Chemistry 0620/31 May/June 2025: question paper and mark scheme

Question

A list of substances is shown. aluminium ammonia argon bromine carbon dioxide fluorine iron magnesium magnesium chloride nitrogen oxygen potassium Answer the following questions about these substances. Each substance may be used once, more than once or not at all. State which substance is: (a) an element which forms an ion with a 1+ charge …… [1] (b) a metal that is extracted in the blast furnace …… [1] (c) a soft metal that is more reactive than sodium …… [1] (d) approximately 78% of clean, dry air …… [1] (e) a gas that is identified using damp red litmus paper …… [1] (f) a liquid at room temperature and pressure …… [1] (g) an element used in food containers because of its resistance to corrosion …… [1] (h) a transition element. …… [1] [Total: 8]

Question

This question is about sea water and the substances found in sea water. (a) Table 2.1 shows the masses of the compounds formed when 1000 cm3 of sea water is evaporated. Table 2.1 compound formula mass of compound / g sodium chloride NaCl 14.0 magnesium sulfate MgSO4 3.0 potassium chloride KCl 1.0 CaCO3 1.0 Answer these questions, using the information from Table 2.1. (i) State the chemical name of CaCO3. …… [1] (ii) The total mass of compounds formed from 1000 cm3 of sea water is 19.0 g. Calculate the total mass of compounds formed from 1750 cm3 of sea water. mass = …… g [1] (iii) Magnesium sulfate is soluble in water. Choose one other compound that is soluble in water. Tick (3) one box. lead(II) chloride magnesium carbonate potassium hydroxide silver chloride [1] (b) Potassium chloride is found in sea water and contains chloride ions. Describe a test for chloride ions. test …… observations …… [2] (c) Sodium ions are in sea water. Complete Fig. 2.1 to show: • the electronic configuration of a sodium ion • the charge on the ion. Na Fig. 2.1 [2] (d) Sodium chloride forms a liquid when heated. Describe the arrangement and motion of the particles in a liquid. arrangement …… motion …… [2] (e) Sodium chloride is an ionic compound that dissolves in water. State two other properties of an ionic compound. 1 …… 2 …… [2] (f) Sea water contains dissolved gases. Name the gas that is essential for aquatic life. …… [1] [Total: 12]

Question

This question is about sulfur and its compounds. (a) (i) Explain why sulfur is placed in Group VI of the Periodic Table. …… [1] (ii) Two isotopes of sulfur are shown in Fig. 3.1. 33 S 36 S 16 16 Fig. 3.1 Complete Table 3.1 to show the number of protons, neutrons and electrons in one atom of these isotopes. Table 3.1 protons neutrons electrons 33 S 16 36 S 16 [3] (b) Sulfur dioxide is an air pollutant. (i) State one source of sulfur dioxide in the air. …… [1] (ii) State one adverse effect on the environment of sulfur dioxide. …… [1] (iii) Sulfur dioxide reacts with hydrogen sulfide. Complete the symbol equation for this reaction. SO2 + 2H2S ……S + ……H2O [2] (iv) State the type of bonding between the atoms in sulfur dioxide. …… [1] (c) A compound of sulfur has the formula Al 2(SO4)3. Complete Table 3.2 to calculate the relative formula mass of Al 2(SO4)3. Table 3.2 atom number of atoms relative atomic mass oxygen 12 16 12 × 16 = 192 aluminium 27 sulfur 32 relative formula mass = …… [2] [Total: 11]

Question

This question is about organic chemistry. (a) (i) Name the process that separates petroleum into its useful components. …… [1] (ii) Fuel oil is obtained from petroleum. State one use of fuel oil. …… [1] (iii) Natural gas is a fossil fuel. Draw a circle around one compound that is the main constituent of natural gas. carbon dioxide ethane ethanol methane [1] (b) (i) Describe how long chain hydrocarbon molecules can be made into short chain molecules. Include in your answer: • the name of this process • the conditions needed for this process to take place • the products of this process. …… [4] (ii) State one reason why long chain hydrocarbon molecules are made into short chain hydrocarbon molecules. …… [1] (c) Draw the displayed formula of a molecule of ethane. [1] (d) (i) Ethanol is manufactured by fermentation of aqueous glucose. State two conditions for fermentation. 1 …… 2 …… [2] (ii) State one use of ethanol. …… [1] (e) Fig. 4.1 shows the displayed formula of an organic molecule. H O H H H O H H O C C C C C C H H H H Fig. 4.1 (i) Deduce the molecular formula of this molecule. …… [1] (ii) Explain why the molecule in Fig. 4.1 is unsaturated. …… [1] [Total: 14]

