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Group 2, the alkaline earth metals
This topic links Group 2 reactivity and solubility trends to practical applications.
7
Objectives
10
Flashcards
10
Questions
90 min
Study time
AqaA LevelChemistryInorganic chemistry
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Syllabus checklist
What you need to know
7 objective pages available
Group 2 trends and reactions4 objectives
- Explain trends in atomic radius and first ionisation energy down Group 2.
- Describe reactions of Group 2 metals with oxygen, water and acids.
- Explain the trend in reactivity down Group 2.
- Explain trends in solubility of Group 2 hydroxides and sulfates.
Group 2 applications3 objectives
- Explain why barium sulfate can be used in medicine despite barium compounds often being toxic.
- Explain uses of magnesium hydroxide and calcium carbonate in neutralising acidity.
- Link Group 2 solubility trends to applications.
Key terms
Atomic radiusIonisation energyAlkaline Earth MetalsHydroxideIonization EnergyLattice enthalpyHydration enthalpyInsolubleRadiocontrast agentNeutralizationpHLattice energy
Exam tips
- Use diagrams to illustrate trends: When explaining trends, consider drawing a simple diagram to show atomic structure changes.
- Use clear and precise chemical notation: When writing equations, ensure that all reactants and products are correctly represented with their chemical formulas.
Common mistakes
- Confusing atomic radius with ionic radius: Remember that atomic radius refers to neutral atoms, while ionic radius refers to charged ions.
- Incorrect balancing of equations: Always check that the number of each type of atom is the same on both sides of the equation.
Practice preview
- Which of the following statements correctly describes the trend in atomic radius as you move down Group 2?
- Explain why the first ionisation energy decreases as you move down Group 2.
- Magnesium has a first ionisation energy of 738 kJ/mol, while barium has a first ionisation energy of 503 kJ/mol. Calculate the percentage decrease in first ionisation energy from magnesium to barium.
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