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Group 2

AQA A Level Chemistry

QuestionAnswer
"Why are elements in Group I (alkali metals) and Group II (alkaline earths) known as s-block elements ? " their highest energy (bonding) electrons are in s orbitals.
Why does atomic radius increase down group 2? "the greater the atomic number the more electrons there are; these go into shells increasingly further from the nucleus
" Why does melting point decrease down group 2? "each atom contributes two electrons to the delocalised cloud, metallic bonding gets weaker due to increased size of ion, Larger ions mean that the electron cloud doesn’t bind them as strongly
" Why does first ionisation energy decrease down group 2? Despite the increasing nuclear charge the values decrease due to the, extra shielding provided by additional filled inner energy levels
Why is the second ionisation energy of Magnesium higher than the first ionisation energy? There are now 12 protons and only 11 electrons. The increased ratio of protons to electrons means that it is harder to pull an electron out
Why is there such a big jump between the 2nd ionisation energy and the 3rd Ionisation energy of Magnesium? Because the electron being removed is from a shell nearer the nucleus; there is less shielding
Write an balanced equation with state symbols for the reaction of Magnesium with steam. "Mg (s) + H2O (g) → MgO (s) + H2 (g)
" Write an balanced equation with state symbols for the reaction of Barium water Ba (s) + 2H2O (l) → Ba(OH)2 (aq) + H2 (g)
What is the trend in solubility of the Group 2 Hydroxides? They get more soluble down the group.
Why do the group 2 metals get more reactive as you go down the group? Reactivity of metals is related to their ionisation energy. The ionisation energies of metals decreases down the group due to increased shielding and increased distance from the nucleus to the outer shell
What is the trend in solubility of the Group 2 Sulphates? They get less soluble down the group.
Why is calcium hydroxide more soluble than magnesium hydroxide and more strongly alkaline? "Lower charge density of the larger Ca2+ ion means that it doesn’t hold onto the OH¯ ions as strongly. More OH¯ get released into the water. It is more soluble and the solution has a larger pH.
" Describe the chemical test for sulfate ions Use barium chloride in the presence of dilute hydrochloric acid. This will produce a white precipitate if sulfate ions are present.
Write an ionic equation with state symbols for the reaction in the sulfate test. Ba2+ (aq) + SO42– (aq) → BaSO4 (s)
Write a balanced equation with state symbols for the combustion of Barium in air. 2Ba (s) + O2 (g) → 2BaO (s)
Write a balanced equation with state symbols for the reaction of calcium with sulfuric acid Ca + H2SO4 →CaSO4 + H2
Write a balanced equation with state symbols for the reaction of strontium with nitric acid Sr + 2HNO3 → Sr(NO3)2 + H2
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