Heisenberg Uncertainty Principle
What is Heisenberg Uncertainty Principle?
The Heisenberg uncertainty principle states that it is fundamentally impossible to simultaneously determine both the exact position and exact momentum of a subatomic particle with arbitrary precision. Mathematically, Δx · Δp ≥ ħ/2, where Δx is the uncertainty in position, Δp is the uncertainty in momentum, and ħ is the reduced Planck constant. This principle has profound implications for atomic models, leading to the replacement of Bohr's fixed electron orbits with probabilistic atomic orbitals.
Key Facts
Frequently Asked Questions
The Heisenberg uncertainty principle states that it is fundamentally impossible to simultaneously determine both the exact position and exact momentum of a subatomic particle with arbitrary precision. Mathematically, Δx · Δp ≥ ħ/2, where Δx is the uncertainty in position, Δp is the uncertainty in momentum, and ħ is the reduced Planck constant. This principle has profound implications for atomic models, leading to the replacement of Bohr's fixed electron orbits with probabilistic atomic orbitals.