Edexcel A Level Chemistry Paper 1: Advanced Inorganic and Physical Chemistry June 2022 question paper 9CH0/01

1h 45m 90 marks

8 questions

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This question is about atomic structure and the Periodic Table.

(a)

Complete the table to show the relative charges and masses for a neutron and an electron.

(2)

Answer

(b)

Atomic emission spectroscopy provides evidence for the existence of

$Question 1, shown as an image$

(1)

Answer

(c)

Draw the shape of a p orbital.

(1)

Answer

(d)

The melting temperatures of two elements in Period 3 are given in the table.

Element	silicon	chlorine
Melting temperature / K	1683	172

Explain, in terms of the structure and bonding of each element, the difference between these values.

(3)

Answer

This question is about the elements in Group 2 of the Periodic Table.

(a)

Magnesium powder is added to a beaker of water containing a few drops of Universal Indicator.

The apparatus is set up as shown and allowed to stand for a few days.

State two changes that will be seen after a few days.

(2)

Answer

(b)

Explain how the trend in the reactivity of the Group 2 elements is determined by their electronic configurations.

(3)

Answer

(c)

Calcium reacts with chlorine.

$Question 2, shown as an image$

Explain, in terms of electrons, why this is a redox reaction.

(2)

Answer

(d)

An experiment was carried out to determine the molar volume of hydrogen at room temperature.

0.035 g of magnesium was added to excess hydrochloric acid and 32 cm³ of hydrogen was produced.

$Question 2, shown as an image$

Calculate the molar volume of hydrogen from the results of this experiment. Include units in your answer.

(2)

Answer

This question is about the elements in Group 7 of the Periodic Table and some of their compounds.

(a)

What is the colour of iodine in the solid and gas states?

(1)

Answer

(b)

Which of these reactions occurs?

$Question 3, shown as an image$

(1)

Answer

(c)

The halogens can form halide ions during reactions.

Complete the electronic configuration of the chloride ion.

(1)

Answer

(d)

The standard electrode potentials for two half‑equations involving bromine are given.

$Question 3, shown as an image$

(d)(i)

Explain why the disproportionation of bromine in water is not thermodynamically feasible under standard conditions. Include the overall equation for the disproportionation and its $fraction$ value.

(3)

Answer

(d)(ii)

Bromine disproportionates in water to a small extent at 298 K.

Give a possible reason why this reaction occurs.

(1)

Answer

(e)

The hydrogen halides have the general formula HX, where X represents the symbol of the halogen.

(e)(i)

(1)

Answer

(e)(ii)

What type of reaction occurs when ammonia gas reacts with hydrogen chloride gas?

$Question 3, shown as an image$

(1)

Answer

This question is about structure and bonding.

(a)

Ionic bonding is the strong electrostatic attraction between

$Question 4, shown as an image$

(1)

Answer

(b)

An aqueous solution of copper(II) chromate(VI) was electrolysed using the apparatus shown in the diagram.

Deduce the colours of the solutions in regions E and F after the electrolysis has occurred.

Colour in region E_........

Colour in region F_........

(2)

Answer

(c)

Some ionic radii are given in the table.

Ion	Ionic radius / nm
Na⁺	0.102
Mg²⁺	0.072
Cl^–	0.180
Br^–	0.195

Deduce the formula of the compound, formed from the ions in the table, that has the strongest ionic bonding.

(1)

Answer

(d)

The names of four substances are given.

Substance	Name
P	copper
Q	iodine
R	silicon(IV) oxide
S	sodium chloride

(d)(i)

Which of these substances exists at room temperature as a giant lattice of oppositely charged ions?

$Question 4, shown as an image$

(1)

Answer

(d)(ii)

Which of these substances has a high melting temperature, and conducts electricity when solid and when molten?

$Question 4, shown as an image$

(1)

Answer

(e)

*(e) Water has two significant anomalous properties:

• it has a higher melting temperature than hydrogen sulfide, H₂S, even though it has fewer electrons in its molecules

• the density of ice at 0 maths symbol C is less than that of water at 0C.

Explain these properties.

You should include a labelled diagram to show the intermolecular forces between two molecules of water.

(6)

Answer

This question is about enthalpy changes and energy changes.

(a)

Magnesium carbonate reacts with dilute hydrochloric acid at room temperature.

$Question 5, shown as an image$

When the reaction is carried out in a sealed container with a constant volume, the heat energy change is not the same as the enthalpy change for this reaction.

Give a reason why this is so.

(1)

Answer

(b)

State what is meant by the standard enthalpy change of formation of aluminium oxide, Al₂O₃(s). Include standard conditions.

(3)

Answer

(c)

Use the data in the table to answer the questions.

(c)(i)

Name the two properties of ions that affect the value of their enthalpy change of hydration.

(2)

Answer

(c)(ii)

(3)

Answer

This question is about acids and bases.

(a)

State what is meant by a Brønsted‑Lowry base.

(1)

Answer

(b)

Write the ionic equation for the reaction between magnesium oxide and an acid. State symbols are required.

(2)

Answer

(c)

Calculate the concentration of hydrogen ions, in mol dm^–3, in a solution with a pH of 9.43

(1)

Answer

(d)

The pH of two salt solutions, J and K, are

solution J pH = 5

solution K pH = 9

The solutions are equimolar.

Which acids and bases could form the salts in solutions J and K ?

(1)

Answer

(e)

The ionic product of water, K_w, varies with temperature as shown.

