I was out with my bio class on a field trip so I missed this in school, and the trip made me sick therefor i lost even more days of school. But thanks to you i know i can catch up again, this is my first time on your channel hope you have more vids like this one! thanx
oh wow the method my teacher taught us is much much simpler, basically just shortcuts through most of the legwork, i'll try and write it out if you're looking for something more brief 1. write out oxidation states, as you do, as well as adding 1/2 in front of things like Cl2 etc 2. count how much each thing got reduced or oxidized; switch the numbers, and multiply them into the equation 3. count the total charge on each side, by counting, and add H+ or OH- to balance it 4. count the oxygens, and add water where appropriate, and then count the H's to check
OMG thank you! Btw I thought you have Pakistani ethnicity because of you're last name than I went on you're Wikipedia and it says that you're actually a Bengali, and I was like OMG, I am a bengali too and I am so proud because you're so smart and you're helping so many students and you are one of us. Haha.
Don't we have in the end on the left side 2*7 O=14O --> on the left side we have only 7*O=7O so don't we have to multiply the H2O and H+ with 2 that we get it completly balanced?
In my 8th grade class, basically the reason why electrons are needed to be balanced because if there is at least one electron remaining in the reaction, it will unbalance everything. As long as if there are no signs of electrons in your balanced reaction, it is balanced. Electrons counts like a negative charge so if you add it to any sides depending on its side, your reaction isn't balanced.
Due to law of conservation of mass. Although the mass of an electron is considered negligible , you cant do that with conservation of mass law cuz even such a small mass defect gives out considerable energy. So ya . U habe to balnce charge.
I dont understand, why didn't he come up with the charge of 7H2O in the reduction half reaction.... He just did got the charge of 2Cr wich was 6+, why not the one of h2o
remember this memory tip....... OIL RIG...... oxidation is loss of electron.... reduction is gain of electron .... so as cl- goes from -1to 0 .i.e if cl- looses 1e then it goes to 0 state thus oil i.e. oxidation
Khan Academy is always there for me when my teacher isn't. Which is always!
true fact!!
bro, you just saved my life.
I was out with my bio class on a field trip so I missed this in school, and the trip made me sick therefor i lost even more days of school. But thanks to you i know i can catch up again, this is my first time on your channel hope you have more vids like this one! thanx
Best video that i have seen on this topic . thankyou very much for making me understand this
I needed this clarification. Makes a lot more sense now. I like this guy better than the other guy
Just know that even after 8 years, your explanations are better than my lecturers and tutors
Khan academy is best way for learning from youtube i got first in class from khan academy thanks ☺️☺️☺️☺️
Thank you so much! My chemistry teacher confused me so much with redox reactions and you clarified!
god bless you
This is a gift for everyone who's interested to learn. Thank you so much.
why is it so hard for my professor to explain such basic concepts while this man can do it very easily.
I will be very thankful if you give a video on balancing the redox reaction using oxidation no. method of acids and bases.
OIL RIG
Oxidation is loss and reduction is gain. (Of electrons)
this is so much better than leo says ger
This is a really clear step-by-step explanation. Thank you!
The Best Explanation!!♥♥♥
Thanks a lot.
My teachers confused me in those last two steps!!! But now I got it!!!
The electron part was confusing me. Thanks for clearing it up!
Same
wow you have the skill to break something down.thanks saved me
The best video ever on youtube
oh wow the method my teacher taught us is much much simpler, basically just shortcuts through most of the legwork, i'll try and write it out if you're looking for something more brief
1. write out oxidation states, as you do, as well as adding 1/2 in front of things like Cl2 etc
2. count how much each thing got reduced or oxidized; switch the numbers, and multiply them into the equation
3. count the total charge on each side, by counting, and add H+ or OH- to balance it
4. count the oxygens, and add water where appropriate, and then count the H's to check
Putting half equations together used to be pain in the ass. Now it's a bliss for my brain.
very good explanation, steady watching in 2016
Never thought it was this simple. Thanks man
nicely done and very simple, got it
Really cant thank you people enough!
Man u r awesome.Thanks to khan academy.
You never let me down!!❤️
This just clarified a lot for me, thanks for sharing!
That's really a wonderful job.keep going. Thank u soooo.... much
you saved my life, thank you so so much!!!
Thank god for this video, finally understand it!
Will you be organizing these MCAT videos in a playlist?
This is just what I needed!
Very helpful
Deeksha Aggarwal true
Deeksha Aggarwal where do u live in india
Skipper did an excellent job in the place of Salman
Love the content, but next time, please don't screencast in 360p. It makes it a bit hard to read.
Awesome. khan Academy, u teach brilliant
super helpful, thank you
Very Good video. Thanks!!!!!!!!!!
