4.1.3 Oxidation and reduction in terms of electrons

• Oxidation is the process where an atom, ion, or molecule loses electrons
• The mnemonic OIL RIG stands for Oxidation Is Loss and Reduction Is Gain of electrons


  True
• Steps to recognize electron transfer in redox reactions:

  1️⃣ Look for changes in oxidation state

  2️⃣ Identify elements that gain or lose electrons

  3️⃣ Use the OIL RIG mnemonic
• What happens during oxidation in terms of electrons?

  Loss of electrons
• Reduction is the process where an atom, ion, or molecule gains electrons.
• Magnesium has an oxidation state of +2 in the reaction \( Mg \rightarrow Mg^{2+} + 2e^- \).
• What is the role of an oxidizing agent in a redox reaction?

  Accept electrons
• Which metal is the most reactive according to the table in the study material?

  Potassium
• Reduction is the process where an atom, ion, or molecule gains electrons
• The oxidation state of a metal indicates the number of electrons it has lost when forming a positive ion
• What is the oxidation state of iron in the compound Fe^{2+}?

  +2
• What happens during reduction in terms of electrons?

  Gain of electrons
• What does the oxidation state of a metal indicate?

  Electrons lost
• More reactive metals lose electrons more readily in redox reactions.


  True
• The mnemonic ORA stands for Oxidizing Agent gains electrons and undergoes reduction.
• Match the process with its definition in terms of electrons:

  Oxidation ↔️ Loss of electrons

  Reduction ↔️ Gain of electrons
• Electron transfer is central to redox reactions.

  True
• In redox reactions, oxidation and reduction always occur together
• The mnemonic OIL RIG stands for Oxidation Is Loss, Reduction Is Gain of electrons.


  True
• What is the oxidation state of sodium in the reaction \( Na \rightarrow Na^+ + e^- \)?

  +1
• What happens to iron (Fe) in the reaction \( Fe + Cu^{2+} \rightarrow Fe^{2+} + Cu \)?

  Oxidized
• Why do more reactive metals act as stronger reducing agents?

  Lose electrons easily