Chemistry MCQs 2nd year 2nd Year Chemistry Notes

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Five Year Papers

1. On passing steam over red-hot coal we get __________.

(Water gas, Ethane, Carbonmonoxide)

2. ‘d’ and ‘f’ block elements are called __________.

(Heavy metals, Rare elements, Transition elements)

3. The correct formula of pyrosulphuric acid is __________.

(H2SO4, H2S2O7, H3S2O5)

4. Aqua regia is mixture of one part of __________ by volume and three parts of __________.

(H2SO4, H3PO4, HNO3, HCl)

5. Heavy hydrogen is also called __________.

(Proteum, Deuterium, Hydronium)

6. When boric acid (H3BO3) is heated of 140°C, it forms __________.

(Boric Acid, Pyroboric acid, Metaboric acid)

7. Photographic film is made of sheets of __________.

(Cellulose Acetate, P.V.A, Nylon)

8. C4H8 is a saturated hydrocarbon because it is __________.

(Cyclic, Open chain, Polymer)

9. n-Octane is __________ at room temperature.

(Gas, Liquid, Semi-solid)

10. The compound formed between an element A of group IIIA and an element B of group VIA has the formula __________.

(AB, A2, B3, A2B3)

11. The oxide formed by AI is __________.

(Acidic, Amphoteric, Basic)

12. Bakelite is a polymer of __________ and form aldehyde.

(Ethane, Methanol, Phenol)

13. The plastics, which can be heated only once, are known as __________ plastics.

(Perspex, Thermoplastic, Thermosetting)

14. The deficiency of __________ in the human body is the cause of diabetes.

(Insulin, Alamin, Ptyalin)

15. If the level of cholesterol increases in the blood serum, it causes __________.

(Diabetes,Heart attact, High blood pressure)

16. The formula of baking soda is __________.

(NaHCO3, Na2CO3, Na2CO310H2O)

17. The formula of Plaster of Paris is __________.

(CaSO4.2H2O, 2CaSO4.H2O, (CaSO4)2H2O)

18. The atoms of the elements belonging to the same period of the Periodic table have __________.

(Same number of protons, same number of neutrons, same number of valence shells)

19. Sodium thiosulphate is used in photography because of its __________.

(Reducing power, Complex formation, Oxidizing behaviour)

20. The outer electronic configuration of copper is __________.

(4s14d10, 4s23d10, 4s13d10)

21. H2S solution in water is __________.

(Neutral, Acidic, Basic)

22. __________ is isomer of ethanol.

(CH3OH, CH3OCH3, C6H5OH)

23. Petroleum is a mixture of __________.

(Alkanes and alkenes, aromatic hydrocarbons, all of these)

24. Glucose is __________.

(Reducing sugar, oxidizing sugar, none of these)

25. Pentane shows __________.

(Two isomers, three isomers, four isomers)

Chapter 1

Periodic Classification of Elements

1. __________ elements have been discovered so far.

(100, 110, 120, 150)

2. so far 110 elements have been discovered. Out of these __________ elements are naturally occurring.

(100, 96, 92, 94)

3. __________ classified the then known elements into metals, non metals and their derivatives.

(Dobreiner, Al-Razi, Newlands, Mendeleeve)

4. In 1817, a German chemist, __________ made use of the idea of relationship between atomic weights and properties of elements for the classification of elements.

(Dobreiner, Al-Razi, Newlands, Mendeleeve)

5. __________ presented the law of triads.

(Dobreiner, Al-Razi, Newlands, Mendeleeve)

6. Dobreiner’s work led to the law of triads which states that __________.

(Atomic weight of any one lement was found to be approximately the mean of the other two elements of triad, Atomic weight of the middle element was found to be approximately the mean of the other two elements of a triad, Atomic number of any one element was found to be approximately the mean of the other two elements of a triad, Atomic number of the middle element was found to be approximately the mean of the other two elements of triad)

7. The law of octaves was given by __________.

(Dobreiner, Al- Razi, Newlands, None of these)

8. Law of octaves states that __________.

(The properties of every 6th element from the given one were similar to the first, the properties of every 9th element from the given one were similar to the first, the properties of every 8th element from the given one were similar to the first, the properties of every 7th element from the given one were similar to the second)

9. “Physical and chemical properties of elements are periodic functions of their atomic weight.” This is called __________.

(Dobereiner’s Law of Triads, Newlands’ Law of Octaves, Mendeleev’s Periodic Law, None of these)

10. Lother Meyer arranged the elements in order of their increasing atomic weights and found that __________.

(Physical propertis of the elements were the periodic function of their atomic weights, chemical properties of the elements were the periodic function of their atomic number, physical properties of the elements were the periodic function of their atomic number, chemical properties of the elements were periodic function of their atomic weights)

11. Mendeleev’s Periodic table was based on __________.

(Atomic number, Atomic mass, Atomic volume, Electronic Configuration)

12. Mandeleev formulated a rule for the classification of elements and concluded that __________.

(Physical and chemical properties of the elements are periodic functions of their atomic numbers, physical and chemical properties of the elements are periodic functions of their atomic weights, physical properties of the elements are periodic function of their atomic weights, Chemical properties of the elements are periodic functions of their atomic numbers)

13. Modern Classification of elements is based on __________.

(Doberiner’s law of Triads, Newlands’ law of Octaves, Mendeleev’s Periodic Table, None of these)

14. Excluding H and He, the smallest element in the periodic table is __________.

(Lithium, Fluorine, Cesium, Iodine)

15. “Physical and chemical properties of elements are the periodic functions of their atomic numbers.” This is called __________.

(Law of Triads, Law of Octaves, Periodic Law, None of these)

16. Moseley’s work led to the periodic law, which states that __________.

(the number of the electrons in the 1s energy level increases as the atomic number increases, The properties of the elements are a periodic function of their atomic masses, The x-rays spectra of the elements are more complex than the optical spectra, The properties of elements are the periodic function of their atomic number)

17. A pair of elements in the same family in the periodic table classification is __________.

(Chlorine and carbon, calcium and aluminium, nitrogen and neon, sodium and potassium)

18. In the period, the elements are arranged in strict sequence in order of __________.

(Increasing charges in the nucleus, increasing atomic weight, increasing number of electrons in valence shell, increasing valency)

19. Most of the known elements are metals of __________ of periodic table.

(d-block, p-block, III-group, Zero block)

20. __________ reflects combining capacity of an element.

(Valency, atomic number, ionization energy, ionization potential)

21. As we move from left to right in second period of the periodic table, the gram atomic volume of the elements __________.

(Increases at a constant rate, remains unchanged, decreases, will change indefinitely)

22. The volume in cubic centimeters occupied by one gram atom of the element is called __________.

(Atomic Volume, Atomic weight, Mass number, None of these)

23. In a __________, atomic volume increases with atomic number, from top to bottom, as new shells are added up with increase in atomic number.

(Group, Period, Sub-group, None of these)

24. __________ of the following is a transition element.

(Ni, Rb, Al, As)

25. On moving from left to right across a period in the periodic table, the size of atom generally __________.

(decreases, increases, remains constant, decreases up to IV A group and then increases)

26. The amount of energy required to remove an electron from an atom of an element in the gaseous state I called __________.

(Ionization Potential, Ionization energy, Electron volt, both a and b)

27. Each vertical row of the periodic table includes elements with chemical characteristics that are in general __________.

(identical, similar, different, sometimes identical and sometimes differents)

28. The ionization energy __________ in a group from top to bottom with the increase in atomic size.

(Increases, decreases, remains constant, none of these)

29. The lowest ionization energies are found in the __________.

(inert gases, alkali metals, Transition elements, Halogens)

30. Ionization energy is lowest for __________.

(Inert gases, alkali metals, halogens, alkaline earth metals)

31. In the periodic table, the highest ionization energies are for __________.

(Halogens, Noble gases, Alkali metals, Chalcogens)

32. The atomic weight of an element divided by its density is called __________.

(Atomic mass, Atomic volume, Atomic density, Atomic number)

33. Elements in the same family __________.

(have same atomic number, have the same molecular weight, have similar chemical properties, constitute a group of elements with the same electronic configuration)

34. In a given period, the alkali metals have __________.

(smallest atomic size, lowest ionization energy, lowest density, highest electron affinity)

35. Of the following given elements __________ atom has the highest ionization energy.

(Be, F, N, Ne)

36. The value of ionization energy __________ in a period from left to right due to the decrease in atomic size.

(increases, decreases, remains constant, None of these)

37. __________ is the most electronegative element.

