AQA GCSE Chemistry Paper 1 Foundation June 2019 question paper 8462/1F

This question is about atomic structure. Figure 1 represents an atom of element Z.

Name the parts of the atom labelled A and B. Choose answers from the box.

Which particle has the lowest mass? Choose the answer from the box.

Which group of the periodic table contains element Z ? Use Figure 1.

Give the atomic number and the mass number of element Z. Use Figure 1. Choose answers from the box.

Bromine has two different types of atom. The atoms have a different number of neutrons but the same number of protons.

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

The different types of bromine atom can be represented as⁷⁹₃₅Br and⁸¹₃₅Br The relative atomic mass (A_r) of bromine is 80 Which statement is true about the number of each type of atom in bromine?

Tick (✓) one box.

This question is about compounds of oxygen and hydrogen. Figure 2 represents the structure of hydrogen peroxide.

Figure 2

What is the correct formula of hydrogen peroxide? Tick (✓) one box.

Which type of bonding is shown in Figure 2 ? Tick (✓) one box.

Hydrogen peroxide decomposes in the presence of a catalyst. Which elements are often used as catalysts?

Tick (✓) one box.

Figure 3 shows the reaction profile for the decomposition of hydrogen peroxide. The word equation for this reaction is: hydrogen peroxide → water + oxygen

Labels A, B, C and D each represent a different part of the reaction profile. Use Figure 3 to answer Questions 02.4 and 02.5

Which label shows the activation energy? Tick (✓) one box.

Which label shows the energy of hydrogen peroxide? Tick (✓) one box.

The decomposition of hydrogen peroxide gives out energy to the surroundings. What type of reaction is this?

Tick (✓) one box.

Hydrogen and oxygen form water. A hydrogen atom contains one electron. An oxygen atom contains six electrons in the outer shell. Complete Figure 4 to show a dot and cross diagram for a water molecule. Show the outer electrons only.

This question is about elements, compounds and mixtures. Figure 5 shows five different substances, A, B, C, D and E.

Use Figure 5 to answer Questions 03.1 to 03.3

Which substance is only one compound? Tick (✓) one box.

Which substance is a mixture of elements? Tick (✓) one box.

Which substance is a mixture of an element and a compound? Tick (✓) one box.

Substances are separated from a mixture using different methods.

Draw one line from each method of separation to the substance and mixture it would separate.

Method of separation Substance and mixture

Sand does not dissolve in water. A student separates a mixture of sand and water by filtration. Draw a diagram of the apparatus the student could use. You should label:

• where the sand is collected

• where the water is collected.

Diagram

A student distils a sample of salt solution to produce pure water. Figure 6 shows the apparatus.

What temperature would you expect the thermometer to show?

Tick (✓) one box.

Describe how the process of distillation shown in Figure 6 produces pure water from salt solution.

This question is about chemical cells and batteries. A student investigated the voltage produced by different chemical cells. Figure 7 shows the apparatus.

This is the method used.

1. Use cobalt metal as electrode X.

2. Record the cell voltage.

3. Repeat steps 1 and 2 using different metals as electrode X.

Suggest two variables the student should keep the same to make the investigation valid.

Table 1 shows the student’s results.

Write the three metals used for electrode X in order of reactivity. Use Table 1.

Copper is used as electrode X in Figure 7. Predict the voltage of this cell. Give one reason for your answer.

Describe how to make a 12 V battery using 1.5 V cells.

Which is the most suitable use for a non-rechargeable cell? Tick (✓) one box.

Hydrogen fuel cells or rechargeable cells can be used to power electric vehicles. Suggest one advantage and one disadvantage of using a hydrogen fuel cell compared with a rechargeable cell.

Advantage of hydrogen fuel cell

Disadvantage of hydrogen fuel cell

A student investigated the reaction between lumps of calcium carbonate and dilute hydrochloric acid. This is the method used.

1. Pour 100 cm³ of dilute hydrochloric acid into a conical flask.

2. Place the conical flask on a balance.

3. Add 2 g of calcium carbonate lumps to the conical flask.

4. Wait until the calcium carbonate stops reacting.

5. Record the decrease in mass of the conical flask and contents.

6. Repeat steps 1 to 5 three more times.

The equation for the reaction is:

What is the state symbol X in the equation? Tick (✓) one box.

Table 2 shows the student’s results.

Why does the mass of the conical flask and contents decrease during the reaction? Tick (✓) one box.

What is the range of the four results in Table 2 ?

Calculate the mean decrease in mass of the conical flask and contents. Do not include the anomalous result. Use Table 2.

A teacher demonstrated the investigation. The teacher used different masses of calcium carbonate. Figure 8 shows the teacher’s results.

What type of variable is the mass of calcium carbonate? Tick (✓) one box.

Use Figure 8 to answer Questions 05.6 and 05.7

Complete the sentence. As the mass of calcium carbonate used increases, the decrease in mass of

What is the decrease in mass of the conical flask and contents when a 3 g sample of calcium carbonate is used?

This question is about the extraction of metals.

