AQA GCSE Chemistry Paper 1 Foundation June 2024 question paper 8462/1F

This question is about elements, compounds and mixtures.

Figure 1 shows diagrams which represent the atoms and molecules in different substances.

Which diagram in Figure 1 represents a pure compound?

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Which diagram in Figure 1 represents a mixture of an element and a compound?

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Elements are metals or non-metals.

Figure 2 shows an outline of the periodic table.

The periodic table is divided into sections.

Where are metals found in the periodic table?

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Which two of the following are typical properties of a transition metal?

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Potassium and chlorine react to produce potassium chloride.

An atom of potassium loses an electron to form a potassium ion.

An atom of chlorine gains an electron to form a chloride ion.

Complete the dot and cross diagram.

Mixtures are separated by different methods.

Figure 3 shows the apparatus for separating four different types of mixture.

Figure 3

Which apparatus could be used to collect water from sodium chloride solution?

Use Figure 3.

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Which apparatus shows filtration?

Use Figure 3.

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A titration measures the volumes of an acid and an alkali that neutralise each other.

Figure 4 shows the apparatus used.

Name the pieces of equipment labelled A, B and C in Figure 4.

Choose answers from the box.

In Step 2 in Figure 4 the acid is added to the alkali until the solution is neutralised.

The volume of acid added is then read from equipment C.

Name a suitable indicator for use in Step 2 of the titration.

Give one observation that shows the alkali is neutralised.

Give two ways to make sure that the volume of acid added is accurate.

Figure 5 shows the reading on equipment C at the end of Step 2.

What is the reading on equipment C in Figure 5 ?

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A student did a different titration.

Table 1 shows the results.

Which two results should be used to calculate the mean volume of acid added?

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A salt is produced when an acid neutralises an alkali.

Barium chloride is a salt containing the ions Ba²⁺ and Cl_¯

What is the formula of barium chloride?

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This question is about energy changes of reactions.

Zinc reacts with copper sulfate solution.

The word equation for the reaction is:

zinc + copper sulfate → zinc sulfate + copper

What type of reaction is the reaction between zinc and copper sulfate solution?

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Calculate the percentage (%) by mass of copper in copper sulfate (CuSO₄).

Give your answer to 3 significant figures.

Relative atomic mass (A_r): Cu = 63.5

Relative formula mass (M_r): CuSO₄ = 159.5

A student investigated the energy change in the reaction between zinc and copper sulfate solution.

This is the method used.

1. Measure 25 cm³ of copper sulfate solution into a polystyrene cup.

2. Weigh 0.20 g of zinc powder.

3. Add the zinc powder to the copper sulfate solution.

4. Measure the highest temperature reached by the mixture.

5. Repeat steps 1 to 4 using different masses of zinc powder.

Control variables are used to make an investigation a fair test.

Which is a control variable in the investigation?

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Figure 6 shows the results.

What is the minimum mass of zinc powder needed to react with all the copper sulfate solution?

Use Figure 6.

What is the maximum temperature change in the reaction between zinc powder and 25 cm³ of copper sulfate solution?

Use Figure 6.

25 cm³ of copper sulfate solution contained 6.75 g of copper sulfate.

Calculate the concentration of the solution in g/dm³.

You should:

calculate the volume of the solution in dm³ (1000 cm³ = 1 dm³)

use the equation:

Another student investigated the energy change of the reaction between sodium hydrogencarbonate and hydrochloric acid.

This is the method used.

1. Measure 25 cm³ of hydrochloric acid.

2. Weigh 1.0 g of sodium hydrogencarbonate.

3. Add the sample of sodium hydrogencarbonate to the hydrochloric acid.

4. Measure the lowest temperature reached by the mixture.

5. Repeat steps 1 to 4 using different masses of sodium hydrogencarbonate.

Figure 7 shows the results.

Draw two straight lines of best fit on Figure 7.

The lines should cross.

Which statement describes the energy change in the reaction shown in Figure 7 ?

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This question is about small particles.

What is the approximate number of atoms in a nanoparticle?

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Nanoparticles of some elements can be used as catalysts.

Which element is most likely to be used as a catalyst?

Use the periodic table.

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Nanoparticles are used in sun creams and in wound dressings.

A wound dressing is placed next to the skin to prevent infection.

Figure 8 shows a wound dressing.

Table 2 shows some information about substances used in the form of nanoparticles.

Draw one line from each use to the best substance for that use.

Figure 9 shows a cubic nanoparticle.

Calculate:

• the surface area of the cubic nanoparticle

• the volume of the cubic nanoparticle

• the simplest whole number ratio of surface area: volume for the cubic nanoparticle.

