⚡ DAT Redox Reactions Explained: Oxidation, Reduction & Half-Reactions

Redox (reduction-oxidation) concepts appear across:

• General Chemistry

• Electrochemistry

• Thermodynamics

You’ll encounter DAT questions asking:

• What’s oxidized or reduced?

• What are the oxidation numbers?

• What’s the net ionic/half-reaction?

🔁 Oxidation and Reduction Defined

• Oxidation: Loss of electrons → Oxidation number increases

• Reduction: Gain of electrons → Oxidation number decreases

📌 Memory Aid:
OIL RIG → Oxidation Is Loss, Reduction Is Gain

🔢 Oxidation Number Rules (DAT Must-Know)

Rule	Example
Free element = 0	O₂, Cl₂, Fe
Group 1 metals = +1	Na⁺, K⁺
Group 2 metals = +2	Ca²⁺, Mg²⁺
Hydrogen = +1 (−1 w/ metals)	HCl (+1), LiH (−1)
Oxygen = −2 (peroxides = −1)	H₂O (−2), H₂O₂ (−1)
Halogens = −1 (except w/ oxygen)	NaCl (−1), ClO₄⁻

🧪 How to Identify Redox Reactions

Look for:

• Changes in oxidation numbers

• Electron transfer

• Involvement of oxidizing/reducing agents

Oxidizing Agent = species that gets reduced
Reducing Agent = species that gets oxidized

✍️ How to Write Half-Reactions

Split the redox process into:

• Oxidation Half-Reaction

• Reduction Half-Reaction

Balance for:

1. Atoms (except O and H)

2. Oxygen using H₂O

3. Hydrogen using H⁺

4. Charge using e⁻

🧠 DAT Example

Balance this redox reaction in acidic solution:

MnO₄⁻ + Fe²⁺ → Mn²⁺ + Fe³⁺

Steps:

• Mn is reduced: Mn⁷⁺ → Mn²⁺

• Fe is oxidized: Fe²⁺ → Fe³⁺

• Balance charges and atoms → Combine half-reactions
  ✅ This is a classic DAT half-reaction balance question.

📈 Bonus: Redox & Electrochemistry

DAT electrochemistry questions use redox logic:

• Anode = oxidation

• Cathode = reduction

• Electrons flow from anode → cathode

• Use E° cell = E° red (cathode) − E° red (anode)

🎯 Call to Action

Still memorizing without clarity?
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• Interactive visuals

• Redox flowcharts

• Multiplayer challenge questions

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