Definitions
Transfer of electrons occurs in redox (oxidation-reduction) reactions between species (A chemical entity. Chemical entities can be ions, molecules, elements .....) known as
Consider the redox reaction:
Cu2+(aq) + Zn(s)
Cu(s) + Zn2+(aq)
The product arising from the
The direction of the change in charge for species containing a single type of atom is an important clue as to whether the species is an oxidant or a reductant.
- the oxidant (electron acceptor) and
- the reductant (electron donor)
The oxidant is also known as the oxidizing agent.
The reductant is also known as the reducing agent.
The reductant is also known as the reducing agent.
Consider the redox reaction:
Cu2+(aq) + Zn(s)
Cu(s) + Zn2+(aq)The oxidant is Cu2+(aq) and the reductant is Zn(s).
The product arising from the
oxidant has a more negative charge because the oxidant (oxidizing agent) has accepted electrons
In this example: Cu2+ gives Cu
reductant has a more positive charge because the reductant (reducing agent) has donated electrons
In this example: Zn gives Zn2+
In this example: Cu2+ gives Cu
reductant has a more positive charge because the reductant (reducing agent) has donated electrons
In this example: Zn gives Zn2+
The direction of the change in charge for species containing a single type of atom is an important clue as to whether the species is an oxidant or a reductant.
If the charge becomes more positive, the species is a reductant.
If the charge becomes more negative, the species is an oxidant.
If the charge becomes more negative, the species is an oxidant.