(Fluorine, Iodine, Oxygen, Sodium)

38. The unit of ionization energy is __________.

(Joule, Calorie, electron volt, none of these)

39. Of the following elements, __________ element has the highest first ionization potential.

(Boron, carbon, nitrogen, oxygen)

40. The unit of ionization potential is __________.

(Joule, joule per mole, calorie per mole, none of these)

41. In a period, the ensity of normal elements first __________ and then __________ after reaching a maximum value somewhere in the middle.

(Increases, decreases, remains constant, none of these)

42. Most of the known elements are __________.

(Rrystalloids, Metals, Metalloids, Non metals)

43. Melting and boiling points gradually __________ in a periodic table from left to right up to the middle.

(increases, decreases, remains constnt, none of these)

44. The electropositive elements form __________.

(acidic oxides, basic oxides, neutral oxides, none of these)

45. __________ of the following elements has the lowest first ionization energy.

(Na, F, I, Cs)

46. The electronegative elements form __________.

(Acidic oxides, Basic oxides, Neutral oxides, none of these)

47. __________ is the most volatile compound.

(HI, HCl, HBr, HF)

48. The ionization energy of nitrogen is more than oxygen because of __________.

(more attraction of electrons by the nucleus, more peneration effect, the extra stability of half filled p-orbitals, the size of nitrogen atom is smaller)

49. The elements of group IIA are called __________.

(Metals, Non-metals, Alkaline earth metals, Transition elements)

50. __________ ion has the largest radius.

(Al+3, Cl-, F-, O-2)

51. __________ atom has the smallest size.

(C, F, Li, Rb)

52. __________ of the following has highest first ionization energy.

(Br, Cl, F, I)

53. The most electropositive among the following elements is __________.

(Fe, Na, Cs, Pb)

Chapter 2

Hydrogen

1. Large amounts of atomic hydrogen are present in the atmosphere of __________.

(Earth, Sun, Moon, none of these)

2. Hydrogen atom contains __________ electrons.

(1, 2, 3, 4)

3. During the electrolysis of water hydrogen is liberated at the __________.

(Anode, Cathode, Diode, none of these)

4. The atomic weight of hydrogen is __________.

(1.00, 1.008, 1.08, 1.800)

5. In nature hydrogen exists in __________.

(Gaseous state, Solid state, Liquid state, Plasma state)

6. __________ is the lightest gas.

(Nitrogen, Helium, Oxygen, Hydrogen)

7. Alkali metals do not exist in __________.

(Monoatomic, Diatomic, Triatomic, none of these)

8. Hydrogen generally combines with other elements to form __________.

(Ionic bond, Covalent bond, Polar bond, none of these)

9. Hydrogen may be readily prepared by the action of water on __________.

(Fe, HCl, Zn, Na)

10. In organic compounds, __________ element is found in close association with hydrogen.

(C, N, O, none of these)

11. Ionic hydrides are usually __________.

(liquids at room temperature, good reducing agents, good electrical conductors in solid state, Easily reduced)

12. The atoms of the same element, which have the same atomic number but different mass numbers, are called __________.

(Isotopes, Actanides, Isobars, none of these)

13. The difference in atomic weights or mass numbers of the atoms of the same element is due to __________.

(Different number of electrons in them, different number of protons in them, different number of neutrons in them, none of these)

14. A tritium nucleus has __________.

(one proton and two electrons, one proton and two neutrons, one neutrons and two protons, one proton and three neutrons)

15. Physical properties of elements depend upon the number of __________.

(Protons in the nucleus, neutrons in the nucleus, electrons in the valence shell, both protons and neutrons in the nucleus)

16. Chemical properties of elements depend upon the number of __________.

(electrons in the valence shell, protons in the nucleus, neutrons in the nucleus, protons and neutrons in the nucleus)

17. Chemical properties of elements depend upon their __________.

(Atomic number, Atomic weight, volume, none of these)

18. The hydronium ion is a/an __________.

(ion with formula H2O+, ion with the formula H3O+, free radical rather than an ion, ion formed by removal of H- form a water molecules)

19. Hydrogen is an important constituent of __________.

(Water, Petroleum, Natural gas, all of these)

20. When steam is passed over red hot coke at 1000°C, a mixture of carbon monoxide and hydrogen gas is produced. It is known as __________.

(Heavy water, Water gas, Phosgen gas, none of these)

21. The most suitable process for the separation of CO from water gas is __________.

(Bosch Proces, Lane’s Process, Electrolysis of water, None of these)

22. When steam is passed over iron at 500°C, magnetic oxide and hydrogen gas is produced. This is called __________.

(Bosch Process, Lane’s Process, Electrolysis, All of these)

23. The presence of an acid or base renders water __________.

(good conductor of electricity, poor conductor of electricity, very bad conductor of electricity, all of these)

24. The process of loss of oxygen from a substance or addition of hydrogen is called __________.

(Oxidation, Reduction, Hydrogenation, None of these)

25. Hydrogen is a very good __________.

(Reducing agent, Oxidizing agent, Reducing agent as well as oxidizing agent, none of these)

26. Lowering of oxidation state of a metal is termed s __________.

(Oxidation, Reduction, Hydrogenation, All of these)

27. The process of addition of hydrogen (H2) to a molecule is called __________.

(Oxidation, Reduction, Hydrogenation, all of these)

28. Formation of vegetable ghee from vegetable oil is an example of __________.

(Oxidation, Reduction, Hydrogenation, all of these)

29. Ethylene can be hydrogenated to __________ under pressure at about 300°C, when double bond is changed to single compounds.

(Methane, Ethane, Ethyne, None of these)

30. Hydrogen reacts with halogens to give __________.

(Hydrogen halides, hydrogen hydrides, hydrogen sulphides, All of these)

31. Hydrogen is used in the manufacture of __________.

(Fertilizers, CO2, O2, None of these)

32. Hydrogen at the time of its generation during chemical reaction is in the form of atomic state and is called __________.

(Ionic Hydrogen, Nascent hydrogen, atomic hydrogen, none of these)

33. Hydrogen molecule consists of two atoms linked together by a strong __________.

(Ionic bond, Covalent bond, Hydrogen bonding, None of these)

34. Nascent hydrogen is used in the reduction of __________.

(Ionic compounds, Organic compounds, Inorganic compounds, none of these)

35. The compounds formed between two elements are called __________.

(Hydrides compounds, Binary compounds, Tertiary compounds, None of these)

36. Hydrogen reacts with some elements to form binary compounds called __________.

(Halides, Hydrides, Oxides, all of these)

37. The hydrides formed by the transfer of electrons from electropositive metals to hydrogen are called __________.

(Ionic hydrides, covalent hydrides, Complex hydrides, Interstitial hydrides)

38. NaH is an example of __________.

(Ionic hydrides, covalent hydrides, Complex hydrides, Interstitial hydrides)

39. Ionic hydrides ionize to produce __________.

(H-ion, OH-ion, H+ion, all of these)

40. The hydrides, which are good conductors of electricity in the fused state, are called __________.

(Ionic hydrides, covalent hydrides, Complex hydrides, Interstitial hydrides)

41. Covalent hydrides generally exist in __________.

(Solid state, Liquid state, Gaseous state, all of these)

42. Covalent hydrides are prepared by the direct action of __________.

(metals with hydrogen, non-metals with hydrogen, transition elements with hydroge, none of these)

43. Hydrides, which are non-stoichimetric in nature, are called __________.

(Ionic hydrides, covalent hydrides, Complex hydrides, Interstitial hydrides

44. The law of chemical combination is not obeyed by __________.

(Ionic hydrides, covalent hydrides, Complex hydrides, Interstitial hydrides

45. Electron deficient hydrides are called __________.

(Ionic hydrides, covalent hydrides, Complex hydrides, Interstitial hydrides

46. Hydrogen occurs in __________.

(One isotopic forms, two isotopic forms, three isotopic forms, four isotopic forms)

47. Atomic hydrogen is __________.

(More reactive than molecular hydrogen, less reactive than molecular hydrogen, very less reactive than molecular hydrogen, all of these)

48. The process of addition of hydrogen to a molecule is called __________.

(Halogenation, Hydrogention, Sulphonation, Reduction)

Chapter 3

S - Block Elements

1. Out of all the elements of group IA, the highest atomic number is for __________.

(Na, Cs, Rb, K)

2. Out of all the elements of group IA, the highest melting and boiling point is for __________.

(Li, Na, Rb, K)

3. __________ of the following elements has highest ionization potential.

