Five Year Papers
1. Plastics are polymers of __________.
2. From crude oil, additional quantity of petrol is obtained by __________ process.
3. Tertiary alkyl halides react by __________ reaction mechanism.
4. __________ period is incomplete.
5. Elements, which follow actinium, are called __________ elements.
6. Ionic hydrides are also called __________.
7. Compounds with the general formula CnH2n + 2O are called __________.
8. Resorcinol is not an alcohol but a __________.
9. A ketone contianing different alkyl radicals is called __________ ketone.
10. The hydrolysis of fats and oils with a strong alkali is called __________.
11. __________ is active in the stomach of young children.
12. The chemical name of Lunar caustic is __________.
13. Aluminium resists corrosion due to the formation of __________.
14. EDTA is a __________ ligand.
15. The chemical formula of rust is __________.
16. Sub-Group B elements are called __________ elements.
17. The hybridization of carbon in graphite is __________.
18. The chemical name of vitamin B2 is __________.
19. The reactions between metallic sodium and alkyl halides are called __________ reaction.
20. The fractional distillation of crude petroleum yields only __________% petrol.
21. Starch and Cellulose are the examples of __________ carbohydrates.
22. AgCl dissolves in ammonia to form __________.
Chapter 1
Periodic Classification of Elements
1. In 1913 Moseley, A British physicist, found that a __________ is the fundamental property of an atom.
2. In the modern Periodic table recommended by the International Union of Pure and Applied Chemistry (IUPAC) in 1982, the elements are arranged in the ascending order of __________.
3. Horizontal rows of elements in the periodic table are called __________.
4. The vertical columns of elements arranged in the Periodic table are called __________.
5. In the Modern Periodic Table there are __________ periods.
6. The first period of Modern Periodic Table contains __________elements.
7. Hydrogen lies in __________ Period.
8. Helium lies in __________ Period.
9. All the elements belonging to the second period are __________.
10. Second period contains __________ elements.
11. The elements of the second period of the modern Periodic table are __________.
12. Third period of periodic table contains __________ elements.
13. The elements of the fourth period of the modern periodic table are __________.
14. Fourth period of Modern Periodic Table contains __________ elements.
15. Fifth period of Modern Periodic Table contains __________ elements.
16. Those elements, which have ‘d’ orbitals in the process of completion in the form of ions or atoms, are called __________.
17. Elements in IB group are called __________.
18. Those elements, which involve ‘s’ orbital filling in their valence shells, are called __________.
19. The sixth period of Modern Periodic Table contains __________ elements.
20. The longest period of modern Periodic Table is __________.
21. The eight ‘s’ and ‘p’ block elements in the 4th and 5th periods are known as __________.
22. The elements of group IA and IIA are classified as __________ elements.
23. The seventh period of modern Periodic table contains __________ elements.
24. The elements on the right hand side of the Periodic table are called __________.
25. The outer most shell involved in chemical bonding are called __________.
26. The number of electrons in the outermost or valence shells is called __________.
27. Na2O is strongly __________ in nature.
28. Cl2O7 is strongly __________ in nature.
29. Greater the electronegativity of an element, stronger is the __________ character of its oxide.
30. In case of transition elements, the last electrons are received by __________.
31. Elements in group IB, IIB through VIIB are known as __________.
32. Elements in group IB, IIB through VIIB are known as __________.
33. Elements in the group VI A and __________ are the most active non-metals.
34. The correct order of second ionization potential of carbon, nitrogen, oxygen and fluorine is __________.
35. The elements having seven valence electrons are known as __________.
36. The elements of group IIIA to VIIA are called __________.
37. Maximum number of electrons present in sixth period is __________.
38. The elements of group VIIIA are called __________.
39. In case of inner transition elements the last electrons are received by __________.
40. In case of outer transition elements the last electron are received by __________.
Chapter 2
Hydrogen
1. Hydrogen was first prepared by Cavendish in 1766 by the action of __________.
2. Hydrogen is evolved by the action of cold diluted HNO3 on __________.
3. Hydrogen is found in nature in combined state. The most abundant compound of hydrogen is __________.
4. The electronic configuration of hydrogen atom is __________.
5. Hydrogen forms slat like hydrides with the elements of __________.
6. Hydrogen forms interstitial hydrides with the elements of __________.
7. An example of covalent hydride is __________.
8. Alkali metals need __________ electron to complete their outermost shells.
9. The number of isotopes of hydrogen is __________.
10. 1H1 is symbol of __________.
