ICSE Class 10 Chemistry Most Likely Question Bank (2019) PDF

In accordance with the latest syllabus of Council for the Indian School Certificate Examinations. ICSE Most Likely Question Bank...

In accordance with the latest syllabus of Council for the Indian School Certificate Examinations. ICSE Most Likely Question Bank Class X CHEMISTRY by A PANEL OF AUTHORS OSWAL PUBLISHERSA 1/12, Sahitya Kunj, M. G. Road, Agra-282 002 © Publishers Edition : 2018 ISBN : 978-93-87660-06-9 OSWAL PUBLISHERS Head office : 1/12, Sahitya Kunj, M.G. Road, Agra-282 002 Phone : (0562) 2527771– 4 E-mail : [email protected], [email protected] Website : www.oswalpublishers.com Facebook link : https://www.facebook.com/oswalpublishersindia Also available on : amazon.in, Flipkart, snapdeal  Preface Oswal Publishers take great pride in presenting their series of “ICSE Most Likely Question Bank”, especially for the students preparing for CISCE Board Examination. This book will help the students in revising the whole syllabus in a comparatively lesser time and will develop the aptitude for effective learning in the subject. This will enable candidates to acquire knowledge and to develop an understanding of the terms, facts, concepts, definitions, fundamental laws, principles and processes. We hope that this book will instill a sense of confidence in the students and empower them towards achieving their goals and scholastic excellence. Suggestions for the improvement of the book are invited and shall be gratefully acknowledged. —The Publisher How to Prepare for Board Exams Using Oswal’s Most Likely Question Bank Categorywise & Chapterwise The Most Likely Question Bank is a great learning tool for CISCE Examination as it is the most comprehensive and concisely composed set of questions for the students. In order to prepare well for their exams. The students may follow the following approach. Step 1 : Prepare Your Theory Students must go through the theory of the Chapters from their textbooks covering the syllabus as per the Council Guidelines. Step 2 : Understand the Categories The contents have been arranged as per different ‘Category’ of Questions. These ‘Categories’ cover all the different types of questions that the Board asks in their examinations. Each Category in turn covers topics from all the chapters of the syllabus. Eg. Short Answers category will cover the short answer type questions from all the chapters of the syllabus in that subject. Step 3 : Complete Syllabus Revision When students revise questions from any single category, they are revising the entire syllabus in different assemblages. Step 4 : Customised Learning Students with different learning calibers can customize their preparations. They can refer the objective questions first to get a basic understanding of the chapters and topics then they can take up the most complex categories. Step 5 : Check Your Progress Students can check their answers against the solutions given next to the questions. This will save time and help in faster revisions. Students can benefit tremendously from these series by using them optimally for their exam preparations.  CONTENTS 1. Fill in the Blanks 5-15 2. Match the Column 16-18 3. Multiple Choice Questions 19-30 4. Give One Word/Chemical Term 31-41 5. Identification of Gases 42-43 6. State the Observation 44-52 7. Define/Explain the Following 53-57 8. Balancing/Writing the Chemical Equations 58-80 9. IUPAC Naming/Writing the Structural Formula 81-85 10. Chemical Tests 86-91 11. Reasoning Based Questions 92-106 12. Short Questions 107-173 13. Numericals 174-200 14. Figure/Table Based Questions 201-226 Question Set Fill in the Blanks 1 Q. Fill in the blanks in the following statements, with suitable words : Chapter 1. Periodic Properties and Variations of Properties 1. The modern Periodic Table has......................... periods. 2. Each......................... in the Periodic Table is comprised of elements having the same number of electron shells. 3. Elements in a period, all have the same number of................. in their atoms. 4. Elements in a group, all have the same number of.................... 5. The most active metals are located in............... 1 and 2 of the Periodic Table. 6. The most reactive non-metals comprise group................. of the Periodic Table. 7. The elements of................. are known as typical elements. 8. The elements occupying left and right side groups of Periodic Table are called............... elements. 9. The rare gases are placed in............... group at the end. 10. Elements from atomic number 57 to............... occupy same place in Periodic Table. These elements are called.................. 11. Actinides are the elements from atomic number........................... to.............. and are radioactive. 12. The actinides and............... are kept outside the Periodic Table to mark their peculiar properties. 13. The properties of elements are periodic function of their................... 14. The atomic size........................... as we move left to right across the period, because the.................. increases but the..................... remains the same. 15. The metallic character.............. in a group as one moves from top to bottom. 16. The metallic character.............. in a period as one moves from right to left. 17. In a period or in a group, the larger the atomic size of an element, the......................... metallic is the element. 18. Moving across a..................... of the periodic table, the elements show increasing........................... character. 19. The amount of energy involved in the reaction X + energy → X+ + e– is known as the ………………of the element X. 20. Across a period, the ionization potential……………… 21. Down the group, electron affinity…………… 22. The higher the electron affinity of a non-metal,................... chemically reactive the non- metal is. 23. The tendency to gain an electron................. on moving down a group and.............. on moving across a period in the Periodic Table. 24. Elements having high ionization potential have.................. electron affinities. 25. The electronegativity of elements............. across a period and............... down a group. 26. In general, non-metals are.................... electronegative than metals. 27. On moving from left to right in a given period, the number of shells....................... 28. Element X belongs to group 2 and period 3 of the Periodic Table. It has........... electrons in the outer most shell. 29. Each period except period 1 in the Periodic Table begins with................ and ends up with a................ 30. The metallic and non-metallic character depends upon the...................and.................. of the elements. 31. The energy required to remove an electron from a neutral isolated gaseous atom and convert it into a positively charged gaseous ion is called…………. 6 ICSE Most Likely Question Bank, Class : X Ans. 1. 7 2. period 3. electron shells 4. outer electrons 5. groups 6. 17 7. period 3 8. representative 9. zero 10. 71, lanthanides 11. 89, 103 12. lanthanides 13. atomic number 14. decrease, nuclear charge, number of shells 15. increases 16. decreases 17. more 18. period, non-metallic 19. ionization potential 20. increases 21. decreases 22. more 23. increases; decreases 24. high 25. increases; decreases 26. more 27. remains the same 28. 2 (two) 29. an alkali metal; noble gas 30. atomic size, ionization potential 31. ionization potential Chapter 2. Chemical Bonding 1. Ionic compounds consist of........................................ charged ions. 2. Ionic compounds have.............. melting points due to............. ionic bonds. 3. The physical state of ionic compounds is.................. 4. Ionic compound conduct electricity in their................. 5. The nature of bond in compounds of alkali and alkaline earth metals is.................... 6............. compounds have low boiling points because of........... intermolecular forces. 7. In covalent compounds, the bond is formed due to the……………of electrons. 