3.2.1 Balancing Redox Equations

• Oxidation is defined as the loss of electrons
• Match the term with its correct definition:

  Oxidizing Agent ↔️ Accepts electrons

  Reducing Agent ↔️ Donates electrons
• What is the balanced redox equation combining the oxidation and reduction half-reactions for iron and copper?

  $Fe +$$Cu^{2 + } \rightarrow Fe^{2 + } +$$Cu$
• What does the oxidation half-reaction show in a redox reaction?

  Loss of electrons
• In a redox reaction, reduction is the gain of electrons
• A reducing agent in a redox reaction donates electrons
• The reduction half-reaction shows the gain of electrons.

  True
• In alkaline media, hydrogen is balanced using OH⁻.

  True
• To balance the charges in a half-reaction, add electrons to the side with the more positive charge
• Reduction involves the gain of electrons
• What are the two methods for balancing redox equations?

  Oxidation numbers and half-reactions
• What does an oxidation half-reaction demonstrate?

  Loss of electrons
• What is the purpose of balancing atoms in half-reactions?

  Ensure atom equality
• What elements should be balanced first in a half-reaction?

  Non-oxygen and hydrogen
• In alkaline media, where are electrons added to balance the charges?

  Reactant side
• When combining balanced half-reactions, electrons must be canceled
• What are the two fundamental processes involved in redox reactions?

  Oxidation and reduction
• What is the reduction half-reaction example in the study material?

  $Cu^{2 + } +$$2e^ - \rightarrow Cu$
• In the oxidation half-reaction Fe → Fe²⁺ + 2e⁻, iron loses two electrons.


  True
• The element that loses electrons is oxidized in the oxidation half-reaction.


  True
• What is oxidation in a redox reaction?

  Loss of electrons
• What is an oxidizing agent in a redox reaction?

  Accepts electrons
• An element that loses electrons is being oxidized
• In acidic media, oxygen is balanced using H₂O
• To balance charges in acidic media, electrons are added to the side with the more positive charge
• What is the definition of oxidation in a redox reaction?

  Loss of electrons
• Match the key concept with its definition:

  Oxidation ↔️ Loss of electrons

  Reduction ↔️ Gain of electrons

  Oxidizing Agent ↔️ Accepts electrons

  Reducing Agent ↔️ Donates electrons
• The reduction half-reaction shows the gain of electrons
• What is used to balance oxygen in alkaline media?

  H₂O
• In alkaline media, hydrogen is balanced using OH⁻


  True
• Balancing charges in half-reactions involves adding electrons to the more positive side.


  True
• Match the action with its purpose in balancing redox reactions:

  Balancing atoms ↔️ Ensure atom equality

  Balancing charges ↔️ Ensure charge neutrality

  Ensuring equal electrons ↔️ Prepare for combining reactions
• Oxidation increases the oxidation number of an element.


  True
• Balancing redox equations ensures that the number of electrons gained equals the number of electrons lost
• Steps to identify oxidation and reduction half-reactions:

  1️⃣ Identify elements changing oxidation numbers

  2️⃣ Determine oxidation or reduction

  3️⃣ Write half-reactions separately
• An oxidizing agent accepts electrons and causes oxidation
• Oxidation increases the oxidation number of an element.


  True
• How do you identify the oxidation half-reaction in a redox equation?

  Element loses electrons
• What is the first step in balancing atoms in a half-reaction?

  Balance other elements
• What is the first step in balancing charges in a half-reaction?

  Calculate total charge