The Reactivity Series This is to help you write your notes

1. The Reactivity SeriesThis is to help you write your notes

2. The Reactivity Series What are put into order of reactivity in this series? Explain in your own words what you understand by the word 'reactivity' Explain where the most reactive elements are in the series (top or bottom)

3. The Reactivity Series Reactive metals are always found naturally as compounds. Think about extracting a reactive metal from its compound. Would it need more or less energy than the extraction of a less reactive metal from its compound? Explain your ideas Most Reactive metal Compounds very stable relative to the metal Difficult to extract metal from its compounds Metals easy to extract from compounds Compounds less stable relative to the metal Least Reactive metal

4. Group 1– The alkali metals

5. Alkali Metals • Group 1 are always found naturally as compounds – why do you think this is? Explain how these metals are stored in the laboratory and why. Which reactions do we do in the lab to show how reactive these metals are? Which reactions are too dangerous to do?

6. Alkali Metals • Discuss their reactions with cold water Write balanced equations including state symbols for potassium, sodium and lithium Key words to use: flame, ignite, lilac, melt, alkali, fizzing, float,

7. Alkali Metals The resulting solution is an alkali. This is because sodium hydroxide forms and the ______________ ion makes the solution an alkali. • Group 1 metals increase in their reactivity, or tendency to combine with other substances, as you move from top to bottom. Explain this trend. Remember the relationship between an alkali and a base?

8. Alkali Metals • Make some predictions for Rubidium How vigorously will it react with water compared to potassium Will it have a higher or lower melting point than sodium Why does it not float on water? What would an equation for the reaction of rubidium with water be?

9. Alkali Metals • React with other non-metals to form compounds 4Na(s) + O2(g) 2Na2O(s) Orange flame? 2Na(s) + Cl2(g) 2NaCl(s) What type of bonding is present in sodium oxide and sodium chloride? What colour would you expect these solids to be?

10. Potassium + water potassium hydroxide + hydrogen 2K(s) + 2H2O(l) 2KOH(aq) + H2(g) Group 1 – The alkali metals Summary of facts… 1) These metals all have ___ electron in their outer shell 2) Reactivity increases as you go _______ the group. This is because the electrons are further away from the _______ every time a _____ is added, so they are given up more easily. 3) They all react with water to form an alkali (hence their name) and __________, e.g: Words – down, one, shell, hydrogen, nucleus

11. Group 2 The Alkaline Earth Metals Are these metals more or less reactive than the Group 1 metal which is in the same period? Why is it important to compare metals in the same period?

12. Alkaline Earth Metals Calcium and cold water Does it react, what are the observations and balanced chemical equation? Magnesium reacts extremely slowly with cold water. Is magnesium more or less reactive than calcium? Is the trend in reactivity down Group 2 the same as Group 1?

13. Alkaline Earth Metals This equipment is used for the reaction of several metals with steam. Magnesium is one of them, can you name some of teh others? Mg(s) + H2O(g)MgO(s) + H2(g) For all metals which react with steam, the oxide is produced NOT the hydroxide. This is because the hydroxides are not thermally stable. Write the equation for two other metals which react with steam but not cold water

14. Rearrange the boxes in the following table so the summary chart for the reactions of the metals with oxygen, water and acid is correct: