1 霹雳怡保培南独立中学 SM POI LAM (SUWA) IPOH 2 nd MONTHLY TEST 2021 Chemistry DATE: TIME : 6-8-2021 1105-1235 (90 minutes) NAME：______________________ REG NO:_________________ CLASS：S1QI/S1HE Multiple choice 30 questions. (45 marks) 1. In an experiment, 15.0 cm3 of 0.01 mol/dm3 copper(II) sulfate solution is mixed with 5.0 cm3 of 0.01 mol/dm3 sodium carbonate solution in a flask. The equation is shown below. CuSO4 + Na2CO3 → Na2SO4 + CuCO3 What is seen in the flask when the reaction was completed? A. A colourless solution only. B. A green precipitate and a blue solution. C. A green precipitate and a colourless solution. D. A white precipitate and a colourless solution. 2. A dilute aqueous solution of a strong acid, HX, contains molecules of water and the ions H+ and X - . Which statement is correct? A. The pH value of the acid is above 7. B. The solution contains a high concentration of HX molecules. C. The solution also contains OHions. D. The solution contains more H+ ions than water molecules. __________________________________________________________________________________________ This paper consists of 16 printed pages Prepared by ： ………………… (Miss Khoo Yen Teng) Checked by： ………………… (Mr Loke Wai Chuan)
2 3. The diagram below shows the reactions of solution X. What is a possible identity of solution X? A. aluminium chloride B. calcium nitrate C. lead(II) chloride D. zinc nitrate 4. Which of the following reagents can be used to prepare a salt that would involve the steps shown by the diagram below? A. lead(II) carbonate with dilute nitric acid to prepare lead(II) nitrate B. calcium sulfate with dilute hydrochloric acid to prepare calcium chloride C. copper(II) chloride with dilute sulfuric acid to prepare copper (II) sulfate D. sodium carbonate with dilute sulfuric acid to prepare sodium sulfate 5. The statements below give some information about metals R, S, T and U. • Carbonate of U does not decompose on heating. • Only oxides of R and T can be reduced by heating with carbon. • R and S react with dilute hydrochloric acid but not with cold water. • T reacts with neither dilute hydrochloric acid nor water. What is the order of increasing reactivity of the four metals? A. T < R < S < U B. T < S < R < U C. U < S < R < T D. U < T < R < S
3 6. Which of the following is the most powerful reducing agent? A. chlorine atom B. sodium atom C. fluoride ion D. iodide ion 7. Which pair of substance acts as reducing agents in the blast furnace? A. carbon and oxygen B. carbon monoxide and carbon dioxide C. carbon and carbon monoxide D. carbon dioxide and oxygen 8. The formulae of some oxide are shown below Na2O MgO Al2O3 SO2 CO2 Which row in the table below gives the correct number of each type of oxide? Number of each type of oxide Acidic Amphoteric Basic A 1 2 2 B 2 0 3 C 1 1 3 D 2 1 2 9. The labels fell off two bottles each containing a colourless solution, one of which was potassium carbonate solution and other was potassium chloride solution. Which of the following tests would allow the identification of the solutions? A. Addition of lead (II) nitrate solution B. Addition of sodium hydroxide solution C. Addition of aqueous ammonia D. Addition of nitric acid 10. Which of the following is expected of a metal that is positioned between aluminium and lead in the reactivity series? A. It forms a hydroxide that dissolves in water. B. It forms an oxide that decomposes to form the metal on heating. C. It liberates hydrogen from dilute hydrochloric acid. D. It reacts with aluminium oxide when heated.
