qm01 自旋01 matter wave electron is still being thought of as a pointlike particle with charge, but it's location is uncertain, and this uncertainty is where the "waviness" comes from.

If electrons behave as standing waves when they are bound to an atom then how do they carry charge?

 

夸克带电的，正电和负电都有
粒子不确定，任何微小的物体都可以叫粒子
轻子包括电子、μ子（渺子）、τ子（陶子，重轻子）三种带一个单位负电荷的粒子，
传播子没有听过
量子是单位，哪有带电不带电一说
分子不带电
光子不带电

  

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Today in my physics lesson we learnt that the best way of describing the behaviour of an electron that is bound to an atom is to treat it as a standing wave. I understand that this is the wave-particle duality however I was taught that in the wave-particle duality something either acts as a wave or a particle, not both at the same time. With this in mind I'm curious as to how electrons can still carry charge when they are behaving as a wave. I asked my teacher this question and he wasn't able to answer it so hopefully someone on here can explain it to me :) waves electrons charge particles duality share|improve this question asked Feb 6 at 18:34 James Parker 311

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It's likely that your mental picture of the "wave" that describes the electron is misleading you. If you're thinking that the electron itself is spread out in the form of the wave and that it's charge is too, then you should rethink your picture. The electron "is" or "behaves like" a wave in that it's state is described by something called a wavefunction. What does this mean? Well the wavefunction basically tells you the probability of measuring where the electron will be if you try to measure the position of the electron. In this picture, the electron is still being thought of as a pointlike particle with charge, but it's location is uncertain, and this uncertainty is where the "waviness" comes from. So, for example, let's consider the electron in the Hydrogen atom. It's best not to think of the "wavelike" nature of the electron as being represented by a wavy thing circulating around the nucleus or something of that sort. Instead, imagine that the wavefunction of the atom determines a sort of "cloud" with regions of different density where the electron is most likely to be found if one were to measure its position, like in the following image: You might find this hyperphysics link illuminating in this regard. share|improve this answer answered Feb 6 at 20:00 joshphysics 27.5k22367

You are misguided by your mental picture of "probability". There is no experiment which demonstrates that orbitals indeed do look like that. Nobody measured any electron probability in hydrogen atom during 100 years of existence of QM. Even measuring famous angle in water molecule is FAAAAR from obvious. There is NO answer to OP question. –  Asphir Dom Feb 6 at 20:41 2   @AsphirDom A pretty brazen accusation. What I'm describing in my answer is a standard quantum mechanical model. What your saying amounts to "we shouldn't believe the model because our evidence for it is to some extent indirect;" that's as absurd as saying that there is no answer to the OP's question. –  joshphysics Feb 6 at 20:49 Not brazen. Simply your line of thought is invalid (as well as in many QM textbooks). If you would show spectra or something REALISTIC i would have nothing to say. –  Asphir Dom Feb 6 at 20:58 1   Some of the best images in physics right there. –  Kyle Kanos Feb 6 at 21:01 I think I understand what you're saying as it links to what we've been doing in chemistry. Correct me if I'm wrong, but does the wavefunction explain why orbitals are certain shapes because aren't the orbitals just the region in which there is the highest probability of finding an electron (you find them there 95% of the time if I remember correctly)? So if you could somehow freeze an atom at a point in time then the electrons would be particles with point charge however as the electrons are constantly moving the best way of describing them is as waves. Hopefully I've understood correctly :) –  James Parker Feb 7 at 17:37 show 6 more comments

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