1 Which of the following particles in ammonia solution is responsible for its alkaline properties? star A H^+ B OH^- C Na^+ D Cl^- T4 Chapter 6.1 The Role of Water in Showing Acidic and Alkaline Properties
2 What is the meaning of fuel value? star A The amount of energy released when one gram of fuel is burned completely in excess oxygen. B The amount of energy released when one mol of fuel is burned completely in excess oxygen. C The amount of energy absorbed when one gram of fuel is burned completely in excess oxygen. D The amount of energy released when fuel is burned in excess oxygen to form one mole of carbon dioxide gas and water. T5 Chapter 3.3 Application of Exothermic and Endothermic Reactions in Daily Life
3 Which of the following is a slow reaction? star A Rock erosion B Ignition of matches C Fireworks D Electric cell reactions T4 Chapter 7.1 Determining Rate of Reaction
4 The vertical columns in the Periodic Table of Elements are named as star A Group B Period C Row T4 Chapter 4.2 The Arrangement in the Periodic Table of Elements
5 What type of glass is used to make a bulb? star A Borosilicate glass B Fused silica glass C Soda lime glass D Lead glass T4 Chapter 8.2 Composition of Glass and Its Uses
6 Which additive in detergent is used to change stain to colourless substance? star A Anti suspension agent B Biological enzyme C Whitening agent D Fragrance T5 Chapter 5.2 Cleaning Agents
7 The following statement describes the subatomic particle Q. - The relative charge is neutral. - The relative mass is 1. - Located in the atomic nucleus. What is Q? star A Neutron B Proton C Electron D Nucleon T4 Chapter 2.2 The Development of the Atomic Model
8 Table shows the content of transition elements in gems. Which one shows the correct match of the transition element? | | Gems | Transition element | |---|---|---| | A | Ruby | Chromium | | B | Sapphire | Manganese | | C | Amethyst | Titanium | | D | Emerald | Silicone | star A A B B C C D D T4 Chapter 4.7 Transition Elements
9 What type of chemical bond is formed through the transfer of electrons between metal atoms and non-metal atoms? star A Covalent bond B Hydrogen bond C Ionic bond D Double bond T4 Chapter 5.2 Ionic Bond
10 Which of the following is true about the chemical properties of alkalis? star A React with metal carbonates to produce salt, water and carbon dioxide. B React with unreactive metals to produce salt and hydrogen gas. C React with metal oxides to produce salt and water. D React with acids to produce salt and water. T4 Chapter 6.4 Chemical Properties of Acids and Alkalis
11 What is meant by composite material? star A Elements made from combining two or more non-homogeneous substances that is matrix substance and strengthening substance. B Material made from combining two or more homogeneous substances that is matrix substance and strengthening substance. C A compound made from combining two or more homogeneous substances that is matrix substance and strengthening substance. D Material made from combining two or more non-homogeneous substances that is matrix substance and strengthening substance. T4 Chapter 8.4 Composite Materials and Its Importance
12 Which of the following is an alternative hydrocarbon energy source? star A Hydroelectric B Bioethanol C Coal D Solar T5 Chapter 2.1 Types of Carbon Compound
13 Which of the following represent an endothermic reaction? star A Photosynthesis B Combustion C Neutralisation D Displacement T5 Chapter 3.1 Heat Change in Reactions
14 Which of the following polymers is a natural polymer? I Starch II Protein III Cellulose IV Thiokol star A I and II B II and IV C I, II and III D I, II and IV T5 Chapter 4.1 Polymer T5 Chapter 4.3 Synthetic Rubber
15 What is the process of converting unsaturated fats to saturated fats? star A Esterification B Hydrogenation C Polymerisation D Neutralisation T5 Chapter 5.1 Oils and Fats
16 Diagram 1 shows the particle arrangement for the change of state of matter. Diagram 1 Which of the following is Process X? star A Sublimation B Freezing C Condensation D Deposition T4 Chapter 2.1 Basic Concepts of Matter
17 The chemical formula of compound X is WBr_2. What is the chemical formula of the compound formed when cation of X reacts with oxygen? star A WO B WO_2 C W_2O_3 D W_3O_2 T4 Chapter 3.3 Chemical Formula
