OCR GCSE Chemistry A (Gateway) Paper 1 Foundation June 2023 question paper J248/01

1h 45m 90 marks

22 questions

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Where is most of the mass found in an atom?

A Electrons

B Neutrons

C Nucleus

D Protons

$Question 1, shown as an image$

[1]

Answer

Sodium fluoride has the formula NaF. The formula of the sodium ion is Na +. 2

What is the formula of the fluoride ion?

F + A

F – B

F²⁺ C

F^2– D

$Question 2, shown as an image$

[1]

Answer

Which row of results shows that the pH of a solution is acidic ?

	pH	Universal indicator colour
A	3	orange
B	10	blue
C	3	blue
D	10	orange

$Question 3, shown as an image$

[1]

Answer

Thomson discovered the first sub-atomic particle.

Which sub-atomic particle did Thomson discover?

A Atom

B Electron

C Neutron

D Proton

$Question 4, shown as an image$

[1]

Answer

What is the relative formula mass of iron chloride, FeCl₃?

Relative atomic mass (A_r): Cl = 35.5 Fe = 55.8.

A 91.3

B 126.8

C 162.3

D 202.9

$Question 5, shown as an image$

[1]

Answer

An element gains electrons to form a full outer shell.

Which part of the Periodic Table will the element be from?

$Question 6, shown as an image$

[1]

Answer

Why can the mass of a reaction in an open conical flask decrease?

A One of the products is a gas.

B One of the products is a solid.

C One of the reactants is a liquid.

D One of the reactants is a solid.

$Question 7, shown as an image$

[1]

Answer

When the model of the atom was developed, scientists reviewed the work of other scientists.

Why is it important for scientists to review each other’s work?

A They will copy the experiments to complete the research first.

B They will evaluate the data and suggest improvements.

C They will make sure that personal protective equipment is worn.

D They will start an argument about who is correct.

$Question 8, shown as an image$

[1]

Answer

Which reaction profile has an arrow showing the activation energy ?

$Question 9, shown as an image$

[1]

Answer

63.5 g of copper reacts to make 134.5 g of copper chloride, CuCl₂.

$Question 10, shown as an image$

How much copper chloride will be made from 0.635 g of copper?

A 0.01345 g

B 0.1345 g

C 1.345 g

D 13.45 g

$Question 10, shown as an image$

[1]

Answer

Why are nanoparticles useful as catalysts in chemical reactions?

A Nanoparticles are a new technology.

B Nanoparticles have a high surface area to volume ratio.

C Nanoparticles have a large particle size.

D Nanoparticles have a low surface area to volume ratio.

$Question 11, shown as an image$

[1]

Answer

The melting point of magnesium chloride is 714 °C.

Which state symbols are used for magnesium chloride at these temperatures?

	State symbol at 25 °C	State symbol at 110 °C
A	g	g
B	s	s
C	s	g
D	g	s

$Question 12, shown as an image$

[1]

Answer

What changes did Mendeleev make to improve his Periodic Table?

A He arranged elements by mass number.

B He arranged elements by the number of neutrons.

C He put elements with low melting points on the left and high melting points on the right.

D He realised some elements had not yet been discovered so left spaces for them.

$Question 13, shown as an image$

[1]

Answer

Nitrogen monoxide, NO, can be oxidised to form nitrogen dioxide, NO₂.

$Question 14, shown as an image$

What is the oxidising agent in this reaction?

A Nitrogen

B Nitrogen dioxide

C Nitrogen monoxide

D Oxygen

$Question 14, shown as an image$

[1]

Answer

Hydrochloric acid, HC l, reacts with magnesium, Mg.

Magnesium chloride and hydrogen are made.

What is the balanced symbol equation for this reaction?

$Question 15, shown as an image$

[1]

Answer

(a)

Oxygen is a gas at room temperature.

(a)(i)

The diagrams show three different particle models.

Which particle model represents a gas ?

Tick (✓) one box.

$Question 16, shown as an image$

[1]

Answer

(a)(ii)

Oxygen has a melting point of –219 °C and a boiling point of –183 °C.

State a temperature at which oxygen will be a liquid.

[1]

Answer

(a)(iii)

Complete the sentences about the particle models.

Use words from the list.

condensing freezing less melting more

A liquid becoming a solid is called........ In a solid, the particles

move........ than in a liquid. In a solid, the arrangement of particles is

........ random than in a liquid.

[3]

Answer

(b)

Draw lines to connect each particle with its correct description.

[2]

Answer

(c)

The element oxygen has three different isotopes.

Isotope 1 Isotope 2 Isotope 3

(c)(i)

Which isotope has the highest mass?

[1]

Answer

(c)(ii)

Which isotope has the same number of protons and neutrons?

[1]

Answer

(c)(iii)

Atoms of each isotope have the same number of electrons.

How many electrons do these atoms have?

[1]

Answer

(d)

A sample of air contains all three isotopes of oxygen. It contains 99.759% of isotope 1 and 0.037% of isotope 2.

Calculate the percentage of isotope 3 in the sample of air.

[2]

Answer

A scientist measures the melting points of three painkillers.

Painkiller	Melting point (°C)
A	136
B	169
C	76

(a)

All of the painkillers are pure substances.

(a)(i)

Explain what is meant by a pure substance.

[1]

Answer

(a)(ii)

How can you tell that the three painkillers are pure from their melting points?

[1]

Answer

(b)

The scientist uses gas chromatography to investigate a mixture of painkiller A and painkiller B.

How many peaks will the scientist see in the gas chromatogram?

[1]

Answer

(c)

The scientist then analyses painkiller D using thin layer chromatography.

The chromatogram is shown in the diagram.

(c)(i)

Calculate the R_f value of painkiller D.

$Question 17, shown as an image$

Give your answer to 2 decimal places.

[3]

Answer

(c)(ii)

Which components are needed for thin layer chromatography?

$Question 17, shown as an image$

balance
Bunsen burner
mobile phase

paper
stationary phase
thermometer

[2]

Answer

(d)

The scientist thinks that an impure painkiller will only have two spots on the thin layer chromatogram.

Give two reasons why the scientist is incorrect.

[2]

Answer

Molecules can be shown by different models.

(a)

Draw three lines to connect each name to its correct model.

[3]

Answer

(b)

A student wants to use a model to show the location of the electrons in a water molecule as shown in Fig. 18.1.

Fig. 18.1

Model 1 Model 2

Explain why the student uses model 1 instead of model 2.

[2]

Answer

(c)

Fig. 18.2 shows a model of octane.

Fig. 18.2

Key

$Question 18, shown as an image$

(c)(i)

What is the empirical formula of octane?

[1]

Answer

(c)(ii)

Calculate the relative formula mass of octane.

Relative atomic mass (A_r): C = 12.0 H = 1.0.

[3]

Answer

(d)

Fig. 18.3 shows a model of a carbon nanotube.

Fig. 18.3

(d)(i)

What is the diameter of the carbon nanotube in nanometres ?

[1]

Answer

(d)(ii)

Fig. 18.4 shows a model of the structure and bonding in graphite.

Fig. 18.4

Explain why the carbon nanotube is stronger than graphite.

Use Fig. 18.3 and Fig. 18.4.

[2]

Answer

(d)(iii)

A hydrogen atom has a diameter of 2.4 10^–10 m. (iii) maths symbol

Calculate how many times larger the carbon nanotube is than the hydrogen atom.

[2]

Answer

The table shows the type of bonding in three substances.

Substance	Type of bonding
Bromine, Br₂	simple molecular (covalent)
Sodium chloride, NaCl	ionic
Diamond, C	giant covalent

(a)

* Describe and compare the types of bonding in these three substances.

Predict which substance will have the lowest melting point.

[6]

Answer

(b)

Titanium is a metal element. Metal elements can be mixed with other elements to form metal alloys.

Metal element
Metal alloy

(b)(i)

Explain why a metal alloy is harder than a metal element.

[2]

Answer

(b)(ii)

In medicine, titanium alloys are used in hip replacements.

The table shows some properties of alloys. Tensile strength is the amount of load a material can take before it breaks.

Alloy	(g / cmDensity ₃)	Tensile strength (MPa)	Does it contain any toxic elements?
1	4.43	950	yes
2	4.52	950	no
3	5.70	546	no

Which alloy would be best to use in a hip replacement? Explain your answer.

