12. Dip small, clean pieces of Al, Zn, Fe and Cu metal in test tubes A, B, C and D respectively. This series of simple experiments illustrates some of the chemical properties of the halogens following an introduction to the physical properties of the Group 17 elements. Questions based on Procedural and Manipulative Skills Answer: Dip small, clean pieces of Al, Zn, Fe and Cu metal in test tube A, B, C and D respectively. 18. Answer: (a) all the four solutions changed. Answer: (a) This will show displacement reaction. (d) light green solution changes to blue. Name any two metals that are more reactive than iron. Question 10: What is your observation when copper is added in iron (II) sulphate solution? Due to the displacement reaction the blue colour of copper sulphate changes to green colour of iron sulphate. IV. Conclusion: Al metal is not displaced by any of the given metals i.e. II. A more reactive metal can displace a less reactive metal from its salt solution or compounds. Students work in Wash your hands properly after the experiment. Chlorine is more reactive than iodine and hence it displaces iodide ion. 4. (a) prepare copper sulphate solution and dip a zinc strip in it. The water droplets are collected on the inner part of the test tube. 30. (a) copper and zinc > Reactivity series: The arrangement of metals in decreasing order of their reactivity is called reactivity series. Watch this video to show you how to work out the reactivity Series of the metals. (a) I and II (b) I and III A student took four test tubes containing solutions of different colours marked I, II, III, and IV as shown below. Two metals which can displace iron from its solution are: (a) the green solution slowly turns blue. Green iron II sulphate is formed. (d) Cu is the least reactive metal and can be displaced by all the metals given. Observe the changes and record your observations. Precautions Metal A is more reactive than B, because metal A displaces metal B from its salt solution. The colour of the solution changed from: The colour of copper sulphate solution is blue. (b) The final solution becomes colourless. > Reaction with Al2(SO4)3 solution: A student took Cu, Fe, Zn and Al strips separately in four test tubes labelled I, II, III and IV respectively. When we add Fe in FeSO4 solution, no change is seen. (d) add dilute nitric acid on both the strips. Hence, the blue colour of copper sulphate solution becomes colourless. Name some metals that will react with aluminium sulphate solution, i.e., Al2(SO4)3. Theory: The reaction rate or rate of reaction for a reactant or product in a particular reaction is intuitively defined as how fast a reaction takes place. (d) R displaces Q. (d) zinc and aluminium. Answer: Aim In the beaker A is placed a small piece of copper and in the beaker B is placed a small piece of zinc. The blue colour of the crystals is due to these five water molecules. Conclusion: Al, Zn and Fe metals are more reactive than Cu. Overview: The students will develop their own activity series of metals based on lab results. Take test tubes A, B, C, and D, clean them. Procedure (d) A brown mass is deposited on the surface of aluminium. Answer: 21. (a) light green to blue Reactivity Series, Redox Reactions and Extraction of Metals. Specified practical – metal displacement reactions Displacement in solutions There are a number of ways that you could investigate a displacement rractivity. 1. Question 1: 9. (c) I and II (d) III and IV. Aim To observe the action of Zn, Fe, Cu and Al metals on the following salt solutions: ZnSO 4 (aq), FeSO 4 (aq), CuSO 4 (aq), Al 2 (SO 4) 3 (aq) To arrange Zn, Fe, Cu and Al metals in the decreasing order of reactivity based on the above results. (a) it is cooled (c) heat zinc and copper strips. Reactivity Series Of Metals Class 10 Introduction (ii) Salt solution FeSO4. Metal + Acid —> Metal salt + Hydrogen. In order of reactivity the reactivity series shows metals. 29. Developing the Activity Series. (a) white > Hence the displacement reaction is used to arrange the metals in the reactivity series. Questions based on Reporting and Interpretation Skills, 28. When iron nail is dipped in this solution, reaction takes place and blue colour disappears and turns greenish and the iron metal gets coated with pink-brown copper metal. (c) the copper strip became thicker Hypothesis. (d) Iron is less reactive than Zn. Add ZnSO4 solution in each test tube. Aluminium is more reactive than Fe hence it displaces Fe from FeS04 and green colour of FeSO4 disappears. (c) red and greenish-blue > The arrangement of metals in decreasing order of their reactivity is called reactivity series or activity series of metals. Question 3: Pour equal amount of their aqueous solutions into the respective test tubes. What metal is the least reactive? (d) Heat increases the rate of reaction. Question 2: Reactivity of elements Each group recorded the observations as [ given below in the table. > In displacement reactions, the metals compete for the non-metal anion. Which one of the two metals is more reactive? 27. 