00:05 Light passing through a prism results in a visible spectrum. 01:06 Hydrogen emission spectrum shows specific frequencies of light. 02:09 Hydrogen atom's energy levels and electron transitions. 03:15 Hydrogen emission spectrum transitions 04:18 Hydrogen emission spectrum energy levels and transitions 05:28 Explanation of hydrogen emission spectrum lines 06:28 Hydrogen emission spectrum lines represent emissions from higher energy levels to the second energy level. 07:35 Hydrogen emission spectrum reveals discrete energy levels.
I'm in the mid of an MIT lecture on QM here on TH-cam, your video was very well of some help to get a better foundation to understand the content there. and you even enriched it
Why is the absorption spectrum the opposite of emission spectra?if it goes from 1 to 3 then it must absorb uv light cause it emits uv when it comes down directly from 3 to 1? From 3 to 2then it must be in the visible part and from 2 to 1 then in the uv part. The light with the energy given to the electron is in the uv spectrum and the light emitted is in visible part and the other one is in the uv part,then why is it that that the light missing in the absorption spectrum is the light in the emission spectrum??? Light absorbed is not the same as the light emitted.Is it???
See if this helps: 1. By changing the experimental setup, we can identify which frequencies of light are absorbed by electrons jumping up to higher energy levels OR which frequencies of light are released by electrons dropping down again. (This page has a useful diagram: casswww.ucsd.edu/archive/public/tutorial/Stars.html) 2. Yes, if an electron absorbs a certain frequency of UV light to jump up from n=1 to n=3 then it must release exactly the same frequency of UV if it drops down to 1 again. 3. Remember that we can only see frequencies in the visible part of the spectrum with our eyes. So although many other transitions are occurring, we can only see jumps from and drops to the n=2 level because the frequencies of those transitions happen to be the ones that relate to the visible spectrum. 4. For any given transition e.g. n=1 n=4, the frequency absorbed are exactly the same.
The light you will see coming from a normal bulb will probably release a small amount of UV and quite a bit of infrared but remember that we cannot see these frequencies with our eyes.
If the electron is initially in the first shell and moves to a higher energy level, why does it not go back to the first shell when it loses energy and stops at the second shell in the balmer series or 3rd shell in the paschen?
As the hyrogen atoms are being continually excited, the electron is continually moving up and down energy levels. It doesn’t stop anywhere which is why all the different transitions are possible. As soon as the heat or electricity is stopped, the electrons would return to the ground state.
@@cohesivechemistry Thank you so much that made it clear. But isn't at least uv light needed to get the electron out of the hydrogen atom because if moving from anywhere to the first shell would emit uv radiation. That must mean at least uv light is required to move the electron out of the first orbit, right? If yes then why does the other series exist besides lyman.
@@songokukun7248 Yes, an equivalent amount of energy to UV (or greater) would be required which is why we need to heat or pass electricity through the substance for it to begin 'glowing' (releasing visible light).
1. Because this is the only bit we can see with our eyes. To see the UV and IR emissions, we would need specialised equipment that is not found in schools) 2. There would be UV and IR emissions but we can't see them with our eyes!
If the photon in the uv is released when it comes down from 6 to 1 then it also means that it absorbed the same photon of that energy which is the uv then why in the absorption spectrum that uv part is not shown and the other colours are shown which were not in the emission spectrum?
Because we tend to focus on the absorptions and emissions that can be seen with our eyes (the visible part of the spectrum). Absorptions could also be seen in UV and IR parts of the spectrum but more specialist equipment is required.
Electrons can drop to any lower energy levels but it just so happens that when an electron drops to the n=2 level in a hydrogen atom, the amount of energy emitted corresponds to visible light.
hello, I have a question I was stuck with this question and even reading the answer, I could not understand it The Q.was do the lines converge at higher frequencies ? what does converge mean and why is the answer correct?? thank you so much!
'Converge' means that the lines get closer and closer together. And this happens in all atomic emission spectra. The fact that this happens indicates that as we move out from the center of the atom, the energy levels must also get closer and closer. At some point, the energy levels will be so close to each other that we have effectively reached the edge of the atom. Does this help?
@@Xxx87612 A line at a higher frequency means that the electron has released a larger amount of energy - so must have dropped a larger distance from where it started to where it ended up closer to the nucleus.
@@sasssss6265 Because a tungsten lamp uses tungsten in the solid state (and not the gaseous state like a hydrogen lamp), the atoms are very close to each other. This means their electric fields interact with each other and increase the energy states of the electrons. With more energy states, there are many more transitions seen on the spectrum (which ends up looking more like a continuous spectrum than a line spectrum).