8. Melting and boiling points of covalent compounds are generally………… 9. Covalent bond is rigid and directional, it is responsible for.................... 10. Most covalent compounds have density............. than that of water. 11. The electronegativities of atoms giving covalent molecules are generally............. 12. Atoms of the same element combine to form molecules by means of................ bonds. 13. A solution of a............. electrolyte will contain both ions and molecules of the solute. 14. In the sodium chloride crystal, each Na + ion is surrounded by............... Cl– ions and each Cl– ion by.......................... Na + ions. 15. In sodium chloride, the Na+ ion has the......................... configuration and the Cl– ion has the........................ configuration. 16. A compound conducted electricity in the fused state. The compound is made-up of...................... 17. The duplet or octet structure of valence shell makes...................... of an element chemically...................... 18. The atomic number of oxygen is 8. The total number of electrons in the O2– ion is..……. 19. The atomic number of oxygen is 8. The number of protons in the O2– ion is.................. 20. Two nitrogen atoms join together by sharing.......................... pairs of electrons. 21. In NH4+ all the four bonds are...................... 22. The water molecules easily break the.................... bonds between the oppositly charged ions. The ions drift in water in all possible directions and hence electrovalent compounds............. in water. 23. A molecule of……………contains a triple bond. 24...................... are identical to a normal covalent compound. 25. Metals are good ……………because they are electron……………. 26. Electrovalent compounds have……………melting points. Ans. 1. oppositely 2. high, strong 3. solid state 4. fused state as well as in their aqueous solution 5. ionic bond 6. covalent, weak  Fill in the Blanks 7 7. sharing 8. low 9. definite shape of the molecule 10. less 11. high 12. covalent 13. strong 14. six, six 15. neon, argon 16. ions 17. atom, inactive 18. 10 19. 8 20. three 21. identical 22. ionic, dissolve 23. nitrogen 24. co-ordinate bond 25. reducing agents, donors 26. high Chapter 3. Study of Acids, Bases and Salts (a) Salts of strong acids and strong bases in water produce (1)...............solution. Solution of sodium carbonate in water is (2)....................in nature, while the solution of ferric chloride is (3)..................in nature. Ans. (1) Neutral, (2) basic, (3) acidic. (b) A solution X turns blue litmus red, so it must contain : (1) ………ions. Another solution Y turns red litmus blue and therefore, must contain (2) ………ions. When solutions X and Y are mixed together, the products will be a (3)…… and (4) ………. If a piece of magnesium was put into solution X. (5) ……… gas would be evolved. Ans. (1) hydronium, (2) hydroxide, (3) salt, (4) water, (5) hydrogen. (c) In making copper sulphate crystals, a black powder called (1)............ is added to dilute (2)......... acid and the mixture is warmed. Excess black powder is added to a small volume of acid so as to (3)........... The excess insoluble black powder is got rid by (4)......... The resulting clear solution looks (5)........... in colour. This solution is heated to get rid of some of the (6)........... Slow cooling of the remaining solution (7)............. of pure copper sulphate. Ans. (1) Copper oxide, (2) Sulphuric, (3) neutralise the excess of the acid, (4) filtration, (5) blue, (6) copper sulphide as impurity, (7) gives well-defined crystals. (d) Deliquescence takes place because of the difference in (1)..............................of atmospheric (2).................and that of the deliquescent substance. The vapour pressure of atmospheric humidity is (3).........than that of the deliquescent substance. The substances which take up water on exposure to atmosphere, without forming a solution are known as (4)................. substances. Ans. (1) vapour pressure, (2) humidity, (3) higher, (4) hygroscopic. (e) 1. An acid is a compound which when dissolved in water gives....................... ions as the only.................... ions. 2. A....................... acid undergoes almost complete dissociation on dissolving in water. 3. An example of mineral acid is........................ 4. Vinegar contains....................... acid. 5. Sodium acetate on hydrolysis forms sodium hydroxide and........................ 6. The basicity of Acetic Acid is …………. 7. Metal A reacts with cold water forming hydrogen and new compound B. The anion combined with A in a substance B is named.................... 8. The solution of sodium carbonate is alkaline due to.............................. 9. The complete reaction between an acid and a base is called...................... 10. The pH value of a neutral solution is.................................. 11. As the pH of solution decreases, its acidic strength progressively............... 12. As the pH of solution increases, the....................... strength of the solution progressively decreases. 13. pH value of lemon juice is.................. than 7. 14. Ammonium hydroxide is a................ base. 15. Methyl orange turns........................ in acidic solution. 16. The formation of a salt from an acid and a base involves the combination of................... from the acid and the...................from the....................to form....................... molecules. 8 ICSE Most Likely Question Bank, Class : X 17. A salt which absorbs moisture from the air, but does not change in physical state in called.................... salt. 18. Ammonium chloride is a....................... salt. 19. Sodium hydrogen sulphate is................ salt. 20. The salt of the acid HNO2 are called.......................and those of the acid HNO 3 are called...................... 21. Sodium sulphite reacts with dilute sulphuric acid to form sodium sulphate................. gas and water. 22. Copper (II) chloride reacts with sodium hydroxide to form...................... copper hydroxide and sodium chloride. – 23. A chemical reaction between hydronium ions of an acid and OH ions of a base to form unionised water is called............................ 24. Dissolving of aluminium foil in HCl as well as NaOH shows that it is................ in nature. 25. An example of a deliquescent salt is.......................... 26. Superphosphate is an example of a compound called............. 27. The number of H+ ions of an acid which react completely with one molecule of a base is called its.............. 28. When a metallic oxide is dissolved in water, the solution formed has high concentration of……………ions. 29. The metal which does not react with water or dilute H 2 SO4 but reacts with concentrated H2SO4 is……………. 30. The metal whose oxide, which is amphoteric, is reduced to metal by carbon reduction…………. 31. The divalent metal whose oxide is reduced to metal by electrolysis of its fused salt is…………. 32. Higher the pH value of a solution, the more…………it is. Ans. 1. hydronium, positive 2. strong 3. HCl 4. acetic 5. acetic acid 6. 1 7. hydroxyl ion 8. hydrolysis 9. neutralization 10. 7 11. increases 12. acidic 13. less 14. weak 15. pink 16. H+, OH– , base, water 17. hygroscopic 18. soluble 19. acidic 20. nitrites, nitrates 21. Sulphur dioxide 22. insoluble 23. neutralization 25. anhydrous (CaCl2 ) 24. amphoteric 26. acid salt 27. acidity 28. OH– 29. Cu 30. Pb 31. Mg 32. alkaline Chapter 4. Analytical Chemistry 1. Salts of normal elements [1 [IA] to 17 (VIIA)] are generally…………………. 2. Ferrous salts are…………in colour. 3. An example of weak alkali solution…………………. 4. Both ammonium and sodium hydroxide are used in analytical chemistry for identifying.…… of salts. 5. Zinc chloride solution reacts with ammonium hydroxide solution to give a....................... coloured precipitate. 6. Calcium salts with sodium hydroxide give………precipitates. 7. Ammonium hydroxide is a weak alkali which dissociates partially to furnish………OH– ions which precipitate…………metal hydroxides.  