between :
(i) rate of reaction and rate constant of a reaction.
(ii) order of a reaction and its molecularity.
32. Show graphically how the rate of a first order reaction
with only one reactant depends upon the concentration of the reactant.
33. What are photochemical reactions ? Give one exam-ple
to illustrate the course of a photochemical reaction.
34. State the role of activated complex in a reaction and
state its relation with activation energy.
35. Mention the factors that affect the rate of a chemical
reaction.
36. A reaction is first order in A and second order in B.
(i) Write differential rate equation.
(ii) How is the rate affected when the concentration of B
is tripled ?
37.
38.
39.
40.
41.
42.
43.
44.
(iii) How is the rate affected when the concentration of
both A and B is doubled ?
What are the two necessary conditions for the
colliding molecules to yield product ?
What is meant by an elementary reaction ?
Define the order of the reaction.
Can we have fractional, negative or zero order of a
reaction ?
Which step is the rate determining step in a reaction
and why ?
What is the temperature coefficient of a reaction ?
What is its value for most of the reactions.
(a) What are the units of the rate constant in
(i) A zero order reaction (ii) A first order reaction
(iii) A second order reaction
(b) Given an example of pseudo first order reaction.
A first order reaction is 20% complete in 20 minutes.
Calculate the time taken for the reaction to go to 80%
completion.
The rate of a particular reaction doubles when
temperature changes from 27°C to 37°C. Calculate the
energy of activation for such a reaction
(R = 8.314 JK-1 mol-1)
SURFACE CHEMISTRY
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22.
What is Brownian movement due to?
What is the meant by “shape selective catalysis?”
What are micelles? How do they differ from a normal
colloidal solution?
Differentiate between adsorption and absorption.
A sol may be prepared by a precipitation reaction. Give
one such example. How can we find the nature of
electrical charge on the sol particles?
What are emulsions? Describe different types of
emulsions with examples. State any two applications of
emulsions.
How is the physically adsorbed mass of a gas on a unit
mass of adsorbent related to the pressure of the gas?
What is hydrosol?
Give reason why a finally divided substance is more
effective as an adsorbent.
What are multimolecular and macromolecular colloids?
Write four differences between physical adsorption and
chemisorption.
What is an adsorption isotherm? Distinguish between
Frendlich adsorption isotherm and Langmuir adsorption
isotherm.
What do you understand by activation of adsorbent?
How is it achieved?
Give two chemical methods for the preparation of
colloids
What role does adsorption play in heterogeneous
catalysis?
Describe some features of catalysis by zeolites
Explain the terms:
(i) Peptisation
(ii) Electrophoresis
Explain the terms:
(i) Coagulation
(ii) Dialysis
Explain Tyndall effect.
Give four uses of emulsions.
Write a note on Hardy Schulze rule.
Discuss the effect of temperature on adsorption.
23. What is the difference in the nature of a dilute soap
solution and a concentration soap solution?
24. What type of colloidal sols are formed in the following
?
(a) Sulphur vapours are passed through cooled water.
(b) White of an egg mixed with water.
(c) Soap solution.
25. Give reason why a finely divided substance is more
effective as an adsorbent?
26. Sky appears blue. Why?
27. Rivers form delta on meeting with ocean, why?
28. Alum is used in cleaning town water supply.
29. What happens in
(a) Tyndall phenomenon
(b) Electrophoresis
30. What do you mean by activity and selectivity of
catalysts?
31. Why at all a catalyst always lowers the energy of
activation of the reaction?
32. Write down the heterogeneous catalyst involved in
the polymerization of ethylene.
33. A sol of AgI can be positively or negatively charged.
Explain how and why?
34. Explain what is.
(a) aerosol
(b) emulsion
(c) foam
(d) hydrophobic colloid
35. 1 g of characoal adsorbs 100 ml of 0.5 M CH3COOH
to form a monolyer, and thereby the molarity of
CH3COOH reduces to 0.49. Calculate the surface
area of the charcoal adsorbed by each molecule of
acetic acid. Surface are of charcoal = 3.01 × 102 m2/g
36. Write terms for :
(a) Expressing protective power of a lyophilic colloid.
(b) Aggregates of surfactant molecules.
(c) Colloidal dispersion of a solid in benzene
(d) Colloidal solutions of soaps and proteins in water
37. Write chemical equations for making hydrophobic
sols of Fe(OH)3, S and As2S3.
38. What is
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(a) aquadag
(b) oil dag
(c) done in case of arsenic poisoning?
(d) the most important application of Tyndall effect?
39. 50 ml of 1 M oxalic acid is shaken with 0.5g wood
charcoal. The final concentration of the solution after
adsorption is 0.5 M. What is the amount of oxalic acid
adsorbed per gram of carbon?
40. Discuss the effect of temperature on adsorption.
41. For the coagulation of 100 ml of arsenious sulphide
sol, 5 ml. Of 1 M NaCl is required. What is the
flocculation value of NaCl?
42. Give points of differences between Physisorption and
Chemisorption.
43. Explain theory of electrical double layer in colloids.
44. What are
(a) Promotors
(b) Catalytic poisons
(c) Positive catalyst
catalyst
(d)
Negative
EXTRACTION
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
Name two metals which occur in native state.
How is 14C produced in the upper atmosphere ?
What are igneous rocks ? How are these originated?
What are siderophiles?
In general which metals do you expect to occur in
native ? Give examples.
When is electrolytic reduction applied for getting metal
?
What is benefication process?
How does NaCN act as a depressant in preventing ZnS
from forming the froth ?
Metal sulphides occur mainly in rocks, the metal
halides occurs mainly in seas and lakes. What could be
the reasons for this difference in behavioues?
Sea water contains ions such as Na+, K+ and Mg+2 but
it does not contains Cu+2, Pb+2 and Ba2. What ?
Metals like Cu, Ag, Zn, Hg and Pb occur in nature as
sulphides rather than oxides ? Why ?
Name the processes from which chlorine is obtained as
bye product. What will happen if an aqueous solution of
NaCl is subjected to electrolysis ?
You are provided with samples of some impure metals
such as zinc, copper and germanium. Which method
would you recommend for the purification of each of
these metals.
What is aluminothermy ? Explain with one example.
What do you mean by electrometallurgy ?
Name the metals which are associated with the
following terms in their extraction from their ores.
(a) Bessemer’s converted
(b) Blast furnance
(c) Alumino thermic process (d) Magnetic separation.
Which metals are generally extracted by the electrloytic
process ? What positions these
Metals generally occupy in the period table ?
Distinguish between flux and slag.
Name three ores which are concentrated
by froth
floatation process. What is meant by a depresent ?
How the ore is concentrated by gravity separation
method or Levigation method or Hydraulic washing
method ?
How the ore is concentrated by froth flotation process ?
What is the role of a stabilizer and of a depressant ?
Give one example each.
Give a brief account of calciunation and roasting. How
roasting is different from calcinations ?
23. What is the principle of separation of metal ions in
qualitative analysis?
24. Name the method by which Na, K, Mg and Al can be
extracted.
25. Name carbonate ores of (i) Fe, (ii) Zn, (iii) Cu, (iv) Pb,
(v) Ca, (vi) Mg.
26. Give two examples of igneous rocks.
27. What type of elements belong to siderophil ?
28. What is the difference between calcinations and
roasting ?
29. Define smelting by giving an example.
30. Why do some elements occur in native state whereas
most of elements occur in combined state ?
31. Name the second most abundant element in earth’s
crust.
32. What happens when calamide is calcined ? Give
chemical equation.
33. What happens when H2S gas is passed through
acidified solution of CuSO4 ? Give equation.
34. What is potential source of rare metal?
35. What happens when iron pyrities is roasted ? Give
equation.
36. What is the basic principle of liquation? Give an example.
