1. Metals- Reactivity series Lesson 13

2. Lesson objectives using competition in metals, place reactive metals in order of reactivity (9Fd p.74-8) describe how reactive metals (group 1 and 2) are extracted from their compounds (9Fb p.71)

3. Reactivity series Scientists agree to order metals from the most reactive to the least reactive The criteria used is how fast the metal reacts with Oxygen Water Acids

4. Reactivity Patterns

6. Reactivity and chemical reactions A more reactive metal will displace a lesser reactive metal (p.76) Aluminum is more reactive than iron so it displaces it aluminium + iron oxide  aluminium oxide and iron Heat is produced (exothermic) that can melt the iron

7. Copper, Lead and Iron These metal are not very reactive and their bonds with other elements can be broken with Wood and charcoal fires (carbon) Metals with higher reactivity CuSO4 + Fe(II)  Fe (SO4) + Cu

8. Carbon Is not a metal but it is used to extract iron from its ore

9. Where would you put cobalt? Cobalt is made by heating cobalt oxide with either carbon or aluminium It does not react with water It reacts with oxygen at high temperatures It reacts slowly with acids to give off hydrogen

10. Batteries Electricity is created from the movement of electrons created by the different reactivity of metals Simple cells

11. Task 1 Using the reactivity series on page 75 of your textbook predict whether a displacement reaction will occur in the following reactions- complete the products in words and symbols Magnesium + iron chloride  Magnesium + potassium sulphate  Iron + calcium oxide  Zinc and copper nitrate  Copper and silver nitrate 

12. Task 2 Extraction of reactive metals Read page 71 and answer questions 3-5 in your notebook Complete booklet pages on the topic of reactivity WS 58 Reactivity of 5 metals practical lab this week