For anyone who would like a more simplifed version of the cell notation then this is how I do it. So think "ROOR" like Katie perry's song and think R O O R - reduced, oxidised, oxidised , reduced, rather than thinking about how close the ZN2+ is to the salt bridge think about which thing is being reduced or oxidised.
I have a PhD in chemistry and just started teaching chemistry in a secondary school and I find your teaching is brilliant. I even advise my students to watch your channel. So, many thanks for all great videos you have produced.
At 22:00 you mention that reduction is the loss of electrons; is it not gain? And also you mention that a reducing agent gains electrons but will it lose them?
Hi he must have made a mistake, reduction is gain of electrons and a reducing agent loses electron, basically gives electrons to the other species causing reduction (gain of electron)
at 22:02 you said "reduction is lose of electrons and reducing agent gains electrons ," isn't that other way around? reduction is gain of electrons and reducing agent loses electron , is this what you meant ?
a reducing agent reduces something else by getting oxidised. this means a refusing agent does gain electrons, as it itself gets oxidised as it reduces something else. a substance that gets reduced loses electrons. if we were talking about oxidising agents, they oxidised something else and themselves get reduced. i hope that makes like a slight bit of sense😭 good luck tommorow if ur doing it
Hey, thank you very much for your videos, they are really really helpful. The only thing is I'm a little bit confused by the use of the words positive and negative electrodes when talking about the alkaline hydrogen-oxygen fuel cell; from the point of view of current flow isn't it the other way around, isn't no.5 the posotive electrode and no.7 the negative electrode as conventional current flows in the opposite direction to electron flow? I'm probably just misunderstanding, either way your videos are super helpful, you're doing gods work ;) thanks
How does an organic flow battery work? For instance when quinone gets oxidized to a hydroquinone, both quinone and hydroquinone are neutral so how does an organic battery hold a charge?
Question: As the zinc electrode loses its electrons to the voltmeter, does this cause the solution to become Zn2+, or is the solution Zn2+ prior to the Zn electrode losing its electrons and thus increasing the concentration of Zn2+ ions?
No- it is strange but in electrochemistry I'm sure you never multiply by the coefficient. The Value found in the electrochemical series is the same no matter how much there is
It's because the salt bridge connecting the two solutions allows for the flow of ions however this shouldn't be mistaken for a current. We remove the high resistance voltmeter when we want the current to flow and replace it with something like a bulb. The high resistance voltmeter in this instance can be represented by, lets get marreid.
I am having a bit of confusion with the NO PRoblem acronym, if oxidation occurs at the negative half cell, in the example at 15:24 if Zn is oxidised why would it not be the anode? Because at 23:49 if the strongest oxidising agents have the most positive values wouldn't Copper be the anode?
In the fuel cell how does the water from 8 get to the oxygen at 4 to make the oh- ions because the diagram doesnt show how this happens.Or is the water from somewher else?
electrons flow through the voltmeter,, but also the voltmeter is high resistance to stop current (the flow of electrons)? could someone explain this to me TT
So if commas are only added between 2 aqueous ions, what about 2 gaseous ions , would you include commas there? And when else would you include commas in the cell representation?
he just added both the oxidation and reduction equations together. Why Li+ doesn't appear in the overall equation is because it appears on opposite sides of the reduction and oxidation equations (Li+ is on the product side in the negative electrode and also appears on the reactants in the positive electrode) so you cancel it out. when given redox equations, if they appear on different sides, you cancel them out. But if they appear on the same side( ie both on the reactant side or both on the product side of both half equations) you add them in the overall equation I hope this helps :)
reactivity has nothing to do with it necessarily, electrons will flow from the negative to the positive electrode as electrons are negative and attracted to positive electrode. in this context electrons always flow away from the most negative electrode.
IN HALF CELLS:- electrons flow from a more reactive electrode towards a less reactive electrode. so the more reactive electrode is negative and the less reactive electrode is positive (as shown by their standard electrode potential values.)
For anyone who would like a more simplifed version of the cell notation then this is how I do it. So think "ROOR" like Katie perry's song and think R O O R - reduced, oxidised, oxidised , reduced, rather than thinking about how close the ZN2+ is to the salt bridge think about which thing is being reduced or oxidised.
it's also how you write a ester
That's helped so much. Thanks
If u can't even memorize ROOR you are bit fucked bro💀💀💀
you're a hero. Paper 1 is tomorrow and I never understood this until now.