Fill in the Blanks 9 8. Sodium zincate and water is obtained on reaction of …………with concentrated caustic soda. 9. …………… and …………salt dissolve in sodium hydroxide. 10. Oxides and hydroxides of certain metals such as…………are amphoteric in nature. 11. Amphoteric oxides and hydroxides react with an………to give salt and water only. 12. An oxide of a metal which is amphoteric in nature is……… 13. Zn(OH)2, Pb(OH)2 and Al(OH)3 are…………hydroxides. 14. ……………, a white precipitate is soluble in excess NH4 OH. Ans. 1. colourless 2. light green 3. ammonium hydroxide 4. cations 5. white 6. white 7. insufficient, soluble 8. zinc oxide 9. zinc, lead 10. zinc, lead, aluminium 11. acid as well an alkali 12. Lead oxide, PbO 13. amphoteric 14. AgCl Chapter 5. Mole Concept and Stoichiometry 1. An…………is the smaller unit of matter, which may or may not have an independent existence, but always takes part in a chemical reaction. 2. The relative molecular mass is a number that repesents how many times one……… of a 1 substance is heavier than th mass of carbon 6 C. 12 12 [ ] 3. The temperature at which all molecular motion ceases is………… 4. Whenever the gases react chemically, they do so in………… which bear a simple ratio to each other and to the products, if gaseous, provided the temperature and pressure of reacting gases and products remains the same. 5. Equal volumes of all………under similar conditions of temperature and pressure, contain equal number of molecules. 6. The mass of substance containing particles equal to Avogadro’s number is called……… 7. The number of atoms present in one molecule of a substance is its……… 8. The ratio of certain mass of a gas or vapour to the mass of same volume of hydrogen is its………. 9. The volume occupied by one mole of a gas at S.T.P is……… Ans. 1. atom 2. molecule 3. absolute zero 4. volumes 5. gases 6. mole 7. atomicity 8. vapour density 9. gram molecular volume Chapter 6. Electrolysis (a) Molten lead bromide conducts electricity. It is called an (1)........... It is composed of lead ions and bromide (2).......... The lead (3).........are (4).........charged and are called (5)............. The bromide (6).........are (7)..........charged and are called (8).......... During electrolysis, the lead (9)...........are attracted to the (10).............charged electrode which is called (11)............and the bromide. (12).............are attracted towards the (13).............. charged electrode which is called (14)............. Ans. (1) electrolyte (2) ions (3) ions (4) positively (5) cations (6) ions (7) negatively (8) anions (9) ions (10) negatively (11) cathode (12) ions (13) positively (14) anode 10 ICSE Most Likely Question Bank, Class : X (b) Solid lead (II) bromide will not conduct an (1)......................The (2)..........are held in a rigid crystal (3)............and are not free to move to the (4)............. When the solid is (5)................, it (6)..............and allows the passage of an electric current (7).............is liberated at the cathode and (8).................at the anode. The decomposition of an electrolyte by an electric current is called (9)................ Ans. (1) Electric current (2) ions (3) lattice (4) electrodes (5) heated (6) melts (7) lead (8) bromine (9) electrolysis (c) For electroplating an article with nickel require an (1) ……… which must be a solution containing (2) ……… ions. The article to be plated is placed as the (3) ……… of the cell on which the plating is carried out. The (4) ……… of the cell is made from pure nickel. The ions which are attracted to the negative electrode and discharged are called (5) ………. Ans. (1) electrolyte (2) nickel (3) cathode (4) anode (5) cations (d) 1. Electrolysis is the passage of...................... through a liquid or a solution accompanied by a...................... change. 2. An electrically charged atom is called............ 3. The solution of a substance which conducts electricity is called...................... 4. An electrolyte is a................... 5. A weak electrolyte is one which...................... 6. A strong electrolyte is one which....................... 7. Sodium chloride is................. 8. Water is......................... 9. The electrode where the current enters the electrolyte is called the........... 10. Negative electrode is called the........... 11. Cations migrate to............during electrolysis. 12. During electrolysis, anions undergo……………………at the……………… 13. The reactions occurring at the cathode during electrolysis involve…………………… 14. ………… is a non-electrolyte. 15. Pure water consists almost entirely of …………… 16. We can expect that pure water………normally conduct electricity. 17. Elements liberated at the anode during electrolysis are said to be……………… 18. In solution or in molten state a ……………… electrolyte consists almost entirely of ions. 19. As we descend the electrochemical series containing cations, the tendency of the cations to get.......................... at the cathode increases. 20. The.................... the concentration of an ion in a solution, the greater is the probability of its being discharged at its appropriate electrode. 21. In the electrolysis of acidulated water, oxygen is produced by the discharge of…………… ions at the anode. 22. ………… lead bromide does not conduct electricity. 23. Ionization is a ……………… process. 24. Hydrogen chloride ………………when dissolved in water. 25. A solution of hydrogen chloride gas in water conducts electricity because................... but a solution of hydrogen chloride gas in toluene does not conduct an electric current because................................. 26. The gas given off at cathode during the electrolysis of acidulated water is................. 27. With platinum electrodes, hydrogen is liberated at the ………… and oxygen at the ………… during the electrolysis of acidified water. Ans. 1. electricity, chemical 2. an ion 3. an electrolyte 4. good conductor of electricity 5. is feebly ionized in the solution 6. is completely ionized in the solution  Fill in the Blanks 11 7. strong electrolyte 8. a weak electrolyte 9. anode 10. cathode 11. cathode 12. oxidation, anode 13. reduction 14. sugar 15. molecules 16. will not 17. electronegative 18. strong 19. reduced 20. higher 21. OH– 22. solid 23. reversible 24. ionizes 25. it ionizes in solution to form free ions; it remains as a single molecule in solution. 26. hydrogen 27. cathode, anode Chapter 7. Metallurgy (a) X Y Normal Electronic 2,8,7 2,8,2 Configuration Nature of oxide Dissolves in water and turns Very low solubility in water. blue litmus red Dissolves in hydrochloric acid Tendency for oxidising and Tends to oxidise elements and Tends to act as a reducing reducing reactions compounds agent Electrical and Thermal Very poor electrical conductor Good electrical conductor good conductivity Poor thermal conductivity thermal conductor Tendency to form alloys and No tendency to form alloys Forms alloys amalgams Using the information above, complete the following : 1. _________ is the metallic element. 2. Metal atoms tend to have a maximum of _______ electrons in the outermost energy level. 3. Non-metallic elements tend to form______oxides while metals tend to form______oxides. 4. Non-metallic elements tend to be ________ conductors of heat and electricity. 5. Metals tend to _________ electrons and act as _________ agents in their reactions with elements and compounds. Ans. 1. Y 2. eight 3. acidic, basic 4. very poor 5. lose, reducing (b) Fill in the blanks with a suitable word in the following paragraph : In the smelting, the ore is heated (1)............................. the melting point either along or with some (2)............................. In calcination, the ore is heated (3).................... the melting point and thus no (4)..................... occurs in this process. Similar to calcination, (5).................. involves heating at high temperature but chemical change occurs here. The (6).................... is used only when ore or impurity is (7).................... in nature. Ans. (1) above (2) flux, (3) below, (4) chemical change, (5) roasting, (6) magnetic separation, (7) magnetic. (c) X is an element in the form of a powder. X, burns in oxygen and the product is soluble in water. The solution is tested with litmus. Write down only the word, which will correctly complete each of the following sentences. 