AQA GCSE Chemistry Paper 1 Foundation November 2021 question paper 8462/1F

This question is about elements, compounds and mixtures.

Substance A contains only one type of atom.

Substance A does not conduct electricity.

Which type of substance is A ?

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Substance B contains two types of atoms.

The atoms are chemically combined together in fixed proportions.

Which type of substance is B ?

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What is the name of the elements in Group 0 of the periodic table?

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Which statement about the elements in Group 0 is correct?

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Neon is in Group 0.

What type of particles are in a sample of neon?

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Figure 1 represents part of the structure of an oxide of a metal.

Determine the empirical formula of this oxide.

Empirical formula = XO___

A nanoparticle of a metallic element is a cube.

Figure 2 shows a diagram of the nanoparticle.

The surface area of a cube is given by the equation:

surface area = length of side² × 6

Calculate the surface area of the cube in Figure 2.

Give your answer to 2 significant figures.

Fine and coarse particles of the metallic element are also cubes.

The length of a fine particle cube is 10 times smaller than the length of a coarse particle cube.

How does the surface area to volume ratio of the fine particle cube compare with that of the coarse particle cube?

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This question is about chemical cells and batteries.

Three different types of battery can be used to power a TV remote control.

Table 1 gives information about these batteries.

Give one advantage of each type of battery.

Nickel-metal hydride

Figure 3 shows a symbol printed on batteries.

This symbol shows that batteries should not be put in household waste.

Suggest why batteries should not be put in household waste.

Figure 4 shows a chemical cell.

The order of reactivity of three metals is shown below.

Which combination of metal electrodes would give the highest voltage in the chemical cell in Figure 4 ?

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The voltage produced by the cell in Figure 4 depends on the type of electrodes and the type of electrolyte.

Suggest one other factor that could affect the voltage produced.

Water is produced in a hydrogen fuel cell.

Complete the word equation to show the reaction that produces water in a hydrogen fuel cell.

This question is about Group 1 elements.

Complete Table 2 to show the electronic structure of a potassium atom.

Why do Group 1 elements have similar chemical properties?

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What is the type of bonding in sodium?

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Table 3 shows observations made when lithium, potassium and rubidium react with water.

Give two observations you could make when sodium reacts with water.

Write your answers in Table 3.

How does the reactivity of the elements change going down Group 1?

Give two ways in which the observations in Table 3 show the change in reactivity going down Group 1.

Which gas is produced when Group 1 elements react with water?

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Sodium fluoride is an ionic compound.

Figure 5 shows dot and cross diagrams for a sodium atom and a fluorine atom.

Complete Figure 5 to show what happens when a sodium atom and a fluorine atom react to produce sodium fluoride.

You should:

• complete the electronic structures of the sodium ion and the fluoride ion

• give the charges on the sodium ion and the fluoride ion.

Figure 5

A student investigated the reactivity of metals with hydrochloric acid.

This is the method used.

1. Measure 50 cm³ of hydrochloric acid into a polystyrene cup.

2. Measure the temperature of the hydrochloric acid.

3. Add one spatula of metal powder to the hydrochloric acid and stir.

4. Measure the highest temperature the mixture reaches.

5. Calculate the temperature increase for the reaction.

6. Repeat steps 1 to 5 three more times.

7. Repeat steps 1 to 6 with different metals.

Table 4 shows the student’s results.

Calculate the mean temperature increase X for magnesium in Table 4.

Do not include the anomalous result in your calculation.

Determine the order of reactivity for the metals cobalt, magnesium and zinc.

Use Table 4.

The range of measurements either side of the mean shows the uncertainty in the mean temperature increase.

Complete the sentence.

Use Table 4.

What type of variable is the volume of hydrochloric acid in this investigation?

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Suggest one way of improving step 3 in the method to give results which are more repeatable.

Figure 6 shows a reaction profile for the reaction of magnesium with hydrochloric acid.

What do labels A, B and C represent on Figure 6 ?

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This question is about acids and alkalis.

Which ion do acids produce in aqueous solution?

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Acids react with alkalis.

What is the name of this type of reaction?

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Balance the equation for the reaction between sulfuric acid and potassium hydroxide.

Universal indicator turns purple in potassium hydroxide solution.

What is the pH of the solution?

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A student does a titration to find the volume of sulfuric acid that reacts with 25 cm³ of potassium hydroxide solution.

Figure 7 shows the equipment used.

The 25 cm³ of potassium hydroxide solution is measured with the measuring cylinder.

Which piece of equipment could the student use to measure the 25 cm³ of potassium hydroxide solution more accurately?

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Describe how the student would use the equipment in Figure 7 to complete the titration.

This question is about metal carbonates.

A student investigated the reaction of copper carbonate with an acid.

Figure 8 shows the apparatus.

This is the method used.