11. 1H2 is the symbol of __________.
12. 1H3 is the symbol of __________.
13. The number of neutrons in the nuclei of tritium atom is __________.
14. The number of neutrons in the nucleus of protium is __________.
15. The mass number of deutrium is __________.
16. Tritium is present to the extent of one atom in __________ atoms.
17. Chemical formula of heavy water is __________.
18. Hydrogen is obtained industrially as a by-product during electrolysis of __________.
19. Hydrogen is commercially prepared by the thermal decomposition of
20. Hydrogen burns in air with __________ flame.
21. Density of hydrogen is about of 1/14th of that of __________.
22. The electronegativity of hydrogen is __________.
23. The bond energy of hydrogen is __________.
24. Hydrogen liquefies at __________.
25. Hydrogen freezes at __________.
26. The symbol of hydride ion is __________.
27. Hydrogen burns on ignition in the presence of oxygen to produce __________.
28. Hydrogen reacts on heating with P directly to form __________.
29. The hydrides formed by the combination of non-metals of groups IVA, VA, VIA and VIIA with hydrogen are called __________.
30. LiAlH4 is an example of __________.
31. The atomic weight of heavy hydrogen is __________.
32. __________ is the commonest gas in the atmosphere.
33. The element, which does not make salt like hydride is __________.
Chapter 3
S-Block Elements
1. In s-block elements the outermost orbitals are filled with __________ electrons at the outer most.
2. S-block elements consist of __________.
3. The colour of the flame of potassium is __________.
4. On bunsen flame sodium gives __________.
5. On bunsen flame Potassium gives __________.
6. On bunsen flame Cesium gives __________.
7. On bunsen flame Calsium gives __________.
8. On bunsen flame Strontium gives __________.
9. On bunsen flame Barium gives __________.
10. Alkaline earth metals are relatively __________ reactive than alkali metals.
11. An apparatus used for commercial preparation of sodium is named as __________.
12. Baking soda is also called __________.
13. The radius of K-atom is 2.31A°. The radius of K+ will be __________.
14. Bicarbonate of alkali metals and alkaline earth metals are formed by passing __________ through a solution of the carbonates of alkali metals or a suspension of carbonates of alkaline earth metals in water.
15. Metallic sodium was first obtained by Sir H. Davy in 1807 by the electrolysis of fused __________.
16. Gay Lussac and Thenard in 1811 prepared sodium by reducing sodium hydroxide with __________.
17. The process in which sodium was prepared by distilling sodium carbonate with carbon and a small amount of chalk as a catalyst was introduced by __________.
18. Down’s cell is used for the production of __________.
19. The density of sodium metal is __________.
20. Melting point of sodium is __________.
21. Boiling point of sodium is __________.
22. The annual consumption of NaCl is about __________.
23. __________ percentage of NaCl is present in sea water.
24. __________ percentage of NaCl or Common salt is present in rock salt.
25. Sodium carbonate is generally called __________.
26. Sodium carbonate is prepared by __________.
27. Aqueous solution of sodium carbonate on heating gives sodium carbonate and __________.
28. __________ is medically used for the treatment of hyperacidity in the stomach.
29. In firge extinguishers __________ is used as a source of carbon dioxide.
30. Mixture of sodium bicarbonate and crystals of vegetable acids, e.g. tartaric acid or citric acid is known as __________.
31. Anhydrous sodium carbonate is called __________.
32. Industrial use of sodium carbonate is in the manufacture of __________.
33. __________ is used in the smelting of iron ores of high sulphur content.
