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Chemistry is a branch of physical science that studies the composition, structure, properties and change of matter. Chemistry is sometimes called the central science. The history of chemistry can be traced to certain practices, known as alchemy, which had been practiced for several millennia in various parts of the world.

Ali Raza Fauji Foundation Higher Secondary

School (Inter College) Talagang June 9th, 2015

Tuesday

SECOND YEAR CHEMISTRY

Objective Portion, Short Questions,

Memory Tricks, Conceptual Questions,

Experiment Based Questions, Labeled Diagrams

2015-16

ALI RAZA KAMAL

ALI RAZA KAMAL

CHAPTER 1: PERIODIC CLASSIFICATION OF ELEMENTS AND PERIODICITY

Chemistry Class: XII

(Objective) Time: 30 min Marks: 17

Scheme (9)

Weightage = 7% MCQ’s = 1 Short Questions = 2 Extensive Question = 1(Theory)

Section-I (Objective Type Questions-17)

Q: 1 Encircle the right option from the following. (6 x 1 = 6)

(i) Which of the following has greatest tendency to lose electron?

(a) F (b) Fr (c) S (d) Be

(ii) Ca2+ ion is isoelectronic with:

(a) Mg2+ (b) Na+ (c) Ar (d) Kr

(iii) Electron affinity depends on:

(a) Atomic size (b) Nuclear charge (c) Atomic number (d) Both ‘a’ and ‘b’

(iv) Which of the following possess maximum hydration power?:

(a) Na+ (b) K+ (c) Mg2+ (d) Ca2+

(v) The outer most orbital involved in chemical bonding is called:

(a) Molecular orbital (b) Complete orbital (c) Valence orbital (d) Free orbital (vi) The electron affinity of fluorine is:

(a) – 348.8 kJ/mol (b) – 337 kJ/mol (c) 337 kJ/mol (d) 348.8 kJ/mol

Q: 2 Fill in the blanks with appropriate word. (6 x 0.5 = 3)

(i) Mendeleev in his periodic table, arranged the elements according to their atomic ____________.

(ii) Metals form ____________ oxides and non-metals form ____________ oxides.

(iii) Melting and boiling points of halogens ____________ down the group.

(iv) Hydrogen can be placed above the groups ____________ of the periodic table.

(v) Members of group VII A are called and alkali metals is the family name of ____________ group

members.

(vi) Vertical columns in modern periodic table are called ____________.

Q: 3 State the following statements as true or false. (6 x 0.5 = 3)

(i) In Mendeleev's periodic table elements Be, Mg, Zn and Cd are placed in the same group.______

(ii) Metals are present in the top right comer of the periodic table. ______

(iii) Oxidation state of an element is related to the number of period it belongs. ______

(iv) Melting points of halogens decrease down the group. ______

(v) Hydrogen forms uninegative ion like halogens. ______

(vi) Metalloids are present in the lower half of Groups IV A, V A and VI A. ______

Q: 4 Pen down reason for the justification of following statements. (5 x 1 = 5)

(i) Alkali metals give ionic hydrides.

________________________________________________________________________________

(ii) d-block and f-block elements are called transition elements.

________________________________________________________________________________

(iii) Higher oxidation state of an element gives greater % covalent character.

________________________________________________________________________________

(iv) The first electron affinity of the oxygen is negative but second is positive.

________________________________________________________________________________

(v) The hydration energies of the ions are in the following order: Al3+ > Mg2+ > Na+.

________________________________________________________________________________

ALI RAZA KAMAL

ALI RAZA KAMAL

(Subjective) Time: 3:00 hours Marks: 83

Section-II (Short Questions-60)

Q: 5 Write short answers of following questions. (10 x 1 = 10)

(i) How does Mendeleev's periodic table help us to correct the atomic masses of some of the elements?

(ii) How does Moseley's periodic table help to correct the rearrangements of some elements?

(iii) Zn, Cd and Hg we're placed with alkaline earth metals in Mendeleev's periodic table, how this

confusion is removed in the modern periodic table?

(iv) d-block and f-block elements are called transition elements. Why?

(v) What are s-block elements and why are they called so?

(vi) Why the elements of group III-A to group VII-A are called p-block elements?

(vii) What is the first d-block series and what is the name of the coinage metals in it?

(viii) How lanthanide contractions control the atomic sizes of the elements of 6th and 7th periods?

(ix) Why the elements of group I-A and II-A are good metals of Periodic Table?

(x) Describe essential features of period six of periodic table.


(i) How does hydrogen resemble with alkali metals?

(ii) In what respects does hydrogen differ from the halogens?

(iii) How does hydrogen resemble with elements of group IV-A?

(iv) Why the atomic radii decrease from left to right and increase from top to bottom in the periodic table?

(v) How the shielding effect is one of the important parameters to determine the size of an atom?

(vi) Inspite of decreasing the nuclear charge down the group the atomic radii increase. Why?

(vii) Why the ionic radius of a positive ion is smaller than its neutral atom?

(viii) Why the ionic radius of a negative ion is greater than its atomic radius?

(ix) How do you justify that the size of an ion shrinks with the increasing positive charge?

(x) The ionization energy is measured by taking the atom in the isolated state. Give reasons.


(i) Why the ionization energies decrease down the groups?

(ii) Why the ionization energies increase from left to the right in a period?

(iii) Why is there a big gap in first and second ionization energies of sodium, but a big gap is overfeed in

second and third ionization energies of magnesium?

(iv) How does the nature of orbital influence the value of ionization energies of elements?

(v) Why the elements of group III-A have less ionization energy values than II-A?

(vi) Why the elements of group VI-A have less ionization energy values than V-A?

(vii) Why most of the elements release energies when electrons are added in their outermost orbitals?

(viii) Why the addition of electron in the outermost orbital can be studied by taking the element in the

isolated state?

(ix) The first electron affinity of the oxygen is negative but second is positive. Why?

(x) Why the second value of electron affinity is positive?


(i) Why the electron affinities of element of group II-A are less than those of group I-A?

(ii) Define election affinity. How electron affinity values vary in the periodic table?

(iii) Why the elements on top right of the periodic table are non-metallic in nature?

(iv) Why is the metallic character increase down the group of s-block elements?

(v) The melting and boiling point of the elements increase from left to right up to the middle of s-block

and p-block elements and decrease onwards. Why?

(vi) Why the melting and boiling points of halogens increase from top to the bottom?

(vii) The oxidation states vary in a period but almost remain constant in a group. Why?

(viii) Elements of group VI-A show variable oxidation states except oxygen. Why?

(ix) Why the oxidation states of noble gases are usually zero?

ALI RAZA KAMAL

ALI RAZA KAMAL

(x) Mostly it is observed that the elements of group VIII-A have zero oxidation numbers. Why?


(i) Why the electrical conductivities of the elements are related with the free electrons?

(ii) Why the elements of I-A, II-A and III-A have high electrical conductivities?

(iii) Why graphite is a good conductor of electricity, but diamond is not?

(iv) Why the hydration energy depend upon size of the ion?

(v) The hydration energies of the ions are in the following order. Give reasons.

Al3+ > Mg2+ > Na+.

(vi) Why the hydration energy of halide ions decrease from F- to I-?

(vii) Why the ionic halides are mostly given by the elements of group I-A and II-A?

(viii) How covalent halides differ from ionic halides? Give reasons and examples.

(ix) Why the melting points of halides decrease from left to the right in a period?

(x) Why is it true that the higher oxidation state of an element gives greater % covalent character?


(i) Alkali metals give ionic hydrides. Give examples.

(ii) Why the ionic hydrides have high melting and boiling points and conduct electricity in the molten

state?

(iii) Why the melting and boiling points of covalent hydrides of group IV-A increase from upper to the

downward direction?

(iv) What is trend of hydrides group VI-A in boiling point?

(v) How do you justify that ZnO is amphoteric in nature?

(vi) How does the nature of oxide state from basic to acidic character when one moves from left to the

eight in a period?

(vii) How does the acidic nature of oxide change with the increase of oxidation number of the central

atom?

(viii) Why CO2 is acidic in character?

(ix) Basic character of oxides increases down the group. Justify it.

(x) Give two defects in Mendeleev's periodic table.

Section-III (Essay Type-8)

Q: 11 Attempt FOUR questions. (4 x 2 = 8)

1. Explain briefly the groups and periods of Modern Periodic Table.

2. Give a brief account on oxides.

3. What is ionization energy? Explain its variation across the period.

4. What do you know about the position of hydrogen in the periodic table? Elaborate.

Section-IV (Practical-15)

Q: 12 Pen down the answers of following questions. [(2 + 4) + 3 + 6 = 15]

A. (a) Give the following tests for the acidic radical Carbonate CO32- (water-insoluble).

(i) Wet Test

(ii) Dry Test

(b) Give the following tests for the basic radical Silver Ag+ and Mercurous Hg22+.

(i) Confirmatory Test

(ii) Filter Ash Test

B. Write down the procedure for the preparation of aspirin.

C. Write brief answers of following questions:

(i) What do you mean by

(a) salt

(b) acid radical

(c) basic radical?

(ii) What is an ion?

(iii) What do cation, anion and metallic radical mean?

(iv) What is the difference between an ion and an atom?

ALI RAZA KAMAL

ALI RAZA KAMAL

(v) What is the difference between an ion and a radical?

(vi) What is aqua regia?

(vii) What is meant by precipitate?

(viii) How is a precipitate formed?

(ix) Define solubility.

(x) Define valency.

(xi) Name the acid radicals of dilute acid group.

(xii) Write down the chemical equation for the passage of CO2 through limewater.

ALI RAZA KAMAL

ALI RAZA KAMAL

CHAPTER 2: S-BLOCK ELEMENTS



Scheme (9)




(i) The oxides of beryllium are:

(a) Acidic (b) Basic (c) Ba+2 (d) Mg+2

(ii) Which element is deposited at the cathode during the electrolysis of brine in Nelson's cell?

(a) H2 (b) Na (c) CI2 (d) O2

(iii) Among alkali metals the lowest atomic number is of:

(a) Rb (b) K (c) Sr (d) Li

(iv) Dolomite is a compound of which elements:

(a) Be (b) Mg (c) Ca (d) Ba

(v) The root system of several plants have been greatly enlarged by the application of:

(a) Sulphur (b) Gypsum (c) Both (d) None

(vi) The elements which are very abundant in earth crust are:

(a) Si & Al (b) Ca & Mg (c) B & Al (d) All


(i) Spodumene is an ore of ____________ metal.

(ii) Alkali metal nitrates on heating give the corresponding ____________ and oxygen.

(iii) Na2CO3.H2O is the chemical formula of a mineral of sodium, which is known as ____________.

(iv) Metallic bicarbonates are decomposed on heating into their carbonates, along with ____________

and ____________.

(v) Alkali metals are ____________ reactive than alkaline earth metals.

(vi) The elements of group I are termed as alkali metals because their ____________ are alkaline.


(i) Alkali metals are very good conductor of electricity. ______

(ii) All alkali metal sulphates are insoluble in water. ______

(iii) Trona is a mineral of lithium. ______

(iv) Alkaline-earth metals are stronger reducing agents than alkali metals. ______

(v) Plaster of Paris is a hemihydrate. ______

(vi) Group I A elements are called alkali metals because their chlorides are alkaline in nature.______


(i) The alkali earth metals are strong reducing agents.

________________________________________________________________________________

(ii) The compounds of alkali and alkaline earth metals are colourless but some of them are coloured.

________________________________________________________________________________

(iii) The aqueous solution of Na2CO3 is alkaline in nature.

________________________________________________________________________________

(iv) The limewater turns white after the white wash on the walls.

________________________________________________________________________________

(v) The Plaster of Paris is called the half hydrate.

________________________________________________________________________________

ALI RAZA KAMAL

ALI RAZA KAMAL




(i) Why the elements of group I-A are called alkali metals?

(ii) Why the elements of group II-A are called alkaline earth metals?

(iii) What are the most abundant elements among the alkali metals in the earth's crust?

(iv) Why the alkali metals are not found free in nature?

(v) What are the important ores and minerals of sodium?

(vi) What are the important ores and minerals of potassium?

(vii) Why the melting and boiling points of group I-A and II-A elements decrease down the group?

(viii) Why the alkali earth metals are strong reducing agents?

(ix) Why the alkaline earth metals are reducing agents but less than those of I-A group elements?

(x) What are the flame tests of alkali metals?


(i) The compounds of alkali and alkaline earth metals are colourless but some of them are coloured.

Give reasons.

(ii) Lithium only gives a simple oxide with oxygen but sodium and potassium give peroxide and

superoxide. Give reasons.

(iii) Why sodium reacts with water, the hydrogen, which evolved, catches fire?

(iv) Why the ionic hydrides are very good reducing agents?

(v) Which element of group I-A reacts with nitrogen and carbon?

(vi) Why does lithium differ from its own family members?

(vii) Which salts of lithium are insoluble in water but corresponding salts of other alkali metals are water-

soluble?

(viii) What is the effect of heat on hydroxides of alkali metals?

(ix) How do you compare the carbonate of lithium with the carbonates of other family members?

(x) How do you compare LiNO3 with the nitrates of other alkali metals?


(i) Give the names and formulas for the common minerals of beryllium.

(ii) Give the names and formulas for the common minerals of magnesium.

(iii) Give the names and formulas for the common minerals of calcium.

(iv) Heat of hydration of alkaline earth metals go on decreasing from upper to downward direction. Why?

(v) Mention the flame test of II-A group elements.

(vi) How do you compare the polarizing powers of ions of II-A and that of I-A group elements?

(vii) How magnesium and calcium react with nitrogen to give nitrides, which on hydrolysis give ammonia?

(viii) How do you discuss the effect of heat on the carbonates of group I-A and II-A?

(ix) Solution of Na2O in water is alkaline. Justify the statement.

(x) How do you compare the carbide of beryllium with carbide of calcium?


