0620_s24_qp_32
A paper of Chemistry, 0620
Questions:
8
Year:
2024
Paper:
3
Variant:
2
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1
shows the structures of seven substances, A, B, C, D, E, F and G. A B C D E F G H N H H H C H H O H O O H C H N N O O Cl – Cs+ Cl – Cs+ Cl – Cs+ Cl – Cs+ Cl – Cs+ Cl – Cs+ Answer the following questions using only the structures in . Each structure may be used once, more than once or not at all. State which structure represents: a gas that forms 78% by volume of clean, dry air a compound with a high melting point a giant covalent structure a compound in the same homologous series as ethanol a product of photosynthesis a non-metallic element that conducts electricity. Complete to show the dot-and-cross diagram for structure G. Show the outer electron shells only. N H H H , ,
2. Atoms, elements and compounds  →  2.5. Simple molecules and covalent bonds
1. States of matter  →  1.1. Solids, liquids and gases
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Blood plasma is the liquid part of blood. Table 2.1 shows the mass, in mg, of some ions present in 100 cm3 of blood plasma. Table 2.1 name of ion formula of ion mass of ion in 100 cm3 of blood plasma / mg calcium Ca2+ 10.0 chloride Cl – 365.6 hydrogencarbonate HCO3 – 164.7 hydrogen phosphate HPO4 2– 9.6 magnesium Mg2+ 3.6 potassium K+ 19.5 sodium Na+ 326.6 SO4 2– 4.8 Answer these questions using information from Table 2.1. Name the positive ion in Table 2.1 that is present in the lowest concentration in blood plasma. Name the ion in Table 2.1 that contains an element in Group V of the Periodic Table. Name the compound containing Na+ ions and SO4 2– ions. Describe a test for chloride ions. test observations Choose from the list the salt that is insoluble in water. Tick (✓) one box. calcium sulfate magnesium chloride potassium sulfate sodium chloride Table 2.2 shows some properties of the Group I metals. Table 2.2 metal density in g / cm3 observations on reaction with water lithium 0.53 bubbles form very slowly and no flame sodium 0.97 potassium 0.86 bubbles form very rapidly and flame rubidium explodes Use the information in Table 2.2 to: ● suggest why it is difficult to predict the density of rubidium ● describe the observations when sodium reacts with water. State how the melting point of the Group I elements changes down the Group. Sodium oxide, Na2O, can be made by heating sodium in a limited supply of oxygen. Complete the symbol equation for this reaction. Na + O2 → Na2O , ,
12. Experimental techniques and chemical analysis  →  12.5. Identification of ions and gases
9. Metals  →  9.4. Reactivity series
8. The Periodic Table  →  8.1. Arrangement of elements
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shows the apparatus used to electrolyse molten magnesium chloride. + – power supply unreactive gas molten magnesium Label the anode in . Name a non-metal that can be used as the anode. Name the product formed at each electrode. positive electrode negative electrode Use your knowledge of the reactivity of magnesium to suggest why an unreactive gas is blown into the electrolysis cell. Alloys of magnesium and aluminium are used to make aircraft. State the meaning of the term alloy. Magnesium reacts with hydrochloric acid. Write the formula of the ion that is present in all acids. Name the gas produced when hydrochloric acid reacts with magnesium. Dilute hydrochloric acid is added to a solution of thymolphthalein in aqueous sodium hydroxide until the acid is in excess. State the colour change of the thymolphthalein. from to Name the indicator that can be used to determine the pH of a sample of dilute hydrochloric acid. , ,
4. Electrochemistry  →  4.1. Electrolysis
9. Metals  →  9.4. Reactivity series
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Some plants produce ethene gas. Draw the displayed formula for a molecule of ethene. The incomplete combustion of ethene produces a small amount of carbon dioxide. Name two other products of the incomplete combustion of ethene. and A student extracts a mixture of coloured compounds from a plant. shows the results of chromatography of this mixture. chromatography paper Complete , to show: ● where the mixture of coloured compounds is placed on the chromatography paper at the start of the chromatography ● the level of the solvent at the start of the chromatography. State two characteristics of a mixture.