18 2Li + 2H2O → 2LiOH + H2 Chemical equation above represents the reaction between lithium metal and water. Which of the following observations may happen when lithium metal is replaced by potassium? star A Blue litmus paper turn to red when dipped into the solution. B Metal moves by emitting sparks. C 'Hiss' sound getting less. D Glass basin perforated. T4 Chapter 4.4 Elements in Group 1
19 Diagram 2 shows the bond formed between water molecules. Diagram 2 Which of the following has the same bond as Diagram 2? star A H F----H F B H^+----:N-H H C H Cl----H Cl D H H^+----:O H T4 Chapter 5.4 Hydrogen Bond
20 Diagram 3 shows two solutions of the same concentration and their pH values. Diagram 3 The difference in the pH because star A the concentration of hydroxide ions in R is greater than in S. B the number of moles of hydroxide ions in S is lower than in R. C R ionises partially whereas S ionises completely in water. D the degree of ionisation of R is higher than S. T4 Chapter 6.3 Strength of Acids and Alkalis
21 When the temperature of a reacting mixture increases, the rate of reaction increases. Which statements explain why the rate of reaction increases? star A The total surface area of the reactant particles increases. B The total number of the reactant particles per unit volume increases. C The reactant particles move faster and collide more often with one another. D The reactant particles which collide more often are able to overcome the lower activation energy. T4 Chapter 7.4 Collision Theory
22 Diagram 4 shows the formation of alloy Y. Diagram 4 Which of the following is a characteristic of the alloy formed? star A Can conduct electricity at high temperatures. B High stretching strength and more durable. C Darkens when exposed to sunlight. D Easy to rust when exposed to sea water. T4 Chapter 8.1 Alloy and Its Importance
23 There are three stable isotopes of silicon that exist in the environment namely Si-28, Si-29 and Si-30. The relative abundance of Si-28, Si-29 and Si-30 is 92.23%, 4.67% and 3.10% respectively. Calculate the relative atomic mass for silicone. star A 28.10 B 28.11 C 29.00 D 29.11 T4 Chapter 2.4 Isotopes and Its Uses
24 This is the oxidation half equation. 2I^- (aq) -> I_2 (aq) + 2e^- Based on the equation, which statement is true? star A Electrons are donated by iodine. B Electrons are accepted by iodine. C Electrons are donated by iodide ions. D Electrons are accepted by iodide ions. T5 Chapter 1.1 Oxidation and Reduction
25 An organic compound Y has the structure as shown in Diagram 5. Diagram 5 Which pair of compounds will react to produce organic compound Y? star A Methanol and propanoic acid B Hexanol and ethanoic acid C Ethanol and ethanoic acid D Ethanol and hexanoic acid T5 Chapter 2.3 Chemical Properties and Interconversion of Compounds Between Homologous Series
26 Diagram 6 shows the apparatus set-up for an experiment to determine the rate of reaction. Diagram 6 Which of the following techniques is the most suitable to determine the rate of reaction? star A Record the time as soon as precipitate is formed. B Record the time taken to obtain the maximum temperature. C Record the time as soon as the cross mark cannot be seen. D Record the time taken for the change of the pH value until a fixed pH value is obtained. T4 Chapter 7.1 Determining Rate of Reaction
27 Diagram 7 shows two sets of experiments conducted by Farah to determine the heat of displacement. Diagram 7 Farah found that the temperature of the mixture in set II is higher than in set I. What is the reason for the observation that was obtained? star A Metal X produces more hydrogen ions than metal Y. B Metal Y produces more hydrogen ions than metal X. C Metal X easily releases electrons than metal Y. D Metal Y easily releases more electrons than metal X. T5 Chapter 3.2 Heat of Reaction
28 Which pairs will produce covalent compounds? I Copper and chlorine II Carbon and fluorine III Hydrogen and chlorine IV Magnesium and fluorine star A I and II B II and III C III and IV D I and IV T4 Chapter 5.3 Covalent Bond
29 Diagram 8 shows the apparatus set-up for determine properties of rubber. Diagram 8 After a few minutes the weights are hung, the rubber strip is elongated. Which statement best explains the observation? star A Resistant to high heat B More elastic C Has strong hardness D Has low strength T5 Chapter 4.2 Natural Rubber
30 Diagram 9 shows a mother calms her 6-year-old son because he is in pain. Diagram 9 Which of the following is suitable to replace aspirin? star A Codeine B Morphine C Haloperidol D Paracetamol T5 Chapter 5.4 Medicines and Cosmetics