4 11. Brass, made of copper and zinc, is suitable to make musical instruments as compared to pure copper because brass is harder than pure copper. Which statement best explains why brass is harder than pure copper? A. The zinc atoms have more valence electrons than copper atoms. B. The zinc atoms form strong metallic bonds with copper atoms in brass. C. The zinc atoms prevent the ‘sea of electrons’ from moving freely in the lattice. D. The zinc atoms prevent layers of copper atoms from sliding over each other easily. 12. Which of the following can be used to distinguish between aqueous zinc nitrate and aqueous calcium chloride? 1 aqueous sodium carbonate 2 aqueous lead(II) nitrate 3 dilute sulfuric acid A. 2 only B. 1 and 2 C. 2 and 3 D. 1 and 3 13. Different types of steel differ in how much carbon they contain. What are the properties of a high carbon steel? A. strong and brittle B. soft and easily shaped C. soft and brittle D. strong and easily shaped 14. Which is not an essential raw material in the extraction of iron in a blast furnace? A. air B. coke C. haematite D. bauxite
5 15. The following tables gives some information about four solutions P, Q, R and S of the same concentration. Solution Effect of adding zinc Electrical conductivity Effect of warming ammonium chloride P No effervescence Low Ammonia gas Q Effervescence High No change R No effervescence High Ammonia gas S Effervescence Low No change What is the order of the solutions in increasing pH? A. Q, S, P, R B. P, R, S, Q C. S, Q, P, R D. R, P, S, Q 16. Which statement about the production of iron from iron (III) oxide in the blast furnace is correct? A. Calcium carbonate removes the basic impurities. B. Carbon is oxidised to carbon monoxide by carbon dioxide. C. Carbon monoxide oxidises iron (III) oxide to iron. D. Molten iron floats on the molten slag. 17. Which of the following statements correctly describe a trend in the properties of the elements across the period 3 of the periodic table? A. The ability of the elements to conduct electricity increases B. The number of neutrons in the atom increases C. The number of valency electron decrease by 1 D. The tendency to gain electron increases 18. Which of the following statements concerning the element caesium is not consistent with its position in group I? A. It is stronger reducing agent than potassium B. It reacts with chlorine to form an ionic compound C. It has a higher density than sodium D. It has a higher melting point than lithium 19. Methods used to stop iron from rusting include: coating with zinc, connection to magnesium rods Which metal is most often used to protect iron in food containers, in oil pipelines and in roofing sheets? Food containers Oil pipelines Roofing sheets A Magnesium Tin Zinc B Tin Zinc magnesium C Tin magnesium Zinc D Zinc magnesium Tin
6 20. Which process is involved in the extraction of zinc from zinc ore? A. Cryolite is added to lower the melting point of zinc ore. B. Molten zinc ore is electrolysed. C. Zinc ore is heated with carbon. D. Zinc ore is roasted in air. 21. Hydrogen chloride gas is soluble in both methylbenzene, an organic solvent, and in water. In an experiment, hydrogen chloride gas is bubbled into the different solvents. When a few drops of Universal Indicator solution is added into flask A, the indicator remained green but when added to flask B, it turned red. What could be the reason? A. HCl does not produce hydrogen ions in methylbenzene B. HCl undergoes a redox reaction with methylbenzene C. HCl neutralises the Universal Indicator solution D. HCl neutralises methylbenzene 22. Which reaction occurring in the blast furnace is a neutralisation reaction? A. C + CO2 →2CO B. CaCO3 → CaO + CO2 C. CaO + SiO2 →CaSiO3 D. Fe2O3 + 3CO →2Fe + 3CO2 23. The diagram shows the structure of an alloy. Which statement about alloys is correct? A. Alloys can only be formed by mixing copper or iron with other metals. B. Turning a metal into alloy does not change its properties. C. In an alloy there is attraction between positive ions and a ‘sea of electrons’. D. The alloy brass contains 70% copper and 30% tin
7 24. The table below shows the result of heating the carbonates and nitrates of three metals to the same temperature Metal Products of decomposition Metal carbonate Metal nitrate W No change Metal nitrite and oxygen X Metal oxide and carbon dioxide Metal oxide, nitrogen dioxide and oxygen Y No change Metal oxide, nitrogen dioxide and oxygen What is the order of these metals in the reactivity series likely to be? Most reactive least reactive A W X Y B W Y X C X Y W D Y W X 25. The apparatus used for the extraction of aluminium oxide by electrolysis is shown Which equation represents a reaction taking place at the anode? A. C + O2 → CO2 B. Al3+ +3e- → Al C. O 2-→ O2 + 2eD. O2 + 4e-→ 2O2- 26. The list shows the position of metal X in the reactivity series of metals. Na Al Ni X Cu Au Which methods could be used to extract metal X? 1 electrolysis of the solid metal oxide 2 heating the metal oxide with carbon 3 heating the metal oxide with copper A. 1, 2 and 3 B. 1 and 2 only C. 2 and 3 only D. 2 only
8 27. Aluminium is used to make saucepans because of its apparent lack of reactivity. Which property of aluminium explains its unreactivity? A. It has a low density. B. It does not resist corrosion. C. It is in Group III of the Periodic Table. D. It has a layer of oxide on its surface. 28. In an accident at a factory, some nitric acid was spilt. Which substance, when added in excess, neutralises the acid without leaving an alkaline solution? A. aqueous ammonia B. aqueous sodium hydroxide C. calcium carbonate D. distilled water 29. Which is not a product of the following reaction sequence? A. Copper B. iron(III) oxide C. oxygen D. water vapour 30. in a titration between acid (in burette) and an alkali, you need to reuse the same titration flask Which is the best procedure for rinsing the flask A. rinse with distilled water then with the alkali B. rinse with tap water and then with distilled water C. rinse with distilled water and then with the acid D. only rinse with alkali
