0620_s22_qp_33
A paper of Chemistry, 0620
Questions:
8
Year:
2022
Paper:
3
Variant:
3
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1
A list of symbols and formulae is shown. Al 2O3 C2H5OH CO2 Fe2O3 H2 He K+ Li+ N2 Na+ O2– Answer the following questions using these symbols or formulae. Each symbol or formula may be used once, more than once or not at all. State which symbol or formula represents: an element that is monoatomic an ion that gives a red colour in a flame test an element that can be used as a fuel a gas that contributes to climate change an ion that is formed when an atom gains electrons. Complete the table to show the relative charges of a proton, neutron and electron. type of particle relative charge proton neutron electron  Choose the two correct statements about nitrogen and hydrogen in a mixture. Tick (✓) two boxes. The nitrogen and hydrogen mixture can be separated by physical means. The nitrogen and hydrogen mixture is liquid at room temperature. The atoms of nitrogen and hydrogen in the mixture are chemically combined. Air is mainly a mixture of nitrogen and hydrogen. The bonding in both nitrogen and hydrogen molecules is covalent.  
2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table
7. Acids, bases and salts  →  7.1. The characteristic properties of acids and bases
3. Stoichiometry  →  3.1. Formulae
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2
The table shows the masses of some ions in a 1000 cm3 sample of toothpaste. name of ion formula of ion mass of ion in 1000 cm3 of toothpaste / g NH4 + 0.2 calcium Ca2+ 0.8 CO3 2– 0.7 chloride Cl – 0.9 fluoride F– 2.2 magnesium Mg2+ 2.0 phosphate PO4 3– 24.4 sodium Na+ 34.2 sulfate SO4 2– 10.1 tin(Sn2+ 0.4 zinc Zn2+ 0.1 Answer these questions using only the information in the table. State which negative ion has the highest mass in 1000 cm3 of toothpaste. Name the compound that contains NH4 + and CO3 2– ions. Calculate the mass of fluoride ions in 250 cm3 of toothpaste.  mass = g Describe the observations when aqueous ammonia is added drop by drop to a solution containing zinc ions until the ammonia is in excess. observations with a few drops of ammonia observations with ammonia in excess  Toothpaste also contains compound A. The structure of compound A is shown. H C H H H H C O H H C O H Deduce the formula of compoundA to show the number of atoms of carbon, hydrogen and oxygen. CompoundA is an alcohol. EthanoI, C2H5OH, is also an alcohol. Complete these sentences about ethanol using words from the list. different formula group identical molecule similar Ethanol is part of the alcohol homologous series. Each member of the alcohol homologous series has the same functional . Members of the same homologous series have chemical properties that are .  When ethanol undergoes incomplete combustion, a small amount of carbondioxide is produced. Name two other substances that are produced when ethanol undergoes incomplete combustion. and ��������������������������������������������������������������� 
12. Experimental techniques and chemical analysis  →  12.5. Identification of ions and gases
11. Organic chemistry  →  11.6. Alcohols
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3
This question is about GroupI and GroupVII elements. Deduce the number of electrons, neutrons and protons in one atom of the isotope of sodium shown. 23Na number of electrons number of neutrons number of protons  Sodium reacts with chlorine to produce sodium chloride. State the colour of chlorine gas. Chlorine is a diatomic molecule. State the meaning of the term diatomic. Complete the chemical equation for the reaction of sodium with chlorine. 2Na + → NaCl Sodium chloride is an ionic compound. Describe two physical properties of ionic compounds.  The table shows some properties of four GroupI elements. element melting point / °C boiling point / °C atomic radius / nm lithium 0.157 sodium potassium 0.235 rubidium 0.250 Complete the table by predicting: ● the melting point of potassium ● the atomic radius of sodium. Predict the physical state of rubidium at 700 °C. Give a reason for your answer. Give two physical properties of GroupI metals that are different from transition elements and state how they are different.  Aqueous chlorine reacts with aqueous sodium iodide. Cl 2 + 2NaI → 2NaCl + I2 Explain how this equation shows that chlorine is more reactive than iodine. 
