UNIT 1
Periodic Classification of Elements
And Periodicity
Q.1 What is Periodic Table? Give
its purpose also. 12201001
Q.2 Give brief history of
development of periodic table. 12201002
Q.3 State Mendeleev’s Law. Give
its merits and demerits. 12201003
Q.4 State Modern Periodic Law.
Give improvements made by Moseley in Periodic Table.
OR
12201004
How modern periodic law
has removed the discrepancies present in Mendeleev’s Law?
Q.5 Give essential features of
the periodic table. 12201005
Q.6 Briefly explain Groups and Periods. 12201006
Q.7 Briefly write down about Lanthanides and
Actinides. 12201007
1. Q.8 Briefly
write about 12201008
(a) Group
IA, (b) II-A, (c)
VII-A (d) VIII-A
Q.9 Briefly write about the classification of
elements into blocks. 12201009
Q.10 Discuss metals, non-metals and metalloids of
periodic table. 12201010
Q.11 Discuss and justify the position of hydrogen
in periodic table. 12201011
Q.12 Give briefly some trends of properties in
periodic Table. 12201012
2. Q.13 Why
Elements show gradual change in properties? 12201013
Q.14 Explain following in detail.
1. What
is the difference between Atomic and Ionic Radius? Discuss their trends in the
periodic table. 12201014
2. Ionization
Energy 12201015 3. Electron
Affinity 12201016
4. Metallic
Character 12201017 5. Non-metallic Character 12201018
6. Melting
and Boiling points 12201019 7. Oxidation
state 12201020
8. Conductance 12201021 9. Halides 12201022
10. Hydrides 12201023 11. Oxides 12201024
12. Hydration
Energy 12201025
EXERCISE
Q.1 Fill in the blanks.
|
(i) |
Mendeleev,
in his periodic table, arranged the elements according to their atomic
______. 12201026 |
|
(ii) |
Vertical
columns in modern periodic table are called __________ and horizontal rows
are called __________. 12201027 |
|
(iii) |
Members
of group VIIA are called __________ and “alkali metals” is the family name of
__________ group members. 12201028 |
|
(iv) |
Metals
form __________ oxides and non-metals form __________ oxides. 12201029 |
|
(v) |
Hydrogen
can be placed above the groups _______ of the periodic table. 12201030 |
|
(vi) |
Shielding
effect is actually the __________ due to electrons in between the nucleus and
the outermost shell. 12201031 |
|
(vii) |
Noble
gases have the __________ values of ionization energy due to their complete
outermost shells. 12201032 |
|
(viii) |
When
a second electron is added to a uninegative ion, the incoming electron is
__________ by the already present negative charge. 12201033 |
|
(ix) |
Due
to having partly filled d orbitals __________ metals usually show variable
valency. 12201034 |
|
(x) |
Melting
and boiling points of halogens ______________ down the group. 12201035 |
Q.2 Indicate True or False.
|
(i) |
In
Mendeleev’s table, elements Be, Mg, Zn and Cd are placed in the same group. 12201036 |
|
(ii) |
The
second and third periods contain eighteen elements each. 12201037 |
|
(iii) |
Alkaline
earth metals are present in Group IIA. 12201038 |
|
(iv) |
Metals
are present in the top right corner of the Periodic table. 12201039 |
|
(v) |
Metalloids
are present in the lower half of Groups IVA, VA and VIA. 12201040 |
|
(vi) |
Hydrogen
forms uni-negative ion like halogens. 12201041 |
|
(vii) |
Oxidation
state of an element is related to the number of period it belongs. 12201042 |
|
(viii) |
Diamond
is a good conductor of electricity. 12201043 |
|
(ix) |
Melting
points of halogens decrease down the group. 12201044 |
|
(x) |
Zinc
oxide is an example of amphoteric oxides. 12201045 |
Q.3 Multiple
choice questions. Encircle the correct answer . 12201046
Q.4 What are the
improvements made in the Mendeleev’s
Periodic Table 12201047
Q.5 How the
classification of elements in different blocks helps in understanding their
chemistry? 12201048
Q.6 How do you justify
the position of hydrogen at the top of various groups? 12201049
Q.7 Why the ionic radii
increases than its parent ion in the case of negative ion? 12201050
Q.8 Why ionization energy
decreases from top to bottom in a group and increases along a period? 12201051
Q.9 Why the second value
of electron affinity of an element is usually shown with a Positive sign?
3.
Q.10 Why metallic character increases down the
group of metals? 12201053
Q.11 Explain the variation
in melting points along the short periods. 12201054
4.
Q.12 Why the oxidation state of noble gases is
usually zero? 12201055
5.
Q.13 Why diamond is a non-conductor and
graphite is a conductor? 12201056
6.
Q.14 Give brief reason for the following: 12201057
a) d and f-block elements are called
transition elements.
b) Lanthanide contraction controls the
atomic sizes of elements of 6th and 7th periods.
c) The melting and boiling points of the
elements increase from left to the right upto the middle of s and p block
elements and decrease onward.
d) The oxidation states vary in a period
but remain almost constant in a group.
e) The hydration energies of the ions are
in the following order:
Al+3 > Mg2+
> Na+
f) Ionic
character of halides decreases from left to the right in a period.
g) Alkali
metals give ionic hydrides.
h) Although
both sodium and phosphorus are present in the same period of the periodic table
yet their oxides are different in nature, Na2O is basic while P2O5
is acidic in character.
UNIT 2
s-Block Elements
Q.1 (a) What
are s-block elements? 12202001
(b) What
are alkali metals? Why are they called so? 12202002
(c) Give the names, electronic
configurations and occurrence of alkali
metals. 12202003
Q.2 (a) What
are alkaline earth metals? Why are they called so? 12202004
(b) Give
the names, electronic configurations and occurrence of alkaline earth metals. 12202005
Q.3 (a) What
is meant by peculiar behaviour of elements? 12202006
(b) Discuss
the peculiar behaviour of lithium with respect to the other members of alkali
metals. 12202007
(c) What
is the cause of this peculiar behaviour? 12202008
Q.4 Discuss
the peculiar behaviour of beryllium with respect to the other members of
alkaline earth metals. What is the cause of this behaviour? 12202009
Q.5 Discuss the trends in the
chemical properties of alkali metals. 12202010
Q.6 Discuss trends in chemical properties of
alkaline earth metals. 12202011
Q.7 (a) Discuss the trends in chemical
properties of compounds like oxides, hydroxides, carbonates, nitrates and
sulphates of group I-A and II-A elements.
12202012
(b) Define:- 12202013
(i) Washing
soda (ii) Soda ash
(iii) Lime
water (iv) Milk of magnesia
Q.8 (a) Compare
the physical and chemical properties of alkali metals with those of alkaline –
earth metals. 12202014
(b) What
happens when:- 12202015
(i) Lithium
carbonate is heated.
(ii) Lithium
hydroxide is heated to red hot.
(iii) Beryllium
is treated with sodium hydroxide.
(iv) Lithium
hydride is treated with water.
Q.9 (a) Describe
with diagram the manufacture of sodium by Down’s Cell. 12202016
(b) Point
out the three advantages of this process.
12202017
Q.10 (a) Discuss the commercial preparation of
sodium hydroxide by Nelson’s Cell or Diaphragm Cell. 12202018
(b) What are the two major problems in the working
of the Nelson’s cell? How are they removed? 12202019
1. Q.11 (a) What is gypsum? 12202020
(b) Discuss
the role of gypsum in agriculture and industry. 12202021
(c) What
is plaster of Paris? How it sets? 12202022
(d) What
is special plaster? What are its different types? 12202023
(e) How
is Portland cement made? 12202024
Q.12 (a) Define
lime. 12202025
(b) What
do you mean by slaking of lime? 12202026
(c) What
are the applications of lime in agriculture and industry? 12202027
EXERCISE
Q.1 Fill in the blanks:
1. Alkali metals are __________ reactive than alkaline-earth metals. 12202028
2. Alkali metals decompose water vigorously, producing __________ and
hydrogen. 12202029
3. When heated in a current of dry
hydrogen, alkaline earth metals form white crystalline __________ of the type
MH2. 12202030
4. The beryllium hydroxide, like the
hydroxide of aluminium is amphoteric, while the hydroxides of the other members
of the group IIA are __________. 12202031
5. The elements of the group IA are termed
as alkali metals, because their __________ are alkaline. 12202032
6. Spodumene is an ore of__________ metal. 12202033
7. Alkali metal nitrates on heating give the corresponding __________
and oxygen.
12202034
8. Na2CO3.H2O is the chemical
formula of a mineral of sodium which is known as __. 12202035
9. Metallic bicarbonates are decomposed on
heating into their carbonates, alongwith ________ and __________. 12202036
10. Metal nitrates other than the alkali
metals on heating decompose into the corresponding metal __________ alongwith
the evolution of nitrogen peroxide and oxygen. 12202037
Q.2 Indicate True/False:
1. Group IA elements are called alkali metals because their chlorides
are alkaline in nature.
12202038
2. Alkali metals are very good conductor of electricity. 12202039
3. The hydroxides of alkali metals and alkaline earth metals are
soluble in water. 12202040
4. Plaster of Paris is hemihydrate. 12202041
5. Alkali metals have low melting and
boiling points as compared to those of alkaline earth metals. 12202042
6. Lithium carbonate is decomposed to its
oxide, but the carbonates of the other alkali metals are stable towards heat. 12202043
7. All alkali metal sulphates are insoluble in water. 12202044
8. Lithium combines with nitrogen to form
lithium nitride but other alkali metals do not react with nitrogen. 12202045
9. Trona is an ore of lithium. 12202046
10. Alkaline earth metals are stronger reducing agents than alkali
metals. 12202047
Q.3 Multiple Choice Questions.
Encircle the correct answer. 12202048
Q.4(a) Give
the names, electronic configurations and occurrence of s-block elements. 12202049
(b) Discuss the peculiar behaviour of lithium
with respect to the other members of alkali metals. 12202050
Q.5 Discuss the trends in chemical properties of compounds like
oxides, hydroxides, carbonates, nitrates and sulphates of IA and IIA group
elements. 12202051
Q.6 Compare the chemical behaviour of lithium with magnesium. 12202052
Q.7 (a) Mention the
properties of the beryllium in which it does not resemble with its own family. 12202053
(b) Why the aqueous solution of Na2CO3
is alkaline in nature? 12202054
Q.8 (a) Describe with diagram the manufacture of sodium by Down’s
cell. 12202055
(b) Point out the three advantages of this process. 12202056
Q.9 (a) Compare the
physical and chemical properties of alkali metals with those of alkaline-earth
metals. 12202057
(b) What happens when? 12202058
(i) Lithium carbonate is heated. 12202059
(ii) Lithium hydroxide is heated to red hot 12202060
(iii) Beryllium is treated with sodium hydroxide. 12202061
(iv) Lithium hydride is treated with water.