37. Name the method used for getting ultra pure silicon
and germanium.
38. Why is leaching of gold by metal cyanides carried out
in the presence of oxygen? Give the chemical
equation. Name the meal used as reducing agent./
39. Of the metals Ca, Pb, Al and Cu, which one is
extracted from its ore by the electrolytic method and
why ?
40. Explain the process of zone refining. Give two
examples of elements purified by this process.
41. Describe the principle of froth flotation process. What
is the role of a stabilizer and of a depressant ? Give
one example each.
42. Describe the principle of each of the processes in
detail : Mond’ process.
43. You are provided with samples of some impure metals
such as zinc, copper and germanium. Which methods
would you recommend for the purification of each of
these metals ?
44. The choice of a reducing agent in a particular case
depends on thermodynamic factor. How far do you
agree with this statement ? Support your opinion with
examples.
P-BLOCK
1.
2.
Write the structure of pyrophosphoric acid, H4P2O7.
Which compound led the discovery of noble gases ?
3.
4.
On being slowly passed through water, PH3 forms
bubbles but NH3 dissolves. Why is it so?
Mention an important property of hydrazine.
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BRILLIANT
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
Guess Paper
Institute of advanced studies
How does BF3 act as catalyst in industrial processes ?
What is carbogen ? What is its use ?
What are ‘fullereners’?
Why does phosphorus glow in the dark ?
Fluorine does not form oxyacids but other halogens
do. Why ?
Arrange the following in the order of property indicated
for each set :
(a) M  F, M  Cl, M  Br, M  I : decreasing ionic
character
(b) NH3, Ph3, AsH3, SbH3, BiH3 : increasing basic
strength.
Discuss two similar and two dissimilar properties from
the chemistry of nitrogen and that of phosphorus.
Write the resonance structure of
(a) SO4 2 (b) PO4 3
Discus why acidic strength of oxoacids of halogens
decreases with the increasing atomic number of
element.
Discuss the structure of diborane
or
Draw the structure of B2H6
Explain why CO2 is a gas at room temperature but
SiO2 is a high melting solid.
Oxygen exhibits only -2 oxidation state while other
members of this family shows +4 and +6 oxidation
states as well. Explain why it is so.
or
Why does oxygen not show +4 and +6 oxidation
states like sulphur?
or
Sulphur shows +4 and +6 oxidation states in its
compounds but oxygen can’t show these oxidation
states.
Phosphinic acid behaves as a monoprotic acid
CCl4 is resistant to hydrolysis but SiCl4 is readily
hydrolysed. Explain.
How are XeO3 and XeOF4 prepared ? Describe their
molecular shape.
or
Draw the structure of XeOF4.
Draw molecular structure of :
(a) Peroxodisulphuric acid
(b) Iodine pentafloride.
Account for the following :
(a) SnCl2 is a solid while SnCl4 is a liquid.
(b) All AlCl bonds in the Al2Cl6 are equivalent.
(c) BCl3 reacts with water, whereas CCl4 does not.
(d) BF3 and BCl3 do not form dimmers, while BH3 does
so.
(e) Carbon and silicon are almost tetravalent but Ge,
Sn and Pb show bivalency.
(f) Some noble gases react with fluorine to form fluorides.
Which do, and which do not ?
Give appropriate reasons for each of the following
observations :
(a) Sulphur vapors exhibit some paramagnetic
behaviour
(b) Silicon has no allotrophic form analogous to
graphite.
(c) Of the noble gases, only Xenon is known to form
real chemical compounds.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
(a)
(b)
(c)
36.
37.
38.
(d) Despite its lower electron affinity, fluorine is a
stronger oxidizing agent than chlorine.
B(OH)3 is an acid, Al(OH)3 is amphoteric and Tl(OH)3
is basic. Explain.
AlF3 is a high m.pt. solid while AlCl3 is low m.pt.
volatile solid. Explain.
Finely powered aluminium when exposed to air
becomes hazardous. Why ?
Graphite is used as lubricant, Explain.
Tin vessels are not used for packing in cold countries.
Explain.
Why HPO2 is not formed like HNO2?
H2S acts only as reducing agent while SO 2 can act
both as reducing agent and oxidizing agent.
Fluorine cannot be prepared from fluorides by
chemical treatment. Why ?
A mixture of He and O2 is used for respiration for deep
see divers. Why ?
HF a lower boiling point than water even though it has
stronger hydrogen bonds than water. Why ?
What are silicones ? How are they manufactured ?
How is lithium aluminium hydride (LiAlH4) prepared ?
What is its important use ?
Give appropriate reasons for each of the following
observations :
Sulphur vapours exhibit some paramagnetic behaviour.
Silicon has no allotropic form analogous to graphite.
Nitrogen shows only a little tendency for catenation
whereas phosphorus shows a clear tendency for
catenation.
How does BF3 act as catalyst in industrial processes ?
Why is the bond dissociation energy of fluorine
molecule less than that of chlorine ?
(a) Explain why (CH3)3N is pyramidal whereas
(SiH3)3N is planar.
(b) Complete and balance the following reactions :
(i) NH3 + NaOCl  (ii) Pb(NO3)2
673K
39.
40.
41.
42.
43.
 (iii) XeF6 + KF 
State the trends observed in case of each of the
following :
(b) Oxidising power of the members of the halogen
family.
(b) Basic character of the hydrides of the elements of
Group 15.
(c) Oxidation states of the elements of Group 14.
What is meant by ‘catenation’? How does the
catenation tendency for elements of Group 14 vary?
or
Give reason, why the tendency for catenation
decreases down the group in group 14.
Compare and contrast the following :
(a) Structures of oxides of nitrogen and phosphorus
(b) Electron affinities of fluorine and chlorine.
(c) Maximum covalency of oxygen and sulphur
Calculate the volume of 0.1 M NaOH solution required
to neutralize the solution produced by dissolving 1.1 g
of P4O6 in water.
Write balanced equations for the following reactions
(a) Aqueous sodium hydroxide is added dropwise to a
solution of gallium chloride in water. A precipitate is
formed initially which dissolves on further addition
of NaOH solution.
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(b) SnO is treated with dilute HNO3
(c) Tin is heated with an excess of chlorine gas
(d) Lead sulphide is heated in air.
44. Arrange the following in the order of property indicated
for each set :
(a) F2, Cl2, Br2, I2  increasing bond energy
(b) HF, HCl, HBr, HI – increasing acid strength
(c) As2O3, ClO2, GeO3increasing acidity
(d) H2O, H2S, H2Se, H2Te  increasing acid strength
D & F BLOCK
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
Chemistry of all lathanides is quite identical, why?
The ionization energies of first five members of 3dseries increase with increase in atomic number and
then become constant or irregular for next five
members. Explain.
Transition metals have high m.pt and b.pt., why? They
exhibit high enthalpies of atomization. Why ?
Cu+2 is more stable than Cu+. Explain.
Copper dissolves in dil nitric acid but not in dil HCl.
Why?
AgNO3 is kept in brown coloured bottles.
The colour of mercurous chloride changes from white
to black when treated with ammonia solution.
Polling process is used for the removal of Cu2O from
copper.
AgBr is used in photography. Explain.
Write balanced chemical equations for the following
reactions :
(a) A mixture of potassium dichromate and sodium
chloride is heated with concentrated H2SO4.
(b) Potassium permanganate is added to a hot
solution of magnaous sulphate.
In what way do the d-block metals differ from alkali and
alkaline earth metals?
Write equation to show how H2O2 reduces MnO4 to
Mn+2 in acidic solution.
Complete and balance the following reactions :
(i) [MnO4]2 + H+  …. + [MnO4] + H2O
(ii) SO2(aq) + Cr2O72 + 2H+  …. + ….
Complete and / balance the following equations
(i) Ag2S + 2CuCl2 + 2Hg … + …. + S + 2Ag
(ii) SnCl4 + 2C2H2Cl + 2Na
Why is chalcocite roasted and not calcined in the
recovery copper ?
Complete the following by identifying [A] to [H]
100o C
280o C
o
800 C
(i)CuSO4.5H2O [ A ]   [B]  [C] +
[D]
red heat
(ii) AgNO3 
 [E] + [F] + O2
740o C
17.
18.
19.
20.
(iii) Na2B4O7  [G] + [H]
Describe the preparation of potassium dichromate from
iron chromite ore. What is the effect of increasing pH
on a solution of potassium dichromate ?
Describe two uses of each of the following :
(a) Copper sulphate