(K, Rb, Cs, Li)

4. Out of all the elements of group IA, the highest heat of hydration is for __________.

(Li, Na, K, Rb)

5. __________ of the elements has highest melting and boiling point.

(Be, Ca, Mg, Ba)

6. __________ of the following elements have highest oxidation potential.

(Na, Li, Rb, K)

7. Out of all the elements of group IIA, the highest density at 20°C is for __________.

8. Out of all the following elements of group IIA, the highest atomic number is for __________.

(Be, Ba, ca, Sr)

9. The alkali metals possesses __________ electrons in their outermost orbitals.

(1, 2, 3, 4)

10. Out of all the elements of group IIA, the highest heat of hydration is for __________.

(Be, Ba, Ca, Mg)

11. __________ of the elements has highest ionic radius.

(Be, Ba, Sr, Ca)

12. Out of all the elements of group IA, the highest heat of hydration is for __________.

(Li, Na, K, Cs)

13. Of all the group II elements, the highest oxidation potential is for __________.

(Li, Be, Ba, Ra)

14. Sodium is not observed in +2 Oxidation State because of its __________.

(high first ionization potential, high second oxidation potential, high ionic radius, high electronegativity)

15. The metallic lustre of sodium is explained by the presence of __________.

(Na+ ions, conduction electrons, free protons, a body centred cubic lattice)

16. __________ of the following substances is manufactured by electrolysis of NaCl solution.

(NaOH, Na2ClO3, NaClO3, Na)

17. When NaCl is dissolved in water, the sodium ions become __________.

(Oxidized, Reduced, Hydrolyzed, Hydrated)

18. NaCl imparts a golden yellow colour to the Bunsen flame. This can be interpreted due to __________.

(Low ionization potential of sodium, Photosensitivity of sodium, Sublimation of metallic sodium to give yellow colour, Emission of excess energy absorbed as a radiation in the visible region)

19. The alkaline earth metals possess __________ electron or electrons in their outermost orbitals.

20. Alkali metals form __________.

(Ionic bond, covalent bond, non-polar, Vander waal’s forces)

21. Sodium salts constitute __________% of earth’s crust.

(2.40, 2.35, 2.30, 2.25)

22. Potassium salts constitute __________% of the earth’s crust.

(2.40, 2.35, 2.30, 2.25)

23. Alkaline earth metals occur in nature in __________.

(free state, combined state, both free and combined state, none of these)

24. In general alkali metals act as __________.

(Reducing agents, Oxidizing agents, Both reducing and oxidizing agents, none of these)

25. All alkaline metals except __________ are white in colour.

(Be, Mg, Ca, None of these)

26. In the alkali metal series __________ of the following is most reactive.

(Li, Na, K, Rb)

27. In the alkali metal series, Cesium is the most reactive metal because __________.

(its incomplete shell is nearest to nucleus, the valence electron has a larger orbit than the orbit of the valence electron of any of the others, it exerts considerable Beautiful force on the valence electrons, it is a heavier metal)

28. Alkali metals are __________.

(lighter than water, heavier than water, enlarged than water , all of these)

29. __________ does not belong to alkali metals.

(Li, Na, Rb, K)

30. A graphite anode is used in Down’s cell for the production of sodium because __________.

(It does not react with sodium, it does not react with chorine, it is easy to fashion in circular form, it floats on the fused sodium chloride)

31. __________ is a reducing agent and a constituent of a gun powder.

(KNO3, C, CaCO3, Na)

32. Alkaline earth metals form __________ carbides on heating with carbon.

(Stable, Unstable, soluble, none of these)

33. Except lithium, all alkali metal hydroxides are strongly __________.

(acidic in nature, basic in nature, neutral in nature, none of these)

34. Alkaline earth metal carbonates, sulphates and phosphates are __________.

(soluble in water, insoluble in water, sometimes soluble and sometimes insoluble in water, none of these)

35. Alkali metal carbonates, sulphates and phosphates are __________ in water with the exception of Li2CO3 and Li3PO4.

(soluble, insoluble, Both soluble and insoluble, none of these)

36. LiCl is soluble in organic solvents while NaCl is not. This is because __________.

(Lattice energy of NaCl is less than LiCl, Li+ has higher value of hydration energy than that of Na+, LiCl is more covalent in nature than NaCl, Li+ has lower value of hydration energy than Na+)

37. When burnt in air, Lithium forms __________.

(Normal oxide, Peroxide, Super oxide, none of these)

38. The chlorides of alkali metals and alkaline earth metals are generally __________.

(Ionic, Covalent, non polar, vander waal’s forces)

39. Sodium is a __________.

(good conductor of electricity, poor conductor of electricity, bad conductor of electricity, none of these)

40. Sodium reacts vigorously with oxygen on heating to form __________.

(Sodium oxide, Sodium peroxide, sodium superoxide, all of these)

41. Sodium is very reactive with water. Hence due to its high reactivity with water, it is stored in __________.

(Alcohol, Kerosine oil, Benzene, all of these)

42. Sodium reacts vigorously with water, liberating __________.

(Oxygen, hydrogen, Carbonoxide, Neon)

43. Sodium is a powerful __________.

(Reducing agent, oxidizing agent, bleaching agent, all of these)

44. __________ is used s a reducing agent in the preparation of such metals as titanium and zicronium from their chlorides or oxides.

(Mg, Na, Cu, Ag)

45. __________ is used in the synthesis of rubber.

(Mg, Cu, Na, Fe)

46. __________ reducing action is used in the manufacture of certain dyes and drugs.

(Na, Mg, Cu, Ca)

47. __________ is used often in highway lamps as filaments to produce yellow light.

(Na, Tungston, Mg, Fe)

48. Purification of sodium chloride is accomplished by __________.

(Sublimation, Crystallization, Hydrogenation, Melting)

49. Ice and sodium chloride form a freezing mixture, which is used in __________.

(Refregeration, Preserving fish, Sublimation, None of these)

50. Sodium bicarbonate is commonly called __________.

(Soda Ash, Baking soda, Caustic soda, none of these)

51. Soap is often composed of __________.

(sodium carbonate, calcium carbonate, rubidium carbonate, sodium stearate)

52. Solvay’s process is also called __________.

(Haber’s Proess, Ammonia Soda Process, Washing Soda Process, Down’s Process)

53. __________ is a stronger base.

(NaOH, KOH, LiOH, HCl)

54. Na2CO3 is marketed as __________.

(Soda ash, baking soda, caustic soda, none of these)

55. When a solution of sodium carbonate is evaporated, Na2CO3.10H2O crystallizes out t room temperature and marketed as __________.

(Soda ash, baking soda, caustic soda, washing soda)

56. By the action of aqueous NaOH on aluminium, __________ is produced.

(H2, CO2, H2O, O2)

57. __________ is used for weighing cotton cloth.

(Gypsum, Soda ash, Magnesium Sulphate, Washing soda)

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Chapter 4

P - Block Elements

1. __________ of the following is non-metal.

