0620_s23_qp_32
A paper of Chemistry, 0620
Questions:
8
Year:
2023
Paper:
3
Variant:
2
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1
Fig.1.1 shows part of the Periodic Table. I II III IV V VI VII VIII Cl C N O Sr He Ne K Ca Cr Cu Zn 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 21% by volume of clean, dry air has an atom with only three occupied electron shells has an atom with only one electron in its outer shell is a grey-black solid at room temperature forms an ion that gives a green precipitate on addition of aqueous ammonia is used in electrical wiring because of its good ductility. 
2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table
9. Metals  →  9.2. Uses of metals
8. The Periodic Table  →  8.1. Arrangement of elements
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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 chlorine –101 –35 0.003 bromine –7 +59 3.12 iodine +114 4.93 astatine +302 +337 Use the information in Table 2.1 to predict: the boiling point of iodine ���������������������������������������������������������������������������������������������� the density of astatine at room temperature and pressure ������������������������������������������� the physical state of bromine at +50 °C. Give a reason for your answer. physical state reason  Aqueous bromine reacts with aqueous potassium iodide. Complete the word equation for this reaction. bromine + potassium iodide → +  Explain why aqueous iodine does not react with aqueous potassiumbromide. Describe a test for iodide ions. test observations  
11. Organic chemistry  →  11.5. Alkenes
8. The Periodic Table  →  8.3. Group VII properties
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Water from natural sources can contain metal compounds and phosphates. Name two other substances found in water which are harmful to aquatic life.  State why phosphates 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 ammonium NH4 + 0.5 calcium Ca2+ 1.8 chloride Cl – 2.0 copper(Cu2+ 0.3 hydrogencarbonate HCO3 – 8.0 magnesium Mg2+ 1.6 NO3 – 0.6 potassium K+ 8.3 silicate SiO3 2– 5.0 sodium Na+ 5.2 sulfate SO4 2– 0.2 Answer these questions using information from Table3.1. Name the positive ion present in the highest concentration. State the name of the NO3 – ion. Calculate the mass of magnesium ions present in 250 cm3 of polluted water.  mass = mg Water is produced when blue copper(sulfate is heated. CuSO4•5H2OCuSO4+ 5H2Oblue copper(white copper(sulfate sulfate Describe how white copper(sulfate can be changed to blue copper(sulfate. Choose a word from the list which best describes white copper(sulfate. Draw a circle around your chosen answer. anhydrous aqueous hydrated oxidised Complete the symbol equation for the reaction of calcium with water. Ca + H2O → Ca(OH)2 +  
10. Chemistry of the environment  →  10.1. Water
9. Metals  →  9.4. Reactivity series
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This question is about chlorine and compounds of chlorine. Chlorine has diatomic molecules. Define the term diatomic. Deduce the number of protons, neutrons and electrons in the chloride ion shown. 37Cl – number of protons number of neutrons number of electrons  Chlorine reacts with hydrogen to produce hydrogen chloride. The reaction is exothermic. State the meaning of the term exothermic. Fig.4.1 shows an incomplete reaction pathway diagram for the reaction of chlorine with hydrogen. energy progress of reaction Complete Fig.4.1 by writing these formulae on the diagram: ● Cl 2 + H2 ● 2HCl. Explain how Fig.4.1 shows that the reaction is exothermic. A few drops of methyl orange indicator are added to dilute hydrochloricacid. State the colour of the solution. Dilute hydrochloricacid reacts with sodium hydroxide. Complete the word equation for this reaction. hydrochloric acid + sodium hydroxide → +  Sodiumhydroxide is an alkali. Write the formula of the ion present in all alkalis. shows the apparatus used for the electrolysis of concentrated aqueous sodiumchloride using graphite electrodes. power supply + – Label Fig.4.2 to show: ● the anode ● 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  
4. Electrochemistry  →  4.1. Electrolysis
11. Organic chemistry  →  11.4. Alkanes
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This question is about metals. Carbon is used to extract iron from iron ore in a blast furnace. Name the main ore of iron. Iron(oxide in the iron ore is reduced by carbonmonoxide. Name the two substances which react in the blast furnace to produce carbon monoxide. and ��������������������������������������������������������������� Iron rusts in the presence of oxygen and water. State one method of preventing rusting. Table5.1 shows some information about the reaction of four metals with steam. Table 5.1 metal reaction with steam when metal is cold beryllium reacts slowly chromium reacts slowly only when the metal is very hot magnesium reacts rapidly silver no reaction Put the four metals in order of their reactivity. Put the least reactive metal first. least reactive most reactive  