Alloy........

Reason........

[3]

Answer

A teacher wants to make hydrogen and chlorine using electrolysis.

(a)

Some possible steps they can use in the electrolysis experiment are listed.

1. Put test tubes over the electrodes to collect gases.

2. Weigh each electrode.

3. Put the electrodes into a solution of sodium chloride.

4. Put on safety goggles.

5. Connect the battery.

6. Put the electrodes into solid sodium chloride.

Put the four steps that the teacher should use in the correct order.

[3]

Answer

(b)

Chlorine is in Period 3 and Group 7 of the Periodic Table.

Which statements about chlorine are correct ?

Tick (✓) two boxes.

$Question 20, shown as an image$

[2]

Answer

(c)

The teacher sets up another electrolysis experiment using copper sulfate solution, CuSO

The table shows their results.

Experiment	Mass of copper made (mg)	Volume of oxygen made (cm₃)
1	7.9	2.8
2	21.1	7.5
3	28.2	10.0
4	35.3
5	42.4	14.9

(c)(i)

Estimate how much oxygen will be made in experiment 4.

[1]

Answer

(c)(ii)

Describe the relationship between the amount of copper made and the amount of oxygen made.

[1]

Answer

(d)

Copper sulfate solution is an electrolyte.

What type of compound is an electrolyte?

Tick (✓) one box.

$Question 20, shown as an image$

[1]

Answer

(e)

Another teacher repeats the electrolysis experiment.

They record the mass of the electrode at the start of the experiment.

At the end of the experiment, they remove the electrode from the solution and record the mass immediately as shown in the diagram.

They notice that the mass is higher than they expect.

Suggest two changes the teacher could make to get a more accurate mass.

[2]

Answer

A scientist is studying acids and alkalis.

(a)

Which statement about acids and alkalis is correct ?

Tick (✓) one box.

$Question 21, shown as an image$

[1]

Answer

(b)

The scientist reacts sulfuric acid with insoluble magnesium carbonate, MgCO₃.

They repeat the experiment two more times.

The table shows their results.

	Experiment 1	Experiment 2	Experiment 3
Mass of magnesium sulfate, MgSO₄, produced (g)	4.37	4.31	4.38
Mass of magnesium carbonate, MgCO₃, remaining (g)	1.33	1.38	1.32

(b)(i)

Calculate the mean mass of magnesium sulfate, MgSO₄, made.

Give your answer to 3 significant figures.

[3]

Answer

(b)(ii)

Complete the balanced symbol equation for the reaction.

Include state symbols.

$Question 21, shown as an image$

[2]

Answer

(b)(iii)

How does the scientist remove the unreacted solid magnesium carbonate, MgCO₃(s)?

[1]

Answer

(b)(iv)

How does the scientist obtain pure dry magnesium sulfate crystals from magnesium sulfate solution?

[1]

Answer

(a)

A student does an experiment to find out the temperature change of the reaction between an acid and an alkali.

The diagram shows the student’s experiment.

(a)(i)

Label the equipment in the diagram.

[3]

Answer

(a)(ii)

Suggest one change the student can make so that the temperature change is measured more accurately. Use the diagram.

[1]

Answer

(b)

The student adds the acid, 5 cm³ at a time, to the alkali in the beaker. (b)

The student records the temperature of the solution after each addition of acid.

The table shows their results.

Volume of acid (cm₃)	Temperature (°C)
0	18
5	20
10	23
15	26
20	27
25	26
30	24

(b)(i)

Plot the results from the table on the grid.

[2]

Answer

(b)(ii)

Describe what happens to the temperature measured as the acid is added.

[2]

Answer

(b)(iii)

The reaction is exothermic.

Explain how you can tell this from the student’s results.

[1]

Answer

(c)

The activation energy for the student’s reaction is 132 kJ / mol.

Complete the sentence to state the meaning of activation energy.

Activation energy is the minimum........

[1]

Answer

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OCR J248 · Paper 1

Question 1

Question 2

Question 3

Question 4

Question 5

Question 6

Question 7

Question 8

Question 9

Question 10

Question 11

Question 12

Question 13

Question 14

Question 15

Question 16

Question 17

Question 18

Question 19

Question 20

Question 21

Question 22