(Boron, Aluminium, Indium, Thallium)

2. __________ of the following was isolated by Davy in 1807 by electrolysis of moist boric acid.

(Boron, Indium, Aluminium, Gallium)

3. __________ of the following is chemically inert.

(Boron, Indium, Aluminium, Gallium)

4. __________ is not the member of group IIIA.

(B, In, C, Al)

5. The oxides of Boron are __________ in nature.

(Acidic, Basic, Neutral, None of these)

6. __________ forms the most acidic oxide.

(B, Al, Ga, In)

7. Boron bursts into flame at __________.

(600°C, 700°C, 800°C, None of these)

8. B3+ cannot exist in aqueous solution because of its __________.

(Strong reducing ability, large size and small charge, small size and large charge, strong oxidizing ability)

9. Orthoboric acid on heating to about 100°C looses a water molecule to form __________.

(Metaboric acid, Pyroboric Acid, Metaboric and Pyroboric acid, none of these)

10. The reduction of metal oxides is sometimes accomplished by using aluminium in the __________.

(Goldshmidt’s reaction, Silberchmdit’s reaction, Baeyer’s reaction, Zilch’s reaction)

11. Baeyer’s Process is used for the purification of __________.

(Alum stone, Cryolite, Bauxite, none of these)

12. Hall’s Process is based on electrolysis of __________.

(Alumina, Gypsum, Borax, none of these)

13. __________ is a better conductor of heat.

(Fe, Sn, Al, none of these)

14. Al2O3 formation involves evolution of a larger quantity of heat, which makes its use in __________.

(Deoxidizer, confectionary, indoor photography, thermite welding)

15. A mixture of iron oxide and aluminium is called __________.

(Thermite, Bauxite, Alum, none of these)

16. Aluminium is used in __________.

(X-ray welding, Spot welding, Thermite welding, none of these)

17. __________ metal is used in photo-flash bulbs.

(Ca, Na, W, Al)

18. The alloy of aluminium, which contains small quantities of manganese, copper and magnesium, is called __________.

(duralumin, Magnalium, Alnico, none of these)

19. The alloy of aluminium with small percentage of magnesium is called __________.

(Duralumin, Magnalium, Alnico, none of these)

20. The aluminium which contains 20% nickel, 20% aluminium, 50% iron and 10% cobalt is called __________.

(Duralumin, Magnalium, Alnico, none of these)

21. A magnet made of __________ will lift approximately 4000 times of its own weight of iron.

(Duralumin, Magnalium, Alnico, none of these)

22. An alloy of aluminium made by alloying 5-15% aluminium and has a golden lustre is called __________.

(duralumin, Magnalium, Aluminium Bronze, none of these)

23. All the alums crystallize to yield __________.

(Octahedral crystal, Tetrahedral crystal, Trigonal crystal, Linear crystal)

24. The process of permanent dyeing is called __________.

(Mordanting, Painting, Calination, none of these)

25. The solvent used in the extraction of aluminium from its ore is __________.

(Cryolite, Bauxite, Molten sodium chloride, Water)

26. The group IV-A of the periodic table consists of __________ elements.

(three, four, five, six)

27. In group IV-A the metallic character down the group __________.

(Increases, Decreases, remains constant, none of these)

28. __________ does not contain aluminium.

(Felsper, Cryolite, Kaoline, Anhydrite)

29. Carbon differs from other members of its group due to the absence of __________ electrons.

(s, p, d, none of these)

30. Elements, which exist in two or more physical or molecular forms, are called __________.

(Isotopes, Allotropes, Isobars, none of these)

31. Out of the following elements of group IV A of the periodic table the higher density is for the element __________.

(C, Si, Ge, Pb)

32. Diamond is a __________ conductor of electricity and heat.

(Poor, Good, None, none of these)

33. Out of all the elements of group IV the higher density is for __________.

(C, Si, Ge, Pb)

34. __________ is used as a lubricant for machinery and also as a moderator in nuclear reactors.

(Diamond, Graphite, Epsom, Gypsum)

35. Highest melting and boiling point is for __________.

(C, Ge, Si, Pb)

36. PbO behaves as a/an __________.

(Amphoteric oxide, basic oxide, super oxide, sub oxide)

37. White lead is prepared by __________.

(Dutch process, Solvay’s Process, Down’s Process, none of these)

38. __________ member of the group V-A show several oxidation states such as –1, +2, +3, +4 and +5.

(P, As, Sb, N)

39. __________ member of the group V-A forms multiple bonds.

(P, Bi, As, N)

40. __________ member of group V-A does not show allotropy.

(P, Sb, N, As)

41. In __________ solution glass is soluble.

(HNO3, HCl, HF, H2CO3)

42. On industrial scale Nitric acid is prepared by __________.

(Dutch Process, Birkland-Eyde’s Process, Solvay’s Process, Down’s Process)

43. In Ostwald’s Process the substance used to oxide ammonia is __________.

(Zn, Pt, CO, none of these)

44. Copper reacts with dilute nitric acid to form __________.

(Nitric oxide, nitrogen peroxide, nitrous oxide, none of these)

45. Nitric acid is a strong __________.

(reducing agent, bleaching agent, oxidizing agent, none of these)

46. A mixture consisting of one volume of concentrated HNO3 and three volumes of concentrated HCl is called __________.

(Aqua regia, Meta stannic acid, Alum, Sandhur)

47. Lead tertraethyle is used as __________.

(Fire extinguisher, Pain Killer, Mosquito repellent, Petroleum Additive)

48. Nitric acid is used in the manufacture of __________.

(Cellulose, Varnishes, T.N.T, all of these)

49. __________ allotropic form of coal is hard.

(Peat, Lignite, Anthracite, Graphite)

50. __________ molecule is paramagnetic nature.

(O, S, Se, Po)

51. __________ element edhibits the largest number of allotropic forms amongst the elements.

52. __________ element is the most abundant element in earth’s crust.

(Ca, Si, C, O)

53. There are __________ rings in unit cell of Rhombic sulphur.

(12, 16, 20, 24)

54. Graphite is used in nuclear reactor as __________.

(A Lurbicant, A fuel, for lining the inside of reactor as an insulator, for reducing the velocity of neutrons)

55. In its unit cell, monoclinic sulphur possesses how many S8 rings.

(12, 6, 3, 0)

56. H2S is a good __________.

(reducing agent, oxidizing agent, bleaching agent, none of these)

57. In the aqueous solution H2S ionizes to produce __________ ions and behaves as a weak acid.

(H+, H-, OH-, none of these)

58. H2S reduces halogens to __________.

(hidrides, halides, halogens, none of these)

59. By __________ process the H2SO4 produced is pure and can be produced of any desired strength.

(Lead Chamber Process, Contact Process, Down’s Cell, none of these)

60. __________ gas is responsible for rising of bread.

(CO, CO2, NH3, O2)

61. At what temperature H2SO4 completely dissociates into sulphur trioxide and water.

(416°C, 516°C, 616°C, 716°C)

62. Concentrated sulphuric acid acts as a __________.

(Reducing agent, Oxidizing agent, Dehydrating agent, None of these)

63. __________ charcoal is used to decolourise brown sugar solution.

(Wood, Coconut, Animal, Sugar)

64. In the sale of diamonds the unit of weight is carat. One cart is equal to __________.

(100mg, 200mg, 300mg, 400mg)

65. Hot concentrated sulphuric acid acts as an __________ usually itself reduced to sulphur dioxide.

(Dehyrating, Oxidizing, Reducing, none of these)

66. __________ are the two elements that find wide application in transistor industry.

(Silicon and Germinium, Carbon and Platinium, Iridium and Germanium, Tungsten and Platinium)

67. In the manufactur of certain explosives such as nitroglycerine, trinitrotoluene and gun-cotton etc. Sulphuric acid is used as a __________.

(Oxidizing agent, Reducing agent, Dehydrating agent, none of these)

68. __________ prepared chlorine in 1774, by the action of hydrochloric acid on manganese dioxide.