12202062
Q.10 Give formulas of the following minerals:
(a)
Dolomite 12202063
(b) Asbestos 12202064
(c) Halite 12202065
(d)
Natron 12202066
(e) Beryl 12202067
(f) Sylvite 12202068
(g)
Phosphorite 12202069
(h) Chile saltpeter 12202070
Q.11 Answer the following questions briefly:
(a) Why alkali and alkaline earth metals are among the reactive
elements of the periodic table? 12202071
(b) Why lime water turns milky with CO2 but becomes
clear with excess CO2? 12202072
(c) How is gypsum converted into plaster of paris? 12202073
(d) Why is 2% gypsum added in the cement? 12202074
(e) Why is lime added to an acidic soil? 12202075
(f) How are lime and sand used to make glass? 12202076
(g) How is lime mortar prepared? 12202077
|
Q.1 (a) Give
the names and the electronic configuration of Group IIIA elements of the
periodic table. 12203001
(b)
Discuss some important physical
properties of Boron family or Group IIIA elements. 12203002
Q.2 How
IIIA group elements exist in nature? Name their important minerals and write
their formulae. 12203003
Q.3 Discuss
the peculiar behaviour of Boron with respect to the other members of the Group
IIIA elements. 12203004
Q.4 (a) What is Borax? How it occurs in nature? 12203005
(b)
Describe the commercial preparation
of Borax. 12203006
(c) Write
down some important physical properties of Borax. 12203007
(d)
Give the reactions of Borax with: 12203008
(i)
An Acid (ii) NH4Cl (iii)
Water
(e)
What happens when Borax is heated? 12203009
(f)
What is Borax Bead Test? 12203010
(g)
Outline the principle uses of the
Borax. 12203011
(h)
How does Borax serve as water
softening agent? 12203012
Q.5 (a) Give the names and the formulas of acids
of boron. 12203013
(b) Which
one of the boric acids is stable? How metaboric acid (HBO2) and
tetra-boric acid (H2B4O7) and pyroboric acid
(H6B4O9) behave in water solution?
12203014
(c) What
is boric acid? Describe its preparation on commercial scale.
12203015
(d) Give properties and uses of Boric Acid. 12203016
Q.6 (a) Give the names alongwith the formulas of
three important ores of aluminium.
12203017
(b) How and under what conditions does aluminium
react with the following?
12203018
(i) Oxygen 12203019 (ii) Hydrogen 12203020 (iii) Halogens 12203021
(iv) Acids 12203022 (v)
Alkalies 12203023 (vi) Salt Solution 12203024
(c) Describe the important uses of aluminium.
Q.7 (a) Give
the names, electronic configurations and some important physical properties of
Group IVA elements of the Periodic Table. 12203025
(b) What
are the common chemical properties of Group IVA elements of the Periodic Table? 12203026
(c) What is
inert pair effect? 12203027
Q.8 Discuss
the peculiar behaviour of carbon with respect to the other members of Group IVA
of the periodic table. 12203028
Q.9 Write
down names and chemical formulas of some important minerals of carbon and
silicon. 12203029
Q.10 (a) Name the important oxides of carbon. 12203030
(b) Write
down some important features of structure of carbon monoxide and carbon
dioxide. 12203031
Q.11 (a) What is silica? Name some important
types of silica and write down their properties. 12203032
(b) What
is difference between structure of carbon dioxide and silicon dioxide?
(c) What is vitreous silica or silica glass? How is it produced?
12203033
Q.12 (a) Discuss the preparation, properties and
important uses of following silicates.
12203034
(1) Sodium Silicate 12203035 (2) Aluminium
Silicate 12203036
(3) Talc or soapstone 12203037 (4) Asbestos
12203038
(b) (i) How is stoneware
Glazed? 12203039
(ii) How is Clay Hardened? 12203040
Q.13 (a) What are silicones? 12203041
(b) Discuss
that chemistry of silicon resembles in many respects to that of carbon. 12203042
(c) How are silicones prepared? 12203043
(d) Give a brief summary of the principle properties of silicones. 12203044
(e) Outline the uses of silicones. 12203045
Q.14 (a) What are semiconductors? Why are they named so? 12203046
(b) What is the effect of temperature on semiconductors? 12203047
(c) Write some important uses of semiconductors. 12203048
Q.15 What
are lead pigments? Give their preparations, properties and uses. 12203049
EXERCISE
Q. 1 Fill in the blanks:
1. __________ acid has the
chemical formula HBO2. 12203050
2. Aluminium
normally occurs as __________ minerals found in the rocks of outer portion of
the earth. 12203051
3. Aluminium gives________ gas
with hot concentrated H2SO4. 12203052
4. Boron
forms __________ bond in its compounds. 12203053
5. The
chemical formula of white lead is __________. 12203054
6. __________
is the only element with less than four electrons in the outer most shell that
is not a metal. 12203055
7. In the Group IIIA of the
Periodic table, __________ is a semi-metal. 12203056
8. Borax
that occurs as a natural deposit, is called __________. 12203057
9. Cryolite
is an important mineral of aluminium and its formula is __________.
12203058
10. A
__________ is a substance that has different resistances to the passage of an
electric current under different circumstances. 12203059
Q.2 Indicate
True/False:
1. Boron
always uses all the three of its valence electrons for bonding purposes.
12203060
2. Diaspore is an ore of carbon. 12203061
3. Emerald
is an ore of aluminium that has the chemical formula Al2O3.2SiO2.2H2O. 12203062
4. An aqueous solution of borax is
feebly acidic in nature. 12203063
5. In
case of borax bead test of cupric oxide, the beads are coloured blue in the
reducing flame. 12203064
6. Boric acid can be titrated with
sodium hydroxide. 12203065
7. Carbon and silicon are the only
non-metals in Group IVA. 12203066
8. PbO is commonly known as
litharge. 12203067
9. Basic lead carbonate is a
reddish brown pigment. 12203068
10. Aluminum oxide (Al2O3)
is also called bauxite. 12203069
Q.3 Multiple
Choice Questions. Encircle the correct answer. 12203070
Q.4 What
is the action of an aqueous solution of borax on litmus? 12203071
Q.5 Give
equations to represent the following reactions. 12203072
(a) Borax is heated with CoO 12203073
(b) Al2O3
is heated with NaOH solution 12203074
Q.6 Why is aluminium not
found as a free element? Explain the chemistry of borax bead test. 12203075
Q.7 How
does orthoboric acid react with: 12203076
(a) Sodium hydroxide (b)
Ethyl alcohol
Q.8 How
will you convert boric acid into borax and vice versa? 12203077
Q.9 Why are liquid silicones preferred over
ordinary organic lubricants? 12203078
Q.10 Explain:
(a)
CO2 is non-polar in nature. 12203079
(b) CO2 is acidic in character. 12203080
Q.11 Why is CO2 a gas at room temperature while SiO2
is a solid? 12203081
Q.12 Give the names and the formulas of different acids of boron. 12203082
Q.13 What is the importance of oxides of lead in paints? 12203083
Q.14 Give the names, electronic configurations
and occurrence of Group-IIIA elements of the Periodic Table. 12203084
Q.16 (a) What
is Borax? 12203086
(b) Describe its commercial preparation. 12203087
(c) Outline the principal uses of borax. 12203088
(d) How does borax serve as a water softening
agent? 12203089
Q.17 (a) What is boric acid? 12203090
(b) How is boric acid prepared in laboratory? 12203091
(c) Give properties and uses of boric acid. 12203092
Q.18 (a) Give
the names alongwith the formulas of three important ores of aluminium. 12203093
(b) How and under what conditions does aluminium
react with the following:
(i)
Oxygen, (ii) Hydrogen, (iii) Halogens, (iv) Acids, (v) Alkalies. 12203094
Q.19 Give the names, electronic configurations
and occurrence of Group-IVA elements of the Periodic Table. 12203095
Q.21 (a) What are silicones? 12203097
(b) Give a brief summary of the principal
properties of silicones. 12203098
(c) Outline the uses of silicones. 12203099
(d) What are silicates? 12203100
(e) Describe the important uses of silicates. 12203101
|
Q.1 (a) Discuss the trend in physical properties of VA elements. 12204001
(b) Describe the occurrence of
nitrogen and its compounds. 12204002
Q.2: Describe oxides of nitrogen with their preparation and reactions. 12204003
Q.3 Write a detailed note on
oxyacids of nitrogen. 12204004
Q.4: (a) Explain the Birkeland
and Eyde’s process for the manufacture of nitric acid. 12204005
(b) Discuss reactions and uses of
nitric acid. 12204006
Q5.
Write a note on occurrence of Phosphorus and its compounds. Discuss allotropes
of phosphorus. 12204007
Q. 6: Discuss the trends in
physical properties of group VIA elements. 12204008
Q. 7: Describe the chemistry of
the industrial preparation of sulphuric acid by the contact process. 12204009
Q8. Give chemical properties and uses of
sulphuric acid. 12204010
EXERCISE
Q.1 Fill
in the blanks:
1. The
elements __________ of group VA are called metalloids. 12204011
2. During
Birkeland and Eyde’s process _______ is prepared from atmospheric oxygen and nitrogen. 12204012
3. The
tendency to form long chain of atoms is called __________. 12204013
4. All
the elements of group VIA show the property of __________. 12204014
5. Selenium
shows two allotropic forms which are called __________ forms. 12204015
6. Specific
gravity of H2SO4 at 18°C is __________. 12204016
7. H2
is produced by reacting H2SO4 with metals, like
__________. 12204017
8. The
elements of group VA exhibit maximum oxidation state of __________.
12204018
9. The
outermost shell of group __________ elements contain six electrons. 12204019
10. Oxygen
shows __________ behaviour due. to the presence of unpaired electrons. 12204020
11. Conc.
phosphoric acid acts as a __________. 12204021
12. Nitrogen
is a gas while other elements of the same group are __________. 12204022
13. Noble
metals like gold and platinum are dissolved in __________. 12204023
14. Sulphur
is different from oxygen because it shows __________ oxidation states.
12204024
15. HNO3
is used in the manufacture of __________ fertilizers. 12204025
Q.2 Indicate
True/False:
1. The
metallic character in group VA and VIA elements increases down the group. 12204026
2. The
elements of group VA exhibit maximum oxidation state of +5. 12204027
3. Ionization
energy of phosphorus is greater than that of nitrogen. 12204028
4. The
electronegativity of oxygen is greater than all other elements of groups VA and
VIA. 12204029
5. V2O5
is used as catalyst for the oxidation of SO2 to SO3. 12204030
6. The
oxides of nitrogen are basic in nature. 12204031
7. Aqua
regia is prepared by mixing 3 parts of Conc. HNO3 with one part of
conc. HCl. 12204032
8. TNT is
prepared by the reaction of nitric acid with toluene.
