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Metals

Metals. Metals are on the LHS of The Periodic table Properties of Metals. 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)

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Metals

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  1. Metals • Metals are on the LHS of The Periodic table • Properties of Metals

  2. 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.

  3. 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 O2 in air. • Other metals react more slowly.

  4. Metal + Water • Metal + Water —> Metal hydroxide + Hydrogen • Example • Sodium + Water —> Sodium hydroxide + Hydrogen • 2Na + 2 H2O —> 2 NaOH + H2

  5. Metal + Acid • Metal + Acid —> Salt + Hydrogen • Example • Magnesium + Hydrochloric Acid —> Magnesium chloride + Hydrogen Mg +2 HCl —> MgCl2 + H2

  6. Metal Reactions

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

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

  9. 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

  10. 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.

  11. Alloys Alloys are metals melted together. They are made to enhance the properties of the metals.

  12. Calculations using Equations • What mass of Cu will be produced when 6.5g of Zn are added to CuSO4 ? • 1. Balanced Equation • Zn + Cu SO4 ------> ZnSO4 + 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

  13. 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 elementsCu O • 2. Mass present 6.4 1.6 • 3. Mass of 1 mole 64 16 • 4.Number of moles 6.4/64 1.6/16 ( mass given/mass 0.1 0.1 of 1 mole) 5. Convert to whole 0.1/0.1 0.1/0.1 number – 1 1 divide both by smallest no. 6. Ratio 1 : 1 Empirical FormulaCu O

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