1. Which of the following hazard warning labels should be displayed on the reagent bottle storing sodium carbonate?

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1 Sing Yin Secondary School Final Examination, Chemistry Form Four Time allowed: 2 hours Instructions: Answer ALL questions A Periodic Table is printed on page 9 of this question paper. Atomic numbers and relative atomic masses of elements can be obtained from the Periodic Table. SECTION A: Multiple Choice Questions (35%) Answer ALL questions, mark the answers on the multiple choice answer sheet provided. 1. Which of the following hazard warning labels should be displayed on the reagent bottle storing sodium carbonate? (1) (2) (3) A. (1) only B. (2) only C. (1) and (3) only D. (2) and (3) only 2. Element Q belongs to Group II of the Periodic Table. It combines with element R to give an ionic compound with chemical formula Q 3 R 2. Which group of the Periodic Table does R belong to? A. Group III B. Group V C. Group VI D. Group VII 3. Element X has three isotopes, 86 X, 87 X and 88 X. The graph on the right shows the relative abundance of the isotopes. What is the relative atomic mass of X? A B C D. 88.1

2 F.4 Final Exam Chemistry Page 2 of 9 4. What colour can be observed when a sample of solid potassium chloride is heated in a Bunsen flame? A. Golden yellow B. Red C. Green D. Lilac 5. A metal M forms an oxide with the formula M 2 O 3 and its ion is isoelectronic with neon. What is the electronic configuration of the metal M? A. 2, 3 B. 2, 8 C. 2, 8, 2 D. 2, 8, 3 6. Which of the following ionic formulae is incorrect? A. Ag 2 O B. Na 2 HPO 4 C. Ca(HCO 3 ) 2 D. SrCl 7. Which of the following ions contains the same number of electrons as an argon atom? A. K + B. Mg 2+ C. O 2 D. N 3 8. Which of the following molecules do NOT have any lone pair of electrons on the central atom? (1) H 2 S (2) CS 2 (3) CCl 4 A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) 9. Which of the following statements concerning the Periodic Table is correct? A. The elements are arranged in the order of increasing relative atomic mass. B. The melting point of the Group I elements increases down the group. C. The boiling point of the Group VII elements increases down the group. D. The reactivity of the Group I and Group VII elements increases down the group. 10. A substance has a high melting point and does not conduct electricity when in solid state. It may be (1) a compound with giant ionic structure. (2) a compound with simple molecular structure. (3) an element with giant metallic structure. A. (1) only B. (2) only C. (1) and (3) only D. (2) and (3) only 11. Which of the following substances can conduct electricity in molten state but NOT in solid state? A. Silver B. Quartz C. Sugar D. Lead(II) bromide

3 F.4 Final Exam Chemistry Page 3 of A gel containing NaCl(aq), K 3 Fe(CN) 6 (aq) and phenolphthalein is yellow in color. An iron nail is put into the gel and corrodes after a period of time. Which of the following colors would NOT be observed in the gel after the iron nail corrodes? A. blue B. pink C. grey D. yellow 13. The action of dilute nitric acid on copper is represented by the following equation : xcu(s) + yhno 3 (aq) xcu(no 3 ) 2 (aq) + zno(g) + 4H 2 O(l) The values of x, y and z in the balanced equation are respectively A. 4, 3 and 1. B. 2, 5 and 1. C. 1, 4 and 2. D. 3, 8 and Which of the following metal oxides CANNOT be reduced to form metal when heated with carbon? A. Copper(II) oxide B. Iron(III) oxide C. Zinc oxide D. Magnesium oxide 15. Consider the following set-ups: Which hook would corrode first? A. iron hook (1) B. iron hook (2) C. copper hook (3) D. copper hook (4) 16. Anodised aluminium is more commonly used than iron for making window frames. This is because (1) the cost for extracting aluminium is lower than the cost for extracting iron. (2) anodised aluminium is more corrosion resistant than iron. (3) anodised aluminium is harder than iron. A. (1) only B. (2) only C. (1) and (3) only D. (2) and (3) only