(b) Silver nitrate
(c) Silver bromide
Name the members of lanthanoid series which exhibit
+4 oxidation states and those which exhibit +2
oxidation states. Try to correlate this type of behaviour
with the electronic configuration of these elements.
(a) K2Cr2O7 reacts with acidified solution of KI.
(b) CuSO4.5H2O is heated.
(c) KIaq reacts with acidified KmnO4.
(d) Silver chloride is treated with aqueous NaCN and the
product so formed is allowed to react with zinc in
alkaline medium.
(e) AgCl is treated with hypo solution
21. When a white crystalline compound X is heated with
K2Cr2O7 and concentrated H2SO4, a readish brown
gas A is evolved. On passing A into caustic soda
solution, a yellow coloured solution of B is obtained.
Neutralizing the solution B with acetic acid and on
subsequent addition of lead acetate, a yellow
precipitate C is obtained. When X is heated with
NaOH solution, a colourless gas is evolved and on
passing this gas into K2HgI4 solution, a reddish brown
precipitate D is formed. Identify A, B, C, D and X.
Write the equations of the reactions involved.
22. What is the most characteristic oxidation state of
lanthanides?
23. Out of Cr2+ and Cr3+ , which one is stable in aqueous
solution?
24. Why is hydrochloric acid not used to acidify a
permanganate solution in volumetric estimation of
Fe2+ or C2O42-?
25. Why is copper sulphate pentahydrate coloured?
26. Why is that an orange solution of K2Cr2O7 turns
yellow on adding NaOH to it?
27. Write down the electronic configuration of Pm 3+.
28. What is Duplexing?
29. What is an amalgam?
30. What is “Vermilion”?
31. What is lithopone?
32. What is philosopher’s wool?
33. Account for the following:
(a) Enthalpies of atomization of the transition
elements are quite high.
(b) Transition elements form many interstitial
compounds.
34. Write the chemical equations for the conversion of :
(a) Chromite ore to sodium chromate
(b) Pyrolusite to potassium manganese dioxide.
(c) Potassium permanganate to manganese dioxide
35. The sums of the first and second ionization energies
and those of third and fourth ionization energies of
Nickel and platinum are given below:
IE1 + IE2 (KJ mol-1) IE3 + IE4 (KJ mol-1)
Ni
2.49
8.80
Pt
2.66
6.70
Taking these values into account, write
(a) The most common oxidation state for Ni and Pt
and its reason.
(b) The name of the metal (Ni or Pt) which can form
compounds in +4 oxidation state more easily and
why?
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Fe2+
Fe3+
36. Which of the two
and
is more stable and
why?
37. Why Sc3+, Ti4+, Zn, Cd, Hg compounds are white?
38. [Ti(H2O)6]+3 is purple coloured while [Sc(H2O)6]+3 is
colourless. Why?
39. Why Ni+2 compounds are thermodynamically more
stable than Pt+2 compounds while Ni+4 compounds are
less stable than Pt+4 compounds? Explain.
40. What is Alnico? Give it composition and uses.
41. What is Baeyer’s reagent? What is its use?
42. Give the chemistry of chromyl chloride test.
(a) What happens when:
(i) KmnO4 is heated
(ii) K2Cr2O7 is heated
(iii) Ki is added to acidified solution of KmnO4?
(b) Why does a transition series contain ten
elements?
(c) Why properties of third transition series are very
similar to second transition series?
(d) La(OH)3 is more basic than Lu(OH)3. Explain
CO-ORDINATION
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
Give an example of an organometallic compound used
as a homogeneous catalyst.
Give the IUPAC name of the ionization isomer of
[(NH3)3Ni(NO2)]Cl.
Give the IUPAC name of the linkage isomer of
[(NH3)2(H2O)PtNO2]Br.
Write the name of the complex [Cr(en)3][CO(CN)6]
How many isomers are there for the complex
[Co(NH3)4Cl2]Cl ?
Write the IUPAC name of [Ni(CN)4]2 ion.
Name the two broad categories of organometallic
compounds.
Define a ‘ligand’. Give an example also.
What is the coordination number of central metal ion in
[Co(NH3)3Cl3] and [Fe(C2O4)3]3 ?
Write the IUPAC name of [Ni(H2O)6] (ClO4)2.
What are  complexes ? Describe one method for
preparation of  complexes.
Describe the hybridization scheme, the resultant
geometry and the magnetic behaviour of [Co(NH3)6]+3.
Draw correctly the structures of the following :
(i) Fe(CO)5 (ii) [NiCl4]2 (iii) [Co(NH3)6]+3.
How would you account for the following
(a) [Fe(CN)6]3 is weakly paramagnetic while
[Fe(CN)6]4 is diamagnetic.
(b) [Ni(CO)4] possesses tetrahedral geometry while
[Ni(CN)4]2 is square planar.
Draw the structure of
(a) is-[Pt(NH3)2Cl2] (b) [Co(NH3)6]+3
(b) Ferrocene.
Give a chemical test to distinguish between
[Co(NH3)5Br]SO4 and [CO(NH3)5SO4]Br. What kind of
isomerism do they exhibit?
What are ambivalent ligands ? Give examples.
Describe one method of preparation of each of the
following : (i) [C2H4)PtCl3] and
(ii) Ni(CO)4.
Giving a suitable example, describe the importance of
the formation of complex compounds in
(a) the estimation of hardness of water, and
(b) the extraction of a particular metal from its natural
source.
Draw the structure and write the hybridization state and
oxidation state of the central atom in each of the
following species :
(a) Fe(CO)5
(b) trans-[Co(NH3)4Cl2]+
Explain geometrical isomerism with reference to square
planar complexes giving one example. How is it that
tetrahedral complex with simple ligands do not exhibit
geometrical isomerism ?
22. Draw the structures of optical isomers of
(a) [Cr (OX)3]3 (b) [PtCl2(en)2]+2 (c)
CrCl2(en)(NH3)2]+
23.
Draw figure to show splitting of degenerate d
orbtials in an octahedral crystal field.
24. Discuss briefly the role of coordination compounds in
:
(a) medicinal chemistry and (b) analytical chemistry
25. Write the formula of Everitt’s salt.
26. Why does AgCl dissolve in ammonia?
27. Name the metal is present in Vitamin B12 and
Plastocyanin.
28. What is flexidentate character of a ligand?
29. What are the main postulates (or points) of Werner’s
coordination theory ?
30. What are outer orbital and inner orbital complexes?
Give examples.
31. Show diagrammatically the splitting of degenerate dorbitals in tetrahedral crystal field.
32. What is EAN? How can it be determined? Give
example.
33. Are the compounds Ti(OC3H7)4 and C6H5Ti(OC3H7)3
organometallics) Comment.
34. Write the structures of the following :
(i) Trimethyl aluminium (ii) Zeise’s salt.
35. Discuss
the
applications
of
organometallic
compounds.
36. Briefly discuss the nature of bonding in metal
carbonyls.
37. What are chelating ligands and chelate complexes ?
Give examples. Give applications of chelate
complexes.
38. Which of the two [Fe(CN)6]4 and [Fe(CN)6]3 is more
stable and why ?
39. How does Werner’s co-ordination theory account for
the non-ionic nature of the complex CoCl3. (NH3)3?
40. Name the following complexes :
(i) K3[Al(C2O4)3
(ii) [Co(NH3)5CO3]Cl
41. Write the formula of Fisher salt and Magnus green.
42. Draw isomers for the complex [Pt(NH3)(py) (Br)Cl]
43. Why does ammonia readily from a complex whereas
ammonium ion does not?
44. Why metals are complexed in biological systems?
45. A complex CrCl3.4H2O precipitated AgCl when treated
with AgNO3. The molar conductance shows the
presence of 2 free ions. Write the formula of the
complex
FG(I)
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GUESS PAPER
CHEMISTRY
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
Name the only primary alcohol which gives haloform
test
How can you chemically distinguish between
methoxymethane and ethanol?
What is the directive influence of phenolic group?
Name three derivatives of salicylic acid which have
medicinal importance. Give one application of each
one of them.
Name the test which can be employed to distinguish
between ethylene glycol and glycerol.
What is the product of oxidation of glycerol with
Fenton’s reagent?
What is proof spirit?
Name the enzyme which converts glucose into ethanol.
What is meant by molasses?
What is composition of blasting gelatin and cordite?
Explain why
(a) tert-Butyl alcohol is much more soluble in water
than n-butyl alcohol.
(b) n-Hexanol is not soluble in water.
Explain why o-nitrophenol is less soluble in water than
p-nitrophenol.
Can we sodium metal to remove last traces of water
from (i) benzene (ii) ethanol?
Complete the following equations supplying A and B
22.
23.
24.
25.
26.
27.
28.
29.
30.
OH
(a)
Zn dust
31.
H SO
4 B
 A 2
OH
SO3
(b)
Sn / HCl
(i) NaNO / HCl
2 
A  B 