9 Subjective questions. (55 marks) 1. Use the list of substances to answer the questions. ammonia ammonium sulfate nitrogen dioxide calcium sulfate slaked lime potassium nitrate water vapour coke hydrogen lead(II) nitrate limestone Each substance can be used once, more than once or not at all A. Which substance liberates a colourless gas when added to sulfuric acid? ___________________________________________________________________[1] B. Which substance can be prepared by reacting an acid with an alkali? ___________________________________________________________________[1] C. Which substance is displaced from its salts in alkaline conditions? ___________________________________________________________________[1] D. Which substance is added to remove impurities during the extraction of iron in the blast furnace? ___________________________________________________________________[1] E. Which substance can be used to detect the presence of chloride ions in an aqueous solution? ___________________________________________________________________[1] F. Which substance is used to extract zinc from zinc oxide? ___________________________________________________________________[1] G. Which substance release a brown gas when break down by using heat. ___________________________________________________________________[1] Total: [7]
10 2. Nitrogenous fertilisers are soluble salts used to increase crop yield. Two commonly used nitrogenous fertilisers are ammonium chloride and ammonium phosphate. A. Ammonium chloride can be prepared by reacting aqueous ammonia with dilute hydrochloric acid. Write an ionic equation with state symbol for this reaction. _________________________________________________________________[2] B. Ammonium phosphate can be prepared by reacting dilute phosphoric acid and aqueous ammonia. Phosphoric acid is a weak acid. i. Describe the difference between strong and weak acids. _____________________________________________________________________ __________________________________________________________________[1] ii. Describe a chemical test to distinguish the strong acid and the weak acid. _____________________________________________________________________ _____________________________________________________________________ ___________________________________________________________________[2] C. Suggest why slaked lime should not be added to soil together with ammonium fertilisers such as ammonium chloride. Use an equation to support your answer. _____________________________________________________________________ _____________________________________________________________________ ___________________________________________________________________[4] Total: [9]
11 3. A. The diagram shows a wire fence which is held up by steel posts. The fence was recently blown down by strong winds. It was found that the steel posts had rusted badly at ground level. I. Suggest one reason why the steel posts had rusted much more at the ground level as shown in the diagram. __________________________________________________________________[1] II. One way to protect the steel post is by galvanising. Explain how galvanising protects against rusting and why galvanising is preferred to painting. _____________________________________________________________________ ___________________________________________________________________[2] B. Use your knowledge of the structure of metals to explain why steel is stronger than pure iron. You must include a labelled diagram in your answer. ___________________________________________________________________________ _________________________________________________________________________[3] C. Draw a labelled diagram to show how a steel rod can be electroplated with copper. [2]
12 D. Transition metals have characteristic physical properties such as good electrical and thermal conductivity. Give two chemical properties which are characteristic of transition metals. ___________________________________________________________________________ _________________________________________________________________________[2] Total:[10] 4. Sodium nitrate, NaNO3 is a soluble salt, is a kind of salt that has long been used to preserve foods. Using standard laboratory apparatus and reagents, explain how you would obtain dry crystals of sodium nitrate. Your answer must Include a balance chemical equation _____________________________________________________________________ _____________________________________________________________________ _____________________________________________________________________ _____________________________________________________________________ _____________________________________________________________________ _____________________________________________________________________ _____________________________________________________________________ ___________________________________________________________________ Total:[6]