(i) What is the trend of changing basicity of oxides down the group?

(ii) How does beryllium react with NaOH to give a salt and evolve hydrogen?

(iii) BeO is an amphoteric oxide. Justify it.

(iv) How KO2 can be used by mountaineers?

(v) Why the aqueous solution of Na2CO3 is alkaline in nature?

(vi) What is the trend of solubilities of oxides of alkaline earth metals?

(vii) How do you compare the solubilities of hydroxides of alkaline earth metals?

(viii) What is lime and lime water?

(ix) What is milk of magnesia? What is its use?

(x) What is the effect of temperature on Na2CO3?

ALI RAZA KAMAL

ALI RAZA KAMAL


(i) What is difference between soda ash and washing soda?

(ii) What happens when CO2 gas is passed through limewater?

(iii) What happens when excess CO2 gas is passed through limewater?

(iv) Why the limewater turns white after the white wash on the walls?

(v) In what respect, nitrates of Li, Mg and Ba are related with each other?

(vi) How do you compare the solubilities of sulphates of alkaline earth metals?

(vii) What is gypsum? How is it related with plaster of Paris?

(viii) What are the advantages of Down's cell for preparation of sodium on commercial scale?

(ix) Why CaCl2 is added in molten NaCl in Down's cell?

(x) Which substances are deposited at cathode and anode in the Nelson's cell?


(i) What is importance of sulphur for the plants?

(ii) Why the Plaster of Paris is called the half hydrate?

(iii) What do you mean by setting of Plaster of Paris? What are the main uses of plaster of Paris?

(iv) What is hard finish plaster?

(v) What is the use of material, which is produced when the plaster of Paris is mixed with the wood

pulp?

(vi) What is the role of gypsum in the cement industry?

(vii) What do you mean by dead burnt gypsum?

(viii) What is the function of calcium in the plant growth?

(ix) Indicate the processes in which lime acts as dehydrating reagent.

(x) What is lime mortar? Give equations for its hardening.



1. Give an account on peculiar behaviour of Beryllium.

2. Give any five trends in chemical properties of Alkali Metals and Alkaline Earth Metals.

3. How sodium is commercially prepared by Down’s Cell?

4. What is the role of lime and gypsum in agriculture?



A. (a) Give the following tests for the acidic radical Carbonate CO32- (water-soluble).

(i) Wet Test

(ii) Confirmatory Test

(b) Give the following tests for the basic radical Plumbous Pb2+ and Cadmium Cd2+.

(i) Wet Test

(ii) Charcoal Cavity Test

B. Write down the procedure for the preparation of iodoform from alcohol.


(i) What is limewater?

(ii) Can we use any other solution in place of limewater for detection of carbonates?

(iii) How will you distinguish between CO32- and HCO3

1-?

(iv) Name two soluble carbonates and two insoluble carbonates.

(v) Can a paper dipped in AgNO3 be used in place of a lead acetate paper in the detection of a

sulphide?

(vi) Why in confirmatory test for SO32- the acidified potassium dichromate paper is turned green?

(vii) Why in confirmatory test for S2O32- the iodine solution is decolourized?

(viii) How will distinguish between SO32- and S2O3

2-?

(ix) Does nitrate give “Ring test”?

(x) Name the acid radicals of conc. H2SO4 group.

(xi) Salt is warmed with conc. H2SO4 instead of boiling. Why?

(xii) What is the difference between hydrogen chloride and hydrochloric acid?

ALI RAZA KAMAL

ALI RAZA KAMAL

CHAPTER 3: GROUP III A AND GROUP IV A ELEMENTS



Scheme (9)

Weightage = 7% MCQ’s = 1 Short Questions = 4 Extensive Question = -



(i) Which metal is used in the thermal process because of its activity?

(a) (b) (c) (d)

(ii) Group IV A elements form:

(a) Super oxide (b) Oxides (c) Dioxide (d) All

(iii) Which of the following does not give Borax bead test?

(a) Cu (b) Cr (c) Ni (d) Al

(iv) Silicon differ from silica by a group of:

(a) CH3 (b) –OH (c) OCH3 (d) O2

(v) Crystalline boron has structure:

(a) Cubic (b) Monoclinic (c) Hexagonal (d) Trigonal

(vi) Which of the following can form nitride, which react with water to give ammonia?

(a) Boron (b) Gallium (c) Indium (d) Thallium


(i) ____________ acid has the chemical formula HBO2.

(ii) Aluminium normally occurs as ____________minerals found in rocks of outer portion of the earth.

(iii) Aluminium gives ____________ gas with hot concentrated H2SO4.

(iv) In the Group III A of the periodic table, ____________ is a semi-metal.

(v) Borax that occurs as a natural deposit is called ____________.

(vi) Cryolite is an important mineral of aluminium and its formula is ____________.


(i) Diaspore is an ore of carbon. ______

(ii) Emerald is an ore of aluminium that has the chemical formula Al2O3.2SiO2.2H2O. ______

(iii) Boron always uses all the three of its valence electrons for bonding purposes. ______

(iv) An aqueous solution of borax is feebly acidic in nature. ______

(v) In case of borax bead test, of cupric oxide, the beads are coloured blue in the reducing flame.

______

(vi) Boric acid can be titrated with sodium hydroxide. ______


(i) The hydrides of boron have different structures from the hydrides of other family members.

________________________________________________________________________________

(ii) The aqueous solution of borax turns red litmus blue.

________________________________________________________________________________

(iii) Al is not found free in nature.

________________________________________________________________________________

(iv) Diamond is non-conductor of electricity.

________________________________________________________________________________

(v) Liquid silicons preferred over ordinary organic lubricants.

________________________________________________________________________________

ALI RAZA KAMAL

ALI RAZA KAMAL




(i) Define How the elements of group III-A show the valency of three?

(ii) Why the heat of sublimation in group III-A elements decrease down the group?

(iii) B+3 ion does not exist but Al+3 does. Why?

(iv) How the nature of the oxides of the group III-A change from upper to the downward direction?

(v) The hydrides of boron have different structures from the hydrides of other family members. Why?

(vi) Give the names and formulas of different acids of boron.

(vii) How will thou convert boric acid into borax and vice versa?

(viii) How the solubility of borax changes with the change of temperature?

(ix) How does the temperature influence the water of crystallization of borax?

(x) Justify that the aqueous solution of borax turns red litmus blue.

(xi) How borax can be converted onto orthoboric acid?


(i) Outline four uses of borax.

(ii) How the glassy mass is produced from borax?

(iii) Which basic radicals give the response to borax bead test?

(iv) What is the natural of compounds, which give coloured beads in borax bead test?

(v) Give the names and formulas of oxyacids of boron.

(vi) How H3BO3 can be prepared from colemanite?

(vii) How H3BO3 can be prepared from Na2B4O7?

(viii) How does H3BO3 acts as an acid?

(ix) What is e the effect of heat on H3BO3?

(x) Give uses of boric acid.

(xi) What are the important ores and minerals of Al?


(i) What is anodizing?

(ii) Why Al is not found free in nature?

(iii) How does Al react with dilute and conc. H2SO4?

(iv) How does Al react with conc. HNO3?

(v) How does Al become water-soluble by using NaOH?

(vi) How inert pair effect controls the oxidation states of Sn and Pb?

(vii) How carbon behaves differently, from the other members of its own group?

(viii) Mention various allotropic modifications of elements of group IV-A.

(ix) What are the important ores of SiO2?

(x) What are the different forms in which SiO2 exists in the earth crust?

(xi) Why diamond is non-conductor of electricity?


(i) What is quartz and what are its properties?

(ii) Why is CO2 a gas at room temperature while SiO2 is a solid?

(iii) Explain (a) CO2 is non-polar in nature (b) CO2 is acidic in character.

(iv) What is silica gel?

(v) How sodium silicate is prepared?

(vi) What are the properties of water glass?

(vii) What are the uses of sodium silicate?

(viii) What is chemical garden?

(ix) What are the uses of aluminium silicates or clay?

(x) How the clay is hardened?

ALI RAZA KAMAL

ALI RAZA KAMAL


(i) Give the formula of talc or soap stone. Give its properties and uses.

(ii) What is asbestos? Give its uses.

(iii) What are silicons? Give their uses.

(iv) Why are liquid silicons preferred over ordinary organic lubricants?

(v) Which elements and compounds act as semiconductor?

(vi) What is the effect of temperature on semiconductor?

(vii) Define semiconductor. Give one example.

(viii) What are lead pigments? Give their common names as well.

(ix) How litharge changes its colour?

(x) What is the formula of white lead? Give its properties and uses.


Q: 10 Attempt FIVE questions. (5 x 3 = 15)

1. Explain occurrence and properties of borax.

2. Give the properties and uses of boric acid.

3. Give the reactions of aluminium with non-metals, acids and alkalies.

4. Elaborate the properties and uses of (a) Sodium Silicate (b) Aluminium Silicate

5. Give the uses of lead compounds in plants.



A. (a) Give the following tests for the acidic radical Bicarbonate HCO31-.

(i) Dry Test


(b) Give the following tests for the basic radical Mercuric Hg2+ and Bismuth Bi3+.

(i) Wet Test


B. Write down the procedure for the preparation of phenyl glucosazone.


(i) What is meant by Cl, Cl1- and Cl2?

(ii) Why the brown vapours are intensified with manganese dioxide in the case of Br1-?

(iii) Why do bromides and iodides not respond to the chromyl chloride test?

(iv) Give the chemical equations for (a) Ring test (b) Chromyl Chloride Test.

(v) What is the chemical name for the brown ring formed in the test for nitrates?

(vi) Why do we use freshly prepared ferrous sulphate solution for testing nitrites or nitrates?

(vii) How will you distinguish between NO31- and Br1-?

(viii) Why the acidified KMnO4 solution is decolourized in the confirmatory test for C2O42-?

(ix) Write down the formulas of chromyl chloride and diphenylamine.

(x) Name the acid radicals of special group.

(xi) Name two soluble sulphates and insoluble sulphates.

(xii) Write down the formulas of ammonium molybdate and sodium nitroprusside.

ALI RAZA KAMAL

ALI RAZA KAMAL

CHAPTER 4: GROUP V A AND VI A ELEMENTS



Scheme (11)




(i) In group VA elements the most electronegative elements is:

(a) Sb (b) N (c) P (d) As

(ii) Which catalyst is used in contact process?

(a) Fe2O3 (b) V2O5 (c) SO3 (d) Ag2O

(iii) Allotropes of phosphorus are of:

(a) Three types (b) Four types (c) Two types (d) Six different types

(iv) In group VI A the radioactive metal is:

(a) Te (tellurium) (b) O (oxygen) (c) N (nitrogen) (d) None of the above

(v) In Ostwald’s Process the substance used to oxide ammonia is:

(a) Zn (b) Pt (c) CO (d) None of these

(vi) Oelum is formed by combining H2SO4 with:

(a) SO2 (b) MnO2 (c) Al2O3 (d) CrO3


(i) HNO3 is used in the manufacture of ____________fertilizers.

(ii) Specific gravity of H2SO4, at 18 °C is ____________.

(iii) Conc. Phosphoric acid acts as a ____________.

(iv) Nitrogen is a gas while other elements of the same group are ____________.

(v) Sulphur is different from oxygen because it shows ____________ oxidation states.

(vi) Noble metals like gold and platinum are dissolved in ____________.


(i) The oxides of nitrogen are basic in nature. ______

(ii) TNT is prepared by the reaction of nitric acid with toluene. ______

(iii) V2O5 is used as a catalyst for the oxidation of SO2 to SO3. ______

(iv) Ionization energy of oxygen is greater than that of nitrogen. ______

(v) The elements of group V A exhibit maximum oxidation state of +5. ______

(vi) Sulphur occurs in many organic compounds of animal and vegetable origin. ______


(i) The outermost p-subshells of the elements of group V-A are extra stable.

________________________________________________________________________________

(ii) P2O5 react with water in cold and hot state.

________________________________________________________________________________

(iii) SO3 gas is dissolved in H2SO4, but not in water in the contact process.

________________________________________________________________________________

(iv) H3PO3 is dibasic acid, although it has three hydrogen atom in it.

________________________________________________________________________________

(v) P2O5 is the dehydrating reagent.

________________________________________________________________________________

ALI RAZA KAMAL

ALI RAZA KAMAL




(i) What is general occurrence of elements of group V-A?

(ii) How allotropy is associated with nitrogen and phosphorus?

(iii) How the melting and boiling points for the elements of group V-A vary down the group?

(iv) How the involvement of d-orbital increases the oxidation number of phosphorus?

(v) Why the outermost p-subshells of the elements of group V-A are extra stable?

(vi) What type of oxides are mostly given by the elements of group V-A?

(vii) Write down the formulas and names of the oxyacids of nitrogen, phosphorus, arsenic and antimony

with oxidation number +5.

(viii) How does nitrogen differ from its family members in physical state, atomicity and variety of oxidation

states?

(ix) Write down the names, formulas and colours of oxides of nitrogen along with the oxidation states of

nitrogen in them

(x) How do you justify that N2O is a supporter of combustion?

(xi) How do you compare the structure of N2O and NO?


(i) What is the reaction on NO with FeSO4 solution?

(ii) Justify that NO acts as an oxidizing agent.

(iii) How NO2 prepared from PbNO3?

(iv) How NO2 prepared from Cu and HNO3?

(v) What is the effect of temperature on N2O4?

(vi) How does NO2 acts as an oxidizing agent?

(vii) How does HNO2 acts as an oxidizing agent?

(viii) How does HNO2 acts as a reducing agent?

(ix) Write down the reactions involved in the preparation of HNO3 by Brikeland Eyde's process.

(x) How dilute HNO3 can be concentrated on the commercial scale?

(xi) Give the reactions of HNO3 in which it acts as an oxidizing agent.


