Reactivity of metals

• Place zinc, copper and magnesium in order of reactivity

  Magnesium

  Zinc

  Copper
• Name the element used to reduce iron oxide.

  Carbon
• Suggest two reasons why copper should not be disposed of in landfill sites.

  Copper ores are limited

  Copper can be recycled
• The alloy stainless steel is used instead of pure iron for the ball of the pen. Give two reasons why.

  Stainless steel is hard

  Its resistant to corrosion
• Copper is now extracted from ores containing a low percentage of copper compounds

  Copper is hard to find

  Copper is very expensive
• Suggest one reason why it is difficult to dispose of the waste rock.

  Large amounts
• Pure copper is produced by electrolysis of copper sulphate solution. Which electrode do the copper ions move towards?

  The negative electrode as copper ions is oppositely charged
• Write down two differences you would see between the reactions of potassium and lithium with water.

  Potassium reacts faster

  Potassium produces a lilac flame
• What is the meaning of ore?

  Contains enough metal to make it economical to extract
• Write a word equation for the overall reaction that takes place in a hydrogen fuel cell.

  Hydrogen+ oxygen -> water
• State one property that makes aluminium more suitable than copper for overhead cables.

  Aluminium has low density
• Copper can be extracted from solutions of copper salts by adding iron. Explain why

  iron is more reactive so copper is displaced
• The use of titanium is limited because it is expensive. Explain why titanium costs more than steel

  takes a long time to process

   low abundance

   small amount produced
• State why argon is used in the light bulb. Explain your answer in terms of the electronic structure of an argon atom.

  Its very unreactive as it has a full outer shell so it doesn’t need to gain or lose any electrons

   
• List all the elements in the reactivity series in order of most reactive to least.

  Potassium, sodium, lithium, calcium, magnesium, carbon, zinc, iron, hydrogen, copper, silver, gold.
• Write a general word equation for the reaction of metal with oxygen.

  Metal + Oxygen --> Metal oxide
• Why are reactions of metals with oxygen described as oxidation?

  Because the metal gains oxygen.
• What type of ion do metals form when they react?

  Positive ions (cations)
• Why can't potassium be with acid in school?

  It will explode.
• Write a general word equation for the reaction of metal with acid.

  Metal + Acid --> Salt + Hydrogen
• Describe the test of hydrogen gas.

  Ignite the gas with a lit splint.
• Describe the observation of the hydrogen gas test.

  A squeaky pop.
• How can the reactions of metals with acid be compared?

  By measuring the temperature change during the reaction.
• What is a metal displacement reaction?

  A reaction whereby a more reactive metal takes the place of a less reactive metal from it's salt.
• Write a word equation for the displacement reaction between zinc and iron chloride.

  Zinc + iron chloride --> zinc chloride + iron
• Write a balanced symbol equation for the reaction of zinc with iron chloride.

  Zn + FeCl2 --> Fe + ZnCl2
• What is an ore?

  A metal combined with other elements found in rock.
• Describe 'reduction' as a form of extraction.

  Metals below carbon can be extracted from compounds by reacting with carbon.
• Why is carbon used in 'reduction' of metal oxides?

  It is more reactive than the metal being extracted.
• Why can't metals placed above carbon in the reactivity series be extracted by reduction?

  Because they are more reactive than carbon.
• What is meant by reduction?

  Reduction is loss of oxygen.
• What is electrolysis?

  Breaking down of a compound using electrical energy.
• When is electrolysis used in extraction?

  With compounds containing metals above carbon in the reactivity series.
• What is the disadvantage of electrolysis?

  It requires a large amount of electrical energy and is expensive.
• Define oxidation in terms of electrons.

  Loss of electrons.
• Define reduction in terms of electrons.

  Gain of electrons.
• What is a spectator ion?

  An ion that does not change in a reaction.
• How can a spectator ion be identified?


  It hasn't changed its state or its charge.
• Write an ionic equation for this reaction: Ca(s) + MgSO4(aq) --> CaSO4(aq) + Mg(s) 


  Ca(s) + Mg2+(aq) --> Ca2+(aq) + Mg(s)
• Write an ionic equation for this reaction: Cl2(aq) + 2NaI(aq) -->

  2NaCl(aq) + I2(aq) +Cl2(aq) + 2I-(aq) --> 2Cl-(aq) + I2(aq)