4 F.4 Final Exam Chemistry Page 4 of Decomposition of solid KClO 3 gives KCl and O 2 as the only products. What is the mass of O 2 produced when 49.0 g of KClO 3 undergo complete decomposition? (Relative atomic masses: O = 16.0, Cl = 35.5, K = 39.1) A g B g C g D g 18. Rhenium chloride contains 63.6% by mass of Re. Which of the following empirical formulae of rhenium chloride is correct? (Relative atomic masses: Re = 186.2, Cl = 35.5) A. ReCl B. ReCl 2 C. ReCl 3 D. ReCl If 1.50 g of hydrated solid, H 2 C 2 O 4 2H 2 O, were heated to drive off the water of crystallization, how many grams of anhydrous H 2 C 2 O 4 solid would remain? (Relative atomic masses: O = 16.0, C = 12.0, H = 1.0) A g B g C g D g 20. If 1 mole of ozone (O 3 ) contains x atoms, 1 mole of oxygen gas will contain A. x atoms. B. atoms. 3 3x C. atoms. D. 6x atoms. 2 2x 21. When a fizzy tablet is added into a glass of water, bubbles are evolved. Which of the following is the correct explanation of the phenomenon? A. The tablet reacts with water to give oxygen. B. The tablet contains solid carbon dioxide. When the tablet dissolves in water, carbon dioxide is released. C. When the tablet dissolves in water, a lot of heat is released which boils the water. D. The tablet contains a solid acid and a solid carbonate. When the tablet dissolves in water, the acid and the carbonate react together to release carbon dioxide. 22. Solid citric acid does NOT turn dry blue litmus paper red because A. hydrogen ions are not formed when there is no water. B. the ions in solid citric acid are not mobile. C. there are no hydrogen atoms in solid citric acid. D. citric acid is an ionic compound when it is a solid.

5 F.4 Final Exam Chemistry Page 5 of Propane (C 3 H 8 ) can be used as a fuel. It reacts with oxygen according to the following equation: C 3 H 8 (g) + 5O 2 (g) 3CO 2 (g) + 4H 2 O(l) 22.0 g of propane are allowed to react with 57.6 g of oxygen. What is the mass of carbon dioxide produced? (Relative atomic masses: H = 1.0, C = 12.0, O = 16.0) A g B g C g D g 24. Which of the following substances, when mixed, would produce a precipitate? A. copper(ii) sulphate solution and ammonia solution B. sodium hydroxide solution and ethanoic acid C. sodium sulphate solution and magnesium chloride solution D. sodium chloride solution and calcium nitrate solution 25. In a titration experiment, which of the following apparatus can be used after rinsing with distilled water only beforehand? (1) Burette (2) Conical flask (3) Pipette A. (1) only B. (2) only C. (1) and (3) only D. (2) and (3) only 26. In an experiment to prepare calcium sulphate, excess dilute sulphuric acid is added to 10.0 cm 3 of 1.0 mol dm 3 calcium nitrate solution. Which of the following is the theoretical mass of the calcium sulphate obtained? (Relative atomic masses: O = 16.0, S = 32.1, Ca = 40.1) A g B g C g D g 27. Which of the following statements is correct? A. All aqueous solutions contain H + (aq) ions. B. The ph of all acid solutions is greater than zero. C. All acidic compounds contain hydrogen as their constituent elements. D. A 'corrosive' hazard warning label must be displayed on all reagent bottles containing acid solution. 28. Which of the following salts CANNOT be prepared from the reaction of a metal with a dilute acid? A. zinc sulphate B. iron(ii) chloride C. calcium chloride D. copper(ii) sulphate 29. A standard sodium hydroxide is titrated against a sample of hydrochloric acid using methyl orange as an indicator. Which of the following correctly describes the colour change at the end point? A. From yellow to orange. B. From orange to yellow. C. From orange to red. D. From red to orange.

6 F.4 Final Exam Chemistry Page 6 of What volume of water is required to dilute 50.0 cm 3 8 M sulphuric acid to a concentration of 1.0 M? A. 8.0 cm 3 B cm 3 C cm 3 D cm Anhydrous sodium carbonate can be used as a primary standard for preparing standard solutions because (1) it can be obtained in a very pure form. (2) it dissolves in water completely at room conditions. (3) it is hygroscopic. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) 32. A student performed a titration experiment in which he added an acid from a burette to an alkali in a conical flask. The following diagrams show the initial and final readings of the burette. What was the volume of the acid added from the burette to the conical flask? A cm 3 B cm 3 C cm 3 D cm 3 Directions: Each question below (Question Nos ) consists of two separate statements. Decide whether each of the two statements is true or false; if both are true, then decide whether or not the second statement is a correct explanation of the first statement. Then select one opinion from A to D according to the following table: A. Both statements are true and the 2nd statement is a correct explanation of the 1st statement. B. Both statements are true but the 2nd statement is NOT a correct explanation of the 1st statement. C. The 1st statement is false but 2nd statement is true. D. Both statements are false. 1st statement 33. Magnesium can displace iron from iron(ii) nitrate solution. 2nd statement Magnesium is more reactive than iron. 34. Equal masses of Li and Na are added to water separately, greater amount of gas will be produced by Na than Li. According to the metal reactivity series, Na is more reactive than Li. 35. Sodium hydrogencarbonate solution is acidic. Sodium hydrogencarbonate is an acid salt.

