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?
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
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.:)
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.
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.
Wow thanks, this cleared up all the confusions I had with this topic!
This video was indeed helpful!!! Well explained. Thank you veryyy much✨
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?
Could you post some more examples with the oxidizing and reducing agent equations please?
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
Thank you. I'll be looking forward to the video.
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.:)
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.
Thanks alot
This really helped me to understand Redox reactions a little better
Redox can get a bit confusing
@@csecchemistry There was nothing in the exam involving redox reactions today
@@isabellina50💀
Thankyou for this
Thanks so much. I understand perfectly now.
Thanks this helped
Good morning Mr Terry notes
I how can I get a one grade in chemistry
You have to review your notes every week and practices past papers
@@csecchemistry thank you
@@csecchemistry I some problems with redox calculations
Is this all we need to know on this topic?
Yes
Thank you so much, you teach so calmly I finally understand this topic 🙏
Glad it was helpful!
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.
Do you help with SBA