1. If X is a metal, then the litmus will turn............. 2. If X is a non-metal, then the litmus will turn.............. 3. If X is a reactive metal, then..........will be evolved when X reacts with dilute sulphuric acid. 4. If X is a metal it will form........oxide, which will form.........solution with water. Ans. 1. blue, 2. red, 3. hydrogen, 4. basic, alkaline. 12 ICSE Most Likely Question Bank, Class : X (d) 1. The metal other than aluminium present both in magnalium and duralumin is……… 2. The ore from which aluminium is extracted must first be treated with...................... so that pure aluminium oxide can be obtained. 3. Aluminum is an important constituent metal in duralumin since it is………… 4. In a thermetic mixture, aluminium…………iron (III) oxide. 5. Pure aluminium oxide is dissolved in................. to make a conducting solution. 6. ………is a dark coloured crystalline solid. 7. The divalent metal whose oxide is reduced to metal by electrolysis of its fused salt is ……… 8. Pine oil used in froth floatation process act as a ………… 9. In dry cells, the zinc container acts as an ………… 10. An............... is a homogeneous mixture of two or more metals or a metal and a............... 11. The properties of an alloy are not necessarily........... between those of its.............. The M.P. of an alloy is always less than the melting point of its constituent............. 12. An alloy in which............. is present as one of the constituents is called........... alloy. 13. The alloy that contains lead is.......................... 14. The alloy of nickel and iron is known as………… 15. An alloy which is sonorous is……… 16. An alloy used for making cases for cartridges is ……… 17. The alloy used for making magnets is........................ 18........................ is a ferrous alloy. 19. Brass is an alloy of............................... 20. Bell metal is an alloy of............................ 21. Type metal is an alloy of................................. 22. Addition of Tin to………lowers the melting point of alloy solder. 23. Alnico is a mixture of..................... 24. …………is used in machine parts due to its……………tensile strength. 25. The non-metallic component in stainless steel is ……… 26. Carbon content of steel is......................... 27. Stainless steel contains......................... Ans. 1. magnesium 2. sodium hydroxide solution 3. light 4. reduces 5. cryolite 6. Iodine 7. magnesium 8. water repellant 9. anode 10. alloy, non-metal. 11. intermediate, constituents, metals. 12. iron, ferrous 13. solder 14. invar 15. bell metal 16. brass 17. alnico 18. manganese steal 19. Cu and Zn 20. Cu and Sn 21. Pb, Sn and Sb 22. lead 23. Al, Ni and Co 24. steel, high 25. carbon 26. (0.5 to 1.5)%. 27. Cr, Ni and C Chapter 8 (b). Study of Compounds : Ammonia and Nitric Acid (a) Most of the nitric acid today is manufactured by Ostwald’s process. In this process a mixture of pure dry ammonia and air in the ratio of (1) ………by volume is first compressed and then passed over (2) ………at about (3) ………°C. This results in the oxidation of ammonia into (4) ……… which combines with (5) ………of the air to give (6) ………. This is an acidic gas from which nitric acid can be obtained by simply dissolving in (7) ……….  Fill in the Blanks 13 Ans. (1) 10 : 1 (2) platinum gauze (3) 800 (4) nitric oxide (5) oxygen (6) nitrogen dioxide (7) water (b) Nitrogen and hydrogen combine in the presence of a catalyst to give (1)______ gas. When the above mentioned gas is passed through water it forms a solution which will be (2) _______ in nature and the solution contains (3)________ ions and (4) ________ ions. The above solution when added to iron (II) sulphate solution, gives a (5) ________ coloured precipitate of iron (II) hydroxide. Ans. (1) ammonia (2) alkaline (3) ammonium (4) hydroxyl (5) dirty green. (c) 1. Ammonia in liquid form is …………… 2. Ammonia gas is collected by ……… 3. Nitric acid is also called as…………… 4. The alkaline behaviour of liquor ammonia is due to the presence of ………… 5. ……………is used as a catalyst during preparation of ammonia. 6. Liquor ammonia fortis is a saturated solution of …………… 7. ……………turns turmeric paper brown. 8. The salt solution which gives white ppt. on the addition of ammonium hydroxide solution is …………… 9. Excess of ammonia reduces chlorine to ……………… 10. The gas most difficult to liquefy is……………… 11. When ammonium chloride is heated, it undergoes..................... 12. Heating ammonium chloride with sodium hydroxide produces..................... 13. Heating a solution of ammonium chloride and sodium nitrite produces..................... 14. Cold, dilute nitric acid reacts with copper to form………… 15. The reaction of …………with dil. nitric acid is an example of neutralisation reaction. 16. Lead nitrate is a…………salt of nitric acid. 17. The mineral acid obtained from conc. nitric acid on reaction with a non-metal is……… 18. A nitrate which leaves a black residue on heating is………… 19. The nitrate which on heating melts and liberates only one neutral gas is ………… 20. The oxidised product obtained on reaction with H 2 S gas and dil. HNO3 is ………… 21. Ammonium nitrate is used in preparing ……………… 22. Nitric acid is manufactured by ……………… process. Ans. 1. neutral 2. a downward displacement of air 3. aqua fortis 4. OH– ions 5. Molybdenum 6. NH 4 OH 7. Ammonia 8. magnesium chloride 9. NH 4 Cl 10. hydrogen 11. thermal dissociation 12. ammonia 13. nitrogen 14. nitric oxide 15. CaO 16. normal 17. H2SO4 18. Cu(NO 3 )2 19. NaNO3 20. sulphur 21. explosives 22. Ostwald’s 14 ICSE Most Likely Question Bank, Class : X Chapter 8 (c). Study of Compounds : Sulphuric Acid (a) The conversion of sulphur dioxide into sulphur trioxide is an (1)...........therefore, (2)...... during the reaction. The reaction is (3)......... by (4)............ At low temperature, the reaction is (5).......... so an (6).......... of 500° C and a catalyst is needed, the reaction is accompanied by (7)........... in volume and (8).................. pressure (9)……………the yield of sulphur trioxide. Ans. (1) exothermic reaction, (2) heat is evolved, (3) favoured, (4) low temperature, (5) slow, (6) optimum temperature, (7) decrease, (8) high, (9) favours. (b) 1. Sulphuric acid is a………acid. 2. The physical property of concentrated sulphuric acid that makes it valuable in preparing other acids is its......................................... 3. Sulphuric acid absorbs sulphur trioxide and forms…………… 4. The acid anhydride of sulphuric acid is................................ 5. When hot concentrated sulphuric acid is added to sulphur, it gets oxidised to……………. 6. The reduced product obtained when hydrogen sulphide reacts with conc. sulphuric acid is………… 7. The salt which reacts with dil. sulphuric acid to form insoluble ppt is………… 8. The type of salt formed when excess of caustic soda reacts with sulphuric acid is………… 9. The gas produced by the action of concentrated sulphuric acid on sodium chloride is…………. 10. The dehydrated product obtained when sugar reacts with conc. sulphuric acid is……… 11. The chemical formula of oxalic acid is………… 12. The sulphur compound used for the identification of several cations is.................... 13. An explosive prepared by using sulphuric acid is……… 14. Sulphuric acid used for making fertilizers is made by the............................... process. Ans. 1. non-volatile 2. high boiling point 3. pyrosulphuric acid 4. sulphur trioxide 5. sulphur dioxide, SO2 6. sulphur 7. Lead nitrate [Pb(NO3)2] 8. normal salt 9. HCl 10. carbon 11. C2 H2O4 12. hydrogen sulphide 13. trinitrotoluene 14. lead-chamber Chapter 9. Organic Chemistry (a) The alkanes form an (1)..................... series with the general formula (2)........................ The alkanes are (3).......................... (4)..................... which generally undergo (5)........................... reactions. Ans. 1. homologous 2. Cn H2n+2 3. saturated 4. hydrocarbons 5. substitution (b) 1................... was the first organic compound prepared in laboratory. 2. Organic compounds are generally insoluble in...................... 3. The compounds of carbon and hydrogen are called............... 4. The hydrocarbon containing only single bonds are known as............... 5. Alkanes are.............. hydrocarbons. 6. Alkanes are open-chain hydrocarbons in which the carbon atoms are joined by........................ only. 7. The four C—H bonds in the methane molecule are directed towards the corners of a regular....................... 8. Methane can be prepared by heating..................... with solid........................ 9. When methane reacts with excess of chlorine, the product obtained is................... of the molecular formula..................  Fill in the Blanks 15 10. Ethane is an......................................... 11. Ethene reacts with chlorine to give............... products. 12.................................does not react with hydrogen. 13. When methane is heated to a high temperature in the absence of oxygen, it yields................. and................. This reaction is known as................... or...................... 14. The general formula C n H2n represents............... 15. Ethene is prepared by the............... of ethyl alcohol by heating it with..................... 16. Ethene reacts with chlorine to give........................ the molecular formula of which is............................... 17................ has two carbon atoms joined by a triple covalent bond. 18. Ethene and ethyne are.................... hydrocarbons. 19................ reacts with bromine to give two different addition products. 20. Ethyne is prepared by the action of.......................... on....................... 21. When ethyne is hydrogenated, the first product is....................... and the final product is......................... 22. The conversion of ethene to ethane is an example of.......................... 23. The catalyst used in the conversion of ethene to ethane is commonly...................... 24. The product formed when ethene gas reacts with water in the presence of sulphuric acid is………… 25. The product of the dehydration of ethyl alcohol is........................... 26. The conversion of ethanol to ethene is an example of....................... 27. Converting ethanol to ethene requires the use of.............................. 28........................ is commonly called as wood spirit. 29. When acetaldehyde is oxidized with acidified potassium dichromate, it forms…… 30. Ethanoic acid reacts with ethanol in presence of concentrated H2SO4 , so as to form a compound and water. The chemical reaction which takes place is called……… 31. The ability of carbon atom to link with other carbon atom is known as............... 32. Compounds represented by a single molecular formula but having different structural formulae are called.............. and this phenomenon is known as.............. 33. The name of the compound CH2 Cl2 is................................ 34. The compound formed when ethene reacts with hydrogen is…………. 35. Conversion of ethene to ethane is an example of…………. Ans. 1. Urea 2. water 3. hydrocarbons 4. alkanes 5. saturated 6. single covalent bonds 7. tetrahedron 8. sodium acetate, sodium hydroxide 9. carbon tetrachloride, CCl4 10. alkane 11. substitution 12. Ethane 13. carbon, hydrogen, pyrolysis, cracking 14. alkene 15. dehydration, concentrated sulphuric acid 16. ethene dichloride, CH 2 Cl2 17. Ethyne 18. unsaturated 19. Ethyne 20. water, calcium carbide 21. ethene, ethane 22. hydrogenation 23. nickel 24. ethanol 25. ethene 26. dehydration 27. concentrated sulphuric acid 28. Methyl alcohol or methanol 29. acetic acid 30. esterification 31. catenation 32. isomers, isomerism 33. dichloromethane 34. Ethane 35. hydrogenation ❐ Question Set Match the Column 2 Q. Match the column A with column B : Chapter 1. Periodic Properties and Variations of Properties Column A Column B 1. Proton An alkaline earth metal 2. Sodium Halogen 3. Barium Noble gas 4. Chlorine An alkali metal 5. Electron Responsible for nuclear charge 6. Completed shell Occupied sub-shell. Ans. Column A Column B 1. Proton Responsible for nuclear charge 2. Sodium An alkali metal 3. Barium An alkaline earth metal 4. Chlorine Halogen 5. Electron Occupied sub-shell. 6. Completed shell Noble gas Chapter 2. Chemical Bonding Column A Column B 1. Metal Methane (CH4 ) 2. Covalent compound Sodium chloride (NaCl) 3. Non-polar Selenium (Se) 4. Polar Chloride ion (Cl – ) 5. Non-metal Aluminium (Al) 6. Electrovalent compound Carbon dioxide (CO 2 ) 7. Anion Hydrogen chloride (HCl) 8. Cation Potassium ion (K+) Ans. Column A Column B 1. Metal Aluminium (Al) 2. Covalent compound Carbon dioxide (CO 2 ) 3. Non-polar Methane (CH4 ) 4. Polar Hydrogen chloride (HCl) 5. Non-metal Selenium (Se) 6. Electrovalent compound Sodium chloride (NaCl) 7. Anion Chloride ion (Cl – ) 8. Cation Potassium ion (K+) Chapter 3. Study of Acids, Bases and Salts (a) Column A Column B 1. Acid salt Ferrous ammonium sulphate 2. Double salt Contains only ions 3. Ammonium hydroxide solution Sodium hydrogen sulphate 4. Dilute hydrochloric acid Contains only molecules 5. Carbon tetrachloride Contains ions and molecules  Match the Column 17 Ans. Column A Column B 1. Acid salt Sodium hydrogen sulphate 2. Double salt Ferrous ammonium sulphate 3. Ammonium hydroxide solution Contains ions and molecules 4. Dilute hydrochloric acid Contains only ions 5. Carbontetrachloride Contains only molecules (b) Column A Column B 1. Acid salt Sodium potassium carbonate 2. Mixed salt Alum 3. Complex salt Sodium carbonate 4. Double salt Sodium zincate 5. Normal salt Sodium hydrogen carbonate Ans. Column A Column B 1. Acid salt Sodium hydrogen carbonate 2. Mixed salt Sodium potassium carbonate 3. Complex salt Sodium zincate 4. Double salt Alum 5. Normal salt Sodium carbonate Chapter 4. Analytical Chemistry (a) Column A Column B 1. Copper (II) nitrate Green 2. Iron (II) sulphate White 3. Magnesium chloride Reddish brown 4. Cobalt chloride Orange 5. Iron (III) chloride Blue 6. Potassium dichromate Black 7. Copper (II) oxide Yellow Ans. Column A Column B 1. Copper (II) nitrate Green 2. Iron (II) sulphate Reddish brown 3. Magnesium chloride White 4. Cobalt chloride Blue 5. Iron (III) chloride Yellow 6. Potassium dichromate Orange 7. Copper (II) oxide Black (b) Column A Column B 1. Pb 2+ Reddish brown 2. Fe2+ White insoluble in excess 3. Zn2+ Dirty green 4. Fe3+ White soluble in excess 5. Cu2+ White insoluble in excess 6. Ca2+ Blue Ans. Column A Column B 1. Pb 2+ White soluble in excess 2. Fe2+ Dirty green 3. Zn2+ White soluble in excess 4. Fe3+ Reddish brown 5. Cu2+ Blue 6. Ca2+ White insoluble in excess 18 ICSE Most Likely Question Bank, Class : X (c) Column A Column B 1. Pb(NO3 )2 from PbO Simple displacement 2. MgCl2 from Mg Titration 3. FeCl3 from Fe Neutralization 4. NaNO3 from NaOH Precipitation 5. ZnCO3 from ZnSO4 Combination Ans. Column A Column B 1. Pb(NO3 )2 from PbO Neutralization 2. MgCl2 from Mg Simple displacement 3. FeCl3 from Fe Combination 4. NaNO3 from NaOH Titration 5. ZnCO3 from ZnSO4 Precipitation ❐ Question Set Multiple Choice Questions 3 Q. Choose the correct answer out of the four available choices A, B, C and D given under each question : Chapter 1. Periodic Properties and Variations of Properties 1. In the periodic table, alkali metals are placed in the group : (a) 1 (b) 11 (c) 17 (d) 18 2. An alkaline earth metal is : (a) Palarium (b) Calcium (c) Lead (d) Copper 3. The number of electrons present in the valence shell of halogen is : (a) 1 (b) 3 (c) 5 (d) 7 4. If an element A belongs to period 3 and Group II then it will have : (a) 3 shells and 2 valence electrons (b) 2 shells and 3 valence electrons (c) 3 shells and 3 