12. Experimental techniques and chemical analysis  →  12.3. Chromatography
11. Organic chemistry  →  11.2. Naming organic compounds
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An atom of sulfur is represented by the symbol shown. 34S Describe this atom of sulfur in terms of: ● the position of the electrons, neutrons and protons in the atom ● the number of neutrons and number of protons ● the electronic configuration. Sulfur burns to produce sulfur dioxide. State one adverse effect of sulfur dioxide in the air. Complete the symbol equation for the reaction of sulfur dioxide with magnesium. + 2Mg → MgO + S shows the displayed formula of a compound of sulfur. F S O O O S O O F Deduce the molecular formula of this compound. Another compound of sulfur has the formula Na2S2O7. Complete Table 5.1 to calculate the relative formula mass of Na2S2O7. Table 5.1 type of atom number of atoms relative atomic mass sodium 2 × 23 = 46 sulfur oxygen relative formula mass = , ,
6. Chemical reactions  →  6.3. Reversible reactions and equilibrium
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Solid nitrogen pentoxide, N2O5, decomposes to produce nitrogen dioxide gas and oxygen gas. Complete the equation by adding the missing state symbols. 2N2O5→ 4NO2( ) + O2( ) shows how the mass of nitrogen pentoxide changes as the reaction proceeds. time / minutes mass of nitrogen pentoxide / g On , draw an X to show where the rate of reaction is fastest. Deduce the mass of nitrogen pentoxide 12 minutes from the start of the reaction. At 50 °C, the reactant and products are all gases. Describe the effect each of the following has on the rate of decomposition of nitrogen pentoxide. All other conditions stay the same. ● The pressure is decreased. ● A catalyst is added to the reaction mixture. Increasing the concentration of nitrogen pentoxide increases the rate of decomposition. Choose the correct unit of concentration from the list. Draw a circle around your chosen answer. dm3 / g g / dm g / dm2 g / dm3 Some oxides of nitrogen such as nitrogen dioxide are acidic air pollutants. Choose the pH value which is acidic. Draw a circle around your chosen answer. pH 1 pH 7 pH 8 pH 14 State one way of reducing the emissions of nitrogen dioxide in cars. Nitrogen dioxide is a yellow liquid which evaporates to form a brown gas at room temperature. A long glass tube is set up as shown in . glass tube small dish containing liquid nitrogen dioxide At first, the brown gas can only be seen above the small dish. After a short time, the brown gas has completely filled the tube. Explain these results in terms of kinetic particle theory. , ,
6. Chemical reactions  →  6.2. Rate of reaction
10. Chemistry of the environment  →  10.3. Air quality and climate
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Iron and copper are transition elements. They are malleable and are good thermal and electrical conductors. State three other physical properties of iron. shows some clean iron nails placed in four test-tubes, M, N, O and P, under different conditions. boiled water dry air oil air iron nail M N O water P State in which test-tube, M, N, O or P, the iron nail is most likely to rust. Choose from the list the compound in rust. Tick (✓) one box. anhydrous iron(oxide anhydrous iron(sulfate hydrated iron(chloride hydrated iron(oxide Copper is used in electrical wiring because of its good electrical conductivity. State one other reason why copper is used in electrical wiring. Copper(oxide reacts with hydrochloric acid. Complete the word equation for this reaction. copper(oxide + hydrochloric acid → + Copper can be produced by heating copper(oxide in hydrogen. CuO + H2 → Cu + H2O Describe how this equation shows that copper(oxide is reduced. The list shows five metals. aluminium copper gold magnesium potassium Put these metals in order of their reactivity. Put the most reactive metal at the top. least reactive most reactive , ,
9. Metals  →  9.5. Corrosion of metals
9. Metals  →  9.2. Uses of metals
9. Metals  →  9.4. Reactivity series
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This question is about carboxylic acids and alkanes. Table 8.1 shows the names, formulae and boiling points of some carboxylic acids. Table 8.1 name formula boiling point / °C methanoic acid HCOOH ethanoic acid CH3COOH propanoic acid C2H5COOH butanoic acid C3H7COOH Use the information in Table 8.1 to answer these questions. State the trend in the boiling points of the carboxylic acids. Deduce the general formula for carboxylic acids. Complete the word equation for the reaction of ethanoic acid with sodium carbonate. ethanoic acid + sodium carbonate → sodium ethanoate + + Choose the correct formula of sodium ethanoate from the list. Draw a circle around your chosen answer. CH3CH2ONa CH3CH2COONa CH3COONa (CH3COO)2Na Methane, ethane and propane belong to the alkane homologous series. Define the term homologous series. State the type of bonding in a methane molecule. State two types of reaction of the alkanes. , ,
11. Organic chemistry  →  11.7. Carboxylic acids
11. Organic chemistry  →  11.2. Naming organic compounds
11. Organic chemistry  →  11.1. Formulae, functional groups and terminology
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