Aplications of the oxidation-reduction process

Oxidation and reduction concepts

Whenever one species is reduced, there is another that is oxidized

Oxidation: loss of electrons

Reduction: electron gain

Oxidizing agent

Gain electrons

Decreases its oxidation number

Reducing agent

Loses electrons

Increases its oxidation number

Are the assigned charges to the different atoms involved of a species

Assign the oxidation numbers to each element in the reaction

Identify the elements that change their oxidation state or charge

Write the two oxidation and reduction half-reactions

Perform the balance of mass. Same number of chemical species on both sides

Balance the charge in each equation. This should be done after the balance of mass.

Match the number of electrons lost in oxidation to the number of electrons gained in reduction

Transfer the coefficient that appears in front of each substance in the half-balanced reactions

Balance the remaining elements that do not oxidize or reduce to obtain the balanced equation

Check that both sides of the equation have the same number of atoms of each element

Definition

Devices capable of generating an electric current from a spontaneous chemical reaction of oxidation-reduction

Function

To supply electrical current through a redox reaction to the transfer of electrons

Definition

Electrochemical cell in which electrical energy is used to drive a non-spontaneous oxidation-reduction reaction

Function

To force a chemical reaction that would otherwise not occur

Nature

Nerve impulses generated neurons

Electric eels

Corrosion in metals

Industry

Electric batteries: They are the industrialized and commercial formats of galvanic cells. (car batteries are the traditional battery model)

Mettalic coatings, electroplating: applying a thin layer of metal on an electronic current conducting surface

Molten NaCl electrolysis: method widely used in industry to obtain sodium and chlorine in its elemental state