AQA GCSE Chemistry Paper 1 Higher June 2022 question paper 8462/1H

This question is about metals and non-metals. Figure 1 shows an outline of part of the periodic table.

Element Q is a dull solid with a melting point of 44 °C. Element Q does not conduct electricity. Which section of the periodic table in Figure 1 is most likely to contain element Q ?

Tick (✓) one box.

Element R forms ions of formula R²⁺ and R³⁺ Which section of the periodic table in Figure 1 is most likely to contain element R ?

Tick (✓) one box.

Give two differences between the physical properties of the elements in Group 1 and those of the transition elements.

Complete Figure 2 to show the electronic structure of an aluminium atom. Use the periodic table.

Aluminium is a metal. Describe how metals conduct electricity. Answer in terms of electrons.

Name the type of bonding in compounds formed between metals and non-metals.

Magnesium oxide is a compound formed from the metal magnesium and the non-metal oxygen. Describe what happens when a magnesium atom reacts with an oxygen atom. You should refer to electrons in your answer.

Sodium carbonate reacts with hydrochloric acid in an exothermic reaction. The equation for the reaction is:

A student investigated the effect of changing the mass of sodium carbonate powder on the highest temperature reached by the reaction mixture.

Plan a method to investigate the effect of changing the mass of sodium carbonate powder on the highest temperature reached.

Figure 3 shows a line of best fit drawn through the student’s results.

Determine the gradient of the line of best fit in Figure 3. Use the equation:

Give the unit.

The initial temperature of the reaction mixture is where the line of best fit would meet the y-axis. Determine the initial temperature of the reaction mixture. Show your working on Figure 3.

Another student repeated the investigation but added sodium carbonate until the sodium carbonate was in excess. Which sketch graph shows the results obtained when sodium carbonate was added until in excess? Tick (✓) one box.

Figure 4 shows a reaction profile for the reaction of sodium carbonate with hydrochloric acid.

What do labels X and Y represent on Figure 4 ?

How does the reaction profile show that the reaction is exothermic? Use Figure 4.

This question is about different forms of carbon. Figure 5 represents the structure of diamond.

Describe the structure and bonding of diamond.

Explain why diamond has a very high melting point.

Figure 6 represents the molecule C₇₀

What is the name of this type of molecule? Tick (✓) one box.

Molecules such as C₇₀ can be used in medicine to move drugs around the body. Suggest one reason why the C₇₀ molecule is suitable for this use.

Calculate the number of C₇₀ molecules that can be made from one mole of carbon atoms. The Avogadro constant = 6.02 × 10²³ per mole

Number of molecules =

This question is about zinc and compounds of zinc. A student produces pure crystals of zinc chloride by reacting zinc oxide with hydrochloric acid. The equation for the reaction is:

The student adds zinc oxide to hydrochloric acid until the zinc oxide is in excess. Give one observation that the student could make to show that the zinc oxide is in excess.

Why is excess zinc oxide used rather than excess hydrochloric acid?

Name one other compound that the student could add to hydrochloric acid to produce zinc chloride.

Describe how the student should obtain crystals of zinc chloride from a solution of zinc chloride.

Zinc chloride is also produced in a displacement reaction between zinc and copper chloride solution. The equation for the reaction is:

Complete the ionic equation for this reaction.

Why is zinc described as being oxidised in this reaction?

Zinc and copper can be used with another substance to produce electricity. Complete Figure 7 to show how zinc, copper and another substance can be used to light a lamp. Label:

• zinc

• copper

• the other substance used.

The symbol represents the lamp.

This question is about groups in the periodic table.

The elements in Group 1 become more reactive going down the group. Rubidium is below potassium in Group 1.

Rubidium and potassium are added to water. Predict one observation you would see that shows that rubidium is more reactive than potassium.

Explain why rubidium is more reactive than potassium.

Complete the equation for the reaction of rubidium with water. You should balance the equation.

The noble gases are in Group 0.

Which is a correct statement about the noble gases? Tick (✓) one box.

Table 1 shows information about the three isotopes of neon.

Calculate the relative atomic mass (A_r) of neon. Give your answer to 3 significant figures.

This question is about electrolysis. Molten sodium chloride is electrolysed in an industrial process to produce sodium. Figure 8 shows a simplified version of the electrolysis cell used.

Which is the correct half equation for the production of sodium? Tick (✓) one box.

A mesh is used to keep the products of the electrolysis apart.

Suggest one reason why the products of the electrolysis must be kept apart.

Which type of particle passes through the mesh in the electrolysis of molten sodium chloride? Tick (✓) one box.

Aqueous sodium chloride solution is electrolysed in a different industrial process. Two gases and an alkaline solution are produced.

Which two ions are present in aqueous sodium chloride solution in addition to sodium ions and chloride ions?

Name the alkaline solution produced.

Explain how the alkaline solution is produced. You should refer to the processes at the electrodes.

This question is about silicon and compounds of silicon.

The reactivity series sometimes includes non-metals such as carbon, hydrogen and silicon. Silicon can be extracted by reducing silicon dioxide with different substances. The equation for one possible reaction is:

Explain what this reaction shows about the position of silicon in the reactivity series.

Aluminium also reduces silicon dioxide. Carbon is used rather than aluminium to reduce silicon dioxide because carbon is cheaper than aluminium. Carbon can be obtained by heating coal. Aluminium is obtained from aluminium oxide. Explain why aluminium is more expensive than carbon.

Magnesium also reduces silicon dioxide. The equation for the reaction is:

Give one reason why the products are difficult to separate if magnesium is used to reduce silicon dioxide.

Calculate the minimum mass in grams of magnesium needed to completely reduce 1.2 kg of silicon dioxide. Relative atomic masses (A_r): O = 16 Mg = 24 Si = 28

Si₂H₆ is a covalent compound of silicon and hydrogen.

Complete Figure 9 to show the outer shell electrons in a molecule of Si₂H₆

Si₂H₆ reacts with oxygen. The equation for the reaction is:

30 cm³ of Si₂H₆ is reacted with 150 cm³ (an excess) of oxygen.

Calculate the total volume of gases present after the reaction. All volumes of gases are measured at the same temperature and pressure.

This question is about acids and alkalis.

Explain why the pH of an acid depends on:

• the strength of the acid

• the concentration of the acid.

A student titrated 25.00 cm³ of hydrochloric acid with 0.100 mol/dm³ barium hydroxide solution. Table 2 shows the results.

The student calculated the volume of barium hydroxide solution to be used in the

Explain why the student used a volume of 23.50 cm³ of barium hydroxide solution in the titration calculation.

25.00 cm³ of the hydrochloric acid reacted with 23.50 cm³ of the 0.100 mol/dm³ barium hydroxide solution. The equation for the reaction is:

Calculate the concentration of the hydrochloric acid in mol/dm³.

Another student titrated sulfuric acid with barium hydroxide solution. The equation for the reaction is:

The student measured the electrical conductivity of the mixture during the titration. The better a conductor, the higher the electrical conductivity value. Figure 10 shows the results.

Explain why the electrical conductivity of the mixture was zero when the sulfuric acid had just been neutralised. Use the equation for the reaction. Refer to ions in your answer.

The student then added a further 10 cm³ of barium hydroxide solution. The electrical conductivity of the mixture increased. Give one reason why.