(ii ) H2O
32.
33.
15. Complete the following equations supplying A and B
(a)
Cl
aq. NaOH
2  A 

 B
AlCl3
(b)
575K, 300 atm OH
A   B 
CHCl 3
PCl 5
KOH
34.
CHCl2
(b) Ethanol and phenol
(c) 1-Propanol and 2-Propanol
(d) Impure ether and pure ether
(e) Ethanol and propanol-1
Compound (A) gives positive Lucas test in 5 minutes.
When 6.0 g of (A) is treated with sodium metal, 1120
ml of hydrogen is evolved at STP. Assuming (A) to
contain one atom of oxygen per molecule, write the
structural formula of (A).
Compound (A) when
treated with PBr3, gives compound (B) which when
treated with benzene in the presence of aluminium
chloride gives compound (C). Write down the
structural formula of (B) and (C).
What is dynamite.
Name an ether used as an anaesthetic and an ether
used as flavouring agent.
What are crown ethers? What is their important
property?
What is denaturation of alcohol?
Glycerol is a by-product of soap industries, and is
chiefly used in cosmetics.
CH3SH is a stronger acid than CH3 OH. Why?
t-Butyl alcohol reacts less rapidly with metallic
sodium than the primary alcohol. Why?
CO bond is much shorter in phenol than in ethanol.
Why?
Phenol is acidic but does not react with NaHCO 3
solution.
A small quantity of ethanol is added to chloroform
bottles. Why?
An alcohol (A) of unknown structure gave a positive
Lucas test in about 5 minutes. When alcohol was
treated with hot conc. H2SO4, an alkene (B) was
formed which has the formula C4H8.
Distinguish between
(i) Primary, secondary and tertiary alcohols
(ii) Ethanol and phenol
16. An organic compound A, C8H6 on treatment with dilute
sulphuric acid containing mercuric sulphate gives a 35. Distinguish between
(a) Methyl alcohol and ethyl alcohol
compound B, which can also be obtained from a
(b) Impure ether and pure ether
reaction of benzene with an acid chloride in the
Give the main product of the following equations:
presence of anhydrous aluminium chloride. The 36.
I2 NaOH
compound B, when treated with iodine in aqueous