12204033
9. P2O3
when reacts with cold water gives phosphorus acid and with hot water it gives
phosphoric acid. 12204034
10. Sulphur occurs
in many organic compounds of animal and vegetable origins. 12204035
Q.3 Multiple
Choice Questions. Encircle the correct answer 12204036
Q.4 Short
questions:
(i) How
does nitrogen differ from other elements of its group? 12204037
(ii) Why does aqua regia dissolve gold and platinum? 12204038
(iii) Why the elements of
group VIA other than oxygen show more than two oxidation states? 12204039
(iv) Write down a comparison of the properties of oxygen and sulphur. 12204040
(v) Write down the equation
for the reaction between conc. H2SO4 and copper and
explain what type of reaction is it. 12204041
Q. 5. (a) Explain the
Birkeland and Eyde’s process for the manufacture of nitric acid.
12204042
(b) Which metals evolve
hydrogen upon reaction with nitric acid? Illustrate alongwith chemical
equations. 12204043
(c) What is meant by fuming nitric acid? 12204044
Q.6 (a) Sulphuric acid is said to act as an acid, an oxidizing agent
and a dehydrating agent, describe two
reactions in each case to illustrate the truth of this statement. 12204045
(b) Give the advantages of contact process for the
manufacture of sulphuric acid.
Q.7 (a) Describe the chemistry of the industrial preparation of
sulphuric acid from sulphur by the contact process. 12204047
(b) Why is SO3 dissolved in H2SO4
and not in water? 12204048
(c) Explain the action of sulphuric acid on metals alongwith chemical
equations. 12204049
Q.8 Describe the preparation of NO2 gas. Also give its
reactions. 12204050
Q.9 How PCl3 and PCl5 can be used for the
preparation of other chemical compounds?
12204051
Q.10 Answer the following questions:
(i) Describe “Ring test” for the confirmation of the presence of
nitrate ions in solution.
(ii) NO2 is a strong oxidizing agent. Prove the truth of this
statement giving examples.
12204053
(iii) Write down the chemical
equations and names of the products formed as a result of the reaction of HNO3
with arsenic and antimony.
12204054
(iv) Give the methods of preparation of PCl3.
12204055
(v) P2O5 is a powerful dehydrating agent. Prove
giving example. 12204056
Q.11 Complete and balance the following chemical equations. 12204057
1. P + NO2 ¾¾® 2. NO + Cl2 ¾¾®
3. H2S + NO ¾¾® 4. Pb(NO3)2 ¾¾®
5. NO2 + H2O ¾¾® 6. NO2 + H2SO4
¾¾®
7. HNO2 + HI ¾¾® 8. HNO2+NH3 ¾¾®
9. HNO2 + CO(NH2)2 ¾¾® 10. KNO3+H2SO4
¾¾®
Q.12 Describe the methods of preparation of phosphorus pentoxide and
explain its reactions. 12204058
Q.13 Discuss the trends in physical properties of group VIA
elements. 12204059
|
Q2. How fluorine differs from the other
members of its own group? 12205002
Q3. Write a note on oxidizing properties of
halogens. 12205003
Q4. Discuss
different compounds of halogens and their properties in detail.
12205004
Q5: What is Bleaching powder? How is it
prepared commercially? Give its uses. 12205005
Q6: Discuss the various commercial uses of
halogens and their compounds. 12205006
Q7. (a) What
are noble gases? Explain their inertness on the basis of their electronic
configuration. 12205007
(b) Discuss
general properties of noble gases. 12205008
Q8. What type of compounds are formed by
Xenon? Discuss their chemical reactions.
12205009
Q9: a:
Write a note on oxyfluorides and oxides of xenon. 12205010
b: Write a
note on applications of noble gases.
12205011
EXERCISE
Q.1 Fill in the Blanks.
(i) The halogen
with the highest electronegativity is _________. 12205012
(ii) HI is
__________ agent. 12205013
(iii) The
only halogen acid which is not a strong acid is _________. 12205014
(iv) Tincture of
__________ is common antiseptic. 12205015
(v) The
halogen with the lowest melting and boiling points is ______. 12205016
(vi) Bleaching
powder is prepared from __________ and . 12205017
(vii) __________
is the halogen which causes burns on the skin which heal slowly.
12205018
(viii) __________ is used for making
unshrinkable wool. 12205019
(ix) A
mixture of __________ and __________ is used for breathing by the sea divers. 12205020
(x) Noble gas used to fill fluorescent tubes is
__________. 12205021
Q.2 Indicate True or False.
(i) HF is used
for etching glass. 12205022
(ii) HI is
weaker reducing agent as compared to HF. 12205023
(iii) Bleaching
powder is completely soluble in water.
12205024
(iv) The formula
of perchloric acid is HClO2. 12205025
(v) On warming
aqueous KOCl disproportionate as follows: 12205026
3KOCl ¾¾® 2KCl
+ KClO3
(vi) a - Particles emitted by radioactive elements are ions
of radon. 12205027
(vii) Radon
is the only one of the noble gases that is radioactive. 12205028
(viii) The
molecules of the noble gases are all monoatomic. 12205029
(ix) Argon is
used to fill electric bulbs. 12205030
(x) The
noble gas which is present in the largest amount in atmosphere is krypton.
12205031
Q.3 Multiple Choice Questions. Encircle the correct answer. 12205032
Q.4 Short Questions.
(i) What is “Iodized Salt? 12205033
(ii) What are Freons and Teflon. 12205034
(iii) Arrange
the following ions in order of increasing size: 12205035
F-, Cl-, I-, Br-
(iv) Why iodine has metallic luster? 12205036
(v) Which halogen sublimes to violet vapours? 12205037
(vi) Which halogen is used as an antiseptic? 12205038
(vii) Which halogen is used in water treatment
to kill bacteria? 12205039
(viii) Name the gas which is used for earthquake
prediction. 12205040
(ix) Name the gas which is used in bactericidal
lamps. 12205041
Q.5 What is bleaching powder? How it is
prepared commercially? Give its uses.
12205042
Q.6 (a) Discuss the oxides of chlorine. 12205043
(b) What
are disproportionation reactions? Explain your answer with an example.
Q.7 Discuss the system of nomenclature used
for oxyacids of halogens. Supply your answer with examples. 12205045
Q.8 (a) How the halogen acids are
ionized in water? 12205046
Q.9 In the following sets, arrange the
substances in order of the property indicated. Give reasons. 12205048
(a) Increasing
acidic character 12205049
HClO,
HClO2, HClO3, HClO4
(b) Increasing
oxidizing power 12205050
F2
> Cl2 > Br2 > I2
Q.10 What happens when bleaching powder reacts
with the following reagents; Dil. H2SO4, excess of Conc.
H2SO4, NH3, HI and CO2. 12205051
2CaOCl2 + Conc. H2SO4(excess)
¾¾® CaSO4
+ H2O + Cl2
2CaOCl2 + dil H2SO4
¾¾® CaSO4
+ CaCl2 + 2HClO¯
3CaOCl2+2NH3 ¾¾® 3CaCl2
+ 3H2O + N2
CaOCl2+ CO2 ¾¾® CaCO3
+ Cl2 OR
2CaOCl2 + H2O + CO2
¾¾® CaCO3
+ CaCl2 + 2HOCl
Q.11 Discuss the various commercial uses of
halogens and their compounds. 12205052
Q.12 What are noble gases? Explain their
inertness on the basis of their electronic configuration. 12205053
Q.13 Write
notes on the followings:
(i) Oxyfluorides of xenon. 12205054
(ii) Applications of noble gases 12205055
UNIT 6
Transition Elements
Q1. What are
transition elements? Discuss general characteristics of transition elements.
12206001
Q2. What are coordination compounds?
Discuss their components with suitable examples. 12206002
Q3. Describe
the rules for naming the coordination complexes and give examples. 12206003
Q4. (a)
What are the important ores and commercial forms of Iron? 12206004
(b) How can
Wrought iron be manufactured from cast iron? 12206005
Q5. (a) What is steel? How is it
classified? 12206006
(b) Give methods for the manufacture of
steel? 12206007
Q6. Define
corrosion. Explain acid and electrochemical theory of corrosion in detail.
12206008
Q7. Describe
how corrosion of metals can be prevented? 12206009
EXERCISE
Q.1 Fill
in the Blanks.
1. The property of paramagnetism is due to the presence
of_____ electrons. 12206010
2. MnO41- ion has __________ colour and Cr2O72- has __________ colour. 12206011
3. When potassium chromate is treated with an acid
__________ is produced. 12206012
4. The d-block elements are located between _________ and
__________ elements. 12206013
5. Oxidation number of Fe in K4[Fe(CN)6]
is _____ while in K3[Fe(CN)6] it is___. 12206014
6. The presence
of __________ in a metal promotes corrosion. 12206015
7. If Cu is in
contact with Aluminium __________ gets corroded. 12206016
8. Complexes
having sp3d2 hybridization have __________ shapes. 12206017
9. In naming the complexes, all the ligands are named in
__________. 12206018
10. In an aqueous solution CrO42- and Cr2O72- exist in the form of __________. 12206019
Q.2 Indicate
True or False.
1. A substance which is attracted into a magnetic field is
said to be diamagnetic. 12206020
2. Compounds of
the transition elements are mostly coloured. 12206021
3. Fe3+
ions are blue when hydrated. 12206022
4. An extreme
case of paramagnetism is called diamagnetism. 12206023
5. Tin plating is
used to protect iron sheets from corrosion. 12206024
6. In
Galvanizing, Zinc prevents corrosion of iron. 12206025
7. Tin plated iron gets rusted more rapidly when the
protective coating damaged than unplated
iron. 12206026
8. The name of anionic
ligands in a complex end in suffix ‘O’. 12206027
9. Pig iron
contains greater percentage of carbon than steel. 12206028
10. Complex compounds having dsp2 hybridization have
tetrahedral geometry. 12206029
Q.3 Multiple
Choice Questions. Encircle the correct answer 12206030
Q.4 How does the electronic configuration
of valence shell affect the following properties of the transition elements? 12206031
(a) Binding energy (b) Paramagnetism
(c) Melting points (d) Oxidation states
Q.5 Explain the following terms, giving
examples. 12206032
(a) Ligands 12206033 (b) Coordination sphere 12206034
(c) Substitutional
alloy 12206035 (d) Central metal atom 12206036
Q.6 Describe the rules for naming the
coordination complexes and give examples. 12206037
Q.7 What is the difference between wrought
iron and steel? Explain the Bessemer process for the manufacture of steel. 12206038
Q.8 Explain the following giving reasons: 12206039
(a) Why
damaged tin plated cause should be avoided? 12206040
(b) Under
what conditions aluminium corrodes? 12206041
(c) How
does the process of galvanizing protect iron from rusting? 12206042
Q.9 How chromate ions are converted into
dichromate ions? 12206043
Q.10 Describe the preparation of KMnO4
& K2CrO4. 12206044
Q.11 Give systematic names to following
complexes. 12206045
(a) [Fe(CO)5] 12206046 (b) [Co(NH3)6]Cl3 12206047
(c) [Fe(H2O)6]+2 12206048 (d) Na3[CoF6] 12206049
(e) K2[Cu(CN)4] 12206050 (f) K2[PtCl6] 12206051
(g) [Pt(OH)2(NH3)4]SO4
12206052 (h) [Cr(OH)3(H2O)3] 12206053
UNIT 7
Fundamental Principles of
Organic
Chemistry
Q1a. What is organic chemistry? Explain the
importance of Wohler’s work in the development of organic chemistry. 12207001
b. Discuss some characteristic features of
organic compounds. 12207002
c. What are the sources of organic compounds? 12207003
d. What is the importance of organic chemistry? 12207004
Q2. Write a short note on cracking of
hydrocarbons. 12207005
Q3. Explain reforming of petroleum with the
help of suitable example. 12207006
Q4. How organic compounds are classified?
