AQA GCSE Trilogy Chemistry Paper 1 Foundation June 2018 question paper 8464/C/1F

This question is about structure and bonding.

Figure 1 shows part of the structure of calcium oxide (CaO).

What type of bonding is present in calcium oxide?

Tick one box.

02

Figure 2 shows a particle of methane (CH₄).

What type of particle is present in Figure 2 ?

Tick one box.

Figure 3 shows the structure of C₆₀

Complete the sentence. Choose the answer from the box.

Figure 4 shows the structure of graphite.

What type of bond is labelled A in Figure 4 ? Tick one box.

In graphite, each carbon atom forms bonds with other carbon atoms as shown in

Figure 4

How many electrons does one carbon atom use to form one bond? Tick one box.

An electric current is passed through copper. Figure 5 shows the apparatus used.

Complete the sentence. Choose the answer from the box.

Complete the sentence. Choose the answer from the box.

Figure 6 shows the apparatus used to investigate the effect of electricity on sodium chloride solution.

Complete the sentence. Choose the answer from the box.

Sodium chloride is made up of ions. Figure 7 shows the apparatus used to investigate the effect of electricity on solid sodium chloride and molten sodium chloride.

Table 1 shows the results.

Draw one line from each statement to the correct reason.

This question is about the halogens.

Which group in the periodic table is known as the halogens? Tick one box.

A fluorine atom has 7 electrons in the outer shell. Figure 8 shows part of a dot and cross diagram to represent a molecule of

Complete the dot and cross diagram. You should show only the electrons in the outer shells.

Chlorine reacts with potassium bromide solution. Complete the word equation.

What type of reaction happens when chlorine reacts with potassium bromide solution? Tick one box.

Complete the sentence. Choose the answer from the box.

Chlorine is more reactive than bromine.

How does the size of a chlorine atom compare with the size of a bromine atom? Complete the sentence. Choose the answer from the box.

Give a reason for your answer to question 02.6

Fluorine reacts with chlorine to produce ClF₃ Balance the chemical equation for the reaction.

Explain why fluorine is a gas at room temperature. Use the following words in your answer: energy forces molecules weak

This question is about acids and bases.

Which ion is found in all acids? Tick one box.

Zinc nitrate can be produced by reacting an acid and a metal oxide. Name the acid and the metal oxide used to produce zinc nitrate.

In an equation, zinc nitrate is written as Zn(NO₃)₂(aq). What does (aq) mean? Tick one box.

The pH of a solution is 8 Some hydrochloric acid is added to the solution. Suggest the pH of the solution after mixing.

Table 2 shows the solubility of three solids in water at room temperature.

A teacher labelled these three solids A, B and C. She gave a student the information shown in Table 3

Describe a method that could be used to identify each of the three solids A, B and C. You must use an indicator in the method. Use information in Table 2 and Table 3

This question is about the elements in Group 2 of the periodic table.

Figure 9 shows the positions of four elements, A, B, C, and D, in the periodic table.

Which element is in Group 2? Tick one box.

Group 2 metal carbonates break down when heated to produce a metal oxide and a gas. metal carbonate metal oxide + gas

Name the two products when calcium carbonate (CaCO₃) is heated.

What type of reaction happens when a compound breaks down? Tick one box.

The metal carbonate takes in energy from the surroundings to break down. What type of reaction takes in energy from the surroundings? Tick one box.

Figure 10 shows the volume of gas produced when a Group 2 metal carbonate is heated.

The student collected 5.2 dm³ of gas. What mass of the Group 2 metal carbonate is heated?

Calculate the mass of the Group 2 carbonate needed to produce 24 dm³ of gas. Use your answer from question 04.5 to help you.

A student heated different masses of a Group 2 carbonate. The student measured the volume of gas produced. Figure 11 shows a graph of the student’s results. The student calculates the gradient of the line in Figure 11 The student makes two mistakes.

Identify the two mistakes the student makes. Calculate the correct gradient of the line.

A student repeated the experiment with a different Group 2 metal carbonate (XCO₃). The relative formula mass (M_r) of XCO₃ is 84 Relative atomic masses (A_r): C = 12 O = 16 Calculate the relative atomic mass (A_r) of X. Name metal X. Use the periodic table.

This question is about electrolysis. A student investigates the mass of copper produced during electrolysis of copper chloride solution. Figure 12 shows the apparatus.

Which gas is produced at the positive electrode (anode)? Tick one box.

Copper is produced at the negative electrode (cathode). What does this tell you about the reactivity of copper? Tick one box.

Table 4 shows the student’s results.

Determine the mean mass of copper produced after 3 minutes.

Calculate the mass X of copper produced in Experiment 2 after 5 minutes. Use Table 4 on page 19

The copper chloride solution used in the investigation contained 300 grams per dm³ of solid CuCl₂ dissolved in 1 dm³ of water. The students used 50 cm³ of copper chloride solution in each experiment. Calculate the mass of solid copper chloride used in each experiment.

This question is about sodium and chlorine. Figure 13 shows the positions of sodium and chlorine in the periodic table.

State one difference and one similarity in the electronic structure of sodium and of chlorine.

Sodium atoms react with chlorine atoms to produce sodium chloride (NaCl). Describe what happens when a sodium atom reacts with a chlorine atom. Write about electron transfer in your answer.

The reaction between sodium and chlorine is an exothermic reaction. Complete the reaction profile for the reaction between sodium and chlorine.

A student plans a method to prepare pure crystals of copper sulfate. The student’s method is:

1. Add one spatula of calcium carbonate to dilute hydrochloric acid in a beaker.

2. When the fizzing stops, heat the solution with a Bunsen burner until all the liquid is gone.

The method contains several errors and does not produce copper sulfate crystals. Explain the improvements the student should make to the method so that pure crystals of copper sulfate are produced.