(i) What is aqua regia? And how does it dissolve the noble metals?

(ii) What is meant by fuming nitric acid?

(iii) Describe the Ring test for the confirmation of nitrate ions in the solution.

(iv) How phosphorus does occurs in form of minerals, in plants and in animal tissues?

(v) How do you compare the properties of white and red phosphorus?

(vi) How do you compare the structures of PCl3 and NH3?

(vii) How PCl3 and PCl5 react with alcohols and carboxylic acids?

(viii) Give the names and formulas of various oxides of phosphorus.

(ix) How does P2O3 react with water in cold and hot state?

(x) How does P2O5 react with water in cold and hot state?


(i) Justify that P2O5 is the dehydrating reagent.

(ii) Give the names and formulas of oxyacids of phosphorus and indicate the oxidation number of

phosphorus in them.

(iii) H3PO3 is dibasic acid, although it has three hydrogen atom in it. Justify the statement.

(iv) Give reactions to justify that H3PO3 is a reducing agent.

(v) How H3PO3 is affected at high temperature?

(vi) How do you compare the elements of group VI-A in their physical states?

(vii) How sulphur can increase its oxidation number but oxygen cannot?

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ALI RAZA KAMAL

(viii) Mention various allotropic forms of the elements of group VI-A.

(ix) How does oxygen differ from its own family members especially sulphur?

(x) How does oxygen occur in nature?


(i) How does sulphur occur in nature?

(ii) Mention the catalytic condition for the manufacture of H2SO4 in the contact process.

(iii) What are the optimum conditions for the manufacture of H2SO4 in the contact tower?

(iv) Give the advantages of contact process for the manufacture of sulphuric acid.

(v) Why SO3 gas is dissolved in H2SO4, but not in water in the contact process?

(vi) How does H2SO4 acts as the dehydrating reagent?

(vii) Write down the equation for the reaction between conc. H2SO4 and copper and explain what type of

reaction is it?

(viii) How KMnO4 and K2Cr2O7 react with H2SO4?

(ix) Justify that H2SO4 is a king of chemicals.

(x) Discuss the structure of H2SO4 and phosphoric acid.



1. Give an account on properties and reactions of nitrogen dioxide.

2. Define phosphorous. Explain its halides.

3. What is nitric acid? How is it manufactured by Brikeland and Eyde’s process.

4. Compare oxygen and sulphur.

5. How sulphuric acid is manufactured on commercial scale?

6. Give an account on following:

(a) Reactions of H2SO4 as oxidizing agents

(b) Reactions of H2SO4 with salts

(c) Four physical properties of H2SO4



A. (a) Give the following tests for the acidic radical Sulphide S2-.

(i) Dry Test

(ii) Wet Test

(b) Give the following tests for the basic radical Copper Cu2+ and Antimony Sb3+.

(i) Flame Test

(ii) Charcoal Cavity Test

B. Write down the procedure for the preparation of copper amine complex.


(i) Why some basic radicals are coloured and others not so?

(ii) What is a paramagnetic ion?

(iii) What is a diamagnetic ion?

(iv) Define bead, scales and incrustation.

(v) What is decrepitation?

(vi) What is deflagration?

(vii) Why is platinum wire employed in the flame test?

(viii) How platinum wire is washed? Can we use Cu wire in flame test?

(ix) Why do we treat a salt with HCl before performing performing its flame test?

(x) Write the formula of borax.

(xi) What is the composition of the bead, which is obtained in the borax bead test?

(xii) What is the basic theory for

(a) Flame test (b) Borax bead test (c) Charcoal cavity test

(d) Cobalt nitrate test (e) Filter ash test?

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ALI RAZA KAMAL

CHAPTER 5: THE HALOGENS AND THE NOBLE GASES



Scheme (15)




(i) Which is the most volatile compound?

(a) HI (b) HCI (c) HBr (d) HF

(ii) The element which liberated O2 from water is:

(a) P (b) N (c) F (d) I

(iii) Which member of group VII A combines with one more halogen:

(a) Cl (b) F (c) Br (d) I

(iv) Which one halogen directly reacts with noble gas:

(a) F (b) Cl (c) Br (d) I

(v) The average available chlorine in bleaching powder is:

(a) 30 – 35% (b) 35 – 40% (c) 40 – 45% (d) 45 – 50%

(vi) The known fluorides of xenon are:

(a) XeF2 (b) XeF4 (c) XeF6 (d) All of the above


(i) The halogen with the highest electronegativity is ____________.

(ii) ____________ is the halogen, which causes bums on the skin, which heal slowly.

(iii) The sea divers use a mixture of ____________ and ____________ for breathing.

(iv) Bleaching powder is prepared from ____________ and ____________.

(v) HI is ____________ agent.

(vi) Noble gas used to fill fluorescent bulbs is ____________.


(i) HF is used for etching glass. ______

(ii) Radon is the only one of the noble gases that is radioactive. ______

(iii) Bleaching powder is completely soluble in water. ______

(iv) HI is weaker reducing agent as compared to HF. ______

(v) α-particles emitted by radioactive elements are ions of radon. ______

(vi) The formula of perchloric acid is HClO2. ______


(i) The elements of group VII-A are called halogens.

________________________________________________________________________________

(ii) The dissociation energies of the halogens go on decreasing down the group.

________________________________________________________________________________

(iii) Fluorine and chlorine act as decolourizing agents.

________________________________________________________________________________

(iv) HClO4 is a stronger acid than HBrO4 than HIO4.

________________________________________________________________________________

(v) Oxidation states of noble gases are usually zero.

________________________________________________________________________________

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ALI RAZA KAMAL




(i) Why the elements of group VII-A are called halogens?

(ii) How does astatine differ its own family members?

(iii) What are the important press and minerals of fluorine and iodine?

(iv) What is iodized salt?

(v) Compare the physical states and colours of halogens at room temperature.

(vi) Why the dissociation energies of the halogens go on decreasing down the group?

(vii) Halogens are strong oxidizing agents. Justify it.

(viii) Due to which reasons fluorine shows peculiar behaviour from other family members.

(ix) How does the hydrogen bonding in HF changes the properties of this compound from other halogen

acids?

(x) Arrange the halogen ions in the order of increasing sizes.


(i) What are those factors, which affect the oxidizing power of the halogens?

(ii) Why iodine has metallic luster?

(iii) Why fluorine and chlorine act as decolourizing agents?

(iv) Which halogen is used as an antiseptic?

(v) Which halogen is used in water treatment to kill bacteria?

(vi) How do you compare the preparations of halogen acids?

(vii) How are halogen acids ionized in water?

(viii) How do you justify the decreasing bond dissociation energies of halogen acids?

(ix) How the thermodynamic properties of halogen acids change in a group from upper to downward

level?

(x) Compare the halogen acids in their reducing properties.


(i) Why HF is weaker acid than HCl and HI is stronger in the series?

(ii) Give the formulas and names of important oxides of chlorine and bromine.

(iii) How do you justify that Cl2O7 is the anhydride of perchloric acid?

(iv) Justify that reaction of chlorine with NaOH in the cold state is disproportionation reaction.

(v) Justify that reaction of chlorine with NaOH in the hot state is disproportionation reaction.

(vi) Give the names and formulas of oxyacids of chlorine and iodine.

(vii) How do you compare the stabilities of oxyacids of halogens?

(viii) Give the structures of oxyacids of chlorine.

(ix) How do you justify the increasing acid strengths of oxyacids of chlorine?

(x) Why HClO4 is a stronger acid than HBrO4 than HIO4?


(i) HClO4 may cause explosion. Give reasons. Give its preparations.

(ii) How bleaching powder can act as an oxidizing agent?

(iii) What do you mean by available chlorine and how is it calculated?

(iv) How does bleaching powder acts as an oxidizing agent towards halogen acids?

(v) How does bleaching powder acts as a bleaching agent for fabrics?

(vi) What are freons? Give their uses.

(vii) What are teflons? Give their uses.

(viii) Give important uses of chlorine.

(ix) Give important uses of bromine and iodine.

(x) Why the elements of group VIII-A are called noble gases?

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ALI RAZA KAMAL


(i) What are noble gases? Why are they inert?

(ii) Why the oxidation states of noble gases are usually zero?

(iii) How does radon differ from its own family member?

(iv) How the solubilities of noble gases are affected in water?

(v) Give the names and formulas of important compounds of xenon. Give the oxidation state of xenon in

these compounds.

(vi) How hydrogen does reacts with the fluorides of xenon?

(vii) How XeF6 reacts with water and SiO2 separately?

(viii) Give the important applications of helium and argon.

(ix) Give the important uses radon.

(x) What is the effect of high voltage on noble gases?



1. Give an account on the peculiar behaviour of fluorine.

2. What are the properties of hydrogen halides?

3. Explain the Beckmann’s method for the manufacturing of bleaching power on commercial scale.

4. Explain fluorides of xenon.

5. Explain the oxides of xenon. Also, elaborate the application of noble gases.

6. Give the reactions of chlorine with cold and hot NaOH.



A. (a) Give the following tests for the acidic radical Sulphite SO32-.

(i) Wet Test


(b) Give the following tests for the basic radical Stannous Sn2+ and Ferrous Fe2+.

(i) Dry Test

(ii) Wet Test

B. Write down the procedure for estimation of barium in given sample of solution gravimetrically as

chromate.


(i) Why do we prefer HCl for preparing original solution for basic radicals?

(ii) What is the group reagent for the group I?

(iii) Name insoluble chlorides.

(iv) Can we use conc. HCl as group reagent for group I?

(v) What happen when NH4OH is added to AgCl?

(vi) Why is silver nitrate solution kept in a coloured bottle?

(vii) What is hydrargyrum?

(viii) Name one chemical which reacts with all radicals of group I.

(ix) Name the basic radicals for group II A and II B.

(x) What is the group reagent for group II?

(xi) Why dilute HCl is added in group II?

(xii) Why is the solution diluted in group II before passing H2S gas?

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ALI RAZA KAMAL

CHAPTER 6: TRANSITION ELEMENTS



Scheme (7)




(i) Which of the following is a typical transition metal?

(a) Sc (b) Y (c) Ra (d) Co

(ii) Group VI B of transition elements contains:

(a) Zn, Cd , Hg (b) Fe, Ru, Os (c) Cr, Mo, W (d) Mn, Te, Re

(iii) The total number of transition elements is:

(a) 10 (b) 14 (c) 40 (d) 50

(iv) In transition elements the orbital which is responsible for the colour development is:

(a) s-orbital (b) f-orbital (c) d-orbital (d) o-orbital

(v) Wrought iron is manufactured from:

(a) Pig iron (b) Cast iron (c) Pig iron or cast iron (d) Steel

(vi) Compounds attracted by applied magnetic field are called:

(a) Diamagnetic (b) Paramagnetic (c) Good conductor (d) Ferromagnetic


(i) The property of paramagnetism is due to the presence of ____________ electrons.

(ii) MnO4- ion has ____________ colour and Cr2O7

2- has ____________ colour.

(iii) When potassium chromate is treated with an acid ____________ is produced.

(iv) The d-block elements are located between____________ and ____________ block elements.

(v) The presence of ____________ in a metal promotes corrosion.

(vi) Complexes having sp3d2 hybridization have ____________shape.


(i) Tin plating is used to protect iron sheets from corrosion. ______

(ii) In galvanizing, zinc prevents corrosion of iron. ______

(iii) Fe3+ ions are blue when hydrated. ______

(iv) The name of anionic ligands in a complex ends is suffix ‘O’. ______

(v) Pig iron contains greater percentage of carbon than steel. ______

(vi) Complex compounds having dsp2 hybridization have tetrahedral geometry. ______


(i) The corrosion of metals is more rapid in presence of water.

________________________________________________________________________________

(ii) d-block and f-block elements are called transition elements.

________________________________________________________________________________

(iii) The maximum paramagnetic strength is associated with the middle elements of d-block series.

________________________________________________________________________________

(iv) The catalytic properties are associated with the transition elements.

________________________________________________________________________________

(v) Damaged tin plated iron get rusted quickly.

________________________________________________________________________________

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ALI RAZA KAMAL




(i) What are d-block elements? Why are they called so?

(ii) What are f-block elements? Why are they called so?

(iii) Why d-block and f-block elements are called transition elements?

(iv) Why the electronic distribution of chromium and copper is different from the from the rest of the

elements of 3d series?

(v) What are typical and non-typical transition elements? Why are they called so?

(vi) How do you distinguish between outer transition and inner transition elements?

(vii) What is lanthanide contraction?

(viii) How the atomic radii of the d-block elements vary from left to right in the period?

(ix) How the ionization energy values changes from left to right in period of d-block elements?

(x) Justify the variation of binding energies in d-block elements from left to right.

(xi) Why the melting points and boiling points are maximum somewhere in the middle of series of the d-

block elements?


(i) What is paramagnetism? What are its units?

(ii) How the property of paramagnetism developed in the substances?

(iii) Why the maximum paramagnetic strength is associated with the middle elements of d-block series?

(iv) What is the reason for variations of oxidation states of transition elements?

(v) What is the reason for the development of the colours in the compounds of transition elements?

What is d-d transition?

(vi) What are complementary colours? Give examples.

(vii) Why the catalytic properties are associated with the transition elements?

(viii) What are interstitial compounds? Give their examples.

(ix) Give examples of alloys and give their properties.

(x) How many types of various groups are present in the transition metal complex?

(xi) Give the nature of ion which are produced in water when K4[Fe(CN)6] and [Cu(NH3)4]SO4 are

dissolved in water.


(i) Indicate the central metal atom or ion along with its oxidation numbers in the complexes.

(a) K4[Fe(CN)6]

(b)K3[Fe(CN)6]

(c) [Ag(NH3)2]Cl

(ii) Give three examples of

(a) Monodentate neutral ligands

(b) Bidentate ligands.

(iii) What is co-ordination number and co-ordination sphere of complex compounds?