8. The Periodic Table  →  8.1. Arrangement of elements
8. The Periodic Table  →  8.3. Group VII properties
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4
This question is about acids and carbonates. Describe the colour change when excess acid is added to a solution of methyl orange in alkaline solution. from to ���������������������������������������������������������������� Complete the word equation for the reaction of hydrochloricacid with calcium carbonate. hydrochloric acid + calcium carbonate + + water  Calcium carbonate decomposes when heated. calcium carbonate → calcium oxide + carbon dioxide Calcium carbonate is used in the manufacture of lime (calcium oxide). State one other use of calcium carbonate. The decomposition of calcium carbonate is endothermic. State the meaning of the term endothermic. The energy level diagram for the decomposition of calcium carbonate is shown. energy progress of reaction CaCO3 CaO + CO2 Explain how the energy level diagram shows that this reaction is endothermic. When 0.50 g of calciumcarbonate decomposes, 120 cm3 of carbondioxide gas is produced. Calculate the volume of carbondioxide gas produced when 0.10 g of calciumcarbonate is used.  volume of carbon dioxide gas = cm3 
11. Organic chemistry  →  11.7. Carboxylic acids
9. Metals  →  9.4. Reactivity series
5. Chemical energetics  →  5.1. Exothermic and endothermic reactions
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5
This question is about GroupVI elements and their compounds. Name the changes of physical state when: ● oxygen gas is converted to liquid oxygen ● solid sulfur is converted directly to sulfur gas.  Use the kinetic particle model to describe the differences between solid sulfur and sulfur gas in terms of: ● the arrangement of the particles ● the motion of the particles.  Deduce the electronic structure of sulfur. Use the Periodic Table to help you. Sulfur is used in the manufacture of sulfuric acid. The equation shows one of the reactions. 2SO2 + O2 2SO3 State the meaning of the symbol . Give one use of sulfur dioxide other than in making sulfuric acid. Acid rain is formed when sulfurdioxide reacts with water vapour in the atmosphere. Choose the pH value which is acidic. Draw a circle around your chosen answer. pH 4 pH 7 pH 10 pH 14 Describe one effect of acid rain on buildings. 
6. Chemical reactions  →  6.3. Reversible reactions and equilibrium
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6
The structures of four organic compounds, B, C, D and E, are shown. H H C H H C H H C H H H H C H H C H H O H H C H C O O H C C H H H H C H H B C D E State which compound, B, C, D or E, dissolves in water to form an acidic solution. State which compound, B, C, D or E, is a saturated hydrocarbon. State which compound, B, C, D or E, is an unreactive compound except in terms of burning. State which compound, B, C, D or E, decolourises aqueous bromine. Ethanol can be manufactured from ethene and one other reactant. Describe the manufacture of ethanol from ethene to include: ● the formula of ethene ● the name of the other reactant ● the conditions needed.  Complete the table to show the name and uses of some petroleum fractions. name of fraction use of fraction making chemicals kerosene fuel oil  
11. Organic chemistry  →  11.6. Alcohols
11. Organic chemistry  →  11.2. Naming organic compounds
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7
This question is about lithium and compounds of lithium. Lithium reacts with nitrogen to produce lithium nitride, Li3N. Complete the chemical equation for this reaction. Li + N2 → Li3N Molten lithium bromide is electrolysed using carbon electrodes. The apparatus is shown. power supply – + Complete the diagram by labelling: ● the anode ● the electrolyte. Name the products formed at each electrode. positive electrode negative electrode  The carbon electrodes conduct electricity. Give one other property that these electrodes must have. A compound of lithium has the formula C3H5O2Li2. Complete the table to calculate the relative molecular mass of C3H5O2Li2. atom number of atoms relative atomic mass carbon 3 × 12 = 36 hydrogen oxygen lithium  relative molecular mass = 
4. Electrochemistry  →  4.1. Electrolysis
12. Experimental techniques and chemical analysis  →  12.5. Identification of ions and gases
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8
A student investigates the rate of decomposition of aqueous hydrogenperoxide using 0.2 g of a catalyst. 2H2O2 → 2H2O + O2 The rate of reaction is found by measuring the volume of oxygen gas produced as time increases. The results are shown on the graph. volume of oxygen gas produced / cm3 time / s Deduce the time taken to collect 35 cm3 of oxygen gas.  time = s The experiment is repeated using 0.2 g of smaller pieces of the catalyst. All other conditions stay the same. Draw a line on the grid to show how the volume of oxygen gas produced changes as time increases.  Describe the effect each of the following has on the rate of decomposition of hydrogen peroxide. All other conditions stay the same. ● The reaction is carried out at a higher temperature. ● The reaction is carried out using a lower concentration of hydrogen peroxide.  Hydrogen peroxide reduces sodium chlorate(, NaCl O, to sodium chloride. H2O2 + NaCl O → NaCl + H2O + O2 Describe how this equation shows that sodium chlorate(has been reduced. 
6. Chemical reactions  →  6.2. Rate of reaction
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