#Electrochemistry: Your Ultimate Review ⚡

Hey there! Let's dive into electrochemistry, where we explore how redox reactions create electrical energy. This is a crucial area, so let's make sure you're feeling confident!

Electrochemistry is a high-value topic, often accounting for a significant portion of both multiple-choice and free-response questions. Mastering this unit can greatly boost your score.

# Review of Redox Reactions

#What are Redox Reactions?

• Redox reactions (oxidation-reduction reactions) involve the transfer of electrons. 🔄
• A reducing agent loses electrons and is oxidized. ⬆️
• An oxidizing agent gains electrons and is reduced. ⬇️

#Example:

Consider the reaction: 2AgNO₃ + Cu → Cu(NO₃)₂ + 2Ag

• Copper (Cu) is oxidized (0 → +2 oxidation state).
• Silver (Ag⁺) is reduced (+1 → 0 oxidation state).
• Electrons move from copper to silver.

Image From SciencePhoto

#Half-Reactions:

• Oxidation: Cu → Cu²⁺ + 2e⁻
• Reduction: 2Ag⁺ + 2e⁻ → 2Ag

# Reduction Potentials

#What are Reduction Potentials?

• Electromotive force (EMF) is the force that pushes electrons in a redox reaction. It's measured in volts (V). ⚡
• Standard reduction potentials are the voltages of reduction half-reactions. They're provided in a table (like this one).
• Negative voltage means energy is needed for the reaction to occur.

#Calculating Cell Potential (E°)

Let's use the reaction: Zn(s) + Pb²⁺(aq) → Zn²⁺(aq) + Pb(s)

1. Half-Reactions:
   • Oxidation: Zn → Zn²⁺ + 2e⁻
   • Reduction: Pb²⁺ + 2e⁻ → Pb
2. Reduction Potentials (from the table):
   • Pb²⁺ reduction: -0.13 V
   • Zn²⁺ reduction: -0.76 V
3. Flip the sign for the oxidat...