(a) C2H5 OH 
KOH, yields C and a yellow compound D. Identify A, B,
SOCl2
KCN
Sn / HCl
 B  
 C
(b) CH3 CH2 OH  A 
C and D with justification. Show how B is formed from
A.
37.
Give the main product of the following equations:
HBr
17. (a) Ethylene to n-propyl alcohol (b)
Glycerol
to
Alc.KOH
HBr
CH

C
H

CH
(a)
A
B











C
3
3
acrolein
|
perox ide
18. Complete the following sequences of reactions by
OH
supplying X, Y and Z:
(i) CH3MgBr
[O]
PBr 3
Na
Cl 2
(c) CH3  C H  CH2  CH3  A 

 B
X  
 Y 
 CH 3 CH 3 

ether
Heat
19. Complete the following sequences of reactions by
supplying X, Y and Z:
38.
H O / H
X 2 
 CH
Cu / 575K
(i) C H5MgI
 Y 2 

 Z
3 CH CH 3   
|
(ii) H2O / H
OH
20. The b.pt. of the three alcohols are in the order:
n-butyl alcohol > sec-butyl alcohol > t-butyl alcohol.
Why?
21. Distinguish between:
(a) Primary, secondary and tertiary alcohols
39.
|
OH
(ii) H / H2O
Alkylation of phenoxide ion with an active alkyl
halide such as CH2 = CHCH2 Cl gives phenyl ethyl
ether and also some o-allyl phenol.
Isopropyl alcohol on treatment with excess of hot
conc. H2SO4 gives a compound (A) which on
treatment with hydrogen bromide gives (B). (B)
when dissolved in ether and treated with sodium
gives (C). What is (C)?
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BRILLIANT
40.
41.
42.
43.
Guess Paper
Institute of advanced studies
Explain the fact in aryl alkyl ethers (i) the alkoxy group
activates the benzenering towards electrophilic
substitution, and (ii) it directs the incoming
substitution, to ortho and para positions in benzene 44.
ring.
Write short notes on:
(a) Koble reaction, and (b) Reimer-Tiemann reaction
Write notes on (i) oxymercuration-demercuration, and
(ii) hydroboration.
Name the reagents used in the following reactions:
(a) oxidation of a primary alcohol to carboxylic acid.
(b) Oxidation of a primary alcohol to an aldehyde
(c) Bromination of phenol to 2, 4, 6-tribromophenol.
(d) Benzyl alcohol to benzoic acid
(e) Dehydration of propan-2-ol to propene
Give the equations of the following reactions:
(a) Reaction of propene with mercuric acetate
followed by hydrolysis
(b) Oxidation of propan-1-ol with alkaline KMnO4
solution
(c) Reaction of bromine in CS2 with phenol
(d) Action of dilute HNO3 with phenol
(e) Treating phenol with chloroform in presence of
aqueous NaOH at 343 K.
FG (II)
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
Arrange in decreasing order boiling point
(i) CH3CONH2
(ii) (CH3CO)2O
(iii) CH3COOH
(iv) CH3COCl
Arrange in decreasing order water solubility
(i) CH3COOH
(ii) HCOOH
(iii) C6H5COOH
(iv) C15H31COOH
Arrange in decreasing order Ease of hydrolysis
(i) CH3CH2CH2COOH
(ii) (CH3)2CHCOOH
(iii) (CH3)3COOH
Arrange in decreasing order Acidic nature
(i) HCOOH
(ii) CH3COOH (iii) C6H5COOH
Arrange in decreasing order Boiling point
(i) Propanone
(ii) Propanal
(iii) Propane
(iv) Propan-l-ol
Arrange in decreasing order Boiling point
(i) C3H7CHO
(ii) CH3COC2H5
(iii) C2H5COOCH3
(iv) (CH3CO)2O
Arrange in decreasing order Boiling point
(i) C2H5OC2H5 (ii) C3H7COOH
(iii) C4H9OH
Arrange in decreasing order Ease of hydrolysis
(i) CH3CONH2
(ii) CH3COOCH3
(iii) (CH3CO)2O
(iv) CH3COCl
Chloral hydrate is a stable molecule through it contains
2 OH-groups on the same C. Why ?
Carbonyl compounds show nucleophilic addition. Why
?
Describe the following :
(a) Acetylation
(b) Cross aldol condensation
Describe the following :
(a) Cannizzaro reaction
(b) Hoffmann bromamide reaction
Predict the organic products of the following reactions :
16. How will you bring about the following conversions in
not more than two steps ?
(a) Propanoyl Chloride to Dipropyl amine
(b) Propanoic acid to Propenoic acid
17. How will you bring about the following conversions in
not more than two steps ?
(a) Benzoyl chloride to Benzonitrile
(b) Bromobenzene to 1-Phenylethanol
18. Give simple chemical tests to distinguish between the
following pairs of compounds.
(a) Propanoyl chloride and propanoic acid
(b) Propanal and Diethyl ether
19. Give simple chemical tests to distinguish between the
following pairs of compounds.
(a) Benzamide and p-Aminobenzoic acid
(b) Phenol and Benzoic acid
20. Give simple chemical tests to distinguish between the
following pairs of compounds.
(a) Methyl acetate and Ethyl acetate
(b) Benzoic acid and Ethyl benzoate
21. Complete the following by supplying (A) to (F)
P / Br
Alcoholic KOH
2  CH3CH2CH2Br 
[A] 

[B]
Br
KOH ( alc.)
Hg 2
Follow edby NaNH2
dil. H2SO4
2

[C]  [D] 
 [E]
CCl4
NH2OH

 [F]
H
22. Bring out the following conversions :
(a) Ethanol to Propanone
(b) Ethanal to 2-hydroxybut-3-enoic acid
(c) Benzamide to Toluene
13.
(d) Benzoic acid to Benzophenone

O
[ Ag(NH3 )2 ]


(a)
(e) Acetone to 2-Methylpropan-2-ol
23. Carbonyl compounds do not undergo nucleophilic
CHO
substitution reactions. Explain why?
(i) NaCNHCl
24.
Pure HCN fails to react with carbonyl compounds.
CHO
(b)

Why?
COOH
25. Chloral usually exists as hydrate. Why?
14. Predict the organic products of the following reactions :
26. The formation of oximes and hydrazones from
C 6 H 5 CHO
aldehydes and ketones requires slightly acidic media
dil. NaOH

