Why do electrons not fall into the nucleus despite attractive force ?

Umesh Sanjyal . 1 week ago

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Due to the quantum mechanics, in particular the principle of Heisenberg's uncertainty and the concept of low energy levels, electrons do not fall into the nucleus despite the attractive electrostatic force between negative charges and positive load nuclei.

1. The principles of Heisenberg uncertainty This principle is as follows:

• It is impossible to know both the exact places and the movement of a particle at the same time.
• If the electron falls to the core:
• Its position is probably very well known (in a small nucleus)
• But the move will be very unclear.
• This means very high kinetic energy and makes the system unstable.
• Therefore, nature prevents the trap of electrons in such a small space.

2 quantum energy levels Atom:

• There are electrons at a specific or orbital level, not in the middle.
• The lowest level (called the land state) is the closest stable state that an electron can occupy.
• For example, the electrons in a hydrogen atom are currently in the least possible state of energy and lose their energy and cannot be reduced further.

3. The nature of the electron waves

• Only a specific wave pattern (standing wave) can be placed around the nucleus.
• Even if you fall into a nucleus, no reputable wave patterns are permitted, and quantum rules prohibit it.

In Summery 

• The electrons do not place in the nucleus
• Quantum rules (such as the principle of uncertainty) prevent accurate localization.
• Electrons occupy sustainable energy levels that do not spread energy.
• Wave behavior only enables certain paths. This is not a direct collapse to the nucleus.