(Cavendish, C.W. Scheele, Sir Humphry Davy, Lane)

69. __________ suggested the name chlorine for the gas produced by the action of hydrochloric acid on manganese dioxide.

(Sir Humphry Davy, C.W. Scheele, Cavendish, none of these)

70. Chlorine is obtained by reacting concentrated HCl with __________ agent, such as MnO2, KClO3, KMnO4.

(Reducing, oxidizing, dehydrating, none of these)

71. Electrolysis of Brine produces __________.

(Chlorine, Hydrogen, H2S, Nitrogen)

72. The process based on the oxidation of hydrochloric acid with oxygen is __________.

(Nelson’s Cell, Contact Process, Down’s Process, Deacon’s Process)

73. __________ process is used for the production of chlorine gas.

(Deacon’s, Contact, Solvay’s, Electrolysis of water)

74. Chlorine gas is __________ in colour.

(Yellow, Greenish Yellow, Violet, Blue)

75. __________ produces inflammation of the nose and throat when breathed in considerable quantities.

(Nitrogen, Carbon dioxide, Chlorine, Hydrogen Sulphide)

76. To kill bacterial, molst of the drinking water is treated with __________.

(Nitrogen, Carbon dioxide, Chlorine, Hydrogen Sulphide)

77. Chlorine is used in the preparation of poisonous gases of warfare, such as __________.

(COCl2, H2S, HCl, none of these)

78. In phosphorus oxide the number of oxygen atoms bonded to each phosphorus atom is __________.

(1, 2, 3, 4)

79. Of the following elements the only one which does not exhibit allotropy is __________.

(P, As, Sb, Bi)

80. Phosgene is the common name of __________.

(Carbon dioxide and Phosphine, Phosphoryle chloride, Carbonyle Chloride, Carbon Tetrachloride)

81. Out of all the elements of group VI A, the highest melting and boiling point is for __________.

(Te, Se, S, Pb)

82. In group VIA highest electronegativity is for __________.

(S, O, Pb, Se)

83. Large deposits of sulphur in nature are found as __________.

(Sulphuric acid, hydrochloric acid, free sulphur, none of these)

84. On the basis of available data of the structure of monoclinic sulphur, it probably consists of __________ chains.

(S6, S2, S4, S8)

85. Rhombic sulphur consists of __________.

(S8 chains, S2 chains, S4 rings, S8 rings)

86. Pure sulphuric acid is a solid compound which __________.

(Is always colloidal, slowly decomposes to form SO2, Seves as a useful source for H2S, has never been observed)

87. The form of sulphur, which is stable at room temperature and normal atmospheric pressure, is __________.

(orthorhombic, hexagonal, mono clinic, amorphous)

88. When H2S gas is dissolved in aqua regia, the function of HCl in the mixture is to __________.

(oxidize the sulphur, oxidize the mercury, complex the sulphur, complex the mercury)

89. When liquid sulphur at one atmosphere pressure is very slowly cooled, unless super cooling occurs, the first solid to appear is __________.

(monoclinic sulphur, Rhombic sulphur, Hexagonal sulphur, metallic sulphur)

90. The synthesis of ethers from alcohol depends on the fact that sulphuric acid is a good __________.

(oxidizing agent, reducing agent, complexing agent, dehydrating agent)

91. __________ of the following has the highest catenation capability.

(Oxygen, Sulphur, Selenium, Tellurium)

92. the halogen with the highest ionization potential is __________.

(F, Cl, I, At)

93. The halide ion with the highest hydration energy is __________.

(F-, Cl-, I-, At-)

94. Hydrofluoride acid is __________.

(a powerful oxidizing agent, a weak acid, a strong acid, a good reducing agent)

95. __________ of the following is most powerful oxidizing agent.

(F2, Cl2, Br2, I2)

96. __________ of the following exhibits the largest electrical conductivity in the liquid state.

(F2, Cl2, Br2, I2)

97. __________ of the following exhibits the highest bond energy.

(F2, Cl2, Br2, I2)

98. __________ does not form its oxy acids.

(F2, Cl2, Br2, I2)

99. The colour of I2 solution can be discharged by shaking a aqueous solution of __________.

(Sulphur dioxide, sodium thiosulphate, sodium sulphite, sodium sulphate)

100. Bleaching powder is obtained by the interaction of Cl2 and __________.

(a dilute solution of Ca(OH)2, conc. Solution of Ca(OH)2, dry CaO, dry slaked lime)

Chapter 5

Transition Elements

1. Transition elements are those in which __________ orbitals are in the process of completion.

(d, f, s, d or f)

2. Transition elements are located between __________ elements in the periodic table.

(s and p block, s and f block, d and p block, none of these)

3. Out of total 110 elements known, there are more than __________ transition elements.

(40, 50, 60, 70)

4. Elements in which d-orbitals are in the process of completion are called __________ elements.

(outer transtion, inner transition, non-transition, none of these)

5. __________ of the following is transition element.

(Sr, Sn, Cr, B)

6. __________ of the following elements is not included in the list of transition elements.

(Ca, Cu, Cr, CO)

7. Due to the addition of electrons in inner f-robitals atomic and ionic radii or f-block elements have a regular trend. This is called __________.

(Contraction, Lanthanide contraction, actanide, contraction, none of these)

8. The transition elements usually have very __________ melting and boiling points.

(low, high, intermediate, none of these)

9. Transition elements show a tendency of __________.

(high reactivity, less reactivity, very high reactivity, none of these)

10. Finely divided iron is used in __________.

(Haber Process, Catalytic Hydrogenation, Oxidation of ammonia to nitric oxide, Contact Process)

11. __________ reagent can be used to identify Cu2+ ion.

(Nitric acid, Sulphuric acid, Sodium hydroxide, Potassium chromate)

12. Vanadium pentaoxide is used in __________.

(Haber Process, Oxidation of sulphur dioxide to sulphur trioxide, oxidation of ammonia to nitric oxide, Contact Process)

13. __________ is the important ore of copper.

(Malachite, Bauxite, Blue Vitriol, Alumina)

14. Copper is used in __________.

(Haber Process, Oxidation of ethyl alcohol to acetaldehyde, oxidation of ammonia to nitric oxide, Contact Process)

15. Bessemer converters are used to get __________.

(Aluminium, Copper, Steel, Sodium)

16. Titanium is used as catalyst in __________.

(Haber Process, Catalytic Hydrogenation, Oxidation of ammonia to nitric oxide, Polymerization of ethyle into polyethylene)

17. Platinium or Palladium is used as catalyst in __________.

(Haber Process, Catalytic Hydrogenation, Oxidation of ammonia to nitric oxide, Contact Process)

18. __________ of the following does not belong to d-block elements.

(Chromium, Cobalt, Silicon, Copper)

19. Compounds attracted into a magnetic field are called __________.

(Magnets, Paramagnets, Dimagnets, none of these)

20. Transition metal compounds, which show paramagnetism, have __________.

(unpaired electrons, paird electrons, unpaired protons, paired protons)

21. A substance, which have even number of electrons and have paired spin is called __________.

(Ferromagnetic, Paramagnetic, Dimagnetic, none of these)

22. Magnetic movement is measured with help of __________.

(Guoy’s balance, Spring balance, Physical balance, Cavendish Appratus)

23. __________ property provides information about the presence of unpaired electrons in an atom or ion.

(Dipole moment, Magnetic moment, torque, none of these)

24. By measuring the magnetic moment values we can measure __________.

(Nature of the transition metal compound, oxidation state of the transition metal, both nature and oxidation state of transition metal compound, none of these)

25. Transition elements show variable valencies because of the involvement of the d-electrons in addition to __________.

(p-electrons, f-electrons, d-electrons, e-electrons)

26. The empty spaces between atoms of transition metals in their crystal lattices are called __________.

(Vacant spaces, valence spaces, interstices, none of these)

27. The formation of non-stoichiometric compounds is due to the defects in solid structure and __________.

(Variabel valency of transition elemennts, even number of electrons, even number of protons, unpaired electrons)

28. Interstitial compounds have __________ formula.

(definite, half, indefinite, no)

29. Strong paramegnetism is called __________.

(dimagnetism, ferromagnetism, both dimagnetism and ferromagnetism, none of these)

30. When a number of molecules or negatively charged ions combine with a central d-block atom or ion to form complex ion or molecule, __________ is formed.

