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20 Cards in this Set
- Front
- Back
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What happens to the atomic radii of the elements as you go down group two? |
It increases |
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State and explain what happens to the first ionisation energy as you go down group two |
It decreases due to extra shielding from additional electron shells and the greater distance between the nucleus and outer shell causing the electrons to be less attracted to the nucleus so less energy is needed to remove them |
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State and explain what happens to the reactivity as you go down group two |
It increases due to lower ionisation energies as you go down the group so electrons can easily be lost |
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State and explain what happens to the melting points of the elements as you go down group two |
They decrease due to bigger metal ions with the same number of delocalised electrons per ion so outer electrons are less attracted to the nucleus meaning less energy is required to overcome this attraction |
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State the equation for calcium reacting with water and state the type of reaction taking place |
Ca + 2H2O → Ca(OH)2 + H2 Oxidation |
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Why does magnesium have a much lower melting point than the other group two elements |
The arrangement of the metallic ions changes |
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Describe how the solubility of the group two elements changes down the group when bonded to singly charged negative ions
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Solubility increases down the group magnesium hydroxide is sparingly soluble barium hydroxide is most soluble |
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Describe how the solubility of the group two elements changes down the group when bonded to doubly charged negative ions
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Solubility decreases down the group magnesium sulphate is soluble barium sulphate is insoluble |
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Describe how you would test for sulphate ions using barium chloride and state what you would observe |
Acidify the solution with hydrochloric acid to get rid of unwanted sulphate or carbonate ions that will cause a false positive result add barium chlorate to the sample solution a white precipitate of barium sulphate will form |
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Why would you not use sulphuric acid to remove unwanted ions when testing for sulphate ions?
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The sulphur would react with barium and form a white precipitate of barium sulphate, causing a false positive result |
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State the ionic equation for the reaction between barium ions and sulphate ions
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Ba²⁺+ SO4²⁻→BaSO4 |
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State the ionic equation for the neutralisation of an acid
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H⁺ + OH⁻→H2O |
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State a use of magnesium hydroxide
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Antacids (neutalising excess stomach acid) |
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State a use of calcium hydroxide
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Neutralising acidic soil |
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Explain why barium sulphate is used in barium meals |
It is opaque in x-ray scans so it can be used by doctors to check for problems in the digestive system |
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Barium is a toxic chemical, why can it be used in barium meals? |
It is insoluble so it can't damage tissues |
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Describe how magnesium is used in the extraction of titanium |
The titanium (IV) oxide ore is heated with carbon in a stream of chlorine gas converting it to titanium (IV) chloride then it is purified by fractional distillation and reduced by magnesium in a furnace at 1000°C |
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Describe how calcium oxide and calcium carbonate remove sulphur dioxide from flue gasses |
Calcium oxide or calcium carbonate are mixed with water to form a slurry the slurry is sprayed onto the flue gasses sulphur dioxide reacts with the alkaline slurry and produces solid calcium sulphite |
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State the equation for the extraction of titanium |
TiCl4 + 2Mg → Ti + 2MgCl2 |
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State the equations for the reaction of calcium oxide reacting with sulphur dioxide and calcium carbonate reacting with sulphur dioxide |
CaO + H2O + SO2 → CaSO3 + H2O CaCO3 + H2O + SO2 → CaSO3 + CO2 + H2O |
