reactivity series

• metal has a high melting point
• metal has a giant lattice structure
• metal has strong attractive forces between positive and negative ions. thus a large amount of energy is needed to break these attractive forces apart
• metal/alloys is a good conductors of electricity as there are free moving delocalized electrons which can carry electrical charges from one end to the other
• why is metal malleable?

  the particles are neatly arranged. hence, when a force is applied, the metal atoms slide past one another easily
• an alloy is a mixture of a metal and other elements
• brass is made out of copper and zinc
• stainless steel is made out of chromium and nickel
• steel is a made out of iron and carbon
• bronze is made out of copper and tin
• why is steel/alloys harder than other elements?

  they are made out of different size atoms which distrupt the regular arrangement of atoms. Hence, when a force is applied, the atoms will not slide over one another easily
• properties of metals


  high meting point, malleable and good electrical conductors
• magnesium and aluminum reacts with steam violently to form magnesium oxide and hydrogen gas
• if the metals are unreactive, they can be extracted by carbon
• potassium, sodium, calcium, magnesium reacts with cold water to form hydrogen gas and metal hydroxide
• potassium -> lead reacts with acid to form hydrogen and salt
• zinc and iron reacts steam to form hydrogen and metal oxide
• potassium, sodium and calcium react with steam explosively
• reactivity decreases down the series
• potassium + hydrochloric acid

  2k + 2HCL -> H2 + 2KCL
• a more reactive metal is able to displace a less reactive metal from its salt solution
• the acid in the reactivity series is hydrochloric acid
• when displacement occurs, 2 changes are observed


  solid metal is deposited at the bottom and color of solution changes
• a less reactive metal cannot displace a more reactive metal from its solution
• if a less reactive metal were to react with a more reactive metal, there'll be no visible change
• if it is a copper metal

  a brown solution will be observed
• for all other metals

  a grey solid is formed
• iron ore reacts with carbon monoxide to form iron metal in a blast furnace


  FE2O3 + 3CO -> 2FE +3CO2
• lead oxide + carbon -> lead + carbon dioxide 


  2 PbO + C → 2 Pb ( s ) + CO 2 
• conditions for rusting


  oxygen and water
• what is meant by rusting?

  rusting in an oxidation process where iron changes into brownish orange iron oxide in the presence of oxygen and water
• other factors of rusting

  acid and salt
• there must be both oxygen and water for rusting to commence
• rusting methods


  painting, greasing, tin plating or stainless steel
• how does painting, greasing and tin plating protect?

  it forms a protective layer on iron metal and prevents direct contact with oxygen and water
• how does stainless steel protect?

  presence of nickle and cobalt make metal resistant to corrosion
• oil prevents oxygen and water from entering
• boiled water has no oxygen
• anhydrous calcium chloride is a drying agent to remove water
• chemical reaction for zinc oxide + carbon

  ZnO2 ( Zinc oxide ) + C ( Carbon ) → Zn ( Zinc ) + CO2