Redox Reactions-How do u find the oxidizing and thereducing agents/?

Question

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Answer 1

Look at the reactants (They are always the reducing and oxidizing agents)
Look for elements that are changing oxidation states
For example KMnO4 on one side and MnO2 on the other.
Mn is +7 in KMnO4 and +4 in MnO2
The Mn has GAINED electrons
The Mn is REDUCED
The KMnO4 is the OXIDIZING AGENT

Elements that have several oxidation states will normally be the elements changing.
Sb +3, +5
As +3, +5
Bi +3, +5
Br -1, +3, +5, +7 (also Cl and I)
Cu, Fe, Sn, Mn, etc.

If an element changes oxidation state it is either oxidized or reduced.


The oxidizing reagent is reduced (gains electrons)
The reducing agent is oxidized (loses electrons)

Answer 2

Okay, let's start at the top. Do you know how to find which is oxidized or reduced? If not, I'll review. If you assign oxidation numbers to every, EVERY, atom in the reaction, both reactants and products you should notice that some of the oxidation states changed on some of the atoms. An element is reduced if it gains electrons and becomes more negative. It is oxidized if it loses electrons if it becomes more positive. The oxidizing agent is the element that was reduced, and the reducing agent is the one that was oxidized. It really is as simple as that.

Answer 3

Count up all the oxidation numbers. If the oxidation number of an element increases from left to right, that's the reducing agent. In the oxidation number decreases left to right, that's the oxidizing agent.