Question

This question is about metals and their reactions. (a) A student investigates the reaction of four different metals, A, B, C and D, with dilute hydrochloric acid. All other conditions are the same in each test-tube. The results of the experiment are shown in Fig. 5.1. bubbles A B C D Fig. 5.1 (i) Put the metals, A, B, C and D, in their order of reactivity. most reactive …… least reactive …… [1] (ii) One way the student can increase the rate of the reaction in the experiment is to use a higher concentration of acid. State two other ways to increase the rate of this reaction. 1 …… 2 …… [2] (iii) Hydrogen gas is produced in this experiment. Describe a test for hydrogen gas. test …… observations …… [1] (iv) State the formula of the ion that is present in all acids. …… [1] (b) Stainless steel is an alloy. (i) State the meaning of the term alloy. …… [1] (ii) State one property of stainless steel that makes it suitable for cutlery. …… [1] [Total: 7]

Question

This question is about ionic and covalent compounds. (a) Complete the word equation to show the reaction between magnesium carbonate and nitric acid. magnesium + …… + …… + nitric acid …… carbonate [3] (b) Crystals of copper(II) chloride are prepared by adding excess copper(II) oxide powder to dilute hydrochloric acid. Describe how to prepare a sample of pure, dry copper(II) chloride crystals after the reaction is complete. In your answer, describe how to: • remove the excess copper(II) oxide from the reaction mixture • crystallise the copper(II) chloride • dry the crystals. …… [3] (c) (i) Fig. 6.1 shows the apparatus for the electrolysis of molten lithium iodide, using inert electrodes. – power + supply heat Fig. 6.1 Label Fig. 6.1 to show the: • anode • molten lithium iodide. [2] (ii) Platinum metal is used as an inert electrode in this electrolysis experiment. Name one other suitable material that can be used as an inert electrode. …… [1] (iii) Name the products formed at the positive and negative electrodes when molten lithium iodide is electrolysed. positive electrode …… negative electrode …… [2] (d) Table 6.2 shows some properties of five compounds, A, B, C, D and E. Table 6.2 electrical conductivity compound density in g / cm3 melting point in °C when molten A does not conduct 3.53 1856 B does not conduct 1.57 –157 C conducts 1.93 110 D conducts 3.03 1256 E does not conduct 4.93 –83 State which two of the compounds, A, B, C, D and E, are simple molecules. Give two reasons for your answer. compounds …… and …… reason 1 …… reason 2 …… [3] [Total: 14]

Question

This question is about energy changes in reactions. (a) Table 7.1 shows the results of four experiments. Table 7.1 experiment initial temperature / °C final temperature / °C 1 17 23 2 21 13 3 18 14 4 19 26 (i) State which experiment shows the greatest temperature change. …… [1] (ii) In experiment 4, zinc was added to dilute hydrochloric acid. Complete the symbol equation. Zn + ……HCl ZnCl 2 + …… [2] (iii) Fig. 7.1 shows the incomplete reaction pathway diagram for the reaction in Experiment 4. Fig. 7.1 Complete Fig. 7.1 by labelling: • the vertical axis • the reactants • the products. [2] (b) Fig. 7.2 shows the changes of state of copper. G solid liquid gas H Fig. 7.2 Name the changes of state labelled G and H. G …… H …… [2] [Total: 7]

Question

This question is about water and air. (a) River water needs to be treated to make it safe to drink. Two of the stages used in the treatment of domestic water are the addition of carbon and chlorination. Describe the reason for each of these stages. addition of carbon …… chlorination …… [2] (b) Describe how to test whether a sample of water is pure using boiling point. …… [2] (c) Explain why distilled water is used in practical chemistry rather than tap water. …… [1] (d) A sample of polluted air contains carbon monoxide and methane. State one harmful effect of each of these air pollutants. carbon monoxide …… methane …… [2] [Total: 7] The Periodic Table of Elements Group I II III IV V VI VII VIII 1 2 H He hydrogen helium Key 1 4 3 4 atomic number 5 6 7 8 9 10 Li Be atomic symbol B C N O F Ne lithium beryllium name boron carbon nitrogen oxygen fluorine neon 7 9 relative atomic mass 11 12 14 16 19 20 11 12 13 14 15 16 17 18 Na Mg Al Si P S Cl Ar sodium magnesium aluminium silicon phosphorus sulfur chlorine argon 23 24 27 28 31 32 35.5 40 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr potassium calcium scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton 39 40 45 48 51 52 55 56 59 59 64 65 70 73 75 79 80 84 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon 20 85 88 89 91 93 96 – 101 103 106 108 112 115 119 122 128 127 131 55 56 57–71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 lanthanoids Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn caesium barium hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon 133 137 178 181 184 186 190 192 195 197 201 204 207 209 – – – 87 88 89–103 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118 actinoids Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og francium radium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium copernicium nihonium flerovium moscovium livermorium tennessine oganesson – – – – – – – – – – – – – – – – – 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 lanthanoids La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu lanthanum cerium praseodymium neodymium promethium samarium europium gadolinium terbium dysprosium holmium erbium thulium ytterbium lutetium 139 140 141 144 – 150 152 157 159 163 165 167 169 173 175 89 90 91 92 93 94 95 96 97 98 99 100 101 102 103 actinoids 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 – – – – – – – – – – – The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).