Are you sure the electrons can drop back down to any of the lower levels ? My teacher said that it doesnt because the atom wants to be stable so the electron is always going to drop back down to the fundamental state where n=1
Yes, once we stop passing energy through the gas, the electrons will eventually end up in the ground state. But they can drop one/two/three levels at a time, or drop straight to n=1. This is why we have different series of lines in different regions of the electromagnetic spectrum. Does that clarify?
Why do certain English accents mix up their vowel sounds for no reason? I understand that diphthongs and the vowel's position relative to other vowels, consonants and accentuation can affect sound production but GAS & PASS? Ignoring the double S on pass (irrelevant here), why is it GAS but PAHS? Shouldn't it be either GAS & PAS or, if the A is lengthened in PAS, why do we not then also say GAHS? It's like when American's drop the T in Latin but not in Plato, so its LADIN on the one hand but PLATO on the other, even though the T is sandwiched between two vowels in each case! I'll shut up now. Superb video BTW.
![S1.3.2 The Line Spectrum of Hydrogen [SL IB Chemistry]](http://i.ytimg.com/vi/6rHerkru60E/mqdefault.jpg)
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Really awesome video. I was struggling with this topic for a while. But, now my concept is much more clear.
Glad it helped!
All the stress gone after watching this, god bless you thank you so much
BEST. So clearly explained. Thank you so much for making this video!
Glad it was helpful!
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Very well explained. I have seen so many videos but non of the video has explained the way you have explained. Thank you sooooo much
Very cohesive! Thank you sir! You've gained a new loyal subscriber!
Thank you so much i am from Pakistan and i have viewed all indian and Pakistani and all other chemistry channels but no one explained like you 🙌
Was searching for a video which was straight to the point and yeah, this is it.
really nice video. In my chemisrty class i was learning about this subject. Hearing you explain one line spectrum helped visualizing it!
Glad to hear it helped!
Go see mems
00:05 Light passing through a prism results in a visible spectrum.
01:06 Hydrogen emission spectrum shows specific frequencies of light.
02:09 Hydrogen atom's energy levels and electron transitions.
03:15 Hydrogen emission spectrum transitions
04:18 Hydrogen emission spectrum energy levels and transitions
05:28 Explanation of hydrogen emission spectrum lines
06:28 Hydrogen emission spectrum lines represent emissions from higher energy levels to the second energy level.
07:35 Hydrogen emission spectrum reveals discrete energy levels.
I'm in the mid of an MIT lecture on QM here on TH-cam, your video was very well of some help to get a better foundation to understand the content there. and you even enriched it
Glad to hear it helped, Alex!
Thanks so much, my modern physics exam is coming up soon and this helped a lot!
lovely video, had a presentation for my formatives on this. This video helped allot. Thank you < 3
Thank you so much! Cleared all my doubts about this topic :)
Wow, that is such a clear explanation, thankss :)
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Very well explained... thank you sir❤
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Enriching content and well explained. Thank you sir!
Good to hear ;)
So clearly explained. thank you
nice, this video gave me a full clarity
Glad to hear it!
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Well explained! Helped a lot :)
Glad to hear it!
Thank you so much sir!! This helped me a lot.
Excellent. Thanks for letting me know!
great video and graphics. Please explain visible light waves as hydrogen only has limited electrons therefore limited drop levels. Thank you.
I'm not sure I understand your question. What are you asking?
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Honestly wonderful. Tysm!
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Thanks for watching!
Why is the absorption spectrum the opposite of emission spectra?if it goes from 1 to 3 then it must absorb uv light cause it emits uv when it comes down directly from 3 to 1? From 3 to 2then it must be in the visible part and from 2 to 1 then in the uv part.
The light with the energy given to the electron is in the uv spectrum and the light emitted is in visible part and the other one is in the uv part,then why is it that that the light missing in the absorption spectrum is the light in the emission spectrum???
Light absorbed is not the same as the light emitted.Is it???
See if this helps:
1. By changing the experimental setup, we can identify which frequencies of light are absorbed by electrons jumping up to higher energy levels OR which frequencies of light are released by electrons dropping down again. (This page has a useful diagram: casswww.ucsd.edu/archive/public/tutorial/Stars.html)
2. Yes, if an electron absorbs a certain frequency of UV light to jump up from n=1 to n=3 then it must release exactly the same frequency of UV if it drops down to 1 again.
3. Remember that we can only see frequencies in the visible part of the spectrum with our eyes. So although many other transitions are occurring, we can only see jumps from and drops to the n=2 level because the frequencies of those transitions happen to be the ones that relate to the visible spectrum.
4. For any given transition e.g. n=1 n=4, the frequency absorbed are exactly the same.
Does the light we supply contain uv and infrared also?
The light you will see coming from a normal bulb will probably release a small amount of UV and quite a bit of infrared but remember that we cannot see these frequencies with our eyes.
@@cohesivechemistry the ones we see are which type of waves??
@@ASMR_Comfort24 They are the waves which have a wavelength between approximately 400-700 nm (known as 'visible light').
