Chemical reactions in which the oxidation states or oxidation numbers of the atoms are reformed is known as oxidation-reduction reaction.

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2.  Chemical reactions in which the oxidation states or oxidation
numbers of the atoms are reformed is known as oxidation-
reduction reaction.
 These reactions are also known as redox reactions, which is
short form for reduction-oxidation reaction. Oxidation is the
process of losing of electrons throughout a reaction by a
molecule an atom or an ion.
 Oxidation arises when the oxidation state of a molecule, atom
or ion is higher.
 The contrast process is known as reduction, which happens
when the electrons are gained or when oxidation state of an
atom, molecule, or ion lowers.
 An example for redox reaction is as follows:
2 Al +3 Br2 -> Al2Br6
 In this reaction Bromine is been oxidized and Aluminum is being
reduced
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3.  Redox reactions are a vital class of chemical reactions
confronted in daily processes.
 These reactions take place all around us. Iron corrodes,
batteries produce electricity, and wood, oil and coal which
are hydrocarbon fuels are scorched to produce energy.
 Oxidation-reduction reactions are significant for
biochemical reactions and industrial procedures.
 The system in cells that transfers electron and the process
of oxidation of glucose in the humans are common
examples of redox reactions.
 Using redox reactions the ores are condensed to attain
metals, to manufacture electrochemical cells, to
transform ammonia into nitric acid for fertilizers and also
compact discs coating.
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4.  Oxidation in general is the losing of electrons or hydrogen
or gain of oxygen or increase in oxidation state Reduction
involves the gain of electrons or hydrogen or loss of
oxygen or decrease in oxidation state.
 Redox reactions are immensely common in nature,
particularly in oxidizing the metals and other minerals.
 Oxidation reactions were initially named when the
bonding of oxygen which was because oxygen gas was
first known as oxidizing agent.
 The word was soon rephrased to any reaction in which any
chemical losses their electrons another chemical.
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5.  Foreseeing a redox reaction is based on the
oxidation number of a given element or chemical
compound.
 The most recurrent chemical is basic oxygen,
which has an oxidation number of minus 2.
 To equalize a redox reaction relating oxygen, the
chemical that is the reducing agent must have a
positive oxidation number.
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6.  The rusting of iron is a common redox
reaction.
 During oxidation process iron metal reacts
with moist air to form hydrated iron oxide.
 Though aluminum oxide which provides a
protective coating, iron oxide fragments off
at the surface, revealing more iron
throughout the oxidation process.
 Ultimately, the iron loses its structural form
because of corrosion.
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7.  The modern studies of oxidation and reduction reaction
concerns on electrons.
 Addition of electrons is known as reduction in a molecule
since the total charge is been reduced, which means if more
electrons are added the compound turn more negative.
 While in oxidation the compound losses electrons. So simply
put one compound losses electrons while the other gains.
 “To remember which chemical species is oxidized and which
is reduced is to rememberOIL RIG. It states Oxidation is
losing and reduction is gaining”.
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