Emission spectrum Puns

The title says it all. Couldn't find an answer on Google. Is the colour of the flame simply due to it burning so hot and emitting Plankian/blackbody radiation (like a red-hot poker), or due to the presence of magnesium ions (like copper burns with a green flame)?

Mg burns in air at 2500 K if that helps.

Edit: Question has been answered, thanks to all.

Hi,
I'm a research student in chemical engineering versing myself with instrument analysis techniques. I came across an emission of spectrum (image here) through an introductory book I'm reading. Was thinking about the continuum portion of the spectrum. The book says thermal emissions caused by incandescent particles are the cause of the continuum. Just want to clarify whether these emissions are different from electronic transitions that cause the lines and bands on the spectrum? Also, what phenomena in the atoms/ions cause this thermal emission, is it energy loss via vibrational state transitions, long wavelength emissions? (Would it be a correct deduction that long wavelength light e.g. infrared are not associated with electronic transitions?) Would appreciate help to have a good understanding of the continuum section of the spectrum.

Serious question. Why not just spend some time sitting next to a fireplace? I guess I should qualify my question a bit. Apparently, the theory holds that these lights work because humans used to run around in the daylight and sit by fires at night. Both are great sources of infrared light that science is just now figuring out has some biological activity. Our artificial indoor lives (little sun exposure) and artificial lights from electronics and LED bulbs are not providing the IR light that our bodies need. However, many people, me included, have a fireplace in their homes. So why can we not get the same benefit by sitting shirtless next to the fire? It's there something special about these lights that you can't get from a natural gas or wood burning fireplace?

What I'm trying to do is determine which of two lights are brighter at 650nm. One is a 3200k incandescent and the other is an overall brighter 5600k hmi. I have the emission spectrum and total visable luminous output of the lamps.

I know

-orbitals of the same principle quantum number are degenerate so they wont be responsible for any emission

-S to S transitions are not allowed

-Emission only comes from going down in energy

What else am I missing to figure out this question?

https://isaacphysics.org/questions/chem_16_e_5

If it only has one electron then won’t that electron only be able to emit one frequency of light at a time.

(Reading that I realise separate measurements might be taken. If that’s true, how do can well the emission spectra from different elements apart?)

Journal of the American Chemical SocietyDOI: 10.1021/jacs.0c08182

Andrés Zavaleta, Aleksandr O. Lykhin, Jorge H. S. K. Monteiro, Shoto Uchida, Thomas W. Bell, Ana de Bettencourt-Dias, Sergey A. Varganov, and Judith Gallucci

https://ift.tt/3kKAVGx

Hello everyone,

I've googled this a couple times, and for some reason I'm not getting a suitable answer to this question. By emission, I mean emission of a certain frequency by excitation with another. I read that certain spin interactions/changes(forgive me for not being particularly knowledgeable on this subject) can emit lower-energy radio bands. But aside from this, it seems like infared is the predominate frequency of the lowest energy emitted in most materials.

In case your wondering what the application of this question is, it relates to power generation. It seems like if such a material existed that emitted ELF radio waves that it would be exploited for this purpose, given that ELF can be directly converted to electrical power by electromagnetic induction. So, in the case of a nuclear reactor, suppose we have material A, that absorbs gamma rays and emits ultraviolet. Then, this ultraviolet hits material B. Material B absorbs the radiation, and simultaneously emits infared. Finally, material C absorbs infared and emits[ideally] ELF radio waves, or even just microwaves. Now the argument might arise that the energy output of such a system is less efficient.

First and foremost, the system of a fission reactor is not particularly efficient to begin with. There is tremendous heat loss through friction of the generator and conduction away from the reactor itself.

Secondly, even though higher energy radiation becomes lower energy radiation, I assume that there is more of the lower energy radiation(that is, more waves) then there would be absorbed high energy radiation.

Because of this, it leads me to assume that the output of such an absorption-emission would be extremely low voltage and high current. Of course, the dynamics of the output could be optimized through the use of several transformer stages, and then the power would be more usable for long-distance applications.