Give suitable example of each type. 12207007
Q5. What is
meant by functional group? Name typical functional groups containing oxygen.
Functional
Groups: 12207008
Q.6. What is
orbital hybridization? Explain sp3, sp2 and sp modes of
hybridization of carbon.
12207009
EXERCISE
Q.1 Fill in the Blanks.
1. Organic
compounds having same molecular formula but different _________ are called
isomers. 12207010
2. The
state of hybridization of carbon atom in _________ is sp2. 12207011
3. Alkenes
show _________ due to restricted rotation around a carbon-carbon double bond. 12207012
4. Heating
an organic compound in the absence of oxygen and in the presence of _________
as a catalyst is called cracking. 12207013
5. A
group of atoms which confers characteristic properties to an organic compound
is called _________. 12207014
6. 2-Butene
is _________ of l-butene. 12207015
7. Carbonyl
functional group is present in both _________ and ketones. 12207016
8. A
heterocyclic compound contains an atom other than _________ in its ring. 12207017
9. The
quality of gasoline can be checked by finding out its _________. 12207018
10. A
carboxylic acid contains _________ as a functional group. 12207019
Q.2 Indicate True/False:
1. There are
three possible isomers for pentane. 12207020
2. Alkynes do
not show the phenomenon of cis-trans isomerism. 12207021
3. Organic
compounds can not be synthesized from inorganic compounds. 12207022
4. All close
chain compounds are aromatic in nature. 12207023
5. The
functional group present in amides is called an amino group. 12207024
6. Government
of Pakistan is trying to use coal for power generation. 12207025
7. Crude
petroleum is subjected to fractional distillation in order to separate it into
different fractions. 12207026
8. A
bond between carbon and hydrogen serves as a functional group for alkanes. 12207027
9. o-Nitrotoluene
and p-nitrotoluene are the examples of functional group isomerism. 12207028
10. Almost
all the chemical reactions taking place in our body are inorganic in nature. 12207029
Q.3 Multiple Choice Questions. Encircle the correct answer. 12207030
Q.4. How
are organic compounds classified? Give suitable example of each type. 12207031
Q.5. What
are homocyclic and heterocyclic compounds? Give one example of each.
(Board 2007) 12207032
Q.6 Write
the structural formulas of the two possible isomers of C4H10. 12207033
Q.7 Why is ethene an important industrial
chemical? 12207034
Q.8 What is
meant by a functional group? Name typical functional groups containing oxygen. 12207035
Q.9 What is
an organic compound? Explain the importance of Wohler’s work in the development
of organic chemistry. 12207036
Q.10 Write a
short note on cracking of hydrocarbons. 12207037
Q.11 Explain
reforming of petroleum with the help of suitable example. 12207038
Q.12 Describe important sources of organic
compounds. 12207039
Q.13 What is
orbital hybridization? Explain sp3, sp2 and sp modes of
hybridization of carbon. 12207040
Q.14 Explain
the type of bonds and shapes of the following molecules using hybridization
approach. 12207041
CH3-CH3, CH2 = CH2, CH º CH, HCHO, CH3Cl
Q.15 Why there
is no free rotation around a double bond and a free rotation around a single
bond? Discuss cis-trans isomerism. (Board 2013)
12207042
UNIT 8
Aliphatic
Hydrocarbons
Q.1: What are hydrocarbons? Give their classification. 12208001
Q.2: (a)
According to which system, hydrocarbons
are named? 12208002
(b) What are the rules for naming alkanes, alkenes
and alkynes according to IUPAC system? 12208003
1.
Q. 3: Define
Alkanes. Give general methods of preparation of alkanes. 12208004
Q. 4: Write
a note on physical characteristics and reactivity of Alkanes. 12208005
Q.5: Why
alkanes are called paraffins? Why is sigma bond inert? 12208006
2. Q.6: (a)
Discuss chemical reactions of Alkanes in detail. 12208007
(b) Give uses of methane. 12208008
Q.7: Why are alkenes called olefins? Give
general methods of preparation of alkenes. 12208009
Q. 8: (a)
Discuss physical properties of alkenes.
12208010
(b) Discuss reactivity of a p bond. 12208011
i.
Q.9: Discuss reactions of Alkenes in detail. 12208012
Q. 10: Give
uses of ethene. 12208013
Q.11: (a) What
are Alkynes? 12208014
(b) Give general methods of preparation of Alkynes. 12208015
Q.12: Discuss physical characteristics of Alkynes and their reactivity. 12208016
Q.13: Write a note on addition,
oxidation and polymerization reactions of Alkynes. 12208017
Q.14: Write a note on acidic
nature of Alkynes. 12208018
Q.15: Give uses
of ethyne. 12208019
Q.16: Give comparison of
reactivity of alkanes, alkenes and alkynes. 12208020
EXERCISE
Q.1 Fill
in the Blanks.
1.
Ozone reacts with ethene to form ___________. 12208021
2.
Lindlar’s catalyst is used for ___________ of alkynes. 12208022
3.
Divinyl acetylene is a ___________ acetylene. 12208023
4.
Vicinal dihalides have two halogens on ___________ carbon atoms. 12208024
5.
Ethyne is acidic in character because of ___________ hybridization. 12208025
6.
Halohydrins are formed due to addition of ___________ in ethene. 12208026
7.
Ethylene glycol is produced when ___________reacts with cold alkaline
KMnO4 solution. 12208027
8.
Mustard gas is a high boiling ___________. 12208028
9.
Ethyne has ___________ like odour. 12208029
10.
Ethyne is obtained by the reaction of ___________ with calcium carbide. 12208030
Q.2 Indicate
True/False:
1. Addition of HX to
unsymmetrical alkanes takes place according to Markownikov’s rule.
12208031
2. Methane reacts with bromine
water and its colour is discharged. 12208032
3. Mustard gas is a blistering
agent. 12208033
4. Methane is also called marsh
gas. 12208034
5. Ethyne is a saturated
compound. 12208035
6. Baeyer’s reagent is used to
locate a double bond in an alkene. 12208036
7. Alkanes usually undergo
substitution reactions. 12208037
8. Benzene is a polymer of
ethene. 12208038
9. Acrylonitrile can be
obtained from ethyne. 12208039
10. Ethyne is more reactive
towards electrophilic reagents than ethene. 12208040
Q.3. Multiple choice
questions. Encircle the correct answer. 12208041
Q.4. Write the structural
formula for each of the following compounds.
(i) 2-Methylpropane. 12208042 (ii) Neopentane. 12208043
(iii) 3-Ethylpentane 12208044 (iv) 4-Ethyl 3,4 dimethyl heptane
12208045
(v) 2,2,3,4 Tetramethyl pentane 12208046 (vi) 4-iso-propylheptane. 12208047
(vii) 2,2-Dimethylbutane. 12208048 (viii) 2,2-Dimethylpropane 12208049
Q. 5. Write down the names of
the following compounds according to IUPAC system.
12208050
Q. 6. What are the rules for
naming alkanes? Explain with suitable examples. 12208051
Q. 7. (a) Write
down the structural formulas for all the isomeric hexanes and name them
according to IUPAC system. 12208052
(b) The following names are incorrect. Give the correct IUPAC names. 12208053
Q. 8. (a) Explain
why alkanes are less reactive than alkenes? What is the effect of branching on
the melting points of alkanes? 12208054
3. (b) Three
different alkenes yield 2-Methylbutane when they are hydrogenated in the
presence of a metal catalyst. Give their structures and write equations for the
reactions involved. 12208055
Q. 9. (a) Outline the methods available for the
preparation of alkanes. 12208056
(b) How
will you bring about the following conversions? 12208057
(i) Methane to Ethane 12208058 (ii) Ethane to Methane 12208059
(iii) Acetic acid to Ethane 12208060 (iv) Methane
to Nitromethane 12208061
Q. 10. (a) What is meant by Octane Number? Why does a
high octane fuel has less tendency to knock in an automobile engine? 12208062
(b) Explain
free radical mechanism for the reaction of Chlorine with methane in the presence of sunlight. 12208063
Q. 11. (a) Write structural formulas for each of the
following compounds.
(i) iso –
Butylene 12208064 (ii)2,3,4,4 –
Tetramethyl – 2 – pentene 12208065
(iii) 2, 5 – Heptadiene 12208066 (iv) 4,5 – Dimethyl – 2 – hexene 12208067
(v) Vinylacetylene 12208068 (vi) 1,3 – Pentadiene 12208069
(vii) 1 - Butyne 12208070 (viii)3 – n
propyl – 1, 4 – Pentadiene 12208071
(ix) Vinylbromide 12208072 (x) But - 1 en - 3 - yne 12208073
(xi) 4 – Methyl – 2 – pentyne 12208074 (xii) iso-Pentane 12208075
(b) Name the following Compounds by IUPAC
system. 12208076
(i) CH3–CH=CH(CH2)2CH3
(ii) (CH3)2 C = CH2
(iii)
(iv) CH2 = CH – CH = CH2
(v) CH2
= C – CH2– CH2– CH3
|
C2H5
(vi) CH
º C – CH3
(vii) CH3
– C º C – CH3
(viii) CH2
= CH – C º C – CH = CH2
(ix) CH
º C – CH = CH – C º C – H
(x) CH2
= CH – C º C – H
Q.12. (a) Describe different methods for the
preparation of alkanes. How would you establish that ethylene contains a double
bond? 12208077
(b) Give structural formulas
of the alkenes expected to form by the dehydrohalogenation of the following
compounds by a strong base. 12208078
(i) Chloropentane 12208079
(ii) 2
– Chloro – 3 – methyl butane 12208080
(iii) 1
– Chloro – 2, 2 – dimethyl propane 12208081
(i) Dehydrohalogenation of
chloropentane. 12208082
Q.13 (a) Write down chemical equations for the
preparation of propene from the following compounds. 12208083
(i) CH3
– CH2 – CH2 – OH 12208084 (ii) CH3
– C º C – H 12208085
(iii) iso
– Propyl chloride 12208086
(b) Write
skeleton formula showing only the arrangement of carbon atoms for all possible
alkenes of the molecular formula C5H10. 12208087
Q.14 (a) How may ethene be converted into
ethylalcohol? 12208088
(b) Starting from ethene, outline the reactions for the preparation of
following compounds.
