Redox reactions definition?
Any chemical reaction which includes the switching of
electrons between species is called oxidation-reduction reaction or redox
reaction. In
such type of reaction, the oxidation number of the molecule or an atom or ion
changes either by gaining or losing an electron. Such reactions are normal and
significant for some essential functions such as photosynthesis, combustion,
respiration, corrosion, etc.
Oxidation
definition
When electrons are lost by a molecule, an ion, or atom
during a chemical reaction it is an oxidation reaction. This type of reaction
takes place when the oxidation state of a molecule, an atom or ion is
increased.
Reduction definition
When electrons are gained by a molecule, an ion, or atom
during a chemical reaction, it is an oxidation reaction. This type of reaction
takes place when the oxidation state of a molecule, an atom or ion is
decreased.
Redox reaction examples
Formation of hydrofluoric acid (HF)
by reacting fluorine gas and hydrogen. The reaction occurs in the following
way:
H2 + F2
→ 2 HF
In this reaction,
Hydrogen undergoes oxidation whereas fluorine is undergoes
reduction. Let us understand the reaction better. Therefore, by dividing the
equation into two half-reactions, we get the following:
H2 → 2 H+ + 2 e-
F2 + 2 e- → 2 F-
Oxidizers definition with examples
Oxidizers are the substances that are
accountable for losing electrons of other substances. Their role is to oxidize
the substances. They are also termed as oxidizing agents, oxidizers, or
oxidants. It is reduced by eliminating electrons from other substances. One
common example of oxidizer is CrO3.
Reducers definition with examples
Reducers are substances that are
accountable for gaining electrons from other substances. Their role is to
reduce substances. They are also termed as reducing agents, reductants, or
reducers. It is oxidized by giving electrons to other substances. Examples of
reducers are lithium, sodium, zinc, etc.
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