1. Pour 25 cm³ of the acid into a conical flask.

2. Weigh 0.10 g of copper carbonate.

3. Remove the stopper and add the copper carbonate to the flask.

4. Quickly replace the stopper.

5. Record the maximum volume of gas collected in the gas syringe.

6. Repeat steps 1 to 5 with different masses of copper carbonate.

Figure 9 shows the gas syringe during the experiment.

What is the reading on the gas syringe?

The student plotted the results on a graph.

Figure 10 shows the student’s graph.

Determine the gradient of the line of best fit.

You should:

• calculate the values of the change in y and the change in x

• calculate the gradient of the line of best fit.

Copper chloride was produced in the reaction.

Which acid reacts with copper carbonate to produce copper chloride?

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The reaction between copper carbonate and the acid produced a gas.

What was the gas?

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A different student produced a pure, dry sample of copper chloride using the same reaction.

This is the method used.

1. Add excess copper carbonate to the acid.

2. Filter the mixture.

3. Heat the solution gently until crystals start to form.

4. Leave for 24 hours.

5. Remove the crystals.

6. Rinse with water and dry the crystals.

Why was the solution heated gently in step 3 ?

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How should the solution be heated gently in step 3 ?

This question is about electrolysis.

Some students investigated the electrolysis of silver nitrate solution.

This electrolysis produces silver at the negative electrode.

Figure 11 shows the apparatus.

This is the method used.

1. Weigh the negative electrode.

2. Set up the apparatus shown in Figure 11.

3. Switch on the power supply.

4. Switch off the power supply after five minutes.

5. Rinse the negative electrode with water and allow to dry.

6. Reweigh the negative electrode.

7. Repeat steps 1 to 6 for different times.

Some silver did not stick to the negative electrode but fell to the bottom of the beaker.

The students needed to weigh this silver.

How could the students separate the silver from the silver nitrate solution?

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Table 5 shows the students’ results.

Draw a graph on Figure 12.

You should:

• use a suitable scale for the x-axis

• plot the data from Table 5

• draw a line of best fit.

Determine the mass of silver that would be produced after 12 minutes.

Use Figure 12.

A student investigated the electrolysis of two aqueous salt solutions.

Hydrogen is produced at the negative electrode when the metal in the salt solution is more reactive than hydrogen.

Complete Table 6 to show what the student would observe at the negative electrode for each salt solution.

A teacher demonstrates the electrolysis of molten lead bromide.

The products at the electrodes are lead and bromine.

Why should the teacher do the demonstration in a fume cupboard?

Two other molten compounds are electrolysed.

Complete Table 7 to show the molten compounds and the products.

This question is about carbon and its compounds.

Fullerenes are molecules of carbon atoms.

The first fullerene to be discovered was Buckminsterfullerene (C₆₀).

What shape is a Buckminsterfullerene molecule?

Give one use of a fullerene.

Propanone is a compound of carbon, hydrogen and oxygen.

Figure 13 shows the dot and cross diagram for a propanone molecule.

Complete Figure 14 to show a propanone molecule.

Use a line to represent each single bond.

Use Figure 13.

Figure 14

Determine the molecular formula of propanone.

Use Figure 13.

Propanone is a liquid with a low boiling point.

Why does propanone have a low boiling point?

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Figure 15 represents the structure of graphite.

Explain why graphite is:

• a good electrical conductor

• soft and slippery.

You should answer in terms of structure and bonding.

This question is about atomic structure and the periodic table.

Gallium (Ga) is an element that has two isotopes.

Give the meaning of ‘isotopes’.

You should answer in terms of subatomic particles.

Table 8 shows the mass numbers and percentage abundances of the isotopes of gallium.

Calculate the relative atomic mass (A_r) of gallium.

Give your answer to 1 decimal place.

Gallium (Ga) is in Group 3 of the modern periodic table.

Give the numbers of electrons and neutrons in an atom of the isotope⁶⁹₃₁Ga

What is the most likely formula of a gallium ion?

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Gallium was discovered six years after Mendeleev published his periodic table.

Give two reasons why the discovery of gallium helped Mendeleev’s periodic table to become accepted.

This question is about the extraction of metals.

Element R is extracted from its oxide by reduction with hydrogen.

The equation for the reaction is:

The sum of the relative formula masses (M_r) of the reactants (3 H₂ + RO₃) is 150

Calculate the relative atomic mass (A_r) of R.

Relative atomic masses (A_r): H = 1 O = 16

Identify element R.

You should use:

• your answer to question 10.1

• the periodic table.

Carbon is used to extract tin (Sn) from tin oxide (SnO₂).

The equation for the reaction is:

Calculate the percentage atom economy for extracting tin in this reaction.

Relative atomic masses (A_r): C = 12 O = 16 Sn = 119

Tungsten (W) is a metal.

Tungsten is extracted from tungsten oxide (WO₃).

All other solid products from the extraction method must be separated from the tungsten.

Table 9 shows information about three possible methods to extract tungsten from tungsten oxide.

Evaluate the three possible methods for extracting tungsten from tungsten oxide.