(iv) What are chelates?

(v) While naming the complex compounds, how do you end with negatively charged ligands, positively

charged ligands and neutral ligands?

(vi) Name the following complexes.

(a) K2[PtCl6]

(b) Na[Mn(CO5)]

(c) [Co(en)2Cl2]Cl

(d) K2[Cu(CN)4]

(e) [Fe(CO)5]

(vii) Indicate the shapes of transition metal ions in which the central atom or an ion has sp3, dsp2 and

dsp3 hybridization.

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ALI RAZA KAMAL

(viii) Give the names and formulas for important ores of iron.

(ix) How do you compare the cast iron, wrought iron and steel with respect to the percentage of carbon?

(x) What are the uses of wrought iron?

(xi) How do you compare the wrought iron and steel with respect to the carbon, sulphur, manganese and

phosphorus?


(i) How do you compare mild steel, medium carbon steel and high carbon steel with respect to their

carbon contents and their properties?

(ii) What is the role of acidic and basic lining in the open-hearth process for manufacture of steel?

(iii) Discuss the general shape of Bessemer's converter.

(iv) How do you remove the entrapped gases from the steel?

(v) How do you compare the cast iron, wrought iron and steel keeping in view their hardness,

malleability and melting points?

(vi) Why the corrosion of metals is more rapid in presence of water?

(vii) How does electrochemical theory explain the corrosion of aluminium in the presence of copper?

(viii) How does the metallic coating prevent the corrosion?

(ix) What do you mean by cathode coating?

(x) What are chromates and dichromates?

(xi) How the acidic medium develops equilibrium between chromate and dichromate ions?


(i) Give the uses of potassium chromate and its structure.

(ii) How does K2Cr2O7 act as oxidizing agent in the presence of H2SO4?

(iii) How the mixture of K2Cr2O7 and H2SO4 oxidizes H2S gas and FeSO4 separately?

(iv) What is chromyl chloride test?

(v) Give the uses of K2Cr2O7.

(vi) Give the structure of dichromate ion.

(vii) How do you compare KMnO4 and K2MnO4?

(viii) How KMnO4 and H2SO4 act as oxidizing agents?

(ix) How KMnO4 oxidizes SO2 to H2SO4?

(x) How KMnO4 can be prepared by an electrolytic method?

(xi) Write down the structure of MnO4- ion.


Q: 10 Attempt FOUR questions. (4 x 3.25 = 13)

1. Define transition elements. Elaborate a short note on paramagnetism and colour in transition elements.

2. How wrought iron is manufactured form cast iron?

3. What is open-hearth process? For what purpose is it used?

4. Elaborate a comprehensive note on Bessemer’s Process for manufacture of steel.



A. (a) Give the following tests for the acidic radical Thiosulphate S2O32-.


(ii) Wet Test

(b) Give the following tests for the basic radicals Ferric Fe3+ and Aluminium Al3+.

(i) Borax Bead Test

(ii) Lake Test

B. Write down the procedure for the confirmatory tests of phenolic group in organic compounds.


(i) Why is the solution diluted in group II before passing H2S gas?

(ii) Why lead is precipitated in group I as well as in group II?

(iii) Why mercurous ion is written as Hg22+ rather than as Hg1+?

(iv) What is meant by read lead and white lead?

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ALI RAZA KAMAL

(v) How will you prepare artificial milk?

(vi) What is blue vitriole?

(vii) What will happen when you heat CuSO4.5H2O?

(viii) What is the reagent used for the separation of group II A and group II B?

(ix) What are the colours of

(a) CuS

(b) CdS

(c) Sb2S3?

(x) What is ‘butter of tin’?

(xi) Define common ion effect and its application.

(xii) Why sometimes white or yellow ppt. is formed when H2S is passed through the solution for

group II?

ALI RAZA KAMAL

ALI RAZA KAMAL

CHAPTER 7: FUNDAMENTAL PRINCIPALS OF ORGANIC CHEMISTRY



Scheme (7)




(i) Select from the following the one which is alcohol:

(a) CH3-CH2-OH (b) CH3-O-CH3 (c) CH3COOH (d) CH3-CH2-Br

(ii) Rate of reactions of most organic compounds are:

(a) Very slow (b) Very fast (c) Medium (d) No regular character

(iii) Coal is produced after a long time decay of:

(a) Animals (b) Fossils (c) Wood (d) Ores

(iv) In sp3 hybridization, the geometry of molecules will be:

(a) Square planar (b) Trigonal pyramidal (c) Tetrahedral (d) All are possible

(v) The fuel having 40% n-heptane & 60% iso-octane will have octane number:

(a) 40 (b) 60 (c) 80 (d) 90

(vi) Which process increases the yield of gasoline from petroleum?

(a) Cracking (b) Polymerization(c) Reforming (d) Sublimation


(i) The state of hybridization of carbon atom in ____________ is sp2.

(ii) 2-Butene is ____________ of 1-butene.

(iii) Carbonyl functional group is present in both ____________ and ____________.

(iv) A carboxylic acid contains ____________ as a functional group.

(v) A heterocyclic compound contains an atom other than ____________ in its ring.

(vi) A group of atoms, which confers characteristic properties to an organic compound, is called

____________.


(i) There are three possible isomers for pentane. ______

(ii) Alkynes do not show the phenomenon of cis-trans isomerism. ______

(iii) Organic compounds cannot be synthesized from inorganic compounds. ______

(iv) All close chain compounds are aromatic in nature. ______

(v) The functional group present in amides is called an amino group. ______

(vi) Government of Pakistan is trying to use coal for power generation. ______


(i) Restricted rotation is necessary to show the geometrical isomerism.

________________________________________________________________________________

(ii) Catenation is the property, which makes carbon different from the other elements of periodic table.

________________________________________________________________________________

(iii) All the bond angles of propane are not equal.

________________________________________________________________________________

(iv) We need cracking of petroleum.

________________________________________________________________________________

(v) The phenomenon of isomerism makes the organic compounds greater in number.

________________________________________________________________________________

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ALI RAZA KAMAL




(i) What is vital force theory? Who discarded this theory?

(ii) Which organic compound was first of all prepared in the laboratory?

(iii) What is the modern definition of organic chemistry? Which of the other elements except carbon and

hydrogen may be present in organic compounds?

(iv) Mention those compounds of carbon, which are not organic in nature.

(v) Catenation is the property, which makes the carbon different from the other elements of periodic

table. Justify.

(vi) How the phenomenon of isomerism makes the organic compounds greater in number?

(vii) Organic compounds mostly give slow reactions than inorganic compounds. Give reasons.

(viii) Organic compounds are mostly non-ionic in character. Give reasons.

(ix) What are the most important solvents that are used to dissolve the organic compounds?


(i) How the organic compounds are closely associated with the human body?

(ii) Coal is one of the major sources of organic compounds. How do you justify it?

(iii) Indicate five fractions, which are obtained from the destructive distillation of coal.

(iv) What is coal tar? Give its fractions.

(v) What is composition of natural gas?

(vi) Give important uses of natural gas.

(vii) What is petroleum? Give its origin.

(viii) Name the fractions, which are obtained by the fractional distillation of petroleum.

(ix) What is an oil refinery? Name the oil refineries in Pakistan.


(i) What is cracking of petroleum? Why do we need cracking of petroleum?

(ii) Give the products by the cracking of n-butane.

(iii) What is thermal cracking?

(iv) What is catalytic cracking?

(v) What is steam cracking?

(vi) What do you mean by knocking of petroleum?

(vii) How do you define octane number? How it can be improved?

(viii) What is reforming of petroleum? Give one example.

(ix) Give at least five compounds, which are homocyclic but are not aromatic.


(i) Give four examples of aromatic heterocyclic compounds and two examples of homocyclic aromatic.

(ii) What are aromatic hydrocarbons? Give two examples.

(iii) What is meant by functional group? Name and represent two functional groups containing oxygen.

(iv) Give the characteristics of homologous series.

(v) Draw the structure of CH4 and CCl4, indicating the hybridization of central atom.

(vi) Draw the structure of C2H4 and indicate the bond lengths and bond angles.

(vii) Draw the structure of C2H2 and indicate the bond lengths and bond angles.

(viii) Why all the bond angles of propane are not equal?

(ix) What is isomerism? Give the names of four structural isomerisms.


(i) Give the examples of chain isomers an alkane having three chain isomers.

(ii) Give the examples of positional isomers in alkenes and alkynes.

(iii) Write isomers of C4H10. Give two examples of functional group isomers.

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(iv) 1-Butene does not show geometrical isomerism but 2-Butene does. Give reasons.

(v) 2-Butyne does not show geometrical isomerism but 2-Butene does. Give reasons.

(vi) Why is restricted rotation necessary to show the geometrical isomerism?

(vii) How the restricted rotation of the cyclic compounds gives birth to geometrical isomerism?

(viii) Define tantomerism with example.


Q: 10 Attempt SIX questions. (6 x 4 = 24)

1. Define organic chemistry. Give any four features of organic compounds.

2. Sketch a table showing principal fractions obtained from the petroleum. Mention following features:

(a) Boiling Point Range (°C) (b) Composition (c) One Use

3. What is meant by cracking? Fill the following table related to it.

TYPE OF CRACKING DEFINITION USES

Thermal Cracking

Catalytic Cracking

Stream Cracking

4. Classify the organic compounds giving one example in each case.

5. Explain sp2 hybridization in carbon.

6. Define isomerism. Fill the following table related to it.

STRUCTURAL ISOMERISM

DEFINITION EXAMPLES

Chain Isomerism

Position Isomerism

Functional Group Isomerism

Metamerism



A. (a) Give the following tests for the acidic radical Nitrite NO21-.

(i) Dry Test

(ii) Wet Test

(b) Give the following tests for the basic radicals Chromium Cr3+ and Cobalt Co2+.

(i) Borax Bead Test


B. Write down the procedure for the preparation of acetyl salicylic acid.


(i) What will happen if bismuth or zinc salts are heated in a dry test tube?

(ii) Name the radicals of group III.

(iii) What is the group reagent for group III?

(iv) Why conc. HNO3 is added in group III?

(v) Why the large excess of NH4OH is avoided in group III?

(vi) Can we add NH4OH first and then NH4Cl?

(vii) How will you differentiate between ferrous and ferric salts?

(viii) What is green vitriole?

(ix) Can we test chromium in K2Cr2O7 by its usual tests?

(x) Which basic radical gives gelatinous white ppt.?

(xi) Explain the lake test.

(xii) Why radicals of group IV and Mg2+ ions are not precipitated along with group III though their

hydroxides are water-soluble?

ALI RAZA KAMAL

ALI RAZA KAMAL

CHAPTER 8: ALIPHATIC HYDROCARBONS



Scheme (8)




(i) Alkanes containing one branch on main chain are called:

(a) Iso (b) Normal (c) Neo (d) Branched

(ii) Sabatier’s Sendern’s reaction involves _________ in presence of Ni.

(a) Alkene & H2 (b) Alkene & O2 (c) Alkene & N2 (d) Alkene & Cl2

(iii) Malozonide changes into:

(a) Epoxide (b) CO2 + H2O (c) Ozonide (d) CO + H2O

(iv) General formula of alkenes is:

(a) CnH2n+2 (b) CnH2n-2 (c) CnH2n (d) CnH2n-x

(v) Which member of IV A has little tendency to form anions or cations?

(a) Pb (b) Sn (c) Ge (d) C

(vi) Methane and other members of paraffins do not react with aqueous solution of acids, alkalies,

KMnO4 or other oxidizing agents this lack of reactivity is due to its nature:

(a) Polar (b) Non-polar (c) Acidic (d) Basic


(i) Ozone reacts with ethene to form ____________.

(ii) Vicinal dihalides have two halogens on ____________ carbon atoms.

(iii) Ethene is acidic in nature because of ____________ hybridization.

(iv) Mustard gas is a high boiling ____________.

(v) Ethene has a ____________ like odour.

(vi) Ethyne is obtained by the reaction of ____________ with calcium carbide.


(i) Mustard gas is a blistering agent. ______

(ii) Methane is also called marsh gas. ______

(iii) Alkanes usually undergo substitution reactions. ______

(iv) Benzene is a polymer of ethene. ______

(v) Acrylonitrile can be obtained from ethyne. ______

(vi) Ethyne is more reactive towards electrophilic reagents than ethene. ______


(i) The saturated hydrocarbons act as good-fuels.

________________________________________________________________________________

(ii) Alkenes are called olefins.

________________________________________________________________________________

(iii) The pie bond is more reactive than sigma bond.

________________________________________________________________________________

(iv) Ethyne reacts with alkaline KMnO4.

________________________________________________________________________________

(v) Alkanes are less reactive than alkenes.

________________________________________________________________________________

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ALI RAZA KAMAL




(i) What are hydrocarbons? Give one example of each type.

(ii) Give the general formulas for alkanes, alkenes and alkynes.

(iii) Explain, why alkanes are less reactive than alkenes?

(iv) What is the effect of branching on the melting point of alkanes?

(v) How many alkyl groups can be generated by alkane with molecular formula C4H10? Give the names

of alkyl groups.

(vi) Why some hydrocarbons are saturated and other unsaturated? What type of reactions are

characteristics of them?

(vii) How can you justify that bond angle in propane and butane between carbon-carbon bonds is greater

than 109.5°?

(viii) What is Sabatier Sendern's reaction?

(ix) What is the importance of hydrogenation of unsaturated compounds?

(x) What are the reduction products of alkyl halides? Indicate the important reducing agents for this

purpose.

(xi) What is hydrogenolysis?


(i) What is importance of Wurtz synthesis for the manufacture of alkanes? Prepare n-butane.

(ii) What do you mean by decarboxylization of carboxylic acids?

(iii) Give the nature of products when the sodium salt of propanoic acid is electrolyzed in Kolbe's

electrosynthesis.

