27
$\begingroup$

I'm just starting to learn physics and I have a question (that is probably stupid.)

I learned that energy levels that the bound electron can have are discrete. I also learned that when an electron transitions from one level to another, a photon with a specific wavelength (energy) is created and released into the wild.

My question is this: are there holes in the electromagnetic spectrum, values of frequency that the created photon can't possibly have?

$\endgroup$
0

4 Answers 4

25
$\begingroup$

No, there aren't any holes like that in the EM spectrum.

There are other ways of creating photons than by having electrons bound in atoms transition from one level to another. (For example, you can create pretty much any frequency of photon you want by accelerating a free electron.)

$\endgroup$
5
  • $\begingroup$ Ah, I see. That was one of my presumptions - that there are other ways of creating a photon. Thank you. $\endgroup$
    – Andrej T.
    Commented Aug 12, 2013 at 15:01
  • 3
    $\begingroup$ You can also continuously vary the frequency of an existing photon with relativistic effects, e.g. gravitational redshift/blueshift. $\endgroup$
    – Kyle Oman
    Commented Aug 12, 2013 at 16:41
  • 2
    $\begingroup$ any frequency - isn't it limited by the Planck constant? $\endgroup$
    – vsz
    Commented Aug 12, 2013 at 20:01
  • 2
    $\begingroup$ Even with electrons bound in atoms transition from one level to another, EM radiation is not discrete, due to natural broadening, pressure broadening, thermal broadening. $\endgroup$
    – gerrit
    Commented Aug 12, 2013 at 23:13
  • 2
    $\begingroup$ @vsz: It may be possible that there is discreteness of some intrinsic properties of photons at a very low level. If it is the case, then is beyond any current measurement, and there is no widely-accepted theory that links any such property to frequency. If there was such a theory it would probably also involve discreteness of space/time. $\endgroup$ Commented Aug 13, 2013 at 8:26
19
$\begingroup$

The other answers are correct, but I think they miss one important point.

The energy levels are not really discrete, because:

  • Frequencies are not exactly defined. Due to the Heisenberg uncertainty principle, the location and frequency of a photon cannot both be exactly determined. Therefore, emission (and absorption) does not happen at an exact frequency, but at a finite range of frequencies. This is called natural broadening.

  • Next, molecules do not exist in isolation. They collide with other molecules, which again changes the energy levels. This is called pressure broadening.

  • Next, molecules are not stationary, but are quickly moving. This also causes the energy levels (absorption/emission lines) to broaden. This is called thermal broadening.

The latter two are much stronger than the first one (at least in the Earth's atmosphere), but the first one is very fundamental as well. Energy levels are not really discrete. Therefore, the electromagnetic spectrum is not, either.

$\endgroup$
1
5
$\begingroup$

You mention that the energy levels of a bound electron are discrete. Have you considered the energy levels of a unbound electron? In this case, the energy levels are not discrete, but rather continuous and can take on any frequency.

$\endgroup$
1
  • 1
    $\begingroup$ Yes. The most obvious example is black-body radiation. $\endgroup$
    – gigacyan
    Commented Aug 13, 2013 at 7:58
5
$\begingroup$

Even if a photon is created by the transition of electrons in an atom, if the atom is moving relatively to the observer, the Doppler shift changes the frequency. In principle, any frequency can be obtained like this.

$\endgroup$
2
  • $\begingroup$ Isn’t that only the observed frequency from the observers perspective? The actual frequency stays the same, no? $\endgroup$
    – Hisham
    Commented Apr 20, 2019 at 18:26
  • $\begingroup$ @Hisham The observed frequency is the only frequency. Everything is relative. $\endgroup$ Commented Feb 14 at 8:58

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service and acknowledge you have read our privacy policy.

Not the answer you're looking for? Browse other questions tagged or ask your own question.