Use the equation:

surface area of cubic nanoparticle = 6 × surface area of one face

Simplest whole number ratio of surface area: volume =

This question is about carbon and carbon compounds.

An atom of carbon is represented as:

What is the number of protons in this atom of carbon?

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What is the number of neutrons in this atom of carbon?

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What is the number of electrons in this atom of carbon?

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Figure 10 shows the structure of a carbon compound.

Complete the formula of the carbon compound.

C__ F__

Methane:

• is a carbon compound

• exists as small molecules

• has a low boiling point.

What is the reason for the low boiling point of methane?

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Buckminsterfullerene (C₆₀) is a form of carbon.

Buckminsterfullerene was the first fullerene to be discovered.

What is the shape of a buckminsterfullerene molecule?

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Graphite is a form of carbon.

Figure 11 represents the structure of graphite.

How many covalent bonds does each carbon atom form in graphite?

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Diamond is another form of carbon.

Figure 12 represents the structure of diamond.

Describe the structure and bonding in diamond.

This question is about electrolysis and the extraction of metals.

Why can some molten substances be electrolysed?

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Table 3 shows the products of the electrolysis of some molten compounds.

Complete Table 3.

Aluminium is extracted by electrolysing molten aluminium oxide.

Balance the equation for the reaction.

Choose numbers from the box.

Calculate the relative formula mass (M_r) of aluminium oxide (Al₂O₃).

Relative atomic masses (A_r): O = 16 Al = 27

Figure 13 shows part of the reactivity series of metals.

The non-metal carbon has been included.

Metals can be extracted from their compounds by:

electrolysis

reduction with carbon.

Electrolysis is more expensive than reduction with carbon.

Predict one metal that would be extracted by each method.

Use Figure 13.

This question is about chemical cells.

A student connects four 1.5 V cells in series to make a battery.

What is the total voltage produced by the battery?

A chemical cell can be made using two different metals in contact with an electrolyte.

Figure 14 shows a chemical cell.

Which is a suitable electrolyte for a chemical cell?

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A student made the hypothesis:

‘The voltage produced by a cell depends on the difference in the reactivity of metal A and metal B.’

Plan an investigation to test this hypothesis.

Your plan should produce valid results.

Use Figure 14.

A student produced a salt by reacting copper carbonate with sulfuric acid.

This is the method used.

1. Measure 50 cm³ of sulfuric acid into a beaker.

2. Add copper carbonate powder.

3. Stir the mixture.

4. Repeat steps 2 and 3 until copper carbonate is in excess.

5. Filter the mixture.

6. Warm the filtrate gently until crystals start to appear.

7. Leave the solution to cool and crystallise.

Complete the word equation for the reaction.

copper + sulfuric → + + carbon

Give one observation the student could make during Step 4 which shows that the copper carbonate is in excess.

Give one reason for filtering the mixture in Step 5.

Name the equipment that can be used to warm the filtrate gently in Step 6.

The maximum theoretical mass of the salt that could be produced using 50 cm³ of the sulfuric acid is 12.5 g.

The percentage yield of the salt is 92.8%.

Calculate the mass of salt actually produced.

Use the equation:

Some salts can be produced by reacting sulfuric acid with a metal.

Neither copper nor sodium is used to produce a salt with sulfuric acid.

Give one reason why each metal is not used.

This question is about the periodic table.

Sodium and potassium are in Group 1 of the periodic table.

Give one similarity and one difference between the electronic structures of sodium and potassium.

Group 1 elements react with water.

Give two observations made when potassium reacts with water.

Potassium hydroxide solution is produced when potassium reacts with water.

What is the colour of universal indicator when added to potassium hydroxide solution?

Give one reason for your answer.

Colour of universal indicator

Table 4 shows the densities of some of the elements in Group 0 of the periodic table.

Plot the data from Table 4 on Figure 15.

Estimate the density (X) of krypton.

Use Figure 15 and Table 4.

The elements in Group 7 are called the halogens.

A more reactive halogen can displace a less reactive halogen from a solution of its salt.

Which combination of solutions will produce a reaction when mixed?

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Which of the following describes the trends going down Group 7?

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This question is about models of the atom.

Figure 16 shows two early models of the atom.

Name the models of the atom shown in Figure 16.

Compare model A with the model of the atom used today.

Use Figure 16.

Chadwick’s experiments showed the existence of neutrons in an atom.

This led to an understanding of isotopes.

Define the term ‘isotopes’.

Refer to subatomic particles in your answer.