CSEC Chemistry - Oxidation and Reduction

[@darion3780]

Wow thanks, this cleared up all the confusions I had with this topic!

[@sherikawilliams7868]

This video was indeed helpful!!! Well explained. Thank you veryyy much✨

[@isabellina50]

Thanks alot This really helped me to understand Redox reactions a little better

[@csecchemistry]

Redox can get a bit confusing

[@isabellina50]

@@csecchemistry There was nothing in the exam involving redox reactions today

[@Jerry_JesusChrist]

@@isabellina50💀

[@stargirl3459]

Thankyou for this

[@ares8752]

At 17:53 wouldn't it be hydrogen? Since hydrogen is in nitrogen hydride so the charge of hydrogen would be -1 and since the hydrogen in water has a charge of +1 wouldn't it have increased in oxidation number?

[@tiff_samaroo]

Thank you so much, you teach so calmly I finally understand this topic 🙏

[@csecchemistry]

Glad it was helpful!

[@shalinilalchan4812]

I understand how manganese is an oxidising agent but I made the mistake of using hydrogen as a reducing agent since it went from a 0 to 1 I think.My problem is I am confused how you used iron because aren't you supposed to put it as 0 since it is in it's free state?I get confused when to put the 0.Please explain.:)

[@csecchemistry]

When we say free state we mean how does it exist at normal temp pressure etc. Iron (III) is an oxidizing agent. It's oxidation state is +3 initially. When it acts as an oxidizing agent it changes into iron (II) which has an oxidation state of +2. It is therefore reduced in the process.

[@tysam5867]

Thanks so much. I understand perfectly now.

[@ThaMemeMaster]

Thanks this helped

[@daniellerowe2111]

Could you post some more examples with the oxidizing and reducing agent equations please?

[@csecchemistry]

Danielle Rowe Hi Danielle, The ones presented in this video are the most common ones brought in the exams. Focus on the following:1. How to determine oxidation numbers? 2. Once you've determined oxidation numbers it is easy to figure out what is being oxidized or reduced. 3. If the oxidation number of a particular species has increased, then it has been oxidized. 4. If the oxidation number of a particular species has decreased, then it has been reduced. If I come across any other equations. I'll post them. Regards Terry

[@daniellerowe2111]

Thank you. I'll be looking forward to the video.

[@eric3524]

Is this all we need to know on this topic?

[@csecchemistry]

Yes

[@debraplummer1117]

Good morning Mr Terry notes I how can I get a one grade in chemistry

[@csecchemistry]

You have to review your notes every week and practices past papers

[@debraplummer1117]

@@csecchemistry thank you

[@debraplummer1117]

@@csecchemistry I some problems with redox calculations

[@ownitervi241]

9:45 a tip my teacher gives us is: an substances is never the agent of what it undergoes. So if its being oxidized, it can only be a reducing agent, never an oxidizing agent.

[@debraplummer1117]

Do you help with SBA