IGCSE Chemistry 0620 Paper 33, Oct/Nov 2024

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: is in brass

produces an orange-red colour in a flame test

is a reactant in a fuel cell

has an atom with only three occupied electron shells

forms an ion that gives a red-brown precipitate on addition of aqueous ammonia

forms an ion with a charge of 1–.

Explain why Li, K and Rb have similar chemical properties.

State the percentage of oxygen in clean, dry air.

Complete Fig. 2.1 to show the dot-and-cross diagram for a molecule of water. Show outer shell electrons only. Fig. 2.1

Ethene is a small molecule used to make polymers. State the name of the polymer formed from ethene.

Complete this sentence about polymers. Polymers are large molecules built up from many smaller molecules called ........................................ .

Potassium chloride is an ionic compound. State two physical properties of ionic compounds. 1 .......................................................................................................................................... 2 ..........................................................................................................................................

Choose the correct statement that describes ionic bonding. Tick (✓) one box. It is a weak electrostatic attraction between anions and cations. It is a weak electrostatic attraction between cations. It is a strong electrostatic attraction between anions. It is a strong electrostatic attraction between cations and anions.

The list shows some gases in a sample of water. 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 contains harmful substances. Link each harmful substance on the left to the correct effect on the right. One has been done for you.

Table 3.1 shows the masses of ions, in mg, present in a 1000 cm${}^3$ sample of polluted water. Table 3.1 Answer these questions using the information from Table 3.1. Name the positive ion that has the lowest concentration.

State the name of the $\mathrm{S}{\mathrm{O}}_4^{2-}$ ion.

Calculate the mass of potassium ions in 125 cm${}^3$ of polluted water.

Name two substances used in the treatment of the domestic water supply. For each substance give a reason for its use. substance 1 ............................................................................................................................... reason ........................................................................................................................................ substance 2 ............................................................................................................................... reason ........................................................................................................................................

Complete the symbol equation for the reaction of silicon(IV) chloride, $\mathrm{S}\mathrm{i}\mathrm{C}{\mathrm{l}}_4$, with water. $$\mathrm{S}\mathrm{i}\mathrm{C}{\mathrm{l}}_4+\mathrm{.}\mathrm{.}\mathrm{.}\mathrm{.}\mathrm{.}{\mathrm{H}}_2\mathrm{O}\to \mathrm{S}\mathrm{i}{\mathrm{O}}_2+\mathrm{.}\mathrm{.}\mathrm{.}\mathrm{.}\mathrm{.}\mathrm{H}\mathrm{C}\mathrm{l}$$

Fig. 4.1 shows the displayed formula of compound A. Fig. 4.1 On Fig 4.1 draw a circle around the carboxylic acid functional group.

Deduce the molecular formula of compound A.

Compound A reacts with ethanol to produce a compound with the molecular formula ${\mathrm{C}}_5{\mathrm{H}}_{11}\mathrm{N}{\mathrm{O}}_3$. Complete Table 4.1 to calculate the relative molecular mass of ${\mathrm{C}}_5{\mathrm{H}}_{11}\mathrm{N}{\mathrm{O}}_3$. Table 4.1

Table 4.2 shows the names, formulae and boiling points of methanol, ethanol, propanol and butanol. Table 4.2 Use the information in Table 4.2 to answer these questions. Name the homologous series that includes methanol, ethanol, propanol and butanol.

Deduce the general formula of this homologous series.

State the trend in the boiling point of this homologous series as the number of carbon atoms increases.

Ethanol can be manufactured by an addition reaction. Name two substances and state two conditions required. substance 1 ........................................................................................................................ substance 2 ........................................................................................................................ condition 1 .......................................................................................................................... condition 2 ..........................................................................................................................

Draw the displayed formula of ethanol.

Name the toxic gas produced when ethanol undergoes incomplete combustion.

Table 5.1 shows some properties of five halogens. Table 5.1 Use the information in Table 5.1 to predict: the melting point of astatine

the atomic volume of fluorine

the physical state of fluorine at –240 °C. Give a reason for your answer. physical state ...................................................................................................................... reason ................................................................................................................................. .............................................................................................................................................

Aqueous chlorine reacts with aqueous sodium iodide. Complete the word equation for this reaction. chlorine + sodium iodide → [ ] + [ ]

Explain why aqueous bromine does not react with aqueous sodium chloride.