So, overall, the question that I'm asking is are there any materials that have radio waves in their emission spectrum? And I'm talking about emission by absorption of a higher frequency.

Sorry if this is a little out of the topic of chemistry, I figured that it was something most people versed in the field know about and both relate to materials science.

Thanks and all response is much appreciated, Reece.

Hi Reddit! I am given the following photo, and the question is which spectrum is an emission one, and which one is an absorbion spectrum(related to spectral lines and Rydberg constant) https://imgur.com/a/2kGVMiJ

As far as I remember, the emission and absorbion spectrums are the same, and in my opinion, the corect answer would be that we cannot tell which spectrum is emission/absorbion. However, I am not sure and I would appreciate some help.

When you put prism in the path of the sunlight you get a nice spectrum spread from red to violet (and beyond the visible part). Why do we get that spectrum? Why don't we see emission lines from hydrogen or helium? Where do other wavelengths come from? How do you "take out all those photons to see say He lines (how helium was first discovered)? I think I read somewhere you can sometimes see absorption lines from atmosphere gases, but why not original source bands? How does it work that we can determine composition of other stars or even exoplanets from their light if everything we get is "white"?

Sorry for lots of questions, it just popped in my head.

For example does hydrogen and deuterium have the same electron energy levels or do they depend on neutrons too?

If it's too much to ask would someone explain and or show an example as to how to do the assignment below. Sorry if the post is a bit long.

This is what was given

The thing that confuses me is how would I record the wavelengths if the lines are close to each other. The professor mentioned that we could create a range but it creates a new problem in the next image.

The problem is that: What would I enter for the wavelength in the equation above since I would have a range instead of a single integer. Also, correct me if I'm wrong but to get RH would divide (1/n - 1/n) from the 1/ wavelength.

Any help would be greatly appreciated.

Where could I find data on the emission spectrums of different stars (MK, neutron, white dwarfs, etc).
I'm looking more for data on neutron stars since I looked at the wikipedia page and it mentioned it put out mostly radio waves, except that some don't and some portion of the EM emitted is x-rays which has got me curious now. Any point in the right direction would be appreciated.

Hello!!! so i have a few problems in which i have to use rydbergs equation for energy (E= RH (1/n²-1/n²)) and the value for Rh i use is: 2,179x10^-18. Now i know that when the transition causes emission of energy the result will be negative, and if it causes absortion of energy it should be positive, but in the exercises i have the results i get are opposite to what they should be, so im wondering if what im doing wrong would be the order im using for the levels of energy??? Im using it like a delta aka Final energy level-Initial energy level, is this right? sorry for my english, im not a native english speaker 😅 and thank you!!!

Atoms have different absorption/emission spectra and the lines correspond to the difference in energy between states. But if the differences between energies were infinitely precise there would be no emission/absorption at all. So I wonder how it can be not exactly precise. Now my textbook refers to the Heisenberg uncertainty principle for energy, but I thought this only tells us that we don't know the energy of a state precisely, but that it is still assumed that there IS a precise energy. Not that the energy is distributed over a small range of values.

So the question boils down to: is it correct that the energy of an energy level in an atom is distributed over a small value as opposed to being exact?

I have been wondering about the spectroscopy of exoplanets and so far I have not encountered a paper where the thermal emission has been measured for a transiting exoplanet, but without having done anything close to a proper literature search. Has this been done? If it has been done (for extrasolar planets) can someone provide a reference and if not, are there proposals in the literature for doing so? What spectroscopic techniques are there for determining the surface temperatures of transiting exoplanets experimentally? E.g. would fitting the bands in transmission spectra be one such method? I was thinking that it should be easier to extract blackbody emission from the extremely strong background of the star than a high-resolution spectrum due to the very fact that it would need a far lower resolution than what is needed for identifying individual IR absorption bands.

Please don’t tell me to Google it because there’s nothing there.