1. Metals and non- metals The BasicsReactivity Reactions with metals

2. The Periodic Table is divided into…. Metals

3. and non-metals The Periodic Table is divided into….

4. Metals all have similar physical properties… They have high melting and boiling points (except mercury) They conduct electricity and heat. They have a high density. They are shiny (lustrous). They are malleable (can be moulded) They are ductile (can be stretched)

5. Non-metals…. Have low melting and boiling points. Are brittle. Do not conduct heat or electricity well. (except carbon)

6. Different metals are suitable for different jobs. Gold, silver and platinum are very unreactive but very malleable - making them suitable for jewellery

7. Copper is malleable, ductile and it conducts heat and electricity well. It is also unreactive making it suitable for holding and carrying water.

8. Aluminium is a reactive metal, but it forms a coating of very stable aluminium oxide. This, together with its lightness and malleability gives it many uses from window frames to insulation foil.

9. Iron ore is common and iron itself is very strong. It can be moulded into many shapes

10. Remember: Only iron oxide is called rust. No other metal rusts! Unfortunately iron is quite brittle (for a metal) and also oxidises (rusts) easily. As it forms, iron oxide constantly flakes away exposing more of the iron underneath.

11. Like aluminium, zinc oxidises to form a stable coating of zinc oxide which protects the iron underneath it. This is called galvanising. To prevent this happening, iron is often covered with a thin layer of zinc.

12. Lead is very dense, unreactive and malleable - making it suitable for fishing weights and roof sealing. Lead fumes have been linked to brain damage so it is now considered too toxic to be used inside houses (e.g. as in old-fashioned water pipes) Back

13. Sodium, Calcium and Magnesium These three metals are all far too reactive to be much use in their pure form. They all make important compounds though.

14. Sodium Sodium metal is so reactive it has to be kept in oil to keep it away from the oxygen in the air.. Without the oil, sodium quickly oxides into useless sodium oxide All the same, sodium is essential for both plants and animals. The commonest source of sodium is common table salt – Sodium Chloride.

15. Calcium Calcium is less reactive than sodium, but it still oxidises too rapidly for the pure metal to have any uses. Calcium compounds, however, are very important. Calcium carbonate makes up about 10% of the earth’s surface – limestone, marble and chalk. Calcium compounds are essential for life – such as for making bones and milk.

16. Magnesium Magnesium is less reactive then sodium or calcium. It is still too reactive to have any uses in its pure form though. Magnesium is easily obtainable from salts in sea water Amongst other things, magnesium is essential for making chlorophyll.

17. Metals get more reactive as you move left in the periodic table …. so Group 1 metals are the most reactive Reactivity

18. …They also get more reactive as you go down the table Reactivity

19. Group 1 metals are the most reactive. then Group 2 and potassium is more reactive than sodium Reactivity

20. These group 1 metals are too reactive to be allowed in labs. On the other hand, its difficult to get copper and zinc to do anything! Reactivity

21. Metals all form (They do this by LOSING electrons)

22. Most non- metals form (They do this by GAINING electrons)

23. Groups 1 – 13 form positive ions Na + Mg 2+ Al 3+

24. Group 14 elements don’t form ions This is because they have 4 electrons in their outer shell. It isn’t easier to gain 4 more or lose 4 - so they don’t do either!

25. Groups 15, 16 and 17 all gain electrons to form negative ions Cl - S 2- N 3-

26. Group 18 elements don’t form ions either. This is because they already have the full 8 electrons in their outer shell.

27. Group 1 metals all have one electron in their outer shell. They can lose this electron to form a 1+ positive ion Fr Cs Rb K Na Li 3 11 19

28. Fr Cs Rb K Na Li 3 11 19 + LiLi + e-e- + lithium lithium ion electron + For instance:

29. Fr Cs Rb K Na Li 3 11 19 + Li +

30. + Fr Cs Rb K Na Li 3 11 19 Li + Na +

31. Fr Cs Rb K Na Li Li + 3 11 19 Na + + K+K+

32. Fr Cs Rb K Na Li Li + 3 11 19 Na + K+K+ Rb + Cs + Fr +

33. Ra Ba Sr Ca Mg Be 4 12 20 Group 2 metals have 2 electrons in their outer shell…. ….. so they form 2 + ions Ba 2+ Sr 2+ Ca 2+ Mg 2+ Be 2+ Ra 2+

34. Some metals, like iron, can form 2+ or 3+ ions Fe Fe 2+ Fe 3+ + + 2 e - 3 e -

35. Non-metals can form two types of ion: Monatomic ions (the ion is made from just one non-metal element) Cl - = chloride I - = iodide Br - = bromide O 2 - = oxide S 2 - = sulphide Polyatomic ions (the ion is made from more than one non-metal element) OH - = hydroxide SO 4 2 - = sulphate NO 3 - = nitrate CO 3 2 - = carbonate HCO 3 2 - = hydrogen carbonate

36. Metal and non-metals join together to make IONIC compounds. +2CuO2Cu copper O2O2 oxygencopper oxide Mg+Cl 2 MgCl 2 magnesiumchlorinemagnesium chloride

37. Reactions with Metals. 1.Metals react with oxygen to from oxides. 2.Metals react with water to form hydroxides and hydrogen gas. 3.Metals react with acids to form salts and hydrogen gas.

38. 1. Metals react with oxygen (O 2 ) to form oxides. sodium + oxygen  sodium oxide 4Na O2O2 +  2Na 2 O calcium+oxygen +   O2O2 calcium oxide 2Ca2CaO oxygen + +   3O 2 ironiron oxide 4Fe2Fe 2 O 3

39. 2. Metals react with water to produce hydroxides and hydrogen gas. sodium + water  sodium hydroxide + hydrogen gas 2Na2H 2 O+  2NaOH + H2H2 calcium + water  calcium hydroxide + hydrogen gas Ca(OH) 2  Ca2H 2 O++H2H2 *Soluble hydroxides are called alkalis*

40. 3.Metals react with acids to form salts and hydrogen gas potassium + hydrochloric acid  potassium chloride + hydrogen 2K+2HCl  2KCl+H2H2 ++ potassium + sulphuric acid  potassium sulphate + hydrogen 2KH 2 SO 4  K 2 SO 4 H2H2

41. potassium + hydrochloric acid  potassium chloride + hydrogen 2K+2HCl  2KCl+H2H2 The metal forms the first part of the salt’s name. The non-metal forms the second part of the salt’s name. Naming Salts