(a co-ordinate compound, interstitial compound, di-atomic compound, none of these)

31. In coordinate bonding the molecules or ions, which bond onto the central metal ion or atom, are called __________.

(actanides, Lanthanides, Ligands, none of these)

32. Ligands are __________.

(electron pair donors, electron pair acceptros, neutral, none of these)

33. [Ni(CN)4]2- is an example of __________.

(Squre planar, tetrahedral complexes, octahedral complexes, none of these)

34. [Cu(NH3)4]2+ is an example of __________.

(Squre planar, tetrahedral complexes, octahedral complexes, none of these)

35. MnO4- is an example of __________.

(Squre planar, tetrahedral complexes, octahedral complexes, none of these)

36. CrO42- is an example of __________.

(Squre planar, tetrahedral complexes, octahedral complexes, none of these)

37. [Cu(CN)4]3- is an example of __________.

(Squre planar, tetrahedral complexes, octahedral complexes, none of these)

38. [Zn(NH3)4]3- is an example of __________.

(Squre planar, tetrahedral complexes, octahedral complexes, none of these)

39. [Fe(CN)6]3- is an example of __________.

(Squre planar, tetrahedral complexes, octahedral complexes, none of these)

40. [Fe(CN)6]4- is an example of __________.

(Squre planar, tetrahedral complexes, octahedral complexes, none of these)

41. [Ni(NH3)6]2+ is an example of __________.

(Squre planar, tetrahedral complexes, octahedral complexes, none of these)

42. [Co(NH3)6]3+ is an example of __________.

(Squre planar, tetrahedral complexes, octahedral complexes, none of these)

43. In the system of naming complex coordinate compounds cations are named __________ anions.

(after, beforem, inbetween, none of these)

44. The names of __________ are usually unchanged.

(anionic ligands, cationic ligands, neutral ligands, none of these)

45. NH3 is an example of __________ ligand.

(anionic, cationic, neutral, none of these)

46. H2O is an example of __________ ligand.

(anionic, cationic, neutral, none of these)

47. The suffix “ate” at the end of the name of the coordinate complex ion represents a/an __________.

(cation, anion, cathode, anode)

48. A mixture of iron sulphide and copper sulphide is called __________.

(gangue, matte, matter, residue)

49. Sulphide ore is concentrated by __________.

(Froth floatation Process, Dutch Process, Bessemerization, none of these)

50. __________ does not copper.

(Carborundum, Azurite, Blue Vitriol, Malachite)

51. Utensils used to carry out fermentation are made of __________.

(Cu, Fe, Al, Ca)

52. An alloy of copper, which contains 80% copper and 20% zinc, is called __________.

(Brass, Bronze, Bell metal, none of these)

53. Copper sulphate reacts with solution of potassium iodide giving __________.

(sulphur dioxide, iodine, copper oxide, potassium oxide)

54. An alloy of copper, which contains 90% Cu and 10% Sn is called __________.

(Bronze, Brass, Bell Metal, all of these)

55. An alloy of copper, which contains 80% Cu and 20% Sn is called __________.

(Bronze, Brass, Bell metal, all of these)

56. The substance attracted by magnetic field is known as __________.

(diamagnetic, paramagnetic, antimagnetic, all of these)

57. Copper sulphate is commonly called __________.

(Nila Thotha, Lunar Caustic, Surkh Kahi, none of these)

58. Silver nitrate is commonly called __________.

(Nila Thotha, Lunar Caustic, Surkh Kahi, none of these)

59. Stainless steel is __________.

(a mixture, a compound, an element, all of these)

60. Potassium dichromate is commonly called __________.

(Nila Thotha, Lunar Caustic, Surkh Kahi, none of these)

61. Manganese differs from most other transition elements because it reacts with __________.

(oxygen, water, sulphur, iodine)

62. __________ of the following elements can be included in the category of transition elements.

(Cu, Al, Ar, At)

63. Potassium ferrocyanide is a __________.

(normal salt, mixed salt, double salt, complex salt)

64. __________ of the following combination is included in the Iron triad of elements.

(Pd and Pt, Mn and Hg, Co and Ni, V and Ti)

65. __________ is a blue crystalline solid which is freely soluble in water.

(Nila Thotha, Lunar Caustic, Surkh Kahi, none of these)

66. __________ is an orange crystalline solid which is freely soluble in water.

(Nila Thotha, Lunar Caustic, Surkh Kahi, none of these)

67. __________ is a yellow crystalline solid which is freely soluble in water.

(Nila Thotha, K2CrO4, Surkh Kahi, none of these)

68. __________ is a colourless crystalline solid.

(Nila Thotha, Lunar Caustic, Surkh Kahi, none of these)

69. __________ is used as fungicide and germicide.

(Nila Thotha, Lunar Caustic, Surkh Kahi, none of these)

70. Ferric oxide is __________.

(a basic anhydride, an acid anhydride, an amphoteric anhydride, green in colour)

71. Potassium dichromate is a strong __________.

(reducing agent, oxidizing agent, dehydrating agent, all of these)

72. The densest element is __________.

(Pb, Hg, Pt, Os)

73. The most strongly ferromagnetic element is __________.

(Fe, Co, Ni, Os)

74. Alloying of metals serves to inhibit __________.

(Corrosion, Froth Floatation, Erossion, None of these)

75. Mechanical strains can be removed by __________.

(heat treatment, polishing the metal surface, both heat treatment and polishing the metals surface, none of these)

76. __________ has the lowest density.

(Cu, Ni, Sc, Zn)

77. Galvanizing is done by dipping clean iron sheet in a zinc chloride bath and __________.

(heating, rusting, froth floatation, alloying)

78. There are two well known theories to explain the phenomenon of corrosion namely __________.

(Acid theory, Electromechanical theory, electrochemical theory, acid and electromechanical theory)

79. __________ one of the following metals exists in liquid form.

(Sc, Y, La, Hg)

80. The process of depositing a thin layer of tin on base metals to protect them from corrosion is called __________.

(Exposure, tin plating, Fixing, none of these)

81. The most strongly ferromagnetic element is __________.

(Fe, Ni, S, C)

82. The property of a substance which permits it being drawn into wire is called __________.

(softness, Ductility, Brittleness, Hardness)

83. One of the constituent of German silver is __________.

(Ag, Cu, Mg, Al)

84. When potassium permanganate is added to a saturated aqueous solution of potassium hydroxide, __________ gas is evolved.

(Hydrogen, Oxygen, Carbon dioxide, none of these)

85. __________ reagent can be used to identify nickle ion.

(Resorcinol, Dimethyl glyoxime, Dimethyl Benzidine, Potassium Ferrocyanide)

86. __________ of the following is the transition element.

(Sr, Sn, Cr, Fe)

87. Bessemer converters are used to get __________.

(Aluminium, copper, steel, none of these)

88. __________ is not the ore of copper.

(Blue vitriol, Cuprite, Chalcocite, Steel)

89. __________ of the following elements is not included in the list of transition elements.

(Ca, Cu, Cr, Co)

90. __________ one of the following does not belong to d-block elements.

(Chromium, Silicon, Cobalt, Nickel)

[admin]

Chapter 6

Organic Chemistry

1. The branch of chemistry which deals with the study of compounds containing carbon as a essential element is called __________.

(Organic chemistry, In organic chemistry, Physical chemistry, all of these)

2. The first organic compound synthesized in the laboratory is __________.

(Methane, Urea, Acetic Acid, Glucose)

3. __________ of the following is not an organic compound.

(CH4, CO2, CH2-CH2, CH3OH)

4. __________ of the following is not an organic compound.

(Penicillin, Urea, Oxalic acid, Plaster of Paris)

5. __________ is the important sources of naturally occurring compounds of carbon.

