C5 Chemical Changes 5.0 / 5 based on 1 rating ? ChemistryChemical patterns and reactivity seriesGCSEAQA Created by: FannonCreated on: 10-11-16 19:38 What is an ore? An ore is a rock from which it is economical to extract the metals that they contain. 1 of 36 What is the meaning of oxidisation in terms if oxygen? To have oxygen added. 2 of 36 How must metals be extracted from their oxides? By reducing them. 3 of 36 What is the reactivity series? A list of metals in order of their reactivity. 4 of 36 Do most metals act vigorously with water? No 5 of 36 Why can copper be used in water pipes? It does not react with water. 6 of 36 Why do you use dilute acids to order reactivity? Reactions with water are too slow. 7 of 36 What makes aluminium different from other metals? It is protected by a layer of aluminium oxide so while it is a fairly reactive metal it can be used outside without corrosion. 8 of 36 What is the general equation for metal and water? Metal + Water --> Metal Hydroxide + Hydrogen 9 of 36 What is the general equation for metal and acid? Metal + Acid --> Salt + Hydrogen 10 of 36 How can you tell if a chemical reaction has taken place? Colour change, Bubbles of gas, Solid formed 11 of 36 Why can gold, silver and platinum be used in jewellery? They are unreactive 12 of 36 Why are potassium, lithium and sodium stored in jars of oil? They would react with the oxygen in the air. 13 of 36 Why are food cans plated with tin and not zinc? Tin is less reactive than zinc. 14 of 36 How else can you judge reactivity? Putting the metals in competition with each other. 15 of 36 Why does magnesium replace copper from its salt? It is more reactive. 16 of 36 What is the reaction called when a more reactive metal replaces a less reactive metal from its salt? A displacement reaction 17 of 36 What is an ionic equation? An equation that only shows the atoms/ions that change in thereaction. 18 of 36 What would you use the placement of hydrogen in the reactivity series for? To predict whether a metal would react with an acid. 19 of 36 What is the use of carbon in the reactivity series? It can displace metals from their ores. 20 of 36 What is the wider definition of oxidation? The loss of electrons. 21 of 36 What is the wider definition of reduction? The gain of electrons. 22 of 36 What is a half equation used for? To show what happens to each reactant. 23 of 36 Why can't Tungsten Oxide be reduced with carbon? It would form tungsten carbide. 24 of 36 How are metals that are more reactive than carbon extracted? Electrolysis of the molten metal compound. 25 of 36 What is a salt? The compund formed when the hydrogen in an acid if wholly or partially replaced by metal or ammonium ions. 26 of 36 What is a base? A compund that can neutralise an acid. 27 of 36 What differs a base from an alkali? An alkali is a soluble base. 28 of 36 What is the general equation for a neutralisation reaction? acid + base --> a salt + water 29 of 36 How can you make ammonium salts? By reacting an acid with ammonia and water 30 of 36 How would you make a pure, dry salt when reacting an acid and alkali? Doing a titraton 31 of 36 What is the general equation for an acid and metal carbonate? acid + carbonate --> salt + water + carbon dioxide 32 of 36 What is a soluble hydroxide called? An alkali 33 of 36 What must happen for an acid to show its properties? It must dissolve first in water. 34 of 36 What happens to acids in water? They ionise 35 of 36 What is the difference in ionisation in strong and weak acids? Strong acids ionise completely 36 of 36
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