(iv) Write the equation for the conversions of aldehydes and ketones into corresponding alkanes.

(v) How the reactions of Grignard's reagent with active hydrocarbons give alkanes with the same

number of carbon atoms as present in the alkyl group of Grignard's reagent?

(vi) Reason out the low reactivity of alkanes among the hydrocarbon family.

(vii) Why the saturated hydrocarbons act as good-fuels?

(viii) Give the nature of products in the chemical equation by the catalytic oxidation of methane.

(ix) The nitration of the higher hydrocarbons break the carbon-carbon bond. How HNO3 reacts with CH4?

(x) The reaction of a chlorine with CH4 has a free mechanism. Justify it.

(xi) Why alkenes are called olefins?


(i) What are monoenes, dienes and polyenes? Give one example of each.

(ii) Justify that dehydrohalogenation of alkyl halides give alkenes.

(iii) What are the most important dehydrating reagents which converts the alcohols into alkenes?

(iv) Justify that the order of reactivity of alcohols for dehydration purposes is as follow:

(Tertiary Alcohol > Secondary Alcohol > Primary Alcohol)

(v) Give the reaction conditions and reagents, which are necessary for dehydrohalogenation of vicinal

dihalides.

(vi) How Kolbe's electrosynthesis gives us ethane from sodium succinate?

(vii) How do you convert alkynes into cis and trans alkenes?

(viii) Why the pie bond is more reactive than sigma bond?

(ix) What is Raney nickel and where is it used?

(x) What are the applications of hydrogenations of unsaturated compounds to saturated compounds in

laboratory and in industry?

(xi) Indicate the mechanism for the addition of a bromine on propene.


(i) What is Markownikoff's rule? Give its applications for the addition of HBr on propene.

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(ii) How the alkenes can be converted into alcohols?

(iii) How the alkenes are converted into epoxide and what are their applications?

(iv) What is Baeyer's test to check the presence of carbon carbon double bond?

(v) Give the mechanism for ozonalysis of propene.

(vi) Give the equation and necessary conditions for the polymerization of ethene into polythene.

(vii) How mustard gas is prepared? Give its properties and uses.

(viii) How vicinal dihalides are converted into corresponding alkynes?

(ix) How ethyne can be prepared by Kolbe's electrosynthesis?

(x) How ethyne can be prepared commercially from calcium carbide?

(xi) Give the equation and necessary conditions for the addition of water at propyne.


(i) How ethyne reacts with alkaline KMnO4?

(ii) What is a role of combustion of ethyne in daily life?

(iii) How chloroprene is produced by the polymerization of acetylene?

(iv) Benzene can be prepared commercially from acetylene. Give reaction conditions.

(v) How sodamide does reacts with alkynes? What are the applications of this reaction?

(vi) How ammonical solution of AgNO3 can be used to distinguish between 1-butyne and 2-butyne?

(vii) How ammonical solution of Cu2Cl2 can be used to distinguish between 1-butyne and 2-butyne?

(viii) What are the applications of ammonical solutions of AgNO3 and Cu2Cl2?

(ix) Give the uses of acetylene.

(x) How do you distinguish between ethene and ethyne?

(xi) How do you distinguish between an alkane and alkyne?



1. Define alkanes. Give the nomenclature of alkanes.

2. Elaborate Kolbe’s electrolytic method for the preparation of alkanes. Also, give any four physical

properties of alkanes.

3. What do you mean by alkenes? Give the oxidation reactions of alkenes.

4. Justify the polymerization and acidic nature of alkynes through different examples.



A. (a) Give the following tests for the acidic radical Chloride Cl1-.

(i) Dry Test


(b) Give the following tests for the basic radicals Nickel Ni2+ and Zinc Zn2+.

(i) Borax Bead Test

(ii) Dry Test

B. Write down the procedure for the preparation of iodoform from acetone.


(i) Write down the formulas of pot.ferrocyanide, pot.ferricyanide and Mohr’s salt.

(ii) Name the basic radicals of group IV.

(iii) What is the reagent for group IV?

(iv) Suppose no black ppt. is obtained in group IV. What does this indicate?

(v) For which radical, dimethylglyoxime is used to test and what is the colour of ppt. formed?

(vi) What is the difference between Co and CO?

(vii) What is philosopher’s wool?

(viii) Name any salt of flesh colour.

(ix) Name certain insoluble sulphides.

(x) Name radicals of group IV, which give test with Na2HPO4.

(xi) Write down the formula of dimethylglyoxime.

(xii) Name the basic radicals of group V.

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CHAPTER 9: AROMATIC HYDROCARBONS



Scheme (9)




(i) The molecular formula of toluene is:

(a) C7H7 (b) C7H8 (c) C8H8 (d) C8H7

(ii) Which pair of groups contains both ortho & para directors?

(a) –OH, –RCO (b) –NR3, –CN (c) –OCH3, –CHO (d) –N (CH3)2, –NH2

(iii) What is the ratio of conc. HNO3 & conc. H2SO4 when nitration of benzene is done at 50 °C?

(a) 1:1 (b) 2:1 (c) 1:2 (d) 2:3

(iv) Acetophenone is a:

(a) Quinone (b) Ketone (c) Aldehyde (d) Other

(v) Toluene on reaction with acidic KMnO4 produces:

(a) Phenol (b) Benzoic acid (c) Benzyl alcohol (d) Benzophenone

(vi) Aspirin is obtained by reaction of sulphuric acid and:

(a) Phenol (b) Benzene (c) Acetyl chloride (d) None of these


(i) Benzene has ____________ structure.

(ii) On oxidation in the presence of V2O5 benzene gives ____________.

(iii) The introduction of halogen group in benzene ring is called ____________.

(iv) ____________ is recognized as the simplest member of the class of aromatic hydrocarbons.

(v) Benzene was discovered by Michael Faraday in ____________.

(vi) The molecular formula of C6H6 indicates that it is highly ____________ compound.


(i) Benzene is more reactive than alkene and less reactive than alkane. ______

(ii) Benzene has a pentagonal structure. ______

(iii) The C-C bond length in benzene molecule is 1.397 Å. ______

(iv) The state of hybridization of carbon in benzene molecule is sp3. ______

(v) There are six sigma bonds in benzene molecule. ______

(vi) Halogenonium produced in electrophilic substitution reactions is powerful electrophile. ______


(i) 150.5 kJ mol-1 is resonance energy of benzene.

________________________________________________________________________________

(ii) Oelum is required for sulphonation of benzene.

________________________________________________________________________________

(iii) Nitrification of toluene gives ortho and para nitrotoluene, while the bromination of nitrobenzene give

m-bromonitro benzene.

________________________________________________________________________________

(iv) Hexane and heptane can give benzene and toluene respectively.

________________________________________________________________________________

(v) Ozone affects benzene to give glyoxal.

________________________________________________________________________________

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(i) What do you mean by term 'aromatic'?

(ii) What are non-benzoid aromatic compounds?

(iii) What are the characteristics of aromatic compounds?

(iv) Give three examples of condensed aromatic hydrocarbons and give their names.

(v) Write the reaction, which give the evidence for the ring structure of benzene.

(vi) What information do we get from x-rays analysis of benzene?

(vii) There are three alternate double bonds in the benzene ring. However, why all the carbon-carbon

bonds are of equal length?

(viii) Which orbitals in benzene give stability to benzene but not to alkenes?

(ix) Write down the resonance structures of benzene and indicate their relative contributions to the actual

structure of the benzene.


(i) How do you justify that 150.5 kJ mol-1 is resonance energy of benzene?

(ii) How hexane and heptane can give benzene and toluene respectively?

(iii) Prepare maleic acid from benzene.

(iv) What is Wurtz-Fitting reaction?

(v) What do you mean by electrophilic substitution reactions of benzene? Give general mechanism.

(vi) What is sigma complex and how does it get the stability?

(vii) What is role of FeCl3 and AlCl3 in the electrophilic substitution reactions of benzene?

(viii) What are major products when chlorine reacts with toluene in the presence of sunlight?

(ix) Give the mechanism for the nitration of benzene.


(i) Why oelum is required for sulphonation of benzene?

(ii) Give the general mechanism for Friedal Craft's alkylation.

(iii) How benzene can be converted into acetophenone? Give its mechanism.

(iv) What are those reactions, which show that benzene is unsaturated hydrocarbon?

(v) How does ozone affect benzene to give glyoxal?

(vi) How toluene can be converted into benzoic acid?

(vii) Nitrification of toluene gives ortho and para nitrotoluene, while the bromination of nitrobenzene give

m-bromonitro benzene. Give reasons.

(viii) If the groups like -OH, -SH and -NH2 are present on the benzene ring, the ring is activated and ortho,

para products are obtained. Give reasons.

(ix) If -COOH and -CN groups are present on the benzene ring, they deactivate the ring and meta

products are obtained. Give reasons.



1. Elaborate the nomenclature of monocyclic aromatic hydrocarbons and their derivatives.

2. What is Kekule’s structure? Explain.

3. Give the following preparatory reactions of benzene.

(a) Dehydrogenation of Cyclohexane

(b) From Acetylene

(c) From Alkanes

(d) Preparation in the laboratory

(e) Wurtz-Fittig Reaction

4. Discuss the orientation in electrophilic substitution reactions.

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A. (a) Give the following tests for the acidic radical Bromide Br1-.

(i) Dry Test


(b) Give the following tests for the basic radicals Manganese Mn2+ and Barium Ba2+.

(i) Charcoal Cavity Test

(ii) Filter Ash Test

B. Write down the procedure for the preparation of tetra amine cupric sulphate.


(i) What is the reagent for group V?

(ii) Why is NH4Cl essential in the precipitation of the calcium group?

(iii) Does the excess of NH4Cl interfere with the precipitation of the calcium group?

(iv) Why is NH4OH added before adding (NH4)2CO3, the precipitating agent for the calcium group?

(v) Name one salt, which is insoluble even in conc. HNO3.

(vi) What is gypsum salt?

(vii) Give the formulas of

(a) Quick Lime

(b) Slaked Lime

(c) Soda Lime

(viii) Why the metals are called alkaline earth metals?

(ix) Name one test given by all basic radicals of group V.

(x) Name the basic radicals of group VI.

(xi) What is the reagent for group VI?

(xii) What is epsom salt?

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CHAPTER 10: ALKYL HALIDES



Scheme (7)




(i) Which C-X bon has the highest bond energy per mole?

(a) C-F (b) C-Cl (c) C-Br (d) C-I

(ii) During SN2 mechanism, carbon atom changes it state of hybridization from:

(a) sp → sp2 (b) sp2 → sp3 (c) sp3 → sp (d) sp3 → sp2

(iii) For which mechanisms, the first step involved is the same?

(a) E1 + E2 (b) E2 + SN2 (c) S1 + SN1 (d) SN1 + SN2

(iv) SN2 reactions can be lest carried out with ________ alkyl halides.

(a) Primary (b) Secondary (c) Tertiary (d) All of these

(v) Which monohaloalkane cannot be obtained by the direct action of halogen and alkane?

(a) RCl (b) RBr (c) RI (d) None

(vi) Which of the following is an electrophile?

(a) OH̅ (b) NH3 (c) ROH (d) BF3


(i) An alkyl group wit a partial positive charge on the carbon atom is called ____________ centre.

(ii) The mechanism is called ____________ if it involves one molecule in the rate-determining step.

(iii) The best method for the preparation of alkyl halides is the reaction of ____________ with inorganic

reagents.

(iv) Wurtz synthesis is useful for the preparation of ____________.

(v) The molecularity of E2 reactions is always two and the reaction shows ____________ order kinetics.

(vi) Molecularity of a reaction is defined as the number of molecules taking part in the ____________.


(i) Methyl magnesium iodide on hydrolysis yields ethyl alcohol. ______

(ii) The reactivity order of alkyl halides is determined by the strength of carbon-halogen bond. ______

(iii) Order of reactivity of alkyl halides for a particular alkyl group is: I > Br > Cl > F. ______

(iv) Alcohols react with thionyl chloride in ether as solvent to give alkyl halides. ______

(v) In secondary alkyl halides, the halogen atom is attached to a carbon, which is further attached to two

carbon atoms directly. ______

(vi) Primary, secondary and tertiary amines react with Grignard reagents in the same way. ______


(i) Tetraethyl lead can be prepared from alkyl halides.

________________________________________________________________________________

(ii) The nature of alkyl group changes when alkyl halide can be converted into Grignard's reagent.

________________________________________________________________________________

(iii) We get alkyl nitriles from Grignard's reagent.

________________________________________________________________________________

(iv) Primary alcohols are produced when ethene epoxide is reacted with Grignard's reagent.

________________________________________________________________________________

(v) Tertiary alkyl halides give SN1-mechanism.

________________________________________________________________________________

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(i) What are alkyl halides? Give their general formula and name two monohaloalkenes.

(ii) What are primary, secondary, and tertiary alkyl halides? Give examples of each.

(iii) What are necessary conditions to convert alcohols into alkyl halides by using halogen acids?

(iv) SOCl2 is the best reagent to get alkyl halides from alcohols. Which solvent is necessary to complete

the reaction?

(v) Convert ethyl alcohol to get alkyl halides respective halides by using PCl3 and PI5.

(vi) Which two factors are responsible for reactivity of alkyl halides as compared to the alkenes?

(vii) Define and give one example of each (a) nucleophile (b) leaving group.

(viii) Give the general pattern of reaction of SN2-mechanism. What is its rate expression? Give examples.


(i) Give the general pattern of reaction of SN1-mechanism. Why tertiary alkyl halides give this

mechanism?

(ii) What is a role of steric hindrance to decide about SN1 and SN2 mechanisms?

(iii) What is a role of stability of carbonium ions for determining SN1 or SN2 mechanism?

(iv) How do you compare SN1 and SN2 mechanisms?

(v) What are elimination reactions? Give examples of E1 and E2.

