1 Which of the following is not a hydrocarbon compound? star A Alkane B Alkene C Alkyne D Alcohol T5 Chapter 2.1 Types of Carbon Compound
2 Which of the following is not the component of soda lime glass? star A Sand B Boron oxide C Calcium carbonate D Sodium carbonate T4 Chapter 8.2 Composition of Glass and Its Uses
3 Diagram 1 shows the electron arrangement of an atom of element Q. What is the number of valence electrons in atom Q? star A 17 B 15 C 10 D 7 T4 Chapter 2.3 Atomic Structure
4 Which of the following uses of carbon-14 isotope? star A To treat cancer patient B To estimate the age of fossils C To control the thickness of plastic D To detect the leakage of underground pipes T4 Chapter 2.4 Isotopes and Its Uses
5 Chemical formula of copper(I) oxide is star A CuO B CuO_2 C Cu_2O D Cu_2O_2 T4 Chapter 3.3 Chemical Formula
6 Diagram 2 shows the apparatus set-up to determine the empirical formula of magnesium oxide. Which of the following, is the step that should be taken to ensure that all magnesium are react with oxygen and burnt completely? I Open and close the lid quickly occasionally during heating. II Heat the magnesium ribbon strongly in the crucible without its lid. III Observe the white solid produced IV Repeat heating, cooling and weighing until a constant mass is obtained. star A I and II B I and III C I and IV D III and IV T4 Chapter 3.3 Chemical Formula
7 What is the basic principle used to arrange the elements in the modern Periodic Table of Elements? star A Increasing proton numbers B Increasing relative atomic mass C Increasing number of neutrons D Increasing nucleon numbers T4 Chapter 4.2 The Arrangement in the Periodic Table of Elements
8 Which characteristic is correct about elements in Group 17 in the Periodic Table as going down the group? star A The intensity of colour decreases B The tendency to accept an electron decreases C The physical state changes from liquid to gas D Force of attraction between nucleus and electron become stronger. T4 Chapter 4.5 Elements in Group 17
9 Diagram 3 shows the bond formation of two types of particles. What is the type of chemical bond formed? star A Ionic bond B Dative bond C Metallic bond D Hydrogen bond T4 Chapter 5.2 Ionic Bond
10 Which of the following is the property of covalent compound? star A Conduct electricity in solid state B High melting and boiling points C Dissolves in organic solvent D Not easily volatile T4 Chapter 5.7 Properties of Ionic Compounds and Covalent Compounds
11 Which of the following is a base? star A Apple juice B Bamboo salt C Baking soda D Soft drink T4 Chapter 6.7 Neutralisation
12 Which of the following is true about weak acid? I The pH is less than 7 II Turn red litmus paper to blue III Has low concentration of hydrogen ions IV Completely ionises in the water to produce hydrogen ions, H+ star A I and II B I and III C II and IV D III and IV T4 Chapter 6.3 Strength of Acids and Alkalis
13 The following equation represent the reaction between zinc strip and hydrochloric acid. Zn + 2HCl \longrightarrow ZnCl_2 + H_2 Which method is most suitable to increase the rate of reaction? star A Use zinc powder B Reduce the volume of hydrochloric C Reduce the temperature of hydrochloric acid D Reduce the concentration of hydrochloric acid T4 Chapter 7.2 Factors Affecting Rate of Reactions
14 Substance R is used to manufacture the body frame of a racing bike. Substance R has the following properties: Resistant to corrosion, Strong, Light What is substance R? star A Stainless steel B Duralumin C Cupro-nickel D Steel T4 Chapter 8.1 Alloy and Its Importance
15 Diagram 4 shows a telescope used to see distance objects. Which of the following glass is suitable to be used in making telescope lens? star A Soda-lime glass B Borosilicate glass C Fused silica glass D Lead crystal glass T4 Chapter 8.2 Composition of Glass and Its Uses
16 Which of the following is a synthetic rubber? star A Nylon B Thiokol C Terylena D Polyvinyl chloride T5 Chapter 4.3 Synthetic Rubber
