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Earlier foundation: C1.2 States of matter
12 questions · 68 marks, in lesson order.
States of matter
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Bromine is a liquid at room temperature. A few drops of bromine evaporate and the brown vapour fills a gas jar.
Explain, using the particle model, why bromine is a liquid.
(3)Explain why the vapour fills the gas jar.
(3)Total for this question: 6 marks
States of matter
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The table gives the melting points and boiling points of three substances.
| substance | melting point / °C | boiling point / °C |
|---|---|---|
| ethanol | −114 | 78 |
| oxygen | −218 | −183 |
| sodium chloride | 801 | 1413 |
Give the state of each substance at 25 °C.
(2)Explain, in terms of particles, why energy is needed to boil ethanol.
(2)What is the state of ethanol at −120 °C?
(1)Oxygen is heated from −200 °C to 25 °C. Describe the change of state that happens. Use the data.
(1)Total for this question: 6 marks
Diffusion and changes of state
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A smell spreads through a room faster from a warm liquid than from the same liquid when cold.
Explain why more vapour forms from the warm liquid.
(2)Explain why the smell spreads faster.
(3)Total for this question: 5 marks
Elements, compounds and mixtures
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A student has a white solid. It may be a pure compound or a mixture of two compounds.
Describe what is meant by a pure compound.
(2)Explain how melting point evidence could tell the two apart.
(3)Total for this question: 5 marks
Filtration and crystallisation
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Excess insoluble copper oxide has been reacted with dilute sulfuric acid. The mixture contains unreacted copper oxide and copper sulfate solution.
Describe how to remove the unreacted copper oxide.
(2)Describe how to obtain pure, dry crystals from the filtrate.
(4)Total for this question: 6 marks
Distillation
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Fractional distillation separates two miscible liquids with different boiling points.
Describe what happens when the mixture is heated.
(2)Explain how the fractionating column separates the liquids.
(4)Total for this question: 6 marks
Chromatography
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A student makes a chromatogram. The ink baseline is below the solvent level and the solvent front is not marked.
Evaluate the method. Identify the errors and their effects.
(4)Suggest improvements and state what a matching spot shows.
(2)Total for this question: 6 marks
Atomic structure
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Copper is 69.2% copper-63 and 30.8% copper-65.
Calculate the relative atomic mass of copper. Give your answer to 1 decimal place.
(4)Explain why the relative atomic mass is not a whole number.
(1)Total for this question: 5 marks
Atomic structure
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An atom of sodium has 11 protons, 12 neutrons and 11 electrons.
Give the atomic number and the mass number of this atom.
(2)atomic number = mass number =
Explain why the atom has no overall charge.
(1)A second sodium atom has a mass number of 24. What name is given to atoms like these two? Explain how the second atom is the same as and different from the first.
(3)Total for this question: 6 marks
Electronic configuration
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Sodium (atomic number 11) and chlorine (atomic number 17) react to form sodium chloride.
Explain how the electronic configurations relate to their positions in the Periodic Table.
(3)Explain how they form ions.
(3)Total for this question: 6 marks
Electronic configuration
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The electrons in an atom are arranged in shells. The first shell holds up to 2 electrons and the second shell holds up to 8.
Write the electronic configuration of magnesium (atomic number 12).
(1)magnesium:
Sodium is 2,8,1 and potassium is 2,8,8,1. Use these electronic configurations to explain why sodium and potassium are in the same group and react in similar ways.
(2)Neon is 2,8. Explain why neon is unreactive.
(2)Total for this question: 5 marks
Group 1 metals
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Lithium, sodium and potassium are in Group 1. Each reacts with water.
Describe the similarities in their reactions.
(2)Explain the trend in reactivity.
(4)Total for this question: 6 marks