34. Sodium Hydroxide is manufactured on large scale by electrolysis of aqueous solution of __________.
35. Nelson’s cells is used for the manufacture of __________.
36. Castner-Kellner Process is used for the production of __________ on industrial scale.
37. The melting point of NaOH is __________.
38. NaOH decomposes into its elements at about __________.
39. Bleaching powder is manufactured by treating lime with chlorine in __________.
40. The colour of bleaching powder is __________.
41. Bleaching powder smells strongly like __________.
42. When bleaching powder is treated with strong solution of ammonia, __________ gas is evolved.
43. Calsium sulphate occurs in nature as dihydrate salt called __________.
44. Gypsum can be prepared by the action of dilute sulphuric acid on __________.
45. At __________ temperature gypsum loses its three fourth of water.
46. Gypsum is sparingly soluble in water. Its solubility increases with rising temperature up to __________.
47. Magnesium sulphate is usually sold as hydrated salt called __________.
48. Epsom salt is prepared from magnesite MgCO3 on boiling with dilute __________.
49. Epsom salt loses six molecules of water at __________.
50. Epsom salt becomes anhydous at __________.
51. Epsom salt is converted into magnesium oxide by heating it with carbon at about __________.
52. __________ is used in medicine as purgative.
Chapter 4
P-Block Elements
1. The elements, which belong to III-A group to VIII-A group, are called __________.
2. In p-block elements the metallic character __________ down the group.
3. In p-block elements the orbital in the process of completion is __________.
4. Crystalline boron is a hard substance which is __________ in colour.
5. Out of all the elements of group IIIA, the highest Ionization potential is for __________.
6. Boron possesses close resemblance with __________.
7. Orthoboric acid is prepared by the acidification of hot concentrated solution of borax with calculated quantity of __________.
8. In the Hall-Berou.t process for producing aluminium the substance produced at the cathode is __________.
9. Hydrogen gas many be produced by the reaction of aluminium with a concentrated solution of __________.
10. The most widely distributed element in the earth’s crust after oxygen and silicon is __________.
11. Aluminium resists corrosion due to the formation of a coat of __________.
12. Hall’s Process is used for the production of __________.
13. Duralum is an alloy which contains Mg + Cu + __________ + Mn.
14. The group IV-A of the periodic table consists of __________.
15. Diamond has a high refractive index of __________.
16. At 700°C graphite burns in air to form __________.
17. Red lead is commonly known as __________.
18. __________ is the product of thermal decomposition of sodium bicarbonate.
19. Lead Monoxide is a yellow powder and also called __________.
20. Nitrogen, phosphorus, arsenic, antimony and bismuth are the members of the group __________.
21. All members of group VA exhibit maximum oxidation state of __________.
22. The shape of diamond is __________.
23. On an industrial scale nitric acid is prepared by __________.
24. Poisonous gas present in the exhaust fumes of car is __________.
25. The boiling point of nitric acid is __________.
26. The freezing point of nitric acid is __________.
27. Oxygen, sulphur, selenium, tellurium and polonium are the members of group __________.
28. The first four members of the group VI-A are collectively called __________.
29. There are __________ electrons in the valence shell of elements of group VI-A.
30. The maximum valency of oxygen is __________.
31. Oxygen has __________ allotropic forms.
32. The transition temperature of sulphur is __________.
33. X-rays analysis shows that __________ sulphur consists of chains of sulphur atoms.
34. The purest H2S is obtained by passing vapours of sulphur and hydrogen over finely divided __________ at 450°C.
35. __________ was first prepared in the laboratory by Jabir Bin Hayyan.
36. __________ is called king of chemicals.
37. Lead Chamber process is used for the preparation of __________.
38. Contact Process is used for the production of __________.
39. __________ is called Oleum.
40. Freezing point of pure sulphuric acid is __________.
41. Dilute sulphuric acid dissolves many metals with the evolution of __________ and the corresponding sulphates are formed.
42. Formic acid is converted into carbon monoxide by the action of concentrated __________ and heating.
43. Gases such as oxygen, hydrogen, carbon dioxide, chlorine and sulphur dioxide are often dried by bubbling them through __________.
