Excited state.. atomic structure
so when we irradiate or heat a sample, it gets excited - does that mean that photons pushed electrons from there original position??
and when the unstable atoms(atoms or electrons?) tend to get stable again, they go back to there original position by emitting the absorbed radiation again.
Now we will measure the wavelength of the emitted radiation and the book says we will get the emission spectrum by measuring the wavelength now the question:-
How can we get a whole spectrum when we have just measured a single wavelength?( acc. to me we will just get one color)
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@Dexter
Note for OP
+solved @user to close the thread when your doubt is solved. Mention the user who helped you solve the doubt. This will be added to their stats.To the best of my knowledge, in an experiment, a single electron may not get excited... it'd be a cluster of electrons. They'll get excited into different orbitals according to the energy they've consumed. While coming back to ground state they'll follow different paths...
For eg: an electron in n=5 will jump to 3 then to 2 then to 1. Another one at n=6 will jump to 5 and directly to 1.
So in this case the whole spectrum is obtained.
If we take a single electron species then a similar thing happens. The single electron will get excited into let's say n=5. To reach 1st excited state (n=2) it could follow 6 different paths, emitting different wavelengths in each of them thus forming a spectrum
I'm not 100pc sure so it'd be better if @iTeachChem clarifies this..
thanks mate i got better at understanding these minute particles
i have not learned anything about "orbitals" as these spectra thing comes earlier than these things so i think i will get better by reading further
yes @iTeachChem I think i need your help too
this is a brilliant example. also, the excitation can happen due to heat or anything else too, not necessarily photons
this is about orbits. orbitals are different
have you checked my session about this? i taught this in the first session of atomic, absorption and emission. emission will be a few scattered lines, absorption will be alll but the lines (ie som missing)
emission is by a hot gas,
absorption is by a cold gas
the book is right, emission spectra is usually just a few lines (esp for hydrogen)
for multi electron species you get a more complicated spectrum
https://webbtelescope.org/contents/articles/spectroscopy-101--how-absorption-and-emission-spectra-work
see this
ok sir will check out ur session too
just read this, should suffice 🙂
okayy
+solved @Flint
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