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When an electron is moving around in its orbital, is it actually moving around like a wave, like this video shows? (By wave-like, I mean, the 'electron' in this video is showing it following a predictable wave-like path, which would mean you could precisely determine its position which obviously you can't).

http://i.imgur.com/DrBIfBV.png

Or, instead, does it just have some probability to be in that orbital's space, and just randomly jumps around from one point to another? Or if not that, how does the electron move around in its orbital?

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Orbitals are solutions to time-independent quantum wave equations.

That is, there is no time-dependence. There is no little ball in there moving around, the electron has a quantum characteristic and exists with neither a well defined position nor a well defined momentum.

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    $\begingroup$ However, it does have a well defined angular momentum, just to make things confusing. $\endgroup$ – Jerry Schirmer Sep 14 '14 at 21:41
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    $\begingroup$ Worth repeating: There is no little ball in there moving around. $\endgroup$ – garyp Sep 14 '14 at 23:49
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    $\begingroup$ Confusingly enough, you can however take a picture of the little ball in there, with a definite position. Even though there is not little ball moving around... However, when you do that, the little ball is no longer "in" the orbital. $\endgroup$ – Aron Sep 15 '14 at 3:25
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dmckee is right. However I would like to add some notes to provide an intuitive connection between the asker's question and the answer.

When we conceive of the orbital as a 2-dimensional surface in 3-dimensional space, as in the video above, we are not looking at the orbital. We might be tempted to say we are looking at the outline of the orbital, but the orbital extends infinitely into space. What we are actually looking at is a surface, within which the probability for the electron to be found is less than some number, for example 90%. Generally, a different choice of probability will not change the shape of the surface. This is convenient for the purpose of understanding what orbitals look like.

That being said, the orbital is not a 2-dimensional surface in 3-dimensional space. The orbital is a complex scalar in 3-dimensional space, meaning that for every point $(x,y,z)$ the orbital has a real and imaginary part. That being said, we generally only care about the magnitude which is a positive real number. The physical meaning of this number is the probability per unit volume, for the electron to be found at this point in space.

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    $\begingroup$ FYI, calculating the surface within which there is 90% probability is actually quite challenging unless the orbital is really simple and analytic. So usually what is plotted is just an isosurface on which the probability density is at a given figure, because that's much easier. $\endgroup$ – Phil H Sep 15 '14 at 13:16
  • $\begingroup$ Isosurface, that's the word i was looking for. Thank you $\endgroup$ – Anthony Sep 15 '14 at 16:49
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Neither. Electrons in "orbitals" are not moving (I don't like the term "orbital". I leave it to chemists. I prefer "wave function". More exactly, wave function of a stationary state. This means that nothing changes in time.)

It isn't even correct to identify a wave function with a "probability amplitude", i.e. as giving probability density with its modulus squared. It is true, but it isn't all. A wave function allows you to compute the mean value of any observable you want, e.g. angular momentum. As @JerrySchirmer notes, an electron in a stationary state may well have a definite (non-zero) angular momentum (not necessarily, however).

The electron does not have a definite position, neither can you say it is moving ... and so on. If all this sounds paradoxical, welcome to quantum mechanics. One point is never too much emphasized: you cannot understand QM concepts by reducing them to classical world. Entirely new ideas are at work there, and current language has no hope to express them, not even approximately.

Feynman speaks about this in several pages of QED. Just one quotation:

"The theory of quantum electrodynamics describes Nature as absurd from the point of view of common sense. And it agrees fully with experiment. So I hope you can accept Nature as She is - absurd."

Just a little comment to these words. Nature is not only absurd for common sense. It is so for a classical physicist too, when it comes to the phenomena we began to encounter a century ago or little more. Moreover, I am less optimist than Feynman was in that conference. I don't believe Feynman's listeners will have accepted something. More likely, they will have left the conference room thinking "I can't believe it, but if a great man like Feynman says it's so, I'll bow my head, respectful."

I also visited the link given by @ImmortalPlayer. I'm sorry but I think those answers too miss the point. There's nothing wrong, but in my opinion the real difficulty is not addressed - just touched. He who wants to approach QM must accept that an entirely new way of thinking of physical phenomena and theories is needed - a new paradigm, to use a word coined by Thomas Kuhn. It's not impossible, and the first steps can also be taken before immersing oneself into advanced physics study. But the right attitude is essential: not to demand that the new physical world be understandable remaining within old thinking habits.

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According to the wave particle duality, an electron behaves like a wave and as a particle in certain cases. but when we specifically talk about the movement of an electron around a nucleus, it behaves like a wave. hence in electron capture phenomenon we know that the nucleus capture the electron as it moves like a wave.

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    $\begingroup$ "nucleus capture the electron as it moves like a wave" doesn't make much sense to me. $\endgroup$ – user191954 Oct 18 '18 at 8:50

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