17 Which of the following is true to explain the coagulation of latex? star A Rubber particles combine which causes the coagulation of latex B Hydrogen ions from the acid neutralise the negative charges on the protein membrane C Hydroxide ions from the ammonia solution neutralise the hydrogen ions from the lactic acid D Repulsion between the negatively charged particles from coming to closer to each other T5 Chapter 4.2 Natural Rubber
18 Which reaction is the fastest? star A 1 g limestone powder, 100 cm^3 of 1 mol dm^-3 acid and 30°C B 1 g limestone solid, 100 cm^3 of 1 mol dm^-3 acid and 40°C C 1 g limestone powder, 100 cm^3 acid of 1 mol dm^-3 and 40°C D 1 g limestone solid, 100 cm^3 acid of 1 mol dm^-3 and 30°C T4 Chapter 7.2 Factors Affecting Rate of Reactions
19 Diagram 5 shows inland lake known as dead sea. In dry season, solid X formed. During raining season all the solid X disappear. What are the properties of the solid X? I Can be purified using recrystallization II Can conduct electricity in molten state III Consist of chloride and sulphate IV Low melting and boiling point star A I and II B I and III C II and III D III and IV T4 Chapter 5.7 Properties of Ionic Compounds and Covalent Compounds T4 Chapter 6.9 Preparation of Salts
20 The following chemical equation represents the reaction of ethane with chlorine gas. CH_4(g) + Cl_2(g) -> CH_3Cl(g) + HCl(g) What is the name of the reaction? star A Combustion B Additional C Polymerisation D Substitution T5 Chapter 2.3 Chemical Properties and Interconversion of Compounds Between Homologous Series
21 Diagram 6 shows a production of potassium palmitate through process X. What is process X? star A Esterification B Combustion C Saponification D Coagulation T5 Chapter 5.2 Cleaning Agents
22 Which of the following does not happen when the temperature is increased? star A Particles move faster B Particles collide more often C Particles collide with more energy D More particles collide in the correct orientations T4 Chapter 7.4 Collision Theory
23 The proton number of atom R is 14 and its relative atomic mass is 28. Which statements is correct about R? star A The mass of 1 atom R is 28 g B The molar mass of R is 28 gmol⁻¹ C 14 g of R contains 6.0x 10^23 atoms D Atom R has 14 protons, 14 electrons and 28 neutrons T4 Chapter 3.1 Relative Atomic Mass and Relative Molecular Mass T4 Chapter 3.2 Mole Concept
24 Diagram 7 shows the apparatus set-up for electrolysis of ammonia solution and sodium hydroxide solution. Which statement explains the difference in the brightness of the bulb? star A The reacting particles in sodium hydroxide solution gain more kinetic energy B The movement of ions in sodium hydroxide solution is faster C The number of free moving ions per unit volume of sodium hydroxide solution is higher D The total surface area of carbon electrod in sodium hydroxide solution is bigger T5 Chapter 1.4 Electrolytic Cell
25 Diagram 8 shows two chemical reactions. What is X ? star A Tin B Lead C Silver D Copper T5 Chapter 1.1 Oxidation and Reduction
26 Which of the following is the electron arrangement diagram for the formation of ionic compound? star A A Figure B B Figure C C Figure T4 Chapter 5.2 Ionic Bond
27 Diagram 9 shows the vulcanisation process of rubber. Which of the following are true about vulcanised rubber? star A Less resistant to high heat B Easier to be oxidised C More elastic D Soft T5 Chapter 4.2 Natural Rubber
28 Diagram 10 shows the structure of a polymer. Which of the following is the monomer of the polymer? star A A Figure B B Figure C C Figure D D Figure T5 Chapter 4.1 Polymer
29 What is the oxidation number of chlorine in KClO3? star A -2 B -1 C +1 D +5 T5 Chapter 1.1 Oxidation and Reduction