(Animals, Plants, Rock salts, Sea water)

6. __________ is not a component of coal.

(H, O2, N, Si)

7. Hard black form of coal containing 92 – 98% carbon is called __________.

(Anthracite, Sub-bituminous coal, Bituminous coal, Lignite)

8. The most abundant form of coal and is used as energy souce and carbonization for coke, coal tar and coke-oven is called __________.

(Anthracite, sub-bituminous coal, Bituminous coal, Lignite)

9. Form of coal used at power generating stations is called __________.

(Antracite, Sub-bituminous coal, Bituminous coal, Lignite)

10. A soft and brown form of coal which contains 50 to 60% carbon is called __________.

(Anthracite, Sub-bituminous coal, Bituminous coal, Lignite)

11. In Pakistan deposits of lignite are found at __________.

(Dandot, Saindak, Khewra, none of these)

12. __________ is a pure carbon.

(Coke, Coal gas, Coal tar, none of these)

13. Its major constituents are hydrogen (50%), methane (35%) and carbon monoxide (8%).

(Coke, coal gas, coal tar, none of these)

14. Number of organic compounds present in coal tar is __________.

(115, 215, 315, 415)

15. Residue left after fractional distillation of coal tar is called __________.

(Pitch, Dutch, Gangue, Matte)

16. Petroleum in the unrefined form is called __________.

(Coke, Coal gas, Crude oil, Rock oil, both crude oil and rock oil)

17. Natural gas mainly consists of __________.

(Methane, Ethane, propane, Butanes)

18. In Pakistan there are vast reserves of natural gas at __________ in Baluchistan.

(Bandot, Khewra, Saindak, Sui)

19. __________ is a mixture of methane, ethane, propane and butane, used as a fuel and for making other organic chemicals.

(Refinary gas, Gasoline, Kerosene oil, gas oil)

20. __________ is a mixture of hydrocarbons containing 5-8 carbon atoms and boiling in the range of 40-180°C.

(Refinary gas, Gasoline, Kerosene oil, gas oil)

21. __________ is a mixture of hydrocarbons having 11-12 carbon atoms and boiling point in the range of 250°C.

(Refinary gas, Gasoline, Kerosene oil, gas oil)

22. A mixture of hydrocarbons having 13-25 carbon atoms is called __________.

(Refinary gas, Gasoline, Kerosene oil, gas oil)

23. On strong heating the fractions containing the larger hydrocarbon molecules are broken up into smaller and more volatile molecules, this is called __________.

(Sublimation, Cracking, Roasting, Refining)

24. Cracking is also termed as __________.

(Pyrolysis, Refining, Polymerization, Hydrohalogenation)

25. A large number of organic compounds, especially the unsaturated ones, show a great tendency to unite. This process is termed as __________.

(Pyrolysis, Cracking, Polymerization, none of these)

26. An isomer of ethanol is __________.

(Dimethyl ether, Diethyl ether, Ethylene glycol, Methanol)

27. Organic compounds made up of carbon and hydrogen are called __________.

(Polymers, Hydrocarbons, Butanes, none of these)

28. Organic compounds other than the hydrocarbons may be considered to be derived from the hydrocarbons by the replacement of one or more of their __________ atoms with atoms or groups of atoms of other element.

(Carbon, Hydrogen, Nitrogen, none of these)

29. When ethylene is heated under pressure, a transparent solid polymer, __________ is obtained.

(Polyethene, Ethane, Methane, None of these)

30. An atom or group of atoms, which confers characteristic properties to an organic molecule, is called __________.

(Radical, Functional group, Polymer, none of these)

31. Compounds having same molecular formula but different structures are said to be __________.

(Polymers, Isomers, Radical, Functional group)

32. The quality of petroleum is determined by __________.

(Decane number, octane number, hexane number, none of these)

33. __________ of the following obey isomerism.

(CO2, C2H6O, CuSO4, none of these)

34. Two or more than two different compounds having the same molecular formula but different carbon chains or skeletons are said to be __________.

(Chain isomers, position isomers, functional group isomers, metamers)

35. The kind of isomerism which depends upon the relative position of the group, or the position of double or single bond in case of unsaturated compounds in termed as __________.

(Chain isomerism, Position isomerism, Functional Group isomerism, Metamerism)

36. Isomerism, which involves compounds having the same molecular formula, but different functional groups are called __________.

(Chain isomerism, Position isomerism, Functional Group isomerism, Metamerism)

37. __________ is exhibited by compounds having the same functional group but different alkyl attached to the same multivalent atom.

(Chain isomerism, Position isomerism, Functional Group isomerism, Metamerism)

38. In cracking usually catalyst used is __________.

(Pt, Aluminosilicate, Ni, Tetra-ethyl lead)

39. Iso-butane exhibited __________.

(Chain Isomerism, Position Isomerism, Functional group Isomerism, Metamerism)

40. In CCl4 molecule the four valencies of carbon atom are directed towards the corners of a __________.

(Cube, Hexagon, Prism, Tetrahedron)

41. Tetrahedral nature of bonding in carbon atom was first shown by __________.

(Wohler, Vant Hoff and LeBel, Lewis, Kekule)

42. The general formula (RCO)2O represents __________.

(An ether, ketone, an ester, an acid anhydride)

43. Formation of alkane by the action of zinc on alkyl halide is called __________.

(Frankland reaction, Wurtz reaction, Cannizzaro’s reaction, Kolbe’s reaction)

44. __________ of the following are isomers.

(Methyl alcohol and dimethyl ether, Ethyl alcohol and dimethyl ether, Acetone and Acetaldehyde, Proponoic acid and proponanone)

45. The isomers must have the same __________.

(Structural formula, molecular formula, chemical properties, physical properties)

46. __________ has the longest bond length.

(C = C, C º C, C – C, all of these)

47. In alkanes all C – C bonds have __________.

(single bond, double bond, triple bond, none of these)

48. Removal of one of the hydrogen atoms of an alkane produces a __________.

(alkyl group, ethyl group, methyl group, none of these)

49. Compounds in which two alkyl groups are attached to an oxygen atom are called __________.

(alkanes, ethers, alcohals, isomers0

50. Many hydrocarbons contain more than one OH groups in a molecule. Molecules of this type are called __________.

(Ethers, Polyhydroxy alcohols, aldehydes, none of these)

51. __________ is the common name of methanol.

(formaldehyde, acetaldehyde, propionaldehyde, none of these)

52. Compounds which contain carbonyl group but differ from aldehydes in that two alkyl groups are attached to the carbon of carbonyl group are called __________.

(Ethers, Ketons, Alcohols, none of these)

53. __________ is the common name of propanone.

(Acetone , ketone, Diethyl Ketone, none of these)

54. Benzene is a __________.

(Heterocyclic compound, Alicyclic compound, Aromatic compound, Acyclic)

55. Common name of formic acid is __________.

(Methanoic acid, Ethanoic acid, Propanoic acid, none of these)

56. The properties of organic compounds are due to __________.

(Covalent bonds, Functional groups, Ionic bonds, None of these)

Chapter 7

Hydrocarbons

1. Organic compounds, which contain element carbon and hydrogen only are called __________.

(Hyrocarbons, Ethers, Ketones, none of these)

2. The number of hydrocarbons is very large because of the property of hydrogen to __________, with it self in the form of chains and rings.