13 5. A. Chromium is a transition element and is often added to steel to make stainless steel. The iron in the stainless steel does not rust due to the formation of a thin layer of chromium(III) oxide that forms over the steel object over time. A student investigated the reactivity of three metals, zinc, chromium and copper by placing a small amount of each metal into the aqueous nitrate solutions of the other two metals. The results are shown in the table below. I. zinc nitrate(aq) chromium(III) nitrate(aq) copper(II) nitrate(aq) zinc chromium copper Complete the table of the remaining six reactions. If there is reaction occur, put () ; if there is no reaction, put (✘) [3] II. Write an ionic equation for the reaction that occurs when zinc is placed in aqueous chromium(III) nitrate. _________________________________________________________________[2] III. Arrange iron, chromium, copper and zinc in decreasing order of chemical reactivity _________________________________________________________________[1] B. I. Describe the observation when zinc powder added into copper (II) nitrate. __________________________________________________________________ ________________________________________________________________[2] II. is the reaction above exothermic or endothermic? Explain your answer. _________________________________________________________________[1]
14 C. The graph below shows the rate of decomposition of three different carbonates. In each experiment, 0.010 moles of the metal carbonate was heated to the same temperature. The volume of carbon dioxide gas produced was measured every minute. Time/min I. Sketch on the same axes, label the graph of magnesium carbonate [1] II. How could you tell from the graph that the decomposition of the carbonates was not completed . ___________________________________________________________________[1] III. Which carbonate decomposed at the slowest rate? Explain you answer. ________________________________________________________________________ _____________________________________________________________________[2] IV. Suggest the trend between the reactivity of the metals and the rate of thermal decomposition of their carbonates ______________________________________________________________________[1] Total: [14] Volume of carbon dioxide (Cm3 ) CuCO3 ZnCO3 CaCO3
15 6. Zinc is extracted from its ore. The ore contains zinc sulfide. The zinc sulfide is roasted in air to produce zinc oxide and sulfur dioxide. A. Calculate the mass of zinc in 30.0 tonnes of ZnS Mass of zinc:______tonnes [1] B. I. Give the name of the ore of zinc that contains zinc sulphide ______________________________________________________________________[1] II. Write a chemical equation for the reaction that takes place when zinc sulfide is roasted in air ______________________________________________________________________[2] III. Then the oxide can be heated with carbon .write a balance chemical equation of this reaction ______________________________________________________________________[1] C. I. Zinc oxide is reacted with dilute sulfuric acid to form aqueous zinc sulfate. Construct the equation for this reaction ______________________________________________________________________[1] II. Pure zinc is made by the electrolysis of aqueous zinc sulfate. Zinc forms at the negative electrode. Hydroxide ions react at the positive electrode. Construct the equations for the reactions at both electrodes. Anode:________________________________________________________________ Cathode:______________________________________________________________[2] D. State one use of zinc metal ______________________________________________________________________[1] Total:[9]
The Periodic Table of Elements Group I II III IV V VI VII VIII Key 1 H hydrogen 1 2 He helium 4 3 Li lithium 7 4 Be beryllium 9 atomic number atomic symbol name relative atomic mass 5 B boron 11 6 C carbon 12 7 N nitrogen 14 8 O oxygen 16 9 F fluorine 19 10 Ne neon 20 11 Na sodium 23 12 Mg magnesium 24 13 Al aluminium 27 14 Si silicon 28 15 P phosphorus 31 16 S sulfur 32 17 Cl chlorine 35.5 18 Ar argon 40 19 K potassium 39 20 Ca calcium 40 21 Sc scandium 45 22 Ti titanium 48 23 V vanadium 51 24 Cr chromium 52 25 Mn manganese 55 26 Fe iron 56 27 Co cobalt 59 28 Ni nickel 59 29 Cu copper 64 30 Zn zinc 65 31 Ga gallium 70 32 Ge germanium 73 33 As arsenic 75 34 Se selenium 79 35 Br bromine 80 36 Kr krypton 84 37 Rb rubidium 85 38 Sr strontium 88 39 Y yttrium 89 40 Zr zirconium 91 41 Nb niobium 93 42 Mo molybdenum 96 43 Tc technetium – 44 Ru ruthenium 101 45 Rh rhodium 103 46 Pd palladium 106 47 Ag silver 108 48 Cd cadmium 112 49 In indium 115 50 Sn tin 119 51 Sb antimony 122 52 Te tellurium 128 53 I iodine 127 54 Xe xenon 131 55 Cs caesium 133 56 Ba barium 137 57–71 lanthanoids 72 Hf hafnium 178 73 Ta tantalum 181 74 W tungsten 184 75 Re rhenium 186 76 Os osmium 190 77 Ir iridium 192 78 Pt platinum 195 79 Au gold 197 80 Hg mercury 201 81 Tl thallium 204 82 Pb lead 207 83 Bi bismuth 209 84 Po polonium – 85 At astatine – 86 Rn radon – 87 Fr francium – 88 Ra radium – 89–103 actinoids 104 Rf rutherfordium – 105 Db dubnium – 106 Sg seaborgium – 107 Bh bohrium – 108 Hs hassium – 109 Mt meitnerium – 110 Ds darmstadtium – 111 Rg roentgenium – 112 Cn copernicium – 114 Fl flerovium – 116 Lv livermorium – lanthanoids actinoids The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.). 16 57 La lanthanum 139 58 Ce cerium 140 59 Pr praseodymium 141 60 Nd neodymium 144 61 Pm promethium – 62 Sm samarium 150 63 Eu europium 152 64 Gd gadolinium 157 65 Tb terbium 159 66 Dy dysprosium 163 67 Ho holmium 165 68 Er erbium 167 69 Tm thulium 169 70 Yb ytterbium 173 71 Lu lutetium 175 89 90 91 92 93 94 95 96 97 98 99 100 101 102 103 Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr actinium thorium protactinium uranium neptunium plutonium americium curium berkelium californium einsteinium fermium mendelevium nobelium lawrencium – 232 231 238 – – – – – – – – – – –