(i) (1,2–Dibromoethane) Ethylene dibromide 12208089
(ii) Ethyne 12208090
(iii) Ethane 12208091
(iv) Ethylene glycol 12208092
(c) How will you bring about the
following conversions? 12208093
(i) 1 – Butene to 1–Butyne 12208094
(ii) 1 – Propanol to 12208095
Q.15 Show by means of chemical
equations how the following cycle of changes may be affected. 12208096
¯¾¾¾¾¾¾¾¾¾¾¾¾¾¾¾|
Ethane
¾¾¾® Ethene ¾¾¾® Ethyne
(i) H2, Pt. 12208098 (ii) Br2 in CCl4 12208099
(iii) Cold dil KMnO4/OH- 12208100 (iv) HBr 12208101
(v) O2 in the presence of Ag 12208102 (vi) HOCl 12208103
(vii) Dil H2SO4 12208104
Q.17 In the following
reactions, identify each lettered product. 12208105
(i) Ethyl alcohol 
A
B 
C 12208106
(ii) Propene D 
E 
F 12208107
Q.18. After an
Ozonolysis experiment, the only product obtained was acetaldehyde, CH3CHO.
Can you guess the structural formula of this compound? 12208108
Q.19. (a) The addition of Sulphuric acid to an
alkene obeys Markownikov’s Rule,predict the structures of the alcohols obtained
by the addition of the acid to the following compounds. 12208109
(i) Propene (ii) 1 – Butene (iii) 2- Butene
(b) Predict
the most likely product of the addition of HCl to 2 – Methyl – 2 – butene.
Explain the formation of this product. 12208110
Q.20. Why are some
hydrocarbons called saturated and other unsaturated? What type of reactions are
characteristics of them? 12208111
Q. 21. (a) Describe
methods for the preparation of Ethyne. 12208112
(b) How does
ethyne reacts with 12208113
(i) Hydrogen 12208114
(ii) Halogen acid 12208115
(iii) Alkaline KMnO4 12208116
(iv) 10%
H2SO4 in the presence of HgSO4 12208117
(v) Ammonical cuprous chloride 12208118
(c) Mention
some important uses of methane, ethene and ethyne. 12208119
Q.22. Describe how you
could distinguish ethane, ethene and ethyne from one another by means of
chemical reactions. 12208120
Q.23. (a) How will you synthesize the following
compounds starting from ethyne? 12208121
(b) Write a note on the
acidity of ethyne. 12208122
Q.24. (a) Compare the reactivity of ethane,
ethene and ethyne. 12208123
(b) Compare
the physical properties of alkanes, alkenes and alkynes. 12208124
4. Q.25. How does propyne react with the following reagents? 12208125
(a) AgNO3/NH4OH
12208126 (b) Cu2Cl2/NH4OH 12208127
(c) H2O/H2SO4,
HgSO4 12208128
Q.26. A
compound has a molecular formula C4H6 when it is treated
with excess hydrogen in the presence of Ni-catalyst, a new compound C4H10
is formed. When C4H6 is treated with ammonical silver
nitrate solution a white precipitate is formed. What is the structural formula
of the given compound? 12208129
5. Q.27. (a) Identify A and B 12208130
CH3 – CH2 – CH2
– OH A B
(b)
Give the general mechanism of electrophilic addition reactions of
alkenes. 12208131
UNIT 9
Aromatic
Hydrocarbons
Q1: What are aromatic hydrocarbons? Discuss
their classification in detail. 12209001
i.
Q2: Discuss Nomenclature of Aromatic hydrocarbons. 12209002
Q3: (a) When and how Benzene was discovered?
Discuss why straight chain structures of Benzene were ruled out. 12209003
(b) Discuss
structure of Benzene proposed by Kekule. 12209004
(c) What were the objections to Kekule’s
formula of structure of benzene?
12209005
Q4: (a) Describe the structure of benzene on the
basis of: 12209006
i)
Atomic orbital
treatment 12209007
ii)
The
resonance method 12209008
(b) Discuss the stability of Benzene by
Resonance method. 12209009
Q5: Discuss different methods of
preparation of benzene in detail. 12209010
Q6. (a) Discuss
general pattern of reactivity of Benzene towards electrophiles.
12209011
(b) Write a note on halogenations, sulphonation
and Nitration of Benzene with their
mechanism. 12209012
6.
Q7. (a)
What are Friedel-crafts reactions? Explain Friedel-crafts alkylation and
acylation reactions with examples. Also give their mechanism. 12209013
7.
(b)
Discuss the reactions of benzene in which benzene ring is involved. 12209014
8.
Q8: (a) What
is meant by “orientation is Electrophilic substitution reactions? 12209015
9.
(b) What
are ortho, para and meta-directing groups? 12209016
10.
Q9: How will you compare the reactivities of
Alkanes, Alkenes and Benzene? 122090017
EXERCISE
Q. 1. Fill in the Blanks.
1. The
term aromatic was derived from Greek word ________ meaning ________. 12209018
2. Aromatic
hydrocarbons include benzene and all those compounds which are ________ related
to benzene. 12209019
3. _____
is recognized as the simplest member of the class of Aromatic Hydrocarbons. 09(001)
4. Benzene
has ________ structure. 12209020
5. The
removal of hydrogen atom from benzene molecules gives a radical. The radicals
of aromatic hydrocarbons are called ________. 12209021
6. Benzene
was discovered by Michael Faraday in __________. 12209022
7. The
unhybridized 2pz orbitals in benzene partially overlap to form a
____________ of electron cloud. 12209023
8. The
introduction of halogen group in benzene ring is called ________. 12209024
9. The
molecular formula of C6H6 indicates that it is highly
__________ compound. 12209025
10. On
oxidation in the presence of V2O5 benzene gives ________. 12209026
Q. 2. Indicate True/False:
1. Benzene
is more reactive than alkene and less reactive than alkane. 12209027
2. Benzene
has a pentagonal structure. 12209028
3. The
C-C bond length in benzene molecule is 1.397 
. 12209029
4. The
site of hybridization of carbon in benzene molecule is sp3. 12209030
5. There
are six sigma bonds in benzene molecule. 12209031
6. Halogenonium
ion produced in electrophilic substitution reactions is a powerful
electrophile. 12209032
7. In
electrophilic substitution reactions, addition products are favourable. 12209033
8. Sulphonation
is carried out when benzene is heated with conc. HNO3. 12209034
9. In
ozonolysis benzene directly gives glyoxal. 12209035
10. Benzene
has five resonance contributing structures. 12209036
Q3. Multiple – Choice questions: 12209037
Q. 4. What
are aromatic hydrocarbons? How are they classified? 12209038
11. Q. 5. What
happens when
(a) Benzene
is heated with Conc. H2SO4 at 250°C 12209039
(b) Chlorine is passed through benzene in
sunlight. 12209040
(c) A mixture of benzene vapours and air are
passed over heated vanadium pentoxide. 12209041
(d) Benzene is burnt in free supply of air. 12209042
12.
Q. 6. What is meant by the terms: 12209043
(i) Aromatic (ii) Oxidation
(iii) Sulphonation (iv) Nitration
(v) Halogenation
Q. 7. (a) Draw the structural formulas for the following
compounds 12209044
(i) m-chlorobenzoic
acid
(ii) p-Hydroxybenzoic
acid
(iii) o-Bromonitrobenzene
(iv) o-Ethyl
toluene
(v) p-Nitroaniline
(vi) 2,4,6-Trinitrotoluene
(vii) m–Nitrophenol
(viii) p-Dibenzylbenzene
(ix) 2-Amino-5-bromo-3-nitrobenzene
sulphonic acid
(b) Give
names and the possible isomeric structures of the following: 12209045
(i) Xylenes (ii) Trimethyl benzene (iii) Bromonitrotoluene
Q. 8. Write IUPAC names of the following
molecules. 12209046
Q. 9. Give general mechanism of the electrophilic aromatic
substitution reactions. 12209047
Q.10. (a) Describe the structure of benzene on the
basis of following: 12209048
(i) Atomic orbital treatment
(ii) Resonance method.
(b) Prove that benzene has a cyclic
structure. 12209049
Q. 11. Predict the major products of bromination of the following
compounds. 12209050
(a) Toluene (b) Nitrobenzene
(c) Bromobenzene (d) Benzoic Acid
(e) Benzaldehyde (f) Phenol
Q.12 How will you prepare the following compounds from benzene
in two steps. 12209057
(a) m-chloronitrobenzene. (b) p-chloronitrobenzene.
Q.13 Complete the following reactions. Also mention the
conditions needed to carry out these reactions. 12209058
Q.14. Detail out three reactions in which benzene behaves as if
it is saturated hydrocarbon and three reactions in which it behaves as if it is
unsaturated. 12209059
Q.15. What are Friedel Crafts reactions? Give mechanism with
example of the following reactions; 12209060
(i) Friedel Crafts alkylation reactions 12209061
(ii) Friedel Crafts acylation reactions 12209062
UNIT 10
Alkyl Halides
Q1. (a) What
are alkyl halides? How are they classified? 12210001
(b) Discuss
nomenclature of Alkyl halides. 12210002
1. Q2: Discuss
different methods of preparation of Alkyl halides. 12210003
2. Q3: (a) What factors affect the reactivity
of alkyl halides? 12210004
(b) Discuss
Nucleophlilic Substitution reactions of alkyl halides. 12210005
Q4: What are b-Elimination reactions? Discuss with the help of
examples.
12210006
Q5. Discuss some
reactions of Alkyl halides which have synthetic importance. 12210007
Q6: What are Grignard Reagents? How are they
prepared? Discuss their reactivity.
12210008
Q7: Give synthetic applications of Grignard’s
reagents. 12210009
EXERCISE
Q. 1. Fill in the blanks:
(i) In tertiary alkyl halides the halogen
atom is attached to a carbon which is further attached to __________ carbon
atoms directly. 12210010
(ii) The best method for the preparation of
alkyl halides is the reaction of __________ with inorganic reagents. 12210011
(iii) An alkyl group with a partial positive
charge on the carbon atom is called __________ centre. 12210012
(iv) The mechanism is called __________ if it
involves one molecule in the rate determining step. 12210013
(v) Molecularity of a reaction is defined as
the number of molecules taking part in the __________. 12210014
(vi) The molecularity of E2 reactions is always
two and the reactions show __________ order kinetics. 12210015
(vii) Wurtz synthesis is useful for the
preparation of __________ alkanes. 12210016
(viii) Grignard reagents are prepared by the
reaction of magnesium metal with alkyl halides in the presence of __________. 12210017
Q. 2. Indicate True or False.
(i) In
secondary alkyl halides, the halogen atom is attached to a carbon which is
further attached to two carbon atoms directly.
