0620_s23_qp_31
A paper of Chemistry, 0620
Questions:
8
Year:
2023
Paper:
3
Variant:
1
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Fig.1.1 shows part of the Periodic Table. I II III IV V VI VII VIII Na Al Cl C N O Mg H He K Ca Fe Cu Br I Answer the following questions using only the elements in Fig.1.1. Each symbol of the element may be used once, more than once or not at all. Give the symbol of the element that: forms 78% by volume of clean, dry air has an atom with a complete outer electron shell has an atom with five occupied electron shells forms an ion with a charge of 2– forms an ion that gives a green precipitate on addition of aqueous sodiumhydroxide is used in food containers because of its resistance to corrosion. 
8. The Periodic Table  →  8.1. Arrangement of elements
2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table
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Table2.1 shows some properties of the halogens. Table 2.1 halogen melting point in °C boiling point in °C density at room temperature and pressure in g / cm3 fluorine –220 –188 0.0016 chlorine –101 –35 0.0032 bromine +59 3.1 iodine +114 +184 Use the information in Table2.1 to predict: the melting point of bromine ��������������������������������������������������������������������������������������������������������������������������������������� the density of iodine at room temperature and pressure ��������������������������������������������������������������������������������������������������������������������������������������� the physical state of chlorine at –10 °C. Give a reason for your answer. physical state reason  The equation for the reaction of aqueous chlorine with aqueous potassiumiodide is shown. Cl 2 + 2KI → I2 + 2KCl Choose the word which best describes this type of chemical reaction. Draw a circle around your chosen answer. addition displacement neutralisation polymerisation Explain why aqueous iodine does not react with aqueous potassiumchloride. Complete the diagram in Fig.2.1 to show the electronic configuration of a chlorine atom. Cl  Describe a test for chlorine. test observations  
8. The Periodic Table  →  8.3. Group VII properties
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Water from natural sources contains dissolved gases. Choose from the list, the gas that is essential for aquatic life. Draw a circle around your chosen answer. argon hydrogen nitrogen oxygen Polluted water may contain harmful substances such as metal compounds, plastics, nitrates and phosphates. Name one other harmful substance which is present in polluted water. State why nitrates are harmful to aquatic life. Table3.1 shows the masses of ions, in mg, present in a 1000 cm3 sample of polluted water. Table 3.1 name of ion formula of ion mass of ion present in mg / 1000 cm3 of polluted water NH4 + 0.5 calcium Ca2+ 2.2 chloride Cl – 2.5 hydrogencarbonate HCO3 – 12.0 magnesium Mg2+ 0.8 nitrate NO3 – 0.4 potassium K+ 8.3 silicate SiO3 2– 8.0 sodium Na+ 10.2 sulfate SO4 2– 0.2 tin(Sn2+ 0.4 Answer these questions using information from Table3.1. Name the negative ion present in the highest concentration. State the name of the NH4 + ion. Calculate the mass of calcium ions present in 200 cm3 of polluted water.  mass = mg Copper(sulfate can be used to test for the presence of water. CuSO4+ 5H2OCuSO4•5H2Oanhydrous hydrated copper(sulfate copper(sulfate State the meaning of the term hydrated. Describe how hydrated copper(sulfate is changed to anhydrous copper(sulfate. Complete the symbol equation for the reaction of sodium with water. 2Na + H2O → 2NaOH +  
10. Chemistry of the environment  →  10.1. Water
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This question is about sulfur and compounds of sulfur. Sulfur has several isotopes. Define the term isotopes. Deduce the number of protons, neutrons and electrons in the sulfide ion shown. 36S2– number of protons number of neutrons number of electrons  Sulfur burns in oxygen to produce sulfurdioxide. Fig.4.1 shows an incomplete reaction pathway diagram for this reaction. energy progress of reaction Complete Fig.4.1 by writing these formulae on the diagram: ● S + O2 ● SO2. Explain how Fig.4.1 shows that the reaction is exothermic. Complete this sentence about an exothermic reaction using a word from the list. products reactants sulfur surroundings An exothermic reaction transfers thermal energy to the . Fig.4.2 shows the apparatus used for the electrolysis of dilute sulfuricacid using graphite electrodes. power supply + – Label Fig.4.2 to show: ● the cathode ● the electrolyte. Name the products and state the observations at the positive and negative electrodes. product at the positive electrode observations at the positive electrode product at the negative electrode observations at the negative electrode  Complete the word equation for the reaction of dilute sulfuricacid with sodiumcarbonate. sulfuric acid + sodium carbonate + +  A few drops of thymolphthalein indicator are added to dilute sulfuricacid. State the colour of the solution. 
