What is Atomic spectra: Definition and 21 Discussions
The emission spectrum of a chemical element or chemical compound is the spectrum of frequencies of electromagnetic radiation emitted due to an atom or molecule making a transition from a high energy state to a lower energy state. The photon energy of the emitted photon is equal to the energy difference between the two states. There are many possible electron transitions for each atom, and each transition has a specific energy difference. This collection of different transitions, leading to different radiated wavelengths, make up an emission spectrum. Each element's emission spectrum is unique. Therefore, spectroscopy can be used to identify elements in matter of unknown composition. Similarly, the emission spectra of molecules can be used in chemical analysis of substances.
(I need help with the 2nd part as I can answer the theory part properly).
For E=4 eV we can find the wavelength of emitted photon.
E= 4 eV = 6.4087e-19 J
Using E= hc/λ we get λ=310 nm (approx)
My doubt is that this should fall in the Balmer Series but we know that the lowest wavelength value...
My book says that emission spectra are produced when an electron in excited state jump from excited to lower energy states. It also states that solids and liquids produce continuous spectra and it depends upon temperature only (is this black body radiation?).
I know, Electrons around a nucleus...
I was studying about atomic spectra of mono-electron species and in the pic it describes the ##4## series (principal, sharp, diffuse and fundamental).
However I'm a little confused by the formula.Here my doubts are:
Thanks for reading. [1]:
[2]...
If the spectral line of Hydrogen contains four colors, I don’t understand how the electron can jump four times to four different energy levels in the same moment?
I've seen the equation I think is just for hydrogen. is this just for hydrogen?
of course this doesn't return the atomic spectra, it returns the energy.
So using E=h*v and Planck's constant. a simple factor of 1/h would return the frequency.
right? Energy is directly proportional to frequency...
Consider a piece of pure Fe hot enough to have a bright white color (about 2 000 ºC, e.g.) and the characteristic yellow narrow yellow emission of the Na atom.
Does the Na yellow band will be present at the thermal spectra of the pure Fe?
My guess: Yes.
Homework Statement
Hi!
I have a a question regarding the Atomic Spectra of Hydrogen and Mercury. My problem involves the value of m and Rydberg's constant. I used a spectrometer for this lab and calculated all the necessary angles.
Homework Equations
See below
The Attempt at a Solution...
Scientists have measured both the blackbody spectrum and also the atomic spectra of various elements in the Sun.
How do they distinguish between the two and filter out the light from either one?
Hello all,
What is mean the Ritz Wavelengths in the NIST Atomic Spectra Database?
Why the Ritz or Observed value for some Wavelength are very different?
Thanks,
Lil
i am now studying the Doppler effect in a thermal atomic gas
If an atom travels in velocity v along x direction
at some time, it emits a photon in some direction
the momentum of the emitted photon can be well approximated with the free one
thus the momentum of the atom after the...
i am now studying the Doppler effect in a thermal atomic gas
If an atom travels in velocity v along x direction
at some time, it emits a photon in some direction
the momentum of the emitted photon can be well approximated with the free one
thus the momentum of the atom after the...
Homework Statement
A molecule with angular momentum L and moment of inertia I has a rotational energy that can be written as E=\frac{L^2}{2I}. Assuming that angular momentum is quantized according to Bohr's rule L = n\hbar, find the wavelength of the photons emitted in the n=2 to n=1...
In the hydrogen atom, an electron is in the 3d state.
(i) Find the orbital angular momentum of the electron (in units of
n =3, l = n - 1, l = 1. L = [sqrt( l (l + 1) )]hbar therefore L = sqrt(2).hbar
(ii) Find the energy of the electron (in eV).
En = -13.6ev / n^2. E = - 13.6eV / 9 (iii)...
In L. I. Schiff book, one can follow his derivation of the Hamiltonian from Dirac relativistic equation and obtain the following..
\left[\frac{\vec{p}^2}{2m}+V-\frac{\hbar^2}{4m^{2}c^{2}}\frac{dV}{dr}\frac{\partial}{\partial r}+\frac{1}{2m^{2}c^{2}}\frac{1}{r}\frac{dV}{dr}\vec{S}\cdot...
Hi! to everyone on the forum. I am new and did not really know where i should of posted this thread its not homework its just a question i have.
A friend of mine asked me a question about a book he read about (atomic spectra and atomic structure by Gerhard Herzberg). Gerhard Herzberg said...
An emission spectrum can contain wavelengths produced when an electron goes from the third to the second leve. So could you see this like in the absorption spectrum? Why?
I did a spectroscope experiment with a hydrogen discharge tube.
So far I got this data:
Line 1:
Color=Red
\lambda(nm)=700
\nu(Hz)=4.2*10^{14}
n1=?
n2=?
\Delta{E}(J)=2.8*10^{-19}
E(J)=?
This is only the data for the Red line. I figured if i knew how to do this, I'll...
I don't know a whole lot about quantum mechanics and there is something that dosen't make sense to me. An atom absorbes radiation in only certin frequencies. Do these frequencies have to be exact? Can they vary over a small range like say 1.000 to 1.001 or do they have to be perfectly exact...
Can somebody explain quantum tunneling to me? And the thing about why amplitudes when they are trapped, the energies must choose from a distinct set of values? And why when particles that are totally free to wander will have any energy that they like?
Also, why in the atomic spectra, more...
We all know that Maxwell did such a great work for all physicist. BUT, anyone knows that how Maxwell's theory of radiation could not explain atomic spectra?