12210018
(ii) Alcohols
react with thionyl chloride in ether as solvent to give alkyl halides. 12210019
(iii) Order
of reactivity of alkyl halides for a particular alkyl group is
Iodide>Bromide>Chloride>Fluoride.
12210020
(iv) In SN2 reactions the attacking
nucleophile always attacks from the side in which the leaving group is
attached.
12210021
(v) Methyl
magnesium iodide on hydrolysis yields ethyl alcohol. 12210022
(vi) Primary,
secondary and tertiary amines react with Grignard reagents in the same way.
12210023
(vii) The
reactions of secondary alkyl halides may follow both SN1 and SN2
mechanisms.
12210024
(viii) SN1
mechanism is a one stage process involving a simultaneous bond breakage and
bond formation. 12210025
(ix) In
b-elimination
reactions the two atoms or groups attached to two adjacent carbon atoms are
lost under the influence of an electrophile. 12210026
(x) The
reactivity order of alkyl halides is determined by the strength of
carbon-halogen bond. 12210027
Q3. Multiple-choice
questions.
Q.4 Define alkyl halides. Which is the best method of preparation of
alkyl halides? 12210028
Q. 5. Write down a method for the preparation of ethyl magnesium bromide in the laboratory.
Q. 6. Give IUPAC names of the following compounds.
Q. 7. Draw all
the possible structures that have the molecular formula C6H13Cl.
Classify each as primary, secondary or tertiary chloride. Give their names
according to IUPAC system. 12210031
Q.8 Using ethyl bromide as a starting material how would you prepare
following compounds. Give also the reagent and conditions necessary for these
reactions. 12210032
(a) n-Butane 12210033 (b) Ethyl
Alcohol 12210034
(c) Ethyl cyanide 12210035 (d) Ethane 12210036
(e) Ethene 12210037 (f) Propanoic
acid 12210038
(g) Propane 12210039 (h) Ethyl
amine 12210040
Q. 9. Write a detailed note on the mechanism of nucleophilic substitution reactions.
Q.10. What do you know by the term “b-elimination reaction.” Explain briefly the two
possible mechanisms of b-elimination reactions. 12210042
Q.11. What products are formed when following compounds are reacted with ethyl bromide followed by hydrolysis in the presence of.
(i) HCHO (ii) CH3 – CHO
(iii) CO2 (iv) (CH3)2 CO
(v) (vi) Cl.CN
Q.12. How will you carry out the following conversions?
UNIT 11
Alcohols, Phenols
& Ethers
Q1: Define alcohol. Give the classification of alcohols. 12211001
Q.2 Explain the nomenclature
of alcohols. 12211002
Q. 3. What is wood spirit? How CH3OH is prepared on
commercial scale?
12211003
Q.4 (a) Give the preparation of ethyl alcohol by
fermentation process. 12211004
(b) What is meant by denaturation
of alcohol? 12211005
(c) Discuss the physical properties of alcohols. 12211006
Q.5 Give the following
chemical reactions of alcohols.
(i) In which C - O bond is
broken 12211007
(ii) In which O - H bond is
broken 12211008
(a) With Oxidizing agents
(b) With Dehydrating agents
(c) With Halogenating agents
2.
Q.6 Give the difference between
(i) Primary,Secondaryand TertiaryAlcohols 12211009
(ii) CH3 OH and C2H5OH 12211010
Q. 7. Write down uses of
methanol and ethanol. 12211011
Q. 8. What is phenol? Explain with examples the nomenclature of
phenols. 12211012
Q.9 Give various methods of preparation of phenol
and write its physical properties. 12211013
Q. 10. Phenol is acidic while an alcohol is not.
Explain on the basis of their structures. 12211014
Q.11. (a) What are the
different chemical reactions of phenol. Explain with examples.
(b) Give uses of Phenol. 12211016
Q.12 Define ether. Give the classification and nomenclature of ethers. 12211017
Q.13 Give three methods of ether preparation. Write physical and
chemical properties of diethylether. 12211018
EXERCISE
Q.1 Fill in the blanks.
(i) Primary,
Secondary and Tertiary alcohols can be identified by ______test. 12211019
(ii) Oxidation
of __________ alcohols give ketones. 12211020
(iii) Alcohols
on heating with __________ give alkenes at high temperature. 12211021
(iv) Alcohols
have __________ boiling points than ethers due to stronger hydrogen bonding. 12211022
(v) Williamsons
synthesis is used to prepare __________. 12211023
(vi) __________is
also called wood spirit. 12211024
(vii) Carbolic
acid is the other name of __________. 12211025
(viii) Primary,
secondary and tertiary alcohols can be prepared by reacting Grignard’s reagent with______. 12211026
(ix) Alcohols
and __________ react to produce ester. 12211027
(x) __________
is used as anti-freezing agent in automobile radiator. 12211028
(xi) The
conversion of starch into alcohol with the help of micro-organisms is called __________. 12211029
(xii) Ketones
on reduction give __________ alcohols. 12211030
Q. 2. Write True or False.
(i) Methylated spirit contains 95% methyl
alcohol and 5% ethyl alcohol. 12211031
(ii) Ethyl alcohol is a very good
anti-freezing agent. 12211032
(iii) Methanol is also called wood spirit. 12211033
(iv) Only 14% ethyl alcohol can be prepared by
fermentation. 12211034
(v) Ethers do not show hydrogen bonding. 12211035
(vi) Alcohols are more acidic than phenols. 12211036
(vii) Phenol is more soluble in water than lower
alcohols. 12211037
(viii) Alcohols are more basic than ethers. 12211038
(ix) Ethers have higher boiling points than
alcohols and phenols. 12211039
(x) Methanol and Ethanol can be identified
by iodoform test. 12211040
Note: Methyl alcohol and ethylene
glycol are very good anti-freezing agents. Ethyl alcohol is also an
anti-freezing agent but not very good anti-freezing agent.
Q.3 Multiple Choice Questions:
SHORT QUESTIONS
Q.4 What are alcohols? How are they classified? How will you
distinguish between primary, secondary and tertiary alcohols? 12211041
Q.5 How is methyl alcohol obtained on large scale? How it may be
distinguished from ethyl alcohol? 12211042
Q.6 What is fermentation? What compounds may be obtained on
industrial scale by fermentation? 12211043
Q.7 Explain the following terms: 12211044
Absolute alcohol, methylated spirit, rectified spirit,
denaturing of alcohol.
Q.8 How does ethyl alcohol reacts with:
(i) Conc. H2SO4 12211045 (ii) Na 12211046
(iii) PCl5 12211047 (iv) CH3COOH 12211048
(v) SOCl2 12211049
Q.9 How will you obtain primary, secondary and tertiary alcohols by
reacting Grignard reagent with suitable carbonyl compounds? 12211050
Q.10 How will you distinguish between:
1. An
alcohol and a phenol 12211051
2. An
Alcohol and an ether 12211052
3. Methanol
and ethanol 12211053
4. A tertiary
alcohol and a primary alcohol 12211054
5. 1-Propanol
and 2-Propanol 12211055
Q.11 Give reasons for the following:
(i) Ethyl
Alcohol is a liquid while ethyl chloride is a gas. 12211056
(ii) Ethanol has
higher boiling point than diethyl ether. 12211057
(iii) Absolute
alcohol can not be prepared by fermentation process. 12211058
(v) Water has
higher boiling point than ethanol. 12211060
Q.12 How will you convert:
(i) Methanol
into Ethanol. 12211061
(ii) Ethanol
into methanol 12211062
CH3¾ CH2OH
¾¾® CH3¾ OH
(iii) Ethanol
into isopropyl alcohol 12211063
CH3¾ CH2OH ¾¾® CH3¾
¾CH3
(iv) Formaldehyde
into ethyl alcohol
HCHO ¾® CH3¾ CH2OH 12211064
(v) Acetone into Ethyl alcohol 12211065
Q.13 Explain the following using ethyl alcohol as an example.
(i) Oxidation 12211066 (ii) Dehydration 12211067
(iii) Esterification 12211068 (iv) Ether formation 12211069
Q14. Compare the reactions of phenol with those of ethanol. Discuss the
difference if any:
12211070
Q.15 Arrange the following compounds in order of their increasing
acidic strength and give reasons. 12211071
H2O,
C2H5OH, C6H5OH, C6H5COOH
Q.16 Write down two methods for preparing phenol. What is the action
of following on phenol? 12211072
HNO3, NaOH, Zn, Bromine Water.
Q.17 Give uses of phenols. How
bakelite is prepared from it? 12211073
Q.18 (a) Write
IUPAC names of the following compounds: 12211074
(b) Write down
structural formula for the following compounds: 12211075
Q.19 (a) Name the following compounds: 12211076
(b) Write down
structural formulas for the following compounds: 12211077
UNIT 12
Aldehydes And Ketones
Q1: Give one laboratory and one industrial method for the preparation of formaldehyde.
Q4: Explain with mechanism the addition of sodium bisulphite to acetone. 12212004
Q8: (a) Give
general mechanism of acid-catalysed addition reactions. 12212008
(b) Discuss
acid-catalysed addition reactions of carbonyl compounds in detail.
(b) What
is the product of reaction of carbonyl compounds with alcohols? 12212011
Q10. (a) Discuss
oxidation reactions of carbonyl compounds. 12212012
(b) How
can we identify different carbonyl compounds by chemical tests? 12212013
(c) Give
uses of formaldehyde and acetaldehyde. 12212014
EXERCISE
Q. 1. Fill in the Blanks.
1. Aldehydes are the
first oxidation product of ________. 12212015
2. Ketones are the
first oxidation product of ________ . 12212016
3. Aldehydes and
ketones undergo ________ addition reactions. 12212017
4. Formaldehyde reacts
with ________ to give primary alcohol. 12212018
5. Acetaldehyde reacts
with ________ to give 2-butanol. 12212019
6. Aldehydes are
strong ________ agents. 12212020
7. The oxidation of an
________ always gives a carboxylic acid. 12212021
8. The reduction of a
________ always gives a secondary alcohol. 12212022
9. Formaldehyde gives
________ test with Tollen’s reagent. 12212023
10. Acetaldehyde gives a
________ precipitate with Fehling’s solution. 12212024
Q. 2. Indicate True/False:
1. Formaldehyde is
used in the silvering of mirrors. 12212025
2. Ketones combine
with alcohols in the presence of HCl gas to form acetals. 12212026
3. Acetaldehyde
undergoes cannizzaro’s reaction. 12212027
4. Formaldehyde is
used to prepare urotropin. 12212028
5. Aldol condensation
reaction is given by only those aldehydes and ketones which contain α-hydrogen atom. 12212029
7. Propanal and
propanone behave differently with Tollen’s reagent. 12212031
8. Acetone reacts with
sodium bisulphite to give a yellow crystalline product. 12212032
9. Acetone on
reduction gives a primary alcohol. 12212033
10. 40% aqueous solution
of formaldehyde is called formalin. 12212034
Q. 3. Multiple-choice
questions. 12212035
Q. 4. Give
one laboratory and one industrial method for the preparation of formaldehyde.