(vi) How tetraethyl lead can be prepared from alkyl halides?

(vii) How the nature of alkyl group changes when alkyl halide can be converted into Grignard's reagent?

(viii) Why dry ether is necessary for the preparation of Grignard's reagent?


(i) How do we get alkyl nitriles from Grignard's reagent?

(ii) Give the mechanism for the addition of Grignard's reagent at CO2 to give carboxylic acids.

(iii) Give the mechanism for the reaction of formaldehyde with ethyl magnesium bromide.

(iv) What is mechanism for the reaction of Grignard's reagent with acetaldehyde?

(v) Show the mechanism for the reaction of acetone with Grignard's reagent.

(vi) How primary alcohols are produced when ethene epoxide is reacted with Grignard's reagent?


Q: 8 Attempt SIX questions. (6 x 4 = 24)

1. Elaborate the nomenclature of alkyl halides with respect to IUPAC.

2. How the alkyl halides are prepared?

3. What do you know about reactivity of alkyl halides?

4. Explain nucleophilic substitution reactions of alkyl halides.

5. Explain the β-elimination reactions of alkyl halides.

6. Give the reactions of Grignard's reagent with:

(a) Cyanogen chloride

(b) Alcohols

(c) HCHO

(d) CH3CHO

(e) Epoxide

(f) CH3COCH3



A. (a) Give the following tests for the acidic radical Iodide I1-.

(i) Wet Test


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(b) Give the following tests for the basic radicals Strontium Sr2+ and Calcuim Ca2+.

(i) Wet Test


B. Write down the procedure for the confirmatory tests of carboxylic group in organic compounds..


(i) What is a Magneson’s reagent?

(ii) Are all basic radicals metallic?

(iii) What is Nessler’s reagent?

(iv) What is potash alum?

(v) Name three coloured salts of alkali metals.

(vi) Name two alkali metals.

(vii) What is glauber’s salt?

(viii) What is meant by baking soda and washing soda?

(ix) Write down the formulas of following:

(a) Pot. Pyroantimonate _____________________

(b) Sodium Cobaltinitrite _____________________

(c) Picric Acid _____________________

(d) Tartaric Acid _____________________

(x) Why do we not detect C and H in organic compounds?

(xi) In what respect, does the reaction between organic compounds differ from that between

inorganic compounds?

(xii) Two solutions are given:

(a) NaCl

(b) Chloroform

Which of solutions will give a white ppt. with silver nitrate (AgNO3) solution?

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CHAPTER 11: ALCOHOLS, PHENOLS AND ETHERS



Scheme (15)




(i) Which one of the following is termed as benzyl alcohol?

(a) C6H5OH (b) C6H5CH(OH)2 (c) C6H5CH2OH (d) None

(ii) Hydrolytic conversion of sucrose into glucose and fructose is known as:

(a) Induction (b) Inversion (c) Insertion (d) Inhibition.

(iii) Alcoholic beverages are made of:

(a) Ethanol (b) Acetic acid (c) Formic acid (d) None of these

(iv) Denatured Alcohol is known as:

(a) Absolute alcohol (b) Wood spirit (c) Methylated spirit (d) Vinegar

(v) Which one is methoxy methane?

(a) Olefins (b) Paraffins (c) Dimethyl ether (d) Dimethyl ketone

(vi) Ethyl alcohol is produced on commercial scale by the biological break down of:

(a) Starch (b) Minerals (c) Cellulose (d) None of these


(i) Primary, secondary and tertiary alcohols can be identified by ____________ test.

(ii) Williamson’s synthesis is used to prepare ____________.

(iii) Carbolic acid is another name of ____________.

(iv) Oxidation of ____________ alcohols give ketones.

(v) Alcohols and ____________ react to produce esters.

(vi) Ketones on reduction give ____________ alcohols.


(i) Ethers do not show hydrogen bonding. ______

(ii) Alcohols are more acidic than phenols. ______

(iii) Methanol and ethanol can be distinguished by iodoform test. ______

(iv) Only 14% ethyl alcohol can be prepared by fermentation. ______

(v) Methanol is also called wood spirit. ______

(vi) Alcohols are more basic than ethers. ______


(i) Ethers are less reactive than alcohols.

________________________________________________________________________________

(ii) Ethyl alcohol is a liquid while ethyl chloride is a gas.

________________________________________________________________________________

(iii) Ethanol gives different products with concentrated H2SO4 under different conditions.

________________________________________________________________________________

(iv) phenol is acidic but alcohol is not.

________________________________________________________________________________

(v) Ethers belong to an inert class of organic compounds.

________________________________________________________________________________

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(i) What is similarity of water with alcohols, phenols and ethers?

(ii) Define and give examples of monohydric, dihydric and trihydric alcohols.

(iii) How primary, secondary and tertiary alcohols are different from each other in structures?

(iv) How water gas is converted into methyl alcohol on commercial scale?

(v) What is fermentation of alcohols? Give the necessary conditions for fermentation.

(vi) What is the raw material for the manufacture of ethyl alcohol on commercial scale?

(vii) Absolute alcohol cannot be prepared by fermentation process. Why?

(viii) What is rectified spirit, commercial alcohol and absolute alcohol?

(ix) What do you mean by denaturing of alcohol?

(x) Ethyl alcohol is a liquid while ethyl chloride is a gas. Give reason.

(xi) Why ethanol has higher boiling point than diethyl ether?


(i) Why alcohols are miscible with water?

(ii) What is esterification? Give the necessary conditions for this reaction.

(iii) How the strong oxidizing agents affect the primary and secondary alcohols?

(iv) Ethanol gives different products with concentrated H2SO4 under different conditions. Justify.

(v) What are dehydrogenation products of primary and secondary alcohols in the presence of copper?

(vi) What is Lucas test, which is used to distinguish between the primary, secondary and tertiary

alcohols?

(vii) How haloform reaction can be used to distinguish between certain types of alcohols?

(viii) How iodoform can be used to distinguish between methyl alcohol and ethyl alcohol?

(ix) Give the uses of ethyl alcohol.

(x) Give the uses of methyl alcohol.


(i) What are three important dihydroxyl benzenes? Give their IUPAC names and old names.

(ii) How chlorobenzene is converted into phenol?

(iii) How benzene sulphonic acid can be converted into phenol?

(iv) Give physical properties of phenol.

(v) Why phenol is acidic but alcohol is not?

(vi) How the resonance structure of phenoxide ion make phenol acidic?

(vii) How phenol can be converted into benzene?

(viii) What is the reaction of bromine water with phenol? How it is used to distinguish between phenol and

alcohol?

(ix) How conc. HNO3 reacts with phenol to give picric acid?

(x) What important polymer is produced by the reaction of phenols with methanol?


(i) Give the uses of phenol.

(ii) How do you phenol and ethyl alcohol?

(iii) What is Williamson's synthesis of ethers?

(iv) How silver oxide reacts with alkyl halides to give ethers?

(v) How do acids reacts with ethers to give oxonium ions?

(vi) Give the mechanism of the reaction of halogen acids with ethers.

(vii) Give the uses of diethyl ether

(viii) What are mixed ethers? Give examples.

(ix) Ethers belong to an inert class of organic compounds. Discuss.

(x) Ethers are less reactive than alcohols. Justify.

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1. Define alcohols and give their nomenclature.

2. Fill the following table:

ALCOHOLS

COMMON NAME FORMULA IUPAC NAME

Methyl alcohol

Ethyl alcohol

Propyl alcohol

Isopropyl alcohol

3. (a) How alcohols are industrially prepared from molasses and starch?

(b) What do you know about denaturing of alcohol?

4. Give the following reactions of alcohols.

NAME REACTION

(a) Reactions in which C-O bond is broken

(b) Reactions with Phosphorous Halides

(c) Dehydration

5. Define phenols. Prepare it from chlorobenzene. Also, name this method of preparation.

6. Justify the acidic behavior of phenol.

7. Give the following reactions of phenols.

NAME REACTION

(a) Ester Formation

(b) Sulphonation

(c) Reaction with formaldehyde

8. Define ethers. Fill the following table:

ETHERS

FORMULA COMMON NAME IUPAC NAME

CH3OCH3

CH3OC2H5

C2H5OC2H5

C2H5OCH2-CH2-CH3

CH3OC6H5

9. Elaborate the chemical reactivity of ethers.

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A. (a) Give the following tests for the acidic radical Nitrate NO31-.

(i) Wet Test

(ii) Dry Test

(b) Give the following tests for the basic radicals Magnesium Mg2+ and Sodium Na1+.

(i) Filter Ash Test

(ii) Flame Test

B. Write down the procedure for the confirmatory tests of aldehydic group in organic compounds.


(i) What is Lassigne’s solution?

(ii) If the sodium extract is not colourless, what does it indicate?

(iii) Why is the sodium extract usually alkaline?

(iv) Can potassium metal be used in the Lassigne’s test?

(v) Why is sodium metal preserved in kerosene oil?

(vi) Before testing for halogens, it is necessary to acidify the extract with conc. HNO3 and then to

boil it. Why?

(vii) Why chlorine water is added in layer test?

(viii) Why H2SO4 is added in “nitrogen test”?

(ix) Write down the chemical equations for the detection of following compounds:

COMPOUND CHEMICAL EQUATION

C

H

N

S

X (Halogens)

(x) Name the compound formed in nitrogen test with prussion blue colouration.

(xi) Which complex compound is formed in sulphur test?

(xii) What is a functional group?

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CHAPTER 12: ALDEHYDES AND KETONES



Scheme (11)




(i) The reaction of acetaldehyde with conc. H2SO4 at room temperature gives:

(a) Paraldehyde (b) Metaldehyde (c) A mixture of a & b (d) None

(ii) Dry distillation of calcium format yields:

(a) Ether (b) Formaldehyde (c) Acetic acid (d) None of these

(iii) Aldehydes can be distinguished from ketones by the use of:

(a) Bayer’s test (b) Grignard reagent(c) Iodoform test (d) Fehling solution

(iv) If formaldehyde and KOH are heated them we get:

(a) Acetylene (b) Methane (c) Methyl alcohol (d) Ethyl formate.

(v) Which of the following compounds gives a ketone with Grignard's reagent?

(a) Formaldehyde (b) Ethanenitrile (c) Ethyl alcohol (d) Methyl iodide.

(vi) An aldehyde on oxidation gives:

(a) An alcohol (b) An acid (c) A ketone (d) An ether


(i) Aldehydes are the first oxidation products of ____________.

(ii) Formaldehyde reacts with ____________ to give primary alcohol.

(iii) Formaldehyde gives ____________ test with Tollen’s reagent.

(iv) Ketones are the first oxidation products of ____________.

(v) The oxidation of an ____________ always gives a carboxylic acid.

(vi) Aldehydes are strong ____________ agents.


(i) Ketones combine with alcohols in the silvering of mirrors. ______

(ii) 40% aqueous solution of formaldehyde is called formalin. ______

(iii) Acetaldehyde undergoes Cannizarro’s reaction. ______

(iv) Aldol condensation reaction in given by only those aldehydes and ketones which contain an

α-hydrogen atom. ______

(v) Cannizarro’s reaction is given by only those aldehydes containing no α-hydrogen atom. ______

(vi) Acetone reacts with sodium bisulphite to give a yellow crystalline product. ______


(i) Aldehydes with no α-hydrogen give Cannizarro's reaction.

________________________________________________________________________________

(ii) HCN is not directly used in aldehydes and ketones.

________________________________________________________________________________

(iii) The addition product of an aldehyde and a ketone with NaHSO3 is very useful reaction.

________________________________________________________________________________

(iv) Benedict's solution reacts with aldehydes to give red ppt.

________________________________________________________________________________

(v) 2, 4 Dinitrophenylhydrazine can be used to have a distinction between aldehydes and ketones from

other organic compounds.

________________________________________________________________________________

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(i) How aldehydes and ketones occur in nature?

(ii) What are those factors, which make aldehydes more reactive than ketones?

(iii) How formalin is prepared on the commercial scale by methyl alcohol?

(iv) How acetaldehyde is prepared from ethyl alcohol in the laboratory?

(v) Which product is obtained by heating calcium acetate?

(vi) What type of polarity is present in carbonyl group?

(vii) How acids and bases acting as catalysts increase the reactivity of the aldehydes and ketone?

(viii) Addition of HCN on aldehydes and ketones is a base catalyzed reaction. How?

(ix) HCN is not directly used in aldehydes and ketones. Give reasons.

(x) How α-hydroxyl acids are produced from aldehydes and ketones?

(xi) The addition product of an aldehyde and a ketone with NaHSO3 is very useful reaction. Justify it.

(xii) Why NaHSO3 does not give the reaction with 2-pentanone?

(xiii) How acetaldehyde in the presence of strong base give 2-butenal?


(i) For aldol condensation, the presence of -hydrogen is must in aldehydes and ketones. Give reasons.

(ii) Why the aldehydes with no α-hydrogen give Cannizarro's reaction?

(iii) Justify that Cannizarro reaction is self oxidation-reduction reaction.

(iv) What products are obtained when benzaldehyde reacts with 50% KOH?

(v) How iodoform is prepared from ethanol and acetaldehyde?

(vi) Only methyl ketones are able to give haloform reactions but other ketones do not. Give reasons.

(vii) With the haloform reaction, we can decrease the number of carbon atoms in aldehydes and ketones.

Give reasons.

(viii) How acetophenone can be converted into sodium salts of benzoic acid?

(ix) Polymerization of formaldehyde gives six membered cyclic compound. Justify it.

(x) Justify that carbonyl group of acetaldehyde is no more there its polymer i.e. paraldehyde.

(xi) NH3 reacts with aldehydes and ketones to give cyanohydrins and then hydrazones. Justify it.

(xii) The reaction of hydroxylamine, hydrazine and phenyl hydrazine with aldehydes and ketones are just

like the reaction of NH3 with aldehydes and ketones. Justify it.


