Emission spectrum of hydrogen | Chemistry | Khan Academy
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- Опубликовано: 11 сен 2024
- Using Balmer-Rydberg equation to solve for photon energy for n=3 to 2 transition. Solving for wavelength of a line in UV region of hydrogen emission spectrum. Created by Jay.
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Chemistry on Khan Academy: Did you know that everything is made out of chemicals? Chemistry is the study of matter: its composition, properties, and reactivity. This material roughly covers a first-year high school or college course, and a good understanding of algebra is helpful.
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you are more than just a youtuber..i just cannot express how much your videos help me in emergency situatuions( tests) ..thanks a loot
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Same
this went in through one ear and out the other
Dude u are great .... Finally i understood this topic well . Khan academy ur my life line xD
im going to fail out of college lol
same
College , we Indians have this in high school
PERSEVERE PUSSBOI!
college??? Im here for 10th grade chem lmao.
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So much help! Wish the volume was louder. Thank you
thank you very much for the video. at video time 09:25 you omitted one zero on the reciprocal of lambda =8227500
THANK YOU! I love what you've done with the Rydberg equation.
What is the significance of going from the 6th level to the 2nd as opposed to going from the 2nd level down to the 1st?
My science project is on air temp+ the hydrogen emission spectrum. This helps a bunch!!
great videos
I can’t find the previous video, so can someone explain why hydrogen starts off with n=2
Cuz the line spectrum formed is for Balmer series, which is n=2, where an electron cannot fall from 2 to 2.
@@yugeneshr.k.anumanthan1152Ik this is 3 years later and ur prolly in college or sm, but the balmer series (which emits only visible spectrum of light/electromagnetic radiation), only emits visible light when it falls from the excited state to the n=2 state?
And I thought Khan Academy wouldn’t be able to help me through college too
Really insightful, kinda hard when I’m just reading from a book
Awesome ❤️
Since we know that the Energy of the radiation emitted is equal to the difference in the energy of the atom before and after emmission, can we just calcuate that difference and then use E=hc/λ?
Do you get half the day to work on an exam?
you've taken
Ej -Ei = hc/wave length
by this equation you are saying that only one photon is emitted during emission.
Is it correct ??
I'll be waiting for your answer..
There's no answer
Thanks dude you're amazing!
Thank you! This is awesome and helpful. Some constructive criticism: might want to be a bit more careful about keeping the units through the equation. You had it covered, but it's helpful for me to see that.
So if Hydrogen has only 1 electron, why would there be multiple electron transitions/multiple wavelengths of light produced? Shouldn't there only be one transition occurring producing one wavelength of photon?
KevNoonz according to me, to excite hydrogen particles current is passed through some quantity of hydrogen gas. in it some particles would get more excited than others - the emission Spectra covers all of the possibilities. again this is only my understanding and I'm just a student
KevNoonz hydrogen does'nt hav any e- it has only one proton and the proton is excited frm 1 enrgy lvl 2 anthr.. that's just one
okay so ignore everything Manju said
Where did you pull that lie from? Hydrogen has one electron and proton.
It's true that there is only one electron in an hydrogen atom, but there can be many different energy states of this electron. What this means is that depending upon the energy being supplied to the electron it gains that amount of energy , becomes excited and jumps to the corresponding energy level. There are hence multiple energy levels (infinite) that the electron can transit to, the infinite one having 0 energy (free electron). After the electron becomes excited and jumps to another energy level, it is unstable hence transits back to it's initial enegry level by releasing the difference energy in the form of EM waves. Hence depending upon the difference between the two energy levels the energy of the emitted wave is different and hence the possible wavelengths are many and different.
What happens after an electron falls from higher energy level to the 2nd energy level? It emits photon...then it must fall to the ground energy level and emits UV. BUT is the photon first emitted still visible?? If yes,then for how much time does it remain visible and for how much time is the spectrum visible?
Very neat explanation. Thank you very much.
Excuse me if I'm wrong, but instead of drawing the squiggly arrows representing the colour of light emitted, shouldn't they be dots? (Because light is quantized in packets of energy)
Light behaves as photons but also as waves, which is why we talk about them having a wavelength (eg. 656 nanometeres).
So i = lower energy level, not initial??