valence electrons (d) 2 shells and 2 valence electrons 5. On moving from left to right across a period of the periodic table, the atomic size : (a) Decreases (b) Increases (c) Remains the same (d) Sometimes increases and sometimes decreases 6. On moving from left to right across a period of the periodic table, the non-metallic character of the elements : (a) Decreases (b) Increases (c) Remains the same (d) Depends on the period 7. On moving from left to right across a period of the periodic table, the ionization potential : (a) Goes up and down (b) Decreases (c) Increases (d) Remains the same 8. Ionisation potential increases over a period from left to right because the : (a) Atomic radius increases and nuclear charge increases (b) Atomic radius decreases and nuclear charge decreases (c) Atomic radius increases and nuclear charge decreases (d) Atomic radius decreases and nuclear charge increases 9. On moving from left to right across a period of the periodic table, the electron affinity of the elements in groups 1 to 7 : (a) Goes up and then down (b) Decreases and then increases (c) Increases (d) Decreases 10. An element in period 3 whose electron affinity is zero : (a) Neon (b) Sulphur (c) Sodium (d) Argon 11. Among the period 2 elements, the element which has high electron affinity is : (a) Lithium (b) Carbon (c) Chlorine (d) Fluorine 20 ICSE Most Likely Question Bank, Class : X 12. On moving from left to right across a period of the periodic table, the electronegativity : (a) Depends on the number of valence electrons (b) Remains the same (c) Decreases (d) Increases 13. Among the elements given below, the element with the least electronegativity is : (a) Lithium (b) Carbon (c) Boron (d) Fluorine 14. Which of the following would weigh the least ? (a) 2g atoms of nitrogen (b) 1 mole of silver (c) 22·4 litres of oxygen gas at 1 atmospheric pressure and 273 K (d) 6·02 × 1023 atoms of carbon [Atomic masses : Ag = 108, N = 14, O = 16, C = 12] 15. The ratio between the number of molecules in 2 g of hydrogen and 32 g of oxygen is : (a) 1 : 2 (b) 1 : 0·01 (c) 1 : 1 (d) 0·01 : 1 [Given that H = 1, O = 16] 16. An element with the atomic number 19 will most likely combine chemically with the element whose atomic number is : (a) 17 (b) 11 (c) 18 (d) 20 Ans. (1) (a) (2) (b) (3) (d) (4) (a) (5) (a) (6) (b) (7) (c) (8) (d) (9) (c) (10) (d) (11) (d) (12) (d) (13) (a) (14) (d) (15) (c) (16) (a). Chapter 2. Chemical Bonding 1. Molecular reactions which are generally slow reactions are shown by : (a) Covalent compounds (b) Ionic compounds (c) Co-ordinate compounds (d) Both ionic and covalent compounds 2. The number of electrons lost or gained by an atom refers to : (a) Electrovalency (b) Covalency (c) Donation (d) Acceptance 3. The capacity of an atom to attract the shared pair of electrons towards itself is called : (a) Electronegativity (b) Electron affinity (c) Sharing of electrons (d) Electron donation 4. Which of the following doesn’t represent oxidation ? (a) Loss of electrons (b) Addition of oxygen (c) Increase in oxidation number (d) Addition of hydrogen 5. Sodium and sodium ions : (a) Are chemically same (b) Have same number of electrons (c) Have same number of protons (d) None of the above 6. A compound which contains all the three types of bonds i.e., ionic, covalent and co- ordinate is : (a) Sodium chloride (b) Ammonia (c) Calcium chloride (d) Ammonium chloride 7. The most ionic compound of periodic table is : (a) Sodium chloride (b) Potassium chloride (c) Magnesium chloride (d) Caesium chloride 8. The molecule containing a triple covalent bond is : (a) Ammonia (b) Methane (c) Water (d) Nitrogen  Multiple Choice Questions 21 9. A compound having one lone pair of electrons : (a) Water (b) Methane (c) Ammonia (d) Hydrogen sulphide 10. A compound X consists of only molecules. Hence X will have : (a) A crystalline hard structure (b) A low melting point and low boiling point (c) An ionic bond (d) A strong force of attraction between its molecules 11. Bonding in this molecule can be understood to involve coordinate bonding : (a) Carbontetrachloride (b) Hydrogen (c) Hydrogen chloride (d) Ammonium chloride 12. Which of the following is a common characteristic of a covalent compound ? (a) High melting point (b) Consists of molecules (c) Always soluble in water (d) Conducts electricity when it is in the molten state Ans. (1) (d) (2) (a) (3) (a) (4) (d) (5) (c) (6) (d) (7) (d) (8) (d) (9) (c) (10) (b) (11) (d) (12) (b) Chapter 3. Study of Acids, Bases and Salts 1. A particular solution contains molecules and ions of the solute so it is a : (a) Weak acid (b) Strong acid (c) Strong base (d) Salt solution 2. Select the acid which contains four hydrogen atoms in it : (a) Formic acid (b) Sulphuric acid (c) Nitric acid (d) Acetic acid 3. An organic weak acid is : (a) Formic acid (b) Sulphuric acid (c) Nitric acid (d) Hydrochloric acid 4. The aqueous solution of the following compounds which contains both ions and molecules is : (a) Sulphuric acid (b) Hydrochloric acid (c) Nitric acid (d) Acetic acid 5. An acid which is not a hydro acid is : (a) H2S (b) H2SO3 (c) HBr (d) HCl 6. Which one of the following will not produce an acid when made to react with water ? (a) Carbon monoxide (b) Carbon dioxide (c) Nitrogen dioxide (d) Sulphur trioxide 7. The metal oxide which can react with acid as well as alkali is : (a) Silver oxide (b) Copper (II) oxide (c) Aluminium oxide (d) Calcium oxide 8. During ionization metals lose electrons, this change can be called : (a) Oxidation (b) Reduction (c) Redox (d) Displacement 9. The salt which in solution gives a pale green precipitate with sodium hydroxide solution and a white precipitate with barium chloride solution is : (a) Iron (III) sulphate (b) Iron (II) sulphate (c) Iron (II) chloride (d) Iron (III) chloride 22 ICSE Most Likely Question Bank, Class : X 10. An example of a complex salt is : (a) Zinc sulphate (b) Sodium hydrogensulphate (c) Iron (II) ammonium sulphate (d) Tetrammine copper (II) sulphate 11. To increase the pH value of neutral solution, we should add : (a) An acid (b) An acid salt (c) An alkali (d) A salt Ans. (1) (a) (2) (d) (3) (a) (4) (c) (5) (b) (6) (a) (7) (c) (8) (a) (9) (b) (10) (d) (11) (c). Chapter 4. Analytical Chemistry 1. Salts of which elements are generally coloured : (a) Transition (b) Normal (c) Lanthanides (d) Inner-transition. 2. Which one of the following salt solutions on reaction with excess of ammonium hydroxide solution gives a deep blue solution ? (a) FeCl3 (aq.) (b) CuSO4 (aq.) (c) Al 2 (SO4)3 (aq.). (d) ZnSO 4 (aq.) 3. Which one of the following salt solutions on reaction with excess sodium hydroxide solution gives a clear solution finally ? (a) (PbNO3 )2 (aq) (b) CuSO4 (aq) (c) FeCl3 (aq) (d) ZnSO 4 (aq.) 4. The precipitate of which of the following compounds is soluble in excess of ammonia solution ? (a) Iron (II) chloride (b) Magnesium chloride (c) Copper (II) sulphate (d) Lead nitrate 5. Which one of the following salt solutions on reaction with excess of ammonium hydroxide solution results finally in dissolution of the precipitate first formed ? (a) AlCl 3 (aq.) (b) FeSO4 (aq.) (c) Fe(SO4 )3 (aq.) (d) ZnSO 4 (aq.) 6. Hydroxide of this metal is soluble in sodium hydroxide solution. (a) Magnesium (b) Lead (c) Silver (d) Copper 7. The hydroxide which is soluble in excess of NaOH is : (a) Zn(OH)2 (b) Fe(OH)2 (c) Fe(OH)3 (d) Al(OH) 3 8. Name the reagent from the following which can be used to distinguish zinc nitrate solution from magnesium nitrate. (a) NH 4 OH (aq.) (b) NaOH (aq.) (c) BaCl2 (d) H2SO4 9. The oxide and hydroxide of which metal is amphoteric : (a) Zinc (b) Copper (c) Iron (d) Manganese 10. Anhydrous iron (III) chloride is prepared by : (a) Direct combination (b) Simple displacement (c) Decomposition (d) Neutralization 11. A chloride which forms a precipitate that is soluble in excess of ammonium hydroxide is : (a) Calcium chloride (b) Ferrous chloride (c) Ferric chloride (d) Copper chloride  Multiple Choice Questions 23 Ans. (1) (b) (2) (b) (3) (a) (4) (c) (5) (d) (6) (b) (7) (a) (8) (a) (9) (a) (10) (a) (11) (d). Chapter 5. Mole Concept and Stoichiometry 1. The temperature at which all molecular motion ceases is : (a) 0°C (b) 100°C (c) Zero power (d) Absolute zero 2. The volume occupied by 1 mole of gas at STP is : (a) 2·24 litres (b) 22·4 litres (c) 2·42 litres (d) 2·44 litres 3. The volume occupied by 7 g of nitrogen at STP is : (a) 5·4 litres (b) 4·8 litres (c) 5·6 litres (d) 4·6 litres 4. Which law states that “under the same conditions of temperature and pressure, equal volumes of all gases contain the same number of molecule.” (a) Avogadro’s law (b) Gay Lussac’s Law (c) Mole Law (d) Law of conservation of mass 5. What is the value of Avogadro number ? (a) 6·022 × 1023 (b) 6·022 × 10– 23 (c) 6·22 × 1023 (d) 6·22 × 10– 23 6. One atomic mass unit is how much part the mass of carbon-12 atoms ? 