Uncertainty Principle Explained in 60 seconds | Quantum Theory

The uncertainty principle is a fundamental concept in quantum physics, introduced by the German physicist Werner Heisenberg in 1927. It states that it is impossible to simultaneously know a particle's exact position and momentum (or velocity). This principle highlights the intrinsic limitations of measurement at the quantum level and has profound implications for our understanding of nature.
One of the key ideas behind the uncertainty principle is wave-particle duality, which states that particles such as electrons exhibit both wave-like and particle-like properties. When we try to measure the position of a particle precisely, we are dealing with its particle-like properties. However, when measuring momentum, we are dealing with its wave-like properties. Since waves do not have a precise location, measuring one aspect (like position) disturbs the other aspect (like momentum), leading to inherent uncertainty.
The uncertainty principle explains why certain phenomena, such as the stability of atoms, occur. Electrons in an atom do not spiral into the nucleus because their positions and momenta are governed by quantum probabilities rather than classical trajectories.

[@heman2019]

🥇 ❤

[@geenethmethmin2487]

Poor turtle is still a size of an electron 😢

[@3D_Printing]

But if you change time then it could make it more certain

[@arnoldpaschal8368]

Why?

[@Jack-r2v9b]

Why not

[@manepepe4776]

it's very fast