Thank you! it was really clear and easy to understand :)
guys you don't know how thankful I am right now . thank you so very much our book added two extra steps which made it complicated
great explanation as all ways.
Very helpful! Thank you
Thanks a lot now i get it :D
Thanks! Ur the best
This was brilliantly explained. Thank you! :D
4:30 But since there are 2Cl- isn't that two chlorines with a -1 oxidation states???
Sir, how did the chemical equation Cr2O7 ^ -2 ---> Cr^3 become the reduction reaction? It also lost electrons, right?
It didn't lose electrons there is gain of electron,analyse carefully! (+12------>+3 i.e 9 electrons are gained)
VERY NICE!!!!!
Thank you sooooooooooo much!
Thank you!
OMG thank you! Btw I thought you have Pakistani ethnicity because of you're last name than I went on you're Wikipedia and it says that you're actually a Bengali, and I was like OMG, I am a bengali too and I am so proud because you're so smart and you're helping so many students and you are one of us. Haha.
That is not Sal that is speaking in this video. It's a friend of his, Jay. Jay does most of the advanced chemistry videos.
stfu it doesnt matter what he was before, what matters is what he is now, he is american
reduction is a reduction of charge (gaining electrons, gaining negative charges)
Don't we have in the end on the left side 2*7 O=14O --> on the left side we have only 7*O=7O so don't we have to multiply the H2O and H+ with 2 that we get it completly balanced?
thankx a lot.
How did you get oxidation number 0 for Cl2 ??
Suzan Razak The oxidation number of free or isolated atoms is equal to zero.
Wasif Shakil thnk u....i also had the same question
Great video and explanation but the 360p hurts my eyes
Max Patten cmon you r studying .not watching a movie
OIL RIG
Oxidation is Loss Reduction is Gain ( of electrons)
Oh my God thank you so much
God bless y'all
SIR U ARE 2 G00D
Thank you
Because Cl2 is covalently bonded, there is no exchange of electrons and the charge of each Cl is zero.
Thank you so much!
wow you are the best
its just not the same without sal's voice.
Thanks anyway
Sal goes too slowly. This guy is much better--he goes directly to the point
Both are equally good
ger --gold experience requiem
where did that come from?
In the last step why do you have to balance the electrons?
In my 8th grade class, basically the reason why electrons are needed to be balanced because if there is at least one electron remaining in the reaction, it will unbalance everything. As long as if there are no signs of electrons in your balanced reaction, it is balanced. Electrons counts like a negative charge so if you add it to any sides depending on its side, your reaction isn't balanced.
Due to law of conservation of mass. Although the mass of an electron is considered negligible , you cant do that with conservation of mass law cuz even such a small mass defect gives out considerable energy. So ya . U habe to balnce charge.
This was beautiful, I actua
please give me this as soon as possible.
omg i wish i saw this vedio earlier
Why is it necessary to break it up into the half reactions? Why are we not allowed to just balance the equation as normal?
Then balancing Electrons would be hard
I dont understand, why didn't he come up with the charge of 7H2O in the reduction half reaction.... He just did got the charge of 2Cr wich was 6+, why not the one of h2o
Thanks
If cl (-1) goes to cl (0) isn't that a reduction and not an oxidation?????
remember this memory tip....... OIL RIG......
oxidation is loss of electron....
reduction is gain of electron ....
so as cl- goes from -1to 0 .i.e if cl- looses 1e then it goes to 0 state thus oil i.e. oxidation
Boss boss boss that all what I can say !
Why don't the elements in the beginning have an oxidation number of 0?
Madison Barney
Elements that stand alone always have 0 charge. It's a rule
Madison Barney eell why dont u simply check out the rules to find oxd state(not number . Both are different) or else i have to write alot.
WHAT HOW? EITHER WAY THE REACTION GOES FROM 0-1 3-6 or 6-3 1-0 HOW DOES THAT WORK THATS BOTH INCREASE OR BOTH DECREASE
Why is cromime 12?
+Avantika Badgujar (-14) goes to the other side and become (14 - 2 = 12)
Avantika Badgujar u indian
The compound's charge is -2 so you need to assign Chromine's oxidation number that if you add it to -14, it becomes -2.
bless
Still don't understand about the assigning oxidation states
I love you.
If you pretend, it sounds like Taco from The League giving the lesson.
gr..8 dude :)
THANK YOUUUU!!! T___T
This method is not working for me for all problems. Try
ClO3- + I2 = Cl- + IO3-
This method is useless to me for that problem
Ger
BRING SALL BACKK LMAOO
What. The. Heck.
You aren't sal !
stop going soo fast dude!
Thanks a lot.
Thank you so much.
thanks a ton