9. Metals  →  9.4. Reactivity series
9. Metals  →  9.6. Extraction of metals
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A student investigates the reaction of different-sized pieces of calciumcarbonate with dilute hydrochloricacid. The sizes of the pieces of calcium carbonate are: ● large ● medium ● small. All other conditions stay the same. Table6.1 shows the time taken for each reaction to finish. Table 6.1 size of pieces of calcium carbonate time taken for the reaction to finish / s Complete Table6.1 by writing the sizes of the pieces of calciumcarbonate in the first column. Describe the effect on the time taken for small pieces of calciumcarbonate to finish reacting with dilute hydrochloricacid when the temperature is increased. All other conditions stay the same. Describe the effect on the time taken for small pieces of calcium carbonate to finish reacting with dilute hydrochloric acid when the concentration of hydrochloric acid is decreased. All other conditions stay the same. Crystals of calcium chloride can be prepared by reacting excess calcium carbonate with dilute hydrochloric acid. Name the process used to separate the unreacted calciumcarbonate from the rest of the reaction mixture. Calciumcarbonate is insoluble in water. Choose one other compound that is insoluble in water. Tick (✓) one box. ammonium sulfate potassium nitrate silver chloride sodium hydroxide  
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 compoundD. C C H O H C H O H C C H O O H O On Fig.7.1 draw a circle around the alcohol functional group. Deduce the molecular formula of compoundD. Explain, by referring to the structure in Fig.7.1, why compoundD is unsaturated. Ethene is also an unsaturated compound. Draw the displayed formula of ethene.  Describe a test for unsaturated compounds. test observations  Ethene can be manufactured by cracking larger alkane molecules. State two conditions for cracking.  Complete the symbol equation for the cracking of decane, C10H22, to produce ethene and one other hydrocarbon. C10H22 → C2H4 +  Ethanol can be manufactured by the reaction of ethene with steam. Name one other method of manufacturing ethanol. Ethanol can be oxidised to ethanoicacid. Ethanoicacid reacts with sodium. Name the salt formed when ethanoicacid reacts with sodium. Ethanoicacid reacts with propanol. The organic product has the molecular formula C5H10O2. Complete Table7.1 to calculate the relative molecular mass of C5H10O2. Table 7.1 atom number of atoms relative atomic mass carbon hydrogen oxygen 2 × 16 = 32  relative molecular mass = 
11. Organic chemistry  →  11.2. Naming organic compounds
11. Organic chemistry  →  11.6. Alcohols
11. Organic chemistry  →  11.5. Alkenes
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This question is about non-metals and compounds of non-metals. Describe two physical properties which are typical of non-metals.  Methane is a compound of carbon and hydrogen. Complete Fig.8.1 to show the dot-and-cross diagram for a molecule of methane. Show outer shell electrons only. C H H H H  Methane is an alkane. Write the general formula for alkanes. Methane is an air pollutant. State one source of methane in the air. State one adverse effect of methane in the air. Carbon particulates and water are two of the products of the incomplete combustion of methane. Name one other compound formed during the incomplete combustion of methane. Sulfurdioxide is an air pollutant which contributes to acid rain. Choose from the list the pH value that is acidic. Draw a circle around your chosen answer. pH 4 pH 7 pH 9 pH 13 State two methods of reducing acid rain.  Sulfur dioxide gas turns aqueous acidified potassium manganate(from purple to colourless. Fig.8.2 shows a gas jar of sulfurdioxide separated from a gas jar of air by a glass plate. A piece of filter paper soaked in aqueous acidified potassiummanganate(is glued to the top of the gas jar of air. glass plate present filter paper soaked in aqueous acidified potassium manganate(a short time after the glass plate is removed air sulfur dioxide glass plate The glass plate is removed. At first, the filter paper remains purple. After a short time, the filter paper turns colourless. Explain these results in terms of the kinetic particle theory. 
10. Chemistry of the environment  →  10.3. Air quality and climate
9. Metals  →  9.1. Properties of metals
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