Redox Reactions & Electrochemistry Cheatsheet

Cheat Codes & Shortcuts

• Redox Reaction: Reaction involving transfer of electrons (oxidation and reduction).
• Oxidation: Loss of electrons.
• Reduction: Gain of electrons.
• Oxidizing Agent: Species that gets reduced.
• Reducing Agent: Species that gets oxidized.
• Electrochemical Cell: Device converting chemical energy to electrical energy or vice versa.
• Galvanic/Voltaic Cell: Spontaneous redox reaction producing electricity.
• Electrolytic Cell: Uses electricity to drive non-spontaneous redox reaction.
• Standard Electrode Potential (\(E^\circ\)): Measures tendency to gain electrons under standard conditions.
• Nernst Equation: Calculates electrode potentials under non-standard conditions.

Quick Reference Table

Term	Definition / Formula	Example / Note
Oxidation	Loss of electrons (e.g., Zn → Zn\(^{2+}\) + 2e\(^{-}\))	Zn is oxidized
Reduction	Gain of electrons (e.g., Cu\(^{2+}\) + 2e\(^{-}\) → Cu)	Cu\(^{2+}\) is reduced
Cell Potential \(E_{cell}\)	\(E_{cell} = E^\circ_{cathode} - E^\circ_{anode}\)	Positive means spontaneous reaction
Nernst Equation	\(E = E^\circ - \frac{RT}{nF} \ln Q\)	Calculates cell potential at non-standard conditions
Galvanic Cell	Produces electricity through spontaneous reaction	Zinc-Copper cell

Advice

Redox & Electrochemistry Quick Tips

• Oxidation number: Key for identifying electron transfer.
• SHE: Standard Hydrogen Electrode, defined as 0 V.
• More positive \(E^\circ\): Stronger oxidizing agent.
• Galvanic cell: Spontaneous, produces current.
• Electrolytic cell: Non-spontaneous, requires external voltage.

Redox Reactions & Electrochemistry Speed Quiz

Test your speed with 5 questions! You have 30 seconds per question.