S1.3.1 - The hydrogen emission spectrum

[@leonardonicologentile7013]

mental clarity after this is WILD

[@cohesivechemistry]

🙌

[@justanorange10598]

ong

[@kiyajeon]

FOR REAL

[@AhmadAli_1.0]

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 🙌

[@isuofficial9240]

Really awesome video. I was struggling with this topic for a while. But, now my concept is much more clear.

[@cohesivechemistry]

Glad it helped!

[@dipteeshukla7]

BEST. So clearly explained. Thank you so much for making this video!

[@cohesivechemistry]

Glad it was helpful!

[@parislondon9014]

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

[@kiyajeon]

lovely video, had a presentation for my formatives on this. This video helped allot. Thank you < 3

[@amberhuo206]

Very cohesive! Thank you sir! You've gained a new loyal subscriber!

[@dubudubuur]

sir thank you, everything was so clear and it makes sense now! you've just earned a subscriber

[@colinvanh251]

really nice video. In my chemisrty class i was learning about this subject. Hearing you explain one line spectrum helped visualizing it!

[@cohesivechemistry]

Glad to hear it helped!

[@4shm1t37]

Go see mems

[@shmaptainshmerica6152]

Wow, that is such a clear explanation, thankss :)

[@AlexTrusk91]

I'm in the mid of an MIT lecture on QM here on KZbin, your video was very well of some help to get a better foundation to understand the content there. and you even enriched it

[@cohesivechemistry]

Glad to hear it helped, Alex!

[@vxillity9917]

Thanks so much, my modern physics exam is coming up soon and this helped a lot!

[@mahanbabaee8998]

Loved it!

[@camilamartins3439]

Aula maravilhosaaaa! Muito obrigada por fazer esses vídeos

[@Shekhar.-_-]

Wonderful explaination,Loved it sir🙏

[@blackbear92201]

Awesome video. Subscribed. thanks for posting! :D

[@mecatx]

great video and graphics. Please explain visible light waves as hydrogen only has limited electrons therefore limited drop levels. Thank you.

[@cohesivechemistry]

I'm not sure I understand your question. What are you asking?

[@patrickurey7983]

Enriching content and well explained. Thank you sir!

[@cohesivechemistry]

Good to hear ;)

[@DEV.estaAqui_]

nice, this video gave me a full clarity

[@cohesivechemistry]

Glad to hear it!

[@matejkunz2719]

Well explained! Helped a lot :)

[@cohesivechemistry]

Glad to hear it!

[@sujeewaweerasingha1592]

Thank you so much sir!! This helped me a lot.

[@cohesivechemistry]

Excellent. Thanks for letting me know!

[@catalinaginer]

thanks goat

[@ChandrikaJayamini-pu9sb]

Nice. Thanks a lot❤

[@malwre_android1617]

Honestly wonderful. Tysm!

[@cohesivechemistry]

Glad to hear it!

[@yoihenbath]

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???

[@cohesivechemistry]

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.

[@rats1740]

thanks a bunch :)

[@comfortonuoha805]

Very educative 🤗

[@cohesivechemistry]

Thanks for watching!

[@yoihenbath]

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?

[@cohesivechemistry]

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.

[@yoihenbath]

Why is the emission spectra only the visible part ? Why is there no uv or infrared

[@cohesivechemistry]

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!

[@yoihenbath]

Does the light we supply contain uv and infrared also?

[@cohesivechemistry]

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.

[@comfortonuoha805]

@@cohesivechemistry the ones we see are which type of waves??

[@cohesivechemistry]

@@comfortonuoha805 They are the waves which have a wavelength between approximately 400-700 nm (known as 'visible light').

[@aureliem1762]

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

[@cohesivechemistry]

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?

[@aureliem1762]

@@cohesivechemistry thank you, it clarifies ! Thank you for your channel i learn a lot of things

[@yoihenbath]

Are the electron of the hydrogen atoms in the same initial energy level??

[@cohesivechemistry]

Yes, in its 'ground state' each hydrogen atom would have 1 electron in the first energy level.

[@Xxx87612]

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!

[@cohesivechemistry]

'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]

@@cohesivechemistry thank you and what does higher frequency means here??

[@cohesivechemistry]

@@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]

@@cohesivechemistry that explain why tungsten emission spectrum seems really dense at the “blue edge”

[@cohesivechemistry]

@@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).

[@nickbassan-iw2uc]

que vídeo BOM

[@air81235]

Niceee video

[@edaibrahimoglu1308]

thank you so muuuch

[@cohesivechemistry]

No problem.

[@mickey4984]

Why is it that the light emitted is mainly red?

[@cohesivechemistry]

That is actually just because of my limited drawing ability. The white light should contain an even distribution of the different colours.

[@dominicestebanrice7460]

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.

[@cohesivechemistry]

Hmm, valid questions but possibly a little beyond my area of expertise 😅

[@user-zc7qn7gl4d]

Why are we using the second energy level

[@cohesivechemistry]

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.

[@jasonbrar7996]

What’s the frequency of white light ?

[@cohesivechemistry]

'White light' contains all the frequencies in the visible part of the spectrum so has no specific frequency itself.

[@boonaaoromoo1690]

how to change if get n=3.78 when we calculate

[@cohesivechemistry]

Can you explain your question in a bit more detail? What are you trying to calculate and what data are you given?

[@delulu28]

may your pillow always be cold

[@cohesivechemistry]

😂

[@shaistabadar3529]

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