How do you work out oxidising and reducing agents?

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username1421435
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#1
Report Thread starter 6 years ago
#1
I just cant get my head around how to identify the oxidising and reducing agent.

What rules do you follow, and can you identify them by oxidation numbers or something?
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Protoxylic
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An oxidising agent is a reagent that itself has been reduced. And a reducing agent is a reagent that itself has been oxidised. In a redox reaction, if you identify the substance that has been oxidised, namely that which has undergone an increase in oxidation state, that is the reducing agent and vice versa.
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PepperPotts
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An oxidising agent oxideses another reactant: so is itself reduced, and it's oxidation number decreases (that's how you identify it)
The reverse is obvs true for reducing agents
Hope that helps!
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KingThomas
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I can help you guys follow me on Twitter: https://twitter.com/AlevelExaminer
An oxidizing agent or oxidant gains electrons and is reduced in a chemical reaction. Also known as the electron acceptor, the oxidizing agent is normally in one of its higher possible oxidation sates because it will gain electrons and be reduced.

e.g HNO3, KNO3

Cheers bro
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CERC
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look at the oxidation numbers!!
for example
Cl2 + 2KBr -------------2KCl + Br2

Cl2 has an oxidation number of zero in Cl2. This is reduced to -1 in KCl. Then, because it has been REDUCED it must have been the oxidising agent as oxidising agents can be defined as 'a species who takes electrons from another species and is itseld reduced.'
Similarly in KBr , Br2 as an oxidation number of -1. This is then oxidised to zero in Br2. Br2 is the reducing agent as reducing agents are defined as 'a species who donates electrons to another species and is itself oxidised'.
Complicated? Yes. just think: if it has been oxidised its the reducing agent and if it has been reduced its the oxidising agent.

Think of it as being opposites!!! Tell me how you get on!!!
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