1 1 (a) (b) 4 12 1 1 (c) (d) 8 16 7. The number of atoms present in one molecule of an element is called its : (a) Molecular number (b) Atomic number (c) Avogadro's number (d) Atomicity 8. The vapour density of carbon dioxide [C = 12, O = 16] is : (a) 12 (b) 16 (c) 44 (d) 22 9. The empirical formula of hexane is : (a) C2 H7 (b) C5 H8 (c) C3 H7 (d) C4 H7 10. If empirical formula of an organic compound is CH 2 O then its molecular formula can be : (a) C2 H2O2 (b) C2 H4O (c) C3 H6O (d) C6 H12O6 Ans. (1) (d) (2) (b) (3) (c) (4) (a) (5) (a) (6) (b) (7) (d) (8) (d) (9) (c) (10) (d). Chapter 6. Electrolysis 1. Identify the weak electrolyte from the following : (a) Sodium Chloride solution (b) Dilute Hydrochloric acid (c) Dilute Sulphuric acid (d) Aqueous acetic acid 24 ICSE Most Likely Question Bank, Class : X 2. Which of these will act as a non-electrolyte ? (a) Liquid carbon tetrachloride (b) Acetic acid (c) Sodium hydroxide aqueous solution (d) Potassium chloride aqueous solution 3. During ionisation metals lose electrons, this change can be called : (a) Oxidation (b) Reduction (c) Redox (d) Displacement 4. The metallic electrode which does not take part in an electrolytic reaction. (a) Cu (b) Ag (c) Pt (d) Ni 5. When dilute sodium chloride is electrolysed using graphite electrodes, the cation is discharged at the cathode most readily. (a) Na+ (b) OH– (c) H+ (d) Cl– 6. During electrolysis of NaCl, the gas released at anode is : (a) Chlorine (b) Oxygen (c) Hydrogen (d) None of the above 7. During the electrolysis of molten lead bromide which of the following takes place : (a) Bromine is released at the cathode (b) Lead is deposited at the anode (c) Bromine ions gain electrons (d) Lead is deposited at the cathode 8. A compound which liberates reddish brown gas around the anode during electrolysis in its molten state is : (a) Sodium chloride (b) Copper (II) oxide (c) Copper (II) sulphate (d) Lead (II) bromide 9. When fused lead bromide is electrolysed we observe : (a) a silver grey deposit at anode and a reddish brown deposit at cathode (b) a silver grey deposit at cathode and a reddish brown deposit at anode (c) a silver grey deposit at cathode and reddish brown fumes at anode (d) silver grey fumes at anode and reddish brown fumes at cathode. 10. The vessel in which electrolysis of Lead bromide is carried out is : (a) Clay crucible (b) Glass vessel (c) Silica crucible (d) Aluminium vessel 11. The ion which is discharged at the cathode during the electrolysis of copper sulphate solutions using copper electrodes as anode and cathode. (a) Cu2+ (b) OH– (c) SO4 2– (d) H+ 12. An aqueous electrolyte consists of the ions mentioned in the list, the ion which could be discharged most readily during electrolysis. (a) Fe2+ (b) Cu2+ (c) Pb 2+ (d) H+ 13. During silver plating of an article using potassium argentocyanide as an electrolyte, the anode material should be : (a) Cu (b) Ag (c) Pt (d) Fe 14. The particles present in strong electrolytes are : (a) only molecules (b) mainly ions (c) ions and molecules (d) only atoms  Multiple Choice Questions 25 Ans. (1) (d) (2) (a) (3) (a) (4) (c) (5) (c) (6) (b) (7) (d) (8) (d) (9) (c) (10) (c) (11) (a) (12) (b) (13) (b) (14) (b) Chapter 7. Metallurgy 1. An element of an inorganic compound found in nature is known as : (a) Mineral (b) Ore (c) Both (a) and (b) (d) None of these 2. Which one of the following is not true of metals ? (a) Metals are good conductors of electricity. (b) Metals are malleable and ductile. (c) Metals form non-polar covalent compounds. (d) Metal will have 1 or 2 or 3 electrons in their valence shell. 3. Which ore is metalloid ? (a) C (b) Germanium (c) Si (d) Tin 4. A chemical process of extracting a metal from its ore is known as : (a) Mineralogy (b) Metallurgy (c) Liquation (d) None of the above 5. A mineral from which the metal is extracted economically is known as : (a) Matrix (b) Gangue (c) Ore (d) None of these 6. An unwanted earthly material associated with tin ore as impurity is known as : (a) Gangue (b) Flux (c) Froth (d) None of these 7. The process of heating the ore strongly in excess of air so that the volatile impurities are removed and the ore is changed to oxide is known as : (a) Calcination (b) Roasting (c) Froth floatation (d) Leaching 8. Heating an ore in a limited supply of air or in the absence of air at a temperature just below its melting point is known as : (a) Smelting (b) Ore dressing (c) Calcination (d) Bessemerisation 9. Smelting is carried out in : (a) Blast furnace (b) Muffle furnace (c) Open Heat furnace (d) Electric furnace 10. The salt which is least likely to be found in minerals is : (a) Chloride (b) Sulphate (c) Sulphite (d) Nitrate 11. The commonest method of extraction of metals from oxide ores involves : (a) Reduction with carbon (b) Reduction with aluminium (c) Reduction with hydrogen (d) Electrolytic method 12. Froth floatation process for the concentration of ores is an illustration of the practical application of : (a) Adsorption (b) Absorption (c) Sedimentation (d) Coagulation 13. In the froth floatation process for the purification of ores, the ore particles float because : (a) They are light (b) Their surface is not easily wetted by water (c) They bear electrostatic charge (d) They are insoluble 26 ICSE Most Likely Question Bank, Class : X 14. Froth floatation method may be used to increase the concentration of mineral in : (a) Chalcopyrites (b) Bauxite (c) Haematite (d) Calamine 15. Sulphide ore is generally concentrated by : (a) Roasting (b) Froth floatation process (c) Reduction by carbon (d) Tempering 16. The main ore used for the extraction of iron is : (a) Haematite (b) Calamine (c) Bauxite (d) Cryolite 17. The process used to convert impure alumina to pure alumina is : (a) Roasting (b) Electrolytic refining (c) Purification (d) Baeyer’s Process 18. The part of fluorspar (CaF 2 ) which is added in small quantities in the electrolytic reduction of alumina dissolved in fused cryolite (Na3 AIF6 ) is : (a) As a catalyst (b) To make the fused mixture very conducting (c) To lower the temperature of the melt (d) To decrease the rate of oxidation of carbon at the anode 19. The electrolyte used for electroplating an article with silver is : (a) Silver nitrate solution (b) Silver cyanide solution (c) Sodium argentocyanide solution (d) Nickel sulphate solution 20. Aluminium powder is used in thermite welding because : (a) It is a strong reducing agent (b) It is a strong oxidising agent (c) It is corrosion resistant (d) It is a good conductor of heat 21. The metals zinc and tin are present in the alloy : (a) Solder (b) Brass (c) Bronze (d) Duralumin 22. In electrolytic refining of metals the impure metal is made : (a) Cathode (b) Salt bridge (c) Anode (d) Electrode 23. Stainless steel does not contain : (a) Cr (b) Al (c) C (d) Ni 24. This is not an alloy of copper : (a) Brass (b) Bronze (c) Solder (d) Duralumin 25. The two main metals in bronze are : (a) Copper and zinc (b) Copper and lead (c) Copper and nickel (d) Copper and tin Ans. (1) (a) (2) (c) (3) (a) (4) (b) (5) (c) (6) (a) (7) (b) (8) (c) (9) (a) (10) (d) (11) (a) (12) (b) (13) (b) (14) (a) (15) (b) (16) (a) (17) (d) (18) (c) (19) (c) (20) (a) (21) (c) (22) (c) (23) (b) (24) (d) (25) (c).  