2. Metals  Metals are on the LHS of The Periodic table  Properties of Metals MetalUseProperty MercuryThermometersLiquid at room T AluminiumAircraft bodyStrong/ low density GoldJewelleryUnreactive LeadWeightsVery dense TitaniumAircraft engineVery high MP CopperCablesGood electrical conductor

3. Properties  Malleable – can be beaten into shape  Ductile – can be drawn out into a wire  Strong, hard.  Shiny – metallic lustre.  Good conductors of heat and electricity.  Density – varies ( data book)  Metals usually have High MP and BP  They are solids at room temperature – Mercury is the only liquid metal at room T.

4. Metal reactions  Metal + Oxygen —> Metal oxide  The energy change in the reaction depends on how reactive the metals are.  Alkali metals stored in oil. They react with O 2 in air.  Other metals react more slowly.

5. Metal + Water  Metal + Water —> Metal hydroxide + Hydrogen  Example  Sodium + Water —> Sodium hydroxide + Hydrogen  2Na + 2 H 2 O —> 2 NaOH + H 2

6. Metal + Acid  Metal + Acid —> Salt + Hydrogen  Example  Magnesium + Hydrochloric Acid —> Magnesium chloride + Hydrogen Mg +2 HCl —> MgCl 2 + H 2

7. Metal Reactions MetalReact with O 2 React with H 2 OReact with H + PotassiumYES YES!!!! LithiumYES YES!!! MagnesiumYES AluminiumYES IronYes - surfaceYES LeadYes - surfaceYES CopperYes - surface Silver Mercury

8. The Reactivity Series  This is a list of metals in the order they react,  The most reactive metal is at the top. KK  Na  Li  Ca  Mg  Al  Zn  Fe  Sn  Pb  Cu  Hg  Ag  Au

9. Metal Ores AA metal ore is a naturally occurring compound of a metal. WWe have to extract the metal from its ore to use it. MMetals are a finite resource – they will run out. TThey can be recycled. SSome metals are found un combined in the earth – not in a compound e.g. Gold, Silver.

10. Extracting Metals from their Ores  Some metals can be removed by heat alone – un reactive metals e.g. Copper, Silver.  Others need to be heated with C or CO or H – they remove the O in the compound leaving the metal element. ( Zn ---> Pb)  Example  Iron oxide + Carbon monoxide ----> Iron + Carbon dioxide  The more reactive metals have to removed by electrolysis e.g. Al ---->K

11. The Blast Furnace  Iron is separated from Iron Oxide in a structure called the Blast Furnace.  3 raw ingredients are added at the top. Coke, Iron Ore and limestone.  A blast of hot air enters at the bottom, this provides heat for the reactions:  Carbon monoxide + Iron Ore -----> Iron + carbon dioxide.  Carbon dioxide + Coke -----> Carbon monoxide  Coke + Oxygen ------> Carbon dioxide  The molten iron runs out at the bottom.  The limestone decomposes to impurities – SLAG. Slag can be used for insulation in building industry.

12. Alloys are metals melted together. They are made to enhance the properties of the metals. AlloyElements in itProperties BrassZn, CuLow MP, shapes easy SolderSn,PbLow MP SteelFe, Cr, NiStrong, no corrosion Cupro NickelCu, NiCheap, hard

13. Calculations using Equations  What mass of Cu will be produced when 6.5g of Zn are added to CuSO 4 ?  1. Balanced Equation  Zn + Cu SO 4 ------> ZnSO 4 + Cu  2.Mole Ratio:  Zn:Cu = 1:1  3. Actual number of moles – Mass given/mass of 1 mole  Zn = 6.5/65 = 0.1  4. New ratio  If 1 mole Zn gives you 1 mole of Cu then 0.1 moles will give you 0.1 moles of Cu.  5. Mass produced  I mole Cu = 64g x 0.1 = 6.4g

14. Empirical Formula – basic formula  Calculate the Empirical formula of a metal ore if it contains6.4g of Cu and 1.6g of O  1. List elements CuO  2. Mass present6.41.6  3. Mass of 1 mole6416  4. Number of moles 6.4/641.6/16 ( mass given/mass0.10.1 of 1 mole) 5. Convert to whole 0.1/0.10.1/0.1 number – 11 divide both by smallest no. 6. Ratio1 : 1 Empirical FormulaCu O