Why Don’t Electrons Stick to Protons Despite Their Opposite Charges?

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SUMMARY

Electrons do not stick to protons despite their opposite charges due to the principles of quantum theory. In a hydrogen atom, the ground state represents the lowest energy level, where the electron occupies a probabilistic cloud rather than a fixed position. This behavior diverges from classical physics, as electrons and protons are not solid objects but rather exhibit wave-particle duality. A comprehensive understanding of this phenomenon necessitates a study of quantum mechanics.

PREREQUISITES
  • Basic understanding of atomic structure
  • Familiarity with quantum mechanics principles
  • Knowledge of wave-particle duality
  • Concept of energy levels in atoms
NEXT STEPS
  • Read "Introduction to Quantum Mechanics" on Wikipedia
  • Explore the concept of wave functions in quantum mechanics
  • Study the implications of the Heisenberg Uncertainty Principle
  • Investigate the behavior of electrons in various atomic states
USEFUL FOR

Students of physics, educators in quantum mechanics, and anyone interested in the fundamental behavior of atomic particles.

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If positive and negative charges attract each other, why don't electrons just stick to the protons?
 
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Explanation from quantum theory. Esssentially a hydrogen atom ground state is the lowest energy level.
 
JML said:
If positive and negative charges attract each other, why don't electrons just stick to the protons?

Because electrons and protons are not like small, solid billiard balls. They behave VERY differently than how you're used to objects behaving. There's no simple answer and a proper understanding would require getting into Quantum Theory. If you're interested you can start with the following article: https://en.wikipedia.org/wiki/Introduction_to_quantum_mechanics
 

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