1 Which of the following atoms has three valence electrons? star A A Figure B B Figure C C Figure D D Figure T4 Chapter 2.3 Atomic Structure
2 The following statement refers to the contribution of a scientist in the development of ideas about atomic structure. - Discovered the proton - Nucleus as the centre of an atom - Electrons move outside the nucleus Who is the scientist? star A Niels Bohr B John Dalton C James Chadwick D Ernest Rutherford T4 Chapter 2.2 The Development of the Atomic Model
3 Element X and element Y are located in Group 1 and Group 16 respectively in the Periodic Table of Elements. Element X reacts with element Y to form a compound. What is the chemical formula of the compound? star A XY B XY_2 C X_2Y D X_2Y_3 T4 Chapter 3.3 Chemical Formula
4 Which of the following physical properties are the same for the elements in Group 17 of the Periodic Table of Elements? star A Colour B Atomic size C Melting point D Does not conduct electricity T4 Chapter 4.5 Elements in Group 17
5 Which of the following statements is true about the role of water in showing acidic properties? star A Acid molecules will dissolve in water to produce hydroxide ions B The presence of water will cause red litmus paper to turn blue C Neutralisation of acid will occur in water to produce hydrogen ions D Acid molecules will ionise in water to produce hydrogen ions T4 Chapter 6.1 The Role of Water in Showing Acidic and Alkaline Properties
6 The following are the characteristics of elements L and M. - Forms complex ions - Forms coloured compounds What are L and M? I Iron II Barium III Chromium IV Magnesium star A I and II B I and III C II and IV D III and IV T4 Chapter 4.7 Transition Elements
7 Which of the following statements explains about dative bond? star A Covalent bond that formed when only one atom shares electrons B Covalent bond that formed when electron is transferred from one atom only C Covalent bond that formed when a pair of electrons is shared by two non-metal atoms D Covalent bond that formed when a pair of electrons that is shared comes from one atom only T4 Chapter 5.5 Dative Bond
8 Which of the following reactions is a slow reaction? star A Fermentation of glucose B Sparks of fireworks C Combustion of methanol D Precipitation of silver chloride T4 Chapter 7.1 Determining Rate of Reaction
9 Diagram 1 shows a LED bulb. Which of the following glass is suitable for producing part X? star A Lead crystal glass B Borosilicate glass C Soda-lime glass D Fused silica glass T4 Chapter 8.2 Composition of Glass and Its Uses
10 Which of the following is matched correctly? star A Glass fibre, Plastic, Fibre glass B Optical fibre, Plastic, Silica glass fibre C Reinforced concrete, Wire mesh, Concrete D Photochromic glass, Silver chloride and copper(I) chloride, Glass T4 Chapter 8.4 Composite Materials and Its Importance
11 Diagram 2 shows a chemical cell. What happen at P and Q? star A Loss of oxygen, Gain of oxygen B Gains of hydrogen, Loss of hydrogen C Gains of electrons, Loss of electrons D Increase in oxidation number, Decrease in oxidation number T5 Chapter 1.3 Voltaic Cell
12 Table 1 shows the standard electrode potential value of half-cells in a chemical cell. | Half-cell equation | E° (V) | |---|---| | Cu²⁺ (aq) + 2e⁻ ⇌ Cu (s) | + 0.34 | | Ag⁺ (aq) + e⁻ ⇌ Ag (s) | + 0.80 | Which of the following reducing agents is the strongest? star A Cu²⁺ B Ag⁺ C Cu D Ag T5 Chapter 1.2 Standard Electrode Potential
13 Diagram 3 shows the formulae for two different types of cleaning agent X and Y. Which of the following statements is correct about cleaning agent X and Y? star A Biodegradable, Most are not biodegradable B Effective in hard water only, Effective in hard water and soft water C Does not form scum in hard water, Forms scum in hard water D Produced from fraction of petroleum, Produced from oil or fat T5 Chapter 5.2 Cleaning Agents
14 The reaction between calcium nitrate solution and sodium carbonate solution is an endothermic reaction. Which of the following energy level diagrams represents the reaction? star A A Figure B B Figure C C Figure D D Figure T5 Chapter 3.1 Heat Change in Reactions