44. Concentrated sulphuric acid absorbs sulphur trioxide forming __________.
45. Carbon is oxidized to __________ in the presence of sulphuric acid.
46. In a process called pickling the metal sheets are soaked in __________ to remove rust or by chemical action.
47. Phosphine may be produced by the action of water on __________.
48. In the refining of petroleum, __________ is employed to remove tarry materials and sulphur compound.
49. In the Ostwald process, the substance which is used to oxidize NH3 is __________.
50. In the periodic table, halogens, namely fluorine, chlorine, bromine, iodine and astatine are placed in group __________.
51. The brown gas formed when metals reduce HNO3 is __________.
52. __________ is used as catalyst in the Contact Process.
Chapter 5
Transition Elements
1. Annual production of antimony being mined in Pakistan is __________.
2. Annual production of Orchro being mined in Pakistan is __________.
3. Annual production of Chromite being mined in Pakistan is __________.
4. Annual production of manganese being mined in Pakistan is __________.
5. Transition elements other than Sc, Y and Ti have density above __________.
6. Due to d-d transition of electrons, Cu2+ ion appears __________ in colour.
7. The colour of Fe3+ ion is __________.
8. The colour of Fe2+ ion is __________.
9. The colour of Cr3+ ion is __________.
10. The colour of Mn3+ ion is __________.
11. The colour of Mn2+ ion is __________.
12. The colour of the fmale of potassium is __________.
13. The magnetic moment is related to the number of unpaired electron ‘n’ by the equation __________.
14. All the 3-d series elements show an oxidation state of __________ in addition to higher oxidation states except Sc.
15. The majority of transition metal’s ion complexes contain __________ ligands surrounding the central octrahedrally.
16. Copper is known since __________.
17. In Pakistan copper mines at Saindak in __________ were first discovered in 1962.
18. It is estimated that the Saindak mines will yield an annual production of __________ tones of copper from its sulphide ore for a period of 16 years on the commencement of production.
19. __________ percentage of total copper metal is obtained from sulphide ore.
20. The colour of copper is __________.
21. Copper becomes __________ when it is heated.
22. Copper melts at __________ °C.
23. Cu2O is __________ in colour.
24. The colour of CuO oxide is __________.
25. When copper is heated in air, then CuO + __________ are formed.
26. Bronze contains __________% Cu and 10% Sn.
27. __________ is prepared in the laboratory by the action of dilute sulphuric acid on cupric oxide or cupric carbonate.
28. __________ is prepared by dissolving metallic silver in warm dilute nitric acid.
29. The highest common oxidation state of chromium is __________.
30. __________ is prepared in the laboratory by the addition of potassium chloride to hot concentrated solution of sodium dichromate.
31. __________ is used an an indicator in silver nitrate titration for the estimation of halide ions.
32. Potassium permanganate oxidizes acid in presence of dilute __________.
33. __________ is used as a disinfectant for purification of water.
34. __________ is used in bleaching paper pulp.
35. The rusting of iron is catalyzed by __________.
36. Conversion of any metal into its oxide by the action of environment is called __________.
37. Rusting of iron is an example of __________.
38. Aluminium resists the process of corrosion due to the formation of __________.
39. An alloy of iron, which contains chromium 18%, nickel 8% and carbon 0.18% is __________.
40. The black image on an exposed and developed photographic film is composed of __________.
41. In photography printing is accomplished by using an emulsion of __________.
42. All transition elements are __________.
43. Iron rust has the composition of __________.
44. When hydrated, Fe2+ ions are __________.
Chapter 6
Organic Chemistry
1. The main component of coal is __________.
2. When coal is heated in the absence of air, temperature ranging from __________, it is converted into coke, coal gas and coal tar.
3. The octane number of gasoline may also be increased by ading __________ as knoc inhibitor.
4. In Houdry process the breaking down of long-chain hydrocarbons is accelerated in the presence of a catalyst, made up of a mixture of __________.