Q. 5. How does formaldehyde
react with the following reagents?
(i) CH3MgI 12212037 (ii) HCN 12212038
(iii) NaHSO3 12212039 (iv) conc. NaOH 12212040
(v) NaBH4/H2O 12212041 (vi) Tollen’s reagent 12212042
(vii) Fehling’s reagent 12212043
Q. 6. Give one laboratory and
one industrial method for the preparation of acetaldehyde.
Q. 7. How does acetaldehyde
react with the following reagents?
(i) C2H5MgI 12212045 (ii) HCN 12212046
(iii) NaHSO3 12212047 (iv) dilute NaOH 12212048
(v) I2/NaOH 12212049 (vi) NaBH4/H2O 12212050
(vii) NH2OH 12212051 (viii) K2Cr2O7/H2SO4 12212052
Q. 8. Describe briefly the
mechanism of nucleophilic addition to a carbonyl compound.
Q. 9. Explain with mechanism
the addition of ethylmagnesium bromide with acetaldehyde. What is the
importance of this reaction? 12212054
Q. 10. Explain with mechanism the
addition of sodium bisulphite to acetone. What is the utility of this reaction? 12212055
Q. 11. Describe with mechanism
aldol condensation reaction. Why formaldehyde does not give this reaction? 12212056
Q. 12. What types of aldehydes
give Cannizzaro’s reaction? Give its mechanism.
Q. 13. Explain the mechanism of
the reaction between phenylhydrazine and acetone. 12212058
Q. 14. Using ethyne as a starting
material how would you get acetaldehyde, acetone and ethyl alcohol? 12212059
(iii) Ethyl alcohol from acetylene: 12212060
Q. 15. Give the mechanism of
addition of HCN to acetone. 12212061
Q. 16. How would you bring about
the following conversions?
(i) Acetone into t-Butyl alcohol 12212062 (ii) Propanal into 1-propanol 12212063
(iii) Propanone into 2-propanol 12212064 (iv) Methanal into ethanal 12212065
(v) Ethanal into propanone 12212066 (vi) Ethanal into 2-propanol 12212067
(vii) Ethyne into ethanal 12212068 (viii) Ethene into ethanal 12212069
(ix) Ethanal into ethanol 12212070 (x) Ethanal into 2-Butanone 12212071
(xi) Methanol into ethanal 12212072 (xii) Ethanol into ethanoic acid 12212073
Q. 17. How will you distinguish
between.
(i) Methanal and ethanal 12212074
(ii) Ethanal and propanone 12212075
(iii) Ethanal and propanal 12212076
(iv) Acetone and ethyl alcohol 12212077
(v) Butanone and 3-pentanone 12212078
(vi) Acetaldehyde and Benzaldehyde 12212079
(vii) 2-Pentanone and 3-pentanone 12212080
Q. 18. Discuss oxidation of (a)
aldehydes (b) ketones with:
(i) K2Cr2O7/H2SO4 12212081 (ii) Tollen’s reagent 12212082
(iii) Fehling’s
solution 12212083
Q. 19. Discuss reduction of (a)
aldehydes (b) ketones with 12212084
(i) NaBH4/H2O (ii) H2/Pd
Q. 20. Give three uses for each
of formaldehyde and acetaldehyde. 12212085
UNIT 13
Carboxylic Acids
Q1. (a) What are Carboxylic
acids? 12213001
(b) Discuss Nomenclature
of Carboxylic acids. 12213002
Q2. Give different methods of preparation of
Carboxylic acids. 12213003
Q3: (a) Give physical properties of Carboxylic
acids. 12213004
(b) Discuss different reactions of Carboxylic acids in detail. 12213005
Q4. Discuss methods of
preparation of acetic acid. 12213006
Q5: Describe physical
properties and uses of acetic acid. 12213007
Q6: Write a detailed note
on the structure and classification of “Amino Acids”. 12213008
Q7: (a) Discuss chemical properties of amino
acids. 12213009
(b) What is the test for the identification of an “Amino acid”? 12213010
(c) What is the difference between peptides and proteins? 12213011
EXERCISE
Q. 1. Fill in the Blanks.
1. Formula of malonic acid is _______. 12213012
2. Methyl nitrile upon acidic hydrolysis
produces ______. 12213013
3. Melting points of carboxylic acids
containing even number of carbon atoms are ____than the next lower and higher
members containing odd number of carbon atoms. 12213014
4. Acetic acid on heating with _______ produces
acetic anhydride. 12213015
5. Acid chloride and acid anhydride are called
_______ of acid. 12213016
6. Pure acetic acid is called _______. 12213017
7. Formula of alanine is ________. 12213018
8. Proline is a _________amino acid. 12213019
9. A peptide having a molecular mass
more than 10000 is called _______. 12213020
Q. 2. Indicate True/False:
1. Acetic acid exists as dimer in benzene. 12213021
2. First three aliphatic acids have fruity
smell. 12213022
3. Carboxylic acids on reduction with LiAlH4
produce alkenes. 12213023
4. Acetic acid on dehydration produces CO and H2. 12213024
5. Sodium
formate on heating with soda lime produces NaHCO3 and hydrogen. 12213025
6. Amino acids exist as Zwitter ion. 12213026
7. Histidine is an acidic amino acid. 12213027
8. A peptide having molecular mass upto 10000 is
called protein. 12213028
9. Phthalic acid is a monocarboxylic acid. 12213029
10. Formula of Glycine is CH2COOH. 12213030
Q. 3. Multiple Choice
Questions. 12213031
Q.4. Write
down the structural formula of the followings: 12213032
(i) Valeric acid 12213033 (ii) Propionic
acid 12213034
(iii) Oxalic acid 12213035 (iv) Benzoic acid 12213036
(v) Acetic anhydride 12213037 (vi) Acetyl chloride 12213038
Q.5. Write down the names of
the following compounds by IUPAC system. 12213039
Q.6. (a) How is acetic acid manufactured? What is
glacial acetic acid? 12213040
(b) How would you convert acetic acid into: 12213041
(i) Methane 12213042 (ii) acetyl chloride 12213043
(iii) Acetamide 12213044 (iv) Acetic anhydride 12213045
Q. 7. (a) What are fatty acids? 12213046
(b) What is vinegar? Describe how is vinegar prepared from ethanol. 12213047
Q. 8. How
would you convert the following: 12213048
(i) Acetic acid into acetamide 12213049
(ii) Acetic acid into acetone 12213050
Q.9. Write
down the mechanism of the following reactions: 12213051
(i) between acetic acid and ethanol 12213052
(ii) between
acetic acid and ammonia 12213053
(iii) between acetic acid and thionyl chloride 12213054
Q. 11. What
happens when following compounds are heated: 12213055
(i) calcium acetate 12213056 (ii) sodium formate and soda lime 12213057
(iii) ammonium acetate 12213058
Q.11. What are amino acids?
Explain their different types with one example in each case.
12213059
Q. 12. Write
a short note on acidic and basic character of an amino acid. 12213060
Q. 13. What
is peptide bond? Write down the formula of a dipeptide? 12213061
Q. 14. What
are zwitter ions? 12213062
Q. 15. What
are amino acids, proteins and peptides? How are they related? 12213063
Q.16. Study the facts given in
(a), (b) and (c) below and then answer questions which follow: 12213064
(a) A is an organic
compound made up of C, H, and O. It has a vapor density 15. (Hint Molecular
mass = 2 ´ vapour density]. 12213065
(b) On reduction A gives a
compound ‘X' which has the following properties: 12213066
(i) X is a colourless liquid miscible with
water.
(ii) X is neutral to litmus
(iii) When X is warmed with a few drops of
conc. H2SO4 followed by a little salicylic acid a
characteristic smell is produced.
(c) When X is subjected to
strong oxidation, it gives compound B, which has the following properties. 12213067
i) B is a pungent smelling mobile liquid.
ii) It is miscible with water, alcohol or
ether.
iii) It is corrosive and produces blisters on
contact with skin.
iv) B can be obtained by passing the vapours
of A with air over platinum black catalyst.
v) B liberates H2 with sodium.
vi) It gives CO2 with NaHCO3.
1) What is the molecular weight of A?
2) Identify A, X and B.
3) Give five appropriate reactions to
confirm the identities of A, X or B.
4) State one large-scale use of either A,
X or B.
UNIT 14
Macromolecules
Q.1(a) What
are macromolecules? 12214001
(b) Define polymer. Discuss the general
structure of polymers. 12214002
(c)
What is meant by degree of polymerization? 12214003
(d)
Discuss the different types of polymers on the basis of type of
monomers. 12214004
Q2. (a)
Classify polymers on the basis of their thermal properties. 12214005
(b) Discuss the types of
polymerization process on the basis of the way of polymer formation. 12214006
Q.3. Write a note on different types of synthetic
polymers. 12214007
Q4.(a) What
are biopolymers? 12214008
(b)
What are carbohydrates? Give their classification. 12214009
Q.5(a) Define proteins. Discuss their classification
in detail. 12214010
(b) Discuss the structures of different types of proteins. 12214011
(c) What is meant by denaturation of proteins? 12214012
(d) Give importance of proteins.
12214013
Q.6.(a)
What are lipids? Describe different sources of lipids. 12214014
(b)
Discuss general structure and composition of fats and oils. 12214015
(c)
Discuss classification of lipids. 12214016
(d)
Discuss physical and chemical properties of lipids in detail. 12214017
Q7: In what way fats and oils are different? 12214018
Q.9. Discuss some basic terms
related to lipids. 12214019
Q.8.(a) What are steroids?
Discuss different compounds belonging to steroids. 12214020
(b) Discuss the importance
of lipids. 12214021
Q.9 What are
enzymes? Discuss their properties and classification in detail? 12214022
Q.10(a) Describe the factors affecting enzyme activity. 12214023
(b) Discuss the importance of enzymes. 12214024
Q.11. Write a
note on nucleic acids. 12214025
EXERCISE
Q.1. Fill in the blanks.
1. Macromolecules are built up from small units called
_________. 12214026
2. Nylon is polyamide and terylene is a _____________. 12214027
3. Nylon is prepared by the reaction of ___________ and
hexamethylenediamine. 12214028
4. Based on their thermal properties, plastics are divided into
_______ main classes. 12214029
5. Polyvinyl chloride is a __________ plastic. 12214030
6. Glucose is stored as _____ in the liver. 12214031
7. Glucose and fructose are water _________ carbohydrates. 12214032
8. Protein after digestion changes to ___________. 12214033
9. Purines and pyrimidines are ___________ of nucleic acids. 12214034
10. Addition of a plasticizer ____________ the flexibility of the
polymer. 12214035
Q.2. Indicate True or False.