(Cmbine, Catenate, Sulphonation, none o these)

3. Carbon usually exhibits a covalency of __________.

(Two in most of its compounds, three in most of its compounds, four in most of its compounds, none of these)

4. Hydrocarbons, which contain single bonds, are called __________.

(alkanes, alkenes, alkynes, none of these)

5. Hydrocarbons, which contain double bonds, are called __________.

(alkanes, alkenes, alkynes, none of these)

6. Hydrocarbons, which contain triple bonds, are called __________.

(alkanes, alkenes, alkynes, none of these)

7. The alkanes have __________.

(tetrahedral frame work, planar molecules, linear structure, none of these)

8. The alkynes have __________.

(tetrahedral frame work, planar molecules, linear structure, none of these)

9. The alkenes have __________.

(tetrahedral frame work, planar molecules, linear structure, none of these)

10. Saturated Hydrocarbons are also called __________.

(Alkanes, Olefins, Alkenes, Alkanes and Olefins)

11. Unsaturated hydrocarbons are also called __________.

(Alkenes, Paraffins, alkanes, none of these)

12. Alkenes are characterized by the presence of __________ bond between two carbon atoms.

(single, double, triple, none of these)

13. Alkanes or paraffins are characterized by the presence of __________ bond between two carbon atoms.

(Single, double, triple, none of these)

14. Alkynes are characterized by the presence of __________ bond between two carbon atoms.

(single, double, triple, none of these)

15. Alkanes are also called __________.

(Paraffins, Olefins, Aldehydes, none of these)

16. Alkenes are also called __________.

(Paraffins, Olefins, Carbonyl, none of these)

17. An alkane hydrocarbon chain on cyclization would result in the formation of __________.

(Alicyclic compound, aromatic compound, ethers, none of these)

18. Benzene is the simplest example of hydrocarbon called __________.

(Alicyclic, aromatic, open chain, none of these)

19. Solid CH4 is __________.

(molecular solid, covalent solid, ionic solid, does not exist)

20. Methane is also known as __________.

(oil gas, marsh gas, gasoline, none of these)

21. A liquid hydrocarbon is converted into a mixture of gaseous hydrocarbon by __________.

(Cracking, Hydrolysis, Oxidation, Reduction)

22. __________ is obtained in the laboratory by heating a mixture of sodium acetate and soda lime.

(Alcohol, Ethene, Methane, none of these)

23. Alkenes undergo __________.

(addition reaction, substitution reaction, both addition and substitution reaction)

24. __________ does not react with aqueous solution of acids, alkalies, or potassium permanganate or other oxidizing agents and most of the usual laboratory reagents.

(Benzene, Ether, Methane, Acetic acid)

25. Bromine reacts with methane when the reaction is catalyzed by __________.

(Sunlight, high frequency radiation, diffused sunlight, nickel)

26. In methane the replacement of hydrogen by _ NO2 is called __________.

(Pyrolysis, Nitration, Halogenation, none of these)

27. Methane when heated to extreme temperature in the absence of air undergoes thermal decomposition, called __________.

(Nitration, Catalytic oxidation, Pyrolysis, none of these)

28. Urea, a useful fertilizer, is prepared on industrial scale from __________.

(Natural gas, Coal, Coke, Petroleum)

29. Carbon black is a raw material for paints and automobile tyres and is prepared from __________.

(Ethane, Ethene, Methane, none of these)

30. C2H6 is called __________.

(Methane, Ethane, Methanol, none of these)

31. __________ is obtained in the laboratory by heating sodium proponoate and soda lime.

(Methane, Ethane, Ethene, none of these)

32. In the laboratory ethane is prepared by the reaction called __________.

(Sabatier-Senderens Reaction, Pyrolysis, Catenation, Hydrohalogenation)

33. When an aqueous solution of sodium or potassium salt of mono-carboxylic acid is subjected to electrolytic, corresponding alkane is formed. This reaction is called __________.

(Sabatier-Senderens Reaction, Kolbe’s Electrolysis, Polymerization, chlorination)

34. On burning __________ produces a considerable amount of heat energy which may be used for welding process.

(Ethane, Benzene, Ethene, none of these)

35. __________ is found to be present in wood gas and coal gas.

(Methane, Ethene, Ethane, Benzene)

36. __________ is prepared on a small scale in the laboratory by heating together ethyl alcohol and sulphuric acid.

(Methane, Ethane, Ethylene, none of these)

37. The elimination of hydrogen halide (HX) from adjacent carbon atoms is called __________.

(Pyrolysis, Chlorination, Dehydrohalogenation, none of these)

38. __________ process is important in the hardening of vegetable and animals oils to produce solid fats which are used to make margarine.

(Pyrolysis, Catenation, Hydrogenation, Dehydrohalogenation)

39. When a mixture of ethene and air is passed over heated silver under pressure, we get __________.

(Epoxide, Superoxide, Suboxide, none of these)

40. The negative part of the addendum adds on to the carbon atom joined to the least number of hydrogen atoms. The statement is called __________.

(Markownikoff’s rule, Peroxide effect, Theile’s theory, Baeyer’s strain theory)

41. Baeyer’s test is the basis for detection of a __________ bond in an organic molecule.

(single, double, triple, none of these)

42. __________ was used in first world war.

(Phosgene gas, Mustard gas, Oil gas, Coal gas)

43. When a mixture of CO, C2H4 and C2H2 is passed through ammonical cuprous chloride solution then __________.

(Acetylene and CO are absorbed, CO is absorbed, C2H4 is absorbed, Nothing happens)

44. Ethylene dichloride is also called __________.

(Mustard gas, Dutch liquid, Polyethene, none of these)

45. __________ is used to manufacture mustard gas which is poisonous gas used as war gas.

(Ethane, Methane, Ethylene, none of these)

46. __________ is most found in alkenes.

(Chain isomerism, Geometrical isomerism, Mesomerism, Position Isomerism)

47. __________ poisonous gas is present in the exhaust fumes of car.

(Methane, Acetylene, HCl, Carbon dioxide)

48. __________ is used to import colour to stile green citrus fruit form ripening.

(Ethylene, Methane, Ethane, none of these)

49. The number of xylene isomers is __________.

(2, 3, 4, 5)

50. Ethylene dichloride and ethylene chloride are isomeric compounds. The statement which is not applicable to both of them is __________.

(react with alcoholic potash, react with aqueous potash and give the same product, are dihalides, answer Beilstein’s test)

51. Structure of benzene is __________.

(Diagonal, Planner, Pyramidal, Tetrahedral)

52. __________ is used in the manufacture of plastic and synthetic rubber.

(Styrene, Mustard gas, Polythene, none of these)

53. The polythene is a polymer of __________.

(Ethylene, Aceton, Propylene, Butadiene)

54. Acetylene or ethyne was discovered accidentally in 1899 by the American chemist __________.

(Wilsson, Lane, Nelson, none of these)

55. Acetylene is present in small proportions (about 0.06% by volume) in __________.

(Natural gas, Coal gas, Gasoline, Petroleum)

56. __________ is prepared in the laboratory by dropping water on calcium carbide.

(Ethylene, Acetylene, Methane, none of these)

57. The process used for the preparation of acetylene is __________.

(Berthelot Process, Sabatier-Senderns Reaction, Kolbe’s Process, none of these)

58. Acetylene has a characteristic ethereal smell resembling that of __________.

(Rotten egg, Garlic, Benzene, none of these)

59. Acetylene burns with __________ flame.

(Greenish, Bluish, Smoky, none of these)

60. Benzene was found by __________ in 1825 in the gas produced by the destructive distillation of vegetable oils.

(Hofmann, Michael Faraday, Solvay, none of these)

61. __________ found benzene in coal-tar.

(Hofmann, Michael Faraday, Solvay, none of these)

62. When n-hexane obtained from petroleum is heated in the presence of platinum at 500°C under 10 – 20 atmosphere pressure, it cyclises to give __________.

(Ether, Benzene, Mustard Gas, none of these)

63. Phenol is reduced to __________, when its vapours are passed over red hot zinc dust.

(Ether, Benzene, Ethane, Acetylene)

64. Replacement of hydrogen atom by – SO2 OH is called __________.

(Nitration, Sulphonation, Alkylation, Hydrogenation)

65. _ SO2OH is called __________.

(Sulphonic Group, Carbonyl group, Methyl group, none of these)

66. Under the influence of anhydrous aluminium chloride as a catalyst, benzene reacts with alkyl and acyl halides giving alkylated and acylated benzens. The reaction is called __________.

(Friedel-Cracts Reactions, Berthelot’s Reaction, Sabatier-Senderens Reaction, none of these)