Temperature /C	K_w / mol²dm^–6
0	0.1110^–14
10	0.2910^–14
20	0.6810^–14
30	1.4710^–14
40	2.9210^–14
50	5.4810^–14

(e)(i)

Determine the value of K_w at 45 maths symbol C by plotting a suitable graph. You must show your working on the graph.

(3)

Answer

(e)(ii)

The ionic product of water at 30 maths symbol C is 1.4710^–14mol²dm^–6.

Calculate the pH of water at this temperature.

(3)

Answer

(f)

Hydrochloric acid, with a concentration of 0.100 mol dm^–3, is added to 25.0 cm³ of 0.100 mol dm^–3 aqueous sodium carbonate and the pH is measured.

The titration curve is shown.

$Question 6, shown as an image$

The reaction takes place in two steps. The equation for the reaction taking place in the first step is

$Question 6, shown as an image$

(f)(i)

Deduce a suitable indicator to identify the first equivalence point. Justify your answer using values from the Data Booklet.

(2)

Answer

(f)(ii)

Write the equation for the reaction taking place at the second equivalence point. State symbols are not required.

(1)

Answer

(f)(iii)

Explain how the solution at point X on the graph can act as a buffer solution.

(3)

Answer

This question is about chromium and some of its compounds.

(a)

The common oxidation numbers of chromium are +2, +3 and +6.

Give a reason, in terms of ionisation energies, why chromium can show variable oxidation numbers.

(1)

Answer

(b)

The bonding in chromate(VI) ions, CrO₄^2–, is similar to that in sulfate(VI) ions, SO₄^2–.

Draw a possible dot‑and‑cross diagram for a chromate(VI) ion.

(2)

Answer

(c)

A student added some pieces of zinc to an acidified solution of potassium dichromate(VI).

Some standard electrode potentials are given in the table.

(c)(i)

Write the overall equation for the reduction of dichromate(VI) ions to chromium(III) ions by zinc in acid conditions. State symbols are not required.

(2)

Answer

(c)(ii)

Calculate $fraction$ for the reaction in (c)(i).

(1)

Answer

(c)(iii)

Predict whether or not a further reduction of chromium(III) ions to chromium(II) ions will occur. Justify your answer.

(1)

Answer

(c)(iv)

Aqueous solutions containing chromium(III) ions and chromium(II) ions have different colours.

Explain why these solutions differ in colour. An explanation of the origin of the colours is not required.

(2)

Answer

(d)

An iron nail was analysed using the following outline procedure.

• An iron nail was placed in a beaker and excess dilute sulfuric acid was added.

• After all the iron had reacted to form iron(II) ions, the solution was made

$Question 7, shown as an image$

• 25.0 cm³ portions of the solution were acidified and titrated with potassium dichromate(VI) solution of concentration 0.0167 mol dm^–3.

Results

mass of iron nail = 3.54 g

mean titre = 15.50 cm³

The table shows the percentage by mass of iron in four different brands of nail.

Brand of nail	Percentage by mass of iron
A	92
B	94
C	96
D	98

Potassium dichromate(VI) in acid solution oxidises iron(II) ions as shown in the equation

$Question 7, shown as an image$

Determine, using the experimental data, the brand of nail that was analysed.

(5)

Answer

This question is about electrode potentials, cells and equilibrium constants.

(a)

Chlorine gas can be prepared by the oxidation of chloride ions with manganate(VII) ions in acid solution.

$Question 8, shown as an image$

During this reaction, each manganate(VII) ion accepts five electrons.

Calculate the equilibrium constant, K, for this reaction at 298 K using the expression

$Question 8, shown as an image$

where n is the number of electrons transferred in the overall equation, F is the Faraday constant (96 500 C mol^–1) and R is the gas constant (8.31 J mol^–1K^–1). Units of K are not required.

(2)

Answer

(b)

A fuel cell produces a voltage from the reaction between a fuel and oxygen.

The reaction occurring at one electrode in a methanol fuel cell is

$Question 8, shown as an image$

Which reaction occurs at the other electrode?

$Question 8, shown as an image$

(1)

Answer

(c)

Lead‑acid batteries are used as storage cells in some cars.

The electrolyte is sulfuric acid, one electrode is lead and the other is lead(IV) oxide, PbO₂.

As the cell discharges, the lead and the lead(IV) oxide are both converted to solid lead(II) sulfate, PbSO₄, and the concentration of the sulfuric acid decreases.

Deduce, using the information given, the two half‑equations occurring in the lead‑acid battery. State symbols are required.

(3)

Answer

(d)

When solid lead(II) sulfate is added to aqueous sodium iodide, an equilibrium is established.

$Question 8, shown as an image$

The expression for the equilibrium constant, K_c, for this reaction is

$Question 8, shown as an image$

In an experiment, K_c may be determined by adding excess lead(II) sulfate to 25.0 cm³ of 0.100 mol dm^–3 sodium iodide. The volume remains constant at 25.0 cm³. The mixture is left to reach equilibrium at room temperature.

Ice‑cold water is added to freeze the position of equilibrium and the mixture is then titrated with standard silver nitrate solution.

The whole mixture requires 12.20 cm³ of 0.0500 mol dm^–3 silver nitrate solution to react with the aqueous iodide ions at equilibrium.

$Question 8, shown as an image$

Calculate the equilibrium concentrations of the sulfate ions and the iodide ions, and hence the value of K_c at room temperature. Give your answer to an appropriate number of significant figures and include units for K_c, if any.

(7)

Answer

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Edexcel 9CH0 · Paper 1

Question 1

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Question 7

Question 8