Oxidation, reduction and displacement reactions

• What does the reactivity series show?

  The reactivity series shows metals in order of reactivity.
• How is the reactivity of a metal related to its ions?

  The reactivity of a metal is related to its tendency to form positive ions.
• Which metals are extracted from their ores in various ways?

  Iron and aluminium are extracted from their ores in various ways.
• What happens when metals react with oxygen?

  • Metals react with oxygen to form metal oxides.
  • Example: Magnesium burns in air to form magnesium oxide.
• Write the balanced equation for the reaction of magnesium with oxygen.

  2Mg(s) + O$_2$(g) → 2MgO(s)
• Why are the reactions of metals with oxygen classified as oxidation reactions?

  They are classified as oxidation reactions because the metal gains oxygen.
• What is the definition of oxidation?

  Oxidation is the gain of oxygen or loss of electrons by a substance during a chemical reaction.
• What happens to copper oxide in the reaction with carbon?

  Copper oxide is reduced because oxygen is removed from it.
• Write the balanced equation for the reaction of copper oxide with carbon.

  2CuO(s) + C(s) → 2Cu(l) + CO$_2$(g)
• What is a displacement reaction?

  • A displacement reaction occurs when a more reactive metal displaces a less reactive metal from its compound.
  • Example: Magnesium displaces copper from copper sulfate solution.
• What is the general form of a displacement reaction involving metals?

  A more reactive metal displaces a less reactive metal from its compound.
• Write the balanced equation for the displacement reaction between magnesium and copper sulfate.

  Mg(s) + CuSO$_4$(aq) → MgSO$_4$(aq) + Cu(s)
• What happens to the color of the copper sulfate solution during the displacement reaction with magnesium?

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

  • By carrying out several displacement reactions.
  • A piece of metal is dipped into a salt solution.
  • Different combinations of metal and salt solution are tested.
• What is the order of reactivity deduced from the investigation involving magnesium, iron, and copper?

  The order of reactivity is: magnesium > iron > copper.
• Why were some combinations of metal and salt solution not done in the investigation?

  A metal cannot displace itself from a solution of one of its salts, so there would be no reaction.
• What is a balanced equation?

  A balanced equation shows the same number of units of each element on both sides of the arrow.
• What is an ionic equation?

  An ionic equation shows how positively charged ions join with negatively charged ions to make a compound.
• Write the ionic equation for the reaction between magnesium and copper sulfate solution.

  Mg(s) + Cu$^{2+}$(aq) → Mg$^{2+}$(aq) + Cu(s)
• What are half equations in redox reactions?

  Half equations describe the process happening at an electrode, showing the transfer of electrons.
• What is the key fact about oxidation and reduction?

  Oxidation is the loss of electrons, and reduction is the gain of electrons.
• What does the acronym OIL RIG stand for?

  OIL RIG stands for Oxidation Is Loss, Reduction Is Gain.
• What are examples of redox reactions?

  • Displacement reactions
  • Electrolysis reactions
• What is electrolysis?

  Electrolysis is the decomposition of a compound using an electric current.
• How are displacement reactions related to redox reactions?

  Displacement reactions are an example of redox reactions where oxidation and reduction occur simultaneously.
• What are the key concepts of redox reactions?

  • Oxidation involves loss of electrons.
  • Reduction involves gain of electrons.
  • Both processes occur simultaneously in redox reactions.