2. (d) heat iron and add in copper sulphate. (d) Test tube with FeSO4 solution. In one molecule of copper sulphate, five water molecules are present to form crystal. (b) It shows thermite reaction and heat is evolved. (a) I and III (b) II and IV (c) heat the container of reactants 1. Metals can be arranged on the basis of relative reactivity. Hence, the reactivity order is Al > Zn. Question 6: Answer: When a few crystals of copper sulphate are dissolved Iron spoon was placed in a glass container holding zinc sulphate solution. Which one is not observed when aluminium is added to a solution of copper sulphate? (b) Fe is less reactive than Al but more reactive than Cu. Complete the given chemical equation Fe(s) + CuSO4(aq) —> 29. (b) blue to colourless The reactivity series is the arrangement of elements according to their reactivity. (c) it is kept undisturbed Which of the following reaction will take place? (a) Q displaces P Why did the colour of copper (II) sulphate solution, change, when zinc metal was dipped in it? Why is Fe metal more reactive than copper metal? (d) Mg + ZnSO4. What happens when Fe (Iron) metal is added to blue colour copper sulphate solution? > Metals: The atoms of metal will always lose electrons to form positive ions called cations. Copper turnings were added to colourless salt solution. They recorded their observations in the form of table given below: Which student noted the colour change in all the four test tubes correctly? (d) colourless. solution, the time required for the colour of the solution to change from blue to green will be less if: Students should learn about the reactions of metals and are expected to be able to place metals in order of reactivity based on simple experiments such as the reactions of metals with water and acids and also displacement reactions between metals and solutions containing the ions of other metals. Question 6: Practical work: establish the reactivity order for lithium, magnesium and calcium by reacting similar size pieces with cold water. 14. When this layer is removed, the observations are more reliable. zinc rod in each solution and leaving it undisturbed for two hours, they noted the colour of each solution again. (a) add Zn in test tube A and B After 10 minutes it was observed that the colourless solution turned to a coloured solution and a shiny metal deposition appears. Non-metals in the reactivity series It is useful to place carbon and hydrogen into the reactivity series because these elements can be used to extract metals. A piece of granulated zinc was dropped into copper sulphate solution. The elements at the top can displace elements below them from their compounds. (a) blue to pale green (b) blue to dark green (c) blue to colourless (d) blue to reddish-brown. 20. Add Al2(SO4)3 solution in each test tube. Hence, Cu is the least reactive metal among the given four metals. How can you test that a given sample contains water or not? The resource is set out as teachers' notes followed by the students' page which presents the task to be investigated. (c) II and III (d) III and IV. Question 6: (c) I, II, III (d) II, III, IV. (c) yellow Answer: Hydrogen which is a non-metal is also placed in reactivity series. (d) Fe will displace Cu ions to give green colour solution and Cu metal is brown coated. (c) As per reactivity series. 3. It will help you understand the reaction of metals such as zinc, aluminium, copper, and iron with aqueous salt solutions of aluminium sulphate, copper sulphate, ferrous sulphate, and zinc sulphate. (b) green 15. Answer: (c) Iron spoon will get holes in it. On observing the strip the next day, it was noticed that 1. > Reaction of Metals with Salt Solution Al2(SO4)3 solution in each test tube. After some time, the colour of the solution changed from Answer: Conclusion: Al and Zn metals are more reactive than Fe and Cu. 8. Question 4: (d) Zn and Al are more reactive than Fe and can displace it. 28. (d) Zinc salt solutions are colourless. 24. (c) P displaces Q (c) smooth and shining Metals which lie above hydrogen in reactivity series are more reactive than hydrogen. What will happen if Fe metal is added to ZnSO4 solution? In this experiment, a strip of metal is added to a solution of a compound of another metal. Question 12: 2. (c) white (d) green. (b) zinc and tin Question 9: (d) Copper is more reactive than Ag. (c) Equilibrium is seen. The decreasing order of reactivity for these metals follow the order: Observe the changes carefully as few reactions may occur slowly. 2. each of four test tubes. When you keep aluminium strip in FeSO4 solution, what change is seen? 3. Answer: These displacement reactions are used to establish an order of reactivity down Group 17 of the periodic table. (a) Test tube with CuSO4 solution Al > Zn > Fe > Cu. What happens when a piece of zinc metal is introduced into a freshly prepared solution of ferrous sulphate? > If a less reactive metal is added to a more reactive metal salt solution then there will be no reaction. Question 5: The right pair of metals forming the precipitates is Tie-ins include single-replacement reactions (SRR), oxidation-reduction, practical applications such as galvanization, and predicting reactions. Use very small pieces of metal every time. 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