Bless you for actually explaining all the algebra
FINALLY Geez you have no idea how many videos i went through just to see someone do it the right way =_=
You're the best
Me looking at this
👁👄👁
Thank you, you are great.
So, I when you said that "a proton red light is giving off as one electron moves from one energy level to another" does that mean that actually the colors represents the protons colors? Does that has to do with the fact that protons are located in the nucleus where the mass is located?,
A "photon"
how calculate energies of other elements (analogous to Rydberg constant for Hydrogen)?
omg so intresting!!!
Great explanation
THANK YOU
why line spectrum for each element is unique . as the nature of electron is same it should emit light of same wavelenghts when it jumps to any orbit and comes back betwween same energy levels in any atom
saved the day
at 9:40 you write 822750 but it is 8227500, just saying.
Good job though, i really understand this!
im pretty sure this has to do with the rules of sig figs.
Good work you have done.but it is not much audible as your voice is low
Great video
Thank you so much, only complaint is that the volume is too low
I should've found you earlier, better late than never.
I love you!
Brilliant, saving me from doing loads of articles and textbooks.
In which play list can I view the whole series
Khan Academy
Are Protons not to be seen as colours?
If you change the Balmers constant to B=91.126705 by deviding it by 2² (because 364.50682 is the Balmers series) and use the formula Wavelength = BN²(n²/(n²-N²)) N being the series N=1 lyman N=2 balmers etc. Now you can use the Balmers to calculate all the wavelengths of hydrogen with ease and answers in nm so simple =) your welcome.
thanks for this useful video
¿Cómo se obtiene el espectro de la radiación invisible?
Tysm For this
i am confused that how to distinguish between cathode rays and the emission light, both are emitted from a discharge tube ???
when is more energy released. when electron jumps from n=3 to n=2 or n=3 to n=1
N=3 to n=1
it should be 1.097x10 to the -2 not 7
cool
But ,hydrogen has only one orbit ,so how does it hav 2,3,4,5 energy levels?
think of it as this, if H gains an electon, the second e. will be in the 2. orbit. 3,4,5... so on.
Every atom has infinite energy levels but electrons are placed on very few of those energy levels
What does the 1 over lambda mean? - specifically what does the 1 represent?
One over lamda represents wave no.
Thanks, so if I had x2 it represents such?
troy lenny maybe a bit late- but 2 multiplied by the wave number in response to your latest question.
2/lambda is the same as 2 * 1/Lambda.
Is this part of a high school or college course in the US?
High school part in Physics-India
finally, I'm understand this topic, thanks😂😂😂😂😂
No clear sound
What does it mean "electrons falling to 3 to 2?
When electrons absorb enough energy, they will be excited from their ground state (n=2) to a higher energy level (n = 3). They won't stay in that state though because it's unstable. So the electron will release that energy it absorbed and fall back to it's ground state (n = 2). When it does that, the energy it released was in the form of light, which we see as red light.
this was very helpful
Why don’t we get colours like yellow n green
but if the electrons were absorbing energy, why did the emission lines show up at all?
It's my understanding that the electrons absorb energy, but once they absorb a certain amount, they release energy as they fall back to lower levels, and that is when the lines show up.
An electron absorbs energy and stay in hihger energy level for about 10^-6 secs to 10^-8secs. And return back to lower energy levels thus emissions occurs
How do you get wavelengths between these set levels?
xhmeia g lykeiou brought me here
1/4 is 0.25 not 0.75
1/1 - 1/4 =3/4 which is 0.75
check your facts
Correct, but he was subtracting 1/4 from 1 which is 0.75. He wasn't saying that 1/4 was 0.25.
perfect!
1.25 speed.... trust me... Great lecture tho
But doesnt hydrogen only have one electron?
Hydrogen atomS
I am seventh class but I have this concept lol
Thanks bro, I understood this concept just because of you
준호게이야 고맙노
How does the formula came from... :)
Nice video though!!
Hindi
The loud volume is so low that I almost can't hear anything. Other RUclips videos are much louder. Could anyone help me why?
I've never seen it before.
But I suggest you see some interesting videos on SALEH THEORY-com about behaviors of photon.
This is GG shit !!
My teacher sent me this video. I'm dropping out of her class
Spent 4 minutes of the video plugging and chugging. Sad.
Sal I love you!
great video