reactions of metals

• What happens to metal atoms when they react with other substances?

  Metal atoms lose electrons to form positive ions.
• What does the reactivity series of metals show?

  It shows metals in order of decreasing reactivity.
• What is generally true about more reactive metals?

  They have more vigorous reactions and lose electrons more easily.
• What are the products when a metal reacts with water?

  • Metal hydroxide
  • Hydrogen gas
• What is the reaction equation for sodium reacting with cold water?

  2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
• How does the reactivity of metals relate to their reactions with water?

  The more reactive the metal, the more rapid the reaction with water.
• What are the products when a metal reacts with a dilute acid?

  A salt and hydrogen gas are formed.
• What is the reaction equation for magnesium reacting with dilute hydrochloric acid?

  Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
• What happens to metals below hydrogen in the reactivity series when reacting with dilute acids?

  They will not react with dilute acids.
• What do many metals form when they react with oxygen?

  Metal oxides.
• What is the reaction equation for magnesium burning in air?

  2Mg(s) + O2(g) → 2MgO(s)
• Why are the reactions of metals with oxygen classified as oxidation reactions?

  Because the metal gains oxygen during the reaction.
• What happens to copper oxide when it reacts with carbon?

  Copper oxide is reduced as carbon is oxidised.
• What is the definition of oxidation in terms of oxygen?

  Oxidation is the gain of oxygen.
• What is the definition of reduction in terms of oxygen?

  Reduction is the loss of oxygen.
• What is a displacement reaction?

  • A more reactive metal displaces a less reactive metal from its compounds.
  • Example: Magnesium displaces copper from copper sulfate solution.
• What is the reaction equation for magnesium displacing copper from copper sulfate solution?

  Mg(s) + CuSO4(aq) → MgSO4(aq) + Cu(s)
• What happens to the blue color of copper sulfate solution during the displacement reaction with magnesium?

  The blue color fades as it is replaced by colorless magnesium sulfate solution.
• How can a reactivity series be deduced?

  • By carrying out several displacement reactions.
  • Testing different combinations of metal and salt solution.
• What is a balanced equation in the context of displacement reactions?

  A balanced equation shows the ions involved in the reaction.
• What is the balanced ionic equation for the reaction between magnesium and copper sulfate solution?

  Mg(s) + Cu2+(aq) → Mg2+(aq) + Cu(s)
• What do the half equations for magnesium and copper in the displacement reaction represent?

  Magnesium is oxidised and copper ions are reduced.
• What does OIL RIG stand for in redox reactions?

  Oxidation is Loss, Reduction is Gain.
• What are the extraction methods for metals based on their reactivity?

  • Electrolysis for very reactive metals.
  • Heating with carbon for less reactive metals.
• Why is electrolysis expensive for metal extraction?

  It requires large amounts of electrical energy.
• What is the reaction equation for copper oxide being reduced by carbon?

  2CuO(s) + C(s) → 2Cu(l) + CO2(g)
• What happens to iron(III) oxide when it reacts with carbon?

  It is reduced to molten iron.
• What is the reaction equation for iron(III) oxide reacting with carbon?

  Fe2O3(s) + 3C(s) → 2Fe(l) + 3CO(g)
• Why must aluminium be extracted using electrolysis?

  Because aluminium is more reactive than carbon.
• What is the process of electrolysis for aluminium extraction?

  • Aluminium ore is treated to produce pure aluminium oxide.
  • Electrolysis is performed using molten aluminium oxide dissolved in cryolite.
  • At the cathode, aluminium ions gain electrons; at the anode, oxide ions lose electrons.
• What happens to oxide ions during the electrolysis of aluminium oxide?

  Oxide ions lose electrons and are oxidised.
• What is the half equation for the oxidation of oxide ions during electrolysis?

  2O2- → O2 + 4e-