Understanding the Proton-Electron Orbital: Why It Doesn't Stick to the Proton

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In summary, the electron is attracted to the proton because of centrufugal force, but it loses energy and is not able to stay there. The resolution to this problem was found with quantum mechanics, which showed that in bound systems, energy levels are quantized.
  • #1
Imparcticle
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When an electron is orbiting a proton, why is it not compelled to be attracted to the proton? Why doesn't it stick to the proton?
 
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  • #2
kinetic energy, of course.

why does not release its energy via radiation? Because of quantum theory.
 
  • #3
You mean the centerepital force is what keeps them from colliding? Can you expand on this?
 
  • #4
Imp, basically yes. The historical problem was that the electron is a charged body, thus it is supposed to radiate, losing energy and then losing centrufugal force. This was the problem adressed, and solved, with quantum mechanics.
 
  • #5
There is no energy state available that has it sticking to the proton. This is one of the problems that led to QM, as has been noted. Only specific energy states can be occupied.

The s-state electron's orbital actually has it in the nucleus some fraction of the time, but to actually combine with the proton would require a weak interaction, and that has a really small cross-section.
 
  • #6
Imp, basically yes. The historical problem was that the electron is a charged body, thus it is supposed to radiate, losing energy and then losing centrufugal force. This was the problem adressed, and solved, with quantum mechanics.
The fact that it loses energy prevents it from being attracted to the proton?

Just how was it resolved?
 
  • #7
Imparcticle said:
The fact that it loses energy prevents it from being attracted to the proton?

Just how was it resolved?

No, it's still attracted, which is why there is a bound system. QM shows that in bound systems, energy levels are quantized. IOW, not all states are available to the electron - the ground state orbit is as low in energy as it can get.
 
  • #9
You are up against the brick wall of QM where all problems are solved by inventing more names for things or actions that cannot be otherwise defined. This practice takes you around in circles, each step is mathematically perfect but grammatically confusing; there is no final explanation. That is why physicist are now inventing 'strings', 'branes' and 'super-strings'. Any day now there will be 'super-duper-strings'.
It seems that nothing can stop mathematicians from taking physics into the darkest corners of science fiction. If you want to work in this field (and the number of students willing to do so decreases year on year) you will have to jump on the merry-go-round.
 

1. How do protons and electrons interact within an atom?

Protons and electrons interact through electromagnetic force. The positively charged protons in the nucleus attract the negatively charged electrons, keeping them in orbit around the nucleus.

2. Why doesn't the electron stick to the proton?

The electron does not stick to the proton because of the balance between the attractive force of the proton and the centrifugal force of the electron's orbit. If the electron were to stick to the proton, it would lose its velocity and fall into the nucleus.

3. What is the role of the electron's orbital in an atom?

The electron's orbital is the region around the nucleus where the electron is most likely to be found. It determines the size, shape, and energy level of an atom, and is essential for the stability of an atom.

4. How does the distance between the proton and electron affect the atom?

The distance between the proton and electron affects the atom's size and energy level. The closer the electron is to the nucleus, the smaller the atom and the higher the energy level. Conversely, the further away the electron is, the larger the atom and the lower the energy level.

5. Can the electron's orbital change?

Yes, the electron's orbital can change. Electrons can move to different energy levels through the absorption or emission of energy, causing changes in the size and shape of the orbital. The electron can also jump to different orbitals, creating different chemical bonds and reactions.

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