(i) NH3 reacts with formaldehyde in different manner from other aldehydes and ketones. Justify.

(ii) 2, 4 Dinitrophenylhydrazine can be used to have a distinction between aldehydes and ketones from

other organic compounds. Justify.

(iii) How the reduction process of aldehydes and ketones gives alcohols?

(iv) How aldehydes react with alcohols to give hemiacetals and acetals?

(v) Which are those weak oxidizing agents, which can oxidize aldehydes but not the ketones?

(vi) Tollen's test is also called silver mirror test. Justify it.

(vii) Fehling's solution reacts with aldehydes to give red ppt. Justify it.

(viii) Benedict's solution reacts with aldehydes to give red ppt. Justify it.

(ix) Give the uses of formaldehyde.

(x) Give the uses of acetaldehyde.

(xi) How would you compare formaldehyde and acetaldehyde?

(xii) How would you compare aldehydes and ketones?



1. Elaborate the nomenclature of aldehydes and ketones.

2. Explain the Cannizarro’s Reaction.

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3. Explain the methods of preparation for

(a) Formaldehyde (Formalin)

(b) Acetaldehyde

4. Perform following reactions:

(a) Addition of Hydrogen Cyanide

(b) Aldol Condensation

(c) Acid-Catalyzed Addition Reactions

(d) Reaction of Ammonia Derivatives with Phenylhydrazine

(e) Reaction of Ammonia Derivatives with 2, 4 Dinitrophenylhydrazine

(f) Reaction of Ammonia Derivatives with Hydrazine

5. Elaborate the oxidation reactions of ketones and aldehydes.

6. Give the following tests:

(a) Silver Mirror Test

(b) Fehling’s Solution Test

(c) Sodium Nitroprusside Test

(d) Benedict’s Solution Test

(e) 2, 4 DNPH Test

(f) Sodium Bisulphite Test



A. (a) Give the following tests for the acidic radical Acetate CH3COO1-.

(i) Wet Test

(ii) Dry Test

(b) Give the following tests for the basic radicals Potassium K1+ and Ammonium NH41+.

(i) Filter Ash Test

(ii) Flame Test

B. Write down the procedure for the detection of C and H in organic compounds.


(i) What is Fehling’s solution?

(ii) What is the red ppt. obtained in Fehling’s solution test?

(iii) What is Tollen’s reagent?

(iv) What is silver mirror test?

(v) What is esterification?

(vi) What is Schiff’s reagent?

(vii) What is Liberman’s reaction and for which group it is used?

(viii) Carboxylic acids liberate CO2 from NaHCO3 solution. Phenol is also acidic but does not liberate

CO2 from NaHCO3 solution. Explain why?

(ix) What is soot? Generally aliphatic substances burn without soot but aromatic substances burn

with soot. Why?

(x) Name an organic compound, which does not contain hydrogen.

(xi) What types of reactions do the saturated and unsaturated compounds give?

(xii) How would you differentiate between saturated and unsaturated compounds?

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CHAPTER 13: CARBOXYLIC ACIDS



Scheme (5)

Weightage = 4% MCQ’s = 1 Short Questions = - Extensive Question = 1(Theory)



(i) Which of the following is not a primary amine?

(a) Cyclohexylamine (b) 3 – hexylamine (c) 1 – Butylamine (d) Diethylamine (ii) Which class of compound is commonly used for the artificial flavouring in jams?

(a) Aldehyde (b) Ester (c) Carboxylic acid (d) Ketones (iii) The conversion of acetic acid to methane is an example of:

(a) Hydration (b) Dehydration (c) Decarboxylation (d) Oxidation (iv) The solution of which acid is used for seasoning of food?

(a) Formic acid (b) Benzoic acid (c) Acetic acid (d) Butanoic acid (v) Carboxylic ion is represented by how many resonating structure?

(a) 3 (b) 2 (c) 1 (d) 4 (vi) Which one is more acidic?

(a) HCOOH (b) CH3COOH (c) C2H4 – COOH (d) C2H7 – COOH


(i) A peptide having a molecular mass more than 10000 is called____________.

(ii) Formula of malonic acid is ____________.

(iii) Acetic acid on heating with ____________ produces acetic anhydride.

(iv) Pure acetic acid is called ____________.

(v) Proline is a ____________ amino acid.

(vi) Formula of alanine is____________.


(i) Acetic acid exists as a dimer in benzene. ______

(ii) First three aliphatic acids have fruity smells. ______

(iii) Carboxylic acids on reduction with LiAlH4 produce alkenes. ______

(iv) Acetic acid on dehydration produces CO and H2. ______

(v) Sodium formate on heating with soda lime produces NaHCO3 and hydrogen. ______

(vi) Amino acids exist as Zwitterion. ______


(i) The boiling point of aliphatic carboxylic acid is relatively high.

________________________________________________________________________________

(ii) α-amino acid can be converted into α-hydroxyl acids.

________________________________________________________________________________

(iii) Carboxylic acids are converted into α-amino acids.

________________________________________________________________________________

(iv) Acetic acid is prepared on the commercial scale by acethylene.

________________________________________________________________________________

(v) The hydrolysis of nitriles give carboxylic acids.

________________________________________________________________________________

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(i) What are carboxylic acids? Give their general formula.

(ii) How two functional groups create one functional group in carboxylic acids?

(iii) Name at least five dicarboxylic acids and give their formulas.

(iv) Write the formulas for valeric acid, caproic acid and caprylic acid.

(v) What are hydroxyl acids? Give four examples of hydroxyl acid i.e. two from open chain and two from

closed chain.

(vi) What are aromatic carboxylic acids?

(vii) What are fatty acids?

(viii) How the hydrolysis of nitriles give carboxylic acids?

(ix) How ethanol is converted into CH3COOH?

(x) What are dimers of carboxylic acids? Give examples.


(i) Give two reactions of carboxylic acids which show their acidic nature.

(ii) Give mechanism for reaction of carboxylic acids with SOCl2 to give acid chlorides.

(iii) Give the mechanism for esterifcation of carboxylic acids.

(iv) What are acid anhydrides? How are they produced?

(v) How would you covert CH3COOH into CH3CONH2?

(vi) How acetic acid is prepared on the commercial scale by acethylene?

(vii) Why the boiling point of aliphatic carboxylic acid is relatively high?

(viii) What are amino acids? What are essential and non-essential amino acids?

(ix) Give an example of each (a) α-amino acid (b) β-amino acid (c) γ-amino acid.

(x) What is Zwitterion?


(i) What are neutral amino acids? Give two examples.

(ii) What are basic amino acids? Give two examples.

(iii) What are acidic amino acids? Give two examples.

(iv) How carboxylic acids are converted into α-amino acids?

(v) What is Strecker's synthesis?

(vi) How α-amino acid can be converted into α-hydroxyl acids?

(vii) What is ninhydrin test?

(viii) What are peptides and peptide linkages?

(ix) What is polypeptide?

(x) How do you differentiate between peptide and polypeptide?



1. Give the laboratory methods for the preparation of acetic acid.

2. Explain the nomenclature of amino acids. Fill the following table.

NAME NATURE ABBREVIATION STRUCTURAL FORMULA

Glycine

Alanine

Valine

Proline

Aspartic Acid

Glutamic Acid

Lysine

Histidine

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3. How amino acids are synthesized? Also, give its reactions.

4. Give the reactions involving following of carboxylic acids.

(a) H atom

(b) Carboxyl Group (-COOH)


Q: 9 Pen down the answers of following questions. (5 x 3 = 15)

A. Give the following tests for the acidic radical Oxalate C2O42-.


(ii) Dry Test

B. Fill the following table for dry tests of basic radicals.

COLOUR OF THE SALT

S.No OBSERVATIONS INTERFERENCES

(i) White or Colourless

(ii) Blue or Green

(iii) Light Green

(iv) Yellow

(v) Light Pink or Blue

(vi) Reddish Pink

(vii) Bright Green

(viii) Very Dark Green

C. Fill the following table for dry tests of basic radicals.

STATE AND SMELL OF THE SALT


(i) Crystalline and Heavy

(ii) Amorphous and Light

(iii) Ammonical Smell

(iv) Vinegar-like Smell

(v) Rotten Egg Smell

D. Write down the procedure for performance of Lassigne’s Test for detection of N in organic compounds.

E. Write brief answers of following questions:

(i) Which carbonates form osazones?

(ii) Differentiate between aspirin and acetyl salicylic acid.

(iii) Name the chemicals used for recrystallization of aspirin.

(iv) Why hot water should not be used as recrystallizing solvent?

(v) Why aspirin is in taken?

(vi) What is meant by synthesis?

(vii) How will you ascertain that a given organic compound is pure or not?

(viii) Write down the chemical equation for the preparation of iodoform.

(ix) Why is the sodium acetate used in the preparation of glucosazone?

(x) Write down the chemical equation for the preparation of glucosazone.

(xi) Write down the molecular formula of glucose.

(xii) What will happen when cuprammonium sulphate is heated?

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CHAPTER 14: MACROMOLECULES



Scheme (5)




(i) Saponification of coconut oil yields glycerol and:

(a) Palmitic acid (b) Sodium palmitate (c) Oleic acid (d) Satiric acid (ii) The protein responsible for the clotting of blood is:

(a) Fibrinogen (b) Albumin (c) Globulins (d) None of the above (iii) Starch is a polymer of:

(a) Glucose (b) Fructose (c) Lactose (d) Maltose (iv) The trade name of polytetrafluoroethylene (PTFE) plastic is:

(a) Dacron (b) Teflon (c) Saran (d) Nylon (v) Monosaccharide and disaccharides are solid, sweet in taste and soluble in:

(a) C6H6 (b) H2O (c) CHCl3 (d) Acetone (vi) A balanced diet must contain at least:

(a) Two nutrients (b) Four nutrients (c) Six nutrients (d) Three nutrients


(i) Macromolecules are built up from small units called ____________.

(ii) Nylon is a polyamide and terylene is a ____________.

(iii) PVC is a ____________ plastic.

(iv) Addition of plasticizer ____________ the flexibility of the polymer.

(v) Glucose is stored as ____________ in the liver.

(vi) Protein after digestion changes to ____________.


(i) Nylon 6, 6 and terylene are condensation polymers. ______

(ii) The disposal of plastics does not cause any pollution problem. ______

(iii) Fructose is a polysaccharide carbohydrate. ______

(iv) Nucleic acids are biological catalysts. ______

(v) Enzymes are the compounds containing C, H and O only. ______

(vi) Activity of enzyme varies with temperature and pH. ______


(i) The degree of polymerization helps to determine the molar mass of the polymer.

________________________________________________________________________________

(ii) The polymers are classified on the basis of heat effects.

________________________________________________________________________________

(iii) Disaccharides are produced from the monosaccharides.

________________________________________________________________________________

(iv) The fats and oils are sources of other substances.

________________________________________________________________________________

(v) Carbohydrates are made up of H, C and O.

________________________________________________________________________________

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(i) What are macromolecules? Give five examples.

(ii) What are polymers? What is their classification?

(iii) What is the classification of polymers by keeping in view their structural aspects?

(iv) What is the degree of polymerization? Give two examples.

(v) How the degree of polymerization helps to determine the molar mass of the polymer?

(vi) Classify the polymers on the basis of varieties of monomers.

(vii) How the polymers are classified on the basis of heat effects?

(viii) How do you classify the process of polymerization on the basis of reaction mechanism?

(ix) Give the brief description of free radical addition polymerization for the formation of polythene.

(x) What is condensation polymerization? Give the reaction for formation of polyesters.


(i) What are polyamides? Give the formation of nylon 6, 6.

(ii) How PVC is prepared? Give its uses.

(iii) How acrilon is prepared? Give its uses.

(iv) How polystyrene is prepared? Give its uses.

(v) What are acrylic resins? Give their uses.

(vi) What are epoxy resins? Give their uses.

(vii) How do you define biopolymers? Give the major classes of such polymers.

(viii) What are carbohydrates? Why are they called so?

(ix) Give the classification of carbohydrates and give an example of each.

(x) What are aldohexose and aldoketoses? Give examples.


(i) How do you justify the cyclic structure of glucose from its open chain structure?

(ii) How do you justify the cyclic structure of fructose from its open chain structure?

(iii) What are disaccharides? How are they produced from the monosaccharides?

(iv) What is lactose? To which class does it belong?

(v) What are polysaccharides? Give examples.

(vi) Where is starch found? How is its structure made up?

(vii) Where is cellulose found? What is its structure?

(viii) What is glycogen? Give its structure and properties.

(ix) What are proteins? Which elements are present in them?

(x) How proteins are classified?


(i) What are simple proteins? Give their examples.

(ii) What are compound or conjugated proteins?

(iii) What are derived proteins?

(iv) How do you classify the proteins according to their structure?

(v) What information do we get from secondary structure of proteins?

(vi) What do you mean by tertiary structure of proteins?

(vii) What do you mean by denaturalization of proteins?

(viii) Give the brief summary of importance of proteins.

(ix) What are lipids? What are their types?

(x) What are the characteristics of the lipids?


(i) How do you justify that the fats and oils are sources of other substances?

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(ii) What are the major sources of fats and oils?

(iii) What are simple glycerides and mixed glycerides?

(iv) How do you classify the fats and oils on the basis of phase?

(v) What do you mean by hydrolysis of fats and oils?

(vi) What is saponification?

(vii) Classify the lipids into various types.

(viii) What do you mean by hardening of oils?

(ix) What is saponification number?

(x) What do you mean by rancidity of oils and fats?


(i) What do you mean by iodine number?

(ii) What is the acid number of the fats?

(iii) What are steroids? Give examples.

(iv) What are enzymes? Give their types.

(v) What are those factors, which affect the enzyme activity?

(vi) What is the importance of enzymes?

(vii) Give types of nucleic acids. How are they related with proteins?