15 The discovery of graphene has opened a new chapter in the field of nanotechnology. Various existing applications can be improved or replaced with graphene that has superior and distinctive characteristics. Which of the following is a physical property of graphene? star A Heat insulator B Electrical insulator C Hard but brittle D Impermeable T5 Chapter 5.5 Application of Nanotechnology in Industry
16 Which of the following substances can dissolve in water? star A Benzene, C_6H_6 B Hexane, C_6H_14 C Glucose, C_6H_12O_6 T4 Chapter 5.4 Hydrogen Bond
17 Diagram 4 shows the ionic formulae of elements X and elements Y. Which of the following ionic equations represents the reaction between the ions? star A X^3+ + Y^2- → X_2Y_3 B X^3+ + 3Y^2- → XY_3 C 2X^3+ + 3Y^2- → X_2Y_3 D 3X^3+ + 2Y^2- → X_2Y_3 T4 Chapter 3.3 Chemical Formula
18 What type of bond present between carbon atoms in a propyne, C_3H_4 molecule? star A Only single bonds B Only triple bonds C One single bond and one double bond D One single bond and one triple bond T5 Chapter 2.2 Homologous Series
19 Table 2 shows observations when three types of alkali metals are placed into a beaker containing water. | Alkali metal | Observation | |---|---| | Lithium | Moves slowly on the surface of water | | Sodium | Moves quickly on the surface of water with yellow flame | | Potassium | Moves very fast on the surface of water with a lilac flame | Which of the following statements best explains the observation? star A Reactivity of alkali metals decreases when going down the group B The tendency of alkali metal atoms to accept electrons decreases when going down the group C Alkali metal atoms form ionic bond with water easily when going down the group D The atomic size of alkali metals increase and making them easier to lose their valence electrons T4 Chapter 4.4 Elements in Group 1
20 Which of the following is true about weak acid? star A Unable to neutralise alkali B pH value is higher than 7 C Ionises partially in water to produce hydrogen ions D Able to change red litmus paper to blue T4 Chapter 6.3 Strength of Acids and Alkalis
21 Diagram 5 shows the observation when oxide of metal X is added into a beaker. Which of the following substances will show the same observation when added to nitric acid? I Calcium oxide II Sodium oxide III Silicon dioxide IV Copper(II) oxide star A I and II B I and III C II and IV D III and IV T4 Chapter 6.4 Chemical Properties of Acids and Alkalis
22 Which of the following is the correct sequence in preparation of solution by dilution method? I Transfer the solution into a volumetric flask II Calculate the volume of stock solution to be diluted III Use a pipette to measure the volume of solution needed IV Add distilled water until the calibration mark star A II, I, III, IV B II, I, IV, III C II, III, I, IV D II, III, IV, I T4 Chapter 6.6 Standard Solution
23 The following equation represents the reaction between zinc and hydrochloric acid. Zn + 2HCl → ZnCl_2 + H_2 Which of the following methods is the most suitable to increase the rate of reaction? star A Decrease the size of zinc B Reduce the temperature of hydrochloric acid C Reduce the volume of hydrochloric acid D Decrease the concentration of hydrochloric acid T4 Chapter 7.2 Factors Affecting Rate of Reactions
24 Diagram 6 shows an experiment to produce salt X. The experiment is repeated to produce salt Y which has the same solubility as salt X. Which of the following salt solution can be used to replace the Pb(NO_3)_2 solution? star A Ca(NO_3)_2 B Cu(NO_3)_2 C Fe(NO_3)_2 D Mg(NO_3)_2 T4 Chapter 6.9 Preparation of Salts
25 Which of the following methods can use to cook 100 potatoes within the shortest time? star A Boil the potatoes in pressure cooker B Steam the potatoes in steamer C Boil the potatoes in a pan D Fry the potatoes in a wok T4 Chapter 7.3 Application of Factors that Affect the Rate of Reaction in Daily Life
26 Diagram 7 shows the engine of a jet. Why is ceramic used in manufacturing the turbine? star A Flexible B Electrical insulator C Chemically inert D High heat resistance T4 Chapter 8.3 Composition of Ceramics and Its Uses