Did u do well?
Same my paper 1 is in 4.5 hours😭🙏🏾
@@s4lly79 bro a levels are in june
@@neldino1251 Late but it was prob mocks
[Timestamps]
Electrode Potentials and Cells (1.11.1)
2:51 = Half Cells
5:26 = Electrochemical Cell Set-up
10:23 = Electrode Potentials
15:26 = The Standard Hydrogen Electrode (SHE)
20:10 = The Electrochemical Series
24:39 = Calculating Standard Cell Potential
28:15 = Conventional Cell Notation
31:51 = Predicting Reaction Feasibility (+ finding overall equations)
*****
Commercial Applications of Electrochemical Cells (1.11.2)
37:39 = Batteries: Rechargeable/Non-rechargeable
39:52 = Lithium ion battery: half/overall equations
42:20 = Fuel Cells
48:09 = Advantages + Disadvantages of Fuel Cells
god
Rachel Doran? More like LEGEND DORAN TYSM
you are a beauty for this
cheers pal
U absolute angel
bestie ur getting me through my a levels i hope u know that-
Would you like to be my second wife? xx
brilliant teacher, been struggling with this topic a little and this video has really helped my revision and filled some gaps thanks mate :)
i loved how u linked no problem with electrode potential thank you sooooo much!
You're very welcome 😀
wanna make a link with me?... ;) +----- 🔋 ( I'm 23) (resitting for the 5th time) (on u xd)
never assume malice when it can be explained by stupidity
@@AlleryChemistry imagine you replied to that persons comment saying " No Problem" Loool
Have a test on this tomorrow! Thanks for this video it’s really helpful :)
Glad it was helpful!
you no what your a NO PROBLEM teacher and i am sure i would have NO PROBLEM with this for my mocks.. thanks a lot for this
no problem
no problem
I have a PhD in chemistry and just started teaching chemistry in a secondary school and I find your teaching is brilliant. I even advise my students to watch your channel. So, many thanks for all great videos you have produced.
Thanks for using them and for recommending them, really appreciate it.
Why didn’t you go into a job in your field?
@@jafwonta that's what I wonder about alot of teachers
Thank you so much sir I just discovered your channel and you make the most efficient videos ever!!
great videos! can you please do some videos on aqa required practicals please
if I can crack these questions now, all the credit goes to you and miss natalie❤
thank you so much Mr Allery. You single-handedly saved my A-Level. Thank you.
up at 2 fucking hell goodluck not falling asleep
@@Cars.r.us2023 yo how was it bro
At 22:00 you mention that reduction is the loss of electrons; is it not gain? And also you mention that a reducing agent gains electrons but will it lose them?
Hi he must have made a mistake, reduction is gain of electrons and a reducing agent loses electron, basically gives electrons to the other species causing reduction (gain of electron)
Hi, I think that was a minor mistake; reduction is the gain of electrons and reducing agents themselves are oxidised.
Noticed the same thing
Yh it was just the slip of the tongue. A reminder to get it the right way round in ur exams!
Was looking for this comment lmao
@44:44 i thought the negative electron was the ANODE?
physics don't leave me alone
fr
I won't leave you alone.
@@UNKNOWN-jk6wv thats creepy
I hate a level chemistry and I wish i never did it
What grade did you get?
READ THE DESCRIPTION AS HE HAS MADE A SUBTLE ERROR IN THE VIDEO.
Great video understood it so much better
at 22:02 you said "reduction is lose of electrons and reducing agent gains electrons ," isn't that other way around?
reduction is gain of electrons and reducing agent loses electron , is this what you meant ?
yhhh
a reducing agent reduces something else by getting oxidised. this means a refusing agent does gain electrons, as it itself gets oxidised as it reduces something else. a substance that gets reduced loses electrons. if we were talking about oxidising agents, they oxidised something else and themselves get reduced. i hope that makes like a slight bit of sense😭 good luck tommorow if ur doing it
do we need to know word to word the nine steps of the alkaline hydrogen oxygen fuel cell or just the 2 equations on the summary
thankss! do we need to fully know every single step of the reactions in the fuel cells?
this is such a good explanation thank you! love the acronyms too
Hey, thank you very much for your videos, they are really really helpful.
The only thing is I'm a little bit confused by the use of the words positive and negative electrodes when talking about the alkaline hydrogen-oxygen fuel cell; from the point of view of current flow isn't it the other way around, isn't no.5 the posotive electrode and no.7 the negative electrode as conventional current flows in the opposite direction to electron flow?
