Oxidizing Agents and Reducing Agents

This video tutorial shows you how to identify the oxidizing and reducing agent in a redox reaction. The first step in determining which species is the oxidizing agent is to start by finding which reactant was reduced. Likewise, the molecule or element that is was oxidized is also the reducing agent. That's how you can determine it. However, you need to calculate the oxidation numbers or states for every element in the chemical equation. Oxidation involves a loss of electrons and occurs when the oxidation number increases. Reduction involves a gain of electrons and occurs when the oxidation state decreases.
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4 years and nobody corrected his Hcl? It was supposed to be 2 Hcl so that the equation would be balanced but anyway other than that thanks so much for this video u saved another life here because my teacher didn’t teach redox he only touched on oxidation and reduction and expected us to know the rest and scolded us for not knowing how to do and not putting in effort to learn, or if not he just asks us to go home and learn ourselves instead of him teaching. So big thanks to you my life is saved :))
Edit: he keeps forgetting to add a 2 to balance lol but it’s ok

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Sir for zn+hcl== h2+zncl2
Is balancing equation not nessasary

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[@ketamhamadneh2833]

How do I know which element I should find the oxidation number for, knowing that the question did not specify for me the element for which I should find the oxidation number?
For example, O2F2, what element should I find the oxidation number for?

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[@rkmalik159]

What about chlorine in second equation ? 5:42
Is it oxidising agent or reducing agent ?

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State the property exhibited by nitrogen (iv) oxide in each of the following equations:
4Cu + 2NO2--4CuO + N2;
H20 + 2NO2--HNO3 + HNOz.

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Sir can you please tell about 5clo3 + 3as2s3 + 9h20 = 5cl + 6h + 6h2as04 + 9s
Which one is what ??

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Im confused, is bromine the oxidized or is it the sodium bromide as a whole? Gotta ask for my homework.

[@ahhhhhhh_happpy]

what about identifying reducing agent and oxiding agent in a reaction that is written as a decomposition? like product (compound) --> reactants hg + n2 or osomething like that

[@javaughnbullard1995]

Alright let’s use the decomposition of water as an example. The equation would be 2H2O= H2 + O2. The oxidation number will be as followed +1 -1= 0 and 0. Hydrogen is getting reduced as it gained electrons. Oxygen is being oxidized as it lost electrons. Oxygen is being oxidized because of hydrogen so hydrogen is the oxidizing agent. Oxygen is the reducing agent since it is what cause hydrogen to be reduced.

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Why HCl is used in titration mixture?
K2Cr2O7+ 6KI+14HCl- I2 + 2CrCl3+8kCl

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In the second reaction there 2hcl I think so
Becoz product contains cl2 and individual h2

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[@Electric-Wind-Hook-Fist]

Where does it get the +2 charge though. I'm so confused..

[@ChemSimplified]

Because Mg is from Group 2, and it has 2 valence electrons. It will donate 2 electrons to become octet, therefore forming +2 charge. As for Br, it's fro Group 17 (or 7A) and therefore has 7 valence electrons. It will accept 1 electron to become octet, therefore forming -1 charge.

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[@shawnrodrigues2525]

does it matter in which state is each element?

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I don't think so.

[@sciencewithrita1182]

Fe + S =FeS ...can u tell what is oxidized agent and reducing agent in this reaction ???

[@eshitanagaria924]

Fe- Reducing agent
S- oxidising agent
Fe is getting oxidised as it's oxidation state becomes +2 from 0 so Sulphur is oxidising agent
S is getting reduced for its oxidation state becomes -2 from 0 so Fe is reducing agent

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