27 Diagram 8 shows the monomer of latex. What is the name of the monomer? star A Ethene B Styrene C Propene D Isoprene T5 Chapter 4.2 Natural Rubber
28 Which of the following substances is miscible in water in all proportions? star A C_2H_2 B C_2H_4 C C_2H_6 D C_2H_5OH T4 Chapter 5.4 Hydrogen Bond
29 Diagram 9 shows the structural formula of an alkene. What is the product formed when the alkene reacts with steam? star A Butane B But-1-yne C Butan-2-ol D Butanoic acid T5 Chapter 2.3 Chemical Properties and Interconversion of Compounds Between Homologous Series
30 Diagram 10 shows an injured child. Which of the following medicines is used to treat his injury? star A Iodine B Codeine C Antihistamine D Formaldehyde T5 Chapter 5.4 Medicines and Cosmetics
31 The following equation represents the reduction of iron(III) oxide by magnesium. 3Mg + Fe_2O_3 -> 3MgO + 2Fe What is the mass of iron(III) oxide that is reduced if 7.2 g magnesium is used? [Relative atomic mass: Fe = 56, Mg = 24, O = 16] star A 8.0 g B 16.0 g C 32.0 g D 48.0 g T4 Chapter 3.4 Chemical Equation
32 Diagram 11 shows the formation of terylene. What is monomer X? star A A Figure B B Figure C C Figure D D Figure T5 Chapter 4.1 Polymer
33 The following information shows the observation when a solution containing cation R is tested with alkali solutions. - White precipitate is insoluble in excess sodium hydroxide, NaOH solution. - White precipitate is insoluble in excess ammonia, NH_3 solution. What is cation R? star A Al^3+ B Ca^2+ C Mg^2+ D Pb^2+ T4 Chapter 6.11 Qualitative Analysis
34 Diagram 12 shows the apparatus set-up for the titration of sodium hydroxide, NaOH with nitric acid, HNO_3. What is the maximum mass of the salt formed in this reaction? [Relative atomic mass: Na = 23, O = 16, N = 14] star A 0.85 g B 1.12 g C 1.70 g D 2.55 g T4 Chapter 6.7 Neutralisation
35 Diagram 13 shows the setup of apparatus for an electrolytic cell. Which of the following graphs show the change in mass of the anode during electrolysis? star A A Figure B B Figure C C Figure D D Figure T5 Chapter 1.4 Electrolytic Cell
36 Diagram 14 shows the sacrificial metal used in underground iron pipes. Which of the following statements is correct about metal X? star A Metal X increases the corrosion rate of the underground iron pipe B Metal X prevents rusting by acting as a cathode C Metal X protects the underground iron pipe by absorbing oxygen from the water D Metal X has higher tendency to release electrons, and protect the underground iron pipe from rusting T5 Chapter 1.6 Rusting
37 Which of the following are the isomer for C_5H_11OH? I Pentan-2-ol II 2-ethylpropanol III 2,2-dimethylpropan-1-ol IV 2,3-dimethylpropan-2-ol star A I and II B I and III C II and IV D III and IV T5 Chapter 2.4 Isomers and Naming Based on IUPAC Nomenclature
38 Table 3 shows the volume of hydrogen gas collected in the reaction between zinc powder and diluted hydrochloric acid. | Time (min) | 0.0 | 0.5 | 1.0 | 1.5 | 2.0 | 2.5 | 3.0 | 3.5 | |---|---|---|---|---|---|---|---|---| | Volume of gas (cm³) | 0.0 | 4.0 | 7.0 | 10.5 | 12.0 | 14.0 | 16.5 | 16.5 | What is the average rate of reaction at the second minute? star A 4.7 cm³ min⁻¹ B 5.0 cm³ min⁻¹ C 5.5 cm³ min⁻¹ D 6.0 cm³ min⁻¹ T4 Chapter 7.1 Determining Rate of Reaction
39 A student prepared 100 cm³ of sodium hydroxide solution, NaOH by dissolving 4.0 g of sodium hydroxide in distilled water. After that, 150 cm³ of distilled water was added to the solution to dilute it. What is the pH value of the dilute solution? [Relative atomic mass: Na = 23, O = 16, H = 1] star A 10.6 B 13.6 C 13.8 D 14.0 T4 Chapter 6.2 pH Value T4 Chapter 6.5 Concentration of Aqueous Solution T4 Chapter 6.6 Standard Solution
40 The following thermochemical equation shows the combustion of butane gas. C_4H_10 + \frac{13}{2}O_2 \rightarrow 4CO_2 + 5H_2O \Delta H = - 2880 kJ mol^{-1} 2400 cm^3 oxygen gas, O_2 is burnt completely in butane gas. What is the heat change of the reaction? [1 mol of any gas occupies 24 dm^3 at room conditions] star A 44.3 kJ B 288.0 kJ C 1152.0 kJ D 1872.0 kJ T4 Chapter 3.2 Mole Concept T4 Chapter 3.4 Chemical Equation T5 Chapter 3.2 Heat of Reaction