Fluorine reacts with water to produce hydrogen fluoride and oxygen. Complete the symbol equation for this reaction. $$2{\mathrm{F}}_2+\mathrm{.}\mathrm{.}\mathrm{.}\mathrm{.}\mathrm{.}{\mathrm{H}}_2\mathrm{O}\to 4\mathrm{H}\mathrm{F}+\mathrm{.}\mathrm{.}\mathrm{.}\mathrm{.}\mathrm{.}\mathrm{.}$$

Name an anhydrous compound used to test for water. State the colour of the compound after water is added. name of compound .................................................................................................................... colour after water is added ........................................................................................................

Metals are malleable and ductile. State three other typical physical properties of metals. 1 ................................................................................................................................................. 2 ................................................................................................................................................. 3 .................................................................................................................................................

Complete Table 6.1 to show the number of electrons, neutrons and protons in the calcium atom and copper ion shown. Table 6.1

Write the electronic configuration of the calcium atom.

Copper is a transition element. Choose the correct statement about transition elements. Tick (✓) one box. They have low densities. They often act as catalysts. They have low melting points. All their compounds are white.

Table 6.2 shows the observations when four different metals react with concentrated nitric acid. Table 6.2 Put the four metals in order of their reactivity. Put the least reactive metal first.

Manganese(IV) oxide is reduced by aluminium. $$3\mathrm{M}\mathrm{n}{\mathrm{O}}_2+4\mathrm{A}\mathrm{l}\to 3\mathrm{M}\mathrm{n}+2\mathrm{A}{\mathrm{l}}_2{\mathrm{O}}_3$$ Explain how this equation shows that manganese(IV) oxide is reduced.

Crystals of zinc chloride can be made by warming excess solid zinc oxide with dilute hydrochloric acid. $$\mathrm{Z}\mathrm{n}\mathrm{O}(\mathrm{s})+2\mathrm{H}\mathrm{C}\mathrm{l}(\mathrm{a}\mathrm{q})\to \mathrm{Z}\mathrm{n}\mathrm{C}{\mathrm{l}}_2(\mathrm{a}\mathrm{q})+{\mathrm{H}}_2\mathrm{O}(\mathrm{.}\mathrm{.}\mathrm{.}\mathrm{.}\mathrm{.}\mathrm{.}\mathrm{.})$$ Complete the symbol equation by adding the state symbol for water at room temperature.

State the method used to separate the excess solid zinc oxide from the reaction mixture.

Describe how to make dry crystals of zinc chloride from an aqueous solution of zinc chloride.

Choose from the list the ion that is present in all acids. Draw a circle around your chosen answer. $$\mathrm{C}{\mathrm{l}}^{-}{\mathrm{H}}^{+}{\mathrm{O}}^{2-}\mathrm{O}{\mathrm{H}}^{-}$$

The reaction of zinc oxide with hydrochloric acid is exothermic. Define the term exothermic.

Fig. 7.1 shows the incomplete reaction pathway diagram for the reaction of zinc oxide with hydrochloric acid. Fig. 7.1 Complete Fig. 7.1 by writing these formulae on the diagram: ● $\mathrm{Z}\mathrm{n}\mathrm{O}+2\mathrm{H}\mathrm{C}\mathrm{l}$ ● $\mathrm{Z}\mathrm{n}\mathrm{C}{\mathrm{l}}_2+{\mathrm{H}}_2\mathrm{O}$.

Explain how Fig. 7.1 shows that the reaction is exothermic.

Litmus is an acid–base indicator. State the colour of litmus at pH 2 and at pH 12. colour at pH 2 ............................................................................................................................. colour at pH 12 ...........................................................................................................................

A student investigates the reaction of small pieces of magnesium oxide with excess dilute hydrochloric acid of three different concentrations. The time taken for each reaction to finish is recorded. The three concentrations of the acid are: ● 0.4 mol/dm${}^3$ ● 0.8 mol/dm${}^3$ ● 1.6 mol/dm${}^3$. All other conditions stay the same. Table 8.1 shows the time taken for each reaction to finish. Table 8.1 Complete Table 8.1 by writing the concentrations in the first column.

Describe the effect on the time taken for the reaction to finish when the reaction is carried out at a lower temperature. All other conditions stay the same.

Describe the effect on the time taken for the reaction to finish when large pieces of magnesium oxide are used instead of small pieces of magnesium oxide. All other conditions stay the same.

Molten magnesium chloride is electrolysed using inert electrodes. Name the products at the positive and negative electrodes. product at the positive electrode ......................................................................................... product at the negative electrode .......................................................................................

Describe the arrangement, motion and separation of the particles in liquid magnesium chloride. arrangement ....................................................................................................................... ............................................................................................................................................. motion ................................................................................................................................. ............................................................................................................................................. separation ........................................................................................................................... .............................................................................................................................................