 
(a)
for maximum rate while basic or highly acidic
CH 3 CH 2 CHO
conditions lower the rate. Explain.
(i) LiAlH4 ( ether )
27. The addition of KCN solution of a carbonyl compound
(b) C6H5CON(CH3)2 

(ii) H3O
increases the pH of solution. Why ?
28.
Almost all oxygen containing organic compounds
15. How will you bring about the following conversions in
dissolve in conc. H2SO4. Explain .
not more than two steps ?
(a) Benzaldehyde to Benzophenone
29. Halogen acid add to C = C but not to C = O. Why?
(b) Benzaldehyde to 3-Phenylpropan-1-ol
12.
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BRILLIANT
Guess Paper
Institute of advanced studies
30. Acidic chlorides fail to give ketone with RMgX, but with 39. Identify (A), (B) and (C) and give their structures.
R2Cd a ketone is obtained easily.
31. Iodoform is obtained by the reaction of acetone with
hypiodite but not with iodide. Why?
O
Write the structure of the major organic product
CH3
Br2
H
( A )  (B) 
 C(C7H12O)
CH3 
expected from each of the following reactions:
NaOH
CHO + HCHO + KOH 
32. CH3O
O
Alkali

33. CH3CH2CHCl2  
Write the products of the following reactions
Boil
34. Complete
structure:
CH3CH2
the
following

reaction
with
appropriate
(i) O3
OH 

( A )
40.
(ii ) Zn
O
1. KCN/H SO
2 
4  (D)
C = O 
2. LiAlH4
HO
OH

 (B)
H
OH
HO
35. Suggest appropriate structures for the missing
compounds. (The number of carbon atoms remains the
O
same throughout the reactions.)
42. Give the mechanism of the following transformation
CH3
O
OH
Dil.KMnO4
HIO4
OH
O
||
|

( A ) 
(B) (C)
//
H  C  C \  OH   H  C  COO

CH3
|
H
36. Acetophenone on reaction with hydroxylamine
H
hydrochloride can produce two isomeric oximes. Write What is it called ?
the structure of the oximes.
43. Write the missing products in the following reaction
37. Complete the following reaction with appropriate
O
structures of products/reagents:
O
(i) KOHCH3OH
(i) Ba(OH)2
O
(i) LiAlH4

 (A) 
 (B)
[C]




CH.C6H5
41.
(ii) H , 
D
(ii ) CH3I
(ii ) H2SO 4
O
38. Ann organic compound (A), C6H10O, on reaction with
CH3MgBr followed by acid treatment gives compound 44. Why is H2C = O always oxidized in crossed
(B). The compound (B) on ozonolysis gives compound
Cannizzaro reaction?
(C), which in presence of a base gives 1-acetyl 45. Both carbonyl and ethylenic groups undergo addition
cyclopentene (D). The compound (B) on reaction with
reactions, give the basic difference in their nature.
HBr gives some compound (E). Write the structures of
(A), (B), (C), (D) and (E).
FG(III)
1.
2.
3.
4.
5.
Write basicity order in NH3, (C2H5)2NH, (C2H5)3N.
Which is steam volatile : o-Nitrophenol
Nitrophenol.
Write the electronic structure of acetonitrile.
Write the zwitterionic structure of sulphanilic acid.
Tick out the ambident nucleophile


or
p-
R O  ,  CN  ,  CNS  , H 2 O ,  NO 2
6. What is the use of nitroglycerine.
7. Tertiary amines do not undergo acylation. Why ?
8. (CH3)4N+ is neither an electrophile nor a nucleophile.
Why?
9. The amino group in ethyl amine is basic, whereas that in
acetamide, it is not basic. Why ?
10. Boiling point of methylamine (7.5oC) is low as
compared to methyl alcohol (60oC) although both form
hydrogen bond. Why ?
11. Glycine is amphoteric in nature. Why ?
12. Trifluoro trimethylamine (CF3)3N is a weaker base than
trimethylamine (CH3)3N. Explain.
13. Nitrobenzene, but not benzene, is used as a solvent
for the Friedel-Crafts alkylation of bromobenzene.
Why ?
14. Nitration of C6H5C(Me)3 gives only 16% ortho product
while that of C6H5CH3 gives 50%. Explain.
15. Sulphanilic acid has high m.pt . as well as insoluble in
organic solvent. Why ?
16. Write three canonical forms of carbocation
intermediate for m-attack on nitrobenzene.
17. How is it that a ketone reacts with Grignard reagent to
form a tertiary alcohol but in the reaction of a nitrile
with Grignard reagent, a ketone is formed ?
18. How can a carboxylic acid be converted to an amine
having one carbon atom less than the carboxylic acid
used?
19. How can you separate a mixture of primary,
secondary and tertiary amines ? Write chemical
reactions involved in the process.
20. How can you convert p-toluidine to 2-bromo-4methylaniline ?
21. Describe the following reactions :
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BRILLIANT
Guess Paper
Institute of advanced studies
(a) Gattermann’s reaction
filtered, the resulting solution is as strongly alkaline
(b) Diazotisation
as a solution of sodium hydroxide. What is in the
(c) Hoffmann bromamide reaction
solution, and why is it so basic?
(d) Carbylamine reaction
38. The reaction of n-butyl amine with NaNO2 and HCl
(e) Gabriel phthalimide reaction
yields nitrogen and the following mixture, n-butyl
22. Complete the following equations and report the main
alcohol 25%, s-butyl alcohol 13%, 1-butene and 2product formed :
butene 37%, n-butyl chloride 5%, s-butyl chloride
(A)
NH3
( C)
3%.
(a) C6H5COOH 
 C6H5COCl  B 
 C6H5CN
(a) What is the most likely intermediate common to
Br2 / KOH
HNO2
Re dP / I2
(b) C2H5CONH 2 

 
 B 
 C
all of these products, and how it is formed?
CrO3
C6H5NH2
(b) Outline reactions that account for the different
(c) C6H5CH3 
 A 
 B
products.
AgCN
S8
HI
39. An organic compound (X) of formula, C9H17O5N,
(d) CH2 = CH2  A  B 
C
C2H5OH
reacts with dilute NaOH to give C9H16O5N.Na, with
CH3 / KOH
Re dn
Re dn
HNO2
ethyl alcohol to give C11H21O5N, and with hot NaOH
(e) C2H5NO 2 






