Chemistry 0620/11 May/June 2019: question paper and mark scheme

Question

Sodium chloride is a liquid at 900 °C. How are the particles arranged and how do the particles move in sodium chloride at 900 °C? arrangement of particles motion of particles A regular vibrate about a fixed point B regular move randomly C random vibrate about a fixed point D random move randomly

Question

2.00 g of powdered calcium carbonate is added to 50.0 cm3 of hydrochloric acid. Which apparatus is used to measure the calcium carbonate and the hydrochloric acid? calcium carbonate hydrochloric acid A balance burette B balance thermometer C pipette burette D pipette thermometer

Question

Rock salt is a mixture of sand and sodium chloride. Sodium chloride is soluble in water but not in hexane. Sand is insoluble in both water and hexane. What is required to separate the sand from the sodium chloride? 1 filter paper 2 fractionating column 3 hexane 4 water A 1 and 3 B 1 and 4 C 2 and 3 D 2 and 4

Question

The colours in four dyes are separated using chromatography. Which chromatogram shows an insoluble colour? A B C D baseline

Question

Which statement about an atom of fluorine, 199 F, is correct? A It contains more protons than neutrons. B It contains a total of 28 protons, neutrons and electrons. C Its isotopes contain different numbers of protons. D Its nucleus contains 9 neutrons.

Question

Calcium reacts with chlorine to produce calcium chloride. What happens when a calcium ion forms during this reaction? A The calcium atom gains one electron. B The calcium atom gains two electrons. C The calcium atom loses one electron. D The calcium atom loses two electrons.

Question

Which row describes the formation of single covalent bonds in methane? A atoms share a pair of electrons both atoms gain a noble gas electronic structure B atoms share a pair of electrons both atoms have the same number of electrons in their outer shell C electrons are transferred from one both atoms gain a atom to another noble gas electronic structure D electrons are transferred from one both atoms have the same number atom to another of electrons in their outer shell

Question

Diamond and graphite have giant covalent structures of carbon atoms. Which statement describes graphite? A It has a strong, rigid three-dimensional structure. B It has four strong covalent bonds between each carbon atom. C It has layers, which can slide over each other. D It has no free electrons, so does not conduct electricity.

Question

The compound magnesium nitrate has the formula Mg(NO3)2. What is the relative formula mass of magnesium nitrate? A 86 B 134 C 148 D 172

Question

Four substances are electrolysed using inert electrodes. Which row describes the electrode products? substance anode product cathode product A concentrated aqueous sodium chloride hydrogen chlorine B concentrated hydrochloric acid chlorine oxygen C dilute sulfuric acid oxygen hydrogen D molten lead bromide lead bromine

Question

Dissolving ammonium chloride in water is an endothermic change. Which row shows the energy change and temperature change of the mixture during the dissolving of ammonium chloride? energy change temperature change A energy is absorbed decrease B energy is absorbed increase C energy is released decrease D energy is released increase

Question

Which process is a physical change? A burning wood B cooking an egg C melting an ice cube D rusting iron

Question

Hydrogen peroxide solution decomposes very slowly at room temperature to produce oxygen gas. This gas forms a rising foam when liquid detergent is added. Five test-tubes are half filled with hydrogen peroxide solution. A drop of liquid detergent is added to each one. Different metal oxides are added to four of the test-tubes and the height of the foam formed after 1 minute is measured. The results are shown. height of metal oxide foam / cm no metal oxide added 0.1 aluminium oxide 0.1 calcium oxide 0.2 copper(II) oxide 2.3 manganese(IV) oxide 5.4 Which conclusion can be drawn from these results? A Metal oxides do not affect the rate of this reaction. B All metal oxides increase the rate of this reaction and act as catalysts. C Manganese(IV) oxide is the best catalyst of the four metal oxides tested. D Only transition element oxides increase the rate of this reaction.

Question

When blue-green crystals of nickel(II) sulfate are heated, water is produced and a yellow solid remains. When water is added to the yellow solid, the blue-green colour returns. Which process describes these changes? A combustion B corrosion C neutralisation D reversible reaction

Question

In a blast furnace, iron is extracted when iron(III) oxide reacts with carbon monoxide. The equation is shown. Fe2O3 + 3CO → 2Fe + 3CO2 Which substance is oxidised and which is reduced? oxidised reduced A CO Fe2O3 B CO2 Fe C Fe CO2 D Fe2O3 CO

Question

Four different solutions are separately tested with blue litmus and with methyl orange. Each solution is known to be either acidic or alkaline. The results are shown. result with result with solution blue litmus methyl orange 1 red red 2 red yellow 3 blue yellow 4 blue yellow Which statement is correct? A Solutions 1 and 4 are acidic. B Solutions 1 and 2 are alkaline. C Solutions 3 and 4 are alkaline. D Solutions 3 and 4 are acidic.

