Chemistry

A substance that oxidizes another substance

Any chemical substance that has a tendency to accept electrons and thereby undergoing reduction themselves is known as an oxidising agent.

An oxidizer is a compound that supplies its own oxygen and heat when in contact with organic compounds. These chemicals that can react vigorously and explode.

Oxidizers are compounds which are capable of reacting with and oxidizing (i.e., giving off oxygen) other materials. A well known example of oxidation is the process we know as corrosion, where the metal reacts with air to form the metal oxides referred to as "rust".

The primary hazard associated with this class of compounds lies in their ability to act as an oxygen source, and thus to readily stimulate the combustion of organic materials. As you may recall, it takes three components for a fire to happen - a fuel source (usually an organic compound, such as paper), an ignition source (such as a flame, a spark, friction, etc.) and an oxygen source (in this case - a cylinder of OXYGEN, a strong oxidizer).

Oxidizers may be grouped into 4 classes based on their ability to affect the burning rate of combustible materials or undergo self-sustained decomposition. This classification system was established by the National Fire Protection Association (NFPA 43A, 1980) as a means to provide information on safe storage of oxidizing materials.

Class 1: An oxidizing material whose primary hazard is that it may increase the burning rate of combustible material with which it comes in contact

Class 2: An oxidizing material that will moderately increase the burning rate of which may cause spontaneous ignitionof combustible material with which it ocmes in contact.

Class 3: An oxidizing material that will cause a severe increase in the burning rate of combustible material with which it comes in contact or which will undergo vigorous self-substained decomposition when catalyzed or exposed to heat.

Class 4: An oxidizing material that can undergo an explosive reaction when catalyzed or exposed to heat, shock or friction.

Electrons are transferred between atoms.

Stoichiometry relates moles of reactant to moles of product, so if you have the amount of reactant in the equation, you can calculate the amount of product produced.

the number of electrons the element needs to lose or gain to have a full valence shell

if oxidation states change, it is a redox reaction

the oxidation states are always 0 for both atoms

Balancing redox reactions is different from balancing other reactions because both the number of atoms and the amount of charge must be balanced.

4.2 V

Mg2+

AgNO3 #APEX

-1.68 V

Answer this question… Fe3+

It goes from +1 to 0

Silver (Ag)

1