C




D

 A 
 B
to give compound (Y) and -amino propionic acid.
23. Alkyl cyanides have a higher boiling point than the
Its nitrogen is non-basic. What are ‘X’ and ‘Y’? Give
corresponding alkyl halides.
the different reactions involved.
24. Why are amines basic in nature?
40. An optically active amine (A) of molecular formula
25. Ethylamine is more basic than aniline.
C4H11N is subjected to Hofmann’s exhaustive
26. Why amines are more basic than amides?
methylation process when an alkene (B) is produced
27. There is decreasing order in basicity of:
which upon ozonolysis and subsequent hydrolysis
CH3NH2 > CH3N = CHCH3 > CH3CN.
yields formaldehyde and propanol. Identify (A) and
28. Dimethylamine is a stronger base than trimethyl amine.
(B) and write the different reactions involved.
29. An amine (A), C6H15N, on treatment with CH3I and
41.
Four isomeric compounds (A), (B) (C) and (D) have


the composition C = 61.01%, H = 15.25% and N =
then KOH, gives (B), C8H20 N O H . This on heating
23.72%. With HCl each of them forms a
produces isobutene and amines (C), C4H11N. What is
hydrochloride having 37.17% chlorine. (A) and (B)
(A)?
on treatment with HNO2 evolves N2 to form 130. Complete the following equation:
propanol and 2-propanol, respectively. (C) under
RMgBr + CO2  ?
similar treatment gives a yellow oily liquid.
(i) SOCl2
Ag 2O
H O
H

 ?   
?  
 ? 2
Compound (D) forms a salt with cold HNO2 which on
(ii) CH2N2
heating gives methanol and a yellow oily liquid like
31. CH3COCH2Cl + CH2N2  C4H7ClO + C4H7ClO
(C). Deduce the structures of (A) to (D) and write the
(A) is a ketone and (B) is an epoxide. Suggest
necessary reactions that are involved.
structure for (A) and (B) and mechanism for their 42. Compound (A), C3H7NO, gave the following observations:
formation.
(i) On hydrolysis, it gives an amine (B) and
32. The deamination of n-propyl amine yields the following
carboxylic acid (C).
products: propene, propanol-1, n-propyl chloride,
(ii) Amine (B) reacts with C6H5SO2Cl, and gives a
propanol-2 and isopropyl chloride. How these are
product which is insoluble in aq. NaOH solution.
formed?
(iii) Acid (C) on reaction with Tollen’s reagent gives a
33. Explain why amines are more basic than amines?
silver mirror. What are (A) to (C)? Explain the
34. What happens when the following are subjected of
reactions.
Hofmann elimination?
43. The compound (A) contains C, H, O and N. When
(i) (CH3CH2CH2)2CH
(ii) CH3CH2NHCH2CH2CH3
treated with caustic potash and bromine, it gives (B)
35. Complete the following equations and name the
which on reaction with NaNO2 and HCl at 0°C gives
reactions:
ethanol. Identify (A) and (B).
H2O2

44.
A neutral organic compound (A) on strong heating
(i) (CH3)2N–CH – CH3 
 (A)  (B) +(C)
eliminates water and is converted into (B), C3H7NO.
|
(B) on boiling with NaOH gives off NH3 and on
CH3
acidifying yields a monobasic acid (C) which does
(i)
CH
I

3 (D) (E)  (F)
(ii) CH 3  N  CH 2 CH 3  
not contain nitrogen. The silver salt of the acid
|
(ii) Ag2O
OH
contains 59.33% of silver. Deduce the structures of
36. Complete the following equation and give the name of
(A), (B) and (C) and write equations for the
reaction:
reactions.
O
45. An aqueous solution of ethyl amine forms a brown
||
precipitate with ferric chloride. Comment.
NaN3
N2
H2O
46.
Glycine exists as a zwitter ion but anthranilic acid
C–Cl 