Question

The positions of elements W, X, Y and Z in the Periodic Table are shown. W Y X Z Which elements form basic oxides? A W, X and Y B W and X only C Y only D Z only

Question

How could crystals of a pure salt be prepared from dilute sulfuric acid? A add an excess of aqueous sodium hydroxide, filter, evaporate the filtrate to crystallisation point B add an excess of copper(II) carbonate, filter, evaporate the filtrate to dryness C add an excess of copper metal, filter, evaporate the filtrate to crystallisation point D add an excess of zinc oxide, filter, evaporate the filtrate to crystallisation point

Question

The results of two tests on a solution of compound Q are shown. test observation add ammonia solution green precipitate formed add dilute nitric acid followed white precipitate formed by aqueous barium nitrate What is Q? A iron(II) chloride B iron(II) sulfate C iron(III) chloride D iron(III) sulfate

Question

The properties of an element are shown. electrical conductivity density reaction with water high low reacts violently with cold water Which element has these properties? A B C D

Question

Which statement about elements in Group I and Group VII of the Periodic Table is correct? A Bromine reacts with potassium chloride to produce chlorine. B Iodine is a monoatomic non-metal. C Lithium has a higher melting point than potassium. D Sodium is more reactive with water than potassium.

Question

Which row describes the properties of a transition element? melting forms coloured density point compounds A high low no B high high yes C low low no D low low yes

Question

Which statement about elements in Group VIII of the Periodic Table is correct? A They all have a full outer shell of electrons. B They all react with Group I elements to form ionic compounds. C They are all diatomic molecules. D They are all liquids at room temperature.

Question

The diagrams show the structure of two substances used to make electrical conductors. X Y Which statement correctly describes X and Y? A X is a pure metal and Y is a compound. B X is a pure metal and Y is an alloy. C X is a solid and Y is a liquid. D X is harder and stronger than Y.

Question

The reactions of three metals, P, Q and R, are shown. metal reacts with metal reacts dilute hydrochloric acid with water P yes no Q no no R yes yes What is the order of reactivity of the metals? most least reactive reactive A P Q R B Q R P C R Q P D R P Q

Question

Iron is extracted from its ore in a blast furnace. Hematite, coke, limestone and hot air are added to the furnace. Which explanation is not correct? A Coke burns and produces a high temperature. B Hematite is the ore containing the iron as iron(III) oxide. C Hot air provides the oxygen for the burning. D Limestone reduces the iron(III) oxide to iron.

Question

Why is aluminium used to make containers for storing food? A It conducts electricity. B It has a high melting point. C It is resistant to corrosion. D It is strong.

Question

Water can be treated by filtration then chlorination. Which uses do not need water of this quality? 1 water for cooling in industry 2 water for washing clothes 3 water for drinking A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

Question

Four sources of air pollution are listed. 1 burning fossil fuels containing sulfur 2 nitrogen reacting with oxygen in car engines 3 incomplete combustion of carbon fuels 4 adding lead compounds to petrol Which sources produce acid rain? A 1 and 2 B 1 and 3 C 2 and 3 D 3 and 4

Question

The diagram shows an experiment to investigate how paint affects the rusting of iron. P Q iron painted iron air water What happens to the water level in tubes P and Q? tube P tube Q A falls rises B no change rises C rises falls D rises no change

Question

A mixture of two substances, R and S, is heated. The damp red litmus paper turns blue. damp red litmus paper R and S gentle heat What are R and S? R S A a basic oxide ammonium chloride B a basic oxide sodium nitrate C an acidic oxide ammonium chloride D an acidic oxide sodium nitrate

Question

Which statement describes a disadvantage of sulfur dioxide? A It can be used as a bleach when making wood pulp. B It can be used to kill bacteria in food. C It can be used to manufacture sulfuric acid. D It dissolves in water to form acid rain.

Question

The diagram represents a lime kiln used to heat limestone to a very high temperature. waste gases lime kiln limestone fuel in fuel in air in air in X What leaves the kiln at X? A calcium carbonate B calcium hydroxide C calcium oxide D calcium sulfate

Question

What is the structure of ethanol? A B C D H H H H H O H H C C H C C H H C C H C C OH H H H H H OH H H

Question

Which fuel could be gasoline? Is it obtained from petroleum? yes no Is it used as Is it used as fuel for cars? fuel for cars? yes no yes no A B C D

Question

A hydrocarbon W burns to form carbon dioxide and water. W decolourises bromine water. What is the name of W and what is its structure? name of W structure of W H H A ethane H C C H H H H H B ethane C C H H H H C ethene H C C H H H H H D ethene C C H H

Question

Why is ethanol a member of the homologous series of alcohols but propane is not? A Ethanol has two carbon atoms per molecule but propane has three. B Ethanol can be made from ethene but propane is obtained from petroleum. C Ethanol is a liquid but propane is a gas. D Ethanol contains the same functional group as other alcohols but propane does not.

Question

Which statements about ethanol are correct? 1 It can be made by fermentation. 2 It is an unsaturated compound. 3 It burns in air and can be used as a fuel. A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

Question

Which statements about aqueous ethanoic acid are correct? 1 Ethanoic acid contains the functional group –COOH. 2 Ethanoic acid reacts with carbonates to produce hydrogen. 3 Ethanoic acid turns Universal Indicator paper blue. 4 Ethanoic acid has a pH lower than pH 7. A 1 and 2 B 1 and 3 C 1 and 4 D 2 and 4

Question

Which naturally occurring polymers are found in foods? 1 complex carbohydrates 2 nylon 3 salts 4 proteins A 1 and 2 B 1 and 4 C 2 and 3 D 3 and 4 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 85 88 89 91 93 96 – 101 103 106 108 112 115 119 122 128 127 131 16 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 89–103 104 105 106 107 108 109 110 111 112 114 116 actinoids Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Fl Lv francium radium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium copernicium flerovium livermorium – – – – – – – – – – – – – 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.).