4. Electrochemistry  →  4.1. Electrolysis
6. Chemical reactions  →  6.3. Reversible reactions and equilibrium
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This question is about metals. Iron is a transition element. Potassium is an element in GroupI of the Periodic Table. State two differences in the physical properties of iron compared to potassium.  Carbon is used to extract iron from iron ore in a blast furnace. State two uses of carbon in the extraction process.  Steel is an alloy of iron. State the meaning of the term alloy. State why alloys are more useful than pure metals. Table5.1 shows the observations made when four different metals react with dilute hydrochloric acid of the same concentration. Table 5.1 metal observations iron bubbles form slowly lead no bubbles formed magnesium bubbles form rapidly nickel bubbles form very slowly Put the four metals in order of their reactivity. Put the least reactive metal first. least reactive most reactive  
9. Metals  →  9.6. Extraction of metals
9. Metals  →  9.4. Reactivity series
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A student investigates the reaction of small pieces of zinc of the same mass and size with three different concentrations of dilute hydrochloricacid in the presence of a catalyst. The three concentrations of dilute hydrochloricacid are: ● 1.0 mol / dm3 ● 1.5 mol / dm3 ● 2.0 mol / dm3. All other conditions stay the same. Table6.1 shows the time taken for each reaction to finish. Table 6.1 concentration of hydrochloric acid in mol / dm3 time taken for the reaction to finish in s Complete Table6.1 by writing the concentrations of hydrochloricacid in the first column.  Describe the effect on the time taken for the zinc to finish reacting with 2.0 mol / dm3 hydrochloricacid with no catalyst present. All other conditions stay the same. Describe the effect on the time taken for the zinc to finish reacting with 2.0 mol / dm3 hydrochloricacid when the surface area of the zinc is increased. All other conditions stay the same. Crystals of zincchloride can be prepared by reacting excess zinc with dilute hydrochloricacid. Choose from the list, the method used to separate the unreacted zinc from the reaction mixture. Draw a circle around your chosen answer. chromatography crystallisation evaporation filtration Zincchloride is soluble in water. Choose one other compound that is soluble in water. Tick (✓) one box. calcium carbonate lead(chloride silver chloride sodium nitrate  
6. Chemical reactions  →  6.2. Rate of reaction
9. Metals  →  9.4. Reactivity series
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Fig.7.1 shows the displayed formula of mesaconicacid. C C C H O H C O H C O H H H O On Fig.7.1 draw a circle around one carboxylic acid functional group. Deduce the molecular formula of mesaconicacid. Mesaconicacid is a colourless compound. Describe the colour change when excess mesaconicacid is added to aqueous bromine. from to ������������������������������������������������������������� Ethanoicacid belongs to the homologous series of carboxylic acids. Define the term homologous series. Complete the word equation for the reaction of ethanoicacid with magnesium. ethanoic acid + magnesium +  Ethanoicacid reacts with ethanol. The organic product has the molecular formula C4H8O2. Complete Table7.1 to calculate the relative molecular mass of C4H8O2. Table 7.1 atom number of atoms relative atomic mass carbon 4 × 12 = 48 hydrogen oxygen  relative molecular mass = Ethanol can be manufactured by fermentation. Complete the word equation for one other method of manufacturing ethanol. + → ethanol 
11. Organic chemistry  →  11.7. Carboxylic acids
11. Organic chemistry  →  11.2. Naming organic compounds
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This question is about nitrogen and compounds of nitrogen. Nitrogen is a non-metal. Nitrogen is a poor electrical conductor. Describe two other physical properties which are typical of non-metals.  Oxides of nitrogen are air pollutants which contribute to acid rain. State one source of oxides of nitrogen in the air. State one other adverse effect of oxides of nitrogen. Ammonia is a simple molecule with covalent bonds. Describe a covalent bond. Complete Fig.8.1 to show the dot-and-cross diagram for a molecule of ammonia. Show outer shell electrons only. N H H H  Aqueous ammonia is alkaline. Choose from the list, the pH value that is alkaline. Draw a circle around your chosen answer. pH 1 pH 5 pH 7 pH 10 Aqueous ammonia releases ammonia gas. Ammonia gas turns damp red litmus paper blue. A long glass tube is set up as shown in Fig.8.2. long glass tube cotton wool soaked in aqueous ammonia damp red litmus paper At first, the litmus paper does not turn blue. After a short time, the litmus paper turns blue. Explain these results in terms of the kinetic particle theory. 
12. Experimental techniques and chemical analysis  →  12.5. Identification of ions and gases
10. Chemistry of the environment  →  10.3. Air quality and climate
1. States of matter  →  1.1. Solids, liquids and gases
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