Inorganic Chemistry and the Periodic Table
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4.1 Group 2: ionisation energy and reactivity
Group 2 atoms lose their two outer s electrons to form M2+ ions.
First ionisation energy decreases down the group: the outer electrons are in shells further from the nucleus, with more shielding, so they are held less strongly. This outweighs the rise in nuclear charge.
So reactivity increases down the group: the electrons are lost more easily.
Atomic radius increases down the group because each element has an extra shell of electrons.
Check yourself: Why does the first ionisation energy fall down Group 2?
Outer electron further from the nucleus with more shielding, so less strongly attracted
4.2 Reactions of the Group 2 elements and compounds
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4.3 Solubility of hydroxides and sulfates
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4.4 Thermal stability of nitrates and carbonates
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4.5 Flame colours
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4.6 Group 7: physical properties
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4.7 Reactivity and displacement reactions
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4.8 Redox reactions of the halogens
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4.9 Halides with concentrated sulfuric acid
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4.10 Silver halides and the hydrogen halides
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4.11 Predicting fluorine and astatine
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4.12 Tests for ions
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Extra worked questions
Cover the solution, answer on paper, then mark yourself against each step. Each step shows the mark it earns.
All 8 worked solutions are free for members. The first one is open to everyone.
Magnesium with water and steam
Write equations for the reaction of magnesium with (a) cold water and (b) steam.
Try it first, then show the worked solution
| (a) | Mg + 2H2O → Mg(OH)2 + H2 (very slow) | 1 |
|---|---|---|
| (b) | Mg + H2O → MgO + H2 | 1 |
Answer: (a) hydroxide + hydrogen (b) oxide + hydrogen
Examiner tip: Steam gives the oxide, not the hydroxide. This switch is tested often.
Reactivity down Group 2
Explain why barium is more reactive than magnesium.
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Flame tests
Two white powders are known to be calcium chloride and barium chloride. Describe how a flame test would tell them apart, and explain why a colour is produced.
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Heating nitrates
(a) Write equations for the thermal decomposition of magnesium nitrate and of sodium nitrate. (b) Explain why magnesium nitrate decomposes at a lower temperature than barium nitrate.
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Chlorine and potassium bromide
Chlorine water is added to potassium bromide solution. Describe what you see, write the ionic equation, and explain why bromine water does not react with potassium chloride.
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Sodium bromide and sulfuric acid
Concentrated sulfuric acid is added to solid sodium bromide. Give two observations, write equations for the two reactions, and state the role of bromide ions in the second.
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Predicting astatine
Predict, with reasons, (a) the state of astatine at room temperature, (b) whether astatine would displace iodine from potassium iodide, and (c) the result of adding acidified silver nitrate to sodium astatide solution.
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Identify the white solid
A white solid, Z, dissolves in water. With sodium hydroxide solution, a white precipitate forms that does not dissolve in excess. With dilute HCl and then barium chloride, a white precipitate forms. Acidified silver nitrate gives no precipitate. Identify Z and write ionic equations for both precipitates.
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Video walkthroughs
Narrated walkthroughs of exam-style questions from this topic of the book, showing where each mark comes from. Try the question first, then watch. Captions are available in the player.
Chlorine and sodium hydroxide
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Thermal decomposition of nitrates
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Sulfuric acid with bromide and iodide
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Predicting the chemistry of astatine
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Recall cards
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