←Paper 1, Higher
Describe how the plum pudding model of the atom was replaced by the nuclear model.
Explain why the reactivity of Group 1 metals increases down the group.
Describe how sodium and chlorine atoms form an ionic compound. You may use dot-and-cross diagrams.
Calculate the relative formula mass (Mr) of CaCO₃. (Relative atomic masses: Ca = 40, C = 12, O = 16)
Explain how iron is extracted from iron(III) oxide in a blast furnace and why carbon can be used.
Describe how to prepare a pure, dry sample of copper(II) sulfate crystals from copper(II) oxide and dilute sulfuric acid.
Predict the products at each electrode in the electrolysis of copper(II) chloride solution and write the half equation at the cathode.
Explain the difference between exothermic and endothermic reactions, with an example of each.
An atom of potassium has mass number 39 and atomic number 19. Give the numbers of protons, neutrons and electrons.
Describe what you would see when potassium is added to water and write a balanced equation.
Explain why sodium chloride has a high melting point and conducts electricity when molten but not when solid.
Calculate the relative formula mass (Mr) of Mg(OH)₂. (Relative atomic masses: Mg = 24, O = 16, H = 1)
Explain why aluminium is extracted by electrolysis rather than reduction with carbon.
Explain the difference between a strong acid and a weak acid.
Explain the products of electrolysis of sodium chloride solution (brine).
Use the bond energies (kJ/mol) H–H 436, Cl–Cl 243, H–Cl 432 to calculate the energy change for H₂ + Cl₂ → 2HCl.
An element has two isotopes: mass 35 (75%) and mass 37 (25%). Calculate its relative atomic mass.
Explain why chlorine displaces bromine from potassium bromide solution and write an ionic equation.
Explain why methane has a low boiling point.
Calculate the relative formula mass (Mr) of H₂SO₄. (Relative atomic masses: H = 1, S = 32, O = 16)
Write the ionic equation for the reaction of zinc with copper(II) sulfate and identify what is oxidised.
The pH of an acid changes from 2 to 4. By what factor has the hydrogen ion concentration changed?
Explain why ionic compounds must be molten or dissolved to be electrolysed.
Use the bond energies (kJ/mol) H–H 436, O=O 498, O–H 464 to calculate the energy change for 2H₂ + O₂ → 2H₂O.
An element has two isotopes: mass 63 (69%) and mass 65 (31%). Calculate its relative atomic mass.
Explain why the noble gases are unreactive.
Compare the structures and properties of diamond and graphite.
Calculate the relative formula mass (Mr) of Al₂(SO₄)₃. (Relative atomic masses: Al = 27, S = 32, O = 16)
Describe an investigation to place four metals in order of reactivity using dilute acid.
Write the ionic equation for neutralisation.
In the electrolysis of aluminium oxide, the positive electrodes must be replaced regularly. Explain why.
Sketch and describe a reaction profile for an exothermic reaction.
Finished?
Answer every question to finish (32 left), or finish when the time’s up.
Score 0 / 100 · 0 of 32 marked
This paper is written by Plasmo in the style of the AQA GCSE Chemistry exam. It is not a past paper and is not produced or endorsed by the exam board.