Thank you ☆☆☆☆☆
If the electron is initially in the first shell and moves to a higher energy level, why does it not go back to the first shell when it loses energy and stops at the second shell in the balmer series or 3rd shell in the paschen?
As the hyrogen atoms are being continually excited, the electron is continually moving up and down energy levels. It doesn’t stop anywhere which is why all the different transitions are possible. As soon as the heat or electricity is stopped, the electrons would return to the ground state.
@@cohesivechemistry Thank you so much that made it clear. But isn't at least uv light needed to get the electron out of the hydrogen atom because if moving from anywhere to the first shell would emit uv radiation. That must mean at least uv light is required to move the electron out of the first orbit, right? If yes then why does the other series exist besides lyman.
@@songokukun7248 Yes, an equivalent amount of energy to UV (or greater) would be required which is why we need to heat or pass electricity through the substance for it to begin 'glowing' (releasing visible light).
Best vid
Why is the emission spectra only the visible part ?
Why is there no uv or infrared
1. Because this is the only bit we can see with our eyes. To see the UV and IR emissions, we would need specialised equipment that is not found in schools)
2. There would be UV and IR emissions but we can't see them with our eyes!
If the photon in the uv is released when it comes down from 6 to 1 then it also means that it absorbed the same photon of that energy which is the uv then why in the absorption spectrum that uv part is not shown and the other colours are shown which were not in the emission spectrum?
Because we tend to focus on the absorptions and emissions that can be seen with our eyes (the visible part of the spectrum). Absorptions could also be seen in UV and IR parts of the spectrum but more specialist equipment is required.
Why are we using the second energy level
Electrons can drop to any lower energy levels but it just so happens that when an electron drops to the n=2 level in a hydrogen atom, the amount of energy emitted corresponds to visible light.
Are the electron of the hydrogen atoms in the same initial energy level??
Yes, in its 'ground state' each hydrogen atom would have 1 electron in the first energy level.
TYSM
hello, I have a question
I was stuck with this question and even reading the answer, I could not understand it
The Q.was
do the lines converge at higher frequencies ?
what does converge mean and why is the answer correct??
thank you so much!
'Converge' means that the lines get closer and closer together. And this happens in all atomic emission spectra.
The fact that this happens indicates that as we move out from the center of the atom, the energy levels must also get closer and closer. At some point, the energy levels will be so close to each other that we have effectively reached the edge of the atom.
Does this help?
@@cohesivechemistry thank you and what does higher frequency means here??
@@Xxx87612 A line at a higher frequency means that the electron has released a larger amount of energy - so must have dropped a larger distance from where it started to where it ended up closer to the nucleus.
@@cohesivechemistry that explain why tungsten emission spectrum seems really dense at the “blue edge”
@@sasssss6265 Because a tungsten lamp uses tungsten in the solid state (and not the gaseous state like a hydrogen lamp), the atoms are very close to each other. This means their electric fields interact with each other and increase the energy states of the electrons. With more energy states, there are many more transitions seen on the spectrum (which ends up looking more like a continuous spectrum than a line spectrum).
thanks a bunch :)
Are you sure the electrons can drop back down to any of the lower levels ? My teacher said that it doesnt because the atom wants to be stable so the electron is always going to drop back down to the fundamental state where n=1
Yes, once we stop passing energy through the gas, the electrons will eventually end up in the ground state. But they can drop one/two/three levels at a time, or drop straight to n=1. This is why we have different series of lines in different regions of the electromagnetic spectrum. Does that clarify?
@@cohesivechemistry thank you, it clarifies ! Thank you for your channel i learn a lot of things
thanks goat
Why is it that the light emitted is mainly red?
That is actually just because of my limited drawing ability. The white light should contain an even distribution of the different colours.
What’s the frequency of white light ?
'White light' contains all the frequencies in the visible part of the spectrum so has no specific frequency itself.
how to change if get n=3.78 when we calculate
Can you explain your question in a bit more detail? What are you trying to calculate and what data are you given?
thank you so muuuch
No problem.
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i thought thrre was one electron tho?
@@tulsipatel2161 In each atom, yes. But in the sample being excited there will be many.
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Why do certain English accents mix up their vowel sounds for no reason? I understand that diphthongs and the vowel's position relative to other vowels, consonants and accentuation can affect sound production but GAS & PASS? Ignoring the double S on pass (irrelevant here), why is it GAS but PAHS? Shouldn't it be either GAS & PAS or, if the A is lengthened in PAS, why do we not then also say GAHS? It's like when American's drop the T in Latin but not in Plato, so its LADIN on the one hand but PLATO on the other, even though the T is sandwiched between two vowels in each case! I'll shut up now. Superb video BTW.
Hmm, valid questions but possibly a little beyond my area of expertise 😅
America has win zat ho oqat ho
TYSM