Inorganic 1 Section 2 - Unit 9: Group II metals
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State and explain the trend in atomic radius down Group 2 from Mg to Ba (2 marks)
• Increases - Due to an increase in shells
Give the formula of the hydroxide of the element in Group 2 that is most soluble in water.
• Ba(OH)2
State the trend in reactivity with water of the elements down Group 2 (1 mark)
• Gets more reactive
State the ionic equation, with state symbols, to show the reaction of calcium with an excess of water (1 mark)
Ca(s)+ 2H2O(l) ➡ Ca2+(aq) + 2OH–(aq) + H2(g)
State and explain the trend in the first ionisation energies of the elements in Group 2 (3 marks)
• Decreases • Ions get bigger • Sp weaker attraction of ion to lost electron
Explain why drinking magnesium sulfate solution is effective in the treatment of barium poisoning (1 mark)
• Insoluble barium sulfate is produced
State and explain the trend in melting points of the elements in Group 2 (3 marks)
• Decreases • Metallic bonding weakens • Atomic size increases
Explain how magnesium can be used to extract titanium (6)
• TiO2 (solid) is converted to TiCl4 (liquid) • At 900°C • The TiCl4 is purified by fractional distillation • In an argon atmosphere • The Ti is extracted by Mg • In an argon atmosphere at 500°C
State the ionic equation for the formation of Magnesium Hydroxide with state symbols (1 mark)
Mg2+(aq) + 2OH-(aq) ➡ Mg(OH)2
State and explain the trend in the first ionisation energies of the elements in Group 2 from magnesium to barium (3 marks)
• Decreases • More shells • Weaker attraction of ion to lost electron
State a medical use of barium sulfate and explain why this use of barium sulfate is safe (2 marks)
• Used in a barium meal/to absorb X-Rays - Because it’s insoluble
State the equation for the reaction of magnesium hydroxide with hydrochloric acid (1 mark)
• Mg(OH)2 + 2HCl MgCl2 + 2H2O
Describe briefly how you would carry out the test for bromide ions with silver nitrate, acidified with dilute nitric acid, and another reagent - state what you would observe (3 marks)
• Add silver nitrate, then dilute ammonia • Cream precipitate • Precipitate dissolves slightly in dilute ammonia