Redox Rxn

Redox Reactions

Reactions involving the transfer of electrons between two species.

Oxidation

Loss of electrons or increase in oxidation state.

Reduction

Gain of electrons or decrease in oxidation state.

Oxidizing Agent

Species that gains electrons and undergoes reduction.

Reducing Agent

Species that loses electrons and undergoes oxidation.

Oxidation Number (ON)

A measure of the degree of oxidation of an atom in a compound.

Free Elements

Substances that have an oxidation number of 0.

Monoatomic Ions

Ions that have an oxidation number equal to their charge.

Hydrogen's Oxidation State with Non-metals

+1.

Hydrogen's Oxidation State with Metals

-1.

Oxygen's Oxidation State

Usually -2.

Peroxides

Compounds in which oxygen has an oxidation state of -1.

Superoxides

Compounds where oxygen has an oxidation state of -1/2.

Sum of Oxidation Numbers in Neutral Compounds

Equal to 0.

Balancing Redox Reactions

The process of ensuring the number of atoms and the total charge is the same on both sides of the equation.

Ion-Electron Method

A method for balancing redox reactions using half-reactions.

Oxidation Number Method

A method for balancing redox reactions by using oxidation states.

Combination Reaction

A reaction where two or more substances combine to form a single product.

Decomposition Reaction

A reaction where a single compound breaks down into two or more products.

Displacement Reaction

A reaction where one element displaces another in a compound.

Disproportionation Reaction

A reaction where a single element undergoes both oxidation and reduction.

KMnO4 Titration

In acidic medium, it acts as an oxidizing agent and is reduced to Mn2+.

K2Cr2O7 Titration

In acidic medium, it acts as an oxidizing agent and is reduced to Cr3+.

Indicators in Titrations

Substances used to signal the endpoint of a titration.

Oxidation at Anode

Electrons are lost at the anode during a redox reaction.

Reduction at Cathode

Electrons are gained at the cathode during a redox reaction.

EMF Calculation (Nernst Equation)

Ecell=Ecell∘−0.0591nlog⁡Q.

Standard Electrode Potential

Indicates the strength of oxidizing or reducing agents.

Practical Applications of Redox Reactions

Includes electrolysis, batteries, and biological processes like cellular respiration.