Reactivity Series of Metals

1. Reactivity Series of Metals Reactions of Metals Effect of Heat on Metal Carbonates

2. Chemical Properties of Metals • Metal reaction with cold water & steam • Metal reaction with hydrochloric acid • Reaction of Metals: Displacement Reactions • With aqueous ions of another metal • With the oxide of another metal • Reaction of Metal Oxides • With carbon • With hydrogen • Effect of Heat on Metal Carbonates • Thermal stability & reactivity Reactivity Series of Metals

3. Reaction with Water (Cold Water) Metal + Cold Water Metal Hydroxide + Hydrogen Gas Eg. 2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g) Which are some metals that react with cold water? Recap: Chemical Properties of Metals

4. Reaction with Water (Steam) Metal + Steam Metal Oxide + Hydrogen Gas Eg. Mg(s) + H2O(g)  MgO(s) + H2(g) Which metals only react with steam? Recap: Chemical Properties of Metals

5. Reaction with Hydrochloric Acid Metal + Hydrochloric Acid  Salt + Hydrogen Gas Eg. 2K(s) + 2HCl(l)  2KCl(aq) + H2(g) The more vigorous the reaction The higher it is in the reactivity series The more reactive is the metal Recap: Chemical Properties of Metals

6. Displacement of metals from solution • More reactive metals can displace less reactive metals from their salt solutions. • This can be used to find the position of metals in the reactivity series. Reaction of Metals With the Aqueous Ions of Another Metal

7. Iron Nail in Copper(II) Sulphate Solution Copper(II) Sulphate Solution Iron(II) Sulphate Solution Iron Copper Observations: Reddish-brown solid forms on the surface of the iron nail Blue solution becomes pale green Fe (s) + CuSO4 (aq)  FeSO4 (aq)+ Cu (s)

8. Brown solid: Copper metal • Solution turns pale green • Copper has been removed from the solution. • Iron(II) sulphate solution is pale green in colour. We say that… Iron has displaced copper from the copper(II) sulphate solution. Iron Nail in Copper(II) Sulphate Solution

9. What will happen when a piece of magnesium strip is immersed in a solution of copper(II) sulphate? Think!

10. Deposit of the more reactive metal (from its aqueous solution) • Colour of the solution may change • Heat may be given off Some Possible Observations

11. Iron atoms are oxidized to become iron(II) ions The more reactive metal is oxidized The less reactive metal is reduced For example, Chemical Equation: Fe (s) + CuSO4 (aq) FeSO4 (aq) + Cu (s) Ionic Equation: Fe (s) + Cu2+(aq) Fe2+ (aq) + Cu (s) REDOX reaction! Copper(II) ions are reduced to become copper atoms Displacement Reactions are Redox Reactions

12. A more reactive metal: • readily gives up electrons in reactions • has greater tendency to form positive ions As a result… A more reactive metal can displace a less reactive metal, from its solution or metallic oxide. Displacement Reactions are Redox Reactions

13. Displacement of metals from metallic oxides • A more reactive metal can reduce the oxide of a less reactive metal. • For example: Thermit reaction 2Al (s) + Fe2O3 (s) Al2O3 (s)+ 2Fe (l) Reaction of Metals With the Oxide of Another Metal

14. Iron(III) ions are reduced to become iron atoms • Thermit Reaction 2Al (s) + Fe2O3 (s) Al2O3 (s)+ 2Fe (l) • The more reactive the metal is, the more readily it forms compounds. • Unreactive metals tend to stay umcombined. Aluminium atoms are oxidized to become aluminium(III) ions Reaction of Metals With the Oxide of Another Metal

15. Reaction of Metal Oxides With Carbon • Carbon can remove oxygen from the oxides of metals that are not too high up in the Reactivity Series. The lower the position of a metal in the Reactivity Series, the easier it is for carbon to remove oxygen from the metal oxide.

16. Reaction of Metal Oxides With Carbon

17. metals need to be extracted from their ores before we can use them metals below magnesium are often extracted from their ores by reduction with carbon (WHY?) metals above zinc cannot be extracted by reduction with carbon bc they are stable (THEN WHAT?) The Importance! Reaction of Metal Oxides With Carbon

18. Reaction of Metal Oxides With Hydrogen • Hydrogen can remove oxygen from metallic oxides, producing the metal and water(steam). metal oxide + hydrogen  metal + steam The lower the position of a metal in the Reactivity Series, the easier it is for hydrogen to remove oxygen from the metal oxide.

19. Reaction of Metal Oxides With Hydrogen

20. Most carbonates decompose when heated strongly to produce a metal oxide and carbon dioxide gas. • The ease of decomposition depends on the position of the metal in the reactivity series. Recall the reactivity series. Effect of Heat on Metal Carbonates:Thermal Stability & Reactivity

21.  Metal Metal Oxide + Carbon Dioxide Thermal Stability of Metal Carbonates

22. Reactions with water & dilute acids: More vigorous reaction  Higher in the reactivity series  The metal is more reactive • Reaction with metal carbonates: The more stable the metal carbonate is to heat, the higher it is in the reactivity series.

23. Check this out! http://www.chem.iastate.edu/group/Greenbowe/sections/projectfolder/flashfiles/redox/home.html Class Activity & Discussion

24. Displacement Reaction • They are redox reactions. • A more reactive metal can displace a less reactive metal, from its solution or metallic oxide. • Carbonates: Thermal stability & reactivity The more stable the metal carbonate is to heat, the higher it is in the reactivity series. So, what have you learnt today?