Structure (Edexcel A Level Chemistry)

Exam Questions

1 hour8 questions
1a5 marks

This question is about crystalline solids.

Iodine and diamond are crystalline solids at room temperature.

Explain why diamond has a much higher melting temperature than iodine.

1b2 marks

Graphite is also a crystalline solid at room temperature.

Unlike diamond, graphite conducts electricity.

Describe the key feature of the bonding of the carbon atoms in graphite that results in it being an electrical conductor.

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1a2 marks

This question is about methanol, CH3OH.

Draw a dot-and-cross diagram to show the bonding in a molecule of methanol.

Show outer shell electrons only.

1b1 mark

Predict which bond has the shortest bond length in a molecule of methanol.

1c4 marks

Methanol is soluble in water.

i)
State the strongest type of intermolecular force that occurs between molecules of methanol and water.

(1)

ii)
Draw a labelled diagram to show the interaction named in (c)(i) between one molecule of methanol and one molecule of water.
Include any relevant lone pairs and dipoles in your diagram.

(3)

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2a5 marks

This question is about some halogens and their compounds.

The intermolecular attractions between halogen molecules are London forces.

i)
Describe how London forces form between halogen molecules.
(3)

ii)
The boiling temperatures of chlorine and bromine are shown in the table.

Halogen Boiling temperature / °C
chlorine −34
bromine 59

Explain why bromine has a higher boiling temperature than chlorine.
(2)
2b5 marks

A student carries out experiments to determine the order of reactivity of three halogens:
bromine, chlorine and iodine.
The student is provided with aqueous solutions of the following five substances:

  • bromine
  • iodine
  • potassium chloride
  • potassium bromide
  • potassium iodide.

The student has no access to chlorine gas or chlorine water.
The student uses cyclohexane, an organic solvent, to identify the halogen present at the end of each experiment.

The student carries out the smallest number of experiments required to determine the order of reactivity of the halogens.

Describe the experiments and the expected observations.

Include in your answer ionic equations for any reactions that occur.

State symbols are not required.

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3a8 marks

This question is about compounds of Group 5 elements.  

Phosphorus forms two chlorides with the formulae PCl3 and PCI5


i)

Explain the shape of the PCl3 molecule. The bond angle is not required.  

(3)

ii)
Draw a diagram to show the three-dimensional shape of the PCI5, molecule in the gas phase.
Include bond angles and the name of the shape. 

(3)

iii)
Explain why phosphorus forms PCI5, but nitrogen does not form NCI5.  

(2)

3b5 marks

Nitrogen trichloride, NCl3, has a boiling temperature of 344 K, and nitrogen trifluoride, NF3, has a boiling temperature of 144 K.

Explain this difference in boiling temperatures, by referring to all the intermolecular forces present.  

3c1 mark

Which of these compounds produces hydrogen chloride when it reacts with PCl5

  A propanal
  B propan-1-ol
  C propanone
  D propyl propanoate

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4a2 marks

Compound X is a component of synthetic oils used as lubricants, for instance in the gearboxes of ships.

q5-9cho-al-2-oct-2021-edexcel-a-level-chem

Name the three functional groups present in compound X.

4b1 mark

The effectiveness of this synthetic oil is much reduced if it is contaminated with water.

Give, in terms of a chemical reaction, a possible reason for this.

4c3 marks

An alternative to synthetic oil is known as mineral oil and consists solely of hydrocarbons separated from crude oil.

i)
What is the name of the process used to separate different hydrocarbons from crude oil?
(1)

  A cracking
  B reforming
  C fractional distillation
  D heating under reflux

ii)

Explain why compound X is likely to have a higher boiling temperature than hydrocarbons of a similar molecular mass and shape.

A detailed description of how the intermolecular forces arise is not required.

(2)

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5a1 mark

This question is about the solubility of some alcohols.
The table shows the solubility in water of the first six alcohols in a homologous series.

Alcohol Solubility / g dm–3
methanol soluble in all proportions
ethanol soluble in all proportions
propan-1‐ol soluble in all proportions
butan-1‐ol 632
pentan-1‐ol 22
hexan-1‐ol 5.9

State what is meant by a homologous series.

You may use the alcohols in the table to illustrate your answer.

5b3 marks

Explain why methanol and water are ‘soluble in all proportions’.

You must include a diagram in your answer.

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66 marks

The compounds hydrogen fluoride, water and methane, all have simple molecular structures, but they have significantly different boiling temperatures.

Discuss the reasons for the differences in the boiling temperatures of the three compounds, using the data in the table and the Pauling electronegativity values in the Data Booklet.

Compound Boiling temperature / oC Number of electrons
CH4 -161.5 10
H2O 100.0 10
HF 19.5 10

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7a3 marks

The table shows some information about a selection of elements and compounds.

  Graphene Graphite Diamond Magnesium
oxide
Potassium
bromide
Iron
Melting
temperature / K
> 4000 3950 3820 3125 1007 1808
Density
/ g cm−3
not
measured
2.2 to 2.8 3.51 3.58 2.75 7.86
Compressive
strength / GPa
not
measured
2.3 and
15.3
443 152 15 170

Explain the difference in the melting temperatures of magnesium oxide and potassium bromide.

7b2 marks

Explain why the electrical conductivity of solid potassium bromide is poor but an aqueous solution of potassium bromide is a good electrical conductor.

7c6 marks

Graphene, graphite and diamond are all forms of solid carbon.
Explain, in terms of structure and bonding, why graphene and graphite are good electrical conductors but diamond is a poor electrical conductor.

You may include labelled diagrams in your answer.

7d2 marks

Deduce two possible reasons why the density of iron (7.86 g cm−3) is much greater than the density of graphite (2.2 to 2.8 g cm−3).

7e2 marks

The compressive strength is a measure of the energy required to break some of the bonds within a substance.

Deduce possible reasons why there are two widely different values for the compressive strength of graphite.
Both the values (2.3 and 15.3 GPa) are valid experimental results.

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