Why Electrons Don't Stick to Nuclei

In summary, the electron does not stick to the nuclei because of the concept of orbitals and the stability of the nucleus. The electron can occupy a spot in the nucleus, but it is not pulled in because it would involve electron capture, which would turn a proton into a neutron and create an unstable nucleus. The electron remains in its orbital to maintain the stability of the nucleus. This process is known as "K-capture" and more information can be found on Wikipedia.
  • #1
karawan
14
0
why the electron does not stick to the nuclei?
 
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  • #2
Sometimes it does. Look up "K-capture" on Wikipedia.
 
  • #3
The electrons occupy "orbitals" around the nucleus of an atom. These orbitals can only be in certain discrete values. The probability of an electron occupying a spot in the nucleus is NOT zero, it is an actual finite number, however the electron doesn't "stick" to the nucleus. The electron isn't pulled into the nucleus because that would involve electron capture and turn a proton into an neutron. If it is more favorable for the nucleus to remain like it is (AKA the nucleus is stable) then there is no reason for the electron to be captured and it remains in its orbital. Turning the proton into a neutron would form an unstable nucleus and probably result in beta decay (the opposite of electron capture) right back to where the situation was originally.

See here for more info: http://en.wikipedia.org/wiki/Atomic_orbital
 
  • #4
i was looking for the answer to this question when stumbled upon your post... thanks for explanation...
 

1. Why don't electrons stick to nuclei?

Electrons do not stick to nuclei because they are constantly in motion and have a negative charge, which creates a repulsive force between the negatively charged electrons and the positively charged nucleus.

2. How do electrons stay in orbit around the nucleus?

Electrons stay in orbit around the nucleus due to the balance between their kinetic energy and the attractive force of the positively charged nucleus. This balance is maintained by the quantum mechanical properties of electrons.

3. Can electrons ever come into contact with the nucleus?

No, electrons cannot come into direct contact with the nucleus because of the Heisenberg uncertainty principle, which states that it is impossible to know both the position and momentum of an electron at the same time. This means that the electron's position is always uncertain and it can never be exactly at the same point as the nucleus.

4. What happens if an electron gets too close to the nucleus?

If an electron gets too close to the nucleus, the repulsive force between the negatively charged electron and the positively charged nucleus will become stronger than the attractive force. This will cause the electron to be pushed away from the nucleus and back into its stable orbit.

5. Why do electrons have different energy levels in an atom?

Electrons have different energy levels in an atom because they can only exist in specific energy states, as dictated by the laws of quantum mechanics. The closer an electron is to the nucleus, the lower its energy level is. Electrons can move between energy levels by absorbing or emitting energy in the form of photons.

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