Tungsten is a metal. The symbol of tungsten is W Tungsten is produced from tungsten oxide by reaction with hydrogen. The equation for the reaction is:

Calculate the percentage atom economy when tungsten is produced in this reaction. Use the equation:

Relative formula masses (M_r): WO₃ = 232 H₂ = 2

Aluminium is extracted from aluminium oxide.

38% of a rock sample is aluminium oxide. Calculate the mass of aluminium oxide in 40 kg of the rock sample.

The formula of aluminium oxide is Al₂O₃ Calculate the relative formula mass (M_r) of aluminium oxide. Relative atomic masses (A_r): O = 16 Al = 27

60.0 kg of aluminium oxide produces a maximum of 31.8 kg of aluminium. In an extraction process only 28.4 kg of aluminium is produced from 60.0 kg of aluminium oxide. Calculate the percentage yield. Give your answer to 3 significant figures.

Use the equation:

Extracting metals by electrolysis is a very expensive process. Explain why aluminium is extracted using electrolysis and not by reduction with carbon.

This question is about energy changes in reactions.

Ammonium nitrate dissolves in water. The change is endothermic. Which piece of equipment uses this change?

Tick (✓) one box.

A student investigated the temperature change in the reaction between dilute sulfuric acid and potassium hydroxide solution. This is the method used.

1. Measure 25 cm³ of potassium hydroxide solution into a glass beaker.

2. Add 5 cm³ of dilute sulfuric acid.

3. Stir the solution.

4. Measure the temperature of the solution.

5. Repeat steps 2 to 4 until a total of 30 cm³ of dilute sulfuric acid has been added.

Figure 9 shows part of the scales of four thermometers, A, B, C and D.

The student wanted to measure the temperature to a resolution of 0.1 °C Which thermometer should the student use?

Tick (✓) one box.

Energy is lost to the surroundings during the reaction. What type of error does this cause in the results?

Tick (✓) one box.

The student used a glass beaker for the reaction. Name a container the student could use instead of the glass beaker to improve the accuracy of the results.

Table 3 shows the student’s results.

Plot the data from Table 3 on Figure 10. You should:

• draw a line of best fit

• extend your line of best fit to the y-axis.

The intercept on the y-axis of Figure 10 shows the starting temperature of the potassium hydroxide solution. Give the starting temperature of the potassium hydroxide solution.

Another student repeated the investigation and obtained an anomalous result. This result was lower than expected. What could have caused the anomalous result?

Tick (✓) two boxes.

This question is about the periodic table. In the 19th century, some scientists tried to classify the elements by arranging them in order of their atomic weights. Figure 11 shows the periodic table Mendeleev produced in 1869. His periodic table was more widely accepted than previous versions.

The atomic weight of tellurium (Te) is 128 and that of iodine (I) is 127 Why did Mendeleev reverse the order of these two elements?

Mendeleev left spaces marked with an asterisk * He left these spaces because he thought missing elements belonged there. Why did Mendeleev’s periodic table become more widely accepted than previous versions?

Mendeleev arranged the elements in order of their atomic weight. What is the modern name for atomic weight?

Tick (✓) one box.

Complete the sentence. In the modern periodic table, the elements are arranged in order of

Chlorine, iodine and astatine are in Group 7 of the modern periodic table.

Astatine (At) is below iodine in Group 7. Predict:

• the formula of an astatine molecule

• the state of astatine at room temperature.

Formula of astatine molecule State at room temperature

Sodium is in Group 1 of the modern periodic table. Describe what you would see when sodium reacts with chlorine.

This question is about acids and alkalis.

Which ion do all acids produce in aqueous solution? Tick (✓) one box.

Calcium hydroxide solution reacts with an acid to form calcium chloride. Complete the word equation for the reaction.

A student investigates the volume of sodium hydroxide solution that reacts with 25.0 cm³ of dilute sulfuric acid. Figure 12 shows the apparatus the student uses.

Use Figure 12 to answer Questions 09.3 and 09.4

Name apparatus A.

What is the reading on apparatus A ?

The higher the concentration of a sample of dilute sulfuric acid, the greater the volume of sodium hydroxide needed to neutralise the acid. The student tested two samples of dilute sulfuric acid, P and Q. Describe how the student could use titrations to find which sample, P or Q, is more concentrated.

This question is about materials and their properties.

Figure 13 shows a carbon nanotube.

The structure and bonding in a carbon nanotube are similar to graphene. Carbon nanotubes are used in electronics because they conduct electricity. Explain why carbon nanotubes conduct electricity.

Figure 14 shows a badminton racket.

Table 4 shows some properties of materials. The materials could be used to make badminton racket frames.

Evaluate the use of the materials to make badminton racket frames. Use Table 4.

Zinc oxide can be produced as nanoparticles and as fine particles.

A nanoparticle of zinc oxide is a cube of side 82 nm Figure 15 represents a nanoparticle of zinc oxide.

Calculate the surface area of a nanoparticle of zinc oxide. Give your answer in standard form.

Some suncreams contain zinc oxide as nanoparticles or as fine particles. Suggest one reason why it costs less to use nanoparticles rather than fine particles in suncreams.