1. Nylon 6,6 and terylene are condensation polymers. 12214036
2. The disposal of plastics does not cause any pollution
problem. 12214037
3. Fructose is a polysaccharide carbohydrate. 12214038
4. Human beings get no food nutrient from cellulose. 12214039
5. The most abundant and the most important steroid in the
human body is Vitamin-D. 12214040
6. Enzymes are the compounds containing C,H and O only. 12214041
7. The degree of unsaturation of fats is measured by their
iodine number. 12214042
8. Activity of an enzyme varies with temperature and pH. 12214043
9. Nucleic acids are biological catalysts. 12214044
10. The nucleic acids are responsible for protein synthesis in the
human body. 12214045
Q.3. Multiple choice questions. Encircle the
correct answer.
Q.4. Explain the following terms: 12214046
(a) Addition polymer 12214047
(b) Condensation polymer 12214048
(c) Thermoplastic 12214049
(d) Thermosetting plastic. 12214050
Q.5. Write notes on:
(a) Polyester resins 12214051 (b) Polyamide resins 12214052 (c) Epoxy resins 12214053
Q.6. What is the repeating unit in each of
the following polymers? 12214054
(a) Polystyrene:
(b) Nylon 6,6:
(c) Teflon:
(d) Orlon:
Q.7. What are carbohydrates and how are they
classified? 12214055
Q.8. Point out one difference between the
compounds in each of the following pairs: 12214056
(a) Glucose and
Fructose. 12214057
(b) Sucrose and
Maltose. 12214058
(c) Cellulose and
starch. 12214059
Q.9. What are lipids? In what way fats and
oils are different? 12214060
Q.10. Define saponification number and
iodine number. Discuss the term rancidity.
12214061
Q.11.
What is the difference between a glycosidic linkage and a peptide
linkage? 12214062
Q.12.
What is the chemical nature of enzymes? Discuss the classification of
enzymes. 12214063
Q.13.
What are nucleic acids? Write down the role of DNA and RNA in life.
UNIT 15
Common
Chemical Industries
In Pakistan
Q1. What are fertilizers? Discuss their importance. 12215001
Q2a. Define micronutrients and macronutrients. In
which quantity are they required by the plants? 12215002
b. What are the essential qualities of a
good fertilizer? 12215003
c. How fertilizers are classified? 12215004
Q3. What are nitrogenous fertilizers? Discuss different
nitrogenous fertilizers and their importance
for plants. 12215005
Q4a. What is the importance
of phosphatic fertilizers for plants? 12215006
b. Discuss different
types of phosphatic fertilizers and their importance. 12215007
Q5a. Why is potassium required by the plants? 12215008
b. Write a note on potassium nitrate as a fertilizer. 12215009
c. What is the scope of fertilizer industry in Pakistan? 12215010
6a. What is Portland cement? Who
introduced it? 12215011
b. Define cement. Discuss
essential constituents and composition of cement. 12215012
c. What type of processes are
employed for cement manufacture? Write a note on wet process for the manufacturing of cement. 12215013
Q.7.(a) What is meant by the term “setting of cement”? Discuss the
reactions taking place
during this process. 12215014
(b) Discuss the scope of cement industry in
Pakistan. 12215015
Q.8(a) Briefly describe the historical background of paper industry. 12215016
(b) Define paper. Discuss
different raw materials used in the manufacture of paper.
12215017
Q.9(a) What are the principle methods of chemical pulping? 12215018
(b) Write a note on
neutral sulphite semi-chemical process for the manufacture of paper
with the help of flow sheet
diagram. 12215019
EXERCISE
Q. 1. Fill in the blanks
with suitable words.
1. Fertilizers enhance the natural ________ of
the soil. 12215020
2. Micro-nutrients are required in quantity
ranging from ________ per acre. 12215021
3. Ammonia contains ________ nitrogen. 12215022
4. Manure is an ________ material used to
fertilize land. 12215023
5. Cement was first introduced by an English
Mason ________. 12215024
6. Phosphorus is required to stimulate
__________ of plant. 12215025
7. In Pakistan, bleaching of pulp is
carried out with _________. 12215026
8. Cement is generally manufactured using
________ process. 12215027
9. The use of cement in the
construction of building is based on its property of ________ when its paste
with water is allowed to stand for sometime. 12215028
10. Lignin is an _______ polymer and causes paper
to become brittle. 12215029
Q. 2. Indicate True/False:
1. Potassium fertilizers are especially
used for tobacco and corn. 12215030
2. Ammonia is used in gaseous state
while all other fertilizers are used in solid form. 12215030
3. In wet process for the manufacture
of cement, grinding of raw material is done in the presence of water. 12215031
4. The total production of cement in
Pakistan is 56,30,100 metric tons /annum. 12215032
5. In neutral sulphite semi-chemical
process, sodium sulphite is used buffered with sodium carbonate. 12215032
6. Lignin is an inorganic binder. 12215033
7. Paper consumption in Pakistan is
around 5 kg per person per year. 12215034
8. Urea contains 90% nitrogen. 12215035
9. The temperature of the digester in
paper industry should be around 160 - 180°C. 12215036
10. Potassium fertilizers increase the capability
of plants to resist diseases. 12215037
Q. 3. Multiple Choice
Questions.
Q. 4. What
are phosphatic fertilizers? How are they prepared? Mention the role of
phosphorus in the growth of plants. 12215038
Q. 5.(a) What
are fertilizers? Why are they needed? 12215039
(b) Discuss the classification of fertilizers and
their uses. 12215040
(c) How is urea manufactured in Pakistan? Describe
in detail the process used.
Q. 6.(a) What
are the prospects of fertilizer industry in Pakistan? 12215042
(b)
What are essential nutrient elements and
why these are needed for plant growth?
(c) Write down the essential
qualities of a good fertilizer? 12215044
Q.7.(a) Describe
the composition of a good portland cement. 12215045
(b) Discuss the wet process for the manufacturing
of cement with the help of flow sheet diagram. 12215046
(c) What do you understand by the term “setting
of cement”. Also discuss the reactions taking place in first 24 hours? 12215047
Q.8. What
are the essential non-woody raw materials used in the production of pulp and
paper in Pakistan? 12215048
Q.9.(a) What
are the principal methods of chemical pulping used for the production of paper?
(b) Describe the neutral sulphite semi-chemical
process for the manufacturing of pulp and paper. 12215050
Q.10.(a)What are the common bleaching agents used
in paper industry in Pakistan? Briefly describe the bleaching process. 12215051
(b) What are the prospects of paper
industry in Pakistan? 12215052
UNIT 16
Environmental
Chemistry
Q.1.(a) Define environmental chemistry. 12216001
(b) What are the different
components of environment? 12216002
OR
Name the components of
environment.
Give composition of these
components.
Q.2.(a) What are environmental pollutants? What is their effect on
environment? 12216003
(b) Write a detailed note
on sources of air pollution. 12216004
Q.3. What is acid rain? How does it form? What are
its harmful effects on our environment?
12216005
Q.4. Define smog. Discuss its
types and properties. 12216006
Q.5(a) Write a
note on ozone layer and atmosphere. 12216007
(b) What is the role of
chlorofluorocarbons in destroying ozone layer? 12216008
Q.6. What is water
pollution? Discuss its different sources in detail. 12216009
Q.7(a) What
factors affect the quality of water? 12216010
(b) Discuss different methods of
purification of water in detail. 12216011
Q.8(a) What is
solid waste management? 12216012
(b) Discuss different types of solid
wastes and the methods to get rid of them. 12216013
Q9. (a) Explain the process of incineration of industrial waste. 12216014
(b) How can the waste materials be recycled? 12216015
EXERCISE
Q. 1. Fill in the Blanks.
1. Only ________ of the total earth’s water resources are available
as fresh water. 12216016
2. ________ is a smaller unit of biosphere which consists of
community of organisms and their interaction with environment. 12216017
3. Carbon monoxide is highly poisonous gas and causes
suffocation if inhaled, it binds blood ____ more strongly than oxygen thus
excluding oxygen from normal respiration.
12216018
4. The elevated concentration of ________ is harmful for
fish as it clogs the gills thus causing suffocation. 12216019
5. The ozone layer in the ________ surrounds the globe and
filters most of the harmful UV rays in the sunlight before they could reach the
earth. 12216020
6. The presence of ________ in the livestock waste can
contaminate surface and ground water causing various infectious diseases. 12216021
7. The substances which can directly kill the unwanted
organisms are called_____. 12216022
8. ________ is frequently used to disinfect water. 12216023
9. Incineration is not a clean process because it produces
air pollution and toxic_____.
12216024
10. A process in which some of the used or waste materials are not
discarded after their initial use but are processed so that it can be used
again is called ________. 12216025
Q. 2. Indicate True/False:
1. Half of the mass of the atmosphere
is concentrated in lower 10 km. 12216026
2. The oceans cover approximately 71
percent of the earth. 12216027
3. The volcanoes produce 55% of SO2. 12216028
4. The reducing smog is due to the
presence of nitric oxide. 12216029
5. Ozone is produced in the polar
regions by the photochemical reactions of oxygen. 12216030
6. The
temperature in the troposphere decreases with the increasing altitude from 15
to –56°C. 12216031
7. Incineration is a waste treatment
process in which solid waste is dumped in landfill. 12216032
8. Acid rain is due to the presence of
oxides of sulphur and nitrogen which get mixed with the rain water. 12216033
9. The heavy metals have a safe limit
where they are not toxic. 12216034
10. The reprocessing of the plastics is to
convert back to their components by chemical or thermal process so that these
can be used again.
12216035
Q. 3. Multiple-choice
questions. Encircle the correct answer:
Q. 4. Discuss
in detail the components of the environment. 12216036
Q. 5. Describe
the natural and human sources of carbon monoxide, nitrogen oxides and sulphur
oxides. 12216037
Q. 6. What
is acid rain and how does it affect our environment? 12216038
Q. 7. What
is smog? Explain the pollutants which are the main cause of photochemical smog. 12216039
Q. 8. Why
is ozone layer depleting (decreasing)? What will happen when the concentration
of ozone will be decreased? 12216040
Q. 9. How
is oil spillage affecting the marine life 12216041
Q. 10. How
detergents are threat to aquatic animal life? 12216042
Q. 11. Explain
how pesticides are dangerous to human beings. 12216043
Q. 12. Discuss
industrial waste effluents. 12216044
Q. 13. How
the water is purified i.e., made potable? Discuss in detail. 12216045
Q. 14. What
are leachates? (Board 2 12216046
Q. 15. Explain
the process of incineration of industrial waste. 12216047