7 F.4 Final Exam Chemistry Page 7 of 9 SECTION B: Structured Questions (65 %) Answer ALL questions. Put all the answers in the answer book provided. 1. Argon and chlorine are elements in the same period of the Periodic Table. (a) Draw the electron diagram for a molecule of argon, showing electrons in all shells. (1 mark) (b) What is the type of intermolecular force in chlorine gas? (1 mark) (c) Complete the table below by stating the natural source and the method of extraction from the source for each element. (4 marks) Element Natural source Method of extraction Argon (i) (ii) Chlorine (iii) (iv) 2. The simplified diagram below shows a tungsten light bulb. The filament inside is made of metal tungsten (W). (a) (b) Tungsten is extracted by heating tungsten oxide (W 2 O 5 ) with hydrogen at high temperature. Write a balanced equation, with states, to represent the extraction of tungsten from tungsten oxide (W 2 O 5 ). (2 marks) When electricity is passed through tungsten wire, the wire glows white hot. (i) Suggest ONE physical property of tungsten, other than electrical conductivity, which is essential for its use in the light bulb. (ii) Tungsten is stable in air under normal conditions. However, it is not appropriate to fill up a tungsten light bulb with air. Explain. (iii) Suggest, with explanation in terms of electronic arrangement, a suitable gas for filling up a tungsten light bulb. (5 marks) 3. Aluminium and iron are commonly used construction materials. (a) Suggest why iron was used earlier than aluminium in history. (1 mark) (b) A compound contains iron and oxygen only. In an experiment for determining the empirical formula of this compound, 2.31 g of the compound was heated with carbon monoxide. Upon complete reaction, carbon dioxide and 1.67 g of iron were formed. (Relative atomic masses: Fe = 55.8, C = 12.0, O = 16.0) (i) Calculate the empirical formula of this compound. (ii) Write the chemical equation, with appropriate states, for the reaction involved in the experiment. (iii) As carbon monoxide is poisonous, suggest one necessary safety precaution in carrying out the experiment. (6 marks)

8 F.4 Final Exam Chemistry Page 8 of 9 4. For each of the following pairs of substances, suggest a chemical test to distinguish one substance from the other AND state the expected observations. (a) Iron(II) sulphate solution and zinc sulphate solution. (4 marks) (b) Concentrated hydrochloric acid and dilute hydrochloric acid. (4 marks) 5. A student tried to prepare magnesium sulphate by mixing magnesium nitrate solution and sodium sulphate solution. The proposed reagents were considered inappropriate. (a) State ONE reason why the proposed reagents are inappropriate. (2 marks) (b) Suggest suitable reagents to prepare magnesium sulphate. (2 marks) (c) Write a chemical equation, with appropriate states, for the reaction suggested in (b). (2 marks) (d) Briefly describe how the dry magnesium sulphate crystal can be prepared in school laboratory. (3 marks) 6. A group of students tried to prepare dry ammonia gas in the laboratory using the following apparatus : (a) (b) (c) (d) Suggest suitable solid reagents AND a drying agent for this experiment. (2 marks) Write a chemical equation, with appropriate states, for the reaction in preparing ammonia gas. (2 marks) Using only the apparatus given above, draw a labelled diagram for the preparation and collection of dry ammonia gas. Your answer should include the reactants and drying agent suggested in (a). (4 marks) State the expected observation and write the chemical equation(s) for the reaction occurred when excess ammonia gas is bubbled into lead(ii) nitrate solution. (2 marks) 7. Sulphuric acid is a strong acid while ethanoic acid is a weak acid. (a) With the aid of a chemical equation, explain why ethanoic acid is regarded as a weak acid. (2 marks) (b) The ph of an aqueous solution is defined as log[h + (aq)]. (i) The ph of pure water equals 7.0 at 298K. Find the [H + (aq)]. (ii) A dilute sulphuric acid of ph equals Calculate the concentration of the acid. (4 marks) (c) The diagram below shows the colour of an acid-base indicator bromothymol blue in different ph ranges. Given that the hydrogen ion concentration of a solution is 3.2 x mol dm 3. What is the colour of bromothymol blue if it is added to this solution? (2 marks)

9 F.4 Final Exam Chemistry Page 9 of 9 8. A student carried out the following experiment to determine the concentration of ethanoic acid in a brand of commercial vinegar cm 3 of the vinegar was transferred to a cm 3 volumetric flask using an apparatus X. It was then diluted to cm 3 with distilled water cm 3 of the diluted vinegar solution was withdrawn and titrated against 0.10 M sodium hydroxide solution with a suitable indicator. (a) (i) Name apparatus X. (b) (ii) (iii) Suggest ONE reason for diluting the vinegar. Suggest a suitable indicator for the titration AND state the colour change at the end point of the titration. (4 marks) The student carried out four titrations altogether. The titration results are listed in the table below: Titration Burette reading Final reading/cm Initial reading/cm (c) (i) Based on the titration results, calculate a reasonable average for the volume of the sodium hydroxide solution used. (ii) Calculate the concentration, in mol dm 3, of ethanoic acid in the vinegar. (3 marks) Suggest another method for detecting the titration end point without the use of any acid-base indicator or ph meter. Explain your answer briefly. (3 marks) End of Paper

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