Practice Paper 1 (Edexcel IAL Chemistry)

An oxide of lead contains 90.7% by mass of lead.

What is the formula of this oxide?

[A_r values: O = 16.0 Pb = 207.2]

The repeat unit of an addition polymer is shown.

What is the monomer used to make this polymer?

10.00 g of hydrated magnesium sulfate, MgSO₄•7H₂O, is heated to remove the water of crystallisation.

What mass of anhydrous magnesium sulfate, MgSO₄, is formed?

[Molar mass of MgSO₄•7H₂O = 246.4 g mol⁻¹ ]

How many protons, neutrons and electrons are present in a ⁸¹Br^- ion?

Several factors may affect ionisation energies:

I) the number of protons increases

II) the outer electron is further from the nucleus

III) the amount of shielding increases

IV) the number of unpaired outer electrons increases

Which factors explain the decrease in ionisation energy as Group 1 is descended?

The Period 2 element with the highest melting temperature is

What is the formula of magnesium nitride?

Which of these molecules is the most polar?

The displayed formula of a compound is shown.

Which functional group is present in the compound shown?

A single molecule of decane, C₁₀H₂₂ , is cracked.

Which of these mixtures could not be formed?

An organic compound, X, contains only the elements carbon and hydrogen.

When 0.560 g of X is completely combusted in excess oxygen, 1.760 g of carbon dioxide and 0.720 g of water are produced.

Calculate the empirical formula of X. You must show all your working.

The relative molecular mass, M_r, of X is 56.

Deduce the molecular formula of X.

When X is added to bromine water, the orange colour decolourises.

i) Name the functional group in X responsible for this reaction.

ii) Given that X has the C=C double bond at the end of the carbon chain, draw the displayed formula of X.

Compound X has other structural isomers with molecular formula C₄H₈.

Draw the displayed formulae of two other structural isomers of C₄H₈ (other than X), and give the systematic name of each.

Alkanes and alkenes are obtained from crude oil.

Describe how a sample of octadecane can be obtained from a mixture of alkanes.

i) Octadecane can be cracked to produce butene and one other product. Complete the equation. State symbols are not required.

C₁₈H₃₈ → 2C₄H₈ +

ii) One of the products of this cracking reaction is but-1-ene.

Give the skeletal formulae for the other three alkene isomers of C₄H₈

iii) Some reactions of but-1-ene are shown.

Give the name and structural formula of each of the products.

Draw the displayed formula of poly(but-1-ene) showing two repeat units.

State one advantage and one disadvantage of using incineration for the disposal of polymers, other than the effect on climate.

i) Butane is used as a fuel.

The equation for the complete combustion of butane is shown.

2C₄H₁₀(g) + 13O₂(g) → 8CO₂(g) + 10H₂O(l)

35.0 cm³ butane is completely burned in 300 cm³ oxygen.

Calculate the final total volume of gas in cm³.

All volumes are measured at the same temperature and pressure.

ii) Explain the main hazard when using butane as a fuel in a portable heater in an enclosed space.

A 0.210 g sample of a volatile organic liquid C is injected into a gas syringe and heated in an oven. At 100 kPa and 358 K, the syringe contains 72.5 cm³ of gas.

Calculate the molar mass of C. [pV = nRT R = 8.31 J mol⁻¹ K⁻¹ ]

The organic liquid C is a hydrocarbon. Give a possible name or formula for C, using your answer in (a).

This question is about the element sulfur.

Complete the diagram to show the electronic configuration for a sulfur atom in the ground state. Include labels for each subshell.

Write an equation for the first ionisation energy of sulfur. Include state symbols.

Explain why the first ionisation energy of sulfur is less than the first ionisation energies of both phosphorus and chlorine.

A sample of sulfur contains four isotopes.

i) State what is meant by the term isotopes, in terms of subatomic particles.

ii) Calculate the relative atomic mass of sulfur in this sample. Give your answer to two decimal places.

The mass spectrum of a sample of sulfur with ³²S as the only isotope is shown.

i) Calculate the number of sulfur atoms in the molecular ion. You must show your working.

ii) Suggest the formula of the most stable ion shown by this spectrum.

This question is about copper and its compounds.

Complete the electronic configurations of Cu and Cu²⁺.

Cu [A_r].....................................................................................................

Cu²⁺ [A_r].....................................................................................................

A sample of copper contains the isotopes ⁶³Cu and ⁶⁵Cu.

i) Complete the table to show the numbers of subatomic particles in the atoms of these two isotopes of copper.

ii) Explain the term isotopes, using the information in the table.

iii) State why the two isotopes of copper have the same chemical reactions.

iv) The relative atomic mass of copper in this sample is 63.4. Calculate the percentage abundances of the isotopes ⁶³Cu and ⁶⁵Cu in this sample. You must show your working.

Copper(II) sulfate, CuSO₄, can be made by reacting solid copper(II) carbonate with dilute sulfuric acid.

i) Write an equation for the reaction that occurs. State symbols are not required.

ii) An experiment was carried out to produce pure, dry crystals of hydrated copper(II) sulfate, CuSO₄ •5H₂O. Copper(II) carbonate was mixed with 50.0 cm³ of 1.00 mol dm^–3 sulfuric acid until no more reacted. The mass of CuSO₄ •5H₂O obtained was 10.87g.

Calculate the percentage yield for this reaction, giving your answer to an appropriate number of significant figures. [Molar mass of CuSO₄ •5H₂O = 249.6 g mol⁻¹ ]