30 In an experiment, 0.24 g of magnesium powder is added to 50 cm³ of 0.2 mol dm⁻³ zinc sulphate solution. The temperature of the mixture increases by 12 °C. What is the heat of displacement in the experiment? [Specific heat capacity of a solution = 4.2 J g⁻¹°C⁻¹; Relative atomic mass of Mg = 24] star A -126 kJ mol⁻¹ B -252 kJ mol⁻¹ C -378 kJ mol⁻¹ D -504 kJ mol⁻¹ T5 Chapter 3.2 Heat of Reaction
31 CaCO3 (s) + 2HCl (aq) -> CaCl2 (aq) + CO2 (g) + H2O (l) Based on the chemical equation, what is the change can be observed to determine the rate of reaction? star A Volume of gas liberated increased B Mass of reactant increased C The volume of reactants solution is decreased D Precipitation produce is reduced T4 Chapter 7.1 Determining Rate of Reaction
32 The following equation represents a reaction. 3H2 (g) + N2 (g) -> 2NH3 (g) What is the relative molecular mass of the product? [Relative atomic mass of H=1; N=14] star A 2 B 17 C 28 D 34 T4 Chapter 3.1 Relative Atomic Mass and Relative Molecular Mass
33 The following information is about organic compound P. - Has 3 carbon atoms - Soluble in water - Reacts with zinc to produce hydrogen gas What is the name of the organic compound P? star A Propene B Propanol C Propane D Propanoic acid T4 Chapter 6.4 Chemical Properties of Acids and Alkalis T5 Chapter 2.2 Homologous Series
34 Which substance is used to differentiate between hexane and hexene? star A Lime water B Bromine water C Phenolphthalein D Phosphoric acid T5 Chapter 2.3 Chemical Properties and Interconversion of Compounds Between Homologous Series
35 Which substance can be used to convert Fe^2+ to Fe^3+ star A Zinc powder B Bromine water C Sulfur dioxide gas D Potassium iodide solution T5 Chapter 1.1 Oxidation and Reduction
36 Diagram 11 shows the arrangement of the apparatus for the combination of two cells. Given the value of the standard electrode potential as follows. Cu^2+ + 2e \rightleftharpoons Cu + 0.34 V Mg^2+ + 2e \rightleftharpoons Mg + 0.40 V Which of the following statements is correct? I A colorless gas bubble is produced at the X electrode II The R electrode and the Y electrode are thin III Electrode X and electrode Q are anodes IV The blue color of the copper(II) sulfate solution in Cell II does not change star A I and II B I and III C II and IV D III and IV T5 Chapter 1.4 Electrolytic Cell
37 Diagram 12 shows a chemical cell. Which substance undergoes oxidation and reduction? [ E^0 for half cell ; Zn^2+_{(ak)} + 2e \rightleftharpoons Zn_{(p)} E^0 = -0.76 V ] star A Copper | Copper(II) ion B Copper | Hydrogen ion C Zinc | Copper(II) ion D Zinc | Hydrogen ion T5 Chapter 1.3 Voltaic Cell
38 The following equation shows the complete combustion of propene gas. C_3H_6(g) + 9/2 O_2(g) -> 3CO_2(g) + 3H_2O(g) Which of the following statements are true when 1 mol of propene gas is burnt completely? [Relative molecular mass : C_3H_6 = 42, O_2 = 32, CO_2 = 44, H_2O = 18, Molar volume of gas is 22.4 dm^3 mol^-1 at S.T.P.] I Complete combustion of 0.1 mol of propene produces 5.4 g of water II Complete combustion of 1 mol of propene gas produces 2 mol of water III Complete combustion of 4.2 g of propene requires 14.4 g of oxygen. IV Complete combustion of 0.1 mol of propene produces 6.72 dm^3 carbon dioxide gas at s.t.p. star A I and II B II and III C II and IV D I, III and IV T4 Chapter 3.2 Mole Concept T4 Chapter 3.4 Chemical Equation
39 The following equation shows the combustion of heptane, C_7H_16 in excess oxygen. C_7H_16 + 11O_2 → 7CO_2 + 8H_2O ΔH = - 5512 kJ mol^-1 In an experiment the combustion of heptane in excess oxygen releases 1378 kJ energy. What is the mass of heptane used? [Relative atomic mass : H = 1; C = 12] star A 25.0 g B 36.0 g C 77.0 g D 88.0 g T4 Chapter 3.2 Mole Concept T5 Chapter 3.2 Heat of Reaction T5 Chapter 3.3 Application of Exothermic and Endothermic Reactions in Daily Life
40 Diagram 13 shows set up apparatus for titration of potassium hydroxide with sulphuric acid. What is total volume of the mixed solution in the conical flask at the end point of titration in Diagram 13? star A 10 cm^3 B 20 cm^3 C 30 cm^3 D 40 cm^3 T4 Chapter 6.7 Neutralisation