5. The process of cracking takes place between temperature __________.
6. Molecular formula of ethers is __________.
7. Alkanes have general formula __________.
8. How many isomers can be obtained from the alkane C6H14.
9. Each alkane differs from its neighbours by __________.
10. The structural formula of ethane is __________.
11. Alkenes have general formula __________.
12. Alkyl halides have general formula __________.
13. On destructive distillation of 1000 kg of coal amount of coal tar formed is __________.
14. Natural gas consist of methane __________.
15. An alkane forms isomers if the number of least carbon atoms is __________.
16. The functional group of alkyle halids is __________.
17. The formula of alkane is __________.
18. The functional group o primary amines is __________.
19. The functional group of ether is __________.
20. The functional group of primary alcohol is __________.
21. The formula of methanol is __________.
22. The formula of ethanol is __________.
23. The formula of propanal is __________.
24. The formula of butanal is __________.
25. Formula of formic acid is __________.
26. The formula of acetic acid is __________.
27. The formula of propnoic acid is __________.
28. The formula of butyric acid is __________.
29. The formula of valeric acid is __________.
30. The formula of capric acid is __________.
31. Phenyl group is represented by __________.
32. The molecular formula of ethane is __________.
Chapter 7
Hydrocarbons
1. An example of alkane is __________.
2. __________ is the smallest hydrocarbon.
3. Natural gas consists of about __________% of methane.
4. A reaction catalyzed by the presence of __________ is called a photochemical reaction.
5. C2H2 reacts with HCl to produce __________.
6. __________ is used as catalyst in the oxidation of methane.
7. Methane reacts with superheated steam, on passing through hot tubes containing a __________ catalyst to yield carbon monoxide and hydrogen.
8. In methane H – C – H bond angles are __________.
9. The structural formula of ethylene is __________.
10. __________ is called ozone.
11. When ethene is passed through a dilute alkaline solution of KMnO4, the pink colour of the solution __________.
12. __________ reagent distinguishes ethylene from acetylene.
13. __________ polymerizes at 100 atmosphere pressure and 400°C to give polyethylene.
14. The polyethene produced in the presence of __________ and titanium tetrachloride as catalyst, shows improvement in its properties such as higher softening temperature, low permeability and greater rigidity.
15. __________ is called Dutch Liquid.
16. General formula of alkynes is __________.
17. __________ is called Acetylene.
18. Carboxylic acids combine with acetylene in the presence of __________ as catalyst, forming vinyl esters and the reaction is termed as Vinylation.
19. When a mixture of acetylene and nitrogen is submitted to an electric discharge, it forms __________.
20. When acetylene is passed through a copper tube at about 300°C it polymerizes to __________.
21. The brand of synthetic rubber is made by Polymerization of __________.
22. The process in which orbitals of different energies and shapes mix with each other to give equivalent hybrid orbital is called __________.
23. The sp3 signifies that each sp3 orbital is made up of s and p orbitals in the ratio of __________.
24. A molecule of methane has __________sigma bond(s).
25. A molecule of ethane has __________ sigma bond(s).
26. The sp3 hybridization occurs when carbon is bonded to __________ other atoms.
27. Sp2 hybrid orbitals are composed of s and p orbitals in the ratio of __________.
28. __________ bond is weaker.
Chapter 9
Organic Compounds
1. The general formula of alcohol is __________.
2. The general formula of aldehyde is __________.
3. Alcoholic fermentation is brought out by the action of __________.
4. The general formula of carboxylic acid is __________.
5. The general formula of esters is __________.
6. The general formula of ketone is __________.
7. The general formula of ether is __________.
8. The general formula of phenol is __________.
9. Methyl alcohol is used as the starting matrial in the manufacture of __________.
10. The formula of ethyl alcohol is __________.
11. To start the reversibility Estrification we use concentrated __________ used as absorbent of water produced during the reaction.
12. Dehydration means removal of __________.
13. The compound formed when silver powder is ehated with chloform is __________.
14. __________ is used as a fuel for internal combustion engines in many European countries and Brazil.
15. The formula of formaldehyde is __________.
16. The derivatives of carboxylic acids are obtained by replacing the –OH group of the carboxylic group with –OH and __________.
17. The formula of Fehling’s solution is __________.
18. The formula of Iodoform is __________.
19. Melting point of Phenol is __________.
20. Boiling point of Phenol is __________.
21. Phenol when treated with __________, yields both ortho and para sulphonic acids.
22. General formula of Grignard’s Reagent is __________.
23. The formula of Cyanogen chloride is __________.
24. The formula of Chloramine is __________.
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