Redox Reactions and Electrochemistry

Manual: General · Subject: Chemistry

Balance oxidation-reduction chemistry and connect it to galvanic and electrolytic cells.

Electron transfer chemistry

Oxidation and reduction

Oxidation is loss of electrons and reduction is gain of electrons. In terms of oxidation numbers, oxidation corresponds to an increase in oxidation state, while reduction corresponds to a decrease.

Balancing redox in acidic solution

1

Step 1: Split the reaction into oxidation and reduction half-reactions.
2

Step 2: Balance atoms other than $H$ and $O$ .
3

Step 3: Balance $O$ with $H_2O$ and $H$ with $H^+$ .
4

Step 4: Balance charge with electrons and combine the half-reactions.

Electrochemical cells

Galvanic cells convert chemical energy into electrical energy through spontaneous redox reactions. Electrolytic cells use electrical energy to drive nonspontaneous reactions.

Cell components

Part	Function	Example
Anode	Oxidation occurs here	Electron source in a galvanic cell
Cathode	Reduction occurs here	Electron sink in a galvanic cell
Salt bridge	Maintains charge balance	Allows ion migration
External circuit	Carries electrons	Wire or load

In a galvanic cell, oxidation occurs at the

Cathode Anode Salt bridge Electrolyte only

What happens to oxidation number during reduction?

ℹ️

Remember the mnemonic

OIL RIG: Oxidation Is Loss, Reduction Is Gain.

An electrolytic cell is characterized by

A spontaneous reaction producing electricity A nonspontaneous reaction driven by electricity No electron transfer Only acid-base chemistry

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Concept Constellation

Redox Reactions and Electrochemistry

Electron transfer chemistry

Oxidation and reduction

Balancing redox in acidic solution

Electrochemical cells