(viii) What are two important bases, which make up DNA and RNA?

(ix) What are nucleotides?

(x) What is the difference between DNA and RNA?



1. Define polymers. Explain the following types of polymers.

(a) Terpolymer

(b) Homopolymer

2. Briefly describe following synthetic polymers.

(a) PVC

(b) PVA

(c) Polyester Resins

(d) Epoxy Resins

3. Explain polysaccharides. Discuss important polysaccharides.

4. What is meant by lipids? Give the physical and chemical properties of lipids.



A. Give the following tests for the acidic radical Sulphate SO42-.

(i) Wet Test

(ii) Dry Test

B. Define charcoal cavity test. Fill the following table for dry tests of basic radicals.

CHARCOAL CAVITY TEST


(i) The substance deflagrates

(ii) Bright white bead

(iii) White bead which marks paper

(iv) Yellow incrustation when hot, dirty white when cold

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(v) Orange-red incrustation whenhot, yellow when cold

(vi) Red scales of metal

(vii) Residue yellow when hot, white when cold.

(viii) Residue reddish-brown, yellow on fusion with solid Na2S2O3

(ix) Residue white

C. What is cobalt nitrate test? Fill the following table for dry tests of basic radicals.

COBALT NITRATE TEST


(i) Pink

(ii) Green

(iii) Blue

(iv) Dirty-Bluish Green

D. Write down the procedure for performance of Lassigne’s Test for detection of halogens (X) in organic

compounds.

E. Write brief answers of following questions:

(i) Can we pass ammonia gas in copper sulphate in place of adding liquor ammonia?

(ii) What is the effect of air on copper amine complex?

(iii) Give the equation for the preparation of tetramine cupric sulphate monohydrate.

(iv) What is gravimetric analysis? What is meant by ‘digestion’?

(v) Why is the precipitate digested?

(vi) How many filters can be used for filtration?

(vii) What is desiccating agent?

(viii) What are the common desiccating agents used in desiccator?

(ix) What happens if the filter paper is charred at a high temperature?

(x) What is tarred crucible? Define decrepitation.

(xi) Why should not hot objects be weighed?

(xii) What is the difference between a hygroscopic and a deliquescent substance?

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CHAPTER 15: COMMON CHEMICAL INDUSTRIES IN PAKISTAN



Scheme (7)




(i) Asbestos is a:

(a) Mineral fiber (b) Animal fiber (c) Vegetable fiber (d) None of these (ii) The percentage of nitrogen in ammonium sulphate is:

(a) 32 – 33.5 (b) 50 – 55 (c) 80 – 82 (d) 20 – 25 (iii) The industrial abbreviation of Tricalcium aluminate is:

(a) C2S (b) C3S (c) C3A (d) C4AP (iv) Manufacturing of super phosphate fertilizer involves:

(a) Six steps (b) Five steps (c) Four steps (d) Three steps (v) There is only one nitrogen fertilizer which is used as liquid is:

(a) NH4NO3 (b) NH4Cl (c) NH3 (d) (NH4)2HPO4 (vi) Phosphorus helps in the growth of:

(a) Root (b) Leave (c) Stem (d) Seed


(i) Fertilizers enhance the natural ____________ of the soil.

(ii) Cement was first introduced by an English mason ____________.

(iii) Phosphorus is required to stimulate ____________ of plant.

(iv) In Pakistan, bleaching of pulp is carried out with ____________.

(v) Cement is generally manufactured using ____________ process.

(vi) Lignin is an ____________polymer and causes paper to become brittle.


(i) Potassium fertilizers are especially used for tobacco and corn. ______

(ii) Ammonia is used in gaseous state while all other fertilizers are used in the solid form. ______

(iii) The total production of cement in Pakistan is 56,30,100 metric tons/annum. ______

(iv) Lignin is an inorganic binder. ______

(v) Urea contains 90% nitrogen. ______

(vi) The temperature of the digester in paper industry should be around 160-180 °C. ______

Q: 4 Pen down definitions of following. (5 x 1 = 5)

(i) Macronutrients

________________________________________________________________________________

(ii) Fertilizer

________________________________________________________________________________

(iii) Urea Fertilizer

________________________________________________________________________________

(iv) Cement

________________________________________________________________________________

(v) Paper

________________________________________________________________________________

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(i) Why is industry necessary for a country?

(ii) What is a need for a fertilizer?

(iii) What are micronutrients? Give their names.

(iv) What are macronutrients? Give their names.

(v) Give the important properties of fertilizer.

(vi) Give the names and formulas of important nitrogenous fertilizers.

(vii) Why is nitrogen important for plants?

(viii) How NH3 is given to plants?

(ix) What are the important steps for the manufacture of urea?

(x) What do you mean by prilling of urea?

(xi) What are the properties of ammonium nitrate as a fertilizer?

(xii) What are the types of phosphorus fertilizers?


(i) What is the importance of phosphorus for the plants?

(ii) What is di-ammonium hydrogen phosphate? Give its uses.

(iii) What is the importance of potassium fertilizer?

(iv) How potassium nitrate is prepared? Give its composition.

(v) What is the position of fertilizer industry in Pakistan?

(vi) What is historical background of Portland cement?

(vii) How do you define cement? Give the essential constituents of cement.

(viii) Mention three important raw materials for the manufacture of cement.

(ix) How do you compare the wet and dry method for the manufacture of cement and on what grounds

one of them is chosen?

(x) What are the five steps in the manufacture of Portland cement?

(xi) What is the role of rotary kiln in the cement manufacture?

(xii) Give different zones in the rotary kiln and their temperature ranges.


(i) What are clinkers? How are the clinker converted into the cement at the final stage?

(ii) What do you mean by setting of cement?

(iii) Mention the cement industry in Pakistan.

(iv) Define paper. Give important raw materials for the manufacture of paper.

(v) What is N.S.S.C. method for paper manufacture? What physical operations are performed?

(vi) What do you mean by dry cleaning in paper manufacture?

(vii) What process is carried out during digestion in paper manufacture?

(viii) What is lignin?

(ix) What are commonly used bleaching agents in paper manufacture?

(x) What are the requirements to get high brightness of pulp during the paper manufacture?

(xi) What are the major components of paper machine?

(xii) Mention paper industry in Pakistan.



1. How the paper is manufactured in the industry?

2. Explain the process by which cement is manufactured in Pakistan industries.

3. Explain nitrogenous fertilizers with examples.

4. Define following fertilizers:

(a) Diammonium Phosphate

(b) Potassium Nitrate

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A. Give the following tests for the acidic radical Phosphate PO43-.

(i) Wet Test


B. Define Borax bead test. Fill the following table for dry tests of basic radicals.

BORAX BEAD TEST

S.No OXIDIZING FLAME REDUCING FLAME METAL

(i) Green when Hot Blue when Cold

Colourless when Hot Opaque Red when Cold

(ii) Yellow, Hot and Cold Green, Hot and Cold

(iii) Green, Hot and Cold Green, Hot and Cold

(iv) Violet, Hot and Cold Colourless, Hot and Cold

(v) Blue, Hot and Cold Colourless, Hot and Cold

(vi) Reddish-Brown when Cold Grey when Cold

C. What is flame test? Fill the following table for dry tests of basic radicals.

FLAME TEST


(i) Green or blue flame

(ii) Yellowish-Green Flame

(iii) Crimson Flame

(iv) Brick-Red Flame

(v) Violet Flame

(vi) Persistent Golden-Yellow Flame

D. Write down the procedure for performance of Lassigne’s Test for detection of sulphur in organic

compounds.

E. Fill this table for basic radicals.

GROUP BASIC RADICALS REAGENT REASON FOR

USING REAGENT

I

II

III

IV

V

VI

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CHAPTER 16: ENVIRONMENTAL CHEMISTRY



Scheme (7)




(i) The thickness of ozone layer is:

(a) 25 to 50 km (b) 25 to 28 km (c) 3 km only (d) 1 km only (ii) In the purification of portable water, the coagulant used is:

(a) Alum (b) Nickel Sulphate (c) Copper sulphate (d) Barium sulphate (iii) The techniques used to kill pathogens present in drinking water are:

(a) Chlorination (b) Ozone (c) UV irradiation (d) All of these (iv) Clean rain is:

(a) Basic (b) Slightly basic (c) Slightly acidic (d) All of these (v) The main pollutant of leather tanneries in the waste water is_______:

(a) Chromium III (b) Chromium II (c) Sodium (d) Copper (vi) Acid rain is due to increase ion atmospheric concentration of:

(a) Ozone and dust (b) CO2 and CO (c) SO3 and CO (d) SO2 and NO2


(i) ____________ is frequently used to disinfect water.

(ii) Incineration is not a clean process because it produces air pollution and toxic ____________.

(iii) The substances which can directly kill the unwanted organisms are called ____________.

(iv) Only ____________ of the total earth’s water resources are available as fresh water.

(v) The evaluated concentration of ____________ is harmful for fish as it clogs the gills thus causing

suffocation.

(vi) The pH of acid rain is ____________.


(i) Half of the mass of the atmosphere is concentrated in lower 10 km. ______

(ii) The oceans cover approximately 71 percent of the earth. ______

(iii) The volcanoes produce 55% of SO2. ______

(iv) The heavy metals have a safe limit where they are not toxic. ______

(v) Ozone is produced in the polar regions by the photochemical reaction of oxygen. ______

(vi) The reducing smog is due to the presence of nitric oxide. ______


(i) Atmosphere behaves with different type of radiations from the sun.

________________________________________________________________________________

(ii) Ozone act as a pollutant.

________________________________________________________________________________

(iii) Chlorinated hydrocarbons are dangerous for health.

________________________________________________________________________________

(iv) Suspended impurities can be coagulated with water.

________________________________________________________________________________

(v) Pesticides contaminate the soil.

________________________________________________________________________________

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(i) What is the environmental chemistry and which aspects do we study in this branch?

(ii) What are the components of the environment?

(iii) What is the composition of atmosphere and its thickness?

(iv) How atmosphere behaves with different type of radiations from the sun?

(v) Mention the utilities of the gases of atmosphere.

(vi) How water in the hydrosphere is distributed in different parts?

(vii) What is lithosphere? Give its composition.

(viii) What is biosphere and ecosphere?

(ix) What are environmental pollutants and what is reason for the environmental pollution?

(x) What are the primary air pollutants?

(xi) What are the secondary air pollutants?

(xii) What are the main sources of CO?

(xiii) How CO is produced in different reactions?

(xiv) How do you discuss the poisoning of CO?

(xv) What happen to the human body, when it is exposed to CO?

(xvi) Which oxides of nitrogen are air pollutants? What are their sources?

(xvii) What are the main sources of SO2, as air pollutant?

(xviii) What are aerosols? What type of illness do they cause?

(xix) What are the sources of methane as air pollutant?


(i) What is the acid rain or acid deposition?

(ii) How the acid rain produces pollution problem?

(iii) What is the effect of acid rain on the earth?

(iv) What is reducing smog? Give its sources.

(v) What is photochemical smog? Give its properties.

(vi) What is the overall result of photochemical smog?

(vii) What are the conditions for the formation of smog?

(viii) What is the purpose of ozone and what is the ozone hole?

(ix) How does ozone act as a pollutant?

(x) How the concentration of ozone varies on the earth?

(xi) How does ozone protect the earth from U.V. radiations?

(xii) How chlorofluorocarbons destroy the ozone layer? What is ozone layer depleting?

(xiii) What are the various sources, which contaminate water?

(xiv) How livestock wastes become reasonable for water pollution?

(xv) What is oil spillage?

(xvi) How water is polluted by petroleum?

(xvii) How the animal life is affected by hydrocarbons?

(xviii) What are detergents? What are their various types?

(xix) What are pesticides? Give their types.


(i) Which diseases have been eradicated by pesticides?

(ii) How pesticides contaminate the soil?

(iii) How the chlorinated hydrocarbons are dangerous for health?

(iv) What are the metal pollutants of industry?

(v) What is BOD and what is COD?

(vi) How COD is measured?

(vii) What are the stages of water treatments?

ALI RAZA KAMAL

ALI RAZA KAMAL

(viii) What do you mean by aeration of raw water?

(ix) How the suspended impurities can be coagulated with water?

(x) How can we do the chlorination of the water to purify it?

(xi) What are the harmful effects of chlorination of water?

(xii) What is the solid waste management?

(xiii) What are landfills and how do we choose the height of landfills?

(xiv) What is incineration of municipal solid waste?

(xv) What are the side effects of incineration?

(xvi) What is the recycling of the wastes?

(xvii) What is recycling of papers?

(xviii) What is the recycling of the plastics?



1. Explain the effects of acid rain and smog on our environment.

2. Write a detailed note on ozone depletion.

3. How the process of aeration and coagulation can purify water?

4. How the wastes are recycled



A. Write down the procedure for the preparation of solution for wet tests of acid radicals.

B. What is filter ash test? Fill the following table for dry tests of basic radicals.

FILTER ASH TEST


(i) Pink

(ii) Green

(iii) Blue

(iv) Dirty-Bluish Green

C. Define action of NaOH on basic radicals. Fill the following table after your observations.

ACTION OF NaOH


(i) Salt is soluble in H2O but no ppt. is formed with NaOH

(ii) NH3 gas is evolved

(iii) NH3 gas is evolved after the addition of Devarda’s alloy

(iv) H2 gas is evolved

(v) A ppt. is formed which is soluble in excess of NaOH solution with difficulty

(vi) A ppt. is formed. (Insoluble in excess of NaOH)

a. White ppt.

b. Blue ppt.

c. Pink ppt.

d. Brownish-Red ppt.

e. ppt. of solution colour

f. Black ppt.

g. ppt. becomes black on heating

h. White ppt. becomes brown on shaking

i. Greenish ppt. quickly darkens to bluish-black

ALI RAZA KAMAL

ALI RAZA KAMAL

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