Multiple Choice Questions 27 Chapter 8 (a). Study of Compounds : Hydrogen Chloride 1. An aqueous solution of HCl gas is named. (a) Aqua fortis (b) Aqua regia (c) Oil of vitriol (d) Muriatic acid 2. An acid which is not a monobasic acid. (a) HNO3 (b) HCOOH (c) H2SO4 (d) HCl 3. An acid which is not an oxidising agent. (a) H2SO4 (b) HCl (c) HNO3 (d) CH3COOH 4. Hydrogen chloride gas being highly soluble in water is dried by : (a) Anhydrous calcium chloride (b) Phosphorous penta oxide (c) Quick lime (d) Concentrated sulphuric acid 5. A substance which reacts with conc. HCl to liberate chlorine : (a) PbO (b) PbCl 2 (c) PbO2 (d) Pb 3 O4 6. A metal which reacts with dil HCl to liberate hydrogen. (a) Zn (b) Cu (c) Ag (d) Pb 7. Gas liberated when dil. HCl gas is added to iron (II) sulphide. (a) Hydrogen gas (b) Chlorine gas (c) Hydrogen sulphide gas (d) Carbon dioxide gas 8. Gas liberated when hydrochloric acid reacts with galena. (a) Sulphur dioxide (b) Carbon dioxide (c) Nitrogen (d) Hydrogen sulphide 9. The gases which react chemically to form a solid : (a) H2(g) and Cl2 (g) (b) NH 3 (g) and HCl(g) (c) CO2(g) and SO2(g) (d) NO2(g) and CO2(g) 10. Constant boiling mixtures are known as : (a) Constant compounds (b) Woulfe’s compound (c) Distillators (d) Azeotropes 11. Aqua regia is a mixture of : (a) Dilute hydrochloric acid and concentrated nitric acid (b) Concentrated hydrochloric acid and dilute nitric acid (c) Concentrated hydrochloric acid [1 part] and concentrated nitric acid [3 parts] (d) Concentrated hydrochloric acid [3 parts] and concentrated nitric acid [1 part] 12. The aim of the fountain experiment is to prove that : (a) HCl turns blue litmus red (b) HCl is denser than air (c) HCl is highly soluble in water (d) HCl fumes in moist air Ans. (1) (d) (2) (c) (3) (b) (4) (d) (5) (c) (6) (a) (7) (c) (8) (d) (9) (b) (10) (d) (11) (d) (12) (c). Chapter 8 (b). Study of Compounds : Ammonia and Nitric Acid 1. Ammonia can be obtained by adding water to : (a) Ammonium chloride (b) Ammonium nitrite (c) Magnesium nitride (d) Magnesium nitrate 2. Ammonia is soluble in water because : (a) A polar molecule (b) An acid (c) A base (d) A simple covalent compound 28 ICSE Most Likely Question Bank, Class : X 3. Nitrogen gas can be obtained by heating : (a) Ammonium nitrate (b) Ammonium nitrite (c) Magnesium nitride (d) Ammonium chloride 4. The nitrate which evolves laughing gas on decomposition : (a) Ferric nitrate (b) Calcium nitrate (c) Sodium nitrate (d) Ammonium nitrate 5. Rotten egg smell is due to the liberation of : (a) HCl gas (b) Cl2 gas (c) H2S gas (d) SO2 gas 6. The temperature at which catalytic oxidation of ammonia is carried out : (a) 200°C (b) 800°C (c) 1000°C (d) 500°C 7. With excess of chlorine, NH 3 forms : (a) NH 4 Cl (b) NCl3 (c) NOCl (d) N2Cl 8. Liquid NH3 is employed in refrigerator, because : (a) It is more basic (b) It is stable hydride (c) It has a high dipole moment (d) It has high heat of evaporation 9. Ammonia nitrate is used in : (a) Lining vessels (b) Paints (c) Textile industry (d) Preparing explosives 10. The brown ring test is used for the detection of : 2– – (a) CO3 (b) NO3 2– (c) SO 3 (d) Cl– 11. The composition of brown ring formed at the junction is : (a) FeSO4.OH (b) FeSO4.NO (c) FeSO4.H2 O (d) FeSO4 12. Which acid is prepared by Ostwald’s process : (a) Nitric acid (b) Oleic acid (c) Sulphuric acid (d) Tartaric acid Ans. (1) (c) (2) (a) (3) (b) (4) (d) (5) (c) (6) (b) (7) (b) (8) (d) (9) (d) (10) (b) (11) (b) (12) (a). Chapter 8 (c). Study of Compounds : Sulphuric Acid 1. Pyrosulphuric acid is the chemical name of : (a) Green vitriol (b) White vitriol (c) Oleum (d) Gypsum 2. In the given equation identify the role played by concentrated sulphuric acid S + 2H 2 SO4 ⎯→ 3SO2 + 2H2O : (a) Non-volatile acid (b) Oxidising agent (c) Dehydrating agent (d) None of the above 3. When dilute sulphuric acid reacts with iron sulphide, the gas evolved is : (a) Hydrogen sulphide (b) Sulphur dioxide (c) Sulphur trioxide (d) Vapour of sulphuric acid  Multiple Choice Questions 29 4. When sulphuric acid is added to sodium carbonate brisk effervesence is produced which is due to : (a) Evolution of H2 S gas (b) Evolution of Cl2 gas (c) Evolution of CO2 gas (d) Evolution of O2 gas 5. When hot concentrated sulphuric acid is added to sulphur it gets oxidised to : (a) H2 S (b) SO2 (c) O3 (d) HSO4 6. When concentrated sulphuric acid reacts with NaOH, the product formed is : (a) Sodium hydroxide (b) Sodium sulphate (c) Sodium carbonate (d) Sodium hydrogen sulphate 7. Dilute sulphuric acid will produce a white precipitate when added to a solution of : (a) Copper nitrate (b) Zinc nitrate (c) Lead nitrate (d) Sodium nitrate 8. Corrosive action of H2 SO4 on skin is due to : (a) Exothermic nature (b) Volatile nature (c) Dehydrating character (d) Oxidising nature 9. Nitroglycerine and nitrotoluene are : (a) Fertilizers (b) Explosives (c) Fibres (d) Detergents 10. The molecular formula of epsom salt is : (a) MgSO4 · 5H2 O (b) FeSO4 · 7H2O (c) MgSO4 · 7H2 O (d) MgSO4 · 6H2 O Ans. (1) (c) (2) (b) (3) (a) (4) (c) (5) (b) (6) (b) (7) (c) (8) (c) (9) (b) (10) (a). Chapter 9. Organic Chemistry 1. The property of carbon of form chains and rings is called : (a) Catenation (b) Polymerisation (c) Cracking (d) Hydrogenation 2. Two neighbours of a homologous series differ by : (a) CH (b) CH2 (c) CH3 (d) CH4 3. Heating sodium acetate with soda lime produces : (a) Methane (b) Ethane (c) Ethene (d) Ethyne 4. The number of C–H bonds in ethane molecule are : (a) Four (b) Six (c) Eight (d) Ten 5. Halogenation of alkane can be carried out in : (a) Dark (b) Bright light (c) UV light (d) Diffused sunlight 6. The unsaturated hydrocarbons undergo : (a) a substitution reaction (b) an oxidation reaction (c) an addition reaction (d) None of the above 30 ICSE Most Likely Question Bank, Class : X 7. An organic compound undergoes addition reactions and gives a red colour precipitate with ammoniacal cuprous chloride. Therefore, the organic compound could be (a) Ethane (b) Ethene (c) Ethyne (d) Ethanol 8. The I.U.P.A.C. name of acetylene is : (a) Propane (b) Propyne (c) Ethene (d) Ethyne 9. Acetylene polymerises into benzene by joining : (a) 3 molecules (b) 2 molecules (c) 4 molecules (d) 6 molecules 10. The organic compound mixed with ethanol to make it spurious is : (a) Methanol (b) Methanoic acid (c) Methanal (d) Ethanoic acid 11. Dehydrohalogenation of X with alcoholic KOH produces ethene. X is : (a) Ethyl chloride (b) Methyl chloride (c) Ethylene dichloride (d) None 12. The functional group present in acetic acid is : (a) Ketonic C=O (b) Hydroxyl —OH (c) Aldehydic —CHO (d) Carboxyl —COOH 13. The resulting ester, when ethyl alcohol and acetic acid are mixed together : (a) CH3COOCH3 (b) C2 H5COOC2 H5 (c) CH3COOC2 H5 (d) C2 H5COOCH3 14. An acid used for removing ink stains : (a) Acetic acid (b) Oxalic acid (c) Malic acid (d) Formic acid 15. Which compound is used as an antifreeze agent : (a) Propene (b) Acetylene (c) Ethylene glycol (d) Methanol 16. Identify the statement which does not describe the property of alkenes : (a) They are unsaturated hydrocarbons (b) They decolourise bromine water (c) They can undergo addition as well as substitution reactions (d) They undergo combustion with oxygen forming carbon dioxide and water 17. If the molecular formula of an organic compound is C10H18 it is : (a) Alkene (b) Alkane (c) Alkyne (d) Not a hydrocarbon Ans. (1) (a) (2) (b) (3) (a) (4) (b) (5) (d) (6) (c) (7) (c) (8) (d) (9) (a) (10) (a) (11) (a) (12) (d) (13) (c) (14) (b) (15) (c) (16) (c) (17) (c). ❐ Question Set Give One Word/Chemical Term 4 Chapter 1. Periodic Properties and Variations of Properties 1. The law that groups elements in family of three. 2. The law where every 8th element repeats properties. 3. The law where repetition of properties varies periodically. 4. Horizontal arrangement of elements. 5. Vertical arrangement of elements. 6. The elements present in the first period. 7. The first three alkali metals. 8. Elements with 1, 2 or 3 electrons in