Lesson 3.2.2

3.2.2 Group 2, the alkaline earth metals Quiz: AQA Chemistry, Unit 2

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 3.2.2, Group 2, the alkaline earth metals: 20 multiple choice questions for the AQA Chemistry (7405), Unit 2: Inorganic chemistry, written with Revision Ninja.

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The 20 questions

  1. What is the name for the Group 2 elements?

    • Halogens of Group 7
    • Noble gases of Group 18
    • Alkaline earth metals
    • Alkali metals of Group 1

  2. What is the typical product when calcium reacts with cold water?

    • Calcium chloride and oxygen gas
    • Calcium oxide and hydrogen gas
    • Calcium hydroxide and hydrogen gas
    • Calcium carbonate and water

  3. Which Group 2 metal reacts most vigorously with cold water, among Mg, Ca, Sr and Ba?

    • Magnesium
    • Calcium
    • Barium
    • Strontium

  4. What is the product when magnesium reacts with steam?

    • Magnesium hydroxide and oxygen gas
    • Magnesium oxide and hydrogen gas
    • Magnesium carbonate and water
    • Magnesium chloride and hydrogen gas

  5. How does the solubility of the Group 2 hydroxides change down the group?

    • It stays the same for all Group 2 hydroxides
    • It increases, but only for hydroxides that are gases
    • It increases, so barium hydroxide is more soluble than magnesium hydroxide
    • It decreases, so barium hydroxide is less soluble than magnesium hydroxide

  6. How does the solubility of the Group 2 sulfates change down the group?

    • It stays the same, because all Group 2 sulfates dissolve equally well
    • It decreases, but only for sulfates that are gases
    • It increases, so barium sulfate is more soluble than magnesium sulfate
    • It decreases, so barium sulfate is insoluble while magnesium sulfate is soluble

  7. Why is barium sulfate used in medicine?

    • It dissolves completely and releases oxygen, which helps the body absorb nutrients
    • It reacts with stomach acid to produce a neutralising gas that relieves indigestion
    • It is a strong acid, so it is used to treat alkaline conditions in the body
    • It is insoluble and opaque to X-rays, so it can be given safely as a contrast agent

  8. Why is calcium hydroxide used in agriculture?

    • It neutralises acidic soil, raising the pH so that crops grow well
    • It is a fertiliser that supplies calcium as a nutrient in the form of CaCO3
    • It makes the soil more acidic, which helps plants absorb nitrogen
    • It removes all water from the soil, which stops fungal growth

  9. Why is magnesium used in the extraction of titanium from TiCl4?

    • Magnesium acts as a catalyst, so titanium is formed without any change in the magnesium
    • Magnesium reduces TiCl4 to titanium, forming magnesium chloride as a by-product
    • Magnesium oxidises titanium to a soluble salt, which can then be separated from the mixture
    • Magnesium dissolves in TiCl4 to make an alloy, which is then heated to release titanium

  10. Why is acidified barium chloride solution used to test for sulfate ions?

    • Barium ions form a white precipitate of barium sulfate with sulfate ions, and acidifying removes other ions that would also precipitate
    • Acid is added to dissolve any sulfate present, so that the barium chloride can then react with the dissolved sulfate
    • Barium chloride reacts with the acid to release hydrogen gas, which bubbles off and shows that sulfate is present
    • Barium chloride turns the solution red in the presence of sulfate ions, which shows clearly that sulfate is present

  11. What is the ionic equation for the reaction that forms the precipitate in the sulfate test?

    • Ba^2+(aq) + 2Cl^-(aq) -> BaCl2(s)
    • SO4^2-(aq) + 2H^+(aq) -> H2SO4(aq)
    • Ba^2+(aq) + SO4^2-(aq) -> BaSO4(s)
    • BaSO4(s) + 2H^+(aq) -> Ba^2+(aq) + H2SO4(aq)

  12. What is observed when sodium hydroxide solution is added to a solution of magnesium chloride?

    • No change is seen, because magnesium chloride does not react with alkali
    • A white precipitate of magnesium hydroxide forms
    • A red solution forms, because magnesium hydroxide is coloured
    • A blue precipitate of copper hydroxide forms

  13. Why does the solubility of Group 2 hydroxides increase down the group?

    • Hydration enthalpy falls faster than lattice enthalpy, so the hydroxides dissolve less easily
    • Lattice enthalpy rises as the ions get larger, so the solids are more stable
    • The hydroxides become covalent down the group, so they dissolve more readily in water
    • Lattice enthalpy falls faster than hydration enthalpy as the ions get larger, making dissolving more favourable

  14. Why does reactivity of Group 2 metals with water increase down the group?

    • The number of outer electrons falls, so the metals lose them more readily
    • The first ionisation energy falls, so the outer electrons are lost more easily
    • The atoms become smaller, so they can reach the water molecules more easily
    • The first ionisation energy rises, so the outer electrons are lost more easily

  15. A solution of magnesium chloride is treated with excess sodium hydroxide, forming a white precipitate. What happens if more sodium hydroxide is added?

    • The precipitate dissolves completely, forming a colourless solution of magnesium complex
    • The precipitate turns to a gas, which bubbles out of the solution
    • The white precipitate remains, because magnesium hydroxide does not dissolve in excess NaOH
    • The precipitate turns blue, showing that a new hydroxide has formed

  16. Why is barium sulfate not dissolved by the acid used in the sulfate test?

    • It reacts with acid to form barium chloride, which is colourless and clear
    • It is insoluble in acid, so it remains as a white precipitate
    • It is a gas, so it escapes from the acid as bubbles
    • It reacts with acid to give a soluble salt, so it dissolves completely

  17. Which Group 2 element is least reactive with water?

    • Strontium, which reacts most vigorously with steam
    • Magnesium, which reacts only slowly with cold water
    • Calcium, which does not react with water at all
    • Barium, which reacts most vigorously with cold water

  18. What is the product when barium reacts with cold water?

    • Barium hydroxide and hydrogen gas
    • Barium chloride and hydrogen gas
    • Barium oxide and oxygen gas
    • Barium sulfate and water

  19. Which Group 2 hydroxide is only sparingly soluble and is used in medicine as an antacid?

    • Calcium hydroxide, used to neutralise acid in the stomach
    • Barium hydroxide
    • Magnesium hydroxide
    • Strontium hydroxide

  20. Why is calcium oxide or calcium carbonate used to remove sulfur dioxide from flue gases?

    • They dissolve the SO2 to form a clear gas that can then be released safely
    • They react with SO2 to form barium sulfate, which is then burnt in the furnace
    • They convert SO2 into oxygen gas, which is harmless to the atmosphere
    • They react with the acidic SO2 to form calcium sulfite or sulfate, which removes it from the gas

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