31 Diagram 10 shows the elements of P and Q in Periodic Table of Elements. Diagram 10 Why is the atomic size of atom Q bigger than atom P? star A The number of protons increases B The relative atomic mass increases C The number of valence electrons increases D The number of shell filled with electrons increases T4 Chapter 4.2 The Arrangement in the Periodic Table of Elements
32 Diagram 11 shows the arrangement of the apparatus for the titration process of sodium hydroxide solution with sulfuric acid. Diagram 11 What is the volume of sulphuric acid needed to neutralise sodium hydroxide solution in the conical flask? star A 10 cm^3 B 15 cm^3 C 20 cm^3 D 40 cm^3 T4 Chapter 6.7 Neutralisation
33 Diagram 12 shows energy profile of breaking of bond and formation of bond in exothermic reaction. | Bond | Bond energy (kJ mol^-1) | |---|---| | H – H | 436 | | Cl – Cl | 243 | | H – Cl | 432 | Diagram 12 Determine heat of reaction formation of HCl based on Diagram 12. star A +185 kJ mol^-1 B -185 kJ mol^-1 C +247 kJ mol^-1 D -247 kJ mol^-1 T5 Chapter 3.1 Heat Change in Reactions
34 The following equation represents the decomposition reaction of zinc nitrate which is imbalanced. Zn(NO_3)_2 \longrightarrow ZnO + NO_2 + O_2 What is the maximum volume of nitrogen dioxide gas released at standard temperature and pressure (STP) when 18.9 g of zinc nitrate was heated? [Relative formula mass : Zn(NO_3)_2 = 189 g mol^-1; Molar volume of gas at STP = 22.4 dm^3 mol^-1] star A 1.12 dm^3 B 2.24 dm^3 C 3.36 dm^3 D 4.48 dm^3 T4 Chapter 3.2 Mole Concept T4 Chapter 3.4 Chemical Equation T4 Chapter 6.10 Effect of Heat on Salts
35 When 15 g of carbon burns completely in air, the heat produced raises the temperature of 500 cm^3 of water by 23.8 °C. What is the heat of combustion of carbon? [Relative atomic mass : C = 12; Specific heat capacity of water, c = 4.2 J g^-1 °C^-1; Density of water = 1 g cm^-3] star A - 62.5 kJ mol^-1 B - 57.0 kJ mol^-1 C - 50.0 kJ mol^-1 D - 40.0 kJ mol^-1 T5 Chapter 3.2 Heat of Reaction
36 Diagram 13 shows reaction to produce compound P from compound R. Chemical formula for compound R is C4H9OH. Diagram 13 What is the percentage of carbon by mass in compound P? [Relative atomic mass : C = 12, H = 1, O = 16] star A 14.29% B 16.67% C 68.57% D 85.71% T4 Chapter 3.1 Relative Atomic Mass and Relative Molecular Mass T5 Chapter 2.3 Chemical Properties and Interconversion of Compounds Between Homologous Series
37 0.5 mol of J reacts with 24.0 g of oxygen to form J oxide. Which of the following formulas shows the empirical formula for J oxide? [Relative atomic mass: O = 16] star A JO_3 B J_3O C JO D J_2O_3 T4 Chapter 3.2 Mole Concept T4 Chapter 3.3 Chemical Formula
38 Diagram 14 shows cell notation for chemical cells. Zn(s) | Zn^2+(aq) || Cu^2+(aq) | Cu(s) Diagram 14 If the experiment is conducted by using 100 cm^3 of 0.5 mol dm^-3 zinc nitrate solution and 100 cm^3 of 0.5 mol dm^-3 copper(II) sulphate solution. What is the maximum mass of solid deposited at cathode? [Relative atomic mass: Cu = 64, Zn = 65] star A 2.80 g B 3.20 g C 3.25 g D 3.50 g T4 Chapter 6.5 Concentration of Aqueous Solution T5 Chapter 1.3 Voltaic Cell
39 Diagram 15 shows an energy profile diagram obtained from two sets of experiments. Diagram 15 Which of the following statements are correct about Set I and Set II? | | Set I | Set II | |:---|:---|:---| | A | The reaction releases heat without the presence of catalyst. | The reaction releases heat with the presence of catalyst. | | B | The reaction releases heat with the presence of catalyst. | The reaction releases heat without the presence of catalyst. | | C | The reaction absorbs heat with the presence of catalyst. | The reaction absorbs heat without the presence of catalyst. | | D | The reaction absorbs heat without the presence of catalyst. | The reaction absorbs heat with the presence of catalyst. | star A A B B C C D D T4 Chapter 7.4 Collision Theory
40 Diagram 16 shows the apparatus set up to study the elasticity of vulcanised rubber and unvulcanised rubber. Diagram 16 Table 1 shows the result of the experiment. | Type of rubber | P | Q | |---|---|---| | Initial length of rubber (cm) | 10 | 10 | | Length of rubber with weight (cm) | 14 | 16 | | Length of rubber after weight is removed (cm) | 12 | 10 | Table 1 Choose the correct statement about rubber P and rubber Q. star A Rubber Q is weaker than rubber P. B Rubber Q is oxidised easily. C Rubber Q is more elastic than rubber P. D Rubber P has higher resistant towards heat than rubber Q. T5 Chapter 4.2 Natural Rubber