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29 Cards in this Set
- Front
- Back
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Oxidation (oxygen) |
Gain |
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Reduction (oxygen) |
Loss |
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Redox reaction |
Involves both reduction and oxidation |
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Oxidation (electron) |
Loss of electrons |
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Reduction (electron) |
Gain of electrons |
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Sum of all oxidation numbers |
Zero |
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Oxidation number of fluorine |
-1 |
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Oxidation number of oxygen |
-2 unless combined with fluorine +2 |
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Oxidation number of hydrogen |
+1 |
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Why do group 1 and 2 need to be kept away from oxygen |
Form oxides as surface layers appearing dull |
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Metallic radius |
Increases down |
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Ionisation energy |
Decreases down as bigger radius as more shells are added and outer electrons are further away from the nucleus therefore reducing attraction to nucleus |
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Group 1 and 2 metals heated |
Burn vigorously |
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Reactions with Cl |
Combine when heated in Cl gas More vigorous down group |
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Reactions with water |
Mg doesn’t Strontium and barium react Activity increases down the group increases effervescence |
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Metal + water |
Metal hydroxide + hydrogen |
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Mg and steam |
Forms mg oxide white solid and H+ gas in vigorous reaction |
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Reactions with calcium |
Calcium hydroxide goes cloudy as a precipitate of calcium hydroxide is formed |
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Reactions with barium |
Soluble in water |
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Magnesium and steam |
Heated in steam forms magnesium (white solid) and hydrogen gas |
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Beryllium and radium |
Increasing activity down group therefore beryllium less reactive than radium |
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Reaction of oxides in water |
Group 1 and 2 classed as basic oxides meaning they can react with water to form alkalis Solids react to form colourless solution |
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Trend in solubility of group 2 hydroxides |
PH value of alkaline solution formed depends on amounts of oxides and water (affected by differences in the solubility of the hydroxides) |
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Solubility increases or decreases down group |
Increases |
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Equation for testing carbon dioxide |
Calcium carbonate ——> calcium oxide + CO2 (thermal decomposition) |
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Reactions of the oxides and hydroxides with acids |
All group one and two oxides and hydroxides react with acids to form salts and water White solid reacts to form colourless solution |
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Use of lime in agriculture |
Used to control soil acidity greater yield of crops obtained Lime is calcium hydroxide obtained from limestone |
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Trends in solubility of group 2 sulfates |
All group 2 nitrates and and chlorides are soluble Solubility of group 2 sulfates decreases down |
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Testing for sulfate ions |
Adding barium chloride or barium nitrate forms white precipitate of barium sulfate Dilute nitric acid or hcl also added |