 ?  ?  ? 
 ?
CO2
does not. Explain.
37. If a tertiary amine is heated with an alkyl halide and
the product treated with aqueous silver oxide and
POLYMER
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13
GUESS PAPER
CHEMISTRY
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
Name the monomer of Buna-S. What is the
importance of sodium in it ?
Classify the following as addition polymers and
condensation polymers : Nylon 6, PVC, Neoprene and
Bakelite.
What is copolymer ? Give one example.
Give an example of a step-growth polymer.
Name a polymer used to make cups for hot drinks.
Give one example of each of the following :
(i) Natural polymer (ii) Condensation polymer
What is the monomeric unit of Teflon? Write two uses
of this polymer.
What are polyolefins and polydienes?
What is the difference between polyacrylates and
polyesters ?
What is the difference between nylon-6 and nylon-66 ?
What is a polyamide ? How is nylon-6 synthesized ?
Briefly describe the following terms giving one
example of each :
(i) Polyolefins (ii) Polyamides
(iii) Polyesters
Define the terms :
(i) Thermoplastics (ii) Thermosetting polymers
Comment on the structural difference between
thermoplastics and thermosetting polymers.
Draw the structures of monomers of (i) bakelite and
(ii) nylon-6
Write equations for the synthesis of the following
polymers :
(a) Glyptal
(b) Teflon
How is nylon-66 synthesized? Write the chemical
equation for the reaction involved.
Explain the following processes with a suitable
example in each case :
(i) Chain-growth polymerization
(ii) Steo-growth polymerization
Write the monomers for the following :
(a) Teflon
(b) Cellulose
(c) Neoprene
(d) Polythene
What are elastomers ? Write the chemical equation to
represent the preparation of Buna-S.
Write the mode of free radical polymerization of an
alkene.
22. Why is cationic polymerization preferred in case of
vinylic monomers containing electron donating group
?
23. Why does styrene undergo anionic polymerization
easily ?
24. How is bakelite formed ? Explain the reactions with
equations.
25. How is PHBV formed ? What are its uses ?
26. Give three points of difference between linear
polymer and branched chain polymer.
27. What is Backmann rearrangement ?
28. What is artificial silk ?
29. What does SBR stands for ?
30. What makes PVC a strong material ?
31. What is ebonite ?
32. Give preparation and uses of PVC (polyvinyl
chloride).
33. How is styron synthesized ? Give its two uses.
34. Give
the
preparation
of
polymonochlorotrifluoroethylene (PCTFE). Give one
of its uses.
35. Give the preparation and one use of glyptal.
36. How is melamine formaldehyde resin synthesized ?
Give its uses.
37. What do you mean by number average and weight
average molecular weights ? How are they
determined. ?
38. How are low density and high density polythene
manufactured ? What is the difference between
them ?
39. What are plasticizers ? Give examples.
40. What is PDi ? What is its value for natural and
synthetic polymers ?
41. All polymers are macromolecules but all macro
molecules are not polymers. Comment.
42. In a polymer sample, 30% molecules have molecular
mass 20,00, 40% have molecular mass 30,000 and
the rest have 60,000 molecular mass. Calculate the
mass average and number average molecular
weights.What is urea-formaldehyde resin ? Name its
monomer and its use.
43. Write the mechanism of cathonic polymerization.
Biomolecules
1.
2.
3.
4.
5.
6.
7.
8.
9.
Fresh tomatoes are a better source of vitamin C than
those present in tomatoes which have been stored for
some time.
Explain how reactions involving gain in free energy are
carried out in living system.
How are hormones transported to the target tissues ?
Which of the following is not an -amino acid ? Cysteine,
Tyrosine, Trypsin, Proline, Serine
How are nucleosides, nucleotides and nucleic acids
related ?
What are the main functions of the hormone adrenaline ?
What anticodon sequences on the mRNAs are coded for
by the mRNAs in the following base sequence :
CUU – AUG – GCU – UGG – CCC - UAA
What are the polysaccharides that make up starch and
what is the difference between them?
Is a diet consisting mainly of rice an adequate diet ? Why
or why not ?
10. Are functioning systems of antibodies present in new
born babies ?
11. (a) Give two examples of amine hormones? What are
their role ?
(b) Define immune system. How can immunity be
imparted ?
12. Name the deficiency diseases caused due to lack of
vitamin A, C, E, B1, B12B6, and K.
13. Answer the following about protein synthesis,
(a) Name the location where protein synthesis
occurs.
(b) How do 64 codons code for only 20 amino acids
?
(c) During translation which one of the two-end
functional groups of the polypeptide is formed
first ?
(d) Which of the two bases of the codon are most
important for coding, the first two or last two ?
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BRILLIANT
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14. Define enzymes. How do enzymes differ from ordinary
chemical catalysts ? Comment on the specifically of
enzyme action. What is the most important reason for
their specificity ?
15. What type of linkages are responsible for the formation
of
(a) Primary structure of proteins
(b) Cross linking of polypeptide chains
(c) -Heliz formation
(d) -Sheet structure
16. What are essential and nonessential amino acids ?
Give two examples of each. Give reasons for the
following
(a) Amino acids have relatively higher melting point as
compared to corresponding haloacids.
(b) Amino acids are amphoteric in behaviour
(c) On electrolysis in acidic solution amino acids
migrate towards cathode while in alkaline solution
these migrate towards anode.
17.
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20.
21.
22.
(d) The monoamino monocarboxylic acids have two
pK values.
Explain mutarotation. Give its mechanism is case of
D-glucose.
What are Molisch’s and Xanthoproteic tests.
(a) All enzymes are proteins but reverse is not true.
Comment
(b) Enzymes are known as biocatalyst. Why ?
Name the organ of the secretion and give functions of
(a) Androsterone and testosterone
(b) Estrone and estradiol.
Give the functions of each of the following hormones :
(a) Oxytocin (b) Insulin
(c) Thyroxine (d) Adrenaline
What are the hydrolysis products of
(a) Cane sugar (sucrose)
(b) Malt sugar (maltose)
(c) Milk sugar
(d) Starch ?
CHEMISTRY IN EVERYDAY IN LIFE
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20.
Name a food preservative which is most commonly
used by food producers.
Describe and illustrate with an example, a detergent.
Define the following and given one example:
Tranquilizers.
Describe the following giving a suitable example:
Antioxidants
Describe the following types of substances, giving
suitable examples: Antiseptics
List two major classes of antibiotics and give one
example of each class.
Why is bithional added to the toilet soap?
Give an example of a narcotic which is used as an
analgesic.
Name one medicinal compound each that is used to
treat (i) hypertension (ii) general body main.
State an example and function of the following: Wide
spectrum antibiotics.
Mention one important use of each of the following:
(i) Equanil
(ii) Sucralose
Name a broad spectrum antbiotic and state two
diseases for which it is prescribed.
State the function along which one example each of:
(i) Antihistamines
(ii) Antioxidants
Describe the following with an example each:
(i) Antimicrobials
(ii) Analesics
Name the following used for the treatment of th
efollowing diseases:
(i) Tuberculosis
(ii) Typhoid
Describe the following with examples:
(i) Preservatives
(ii) Biodergradable detergents
Describe the following giving an example in each case:
(i) Edible colours
(ii) Antifertility drugs
Define the following and give one example of each:
(i) Antipretics
(ii) Antibiotics
Give one important use of each of the folling:
(i) Bithional
(ii) Chloramphenicol
(iii) Streptomycin
(iv) Paracetamol
Give three examples of sulpha drugs and write their
main uses:
21. What are detergents? How are they classified? Why
are detergents preferred over soaps?
22. Explain the following terms with suitable examples:
(a) cationic detergents (b) anionic detergents and
(c) non-ionic detergents
23. Distinguish between
(a) Antipyretics and antiseptics.
(b) Acid dyes and basic dyes.
24. What are the requirements for a substance to act as a
dye ? Give one example of each of
(a) Vat dyes and
(b) disperse dyes
25. What is an acid dye ? How is it different from a basic
dye ? Give one example of each.
26. (a) What for is each of the following medicines used
(i) Equanil (b) Bithional.
(b) What are mordant dyne ?
27. Sulpha drugs work like antibiotics but they are not
antibio9tics. Is this a valid statement and why ? Give
one example each for sulpha drugs and antibiotics.
28. Name a broad spectrum antibiotic and state tow
diseases for which it is prescribed.
29. State a difference between acid dyes and basic dyes
and basic dyes. Give one example of each type.
30. (a) Name one medicinal compound each that is used
to treat : (i) hypertension (ii) general body pain
(b) Write the formal distinctin between antiseptics and
disinfectants.
31. (a) List two main ualities for a substance to act as a
dye
(b) Write the formula and IUPAC name of aspirin.
Why should it not be taken on an empty stomach.
32. (a) Choice of a modrant change the colour imparted
by a dye. Illustrate with an example.
(b) Soap is a weak antiseptic. What may be added to
soap to improve its antiseptic action ?
33. Why are detergent preferred over soaps ?
34. What are tranquilisers? Give two examples.
35. How does a dye exhibit colour ?
36. Distinguish between Fibre reactive dyes and ingrain
dyes.
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BRILLIANT
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Guess Paper
37. What are broad spectrum
antibiotics. Give two 42. (a) Define spectrum and broad spectrum antibiotics.
examples.
(b)Give the structure of one broad spectrum
38. What are antimalarials? Give examples.
antibiotic. Mention to diseases for which these
39. What is paracetamol? What medicinal effect does it
antibiotic can be used.
produce in the human body?
43. Describe the following with suitable examples.
40. What are antiseptics and disinfectants? How do they
(a) Preservatives
differ ? Name one substance which act both as
(b) Artificial sweeteners.
antiseptic and distinfectant.
44. Describe the following with suitable examples.
41. What are germicides? Give three examples.
(a) Antioxidants
(b) Edible colours
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