I'm probably just misunderstanding, either way your videos are super helpful, you're doing gods work ;) thanks
hi have you found the answer to this? I'm confused aswell :(
I know that electrons flow towards the positive because the species in no.5 are meant to be positive so it can gain electrons therefore reduce. Right?
nah dude you’re right, i was confused too lol
really helpful vid, thanku very much :)
No problem!
THANK YOU !!!!!!!!!!!!!
How does an organic flow battery work? For instance when quinone gets oxidized to a hydroquinone, both quinone and hydroquinone are neutral so how does an organic battery hold a charge?
Thank you!
Thank you so much😭
No problem 😊
why are you crying to another man?.
Thanks
No problem
Question: As the zinc electrode loses its electrons to the voltmeter, does this cause the solution to become Zn2+, or is the solution Zn2+ prior to the Zn electrode losing its electrons and thus increasing the concentration of Zn2+ ions?
At 37:17, do we not multiply E value of Fe by 2 since there’s 2 lots of it ?
No- it is strange but in electrochemistry I'm sure you never multiply by the coefficient. The Value found in the electrochemical series is the same no matter how much there is
If we use a high resistance voltmeter, why does the current still flow from Zn electrode to Cu electrode
It's because the salt bridge connecting the two solutions allows for the flow of ions however this shouldn't be mistaken for a current. We remove the high resistance voltmeter when we want the current to flow and replace it with something like a bulb. The high resistance voltmeter in this instance can be represented by, lets get marreid.
Thank you 🙏
You’re welcome 😊
I am having a bit of confusion with the NO PRoblem acronym, if oxidation occurs at the negative half cell, in the example at 15:24 if Zn is oxidised why would it not be the anode? Because at 23:49 if the strongest oxidising agents have the most positive values wouldn't Copper be the anode?
Here is another acronym..
An Ox ( Anode oxidation)
Red cat ( reduction cathode )
so with the fuel cells in step 5 the electrons flow to the anode and in step 7 the electrons flow away from the cathode to the anode?
In the fuel cell how does the water from 8 get to the oxygen at 4 to make the oh- ions because the diagram doesnt show how this happens.Or is the water from somewher else?
I am confused, I thought the most negative value is the reducing agent so how is magnesium the oxidizing agent at 33:51
do we have to know and memorise the compounds that make up the electrode in the batteries?
electrons flow through the voltmeter,, but also the voltmeter is high resistance to stop current (the flow of electrons)? could someone explain this to me TT
So if commas are only added between 2 aqueous ions, what about 2 gaseous ions , would you include commas there? And when else would you include commas in the cell representation?
I think you add commas between two or more things that are the same state
you use commas when they're in the same phase so it can be used for liquids and gases also
41:12 can someone explain how he got the overall equation on discharge ???? I dont get it ???
he just added both the oxidation and reduction equations together. Why Li+ doesn't appear in the overall equation is because it appears on opposite sides of the reduction and oxidation equations (Li+ is on the product side in the negative electrode and also appears on the reactants in the positive electrode) so you cancel it out. when given redox equations, if they appear on different sides, you cancel them out. But if they appear on the same side( ie both on the reactant side or both on the product side of both half equations) you add them in the overall equation
I hope this helps :)
life.saver.
i hate this topic and i have my a level paper 1 tomorrow help
How did chemistry go
What grade did you get.
me rn
What happens if the voltmeter is replaced with a wire and what would you observe in each half cell?
it wouldn’t work the ions would just reach equilibrium and the whole thing would become 0V
15:45 we are crying LOL
Do electrons flow from a more reactive metal to a less reactive one or from the postive electrode to the negetive electrode?
reactivity has nothing to do with it necessarily, electrons will flow from the negative to the positive electrode as electrons are negative and attracted to positive electrode. in this context electrons always flow away from the most negative electrode.
IN HALF CELLS:- electrons flow from a more reactive electrode towards a less reactive electrode. so the more reactive electrode is negative and the less reactive electrode is positive (as shown by their standard electrode potential values.)
when do you use an iron electrode and when do you use a platinum electrode
Have a watch of 3:20 - 4:49 and let me know if that was helpful. Especially the end of that time frame should clear it up a tad
IMPROTNAT. Read the description as he made an error in teh video which he explains i nthe descriptuni
4:25
im cooked