0620/32 · May/June 2026
Download PDFSix substances, A to F, are shown in Figure 1.1. Figure 1.1 Answer the following questions about these substances. Each substance may be used once, more than once or not at all.
State which substance is: an alcohol
State which substance is: a gas that is approximately 78% of clean, dry air
State which substance is: a compound in the same homologous series as ethanoic acid
State which substance is: a hydrocarbon
State which substance is: a compound that is a product of the complete combustion of an alkane
State which substance is: a gas that turns limewater milky
State which substance is: a pale yellow-green gas at room temperature and pressure.
State which two substances are elements.
Table 2.1 shows some properties of the Group I elements. Table 2.1
Use the information in Table 2.1 to answer the following questions. Predict the melting point of sodium.
Predict the atomic radius of potassium.
Deduce the physical state of lithium at 95 °C. Give a reason for your answer. physical state .................................................................................................................... reason
State how the density of the Group I elements changes down the group.
Potassium hydroxide, KOH, is made by adding potassium to water. Complete the symbol equation for this reaction. .....K + .....H2O → 2KOH + H2
Bubbles of hydrogen gas are observed. State the test for hydrogen gas. test positive result
Complete Figure 2.1 to show the dot-and-cross diagram for a molecule of ammonia. Show outer shell electrons only. Figure 2.1
The equation for the reaction of magnesium carbonate with dilute sulfuric acid is shown.
State the meaning of the symbol (s) in this equation.
Name the salt formed when magnesium carbonate reacts with dilute sulfuric acid.
Name the piece of apparatus used to collect and measure the volume of carbon dioxide produced in this reaction.
A student investigates the reaction of large pieces of magnesium carbonate with dilute sulfuric acid. The magnesium carbonate is in excess. Figure 3.1 shows the total volume of carbon dioxide gas released as the reaction proceeds. Use the graph in Figure 3.1 to determine the total volume of carbon dioxide gas released in 20 s.
Use the graph in Figure 3.1 to deduce the time taken for the reaction to finish.
The student repeats the experiment using the same volume of dilute sulfuric acid but with smaller pieces of magnesium carbonate. Draw a line on the grid in Figure 3.1 to show how the total volume of carbon dioxide gas released changes over time in this second experiment.
State how the rate of reaction differs, if at all, when a higher temperature is used.
State how the rate of reaction differs, if at all, when a lower concentration of dilute sulfuric acid is used.
Write the formula of the ion that is in all acids.
Choose the pH value for an acidic solution. Draw a circle around your chosen answer. pH 2 pH 7 pH 9 pH 12
This question is about organic compounds and their reactions.
Compound P is saturated. Figure 4.1 shows the displayed formula of compound P. Figure 4.1 On Figure 4.1, draw a circle around the alcohol functional group.
Deduce the molecular formula of compound P.
State why compound P is saturated.
Outline how ethanol is manufactured using aqueous glucose. In your answer, include: • the name of this process • two conditions that are needed. name of process ................................................................................................................ condition 1 ......................................................................................................................... condition 2 .........................................................................................................................
State one use of ethanol.
Ethanol is oxidised to ethanoic acid. Complete the word equation for the reaction of ethanoic acid with magnesium. ethanoic acid + magnesium → .......................... + ..........................
Three states of matter are solid, liquid and gas.
State two general properties of a liquid. 1 ................................................................................................................................................ ................................................................................................................................................... 2 ................................................................................................................................................ ...................................................................................................................................................
Complete Table 5.1 to show the motion and separation of particles in a solid and a liquid. Table 5.1
Draw a line from each statement to the correct change of state. statement change of state liquid nitrogen turns into solid nitrogen -> evaporating / freezing / condensing liquid cobalt changes into cobalt gas -> evaporating / freezing / condensing steam changes into liquid water -> evaporating / freezing / condensing
Name the process in which gas particles spread out from an area of high concentration to an area of low concentration.
Nickel is a metal.
State the period number of nickel in the Periodic Table.
Deduce the number of electrons, neutrons and protons in the nickel ion shown. number of electrons .......................................................................................................... number of neutrons ........................................................................................................... number of protons .............................................................................................................
Nickel(II) chloride is a compound with ionic bonding. State the meaning of the term ionic bond.
State two physical properties of an ionic compound. 1 ........................................................................................................................................ 2 ........................................................................................................................................
Nickel reacts with oxygen to form nickel(II) oxide. Complete the symbol equation for this reaction. .....Ni + .......... → 2NiO
State if nickel(II) oxide is an acidic oxide or a basic oxide. Give a reason for your answer.
Nickel(II) bromide is another compound of nickel. Molten nickel(II) bromide is electrolysed using platinum electrodes. Name a non-metal that is used as an inert electrode.
Name the products formed at each electrode during the electrolysis of molten nickel(II) bromide, and give the observations at the positive electrode. product at the negative electrode ...................................................................................... product at the positive electrode ....................................................................................... observations at the positive electrode ............................................................................... ...........................................................................................................................................
Nickel(II) hydroxide has the formula . Complete Table 6.1 to calculate the relative formula mass of . Table 6.1 relative formula mass = .........................................................
Stainless steel is an alloy that contains nickel. State the meaning of the term alloy.
Name two elements in stainless steel, other than nickel.
Natural water sources can be polluted by nitrates and some metal compounds. State one source of nitrates that pollute natural water sources.
State one reason why nitrates in river water are harmful.
State one reason why some metal compounds in river water are harmful.
Sea water contains potassium ions. Name the test to identify potassium ions. Give the observations for a positive test. test ............................................................................................................................................ observations .............................................................................................................................
Potassium reacts with iodine to produce potassium iodide. 13.2 g of potassium reacts with excess iodine to produce 56.2 g of potassium iodide. Calculate the mass of potassium iodide produced when 6.6 g of potassium reacts with excess iodine.
Figure 7.1 shows three stages in the treatment of the domestic water supply. Figure 7.1 State what happens at each stage in the treatment of the domestic water supply. sedimentation and filtration ....................................................................................................... ................................................................................................................................................... addition of carbon ..................................................................................................................... ................................................................................................................................................... chlorination ............................................................................................................................... ...................................................................................................................................................
Explain why distilled water rather than tap water is used in practical chemistry.
State the colour change when water is added to anhydrous cobalt(II) chloride. from ............................................................... to ...............................................................