Chem Metals Worksheet

Topic 17: Metals – The Reactivity Series Date: ………………..…….. For this topic, candidates should be able to:  Describe the general properties of metals as solids having high melting and boiling points, malleable, good conductors of heat and electricity in terms of their structure.  Describe alloys as mixture of a metal with another element, e.g. brass; stainless steel  Identify representations of metals and alloys from diagrams of structures  Explain why alloys have different physical properties to their constituent elements  Place in order of reactivity calcium, copper, (hydrogen), iron, lead, magnesium, potassium, silver, sodium and zinc by reference to o the reactions, if any, of the metals with water, steam and dilute hydrochloric acid, o the reduction, if any, of their oxides by carbon and/or by hydrogen  Describe the reactivity series as related to the tendency of a metal to form its positive ion, illustrated by its reaction with o the aqueous ions of the other listed metals o the oxides of the other listed metals  Deduce the order of reactivity from a given set of experimental results  Describe the action of heat on the carbonates of the listed metals and relate thermal stability to the reactivity series Multiple Choice Questions 1 Brass is an alloy of copper and zinc. Why is brass harder than pure copper? A The zinc atoms form strong covalent bonds with copper atoms. B The zinc atoms prevent layers of copper atoms from slipping over each other easily. C The zinc atoms prevent the ‘sea of electrons’ from moving freely in the lattice. D Zinc atoms have more electrons than copper atoms. ( ) 2 Which of these combinations will not result in a displacement reaction? A magnesium and calcium nitrate solution. B iron and lead(II) nitrate solution. C tin and silver nitrate solution. D zinc and copper(II) nitrate solution. ( ) 3 A student made the following observations in the laboratory: I Metal X did not react with aqueous nitrate solution of Y. II Metal Y dissolved in the aqueous nitrate solution of Z and crystals of Z appeared. III Metal Z did not react with the aqueous nitrate solution of X. The order of increasing reactivity of the three metals would therefore appear to be A Y, X, Z B X, Z, Y C X, Y, Z D Z, X, Y ( ) �

4 Carbon at red heat will remove the oxygen from the oxides of the metals P, Q and R but not from the oxide of metal S. Metal R will remove oxygen from the oxide of P, but not from the oxide of Q. The order of decreasing reactivity of the four metals would be A S, P, R, Q B P, Q, R, S C S, Q, R, P D P, R, Q, S ( ) 5 Which statement about the metals iron, lead and copper is correct? A They react with warm, dilute hydrochloric acid with evolution of hydrogen. B Their sulfates are soluble in water. C All their compounds are coloured. D Their carbonates can all decompose upon heating. ( ) 6 The diagram shows an experiment to produce and collect hydrogen. What is R? A lead B copper(II) oxide C iron D lead(II) oxide ( ) 7 On strong heating, which substance below will produce the highest amount of carbon dioxide in the first few seconds of the reaction? A magnesium carbonate B copper(II) carbonate C potassium carbonate D iron(II) carbonate ( ) 8 A white powder Z turns yellow when heated. When the product is cooled, it turns back to white. What is Z? A magnesium carbonate B lead(II) carbonate C calcium carbonate D zinc carbonate ( ) 9 When an alkali metal reacts with cold water, a colouless solution is formed with the evolution of a colourless gas. What is the pH of the eventual solution and what is the identity of the ga s produced? pH of solution gas evolved A 1 hydrogen B 1 hydrogen C 13 carbon dioxide D 13 carbon dioxide ( ) �

10 Which one of the following oxides will be reduced by hydrogen? A aluminium oxide B copper(II) oxide C zinc oxide D calcium oxide ( ) Structured Questions 1 Write balanced equations, with state symbols, for the following reactions: (a) Action of heat on copper(II) carbonate. …….…………………………….………………………………………………………………...[2] (b) Reduction of zinc oxide by coke. …….…………………………….………………………………………………………………...[2] (c) Reaction of magnesium and steam. …….…………………………….………………………………………………………………...[2] (d) Addition of iron powder into an aqueous solution of copper(II) sulfate. …….…………………………….………………………………………………………………...[2] (e) Reaction between solid calcium oxide and water. …….…………………………….………………………………………………………………...[2] (f) Reaction between solid sodium with water. …….…………………………….………………………………………………………………...[2] 2 Small pieces of each of the follow ing metals were added to cold water and the volume of gas collected in the first two minutes was recorded. metal aluminium barium calcium magnesium potassium volume/ cm3 0 60 25 20 90 (a) (i) What is a metal? ………………………………………………………………………………………………… ……………………………………………………………………………………………...[1] (ii) Use the data provided and arrange the metals in order of decreasing reactivity. ……………………………………………………………………………………………...[1] (b) Write an equation for the reaction between barium and water. …………………………….…………………..…………………………………………………...[1] (c) Describe what you would expect to see when carbon dioxide is passed into the solution from the reaction in (b)? Give a reason for your answer. ………………………..……….…………………...………………………………………………… ……..…………………………….………………………...……………………………………...[2] �

(d) Explain why, although aluminium is a reactive metal, it does not produce any gas in the above reaction. …………………………….……………………………..…………..……………………………… …………………………….………………………………...………..……………………………… ………………………..………….…………………………………..…………………………...[2] 3 You are provided with a list of substances: solid copper(II) sulfate copper wire distilled water powdered zinc chloride zinc powder Describe how you would carry out an experiment to show that zi nc is more reactive than copper. Your answer should include the tests carried out and relevant observations made. …….…………………………….……………………………..…………………………………………… …….…………………………….……………………………..…………………………………………… …….…………………………….………………………………………..………………………………… …….…………………………….…………………………………………………..……………………… ………………………..………….…………………………………………………..…………………...[4] 4 In an experiment, small amounts of three metals were added to three aqueous metal nitrate solutions. The results are shown in the table. aqueous zinc nitrate aqueous X(NO3)2 aqueous copper(II) nitrate zinc green solution fades to colourless and zinc coated with grey solid metal X No reaction was observed copper No reaction was observed (a) Complete the table above. [3] (b) Write an ionic equation, with state symbols, for the reaction between zinc and nitrate of X. ………………………………………………………………..…………………………………...[2] �

(c) Arrange the zinc, metal X and copper in order of reactivity. …………………………….…………..…………………………………………………………..[1] 5 Aluminium is above hydrogen in the reactivity series. The following experiments were set up. (a) Write down the observations you would see in each experiment. …………………………….……………………………..…………..……………………………… …………………………….………………………………...………..……………………………… ………………………..………….…………………………………..…………………………...[2] (b) Explain why the two strips behave differently. …………………………….……………………………..…………..……………………………… …………………………….……………………………..…………..……………………………… …………………………….………………………………...………..……………………………… ………………………..………….…………………………………..…………………………...[2] 6 The diagram show